CHEMISTRY

INDEX
S.NO. EXPERIMENT
1. To prepare M/20 solution of FAS in 250 ml & determine the molarity of strength of the
given KMnO4
2. To prepare standard solution of FAS by dissolving 2.45 gm FAS in 250 ml. Also determine
molarity and strength of given KMnO4.
3. To prepare M/20 solution of oxalic acid in 250 ml using this solution, determine molarity
and strength of given KMnO4
4. To prepare std. sol of 0.7875g oxalic acid in 250 ml & determine the molarity & strength of
the given KMnO4
5. To detect the acidic & basic radical in given salt-i
6. To detect the acidic & basic radical in given salt-ii
7. To detect the acidic & basic radical in given salt-iii
8. To detect the acidic & basic radical in given salt-iv
9. To detect the acidic & basic radical in given salt-v
10. To detect the acidic & basic radical in given salt-vi
11. To detect the functional gp in given org. sample-i
12. To detect the functional gp in given org. sample-ii
13. To detect the functional gp in given org. sample-iii
14. To detect the functional gp in given org. sample-iv
15. To detect the functional gp in given org. sample-v
16. To detect the functional gp in given org. sample-vi
17. To detect the presence of carbohydrate of starch in the given food stuff.
18 To detect the presence of fat in given food sample
19. To detect the presence of protein in given food sample.
Diagram Page
 Experiment – 01

Aim: To prepare M/20 solution of ferrous ammonium sulphate (Mohr’s salt) in 250 ml volumetric flask.
By using this solution find out the molarity and strength of given KMnO4 solution.

Apparatus required : Burette, Pipette, titration flask, test tube, watch glass, weight box, analytical
balance, measuring flask.

Chemicals required : Ferrous Ammonium sulphate crystals. KMnO4 solution, Con H2SO4 dil. H2SO4.

Theory : Potassium permanganate oxidises ferrous ammonium sulphate into ferric ammonium sulphate
and itself get reduced to colourless ions i.e..
2kMnO4 + 8H2SO4 + 10 FeSO4.(NH4)2 SO4.6H2O   k2SO4 + 2MnSO4 + 5Fe2(SO4)3 +
10(NH4)2SO4 + 68 H2O

Ionic Equation
MnO 4  8H   5e  
 Mn 2   4H 2 O
 Fe 2 
 Fe 3  e    5
MnO 4  8H   5Fe 2   5Fe  3  Mn 2  4H 2 O

Indicator : KMnO4 is a self indicator

End Point : Colourless to permanent pink colour.
DIAGRAM PAGE

 For Preparing 250 ml of M/20 Mohr’s salt solution

Mohr’s salt Required (x) :
Molarity  Molar mass  volume in ml
x
1000
Molar mass of Mohr’s salt = 392 g mol–1
1 392  250
x  4.9 gm
20  1000
 Observation
1. Wight of paper = 0.2344 gm
2. Weight of paper + Mohr’s salt = 5.1344 gm
3. Weight of Mohr’s salt = 4.9 gm
4. Volume of Mohr’s salt prepared = 250 ml
5. Molarity of Mohr’s salt solution = M/20
Procedure :
A For preparation of 250 ml of M/20 FAS solution
i. Weigh the clean and dry paper and record its weight in the note book.
ii. Weigh accurately 4.9 g of FAS crystal on the paper and record the weight in the
notebook.
iii. Transfer salt from the paper to 250 ml. beaker, add to this beaker about 5 ml of Con
H2SO4 to check the hydrolysis of ferrous sulphate.
iv. Transfer the clear solution in the beaker into a 250 ml measuring flask.
v. Wash the beaker with distilled water and transfer washing into the
measuring flask.
vi. carefully add distilled water to measuring flask till the solution stand just below the
graduated mark on the flask.
vii. Stopper the measuring flask and shake it vigorously so that solution become
homogenous.
viii. Label the solution as M/20 ferrous Ammonium Sulphate solution.
B Procedure for titration :
i. Rinse and fill the burette with the given KMnO4 solution.
ii. Rinse the pipette with M/20 Mohr’s salt solution and pipette put 20 ml Mohr’s salt
solution in a conical flask.
iii. Add one test tube full of dil H2SO4 (4N) to the solution in titration flask.
iv. Note the initial reading of the burette.
v. Run in KMnO4 solution from the burette with shaking the contents in the titration flask
till a permanent light pink colour is obtained in the solution. This is end point.
vi. Note down the final burette reading.
vii. Take 3 concordant readings and then calculate the result.
DIAGRAM PAGE

Observation Table
S.no. Vol. of pipette used or Burette Reading Volume of kMnO4 Concordant
used Vol.
Vol. of Mohr’s salt Initial Final
(ml) (ml)
1. 20 ml 0.0 14.4 14.4 ml
2. 20 ml 14.4 27.0 12.6 ml 12.6 ml
3. 20 ml 27.0 39.6 12.6 ml

Calculation : At the end point in the titration stoichiometry between the two reactants, kMnO4 &
Mohr’s salt lies in 1 :5 ration.
M1V1 (kMnO 4 ) 1
 where :-
M 2 V2 (Mor 's alt) 5
1
M1V1  M 2 V2 M1 = Molarity of KMnO4 solution
5
1 M
M1 × 12.6 =   20 ml V1 = Volume of KMnO4 Solution
5 20
1 M
M1   M2 = Molarity of FAS solution
5 12.6 63
V2 = Volume of FAS solution
Strength = Molarity × Molar mass of KMnO4
M
 158 Molarity = moles /lit
63
= 2.5079 g /  Molar mass = gm/mol
mole gm
Strength =   gm / lit
lit mol
Result : Molarity of given KMnO4 solution is M/63 and strength is 2.5079 g /  .
Precautions :
1. Read upper meniscus in the burette because KMnO4 solution is highly coloured.
2. Transfer the FAS salt crystals from the paper to the beaker very carefully so that even a single
crystal is not lost.
3. Do not heat the solution in the titration flask.
4. Do not rinse the titration flask.
DIAGRAM PAGE
 Experiment – 2

Aim : To prepare standard solution of FAS by dissolving 2.45 gm FAS in 250 ml. Also determine
molarity and
strength of given KMnO4 solution by using above prepared FAS.

Apparatus required : Burette, Pipette, titration flask, test tube, white tile, watch glass, weight box,
analytical balance, measuring flask.

Chemical required : Ferrous Ammonium Sulphate crystals, KMnO4 solution, con. H2SO4, dil. H2SO4.

Theory : Potassium permanganate oxidises ferrous ammonium sulphate into ferric ammonium sulphate
and itself get reduced to colourless ions i.e.

2KMnO4 +8H2SO4 + 10FeSO4 (NH4)2 SO4.6H2O  K2SO4 +2MnSO4 + 5Fe2(SO4)3 + 10(NH4)2SO4+
68H2O
Ionic Equation :
MnO 4  8H  5e  
 Mn 2  4H 2O
[Fe 2 
 Fe 3  e  ]  5
MnO 4  8H   5Fe 2 
 5Fe 3  Mn 2  4H 2 O
Indicator : KMnO4 is a self indicator.
End point : Colourless to permanent pink colour
DIAGRAM PAGE

Molarity of FAS solution prepared.

Molarity  Molar mass  volume in ml
W=
1000
W  1000 2.45  1000 M
Molarity =  
M.M  Vol.(ml) 392  250 40
Observation
1. Weight of paper = 0.2368 gm
2. Weight of paper +FAS salt = 2.6868 gm
3. Weight of FAS salt = 2.45 gm
4. Volume of FAS sol. Prepared = 250 ml
5. Molarity of FAS sol. = M/40
Procedure :
A. For preparation of 250 ml of M/40 FAS solution.
i. Weigh the clean and dry paper and records its weight in notebook.
ii. Weigh accurately 2.45 gm of FAS crystals on the paper and record the weight in notebook.
iii. Transfer salt from the paper to 250 ml beaker. Add to this beaker about 5 ml of con. H2SO4 to
check the hydrolysis of ferrous sulphate.
iv. Transfer the clean solution in the beaker into a 250 ml measuring flask through funnel.
v. Wash the beaker with distilled water and transfer washing into the measuring flask.
vi. carefully add distilled water to measuring flask till the solution stand just below the graduated
mark on the flask.
vii. Stopper the measuring flask and shake it vigorously so that solution becomes homogenous.
viii. label the solution as M/40 ferrous Ammonium Sulphate solution.

B. Procedure for titration

i. Rinse and fill the burette with given KMnO4 solution.
ii. Rinse the pipette with M/40 Mohr’s salt solution (FAS solution) and pipette put 20 ml Mohr’s
salt solution in a conical flask
iii. Add one test tube full of dil. H2SO4 (4N) to the solution in titration flask.
iv. Note the initial reading of the burette.
v. Run in KMnO4 solution from the burette with shaking the content in titration flask till a
permanent light pink colour is obtained in the solution. This is end point.
vi. Note down the final burette reading.
vii. take 3 concordant readings & then calculate the result.
DIAGRAM PAGE

Observation table

S.no. Vol. of Mohr’s salt Burette Reading Volume of KMnO4 Concordant

or used
Vol. of pipette used Initial Final Final – Initial Reading
(ml) (ml)
1. 20 ml 0.0 8.2 8.2 ml
2. 20 ml 8.2 16.2 8.0 ml 8.0 ml
3. 20 ml 16.2 24.2 8.0 ml

Calculation : At the end point in the titration stoichiometry between the two reactants, KMnO4 &
Mohr’s salt lies 1:5 ratio.
M1 V1 (kMnO 4 ) 1
 where :-
M 2 V2 (Mohr 'salt) 5
1
M1V1  M2 V2 M1 = Molarity KMnO4 solution
5
1 M
M1  8ml   20ml V1 = Volume of KMnO4 Solution
5 40
M
M1  M2 = Molarity of FAS solution
80
V2 = Volume of FAS solution

Strength = Molarity × Molar mass of KMnO4 solution

M
 158
80
= 1.975 g / 
Result : Molarity of given KMnO4 solution is M/80 and strength is 1.975 g /  .

Precautions :
1. Read upper meniscus in the burette because KMnO4 Solution is highly coloured.
2. Transfer the FAS salt crystals from the paper to the beaker very carefully so that even a single
crystal is not lost.
3. Do not heat the solution in the titration flask.
4. Do not rinse the titration flask.
DIAGRAM PAGE
 Experiment – 3
Aim : To prepare M/20 solution of oxalic acid in 250 ml using this solution, find out molarity and
strength of given KMnO4 solution.

Apparatus Required : Burette, pipette, titration flask, test tube, white tile, burner watch glass, weight
box, analytical balance, measuring flask.

Chemical Required : Oxalic acid crystals, KMnO4 solution dil. H2SO4.

Theory : KMnO4 oxidizes oxalic acid into carbon dioxide in acidic medium at a temp. around 60 o C and
itself gets reduced to colourless ions.

2KMnO4 + 3H2SO4 + 5(COOH)2 

 K2SO4 + 2MnSO4 + 10CO2 + 8 H2O

Ionic Equation :
MnO 4  8H   5e  Mn 2 4H 2 O ]  2

C 2 O 42  2CO2  2e ]  5


2MnO4  16H   5C 2 O 42  
 2Mn 2   8H 2 O  10CO2

Indicator : KMnO4 is a self indicator

End Point : colourless to permanent pink colour.
DIAGRAM PAGE

To Prepare 250 ml of M/20 oxalic acid solution ; weight of hydrated oxalic acid required.
Molarity  Molar mass  vol.of solution(ml)
Woxalic Acid =
1000
Molar mass of hydrated oxalic acid (COOH)2 2H2O = 126 g mol–1
126  250
W  1.575gm
20  1000
Observation
1. Weight of oxalic Acid = 1.575 gm.
2. Volume of oxalic Acid solution prepared = 250 ml
3. Molarity of oxalic Acid solution = M/20
4. Volume of oxalic Acid taken for titration = 20.0 ml
Procedure :

1. Weigh 1.575 gm of oxalic acid crystals and dissolve them in water to prepare 250 ml of oxalic acid
solution using a 250 ml measuring flask.
2. Rinse the pipette with the oxalic acid solution and pipette out 20 ml of it in a titration flask.
3. Rinse and fill the burette with the given KMnO4 solution.
4. Add one test tube full of dil. Sulfuric Acid to the solution in titration flask.
5. Note the initial reading of the burette
6. Heat the flask to 60-70o C and add KMnO4 solution from the burette till a permanent light pink colour
is imparted to the solution in the titration flask on addition of a last single drop of KMnO4 solution . This
is end point.
7. Note the final reading of the burette
8. Take 3 concordant readings and then calculate the result.
DIAGRAM PAGE

Observation table

S.no. Vol. of oxalic acid Burette Reading Volume of kMnO4 Concordant

used
Solution/Vol. ot Initial Final Final – Initial Reading
Pipette(ml) (ml) (ml)
1. 20 ml 0.0 19.5 19.5 ml
2. 20 ml 19.5 40.9 21.4 ml 21.4 ml
3. 20 ml 0.0 21.4 21.4 ml

Calculation :
M1 V1 (kMnO4 ) 2
 M1 = Molarity of KMnO4 solution.
M 2 V2 (oxalic Acid) 5
2 M V
M1   2 2 V1 = Vol. of KMnO4 Solution
5 V1
2 M  20
  M2 = Molarity of oxalic Acid Solution.
5 20  21.4
2 M V2 = Vol. of oxalic acid solution
 0.0187M
5  21.4

Strength : Molarity × Molar mass of kMnO4 solution

= 0.0187 × 158
= 2.9546 g/l.
Result : Molarity of the given kMnO4 solution is 0.0187 M and strength is 2.9546 g/l

Precautions :
1. Never pour hot solution to the measuring flask
2. During making up of the volume the last drop of water should be added very carefully
3. Oxalic acid solution should not be heated beyond 70oC
4. Oxalic acid solution should stay warm during titration.
DIAGRAM PAGE
 Experiment -04

Aim: To prepare standard solution of oxalic acid by dissolving 0.7875 gm of oxalic acid crystals in 250
ml water. And determine molarity and strength of given kMnO4 solution by using prepared oxalic Acid.

Apparatus Required : Burette, Pipette, titration flask, test tube, white tile, burner, watch glass, weight
box, analytical balance.

Chemical required : Oxalic acid crystals, KMnO4 solution dil. H2So4.

Theory : kMnO4 solution oxidize oxalic acid to CO2 in acidic medium at temp around 60oC itself gets
reduced to colourless ions.
2kMnO4 + 3H2SO4 + 5 (COOH)2   K2SO4 + 2MnSO4 + 10 CO2 + 8H2O
Ionic Equation :
MnO 4  8H   5e  Mn 2 4H 2 O ]  2

C 2 O 42  2CO2  2e ]  5


2MnO4  16H   5C 2 O 42  
 2Mn 2   8H 2 O  10CO2

Indicator : KMnO4 is a self-indicator.

End point : Colourless to permanent pink colour.
DIAGRAM PAGE

Molarity of oxalic acid solution Prepared

Molarity  molar mass  Vol.in ml
W=
1000
Molar mass  Vol.in ml 126  250
Molarity = 
1000  0.7875 1000  0.7875
= M/40

Observation
1. Weight of oxalic acid = 0.7875
2. Volume of oxalic acid solution prepared = 250 ml
3. Molarity of oxalic acid solution = M/40
4. Volume of oxalic acid solution taken for each titration. = 20 ml
Procedure :
1. Weigh 0.7875 gm of oxalic acid crystals and dissolve them in water to prepare 250 ml of oxalic
acid solution using a 250 ml of measuring flask.
2. Rinse the pipette with the oxalic acid solution and pipette out 20 ml of it in a titration flask.
3. Rinse and fill the burette with the given kMnO4 solution.
4. Add one test tube full of dil. Sulphuric Acid (4N) to the solution in titration flask.
5. Note the initial reading of the burette.
6. Heat the flask to 60-70oC and add kMnO4 solution from the burette till a permanent light pink
colour is imparted to the solution in the titration flask on addition of a last single drop of
KMnO4 solution.
7.Note the final reading of the burette.
8. take 3 concordant reading and then calculate the result.
DIAGRAM PAGE

Observation table
S.no. Vol. of oxalic acid Burette Reading Volume of KMnO4 Concordant
used
Solution/Vol. ot Initial Final Final – Initial Reading
Pipette(ml) (ml) (ml)
1. 20 ml 0.0 ml 9.6 ml 9.6 ml
2. 20 ml 9.6 ml 19.8 ml 10.2 ml 10.2 ml
3. 20 ml 19.8 ml 30.0 ml 10.2 ml

Calculation :
2
M1V1  M 2 V2 M1 = molarity of KMnO4 solution
5
2 M 2 V2
M1  V1 = Vol. of KMnO4 solution
5 V1
2 M  20.0
 M2 = Molarity of oxalic Acid solution
5 40  10..2
M/51 = 0.0196 M V2 = Vol. Of oxalic Acid solution

Strength : = Molarity × Molecular mass

= 0.0196 × 158
= 3.0980 g/lit
Result : Molarity of the given KMnO4 solution is 0.0196 M and strength is 3.0980 g/lit.

Precautions:
1. Never pour hot solution to the measuring flask
2. During making up of the volume the last drop of water should be added very carefully.
3. Oxalic acid solution should not be heated beyond 70oC
4. Oxalic acid solution stay warm during titration.
DIAGRAM PAGE
 Experiment -5

Aim: To analyse the given salt for acidic and basic radicals.

Apparatus required :Test tube, beaker, China dish, funnel, tripod stand, filter paper. burner etc.

Physical test :
Experiment Observation Inference
1. Physical appearance and colour White amorphous solid Cu2+, Ni2+,Fe2+,CO2+, Mn2+
absent
2. Odour Ammonical NH4+ may be present
3. Flame test NO specific Ba2+, Sr2+, Ca2+, Cu2 absent
Observation

Chemical test :
Experiment Observation Inference
1. Salt + dil. H2SO4 Colourless, odourless gas Weak acidic radical gp present
evolved which turned lime CO32- present
water milky

2. Aqueous solution of salt + few White ppt CO32- Confirmed

drops of MgSO4 Solution

3. Aqueous solution of salt + a Pink Colour CO32- Confirmed

drop of phenolphthalein

II For basic Radicol

1. Salt + Con. NaOH & heat colourless gas having Zero gp present NH4+ present
ammonical smell is evolved

2. Brought a glass rod dipped in a white fumes produced NH4+ present

con. HCl near the mouth of the
tube
3. passed the evolved gas in Reddish brown colour ppt NH4+ Confirmed
Nessler’s reagent

Result :Acidic radical CO32- and basic radical NH4+ is present in given salt and salt is Ammonium
carbonate (NH4)2 CO3.
DIAGRAM PAGE
 Experiment – 6
Aim : To detect the acidic and basic radical in given salt.

Apparatus required : Test tubes, beaker, China dish, burner, Tripod stand, filter paper etc.

Physical test :
Experiment Observation Inference
1. Physical appearance and colour Crystalline solid & white Cu2+, Ni2+,Fe2+,CO2+, Mn2+
absent
2. Odour Vinegar smell CH3 COO–may be present
3. Flame test Greenish flashes Zn2+ may be present

Chemical test :
I For Acidic Radical
Experiment Observation Inference
1. Salt + dil. H2SO4 Colourless gas with vinegar Weak acidic radical gp present
like smell turns blue litmus CH3 COO– may be present
red

2. Salt + Con. H2SO4 + ethyl- Pleasant fruity smell CH3COO– confirmed

alcohol + Heat

3. Aqueous solution of salt + Blood red Colour CH3 COO– confirmed

neutral FeCl3

II For basic Radicol

1. Salt + dil. HCl White ppt I gp present

2. Filter the white ppt wash with ppt . Dissolves Pb2+ present
water & add water & heat

3. To one part of hot aq. Solution Yellow ppt Pb2+ confirmed

of salt+ potassium chromate
solution
Yellow ppt Pb2+ confirmed
4. To another part of hot aq.
Solution of salt + KI solution

Result : Acidic radical CH3COO– and basic radical Pb 2+ is present in given salt and the salt is
Pb(CH3COO)2 lead Acetate.
DIAGRAM PAGE
 Experiment - 7

Aim. : To detect the acidic and basic radical in the given salt,

Apparatus Required : Test tubes, beaker, burner, tripod stand, filter paper, funnel etc.
Physical test :
Experiment Observation Inference
1.Colour Blue Cu2+ may be present

2. Odour No specific colour Absence of S 2-, NH4+, CH3COO–,

SO32–
3. Flame test Bluish green Cu2+ may be presnt

Chemical test :
I Test for Acidic Radical
Experiment Observation Inference
1. Salt + dil. H2SO4 and warm No gas evolved Weak acidic radical gp absent

2. Salt + Con. H2SO4 & heat Colourless gas with pungent Strong Acidic radical gp present.
smell gave white fumes with Cl– may be present
NH4 OH

3. Aqueous solution of salt + Curdy white ppt which Cl– present

dil.HNO3 + AgNO3 solution issoluable in NH4OH

4. Salt + solid K2Cr2O7 + Con. Red Vapours evolve which

H2SO4 & heat on passing through NaOH Cl– confirmed
gives yellow solution which
on adding lead acetele gives
yellow ppt
II Test For basic Radical

1. Salt + dil. HCl

No ppt I gp absent
2.Above solution + H2S gas
3. Filter out the above ppt & wash Black ppt . IInd gp present
with water, above ppt + dil. HNO3

4.Divide the above solution in 2 Bluish green solution Cu2+ may be present
parts

To part I, add NH4OH in excess Deep blue coloured complex Cu2+ confirmed
Solution of salt + KI solution

5. II part + CH3 COOH + Potasium Brown ppt Cu2+ confirmed

ferrocyanide solution
Result : Acidic Radical Cl– and basic Radical Cu2+ is present in given salt.
DIAGRAM PAGE
 Experiment -8

Aim : To detect the acidic and basic radical in the given salt.

Apparatus Required : test tube, beaker, china dish, burner, tripod stand, filter paper etc.

Physical test :
Experiment Observation Inference
1.Colour & Appearance White fluffy solid A1+3 may be present

2. Odour No specific colour Absence of S 2-, NH4+, CH3COO–,

SO32–
3. Flame test No specific observation Sr2+, Ca2+, Cu2+, Ba+2 absent

Chemical test :
I Test for acidic Radical
Experiment Observation Inference
1. Salt + dil. H2SO4 and warm No action Weak acidic radical gp absent

2. Salt + Con. H2SO4 & heat No action Strong Acidic radical gp absent

3. Dissolve the salt in dil HCl, heat White ppt Which is insoluble SO42– present
+BaCl2, solution in Con. HCl/HNO3

4. Salt solution in HCl +CH3COOH White ppt which is soluble in SO42– confirmed
+ Lead Acetate excess hot ammonium acetate
solution

II Test For basic Radical

1. Salt solution+ dil. HCl No ppt I gp absent

2.Above solution + passed H2S gas No ppt . II gp absent

3. Heat the above solution to remove White ppt III gp present Al+3 may be
H2S gas, add NH4Cl boil, then cool present
and excess of NH4OH

4. Filter out the above white PPt +

NaOH & boil and divide into 2 parts

I part + Dil. HCl + 2 drops of blue Blue ppt floats over colourless Al3+ confirmed
litmus + NH4OH solution

5. II part + NH4Cl and boil Gelatinous white ppt Al3+ confirmed

2– 3+
Result : Acidic radical SO4 and basic radical Al is present in given salt. And salt is Aluminium
sulphate.
DIAGRAM PAGE
 Experiment -9

Aim: To detect the acidic and basic radical in given salt.

Apparatus Required : test tube, beaker, Burner, Tripod stand, Filter paper etc.

Physical test :
Experiment Observation Inference
1.Physical Appearance Crystalline solid Cu2+, Ni2+, Fe2+, Co2+,
Mn2+absent
2. Colour White Cu2+, Ni2+, Co 2+,Mn 2+, Fe2+
absent
3. Odour Vinegar smell CH3COO– may be present

4. Flame test Greenish flashes Zn2+ may be present

Chemical test :
I Test for acidic Radical
Experiment Observation Inference
1. Salt + dil. H2SO4 Colourless gas with vinegar Weak acidic radical gp present
like smell turns blue litmus CH3COO– may be present
red

2. Salt + Con. H2SO4+ethyl alcohol Pleasant fruity smell CH3COO– confirmed

and heat

3. Aqueous solution of salt + neutral Blood red colour CH3COO– confirmed

FeCl3

II Test For basic Radical

1. Salt + dil. HCl No ppt I gp absent

2.To the above solution, passed H2S No ppt . II gp absent

gas

3. Heat the above solution to remove No PPt III gp absent

H2S gas, add NH4Cl; boil then Cool
and add excess of NH4OH

4. Pass H2S to the above solution White ppt IV gp present Zn2+ may be
present
5. Above ppt + dil. HCl ppt dissolve

6. Above solution + NaOH White ppt dissolves in excess Zn2+ confirmed

of NaOH
7. To the original solution add
potassium ferrocyanide White PPt Zn2+ confirmed
Result : Given salt contain acidic Radical CH3COO– and basic radical Zn2+ . Hence the given salt is
Zn(CH3COO)2
DIAGRAM PAGE
 Experiment -10

Aim : To detect the acidic and basic radical in given salt.

Apparatus Required : Test tube, burner, tripod stand, filter paper etc.

Physical test :
Experiment Observation Inference
1.Colour White Cu2+, Mn2+, Fe2+, Cr2+ Ni2+ are
absent
2. Odour Odourless NH4+,S2–, CH3COO–, may be
absent
3. Flame test No specific observation Zn2+, Ba2+, Ca2+, absent

Chemical test :
I Test for acidic Radical
Experiment Observation Inference
1. Salt + dil. H2SO4 and warmed No gas evolved Weak acidic radical gp absent

2. Salt + Con. H2SO4 & heat No gas evolved Strong Acidic radical gp absent

3. Aqueous solution of salt + dil. White ppt insoluble in con. SO42– confirmed
HCl, heat+ BaCl2 Solution HCl

4. Salt solution in HCl +CH3COOH White ppt which is soluble in SO42– confirmed
+ Lead Acetate solution excess of hot ammonium
acetate solution
II Test For basic Radical

1. Salt + distilled water + dil. HCl No ppt I gp absent

2.Passed H2Sgas to the above No ppt . II gp absent

solution.

3. Heat the above solution + 2-3 No ppt III gp absent

drops of con. HNO3 ; boiled Cooled
+ solid NH4Cl + NH4OH in excess
with shaking
4. Passed H2S gas to the above No ppt IV gp absent
solution

5. Heat the above solution; Cooled ; No ppt V gp absent

dil. HCl + NH4OH + (NH4)2 CO3

6. Above solution + (NH4)2 HPO4 White crystalline PPT VI gp present

7. Above ppt + 2 – 3 drops of cobalt Pink mass Mg2+ may be present

nitrate solution
Result : Acidic Radical : SO42– and basic Radical Mg2+ is present in given salt, and the salt is MgSO4.
DIAGRAM PAGE
 Experiment -11

Aim: To identify the functional group in a given organic compound.

Apparatus Required : Test tube, China dish, filter paper etc.

Physical test
1. Physical state : Liquid
2. Colour : Colourless
3. Odour : Alcoholic smell
4. Litmus paper test : No change; neutral

Chemical test
Experiment Observation Inference
1. Sample + Na metal Brisk effervescence – OH gp present
2. Sample + few drops of cerric Red colour appears – OH gp present
ammonium nitrate
3. Sample + few drops of Fruity smell – OH gp present
CH3COOH + Con. H2SO4 heat

Result : The given organic sample contain alcoholic (–OH) group.

DIAGRAM PAGE
 Experiment -12

Aim : To identify the functional group in a given organic compound.

Physical test
1. Physical state : Crystalline solid
2. Colour : White
3. Odour : Colourless
4. Litmus paper test : Blue Litmus to red

Chemical test
Experiment Observation Inference
1. Sample few drops of neutral Reddish violet colour Phenolic gp – present
ferric chloride
2. Sample + few drops of cerric Brown ppt Phenolic gp present
ammonium nitrate

Result : The given organic compound contain Phenolic group.

DIAGRAM PAGE
 Experiment -13

Aim : To identify the functional group in a given organic compound.

Physical test :
1. Physical state : Liquid
2. Colour : Colourless
3. Odour : Bitter almond
4. Litmus paper : No colour change

Chemical test
Experiment Observation Inference
1. Dissolve the sample in ethyl Orange ppt
alcohol and add 2,4 dintiro C = 0 gp present
phenyl hydrazine and shake

2. Sample + Tollen’s reagent Silver mirror is formed – CHO gp present

and heat

3. Sample + shiff’s reagent Deep red colour appear – CHO gp present

Result : The given organic sample contains aldehyde group (– CHO)

DIAGRAM PAGE
 Experiment -14

Aim : To identify the functional group in a given organic compound.

Physical test :
1. Physical state : Liquid
2. Colour : Colourless
3. Odour : Sweet smell like nail paint remover
4. Litmus test : No colour change

Chemical test
Experiment Observation Inference
1. Sample + ethyl alcohol + 24- Orange ppt.
dinitro phenyl hydrazine C = 0 gp present
solution

2. Sample + Tollen’s reagent No reaction – CHO gp absent

3. Sample + 1 ml of sodium Wine red colour

nitro pruside solution + drop R– C – R' (Ketonic) gp present
wise NaOH and shake O

Result : The given sample has ketonic group.

DIAGRAM PAGE
 Experiment – 15
Aim : To identify the functional group in a given organic compound.

Physical test :
1. Physical state : Liquid
2. Colour : Colourless
3. Odour : Vinegar like
4. Litmus test : Blue litmus turns red

Chemical test
Experiment Observation Inference
1. Sample + solution of sodium Brisk effervescence – COOH gp present
bi carbonate

2. Sample + 4- 5 drops of ethyl Pleasant fruity smell – COOH gp present

alcohol + 2 drops of Con.
H2SO4 and heat

Result : The given organic compound contain – COOH gp (carboxylic group)

DIAGRAM PAGE
 Experiment – 16

Aim : To identify the functional group in given organic compound.

Physical test
1. Physical state : Liquid
2. Colour : Colourless
3. Odour : Pungent smell
4. Litmus test : Red litmus to blue

Chemical test
Experiment Observation Inference
1. Sample + 1 ml of CHCl3 + 2 Unpleasant smell Amino gp is present
ml alc. KOH + Heat

2. Sample + 3 ml of Con. HCl +

5 ml of water; cool the solution Orange dye Amino gp present
into ice + cold sodium nitrite
solution and shake + cold
solution of β naphthol + 4ml of
5% NaOH
(For Aromatic primary Anine)

Result : The given organic sample has Amino group (–NH2).

DIAGRAM PAGE
 Experiment – 17

Aim. To detect the presence of carbohydrate and starch in the given food stuff

Apparatus required: Test tube, Burner, test tube stands

Chemical test
Experiment Observation Inference
1. Sample + few drops of iodine Violet colour Starch is present
solution

2. Sample + Con. H2SO4 & heat Charring with burnt sugar Carbohydrate is present
smell
3. Aqueous solution of sample + Reddish purple ring is formed Carbohydrate is present
2 drops naphthol + Con. H2SO4 at the junction of two layers

Result : Starch / carbohydrate is present in given food stuff.

DIAGRAM PAGE
 Experiment – 18

Aim : To detect the presence of fat in the given food stuff sample.

Apparatus required : test tube, Test tube stand, Holder, Bunsen Burner etc.
Chemical test
Experiment Observation Inference
1. Put a sample on a filter A trans lucent spot appears on Fat is present
paper and press with another filter paper.
filter paper

2. Sample + few drops of Irritating smell appear Fat is present

potassium bisulphite and heat.
Fat is present
3. Sample in 3 test tubes and Sample does not dissolve in
add water, alcohol chloroform water,soluble in alcohol on
in 1,2,3 test tube respectively heating & is soluble in
chloroform
Result : Fat is present in given sample.
DIAGRAM PAGE
 Experiment – 19

Aim : To detect presence of protein in the given food stuff.

Apparatus Required : Test tube , Test tube stand, holder, burner etc.

Chemical test
Experiment Observation Inference
1 Sample + dil. NaOH + CuSO4 Bluish violet colour appears Protein is present
solution .

2. Sample + few drops of con. Yellow PPt Protein is present

HNO3 & heat

3. Sample + 2 drops of Millions White PPt which change to Protein is present

reagent & heat brick red on boiling
Protein is present
4. Sample + few drops of Blue colour appears
ninhydrin solution & boil for 1
minute

Result : Protein is present in given food sample.