Chemistry Lab Advance Notes, Study notes of Chemistry

Download Chemistry Lab Advance Notes and more Study notes Chemistry in PDF only on Docsity!

CHEMISTRY PRACTICAL MANUAL

XII CBSE

ACADEMIC YEAR 2024 – 2025

INDEX

SL

NO

TOPIC

VOLUMETRIC ANALYSIS

1 VOLUETRIC ANALYSIS – I

2 VOLUETRIC ANALYSIS – II

SYSTEMATIC ANALYSIS OF SIMPLE SALT(S)

1 GENERAL SALT PROCEDURE

SAMPLE SALT ANALYSIS PROCEDURE (AMMONIUM

CHLORIDE )

CONTENT BASED EXPERIMENTS

ORGANIC FUNCTIONAL GROUP ANALYSIS (

CARBOXYLIC ACID / ALDEHYDE / KETONE )

PREPARATION OF ONE LYOPHILIC & ONE LYOPHOBIC

SOL

PREPARATION OF INORGANIC COMPOUNDS ( EITHER

FAS (OR) POTASH ALUM )

CHROMATOGRAPHY

(SEPARATION OF PIGMENTS FROM EXTRACTS OF

LEAVES & FLOWERS BY PAPER CHROMATOGRAPHY &

DETERMINATION OF Rf VALUES )

5 LIST OF INVESTIGATORY PROJECT(S)

VOLUMETRIC ANALYSIS - I

AIM: Prepare 250ml of

𝑀

Ferrous ammonium sulphate (Mohr’s salt). Using this

20

solution Find out the Molarity and Strength of the given KMnO 4

solution.

PRINCIPLE:

Molecular Equations

2KMnO 4

• 3H 2

SO 4

→ K 2

SO 4

• 2MnSO 4

• 3H 2

O + 5

[ O

]

2FeSO 4

(NH 4

) 2

SO 4

. 6H 2

O + H 2

SO 4

[ O

] → Fe 2

(SO 4

) 3

• 2(NH 4

) 2

SO 4

• 13H 2

O] × 5

2KMnO 4

• 8H 2

SO 4

• 10FeSO 4

(NH 4

) 2

SO 4

. 6H 2

O → K 2

SO 4

• 2MnSO 4

• 5Fe 2

(SO 4

) 3

• 10(NH 4

) 2

SO 4

• 68H 2

O

THEORY:

𝑀𝑜𝑙𝑎𝑟i𝑡𝑦 (𝑀) =

𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑡ℎ𝑒 𝑠𝑜𝑙𝑢𝑡i𝑜𝑛 i𝑛 𝑙i𝑡𝑟𝑒

Mass of the solute

( FAS

) = Molarity × Molar mass of the solute × Volume of the solution in litre

1

× 392 ×

250

20 1000

TITRATION: Unknown KMnO

4

Vs Standard FAS

Indicator : Self indicator (KMnO

4

Sl.No.

Volume of

FAS (ml)

Burette Reading (ml)

Volume of

KMnO 4

added (ml)

Concordant

Value (ml)

Initial Final

1 20 ml 0

2 20 ml 0

3 20 ml 0

CALCULATION:

a) Molarity of KMnO 4

Solution:

Molarity of KMnO 4

1

Volume of KMnO 4

1

Molarity of Mohr

′

s salt

M

2

= 0. 05 M

Volume of Mohr

′

s salt(𝑉 2

𝑎 1 × 𝑀 1 × 𝑉 1 = 𝑎 2 × 𝑀 2 × 𝑉 2

𝑎 1 = 5

( 𝑡ℎ𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠 𝑔𝑎i𝑛𝑒𝑑 𝑝𝑒𝑟 𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑢𝑛i𝑡 𝑜𝑓 KMnO 4

i𝑛 𝑡ℎ𝑒 𝑏𝑎𝑙𝑎𝑛𝑐𝑒𝑑 𝑒q𝑢𝑎𝑡i𝑜𝑛

)

𝑎 2 = 1 (𝑡ℎ𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠 𝑙𝑜𝑠𝑡 𝑝𝑒𝑟 𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑢𝑛i𝑡 𝑜𝑓 𝐹𝐴𝑆 i𝑛 𝑡ℎ𝑒 𝑏𝑎𝑙𝑎𝑛𝑐𝑒𝑑 𝑒q𝑢𝑎𝑡i𝑜𝑛)

5 × 𝑀𝑜𝑙𝑎𝑟i𝑡𝑦 𝑜𝑓 𝐾𝑀𝑛𝑂 4

× (𝐶𝑜𝑛𝑐𝑜𝑟𝑑𝑎𝑛𝑡 𝑣𝑎𝑙𝑢𝑒 𝑜𝑓𝐾𝑀𝑛𝑂

4

) = 1 × 0. 05 × 20

Molarity of KMnO 4

1

1 × 0. 05 × 20

5 ×

𝐶𝑜𝑛𝑐𝑜𝑟𝑑𝑎𝑛𝑡 𝑣𝑎𝑙𝑢𝑒 𝑜𝑓 KMnO 4

Molarity of KMnO 4

1

= M

b) Strength of KMnO 4

Solution:

Strength of KMnO 4

solution = Molarity × Molar mass of KMnO 4

= × 158

= g / L

RESULT:

i) Molarity of KMnO 4

solution is = M

ii) Strength of KMnO 4

solution is = g / L

VOLUMETRIC ANALYSIS - II

AIM: Prepare 250ml of

𝑀

Oxalic acid solution Using this solution Find out the

10

Molarity and Strength of the given KMnO 4

solution.

PRINCIPLE:

Molecular Equations

4

2

4

2

4

4

2

[

]

60−70°𝐶

2

2

4

2

𝑂 + [𝑂] →−−−−→ 2 𝐶𝑂

2

2

𝑂] × 5

4

2

4

2

2

4

2

2

4

4

2

2

THEORY:

𝑀𝑜𝑙𝑎𝑟i𝑡𝑦 (𝑀) =

𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑡ℎ𝑒 𝑠𝑜𝑙𝑢𝑡i𝑜𝑛 i𝑛 𝑙i𝑡𝑟𝑒

Mass of the solute

( Oxalic Acid

) = Molarity × Molar mass of the solute × Volume of the solution in litre

1

× 126 ×

250

10 1000

TITRATION: Unknown KMnO

4

Vs Standard Oxalic Acid

Indicator : Self indicator (KMnO

4

Sl.No.

Volume of

Oxalic Acid

(ml)

Burette Reading (ml)

Volume of

KMnO 4

added (ml)

Concordant

Value (ml)

Initial Final

1 20 ml 0

2 20 ml 0

3 20 ml 0

CALCULATION:

a) Molarity of KMnO 4

Solution:

Molarity of KMnO 4

1

Volume of KMnO 4

1

Molarity of 𝑂𝗑𝑎𝑙i𝑐 𝐴𝑐i𝑑

M

2

= 0. 1 M

Volume of 𝑂𝗑𝑎𝑙i𝑐 𝐴𝑐i𝑑(𝑉 2

𝑎 1 × 𝑀 1 × 𝑉 1 = 𝑎 2 × 𝑀 2 × 𝑉 2

𝑎 1 = 5

( 𝑡ℎ𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠 𝑔𝑎i𝑛𝑒𝑑 𝑝𝑒𝑟 𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑢𝑛i𝑡 𝑜𝑓 𝐾𝑀𝑛𝑂 4

i𝑛 𝑡ℎ𝑒 𝑏𝑎𝑙𝑎𝑛𝑐𝑒𝑑 𝑒q𝑢𝑎𝑡i𝑜𝑛

)

𝑎 2 = 2 (𝑡ℎ𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠 𝑙𝑜𝑠𝑡 𝑝𝑒𝑟 𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑢𝑛i𝑡 𝑜𝑓 𝑂𝗑𝑎𝑙i𝑐 𝐴𝑐i𝑑 i𝑛 𝑡ℎ𝑒 𝑏𝑎𝑙𝑎𝑛𝑐𝑒𝑑 𝑒q𝑢𝑎𝑡i𝑜𝑛)

5 × 𝑀𝑜𝑙𝑎𝑟i𝑡𝑦 𝑜𝑓 𝐾𝑀𝑛𝑂 4

× (𝐶𝑜𝑛𝑐𝑜𝑟𝑑𝑎𝑛𝑡 𝑣𝑎𝑙𝑢𝑒 𝑜𝑓𝐾𝑀𝑛𝑂

4

= 2 × 0. 1 × 20

Molarity of KMnO 4

2 × 0. 1 × 20

5 × (𝐶𝑜𝑛𝑐𝑜𝑟𝑑𝑎𝑛𝑡 𝑣𝑎𝑙𝑢𝑒 𝑜𝑓 KMnO 4

Molarity of KMnO 4

1

b) Strength of KMnO 4

Solution:

Strength of KMnO 4

solution = Molarity × Molar mass of KMnO 4

= × 158

= g / L

RESULT:

i) Molarity of KMnO 4

solution is = M

ii) Strength of KMnO 4

solution is = g / L

SYSTEMATIC ANALYSIS OF A SIMPLE SALT

Preliminary Tests

S.NO EXPERIMENT OBSERVATION INFERENCE

Action of Heat:

Little amount of the salt is

heated in a dry test tube.

1. Colourless gas with

pungent smell

1. Presence of

Ammonium salt

2. Yellow when hot and

white when cold

2. Presence of Zinc
3. Reddish brown gas with

fishy odour

3. Presence of Nitrate

salt

4. No characteristic

change

4. Absence of

Ammonium and

Nitrate and zinc salt

Flame Test:

A small amount of the salt is

made into a paste with conc.

HCl in a watch glass and

introduced into the non –

luminous part of the Bunsen

flame.

1. Apple Green flame 1. Presence of Barium

Salt

2. No characteristic flame 2. Absence of Barium

salt

IDENTIFICATION OF ACID RADICALS (ANIONS)

Action of dil. H 2

SO

4

To a little amount of salt,

add 1 – 2mL of dil. H 2

SO

4

1. A colourless, odourless

gas is evolved with brisk

effervescence, which

turns lime water milky

1. Presence of

carbonate

2. No brisk effervescence
   2. Absence of

ccarbonate

Action of Conc. H 2

SO

4

To a little amount of the salt,

add 3 – 4 drops of Conc.

H

2

SO

4

and heat it.

1. Colourless gas giving

dense white fumes with a

glass rod dipped in

NH

4

OH evolved

1. Presence of

Chloride

2. No characteristic change
   2. Absence of

Chloride.

Action of Conc. H 2

SO

4

and

Paper ball

To a little amount of the salt,

add 1mL of Conc. H 2

SO

4

and

Paper ball, heat gently.

1. Reddish brown gas with

irritating smell

1. Presence of Nitrate
2. No reddish brown gas

evolves

2. Absence of Nitrate

Action of Leadacetate

solution:

To a little amount of salt,

add lead acetate solution

1.White precipitate is

obtained.

1. Presence of

Sulphate.

2. No white precipitate.
   2. Absence of

Sulphate.

CONFIRMATORY TESTS FOR ANIONS

Preparation of Original Solution: Little amount of the salt is dissolved in 5mL of distilled

water.

Test for Carbonate:

Dil. HCl test:

To little of the original solution,

add dil. HCl

A colourless, odourless

gas is evolved with brisk

effervescence, which

turns lime water milky

Presence of carbonate

is confirmed

Test for Chloride:

Silver Nitrate test:

To a little of the original solution,

add AgNO 3

solution

Curdy white Precipitate

soluble in ammonium

hydroxide is obtained

Presence of Chloride is

confirmed

Test for sulphate:

Barium Chloride test:

To a little of the original solution,

add BaCl 2

solution

Milky White precipitate

insoluble in conc. HCl is

obtained

Presence of Sulphate is

confirmed

Test for Nitrate:

Brown ring test:

To a little of original solution, add

dil. H 2

SO

4

and then freshly

prepared FeSO 4

and add Conc.

H

2

SO

4

along the side of the test

tube

A brown ring is formed

at the junction of two

liquids

Presence of Nitrate is

confirmed

CONFIRMATORY TEST FOR CATIONS

Test for Ammonium:

To a little of the original

solution, Nessler‟s reagent is

added

Reddish brown precipitate

is obtained

Ammonium is confirmed

Test for Lead:

To a little of original solution,

potassium iodide is added

Yellow precipitate is

obtained

lead is confirmed

Test for Aluminium:

To a little of original solution

sodium hydroxide is added

White precipitate

is obtained.

Aluminium is confirmed

Test for Zinc:

To a little of original solution,

sodium hydroxide is added

white precipitate is

obtained

Zinc is confirmed

Test for Barium:

To a little of original solution,

Potassium chromate is added

Yellow precipitate is

obtained

Barium is confirmed

Test for Magnesium:

To a little of original solution,

Magneson reagent and sodium

hydroxide are added

Blue precipitate is formed Magnesium is confirmed

RESULT:

The given simple salt contains

1. Anion:
2. Cation:

SAMPLE SALT PROCEDURE:

SYSTEMATIC ANALYSIS OF AMMONIUM CHLORIDE

AIM: To analyse the given salt for one anion and one cation present in it.

Preliminary Tests

S.NO EXPERIMENT OBSERVATION INFERENCE

1 Action of Heat:

Little amount of the salt is

heated in a dry test tube.

Colourless gas with pungent

smell

Presence of

Ammonium salt

2 Flame Test:

A small amount of the salt is

made into a paste with conc.

HCl in a watch glass and

introduced into the non –

luminous part of the Bunsen

flame.

No characteristic flame Absence of

Barium salt

IDENTIFICATION OF ACID RADICALS (ANIONS)

3 Action of dil. H 2

SO

4

To a little amount of salt, add 1

• 2mL of dil. H 2

SO

4

and warm

it.

No brisk effervescence Absence of

carbonate

4 Action of Conc. H 2

SO

4

To a little amount of the salt,

add 3 – 4 drops of Conc. H 2

SO

4

and heat it.

Colourless gas giving dense

white fumes with a glass rod

dipped in NH 4

OH evolved

Presence of

Chloride

5 Action of Conc. H 2

SO

4

and

C

To a little amount of the salt,

add few copper turnings and

add 1mL of Conc. H 2

SO

4

and

heat gently.

No reddish brown gas

evolves

Absence of

Nitrate

6 Action of dil. NaOH solution:

To a little amount of salt, add

1mL of NaOH solution and heat

gently

Colourless gas with pungent

smell

Presence of

Ammonium

Confirmatory tests for Anions

Preparation of Original Solution: Little amount of the salt is dissolved in 5mL of distilled

water.

1 Test for Chloride:

Silver Nitrate test:

To a little of the original solution,

add AgNO 3

solution.

Curdy white Precipitate

soluble in ammonium

hydroxide is obtained

Presence of Chloride is

confirmed