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I. TITLE : a. Neutralization Titration
“Titration between NaOH solution 0,1N with oxalic acid as standar solution”
b. Aplication of Neutralization Titration
“Determining percent content of H2SO4 in accu zuur”
II. DATE : 22th November 2011, start at : 07:30 am-11:30 am
III. PURPOSE : a. Making and determining standardization of base solution.
b. Determining percent content of H2SO4 in Accu Zuur (Yuasa Merck).
IV. THEORY :
V. TOOLS AND MATERIALS
a. Burette
b. Conical Flask (Erlenmeyer)
c. Measuring Cylinder
d. Volumetric Flask
e. Volumetric pipette
f. Pro pipette
g. Beaker Glass
h. Pipette
i. Funnel
j. Analyst Balance
k. Picnometer
l. Spatula
m. Filter paper
n. Pipette
o. Aquadest
p. NaOH
q. Accu Zuur
r. Oxalic Acid
s. Methyl Orange Indicator
t. Phenolftalein Indicator
H2C2O4.2H2O 0, 6000 grams
taking place in volumetric flask 100 mLdissolving by aquadest until limitation markmixed well
Oxalate acid as standard solution
taking 10 mL of that solution using volumetric pipette (pour into Erlenmeyer 100 mL)pouring by aquadest 25 mL using graduated cylinderpouring by 3 drops of PP indicator
Oxalate acid as standard solution
titrate with NaOH solution until color of indicator is changedone 3 times repetationwritting down the scale of NaOH in the burrette in initial and final titrationcalculate the average concentration of NaOH
2NaOH + H2C2O4 Na2C2O4 + 2H2O
J
VI. PROCEDURE
Standarization of NaOH solution ± 0,1 N with oxalate acid as a standard solution
Accu Zuur
Pouring 2 ml in piknometer with volumetric pipetteClose the piknometer immediately Weight the piknometerDissolving with aquades in volumetric flask 100 mlKeeping it well until become cold
Weight the empty piknometer firstWriting the mass
Accu Zuur solution
Taking 10 ml into ErlenmeyerAdding several drops of methyl orange indicator
Accu Zuur solution + indicator
Titrate with NaOH 0,1 NRepeating until 3 timesCalculate the amount of H2SO4
Result
Determining Percentage of H2SO4 in Accu Zuur
VII.DATA
a. Titration of NaOH with Oxalic Acid
NoBurette Scale V NaOH
N NaOH (N) Titrator NoteBefore After (ml)
1
0
9,2
9,2
0,1034 Miftahul Izzati Laili
Using Burette
with accuracy ±0,05 mL
2 9,2 18,7 9,5 0,1002 Ninik Nigusti Ayu S.3 18,7 27,7 9 0,1057 Fitria Dwi Lestari
Naverage=0,1034+0,1002+0,1057
3
Naverage=0,1031Reaction: H2C2O4.2H2O(aq) + NaOH(aq)Na2C2O4(aq) + 4H2O(l)
b. Application of Acidy-Alkalimetry Titration
NoBurette Scale V NaOH
N NaOH (N) Titrator NoteBefore After (ml)
1
0
15
15
0,1546
Fitria Dwi Lestari
Using Burette
with accuracy ±0,05 mL
2 15 30,3 15,3 0,1577 Miftahul Izzati Laili3 30,3 45,3 15 0,1546 Ninik Nigusti Ayu S.
Naverage=0,1546+0,1577+0,1546
3
Naverage=0,1556Reaction:
H2SO4(aq) + NaOH(aq) Na2SO4(aq) + 2H2O(l)
VIII. ANALYSIS
Standardization of NaOH using oxalic acid
In the standardization of solution required a known concentration solution first. Solution
of known concentration is called standard solution. In the standardization of NaOH solution
required oxalic acid as standard solution. The first step is manufacture of standard solution of
H2C2O4 , we get 0.6000 g of H2C2O4 and then diluted in 100 mL of aquadest in volumetric flask,
this substance is soluble because of the polar.
The reaction is:
H2C2O4. 2H2O (s) + H2O (l) H2C2O4 (aq)
After making standard solution, this solution is taken 10 mL using volumetric pipette because
volumetric pipette has high standard accuracy and then it is poured in conical flask 100 mL and
added with 25 mL of aquadest and 3 drops of PP indicator. This solution is filtrated using NaOH
which have been put in burette until 0 scale. The purpose of addition indicator is to accelerate the
reaction during titration to achieve the end point that is marked by changing of color from
colorless to pink. The reaction that occur is :
H2C2O4 (aq) + NaOH (aq) 2H2O (l) + Na2C2O4(aq)
This titration is done 3 times and the volume of NaOH which is needed are 9.2 ml, 9.5 ml, and
9.0 ml.
In this volume, titration is stopped because it had reached end point of titration, from this
titration we can determine concentration of NaOH. From the calculation, we get the average
value of normality is 0,1031 N. we get this value from :
a. V NaOH x N NaOH = V C2H2O4.2H2O x N C2H2O4.2H2O0,0092 L x N NaOH = 0,01 L x 0,0952 NN NaOH = 0,1034 N
b. V NaOH x N NaOH = V C2H2O4.2H2O x N C2H2O4.2H2O0,0095 L x N NaOH = 0,01 L x 0,0952 NN NaOH = 0,1002 N
c. V NaOH x N NaOH = V C2H2O4.2H2O x N C2H2O4.2H2O0,0090 L x N NaOH = 0,01 L x 0,0952 NN NaOH = 0,1057 N
N average = 0,1034 N+0,1002 N+0,1057 N
3 = 0,1031 N
Reaction :
C2H2O4.2H2O (aq) + NaOH (aq) Na2C2O4 (aq) + 4H2O (l)
Determining percent content of H2SO4 in accu zuur
In this experiment, we have to determine the density of accu zuur first using piknometer. In the piknometer, already labeled the volume 25 ml. we need to know the mass of solution by weight the empty picnometer first and then weight the picnometer which had been filled with the accu zuur and calculate the mass. We can calculate the density directly from this formula :
ρ=mv
The density that we got, can be use to calculate the percentage of H2SO4 in accu zuurafter this titration done well. We use “Yuasa Accu Zuur” that had been titrated with NaOH which the concentration is known from the first experiment and methyl orange as indicator. Our data experiment show the volume of NaOH that we get sequencely are 15 ml, 15.3 ml and 15 ml. And then we have to determine the concentration of NaOH with the calculation below :
a.M eq H2SO4 = M eq NaOH
N H2SO4 = 0,1546 M eqml
= 0,1546 x 2 mmol= 0,3092 mmol
mmol = mgMr
0,3092 = x
49x = 15,1508 mg
in 100 ml solution
x = 15,1508 mg x 100= 1515,08 mg
= 1,51508 gram
Percentage H2SO4 = 1,515082,5614 x 100% = 59,15 %
b. N H2SO4 = 0,1577 M eqml
= 0,1577 x 2= 0,3154 mmol
mmol = mgMr
0,3154 = x
49x = 15,5446 mg
in 100 ml solution
x = 15,5446 mg x 100= 1554,46 mg= 1,55446 gram
Percentage H2SO4 = 1,554462,5614 x 100% = 60,34 %
c. N H2SO4 = 0,1557 M eqml
= 0,1557 x 2 mmol= 0,3114 mmol
mmol = mgMr
0,3114 = x
49x = 15,5286 mg
in 100 ml solution
x = 15,5286 mg x 100= 1552,86 mg= 1,55286 gram
Percentage H2SO4 = 1,552862,5614 x 100% = 59,57 %
% average =59,15 %+60,34 %+59,57 %
3
= 179,06 %
3 = 59,69 %
Thus, the percentage value of H2SO4 in accu zuur is 59,69 %
IX. DISCUSSION
a. Standardization of NaOH using oxalic acid as standard solution
when we did this experiment, we did not face any difficulties. We just have a little in determine the color changing of the analyte that the titrator can finish the titration. It is influence to the volume of NaOH that we need in this experiment for each repetation. So, we have to be more careful when read the burette scale and don’t forget to drop the indicator a moment before do the titration. Because it will influence the analyte and can change the result of the data.
b. Determining percent content of H2SO4 in accu zuur
when we do this experiment, we did some mistakes. We drop yhe indicator before the titration. Finally we repeat the procedure by make the solution again. And then we drop the indicator just a moment before we do the titration. When we still doing the titration, we were careless when read the scale of the burette while we can not determine the color changing. Because of our knowledge about pH trayek is poor so we don’t know the end of this titration.
X. CONCLUSION
From the result of experiment can be concluding that:
a. Standardization of NaOH using oxalic acid as standard solution
from the first experiment, we can know the concentration of NaOH, we can
standardize it using standard solution of oxalic acid using titration. Concentration of
oxalic acid is 0,0552 N and the average of NaOH concentration is 0,1031 N
b. Determining percent content of H2SO4 in accu zuur
using titration we can determine the percentage of H2SO4 in accu zuur from experiment we can know that percentage of H2SO4 in Yuasa Accu Zuur is 59,69%. It is gotten from weight percentage analysis :
% H2SO4 = mass of H 2 SO 4mass of sample x 100%
XI. Answer of Question :
1. Why in the manufacture of NaOH solution must use boiled water?
Answer:
In the manufacture of NaOH solution must use boiled water because it is not pure in
solution consisting of NaOH, but also contained Na2CO3 so that boiling water works to
remove CO2 contained in Na2CO3.
2. What is the difference between:
a. Standard primer solution and standard secondary solution?
b. Acidimetric and alkalimetri?
Answer:
a. In analytical chemistry, a standard solution is a solution containing a precisely known
concentration of an element or a substance i.e, a known weight of solute is dissolved to
make a specific volume. It is prepared using a standard substance, such as a primary
standard. Standard solutions are used to determine the concentrations of other
substances, such as solutions in titrations.
The difference between the primary standard solutions with secondary standard
solution are standard primer solution is a solution of known concentration for certain
and is used to determine the concentration of secondary standard solution, secondary
standard solution is a solution whose concentration has been determined accurately
through the standardization process.
b. Acidimetric i.e. involving base neutralization titration with acid of known
concentration.
Alkalimetri i.e. involving titration of neutralizing acid with a base of known
concentration.
3. Give reasons for the use of indicators in the titration of the above!
Answer: The use of indicators in the titration is useful to know when to stop adding
titrant because indicator will change color, and when there are changes
color is called the equivalence point and end point of titration.
XII. Refferences
Poedjiastuti, Sri., dkk. 2009. Panduan Praktikum Kimia Analitik I Dasar-dasar Kimia
Analitik. Surabaya: Jurusan Kimia FMIPA Unesa.
Day, R. A. 1991. Quantitative Analysis Sixth Edition. New Jersey: Prentice Hall.
Attachments :
Standardization of NaOH using oxalic acid as standard solution
Attachments :
Determining percent content of H2SO4 in accu zuur
Accu Zuur after titration
The color changing of accu zuur before titration and after titration