CHEMISTRY PRACTICALS
CLASS XII
SESSION – 2023-24
Designed By
SARWAN KUMAR
PGT CHEMISTRY
KV NO. 1 AJMER
EXPERIMENT ­ 1
AIM - To prepare M/20 solution of Mohr’s salt and, using this solution find out the molarity and
strength of the given potassium permanganate (KMnO4) solution.
THEORY –Mohr’s salt titration with potassium permanganate is also a redox titration. In this
titration, Mohr’s salt acts as a reducing agent and potassium permanganate works as the oxidising
agent.
MOLECULAR EQUATIONS ­
REDUCTION HALF REACTION -
2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5O
OXIDATION HALF REACTION -
(FeSO4(NH4)2SO4.6H2O +H2SO4 +O→ Fe2(SO4)3 + 2(NH4)2SO4 +13H2O) x 5
---------------------------------------------------------------------------OVERALL REACTION2KMnO4+10FeSO4(NH4)2SO4.6H2O+8H2SO4→K2SO4+2MnSO4+5Fe2(SO4)3+10(NH4)2SO4+68H2O
IONIC REACTIONS –
Oxidation half – [Fe2+→Fe3+ + e-]5
Reduction half - MnO4- + 8H+ + 5e- → Mn2++4H2O
Overall equation - MnO4- + 8H++5Fe2+→ Mn2+ + 5Fe3+ + 4H2O
MATERIALS REQUIRED ­
APPARATUS REQUIRED – weighing bottle, weight box, volumetric flask, conical flask, burette,
pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white tile,
burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate solution.
INDICATOR – KmnO4 is a self indicator.
END POINT -- colour change of KMnO4 from colourless to light pink.
PROCEDURE A. Preparation of 250ml of M/20 solution of Mohr’s salt –
1. weigh 4.9g of Mohr’s salt using a chemical balance and watch glass.
2. dissolve weighed Mohr’s salt conc H2SO4 (5 ml) and 100 ml distilled water in a beaker.
Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with
distilled water according to the required volume.
B. Titrating potassium permanganate solution against standard ferrous ammonium sulphate
(Mohr’s salt)
1. Wash the pipette and the burette with distilled water and then rinse burette
with KMnO4 and pipette with Mohr salt solution.
2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand.
3. Take out 20 ml of standard more Mohr salt solution in the conical flask. Add 10ml of sulfuric
acid to prevent the oxidation of manganese to form manganese dioxide.
4. Note the initial reading of the burette before starting that experiment.
5. Now against the potassium permanganate solution start the titration and slowly still the flask
gently.
6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate. The
appearance of the permanent pink colour indicates the endpoint. Repeat the for 3 time unless
Concordant value is obtained.
CALCULATION:
For Mohr salt preparation molarity
Molarity = Given mass x 1000
Molar mass x V
!
"#
X
=
$ & '(((
)*+ & '((
!"# % &
% #'
= &'
= 1.96 g.
Part -A. Molarity of KMnO4
From the balanced ionic equation 1 mole KMnO4 is reacting with 5 mole of mohr’s salt solution.
M KMnO4 x V KMnO4
&
MMohr x V Mohr
= (
MKMnO4 x 20.0 ml
0.05 x 20.0
=
&
(
OBSERVATION TABLE:
The volume of Mohr’s salt solution taken – 20ml. (by Pippette)
Burette Reading
The volume of KMnO4
S.No.
used in ml
Initial
Final
1.
2.
3.
0 ml
0 ml
0 ml
19.9 ml
20.0 ml
20.0 ml
19.9 ml
20.0 ml
20.0 ml
RESULT – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l
MKMnO4 = 0.01 M
Part -B Strength of KMnO4 solution = Molarity x Molar mass = 0.01 x 158u = 1.58 g/l
Result – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l
PRECAUTIONS –
1. Always rinse the burette and pipette before use.
2. Clean all apparatus with distilled water.
3. Use dilute H2SO4 acid in the experiment.
4. Strength of KMnO4 solution should be taken at least 2 decimal.
5. Don’t use a rubber cork burette as it is can be attacked by KMnO4.
Concordant
Value
20.0 ml
EXPERIMENT ­ 2
AIM - To prepare M/30 solution of Mohr’s salt and, using this solution find out the molarity and
strength of the given potassium permanganate (KMnO4) solution.
THEORY –Mohr’s salt titration with potassium permanganate is also a redox titration. In this
titration, Mohr’s salt acts as a reducing agent and potassium permanganate works as the oxidising
agent.
MOLECULAR EQUATIONS ­
REDUCTION HALF REACTION -
2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5O
OXIDATION HALF REACTION -
(FeSO4(NH4)2SO4.6H2O +H2SO4 +O→ Fe2(SO4)3 + 2(NH4)2SO4 +13H2O) x 5
---------------------------------------------------------------------------OVERALL REACTION2KMnO4+10FeSO4(NH4)2SO4.6H2O+8H2SO4→K2SO4+2MnSO4+5Fe2(SO4)3+10(NH4)2SO4+68H2O
IONIC REACTIONS –
Oxidation half – [Fe2+→Fe3+ + e-]5
Reduction half - MnO4- + 8H+ + 5e- → Mn2++4H2O
Overall equation - MnO4- + 8H++5Fe2+→ Mn2+ + 5Fe3+ + 4H2O
MATERIALS REQUIRED ­
APPARATUS REQUIRED – weighing bottle, weight box, volumetric flask, conical flask, burette,
pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white tile,
burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate solution.
INDICATOR – KmnO4 is a self indicator.
END POINT -- colour change of KMnO4 from colourless to light pink.
PROCEDURE A. Preparation of 250ml of M/20 solution of Mohr’s salt –
1. weigh 4.9g of Mohr’s salt using a chemical balance and watch glass.
2. dissolve weighed Mohr’s salt conc H2SO4 (5 ml) and 100 ml distilled water in a beaker.
Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with
distilled water according to the required volume.
B. Titrating potassium permanganate solution against standard ferrous ammonium sulphate
(Mohr’s salt)
1. Wash the pipette and the burette with distilled water and then rinse burette
with KMnO4 and pipette with Mohr salt solution.
2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand.
3. Take out 20 ml of standard more Mohr salt solution in the conical flask. Add 10ml of sulfuric
acid to prevent the oxidation of manganese to form manganese dioxide.
4. Note the initial reading of the burette before starting that experiment.
5. Now against the potassium permanganate solution start the titration and slowly still the flask
gently.
6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate. The
appearance of the permanent pink colour indicates the endpoint. Repeat the for 3 time unless
Concordant value is obtained.
CALCULATION:
For Mohr salt preparation molarity
Molarity = Given mass x 1000
Molar mass x V
!
,#
X
=
$ & '(((
)*+ & '((
!"# % &
% !'
= &'
= 1.3 g.
Part -A. Molarity of KMnO4
From the balanced ionic equation 1 mole KMnO4 is reacting with 5 mole of mohr’s salt solution.
M KMnO4 x V KMnO4
&
MMohr x V Mohr
= (
MKMnO4 x 12.0 ml
0.03 x 20.0
=
&
(
OBSERVATION TABLE:
The volume of Mohr’s salt solution taken – 20ml. (by Pippette)
Burette Reading
The volume of KMnO4
S.No.
used in ml
Initial
Final
1.
2.
3.
0 ml
0 ml
0 ml
11.9 ml
12.0 ml
12.0 ml
11.9 ml
12.0 ml
12.0 ml
RESULT – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l
MKMnO4 = 0.01 M
Part -B Strength of KMnO4 solution = Molarity x Molar mass = 0.01 x 158u = 1.58 g/l
Result – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l
PRECAUTIONS –
1. Always rinse the burette and pipette before use.
2. Clean all apparatus with distilled water.
3. Use dilute H2SO4 acid in the experiment.
4. Strength of KMnO4 solution should be taken at least 2 decimal.
5. Don’t use a rubber cork burette as it is can be attacked by KMnO4.
Concordant
Value
12.0 ml
AIM- To prepare M/50 solution of oxalic acid .Using this solution find out the molarity and
strength of the given potassium permanganate (KMnO4) solution.
EXPERIMENT ­ 3
AIM- To prepare M/50 solution of oxalic acid .Using this solution find out the molarity and
strength of the given potassium permanganate (KMnO4) solution.
THEORY –Oxalic acid titration with potassium permanganate is also a redox titration.
In this titration, Oxalic acid acts as a reducing agent and potassium permanganate
works as the oxidising agent.
MOLECULAR EQUATIONS ­
REDUCTION HALF REACTION 2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5[O]
OXIDATION HALF REACTION (COOH)2.2H2O +[O]→ 2CO2 + 3H2O )x 5
---------------------------------------------------------------------------OVERALL REACTION2KMnO4 + (COOH)2.2H2O + 3H2SO4 → K2SO4 +2MnSO4 + 10CO2 +18H2O
IONIC REACTIONS –
OXIDATION HALF –
[C2O42-→2CO2 + e-]5
REDUCTION HALF MnO4- + 8H++5e- → Mn2++4H2O} X 2
OVERALL EQUATION - 2MnO4-+ 16H+ + 5 C2O42-→ 2 Mn2+ + 10CO2 + 8H2O
MATERIALS REQUIRED ­
Apparatus Required – weighing bottle, weight box, volumetric flask, conical flask, burette,
pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white
tile, burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate
solution.
Indicator – KMnO4 is a self-indicator.
End point - Colour change of KMnO4 from colourless to light pink.
PROCEDURE A. Preparation of 250ml of M/50 solution of Oxalic acid –
1. weigh 0.63g of Oxalic acid using a chemical balance and watch glass.
2. dissolve weighed Oxalic acid in con H2SO4(5 ml) and 100 ml distilled water in a beaker.
Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with
distilled water according to the required volume.
B. Titrating potassium permanganate solution against standard ferrous ammonium
sulphate (Mohr’s salt)
1. Wash the pipette and the burette with distilled water and then rinse burette
with KMnO4 and pipette with Oxalic acid salt solution.
2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand.
3. Take out 20 ml of standard Oxalic acid salt solution in the conical flask. Add 10ml of
sulphuric acid to prevent the oxidation of manganese to form manganese dioxide.
4. Note the initial reading of the burette before starting that experiment.
5. Now against the potassium permanganate solution start the titration and slowly still the flask
gently.
CALCULATION:
part -A. Molarity of KMnO4
From the balanced ionic equation 2 mole KMnO4 is reacting with 5 mole of Oxalic acid salt
solution.
!
MKMnO4 x VKMnO4
="
M Oxalic acid x VOxalic acid
MKMnO4 x 8.0 ml
0.05
x 10.0
=
2
5
MKMnO4 = 2 x 10.0 x 0.05
8.0 x 5
MKMnO4 = 0.025 M
Part -A Strength of KMnO4 solution = Molarity x Molar mass = 0.025 x 158u = 3.95 g/l
Result – Molarity of given KMnO4 solution 0.025 M Strength 3.95 g/l
6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate.
The appearance of the permanent pink colour indicates the endpoint. Repeat for 3 time unless
Concordant value is obtained.
OBSERVATION TABLE:
The volume of Oxalic acid salt solution taken – 10ml. (by Pippette), M
S.N.
.lo9;;
2.
3.
Burette Reading
Initial
Final
0 ml
0 ml
0 ml
7.89 ml
8.00 ml
8.00 ml
The volume of
KMnO4 used in
ml
7.89 ml
8.00 ml
8.00 ml
Concordant
Value
8.00 ml
RESULT – Strength of KMnO4 solution = Molarity x Molar mass = 0.025 x 158u = 3.95 g/l
Molarity of given KMnO4 solution 0.025 M Strength 3.95 g/l
PRECAUTIONS –
1. Always rinse the burette and pipette before use.
2. Clean all apparatus with distilled water.
3. Use dilute H2SO4 acid in the experiment.
4. Strength of KMnO4 solution should be taken at least 2 decimal.
5. Don’t use a rubber cork burette as it is can be attacked by KMnO4.
AIM- IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – A
RESULT – The experimental observation shows the presence of Alcoholic group – OH .
Equations – ( write on white side of paper)
a) C2H5OH + Na → C2H5ONa + ½ H2
b) C2H5OH + (NH4)2Ce (NO3)6→ (C2H5OH)2Ce (NO3)4 + (NH4)2NO3
c) C2H5OH + CH3COOH → CH3COO C2H5 + H2O
EXPERIMENT -04
AIM- IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – A
PART- A - PHYSICAL PROPERTIES
a. Colour - colourless
b. Odour – order of sprit or wine
c. Solubility in Water - soluble in water
d. Solubility in dil HCl – soluble in Dil Hcl
PART- B - CHEMICAL PROPERTIES
S.N.
1.
Experiment
Observation
Inference
Unsaturation test- To the given
KMnO4 get
organic compound add alkaline
decolourised
KMnO4 solution
Test for carboxylic group- Add a
No CO2 evolve
pinch of NaHCO3 to the given sample
Compound is
saturated (-)
3
Litmus Test – Put a drop of sample
on blue litmus and red litmus
No change is
observed
4.
Test for phenol – to the given
sample add 2- 3 ml of Neutral FeCl3
soln
Sodium metal test- drop a piece of
dried sodium in the given sample .
NO VOILET PPT
obtained
Alcoholic or
carboxyl group is
absent
Phenolic group
absent
Ceric ammonium nitrate test- Add
the drops of ceric ammonium nitrate
solution to the given sample
Red PPT
formation
2.
5
6
Evolution
colourless gas
Carboxylic group
absent
of Alcoholic group –
OH confirm
Alcoholic group –
OH confirm
7
Ester test- to the 1 ml of given
Fruity smell
Alcoholic group –
sample add 1 ml acetic acid and few
OH confirm
drops of Con. H2SO4 and heat on
water bath
RESULT – The experimental observation shows the presence of Alcoholic group – OH .
Equations – ( write on white side of paper)
a) C2H5OH + Na → C2H5ONa + ½ H2
b) C2H5OH + (NH4)2Ce (NO3)6→ (C2H5OH)2Ce (NO3)4 + (NH4)2NO3
c) C2H5OH + CH3COOH → CH3COO C2H5 + H2O
AIM -IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – B
EXPERIMENT - 05
RESULT – The experimental observation shows the presence of Phenolic group
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – B
Ar-OH confirmed
PART- A - PHYSICAL PROPERTIES
a. Colour - colourless
b. Odour – order of sprit or wine
c. Solubility in Water - soluble in water
d. Solubility in dil HCl – soluble in Dil Hcl
EQUATIONS – (write on white side of paper)
a) C6H5OH + FeCl3
b)
→ [(C6H5O) 6Fe]3- + 3HCl
PART- B - CHEMICAL PROPERTIES
S.N.
Experiment
1.
2.
3.
4.
5.
Observation
Inference
Unsaturation test- To the given
organic compound add alkaline
KMnO4 solution
Test for carboxylic group- Add a
pinch of NaHCO3 to the given sample
Litmus Test – Put a drop of sample
on blue litmus and red llitmus
KMnO4 get
decolourised
Compound is
saturated (-)
No CO2 evolve
Test for phenol – to the given
sample add 2- 3 ml of Neutral
FeCl3 soln
Azo dye test:-Compound + NaNO2
+ conc. HCl and add aniline
VOILET PPT
obtained
Carboxylic group
absent
Alcoholic or
carboxyl group is
absent
Phenolic group
confirm
No change is
observed
Orange red dye
Phenolic group
confirmed
RESULT – The experimental observation shows the presence of Phenolic group
Ar-OH confirmed
Equations – (write on white side of paper)
a) C6H5OH + FeCl3
b)
→ [(C6H5O) 6Fe]3- + 3HCl
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – C
RESULT – The experimental observation shows the presence of aldehyde group -CHO
confirmed.
EQUATION -
EXPERIMENT - 06
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – C
PART- A - PHYSICAL PROPERTIES
a. Colour - colourless
b. Odour – order of sprit or wine
c. Solubility in Water - soluble in water
d. Solubility in dil HCl – soluble in Dil Hcl
PART- B - CHEMICAL PROPERTIES
S.N.
Experiment
Observation
1.
2.
3
4.
5.
6.
7.
Unsaturation test- To the
given organic compound add
alkaline KMnO4 solution
Litmus Test – Put a drop of
sample on blue litmus and red
llitmus
Test for carboxylic group- Add
a pinch of NaHCO3 to the given
sample
Test for phenol – to the given
sample add 2- 3 ml of Neutral
FeCl3 soln
Test for carbonyl group – Add
1 ml of sample add 2-3 ml of 2,4
DNP (dinitro phenylhydrazine)
Test for aldehyde group: Added
1ml Fehling solution to given
organic compound & heated on
water bath.
Added Tollen’s reagent to
organic compound and warm it
in water bath
KMnO4 get
decolourised
Inference
Compound is
saturated (-)
No change is
observed
Alcoholic or
carboxyl group is
absent
No CO2 evolve Carboxylic group
absent
NO VOILET
PPT obtained
Phenolic group
absent.
Orange yellow Carbonyl group may
ppt formed
be an aldehyde or
ketone.
Red ppt formed -CHO group
confirmed
Silver mirror on -CHO group
inside wall of
confirmed
the test tube
RESULT – The experimental observation shows the presence of aldehyde group -CHO
confirmed.
EQUATION -
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – D
RESULT – The experimental observation shows the presence of ketonic group
> C=O confirmed.
EXPERIMENT - 07
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – D
PART- A - PHYSICAL PROPERTIES
a. Colour - colourless
b. Odour – order of sprit or wine
c. Solubility in Water - soluble in water
d. Solubility in dil HCl – soluble in Dil Hcl
EQUATION -
PART- B - CHEMICAL PROPERTIES
S.N.
Experiment
1.
Observation
Inference
Unsaturation test- To the given
KMnO4 get
Compound is
organic compound add alkaline
decolourised saturated (-)
KMnO4 solution
2.
Test for carboxylic group- Add a
No CO2
Carboxylic group
pinch of NaHCO3 to the given
evolve
absent
sample
3
Litmus Test – Put a drop of sample No change is Alcoholic or carboxyl
on blue litmus and red llitmus
observed
group is absent
4.
Test for phenol – to the given
NO VOILET Phenolic group
sample add 2- 3 ml of Neutral FeCl3 PPT obtained absent.
soln
5.
Test for carbonyl group – Add 1 ml Orange
Carbonyl group may
of sample add 2-3 ml of 2,4 DNP
yellow
ppt be an aldehyde or
(dinitro phenylhydrazine)
formed
ketone.
6.
Test for Ketonic group: Added 1
Red colour
Ketonic group
appeared
confirmed
ml sodium nitroprusside solution
to given organic
Compound & then added NaOH
solution dropwise
7.
Add 1ml finely powdered mViolet
Ketonic group
colour confirmed
dintrobenzene to given organic
appeared
Compound & then added NaOH
soln.
RESULT – The experimental observation shows the presence of ketonic group
> C=O confirmed.
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – E
EXPERIMENT - 08
AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – E
RESULT – The experimental observation shows the presence of Carboxylic group – COOH .
PART- A - PHYSICAL PROPERTIES
Equations:- a)CH3COOH + Na2CO3 → CH3COO Na + H2O +CO2
a. Colour - colourless
b. Odour – order of sprit or wine
c. Solubility in Water - soluble in water
d. Solubility in dil HCl – soluble in Dil Hcl
b) C2H5OH + CH3COOH → CH3COO C2H5 + H2O.
PART- B - CHEMICAL PROPERTIES
S.N.
Experiment
1
2
3
4
Unsaturation test- To the given
organic compound add alkaline
KMnO4 solution
Litmus Test – Put a drop of
sample on blue litmus and red
llitmus
Test for carboxylic group:
a.- Sodium bi carbonate test:
Added a pinch of NaHCO3 to
small amount of Organic
compound
b.- Ester test: Added ethanol to
organic Compound and then
added 2-3 drops of conc. H2SO4
to it and warmed in water bath for
few min
Observation
Inference
KMnO4 get
decolourised
Compound is
saturated (-)
change
is
observed,
blue
litmus turn red
Effervescence with
evolution of colour
less and odourless
gas which turns
lime water milky
Pleasant fruity
smell
Alcoholic or
carbonyl group
may be present
Carboxylic
group present
Carboxylic
group present
RESULT – The experimental observation shows the presence of Carboxylic group – COOH .
Equations:- a)CH3COOH + Na2CO3 → CH3COO Na + H2O +CO2
b) C2H5OH + CH3COOH → CH3COO C2H5 + H2O.
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt is NH4 Cl in which NH4+ is cation and Cl- as anion radical
EXPERIMENT - 09
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT OBSERVATION
1
Heat a pinch of
No redish brown gas
salt in dry test
Sublimation occurs
tube
No crackling sound
INFERENCE
NO3- absent
Halide may be present
Pb(NO3)2 may be absent
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
1. Dil H2SO4 test
Take a pinch of salt in a test
tube add Dil
H2SO4
OBSERVATION
No effervasence of CO2
No rotten egg smell of H2S
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make
FeSO4 solution black
HCl gas (suffocating smell)
Give white PPT with AgNO3
(soluble in NH4OH)
2.
Conc. H2SO4 test
Take a pinch of salt in a test
tube add Conc H2SO4
3.
CONFIRMATORY TEST
a.To the salt solution add
White PPT – soluble in NH4OH
conc HNO3 and AgNO3 soln
b.To the salt add MnO2 and
Cl2 gas evolves
Conc H2SO4 and
heat .
Red vapours- add NaOH ( yellow
c.Salt + solid K2Cr2O7 +
solution
obtained) add acetic acid
Conc H2SO4 & heat
& lead acetate - Yellow PPT
INFERENCE
CO32- absent
S2- absent
SO32- absent
NO2- absent
Cl- may be present
Cl- Confirm
Cl- Confirm
Cl- Confirm
C. TEST FOR BASIC RADICAL
1.
2.
3.
To the salt solution add
NaOH solution and heat
Bring a glass rod dipped in
Dil HCl over the test tube
Smell of ammonia
Add Nessler’s reagent
Brown PPT formed
White fumes appears
NH4+ may be
present
NH4+ may be
present
NH4+ confirm
RESULT- The given salt is NH4 Cl in which NH4+ is cation and Cl- as anion radical
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt has
NH4+ is
cation and
C2O42-
as anion radical
EXPERIMENT - 10
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT
1
Heat a pinch of salt in
dry test tube
OBSERVATION
No redish brown gas
Sublimation not occurs
No crackling sound
INFERENCE
NO3- absent
Halide may be absent
Pb(NO3)2 may be absent
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
OBSERVATION
1.
Dil H2SO4 test
No effervasence of CO2 No
Take a pinch of salt in a test rotten egg smell of H2S
tube add Dil H2SO4
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make
FeSO4 solution black
INFERENCE
CO32- absent
S2- absent
SO32- absent
NO2- absent
2.
Conc. H2SO4 test
Colorless odourless gas (CO2)
Take a pinch of salt in a test
tube add Conc H2SO4
C2O42-(oxalate)
may be present
3.
CONFIRMATORY TEST
a.To the salt solution add
acetic acid and
calcium chloride
C2O42-(oxalate)
Confirm
White PPT
Pink colour of KMnO4 discharged C2O42-(oxalate)
Confirm
Dil H2SO4 and warm add 23 drops of KMnO4 solution
b.To the salt solution add
C. TEST FOR BASIC RADICAL
1.
To the salt solution add
Smell of ammonia
NaOH solution and heat
2.
Bring a glass rod dipped in White fumes appears
Dil HCl over the test tube
NH4+ may be
present
NH4+ may be
present
3.
NH4+ confirm
Add Nessler’s reagent
Brown PPT formed
RESULT- The given salt has NH4+ is cation and C2O42- as anion radical
AIM- To detect one cation and one anion radical from given salt.
RESULT- The given salt is has Pb++ is cation and NO3- as anion radical.
EXPERIMENT - 11
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- No characteristic pungent smell- NH4+ may be absent
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT
1
Heat a pinch of salt in
dry test tube
OBSERVATION
Reddish brown gas
NO Sublimation occurs
Crackling sound
INFERENCE
NO3- may be present
Halide may be absent
Pb(NO3)2 may be present
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
1.
Dil H2SO4 test
Take a pinch of salt in a test tube
add Dil H2SO4
2.
Conc. H2SO4 test Take a pinch of
salt in a test tube add Conc H2SO4
3.
CONFIRMATORY TEST
a.To the salt solution add conc
H2SO4 and Cu chipps then heat.
b.To the salt solution add FeSO4
soln and Conc H2SO4 by the side
of test tube .
C. TEST FOR BASIC RADICAL
1.
To the salt solution add NaOH
solution and heat
2.
To the salt add dil HCl
3.
CONFIRMATORY TEST
To the above solution
I. add KI soln (one part)
II. add K2CrO4 soln
OBSERVATION
No effervasence of CO2
No rotten egg smell of H2S
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make
FeSO4 solution black
NO2 gas (reddish brown)- turn
FeSO4 solution black
INFERENCE
CO32- absent
S2- absent
SO32- absent
NO2- absent
Reddish brown gas
NO3- Confirm
Dark brown ring
NO3- Confirm
No Smell of ammonia
Zero group NH4+
absent
Pb++ may be
present
White PPT
NO3- may be
present
Yellow PPT formed
Pb++ confirm
Yellow PPT formed
Pb++ confirm
RESULT- The given salt is has Pb++ is cation and NO3- as anion radical.
AIM- To detect one cation and one anion radical from given salt.
RESULT- The given salt is (CH3COO)2Pb in which Pb++ is cation and CH3COO-
as anion radical
EXPERIMENT - 12
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- CH3COO- may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT
1
Heat a pinch of salt in
dry test tube
OBSERVATION
No redish brown gas
Sublimation not occurs
No crackling sound
INFERENCE
NO3- absent
Halide may be absent
Pb(NO3)2 may be absent
B.
TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
1.
Dil H2SO4 test
Take a pinch of salt in a test tube
add Dil
H2SO4
2.
Conc. H2SO4 test
Take a pinch of salt in a test tube
add Conc H2SO4
3.
CONFIRMATORY TEST
To the solid salt add oxalic acid
and 2-3 drops of water- Rub with
finger
ESTER TEST- To the salt
solution add ethanol and Conc
H2SO4 and heat
C. TEST FOR BASIC RADICAL
1.
To the salt solution add NaOH
solution and heat
2.
To the salt add dil HCl
3.
CONFIRMATORY TEST
To the above solution
I. add KI soln (one part)
II. add K2CrO4 soln
OBSERVATION
No effervasence of CO2
No rotten egg smell of H2S
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make
FeSO4 solution black
Colorless vapours of vinegar
smell
Vinegar smell
Fruity smell of ester
No Smell of ammonia
White PPT
INFERENCE
CO32- absent
S2- absent
SO32- absent
NO2- absent
CH3COO(acetate) may be
present
CH3COO(acetate)
Confirm
CH3COO(acetate)
Confirm
Zero group NH4+
absent
Pb++ may be
present
Yellow PPT formed
Pb++ confirm
Yellow PPT formed
Pb++ confirm
RESULT- The given salt is (CH3COO)2Pb in which Pb++ is cation and CH3COO- as anion
radical
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt is NH4 (CO3)2 in which NH4+ is cation and CO32- as anion
radical
EXPERIMENT - 13
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT OBSERVATION
INFERENCE
May be CO32- present
1
Heat a pinch of Colourless odourless gas
which turns lime water milky
salt in dry test
tube
No Sublimation occurs
Halide absent
No crackling sound
Pb(NO3)2 may be absent
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
OBSERVATION
1.
Dil H2SO4 test
Effervesence of CO2,
Take a pinch of salt in a test which turns lime water
milky
tube add Dil H2SO4
2.
CONFIRMATORY TEST
a.To the salt solution add Dil
INFERENCE
CO32- may be
present
CO2 Gas evolved with
brisk effervescence
CO32- Confirm
White PPT
CO32- Confirm
HCl
b.To the salt solution add
MgSO4 solution.
C. TEST FOR BASIC RADICAL
1.
To the salt solution add
Smell of ammonia
NaOH solution and heat
NH4+ may be
present
2.
Bring a glass rod dipped in
Dil HCl over the test tube
White fumes appears
NH4+ may be
present
3.
Add Nessler’s reagent
Brown PPT formed
NH4+ confirm
RESULT- The given salt is NH4 (CO3)2 in which NH4+ is cation and CO32- as anion radical
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt has Al2 (SO4)3 in which A+++ is cation and SO42- as anion
radical
EXPERIMENT - 14
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TESTS.N. EXPERIMENT
OBSERVATION
INFERENCE
1
Heat a pinch of salt in No redish brown gas
NO3- absent
dry test tube
Sublimation not occurs Halide may be absent
No crackling sound
Pb(NO3)2 may be absent
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT OBSERVATION
Dil H2SO4 test
No effervescence of CO2
1.
Take a pinch of salt
in a test tube add Dil
H2SO4
No rotten egg smell of H2S
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make FeSO4
soln black
2.
Conc. H2SO4 test
Take a pinch of salt
in a test tube add
Conc H2SO4
3.
Special group test
Add dil HCl and filter
add BaCl2
No Colorless odourless gas (CO2)
No smell of vinegar
No colourless pungent smell gas
No brown colour gas of pungent smell
No voilet vapour of pungent smell
No reddish brown gas of pungent smell
White PPT
C. TEST FOR BASIC RADICAL
1. To the salt solution add NaOH solution
INFERENCE
CO32- absent
S2- absent
SO32- absent
NO2- absent
C2O42-absent
CH3COO- absent
Cl- absent
Br- absent
I- absent
SO42-(sulphate)
Confirm
No Smell of ammonia
NH4+ is absent (group
0 absent)
2. To the salt solution add Dil HCl
No White PPT appears
3. Pass H2S gas to above solution
No Black PPT formed or
any PPT
White PPT formation
Pb++ is absent (group
1 absent)
Cu++ , Pb++ absent
(group 2nd absent)
Al+++ may be present
and heat
4. To the salt solution add solid NH4Cl, Con
HNO3, and NH4OH till smell of NH3
5. To the white PPT add dil HCl few
drops of Blue litmus + NH4OH soln in
excess
A white PPT (suspended Al+++ may be
present
in colourless medium)
called a lake,
RESULT- The given salt has Al2 (SO4)3 in which A+++ is cation and SO42- as anion radical
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt is Sr(NO3)2 in which Ba ++ is cation and SO42- as anion
radical
EXPERIMENT - 15
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TEST-
S.N. EXPERIMENT
OBSERVATION
INFERENCE
1
Heat a pinch of salt in
Reddish brown gas
NO3- may be present
dry test tube
NO Sublimation occurs
Halide may be absent
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
OBSERVATION
INFERENCE
1. Dil H2SO4 test Take a No effervasence of CO2
CO32- absent
pinch of salt in a test
No rotten egg smell of H2S
S2- absent
tube add Dil
No SO2 gas ( turn K2Cr2O7 green) No
SO32- absent
reddish Brown gas make FeSO4 black
H2SO4
NO - absent
2
No Colorless odourless gas (CO2)
No smell of vinegar
No colourless pungent smell gas
No brown colour gas of pungent smell
No voilet vapour of pungent smell
No reddish brown gas of pungent smell
3. Special group test
White PPT obtained
a. To the salt add dil HCl and filter.
To the filtrate add BaCl2
C. TEST FOR BASIC RADICAL
1. To the salt solution add NaOH No Smell of ammonia
solution and heat
2. To the salt solution add Dil
No White PPT appears
HCl
3. Pass H2S gas to above
No Black PPT formed or any PPT
solution
4. To the salt solution add
No change is observed
NH4Cl and NH4OH in excess
5
Pass the H2S gas to above soln No change is observed
C2O42-absent
CH3COO- absent
Cl- absent
Br- absent
I- absent
6
(group 5th present)
Ba2+,Sr2+Ca2+may be
prsent
2.
Conc. H2SO4 test
Take a pinch of salt in
a test tube add Conc
H2SO4
To the salt solution add solid
NH4Cl , NH4OH , (NH4)CO3
White PPT formation
SO42- (sulphate)
Confirm
NH4+ is absent
(group 0 absent)
Pb++ is absent
(group 1 absent)
Cu++ , Pb++ etc
absent (group 2nd )
(group 3nd absent)
Al3+, Fe3+ absent
(group 4th absent)
Zn2+,NI2+,Co2+ abs.
7
Dissolve the white PPT in CH3COOH and make it 2 parts
8
PART – A + K2CrO4 soln
YELLOW PPT formed
Ba2+ Confirmed
9
Performed Flame test
grassy green flame
Ba2+ confirmed
Result- The given salt is Sr(NO3)2 in which Ba ++ is cation and SO42- as anion radical
AIM- To detect one cation and one anion radical from given salt
RESULT- The given salt is Sr(NO3)2 in which Sr++ is cation and NO3- as anion
radical
EXPERIMENT - 16
AIM- To detect one cation and one anion radical from given salt
A. PHYSICAL EXAMINATION
COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent
ODOUR- characteristic pungent smell- NH4+ may be present
SOLUBILITY- Soluble in water , Soluble in Dil. HCl
DRY HEATING TEST-
S.N. EXPERIMENT
OBSERVATION
1
Heat a pinch of salt in Reddish brown gas
dry test tube
NO Sublimation occurs
B. TEST FOR ACIDIC RADICAL
S.N. EXPERIMENT
Dil H2SO4 test
1.
2.
3.
INFERENCE
NO3- may be present Halide
may be absent
OBSERVATION
CONFIRMATORY TEST
a.To the salt solution add conc
H2SO4 and Cu chipps then heat.
b.To the salt solution add FeSO4
soln and Conc H2SO4 by the side
of test tube .
CO32- absent S2absent
SO32- absent NO2absent
NO3- may be present
Reddish brown gas
NO3- Confirm
Dark brown ring
NO3- Confirm
C. TEST FOR BASIC RADICAL
To the salt solution add NaOH
1.
No Smell of ammonia
2.
solution and heat
To the salt solution add Dil HCl
No White PPT appears
3.
Pass H2S gas to above solution
No Black PPT formed or any PPT
4.
To the salt solution add
NH4Cl and NH4OH in excess
Pass the H2S gas to above soln
No change is observed
5
INFERENCE
No effervescence of CO2
Take a pinch of salt in a test tube
No rotten egg smell of H2S
add Dil H2SO4
No S02 gas ( turn K2Cr2O7 green)
No reddish Brown gas make
FeSO4 solution black
Conc. H2SO4 test - Take a pinch of NO2 gas (reddish brown)- turn
salt in a test tube add Conc H2SO4
FeSO4 solution black
No change is observed
6
To the salt solution add solid White PPT formation
NH4Cl , NH4OH , (NH4)CO3
7
Dissolve the white PPT in CH3COOH and make it 2 parts
NH4+ is absent
(group 0 absent)
Pb++ is absent
(group 1 absent)
Cu++ , Pb++ etc absent
(group 2nd )
(group 3nd absent) Al3+,
Fe3+ absent
(group 4th absent)
Zn2+,NI2+,Co2+ abs.
(group 5th present)
Ba2+,Sr2+Ca2+may be
PART – A + K2CrO4 soln
NO change or No PPT formed
Ba++ absent
8
PART – B + (NH4)2SO4 soln
White PPT obtained
Sr ++ confirmed
9
Crimson red flame
Sr ++ confirmed
10 Performed Flame test
Result- The given salt is Sr(NO3)2 in which Sr++ is cation and NO3- as anion radical
AIM- Preparation of lyophilic sol of starch.
EXPERIMENT - 17
AIM- Preparation of lyophilic sol of starch.
THEORY: When water is used as a dispersion medium, starch has the ability to
form sol. This formation is enhanced with the help of heating. To prepare sol the
mixture of water and starch is heated to about 100° C.
MATERIALS REQUIRED: Tripod stand, Beaker of about 50 to 250 mL, Funnel,
Distilled water, Wire gauze, Glass rod, Pestle and mortar, Burner, Filter paper, 500
mg starch.
PROCEDURE:
1. Take a mortar and add 500 mg of starch to it.
2. Pour a few drops of distilled water and pestle the starch into a thin paste.
3. Transfer the grinded paste to a 50 ml beaker.
4. Take a 250 mL beaker and pour 100 mL of distilled water to it and heat the water
to boiling.
5. Slowly pour the paste into the boiling water and constantly keep stirring with the
help of glass rod.
6. Let it boil for 10 minutes after you have transferred all the paste into the beaker.
7. Allow it to cool.
8. With the help of a filter paper attached to a funnel you can filter out the contents.
9. Label the filtrate as starch sol.
PRECAUTIONS TO BE TAKEN DURING THE EXPERIMENT:
1.The apparatus used for the experiment should be washed with distilled water and
dried before conducting the experiment.
2.Use of distilled water to prepare starch sol.
3.Make sure to convert starch into a smooth paste before adding to the boiling
water beaker.
4.Keep constantly stirring the mixture while preparing starch sol.
AIM: The aim of this experiment – to prepare ferric hydroxide sol.
EXPERIMENT 18
AIM: The aim of this experiment – to prepare ferric hydroxide sol.
THEORY: Ferric hydroxide (Fe(OH)3) has the ability to form a lyophobic sol.
Sulphides or metal hydroxides which colloidal solution, when treated with water,
are termed as lyophobic colloids. Fe(OH)3 sol is obtained by hydrolysis of ferric
chloride with boiling distilled water. The reaction is as follows:
FeCl3(aq) + 3H2O(l) --------------> Fe(OH)3(s) + 3HCl(aq)
The hydrochloric acid formed during the hydrolysis destabilizes the ferric
hydroxide sol and therefore must be removed through the process of dialysis.
MATERIALS REQUIRED:
The apparatus and materials required for this experiment are as follows:
Glass rod, round bottom flask, Boiling tube, Conical flask of 250 mL volume,
Tripod stand, Funnel, Beaker of 250 mL volume, Burette, Wire gauze, Dropper,
Burner, Wire gauze, Iron stand with clamp, Boiling tube, Distilled water, Solution
of ferric chloride
PROCEDURE:
1.Take a conical flask of volume 250 mL and steam clean it.
2.To clean the conical flask by steaming out process take the help of the figure.
3.Prepare 2% solution of ferric chloride by taking 2 g of pure ferric chloride in
100mL of distilled water.
4.Take the conical flask cleaned by steaming out process and add 100mL of
distilled water.
5.Boil the water on a wire gauze.
6.Drop by drop pour 10 mL of ferric chloride solution with the help of a dropper
or burette.
7.Constantly keep stirring the boiling water mixture while adding ferric chloride
solution.
8.Heat the conical flask containing a mixture of distilled water and ferric chloride
solution until you see a brown or deep red coloured ferric hydroxide solution.
9 Allow the mixture in the conical flask to settle at room temperature. 10. Label
the flask containing mixture as ferric hydroxide sol.
PRECAUTIONS TO BE TAKEN DURING THE EXPERIMENT:
1.Fe(OH)3 sol gets affected due to the presence of impurities. Therefore, to avoid
this conical flask is cleaned by steaming out process.
2.The FeCl3 solution is added drop wise.
3. Heat the mixture of distilled water and ferric chloride solution until brown or
deep red colour is obtained.
4. The hydrochloric acid (HCl) formed is removed by the process of dialysis to
avoid destabilization of sol.