Chemistry Chapter 8 Salts

7/26/2019 Chemistry Chapter 8 Salts

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ChemistryChapter 8 : saltsSPM Form 4 Chemistry Chapter 8 Salts

1. Understanding salts2. Solubility of Salts3. Preparing Salts

a. Preparing Soluble Saltsi. Preparing Salts of Potassium, Sodium and Ammoniumii. Preparing Salts of Non-"Potassium, Sodium and Ammonium"

2. Preparing Insoluble Salts2. ualitati!e Analysis1. olour of Ions

2. #eating $ffe%ti. #eating $ffe%t on arbonate Salts

ii. #eating $ffe%t on Nitrate Saltsiii. #eating $ffe%t on Sulp&ate Salts

i!. #eating $ffe%t on &loride Salts2. Identifying 'ases

3. Identifying Anionsi. arbonate

ii. Sulp&ateiii. &loridei!. Nitrate2. Identifying ations

i. (est )it& Sodium #ydro*ide and Ammonium Solutionii. (est )it& &loride Ionsiii. (est )it& Sulp&ate Ions

i!. (est )it& arbonate Ions!. Iodide Solution

!i. (ests to +istinguis& IronII and IronIII ions.2. ind ap
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Understanding Salts

1. A salt is an ioni% %ompound formed )&en t&e &ydrogen of an a%id is partly or %ompletely

repla%ed by a metal ion or ammonium ion.

2. All salts are %&emi%ally and ele%tri%ally neutral.

Example

+iagram abo!e s&o)s t&at )&en t&e &ydrogen ion in nitri% a%id is repla%ed by Na/, a2/, N#0/orAl3/ions, salts are formed.

Example

State )&et&er t&e follo)ing %&emi%al are salt or not salt..

i. barium nitrate

ii. in% sulp&ate

iii. aluminium o*ide

i!. %arbon dio*ide

!. tin nitrate

!i. glu%ose


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!ii. et&anol

Answer

4arium nitrate, in% sulp&ate and tin nitrate are salts.

Aluminium o*ide, %arbon dio*ide, glu%ose and et&anol are not salts.

(&ere are 0 types of salt t&at you need to 5no) in t&e SP syllabus

6our type of Salt, t&ere are

1. Nitrate,

2. &loride,

3. Sulp&ate,

0. arbonate,

Solubility 7f Salts

1. Solubility is t&e ability of a %ompound to dissol!e in a sol!ent.

2. (able belo) s&o)s t&e solubility of t&e salts of nitrate, sulp&ate, %&loride and %arbonate.

Salt Solubility

Salt of potassium, sodium

and ammonium

All solublein water

Salt of nitrate All solublein water

Salt of sulphate Mostly solublein water except:

(Pb) Lead sulphate

(Ba) arium sulphate

(Ca) Calcium sulphate

Salt of chloride Mostly solublein water except:


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(Pb) Lead chloride

(A!) sil"er chloride

(H!) mercury chloride

Salt of carbonate Mostly insolublein water except:

#otassium carbonateSodium carbonate

Ammonium carbonate

Notes

8ead &alide su%& as leadII %&loride Pbl2, leadII bromide Pb4r2 and lead II iodide

PbI2 are insoluble in %old )ater but soluble in &ot )ater.

Solubility of o*ide and &ydro*ideOxide and Hydroxide Solubility

Oxide Mostly insoluble in water except: $%& and 'a%&

Hydroxide Mostly insoluble in water except: $& and 'a&

Preparing Soluble Salts

1. (&ere are 2 t&ings to be %onsidered )&en preparing a salt

a. 9&at are t&e %&emi%al used:

b. #o) to separate t&e salt from ot&er substan%e:

2. et&od used to prepare salt depends on t&e solubility of t&e salt.

3. Soluble salts are prepared from t&e rea%tions bet)een an a%id )it& a metal; base; metal

%arbonate.

0. +iagram belo) s&o)s t&e %&emi%al rea%tion t&at %an be used to prepare t&e soluble salts.


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Example

9rite %&emi%al e


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%. Potassium sulp&ate

7# / #2S70@ 2S70/ #27

d. =in% Sulp&ate 3 e


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Steps to Prepare t&e Salts of Potassium, Sodium and

Ammonium t&roug& (itration

Step 1 Titration to Find the End Point

1. (&e end point is t&e point in a titration at )&i%& t&e 2 rea%tants &a!e %ompletely rea%ted.

2. An endpoint is often mar5ed by a %olor %&ange.


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Step 2 Titrate Without Indicator

1. (&e produ%t obtain in step 1 is %ontaminate by t&e indi%ator.

2. (&e rea%tion is repeated by using t&e same amount of rea%tants as in step 1, )it&out

using any indi%ator.


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Step 3 Crystalisation


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Step 4 Filtration and Drying


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Preparing Salts 7f Non-"Potassium, Sodium And Ammonium"

1. (&e salt non-potassium, sodium and ammonium is prepared by rea%ting a%id )it&

insoluble metal;metal o*ide;metal %arbonate

a. A%id / etal Salt / #ydrogen +ispla%ement rea%tion

b. A%id / etal o*ide Salt / 9ater Neutralisation Bea%tion

%. A%id / etal %arbonate Salt / 9ater / arbon +io*ide

2. 4elo) is t&e steps in preparing t&e soluble non-potassium, sodium and ammonium salts.

Step 1 The eaction

Add metal;metal o*ide;metal %arbonate po)der until e*%ess into a fi*ed !olume of t&e &eateda%id


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Step 2 Filtration 1 to e!o"e E#cess

eactant

6ilter t&e mi*ture to remo!e e*%ess metal;metal o*ide;metal %arbonate


1. $!aporate t&e filtrate until it be%omes a saturated solution

2. +ip in a glass rod, if %rystals are formed, t&e solution is saturated.


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Step 4 Filtration 2 to Collect the Solid Salt

1. ooled at room temperature

2. 6ilter and dry t&e salt %rystals by pressing t&em bet)een filter papers.

Preparing Insoluble Salts

1. Insoluble salts %an be made by ioni% pre%ipitation is also %alled double

de%omposition;double displa%ement.

2. (&is in!ol!es mi*ing a solution t&at %ontains its positi!e ions )it& anot&er solution t&at

%ontains its negati!e ions.

Example

9rite t&e e


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Answer

a. al%ium sulp&ate

al2/ NaS70@ aS70/ 2Nal

aN732/ =nS70@ aS70/ =nN732

b. 8ead %&loride

PbN732/ 2Nal @ Pbl2/ 2NaN73

%. opper %arbonate

uS70/ Na273@ u73/ Na2S70

ul2/ 273@ u73/ 2l

uN732/ Na273@ u73/ 2NaN73

ualitati!e Analysis

Identifi%ation of Ions(&ere are 1C %ations and 0 anions to be studied in our syllabus

Cation

Sodium 'a* +ron (++) e%*

Calcium Ca%* +ron (+++) e-*

Ma!nesium M!%* Lead(++) #b%*

Aluminium Al-* Copper (++) Cu%*

.inc .n%* Ammonium '/*

Anion


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Chloride ion Cl0

sulphate ion S&/%0

nitrate ion '&-0

carbonate ion C&-0

Steps in


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Salt of opperII.-

opperII arbonate

opperII sulp&ate, opperII nitrate, opperII %&loride

opperII o*ide

Salt of Iron II

IronII sulp&ateD IronII nitrateD IronI+ %&loride

Salt of Iron III

IronIII sulp&ateD IronIII nitrateD IronIII %&loride

=in5 o*ide

8eadII o*ide-

agnesium o*ide, Aluminium o*ide

Potassium o*ide, Sodium o*ide, al%ium o*ide

Iron II ion

#eating $ffe%t 7n arbonate Salts

1. All %arbonates salts e*%ept potassium %arbonate and sodium %arbonate %an be

de%omposed by &eat to produ%e %arbon dio*ide gas.

2. (able belo) s&o)s t&e effe%t of &eating on metal %arbonate.


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Carbonate Salt Equation of The Reaction

Potassium carbonate

Sodium carbonate

Will not decompose by heat

Calcium carbonate

Magnesium carbonateAluminium carbonate

Zinc carbonate

Iron (III) carbonate

Lead(II) carbonateCopper(II) carbonate

Calcium carbonate

CaCO! CaO " CO#Aluminium carbonate

Al#(CO)! Al#O" CO#Copper carbonate

CuCO! CuO " CO#

Mercury(II) carbonate

Sil$er carbonate

Aurum(II) carbonate

Sil$er carbonate

#Ag#CO! #Ag " #CO#" O#

Ammonium carbonate (%&')#CO! #%&" #CO#" O

#eating $ffe%t 7n Nitrate Salts

1. All nitrates salts de%ompose )&en &eated.

2. (able belo) s&o)s t&e produ%ts formed )&en different nitrate salts are &eated.

Nitrate Salt Equation of he !ea"tion

Ammonium nitrate Ammonium nitrate de%ompose to nitrogen mono*ide and )ater !apour

)&en &eated.

N#0N73@ N27 / 2#27

Potassium nitrate

Sodium nitrate

Potassium nitrate

2N73@ 2N72/ 72

Sodium nitrate

2NaN73@ 2NaN72/ 72

al%ium nitrate

agnesium nitrate

agnesium nitrate

2gN732@ 2g7 / 0N72/ 72


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Aluminium nitrate

=in5 nitrate

Iron III nitrate

8eadII nitrate

opperII nitrate

IronIII nitrate

06eN733@ 26e273/ 12N72/ 372

8eadII nitrate

2PbN732@ 2Pb7 / 0N72/ 72

er%uryII nitrate

Sil!erI nitrate

AurumII nitrate

Sil!er nitrate

2AgN73@ 2Ag / 2N72/ 72

#eating $ffe%t 7n Sulp&ate Salts

1. ost sulp&ate salts do not de%ompose by &eat. 6or instan%e, sodium sulp&ate,

potassium sulp&ate, and %al%ium sulp&ate are not de%omposable by &eat.

2. 7nly %ertain sulp&ate salts are de%omposed by &eat )&en &eated strongly.

3. 6or instan%e

a. Strong &eating of green %rystal iron II sulp&ate )ill release steam, sulp&ur

dio*ide, sulp&ur trio*ide and lea!e be&ind a reddis& solid iron III o*ide residue.

(&e steam released %omes from t&e &ydrated )ater of t&e %rystallie salt.

26eS70EF#27 @ 6e273p / S72g / S73g / 10#27g

b. ean)&ile, in% sulp&ate, %opper II sulp&ate, and iron III sulp&ate de%ompose

)&en &eated strongly to e!ol!e sulp&ur trio*ide gas and form a metal o*ide.

Example


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=in% sulp&ate

=nS70@ =n7 / S73

opper II sulp&ate

uS70@ u7 / S73

Iron III sulp&ate

6e2S703@ 6e273 / 3SO

%. 9&en ammonium sulp&ate is &eated strongly, t&is )&ite solid sublimate and is

de%omposed to form ammonia gas and sulp&uri% a%id. !apour

N#02S70@ N#3/ #2S70

Preparing Salts 7f Potassium, Sodium And Ammonium

1. Potassium, sodium and ammonium salts are usually prepared t&roug& t&e rea%tions of

a%ids )it& al5alis.

2. Bea%tion a%id )it& al5ali )ill produ%e salt and )ater.

A%id / Al5ali @ Salt / 9ater

3. (&e salt is prepared by titration met&od of a%id and al5ali using an indi%ator.


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Steps to Prepare t&e Salts of Potassium, Sodium and

Ammonium t&roug& (itration

Step 1 Titration to Find the End Point

1. (&e end point is t&e point in a titration at )&i%& t&e 2 rea%tants &a!e %ompletely rea%ted.

2. An endpoint is often mar5ed by a %olor %&ange.


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Step 2 Titrate Without Indicator

1. (&e produ%t obtain in step 1 is %ontaminate by t&e indi%ator.

2. (&e rea%tion is repeated by using t&e same amount of rea%tants as in step 1, )it&out

using any indi%ator.


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Step 4 Filtration and Drying

Identifying 'ases

7*ygen 'lo)ing )ooden splinterA glo)ing )ooden splinter is inserted into t&e test tube t&at %ontain t&e gas.

(&e gas re5indles t&e glo)ing )ooden splinter.

#ydrogen 8ig&ted 9ooden SplinterA lig&ter )ooden splinter is broug&t %lose to t&e mout& of t&e test tube t&at %ontain t&e gas.

A GpopH sound is produ%ed.


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arbon dio*ide 8ime 9ater

(&e gas is dire%ted to flo) t&roug& lime )ater.

(&e lime )ater turn %&al5y.

Sulp&ur +io*ide Potassium +i%&rometeI

(&e gas is dire%ted to flo) t&roug& potassium di%&romateI solution.

(&e orange %olour of potassium di%&romateI solution be%ome green.

&lorine oist 8itmus Paper

oist blue litmus paper is inserted into t&e test tube t&at %ontain t&e gas.

(&e blue litmus paper turn red and t&en )&ite.

Ammonia 'as oist litmus paper

oist red litmus paper is inserted into t&e test tube t&at %ontain t&e gas.

(&e red litmus paper turn blue.

Identifying Anions


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1. In form 0 %&apter F, A%ids and 4ases, you s&ould &a!e learned t&at t&e %arbonate salts

rea%t )it& a%id produ%e %arbon dio*ide and )ater. (&is %&emi%al property of %arbonate is

used to test t&e presen%e of %arbonate in a salt.

732J

/ 2#/

@ #27 / 72

2. +uring t&e test, some dilute &ydro%&lori% a%id ; nitri% a%id ;sulp&uri% a%id is added to

t&e %arbonate salt.

3. If t&e salt %ontain %arbonate, effer!es%en%e o%%urs.

0. If t&e gas gi!en off is passed t&roug& lime )ater, t&e lime )ater )ill turns %&al5y.

>. (&is indi%ates t&at t&e gas is %arbon dio*ide, and &en%e t&e salt %ontain %arbonate.

Identifying Anions - Sulp&ate

1. 9e &a!e learned t&at, all salts of sulp&ate are soluble in )ater, e*%ept leadII sulp&ate,

barium sulp&ate and %al%ium sulp&ate.

2. (&e insolubility of barium sulp&ate is used to test for t&e presen%e of sulp&ate in a salt.

3. 2 %m3 of dilute &ydro%&lori% ; nitri% a%id is added to 2 %m3 of sulp&ate solution. (&is is to

%&e%5 )&et&er %arbonate is presen%e in t&e solution or not be%ause %arbonate may gi!e

t&e same result as sulp&ate.

0. If not effer!es%en%e, t&en 2 %m3 of barium %&loride is added into t&e solution.


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>. If sulp&ate ions are presen%e, a )&ite pre%ipitate )ill form. (&e pre%ipitate is barium

sulp&ate.

?. (&is is a%tually t&e double de%omposition rea%tion t&at you &a!e learned in preparation

of insoluble salt.

4a2// S702J@ 4aS70

Identifying Anions - &loride

1. Kou s&ould &a!e learned t&at, all t&e salts of %&loride are soluble in )ater e*%ept leadII

%&loride, sil!erI %&loride and mer%ury %&loride.

2. (&e insolubility if sil!erI %&loride is used in t&e test of presen%e of %&loride.

3. 2 %mL of dilute nitri% a%id is added to 2 %m3 solution of %&loride ions. (&is is t&e %&e%5 if

%arbonate ions are presen%e be%ause %arbonate ions may gi!e t&e same result.

0. If t&ere is no effer!es%en%e, 2 %mL of sil!er nitrate solution is t&en added into t&e mi*ture.

>. A )&ite pre%ipitate )ill form if %&loride is presen%e in t&e salt.

?. (&e pre%ipitate is sil!er %&loride

Ag// lJ@ Agl

Identifying Anions - Nitrate

(est 1Add dilute sodium &ydro*ide and a little aluminium po)der. If a nitrate is present, ammonia gas

is produ%ed. (&e gas %an be identified as it turns moist red litmus paper blue.

(est 2

1. About 2%m3 of dilute sulp&uri% a%id is added into t&e solution t&at )ants to be tested and

t&en follo)ed by 2%m3 iron II sulp&ate solution.

2. A fe) drops of %on%entrated sulp&uri% a%id are %arefully drop t&roug& t&e in%lined side of

t&e test tube )it&out s&a5ing t&e test tube.

3. A bro)n ring )ill form in t&e middle of t&e solution.


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0. $*planation Iron II sulp&ate redu%e nitri% a%id from t&e rea%tion bet)een nitrate ion

and %on%entrated sulp&uri% a%id to nitrogen mono*ide. After)ards, nitrogen mono*ide

%ombines )it& iron II sulp&ate to form t&e %ompound 6eS70.N7 )&i%& is bro)n in %olour

bro)n ring.

Identifying ations - (est 9it& Sodium #ydro*ide And

Ammonia Solution

1. ations %an be identified by t&eir rea%tion )it& a


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Ca*) 9&ite pre%ipitate. -

M+*) 9&ite pre%ipitate. 9&ite pre%ipitate.

Al()

9&ite pre%ipitate.

,issol-e in ex"ess Na#$

solution.

9&ite pre%ipitate.

/n*)

9&ite pre%ipitate.


solution.

9&ite pre%ipitate.

,issol-e in ex"ess N$(solution.

P0*)

9&ite pre%ipitate.


solution.

9&ite pre%ipitate.

Fe*) +irty green pre%ipitate. +irty green pre%ipitate.

Fe() Bed bro)n pre%ipitate. Bed bro)n pre%ipitate.

Cu*) 4lue pre%ipitate.

4lue pre%ipitate.

,issol-e in ex"ess N$(solution and form a

solution.

N$4)

- -

Identifying ations - (est 9it& &loride Ions

1. 7ut of t&e 1C %ations, only leadII ions )ill form a pre%ipitate )it& %&loride ions.

2. (&is is be%ause leadII %&loride is insoluble in )ater.

3. (&e %&emi%al rea%tion is a double de%omposition rea%tion.

Pb2// 2l-@ Pbl2

0. 8eadII %&loride )ill dissol!e in &ot )ater.

HCl or NaCl

Na+

Ca2+


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Mg2+

Al3+

Zn2+

Pb2+White precipitate

*issol$e in hot +aterFe2+

Fe3+

Cu2+

NH+

Identifying ations - (est 9it& Sulp&ate Ions

1. 7ut of t&e 1C %ations, only %al%ium ions and leadII ions )ill form a pre%ipitate )it&

sulp&ate ions.

2. (&is is be%ause bot& %al%ium sulp&ate and leadII sulp&ate are insoluble in )ater.

3. (&e %&emi%al rea%tion is a double de%omposition rea%tion.

Pb2// S702- @ PbS70

a2// S702- @ aS70

$*S#4or Na*S#4

Na) -

Ca*) 9&ite pre%ipitate.

M+*) -

Al() -

/n*) -

P0*) 9&ite pre%ipitate.

Fe*) -

Fe() -

Cu*) -

N$4) -

Identifying ations - (est 9it& arbonate Ions


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1. All ions, e*%ept sodium ions and ammonium ions )ill form pre%ipitate )it& %arbonate.

2. (&is is be%ause sodium %arbonate and ammonium %arbonate are soluble in )ater.

Na*C#(

Na) -

Ca*) 9&ite pre%ipitate.

M+*) 9&ite pre%ipitate.

Al() 9&ite pre%ipitate.

/n*) 9&ite pre%ipitate.

P0*)

9&ite pre%ipitate.

Fe*) 'reen pre%ipitate.

Fe() 4ro)n pre%ipitate.

Cu*) 4lue pre%ipitate.

N$4) -

Identifying ations - (est 9it& Iodide Ions

1. Iodide ions )ill form pre%ipitate )it& leadII ions and %opperII ions.

2. #o)e!er, in SP you only need to 5no) t&e rea%tion bet)een leadII ions and iodide

ions.

3. (&e yello) pre%ipitate formed )ill dissol!e in &ot )ater.

Pb2// 2I-@ PbI2

12

Na) -

Ca*) -

M+*) -

Al() -


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/n*) -

P0*) Kello) pre%ipitate. +issol!e in &ot )ater

Fe*) -

Fe() A red bro)n solution formed.

Cu*) 9&ite pre%ipitate form in bro)n solution

N$4) -

Identifying ations - (ests (o +istinguis& IronII And IronIII

Ions.

Some (ests to +istinguis& 6e2/ion 6rom 6e3/Ion1. (&e presen%e of 6e2/ion and 6e3/ion in a salt %an be %onfirmed by using solution of

potassium &e*a%yanoferrate II, solution of potassium &e*a%yanoferrate III and

potassium t&io%yanate.

2. (able belo) s&o)s t&e obser!ation of t&e tests.

!ea+ent #0ser-ation 2on presents

Solution of potassium

&e*a%yanoferrate II

8ig&t blue pre%ipitate 6e2/

+ar5 4lue pre%ipitate 6e3/

Solution of potassium

&e*a%yanoferrate III

+ar5 blue pre%ipitate 6e2/

'reenis& bro)n solution 6e3/

Potassium t&io%yanate Pin5is& solution 6e2/

4lood red solution 6e3/


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Chemistry Chapter 8 Salts