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DETECTION, DETERMINATION AND THIN-LAYER CHROMATOGRAPHIC SEPARATION
OF ANIONS
Abstract
THESIS SUBMrrTED FOR THE DEGREE OF
Bottor of $I)Uo!E(opI)p IN
APPLIED CHEMISTRY
'N^.^i;-^t>
BY UNDER THE SUPERVISION OF
SHAR4D TIWARI Dr. AH Mohammad Read«r
DEPARTMENT OF APPLIED CHEMISTRY ZAKIR HUSAIN COLLEGE OF ENGINEERING AND TECHNOLOGY
ALIGARH MUSLIM UNIVERSITY ALIGARH (INDIA)
1991
The thesis comprises of six chapters in all dealing
with detection, identification, separation and quanti
fication of anions. The highlights are the systematic
analysis of anions in the solid state and the development
of new sorbent phases for thin-layer chromatographic
studies of anions.
Chapter-I presents an overview of all important
aspects of chemical analysis with detailed discussion on
spot-test analysis and thin-layer chromatography. An
extensive literature survey has been presented on the
procedures involved in the analysis of inorganic ions.
Significance, mechanism and applications of analytical
solid-state color reactions have also been discussed. The
work done on thin-layer chromatography of anions till date
has been described in tabular form, whereas the comparison
of work done on cations and anions during last decade has
been shown graphically.
Chapter-ri summarizes our efforts of utilizing
capillary solid-state spot-test technique for systematic
analysis of anions. A glass-wool plug modification has been
added to the capillary technique to make a test more
selective or even specific. Several new reagents for solid
state detection of anions have been identified. The color
reactions of powder trituration method have been compared
with those obtained in solution state. Table 1 summarizes
the solid state color reactions of anions with various
reagents. The order of selectivity and sensitivity of these
methods is given below:
Selectivity: Glass-wool plug modified capillary method >
capillary solid-state method > powder trituration method.
Sensitivity: Powder trituration method > contact capillary
solid state method > glass-wool plug modified capillary
method.
Based on the solid-state reactions two schemes for
the systematic analysis of anions in the solid state have
been proposed.
In Chapter-Ill investigations regarding thin-layer
chromatographic behavio r of 17 anions on silica gel
impregnated with inorganic salts such as copper sulfate,
zinc sulfate, cobalt chloride, hexamine cobalt III chloride
and nickel chloride using mixed aqueous-organic eluents
containing formic acid have been summarized. The effect of
mineral acids on the mobility of anions has also been
studied by substituting formic acid with HCl , H^SO, or
HCIO, in the mobile phase. In addition to microgram
separation of NO2 and IO3 from various anionic species,
(Table 2,3), some other important qualitative separations
have been realized. The effect of pH on the sample solution
and loading amount of IO3, Br03 , NO2 and I on their Rp
values have been investigated. The limits of identification
for all anions on impregnated layers have been determined.
The developed procedure has been utilized for the semiquan
titative determination of NC2 and Br03.
Chapter-IV deals with the utility of water as
eluent in thin 1ayer chromatographic separation of various
anions on plain (silica gel G, alumina and cellulose) as
well as on mixed beds containing different combinations of
silica gel, alumina or cellulose. Microgram separation of
_ _ 2-10^ from milligram quantities of IO3, Br03, MoO^ and
Fe(CN)g has been realized. Effect of pH of sample in the
separation of 10^ from accompanying ions has also been
studied. The limits of detection of anions on alumina thin-
layers have been determined, NO2 in artificial sea water
has been detected. Effect of hardness causing ions on some
separations of analytical importance has been examined and
the results are presented in Table 4.
Chapter-V deals with thin-layer chromatographic
studies of some anions on plain and impregnated silica gel
layers in aqueous-organic solvents containing acetone. The
results obtained on plain silica gel have been compared
with those obtained on copper sulfate impregnated layers.
The impregnated layers dramatically change the selectivity
and permit separations not possible on untreated silica.
Aqueous sodium chloride-acetone (9:1) and ammonium
hydroxide-acetone (9:1) were the most effective solvent
systems for differential migration of anions. Better
results in terms of clarity of detection and compactness of
spots were found with HCOOH-acetone as compared to
HCl-acetone. Finally identification limits for all anions
on impregnated layers has been determined as shown in
Table 5.
Chapter-VI summarizes results achieved on the
separation of 10^ from other anions in the presence of
common cations, using silica gel layers as stationary phase
and distilled water as mobile phase. A volumetric method
has been devised for the determination of iodate with
priliminary TLC spearation from preiodate. Some TLC
parameters such as^Rp (Rp of IO3 - Rp of 104), separation
factor ( cK ) , capacity factor (K') and resolution (R ) on
the separation of IO4 from IO3 have been computed as shown
in Table 6.
• J
Q O o
Qi
u re CTi
c 0) M TO OJ Di
OJ B 0 (/)
XI 4J •H
w C o
<
o w c o
•r l 4J O re cu
D.S
•U
w
I
o a (/)
(U 4J re 4J CO I
T ) •H
O CO
!r,
o 0 00
P re
a B
H
I f
t f
I I
4 f +
I I
J + * I I I I I + f I
I I •• I I I I + I + I
I I I ( I I t { I -h (
t- t- f f + -( I I t < f
t t I 4 y i \ (. + (. J.
+ + I I + I I + + +
+ 1 I + I + + I + •-
+ < I I + + I + +
I I I I . I I I
f I I I I I I
I I I I I I I
f I I f -) ^ +• +
I I I I I I I
t i I I I I I
1 1 1 ) 1 ) + +
1 + 1 ) 1 ) )
I I I ) ) I )
I i I I < I )
i I I f ) ) +
I I ) ) ) ) I
+ ) + + + + + + + + + + +
) ( I I ) ) + + + + + ) )
^ i + + + + + + f + + + +
I ) ) ) ) I M I ) I I I
+ + + + + + + + + + + + )
) ) ) ) I I I I ) ) i ) )
) + + ) I + + I ) ) +
) + + ) ) + + I ) + )
/ ( ( ( ( ( ( ( ( + +
+ + ) ) ) + ^ + + ( - ^ •
+ + + » - + i + + + +h +
1 + + + ) + + ) + + +
1 + + I I + + + I ) I
) ) ) ) ) + + + ) + +
I I I +'i ^ + I I + I
I I + I I + + ( I I !
I I I i I + + I I -t I
) + ) + + + + ( - ) + +
] ) I + I I ) ) I + )
I ) )
I I I
) + )
) ) >
) ) )
) I )
) I >
) ) I ) ) ) >
I ) ) I I I )
1 ) 1 ) ) ) )
I + + ) ) + )
) ) + • ) ) + I
I + + ) ) + )
I + + ) ) + +
+ + + + ) + +
! I + I I I I
+ + + ) ) + H
1 + I ) ) I )
+ + + + ) ) +
) > H- ) I ) )
X a. )
i •i
Z _ n
0. Z tn
tri
+
^^ u. n r t
z (A + 0 — z
u.
n
_ j c. 0.
o'
z o '0 u. T r i
00
* X
. 0 Z
< «n r t
!2
+ •— u
^ r» ao <>v o
y " £ < < < * y H I- < < Q a a O O — n r T '
o z z
~ 01 a. — 1 " O + o < Q Q r 2 I- h Q Q t. li i. a a
^ r ^ DO ^ O
+ a a < < + o
< < < a a S 5 c — rt f^ *r *^
3 »\ r>i I - L c
( ORANGE
1 NOCOLOn
o n FEN —»-yELLOV/
CrO 2-
r
NO colon
GHEEN —»'YELLOW
f f (CN)g3"
1
NOCOLO"
1.2 r coLon NOCOLOR
. 1" PINK 5 C N -
NOCOLOR PINK j12 CO32-
BRQWN
VO3-
1 NOCOLOR
I" I
VELLOW
| -
COLOR
_J1L 1
NOCOLOR
1 NOCOLOR
I" RED
5 2 0 6 ^ -
I BROWN
BrO i "
NOCOLOR
O R A N G E - Y E L L O W NOCOLOR
Br- ] ? 6 I
R E O - - * - B L A C K
S ^ O j Z -
1 NO CO
I Y E L L O W . BROWN
I O 4 -
LOR
25
NOCOLOR Hi
I YELLOW
CH3COO-
! NOCOLOR
( BROWN
NO 2
NOCOLOR
Is
COLOR
11"
I NOCOLOR
19
I YELLOW
S 2 -
COLOR 120
1
NOCOLOR
NO COLOR | 2 3
YELLOW NO3-
( ORANGE
5 0 , ; -
23 I
BLUE—"-GREEN
IO3-
NOCOLOR
1"
1
NOCOLOR
LIGHT YELLOW
NO COLOR PO/ ,3-
h9
NOCOLOR
COLOR BROWN
1" MoO 2- i! 0
LiGH r YELLOW
5 0 2 -
YE I I OW
HCU)
NOCOLOR | , 9
I LIGHT YELLOW
NOCOI.CR ^2^^~
i' VELLOW
c r Scheme 1 Reac t ions in a l e f t - h a n d branch are performed before
those in a r i gh t -hand branch. The reagent numbers re fe r to Table 1.
SAMPLE
NO COLOR
I" RED
S206^
NOCOLOR |19
I I PALE YELLOW NO COLOR
103- 22
COLOR 1
NOCOLOR
h5
ORANGE
soa^" NOCOLOR LIGHT YELLOW
| 2 5 C 2 0 , 2 -
YELLOW • B R O W N
IO4"
Scheme 2
TABLE 2
Quantitative Separation of NO2 from I , SCN~, and Br on 0.17. CUSO,-
Impresnated Silica Gel LayersUsin« Formic Acid:Acetone(l :9) as Mobile Phase
Loading amount of individual Separations anion salt in mixture (Ri - R^)
NaN02
50 pg
0.5 mg
1.0 mg
2.0 mg
50 pg
0.5 mg
1.0 mg
2.0 mg
100 pg
4.0 mg
KI 0.125 mg
0.25 mg
0.5 mg
1.0 mg
1.0 mg
NH^SCN
0.125 mg
0.25 mg
0.5 mg
0.5 mg
KBr
0 .5 mg
1.0 mg
2.0 mg
4.0 mg
0.25 mg
0.5 mg
NO2
NO2
NO2 NO-
NO"
NO2
NO2
NO2
NQ-
NO2
NO2 NO;
N02
N02
N02
N02
NO 2
NO2
NO2
(0.63-0.43)
(0.62-0.42)
(0.75-0.55)
(0.77-0.57)
(0.65-0.39)
(0.65-0.32)
(0.67-0.11)
(0.69-0.56)
(0.65-0.43)
(0.82-0.69)
(0.70-0.50)
(0.60-0.31)
(0.63-0.26)
(0.72-0.51)
(0.82-0.64)
(0.80-0.72)
(0.79-0.62)
(0.74-0.50)
(0.87-0.56)
- I~
- l"
- l"
- l"
- r . - I~
- l'
- SCN" - SCN" - SCN" - SCN' - SCN" - SCN"
- Br"
- Br"
- Br"
- Br"
- Br"
- Br"
(1.0-0.87)
(1.0-0.91)
(1.0-0.85)
(1.0-0.83)
(1.0-0.80)
(1.0-0.78)
(1.0-0.80)
(1.0-0.88)
(1.0-0.79)
(1.0-0.89)
(1.0-0.88)
(1.0-0.79)
(1.0-0.75)
(1.0-0.9)
(1.0-0.91)
(1.0-0.95)
(0.96-0.86)
(1.0-0.85)
(1.0-0.94)
Note: Detection of Br is difficult, requiring about 20 min after
spraying the chromatogram with the reagent.
TABLE 3
Qunntltntlvo Sopnrntlon oC TO3 FronRrO", N0~, T~, Br~, mid .S(;N~ on O.JX
CuSO^-Impregnated Silica Gel Layers Using FArDMSOrAcetono (1:1:8)
Loading amount of individual
anion salt in mixture
Separations
(R L Rj)
KIO - 3 50
0.4
50
0.4
P8
mg
Mg
mg
50 pg
0.4 mg
100 pg
1.0 mg
0.4 mg
KBrO,
0.25 mg
0.5 mg
0,1 mg
NaN02
1.0 mg
2.0 mg '
0.2 mg
KI
1.0 mg
2.0 mg
4.0 mg
0.4 mg
KBr
4.0 mg
7.0 mg
4.0 mg
NH^SCN
IO3
10"
10-
IO3
10-
IO3
I03
I03
I03
I03
I03
I03
I03
(0.15-0.0)
(0.17-0.0)
(0.35-0.0)
(0.25-0.0)-
(0.27-0.0)-
(0.36-0.0)-
(0.22-0.0)
(0.21-0.0)
(0.34-0.0)
(0.35-0.0)
(0.41-0.0)
(0.4-0.0)
(0.4-0.0)
- Br03
- Br03
- Br03
- NO"
- NO2
- NO2
- I"
- I"
- I~
- I"
- Br"
- Br'
- Br"
(0.96-0.77)
(0.98-0.56)
(1.0-0.82)
(0.98-0.67)
(1.0-0.51)
(1.0-0.78)
(1.0-0.89)
(1.0-0.84)
(1... 0-0. 75)
(1.0-0.87)
(1.0-0.69)
(1.0-0.65)
(1.0-0.81)
10 pg IO3 (0.3-0.0) SCN (1.0-0.81)
Note; The synthetic mixture of IO3 with SCN'
in the formation of precipitates.
(concentration 17o) results
10
TABLE 4
Effect of CaCl2, MgCi2 and NaUCO^ on Some Selected Separations
Standard Rp value of Individual Ions are in parenthesis. I07
(0.00), IO3 (0.53), VO3 (0.00), SCN" (0.94), BrOj (0.93) and
NO2 (0.92).
Salts Separations (R, - R p)
CaCl2 IO4 (ND) - IO3 (ND) - SCN~ (1.0-0.89)
IO4 (0.02-0.0) - IO3 (0.67-0.49) - Br03 (1.0-0.82)
IO4 (0.02-0.0) - IO3 (0.73-0.54) - NO2 (1.0-0.88)
VO3 (0.02-0.0) - IO3 (0.65-0.44) - SCN" (1.0-0.88)
MgC]2 10^ (ND) - IO3 (ND) - SCN" (1.0-0.87)
I0~ (0.01-0.0) - IO3 (0.63-0.45) - BrO" (1.0-0.87)
10^ (0.03-0.0) - 10" (0,73-0.60) - NO2 (1.0-0.87)
VO3 (0.03-0.0) - IO3 (0.70-0.53) - SCN~ (1.0-0.87)
NaHC03 lO^(ND) - IO3 (ND) - SCN~ (1.0-0.87)
10^(0.02-0.0) - IO3 (0.65-0.46) - Br03 (1.0-0.84)
10^(0.03-0.0) - IO3 (0.76-0.62) - NO2 (1.0-0.90)
VO^ (0.01-0.0) - IO3 (0.70-0.50) - SCN~ (1.0-0.79)
Note: ND, not detected
11
TABLE 5
Limit of Detection and Dilution Limit of Anions and VO 2^ on
Silica Gel Impregnated with O.IZ CuSO^ with Formic Acid:
Acetone (1:9) Mobile Phase
S] .
No.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
Ions
Br" 3-
4
l"
VO3
NO-
NO"
SCN"
Fe(CN)
Fe(CN)
Cro2-
Cr207"
MoO^"
woj-
4-6 3-6
Salts
KBr
Na2HP0^
Kl
V02S0^
NaV02.Il20
NaNO^
NaN02
NH^SCN
K^Fe(CN)g.
K3Fe(CN)g
K2Cr0^
^2^^207
Na2Mo0^.2H
Na2W0^.2H2
3H2O
2O
0
Limit of detection
LOO.O
10.0
10.0
10.0
1.0
1.0
1.0
1.0
1.0
0.5
0.5
0.5
0.1
0.1
Dilution
limit^
? 1:10 -
3 1:10^
3 1 :10
1. 1:10~
1:10'^
1:10'^
J rio'
4 1:10^
1: 10 "
1:2x10^
1 :2xI0^
1:2x10^
1:10^
1:10^
Dl]ution ]imit
1: Volume of test solution (ml) x 10
Limit of detection ( pg)
12
TABLE 6
TLC Parameters for the Separation of IO4 (Rp=0.01) from 10-
(Rp=0.92) in the Presence of Certain Metal Ions
MetaJ ions
Hg^^
Cd2^
Ni2^
Zn2^
Co2^
Cu2^
Fe^^
Al^^
Rp
0.90
0.87
0.85
0.86
0.87
0.86
0.87
0.87
TLC parame
• '10-
19.0
24.0
15.66
10.11
19.0
13.28
13.28
19.0
ters
380.03
244.89
159.79
194.42
220.93
210.79
210.79
220.93
R s
12.05
6.69
5.66
6.29
6.96
6.37
6.96
6.96
DETECTION, DETERMINATION AND THIN-UYER CHROMATOGRAPHIC SEPARATION
OF ANIONS
THESIS SUBMITTED FOR THE DEGREE OF
Mottox of $l^ila)Biopt)p IN
APPLIED CHEMISTRY
BY UNDER THE SUPERVISION OF SHARAD TIIVARI Dr. Ali Mohammad
Readet
DEPARTMENT OF APPLIED CHEMISTRY ZAKIR HUSAIN COLLEGE OF ENGINEERING AND TECHNOLOGY
ALIGARH MUSLIM UNIVERSITY ALIGARH (INDIA)
1991
'. f
Cfl ^ ^ -2.00^
{j^-
T^IES^^ s^ct\ot^
2 5 SeP 1992
ALI MOHAMMAD Ph.D. (Aligarh)
Editor CHEMICAL AND ENVIRONMENTAL RESEARCH
Phone : Office DEPARTMENT OF APPLIED CHEMISTRY
Z.H. College of Engg, & Technology ALIGARH MUSLIM UNIVERSITY
ALIGARH-202 002 (INDIA) TLX : 564-230 AMU IN
CERTIFICATE
Certified that the work incorporated in this
thesis is the original contribution of the
candidate and is suitable for submission to the
award of Ph.D. degree.
1 . wiJ^^^^--^^ (DR. ALI MOHAMMAD)
Supervisor
ACKNOWLEDGEMENTS
At thi'i crucial juncture when a research fellow has
to acknowledge all those concerned with the thesis, I am
finding it a bit difficult to frame a sentence in honor and
praise of my supervisor, Dr. All Mohammad. His constant
encouragement, constructive criticism, a thorough back
ground of the subject and monumental patience made this
work possible. Dr. Mohammad's contribution to my career
would always be a corner stone of my life.
I place on record my profound gratitude to
Professor S.A.A. Zaidi for his unending help and support. I
express my sense of indebtedness to Professor K.T. Nasira
for his cooperation and moral support. My sincere thanks
are due to Professor Mohammad Ajraal, Chairman, Department
of Applied Chemistry, A.M.U., Aligarh, for providing all
the necessary research facilities.
I wish to express my deep sense of appreciation for
my parents and my aunty Mrs. K.R. Mahajan whose good wishes
and sacred blessings have always been a source of
inspiration in accomplishing this task.
Friends and colleagues alway play a significant
role, but I would like to single out Dr. Nairn Fatima and
Mr. Majid Khan for their invaluable help which they
rendered to me, when I needed it most.
I am thankful to Mr. H.S. Sharma for his neat and tidy
electronic typing of my thesis.
Finally, the financial assistance in the form of
Senior Research Fellowship from the Council of Scientific
and Industrial Research, New Delhi, India, is gratefully
acknowledged.
6f^dX\{X^iiw^ ^i
(SHARAD TIWARI)
it
LIST OF PUBLICATIONS
1. Thin-Layer Chromatographic Separation and Identifi
cation of Some Anions on Copper Sulfate Impregnated
Silica Gel Layers.
Chromatographia, 30, 405-409 (1990) (Germany).
2. Chromatography of Anionic PoHutants on Silica Gel
Layers: Selective Microgram Separation of NO^ and I0„.
Microchemical Journal, 44, 39-48 (1991) (U.S.A).
3. Analysis of Anions by Sol id-State Spot-Tests.
Talanta, 1992 (In press) (U.K.).
4. Identification and Separation of Some Anions on Plain
and Mixed Adsorbent Layers Using Water as Eluent.
Microchemical Journal, 1992 (In press) (U.S.A.).
5. Effect of Heavy Metals on Chromatographic Separation of
10^ from 10 3, BrOj , MoO and Fe(CN)g .
Journal of Planar Chromatography, 1992 (In press)
( Swi t/.cr I and ) .
Dedicated to
my Parents
"Only amateurs consider that an idea must be
brand new in order to be good; important in
reality is not he who first had the idea but
he who expressed it better"
CONTIiNTS
Page
Acknowledgement 1
List of publications ii
Chapter - I
(ICMicral J uL r o t l u c L i o n 1
C h a p t e r - I I
Analysis of Anions by Sol id-State Spot-Tests 92
Chpater - III
Microgram Separation and Semiquantitative DoL cnni na L 1 on oi' AnJinis 125
Chapter - IV
Identification and Separation of Some Anions on Plain and Mixed Adsorbent Layers 149
Chapter - V
Thin-Layer Cliromatographic Separation of Anions on Copper Sulfate Impregnated Silica Gel Layers 167
Chapter - VI
Effect of Heavy Metals on Chromatographic Separation of 10^ and Quantitative Determi-nal 1 on of \in 188
CHAPTER - 1
GENERAL INTRODUCTION
AnaJytical Chemistry, a most useful branch of
modern chemical sciences should be considered as the
'Mother of Chemistry' because the development of
traditional branches of Chemistry (organic, inorganic and
physical) depends solely on principles and new methods of
analysis which is the essence of analytical chemistry.
Analytical research, as opposed to synthetic, .Ushered in
the change from magic and alchemy to quantitative,
scientific chemistry. Analytical work led to formulate the
laws of definite and multiple proportions and made possible
Ualton's great achievement, an atomic hypothesis. The
increasing importance of environmental pollution and an
explosive technological development have combined to create
analytical problems which demand increasing instrumentation
for their solution. The trends of recent years have brought
analytical chemistry into the forefront of research in many
exciting areas. Typical examples of such problems are
purification of the environment, utilization of solar
energy, analysis of ores, recovery of precious metals from
the spent fuel or sea water, detection of unusual molecules
in polluted atmosphere of smog-bound cities, determination
of pesticide residues in food products, identifying traces
of impurities in ultra pure semi-conductor materials,
deducing the sequence of different amino acids in a giant
protein molecule and determination of complex organic
molecules in the nucleus of a single cell.
Analytical chemistry is as old, and as new, as the
science of chemistry itself. It is concerned with the
methods and techniques employed in the chemical analysis oi
substances. A chemical analysis may be either qualitative
or quantitative. Qualitative analysis deals with the
identification of substances and is concerned with what
elements or compounds are present in a sample. The
quantitative analysis is concerned with the determination
of how much of a particular substance is present in a
sample. As an example, if a pollutant in a river has been
killing fish, qualitative analysis could be used to find
out the chemical identity of the pollutant, whether the
pollutant was a heavy metal- (Pb, Cd or Hg) or any other
substance. After establishing the identity of a chemical
species, the concentration of that species in the sample
can be determined by quantitative analysis. Any physical or
chemical property characteristic of a particular element
can be made the basis of a method for its analytical
determination.
f>om a historical standpoint, the majority of early
analytical methods were either gravimetric or volumetric
which are termed as classical or non-instrumental methods
of analysis. Procedures based on the measurement of
optical, electrical, thermal and other properties were
developed later, and are called instrumental or modern
methods. In fact, fundamental differences between the two
categories (classical and instrumental methods) do not
exist, both are based upon the correlation of a physical
measurement with concentration; neither is specific and
separations often precede both types of analysis. Thus the
classification of methods as classical or instrumental is
founded largely on chronological development. The
instrumental methods are faster and generally used where
high selectivities or very low concentrations of analyte
are involved. These methods are expensive and require
special maintenance. On the other hand, non-instrumcnLa 1
methods are simple, cost effective, versatile and suited Lc
on field experimentation. These methods are of greater
importance for the developing countries like ours. It is
therefore, worthwhile to develop and strengthen non-
instrumental methods for chemical analysis.
The qualitative analysis can be conducted either in
solutions or in the solid state, employing optical,
chemical or electroanalytical techniques. Of these the
chemical methods have received wide applicability in the
detection and determination of functional groups and
inorganic ions. Qualitative analysis can be performed
easily by using wet procedures. In most cases the chemical
reagents used for the qualitative analysis either
selectively precipitate one particular substance from a
mixture or selectively react to yield a colored reaction
product.
As a result large number of color reactions have
been developed to achieve improved sensitivity,
selectivity, accuracy, reproducibility, and practical
applicability. Because of the availability of wide range ot
reagents, suitable color reactions can be deviled 't
specific cases.
SPOT-TEST ANALYSIS:
The present work is concerned with the system-itii.
analysis of anions by solid-state spot-test technique and
hence now more emphasis would be laid in the subsequent
pages on spot test methods and their significance m
chemical analysis.
The 'spot-test method' as introduced by Feigl and
Stern[l] for the detection and determination of a substmet
is a micro scale analytical procedure commonly carried out
by placing a drop of the reagent and a drop of the test
solution together on a filter paper, spot plate (a
porcelain plate with many small depressions), watch glass
or in a micro test-tube.Alternatively the test can also be
performed either by spotting the drops so that their
peripheries just meet or by bringing into contact the test
solution with a solid reagent and detecting the resulting
gaseous or colored product. Sometines the test is made bv
triturating powdered solid reactants capable of producing
colored product.
The term 'spot-test analysis' is a generic tern-
referring to sensitive and selective tests based on
chemical reactions where the use of a drop of the test or a
reagent solution is the essential step. Inorganic spot-test
analysis is the outstanding field of application of
specific, selective and sensitive reactions with the goal
of rapidly solving problems in qualitative micro analysis.
The spot reactions can also be advantageously applied to
quantitative determinations since they lead lo the
formation of colored products. The sensitivity of H test
depends upon the conditions under which it is carried out.
The first colorimetric determination using
spot-test method was reported by N.A. Tananaeff [2] in
1929. He compared the intensity of the color reactions
carried out in drops of test and standard solutions on
filter paper. In accordance with their limits of
identification and the corresponding dilution, spot
reactions can only be applied within a particui ir
concentration range of the material to be detected.
Sometimes the filter paper becomes an active participant in
the spot reactions although it does not appear in the
stoichiometric representation [3|.
The elegant variations in spot-tests have been
affected by Fujimoto [4] and Qureshi et al . [5j. These
modifications led to the birth of two new spot-test
techniques known as: (1) Resin Spot Test and (2) Capillary
Solid-state Spot-Test.
(1) Resin Spot Test:
In 1960 Fujimoto [4] used ion exchange resins as
reaction media for micro or ultramicro detection tests
which he called as 'resin spot tests'. In this method ion
exchange resin beads are added to the solution containing
ions or charged complexes to be detected. The ions or
charged complexes are taken up by the resin beads and when
these beads are brought into contact with a selective
reagent, a color reaction takes place on the surface of
beads indicating the presence of a particular species. The
important advantages of resin spot test technique are:
a) The sensitivity of the test is high because the colored
species is concentrated on resin beads.
b) It is more selective because cationic or anionic inter
ferences can be easily avoided simply by using an anion
or a cation exchanger.
c) Stabilization of the unstable colored products in the
exchanger phase [6] and the possibility of preserving
the results by drying the colored resin beads.
d) Use of a simple and inexpensive equipment.
e) No special training is required.
f) Ion exchange resin beads can be easily removed from Che
reaction mixture.
The limitation of resin spot test is that it is
applicable only to the solutions containing ions or char '.ed
species.
Resin spot-test technique was originally applied
for the detection of metal ions. Recently its utility has
been extended for the detection and determination of
organic compounds [7-10],
(2) Capillary Solid-State Spot-Test:
Chemistry of the solid state has been the most
neglected aspect of chemical sciences probably of the
feeling that 'Corpora non agunt nisi fluid' as ennncl-jted
by Aristotle. Solid-state reactions have much to offer to
the chemists concerned with synthesis, analysis, reaction
mechanism or the chemistry of natural processes.
Particularly all reactions in various geological processes
take place in the solid phase. Solid-state reactions have
some novel features which distinguish them from reactions
occuring in the fluid/solution state.
a) Solid-state reactions are free from the complicating
influence of the solvent.
b) Their rates are comparatively slower and hence are more
amenable to kinetic and mechanistic studies.
c) They are useful for the study of weak interactions and
for the discovery of new species [11-13].
d) Reactions in crystals proceed with minimum of atonic
and molecular movement and thus governed by the
structures of the reacting crystals.
e) Chemical reactivity of atoms or molecules in solids
depend both on their nature as well as on their
positions in crystals.
f) Molecules in a crystal occur in only a small number of
confrontations leading to a limited number of intcr-
molecular approaches in the crystalline state.
g) The activity of the reactants and products remain
almost the same during the reaction.
h) Solid-state reactions do not reach equilibrium except
in specific cases and are generally exothermic.
It is now fully established fl4] that reactions which
take place in the solution state also occur in the solid
state particularly if there is a close contact between the
reacting substances. Such reactions are called 'contact
reactions'. For example on contacting sodium metavanadaLe
crystals with crystalline potassium bisulfate, a reddish-
orange color develops at the contacting boundary.
The solid-state reactions may be studied ei-ther by
allowing the reactions to occur between single crystals or
by means o£ capillary technique proposed by R.P. Rastogi
[13]. In this technique powdered reactants are filled in a
capillary as shown in figure 1. The progress of a
solid-state reaction in glass capillary is followed by
monitoring the movement of the boundary of the colored
product.
The salient features of this technique are as
fol1ows:
A 10 cm graduated capillary (3 mm interna]
diameter) is partly filled with powdered reagent from one
end with the help of two iron rods and the material (well
powdered) is similarly filled from the other end. Care is
taken to maintain a reproducible packing and both the
materials should come in close contact with one another in
the middle of the capillary. The color of the product
formed at the junction, direction of movement of the
colored boundary and the length of the product boundary are
recorded at desired temperature after specific time
intervals. The start of the reaction is indicated by a
change in color. This technique is very useful to scan a
large number of reactions quickly. The reproducibility of
results mainly depend upon the uniformity of the particle
"size and the amount of pressure exerted in filling the
capil1ary.
10
Fig. 1 Capillary technique for the study of solid-
state reactions of powders.
R. and R^ are reactants and P is the product
a,b,c and d are solid boundaries
arrow indicates the direction of reaction progress
11
In 1976 Qureshi et al. [5] extended the use of this
technique for the detection of organic substances and
called it as 'capillary solid-state spot-test'. This
technique has some distinct advantages over conventional
spot test and resin spot test methods.
In the conventional spot tests, we notice the color
formed on mixing the reactants, but in this case we observe
color at the junction, the length of the product boundary
and the direction of movement of the boundary. As a re-. IL
two substances giving the same color with a reagent can be
distinguished on the basis of boundary movement, if they
move in opposite directions. Thus, the wide choice of
variables in this technique such as (i) the color (ii) the
length and (iii) the direction of movement of the colored
boundary leads to a selective or even specific detection of
compounds.
The capillary solid-state spot-test technique which
was originally applied for the detection and
semiquantitative determination of organic substances
[15-18] was later on extended for the systematic analysis
of cations [19]. We have further extended the use of this
technique in the systematic analysis of anions and a "lass
wool plug modification has also been proposed tci i^nhance
the selectivity of the test.
12
It may be appropriate at this stage to discuss the
analytical applications of solid state reactions. Only one
review by Voskresenskii [20] has appeared till now. The
various parameters affecting solid-state reactions are
summarized below:
(i) the rate of reaction generally increases with an
increase in the degree of grinding of the
reactants.
(ii) Water of crystallization or atmospheric moisture
has an unpredictable effect on the course of
reaction. Water vapor is always present ir
atmosphere and it can accelerate, retard or even
stop a reaction.
(iii) The rate of reaction generally increases with
temperature.
(iv) Effect of pH is less important in the solid-state
than that of in the solution. For example, a
reaction takes place when any aluminium salt Is
triturated with arsenazo 1 whereas a definite pH is
necessary to carry out this reaction in the
solution state.
The following characteristics of solid-state
analytical reactions have also been noted:
(i) If several ions can react with particular reagent,
13
then the ions having the highest valency react
first.
(ii) If ions of the same valency are present, all or
which react with a particular reagent, then ''^TSL
having the hi'gher atomic number or atomic weight
react first.
(iii) The ability of minerals to react depends on their
chemical structure, while the kinetic behavior
(the rate of reaction) depends on their physical
structure.
(iv) All crystal grains do not have identical therMcai
reactivity.
The use of pure metal salts is very convenient for
demonstrating solid-state qualitative analytical reactions.
Let us now illustrate a few examples of such reactions.
Beryllium may be detected by reactions with
quinalizarin or beryllon 2. A little solid sodium hydroxide
is first added to a berrylium salt followed by trituration,
then the reagent is added and the contents are triturated. A
characteristic blue coloration appears with both the
reagents. Any molybdenum compound when mixed with excess of
ammonium sulfate and heated until the evolution of SO,
ceases. A blue colored solid mass of molybdenurr blue
appears. Similarly, on mixing a tin salt and potassiurr
14
iodide, a golden yellow color rapidly appears.
Metal ions sometimes form complexes of low boiling
point on reacting with inorganic substances and thus can ho
separated easily. For example, beryllium as oxy acet-itc and
tin or nickel as dimethylglyoxime complexes have been
separated. Solid-state analytical reactions can also be
used for solid phase colorimetry both visually m-
instrumental 1y.
It is now apparent from the above discussion that
field of solid-state analytical reactions is wide open tu
accelerated research activities for qualitative testing or
minerals, alloys, mineral fertilizers and organic
functional groups. Feigl [21j has shown the existenc ot
new possibilities by using solid-state reactions iri
qualitative organic analysis. The on field application of
solid-state analytical reactions is of special importance
for testing geological samples. As yet only the reactions
which lead to the formation of colored reaction product-
have been found suitable for solid-state analytical
reactions but it may soon be possible to use reactions,
involving the formation of white products with the aid of
luminescence methods of analysis.
The following reaction steps may be assumed in
order to understand the mechanism of solid-state reactions
of inorganic substances.
15
The exchange of particles at the interface between
the two reactants and the formation of the reaction
product for ideal contact between the solids. Iherc
are three possible transport mechanisms after Lhi-
formation of a homogeneous, pore free product layer
as shown in figure 2.
Transport of the particles through the intG-''"'c
I. between the reactant and the reaction prod'u t .
Diffusion of anions and cations of the reactant MO
through the reaction product via volume diffusioii
or grain boundaries and dislocation of crystallite
of the product.
Reaction of the cations and anions of the subst m C(
MO at interface I^ with the reactant A^O^ to for'
the reaction product. The formation of renctio-
product is progressed via heterogeneous nucleatio
followed by crystal growth.
Almost similar reaction steps are followed b\
organic reactions. The only difference is that in organic
reactions the diffusing species in most cases are molecule^
or free radicals instead of ions.
Separation is of utmost importance because in "'an\
cases detection and determination depend on the separation.
Among the most versatile analytical separation techniquos.
16
Orrt^
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en
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2
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O n
CS)
o 2
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4-) O cd
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4-J •H
B if>
•H C ex)
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4-1
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•
17
ion exchange, electrophoresis, and chromatography are of
wider applicabiJity. ion-exchange processes are mostJy used
in nuclear engineerings, such as purification of fuels,
waste disposal enrichment and purification of useful
radioactive isotopes. It is because of selectivity and the
completeness of the separation.
i) Ion ICxchange:
Ion exchange is a process in which reversible
stoichLoincL ric interchange of ions of the same sign take
place between an electrolyte solution (mobile phase) or
molten salt and a solid phase (stationery phase). The
selectivity of an exchanger depends upon the nature of the
ion exchanger and the composition of the liquid phase,
which is in contact with it. it is, therefore, possible to
increase the separation potential of the exchange process
by pro[)er selection of exchanger and cluent. The exchanger
phase may be inorganic or organic in nature. The use of
solid absorbing substances to improve water quality has
been recorded since ancient times. Although most
applications involved in the removal of solid impurities
through filtration, ion exchange was also inadvertently
employed in the exchange of dissolved salts between the
water and the solid material. Earliest of the references
were found in Holy Bible which establishes Moses priority
who succeeded in preparing drinking water from brackish
18
water by ion exchange meLhod. Francis Bacon described a
method for removing salt from sea water and Hales
rccoiiiiiicMulcd LhaL sen waler \)o desalinated by filtration
through stoneware. The use of natural and artificial
aluminosL1icates to purify beet syrup was reported by harm
(i896) and Rumpler (1903). A singnifleant development took
place with the discovery of Adams and Holms [22] regarding
the use of some synthetic high molecular weight organic
polymers bearing ionic functional groups as ion exchangers.
However, organic ion exchangers have two basic drawbacks
(1) low resistance to heat and radiation and (11) their
composition cannot be varied with ease. As a result
emphasis was shifted to the synthesis of inorganic ion
exchangers [23,24] many of which exhibited expected
chemical stability and proved highly selective for certain
ions. Ion-exchange process is well suited for the
sc[)aratioii of inorganic ions (cation and anions) because
the separation is based on the exchange of Ions in
stationary phase, as shown below:
X ' Y — ^ Y I X
The barred symlx^ls denote the ion exchange phase.
An eciu i 1 ibr J uiii is eventually set up in which some of the
ions initially present in the exchanger phase have been
replaced by Y ions from the solution. Separation by ion
exchange combined with spectrophotometry can be applied for
L9
the rapid and LoLaJ analysis of numerous mixed
pharmacGUticaJ products. For example, Dowex-IXI (an anion
exchanger) can be used for the separation of morphine and
codeine [ 25 J ,
11) I'J ecLrophoresls:
I'J ectrophoresis is another separation technique
which can be defined as the migration of particles through
a solution inider the influence of an electric field. The
term 'electrophoresis' is presently applied both to the
111 i)', ra H on of i lul i v i dun 1 ions as well ns to colloidal
aggregates. This technique provides a powerful means of
fractionating the components of a mixture. Separation and
identification of micro amoiuits of high molecular weight
substances such as proteins which are often difficult to
separate by chromatography alone, are well separated and
identified by electrophoresis. Depending upon the
properLics of the medium, the separations may result
primarily from the electrophorotic effect or from a
combination of electrophoresis and adsorption, ion exchange
or other distribution ecjuilibria. Methods based upon
electrophoresis in a stabilizing medium bear a variety of
names, including el ectrochromatography, zone
electrophoresis, electromigration, and ionophoresis.
}J cctrochromatographic methods are indispensable to
the clinical chemists and the biochemists, who use them for
20
the f racLionaL iiip, oC an aiiia/.iug number oC biological
materials, e.g. cJinical diagnosis for the separation of
proteins and other large molecules present in serum, urine,
spinal fluid, gastric juices, and other body fluids. This
technique also provides a convenient means for the
separation of inorganic ions.
iii) Chromatography:
JL is said that when one of the greatest dis
coveries in the chromatographic science was, submitted for
pulil i ca L i on, Llic joiuiral of a renowned chemical society
rejected it. The importance of the work was eventually
emphasized by a Nobel Prize, in fact, such instances are
n(>( iiMcoiiiiiioM In the hl.'dory of HCICMIIM'IC soclolv
l)ub I i ca I i ons . I he paper on ' br ass Lno I Lde ' was rejected by
the journals of learned societies, the impact of which was
realized after its publication in 'Nature' and the journals
of those societies flashed news stories.
Ihe origin of the chromatography go back to Runge's
experimenL on capillary analysis. Davy observed changes in
the composition of crude petroleum when it came in contact
with rocks displaying adsorptive activity. These reports
can be considered as [>art of the development of
chromatography, it was only about 95 years ago that a
Russian botanist Michael Tswett [)ubl ished two papers
[26,27] in 1906, on the separation of plant pigments
21
achievGcJ by percolating Lhe peUroleum ether extract of
green leaves through a glass column packed with fine grains
of calcium carbonate. The separation results into a series
of g,recn and yellow bands and hence the term
'chromatography', chroma (color) + graphy (writing) was
coined by him. Despite this early description, the
importance of Tswett's work was not realized until the
beginning of the 1930s when Kuhn et al . [28,29] applied
chromatographic principles to the separation of natural
substances. Therefore, the birth of column liquid
chromal (\o raphy is ascribed to the work of Tswett.
Another milestone in the development of
chroiiiaLography was reached in 1941 when Martin and Synge
I 30, 31) it'porLcd their discovery of 1 i(juid-l iquid partition
chromatograj^hy. They used one liquid as a sorbent and
auollu'i- li(nii(l was allowed lo pc> rco I a I e L h roug.h lhe foriiior,
thus making, the tochni(|uo a chromatographic process. Their
work set a precedent for the development of other forms of
chromatography.
Mic cii rono 1 ()g, i c a 1 dcwo 1 opiuent in scjiaratlou
tcchnjciucs alter 'I'swctt's discovery of chromatography,
basetl firsL on adsorption and then partition phenomena are
presented in Table I.
Chromatography is the general name given to the
methods by which two or more compounds in a mixture
22
TABLE 1
Chroiiol ()/»] en I Dcvol ()[)nicnl in ChromnLo/;r.-iphic Separation Technic|UGS
Authors Year Separation system
1 . Ma r L i n / i iu l S y i i j ^ c
2. Consdon, Gordan and Martin
3. Craig
4. Mayer and Thompkins
5. Samuel son
6. Haugaard and Kroner
7. Izmailov and Schraiber
8. Kirchnor, MlMcr and Ket tor
9. Barrer
10 . Clacsson
11. James and Martin
1 2 . J nines <-ind M;i r l 1 n
1 3 . J a m e s and M a r t i n
1 4 . S m a l I , S t e v e n s and B.-111111 a n
1941 Partition chromatography
1944 Paper chromatography (PC)
1944 Counter current distribution (CCD)
1947 Ion-exchange chromatography (lEC), adsorption
1963 Il'C (partition)
1948 I'J ectrophoresis
1938 Thin-layer chromatography (TLC), adsorption
1951 TI.C (partition)
1945
1946
1952
19 52
19 74
1975
Gel permeation chromatography (GPC)
Gas chromatography (GO
Gas-liquid chromatography (GLC)
ll[;',h pc r foriiiance llcjuid chromatography (HPLC)
Hi gh-performance thin-1ayer chromatography (IIP ThC )
Ion chromatography
23
ptiysically separated themselves by dlstributinp, themselves
between two phases (i) a stationary phase, which can be a
solid or a liquid supported on a solid and (ii) a mobile
phase, either a gas or a liquid, which flows continuously
over the stationary phase. The separation of individual
components results primarily from differences in their
affinity for the stationary phase. There have been many
definitions of chromatography formulated according to
various classification aspects but to propose a good
definition of chromatography is difficult. It is a
collective term applied to methods which appears diverse in
some regards but share certain common features. Keulemaii's
definition serves as well as any: 'Chromatography is a
physical method of separation, in which the components to
be separated are distributed between two phases, one of
these phases constituting a stationary bed of large surface
area, the other being a fluid that percolates through or
along the stationary bed'. The stationary phase may be
cither a solid or a licjuid, and the moving phase (i.e.
mobile i)hase) may be either a 1 iciuid or a gas.
CLASSIFICATION OF CHROMATOGRAPHIC SYSTEMS:
According Lo the [)hysical arrangement chromato
graphic systems can be divided into planar or column
depending on the geometry of the column support, the
24
columnar systems can be divided as shown in Table 2. The
planar arrangement are represented by paper and thin-layer
chromatography. According to development procedures the
planar systems can be further classified" as ascendent,
horizontal, descendent and occasionally, centrifugal.
Furthermore the development is termed as isocratic if the
composition of the mobile phase remains unchanged during
the development. On the other hand, when the composition of
the mobile phase varies, it is called gradient development.
The chromatographic systems can be classified according to:
1. The state of aggregation of the phases.
2. The physical arrangement of the phases and
3. The mechanism underlying the distribution
equilibrium.
The four possible chromatographic systems derived
from solid, liquid and gaseous phases are: (a) liquid-
liquid, (b) 1 icjuid-sol id, (c) gas-liquid, and (d)
gas-solid. Of these, liquid-liquid and liquid-solid systems
constitute 'liquid chromatography'. A summary of typical
chromatographic systems according to this classification is
given in Tab!e 3.
The overall process of chromatography is a
differential migration phenomenon. The separation of the
components of mixture depends upon their differential
25
TABU' 2
Chromatographic Systems Based on the Geometry of the
Chromatographic Column
Columna r PIanar
Packed coJuiniis
Capi]J ary co]umns
Liquid-] i<iuicl columns
Paper chromatography (PC)
Thin-]ayer chromatography (TLC)
TABLE 3
Chromatographic Systems Classified According to the State of
Aggregation of the Phases
Stationary Phase Mobile Phases
Liquid Gas
Solid
Sol id + Liquid
Liquid
LSC
LSLC
LLC
CSC
GSLC
GLC
L: Liquid S: Solid G: Gas and C: Chromatography
26
pencLration into t;he porous sorbenL. This migration is
produced by a non-selective driving force, the flow of the
wash licjuid. The differential migration results from a
selective resistive action, namely, the selective sorption
of the components of the mixture [32].
Analogous differential migration from a narrow
initial zone of mixture forms the basis of several related
separatory methods. With suitable combinations of driving
force and resistive action, either one or both of which
must be selective, effective separations have been made
under a variety of conditions [32-39].
In column chromatography the separation may proceed
isocratical1y or with a programmed gradient of composition
of the mobile phase, isothermally or with programmed
changes of column temperature, and isobarically or with
programmed changes of mobile phase pressure at the column
inlet. in planar chromatographic systems the solute
compounds are usually not eluted from the chromatographic
bed but rather detected directly in it.
LIQUID CIIROMATOGKAPHIC TECHNIQUES:
It is clear from the above discussion that several
types of licjuid chromatographic techniques have been
developed. Ihe more important liquid chromatographic
techniciues have been illustrated in Fig. 3 . The common
27
1/1 LLI
3
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3 a
cc < 2
Q: UJ >-
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28
liquid coluiiiii chroma togrnphic techniques arc being
described in the following paragraphs.
Adsorption:
In adsorption chromatography the retention of the
solute is a consequence of the interaction with the surface
of the solid adsorbent. The adsorbent surface has a rigid
structure making this type of chromatography useful for
separations of geometric and structural isomers with
molecular weights up to about 1000.
Partition:
Licjuid-l iquid partition chromatography was first
described by Martin and Synge [30,31] in 1941. The
distribution of solutes takes place between two immiscible
solvents. In normal phase (straight phase) chromatography
the more polar liquid often water rich is the stationary
phase, whereas the opposite is true in reversed phase
partition. The stationary phase may be situated on a
variety o^ supports depending on the polarity of the
stationary phase. Partition chromatography is used for
separation of solutes with molecular weights up to a few
thousands, and is a powerful tool in the separation of
scries of homologs.
29
Bonded Phases:
Most applications of liquid column chromatography
are now made on silica which has been chemically modified
(bonded phase chromatography), the modification is made by
chemical reaction between the silanol groups and a
chlorosilane compound. The carbon radicals of the
chlorosilane compound determines the nature of the final
column material. Using silanes containing alkyl carbon
chains with 8-22 carbon atoms gives the particle
hydrophobic surfaces, but more polar surfaces may be
obtained by incorporation of alcohol, amino, cyano and
other groups in the alkyl chain.
The column materials bearing bonded alkyl cliains
are used for reversed phase chromatography, while some of
the more polar, chemically bonded phases may be used in the
straight phase mode as well as in the reversed phase mode,
giving more possibilities for selection of the appropriate
chromatographic system.
Ion Exchange:
'Hie stationary pliase in ion exchange chromatography
is made of a porous polymer to which anionic or cat ionic
exchange groups have been attached. The retention and
separation of solutes are performed according to the degree
of ionization of the solute and its affinity to the ionic
30
sites on the stationary phase. The eluent is usually an
aqueous buffer and the retention may be controlled by
changes in ionic-strength.
Size Exclusion:
In size exclusion chromatography the solid support
is a porous polymer with a controlled pore size, and the
solute molecules are separated according to their size in
solution. The large molecules are excluded and they have
the shortest retention time. The size exclusion may be
performed in aqueous systems (gel filtration), where water
soluble macromolecules can be separated or in non-aqueous
sysLoms (',e 1 permeallon). liy calibration the method can
also be used for determination of molecular weight or
molecular weight distribution.
Affinity:
In order to achieve a high degree of selectivity
special groups with a high affinity to solute or a group of
solutes may be attached to a solid matrix. The ionic
exchange groups in ion exchange chromatography are the most
well known example of this, but many column materials even
more selective have been developed (e.g. immobilized
enzymes). The field of bio-affinity chromatography is
expanding rapidly.
31
Most of the initial developments in chromatography
were for the separation of organic compounds. The beginning
of inorganic chromatography can be attributed to the work
of Runge (1850) on PC; Beyerinck (1889) on thin layer of
gelatin and Schwab (1937) on alumina column.
Since most of the work carried out by us is based
on thin-layer chromatography (TLC), it is justified to
discuss the salient features of TLC in detail. The
following paragraphs will present an overview of all
important aspects of this widely popular and versatile
separation technique.
THIN-LAYER CHROMATOGRAPHY:
Thin-layer chromatography (TLC) together with paper
chromatography comprises 'Planar' or 'flat bed' chromato
graphy. IL is a rapid, inexpensive and highly effective
analytical technique applicable for the analysis of a great
variety of multicomponent mixtures. The stationary phase in
TLC is an active solid termed as the sorbent whereas a
liquid containing a single solvent or a mixture of solvents
is used as mobile phase. A suitable closed vessel
contaLiiiiig iiiobUe jihase and a [ilaLe (gjass or plasLic)
coated with a suitable sorbent (silica, cellulose, alumina,
polyamidc or ion exchanger) are all that required to carry
out qualitative and semiquantitative separations. Ihe
32
mobile phase (solvent;) is usually allowed to migrate up the
plate 10 to 8 cm from the starting line on a TLC plate. The
conventional one-dimensional ascending technique is usually
used for the development of chromatographs. Multiple, two
dimensional, centrifugal and gradient devel oi)ment
techniques have also been used.
Basic TLC is carried out as follows. A drop volume
(0.5-10 pi ) of a sample mixture is spotted on a TLC plate
at about 2 cm from the lower edge of the layer. The spot is
completely dried at room temperature or at an elevated
temperature and the plate is developed with a suitable
mobile phase inside a closed chamber. The components of the
mixture migrate at different rates during the migration of
mobile pliaso Lhrough the stationary phase. After the
devel o[)ment is over, the stationary phase is removed, the
plates are dried and the zones arc detected using suitable
detection reagent. Differential migration results because
of varying degrees of affinity of the mixture components
for the stationary and mobile phase.
Compound identification in TLC is based on Rp, value
which is a measure of the ratio of the distance traveled by
the solvent from the starting line to the distance traveled
by the solute i.e.
distance moved by the solute
^ distance moved by mobile phase front
33
The R,, values are generally noL exactly
reproducible. The contributing factors for this are:
Chamber dimensions, purity and flow direction of mobile
phase, size and nature of layer, humidity, equilibration
conditions, temperature and sample preparation methods.
Further characterization of separated substances can be
achieved by scraping the layer and elution of the analyte
follov 7cd by spectroscopic methods.
History of TLC:
The History of TLC is marked by three dates.
In 1938, Izmailov and Schraiber [40] separated
certain medicinal compounds on binder free
horizontal thin layer of alumina spread on glass
plates. Since the solvent was applied as drops on
the glass plates, containing sample and sorbent,
their method was called 'drop chromatography'.
In 1949 Meinhard and Hall [41] demonstrated that
powdered adsorbent, fixed to a microscope slide by
moans of a suitable binder, [provides a system for
microchromatography called 'surface chromatography'
I'hey separated Fe from Zn on microscope slides
coated with a mixture of alumina and starch
(binder).
34
3. About 1958, Stahl [42,43] introduced the term
'thin-layer chromatography' and standardized
procedures, materials and nomenclature.
Kirchner [44], Heftmann [45], Stahl [46] and Pelick
[47] have nicely reviewed the history of TLC. After the
pioneering work of J. Kirchner [48] and E. Stahl , TLC
became important for the separation of samples not
amenable to analysis by GC. The rapid growth of TLC was
slowed down during the 1970s with the corresponding rise in
popularity of HPLC. The capacity factors in HPLC are more
reproducible than R , values in TLC. However, recent
improvements in TLC have removed many of its limitations.
As a result of the recent improvements in TLC
several new techniques such as high-[)erf ormance (HP) TLC,
over pressurized (OP) TLC, centrifugal layer chromatography
(CLC) and reversed phase (RP) TLC came in light. The
quantification by densitometric scanning have also improved
the efficiency of classical TLC.
lil'TLC layers are smaller, thinner, contain sorbent
of more uniform particle size and are developed for a
shorter distance. All these factors lead to faster
separations, reduced zone diffusion, lower detection
limits, less solvent consumption and better separation
efficiency. Figure 4 shows the practical advantages of
35
Separa t i on d i s t a n c e ( so lvent m ig ra t i on )
100 mm
5 0 mm
30 m i n ^ Runn ing time
F i g . 4 C a i ) i J ] a r y Clow d iag ram
36
HPTLC over conventional TLC.
OPTLC was introduced by Hungarian scientists ,in
1970s. In OPTLC,the vapor phase has been eliminated and the
sorbent layer is completely covered with an elastic
membrane under external pressure. The mobile phase migrates
through thin layer due to the 'cushion system' at over
pressure. Thus, OPTLC combines advantages of the continuous
development technique and elimination of free space in the
chromatographic chamber.
In CLC, the eluent flow is induced by centrifugal
force. The sam])le is applied near the center oC a rotating
disk covered with adsorption material. Concentric zones of
substance migrate towards the outside of the plate during
elution. The circles elute sequentially from the disk and
can be recovered separately. Figure 5 illustrates a
comparison between efficiences of fine and coarse particle
layers as a function of migration distance and development
technique. The detailed comparisons of TLC, HPTLC, and CLC
have been well documented in recent literature [49-52].
Advantages of TLC:
TLC is the most versatile and flexible chromato
graphic method. IL is rapid because precoatcd layers are
available to be used as received, without preparation. It
has highest sample throughput because upto 30 individual
37
E
70
60
50H
01
•^ 40
-.i 3 0
en f<
^ 20 > <
10
-L 2
±
H P T L C Plate
f o r c e d 1^°^
HPTLC Plate
Forced f low development
.L
>• Convent ional TLC Pla te Norma l development
4 6 8 10 12
M i y r a t i o n d i s t ance ( c m )
U 16
Fig. 5 Comparison between efficiences of HPTLC and 'I LC 1 ayers
38
samples and standards can bo apjilied to a single plaLc and
separated at the same time. The automated sample
applicators and developers allow high accuracy and
precision in quantification. There is a wide choice of
layers, developers and detection methods. The wide choice
of detection reagents leads to unsurpassed specificity.
Less pure samples can be applied as the layers are normally
not reused. Being an 'off line' method, different steps of
the procedure are carried out independently.
Chromatographic Systems:
The optimum conditions for separation in TLC are
yielded through mutual harmonization of the stationary and
mobile phases. The following separation mechanisms are
expected to operate, depending upon the nature of analyte,
sorbent layer and the type of mobile phase.
(1) Adsorption (physical sorption of solutes from solution
onto the active surface groups of the sorbent), (2)
Partition (dissolution of solutes into a stationary liquid
held on the layer), (3) Ion exchange (attraction of ions
to sites of opposite charge on the layer) and (4) Size-
exclusion or gel permeation (retention or rejection of
solutes on the basis of their size and/or shape).
Adsorption TLC is wel1 suited to the separation of
structural isomers whereas partion TLC is useful in the
39
separaLion of homologs.
As we have used TLC for the analysis of inorganic
ions, LL is therefore fruitful to say a few words about the
chromatographic systems used for TLC of inorganics in
recent past. The following paragraphs are devoted to bring
out the developments which took place in the last ten years
in this regard.
Stationary Phase (Layer Sorbents):
A large number of sorbents are available whicli can
be used in '1LC, but the need for a perfect sorbent has been
always felt. In the absence of an ideal sorbent the searcli
for a stable, inexpensive, reproducible and readily
avail al)lc sorbent [phases continue. Among the sorbent phases
used, silica gel has been the most favored layer material.
Silica gel, a sorbent of the widest range for TLC
applications, is an amorphous and porous adsorbent referred
to as silica, silicic acid, or porous glass. At the surface
of silica gel the free valencies of the oxygen are
connected either with hydrogen (Si-OH, silanol groups) or
with another silicon atom (Si-O-Si, siloxanc groups) as
shown i n 1igurc 6 .
The silanol groups represent adsorption active
surface centers that are able to interact with sample
40
Fig. 6 Chemical structure of silica gel
41
molecules. The ability of the silanol groups to react
chemically with appropriate reagents is used for controlled
surface modifications. Therefore, silica gels are most
suitable as stationary phases in chromatography.
The various types of sorbent layers used may be
classified as follows:
(I) Unmodified or Untreated Sorbents:
Silica gels, aluminas, inert silicon dioxides
(silica 50,000 and kieselguhrs), cellulose, polyamides
(polymide 6 and i^olyamide II) and scphadex (cross linked
polymeric dcxtran gels ). Kicsclguhr matrix consists of
Si02, AI2O., MgO, Na20, K2O, CaO, Ti02 etc.
(II) Bonded by Chemically Modified Sorbents:
In recent years the importance of using surface-
modified sorbents in ILC has increased. Both hydropliobic
and hydrophilic modified sorbent phases have been used.
(a) Hydrophobic Modified Phases (RP phases):
Ihe non-modified sorbents show polar surface
characteristics, therefore they are not of much practical
utility for ch rom/i Log raph i c separations of solutes having
identical polar characteristics. This problem has been
42
solved using hydrophobic interactions of the stationary
phase with compounds o£ appropriate molecular weight. The
most popular such organo lunctional groups are methyl
(RP-2), Octy] (RP-8), dodecyl (RP-12), Octadecyl (RP-18)
and IMuMiyl residues.
(b) Hydrophilic Modified Sorbents:
Hydrophilic modified sorbents possess amino-,
cyano- and diol residues as a functional group. The polar
functional groups, in each case, are bonded via short-chain
non-[:)olar spacers to the silica matrix.
(Ill) Impregnated Sorbents:
Besides the possibility of changing the
selectivity of sorbent by chemical modification,
iiiiproveniont in selectivity can also be achieved by
impregnating the matrix with suitable organic or inorganic
substances (physisorption).
(a) Organic Imprcgnants:
Silica gel lias been impregnated with diethyl ene-
trianiine, sul f aguanidine , 8-hydroxyquinol ine and
t-buty]amine, 2 , 2-dipyridal , iminodiacetic acid, tributyl-
aminc, ED I'A, pyridinium tung stoarsenate, p-toluidine etc.
MicroLrysta 1]ine cellulose impregnated with chitosan
formate, bis-(2-ethy1hexy1 ) orthophosphoric acid, trioctyl
phosphine oxido-bis-(2-ethy1hoxyl) orthophosphoric acid and
43
dibuty] butyl phosphonate.
(b) Inorganic Impregnants:
Ceric molybdate, sodium molybdate, NH, CI , Ba(NO-,)^,
NaNOr,, NaNO^, potassium ortho dihydrogen phosphate and
CuSO, have been used as the impregnants for silica gel.
(IV) Miscellaneous Sorbents:
In this category one can report numerous types of
sorbent phases, that have been used in TLC. Some of such
sc)rbci\lj; are suiiima r I/.ecl below:
Silica gel II slurried in 47„ ammonium nitrate solution
containing VL sodium carboxy methyl cellulose (CMC), silica
gel G-starch, Silica gel G-Ceric molybdate, silica gel R-
vionite CS ion exchanger, silica gel G- Na carboxy methyl
cellulose, kaolin, chitosan, kieselgel G -chitosan,
microcrystal 1 ine cellulose mixed with powdered chitosan,
diethyl aiiiinoethyl (DEAE) - cellulose layers in H form,
cellulose phosphate in thiocyanate form, p-cellulose +
inicroc ry sL a 11 inc cellulose (2:1) in free hydrogen form,
cellulose phosphate • microcrystal1ine cellulose (3:1),
cellulose (chemapol) with azopyrocatechol group, alumina
with plaster of paris binder, staimic arsenate, stannic
antimonaLc, hydrated sLainiic oxide, /Irconluiii tnngsLaLe In
44
H foi"m, P-stannic arsenate in H form, Ti(IV) antimonate
in H form, styragel R 60 A polystyrene dVB copolymer,
Dowcx 50 WX8 + silica gel (1:1) and Amberlite IRA-400 +
slllea gel (1:1).
Both commercially available (precoated) layers as
well as home made sorbent layers have been used.
Mobile Phases:
Separation of ions by TLC is governed by the
physical interactions of the adsorbent and the coordinative
properties of the mobile phase. The composition of a mobile
phase is usually altered in order to achieve a desired
separation with improved selectivity, resolution -and
clarity.
Mobile phases are most often selected by consulting
the pertinent literature to find suitable solvent for the
separation of interest. Ihis is followed by a trial-and-
crror approach to modify the mobile phase for the
particular layer and other local conditions being used, if
necessary. Based on solvent strength and selectivity
parameters systematic approaches to mobile phase selection
and optimization have been developed. A praiseworthy work
in this direction has been done by 3nyder [53] and Kirklaiid
[54]. In general, solvent systems used for TfC of
45
inorgiinics arc (a) mixture of organic solvcnL with some
acids or a buffer (b) acjueous solution of mono or polybasic
acids or their alkali metal salts and (c) various organic
solvents ranging from low to high boiling points. An
important advantages of TLC with volatile mobile phases
such as acetone, methanol or benzene lies in the fact that
they quickly evaporate from the sorbent layer, after
development, but reproducibility in such cases suffers due
to the presence of mobile phase components in the vapor
phase over the surface. Conversely, TLC with mobile phases
of lower volaLiliLy g,ives better reproducibility, but the
continuous slow advancing of the mobile phase after the
withdrawal of the plate from the chamber may lead to an
additional zone broadening. With different sorbent phases
the organic solvents such as acetyl acetone,
trif1uoroacetyl acetone, monotetradecyl phosphate, tributyl
phospliatc, tctrahydrof uran (TllF), dimethyl sul f oxide ( DMSO ) ,
dimethylformamide (DMF) , and 2-ethyl hexyl phosphate in
combination with other solvents have proved very useful for
the separation of inorg,anic ions. '1 he mobile phases used
durin*', last decade may be categorized into fol it)wing
groups:
1. Inorganic Solvents: (a) acids, (b) bases, (c) salt solu
tions, (d) mixture of acids and bases and their salts.
46
2. Organic Solvents: (a) acids, (b) bases, (c) alcohols,
(d) aldehydes and ketones, (e) esters, (f) mixture of the
above .
3. Mixed Solvents: (a) organic solvents mixed with mineral
acids (b) organic solvents mixed with inorganic bases (c)
organic solvent mixed with water (d) organic solvents mixed
with salt solutions.
4. Complex-forming Organic Solvents
Sample Preparation:
Cations are generally dissolved in water
maintaining a concentration of nearly O.IM. In some cases,
the corresponding acid is added to prevent hydrolysis. Rare
earth solutions are prepared by dissolving their nitrates
in O.IM HNO^ or by fusion followed by dissolution in dilute
HCl or HNOo. Anions are usually taken as their water
soluble sodium, potassium or ammonium salts. Methanol and
ethanol are used as solvents for preparing the sample
solutions of organometal1ics .
Detection and identification:
The detection methods used for inorganic ions fall
into three riajcr categories: (a) Chemical, (b) Physical,
(c) Kni'ymatic or biol ogical.The chromatopl ates are air. dried
prior CO tne deteccioii of ions.
47
Chemical tiicChods of detection involve the spraying
of chromaLoplates with a suitable reagent, which forms
colored compounds with the separated species. Reagents
giving clear and sufficiently sensitive color reactions
with several ions are preferred. Both selective and non
selective reagents may be chosen for detection purposes.
Among the physical methods, visualization in ultraviolet
(UV) light is most common. This method is highly sensitive,
non destructive, and a\ .lable to the visualization of sptits
before undertaking quantitative studies. Enzymatic
detection iiietliods are also quite simple and selective.
For the detection of inorganic ions standard sjjot
test reagents (general as well as specific) have been used
by most of the workers. The reagents used most extensively
are; alizarin Red S, benzidine, dithizone, diphenyl-
carbazide, 8-hydroxyquinoline, Rhodamine-B, potassium
1 or roc vanide, y(Ml(.)w ammonium sulfide, chromotropic acid,
alkaline ;.Uyoxal di thiosemica rbazone , and rubeanic acid for
cations- arsenazo III, chl orophosphonazo-m-NOg,, alizarin,
and t ribroinochl oroph(> -ihonazo for rare earth elements; and
ninhydrin, diphenylamine, alizarin, silver nitrate,
F8CI3 , pyrogallol and 2,6-dichlorophenolindophenol for
anions. Y -specLroscopy or autoradiography [55j for the
detection of rare earths appearing as fission products in a
freshly irradiated fuel. X-ray fluorescence microanalysis
48
with a scannidj:.; collimated primary X-ray beam [56] for
metal ion detection, and Rhodamine-B £or the detection of
silicon in edible oils [57] have also been used. Crystal
violet solutions of standard acidity have been employed for
the detection of phosphoric acid derivatives [58]. Nanda
and Devi have reported an enzymatic method [59] for the
detection of heavy metal compounds in fresh water.
In some cases the detection of certain inorganic
ions has been carried out according to the color reaction
appearing in the sorption zone [60-62] of the element on
the plate during the chromatographic run. Selenium in food
samples has been identified as 2,3-diaminonaphthalene Se
complex, v/hich upon exposure to U.V. light (360 nm) gives
pink fluorescence on a TLC plate [63]. An indirect
fluorimetric niethod for the detection of non - fluorescing
anions has recently been reported [64]. Fluorescent morin-
aluminium complex as a detection reagent for various anions
has been reported [65] by T. Okumura. The Rp values of the
detected zones are used to identify the various ions
present in the sample.
Quantitation:
In recent years quantitative TLC has taken the
world by storm due to the development of ne\^'
instrumental techniques as a result of which a TLC for
49
quantitative analysis has surged to dramatic heights, and
has gathered momentum. The three main approaches associated
with such analysis are: Visual estimation, zone elution
and scanniiig densitometry.
Visual Estimation:
The simplest for semiquantitative analysis by TLC
is to develop a definite sample aliquot alongside standards
containing known weights of analyte. After detection, the
weight of analyte in the sample is estimated by visual
comparison of the size and intensity of the standards and
sample zones. This method has accuracy and reproducibility
in the range of 10-307o which is adequate for the purpose
intended. Visual comparison works well if amounts close to
the detection limit are applied on the chromatoplates and
the sample is accurately bracketed with standards.
In an attempt to standardize the quantification in
TLC, Moha mmad and Fatima [66,67], Mohammad and Tiwari [68],
Nanda and Devi [69] and Mlodzikowski [70] h;r'e established
a linear relationship between the spot size and the amount
of solute.
Zone Elution:
The zone elution method involves:
a) Drying the layer
50
b) Locating the separated analyte zones
c) Scraping the portion of layer containing the
anaJyte from the sorbent and
d) Measurement against standards by an independent
microanalyticaJ method such as solution
spectrometry, gas chromatography or voltametry.
This quantification method is tedious and tine
consuming and seems inaccurate because of difficulties in
locating the exact z . boundaries loss of sorbent during
scrapping and collection, non-reproducible elution from the
sorbent and background interferences due to oluted
impurities from the sorbent. These errors can be minimized
if standards and samples are chromatographed, scrapped and
eluted with full consistency, and an equal size blank area
of layer is scrapped and eluted in an identical fashion.
Scanning Densitometry:
In situ measurements of zones wil , a scanning
densitometer is the preferred technique for quantitative
TLC. Substances separated by I'LC or HPTLC are qualified bv
in situ measurement of absorbed visible or U.V. light or
emitted fluorescence upon excitation with U.V. light.
Absorption of U.V. light is measured either on regular
layers or on layers with incorporated phosphor.
51
A double bed densitometer equipped with a TLC
scanner, an integrator, and a microcomputer have been used
for the simultaneous determination of light rare earth in
monazite sand, CAMAG turner fluorometric scanner for the
estimation of cadmium ion [71], Aminco SPF 125 for spectro-
fluoronietric determination of selemium in food [63], KM-3
densitometer [72] (Zeiss) for HPTLC determination of Se in
biological matrices, ERI-10 densitometer (Carl Zeiss, Jena,
4-GDR) for the determination of NOo and Fe(CN)^ in molasses,
and other anions that produce a blue color with
dipheny]amine have been used [73].
It is clear from what has been discussed above that
there is a necessity of developing non-instrumental methods
of analysis such as solid-state spot-tests and TLC. A look
at the literature presented above shows that very little
work has been done on the TLC of anions and almost no work
on capillary solid-state spot-tests of anions has appeared
til] date. In fact a systematic study on anions regarding
their detection, determination and separation is lacking.
It, therefore, appears quite interesting to couple
capillary solid-state spot-test technique with thin-layer
chromatography to cover a wide spectrum of analysis of
anions present in solid or fluid samples. These techniques
provide a rapid method for the screening of a large number
of anions for their quick detection, identification,
quantification und separation.
52
The present work was taken up with the following
aims:
1. To develop new mixed and impregnated sorbent layers for
some useful separations of anions.
2. To make a comparative study on color reactions of
anions in the solid-state and in solutions.
3. To develop new selective and specific capillary solid-
tests for anions.
4. To devise a scheme for the systematic analysis of
anions in the solid state.
Some exciting results achieved by the present
studies aie being presented in the following chapters.
Literature:
The voluminous work done on TLC of inorganic and
organic substances has been well documented in the form of
several reviews, monographs, books and articles. The work
done on TLC of inorganics till 1972 has been admirably
reviewed by Brinkman et al . [74] whereas the work appeared
during 1972-80 has been summarized by Volynets and Kuroda
[75]. The latest work on thin-layer chromatographic studies
of inorganics and organometal1ics has been presented in a
chapter, in Handbook of Thin-Layer Chromatography published
by Marcel Dekker in 1990 [76].
53
The daca available on the published work on TLC of
cations and anions during the last 10 years has been
compared and graphically shown in Figure 7. Surprisingly
very little work has been carried out on anions as compared
to the cations. Table 4 based on the available data from
reviews, chemical abstracts, monographs and books,
summarizes the work done on TLC of anions till date.
54
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(1964); J. Chromatogr., 29, 190 (1967); J.A. Berger,
G. Meyniel, J. Petit and P. Blanquet, Bull. Soc. Chir-.
Fr., 2662 (1963); J. Petit, J.A. Berger, J.L. Chabard,
G. Besse and G. Voissiere, Bull. Soc. Chim. Fr., 1027
(1969); J. Petit, J.A. Berger, G. Gaillard and G.
Meyniel, J. Chromatogr., 39, 167 (1969).
90
155. P.R. Brady and R.M. Hoskinson, J. Chromatogr. , 54, 55
(1971).
156.
157.
M. Muto, Nippon Kagaku Zasshi (J. Chem. Soc. Japan
Chem. Sect.), 85, 782 (1964); 85 147 (1964).
H.D. Beckstead, W.N. French and J.F. Truelove, Can. J
Pharm., 2, 9 (1967).
158. J. Burianek and J. Cifka, Z. Anal. Chem., 213, 1
(1965) .
159. V.D. Canic, M.N. Turcic, S.M. Petrovic and S.K.
Petrovic, Anal. Chem., 37, 1576 (1965).
160. M. Covello and 0. Schettino, Farmaco, Ed. Prat., 20,
396 (1965).
161. H. Kroschwitz, E. Pungor and S. Ferenczi, Talanta, 19,
6 5 (1972).
162. r.Kossel, Z.Ana]. Chem., 197,333 (1963).
163. H. Seller, Helv. Chim. Acta, 44, 1753 (1961).
164. I.N. Brezgunova, V.V. Smolyaninov and N.I. Kharlamova,
Zh. Fiz. Khim., 45, 1785 (1971).
165. V.D. Canic, M.N. Turcic, M.B. Bugarski-Vojinovic and
N.U. Perisic, Z. Anal. Chem., 229, 93 (1967).
166. E. Crener and E. Seidl , Chromatographia, 3, 17 (1970).
167. K. Kawanabe, A. Fujioka, N. Hirasawa, K. Kobayashi and
K. Maruyama, Bunseki Kagaku, 20, 100 (1971).
91
168. K. Kawanabe, S. Takitani, M. Miyazaki and Z. Tamura,
Bunsekt Kagaku, 13, 976 (1964).
J69. M. Muto, Nippon Kagaku Zasshi (J. Chem. Soc. japan,
Pure Chem. Sect.), 86, 91 (1965).
170. W. Peschke, J. Chromatogr. , 20, 572 (1965).
171. S.M. FeLrovic and V.D. Canlc, Z. Anal. Chem., 228, 339
(1967).
J72. V.V. Smolyaninov, J. Chromatogr., 53, 337 (1970).
173. V. Oi Gr egorio and M. Sinlbaldi, J. Chromatogr. , 129,
407 (1976).
174. M. Sinibaldi and M. Lederer, J. Chromatogr., 107, 210
(1975) .
175. A.K. Sen and 0. Ch. Ghosh, J. Liquid Chromatogr., 3,
71 (1980).
176. R.K. Ghatuary and D. Dhar, J. Inst. Chem., 55, 246
'1983 ) .
1 / / . W. Wernei , l-'resenius Z. Anal, Chem., 321, 374 (1985).
CHAPTER - II
ANALYSIS OF ANIONS BY SOLID-STATE SPOT-TESTS
92
The capillary solid-state spot-test technique
reported by this laboratory [l] offers a simple and
inexpensive tool for identification of many organic and
inorganic solids |2-4], and in some cases for their
determination. I he screening procedure can easily be
adapted for use by mobile laboratories in the field. Ihc
choice of indicative parameters in this technique, such a^
the color, length and direction of movement of the colored
boundary leads to selective or even specific detection,
even of chei'iically closely related compounds. The tests can
11 so be ipi^lied bv trituration of the test compound and the
reageni on i spot-plate.
Another novel feature of capillary solid-state
spot-tests is that the boundary between the product and
reacL.mts can be clearly distinguished even when their
r.l- Z color, rire similar. Colored anions such as CrGf, CroO-,' 4 ' z /
Fe(CN)^~ etc. can be clearly detected in a glass capillary
even il the product is yellow or orange. Likewise, colored
reagents can be easily utilized for detection purposes in a
glass capillary. The enhanced selectivity due to the
surface contact of the reactants is an added advantage.
Reactivity in the solid-state depends not only on the
che'iicil nature of the crystal, but also on the positions
occupied b\ ions, atoms or molecules in it [5],
93
Earlier studies [2] showed that the color produced
by a reaction in solution is not always the same as that
Cor the sati.e reaction in the solid state, since the latter
occur with a minimum of atomic and molecular movement.
Considerable work has been done on the detection and
determination of anions in solution [6,7], but none on
systematic detection of anions in the solid state.
Ihe present work summarizes our efforts to utilize
the capillary solid-state spot-test technique for selective
cietectLon and systematic analysis of anions. It has already
proved Uboful for common cations [2]. The technique has
i)een Modified by use of a glass-wool plug to make the test
inore -^elective or even specific.
EXPERIMENTAL
Reagents
All reagents used were of BDH analytical or
laboratt)ry reagent grade, and ground to 50-100 mesh size.
Ihe rcrigenis used were p-dimethyl aminobenzal dehyde (p~DAB).
p diiiicthvl aminocinnamaldehyde (p-DAC), diphenyl amine ( DPA ) ,
p-toluidme (p-IU), benzidine (BD), benzidine hydrochloride
iBDHCi, diethyl amine hydrochloride (DEAHC), barbituric acid
(BTA), chromotropic acid (CA), sodium nitroprusside (SNP),
Phenolphthalein (PPL), potassium hydrogen sulphate (PHS ) ,
94
ferric chjnrjdo (KeClo), silver nitrate (AgNO^), and 507
w/u int i"iat ' mixtures of p-DAB, DPA, p-DAC, p-TD, BTA, CA,
Kl, N,I^MM()^^, l''f'( 1,, FoSO,(NH/^ ^ Z^'^^ ^^'^ AgNO^ with F HS , and
ot SNf' and PPL with NH^Cl .
For detection in solution, ethanol or
deinineral i zed water, or a mixture of the two when
required, was used as the solvent, and PHS and ammoniun
chloride were replaced by dilute hydrochloric acid and
ammonia solution respectively.
Procedures
Sulid-stale detection. About 5-10 mg of the
powdered test macerial was triturated with several mg of
reageiiL lu a depression on a white spot-plate with a glass
rod. I he colors developed at 30 or 40° and on heating to a
higher temperature (60-100°) were recorded.
Detection in solution. One or two drops of an
aqueous solution of the test material were mixed with a few
drops of a concentrated solution of the reagent in a
depression on the spot-plate. The colors developed at 40'
and at higher temperatures were recorded.
Solid-state detection in capillaries. A 10-cm
length of graduated capillary (3 mm internal diameter) was
partly filled with powdered reagent from one end with the
95
help of two iron rods, and the powdered sample was
similarly packed from the other end. Care was taken to make
the packing reproducible and that the two materials were in
close contact in the middle of the capillary. The color of
the product formed at the junction, and the length and
direction of movement of the colored boundary at the
desired temperature after specified time intervals were
recorded,
Solid-state detection in capillaries modified with
,1 glass -wool plug. An air gap between the reagent and the
test material was created by placing a glass-wool plug (4-8
mm) in the middle of the capillary before filling it with
the reactants. I'he test material and the reagent were then
added from opposite ends of the capillary as usual. The
capillary was kept at the desired temperature in an
electrically heated oven. The color formed either at the
glass~wool/reagent junction or the glass-wool/test material
junction was observed after a fixed time interval and the
thickness ol' the colored boundary was also recorded.
RESULTS AND DISCUSSION
The results obtained for the trituration reactions
are summarized in Table 1. They were compared with those
obtained in solution, and in many instances these colors
96
<
E O O a:
ro to •u C OJ 00
0)
e o w
c o
•r-(
<
o in c o
•H •U o re cu
oi
•U
a; c— " l •u o a
00
0) j j ra u GO I
T5 •r-l r-H
o
o CC
TO I-0) Q-e
f < I
I + I
I ^ I
( i •
f f f
+ + +
I -( 4 I I + +- I I I +
I -t ( I I f + I I f I
I I I I I I I I I + +
t ( I I I 4 4 f 4 I f
+ + + • - + 1 + + + +* - +
+ + + I + + I + + +
+ + I I + + + I I I
i I I I + + + I f +
I I 4 I -t + I I t I
I • ( - I I + + I I I I
I I I I + + I I -4 I
t I f ( + •- h I t t
I I f I f I I I f I
I I I I I I I I t I
I I I I I I I I I I
- ( I I I I I I I I I
I I I I • ( + I I • ( I
I I I I I f I I + I
I I I I f +- I I + I
I I I I -t- f I I + +
t • + + ^ + + f - ^ l ^ l • ^ + t - + l + +
I I I I I I I I I I I I I -I I I I I I
+ + + + -t + f + + (- + + + ) I I f - 4 + + | 1 +
I I I I I I I I I I I I I I I I I I -I I I I I
I I I
I I I
I I I
i < I
I- -t ^
I + I
+ I + + I +
I + t ( +
I I I I I I
I I I I I I
I I I I I I
I t I < t *
I I I I I I
I I I I I I
I I I I f -1-
{ I I I I I
I I I I I I
I I I I I I
I ( I I f I
I I I I I I
t
d
h iii
3 ' ? -Z u- U. X <
-c
0 .
+
O
z z u - !_
I I I I I I
Z Z
0 = ^ 5 - - -•: t/i Z a. i , u; o r » = o
— 1/1
y " r < < < + iJ H I- < < Q CJ a Cj U — r l f ^ T v^
— 1/1 a. — ) ^
O + u < • G = 3 H H Q Q o r- 3o c o
</i
t
< < < ^ ~ a a x i G (L C L G G i . — r i '--1 'T - ^
< < <
97
we re entirely different. For example, VO-. reacts with
p-DAB+PHS Lo give a brown product in the solid state but a
3-red precipitate in solution. Similarly, Fe(CN), gives an
orange-yellow product with p-DAB + PHS at 60° in the solid
state, and a brown product in solution. With the same
reagent in the solid-state Fe(CN). yields a green product
which changes to blue-green, while in solution a yellow
2-color is observed. At 40°, Cr20^ reacts with p-DAB+PHS to
give a red product in the solid-state, which is immediately
converted into a dark brown product, but at 60° only a dark
brown product appears. A red color does not occur in
solution at any temperature. It appears that the red
product is unstable and its formation is only possible in
the solid state at lower temperature.
V r(>:
UFA can be used tor the specific detection oi'
in the solid state because this is the only one of
the anions studied that gives any color (green-yellow at
40 ). In .-.olution DPA forms a bright yellow product with
CrO ", . orange with Cr20-, and green-yellow with Fe(CN), 3-
Fhe colors produced by DPA * PHS with NO" Br0~ 10"
SO, cind Cr20^' are different in the solid state from those
in solution. When BrO^ reacts with DPA + PHS the initial
blue color changes to green within few minutes. In solution
only a yellow-brown precipitate is obtained. lOZ behaves
similarly in the solid state but in solution gives a green
98
product.. 10 " /Jives a green color which changes into
yellow in the soJid state, and in solution a stable green
product is fonned. DPA+PHS reacts with MoO^ only in
2- d solution, to give a green product. With Cr20y an
Fe(CN)^ it gives a yellow color in the solid and green in
solut i on.
p-I)AC produces a green-yellow product with most
anions in solution. The brown species formed with SCN in
the solid state differs from that formed in solution
ives an orange color in the solid
2-
( grcen-yel 1 ov;) . SOo
state but docs nut react in solution. SOt and N0„ produce 4 i
a light orange color in the solid at 40° but in solution
both anions giv - a greenish yellow color. For the detection
r)f most anions on a spot-plate p-DAC + PHS was not suitable
because ef Its 0'jji\ color. However, the colors formed with
S- , MoO^ , Fe(CN)^ , VO and Fe(CN)^ in the solid state
differ fro'i those formed in solution. p-TD+PHS gives
colored species with NO2 (light yellow), NO3 (red brown),
l" I red-black), J O3" (blue-black), 10^ (red-violet), MoO' "
( blue-viol et j , VO 3 (violet) and Fe(CN)^'" (pink) in solution
l)ut does not react with these anions in the solid state. In 2- 2 -
the s o l i d s t a t e , CrO^ and Cr^Oy g i v e p a l e ye l l ow and
o r a n g e - y e l l o w c o l o r s r e s p e c t i v e l y wi th p-TD+PHS whereas in
s o l u t i o n they p roduce v i o l e t and brown c o l o r s r e s p e c t i v e l y .
99
Fe(CN)^ gives a brown-yellow product in the solid state,
but a red-violet product in solution.
With BD only two anions, Cx^Ohj' and FelCN)^" react
in the solid state at 40°, giving brown-yellow and green-
yellow colors respectively, allowing their selective
2- 3-detection. In solution Cr^Oy and FelCN)^^ give violet and
4-green-yellow products respectively, and FeCCN)^^ produces a
2~ brown precipitate. CrO^ forms a green-yellow precipitate
2~ in Jiolution. which interferes in the detection of (^.rJ^n i
whereas in the solid state it does not interfere, because
of its conj^lete inertness. At 80° BD reacts with S^O,
ivellow solution), 10 „ (yellow precipitate) and 10, (brown
precipitate) only in solution. N0„ produces a beautiful red
precipitate with BDHC at 80°, which can be utilized for its
selective detection. I0„ and 10, give yellow and green-
yellow precipitates respectively at 40°, whereas at 80"
they produce brown and blue precipitates respectively,
indicating formation of different species at the two
temperatures. CrO, gives a blue-violet precipitate at 40'
but at 80 it produces a dark brown precipitate along with
a green solution. However, in the solid state only a green
producl is obtained at both temperatures. Cr^O-, gives a
brown product in the solid state but in solution gives
brown-violet (40") and brown (80°) precipitates. Fe(CN)^~
100
does not react in the solid but gives light blue and yellow
precipitates at 40 and 80" respectively. BDHC reacts to
2-^ive colored species with only three anions, CrO/^ (green),
9- 3-
Cr^Oy (brownj and Fe(CN), (orange-yellow) in the solid
state at 40° and can be used for their selective detection.
DEAHC was found to be much less reactive towards
anions both in the solid state and in solution. However, it
can be used for the selective detection of CH^COO and
9 -
S.,OT which produce yellow products in the solid state at
40". At 80 \ NO^ gives a yellow product,and I~ and SCN
[live light pink products.
BTA can be used for the selective detection of
SCN and V0„ at 40". SCN does not give any color in
solution but gives a pink color in the solid state. VO-
gives a brown color in the solid state and a yellow color
in scjlution. None of the other anions studied gives any
folor in the ,s(jlLci state with IJ'l'A at this tenipc ra L ure.
Ilowevc!-, ii! sol til ion tlie selectivity of Bi'A is reduced and
seven cUiions ]:)roduce colored products at 40"; MO2 ,
producing a violet solution can be distinguished from the
4-rest ot the anions. At 80", I''e(CN)g gives a green-yellow
solut-ion but does not react in the solid state.
Solid-state color reactions of BTA+PHS can be used
for the selective detection of Br (orange-yellow). I
101
(yellow), SCN tvioJet), Cr207 (brown), Fe(CN)^ (red) and
Fe(CN)t^ (blue). Fe (CN), can be distinguished from 6 6 / — 7 — 9 — —
Fe(CN)^ , and (C.r r^-j from CrO^ in the solid state. CI
gives no color with BTA + PHS and hence does not interfere
in the detection of I and Br in the solid state. SCN
gives a red-vilet color with aqueous BTA + PHS, but no
colored species was observed in solution when PHS was 2-
repl aced by dilute hydrochloric acid. Cr jO-, produces a
blue-green color with aqueous BTA+PHS, which changes to
blue. Similarly, the yellow color initially formed with
Fe(CN), changes to green, but Fe(CN)p gives only a
green-blue color. With an aqueous solution of Bl A
containing hydrochloric acid, NO2 produces a violet color
which is quickly converted into yellow. A red-brown
2- 4-precipitate is obtained with I . Cr^O-, and Fe(CN)^ gi ve
very stable blue species whereas the green-yellow color
formed with Fe(CN), changes to green-blue. BrO^, VO ,,,
2- 2-SO^ and S,-,0o also give colored species with BTA in the
presence of hydrochloric acid, but these anions do not
react with aqueous BTA+PHS. CA is a selective reagent for
3-
the detection of Fe(CN)^ . The colors obtained in the solid
state with NO^ (brown), CO^" (brown), and Fe(CN)^" (red-
yellow) are different from those obtained in solution. At ?- 4-
8U°, S^O^ and Fe(CN), give light blue and yellow colors 2-
respectivel y, but only in solution. Cr„0-, does not react
102
in the solid state but in solution it gives a dark brown
color at 80°. CA-* PHS gives color reactions with many
anions, and hence it can be used as a general reagent for
detection of anions. It gives a brown color with VC' ,
3- 4-
yellow with Fe(CN)g and light yellow with Fe(CN)(^ in the
solid state, but in solution gives a yellow color with VO^,
green-yellow with Fe(CN)g and blue with Fe(CN) . Thus Fe(CN)^ can be distinguished from Fe(CN), in solution.
6 6
SNF can be used as a selective reagent for the
detect Loii of C'rO - , Cr20^ , 1 and Fe (CN) in the sol id
state, and in solution SO can be detected selectively by
means ot the red color formed. NH,C1 + SNP can be used for
the selective detection of I , S20^ , CrO^ and ^r^^^^ in
the solid state at 40°. Fe(CN)^~, Fe(CN)';~ and S2O?" can
also be selectively detected at 80°. In solution this
reagent produces colored products with most of the anions
and can be used as a general reagent.
It is also clear from Table 1 that PPL which
produces a pink color with most anions in solution, can be
2- 2-used tor the selective detection of CO 3 (pink), CrO^
2- 3-(green-yellow), Cr207 (orange) and Fe(CN)^ (yellow) in
the solid state. Amongst all the anions tested, only CO3
and HCO3 give colored products, violet and pink
respectively, in the solid state at 100°, leading to their
specific detection.
103
.2-in particular SCN , VO^ , CrO^ , 612©^ , i^w.^/.
In solid-state spot-tests PHS has been used as a
source of hydrogen ions [8]. We have observed that it is a
good reagent for the selective detection of a few anions,
Fe(CN)?" and
Fe(CN)^ . it produces an unstable violet product with SCN
at 30". With VO3 an orange color in the solid state and a ) _
dark brown precipitate in solution are observed. CrOt
shows an interesting pattern of color changes with PHS at
30". U gives orange product which changes through yellow
to brown in the solid state, whereas in solution a stable
orange-yellow color is obtained. However, at 80°, a green-3-
yellow color appears in solution. FeiCN). forms a yelJou
product in the solid state and a green one in solution.
4-Fe(CN)j. gives a blue product in both the solid state and
in solution.
KIMMHS does not react with NO3 in Che solid statu
but gives red color with it in solution. CI and I react
only in solution, to give a yellow color and a dark brown
precipitate respectively. BrOo gives blue precipitate in
solution at 30" and in the solid state reacts to give an
orange ' red product. Other anions which react only In
2- 2- 2 -solution arc SO, (red-yellow), COo (yellow), ^O'^A
(yellow), PO^" (yellow) and Fe(CN)^~ (red-yellow). The
colors tormed with IO3, VOo,S , SO^ S„0^ , Cr^O-, and
Fe(CN)^ are different in the solid state from those in
104
solution. AL 30', ^nO. gives a brown precipitate along
with a violet gas but at 80° a red solution. Similarly,
MoO, gives blue precipitate along with a brown gas at 30",
and a green solution at 80°
Na„MoO/+PHS produces yellow-brown and violet
products with I and SCN respectively in the solid state,
whereas in solution it gives a green-blue color with 1 and
veilow with SCN . In the solid state HCOo produces a
.2-colorless gas and no color, whereas CO- gives a light
vellow product along with evolution of a colorless gas. Br
does not give any colo; in solution, but in the solid state
Mives a yellow-brown (30°) or blue-yellow (80°) product.
VO3 produces a blue-red product at 30° and a red-brown one,
2-dl 80 bLiL only a yellow color in solution. Cr.-Oy gives
vellow and blue products at 30" and 80° respectively in the
solid state, and an orange-yellow color in solution. At
elevated temperature Na^MoO,+PHS cannot be used
satisfactorily as a solid-state reagent, because of
possible interferences by its own color.
Feci 3 and FeCK+PHS can be used as general
reagents because they produce colored species with most of
the anions, but they require special care to ensure non-
hygroscopic conditions. Furthermore, their utility in
analytical solid-state spot-tests is restricted because of
105
their own color. The color reactions of FeCl-, with Br , I ,
SCN", VO3, SO3", Fe(CN)^" and Fe(CN)^~ in the solid state
3-differ Lroni those obtained in solution. Fe(CN)(^ and
Fe(CN ) 4- react with FeClT+PHS to give brown and green
products respectively in the solid state, and in solution
both give a blue precipitate. I and SCN give a red
precipitate in solution, whereas in the solid state I
produces dark brown (30°) and green-yellow (80°) products.
2-SCN gives a violet product in the solid state. 32©^ gives
a blue color in solution at 30" and a yellow product in the
sol id state at 80°.
FeSO , ( Nil, ) ,,S0, f PHS can be used for the selective
3- 4 detection o\' VO o (buff), Fe(CN);: (blue) and Fe(CN):
(blue) in the solid state at 30". At this temperature, T
the solid state but produce colors in solution.
2- 2-Cr20-7 and MoO, do not react in
AgNOo reacts with I to give a light yellow color
in the solid state, which changes to black, but in solution
a grey precipitate is obtained. S^O^ shows similar / D
behavior in the solid state but produces an orange brown 2-
precipitate in solution. With 820^ the red product
initially formed becomes dark-brown and then black.
AgNO^+PHS gives violet and yellow-brown products with SCN
at 30" and 80" respectively, but only a white precipitate
106
is formed in solution. I gives light yellow (30°) and grey
(80') products in the solid state whereas in solution only
4-a grey precipitate (30°) is produced. Fe(CN)g gives light
yellow (30°) and green(80°) products in the solid state and
a grey precipitate in solution.
Capillary solid-state tests
In the solid-state spot-tests, the test material is
triturated with the reagent to form an intimate mixture but
in the capillary solid-state spot-tests the reactants are
only in contact at the interface. Thus, many color
reactions which occur on trituration are usually not
noticed in the glass capillary tests. Therefore, the anions
that give color reactions by the trituration method were
selected for further study in glass capillaries. Tables 2
and 5 summarize some of the results obtained for the glass
capillarv reactions. It is observed that many anions giving
a cul(;r reaction on the spot-plate do not react in the
glash capillary, showing the greater selectivity c:if t. he-
latter lechnique. For example, CrO^~, Cr^Oy , Fe(CN)^"' and
4 FP((;N)^J do Dot react with p-DAB in the glass capillary but
form colored products on the spot-plate. Thus, p-DAB can be
used for the specific detection of SCN by the capillary
test (lable 3). It gives a yellow product at the junction,
which moves towards reagent, giving a 6 mm length (of color
after 1 hr at 60 ).
c o C < o B o i/1
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ro 0 !-
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,—, s
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1 ^ pq
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° CN
.,_
CJ 2
O 2
^-1
PQ J
O
m
S H
VH
CQ Q
O
CNI
s H
a 2
O 2
o 2 O
>
u
I
CO
H
o 2
CJ Di O 2
PQ 2 2 2
m 2
o o
>
2 O 2
o CNI > 2 pq
Q O 2
PQl 2 1-
PC a 2
2 2 Z 2 u o
2 V-i 2
Z u z
>H
•Q Q 2
1^
Di
1-1 P 3 | S I 2 O
2 2
P I
O
o
p^
O
pq I
o m PQ
o
2 O O
>
1
r <r ^ J:
1 ONI r o
O •Jl
CNl - ^ O ^O > j
1 CNI
CO
CO vX)
1 CNI m
O CM
m
1 rs i v£3
O Csl
Ul
1 Csl ^
O i^
o
Csl r ^ O
OJ
u o
2 O - <D
Ci.
I
2
CNJ
o cc 00 Q
E O
O CQ
2
O
o > o CM
109
o 2
O
S 2 PQ 2
2
•U
o
o 2 2 Oi
PQ 2 2
CTv
3 CQ
a
X ' -
O CQ
•r-l Q
O cQ
LO Q
O Q
OIJ
<
2 2 P Q | 2
J- ,—,
X -•o S
- a o " ^
O PQ CM G rH U
o 1 .
,-J 1
CC
o • •
s H
o 2
pa |2 CQ
I PS
2
2
I-. PQ I
D5
U 1 ^ It-
2 O 2 O
>
o
O 2 2
o 2 > S
o 2
O 2
O a >
o
Pi a 2
2 O 2
> = 2
O 2
C I
O i-i
CQ
1 m O 1—1
1 2 O 00
1 0-) O >
1 rsi en
O C/l
CNJ -Ct O o s:
rsi en O
og
cyi
2
'^
o z
o z:
L; 2
u Z i
^ M 1
13S
c
>— '
s:
o 2 z
o z
1 N < t
V-
' O
u z
u z
u z
1
1
o z
CJ z
1
c i r^
c CXI
/^ —
o 2
O z
1—1
CQ 2 ; z
;:iil
1 V-i
5: z
CQ
O Q
o
^ #
s: [- '
Z
o 2
1
Z o
" — •
o U-
o z
o z
^ ra
s z
o z
1
s 2 z
Vi 5: z
1
z o • — •
0) t i -
r i f\ r> *^
K ^ 1—1 -1 03
ra -H C CD D -P 0 TO
tU 4_l _C tf) 4-J OJ
• U
U-4 O OJ
X i J -U C
0) vi o s s o
t w
O II
.2 ^ 4-» U 01 « VH • 1 - '
•H C X ) ^
00 r "3 '• 0 )
S ^ Q
^ 2 o ^
X 4 j
—-4J E en E
>> « t-l
o p ^ o
X I CU X ex 0) 0 ^,
<U o
OJ O X) O
5 5 " 0
^ U U 0) TO t—1
X! 0
11 >
II Q
> X 0) X •U) U t—1 03 0) r-1 E J3
II il
S PQ
OJ 3
c o 0 r-l
X ) r-, CD
o „ C II
„ >' 11 „
1 4J x:
C " 3 --^ O V. 11
II
X) l-i QJ
r, II
0 0 t ^ C Ct! '"
V-i C 0 QJ
II ^
O II
c 0) CU E r-H
> a o e II
O I X C
II <U 4J
z -§
° 2 )- ": ' o ^
^ 4-J O CU3
u c dl
11 •""
CQ "
0) _^
1 II II
O O , - . 1 ^ O r-^ Z PQ D-
U) 0)
ra 1—1
OO
0)
-U
C •H
T H
CM
^ a • H
1-1
»< T H
r H
<t
C/) i J C cu 00 TO 0)
u
•r-l
3
•U u CO
J-J o c
o X)
1 CN
1
o
^ 1 ^
O 1—1
1 m o o
1
CQ
r i G ;!
r—1
»- -r-l 1 CO Q . O TO Z U
4-) O P
X I 0
ex.
X3 0)
0 1—1
o o
cu x: 4-1
o 4-)
to V-I
0) U-l 0) V-I
C/5 4J 0)
^ u TO (-1
X)
C •H
•r4
3
C O
• H 4-1 TO E 1-1
0 i-w
T-H
QJ
TO 0
c c •H 3
" x: 4-1
(/I
0 ^ •H 4.) " ^ TO QJ
•H E
> ^ OJ O VH 4 ^
TO ' ~ ' 1—1
TO U -1-1 0) 4J
x; -H 4-1 C O -H
110
I l l
p-DAC can be used for the specific detection of
S I vol low product) at 80° and for the selective detection
2-ol NOo (pink-brown product) or SC3 (yellow product) at
120 by the capillary method. Furthermore, NO3 can be 2-
cl early distinguished from SO 3 on the basis of the length
of the colored boundary: NO3 gives a 4.0 mm boundary length
and SO3 only 1.0 mm after 1 hr at 120°. In both cases the
colored boundaries move towards the test material, showing
that p DAC is the only species diffusing. SCN , SO,, ,
SO, and Cr, 0-, do not react in the glass capillary.
p-TD can be used for the selective detection of
CrO, and Fe(CN)^ by means of the products, green and buff
1espectively, obtained at the junction in capillaries. 1 he
boundary zone moves towards the test material in both
, as for Fe(CN,. . 4 6 2- 4
cases, but is twice as long for CrO, as for Fe(CN, 2- 3-
Interestingly, Cr^O-, and Fe(CN). do not react in 2-
capillaries and hence CrO. can be detected in the presence
4-Similarly, Fe(CN), can be detected in the
3-
of Cr^O 2 2^7
presence of Fe{CN)^
BTA is found to be the most suitable reagent for
f ht' specif [i- deteclion of N0'_; by the capillary method. None
"t Iht anions which give colored products in the
trituration spot-test produces any color at the junction in
the capillary, except N02~. It forms a pink boundary which
112
moves towards the test material, to give a length of 4.0 mni
after 3 hr a I 120'.
Fe(CN) can be specifically detected by observing
the orange product formed at the junction by reaction with
BDHC. NO^ and SCN" can be selectively detected at 80' with
DEAHC as reagent. l", Fe(CN)^~, Cro|~ and Cr20^" do not
react in the capillary at this temperature but at 120° CrO,
3-gives a 1.0 mm red-brown boundary and Fe(CNi, a 2.0 mm
dark green boundary after 1 hr. In all cases the reagent is
the diffusing species, since the colored boundary always
extends towards the test material.
Of all the anions which produce colored products
with CA on the spot-plate, only NOo gives a red-orange ring
at the junction in the capillary within 10 min at 30",
leading to its specific detection. This color reaction is
also specific at 80°. At this temperature NO 2 gives a
violet boundary which develops away from the reagent.-
Hov.ever. at 120 VC3 , MoO'4~ and FelCNjg" also react with CA
to give thin black, red-brown and brown-black rings,
respectively, at the junction, within 3 hr. Under these
conditions NO2 gives a 6.0 mm red-violet boundary which is
specific .
NO2 and N0„ react with p-DAB + PHS to give yellow-
orange products at the junction. In the case of NO^ the
113
product changes to green-brown on keeping for half an hour
at 60", giving a boundary length of 2.0 mm on the reagent
side, and NO2 can be distinguished from NO3 on the basis of
either boundary length or color. Simil arl y , Br~ aixl I~ can be
distinguished from each other by the color of the junction;
I and Br give orange and yellow products respectively
(CI does not produce a color). 10/ gives an unstable
yellow product which at 60° changes to brown within half an
hour, whereas 10 3 forms a quite stable orange product,
which distinguishes it from 10^. The red-brown boundary
(4.0 mm] formed by BrO^ at 60° within half an hour with
p-l)AB^PHS can be utilized to distinguish Br03 from VO3
.. _ 2-K hiii ring), 10, or 10,, (0.5 mm). Similarly, CrO, (thin
ves a
J I \j I JL v_y Q \ \j * .J III III / * t j j _ HI jL J a i -i y 5 \^ 1. \^ ,
orang.e ring) can be distinguished from Cr^O-, which gi
red boundary 4 mm in length. Fe(CN), reacts with p-DABM^HS
to iive a transient orange color which quickly changes to
greenihh-bl ue, v^horeas Fe(CN), gives only a blue product.
The boundary length after half an hour at 60° is 3.0 mm for
the former and 4.0 mm for the latter. In all cases the
colored boundaries move towards the reagent, showing that
the test materials are the only diffusing species.
[3-DAC + PHS gives colored products at the junction
onJv with SCN" (violet), CrO^~ (dark brown) and Fe(CN)^"
(dark brown) within 10 min at 30°. Amongst these only SCN
shows a boundary length of 10.0 mm. Therefore. SCN can be
114
seJecLiveiy delected. CI reacts at 80° to give a dark
brown product (2,00 mm) towards the reagent and a pink
product (6.00 mm) towards the test material after Ihr ; I
and Br do not form colored species, however. Thus, CI can
be detected in the presence of I or Br . NO 2 and NO3 both
react with p-DAC + PHS, NO2 to give a brown boundary (2.00
mm) towards the reagent and NO 3 a violet boundary (2.0 v'^)
towards the test material. Thus, NO 2 can be distinguished
froii NO3 by means of the position of the boundary.
DPA+PHS gives a violet boundary with SCN , yellow
with iip\' and blue with FelCN)"^", NO3, Br03, IO3 . CrO^'
and I r C "" all produce green products. However, the green
boundary moves only in the case of N0„ (1.0 mm) towards
the reagent. Ihus, NO^ can be selectively detected on the
basis of boundary length. The colored boundary formed v ith
SCN gives the greatest length, leading to the selective
detection of SCN .
Capillary solid-state spot-tests can be utilized
for the specific detection of SCN and Fe(CN)^~ with
BTA+PHS and SNP+NH,C1 respectively as reagents. Similarly,
2 -PPI tNH,Cl can be used for the specific detection of CO3 or
HCO3, which form pink products at 120".
PHS can be utilized for the specific detection of
VO at 40° and the selective detection of Fe(CN)^~ or
115
Fe((,N)^ ,\i 80 . I he colored boundaries formed with VO3
(brown) ruid Fr'(rN), or Fe(CN), (blue) do not show anv
niovemenL durinj', 1 hr at 80". It is interesting to note
that o\ 11 anions which produce colored products with
2- 2-Agi\(j , on tiituration, only S^0„ and S^O , form bl ack-
broun pioducl U I he junction within 10 min at 40 . 1 he
{'o 1 01 e d t:i . r.2-
wh
oundary formed with Sr,0, shows no movement,
ereas ^nOo gives a 2.0 mm boundary length, which
distinguishes between them. At 80°, AgNO^ gives colored
l~ (red), PO " products with Fe(CN)-: (red), PO- , (black-brown), I
(black-brown), CrO" ^ (black) and Cr^O^-^ (black) at the
junction. The colored boundary moves only in the case of
PO^" (2.0 mm, 1 hr ).
Ferrous ammonium sulfate can be utilized for the
2 y a..^ iiww / . Lw ^ g i v e s a r e d r i n g - • e l e c t i v e d e t e c t i o n of NO^ and MoC"/ . NO
(80 , 1 h r ) and a r e d - b r o w n b o u n d a r y 1 .0 m.m. i n l e n g t h M
h.r <it 100 l .A[ i i ongs t a l l t h e a n i o n s w h i c h p r o d u c e c o l o r e d
2-
products (lable 2) at 80°, only MoO/^ gives a boundary
length of 2.0 mm, which can be used for its selective
detec tion.
I can be selectively detected with Na^MoO,+PHS on
the basis of the length or direction (which is towards the
test material) of the yellow-brown boundary formed at the
2-junction move towards the test material . S„0^ forms a
116
brown-black boundary (4.0 mm) at 100° which moves towards
2-the reagent. Thus, S O ^ can be distinguished from I on
this basis, but i ot from the color. VOo gives a red ring at
40 but a brown ring at 80 or 100° . Of all the anions
tested (jiiJy SOo 1 orms a blue ring at 40 or 80". Therefore,
it can be selectively detected. However at 100°, PO/ also
forms a blue ring at the junction.
At 40", SCN reacts with KI + PHS to give a violet
boundary (8.0 mm) towards the test material within 10 min.
Ihe other anions which give colored products at the
junction such as N0„ (red), BrO^ (yellow), 10^ or 10,
(orange), S2O3" (red), Fe(CN)^" (blue) and CrO^~ (brown)
show no boundary movement. Thus, SCN can be selectively
detected on the basis of the boundary length. At 80° the
formation of a 10.0 mm thick blue boundary by Fe (CN)
allows its selective detection.
It is apparent from Table 2 that the color
reactions of some anions are temperature- dependent. For
example S^0„ gives only a red product with KI+PHS at 40",
v;hereas at 80°, it gives two colored species. The red
product formed at 40° shows no movement. However, at 80° in
addition to the red ring, a yellow product (2,0 mm) is also
formed which moves towards the test material, and gives
2-selective detection of S^Oo .
117
FeCl ., can be used for the specific detection of
SCN" which gives a red violet ring at 40°. CI , Br and I
can be distinguished from each other at 80° on the basis of
the boundary length measured after half an hour (Table 2).
NOT can be detected in the presence of NO2 because at 80' a
2-red ring appears only with NO^. At 80°, CrO, gives a
2-]ight brown boundary (3.0 mm) after 1 hr , but CrJD-j does
2-not react. Thus, CrO, can be detected in the presence of
2- 2 - 2 - 2-Cr.,Ot and SO,, . S gives a red ring and SO,. forms a
yellow ring with FeClo.
it is clear from the discussion above that the
capillary solid-state spot-tests are more selective than
the conventional solid-state spot-tests and many anions can
be selectively or specifically detected by performing the
tests in a capillary. Table 3 summarizes the results
obtained i or the sel ective/specif ic detection of some
anions by tlie capillary method. The selectivity of the
capillary technicjue can be further enhanced by introducing
a glass-wool plug into the middle of the capillary, between
tli£ reactants. In this way the reactants do not come in
direct contact and the reaction, if any, proceeds by vapor
phase diffusion of the reagent or test material through the
glass-wool plug. Such reactions may be termed solid-vapor
phase reactions rather than solid-solid reactions. The
glass-wool technique was applied to the anions which gave
118
TABLE 3
Specific/Selective Capillary Solid-State Spot-Test for some Anions
Anion
.se>r
s^-
SX)f
NO 3
CrO^'
Fe(CN)
FL'(CN)
XO^
S( N
NO 9
SC N
NO
Fo(CNj
I
VO^
SON"
CO'J"
H(0^ J
4-6 3-6
4-6
Tern
Reagent
1
5
5
5
7
iU
1 ]
11
I i
14
17
17
19
22
25
27
perature,
°C
60
80
LOO
120
40
100
80
120
30
120
80
80
120
40
40
40
120
Time
1 hr
1 hr
1 hr
1 hr
12 hr
1 hr
1 hr
3 hr
10 min
1 hr
1 hr
1 hr
1 hr
10 min
10 min
10 min
1 hr
Color of boundary
Y
Y
LY
RBr
G
Buff
0
Y
V
PK
PK
PK
V
Bl-BK
0
Br
R-V
BK Br
BK-Br
LFK
LPK
Direction of movement
TR
NM
NM
TM
TM
TM
TM
NM
TM
TM
NM
TR and
TM
TM
NM
NM
NM
NM
TM
NM
TM"
TM"
Length,
mm
6.0
-
-
4.0
4.0
2.0
4.0
-
2.0
4.0
-
1 6 . (J
10.0
4.0
-
-
~
2 0
-
"The portion of the tube filled with the test material becomes
oo-[)leLcly i ink. All abbreviations as in Table 2.
119
TABLE 4
Glass-Woo] Plug Modified Capillary Solid-State Spot-Test for some
Anions
.-\n i on
NO 2
NO"
Br"
Hie J
\\('0 ,
HrO
'^'\
Si K
V(i
co:
MoO;
•' ' 6
•f ( ( N )
Rc aoeiiL Teinper ature, Time, Color of °C hr boundary
2
4
2
2 7
.2 0
2
2
2
20
21
27
2
65
40
65
120
80
80
65
65
65
65
80
80
100
120
65
65
25 80
65
65
65
8
8
8
]
0.5
1
8
2
G at GW/R
G-)B1 at GW/R
Y at GW/M
LPK" at GW/M
Y at GW/M
0 at GW/M
G at GW/R
DBr at GW/M
8 DBr at GW/M
0.5 0 at GW/R
0.5 0 at GW/M
1 Y--)Br at GW/M
1 Y- Br at GW/M
1 LPK" at GW/R
0.5 0 at GW/R
2 Y at GW/M
1 BK at GW/R
2 G at GW/M
8 G at GW/M
8 Bl at GW/M
Length, niiii
1.0
2.0
5.0
2.0
6.0
2.0
4.C)
2.0
6.0
GW/R ' glass wool/reagent junction CW/M glass wool/test material junction ^_ " Whole tube containing test material (CO^ or HCO- ) beco-nies pink — > indicates a change in color Other abbreviations as in Table 2
Rea^ent 2 / NH, C] +PP1 4
120
colored products in glass capillaries, and the color
reactions observed are shown in Table 4 and show that the
glass-wool technique is superior to the ordinary capillary
technique in terms of selectivity and specificity.
Applications
For obvious reasons (the main one being the
complexity of the ork thatwouldbe involved) the investigation
was restricted to the sodium and potassium salts of the
anions involved. It is a fairly simple matter to devise a
systematic scheme for identification of one of these salts
in the absence of the others, as shown in Scheme 1. It is
also possible to device a systematic scheme for analysis of
a mixture containing almost all the anions examined in this
work. The major problem in devising such schemes is that in
contrast to schemes based on physical separation by
precipitation or extraction, each test is applied to a
j:)ortion of the original sample, so all the components are
present in every test performed. Hence the classification
i .- based on elimination of groups of anions from
consideration, by their failure to give a color with a
jjarticular group reagent. For instance, if no color is
obtained with DPA+PHS in the trituration test, acetate,
molybdate and phosphate are the only anions (of the 25 in
the scheme) that may be present. However, if a color is
S A M P L E
ORANGE
2 -C r ^ O /
1
r
1 NOCOLOR 121
IL G R F E N i ' Y E L L O W
C r O 2-
NO COLOR
O R E E N — K ' Y E L L O W NOCOLOR
3 - | l 2 ftiCU)^-'
COLOR
PINK
5 C N -
NOCOLOR PINK
NOCOLOR
NOCOLOR
12 CO 2 -
BROWN
VO3-
i l COLOR
In
1 NOCOLOR
YELLOW NOCOLOR
I " f?EO
( 3 R 0 W N
B r O - r r
N O C O L O R
1" O R A N G E - Y E L L O W N O C O L O R
B r ' 26
r R E O — « - B L A C K
S 2 O 3 2 -
n NO CO LOR
25
Y E L L O W - B R O W N NO COLOR
1 ) 1
( Y E L L O W
C H 3 C 0 0 "
( BROWN
NOf
NO COLOR
111 NO COLOR
Is r '
COLOR NOCOLOR
C 0 L 0 W
.All-N O C O L O R
NO C O L O R
V t L L O W NO3-
2 3 ( '
B L U E — a - G R E E N
I O 3 -
r
N O C O L O R
L IGHT Y E L L O W
NO COLOR P O / , 3 -
h9
NO COLOR
ORANGE
^ 0 , 2-
I
N O C O L O R
L IGHT Y E L L O W
B R O W N COLOR
20
MoO 2-
SO 2 -
n Y F 1 l o w
H C O i
„^J NOCOLOR
LIGHT YELLOW 2-
NOCOIbR C20^
I' YELLOW
cr Scheme 1 Reactions in a left-hand branch are performed before
those in a right-hand branch. The reagent numbers refer to Table 1.
I — REU
SpOe^
SAMPLE
NO COLOR
NOCOLOR
PALE YELLOW NO COLOR
i2i COLOR
1
NOCOLOR
15
122
ORANGE
5 0 3 ^ '
NOCOLOR LIGHT YELLOW
25 CpO^^-
Y ELLOW •'BROWN
Scheme 2
123
obtained, these three anions may also be present in
subsequent tests, so their reactions with all subsequent
reagents have to be taken into account in working out the
scheme.
On the other hand, it is comparatively easy to use
I able 1 to find small groups of anions that do not give a
color with a given reagent, and then to devise
Identification schemes such as that in Scheme 2.
[he capillary tests can similarly (and more easily)
be organized into a detection scheme, since additional
information is provided by boundary movement of the
products. Devising such schemes is an excellent exercise in
logical thinking, as a part of student training.
As far as we are aware, this is the first attempt
at systematic solid-state analysis for anions. Further
publications will be concerned with the chemistry of the
new reactions described.
124
REFERENCES
1. M. Qureshi, H.S. Rathore and A. Mohammad, Talanta, 23,
874 ( 1976) .
2. M. Qureshi, A. Mohammad and G. Ganga Raju, Talanta,
28, 817 (1981).
3. M.N. Akhtar, H.S. Rathore and M. Qureshi, Talanta, 25,
235 (1978).
4. A. Mohammad and N. Fatima, Microchem. J., 37, 161
(1988) .
5. M.D. Cohen and B.S. Green, Chem. Brit., 9, 490 (1973).
6. F. Feigl , Spot Tests in Inorganic Analysis, 6th Ed.,
r. Isevier, Amsterdam, 19 72.
7. W.J. Williams, Handbook of Anion Determination,
Butlerworths, London, 1979.
8. P.I. Voskresenskii, Talanta, 12, 11 (1965).
CHAPTER - III
MICROGRAM SEPARATION AND SEMIQUANTITATIVE DETERMINATION OF ANIONS
125
In I'ecent years thin-layer chromatography (TLC) has
grown much in status and has experienced a dramatic surge
due to its simplicity, versatility, and low cost. TLC
provides good resolution and is comparatively fast. TLC,
with optimization of techniques and materials, can be
applied for the quantitation of various compounds present in
environmental, geological, and biological samples. Some
recent applications of TLC such as the identification of
perchlorates in explosive residues [l] and the determination
ol' selenium in foodstuffs [2], total heavy metals in
industrial and waste waters [3], ortho- and polyphosphates
in soft drinks [4], and Hg{II) in river and industrial waste
waters [5] have shown its utility as an effective, rapid,
and simple separation technique. Some important separations
involving microgram to milligram quantities of elements have
also been reported recently [6-8].
As evident from the literature survey, few workers
have attempted the TLC of anions [9-12], in contrast to that
of cations [13-20]. Thin layers of stannic chloride,
cellulc)se, silica gel, silufol , and alumina have been used
for the separation and identification of anionic species. In
most of the cases ammonia [21,22] in combination with
alcohols and ketones has been selected as the mobile phase.
Aqueous salt solutions and aqueous-organic systems
containing mineral or carboxylic acids have also been tried.
126
Recent investigations by Mohammad et al . [23] regarding the
effect of solvent composition on the mobility of anions show
that two component systems containing formic acid mixed with
acetone, ethyl methyl ketone, butanol, or isopropanol were
most useful in producing differential migration of anions.
Our work on TLC of cations [17,24,25] in mixed
organic solvents containing formic acid has clearly
established the practical applicability of these systems as
eluents for several analytically difficult separations on
plain silica gel as well as on slice gel layers impregnated
with aqueous salt solutions. The improved separation
possibilities of cations on impregnated silica gel layers
suggested us to study the applicability of impregnated
layers in the analysis of anions. The present paper
describes a thin-layer chromatographic study of anions on
silici gel impregnated with some aqueous salt solutions.
Mixed iqueous organic solvents containing formic acid have
been used as eluents.
It has been possible to clearly separate the anions
at microgram to milligram levels over a wide pH range oi
sample solutions,
EXPERIMENTAL
Apparatus. A thin-layer chromatographic apparatus (Toshniwal,
India), ^0 x 3.5 cm glass plates, and 24 x 6 cm glass jars
127
were used. An El ico Model LI-IOT pH meter was used for pH
measurements.
Test solutions. The test solutions (17o) were either sodium
or potassium salts of ferrocyanide, ferricyanide, chromate,
dichromate, tungstate, iodide, bromide, phosphate,
molybdate, vanadate, nitrate, nitrite, bromate, iodate,
permanganate, oxalate, except SCN (ammonium thiocyanate).
Double-distilled water having a specific conductivity
K - 1.5 X 10 ohm cm at 25°C was used for solutions.
Reagents. All the reagents used were of analytical grade.
Detectors. For the detection purpose the following reagents
were used:
Sc '0, aturated AgNO., solution in methanol for Br , I , PC, ,
CrO, and CroO^ .
2. DiphenyJamine (0.2-0.5%) in 4M H2SO, for lO" BrO" NO^,
NO^, VO" W0,^~, and MnO" J J 4 4
3. Ferric chloride (10%) in 2M HCl for SCN~, Fe(CN)^~, and
Fe(CNl-^~. b
4. Alcoholic pyrogallol (O,57o) solution for MoO , .
2-5. Aqueous potassium ferrocyanide (1%) for CoO , .
Mobile phase. The following solvent systems were used as
mobile phases:
128
S - Formic acid:acetone (1:9)
S2 DMSO:acetone (1:8, 3:6, 6:3)
S^ - Formic acid:DMSO:acetone (1:1:8, 3:1:6, 1:3:6,
5:1:4)
S^ - H2S0^:DMS0:acetone (1:1:8)
S^ - HclO^:DMSO:acetone (1:1:8)
S^ - HCl:DMSO:acetone (1:1:8)
In all the solvent systems, HCl, HCIO,, H^SO,, and
formic acid (FA) were O.IM aqueous solutions while the
acetone and DMSO (dimethylsulfoxide) were used as received.
Stationary phase. The stationary phases were:
(a) Plain silica gel,
(b) Silica gel impregnated with 0.17o aqueous
solutions of CuSO/ , ZnSo., NiCl^ , CoCl^ , a ncl
CO(NHT).C1T. 3 6 3
Preparation of TLC plates.
(a) Plain silica gel plates: Silica gel was mixed with
conductivity water in the ratio 1:3 with constant
shaking for 5 to 10 min. The resultant slurry wab
coated on well-cleaned glass plates to give a layer
approximately 0.25 mm thick. The plates were dried at
room temperature (30°C) and then heated at 100jt 5°C for
1 hour. After activation the plates were stored in an
air-tight chamber.
129
(b) The impregnated plates were prepared by mixing
an aqueous solution of 0.17„ copper sulfate,
zinc sulfate, nickel chloride, cobalt chloride,
and hexamine cobalt III chloride with silica
gel in 3:1 ratio. Thin layers were then
prepared in a similar fashion as described lor
plain silica gel plates.
Procedure. One or two drops of anion solutions were spotted
on the plates with fine glass capillaries. The spots were
dried and the chromatoplates were developed, allowing the
s(5lvenl to ascend to 10 cm from the starting line in all
cases. After drying the spots were visualized using the
appropridte reagent.
For the study of the loading effect on the K,-,
values, the known volumes of standard solutions of anion
were spotted on the chromatoplates with a micropipette. The
plates were developed with 5^(1:1:8). The spots were
detected and their R. (R„ of leading front) and Rrp(R„ of L F ° I F
trailing front) values were determined. The areas of the
spots produced at different concentrations of anion were
also calculated. Standard solutions of 10., and BrO^
(2.5-107.], NO " (2.5-407o), and T (2.5-80%) were used.
For semiquantitative determination of BrOZ and N0.~,
0.01 ml of various standard solutions of KBrO^(1-10%) and
130
NaNO. (2.5-407„) were spotted on silica gel impregnated with
0. 1';' CuSO, layers. The chromatograms were developed with
S^fl:l:H). After detecting the spot, it was copied onto
tracing paper from the chromatopl ates and then the spot area
was ca1cu1 a ted.
In order to achieve the separation of anions at
different pH values, the pH of the test samples were brought
to the required value by the addition of either glacial
acetic acid or dilute sodium hydroxide solution.
Ihe liiiiits of detection of various anions were
(ietermined by spotting different amounts of anionic
solutions on the chromatoplates. The plates were developed
and detected. The method was repeated with successive
lowering of the amount of anion until no detection of the
spot was achieved. The minimum amount of anion just
detectable was taken as the limit of detection.
RESULTS AND DISCUSSION
Ihe silanol group of hydrated silica gel is weakly
acidic and imr'iersion in an aqueous salt solution causes some
catlDH exchange through a reversible reaction. This cation
M"' + m(- SiOH)^=iM{OSi-)";;;'" + mH".
exchange in the normal pH range of 4-7 is very smail ; n is
the charge of the unhydrolyzed ion and is equal to m for
131
trionovalenL ions. Thus the formation of a metal-surface
complex on the surface of silica gel brings about a change
in the retention behavior of the silica gel surface toward
inorganic species.
The results of this study have been shown in Figs.
1-4 and Fables 1-4 . In many cases it was found possible to
separate one anion from several anions. The R^ values for
all anions on copper sulfate-impregnated layer showed
excellent reproducibility (variation does not exceed 51 of
the average value), except NO^ which gave a variation of
8-1 (); from the average K„ value. Among the solvent system
used. FA:DMSO:acetone (1:1:8), i.e. S2(l:l:8) was the best
and the silica gel layers impregnated with 0.1?o copper
sulfate gave better results compared to other impregnants.
Therefore, the chromatographic system consisting of 0.1%
copper sul fate-impregnated silica gel layers as the
stationary phase and S. (1:1:8) as the mobile phase was
selected for detailed study. Figure 1 illustrates the
dependency of R„ values of anions on the nature of
impregnants. Aqueous solutions [O.Vi) of the chlorides of
24 3+ 2+ 2+ 2+
Co , Co , or Ni and the sulfates of Cu or Zn were
used as impregnants and anions were chromatographed on the
impregnated silica gel layers with the S^ (1:1:8) solvent
system. There is a group of anions that are strongly
absorbed or have a little mobility, and a group of anions
132
100
o o
X
a:
L L
rr sz
o o
CE
Z inc s u l p h a t e
N icke l c h l o r i d e
o o
ex
r.
100 r
100
60
20
r C o b a l t ch lor idt H e x a m m ? c c b a H III c h l o r i d e
_ l . J.
o 7
: 4 i—
o O O ° c a > u 2
Anions
F i g . 1 Coni [ )a r i son of R v a l u e s of a n i o n s on d i f f e r e n t
i i i p r e g n a n t s w i t h FA : DMSO : A c e t o n e ( 1 : 1 : 8 ) s y s t e m .
& 2 Compact s p o t w i t h R, -R^ < 0 . 3
k A B d d l y t a i l e d s p o t s v ; i t h R -R > 0 . 4
133
(NO" SCN", r , and BrO~) migrating with the solvent front
giving high K,. values. Br~ could not be detected on the
impregnated layers, whereas it was easily detectable on
plain silica gel layers. In most of the cases CrO^,Cr2(J7,
and Fe(CN).^~ produced tailed spots. The tailed spots in the
case of Cr0| and Cr20^~ are possibly caused due to the
coexistence of the following species in equilibriun as
expected in acidic media.
Cr20^" + U^O :^-^. 2HCrO^
HCrO: r± H' ^ CroJ"~ 4 4
3-However, the tailing of Fe (CN) spot seems due to
3-the incomplete precipitation of Fe(CN)(^ by the zinc present
as inpurity in silica gel.
Figure 2 summarizes the adsorption behavior of
anions in DMSO:acetone systems containing varying concen
trations of DMSO and acetone in their mixture. DMSO being an
aproLic dipolar solvent with hard oxygen and soft sulfur is
a good solvating agent for anions, while acetone does not
solvate the ions. There is a gradual and slow increase in
the Kp values of anions with increasing DMSO concentration.
NO2 and BrO^ showed a sharp increase in their R^ values uith
increase in DMSO concentration. DMSO, being a stronger
solvent than acetone, interacts strongly with the-solute,
decreasing its adsorption and causing faster migration.
134
rn U3
CD
CO
_i__ o T " "
..J. _ __ J. ao
O
.i_._^ I.,
o o o o 6
c o
- • ->
o <
o to
o
c o
u <
o
Q
1
-^
o
1
CI
o
L rs |
O
•r-<
c o
-v (U
ex
oc o •U 03 E O 1-1
o
(J) c o
•r-l
c CD
o
1—I
03
> Di a
0 1
CO
o
c o
4-1
c 0) u c o u
o
o OJ
CN
00
ex o o
o
CU
cx
OJ
CO
OJ
00
CU
o 0)
4-J
CU ~0
u o
o
o o
u
135
However, the slow evaporation of DMSO from chromatoplates
• iftc-r (.heir cievc 1 opincnt . longer dcvel opiiicnt Lime, .md i oor
detection of anions hamper its applicability at higher
concentration.
There is a little effect on the R^ values obtained r
for KI, KBrO,^, NaN02, and KIO^ between the pH limits of 2.5
to 12 (Fig. 3). I he formation of highly compact spots at d1 1
pH values permits a reliable and reproducible separation of
IO3- 1
i.iethocl can be appl fed for the separation and removal of 10^
from acidic, neutral, and saline waters.
3 iron' NO^ , Br03and I over a wide range of sample pH. I his
An attempt has been made for semiquantitative
deterniination of anions by the measurement of the spot area,
l.ie spots were directly drawn on a piece of transparent
ivtper t'roi;! Lhin layer chroma tograms and the area of each
spot vvjs calculated. A linear relationship was only obtained
for N(K and Br0 7 when the amount of the sample spotted was
plotted against the area of the spot (Fig. 4 ) . The precision
and accuracy is always below + 15%. A similar relationship
has been reported for cations [26] and°^-tocophenols [27].
The results of chromatographic behavior of anions in
robilc phases containing variable proportions of DMSO,
acetone, and formic acid are shown in Table 1. The clarity
of detection and compactness of spots increase with the
136
u
0 8 10 12
PH
Fig. 3 rffect of pH of sample on Rp values of anions
J L OD
o o o
o o 00
137
o o CO
O o <r
en =L_
^ •*->
c D O
E <
o o CNl
-v CO
O
O O
o o
o
on
o o CNl
c D O
E <
o c CO
o 4-) c o E CO
05
> CO CU •H
CO
4-) O a •J)
o 4-1
O
cn O
pa
o
•r-l fa
f UJO) D 2 ) J V
138
I
o CO
O
c o
u <
t3
c o
o <
c TO
:- s
c •H c TO
0 o
c > o
o •H c <
in
;2
o
<r o in
I/)
0)
; 03
-J •o 0)
TO
c 00 CD u
a E
u
O 00
<
c o CU 0 0 u •• ro ,-1
o ^ en — Q
0) u. o •IJ .— dJ ex; o ••
i n o
o o
LO
U-1
ON
TO 00 CNi
TO
Q
LTl
i n o o a> z
X ) u c o o
LO
o c o u — (1) OC
o •• TO - J
O (73
i n
o o o
i n
00 OO
TO r--rs)
TO i n
m rs)
Q 2
i n
a> o o
r^ r--
m
i n CO
i n i n TO
rsi CNI
O o
l / ^
a
TO
r^ ro
TO
m CO Q Z
. ^ a
o o
. r^ 0 0
Q Z
^
T H
r o
00
T , (D
vn
m c^
•> o
i n
• rsj i n CTN
CO O
i n
<r en
r-
c
00 Q
m
i n
c r
O m a
i n a^
o o
i n
• m ON
i n
• r~-c^
i n
in m
rsi
o o
m T-H
CM
O
i n CTN
i n
1-1
a>
C7> 00
TO O en
TO i n
vC
TO i n
o ro
TO O CO
TO i n
^ CO
TO
o CO
Q Z
m <r o
Q z
Q Z
v£>
i n
CX> 00
o o
o o
o o
Q z
i n
T—1
a
ro ON
G Z
o z
i n
• < ) •
00
1 0 0 ^
Z o ^' o
U H
1
z o • — •
QJ LM
1 Z o 00
1 csi<r
o ;-. o
1
O r\(
)-. o
; v-
DQ
1 CO < t
1 C t—I CL.
1 O l
o z
CO
z
i n C
o 0^
c o
o o
o o
o o
m o
oc c o
o c
o o
c c
c o
lO
o c
;^
cr X
c o
^ ^
L ' -
. r^
— m ' J cr-
X O O I I
I I
I "^ C O "•J-J" I ' ^ O C C >- C C C OJ C
X) 0) 4J
o CU
u 0)
X )
4-1
c c *-
Q z;
•' •U
c a w 0)
,—1
- D 3 O -o
• 00 Q
• • Q) U 0 2
. <t
• o A
1 J
i J •H
' 4-1 O
a CD
•o OJ
, — 1
•H 03 i J
> , — 1
-o 03 pq
CO
• CO
o
'X \
oT x: XJ •r-l
3
4-1
o a en
-o OJ
1—1
•H n3
H X i
139
140
TABLE 2a
Quantitative Separation ofIO3 fromBrO , NO , I , Br , and SCN on 0.11
CuSO,-Impregnated Silica (Jel Layers Using FA:DMSO: Acetone (1:1:8)
Loading aiount of individual
anion salt in mixture
Separations
(R L R,
^'3
30 ug
0.4 m g
")0 ug
' ) . - . .10
KBrC)^
0.2 5 mg
0.5 mg
0. 1 mg
NaN02
1.0 mg
2.0 mg
0.2 mg
1O3 ( 0 . 1 5 - 0 . 0 :
1O3 ( 0 . 1 7 - 0 . 0 :
1O3 ( 0 . 3 5 - 0 . 0 :
- BrO" (0.96-0.77
- BrO^ (0.98-0.56
- BrO^ (1.0-0.82)
NO; IO3 (0.25-0.0)
IO3 (0.27-0.0)- NO2
IO3 (0.36-0.0)- NO2
(0.98-0.6 7
(1.0-0.51)
(1.0-0.78)
KI
K) pg
0.4 mg
lUO pg
1.0 •• g
1 .0
2.0
4.0
0.4
KBr
4.0
7.0
mg
mg
mg
mg
mg
mg
4.0 mi
I03
I 0 3
I 0 3
I03
I 0 3
I03
I 0 3
(0
(0
(0
(0,
(0,
(0.
(0.
.22-0.0)
.21-0.0)
.34-0.0)
.35-0.0)
,41-0.0)
,4-0.0)
4-0.0)
- I
- r - i~
- i~
- Br~
- Br"
- Br~
(1
(1
(1,
(1
(1,
(1.
(1.
.0-0
.0-0
.0-0
.0-0
.0-0,
,0-0,
,0-0.
.89)
.84]
.75)
.87)
,69)
,65)
81 )
0.4 ro
NH^^SCN
10 yg IO3 (0.3-0.0) SCN (1,0-0.81)
Note: The synthetic mixture of IO3 with SCN (concentration 17o) results
in the formation of precipitates.
141
TABLE 2b
Quant i t ati vo Separation of NOT, from I , SCN , and Br on 0.17o CUSO,-
Inipro.' nat-cd Silica GeJ ] >ersUsi)ii/ Formic Acid : AcetoneC 1: 9 ) as Mobile Phase
Loading amount of individual Separations
anion salt in mixture (R D L "T'
N iNO, K[
^0 jj^,' 0.125 mg NO" (0.6 3-0.43) - I~ (1.0-().87)
0.25 mg NO^ (0.62-0.42) - l" (1.0-0.91)
0.5 mg NO" (0.75-0.55) - T (1.0-0.85)
1.0 mg NO2 (0.77-0.57) - l" (1.0-0.83)
0.3 -.g 1.0 mg NO" (0.65-0.39) - l" (1.0-0.80)
1.0 mg NO" (0.65-0.32) - I~ (1.0-0.78)
2.0 mg NO2 (0.67-0.11) - I~ (1.0-0.80)
NH^SCN
•;0 Mg 0.125 mg NO" (0.69-0.56) - S C N " (1.0-0.88)
0.25 mg NO2 (0.65-0.43) - S C N " (1.0-0.79)
0.5 mg NO2 (0.82-0.69) - SCN~ (1.0-0.89)
0.5 mg 0.5 mg NO2 (0.70-0.50) - S C N " (1.0-0.88)
l.O mg NO2 (0.60-0.31) - SCN" (1.0-0.79)
2.0 mg NO2 (0.63-0.26) - SCN" (1.0-0.75)
KBr
100 Mg 0.5 mg NO2 (0.72-0.51) - Br" (1.0-0.9)
1.0 mg NO2 (0.82-0.64) - Br" (1.0-0.91)
2.0 mg NO2 (0.80-0.72) - Br" (1.0-0.95)
4.0 mg NO2 (0.79-0.62) - Br" (0.96-0.86)
^•0 ,iig 0,25 mg NO2 (0.74-0.50) - Br" (1.0-0.85)
0.5 mg NO2 (0.87-0.56) - Br" (1.0-0.94)
Note: Detection of Br is difficult, requiring about 20 min after
spraying the chroriatogram with the reagent.
142
TABLE 3
Separations Achieved Experimentally at Different pH Values of
Sample Mixture on Silica Gel Layers Impregnated with 0.17o Copper
Sulfate Using FA:DMSO:Acetone (1:1:8) as Mobile Phase
Sar-ple pH value Separations achieved R ^ - R ^ :
2.6 IO3 (0.12-0.0) - BrO^ (0.95-0.85)
5.4 I0~ (0.12-0.0) - BrO^ (1.0-0.801
11.7 IO3 (0.18-0.0) - BrO^ (1.0-0.85)
2.5 IO3 (0.06-0.0) - I~ (1.0-0.95)
6.2 IO3 (0.05-0.0) - I" (1.0-0.93)
11.5 I0~ (0.22-0.0) - r (1.0-0.96)
2.4 10^ (0.07-0.0) - NO^ (1.0-0.90)
6.4 10^ (0.09-0.0) - NO2 (1.0-0.831
11.0 IO3 (0.18-0.0) - NO2 (1.0-0.85
Note: Ihc amounts of I and NO^ are taken in twofold excess in
the r;iixture to ensure sharp detection.
143
increase in the concentration of acetone in the mobile phase
and hence FA:DMSO:acetone (1:1:8) was the best solvent
system in this regard. CrO?" , Cr20^~ , and FelCN)^" gave
double spots when eluated with FA:DMSO:acetone (5:1:4). Ihe
Kp value of anions obtained in O.IM mineral acids (H^SO, or
HCIO, or HCl ):DMSO:acetone (1:1:8) are also recorded in
lable I. These acids can be put in the following preferred
order if used as eluent in combination with DMSO and
acetone:FA>HC10,>HoSO, cr^ HCl . Results of quantitative 4 Z 4 '— ^
separation of lOZ and NO^ from large excess of I , SCN ,
Br , and BrO-T and vice versa are given in Tables 2a and
2b. The proposed method is very convenient for separating
milligram quantities of an anion from microgram to milligram
amounts of other anions.
Ln order to widen the applicability of the important
separation of 10^ from I , N0~ and BrO^ , its separation
from synthetic mixtures of different pH values has been
investigated. Table 3 reveals that 10^ can be easily
separated from I, NOj and BrOo" in the pH range 2,4-11.0 of
sample soUition. Thus, the method can be utilized Lo
separate iO ' from acidic, neutral, and alkaline (natural or
sviithetici samples containing I , NO2 , and BrO"; without
adhering to close control of sample pH.
144
TABLE 4
Limits of Detection and Dilution Limits of Anions as Their Salts
on Silica Ge] Layers Impregnated with 0.17o CuSO, Solution, Using
HCIO, .-DMSOrAcecone (1:1:8) as Mobile Phase 4
Sample Ions Salts
10
1 I
l.
1 3
14
1 T
V4
MoOr NaoMoO, .ZH^O 4 z 4 z
WO^" Na2W0^.2H^O
C^of Na2C20^
1 KJ
VO^ NaV0..H20
l'o(tN)/" KjFetCN)^ o J b
h ''( h /
10^ KI0
BrO^ KBrO.^
S( N~ NH-SCN
NO; NaNO^ z
MnO/!" KMnO,
CrO;" K,,CrO, 4 / 4
Lr^O^" K2Cr20^
Limit of detection
( Mg)
100.0
100.0
100.0
10.0
10.0
10.0
10.0
10.0
^.0
1.0
1.0
1.0
0.5
0.5
0.5
Dilution 1imit^
1 ilO"
1 :10^
1 ilO'
1 : ] 0
1:10-
1 :10-^
1:10^
1:10^
1 :2xl() '
1 .-10^
1 ilO'^
] :10^
1 :2xl(/*
1 :2xl0"^
1 :2xl0'^
"Dilution limit - l:(Volume of test solution x 10 )/
Limit of detection ( pg)]
145
lable L\ summarizes the limits of detection of soiiie
anions as their metal salts along with their dilution
limits. I(. is evident from this table that the proposed
method is highly sensitive for the detection of several
anions,
146
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25. A. Mohammad and N. Fatima, J. Liquid Chromatogr., 9,
1903 (1986).
26. A. Mohammad and N. Fatima, Chromatographia, 22, 109
(1986).
/ . -A Scher. Mikrochim Acta, 308 (1961)
CHAPTER - IV
IDENTIFICATION AND SEPARATION OF SOME ANIONS ON PLAIN AND MIKED ADSORBENT
LAYERS
149
Thin - Layer Chromatography (TLC) today is a
dyna:iiica 1 1 y developing modern analytical technique because
of its simplicity, rapidity, wide spectrum of selectivity
and iniproved efficiency. The separation of ions in TLC is
generally governed by the physical interactions of the
adsorbent and the coordinative properties of the mobile
phase. As a general practice, the composition of mobile
phases is usually altered to achieve a desired separation
on a particular adsorbent. From the literature [1-4] the
following four main approaches concerning the mobile phases
currently in use are identified.
(ij Inorganic solvents (acids, bases, salt solutions,
mixtures of acids and bases or their salts).
(ii) Organic solvents (acids, bases a 1cohols
ilclehvdes, ketones, esters and their mixtures).
', i i i i l-!ixed aqueous organic solvents (organic solvents
'Lxed with mineral acids, inorganic bases, salt
solutions or water).
(iv) rt)mplex forming organic solvents.
I he modern chromatographers are of the opinion that
the I'lObilc phases consisting of more than four components
should be avoided because of problems associated with
150
ruprocliic i bl e preparation. Our recent studies [5] on TLC of
anions vviith single and mixed organic solvent systems also
point out that three component systems are not of much
practical utility for chromatographic separation of anions
owing to the formation of diffused spots.
It is, therefore, amenable to select mobile phase
as simple as possible and prepared from pure grades of
solvent. Keeping this in view, the present work is
undertaken to explore the possible application of distilled
water in chromatographic separation and identification of
some anions on thin layers of pure as well as mixeci
adsorbents. Several favorable features such as easy
availabilitv at low cost, non-toxic nature, high purity,
low viscosity and volatility of water make it fit for
chromatographic studies. Interestingly, a single phase
scjlvent can be repeatedly used.
This paper describes a simpler method for
i (lent 1 r i c IL i on and separation of anions under variable
"\peri cut a! conditions to make it applicable for
L'nvi roiinuMit al samples. NO 2 in artificial sea water has been
identified on chromatoplates.
EXPERIMENTAL
Test solutions. 11 test solutions were either sodium or
151
[)otassiuin salts of al] anions studied, except SCN which
was Laken as animonium thiocyanate. Double distilled water
was used tor the preparation of solutions.
Reagents. Alumina and cellulose microcrystal1ine from CDH
laboratories (India), silica gel 'G' and methanol froti
(>'J axo laboratories (India), and all other reagents were oi
analar grade obtained from BDH, E. Merck or s.d. fine
chemicals (India).
Detectors. The detection reagents for various anions were
used as reported in chapter III. Diphenylamine (0.2-0.5" )
prepared in 4M H^SO, and saturated solution of AgNO^ in
methanol were used for the detection of 10/ and CI
r ( s p e c t i \' e 1 V .
M o b i l e p h a s e . D i s t i l l e d w a t e r w a s u s e d as m o b i l e p h a s e for
the entire study.
Stationary phase. The stationary phases were:
S,,
So
Silica gel 'C
Alumina
Cellulose microcrystal1ine
Alumina + Silica Gel (1:1, 1:2, 2:1
Alumina + Cellulose (1:1, 1:2, 2:1)
Preparation of TLC plates. The plates were prepared by
152
"lixing silica gel or alumina with conductivity water in 1:3
ratio bv weight. The resultant slurry was mechanically
shaken for 10 minutes after which it was applied on well
cleaned glass plates to give a layer of 0.25 mm thickness.
Ihe [11 Uc^s were air dried at room temperature and then
heated at lOO^^'X for Ihr.After activation the plates were
kept in an air tight chamber. Cellulose coated plates were
similarly prepared using a slurry made in 1:4 ratio o!
cellulose to water by weight. No additional binder was
added to the mixture used for the preparation of plates.
Procedure. Ihe procedures for the development of plates,
detection of anions, qualitative as well as quantitative
separation of anions and pH studies were followed as
described in chapter III.
In order to widen the applicability of the
propo.- eci ii'ethod, it was tested for the detection of NO2 in
sea water in the presence of other anions. For this purpose
1 sodiuiii nitrite was prepared directly in artificial sea
water. Ihe sea water was prepared by mixing together 100 iii 1
each c>l the following solutions:
( a 1 0.6 M NaCl
3 (b) 10 M KBr
(c) 3x10^^ M NaHCO 3
153
I'he pH vaJue (8.3) of the synchetic sea water was verv
close to the pH (8.1) of sea water collected from Arabian
sea. An aliquot (0.01 ml) of the synthetic mixture
containing NO^ <ind 10/ , VO- or MnO^ in 1:1 ratio w is
spotted on the chromatoplate. However, in the case of PO^
3-the mixture consists of NO 2 and PO^ ions in 1:2 ratio. The
plate.s were developed after complete drying of the spots.
NO2 (Kj.. 0,95) was detected as highly compact and we^
separated spot. 10^, VO3, MnO^ or PO remained at the
point of application.
To examine the feasibility of the proposed method
for tine separation of certain anions from hard water
•o.imples some important separations ( IO4 or VC^ - lO-
SCN , BrO o or NO2 ) were carried out in the presence of
hardness causing salt solutions (CaCK, MgCl2 and NaHCO^) .
The sample spotting procedure involves loading of 0.02 ml
of anionic mixture containing 10/^ or VO3 - 10^ " SCN ,
HrOi or NOM (1:1:1) on the chromatoplates followed by the
spotlii,;' ot 0.02 "il of CaCAy, MgCK or NaHCO.. The spots
.vere cc [decelv dried before the development of the plates.
Che anions were detected and their R„ values were compared
with their standard K„ values as determined in the absence
of hardness producing salt solutions.
154
RESULTS AND DISCUSSION
The results of this study are presentee! in
figures 1-2 anci tables 1-3. All the anions except CI and
NOo were v;ell detected on all sorbent phases. Generally,
highly compact sjjots for anions on all sorbent phases were
observed. However, occasional tailed spots (K, -K,p > 0.3]
ior Fe(C;N)f^", FelCN)^", CrO^~ and Cr207'' also appeared on
some sorbent layers. The results showed excellent
reproducibility (variation is less than 107„ of the average
K, value) for all anions. The development time for 10 c,
run on silica gel or alumina containing layers was 30-40
niinutcs whereas it was 10-12 minutes on cellulose
VHMU a 1 n i ng, lied .
Fig. 1 illustrates the dependency of R , values on
f he n.iture and composition of sorbent phases. The anions
producing only single spot on all adsorbents have been
taken in figure 1 . Br , I , SCN , Br03 and NO2 move with the
solvent front (R = 0.92-0.96) regardless the composition
of the adsorbent. On silica gel Fe(CN)^ goes with the
solvent front yielding single spot (Rp = 0.95) whereas it
produces double spots corresponding to R^ values about 0.95
and 0.1 on alumina and mixed beds (alumina + silica gel).
Ihe double spots persist also on alumina - cellulose (2:1)
bed showing the dominating effect of alumina on the
155
r o
CD
f ^
o
in
n
i^ I- _1 L
1
o -
1
CD
O
_ 1 L ^ J
O
-- L . J
: o
1
OJ
O
J
o o
c £1
X3
<
OJ
o X) ra
4-J
C
c o en c o C CT3
M - l
O
<u I—I
ro >
DS
o > o c a) c 0) G. 01
Q
00 • f - l
C
<
<
a
<
re
c
3 1 — I
<
O CO
0) 00
03
O
CO
o +
f
o <
OJ
o
«
t
CJO
+
<
vD
CO +
z
CO
J-J
D
(X
u
156
3-niobiliLy of Fe(CN) . However, the higher proportion ot
cellulose in alumina causes the conversion of well resolved
double spots into a badly tailing spot (R^ = 0.0-1.0).
Fe(CK). is strongly adsorbed (Rp
Tailed spot is also produced on pure cellulose layers.
0.1) on al umina and
aluriina - cellulose (1:1, 1:2 2:1) layers. However, it goes
with the solvent (R„ = 0.93) on silica gel layers. It tails
on cellulose and yields double spots (Rp = 0.15 and 0.95
on mixed beds containing alumina and silica gel in 1:1 and
2:1 ratio. A tailed spot on alumina-silica gel 1:2 was
[)roduced by FelCN)^^ . Chromate or dichromate produces
singU- compact spot on alumina (Rp = 0.1) as well as on
silicii ',el and cellulose layers (Rp =- 0.95) whereas taiK-d
spots result on mixed beds. MnO, is strongly adsorbed (R,,
0.081 on silica gel, cellulose and alumina-cellulose
layers bul tails on silica gel - alumina layers. Molybdale
moves with the solvent on silica gel or cellulose layers.
-strongly retained by alumina and alumina-silica gel (2:1 )
and produces tailed spots on alumina-silica gel layers.
10, exhibits strong sorption (Rp = 0.0) on all sorbent
phases except cellulose and cellulose-alumina bed.
Conversely, it goes with the solvent front on cellulose. It
produces double spots (Rp - 0.0 and 0.90) on mixed bed
containing alumina and cellulose (1:1, 1:2, 2:1). The
formation of double and tailed spots may be attributed to
157
the adsurption/precipitation phenomenon taking place
betv-jeen the surface active centers of adsorbent and the
test subs L ance.
Ihe interesting behavior of I0„ facilitates its
scpar.JtLon from several anions. It migrates to the top
fRp 0.93} with the solvent on silica gel and cellulose
layers, just leaves the point of application on alumina
layers (R,, -- 0.23) and exhibits variable adsorption
tendencies on mixed bed containing alumina and silica gel
or cellulose in different ratios. The resulting R^ values
fall in the range of 0.34 to 0.70 and permits some
inportant ternary separations.
Based on the Rr. values of the individual ions on i
different adsorbent layers, several separations are
possible. A few of the separations realized experimentally
are >',iven in Table 1. In addition to qualitative
separations (50 pg) of 10^ was quantitatively separated
Iron 0.) ng of \i)~ or BrO", 3.0 mg of Fe(CN)f^"" and 2.0 iiy
'>' '''<-''l ''1 silica gel layers. The separation of 10, from
r.>K \
t lies I ions
l'( ((-N'f , 10^, BrO.^, I and SCN is important a^
usually interfere in the sepectrophotometric
procedures !6,7j applied for the determination of I0~. The
reproducibility of I0~ - 10^, BrO~ or Fe(CN)^~ separations
was also checked on commercially available precoated plates
158
ca <:
JJ C (1)
1—1
w
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00 c
•H
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X I
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<
c 0) u
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ra 4-1
c OJ E
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P <u a X w T3 OJ > CJ
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X u < C/3 C o •M
• U
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00
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x; a.
>, VH
rt C
o • H 4-J 03 4J OO
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159
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160
fAnchroni F.nte rp r ibes , Lndia). The results (Fig. 2) are
LclenLLcal to those achieved on hand coated plates.
Ihe Ionic species in solution, in most of the cases
varies with the pH of sample solution. For excjmple.
chroniuhi above pH 8 exists as CrO, ions whereas in acidic
2- - 2-medium (pH 2-6) Cr^O-, , HCrO, and CrO, co-exist in varying
2-amounts. '"''loO/, species predominate in strong alkaline
medium whereas Mo^O-^ and Mo-,0, / exist in solutions of
interi ediate pH value. 10^ is reduced to iodine in
soluLions of moderate acidity (0.1-2.0 M HCl ) whereas in
ilka line [uediuni, iodine reacts with OH ions to give iodide
and io".
10^ t 51 6H -) 31^ t 3H„0
I2 - 20H
310
} I + 10 + H2O
(Unstable)
-} 2I~ + 10"
Because ol this fact we carried out the separation
of 10] from 10" BrO^, l". Mooi "' and Fe(CN)^~ over a wide
pH range of sa,iiple solution. The results are presented in
2-l.il lc J. I he separ.ition of 10, from MoO, at pH 3 is not
10
chromatographed as mixture with MoOf . It seems that
periodaLe it this pH value is masked with molybate to forr
possil)le. 10, could not be detected at pH 3 when
.2-
161
Fig. 2 Separation of 10^ Crom 10^, BrO^ and FeCCN)^'
on precodted plates.
(1)
(2)
(3)
IO4 - 103
ro~ - BrO;
10 7 Fe(CN)
162
TABLE 2
S>eparations at Different pH values of Sample Mixture on Silica
Ge\ Layers Using Distilled Water as Mobile Phase
'J
it)
S i i i p J e pH v a l u e s S e p a r a t i o n s (R. - Rr,. pH Vd
]
1 /
9
i'l
1
0
< • )
] 1
3
6.
8.
1 ue
.0
.0
.0
. 0
.1
0
9
1
9
9
s
IO4
1«4
I«4
104
^04
to.
IO4
^04
IO4
IO4
I«4
(0.14-0.0)
(0.1-0.0)
(0.0-0.0)
(0.0-0.0)
(0.0-0.0)
'0.0-0.0)
(0.0-0.0)
(0.0-0.0)
(ND)
(0.07-0.0)
(0.1-0.0)
- IO3
- IO3
- 10^
- I0~
- BrO^
- BrO~
- BrO-
- BrO^
- MooJ~
- MooJ"
- MoO^~
(1
(1
(1
(1
(1
(1
( 1
(1
(1
(1.
(1.
.0-0
.0-0
.0-0
.0-0
.0-0
.0 0
0-0
0-0.
0-0.
0-0.
0-0.
.85 1
.85 )
.90^
.90)
9 2
90 •
90 '
91
7 V<
89)
90)
n . ' i 10^ ( 0 . 0 6 - 0 . 0 ) - MoO^ ( 1 . 0 - 0 . 8 9 )
i . l I 0 7 ( 0 . 1 7 - 0 . 0 ) - F e ( C N ) f " ( 1 . 0 - 0 . 8 8 '4 6
' . 0 10'^ ( 0 . 0 - 0 . 0 ) - F e ( C N ) ^ " ( 1 . 0 - 0 . 8 8 :
iU_^ ( 0 . 0 - 0 . 0 ) - F e ( C N ) ^ ' ( 1 . 0 - 0 . 9 0 :
1 1 . ^ l i \ ( 0 . 0 - 0 . 0 ) - F P ( C N ) ^ ' ' ~ ( 1 . 0 - 0 . 8 6 ;
163
6-Mol ybdoperiodate [8j which migrates with the solvent
front. I'he separation of 10, from I (sample pH 3-12) could
not be achieved. 10. at all pH values and I at pH 3 could
not be detected on the chromatopl ates. IC, was detected
on 1V when its loading amount was kept three fold in che
sample mixture with I . However, the increasing of 10,
amount offers deleterious effect causing very poor
detection of I .
The lower limit of detection of some anions were
determined on alumina layers. The lowest possible
detectable amoLtnt of anions (given in parenthesis) is as
f O I 1 OV.'S .
MnO, (0.7
SCN^ (7.6
4-5 ^ g ) , VO^ (0.70 pg), Fe(CN)^ (0.54 pg
3 pg), 10^ (8.71 jjg), and 10^ (8.30 pg)
An interesting aspect of this study is to
investigate the effect of most frequently encountered ions
e.g. Oa , Mg , Na , CI and HCO„ in the aquecRis
environment on I07 or V0~ - I0~ - S C N " , BrOo or NO"
4 3 3 ' 3 2
separations. In the case of 10, - 10,. - NO „ separation the
spot of 10 J was perfectly round and compact, but the spot
"! '•'';,: bui-uiie (.dongated. A pronounced effect v;as observed
Jii iO^ iO ^ • SCN separation. In this case only SCN is
derected whereas 10 and 10,. could not be detected. As
164
TABLE 3
Kffect of GaCl^, MgCl2 and NaHCO^ on Some Selected Separations
Standard R„ value of Individual Ions are in Paranthesis. 10/
(0.00), IO3 (0.53), VO3 (0.00), SCN~ (0.94), Br03 (0.93) and
NO2 (0.92).
S <i 1 t s Separations (R, - R,,,
CaCl IO4 (ND)
IOA (0.02-0.0)
IO4 (0.02-0.0)
VO3 (0.02-0.0)
IO3 (ND)
IO3 (0.67-0.49
10- 0.73-0.54)
lOo (0.65-0.44:
SCN (1.0-0.89
Br03 (i.0-0.82
NO2 (1.0-0,88
SCN~ (1.0-0.88:
M"uJ 10^ (ND)
10^ (0.01-0.0)
10; (0.03-0.0)
VO^ (0.03-0.0)
10^ (ND) - SCN
IO3 (0.63-0.45)
10^ (0.73-0.60)
IO3 (0.70-0.53) - SCN
(1.0-0.87)
- BrO^ ( 1.0-0.87)
- NO2 ( 1.0-(. .87)
(1.0-0.87)
N iHCO I04(ND)
10^(0.02-0.0)
10^(0.03-0.0)
VO^ (0.01-0.0)
IO3 (ND) - SCN
IO3 (0.65-0.46
IO3 (0.76-0.62
IO3 (0.70-0.50) - SCN
(1.0-0.87)
Br03 (1.0-0.84
NO" (1.0-0.90
(1.0-0.79)
Note: ND, not detected
165
o idem Iron uit le ^ i ] 1 other separations are not effected
h\ the pre'-ence ot Cd" , Mg and Na etc. The K., of 10,
llucLuite between 0.30 to 0.70 in the mixture.
166
REFERENCES
1. I'.A. rh. Brinkinan, G. De Vries and R. Kuroda, J.
Chromatogr. , 85, 187 (1973) .
2. R. Kuroda and M.P. volynets, in CRC Handbook of
Chroniatography: Inorganics, Vol. I (M. Qureshi, ed. ) ,
CRC Press, Boca Raton, Fla., 1987, p. 89.
i. A. Mohammad and K.G. Varshney, in Handbook of Thin
layer Chromatography (J. Sherma and B. Fried eds.),
Marcel Dekker, Inc., New York, 1990, p. 463.
4. N. Fatima and A. Mohammad, Sep, Sci. Techno!., 19, 429
(1984).
5. M. Ajmal , A. Mohammad, N. Fatima and J. Ahmad, J.
Planar Chromatogr., 3, 396 (1990).
6. C.h. Hendrick and B.A. Berger, Anal. Chem., 38, 791
(1966) .
7. A.M. Escarrilla, P.F. Maloney and P.M. Maloney, Anal.
Chim. Acta, 45, 199 (1969).
S. R. Belcher and A. Townshend, Anal. Chim. Acta, 41, 395
{ l'-)6^ I .
CHAPTER - V
THIN-LAYER CHROMATOGRAPHIC SEPARATION OF SOME ANIONS ON COPPER SULFATE
IMPREGNATED SILICA GEL LAYERS
167
Krot'i the literature the TLC of anions has been much
less extensive co'ipared to that of cations fl-3l. Silica
^]e\ [4 8i, cellulose 19-Ll!, alumina [12], silufol [13] and
hydrated stannic oxide layers [14] have been used for the
separation and identification of anions although no work
has been reported on the use of silica gel impregnated with
inorganic salts.
In the present work, the thin-layer chromato
graphic behavior of some common anions on plain and copper
sulfate - impregnated silica has been investigated in mixed
aqueous-organic solvent systems containing acetone.
EXPERIMENTAL
Test solutions. IX test solutions were either sodium or
potassium salts of all anions studies, except SCN which
was taken as ammonium thiocyanate. Double distilled water
was used for the preparation of solutions.
Reagents. Silica gel (E. Merck, India), formic acid,
hydrochloric acid, hydrobromic acid, sodium chloride.
aiimoniuiii hydroxide and acetone (B.D.H., India) were used.
These and all other reagents were analar grade.
168
Detectors. The detection reagents for various anions were
used as reported in chapter III.
Mobile phases. The following solvent systems were used as
I!:obi 1 e phases :
M HCl: Acetone (1:9)
HCl: Acetone (9:1)
NaCl: Acetone (1:9)
NaCl: Acetone (9:1)
HBr: Acetone (1:9)
HBr: Acetone (9:1)
NH,OH: Acetone (1:9)
NH,OH: Acetone (9:1) 4
Formic Acid: Acetone (1:9)
Formic Acid: Acetone (9:1)
"2
M,
M-
Mr
>\r
M 10
In all the solvent systems, HCl, NaCl, HBr, NH^OH and
formic acid were O.IM aqueous solutions while the acetone
\.'as pure .
Stationary phases,
S, Plain silica gel G
S. Silica gt'l impregnanted with O.l-'j.O/
aqueous solution of copper sulfate.
Preparation of TLC piates-
(i) Plain silica gel plates: Silica gel was mixed with
169
conductivity water in the ratio 1:3 with constant shaking
for 5 to 10 inin. The resultant slurry was coated on well-
cleaned glass plates to give a layer approximately 0.25nim
thick. The plates were dried at room temperature (30°C)
and then heated at 100+ 5°C for 1 hour. After activation
Che plates were stored in an air-tight chamber.
(it) Copper sul fate-impregnated silica gel plates: To
prepare impregnated silica gel layers, a slurry was made
by mixing an aqueous solution of O.l-5.07o, copper sulfate
with silica gel in the ratio 3:1. Thin layers were then
prepared as described above for plain silica gel plates.
Procedure. For qvialitative analysis, one or two drops of
the anion sulutions were spotted on the plates with glass
capillaries. The spots were dried and the plates developed
by the ascending technique, the ascent of the solvent was
fixed ac 10 cm in all cases. After development, the plates
were dried and the anion spots visualized with the
appro[)rlate spray reagent. Rp values of the leading front
(R, ) and of the trailing front (R,p) were measured and
reported as (R,-R^),
Rr. values were calculated from R, \ ' T
The limits of detection of the various anions were
determined as reported in chapter III.
summ
170
RESULTS AND DISCUSSION
The main points which emerge from this study are
arized below:
1. A small change in Rp values was sometimes observed
when mixtures of anions were developed as compared
with single substances.
2. The development time for a 10 cm run ranged between
45-70 min depending upon the mobile phase.
3. Silica gel impregnated with CuSO, gave excellent
results. Thin layers were of good quality. Generally,
the spots were compact and well formed in all solvent
systems at 0.1-17o impregnation. Plates impregnated
with 2-57o copper sulfate solution deformed during
development.
4. R,-, values reported in this paper represent the
averages of triplicate tests and were measured to the
center of the spots on the plates.
5. Sodium chloride-acetone (1:9 and 9:1), NH,OH-acetone
(1:9 and 9:1) and HCl-acetone (1:9) systems were found
most suitable for separations. A few anions showed
occasional tailing. HCl-acetone (1:9) was found to be
the best solvent system for multicomponent separation
with 1% copper sulfate impregnation. Formic acid-
171
acoLcjiu (1 :y) produced highJy compact spots of anions
on (). 1 "', copper sulfate layers,
b. Ihe copper sulfate travels with the solvent front upto
the iiicidle ot the plate in solvents M., , M, and M-IM-
Ihcse systems are therefore unsuitable for iinpregn.i t eci
1 ayers.
7. Solvent.^ containing 907o acetone gave better results
than those containing lOX acetone.
2- 2- 3-o. In all solvent systems, CrO^ , Cr20y , Fe(CN)^ and
l- eiLN'i, produced colored spots on impregnated layers
and thus were self detecting.
9. NO. could not be detected on 17o impregnated layers
while it was clearly detected on plain silica gel as
well as on O.IX impregnated layers.
10. In addition to the other ions, VO2 was also chromato-
graphed to assess the possibility of separating VO 2
fro!!, VOT-
Ihe results have been summarized in Figures 1-3 and Tables
1 and Z. Figure 1 summarizes the results of AR^ values
' A Kp Rp )>T plain silica - R,, on impregnated silica)
with various mobile phases. It is evident from Figure 1
that i.iipregnated layers are more selective (strongly
sorbing) than plain silica for most of the anions, as
.0 r
0.8
0.6
-0.2 -
-O.A -
H C i : A c e t o n e ( 1 : 9 )
( a )
1
1 r^t
O Z
1 1 2 U t / l
1
1 i_
00
1
rsi rx/
O >
1
1
O a
1
1 r-1
r> >
I
172
J Nl ^« O U
O
fvl ^
o o 2
• ^ - ^ O
l i . o
Q: <3
O.A
0?
0.0
-0 .2
-O.A
<3
O.A
0.2
0.0
- 0 2
-O.A
HBr ; A c e t o n e ( 1 : 9 )
( b )
_L _L _l
1 rsi U 2
1
Z U LO
PNI C%*
o >
1 n -t
O a
1 n O >
rsi ^
o L ,
f-J
r-i Z ^ -J ;?: ^ "X^^ y U O
u
F o r m i c A c i d ; A c e t o n e ( 1 : 9 )
(c )
A n i o n s F i g . l contfl
173
N a C i : A c e t o n e ( 1:9
<i
Li.
<3
0
0.4
0,2
0^0
-0 2
-0 4
N a C l : A c e t o n e ( 9 : 1 )
( f ) N H ^ O H : A c e t o n e ( 1 : 9 )
o-- 6 - i 5 ^ = S ^ ^
_1_
o 2
U 03
O > o
>
o
1 r~j v j
O O i
' • ' 7 U t>> u_
•-T ^
z U c u.
o
u o
A n i o n s
Fig . 1 contd.
U-cr < j
174
NH4OH : Ace tone ( 9 ; i )
--1 l- ( -. 1 _ _J I :z u in CD
(-Nj r s i
0 >
m vj 0 Q.
1 r~>
0 >
O U
• z u q
u
An ions
Fig. 1 Plot of ARp (Rp on plain silica gel - Rp on
CuSO, impregnanted silica gel layers) vs.
anions
o 1 Copper sulfate impregnation
A 0 .17„ Copper sulfate impregnation
175
indicate d by positive ARp values. There was no
significant ditt'ercnce in the mobility of anions when
chromatographed cm silica impregnated with \% or 0.1°
copper sulfate using HCl , HBr, NaCl or formic acid-acetone
(1:9) solvent systems. With formic acid-acetone, NO2 showed
increased mobility on VL impregnated layers ( Rp = -0.3)
compared to its mobility on plain silica or silica
impregnated with 0.17o CuSO^ ( A R p = +0.1). The reverse
trend was observed for I which moves faster on plain
silica ( ARp = 0.24) compared to W layers. However, 0.1%
CuSO, impregnation was found to be ineffective in changing
the mobility of I which behaved similarly in NH,OH-acetone
(1:9) where it moves faster on plain silica as compared to
1; CuSO/ layers. Sodium chloride-acetone (9:1) and
NH,OH-acetone (9:1) systems were found the most effective
in changing the mobility of most anions on impregnated
layers and thus open numerous possibilities for
separations. However, the tailed spots produced by some
anions limit their separation from other anions. With
NH^OH-ace tone (9:1), most of the anions were strongly
ndsorbecl on V, layers compared to plain or 0.1% layers.
Figure 2 summarizes the hR„ values of anions
chromatographed on silica gel impregnated with II CuSO,
and developed with solvents M. M„,M,,M^,M^,Mg and MQ.
176
o o r—
X
h. a: • — '
U-
rr X
100
80
60
AO
20
H C I : A c e I o n e ( 1:9 )
0
o o » — •
X Li.
cr —
[i-
ir JZ
100
8 0
60
AO
z'O
1 r-J O z.
t\^
-
-
-
7:
u ID
O L
T O O r
CO
4
r-i fsi O >
1
m <t O a
^ 1 m (J >
o
u ^
o O
u u o u
U
H Br : A c e t o n e ( i : 9 )
F o r t i l ic Ac i d ' A c e t o n e ( 1*.9 )
A ri I o n s
F i g . 2 contci .
100
o o < — X
u_ (T —^ LL
u.
80
60
AO
20
0 L_
I - N a C I : Ace tone ( i: 9 )
: i - N a C i : A c e tone ( 9:1 )
177
100
o 80 o
>< 6 0 tier - AO a: X 20
0
N H / ^ O H ; A c e t o n e ( 1:9 )
N H / O H: A c e ( o n e ( 9:1 )
A n i o n s
Fig. 2 Plot of hRp versus anions
htationarv phase: l7o copper sulfate imprrjniat cd
silica ii e 1
O Compact spots with R. -R. <0.3
L Tailed spots with K, "H^ >().3
¥: Badly tailed spots \M.th R,-R^ >0.4
178
IL is evident that the different mobile phases are able
to bring about different retention sequences of anions
leading to several binary, ternary and quaternary
separations. The mid R^ (Rp - 0.4-0.6) values of NO 2 in
M. and Br in M , My and M^ can be used for their
separations form all other anions with higher or lower Kp
Vi 'alues. Vol^, PO4", Mool", Cr207 , Fe (CN) 5 , Fe ( CN) 5 and
WO^ are strongly adsorbed on the impregnated layers (hRp
(J-IO) in all solvent systems containing 907o acetone
(Figure 2). The mobility of a few anions is increased when
the concentration of sodium chloride or NH/OH is increa' ed
2-ile phase (M, and Mo). However, CrO^ and in the mob
Cr ,0^ showed tailing. Likewise, M. and M^ can be utilized
for the ser)aration of MoO, (hR^ = 90-95) from the anions ' 4 F
with low R„ values. SCN , I , Br and NO,-, gave higher Rp
values in most of the .mobile phases and thus can be
separated from anions with lower Rp values.
In Figure 3, the results obtained on O.IZ copper
sulfate layers in various solvents have been summarized. A
major advantage of this adsorbent is that NO3, which could
not be detected on VL copper sulfate layers, was very
clearly detected on 0.17„ layers. Comparison of Figure 2
and 3 slio\.' almost identical chromatographic behaviour of
tht anions on both the adsorbents in HBr-acetone and
loTi'iic acid-acetone. Conversely, most of the anions do \'0\i
100
c o ; > - ' Lt
>
u J-' J,
8 0
6 0
^ 0
^0
1 Nf1/^UH W
A ( e (( M o ( 1:9 )
11- N H ^ U h l
A c e t o n e (9;1 )
- -. 1 _ 1 1.
1/1
-f o m >
1
1 r-1
o >
u__ 1
o u
(_J
1
1
—
1 1 , ^
nop. U tJ
u.
U3
1
•^z I.J W
u.
KO 1
1
O / • ^
U
179
0 0
r , ^ 0
- b 0 I
• . 1 ) 1 1. 1
20 1
o
- _x f \ ) r td ic Ac i d : Ac e t o n e 1 :9
+ r J fxj O >
1 r-i J O CL
1 r-^ O >
LT
' 0 0 ( 1
80 [ I
' 0 [
i> 0 [ I I
2i)
tU 1 : Ac e t o n e 1:9
A n i o n s
Fig . 3 contd
180
^-~•
o o X
u cr
u. Q:
r
100
fi 0
6 0
A 0
2 0
0
C)--
in O
NaC
NaC
Ac e t o n e 1:9
A c e t o n e 9:1
_L I . ^ 1 _ L
o I
o a
O O
I
o o 5
<f?'^^^'" r j -J-
C) o X
u a
u
1 0 0
8 0
6 0
AO
2 0
0
H B r : A c 0 t o n c f 1 : 9 )
c> <)
1 '••'
C)
^
1
z u 1/1
1 r-1 O 7
4-o >
Fig. 3 Plot of hRp versus anions
Srationary phase: 0 .1/„ copper sulfate i npre,"ii i ti H
silica gel
O Compact spots with R,-R^ <0.3
A lailed spots with R,-R^ >0.3
* Badly tailed spots with Rj-R^ ^0.4
u
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181
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184
TABLE 2
Limit of Detection and Dilution Limit of Anions and VO „ on
Silica Go! Impregnated with 0.1X CuSO, with Formic Acid:
Acetone (1:9) Mobile Phase
S] .
No.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
a Dilution
, . Voli
Ions
Br~
3-PO
l'
2
V0~
NO-
NO'
SCN"
Fe(CN]
Fe(CN)
Cro2-
Cr202-
MoO?~ 4
wo^-
] imit
ame of
't 3-6
test
Salts
KBr
Na2HP0^
KI
V02S0^
NaV02.H20
NaNO^
NaN02
NH^SCN
K^Fe(CM)g.
K3Fe(CN)^
K2CrO^
K2Cr207
Na2Mo0^.2F
Na2W0^.2H2
solution (m
3H2O
I2O
0
1 ) X
Limit of detection
100 .0
10 .0
10 .0
10 .0
1.0
1.0
1.0
1.0
1.0
0 .5
0 .5
0 .5
0 .1
0 . 1
10^
Di1utton
11 n 11
2 1:10^
1:10^
1:10^
1:10^
iiio"^
1:10^
1:10^
IrlO'"''
i.-io''
1 :2x10'^
1 :2xl0'^
I -.ZxHy'
1 : 1 0 '
1:10^
Limit of detection { pg
185
behave similarly on both sorbeni:s in NaCl-acetone and
NH, OH-acctone. Thus, in addition to the separation of \'0 - ,,
from numerous anions on 0.1% layers many other m'-ti
separati(^ns oi' anions can be realized in NaCl -•icotf)n(. r
NH,OH-acetone.
The chromatographic systems developed pro\'ide
numerous possibilities for rapid, reproducible and cloTn
separations of anions from mul ticomponent mixtures. Sn- c
separations experimentally achieved have been .sumnari/ed
in Fabl e 1 .
Table 2 summarizes the limit of detection md
dilution limit of various ions. The proposed mcLhod is
highly sensitive for most ions except Br .
186
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187
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13. J. Franc and E. Kosikova, J. Chromatogr., 187, 46;
(1980).
14. A.K. Sen and U.Gh. Ghosh, J. Liquid Chromator., 3. 7
(1980).
CHAPTER -VI
EFFECT OF HEAVY METALS ON CHROMATOGRAPHIC SEPARATION OF 10^ AND
QUANTITATIVE DETERMINATION OF lOf
188
Since its inception in 1950 by Stahl , thin-layer
chromatography (TLC) is on a regular upswing as a result of
which many reviews, monographs, books and scientific papers
dealing with separation, identification and quantification
of micro amounts of different classes of compounds have
appeared in literature fl-8]. TLC in combination with
sensitive quantitative techniques has widen its scope in
the analysis of various natural and industrial microscale
samples. According to recent literature the TLC of anionic
mixtures is much less extensive than for cations or
organometal1ics. As regards the separation conditions, the
influence of counter ions and varying amounts of ions Lo be
separated on the efficiency of the separation have largel\
been neglected.
In continuation of our earlier studies on TIC of
anions the present work is aimed to the development of a
simple and inexpensive method for the selective separation
of 10^ from IO3, Br03, MoO^~ and Fe(CN)^~ on silica eeJ
layers using distilled water as mobile phase. The effect of
more commonly encountered cations such as Pb , Hg , Cd
Ni^^, Co^^, Zn^^, Cu^^, Al-^^, Fe^^, Bi"^^, Tl and Ag" on
the separation efficacy of 10/ from other anions has been
investigated. Volumetric determination of iodate with
preliminary thin-layer chromatographic separation from
periodate has also been examined.
189
EXPERIMENTAL
Test solutions. The test solution 1% were potassium salts
of periodate, iodate ,'iodide , bromate ferrocyanide except
molybdate which was taken as sodium molybdate. 17o solution
of nitrates of lead, bismuth, aluminium, thallous and
silver, chlorides of cadmium, nickel, cobalt, mercury and
iron, sulfates of copper and zinc were prepared in double
distilled water containing small quantities of correspon
ding acids to prevent hydrolysis.
Reagents. Silica gel 'G' and methanol were from Glaxo
Laboratories (India). All other reagents were of also
analar grade-
Detectors. The detection reagents for various anions were
used as report in chapter III.
Mobile phase. Double distilled water was used as a mobile
phase.
Stationary phase. Plain silica gel was used as a
stationary phase.
Preparation of TLC plates. Plain silica gel plates were
prepared as reported in chapter III.
Procedure. To study the metal ion effect on 10^-10^, 10/ -— _ 9 _ ^ / _„
BrOn, lO^-MoO^ and IO/-Fe(CN)g separations, the samplr
190
containing the mixture of 10, , separating anion and neta]
ion in 1:1:5 ratio were used. The synthetic mixture was
prepared by adding five fold excess of metal solution Into
a mixture containing 10/ and the separating anion (10^,
Br03, MoO^ and Fe(CN)g in 1:1 ratio followed by thorough
mixing to get homogeneous solution. About 10 yl of the
synthetic mixture so obtained was spotted on the
chromatoplates. The spots were completly dried at rooT
temperature and then the plates were developed by the
ascending technique, keeping ascent to 10 cm from the
starting line in all cases. After the development the
plates were air dried and the spots were visualized using
the appropriate spray reagent. The R, and R^ values for
both the anions present in the mixture were determined. For
microgram separation of periodate from milligram quantities
of iodate, 1.0 ml solution of periodate was mixed with 1.0
ml of l-107o solutions of KIO^ in a test-tube. 0.01 ml
volume of the resultant mixture was spotted on the
chromatopl ate with the aid of a micropipettc.
Alternatively, 0.01 ml of KIO^ was first spotted on the
chromatoplate followed by the spotting of 0.01 ml of
standard solutions of KIO^. The spots were dried, plates
were developed and detected. The R, and R^ values for both
the anions were determined.
A volumetric procedure was adopted for the
quantitative determination of iodate after its separation
191
from periodate on thin layer chrona'coplates. A standard
volumetric method [9] was set up using O.OIM sodium
thiosulfate solution as intermediate solution. For the
determination of IOT in the presence of IO4, various
samples containing the mixture of KIO^ and KIO, in variable
amounts were prepared. With the help of a lambda pipette 0.1
ml solution of the resultant mixture was loaded on the
chromatoplates. The plates were developed with distilled
water. A pilot plate was employed simultaneously in order
to locate the exact position of the spot on the working
plate. The area covering IO3 was scratched and lOo was
eluted with l.OM HCl , The adsorbent was separated froc
the solution and washed with l.OM HCl to ensure complete
elution of IO3. The filtrate was added to the blank
prepared by mixing 2 ml KI (1%), 2 ml cone. HCl and 0.2 ml
KIOo (1%). The contents were titrated with O.OIM sodium
thiosulfate solution. The blank was also simultaneously
titrated with O.OIM sodium thiosulfate and the difference^
between the volumes of sodium thiosulfate solution consumed
in both the cases was taken for the determination of 10^ in
the sample.
RESULTS AND DISCUSSION
Data collected in Table 1 demonstrate that all
anions produce well formed and compact spots over a
reasonable ranee of loading amount of anion salts. All
192
TABLE 1
Rp Values of Anions on Silica Gel Layers Using Distilled Water as
Mobile Phase
Anions Range of loading Range of R„ Lower detection
amount (pg) obtained limit of anion(jLig)
10^ 50-250 0.00-0.05 4.15
IO3 25-500 0.93-0.95 A.08
BrO" 20-500 0.90-0.95 0.76
MoO?" 100-2000 0.70-0.95 6.61 'k
50-3000 0.94-0.96 7.65
Fe(CN)^ 50-3000 0.72-0.92 5.24 D
The effect of loading amount on Rp values was examined usins:
standard solutions of KBrO^ or KIO3 (1-107J, KIO^ (1%), Na2Mo()^
(l-407c) , K^ Fe(CN)^.2H20 (l-307o) and KI (l-607o).
The limit of detection was determined by spotting different
volumes of anionic solutions (0.01-]%).
193
anions except IOA show greatest affinity towards the mobile
phase and move with the mobile front. However, 10/ is
retained at the point of application and thus ic is well
separated from accompanying anions. The lowest possible
detectable amount of anions on the chromatoplates as shown
in Table 1 indicates the working limit of the procedure,
Br03 less then 1 pg in a sample can be easily detected
using the proposed method. The small difference in the R .
values over a reasonable range of loading amount of anions
given in Table 1 shows the formation of highly compact
spots.
The most interesting aspect of this study is the
separation of 10/^ from other anions in the presence of
counter ions/metal ions. A pronounced effect of metal ions
on most of the separating anion pairs was observed. IO4-
Fe(CN)g separation was badly effected as all added cations
cause precipitation. Similarly, Ag, Pb, Al and Tl hamper
- 2-the separation of 10, from Br03 or MoO^ by producing
precipitation with anionic mixture. The separation of IO4
from IO3 is not achieved in the presence of Pb, Ag, Bi and
Tl due to the formation of precipitates. However, the
presence of other metal ions do not effect the separation
of anions.
In order to present a clearer picture regarding the
separation of 10^ from IO3 , some TLC parameters such as
194
TABLE 2
TLC Parameters for the Separation of IO4 (Rp=0.01) from 10^
(Rp=0.92) in the Presence of Certain Metal Ions
Metal ions
Hg^^
Cd2^
Ni2^
Zn2^
Co2^
Cu2^
Fe3^
Al3^
Rp
0.90
0.87
0.85
0.86
0.87
0.86
0.87
0.87
TLC parame
""'104
19.0
24.0
15.66
10.11
19.0
13.28
13.28
19.0
ters
380.03
244.89
159.79
194.42
220.93
210.79
210.79
220.93
R s
12.05
6.6 ^
5.66
6.29
6.96
6.37
6.96
6.96
195
ARp (Rp of IO3 - Rp of 107), separation factor ( < ) .
capacity factor (K') and resolution (R ) have been
calculated. The numerical values of these parameters have
been encapsulated in Table 2. The following relationships
were used to calculate the values for c< and R . ^ s
4' 3 R.
where, K' =
(ii Ai
where, /jX is the distance between the center of
spots of the separating ions and d. and d^ are their
respective diameters. Two ions are just separated if R =1.
A perusal of data given in Table 2 shows that IC3 is
well separated from IO4 in the presence of Hg, Cd, Ni, Zn,
Co, Fe, Cu and Al as indicated by high values of A R ^ , and
R . The best separation is achieved in the presence of
mercury. The high value of separation factor and fairly
large value of R (R J 6) are indicative of well resolved ^ s s
spots of IO4 and IO3. The large positive value of capacity
factor for IO4 (K' >10) confirms its strong attraction to
the stationary phase compared to the solvent.
20-50 pg of IO4 can be easily separated from ten
fold amount of IO3. The proposed method clearly demonstrate
1%
TABLE 3
Determination of lodate with Preliminary TLC Separation from
Periodate
Amount of 10^ Amount of 10^ Amount of 10^ '/, Error
taken (mg) loaded (mg) found (mg)
0.415 0 .405 0 .412 -1 .7
0 .365 0 .45 0 .441 +2.0
0 .307 0 .50 0 .489 +2.2
0 .232 0 .59 0 .601 - 1 . 9
197
the influence of sample composicion on the separation of
periodate from other anions. The extension of this work to
other species seems worthwhile to pursue.
Finally the results of quantitative determination of
iodate in the presence of periodate have been presented in
Table 3. The results show that the method used is accurate
and also reproducible. It is applicable for microgram
determination of 10- if present in the presence of 10^.
198
REFERENCES
1. J. Sherma, Anal. Chem., 58, 69 (1986).
2. R.G. Ackman, C.A. McLeod and A.K. Banerjee, J. Planar
Chromatogr., 3, 450 (1990).
3. B. Kratochvil and J. Peak, in Analytical Methods for
Pesticides and Plant Growth Regulators, Vo!. XVII
(J. Sherma, ed. ) , Academic Press, New York, 1988, Chap.
1.
4. F.A.A. Dallas, H. Read, R.J. Ruane, and I.B. Wilson,
eds. , Recent Advances in Thin-Layer Chromatography.
Plenum, New York, 1988.
5. L.R. Treiber, ed. , Quantitative Thin-Layer Chromato
graphy and Its Industrial Applications, Marcel Dckker,
New York, 1987.
6. M. Ajmal, A. Mohammad, and S. Anwar, J. Planar
Chromatogr., 3, 511 (1990).
7. T. Shimizu, Y. Suzuki and C. Inose, Chromatographia,
23, 648 (1987).
8. M. Brown, M. Sutherland and S. Leharne, J. Chem. b:duc . ,
64, 448 (1987).
9. W.W. Scott, in Standard Methods of Chemical Analysis,
5th ed. , Vol. 1 (N.H. Furman, ed. ) , D. Van Nostrand
Company, Inc., New York, 1939.
MKROCHIMKAl JOI RNM 44, <9^!< ( I99I I
Chromatography of Anionic Pollutants on Silica Gel Layers; Selective Microgram Separation of N02^ and IO3
Ai I MOHAMMAD* AND SHARAD TIWARI
Anatxlual l.ahimiu>i\ Dcpiulmenl i>l Applied C'hemisli\. /.akir Hiissain C'dllcvc <>t l.niiinecrim; ami Ici hnoliivx, Alii;tifh Miisliin Universilw Aliiiarli-2()20l)l. India
Received November 15. I'WO; accepted February 10, 1991
investigations regarding lhin-la\ei chromatographic behavior of seventeen anions have been conducted on sihca gel impregnated with inorganic sails such as copper sulfate, zinc sulfate, cobalt chloride, hexamine cobalt ill chloride, and nickel chloride using mixed aqueous-organic eiuents Lonlaimng formic acid. The effect of mineral acids on the mobility of anions has .ilso been studied by substituting formic acid vnth HCl. H,S().,, or H("l()4 in the mobile ph.isc In addition to mrcrogram separation of NO, and lO, from various anionic species some other important quahtative separations have also been realized. The effect of pH ot the sample solution and loading amount of 1(), . BrO, , NO, , and 1 on their /?, values has been investigated. I he limits of identification for all anions on impregnated layers have been determined. Semiquantitative determination of NO-, and BrO, have been attempted usiiii; the spoi .uea mcisuiement method. ' iwi VL.Kk-mu Press, im
INTRODUCTION
In recent yeais thin-la\er chromatography (TLC) has grown much in status and has experienced a dramatic surge due to its simplicity, versatility, and low cost. TL.C provides good resolution and is comparatively fast. TLC, with optimization of techniques and materials, can be applied for the quantitation of various compounds present m environmental, geological, and biological samples. Some recent applications of I l.C such as the identification of perchlorates in explosive residues (/) and the determination of selenium in foodstuffs (2). total heavy metals in industrial and v^iste waters (J), ortho- and polyphosphates in soft drinks (4). and Hg (111 in river and industrial waste waters (5) have shown its utility as an effective, rapid, and smiple separation technique. Some important separations involving microgram lo tnilligram quantities of elements have also been reported recently (6-A).
As evident from the literature survey, few workers have attempted the TLC of anions (9-/2), m contrast to that of cations {13-20). Thin layers of stannic chloride, cellulose, silica gel. sijufol, and alumina have been used for the separation and identification of anionic species. In most of the cases ammonia (2/, 22) in combination with alct)hols and ketones has been selected as the mobile phase. Aqueous salt sokitions and aqueous—organic systems containing mineral or car-boxylic acids have also been tried. Recent investigations by Mohammad ct al. {23) regarding the eftect of solvent composition on the mobility of anions show that two component sv stems containing formic acid mixed with acetone, ethyl methyl ketone, butanol, or isopropanol were most useful in producing differential migration of anions.
^9
()()26-265X'91 $1.50 ( opMi.Kht < IWI b\ Acidemia Press. Iru \li !ij:lils of reprodiiLlion in .in\ l()rm reserved
40 MOHAMMAD AND IIWARI
Our work on TLC of cations (24-26) in mixed organic solvents containing formic acid has clearly established the practical applicability of these systems as eluents for several analytically difficult separations on plain silica gel as well as on silica gel layers impregnated with aqueous salt solutions. The improved separation possibilities of cations on impregnated silica gel layers suggested we study the applicability of impregnated layers in the analysis of anions. The present paper describes a thin-layer chromatographic study of anions on silica gel impregnated with some aqueous salt solutions. Mixed aqueous organic solvents containing formic acid have been used as eluents.
It has been possible to clearly separate the anions at microgram to milligram levels over a wide pH range of sample solutions.
EXPERIMENTAL
Apparatus. A thin-layer chromatographic apparatus (Toshniwal, India), 20 x 3.5-cm glass plates, and 24 x 6-cm glass jars were used. An Elico Model LI-IOT pH meter was used for pH measurements.
Test .solutions. The test solutions (1%) were either sodium or potassium salts of ferrocyanide. ferricyanide, chromate, dichromate, tungstate, iodide, bromide, phosphate, molybdatc, vanadate, nitrate, nitrite, bromate, iodate, permanganate, oxalate, except SCN (ammonium thiocyanate). Double-distilled water having a specific conductivity Af = 1.5 x 10 ''ohm ' cm ' at 25°C was used for solutions.
Rcui^ents. All the reagents used were of analytical grade. Detectors. For the detection purpose the following reagents were used: 1. Saturated AgNO, solution in methanol for Br , I , PO] , CrOj and
Cr,0^ . 2. Diphenylamine {0.2-0.5Vc) in 4 M H,S04 for 10, , BrO, . NO^" . NO," , VO,",
WO5 , and Mn04 . 3. Ferric chloride (10%) in 2 M HCI for SCN , Fe(CN)^ . and Fe(CN)(^ . 4. Alcoholic pyrogallol (0.59f) solution for MoO^ . 5. Aqueous potassium ferrocyanide (1%) for C^Oj . Mobile phase. The following solvent systems were used as mobile phases:
S| Formic acid:acetone (1:9) S, DMSO:acetone (1:8, 3:6, 6:3) S^ Formic acid:DMSO:acetone (1:1:8, 3:1:6, 5:1:4) S4 H.S04:DMSO:acetone (1:1:8) Ss HCI04:DMSO:acetone (1:1:8) S„ HCl:DMSO:acetone (1:1:8).
In all the solvent systems, HCI, HCIO4, H2SO4, and formic acid (FA) were 0.1 M aqueous solutions while the acetone and DMSO were used as received.
Stationary pha.se. The stationary phases were: (a) Plain silica gel. (b) Silica gel impregnated with 0.1% aqueous solutions of CUSO4, ZnS04,
NiCl., CoCU. and Co(NH,)f,CI,. Preparation of TLC plates. (a) Plain silica gel plates were prepared using the method reported earlier (27).
C HROMAIOCRAPHY OI ANIONIC POl.l.U I AN I S 41
(b) The impregnated plates were prepared by mixing an aqueous solution of ().\9c copper sulfate, /inc sulfate, nickel chloride, cobalt chloride, and hexamine cobalt III chloride with silica gel in 3:1 ratio. Thin layers were then prepared in a similar fashion as described for plain silica gel plates {27).
Procedure. One or two drops of anion solutions were spotted on the plates with tine glass capillaries 1 he spots were dried and the chromatoplates were developed, allowing the solvent to ascend to 10 cm from the starting line in all cases. After drying the spots were visualized using the appropriate reagent.
For the stud\ of the loadmg effect on the /?, values, the known volumes of standard solutions of anion weie spotted on the chromatoplates with a micropi-pette. The plates were developed with .S, (1:1:8). The spots were detected and their/?[ (/?, of leading front) and/^i {Ry of trailing front) values were determined. The areas of the spots produced at different concentrations of anion were also calculated. Standard solutions of lO, and BrO, (2.5-10^), NCK (2.5-4()9f), and I (2.5-8()9(^) were used
For semiquantitative determination of BrO, and NO; . O.OI ml of various standard solutions of KBrO, (l-l()'/r)and NaNO^ (2.5-409f) were spotted on silica gel impregnated with O.l'f C'uS04 layers. The chromatograms were developed with S, (1:1:8). After detecting the spot, it was copied onto tracing paper from the chromatoplates and then the spot area was calculated.
In order to achieve the separation of anions at different pH values, the pH of the test samples were brought to the required value by the addition of either glacial acetic acid or dilute sodium hydroxide solution.
The limits of detection of various anions were determined by spotting different amounts of anionic solutions on the chromatoplates. The plates were developed and detected. The method was repeated with successive lowering of the amount of anion until no detection of the spot was achieved. The minimum amount of anion just detectable was taken as the limit of detection.
RESULTS AND DISCUSSION
The silanol gioup of hydrated silica gel is weakly acidic and immersion in an aqueous salt solution caLises some cation exchange through a reversible reaction.
\r • w( SiOH) ^ MtOSi-)"„/" + w H ' .
This cation exchange in the normal pH range of 4-7 is very small; n is the charge of the unhydroly/ed ion and is equal to m for monovalent ions. Thus the formation of a metal-surface complex on the surface of silica gel brings about a change in the retention behavior of the silica gel surface toward inorganic species.
The results ot this studv have been shown in Figs. 1-4 and Tables 1 ^ . In many cases it was found possible to separate one anion from several anions. The /?, values for all anions on copper sulfate-impregnated layer showed excellent reproducibility (variation does not exceed 59^ of the average value), except NO; which gave a variation of 8-10''^ from the average /^, value. Among the solvent system used, FA:DMS():acetone (1:1:8), i.e., S, (1:1:8) was the best and the silica gel layers impregnated with ().\'4 copper sulfate gave better results compared
42 MOHAMMAD AND I IWARl
to Other impregnants Therefore, the chromatographic system consisting of 0.15f copper sulfate-impregnated sihca gel layers as the stationary phase and S, (1:1:8) as the mobile phase was selected for detailed study. Figure 1 illustrates the dependency of Rf values of anions on the nature of impregnants. Aqueous solutions (0.19?) of the chlorides of Co"^, Co^ * , or N r " and the sulfates of Cu"* or Zn" were used as impregnants and anions were chromatographed on the impregnated silica gel layers with the S, (1:1:8) solvent system There is a
o o X u.
ct
LL Ct
100 r
60 -
20
8>-4
\
' ' c
f 1 1 /
A ' /
A/ ) 6 —1—X—
^ \
\
\ 1 1 ».y
Zinc sulphate
Nickel chloride
vx eg >f
O
100 r o o
X
U-tr
u. en
o o
u. tr
u. a. SI
Plain silica gel
- Copper sulphate
Cobalt chloride Hexomme cobalt I I I chloride
Anions PIG 1 Compaiison ot K, values ot anions on ditterenl impregnants with the FA DMSO Acetone
(I 1 8) svsteml ACompaLl spot with « , - / ? , < 0 1 (A) Badly tailed spots with « , - « , 0 4
( HROM \ lOCiRM'HY Ol ANIONIC P O I I U I A N I S 43
0 i -
0 8
0 2 ^
0 L
~ x »
i h
MS A eto
Fe(C N ) ,
Fe(CN)g
" ' 3 ) MoO/ WO,
0 i
0 2
0 0
B rO ,
(1 8) (3 6) (6 3)
DMSO Acetone
1 ic 2 ^ttti.1 ot DMSO Lonti-nli ition i)n the R, \ IIULS ot anions thi()mcitot,idphccl on sihea j,cl l.iycrs impiegn.iltd wilh 0 I Loppti Mill ilt Nl) not dtttclccl
group ot anions ihdt die slionglv adsorbed or have a little mobility, and a group ot anions (N()^ SC N I and BiO, ) migiating with the solvent tront giving high /Ji values Bi could not be detected on the impregnated layers whereas it was easily detectable on picun silica gel lavers In most ot the cases Ci()4 Cr^Oy , and Pe(CN),' pioduccd tailed spots I he tailed spots in the case of Cr04 and Cr^Oy aie possibly caused due to the coexistence ot the following species in equilibiium as expected in acidic media
Ci ,() ' + H ,0 ;=± 2HCr04 HCi()4 — H + Cr()4
However the tailrng ol h e(C N),' spot seems due to the incomplete precipitation ot Pe(CN)^ b\ the /inc present as impurity in silica gel
higure 2 summaii/es ihe adsorptron behavior ot anrons m DMSO acetone systems containing varving concentrations of DMSO and acetone in their mixture
LJ. CE
1
0
0
0
u n
0
9
8
2
-
1 ^ 0 1 1 1 1 1 1 1 1 1
— • KI
• NaN02
_ - ^ K I 0 3
1 1 1
PH
I K ' 1 ticel ol pll ot sample on R, values ot anions
44 MOHAMMAD AND TlWARl
DMSO being an aprotic dipolar solvent with hard oxygen and soft sulfur is a good solvating agent for anions, while acetone does not solvate the ions. There is a gradual and slow increase in the Rp values of anions with inci easing DMSO concentration NO^ and BrO, showed a sharp increase in their /?[. values with inciease in DMSO concentration. DMSO, being a stronger solvent than acetone, interacts strongly with the solute, decreasing its adsorption and causing faster migration However, the slow evaporation of DMSO from chromatoplates after their development, longer development time, and poor detection of anions hamper Its applicability at higher concentration.
There is a little effect on the /?[ values obtained for KI, KBrO,, NaNOj. and KIO, between the pH limits of 2.5 to 12 (Fig. 3). The formation of highly compact spots at all pH values permits a reliable and reproducible separation of 10, from NO, , BrO, and I over a wide range of sample pH. This method can be applied for the separation and removal of 10, from acidic, neutral, and saline waters
An attempt has been made for semiquantitative determination of anions by the measurement of the spot area The spots were directly drawn on a piece of
TABLE I IJR) Values ot Anions in Solvents Containing DMSO and Acetone Mixed with 0 1 M Acids on
0 r-f CuSOj-lmpregnated Layers
hR,
0 I M H,SO. 0 1 M HCIO, 0 I M HCI
' \n ions
Fe(CN)^
Fe(CN)^
SCN
C i o ;
Cr,()^
Br
1
POj N O ,
N O ,
ID,
BrO
M o O j
W O j
vo. CO]
MnO^
0 1
1 1 S
12
02
89
^0 V
^ 0 '
N D
8X S
0(1
9^
84 ^
07
8^
00
00
00
— —
M hormic
^ 1 6
^S
n 91 S
% v
16 5"
94 "i
96
00 91 S
N D
21 9^ "i
00
00
00
— —
acid D M S O
1 1 6
<; <i
00 9S
M)"
Mr
N D
N D
00
N D
N D 5 5
89
00
N D
^ s — —
acetone
•i 1 4
DS 0 9S •;
2 5
9^
DS
0 94 S
DS
0 9"; s
9"
9S
(K) 9S 5
97 "i
80 5''
97
00
(K)
N D
— —
D M S O
ace tone
( 1 1 8 )
22"
00
9*; V"
^'^"
N D
96 "i
00
87 •!
N D ^ "i
80
00
00
00
00
10 ^
D M S O
ace tone
(1 1 8)
10 "i
00
88 "i
27"
21 S"
N D
9'i
00
77
8<i "i
O i
81
00
00
00
00 7 S
D M S O
acetone
(1 1 8)
Q^
00
9^ ^
28"
2^ V
N D
9S S
00
91
N D
OS
96
00
00
00
00
OS
\(>li DS double spot Nt) not detected ' Badly tailed spot wilh « , - /?, ^ 0 4 ' I ailed spot with /?, - /?, > 0 1
l A R I t 2a
Quanti tdi ivc Stp.u. i l ion i>t l O , from B r O , N O , I Br and SC N on 0 1*^
C u S d j Impicuna teJ Silica Ciel 1 avers Using hA D M S O Acetone (1 I Hi
I Odding uiioiinl ol nidividual
anion salt in ni ixtui t
K B t O
0 2^ nig
(1 s nig
0 I nig
N a N O
1 0 nig
2 0 nm
0 2 nig K l
1 0 niK
2 0 nm
4 0 nig
0 4 nm
KBi 4 0 mg " (» nig 4 0 mt;
N H , S( N
IO | ig
l O , S ( ) |
0 4
•>()
0 4
sO|
0 4
IDC
1 0
0 4
u-g
mg
M-g
mg
u-g
mg
t |Xg
mg
mg
Sepai . i l ions
( « , - R,)
l O , (0 1 M ) 0 ) BrO , (0 96-0 77)
l O , (0 17-0 0) - B r O , (0 9 8 - 0 ^ 6 )
l O , (0 ^s -0 0) - B rO , (1 0-0 82)
l O , (0 2s-()0) N O , (0 9X-0 67)
l O , (0 27-0 0) N O , (1 0-0 M) l O , (0 M-^)0) N O , (1 0-0 78)
l O , (0 22-0 0) I
l O , (0 21-0 0) 1
l O , (0 ^4-0 0) I
l O , (0 ^s-c) 0) 1
l O , (0 41-0 0) Br
(1 0-0 89)
(1 (M) 84)
(1 0-0 7" )
(1 0-0 87)
(1 0-0 69)
l O , (0 4-0 0) Br (1 0-0 6S)
l O , (0 4-0 0) Br (1 0-0 81)
l O , (0 M ) 0) SC N (1 0-0 81)
\Mth S( N ( toncen t ra l ion I 'c) results m the tormat ion ot \(>l( 1 he s\nthLliL niivluK ot lO
precipi tates
1 \ B 1 F 2b
Quanti tat ive Sepai ition ot NO t iom I SC N and Br on 0 \'i C u S O j Impregnated Silica Ciel
1 a \ e i s I sing Hoimic Acid Acetone (1 9) as Mobile Phase
1 oadinc imoiinl ot individual
anion salt in nnxtu ie
N a N O
S()|Xg
0 s mg
1 0 mg
2 0 mg
s O n g
0 s mg
1 0 mg 2 0 mg
100 |ig
4 0 mg
Kl I) 12s nm
0 2s mg
0 ^ mg
1 (I nm
I 0 mg
NIl^SC N
0 12s mg
0 2 s mg
0 s nm
0 s mg
IsBi 0 s mg
1 0 mg
2 0 nm
4 0 mu
0 2^ mg
0 s nm
N O ,
N O ,
N O ,
N O
N O ,
N O ,
N O
N O
N O ,
N O ,
N O ,
N O , N O ,
N O ,
N O ,
N O
N O ,
N O ,
N O ,
Sepal
(«,
(0 6 M ) 4 1 )
(0 62-0 42)
(0 7 M ) SS) -
(0 77-0 ^7) -
(0 6S-0 W) (0 6S-0 ^2)
(0 67-0 11)
(0 69-0 %)
(0 6 M ) 4^)
(0 82-0 69)
(0 70-0 M))
(0 60-0 M) -
(0 6 M ) 26) -
(0 72-0 M)
(0 82-0 64) -
(0 8-0 72) -
(0 79-t) 62)
(0 74-0 ^) -
(0 87-A) ';6)
al iens
«,)
1
1
1
1
1
1
1
SCN
SCN
S t N
SCN
SCN
SCN
Br
Bi
Bi
Br
Hi
Bi
11 0-0 87)
(1 0 -0 91)
(1 0-0 S i)
(1 (M) 81)
(1 0-0 80)
(1 0-0 78)
(1 (M) 80)
(1 0-0 88)
(1 0-0 79)
(1 0-0 89)
(1 0-<)88)
(1 0-0 79)
(1 (M)7<i)
(1 0-<) 9)
(1 0-0 91)
(1 0-0 9S)
(0 96-0 86)
(1 0-0 8'i)
11 (M) 94)
\(>!t Detection ot Bi istlilliLull i cqui img about 20 mm after spiaying the ch romatogram with the
leagent
4s
46 MOHAMMAD AND IIWARl
JABLE 1 Separations Achieved txperimentallv at Different pH Values of Sample Mixture on Silica del
Layers Impregnated with 0 I'/r Copper Sulfate Usmg FA DMSO Acetone (I I 8) as Mobile Phase
Sample pH value
t
^ 4 s (l
7 8 9
\(>ic Ihe
detection amounts of 1 and
"i 4 II 7
2 *>
6 2
II " 2 4 6 4
11 0
NO,
lO, K), lO, K), lO, lO, 10, K) K),
Separations achieved
(«, (0 12-0 0) (0 12-0 0) (0 IS-0 0) -(0 06-0 0) -(0 OS-O 0) -(0 22-0 0) -(0 07-0 0) -(0 09-0 0) -(0 18^) 0)
- « , )
BrO, BrO, BrO, 1 1 1 NO, NO, NO,
0 9M) 8*; 1 0^) 80) 1 (M) 8*)) 1 (M) 9<i) ) (M) 9"*) 1 (M) 96) 1 0-0 90) 1 (M) 8 ) 1 0-0 8^)
are taken m twofold excess in the mixture to ensure sharp
transparent paper from thin layer chromatograms and the area of each spot was calculated. A linear relationship was only obtained for NO, and BrO, when the amount of the sample spotted was plotted against the area of the spot (Fig. 4) The precision and accuracy is always below ±l59f. A similar relationship has been reported for cations {28} and a-tocophenols (29).
The results of chromatographic behavior of anions in mobile phases containing variable propoitions ot DMSO, acetone, and formic acid are shown in Table 1. The clarity of detection and compactness of spots increase with the increase in the concentration of acetone in the mobile phase and hence FAiDMSOacetone (11:8) was the best solvent system in this regard. CrO^ , Cr O^ . and Fe(CN)^ gave double spots when eluated with FA.DMSOracetoe (5:1.4). The Ry. value of anions obtained in 0 1 M mineral acids (H2SO4 or HCIO4 or HCI):DMSOacetone (I 1:8) are also recoidcd in Table 1. These acids can be put in the following
100 200 300 i.00 500
Amount ( | j g )
18
U
10
6
2
0
- ® -
• ^^ •-"""^
^ ^ ^ ^ 1
^
• ^ • - ^
1 1 1 1
200 400 600 800 1000
Amount C ug )
FIG 4 Plot of spot area vs amount of anion salt loaded (a) KBrO, (b) NaNO,
( HROM \IOCiRAPHY Ol ANIONIC P O I I U T A N I S 47
I \m h 4 Limits ot DeteLlion ind Dilution I iniits of Anions as Ihcir Salts on Silica (jel Ld\trs Impregnated
with 0 I ( nSO, Solution I sing HC l()4 DMSO Acetone (118) as Mobile Phase
Sample
1 • >
^ 4 s
6 7 8 9
10
II
i :
n 14 | s
Dilution limit
MoO
W O ,
( (), 1
\() I'O
1 e(( N)
l e ( ( \ )
l o
HiO
S( \
NO
MnO
( lO
( I O
1 (Vo
Ions Salts
Ni MoO, 2H O Na WO, 2H O Na C O, Kl N iVO H O N I H P O , K,he(( N), k4Fe(C N), 2H O KIO KBrO, NHjSC N NaNO KMnO, k CiO, K Ci O
I (Volume ot lest si)lution ^ l()'')/|l imit ot detection (n,g)|
Limit ot detection
(|JLg)
100 0 100 0 100 0
10 0 10 0 10 0 10 0 10 0
S 0
1 0
1 0
1 0
0 ^
0 s
0 ^
Dilution
limit
1 10
1 10
1 10
1 10
1 10
1 10'
1 10'
1 10
1 2 >
1 10^
1 lO-"
1 K)-*
1 2 A
1 2 X
1 2 >
10
K)-'
K)-*
K)-*
pretericd order it used .is elucnt in combiridtion with DMSO and dtelone FA > HCIO4 HoSO^ HC 1 Results ot quantitative separation ot 10, and NO^ from large excess ot 1 SC N Bi and BiO, and vice veisa are given in Tables 2a and 2h I he proposed method is veiy convenient tor separating milligram quan titles ot an anion trom microgiam to milligram amounts of other anions
In oidei to widen the applieability ot the important separation ot 10, trom 1 NO^ and BiO, its separation trom synthetic mixtures ot ditterent pH values has been invest mated I able ^ leveals that 10, can be easily separated trom I NOT and BiO in the pH langc 2 4-110 ot sample solution Thus the method can be utilized to separate lO, trom acidic, neutral and alkaline (natural or synthetic) samples containing I NO^ and BrO, without adheiing to close control ot sample pH
Table 4 summaiizes the limits ot detection ot some anions as their metal salts along with then dilution limits It is evident trom this table that the proposed method is highlv sensitive toi the detection ot several anions
ACKNOWLEDGMENTS
Piotcssoi K 1 \ isim i hiiiman Depaitmenl ot Applied Chemistry is thanked toi his generous cooper ilion in pun iding the necessiiv lesearch I icilities 1 hanks ire also due to Anand Rawat toi his help
REFERENCES / Choisli)v.ski I 1 Ihiiiinin W O Jawoiski J J Anon Anal V M H / 1981 5 14 2 leres I Moicno DommgiK/ C oncepeion Ci iieia Moieno Abel Marine Lonl AniUwt 198'? 108
SOS
48 MOHAMMAD AND 1 IWARl
i Voivnels M P Kitaeva I P I imefbaev A P Zh Anal Khim 1986 41, 1989 4 ronogcu Y Iwaida M J hood Piot 1981 44, 8 -i •i Aimal M Mohammad A Falima N Khan, A H Muroclum J 1989 39,^61 6 Aimal M Mohammad A Falima N Munxhem J 1988 37,^14 7 Mohammad A Fatima N J Liquid Chromatof>i 1987 1 0 , 1 ^ 9 fi Ajmal M Mohammad A Fatima N Ahmad J J Liquid Chromulof;i 1989 12,^16^ 9 Chawla H M Ralhan N N Garg N K Chibber S S y Hi>>h Riwhit Choimilom (hio
inaloiii C oniiniin 198(1 3, 6'il 10 Kawanbe K Mamyama K Yakugaku 7 1981 101, 192 Chun Ahsu 1982 96 4M2(1K // Buchbauer O Markis R E S< / Phcinn 1983 51,41 12 Ravindia Nath K Janaidhan P B Chcm Ahsti 1982 97, 6'i<i73m /? DenBlevkei K 1 Sweet T R Chiomatof;raplua 1980 13 114 14 •\]mal M Mohammad A Fatima N Ahmad J J Planui Chromaroni 1988 1,239 h Shimi/ii T lanaka H Ohsawa I Chiomalographm 1982 15, 177 /6 Shimi/ii T Vchara F Ohtani M Chiomcitoi>niphia 1986 21, 17"! 17 Mohammad A Fatima N Chiomiitotiit'pltui 1988 25, S36 /.S Ishid.i K Ninomiya S laked.i Y Walanabe K / Chromalogi 1986 35,489 (9 Fa\mv\ N MohammAj A Stp Sii Tttfinoi WU W, 429 20 Gaihakian 1) S Ro/ylo J K JanicRa M J Liquid C hioimiloKi 198S 8 2969 21 Okiimuia T laUiiUa 1979 26, 171 22 Franc I Kosikova F J Chiomalo^l 1980 187, 462 2< Aimal M Mohammad A Fatima N Ahmad J J Plaiiai C hioiniilovi 1990 in press 24 Mohammad A Fatima N Chionuilo^Kiphui 1988 25, 'i36 2^ Mohammad A Fatima N ChionuiloVi'iphia 1987 23, 6* 3 26 Mohammad A Fatima N J I iquid C hioinaloi;i 1986 9, 1903 27 \)md\ M Mohammad A Fatima N Ahmad J J Phinui C hiomaloin 1990 3 '!96 2<S Mohammad A Fatima N Chroinalovniphia 1986 22, 109 29 Sehei A Mikunhim Ami 1961 308
CHROMATOGRAPHIA
An International Journal for Rapid Communication in Chromatography and Associated Techniques
REPRINT
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H Engelhardt Saarbrucken Federal Republic of Germany
L S Ettre Norwalk Conn USA
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R Stock Keyworth United Kingdom
Publisher
F Lube Wiesbaden Federal Republic of Germany
Friedr. Vieweg & Sohn Pergamon Press
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CHROMATOGRAPHIA An International Journal
for Rapid Communication in Chromatography and Associated Techniques
Distributed internationally, Chromatographia provides a medium for the rapid and widespread communication of current information in the field of chromatography. This includes associated techniques and combined methods, as well as the application of computers and modern data systems.
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FR Germany G. Schay, Budapest, Hungary W. Simon, Zurich, Switzerland E. Smolkova-Keulemansova,
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Friedr. Vieweg & Sohn Pergamon Press
Thin-Layer Chromatographic Separation and Identification of Some Anions on Copper Sulphate Impregnated Silica Gel Layers
A. Mohammad*/S Tiwaii
Analytical Laboratory, Department of Applied Chemistry, Zakir Hussain College of Engineering and Technology, Aligarh Muslim University, Ahgarh-202002, India
Key Words Thin layer chromatography Copper sulphate impregnated silica gel Anion separation Acetone elucnts
In the present work, the thin-layer chromatographic behaviour of some common anions on plain and copper sulphate-impregnated silica has been investi gated in mixed aqueous-organic solvent systems con taming acetone
Summary Thin layer chromatographic behaviour of thirteen anions on plain silica gel and sihca gel impregnated with copper sulphate solution has been investigated in aqueous organic solvents containing dcetonc some of which have achieved reliabk and reproducible sepa rations The effect ot copper sulphate concentration on the mobility of anions has been examined I he results obtained on plain silica gel have been com pared with those obtained on copper sulphate impregnated layers 1 he impregnated layers drama tically change the selectivity and permit separations not possible on untreated silica Aqueous sodium chloride acetone (9 I) and ammonium hydroxide ace tone (9 1) were the most effective solvent s>stems for differential migration ol anions Better results in terms of clarity of detection and ccmipactness of spots were found with HCOOII acetone as compared to HCl acetone
The etiect oi anion loading on Rj values has been investigated and identification limits on impregnated layers determined
Experimental
Apparatus A TLC apparatus (Toshniwal, India) was used for the preparation of 20 x 3 5 cm glass plates The chroma tography was performed in 24 x 6 cm glass jars
Reagents
Silica gel (E Merck, India), formic acid, hydrochloric acid, hydrobromic acid, sodium chloride, ammonium hydroxide and acetone (B D H , India) were used These and all other reagents were Analar grade
Test Solutions
The test solutions (1 %) were either sodium oi potassium salts of nitrate, nitrite, vanadate, molybdate phosphate, bromide, iodide, tungstate, ferrocyanide ferncyanide, chromate and dichromate except SCN (ammonium thiocyanate) Water, double distilled from all-glass apparatus and having a specific conductivity K = 2 x \(y^ mhos cm ' at 25 °C was used for solutions
Introduction 1 rom the literature the TLC of anions has been much less extensive compared to th it ot cations |l-3[ Silica gel [4-S] cellulose [9 11], alumina [12] silufol [13] and hydrated stannic oxide layers [14] have been used for the separation and identification ot anions although no work has been reported on the use of silica gel impregnated with inorganic salts
Detect ion
The following reagents were used
1 Saturated solution of AgNO^ in methanol for Br
I , CrO^ , Cr20-, and PO^ The brown spot due to
Br appeared 30 mm after spraying
2 02 % Diphenylamine m 4M H2SO4 for NO, and
( hronidtographia Vol ' O No " s Otlohcr 1990 Orii^inals
0009 189V90/10 ()40s Os $()^,()()() ^ 1990 Priedr Viewe" <t Sohn VerlnPsoesolKt h^fl nihH
40-
3. 10% Ferric chloride in 2M HCl for SCN",
Fe(CN)^andFe(CN)^".
4. 0.5 % Alcoholic pyrogallol solution for MoO?"
and WO4".
5. 1 % Aqueous potassium ferrocynide for VO^;
VOj^ was also detected with this reagent.
Mobile Phases
The following solvent systems were used as mobile phases:
Ml = HCl : Acetone (1:9) M2 = HCl : Acetone (9:1) Ml, =NaCl : Acetone (1:9) M4 =NaCl : Acetone (9:1) Ms = HBr Acetone (1:9) M6 = HBr • Acetone (9.1) M7 = N H 4 0 H : Acetone (1:9) M8 = N H 4 0 H : Acetone (9:1) M9 = Formic Acid : Acetone (1-9) Mio = Formic Acid : Acetone (9:1)
In all the solvent systems, HCl, NaCl, HBr, NH4OH and formic acid were O.IM aqueous solutions while the acetone was pure.
Stationary Phases
Si ~ Plam sihca gel G S2 = Silica gel impregnated with 0.1-5.0 % aqueous
solution of copper sulphate.
Preparation of Thin-Layer Plates
(i) Plain silica gel plates Silica gel was mixed with conductivity water m the ratio 1:3 with constant shaking for 5 to 10 min. The resultant slurry was coated on well-cleaned glass plates to give a layer approximately 0.25 mm thick. The plates were dried at room temperature (30 °C) and then heated at 100 ± 5 °C for 2 hours. After activation the plates were stored in an air-tight chamber.
(/;) Copper sulphate-impregnated silica gel plates To prepare impregnated silica gel layers, a slurry was made by mixing an aqueous solution of 0.1-5.0%, copper sulphate with silica gel in the ratio 3:1. Thin layers were then prepared as described above for plain silica gel plates.
Procedure For qualitative analysis, one or two drops of the anion solutions were spotted on the plates with glass capillaries. The spots were dried and the plates developed by the ascending technique. The ascent of the solvent was fixed at 10 cm in all cases. After development, the plates were dried and the anion spots visualized with the appropriate spray reagent. Rp values of the leading front ( R L ) and of the trailing front ( R T ) were measured and reported as ( R L - R T ) -
Rp values were calculated from Rp = RL + R ,
The limits of detection of the various anions were determined by spotting different amounts using standard solutions, developing the plates, and estimating the spots. This was repeated with successively smaller
amounts of the test substance until spots could no longer be detected. The smallest amount of anion just detectable was taken as the limit of detection.
Results and Discussion The main points which emerge from this study are summarized below:
1. A small change in Rp values was sometimes observed when mixtures of anions were developed as compared with single substances.
2. The development time for a 10 cm run ranged between 45-70 min depending upon the mobile phase.
3. Silica gel impregnated with CUSO4 gave excellent results. Thin layers were of good quality. Generally, the spots were compact and well formed in all solvent systems at 0.1-1 % impregnation. Plates impregnated with 2-5 % copper sulphate solution deformed during development.
4. Rp values reported in this paper represent the averages of triplicate tests and were measured to the centre of the spots on the plates.
5. Sodium chloride-acetone (1:9 and 9:1), NH4OH-acetone (1:9 and 9:1) and HCl-acetone (1:9) systems were found most suitable for separations. A few anions showed occasional tailing. HCl-acetone (1:9) was found to be the best solvent system for multicomponent separation with 1 % copper sulphate impregnation. Formic acid-acetone (1:9) produced highly compact spots of anions on 0.1 % copper sulphate layers.
6. The copper sulphate travels with the solvent front upto the middle of the plate in solvents M2, M^ and MiQ. These systems are therefore unsuitable for impregnated layers.
7. Solvents containing 90 % acetone gave better results than those containing 10 % acetone.
8. In all solvent systems, CrO^", CrjO^", Fe(CN)^
and Fe(CN)g produced coloured spots on im
pregnated layers and thus were self detecting.
9 NOj could not be detected on 1 % impregnated
layers while it was clearly detected on plain silica gel as well as on 0.1 % impregnated layers
10. In addition to the other ions, VOj^ was also
chromatographed to assess the possibility of
separating V02^ from VO3.
The results have been summarized in Figures 1-3 and Tables I and II. Figure 1 summarizes the results of ARp values (ARp = Rp on plain silica - Rp on impregnated silica) with various mobile phases It is evident from Figure 1 that impregnated layers are more selective (strongly sorbing) than plain silica for most of the anions, as indicated by positive ARp values. There was no significant difference m the mobility of anions when chromatographed on silica impregnated with 1 % or 0.1 % copper sulphate using HCl, HBr, NaCl or formic acid-acetone (1:9) solvent systems (e.g. la) . With formic acid-acetone, NO^ showed increased mobihty on 1 % impregnated layers
406 Chronidtogrdphid Vol 30, No 7/cS October 1990 Originals
Table I. Some experimental separations
Stationary phase Mobile phase Separation achieved ( R L - R I )
Silica Gel impregnated with 1 % CUSO4 solution
HCl Acetone 19
Silica Gel impregnated Formic Acetone with 0 1 % CUSO4 solution dcid
19
Silica Gel impregnated with 1 % CUSO4 solution
HCl Acetone 19
Fe(CN)6 (0 0-0 0)-NO2 (0 38-0 21) - SCN" (0 97-0 78)
Cr04 {00-00)-NO2 (0 43-0 23) - Br" (0 70-0 54)
PO4 (00-00) NO2 (0 50-0 23) r (10-0 85)
M0O4 (00-00) VO, (0 31-O26)-SCN-(10-0 9)
Fe(CN)6 (0 0-0 0)-NO2 (0 62-0 56) - NO3 (0 92-0 83)
CrjOT (0 24-00)-NO2 (0 80-0 60) - NO3 (0 97-088)
POf (00-0 0)-NO2 (0 68-0 4 9 ) - r (10-0 95)
WOi (00-00)-NO2 (0 67-058)-Br-(0 9-075)
Fe(CN)i (0 0-0 0) - NO2 (0 53-0 39) - Br~ (0 76-0 64) - SCN" (1 0-0 87)
Fe(CN)6 (0 0-0 0)-NO2 (0 56-0 4) Br" (0 74-0 63) - SCN (10-0 88)
Cr04 (OO-OO) NO2 (0 50-0 35) - Br-(072-0 59)-SCN'(10-0 85)
CrjO? (0 0-00)~NO2 (0 49-0 35) - Br" (0 75-0 59) - SCN (10-0 87)
PO4 (00-O0)-NO2 (0 56-0 41)-Br (0 72-0 65) SCN-(10-0 9)
v o l (00-0 0)-N02 (0 49-0 35)-Br (0 70-0 65)-SCN-(1 0-086)
M0O4 (00-00)-NO2 (0 6-0 5) - Br" (0 75-0 62) - SCN (10-0 9)
Amount of I and Br in mixture three to Inc lold m excess for sharp detection
Table II. Limit of detection and dilution limit ol anions and VO2 on silica gel impregnated with 0 1 % CUSO4 with formic acid acetone (1 9) mobile phase
2+
SI No
1
2
3
4
5
6
7
8
9
10
11
12
13
14
Ions
Br-
PO4
r vof VO3
NO3
NO2
SCN-
Fe(CN),'
Fc(CN)6^
Cr04
CrjO?
M0O4
wo|
* Dilution limit
= 1
Salts
KBr
Na2HP04
Kl
VO2SO4
NaVO-i Fl20
NdNO^
NaN02
NH4SCN
K4Fe(CN)6 ^H20
K3Fe(CN)(,
K2Cr04
K2Cr207
Nd2Mo04 2H2O
Nd2Vv'04 2HiO
Volume ol test solution (ml) x lo''
Limit ol detection (|ig)
I unit ol detection
(Hg) KXK)
10 0
10 0
10 0
10
10
10
10
10
0 5
0 5
OS
01
01
Dilution limit*
1 1()2
1 103
1 lO-''
1 10-
1 104
1 11)4
1 10*
1 10^
1 Uf
1 2x10"*
1 2x10-*
1 2xU)4
1 103
1 10-''
(ARp = -0.3) compared to its mobility on plain silica or silica impregnated with 0 1 % CUSO4 (ARp = +0.1). The reverse trend was observed for I which moves faster on plain sihca (ARp = 0 24) compared to ) % layers However, 0 1 % CUSO4 impregnation was
found to be ineffective in changing the mobility of 1" which behaved similarly in NH40H-acetone (1 9) where it moves faster on plain silica (Figure Ic) compared to 1 % CUSO4 layers. Sodium chloride acetone (9.1) and NH40H-acetone (9:1) systems were found the most effective in changing the mobility ol most anions on impregnated layers and thus open numerous possibilities for separations (Figures lb and d). However, the tailed spots produced by some anions limit their separation from other anions With NH40H-acetone (9:1), most of the anions were strongly adsorbed on 1 % layers compared to plain or 0.1 % layers.
Figure 2 summarizes the hRp values of anions chromatographed on sihca gel impregnated with 1 % CUSO4 and developed with solvents Mi, M-;, M4, Ms, M7, Mg and M9. It is evident that the different mobile phases are able to bring about different retention sequences of anions leading to several binary, ternarv and quaternary separations. The mid Rp (Rp = 0 4 -0 6) values of NOj in Ml and Br" in Mi, M7 and M<s can be used for their separations form all other anions with higher or lower RF values. VO^" , PO] Mo04^, CrjO^^, Fe(CN)^, Fe(CN)^^ and W o j a r e strongly adsorbed on the impregnated layers (hRp -0-10) in all solvent systems containing 90% acetone (Figure 2). The mobility of a few anions is increased when the concentration of sodium chloride or NH4OH IS increased in the mobile phase (M4 and Ms). However, C r O ^ ' a n d Cr20.y~ showed tailing Likewise, M4 and Mg can be utilized for the se paration ofMo04~(hRp = 90-95) from the anions with low Rp values. SCN", I", Br^ and N 0 2 g a \ e higher RF values m most of the mobile phases and thus can be separated from anions with lower R[ values.
Chronidtographid Vol 30, No 7/(S Oclohcr 1990 Originals 40'
1 0
0.8
0 5
a:
<i 0 2
0 0
- 0 2
- 0 4
H C i : A c e t o n e (1 9 )
a)
r - N a C I . Ace tone ( 1 9 )
I I - N Q C I A c e t o n e ( 9 1
NaCI A c e t o n e ( 1 9 )
100
o 80
I - N H ^ O H A c e t o n e ( 1 9 )
I I - N H 4 O H A c e t o n e O 1 )
Anions
HCI A c e t o n e d 9 )
0
0 4
0 2
0 0
- 0 2
- 0 4
en <
N H ^ O H - A c e t o n e d 9)
- 0 4 I-
o O 2 •^ U S
A n i o n s
NH4OH A c e t o n e O 1)
A n i o n s
Figure 1 ARp (Rp on plain silica gel - Rp on CUSO4 impregnated silica gel layers) vs anions ° 1 % copper sulphate impregnation A 0 1 % copper sulphate impregnation
Figure 2
hRp vs. anions. Stationary phase: 1 % copper sulphate impregnated silica gel. o Compact spots with R L - R T < 0.3 A Tailed spots with RL - RT > 0.3 * Badly tailed spots with RL - RT > 0.4
408 Chromatographia Vol 30, No 7/8. October 1990 Oneinals
1 - N a C l ; A c e t o n e i1 , 9 )
1 1 - N a C I : A c e t o n e ( 9 . 1 )
HCI . A c e l o n e i I - 9
A n i o n s
Figure 3 hRp vs. anions. Stationary phase 0 1 '\> copper sulphate impregnated silica gel. Other details as m Figure 2
In Figure 3, the results obtained on 0.1 % coppci sulphate layers in various solvents have been summarized. A major advantage of this adsorbent is that NOj, which could not be detected on 1 "/o coppci sulphate layers, was very clearly detected on 0.1 ",. layers. Comparison of Figures 2 and 3 show almost identical chromatographic behaviour of the anions on both the adsorbents in HBr-acetone and formic acid acetone. Conversely, most of the anions do not beha\c similarly on both sorbents in NaCl-acetone and NF^OH-acetone. Thus, in addition to the separation of NO^, from numerous anions on 0.1 % layers main other mutual separations of anions can be realized m NaCl-acetone or NH40H-acetone.
The chromatographic systems developed provide numerous possibilities for rapid, reproducible and clean separations of anions from multicotnponent mixtures. Some separations experimentally achieved have been summarized in Table L Table II summarizes the limit of detection and dilution limit of various ions. The proposed method is highly sensitive for most ions except Br^.
Acknowledegement We wish to express our sincere thanks to Prof. K. I. Nasim, Chairman, Department of Applied Chemistry, for providing the necessary research facilities. We also thank Dr. Anand Rawat for his valuable help.
References | 1 | U.A. 'I'h. Brinkman. G. De Vries, R. Kuroda, J. Chromatiitr ,
85,187(1 y?.'?). |2] R. Kuroda, M.P. Volynels, CRC Handbook ol Chroma
tography: Inorganics {M. Qureshi, ed.) Vol I, CRC press. B o o Raton, Fla, 1987.
|3J A. Mohammad, K.G. Varshney, Handbook ol I'hin-l a\er Chromatography («. Fried and J. Sherma, etis), Mare.-I Dekker, Inc., USA (m press).
|4] ./. Benes. Collect. Czech. Chem. Commun.. 44. 1(B4 (1979) l-SJ ./. Benes, Collect. Czech. Chem. Commun., 44. 14(X) (1979; |6| II.M. Chawla, N.N. Ralhan, N.K. Carg, S.S. Chibbcr, J lli <h
Res. Chromatogr./Chromatogr. Commun., 3, 6,S1 (1980). |7| K. Kawanhe, K. Maruyama, Yakugaku Zusshi 1981, 101. 192,
Chem. Abstr., 96,4.5420K, 1982. [S] / Zuanon Nelto, A.I-'.C. Graner, M. lontvihiro, Fcletic Ouini,
9, 1984,4,5; Chem. Abstr., KM, 141201 u, 1986. |9] G. Buchhauer, R.E. MarkLs, Sci. Pharrn., 51, 41 (198.?).
|10] R. Gallego, J.L. Bernal, A. Martinez, Ouim Anal., 31, ,3. !97 \ Chem. Abstr., 1978,88, 1.302267.
|11] R. Gallego, J.L. Bernal, A. Martinez, Ouim Anal., 31, 69, ' ,9/ ; . Chem. Abstr., 18181 la, 1978,
[12| K. Ravindra Nath, P.B. .lanardhan, Chem. Abstr., 97, 6.S,- ' MII, 1982.
|13| J. Franc, F. Koslkova, J. Chromatogr., 187, 462 (1980). [14] K. Sen. il.Ch. Ghosh. J. Liqd. Chromatogr., 3, 71 (1980).
Received: May 22, . f'lO Revised manuscripi received: July 7, I'^'O Accepted: July 18, i9H0 C
Chromatographia Vol 30. No. 7/8, O u o h c r 1990 Originals 40^)
Preparation of Anhydrotrypsin-Immobilized Diol Silica as a Selective Adsorbent for High-Performance Affinity Chromatography of Peptides Containing Arginine or Lysine at Their C-Termini
T. Ohta*/T. Inoue/Y. Fukumoto/S. Takitani Faculty of Pharmaceutical Sciences, Science University of Tokyo, 12 Ichigaya-Funagawara Machi, Shmjuku-Ku, Tokyo 162, Japan
Key Words Column liquid chromatography Affinity chromatography Anhydrotrypsm C-termmal Arg- or Lys-containing peptides Diol silica
Summary Anhydrotrypsm (AHT), a catalytically inert derivative of trypsin in which the active site serine residue was converted to dehydroalanine residue by chemical modification, was immobilized onto diol silica through the activation with tnfluoroethanesulfonyl chloride, and an AHT-diol-silica column was used for high performance affinity chromatography separation of peptides containing arginine or lysine at their C-termini from the others Improved separation in terms of speed was accomplished.
Introduction Anhydrotrypsm (AHT), a catalytically inert derivative of trypsin in which the active site serine residue is converted to dehydroalanine residue by chemical modification, exhibits affinity toward peptides containing arginine or lysine at their C termini [1] Kumazaki et al. [2] reported that immobilized AHT prepared through the activation of agarose with cyanogen bromide was useful for the selective isolation of C terminal peptide fragments from tryptic or chymotryptic digests of proteins. However, several hours are usually required for the separation In addition, immobilization with cyanogen bromide, though employed widely for affinity chromatography, results m formation of charged isourea groups, and coupled hgands tend to leak from the support [3].
High performance affinity chromatography (HPAC) introduced by Ohlson et al [4] has been used for the fast and efficient purification of a number of bio logical molecules In this study, we immobilized AHT onto diol silica, a widely used support in HPAC [5], through the activation with 2,2,2-trifluoroethanesulf onyl chloride (tresyl chloride) that was developed tc overcome the disadvantage arising from the use ol cyanogen bromide [6], and used an AHT-diol-silica column for the HPAC separation of peptides containing arginine or lysine at their C-termini from the others. Improved separation in terms of speed wa' accomplished without reduction in resolution.
Experimental
Materials Tresyl chloride was obtained from Nacalai Tesque (Kyoto, Japan). Bovine pancreas trypsin (type III) and phenylmethanesulfonyl fluoride were from Sigma (St Louis, MO, USA). Peptides were from Peptide Institute (Osaka, Japan), Sigma and Aldnch (Milwaukee, WI, USA). Peptides solution were prepared in water and stored at -20 °C until used.
AHT was prepared by the method of Ishii et al [7] The remaining trypsin activity in the purified AHT was 0.2-0.7 % of the original activity when benzoyl DL-arginine p-nitroanilide was used as a substrate. Ir certain experiments, crude AHT prepared without purification by affinity chromatography [7] was used.
Diol silica was prepared by silanization ol LiChrospher Si 300 (10 (im, E Merck, Darmstadt FRG) with 3-glycidoxypropyltrimethoxysilane undei anhydrous conditions followed by hydrolysis of tht epoxy groups with 0.01 M HCl [8]. In certain experi ments, SEP-PAK diol (Waters Associates. Milford MA, USA) was used as did silica
Deionized water (Millipore RO-Q system) was usee throughout this study
410 Chromatogrdphid Vol 30, No 7/8. October 1990 Oriaiiidls
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Some important papers published during 1989 Characterization of Animal Fats via the GC Pattern of Fame Mixtures Obtained by Transesterification of the Triglycerides L Matter/D Schenker/H Husmann/G Schomburg
Evaluation of Non-Polar Bonded-Phases for the Clean-up of Maize Extracts prior to Aflatoxin Assay by HPTLC K I Tomiins/K Jewers/R 0 Coker
New Approach to the GC-Separation of Hydrocarbons by Using LC-like Microcolumns T Takeuchi/K Ohta/D Ishii
Size Exclusion Chromatography on Porous Fractals F Brochard/A Ghazi/M LeMaire/M Martin
Plananty Recognition of Large Polycyclic Aromatic Hydrocarbons by Various Octadecylsilica Stationary Phases in Non-Aqueous Reversed-Phase Liquid Chromatography K Jinno/S Shimura/N Tanaka/K Kimata/ J C Fetzer/W R Biggs
Preparative HPLC of Carotenoids M Isaksen/G W Francis
Applications of HPLC with Evaporative Light Scattering Detection in Fat and Carbohydrate Chemistry A Bruns/H Waldhoff/W Winkle
Synthesis and Characterization of Novel Bonded Phases for Reversed-Phase Liquid Chromatography A M Stalcup/D E Martire/L C Sander/S A Wise
Determination of Alternaria Mycotoxins in Foodstuffs by Gradient Elution Liquid Chromatography with Electrochemical Detection F Palmisano / P G Zambonin/A Visconti/ A Bottalico
Polymer Encapsulated Stationary Phases Advantages, Properties and Selectivities H Engelhardt/H Low/W Eberhardt/M MauB
A Chemically Bonded Liquid Crystal as a Stationary Phase for High Performance Liquid Chromatography Synthesis on Silica via an Organochlorosilane Pathway J Pesek/Teresa Cash
Hydrodynamic Chromatography of Macromolecules on 2 urn Non-Porous Spherical Silica Gel Packings J C Kraak/R Oostervink/H Poppe/U Esser/ K K Unger
Applications of Electrosorptive Detection in Ion Chromatography T Ramstad
The Strength of Interaction of Highly Retentive Silanols with Hydrocarbons on Porasil C J Nawrocki
Uncertainty Resulting from Inconstancy in the Slope of the Plot of Homologous Series S J Hawkes
Derivatization of Carboxylic Acids with 9-Bromo-methylacridme Using Micellar Phase-Transfer Catalysis F A L van der Horst/M H Post/J J M Holthuis/ U A Th Brinkman
Application of Diode Array Detectors for Solute Identification in Toxicological Analysis H Engelhardt / Th Konig
Physico-Chemical Modelling of Solute Retention in Reversed-Phase HPLC with Ternary Mobile Phases Teresa Kowalska
lon-Pair Chromatogrphy with Divalent Counter Cations in Reversed-Phase Systems C Pettersson/G Schill
Isolation and Quantitative Analysis of Hydroxylysine Glycosides R M Napoli/B S Middleditch / N M Cintron/ Y-M Chen
Optical Resolution HPLC Column Packings Carrying Penicillin Sulfoxide Nucleus Y Saotome/T Miyazawa/T Endo
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