CHEMISTRY PRACTICALS
CLASS-XII
EXPERIMENT No. 1 AIM – (a) To prepare 100ml of M/20 solution of oxalic acid.
(b)Using this calculate the molarity and strength of the given KMnO4 solution.
APPARATUS AND CHEMICALS REQUIRED- Oxalic acid, weighing bottle, weight
box, volumetric flask, funnel, distilled water, chemical balance, beakers, conical flask, funnel, burette, pipette, clamp stand, tile, dilute H2SO4, KMnO4 solution.
THEORY- (a) Oxalic acid is a dicarboxylic acid having molar mass 126gmol-1. It is a
primary standard and has the molecular formula COOH-COOH.2H2O. Its equivalent
mass is 126/2 = 63 as its n factor is 2 as per the following reaction: COOH-COOH → 2CO2 + 2H+ + 2e-.
Calculation of amount of oxalic acid to be weighed to prepare 100ml M/20 solution: wt. X 1000
M =
Mol. Wt V(ml)
PROCEDURE:
1. Weigh a clean dry bottle using a chemical balance.
2. Add more weights to the pan containing the weights for the weighing bottle.
3. Add oxalic acid in small amounts to the weighing bottle, so that the pans are balanced.
4. Remove the weighing bottle from the pan.
5. Using a funnel, transfer the oxalic acid to the volumetric flask. 6. Add a few drops of distilled water to dissolve the oxalic acid. 7. Make up the volume to the required level using distilled water. 8. The standard solution is prepared.
(b) THEORY-
1. The reaction between KMnO4 and oxalic acid is a redox reaction and the titration
is therefore called a redox titration.
2. Oxalic acid is the reducing agent and KMnO4 is the oxidizing agent.
3. KMnO4 acts as an oxidizing agent in all the mediums; i.e. acidic, basic and neutral
medium.
4. KMnO4 acts as the strongest oxidizing agent in the acidic medium and therefore
dil. H2SO4 is added to the conical flask before starting the titration.
5. The titration between oxalic acid and KMnO4 is a slow reaction, therefore heat the
oxalic acid solution to about 600C to increase the rate of the reaction.
6.
IONIC EQUATIONS INVOLVED:
Reduction Half: MnO4- + 8H+ + 5e- → Mn2+ + 4H2O] X 2
Oxidation Half: C2O42- → 2CO2+ 2e- ] X 5
Overall Equation: 2MnO4- + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O
INDICATOR- KMnO4 acts as a self indicator.
END POINT- Colourless to light pink (KMnO4 in the burette)
PROCEDURE-
1. Fill the burette with KMnO4 solution.
2. Pipette out 10ml. of oxalic acid solution into the conical flask.
3. Add half a test tube of dil. H2SO4 and heat the solution to about 600C to increase
the rate of the reaction.
4. Keep a glazed tile under the burette and place the conical flask on it. 5. Note down the initial reading of the burette.
6. Run down the KMnO4 solution into the conical flask drop wise with shaking.
7. Stop the titration when a permanent pink colour is obtained in the solution. 8. This is the end point. Note down the final burette reading.
9. Repeat the experiment until three concordant values are obtained.
OBSERVATION TABLE: (TO BE PUT UP ON THE BLANK SIDE USING A PENCIL)
Volume of Oxalic Acid solution taken =
S.No BURETTE READINGS VOLUME OF KMnO4
INITIAL FINAL USED (ml) 1
2 3 4 5
Concordant Value =
CALCULATIONS: (TO BE PUT UP ON THE BLANK SIDE USING A PENCIL)
Using formula: N1M1V1 = N2M2V2
Where N1=5 (for KMnO4), V1= , M1 =?
N2=2 (for oxalic acid), V2 =10ml, M2 =
Strength = M X Molar Mass.
RESULT- (ON RULED SIDE ) - The Molarity of KMnO4 =
And the strength of KMnO4 =
EXPERIMENT No. 2 AIM – (a) To prepare 100ml of M/50 solution of Mohr’s salt.
(b) Using this calculate the molarity and strength of the given KMnO4 solution.
APPARATUS AND CHEMICALS REQUIRED- Mohr’s salt, weighing bottle, weight
box, volumetric flask, funnel, distilled water, chemical balance, dilute H2SO4, beakers,
conical flask, funnel, burette, pipette, clamp stand, tile, KMnO4 solution.
THEORY- (a) Mohr’s salt having the formula FeSO4.(NH4)2SO4.6H2O has molar mass
392gmol-1. It is a primary standard.
Its equivalent mass is 392/1 = 392 as its n factor is 1 as per the following reaction: Fe2+
→ Fe3+ + e
-Calculation of amount of Mohr’s Salt to be weighed to prepare 100ml M/20 solution: wt. X 1000
M =
Mol. Wt V(ml)
PROCEDURE:
1. Weigh a clean dry bottle using a chemical balance.
2. Add more weights to the pan containing the weights for the weighing bottle.
3. Add Mohr’s salt in small amounts to the weighing bottle, so that the pans are balanced.
4. Remove the weighing bottle from the pan.
5. Using a funnel, transfer the Mohr’s salt to the volumetric flask.
6. Add about 5ml. of dilute H2SO4 to the flask followed by distilled water and
dissolve the Mohr’s salt.
7. Make up the volume to the required level using distilled water. 8. The standard solution is prepared.
(b) THEORY-
1. The reaction between KMnO4 and Mohr’s salt is a redox reaction and the
titration is therefore called a redox titration.
2. Mohr’s salt is the reducing agent and KMnO4 is the oxidizing agent.
3. KMnO4 acts as an oxidizing agent in all the mediums; i.e. acidic, basic and neutral
medium.
4. KMnO4 acts as the strongest oxidizing agent in the acidic medium and therefore
dil. H2SO4 is added to the conical flask before starting the titration.
5.
IONIC EQUATIONS INVOLVED:
Reduction Half: MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
Oxidation Half: 5Fe2+ → 5Fe3+ + 5e
-Overall Equation: MnO4- + 8H+ + 5Fe2+ → Mn2+ + 5Fe3+ + 4H2O
INDICATOR- KMnO4 acts as a self indicator.
END POINT- Colourless to light pink (KMnO4 in the burette)
PROCEDURE-
1. Fill the burette with KMnO4 solution.
2. Pipette out 10ml. of Mohr’s salt solution into the conical flask. 3. Add half a test tube of dil. H2SO4.
4. Keep a glazed tile under the burette and place the conical flask on it. 5. Note down the initial reading of the burette.
6. Run down the KMnO4 solution into the conical flask drop wise with shaking.
7. Stop the titration when a permanent pink colour is obtained in the solution. 8. This is the end point. Note down the final burette reading.
9. Repeat the experiment until three concordant values are obtained. 10.
OBSERVATION TABLE: (TO BE PUT UP ON THE BLANK SIDE USING A PENCIL)
Volume of Mohr’s salt solution taken =
S.No
BURETT
E READINGS
VOLUME OF KMnO4
INITIAL FINAL USED (ml) 1
2 3 4 5
Concordant Value =
CALCULATIONS: (TO BE PUT UP ON THE BLANK SIDE USING A PENCIL)
Using formula: N1M1V1 = N2M2V2
Where N1=5 (for KMnO4), V1= , M1 =?
N2 =1 (for Mohr’s salt), V2 =10ml, M2 =
Strength = M X Molar Mass.
RESULT- (ON RULED SIDE ) - The Molarity of KMnO4 =
And the strength of KMnO4 =
EXPERIMENT No.3 AIM: To prepare a colloidal sol of starch.
THEORY: Starch forms a lyophilic sol with water which is the dispersion medium. The
sol of starch can be prepared by water to about 1000C. The sol is quite stable and is not
affected by the presence of an electrolytic impurity.
PROCEDURE:
EXPERIMENT OBSERVATION INFERENCE
Take 50 ml of distilled water in a A colourless, transluscent sol is Sol of starch has been prepared beaker and heat it to about 1000C. obtained
Add a thin paste of starch to water with stirring.
RESULT- Colloidal sol of starch has been prepared.
EXPERIMENT No.4 AIM: To prepare a colloidal sol of ferric hydroxide.
THEORY: Ferric hydroxide forms a lyophobic sol with water which is the dispersion
medium. It is prepared by the hydrolysis of ferric chloride with boiling distilled water as per the reaction:
FeCl3 (aq) + 3H2O → Fe(OH)3 + 3HCl (aq).
The HCl formed during the reaction tries to destabilize the sol and therefore should be removed from the sol by dialysis. A wine red sol of ferric hydroxide is obtained.
PROCEDURE:
EXPERIMENT OBSERVATION INFERENCE
Take 50 ml of distilled water in a A wine red sol is obtained Sol of ferric hydroxide has been prepared beaker and heat it to about 1000C.
Add the solution of FeCl3 to water
with stirring.
EXPERIMENT No.5
AIM: To prepare crystals of Mohr’s salt.
THEORY: Mohr’s salt i.e. ferrous ammonium sulphate [FeSO4.(NH4)2SO4.6H2O] is a
double salt. It can be prepared by making equimolar solution of hydrated ferrous sulphate and ammonium sulphate in minimum amount of water. A few ml of dil. H2SO4 is added
to prevent the hydrolysis of FeSO4.7H2O. Cooling of the hot saturated solution yields
light green crystals of Mohr’s salt.
FeSO4.7H2O + (NH4)2 SO4 → FeSO4.(NH4)2SO4.6H2O + H2O
RESULT- Colour of the crystals: Light green
Shape of the crystals: Monoclinic.
NOTE – DRY THE CRYSTALS, PUT THEM IN A ZIP POUCH AND PASTE THEM IN YOUR FILES ON THE BLANK PAGE.
EXPERIMENT No.6 AIM: To prepare crystals of Potash alum.
THEORY: Potash alum, a double salt, commonly known as fitkari has the formula
K2SO4.Al2(SO4)3.24H2O. It can be prepared by making equimolar solution of potassium
sulphate and aluminium sulphate in minimum amount of water. A few ml of dil. H2SO4 is
added to prevent the hydrolysis of Al2(SO4)3.18H2O. Cooling of the hot saturated solution
yields colourless crystals of Potash alum.
K2SO4 + Al2(SO4)3.18H2O + 6H2O → K2SO4.Al2(SO4)3.24H2O
RESULT- Colour of the crystals: Colourless
Shape of the crystals: Octahedral.
NOTE – DRY THE CRYSTALS, PUT THEM IN A ZIP POUCH AND PASTE THEM IN YOUR FILES ON THE BLANK PAGE.
EXPERIMENT No.7
AIM: To separate the coloured components present in a mixture of red and blue ink by
ascending paper chromatography and find their Rf values.
THEORY: In this type of chromatography a special adsorbent paper (Whatman filter
paper) is used. Moisture adsorbed on this Whatman filter paper acts as stationary phase and the solvent acts as the mobile phase. The mixture to be separated is spotted at one end of the paper. This paper is then developed in a particular solvent by placing the paper in a gas jar, taking care that the spot is above the solvent. The solvent rises due to
capillary action and the components get separated out as they rise up with the solvent at different rates. The developed paper is called a chromatogram.
Rf (retention factor) values are then calculated, which is the ratio of the distance
moved by the component to the distance moved by the solvent front. Rf = Distance traveled by the component
Distance traveled by the solvent front
OBSERVATIONS AND CALCULATIONS: ( ON THE BLANK PAGE, USING A PENCIL)
S.No SUBSTANCE DISTANCE TRAVELLED BY DISTANCE TRAVELLED BY Rf VALUE
DIFFERENT COMPONENTS SOLVENT 1 RED + BLUE INK
2 RED + BLUE INK
RESULT: (ON RULED SIDE ) - Rf of blue ink =
Rf of red ink =
NOTE: PASTE THE CHROMATOGRAM ON THE BLANK SIDE AND MARK THE DISTANCE TRAVELLED BY THE INDIVIDUAL COMPONENTS AND THE SOLVENT FRONT USING A PENCIL.
EXPERIMENT No.8
AIM: To test the presence of unsaturation in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE 1 BAEYER'S TEST OR alk.KMnO4 TEST
Dissolve organic compound in water/acetone and add a few drop of
Baeyer's reagent and shake Pink colour of KMnOdecolorizes. 4 Unsaturation present in the organic compound.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
2KMnO4 + H2O → 2KOH + 2MnO2 + 3[O]
>C =C< + H2O + [O] → >C(OH) ─ (OH)C< + KOH
RESULT: (ON RULED SIDE ) Unsaturation is present in the given organic compound.
EXPERIMENT No.9
AIM: To test the presence of alcoholic group in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE 1 CERRIC AMMONIUM NITRATE TEST
Organic compound + few drops of cerric ammonium nitrate solution. Shake well.
A pink or red colour appears.
Alcoholic –OH group present.
2
ESTER TEST
Organic compound + few drops of glacial acetic acid + 1-2 drops of conc. H2SO4 +
warm on water bath for 5 min. Cool and pour into 15ml of Na2CO3 solution. Smell
the contents. A fruity smell is obtained Alcoholic –OH group present
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. ROH + (NH4)2Ce(NO3)6 → (NH4)2[Ce(OR)(NO3)5] + HNO3
Cerric amm. nitrate pink or red 2. ROH + CH3COOH → CH3COOR + H2O
RESULT: (ON RULED SIDE ) - Alcoholic –OH present in the given organic
EXPERIMENT No.10
AIM: To test the presence of phenolic group in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE 1 LITMUS TEST
Organic compound + few drops of blue litmus solution.
Blue litmus turns red. Phenolic –OH group present.
2 NEUTRAL FeCl3 TEST
Organic compound + few drops of neutral FeCl3 solution.
A violet colouration is
obtained. Phenolic –OH group present.
3 LIEBERMANN NITROSO TEST
Organic compound + sodium nitrite + conc. H2SO4
A deep blue or green colouration is obtained which turns red on the addition of water. The blue or green colour reappears on the addition of NaOH.
Phenolic –OH group present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. HO —
(PHENOL)
+ FeCl3 →
2. Phenol (structure) NaNO2 + H2SO4 HO –N=O
↔ O = - NOH conc. H2SO4 / PHENOL(structure)
[HO –N= = OH+] HSO
4- H2O
[HO –N= = O] NaOH Sodium salt of phenol indophenol
Phenol indophenol (red) (blue)
RESULT: (ON RULED SIDE) Phenolic –OH present in the given organic compound.
{ equations are incomplete}
EXPERIMENT No.11
PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 2,4-DNP TEST
Organic compound + 2,4-DNP Crystalline orange
ppt. obtained Carbonyl group present.
2 TOLLEN’S TEST
Organic compound + Tollen’s reagent (amm. silver nitrate solution). Heat on water bath.
A silver mirror is obtained the walls of the test tube.
Aldehydic group present.
3 BENEDICT’S / FEHLING’S TEST Organic compound + Benedict’s reagent/ Fehling’s reagent (A mixture of equal amounts of Fehling’s A and Fehling’s B). Heat.
A brick red ppt. is obtained.
Aldehydic group present.
4 SCHIFF”S TEST
Organic compound + Schiff’s reagent A red/ pink/violet colouration is obtained. Aldehydic group present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. RCHO + NH2NH =
(equation 1 is incomplete)
2. RCHO + 2[Ag(NH3)2]+ + 3OH- → RCOO- + 4NH3 + 2Ag ↓ + 2H2O
3. RCHO + 2Cu2+ + 5OH- → RCOO- + Cu
2O + 3H2O
RESULT: (ON RULED SIDE ) Aldehyde present in the given organic compound.
AIM: To test the presence of ketonic group in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 2,4-DNP TEST
Organic compound + 2,4-DNP Crystalline orange ppt. obtained Carbonyl group present. 2 m-DINITROBENZENE TEST Organic compound + m- dinitrobenzene + NaOH A violet colouration is obtained. Ketonic group present.
3 SODIUM NITROPRUSSIDE TEST
Organic compound + sodium nitroprusside + NaOH
A red colouration is obtained.
Ketonic group present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. CH3COCH3 + OH- → CH3COCH2- + H2O
[Fe(CN)5NO]2 - + CH3COCH2- → [Fe(CN)5NO(CH2COCH3)]3
Nitroprusside ion Red complex
RESULT: : (ON RULED SIDE ) Ketone present in the given organic compound.
AIM: To test the presence of carboxylic acid group in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 LITMUS TEST
Organic compound + blue litmus Blue litmus turns red Carboxylic acid
may be present.
2 SODIUM BICARBONATE TEST
Organic compound + aq. NaHCO3 Brisk effervescence
is obtained.
Carboxylic acid group present.
3 ESTER TEST
Organic compound + few drops of alcohol + 2-3 drops of conc. H2SO4
+ heat on a water bath. Cool the contents and pour them into cold water.
A fruity smell is obtained.
Carboxylic acid group present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. RCOOH + NaHCO3 → RCOONa + H2O + CO2↑
2. RCOOH + CH3CH2OH conc. H2SO4 RCOO CH2CH3
RESULT: : (ON RULED SIDE ) Carboxylic acid present in the given organic
compound.
AIM: To test the presence of amino group in the given organic compound. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 LITMUS TEST
Organic compound + few drops of red
litmus solution. Red litmus turns blue Amino group present.
2 SOLUBILITY TEST
Organic compound + 1-2 ml of dil.HCl. Shake well.
Organic compound dissolves. Amino group present 3 CARBYLAMINE TEST Organic compound + CHCl3 + Alc.KOH. Heat An obnoxious smell is obtained. Primary amine present.
4 AZO DYE TEST
Dissolve organic compound in dil.HCl and cool in ice. Add ice cold NaNO2 solution to it. Mix well.
Add ice cold solution of β- naphthol + NaOH.
A red or orange dye is obtained.
Primary aromatic amino group present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. R-NH2 + HCl → R- NH3+Cl-
amine amine salt
2. R-NH2 + CHCl3 + 3KOH → R- N≡ C + 3KCl + 3H2O
Isocyanide or carbylamine 3. NaNO2 + HCl → HNO2 + NaCl
ArNH2 + HNO2 + HCl → Ar- N+≡ N-Cl + 2H2O
Aromatic Aryldiazonium chloride 10amine (stable between 0- 50C)
β- naphthol (draw structure) + Ar- N+≡ N-Cl → (draw structure of the azo dye
obtained) + NaCl + H2O
RESULT: : (ON RULED SIDE ) Amino present in the given organic compound. NOTE: After performing the carbylamine test add 1ml conc.HCl to the reaction mixture and heat to decompose the isocyanide formed and throw the reaction mixture into running water.
AIM: To test the presence of carbohydrate in the given food sample. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 CONC H2SO4 TEST
Food sample + conc. H2SO4. Heat
Charring occurs with smell of burnt sugar
Carbohydrate present.
2 MOLISCH’S TEST
Food sample + Molisch’s reagent (1%
alcoholic solution of α naphthol) + conc. H2SO4 along the sides of the
test tube.
A purple ring is obtained at the junction of the two layers.
Carbohydrate present.
3 BENEDICT’S / FEHLING’S TEST
Food sample + Benedict’s reagent/ Fehling’s reagent (A mixture of equal amounts of Fehling’s A and Fehling’s B). Heat.
A red ppt. is
obtained. Carbohydratepresent.
4 TOLLEN’S TEST
Food sample + Tollen’s reagent (amm. silver nitrate solution). Heat on water bath.
A silver mirror is obtained the walls of the test tube.
Carbohydrate present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
1. CHO(CHOH)4CH2OH + 2Cu2+ + 5OH- → COOH(CHOH)4CH2OH + Cu2O + 3H2O
Glucose Gluconic acid
2. CHO(CHOH)4CH2OH + 2[Ag(NH3)2]+ + 3OH- → COOH(CHOH)4CH2OH + 4NH3
Glucose (Gluconic acid) + 2Ag ↓ + 2H2O
RESULT: : (ON RULED SIDE ) The food sample has been tested for carbohydrate.
AIM: To test the presence of oil or fat in the given food sample. PROCEDURE:
S.No EXPERIMENT OBSERVATION INFERENCE
1 SOLUBILITY TEST Food sample + water
Food sample + chloroform(CHCl3)
Does not dissolve Miscible
Oil / fat present.
2 SPOT TEST
Smear the food sample on paper. A translucent spot is
observed.
Oil / fat present.
3 ACROLEIN TEST
Food sample + KHSO4. Heat An irritating odour
is obtained.
Oil / fat present.
EQUATIONS: (ON BLANK SIDE USING A PENCIL)
Oil/ fat heat glycerol + fatty acid
CH2 (OH)CH(OH) CH2 (OH) KHSO4, Heat CH2═CHCHO (acrolein) + 2H2O
RESULT: (ON RULED SIDE ) The food sample has been tested for oil/fat
NOTE – THE PARER OBTAINED IN SPOT TEST TO BE PUT IN A ZIP POUCH AND PASTED ON THE BLANK SIDE.
EXPERIMENT No.17
PROCEDURE:
S.No f OBSERVATION INFERENCE
1 BIURET TEST
Food sample + few drops of NaOH + CuSO4 solution.
A violet colouration
is obtained. Protein present.
2 XANTHOPROTEIC TEST
Food sample + few drops of conc. HNO3. Heat.
A yellow ppt. is
obtained. Protein present.
3 NINHYDRIN TEST
Food sample + few drops of 0.15
ninhydrin solution. Boil the contents. A blue colour is obtained. Protein present.