MOUNT LITERA ZEE SCHOOL
NH-92, SAI CITY, UDAYPURA, FARRUKHABAD ROAD, ETAWAH
PRACTICALS 2024 – 25
CHEMISTRY – XI
IMPORTANT INSTRUCTIONS
1. Handwriting and Presentation:
It is crucial to maintain neatness and clarity while writing your practicals in the lab manual. Ensure
that your handwriting is legible and consistent throughout, as this will make your work easier to
understand and evaluate. Messy or unclear handwriting may lead to a loss of marks during assessments.
2. Use of Pen:
Only blue or black pens are permitted for writing the practicals in the lab manual. Make sure to avoid
using any other colors or pencils, as consistency in ink is required for professional presentation. This
also ensures that your notes remain permanent and clear, without fading over time.
3. Dates:
Do not write the dates for the practicals yet. The specific dates on which each practical was performed
will be disclosed at a later time. This step is important to ensure uniformity and accuracy when logging
practical sessions in your manual.
4. Order of Practicals:
Follow the exact sequence provided when documenting the practicals in your manual. Deviating from
the given order may result in confusion or disorganization, which could affect the evaluation of your
work. Adherence to this structure is key to meeting the assessment standards.
5. Instructor Contact for Queries:
Should you encounter any difficulties or require clarification while writing your practicals, you are
encouraged to contact me. Ensure that your concerns are addressed promptly to avoid delays in
completing the manual.
Regards
Shobhit Agrawal
PGT - Chemistry
EXPERIMENT NO. 1
Aim:
N
To prepare oxalic acid solution & with its help determine the normality of given NaOH solution.
20
Apparatus Requirement:
Test tube, burette, pipette, funnel, conical flask, glass rod, beaker etc.
Chemical Requirement:
Oxalic acid, given NaOH solution, distilled water.
Chemical Reaction: (Write on the left side page in front of chemical requirement)
H 2 C2 O4 2 NaOH C2 O4 Na2 2H 2 O
Preparation of Standard Solution: (Write below chemical reaction)
EN .V
w
1000
1 63 100
w
20 1000
w 0.315g
Indicator:
Phenolphthalein.
End Point:
Colorless to permanent pink (NaOH is in burette).
Procedure:
1. Dissolve 0.315 g of oxalic acid in 100 ml of distilled water in a volumetric flask.
2. Rinse and fill the burette with given NaOH solution.
3. Pipette out 20 ml of standard oxalic acid solution in a conical flask and add 1-2 drops of
phenolphthalein in it.
4. Note down the initial reading and start adding NaOH solution from the burette dropwise with
continuous stirring until a permanent pink color is imparted.
5. Note down the final reading and repeat the procedure to get 2 – 3 concordant readings.
Observation:
Volume of Oxalic Burette Reading Volume of NaOH
S. No.
acid taken (in ml) Initial Reading Final Reading used
1 20 0
2 20 0
3 20 0
Calculation: (Write on the left side page in front of observation table)
N 1V1 N 2V2
N1
Result:
The normality of given NaOH solution is _____________.
Remark: Record the readings obtained from the experiment conducted in laboratory & perform
the calculations accordingly to get the final result.
EXPERIMENT NO. 2
Aim:
N
To prepare sodium bicarbonate solution & with its help determine the normality of given HCl
20
solution.
Apparatus Requirement:
Test tube, burette, pipette, funnel, conical flask, glass rod, beaker etc.
Chemical Requirement:
Sodium bicarbonate, given HCl solution, distilled water, methyl orange.
Chemical Reaction: (Write on the left side page in front of chemical requirement)
Na 2 CO3 2 HCl 2 NaCl CO2 H 2 O
Preparation of Standard Solution: (Write below chemical reaction)
EN .V
w
1000
1 53 100
w
20 1000
w 0..265g
Indicator:
Methyl orange.
End Point:
Yellow to permanent pink (HCl is in burette).
Procedure:
1. Dissolve 0.265 g of sodium carbonate in 100 ml of distilled water in a volumetric flask.
2. Rinse and fill the burette with given HCl solution.
3. Pipette out 20 ml of standard sodium carbonate solution in a conical flask and add 1-2 drops of
methyl orange in it.
4. Note down the initial reading and start adding HCl solution from the burette dropwise with
continuous stirring until a permanent pink color is imparted.
5. Note down the final reading and repeat the procedure to get 2 – 3 concordant readings.
Observation:
Volume of Na2CO3 Burette Reading
S. No. Volume of HCl used
taken (in ml) Initial Reading Final Reading
1 20 0
2 20 0
3 20 0
Calculation: (Write on the left side page in front of observation table)
N 1V1 N 2V2
N1
Result:
The normality of given HCl solution is _____________.
Remark: Record the readings obtained from the experiment conducted in laboratory & perform
the calculations accordingly to get the final result.
EXPERIMENT NO. 3
Aim:
To determine acidic & basic radicals present in given inorganic salt.
Apparatus Requirement:
Test tube, boiling tube, test tube holder, conical flask, passing tube, glass rod etc.
Chemical Requirement:
Given salt, dil. HCl, lime water, conc. NaOH, conc. HCl, Nessler’s reagent.
Tests for Acidic Radical
S. No. Experiment Observation Inference
1 Salt solution + Dil. HCl. Brisk effervescences. CO32 may be.
2 Pass the gas in lime water. Lime water turns milky. CO32 is present.
Pass the gas in excess
3 Milkness disappears. CO32 is confirmed.
amount.
Tests for Basic Radical
S. No. Experiment Observation Inference
Original solution + Conc.
1 Ammonical smell. Zero group is present.
NaOH + Heat.
Take a glass rod dipped in
2 conc. HCl over the mouth of White dense fumes. NH 4 is present.
test tube.
Pass the gas in Nessler’s
3 Brown precipitate. NH 4 is confirmed.
reagent.
Result:
The given inorganic salt contains
Acidic radical – CO32
Basic radical – NH 4
EXPERIMENT NO. 4
Aim:
To determine acidic & basic radicals present in given inorganic salt.
Apparatus Requirement:
Test tube, boiling tube, test tube holder, conical flask, glass rod etc.
Chemical Requirement:
Given salt, dil. HNO3, AgNO3 solution, MnO2, Conc. H2SO4, conc. NaOH, Conc. HCl, Nessler’s reagent.
Tests for Acidic Radical
S. No. Experiment Observation Inference
Acidify the salt solution with
White precipitate which is
1 dil. HNO3, boil, cool & add Cl is present.
soluble in NH4OH.
AgNO3 solution.
Heat a pinch of salt with Evolution of greenish yellow
2 Cl is confirmed.
MnO2 and conc. H2SO4. gas.
Tests for Basic Radical
S. No. Experiment Observation Inference
Original solution + Conc.
1 Ammonical smell. Zero group is present.
NaOH + Heat.
Take a glass rod dipped in
2 conc. HCl over the mouth of White dense fumes. NH 4 is present.
test tube.
Pass the gas in Nessler’s
3 Brown precipitate. NH 4 is confirmed.
reagent.
Result:
The given inorganic salt contains
Acidic radical – Cl
Basic radical – NH 4
EXPERIMENT NO. 5
Aim:
To determine acidic & basic radicals present in given inorganic salt.
Apparatus Requirement:
Test tube, boiling tube, test tube holder, conical flask, filter paper etc.
Chemical Requirement:
Given salt, diphenylamine, FeSO4, conc. H2SO4, dil. HCl, KI.
Tests for Acidic Radical
S. No. Experiment Observation Inference
Aqueous solution of salt + NO3 is present.
1 Deep blue color.
diphenylamine.
Salt solution + Freshly
Formation of dark brown
prepared FeSO4 solution, NO3 is confirmed.
2 ring at the junction of liquid
then pour conc. H2SO4 along
layers.
the sides of test tube.
Tests for Basic Radical
S. No. Experiment Observation Inference
1 Original solution + dil. HCl. White precipitate. I group is present.
Boil the precipitate with
Precipitate dissolves in hot
2 water and divide in two
water.
parts.
White crystalline
a) Cool one part of the solution. Pb 2 is present.
precipitate.
To the second part add KI
b) Yellow precipitate. Pb 2 is confirmed.
solution.
Result:
The given inorganic salt contains
Acidic radical – NO3
Basic radical – Pb 2
EXPERIMENT NO. 6
Aim:
To study the change in pH of acetic acid by addition of sodium acetate.
Apparatus Requirement:
Test tube, test tube holder, conical flask, dropper etc.
Chemical Requirement:
Acetic acid, sodium acetate, distilled water, pH paper.
Procedure:
1. In a dry test tube, take 10 ml of acetic acid solution.
2. Put a drop of this solution on pH paper strip & note its color and pH value from the pH chart
paper.
3. Now add 1 g of sodium acetate in the test tube containing acetic acid and determine its pH value
again.
4. Repeat the procedure again with more amount of sodium acetate to find out the change in pH.
Observation:
Color Produced on pH
S. No. Sample Solution Approximate pH
Paper
1 CH3COOH
2 CH3COOH + 1 g of CH3COONa
3 CH3COOH + 2 g of CH3COONa
4 CH3COOH + 3 g of CH3COONa
Result:
The pH of the solution goes on increasing on adding more and more of sodium acetate.
EXPERIMENT NO. 7
Aim:
To study the change in pH of ammonium hydroxide solution by addition of ammonium chloride.
Apparatus Requirement:
Test tube, test tube holder, conical flask, dropper etc.
Chemical Requirement:
Acetic acid, sodium acetate, distilled water, pH paper.
Procedure:
1. In a dry test tube, take 10 ml of ammonium hydroxide solution.
2. Put a drop of this solution on pH paper strip & note its color and pH value from the pH chart
paper.
3. Now add 1 g of ammonium chloride in the test tube containing ammonium hydroxide and
determine its pH value again.
4. Repeat the procedure again with more amount of ammonium chloride to find out the change in
pH.
Observation:
Color Produced on pH
S. No. Sample Solution Approximate pH
Paper
1 NH4OH
2 NH4OH + 1 g of NH4Cl
3 NH4OH + 2 g of NH4Cl
4 NH4OH + 3 g of NH4Cl
Result:
The pH of the solution goes on decreasing on adding more and more of ammonium chloride.
EXPERIMENT NO. 8
Aim:
To study the shift in equilibrium between ferric ions and thiocyanate ions by increasing the
concentration of either of the ions.
Apparatus Requirement:
Test tube, test tube holder, conical flask, dropper etc.
Chemical Requirement:
Ferric chloride, potassium thiocyanate, distilled water.
Procedure:
1. Take 10 ml of 0.01 M ferric chloride in a test tube and add 10 ml of 0.01 M potassium thiocyanate
solution. A deep red color is developed.
2. Dilute the red color by adding 50 ml of distilled water.
3. Put 10 ml of the above in three different test tubes A, B & C respectively.
4. Keep the test tube A for comparison and add 2 ml of 0.01 M ferric chloride in test tube B and
observe the change in intensity of color.
5. Add 2 ml of 0.01 M potassium thiocyanate in test tube C and observe the change in intensity of
color.
Observation:
Volume added to Effect on
[Fe(CNS)]2+ solution Effect on
S. No. intensity of Shift in equilibrium
[Fe(CNS)]2+
FeCl3 KCNS red color
Reference
1 Nil Nil - -
color
Intensity
2 2 ml - Increases Right hand side
increases
Intensity
3 - 2 ml Increases Right hand side
increases
Result:
Increase in concentration of either ions shifts the equilibrium in right hand side.
EXPERIMENT NO. 9
Aim:
To detect the presence of element in given organic compound.
Apparatus Requirement:
Test tube, test tube holder, conical flask, boiling tube, filter paper, fusion tube, china dish etc.
Chemical Requirement:
Given compound, sodium metal, distilled water, FeSO4, FeCl3, conc. HCl.
Procedure:
S. No. Experiment Observation Inference
Preparation of Lassaigne
extract
Fuse a small piece of sodium
in a fusion tube. Add a little
1 organic compound and heat. - -
Plunge it in china dish
containing distilled water,
boil the contents and filter.
The filtrate is Lassaigne
extract.
2 ml of Lassaigne extract + 2
ml freshly prepared FeSO4
2 solution, boil & add few Prussian blue color. Nitrogen is present.
drops of FeCl3 solution and
conc. HCl.
Result:
The given organic compound contains nitrogen.
EXPERIMENT NO. 10
Aim:
To detect the presence of element in given organic compound.
Apparatus Requirement:
Test tube, test tube holder, conical flask, boiling tube, filter paper, fusion tube, china dish etc.
Chemical Requirement:
Given compound, sodium metal, distilled water, acetic acid, lead acetate, sodium nitroprusside solution.
Procedure:
S. No. Experiment Observation Inference
Preparation of Lassaigne
extract
Fuse a small piece of sodium
in a fusion tube. Add a little
1 organic compound and heat. - -
Plunge it in china dish
containing distilled water,
boil the contents and filter.
The filtrate is Lassaigne
extract.
2 ml of Lassaigne extract +
2 2-3 drops of acetic acid + 1 Black precipitate. Sulphur is present.
ml of lead acetate solution.
3 ml of Lassaigne extract +
3 sodium nitroprusside Purple color Sulphur is confirmed.
solution.
Result:
The given organic compound contains sulphur.
