CHEMISTRY PRACTICAL NOTEBOOK STANDARD XI
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CHEMISTRY
Standard XI
Practical Notebook
Name of the students :
Name of the Junior college:
Class :
Division :
Roll No. :
Audio - Visual study material about practicals
can be obtained through DIKSHA APP on
your smartphone by using Q.R.Code.
Maharashtra State Bureau of Textbook Production and Curriculum
Research, Pune - 411 004.
A
First Edition : 2019 © Maharashtra State Bureau of Textbook Production and Curriculum Research,
Pune 411 004.
The Maharashtra State Bureau of Textbook Production and Curriculum Research reserves all rights
relating to the practical Notebook. No part of this book should be reproduced without the written
permission of the Director. Maharashtra State Bureau of Textbook Production and Curriculum
Research. 'Balbharati', Senapati Bapat Marg, Pune - 411004.
Subject Committee:
Dr. Chandrashekhar V. Murumkar, Chairman
Dr. Sushama Dilip Joag, Member
Dr. Shridhar Pandurang Gejji, Member
Dr. Satyawati Sudhir Joshi, Member
Dr. Rajashree Vikas Kashalkar, Member
Dr. Laxman Shamrao Patil, Member
Shri. Rajesh Vamanrao Roman
Shri. Rajiv Arun Patole, Member Secretary
Cover and illustration :
Shri. Vivekanand Patil
Shri. Shubham Chavan
Typesetting
DTP Section, Textbook Bureau, Pune
Co-ordination :
Shri. Rajiv Arun Patole
Special Officer for Chemistry
Study group :
Dr. Anjali Deepak Ruikar
Shri. Sachin Ashok Bartakke
Smt. Archana Sanjeev Kale
Smt. Pushpalata Babanrao Gangarde
Smt. Archana Dipak Harimkar
Shri. Vishnu Rustumrao Deshmukh
Shri. Sharad Ajabrao Mankar
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DISCLAIMER Note: All attempts have been made to contact copy righters © but we have not heard from
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B
Foreward
Dear Friends,
The National Curriculum Framework (NCF) 2005 and State Curriculum Frame (SCF)
2010, recommend that children′s life at school must be linked to their daily life. That is why a
new educational system linking school, society and family is forming to replace bookish
education. While the boundaries of different subjects are becoming gray, it has become very
much necessary to develop subject related skills and understanding of the fundamental
concepts, and to cultivate taste for the concerned subject and to nurture analytical and
application oriented abilities among the students.
Chemistry is a subject that must be learnt through experiments and observations.
Laboratory is a place where students have opportunities for clarification of concepts of all
branches of chemistry, e.g. physical chemistry, organic chemistry, analytical chemistry, etc.
Laboratory work includes qualitative analysis experiments like radical detection, analytical
techniques such as filtration, distilation, and quantitative analysis. While performing experiments
in quatitative analysis like titration, students have to estimate the errors in their readings and
observations. These aspects have been covered in the notebook along with supplimentary
information and illustrations, which will facilitate teachers in the proper evaluation of the
students′ work in the laboratory. An opportunity to verify the theoretical part in the textbook
is obtained through the experimental work. All these points are taken into account in this
notebook. It will be possible to evaluate the students, with respect to acquired basic experimental
skills in chemistry, observational methods and accuracy, and calculation abilities.
A detailed procedure is given for the experiments and also activities included in the theory
textbook as per the syllabus. In addition, thought provoking questions based on the practicals
are included. All these should be used not only for the practical examination, but a broader
expectation is that these would be useful for science education through experimental
skill. This notebook could be used as a good supplimentary material for learning
chemistry. QR code is given on first page; by using QR code you can get additional
audio-visual information regarding experiments and activities.
We are sure, you all will welcome this chemistry practical notebook prepared with
due concern and care. Also we take this opportunity to wish you all the best for your
educational career.
(Dr. Sunil Magar)
Director
Pune
Date : 20 June 2019
Bharatiya Saur: 30 Jyeshtha 1941
Maharashtra State Bureau of Textbook
Production and Curriculum Research,
Pune 411 004.
C
General Instructions
Safety guidelines in chemistry laboratory
Do’s
1)
2)
3)
4)
5)
6)
7)
8)
9)
Read the chemical safety information carefully.
Always wear apron or laboratory coat.
Identify the safety equipments.
Use safety goggles whenever necessary.
Handle corrosive chemicals carefully like acids.
Tie long hair back.
Always wash your hands with soap before leaving the laboratory.
In case of any accident, notify the instructor immediately.
Avoid direct contact with chemicals. If chemicals come in contact with your skin or eyes,
flush immediately with copious amount of water and consult with your instructor.
10) Close gas tab before leaving laboratory (if used)
1)
2)
3)
4)
5)
Don’ts
Do not pipette out the solution with mouth. Use of pro-pipette bulb is recommended.
Don’t casually dispose of chemicals down the drain.
Don’t eat or drink in the laboratory.
Don’t play mad scientist.
Don’t haphazardly mix chemicals.
Important: Avoid casual approach towards safety.
Evaluation Scheme of Practical examination in chemistry
First Terminal Practical Examination
Time 2
hours
A
B
C
Std- XI Science
Marks 20
Any one long experiment
(1 hour 30 min)
Passing
Mark 07
10 marks
i) Conduction of experiment
03 marks
ii) Observations
04 marks
iii) Calculation
02 marks
iv) Result with proper unit
01 mark
Any one activity
(30 min)
05 marks
i) Conduction of activity
01 marks
ii) Observation
03 marks
iii) Conclusion/Result
01 mark
Viva / oral based upon experiment / activity performed
during examination
05 marks
(Viva / oral should be taken while experiments / activities are being performed)
D
Handbook and Journal of Experiment in
Subject CHEMISTRY for Std. XI
Annual Practical Examination
Time 3
hours
A
Std – XI Science
Total marks 30
One long experiment Quantitative analysis
1 hour 30 min
Passing
Marks 11
10 marks
i) Conduction of experiment
03 marks
ii) Observations
04 marks
iii) Calculation
02 marks
iv) Result with proper unit
01 mark
OR
B
C
D
long experiment: Qualitative analysis
1 hour 30 min
i) Preliminary Tests
01 mark
ii) Dry tests of basic radical and acidic radical
02 marks
iii) Detection of group of basic radical
01 mark
iv) Detection of basic radical and confirmatory test
02 marks
v) Detection of acidic radical and confirmatory test
02 marks
vi) Result (Basic radical and acidic radical with proper
oxidation state, correct molecular formula and name of
the salt)
02 marks
One short experiment
45 min
05 marks
i) Conduction of experiment
01 marks
ii) Observations
03 marks
iii) Calculation / Conclusion / Result
01 mark
Any one activity
35 min
05 marks
i) Conduction of activity
01 marks
ii) Observation
03 marks
iii) Result / conclusion
01 mark
E
Viva based on experiments / activity performed
during examination
F
Certified laboratory Journal
10 min
05 marks
05 marks
Note: Minimum 15 experiments and 5 activities should
be performed during the year.
1
Index
Sr.
No.
Page
No.
Experiments
Date
Remark
Signature
Introduction to Chemistry laboratory
1
Introduction to apparatus used in chemistry
laboratory.
Basic Chemistry laboratory techniques
2
Study of burner, operating pinch cock /
stopcock and handling of concentrated acid
containers.
Quantitative Analysis (Long Experiments) (Compulsory)
3
To determine concentration in terms of
molarity of NaOH by titrating it against
(0.05M) standard solution of oxalic acid.
4
To determine concentration in terms of
molarity of HCl by titrating it against
(0.05M) standard solution of sodium
carbonate.
Qualitative Analysis (Long Experiment) (Any four water soluble salt)
Detection of one basic radical (cation) and one acidic radical (anion) qualitatively from
given inorganic salt.
5
The given inorganic salt no. 1 contains
1) Basic radical.........2) Acidic radical........
3) Formula of the salt..................................
6
The given inorganic salt no. 2 contains
1) Basic radical.........2) Acidic radical........
3) Formula of the salt..................................
7
The given inorganic salt no. 3 contains
1) Basic radical.........2) Acidic radical........
3) Formula of the salt..................................
8
The given inorganic salt no. 4 contains
1) Basic radical.........2) Acidic radical........
3) Formula of the salt..................................
9
The given inorganic salt no. 5 contains
1) Basic radical.........2) Acidic radical........
3) Formula of the salt..................................
Surface Chemistry (Short Experiments) (Any Two)
10
To prepare colloidal solution of starch.
11
To prepare colloidal solution of ferric
hydroxide [Fe(OH)3]
12
Study of role of emulsifying agent in
stabilizing the emulsion of an oil.
2
Sr.
No.
Page
No.
Experiments
Date
Remark
Signature
Chemical Equilibrium (Short Experiments) (Any One)
13
Study the shift in equilibrium position
between ferric ions and thiocyanate ions by
increasing the concentration of either of the
ions.
14
Study the shift in equilibrium position
between [Co(H2O)6]2+ ions and chloride ions
by increasing the concentration of either of
the ions.
Experiment based on pH change (Short Experiments) (Any One)
15
Study of the pH change in the titration of
strong base (0.1 M NaOH) and strong acid
(0.1 M HCl) using universal indicator.
16
Determination of the pH and nature of
solution of some salts using pH paper or
universal indicator.
(NH4Cl, Na2CO3 , CH3COONa, NaCl,
unknown salt)
Characterization and purification of chemical substances
17
Determination of melting point of given
organic solid.
18
Determination of boiling point of given
organic liquid.
19
Crystallisation of an impure sample of
copper sulfate or benzoic acid.
List of Activities
1
Prepartion of 100 mL of 0.1 M standard
oxalic acid solution.
2
Determination of pH of different fruit juices
by using pH paper or universal indicator.
3
Calibration of pipette by burette.
4
To obtain pure water from impure water
containing ink by simple distillation method
.
5
Checking the adulteration in given food
materials.
6
To determine pH of HCl solution of various
concentrations by using pH paper or
universal indicator.
7
To determine pH of NaOH solution of
various concentrations by using pH paper or
universal indicator.
3
Date:
/
/
Experiment No. 1
Introduction to apparatus used in Chemistry laboratory
In chemistry laboratory students use different apparatus in various experiments. So at first,
students should know the name of each apparatus and its use (Fig. 1.1).
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Fig. 1.1 Chemistry Laboratory apparatus
4
-----------------------------
The most common apparatus used to measure the volume of a solution are :
1. Measuring cylinder
2. Volumetric fl ask
3. Pipette
4. Burette
Measuring cylinders: These are vertical cylindrical glass vessels of different capacities such as
5 mL, 10 mL, 25 mL, 50 mL, 100 mL, 250 mL, 1000 mL, etc. (Fig. 1.2). Measuring cylinders are
used to measure the volume of solution.
Fig. 1.2 Measuring cylinder (100 mL)
Volumetric flasks: These are glass vessels with a fl at bottom and a long neck on which a mark
is etched to show the level to which it is to be filled with a solution. Volumetric fl asks of different
capacities such as 50 mL, 100 mL, 250 mL, 500 mL, 1000 mL, etc. (Fig. 1.3).Volumetric fl asks are
used to prepare standard solution of known concentration.
Fig. 1.3 Volumetric flask (100 mL)
Pipette: It is used for measuring a small definite volume of a solution. It consists of narrow glass
tube blown into a bulb in the middle (Fig.1.4 a and b). At the lower end it is drawn into a jet or
nozzle. A circular mark is etched round the pipette to show the level to which it must be filled so
as to contain the volume stated on its bulb.
Rinsing of pipette: Wash the pipette atleast twice with water and clean it thoroughly before use.
Pipette out a little amount of the solution. Hold the pipette horizontally in your hands and rotate
it slowly so that all of its inner surface is washed with the solution. This process of washing the
pipette with the solution is known as ‘rinsing’. Rinse the pipette atleast twice. The solution used
for rinsing is thrown into the sink. The pipette is thus ready to use.
5
How to use pipette: Now suck fresh volume of the solution into the pipette till the level of the
solution is sufficiently above the mark. At this stage put your dry index finger at once over the
top of the pipette. Gently release the pressure of your index finger, and allow the solution to fl ow
down slowly till its level reaches to etched mark. Arrest the fl ow of the solution by increasing the
pressure of your finger. Hold the pipette vertical and see that the graduation mark is brought in
line with your eye level. The lower meniscus of the solution must be in the line (tangential) with
10
mL
200C
Fig. 1.4 (b) Graduated pipette 10 mL
Fig 1.4 (a) Pipette 10 mL
the etched mark on the pipette. Touch the lower end of the pipette to a clean glass to remove any
adhering drop and then introduce it into the titration fl ask. Remove your index finger. The solution
runs down the pipette into the fl ask leaving a drop of it in the jet or the nozzle. Never blow out this
drop as a pipette is always calibrated to measure the specified volume even when a drop remains
in the nozzle.
Fig 1.5 (a) Burette with stopcock 25 mL
Fig. 1.5 (b) Burette with pinch cock (50 mL)
6
The burette: It is a long glass tube of uniform bore with a stopcock at the bottom. It is used to
deliver a solution for titration. The fl ow of the solution for titration can be regulated or stopped
as desired by means of the stopcock [Fig. 1.5(a)] Sometimes a rubber tube with a pinch cock is
attached to the burette instead of the stopcock [Fig. 1.5 (b)].
How to use burette: The burette is commonly designed to hold 25 mL, 50 mL or 100 mL of the
solution and is graduated in tenths of a mL. The zero mark is always at the top and the final mark
(25, 50 or 100 mL) at the bottom of the burette.
Wash the burette atleast twice with water before use. Then rinse it with the solution (as does in
the case of the pipette). Fill it with the solution sufficiently above the zero mark. Turn the stopcock
or press the pinch cock to allow the solution to run down and fill the nozzle completely. See that
no air bubble is left either in the nozzle or burette. Adjust the level of the solution at the zero
mark. The lower meniscus of the solution must be in line with your eye level and the zero mark.
Always take solution upto the zero mark as the starting point for every titration. (Although it is not
necessary to adjust the burette each time to a zero mark this process avoids the subtraction of two
volumes and hence the possibility of an error.)
Simple method of getting a correct burette reading is to hold a plain white paper behind the
burette. Keep your eye level parallel with the lower meniscus. It is obvious that such a reading is
correct (Fig 1.6, b) while those taken from positions ( a and c) other than this, are incorrect (Fig.1.6 a).
Correct eye level
for reading
Fig 1.6 (a) Incorrect burette reading
Fig. 1.6 (b) Correct burette reading
MCQ
Select [3] or underline the most appropriate answer from the given alternatives of each
sub question.
1. Glass vessel with a fl at bottom and a long neck on which a mark is etched to show the level is
called ................
a. fl at bottom fl ask
b. volumetric fl ask
c. conical fl ask
d. beaker
2. Least count in 100 mL measuring cylinder is ................
a. 10 mL
b) 2 mL
c) 1 mL
d) 0.1 mL
3. The correct burette reading in following diagram is ................
a. 19.5 mL
b. 19.6 mL
c. 19.7 mL
7
d. 19.8 mL
4. What can you do, when last drop of the solution remain in the jet / nozzle of the pipette?
a. Must blow out this drop
b. Never blow out this drop
c. Equal amount of solution is added to solution
d. Remove the drop of solution at any cost.
5. During the observation of burette reading, eye level and solution level in the burette must be in
a. same level
b. slightly upside level
c. slightly below the level
d. middle level
Short answer questions
1. Why it is necessary to rinse the pipette after washing with water?
Ans.....................................................................................................................................................
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2. What will happen if we do not remove the air bubble from nozzle of burette?
Ans.....................................................................................................................................................
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3. What is the simple method of getting a correct reading of burette?
Ans.....................................................................................................................................................
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4. Why it is necessary to rinse the burette after washing with water?
Ans.....................................................................................................................................................
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5. Always take the zero mark of lower meniscus as the starting point for every titration. Give
reason.
Ans.....................................................................................................................................................
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6. Observe the chemistry laboratory apparatus on page no 4. (Fig 1.1) write their names in
space provided.
Remark and sign of teacher: ..................................................................................................
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8
NOTES /CALCULATIONS /ROUGH WORK
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9
Date:
/
/
Experiment No. 2
Basic Chemistry Laboratory Techniques
A) Study of burner
The fl ame with which wax or oil burns is luminous, i.e. light emitting. Luminous fl ame
introduces soot that acts as a reducing agent, hence the fl ame is a reducing fl ame (yellow in color).
This fl ame is rarely used (only for charcoal test) in chemistry laboratory as it does not provide
much heat.
In the year 1855, a German scientist Bunsen designed a burner that is in use even today. This
burner is known as Bunsen burner. It consists of a metal tube with a bore at the base. This bore
is surrounded by a metal collar using which, the bore can be opened or closed (Fig. 2.1).
Outer zone
Inner zone
Colorless fl ame
Upper oxidising zone
Burner tube
Hotest portion of fl ame
Upper reducing zone
Stopcock
Collar
Middle blue zone
Gas tube
Lower reducing zone
Fig 2.1 Bunsen burner
Fig 2.2 Different zones of blue flame
There is a nozzle fitted at the base of the burner. When a jet of fuel gas comes out from the
nozzle with the bore open, air rushes into the tube and a mixture of fuel and air burns at the end of
the metal tube with a blue fl ame.
When the gas burns at the end of metal tube with the bore at base closed, combustion takes
place in restricted supply of air, resulting in yellow or luminous fl ame.
The Fig. 2.2 shows different zones of blue fl ame with which gas burns in Bunsen burner with
the bore open. Outer zone of the fl ame is the hottest zone while inner zone is coldest zone.
B) Operating pinch cock / stopcock
Previously burettes manufactured contained a glass tube calibrated to read volume of solution
in mL, which was fitted to a glass nozzle at the bottom with a rubber tube. The rubber tube is closed
by a pinch cock. By pressing pinch cock with hand, solution from burette can be added dropwise.
However now a days a burette with tefl on stopcock is used instead of a rubber tube with pinch
cock. (Fig 2.3)
10
Burette
Bure e
clamp
Bure e
stand
Stopcock
Erienmeyer
flask
White
porcelain
le
Fig. 2.4 Titration setup
Fig. 2.3 Operating stopcock
C) Handling of concentrated acid containers
Concentrated acids are always kept in glass bottles which are placed in a vessel containing
dry sand. These acids are extremely corrosive to all body tissues, especially eyes and skin. These
acids are highly toxic. However, if handled safely with the right equipment, acids need not be
feared. Use acids confidently by learning how to protect yourself, how to use the proper lab
equipment, what to do in the event of spills and other emergencies and how to dispose used acid.
At first, when you have to take concentrated acid in a test tube, always use test tube holder.
Don’t pipette out concentrated acid by mouth using pipette.
If suppose small amount of acid fall on your skin, don’t wash immediately with water. First
remove that amount of acid by filter paper, napkin or any other cloth. Then wash your, skin by
large amount of water.
When you do such a way there will be little amount of hurt to the skin. If your skin gets
injured by concentrated acid, after washing your skin, do the dressing to the skin by using antiinfl ammatory cream.
After use of concentrated acid, keep the tap of basin on and allow water to fl ush. In this
fl ushing water, pour slowly the used acid in the sink. This is called disposal of acid. Do not throw
concentrated acid directly in basin.
Remark and sign of teacher: ..................................................................................................
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11
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The fl ame with which wax or oil burns is called
a. luminous fl ame
c. oxidizing fl ame
b. non reducing fl ame
d. blue fl ame
2. The figure of Bunsen burner fl ame shows different zones of blue fl ame, which zone of the fl ame
is the hottest zone?
a. Inner zone
c. Outer zone
b. Lower zone
d. Middle zone
3. If acid comes in contact with your skin, then ----- .
a. fl ush immediately with water
b. consult with your instructor
c. take help with laboratory assistant
d. first remove amount of acid with cloth and then fl ush with water.
4. Incorrect statement about easy handling of concentrated acids is ----- .
a. storing the acid in glass containers
b. using a test tube holder while adding it in a test tube
c. using a glass tube with a dropper while adding it in a test tube
d. by pipette out with mouth
Short answer questions
1. Write the name of flame used in charcoal cavity test. Why?
Ans
2. Now a days which type of burette is used instead of rubber tube with pinch cock?
Ans
3. Name the apparatus when you have to take concentrated acid in a test tube?
Ans
4. How would you dispose concentrated acid in sink after use?
Ans
12
5. What is the another name to non-sooty (blue) flame?
Ans
6. Label the given diagram of Bunsen burner with the phrases given below.
1. Burner tube
2. Collar
3. Outer zone
4. Inner zone
5. Gas tube
6. Heat proof surface
7. Gas valve
8. Base of burner
9. Air hole
Remark and sign of teacher: ..................................................................................................
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13
Quantitative Analysis
(Volumetric Analysis)
Introduction: A process of quantitative analysis which involves measurement of volume of
solution of reacting substance is called as volumetric analysis.
The substance or substances to be estimated are in the form of solution. In this process one
solution is subjected to react with another solution of known concentration (standard solution) till
the reaction is complete.
Thus, a volumetric analysis involves a titration between two solutions. The amount of a
substance in the given solutions can be calculated from the volume of standard solution used.
Some Important Terms Used In Volumetric Analysis:
1. Standard solution: It is a solution which contains a known concentration of an element or a
substance.The solution whose concentration is accurately known is called a standard solution. The
concentration of the solution used in volumetric analysis is expressed in terms of molarity.
2. Molarity (M): It represents the number of moles of solute per litre of the solution. The solution
which contains one gram molecular weight or one mol of the solute in one litre of its solution, is
called a molar solution.
? Molarity =
Numbers of gram moles of solute
Volume of solution in litre
Mass of solute in gram
= Molar mass × Volume of solution in litre
? 1M solution means 1 mol of solute per litre of solution.
3. Strength: Amount of the substance in grams dissolved per litre of solution.
? Strength of the solution = Molarity × Molar mass of solute
4. Molar mass: It is an algebraic sum of atomic weights of all the atoms present in a molecule.
5. Titration: The process of carrying out a volumetric analysis by using a suitable standard
solution ,volumetric apparatus and indicator is called titration.
OR
It is the process involvming a chemical reaction between a standard solution and the other
solution whose concentration is to be determined.
Type of Titration: Depending upon nature of reacting species titration methods are generally
classified as followsi. Acidimetric and alkalimetry.
ii. Oxidation-Reduction titration (Redox titration)
iii. Iodometric titration
iv. Precipitation titration
6. Titrant: The term referred to the solution filled in the burette.
7. Titrand: The term referred to the solution taken in the conical fl ask .
14
8. End Point: It is the point when the reaction between the two solutions in a titration has just
been completed. The end point is indicated by a change in color of the reaction mixture during the
reaction.
9. Equivalence Point: It is the point when the reaction between two solutions has been completed
just before color change.
10. Indicator: A substance used in titration to indicate the completion of a reaction (that is end
point) by its change in color is known as an indicator. The choice of indicator depends upon the
nature of acid, base or the substance involved in the titration.
Choice of Indicator in Acid Base Titration
Sr.
No.
1
Acid
Strong
acid
Base
Strong
base
Indicator
Color in acid
solution
Color
in basic
solution
i. Phenolphthalein
Colorless
Pink
ii. Methyl orange
Pink
Yellow
iii. Methyl red
Red
Yellow
2
Strong acid
Weak base
Methyl orange
Pink
Yellow
3
Weak acid
Strong base
Phenolphthalein
Colorless
Pink
15
Date:
/
/
Experiment No. 3
Aim: To determine the molarity of the given solution of sodium hydroxide (NaOH) by titrating it
against standard solution of (0.05M) oxalic acid. (H2C2O4.2H2O).
Apparatus: Burette, pipette, conical fl ask, burette stand, white porcelain tile, etc.
Chemicals: Standard solution of (0.05 M) oxalic acid, NaOH solution, phenolphthalein indicator.
Principle: This is an alkalimetry type of titration. The titration is in between weak acid
(H2C2O4.2H2O) and strong base (NaOH).
Procedure:
1. Wash the burette, pipette and conical fl ask with water.
2. Rinse the burette with given NaOH solution and then fill the burette with NaOH solution
Remove the air bubble from the nozzle and avoid leakage if any.
3. Adjust the level of the solution up to zero mark and fix it on a burette stand.
4. Rinse the pipette with standard oxalic acid solution.
5. Pipette out 10 mL of 0.05M oxalic acid solution and put it carefully in a clean, empty conical
fl ask. Then add 2 drops of phenolphthalein indicator. (The solution remains colorless.)
6. Place the conical fl ask on a white porcelain tile below the burette.
7. Start adding NaOH solution dropwise from the burette in conical fl ask with continuous
stirring, till light / faint pink color is obtained in conical fl ask. Stop adding NaOH, this is the
end point of titration.
8. Keep the fl ask constantly shaking in a circular manner, this is called swirling of solution.
9. See that the color does not disappear even on vigorous shaking. This is the end point of
titration.
10. Note this reading as ‘Pilot’ reading.(Pilot reading is always in whole numbers.)
11. Now fill the burette again with NaOH solution up to the zero mark.
12. Repeat the above procedure and take minimum three more correct burette readings.
13. Note down the constant burette reading .............. ‘x’ mL (C.B.R.)
14. From C.B.R. calculate the molarity of NaOH solution.
Observation:
1. Solution in a burette
2. Solution by a pipette
3. Indicator
4. End point
5. Chemical Equation
Burette reading
Final
Initial
Difference
:
:
:
:
: H2C2O4 + 2NaOH
Na2C2O4 + 2H2O
Observation Table:
Pilot
reading
to
mL
Burette reading in mL
I
II
III
0.0
0.0
0.0
16
C.B.R.
(x) mL
Calculations: From above chemical equation
2 mol of NaOH combines with 1 mol of H2C2O4.2H2O
? 80 g NaOH = 126 g H2C2O4.2H2O
(Molar mass of NaOH = 40 g mol-1, Molar mass of H2C2O4.2H2O = 126 g mol-1)
1. To calculate ‘g’ of NaOH
? 1000 mL 1M H2C2O4 { 80 g NaOH
? 10 mL 1M H2C2O4 { 0.8 g NaOH
? 10 mL 0.05M H2C2O4 { 0.04 g NaOH
Therefore, 0.04 g NaOH is present in .......... (x) mL of NaOH solution of unknown molarity.
? ......... (x) mL NaOH solution contains 0.04 g NaOH
? 1000 mL NaOH solution contains =
1000 × 0.04
........(x)
Space for calculation
2. To calculate molarity of NaOH
?Molarity of NaOH =
=
g of NaOH
1000 × 0.04
........(x) × 40
1
........(x)
Result:
Solution
Molarity
NaOH
.................. M
Remark and sign of teacher: ..................................................................................................
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17
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. A chemical substance indicates completion of the reacting solution by sharp change in its color
is called
a. catalyst
b. an indicator
c. an inhibitor
d. reagent
2. Sodium oxalate is salt of ......
a. strong acid and weak base
b. weak acid and weak base
c. weak acid and strong base
d. strong acid and strong base
3. In the volumetric analysis of NaOH against 0.05M H2C2O4.2H2O constant burette reading was
found to be 9.8 mL. The molarity of NaOH is ..........
a. 0.1020 M
b. 0.1120 M
c. 0.01200 M
d. 0.0980 M
4. Indicator used in the titration of weak acid and strong base is ..........
a. methyl orange
b. phenolphthalein
c. litmus
d. universal indicator
5. When certain volume of one solution completely reacts with the other solution, this stage of
titration is called ..........
a. equivalence point
b. constant burette reading
c. end point
d. initial burette reading
Short answer questions
1. Why molarity is a temperature dependent quantity?
Ans
2. During acid base titration by using phenolphthalein as an indicator, why the color of the
reaction mixture changes from colorless to faint pink?
Ans
3. Calculate the molar mass of the following compounds?
b. Na2CO3 (Atomic mass: C=12, H=1, O=16, S=32 and Na=23)
a. H2SO4
Ans a.
b.
.
4. Define a) molarity b) titrant
Ans a.
b.
.
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18
NOTES /CALCULATIONS /ROUGH WORK
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19
Date:
/
/
Experiment No. 4
Aim: To determine the molarity of the given hydrochloric acid (HCl) solution by using a standard
solution of (0.05M) sodium carbonate (Na2CO3).
Apparatus: Burette, pipette, burette stand, conical fl ask, white porcelain tile, etc.
Chemicals: Standard solution of (0.05 M) Na2CO3, HCl solution, methyl orange indicator.
Principle: This is an acidimetry titration. The titration is between strong acid (HCl) and weak
base (Na2CO3).
Procedure :
1. Wash the burette, pipette and conical fl ask with water.
2. Rinse the burette with given HCl solution and then fill the burette with HCl solution. Remove
the air bubble from the nozzle and avoid leakage if any.
3. Adjust the level of the solution up to the zero mark carefully and fix it on burette stand.
4. Rinse the pipette with Sodium Carbonate solution.
5. Pipette out 10 mL of 0.05 M Sodium Carbonate solution and put it carefully in the conical
fl ask.
6. Add two drops of methyl orange indicator to the solution in the conical fl ask. The solution
becomes yellow in color.
7. Place the conical fl ask on the white porcelain tile below the burette.
8. Start adding HCl solution dropwise from the burette in the conical fl ask with continuous
stirring, till the color of solution changes from yellow to orange pink. Stop adding HCl. This
is end point of the titration.
9. Note this reading as ‘pilot’ reading.
10. Repeat the above procedure and take minimum three more correct burette readings.
11. Note down the constant burette readings ....... x mL (C.B.R.)
Observation:
1. Solution in a burette
2. Solution by a pipette
3. Indicator
4. Color change i.e. end point
5. Chemical equation
:
:
:
:
: Na2CO3 + 2 HCl
2NaCl + H2O + CO2
Observation Table:
Burette
reading
Final
Initial
Difference
Pilot
reading
.................
to
............mL
Burette reading in mL
I
..............
II
..............
0.0
..............
0.0
..............
20
C.B.R.
III
..............
0.0
..............
............ (x) mL
Calculations: From above chemical equation
1 mol of Na2CO3 combines with 2 mol of HCl
? 106 g of Na2CO3 = 73 g of HCl
(Molar mass of Na2CO3 = 106 g mol-1, Molar mass of HCl = 36.5 g mol-1)
1. To calculate ‘g’ of HCl
? 1000 mL of 1M Na2CO3 { 73 g HCl
? 10 mL of 1M Na2CO3{ 0.73 g HCl
? 10 mL of 0.05M Na2CO3 { 0.0365 g HCl
Therefore 0.0365 g HCl is present in ................ (x) mL of HCl solution.
? ....... (x) mL of HCl solution contains 0.0365 g HCl
1000 × 0.0365
? 1000 mL of HCl solution will contain =
...........(x)
g of HCl
2. To calculate molarity of HCl
? Molarity of HCl =
=
Space for calculation
1000 × 0.0365
...........(x) × 36.5
1
...........(x)
Result:
Solution
Molarity
HCl
.................. M
Remark and sign of teacher: ..................................................................................................
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21
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The indicator used in the titration of HCl and Na2CO3 is----a. phenolphthalein
c. universal indicator
b. methyl blue
d. methyl orange
2. A student perform volumetric analysis experiment of HCl against 0.05M Na2CO3 solution,
and record I, II and III burette readings 9.8 mL, 9.6 mL and 9.8 mL, respectively. The constant
burette reading is..........
a. 9.6 mL
b. 9.7 mL
c. 9.8 mL
d. 9.9 mL
3. In the reaction Na2CO3 + 2 HCl o 2 NaCl + H2O + CO2 ; 10 mL of 1M Na2CO3 contains ----grams of HCl (Molar mass: Na2CO3 = 106 g mol-1 and of HCl = 36.5 g mol-1)
a. 0.73 g
b. 0.365 g
c. 3.65 g
d. 7.3 g
4. In the titration of Na2CO3 (in burette) against HCl (in conical fl ask) the color change in conical
fl ask is
a. light orange
b. blue
c. yellow
d. Colorless
5. In titration of Na2CO3 against HCl the burette usually filled with
a. sodium carbonate
c. hydrochloric acid
b. sodium bicarbonate
d. methyl orange
Short answer question
1. Write the chemical reaction when Na2CO3(aq) is titrated against HCl (aq) in volumetric analysis?
Ans
2. Why indicator cannot take part in a chemical reaction?
Ans
3. Calculate the number of moles of HCl present in 500 mL of 0.1M HCl solution.
Ans
4. What are different types of volumetric titration methods?
Ans
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23
Inorganic Qualitative Analysis
Introduction: Qualitative analysis is a branch of chemistry which deals with finding the chemical
composition of unknown substances. In inorganic qualitative analysis the process consists of
finding out basic radical (cation) and acidic radical (anion) present in an inorganic compound.
Qualitative analysis can be performed by using micro scale technique. i.e. quantity about 5
milligrams or volume 0.5 mL.
Detection of one cation and one anion in a given salt:
An ionic compound when dissolved in water gives positive ion and a negative ion. The
positive ion or cation is also called as basic radical and a negative ion or anion is called acidic
radical. In qualitative analysis, we are going to identify a basic radical and an acidic radical from
a simple water soluble salt.
1. Basic radicals (Cations)
Group
Cations
I
II
III A
III B
Pb2+
Cu2+
Al3+, Fe3+
Ni2+, Co2+, Zn2+
IV
V
VI
Ba2+, Sr2+, Ca2+
Mg2+
NH4+
2. Acidic radicals (Anions)
Anions
Cl-, Br-, I-, CO32-, SO32SO42-, PO43NO2NO3CH3COOC2O42-
3. Qualitative analysis of a salt involved the following steps.
a. Preliminary tests
b. Dry tests for basic radical (cations)
c. Dry tests for acidic radical (anions)
d. Preparation of the original solution
e. Wet tests for basic radical (cations)
f. Wet tests for acidic radical (anions)
g. Result
A. Preliminary tests: (General scheme)
Test
Nature
Observation
Inference
Cl, Br, I, NO , SO 2 , etc. may be present.
i. Crystalline (soluble in
water)
ii. Amorphous
iii. Hygroscopic (moist)
3
4
Water insoluble salt may be present like
CO32, S2.
Chlorides or nitrates of Cu2+, Ni2+, Co2+,
Ca2+ may be present
Color of salt
i. Blue
ii. Green
iii. Yellow or Brown
iv. Pink or Violet
v. Light pink or buff
vi. White or colorless
Cu2+ may be present
Ni2+ may be present
Fe3+ may be present
Co2+ may be present
Mn2+ may be present
Pb2+, Al3+, Mn2+, Zn2+, Ba2+, Ca2+, Sr2+, Mg2+,
NH4+ may be present
Solubility
Soluble in water
Crystalline salt present
24
B. Dry Tests for Basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently hold
moist turmeric paper near the
mouth of test tube
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio 1:2
on watch glass, add
few drops of water and prepare a
paste, place this in charcoal cavity
and heat it with a blow pipe in a
reducing fl ame.
Observations
i. Decrepitation
(cracking noise)
ii. Salt fuses
Chloride or nitrites of Na+,
Pb2+, Ba2+ may be present
Salts of Ca2+ and hydrated salt
may be present.
Salt containing water of
crystallization may be
present.
iii. Water vapors
condense on the
cooler part of the test
tube
iv. White sublimate
NH4+ may be present.
v. Residue left in the
test tube
Al3+, Zn2+, Ba2+, Ca2+, NH4+
a. White infusible
may be present
residue
Cu2+, Ni2+, Co2+, Fe3+ may be
b. Colored/ black
present
residue
vi. Colored residue
Hot
Cold
yellow
white
Zn2+ may be present
Pb2+ may be present
brown
yellow
vii. Blue salt turns white Crystalline CuSO4 may be
present
+
Smell of NH3 gas, turning NH4 may be present.
moist turmeric paper
reddish brown
Cu2+ may be present
i. Red scales
Pb2+ may be present
ii. Metallic bead with
yellow incrustation
Pb2+ may be present
iii. Decripitation
iv. White incrustations NH4+ may be present
Zn2+, Al3+, Mg2+, Ba2+, Sr2+
v. White infusible
Ca2+
residue
may be present
vi. Colored or Black,
residue
vii. Residue yellow
when hot and
white when cold
4. Cobalt Nitrate Test:
If white infusible residue is obtained
in charcoal cavity test, add two drops
of cobalt nitrate solution on the white
residue and heat in the blue fl ame.
Inference
i. Residue turns blue
ii. Residue turns pink
iii Residue turns
green
iv Residue turns grey
25
Cu2+, Ni2+, Fe3+, Co2+ may be
present
Zn2+ may be present
Al3+may be present
Mg2+ may be present
Zn2+ may be present
Ba2+, Ca2+ may be present
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame. (non - luminous)
and observe the color of the fl ame
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal of
the salt and heat it again in oxidizing
(blue) fl ame. Observe the color of
the bead.
i. Bluish green
ii. Apple green
iii. Brick red
iv Bluish white
v. No distinct color
Cu2+ may be present.
Ba2+may be present
Ca2+may be present
Pb2+ may be present
Ba2+, Ca2+ may be absent.
i. Greenish blue
ii. Reddish brown
iii. Dark blue
Cu2+ may be present
Ni2+ may be present
Co2+ may be present
C. Dry tests for anions (Acidic radicals)
Test
i. Action of dil HCl:
Salt + dil HCl.
Observation
Inference
i. colorless gas with brisk effervescence CO32- may be present
in cold, turning lime water milky
ii. colorless gas with smell of burning
Sulfur turning acidifid K2Cr2O7 paper
green
SO32- may be present
NO2- may be present
i. colorless gas, giving white dense Cl- may be present
fumes glass rod dipped in NH4OH
iii. Redish brown gas
ii. Action of conc. H2SO4:
Salt + conc. H2SO4+ heat
ii. Brown gas evolve turning moist Br- may be present
starch paper yellow
iii. Brown gas evolve after heating NO3- may be present
does not turn starch paper yellow
iv. violet gas evolved turning starch
I- may be present
paper blue
v. colorless gas with smell of vinegar
CH3COO- may be
present
iii. Action of MnO2 and conc. Colorless gas or greenish yellow gas Cl may be present
turning moist blue litmus paper red
H2SO4:
Salt + a pinch of MnO2 + conc. and then bleaches
H2SO4 and heat
Reddish brown gas turning starch Br- may be present
paper yellowish brown
Light brown fumes, no action on starch NO3- may be present
paper
Violet gas turning starch paper bluish
I- may be present
black
26
iv. Cu-foil test: (If brown gas is
obtained in the above test then
only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
Brown gas, solution turns green
and no action on starch paper
NO3- may be present
(Note: If the anion is not detected in above dry test, then salt may contain SO42- or PO43-)
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of water
in a 50 ml beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
1. O.S. + dil. HCl
Observations
White ppt
No ppt
Black ppt
Inference
Group I (Pb2+) present
Group I absent
Group II (Cu2+) present
No ppt
Group II absent
3. O.S. + NH4Cl + NH4OH till
alkaline
White / brown ppt
Group IIIA (Al3+/ Fe3+) present
No ppt
Group III A absent
4. O.S.+ NH4Cl + NH4OH till
alkaline + H2S gas / H2S
water solution
White / black / pink ppt
Group IIIB (Zn2+/ Ni2+/ Co2+ / Mn2+)
present
Group IIIB absent
Group IV (Ca2+/ Ba2+/ Sr2+) present
Group IV absent
2. O.S. + dil. HCl + H2S gas /
H2S water solution
No ppt
White ppt
No ppt
5. O.S. + NH4Cl + NH4OH till
alkaline + saturated solution
of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till White ppt
alkaline + Na2HPO4
No ppt
7. If all the above groups are
Hence
absent
Group V (Mg2+) present
Group V absent
Group VI (NH4+) present
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group I
Test
O. S.+ dil HCl
Observations
Inference
White ppt
Pb2+ present
C.T. for Pb2+ (Lead)
1. O.S.+ KI Solution
Yellow ppt
Pb2+ confirmed
2. O.S. + K2CrO4 Solution
Yellow ppt
Pb2+ confirmed
Analysis of Group II
Test
O.S. + dil HCl + H2S gas / sol.
C.T. for Cu (Cupric)
1. O.S. + NaOH in excess
2. O.S. + CH3COOH +
K4Fe(CN)6
Observations
Black ppt
Inference
Cu2+ present
Blue ppt
Cu2+ confirmed
Chocolate brown ppt
Cu2+ confirmed
2+
27
Pale blue ppt
Cu2+ confirmed
Observations
Inference
3. O.S. + NH4OH excess
Analysis of Group IIIA
Test
O.S. + NH4Cl + NH4OH till
alkaline
i) White gelatinous ppt
Al3+ Present
ii) Brown ppt
Fe3+ Present
C.T. for Al3+ (Aluminium)
1. O.S .+ NaOH
White ppt soluble in excess of Al3+ confirmed
NaOH and reobtained by adding
NH4Cl
2. O.S. + Na2HPO4
White ppt
Al3+ confirmed
C.T. for Fe3+ (Ferric)
O.S. + NH4SCN
Blood red coloration
Fe3+ confirmed
O.S. + K4[Fe(CN)6]
Deep blue ppt
Fe3+ confirmed
O.S. + NaOH
Green precipitate turns reddish Fe3+ confirmed
brown on exposed to air
Analysis of Group III B
Test
O.S.+ NH4Cl + NH4OH +
H2S gas / water
O.S. + NaOH
Observations
Inference
i) Black ppt
Ni2+ or Co2+ present
ii) White ppt
Zn2+ present
iii) Buff ppt
Mn2+ present
Greenish ppt
Ni2+ is present
Blue ppt
Co2+ is present
OR
Green / Bluish green
Ni2+ is present
Pink / Light pink
Co2+ is present
C.T. for Ni2+ (Nickel)
1.O.S. + NH4OH +
dimethylglyoxime
till
alkaline
Scarlet red ppt
Ni2+ confirmed
2.O.S. + NaOH
Light green ppt soluble in NH4Cl Ni2+ confirmed
3.O.S. + K3Fe(CN)6
(potassium ferricyanide)
Yellowish brown ppt
Observe the color of O.S.
Ni2+ confirmed
C.T. for Co2+ (Cobalt)
i. O.S. + NH4OH + K3Fe(CN)6 Reddish brown ppt
Co2+ confirmed
i. O.S. + NH4SCN + acetone
Blue solution
Co2+ confirmed
ii. O.S. + NaOH solution
Blue ppt turns pink brown on Co2+ confirmed
heating
28
C.T. for Zn2+ (Zinc)
i. O.S. + dil. HCl +K4Fe(CN)6
White ppt
Zn2+ confirmed
i. O.S. + Na2HPO4 solution
White ppt soluble in excess
Zn2+ confirmed
C.T. for Mn2+ (Manganese)
Fleshy ppt
i. O.S. + Na2HPO4 solution
violet coloration
i. O.S. + conc.HNO3+ PbO2,
heat and dilute with water
White ppt turns brown on
iii. O.S. + NH4OH
exposure to air
Analysis of Group IV
Test
i. O.S. + K2CrO4
ii. O. S.+ saturated solution
of (NH4)2SO4 and boil
C.T. for Ba2+ (Barium)
i. O.S.+ K2CrO4
ii. O.S.+ dil H2SO4
Inference
Ba present
ii)No ppt
Sr2+ or Ca2+ present
i) White ppt
Sr2+ present
ii) No ppt
Ca2+ present
2+
Ba2+ confirmed
Yellow ppt
White ppt
Test
Ba2+ confirmed
Sr2+ confirmed
Sr2+ confirmed
Sr2+ confirmed
Observation
White ppt
Test
C.T. for Mg (Magnesium)
i. O.S.+ 2 drops of titan yellow
solution+ 3 drops of 2N NaOH
ii. O.S.+ Hypoiodite reagent
2+
Mn2+ confirmed
Observation
i) Yellow ppt
C.T. for Sr2+ (Strontium)
1. O.S. + (NH4)2 SO4, boil
White ppt
Crimson color to the fl ame
2. O.S. + 2 to 3 drops of
conc. HCl and take it on
platinum foil
3.O.S. + conc. HCl and take Brownish red color spot
drop of it on a paper of add a
drop of sodium rhodizonate
solution
Analysis of Group V.
O.S.+ NH4Cl + NH4OH +
Na2HPO4
Mn2+ confirmed
Mn2+ confirmed
Inference
Mg present
2+
Observation
Rose red color or ppt
Inference
Mg confirmed
Reddish brown color or ppt
Mg2+ confirmed
2+
(Hypoiodite reagent: NaOH solution + equal amount of KI solution + Iodine solution
till the solution becomes yellow)
29
Analysis of Group VI
Test
i. O.S.+ NaOH solution. Heat
Observation
Inference
Smell of NH3
NH4+ present
C.T. for NH4+ (Ammonium)
i. O.S. +2 drops of Nessler’s
Brown precipitate
reagent (2 drops of HgCl2 +
KI drop by drop till scarlet
red ppt formed just dissolves
+ equal amount of NaOH)
ii. O.S. + picric acid (Rub test
tube with glass rod)
NH4 +confirmed
Yellow ppt
NH4+ confirmed
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
i. White ppt soluble in dil.HNO3
CO32-present
acid with effervescence of CO2
which turns lime water milky
SO32-present
ii. White ppt soluble in dil. HNO3
acid with evolution of SO2 gas which
decolorizes KMnO4 solution
iii. White or yellow ppt insoluble in
dil HNO3
Cl-, Br-, I- are present
iv. If no ppt
Cl-, Br-, I-, CO32-
SO 2-are absent
3
Distinction between halides (Cl , Br , I ):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.HNO3)
Test
O.S. + Chloroform + Cl2
water in excess (shake well)
Observations
Inference
i. Chloroform layer is colorless
Cl- present
ii. Chloroform layer is yellow (or
Br-present
yellowish brown)
iii. Chloroform layer is violet/
I-present
pink
Note: (If one of the halide radical is present then further analysis is not necessary.
Perform confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
O.S. + Ba(NO3)2
Observations
i. White ppt, insoluble in dil HNO3
Inference
SO42 present
ii. White ppt, soluble in dil HCl
or dil HNO3 without
effervescence
30
PO42 present
_
3. WET TEST FOR NO2
Test
O.S. + dil.H2SO4 + FeSO4
solution
Observations
i. Deep brown coloration
Inference
NO2 present
-
ii. No deep brown coloration
NO2- present
Observations
i. Evolution of NO2 gas which
turns starch iodidc paper black
Inference
NO3- present
ii. If no evolution of gas
NO3- present
_
4. WET TEST FOR NO3
Test
O.S. + 3-4 drops of
conc.H2SO4+ 2-3 drops
of diphenyl amine
5. WET TEST FOR CH3COO
_
Test
O.S. + FeCl3 solution
6. WET TEST FOR C2O42
Observations
_
Red color appears.
Test
Inference
CH3COO- present
Observations
O.S. +dil. Acetic acid + CaCl2 White ppt is obtained
Inference
C2O42- present
Confirmative tests for acidic radicals
C.T. for CO32 [Carbonate]
Test
i. O.S. + AgNO3 solution
Observations
White ppt soluble in dil. HNO3
Inference
CO32- confirmed
ii. O.S. + Ba(NO3)2 solution
White ppt soluble in dil. HCl
CO32- confirmed
C.T. for SO32- [Sulphite]
Test
Observations
i. O.S. + dil.HCl + K2Cr2O7 sol. Green coloration
Inference
SO32- confirmed
ii. O.S. + dil.HCl + 1-2
drops of KMnO4 solution
iii. O.S. + BaCl2 solution
Pink coloration of KMnO4 dissapper
SO32- confirmed
White ppt soluble in dil. HNO3
SO32- confirmed
iv. O.S. + Ba(NO3)2 solution
White ppt soluble in dil. HCl
SO32- confirmed
Test
i. O.S. + dil.HCl+ 2-3drops
of FeSO4solution
Observations
Brown coloration
Inference
NO2 confirmed
ii. O.S. + AgNO3 solution
White crystalline ppt
NO2- confirmed
iii. O.S. + Acetic acid
+ FeSO4solution
Brown coloration
NO2- confirmed
C.T. for NO2[Nitrite]
-
C.T. for Cl [Chloride]
Test
Observations
Inference
i. O.S.+ MnO2 + 2-3 drops of Greenish yellow gas evolves that turns Cl confirmed
moist blue litmus red and then bleaches it
conc. H2SO4 and heat
31
iii. O.S. + Lead acetate
White ppt
Cl- confirmed
C.T. for Br [Bromide]
Test
i. O.S. + MnO2 + conc. H2SO4
and heat
ii. O.S.+ Lead acetate solution
Observation
Inference
Excess red brown gas evolves
Br- confirmed
Pale yellow ppt soluble in hot
water
Br- confirmed
C.T. for I [Iodide]
Test
Observation
i. O.S. + HgCl2 solution in excess Scarlet ppt
ii. O.S.+ Lead acetate solution
C.T. for NO3 [Nitrate]
Test
Yellow ppt
Inference
I- confirmed
I- confirmed
Observation
i. O.S. + diphenyl amine + conc. Intense blue color
H2SO4
Inference
NO3 confirmed
-
ii. O.S. + conc. H2SO4 heat and
Brown ring forms at the junction NO3- confirmed
of two liquids
cool, add freshly prepared
FeSO4 along sides of the test tube
C.T. for CH3COO [Acetate]
Test
i. O.S. + Neutral FeCl3
iii. O.S. + Ethyl alcohol and
heat carefully
Observation
Blood red color
Fruity smell
Inference
CH3COO- confirmed
CH3COO- confirmed
C.T. for C2O42– [Oxalate]
Test
i. O.S. + Hot acidified KMnO4
Observation
Inference
Decoloration of KMnO4
C2O42- confirmed
C.T. for SO42 [Sulfate]
Test
Observation
Inference
2i. O.S. + Acetic acid + Lead acetate White ppt insoluble in dil. HNO3 SO4 confirmed
but soluble in hot ammonium
solution
acetate
White ppt of BaSO4
SO42- confirmed
ii. O.S. + BaCl2 solution
SO42- confirmed
iii. O.S. + 2 drops of KMnO4 sol. Pink ppt
+ BaCl2 solution
C.T. for PO43- [Phosphate]
Test
Observation
i. O.S. + Ammonium molybdate Canary yellow ppt
solution + conc. HNO3 and heat
ii. O.S. + Neutral FeCl3 solution
Inference
PO4 confirmed
3-
Yellowish white ppt soluble in dil. PO43- confirmed
HCl
32
iii. O.S. + Ba(NO3)2 solution
White ppt soluble in dil. HCl
PO43- confirmed
Result:- Given salt contains
1. Basic radical .......................................................
2. Acidic radical ......................................................
3. Molecular formula of salt .................................
4. Hence the name of the salt ................................ .................................MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The elements of following groups are precipitated in the form of sulfides?
a. I and II
b. II and IIIA
c. II and IIIB
d. IIIB and IV
2. Which of the following Cation (basic radical) belongs to Group IV?
a. Cu2+
b. Ba2+
c. Al3+
d. Mg2+
3. A salt is heated with NaOH produce ammonia gas, which terns color of moist turmeric paper
a. Reddish brown
b. Blue
c. Black
d. Yellow
4. What are the group reagents of group VI?
a. Dil.HCl
b. NH4Cl and NH4OH
c. NH4Cl, NH4OH and Na2HPO4
d. No group reagent
5. The chemical used in the distinction test of chloride, bromide and iodide anions is
a. AgNO3
b. Ba(NO3)2
c. Cl2 water + CHCl3
d. (CH3COO)2 Pb
Short answer questions
1. What is Nessler’s reagent?
Ans
2. Name any two Colored basic radicals?
Ans
3. What is Color of cobalt salt?
Ans
4. Name basic radicals which are absent if given salt is white?
Ans
5. Blue crystals of copper sulfate becomes colorless on heating. Why?
Ans
33
6. What are acidic radicals?
Ans
7. Write the names of chemicals used in preparation of hypoiodite reagent?
Ans
8. Heating is necessary for dry test of nitrate anion, why?
Ans
9. What is decripitation?
Ans
10. Which salts decripitates on heating?
Ans
11. Why do we keep silver nitrate in colored bottle?
Ans
12. Which acidic radicals produce fruity smell?
Ans
Remark and sign of teacher: ..................................................................................................
......................................................................................................................................................
......................................................................................................................................................
34
NOTES /CALCULATIONS /ROUGH WORK
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35
Date:
/
/
Experiment No. 5
Inorganic Qualitative Analysis (Salt no.1)
Aim: Analyse one basic (cation) and one acidic (anion) radical from given inorganic salt.
Apparatus: Test tubes, test tube stand, spatula, glass rod, watch glass, beaker, burner, etc.
A. Preliminary tests: (General scheme)
Test
Observation
Inference
Observations
Inference
Nature
Color of salt
Solubility
B. Dry tests for basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently, hold
moist turmeric paper near the mouth
of test tube.
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio
1:2 on watch glass, add
few drops of water and prepare a
paste, place this in charcoal cavity
and heat it with a blow pipe in a
reducing fl ame.
4. Cobalt Nitrate Test:
If white infusible residue is
obtained in charcoal cavity test, add
two drops of cobalt nitrate solution
on the white residue and heat in the
blue fl ame.
36
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame (non - luminous)
and observe the color of the fl ame
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal
of the salt and heat it again in
oxidizing (blue) fl ame. Observe the
color of the bead.
C. Dry tests for acidic radicals (Anions)
Test
Observation
Inference
i. Action of dil HCl
Salt + dil HCl.
ii. Action of conc. H SO4:
Salt + conc. H2SO4+ heat
2
iii. Action of MnO2 and
conc.H2SO4:
Salt + a pinch of MnO2 + conc.
H2SO4 and heat
iv. Cu-foil test: (If brown gas
is obtained in the above test
then only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
Note: (If the anion is not detected in above dry test, then salt may contain SO42- or
PO43-)
37
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of
water in a 50 mL beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
Observations
Inference
1. O.S. + dil. HCl
2. O.S. + dil. HCl + H2S gas / H2S
water solution
3. O.S. + NH4Cl + NH4OH till
alkaline
4. O.S.+ NH4Cl + NH4OH till alkaline
+ H2S gas /H2S water solution
5. O.S. + NH4Cl + NH4OH till
alkaline + saturated solution
of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till
alkaline + Na2HPO4
7. If all the above groups are absent
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group ..........
Test
Observations
C.T. for.............
1.
2.
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
38
Inference
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
Distinction between halides (Cl–, Br–, I–):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.
HNO3)
Test
Observation
Inference
O.S. + Chloroform + Cl2 water
in excess (shake well)
Note: (If one of the halide radical is present then further analysis is not necessary.
Perform confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
Observation
Inference
Observation
Inference
Observation
Inference
Observation
Inference
O.S. + Ba(NO3)2
3. WET TEST FOR NO2–
Test
O.S. + dil. H2SO4 + FeSO4
solution
4. WET TEST FOR NO3–
Test
O.S. + 3-4 drops of conc.H2SO4
+ 2-3 drops of diphenyl amine
5. WET TEST FOR CH3COO
Test
O.S. + FeCl3 solution
39
6. WET TEST FOR C2O42–
Test
Observation
Inference
Observation
Inference
O.S. +dil. Acetic acid + CaCl2
C.T. for ................................
Test
1.
2.
Result:- Given inoragnic salt no. 1 contains following
1. Basic radical .................................. ................
2. Acidic radical........................................................
3 . Molecular formula of the salt..........................................
4. Hence the name of the salt........................................................................
Remark and sign of teacher: ..................................................................................................
......................................................................................................................................................
......................................................................................................................................................
40
Date:
/
/
Experiment No. 6
Inorganic Qualitative Analysis (Salt no. 2)
Aim: Analyse one basic (cation) and one acidic (anion) radical from given inorganic salt.
Apparatus: Test tubes, test tube stand, spatula, glass rod, watch glass, beaker, burner, etc.
A. Preliminary tests: (General scheme)
Test
Observation
Inference
Observations
Inference
Nature
Color of salt
Solubility
B. Dry tests for basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently, hold
moist turmeric paper near the mouth
of test tube.
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio
1:2 on watch glass, add few drops
of water and prepare a paste, place
this in charcoal cavity and heat
it with a blow pipe in a reducing
fl ame.
4. Cobalt Nitrate Test:
If white infusible residue is
obtained in charcoal cavity test, add
two drops of cobalt nitrate solution
on the white residue and heat in the
blue fl ame.
41
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame (non - luminous)
and observe the color of the fl ame.
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal of
the salt and heat it again in oxidizing
(blue) fl ame. Observe the color of
the bead.
C. Dry tests for acidic radicals (Anions)
Test
Observation
Inference
i. Action of dil HCl
Salt + dil HCl.
ii. Action of conc. H SO4:
Salt + conc. H2SO4+ heat
2
iii) Action of MnO2 and
conc.H2SO4:
Salt + a pinch of MnO2 + conc.
H2SO4 and heat
iv) Cu-foil test: (If brown gas
is obtained in the above test
then only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
Note: (If the anion is not detected in above dry test, then salt may contain SO42- or PO43-)
42
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of
water in a 50 mL beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
Observations
Inference
1. O.S. + dil. HCl
2. O.S. + dil. HCl + H2S gas / H2S
water solution
3. O.S. + NH4Cl + NH4OH till
alkaline
4. O.S.+ NH4Cl + NH4OH till
alkaline + H2S gas/
H2S water solution
5. O.S. + NH4Cl + NH4OH till
alkaline + saturated solution
of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till
alkaline + Na2HPO4
7. If all the above groups are
absent
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group ..........
Test
Observations
C.T. for.............
1.
2.
43
Inference
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
Distinction between halides (Cl–, Br–, I–):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.
HNO3)
Test
Observation
Inference
O.S. + Chloroform + Cl2
water in excess (shake well)
Note: (If one of the halide radical is present then further analysis is not necessary. Perform
confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
Observation
Inference
Observation
Inference
Observation
Inference
Observation
Inference
O.S. + Ba(NO3)2
3. WET TEST FOR NO2–
Test
O.S. + dil. H2SO4 + FeSO4
solution
4. WET TEST FOR NO3–
Test
O.S. + 3-4 drops of conc.
H2SO4 + 2-3 drops of
diphenyl amine
5. WET TEST FOR CH3COO
Test
O.S. + FeCl3 solution
44
6. WET TEST FOR C2O42–
Test
Observation
Inference
Observation
Inference
O.S. +dil. Acetic acid + CaCl2
C.T. for ................................
Test
1.
2.
Result:- Given inoragnic salt no. 2 contains following
1. Basic radical .................................. ................
2. Acidic radical........................................................
3 . Molecular formula of the salt..........................................
4. Hence the name of the salt........................................................................
Remark and sign of teacher: ..................................................................................................
......................................................................................................................................................
......................................................................................................................................................
45
Date:
/
/
Experiment No. 7
Inorganic Qualitative Analysis (Salt no. 3)
Aim: Analyse one basic (cation) and one acidic (anion) radical from given inorganic salt.
Apparatus: Test tubes, test tube stand, spatula, glass rod, watch glass, beaker, burner, etc.
A. Preliminary tests: (General scheme)
Test
Observation
Inference
Observation
Inference
Nature
Color of salt
Solubility
B. Dry tests for basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently, hold
moist turmeric paper near the mouth
of test tube.
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio
1:2 on watch glass, add few drops
of water and prepare a paste, place
this in charcoal cavity and heat
it with a blow pipe in a reducing
fl ame.
4. Cobalt Nitrate Test:
If white infusible residue is
obtained in charcoal cavity test, add
two drops of cobalt nitrate solution
on the white residue and heat in the
blue fl ame.
46
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame (non - luminous)
and observe the color of the fl ame.
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal of
the salt and heat it again in oxidizing
(blue) fl ame. Observe the color of
the bead.
C. Dry tests for acidic radicals (Anions)
Test
Observation
Inference
i. Action of dil HCl
Salt + dil HCl.
ii. Action of conc. H SO4:
Salt + conc. H2SO4+ heat
2
iii. Action of MnO2
and conc.H2SO4:
Salt + a pinch of MnO2 + conc.
H2SO4 and heat
iv. Cu-foil test: (If brown gas
is obtained in the above test
then only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
Note: (If the anion is not detected in above dry test, then salt may contain SO42- or PO43-)
47
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of
water in a 50 mL beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
Observation
Inference
1. O.S. + dil. HCl
2. O.S. + dil. HCl + H2S gas / H2S
water solution
3. O.S. + NH4Cl + NH4OH till alkaline
4. O.S.+ NH4Cl + NH4OH till alkaline
+ H2S gas / H2S water solution
5. O.S. + NH4Cl + NH4OH till alkaline
+ saturated solution of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till
alkaline + Na2HPO4
7. If all the above groups are absent
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group ..........
Test
Observation
C.T. for.............
1.
2.
48
Inference
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
Distinction between halides (Cl, Br, I):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.HNO3)
Test
Observation
Inference
O.S. + Chloroform + Cl2 water
in excess (shake well)
Note: (If one of the halide radical is present then further analysis is not necessary.
Perform confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
Observation
Inference
Observation
Inference
Observation
Inference
Observation
Inference
O.S. + Ba(NO3)2
3. WET TEST FOR NO2–
Test
O.S. + dil. H2SO4 + FeSO4
solution
4. WET TEST FOR NO3–
Test
O.S. + 3-4 drops of conc.H2SO4
+ 2-3 drops of diphenyl amine
5. WET TEST FOR CH3COO
Test
O.S. + FeCl3 solution
49
6. WET TEST FOR C2O42–
Test
Observation
Inference
Observation
Inference
O.S. +dil. Acetic acid + CaCl2
C.T. for ................................
Test
1.
2.
Result:- Given inoragnic salt no. 3 contains following
1. Basic radical .................................. ................
2. Acidic radical........................................................
3 . Molecular formula of the salt..........................................
4. Hence the name of the salt........................................................................
Remark and sign of teacher: ..................................................................................................
......................................................................................................................................................
......................................................................................................................................................
50
Date:
/
/
Experiment No. 8
Inorganic Qualitative Analysis (Salt no. 4)
Aim: Analyse one basic (cation) and one acidic (anion) radical from given inorganic salt.
Apparatus: Test tubes, test tube stand, spatula, glass rod, watch glass, beaker, burner, etc.
A. Preliminary tests: (General scheme)
Test
Observation
Inference
Observations
Inference
Nature
Color of salt
Solubility
B. Dry tests for basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently, hold
moist turmeric paper near the mouth
of test tube.
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio
1:2 on watch glass, add
few drops of water and prepare a
paste, place this in charcoal cavity
and heat it with a blow pipe in a
reducing fl ame.
4. Cobalt Nitrate Test:
If white infusible residue is
obtained in charcoal cavity test, add
two drops of cobalt nitrate solution
on the white residue and heat in the
blue fl ame.
51
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame (non - luminous) and
observe the color of the fl ame.
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal of
the salt and heat it again in oxidizing
(blue) fl ame. Observe the color of the
bead.
C. Dry tests for acidic radicals (Anions)
Test
Observations
Inference
i. Action of dil HCl
Salt + dil HCl.
ii. Action of conc. H SO4:
Salt + conc. H2SO4+ heat
2
iii. Action of MnO2 and
conc.H2SO4:
Salt + a pinch of MnO2 + conc.
H2SO4 and heat
iv. Cu-foil test: (If brown gas
is obtained in the above test
then only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
Note: (If the anion is not detected in above dry test, then salt may contain SO42- or PO43-)
52
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of
water in a 50 mL beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
Observations
Inference
1. O.S. + dil. HCl
2. O.S. + dil. HCl + H2S gas / H2S
water solution
3. O.S. + NH4Cl + NH4OH till alkaline
4. O.S.+ NH4Cl + NH4OH till alkaline
+ H2S gas /H2S water solution
5. O.S. + NH4Cl + NH4OH till alkaline
+ saturated solution of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till alkaline
+ Na2HPO4
7. If all the above groups are absent
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group ..........
Test
Observation
C.T. for.............
1.
2.
53
Inference
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
Distinction between halides (Cl–, Br–, I–):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.
HNO3)
Test
Observation
Inference
O.S. + Chloroform + Cl2
water in excess (shake well)
Note: (If one of the halide radical is present then further analysis is not necessary.
Perform confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
Observation
Inference
O.S. + Ba(NO3)2
3. WET TEST FOR NO2–
Test
Observation
Inference
O.S. + dil. H2SO4 + FeSO4
solution
4. WET TEST FOR NO3–
Test
Observation
Inference
Observation
Inference
O.S. + 3-4 drops of conc.H2SO4
+ 2-3 drops of diphenyl amine
5. WET TEST FOR CH3COO
Test
O.S. + FeCl3 solution
54
6. WET TEST FOR C2O42–
Test
Observation
Inference
Observations
Inference
O.S. +dil. Acetic acid + CaCl2
C.T. for ................................
Test
1.
2.
Result:- Given inoragnic salt no. 4 contains following
1. Basic radical .................................. ................
2. Acidic radical........................................................
3 . Molecular formula of the salt..........................................
4. Hence the name of the salt........................................................................
Remark and sign of teacher: ..................................................................................................
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55
Date:
/
/
Experiment No. 9
Inorganic Qualitative Analysis (Salt no. 5)
Aim: Analyse one basic (cation) and one acidic (anion) radical from given inorganic salt.
Apparatus: Test tubes, test tube stand, spatula, glass rod, watch glass, beaker, burner, etc.
A. Preliminary tests: (General scheme)
Test
Observation
Inference
Observations
Inference
Nature
Color of salt
Solubility
B. Dry tests for basic radicals (Cations)
Test
1. Heating in a dry test tube:Take a small quantity of salt in
a clean, dry test tube and heat it
strongly. Observe the color of the
residue and gas evolved.
2. Test for NH4+
Salt + NaOH, heat gently, hold
moist turmeric paper near the mouth
of test tube.
3. Charcoal cavity test: Take the
salt and solid Na2CO3 in the ratio
1:2 on watch glass, add few drops
of water and prepare a paste, place
this in charcoal cavity and heat
it with a blow pipe in a reducing
fl ame.
4. Cobalt Nitrate Test:
If white infusible residue is
obtained in charcoal cavity test, add
two drops of cobalt nitrate solution
on the white residue and heat in the
blue fl ame.
56
5. Flame test:
Clean a platinum wire with conc.
HCl. Moisten a small quantity of
the substance with concentrated
HCl on watch glass. Dip the cleaned
platinum wire in it and heat it in
oxidizing fl ame (non - luminous)
and observe the color of the fl ame.
6. Borax bead test:
[For colored salt only] Make a small
loop at the end of a clean platinum
wire heat it strongly and dip it in
borax powder.Heat it again till a
glossy bead is obtained. Now touch
the hot bead with a small crystal
of the salt and heat it again in
oxidizing (blue) fl ame. Observe the
color of the bead.
C. Dry tests for acidic radicals (Anions)
Test
Observations
i. Action of dil HCl
Salt + dil HCl.
ii. Action of conc. H SO4:
Salt + conc. H2SO4+ heat
2
iii. Action of MnO2 and
conc.H2SO4:
Salt + a pinch of MnO2 + conc.
H2SO4 and heat
iv. Cu-foil test: (If brown gas
is obtained in the above test
then only perform this test)
Salt + Cu-foil + conc. H2SO4
and heat strongly
57
Inference
Note: (If the anion is not detected in above dry test, then salt may contain SO42- or
PO43-)
D. Preparation of solution (Original Solution): Dissolve about 0.5 gm of salt in 20 mL of
water in a 50 mL beaker. This is called original solution (O.S.)
E. Wet test for basic radical (cations)
Detection of groups
Test
Observations
Inference
1. O.S. + dil. HCl
2. O.S. + dil. HCl + H2S gas/ H2S
water solution
3. O.S. + NH4Cl + NH4OH till alkaline
4. O.S.+ NH4Cl + NH4OH till alkaline
+ H2S gas/ H2S water solution
5. O.S. + NH4Cl + NH4OH till alkaline
+ saturated solution of (NH4)2CO3
6. O.S. + NH4Cl + NH4OH till alkaline
+ Na2HPO4
7. If all the above groups are absent
Analysis of Group: After detection of a particular group do analysis of that group.
Analysis of Group ..........
Test
Observation
C.T. for.............
1.
2.
58
Inference
F. Wet test for acidic radicals:
Detection of acidic radical from water solution:
1. Wet tests for CO32–, SO32–, Cl–, Br –, I–
1. O.S. + AgNO3
Distinction between halides (Cl–, Br–, I–):
Note: (Perform this test only if ppt is obtained for AgNO3 which is insoluble in dil.
HNO3)
Test
Observation
Inference
O.S. + Chloroform + Cl2
water in excess (shake well)
Note: (If one of the halide radical is present then further analysis is not necessary.
Perform confirmatory test for that detected radical.)
2. Wet test for SO42– and PO43–
(This test is required to perform only, if ppt is NOT obtained in AgNO3 test)
Test
Observation
Inference
Observation
Inference
Observation
Inference
Observation
Inference
O.S. + Ba(NO3)2
3. WET TEST FOR NO2–
Test
O.S. + dil. H2SO4 + FeSO4
solution
4. WET TEST FOR NO3–
Test
O.S. + 3-4 drops of conc.
H2SO4 + 2-3 drops of
diphenyl amine
5. WET TEST FOR CH3COO
Test
O.S. + FeCl3 solution
59
6. WET TEST FOR C2O42–
Test
Observation
Inference
Observation
Inference
O.S. +dil. Acetic acid + CaCl2
C.T. for ................................
Test
1.
2.
Result:- Given inoragnic salt no. 5 contains following
1. Basic radical .................................. ................
2. Acidic radical........................................................
3 . Molecular formula of the salt..........................................
4. Hence the name of the salt.........................................................................
Remark and sign of teacher: ..................................................................................................
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NOTES /CALCULATIONS /ROUGH WORK
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61
Surface Chemistry
Theory: Colloid is a state of a substance (matter). A colloid is a heterogeneous system in
which one substance with particle size 1 nm to 1000 nm, dispersed in another substance called
dispersion medium. So colloid is not a substance but a particular state of a substance which
depends on size of particles. Colloids do not pass through animal membrane of parchment
paper.
(Note: 1nm = 1×10-9 m = 1×10-7 cm)
Colloidal system consists of two phases :
a. Disperse phase : It is discontinuous phase of colloidal system having particles of colloidal
size (1 nm to 1000 nm) dispersed in the dispersion medium.
b. Dispersion medium : The medium in which colloidal particles are dispersed is called
dispersion medium. It is a continuous phase of a colloidal system.
Colloidal solutions (sols) are classified into two types :
a. Lyophilic sols : In this type of colloidal solutions (sols), the disperse phase has strong affinity
for the dispersion medium. These are reversible sol as the solid obtained after evaporation of
liquid may be reconverted to the sol by simply shaking with the dispersion medium.
Examples: Starch sol, gum sol etc.
b. Lyophobic sols : In this type of colloidal solutions (sols), the disperse phase has little or
no affinity for the dispersion medium. These are irreversible sol as their precipitated mass
cannot be reconverted to the sol by simply shaking it with the dispersion medium.
Example: Ferric hydroxide sol, Aluminum hydroxide sol etc.
Date:
/
/
Experiment No. 10
Aim: To prepare lyophilic sol (colloid) of starch.
Apparatus: Two beakers (50 mL, 250 mL), glass rod, funnel, filter paper, tripod stand, wire gauze,
burner, etc.
Chemicals: Distilled water, soluble starch (5 g).
Theory: The sols which directly formed simply by mixing substances such as starch, gum, gelatin,
rubber, etc. in liquid dispersion medium (water) are called lyophilic sols.
Starch form a lyophilic sol, when water is used as dispersion medium. The starch sol can be
prepared by heating starch and water at about 100 0C. It is quite stable and is not affected by the
presence of any electrolytic impurity.
Procedure:
1. Take 5 g of starch in a 50 mL beaker and add few drops of distilled water to it and make a thin
paste of starch.
2. Take 100 mL distilled water in a 250 mL beaker and heat water in a beaker till it starts boiling.
3. Pour the paste of the starch slowly with stirring into the boiling water fig. 10.1
4. Continue boiling for about 2-3 minutes and allow the beaker to cool.
5. Filter the containts of beaker through a filter paper fixed in a funnel fig. 10.2.
62
Paste of
starch
Glass rod
Beaker
Wire gauze
Water
Tripod stand
Burner
Fig. 10.1 Pouring of paste of starch in boiling water
Mixture of
solid and
liquid
Stirring
rod
Retort stand
Funnel
Clamp
Filter paper
traps solid
Filtrate (liquid
component of the
mixture)
Fig. 10.2 Filtration
Observations:
Starch forms opaque / transparent sol easily and filtered rapidly through filter paper.
Conclusion:
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63
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. In the lyophilic colloids affinity between the particles of dispersed phase and dispersion medium
is ................
a. strong
b. high
c. low
d. average
2. The lyophilic sol is a
a. irreversible sol
b. reversible sol
c. hydrophobic sol
d. homogeneous colloid
3. In a sol of starch, dispersion medium is ................
a. starch
b. water
c. ethyl alcohol
d. air
4. The colloid of starch in water is ................
a. solid sol
b. emulsion
c. gel
d. sol
5. Which of the following is NOT true about colloidal system?
a. It is heterogeneous
b. Aggregation of molecules or ions
c. The particles are settle down under gravity
d. The particles are invisible under microscope
6. Which one of the following is an example of sol?
a. Butter
b. Jellies
c. Milk
d. Gelatin in water
7. Which one of the following is an example of lyophilic sol?
b. Fe(OH)3 sol
c. As2S3 sol
d. Starch sol
a. Al(OH)3 sol
Short answer questions
1. What is a sol?
Ans.....................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
2. How sols are classified?
Ans....................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
3. What is lyophilic sol?
Ans.....................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
4. Give two examples of lyophilic sols.
Ans.....................................................................................................................................................
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5. Why lyophilic sols are called reversible sols?
Ans.....................................................................................................................................................
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NOTES /CALCULATIONS /ROUGH WORK
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65
Date:
/
/
Experiment No. 11
Aim: To prepare lyophobic sol (colloid) of ferric hydroxide.
Apparatus: Two beakers (250 mL), glass rod, funnel, Bunsen burner, filter paper, dropper etc.
Chemicals: Distilled water, 2 % ferric chloride solution prepared by dissolving 2 g of anhydrous
pure FeCl3 in 100 mL of distilled water.
Theory: Sols which cannot be formed simply by mixing substances such as metals, metal
hydroxides or metal sulfides etc. with liquid dispersion medium (water) are called lyophobic sols
(colloids).These sols are prepared by a separate method. Ferric hydroxide is a lyophobic sol.
Lyo means solvent and phobic means hating. Lyophobic sols are relatively less soluble than
lyophilic sol. Ferric hydroxide sol is prepared by the hydrolysis of ferric chloride with boiling
distilled water.
The reaction can be shown asFeCl3(aq) 3H2O(l) boil
Fe(OH)3(s) + 3HCl(aq)
Procedure:
1. Take 100 mL of distilled water in a clean 250 mL beaker and heat it to boil.
2. Add 2 % of ferric chloride solution dropwise with the help of dropper to the boiling water.
3. Continue heating until deep red or brown solution of ferric hydroxide is obtained.
Note: Add some water to replace the water lost by evaporation during boiling at regular intervals.
4. Keep the containt of the beaker undisturbed for some time at room temperature.
5. Filter the solution to get sol of Fe(OH)3.
2% ferric chloride solution
Glass rod
Beaker
Wire gauze
Tripod stand
Burner
Fig. 11.1 Pouring of 2 % FeCl3 solution in boiling water.
Observation:
Dark red brown sol of ferric hydroxide is formed which cannot be filtered easily through filter
paper.
Conclusion:
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Remark and sign of teacher: ..................................................................................................
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66
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. In lyophobic colloid the affinity between the particles of dispersed phase and dispersion
medium is ...............
a. strong
b. high
c. low
d. average
2. The name of chemical used in preparation of ferric hydroxide sol is ...............
a. ferrous chloride
c. ferric chloride
b. iron (II) chloride
d. ferric sulfate
3. In sol of ferric hydroxide the disperse phase is ...............
a. FeCl3
b. Fe(OH)3
c. water
d. Fe
4. The type of colloid of ferric hydroxide in water is ...............
a. solid sol
b. solid foam
c. gel
d. sol
5. Which one of the following is an example of lyophobic sol?
a. Starch sol
c. Gold sol
b. Gelatin sol
d. Gum sol
6. Which one of the following statement is INCORRECT for lyophobic sol?
a. It has little affinity for the dispersion medium
b. It is reversible in nature
c. It is a hydrophobic sol
d. It is less stable sol
Short answer question
1. What is lyophobic sol (colloid)?
Ans.
2. Classify the following as lyophilic sols and lyophobic sols.
Gold sol, starch sol, gum sol, ferric hydroxide sol, Al(OH)3 sol.
Ans
3. Why lyophobic sol is called irreversible sol?
Ans
Remark and sign of teacher: ..................................................................................................
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67
Date:
/
/
Experiment No. 12
Aim: To study the role of emulsifying agent in stabilizing the emulsion of an oil.
Apparatus: Beakers, test tube stand, test tubes, droppers, stopwatch, etc.
Chemicals: Soap solution detergent solution, paraffin oil, coconut oil, groundnut oil, linseed oil,
engine oil, etc. (any two oils)
Theory:
An emulsion is a mixture of two immiscible liquids. Emulsions prepared by shaking of
two liquids. They are unstable and tends to separate into two layers on standing. In order to get a
stable emulsion, addition of substance is essential called emulsifying agent or emulsifier. Soap and
detergent are acts as emulsifiers.
Soap and detergent are long chain compounds with polar groups. Emulsifier forms an
interfacial film around the droplets of oil or water (disperse phase) and prevent the coalescence of
droplets. Thus emulsion becomes stable.
Procedure:
Take 1 mL paraffin oil in a test tube and 1 mL groundnut oil in another test tube, then add 2
mL distilled water in each test tubes. Mark the liquid junction with marking pencil on both test
tubes. Shake the mixture vigorously and put the test tubes in stands. Start the stopwatch and record
the time required to separate two layers of water and oil in both the test tubes.
Add two drops of soap or detergent solution with the help of dropper in each test-tube
containing mixture. Shake both test-tube vigorously and place in stand and start stop watch. Record
the time required for complete separation of oil and water into two layers.
Observation Table:
Sr.
No.
Emulsion
Time of separation
(s)
I (t1)
II (t2)
Mean
(t1+t2)
2
1
Paraffin oil + water
..............
..............
..............
2
Paraffin oil + water + soap/ detergent
..............
..............
..............
3
Groundnut oil + water
..............
..............
..............
4
Groundnut oil+ water + soap/ detergent
..............
..............
..............
Conclusion: More the time consumed for separation of emulsion more will be the stability of the
emulsion.
Thus order of stability observed as follows.
------------------------------------------------------------------------------------------------------------------Remark and sign of teacher: ..................................................................................................
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68
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. Emulsion is colloidal system in which dispersed phase and dispersion medium are ...............
a. miscible liquids
c. immiscible liquids
b. miscible solids
d. immiscible solid
2. Which of the following is NOT an emulsifier?
a. Soap
b. Shampoo
c. Detergent d. Charcoal
3. Pick out odd emulsifier.
a. Milk
b. Cod liver oil
c. Oil paint d. Sodium lauryl sulfate
4. By addition of emulsifying agents emulsion becomes
a. more stable
c. partially stable
b. unstable
d. highly unstable
5. There are four emulsions namely A, B, C, D take different time to separates in their different
phases. B takes more time than C, C takes more time than D, and D take more time than A.
Which one is more stable emulsion among the given emulsions?
a. A
b. B
c. C
d. D
6. Detergents are used as best emulsifiers because they are ...............
a. non polar compound
b. ionic inorganic compound
c. covalent bonded organic compound
d. long chain compound with polar groups.
7. Milk is .....
a. an emulsion
b. a gel
c. a sol
d. an aerosol
8. When small quantity of an oil paint is stirred in to water, the mixture will be a ...............
a. true solution
c. suspension
b. colloidal solution
d. homogeneous solution
Short answer questions
1. What is an emulsion?
Ans
2. What is emulsifying agent?
Ans
3. What are the types of emulsions?
Ans
4. Give two examples of emulsifying agents.
Ans
Remark and sign of teacher: ..................................................................................................
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69
Date:
/
/
Experiment No. 13
Aim: To study the shift in equilibrium between ferric ions and thiocyanate ions by changing the
concentration of either of ions.
Theory:
Ferric chloride when dissolved in water dissociates as,
FeCl3
Fe3 3Cl–
3+
Fe ions form a complex in aqueous solution as [Fe(H2O)6 ]3+.
Ferric ions react with thiocyanate ion (SCN–) in aqueous solution, yielding bloodred coloration. A series of complexes are formed by Fe3+-SCN-- H2O system by the successive
replacement of water molecules from [Fe(H2O)6 ]3+ complex by SCN- ion.
i. [Fe(H2O)6 ]3+ + SCN–
[Fe(H2O)5(SCN)]2+ + H2O
ii. [Fe(H2O)6 ]3+ + 2SCN–
[Fe(H2O)4(SCN)2]+ + 2H2O
iii. [Fe(H2O)6 ]3+ + 3SCN–
[Fe(H2O)3(SCN)3] + 3H2O
These complexes have blood-red coloration. This fact is utilized in the detection of Fe3 basic
radical by SCN– ion in qualitative analysis. The intensity of blood red coloration depends on
number of SCN– ions in the complex.
Apparatus: Burettes, Five 100 mL beakers and test tubes.
Chemicals: FeCl3 (0.01M), NH4SCN (0.01M) (solutions should be provided to students), distilled
water.
Reaction:
[Fe (H2O)6]3+ + 6SCN[Fe (SCN)6]3– + 6H2O
Procedure:
1. Mix FeCl3 (0.01M), NH4SCN (0.01M) and distilled water in five different 100 ml beakers in
volumes as shown in the following table.
Beaker
0.01M FeCl3
mL
0.01M NH4SCN
mL
Distilled
water mL
Intensity
of color
I
5.0
15.0
5.0
.................
II
5.0
10.0
10.0
.................
III
5.0
5.0
15.0
.................
IV
7.5
15.0
2.5
.................
V
2.5
15.0
7.5
.................
2. Mix the solution well in every beaker and transfer it to five different test tubes.
3. Compare the colors developed in five different test tubes.
Conclusion:
The balanced chemical reaction suggest that for obtaining better yield of the product
[Fe(SCN)6 ]3– (blood red coloration), reactant concentration of FeCl3 and NH4SCN is in ratio 1:3.
Therefore the intensity of color in beaker I is the ideal.
Note: 0.01M FeCl3 and 0.01M NH4SCN.
Remark and sign of teacher: ..................................................................................................
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70
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. Which color obtained when 0.01M FeCl3 solution is mixed with 0.01M NH4SCN solution?
a. Bluish green
b. Blood-red
c. Violet
d. Yellow
2. What is the ratio of reactant concentration of FeCl3 and NH4SCN to give better yield of the
[Fe(SCN)6]3–?
a. 1:1
b. 1:3
c. 3:1
d. 1:2
3. What is the total volume of 0.01M FeCl3, 0.01M NH4SCN and distilled water in each beaker?
a. 10
b. 15
c. 20
d. 25
Short answer questions
1. What is chemical equilibrium?
Ans
2. Which color obtained, when [Fe(H2O)6]3+ treated with NH4SCN?
Ans
3. What is the ratio of concentrated NH4SCN and [Fe(H2O)6]3+ is taken for better yield of
[Fe(SCN)6]3– ?
Ans
4. What is the effect of catalyst on chemical equilibrium?
Ans
5. Chemical equilibrium is dynamic in nature. Justify your answer.
Ans
6. Does law of mass action apply on the following reaction?
[Fe(H2O)6]3+ + 3SCN– o [Fe(SCN)6]3– + 3H2O
Ans
7. How does concentration of reactant affect direction of chemical equilibrium?
Ans
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71
Date:
/
/
Experiment No. 14
Aim: To study the shift in equilibrium between hexaaquacobalt (II) ion [Co(H2O)6]2+ and chloride
ions (Cl-) by changing the concentration of either of the ions.
Theory: When CoCl2 is dissolved in water it ionizes as follows.
CoCl2
Co2+ + 2Cl–
Ionized Co2+ ions form a complex [Co(H2O)6 ]2+ ion with water.
H 2O
H 2O
Co2+ +6 H2O
OH2
CO
OH2
2+
OH2
H2O
OH2 i.e. H2O
OH2
CO
OH2
2+
OH2
OH2
The complex in presence of Cl– ions forms [Co(H2O)6]Cl2 and the color of this complex is
pink. The intensity of the color depends on the concentration of the complex. The equation can
be displayed by changing the concentrations of [Co(H2O)6]2+ and Cl– ions. In general increase in
concentration of reactants shifts the equilibrium in the direction of products and vice versa.
Apparatus: Burette Five 100 mL beakers, test tube, test tube stand
Chemicals: CoCl2 (0.1M), HCl (0.1M) (solutions should be provided to students), distilled water
Reaction:
[Co(H2O)6]2+ + 2 Cl–
[Co(H2O)6]Cl2
Procedure:
1. Mix CoCl2 (0.1M), HCl (0.1M) and distilled water in five different 100 ml beakers in volumes
as shown in the following table.
Beaker
0.1M CoCl2
mL
0.1M HCl
mL
Distilled
water mL
I
10.0
20.0
10.0
II
10.0
30.0
0.0
III
10.0
10.0
20.0
IV
15.0
20.0
5.0
V
5.0
20.0
15.0
Intensity of color
2. Mix well solutions of every beaker and transfer it to five different test tubes.
3. Compare the colors developed in five different test tubes.
Conclusion: The balanced chemical equation suggests that for obtaining better yield of the product
[Co(H2O)6]Cl2 (pink color) reactant concentration of CoCl2 and HCl in the ratio 1:2.
Therefore the intensity of color in beaker I is the ideal. The intensity of color in beaker II and
IV will increase indicating in concentration of product. Whereas in beaker III and IV will decrease
indicating decrease in concentration of product.
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72
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The total volume of 0.1M CoCl2, 0.1M HCl and distilled water in each beaker is
a. 10 mL
b. 20 mL
c. 30 mL
d. 40 mL
2. The color of solution of mixture of 0.1M CoCl2 and 0.1M HCl is .......
a. Red
b. Pink
c. Blue
d. Yellow
3. What is the ratio of reactant concentration of CoCl2 and HCl for obtaining better yield?
a. 1:1
b. 1:2
c. 2:1
d. 1:3
4. In which one of the beaker the intensity of color is an ideal?
a. I
b. II
c. III
d. IV
Short answer questions
1. What is chemical equilibrium?
Ans
2. Which color obtained when [Co(H2O)6]2+ treated with HCl?
Ans
3. What is ratio of concentration of (0.1M) HCl and (0.1 M) CoCl2 is taken for better yield of
[Co(H2O)6]Cl2?
Ans
4. What is effect of catalyst on chemical equilibrium?
Ans
5. Chemical equilibrium is dynamic in nature. Justify your answer.
Ans
6. Does law of mas action apply on the following reaction
[Co(H2O)6]2+ + 2 Cl–
[Co(H2O)6]Cl2?
Ans
7. How does the concentration of reactant affect direction of chemical equilibrium?
Ans
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73
Date:
/
/
Experiment No. 15
Aim: To study the pH change in the titration of strong base (0.1M NaOH) and strong acid (0.1M
HCl) using universal indicator.
Apparatus: Burette, pipette, conical fl ask, beakers, burette stand, funnel, beakers, etc.
Chemicals: 0.1M HCl, 0.1M NaOH, universal indicator.
Theory: The solution of strong base NaOH, due to higher concentration of OH- ions has higher
pH. As HCl is added to the NaOH solution, the pH of the solution decreases which changes the
color of universal indicator which has a wide range of pH from 0 to 14
Procedure:
1. Wash the burette, pipette and conical fl ask with water.
2. Rinse the burette with 0.1M HCl solution and fill it with HCl solution after removing air bubble
from nozzle and adjust lower meniscus of solution at zero mark.
3. Rinse the pipette with 0.1M NaOH solution and pipette out 10 mL of NaOH and transfer in the
conical fl ask.
4. Add 2 to 3 drops of universal indicator into the solution in conical fl ask, shake well, observe the
violet color of solution and record the pH of the solution.
5. Add a drop of 0.1M HCl solution from the burette in conical fl ask till the color of the solution
changes to indigo color. Note the burette reading.
6. Continue addition of 0.1M HCl solution from the burette dropwise, till the color of the solution
changes to blue, then green, yellow, orange and finally red which indicates changes in pH of
solution.
7. Note down the burette readings corresponding to each color change.
8. Don’t fill the burette with HCl solution till color changes from indigo to red.
Observation:
1. Solution in burette : ................................
2. Solution in conical fl ask : ......................
3. Indicator : ............................
Observation Table:
Sr.
No.
1
Color of
solution
Indigo
2
Blue
3
Green
4
Yellow
5
Orange
6
Red
Volume of 0.1M HCl
from burette in mL
pH
Nature
Conclusion:
The pH of the solution goes on decreasing on addition of 0.1M HCl from the burette. The
different concentration of H+ ions gives different colors with universal indicator.
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74
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. In the titration of strong base 0.1M NaOH aginst 0.1M HCl solution, using universal indicator,
the color of the solution changes to blue then pH of the solution is
a. zero
b. 4
c. 7
d. 8
2. In the titration of strong base (0.1M NaOH) aginst 0.1M HCl solution, using universal indicator,
the pH of the solution change to 6 then the color of the solution in the fl ask becomes ...........
a. blue
b. yellow
c. orange base d. green
3. In the titration of strong base 0.1M NaOH aginst 0.1M HCl solution, using universal indicator
the pH of the solution (in the conical fl ask) becomes 1, the nature of fl ask solution is ...........
a. strongly acidic
b. strongly basic
c. weekly acidic
d. neutral
4. In the titration of strong base 0.1M NaOH aginst 0.1M HCl solution, using universal indicators,
the color of the fl ask solution becomes green, what is the burette reading of HCl solution?
a. 10 mL
b. 8 mL
c. 12 mL
d. 6 mL
5. In the titration of strong base 0.1M NaOH aginst 0.1M HCl solution, using universal indicator,
the color of the solution in the fl ask becomes blue the nature of fl ask solution is
a. strongly acidic
b. strongly basic
c. weakly basic
d. neutral
6. What is the color of the solution in conical fl ask, when 10 mL of 0.1M NaOH is neutralized by
0.1M HCl solution?
a. Blue
b. Green
c. Yellow
d. Orange
Short answer questions
1. Why is in given experiment color of the solution changes?
Ans
2. What is color of universal indicator in strong acidic and strong basic medium?
Ans
3. What is change in pH of the 0.1M NaOH while adding 0.1M HCl from the burette?
Ans
4. Why universal indicator is better than litmus paper?
Ans
5. If the color of universal indicator changes from green to yellow, predict the change in pH.
Ans
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75
Date:
/
/
Experiment No. 16
Aim: To determine the pH and nature of salt solution (NH4Cl, Na2CO3, CH3COONa, NaCl) using
pH paper or Universal indicator
Apparatus: Five Test tubes, dropper, test tube stand, etc.
Chemicals: 1 gram of each salt NH4Cl, Na2CO3, CH3COONa and NaCl
Theory: Salts when dissolved in water, undergo hydrolysis and produce acidity, alkalinity (basicity)
or neutrality in the solution, depending upon the nature of the salts.
NH4Cl + H2O
NH4OH + HCl
(Acidic)
Na2CO3 + 2H2O
2 NaOH + H2CO3 (Basic)
CH3COONa + H2O
CH3COOH + NaOH (Basic)
NaCl + H2O
NaOH + HCl (Neutral)
Procedure:
1. Dissolve 1 gm of each salt in 10 mL of distilled water in four different clean test tubes marked
A, B, C and D.
2. Add two to three drops of Universal indicator or dip one small strip of pH paper in each of the
test tubes marked A, B, C and D.
3. Observe the color developed in the solution or pH paper strips and note the corresponding pH
values. (Take one unknown salt and prepare its solution and find out its pH)
Yellow
Observation and result table:
Test
Tube
A
Red
Green
Fig. 16.1 Color of salts
Salt solution Color of pH paper/color
of solution
NH4Cl
B
Na2CO3
C
CH3COONa
D
NaCl
E
Unknown
Blue
pH of
solution
Nature of
solution
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76
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The pH of aqueous solution of NH4Cl salt is
a. ! 7
c. 7
b. equal to 7
d. between 7 to 14
2. The nature of aqueous solution of CH3COONa is
a. basic
c. neutral
b. acidic
d. amphoteric
3. The pH of aqueous solution of NaCl is
a. 7
c. 7
b. ! 7
d. zero
4. When pH paper is dipped in the aqueous solution of Na2CO3 the pH paper develop ----- color.
a. yellow
c. blue
b. green
d. orange
5. The nature of aqueous solution of Na2CO3
a. basic
c. neutral
b. acidic
d. amphoteric
6. When a strip of pH paper is dipped in aqueous solution of NH4Cl the pH paper develops-----color.
a. yellow
c. blue
b. green
d. red
7. Which of the following salt does not undergo hydrolysis?
a. NH4Cl
c. Na2CO3
b. KCl
d. CH3COONa
Short answer questions
1. Write chemical reaction for the hydrolysis of a salt of weak acid and strong base.
Ans
2. Write name and chemical formula of a salt of strong acid and strong base.
Ans
3. When water is added in NaCl, it will undergo hydrolysis or not? Why?
Ans
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77
Date:
/
/
Experiment No. 17
Aim: To determine melting point of given organic compound.
Apparatus: Thiele’s tube, retort stand with clamps thermometer, capillary tube, thread, burner etc.
Chemicals: Given organic compound, liquid paraffin
Theory: A pure organic compound possesses characteristic physical properties such as refractive
index, specific gravity, melting point, boiling point etc. However for practical purpose in laboratory
melting point and boiling point are used as criteria for purity. A pure organic solid has a definite
and sharp melting point, while an impure substance has a lower and indefinite melting point.
The melting point of a substance is the temperature at which the solid and liquid phases exist in
equilibrium with each other.
Procedure: Take a small capillary tube and seal it at one end by heating. Fill the finely powdered
dry organic compound (about 1 cm in height) in the capillary tube by tapping it on porcelain tile.
Tie the capillary tube to the thermometer such that bulb of thermometer and organic substance are
at the some level. Now, suspend the thermometer in Thiele’s tube containing liquid paraffin such
that it should not touch the sides of the Thiele’s tube. Heat gently the side arm only with wavy
fl ame. Stop heating Thieles tube when solid starts melting. Record the temperature when solid is
completely melts. This temperature is melting point of given organic compound.
Observation: Melting point of given compound = -------- 0C
= (-------- 0C+ 273) K = -------- K
Table: Melting point of some organic
compounds
Sr.
No.
Compounds
Melting
Point (0C)
1
Naphthalene
80
2
Oxalic acid
101
3
E-naphthol
122
4
Benzoic acid
122
Fig. 17.1 Determination of melting point
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78
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. Melting point of a solid is
a. The temperature at which a solid is in equilibrium with its liquid, at 1atm pressure.
b. The temperature at which a liquid is in equilibrium with its gas, at 1atm pressure.
c. The temperature at which the vapor pressure of the liquid is equal to atmospheric pressure.
d. The temperature at which solid in capillary tube start melting
2. In the determination of melting point of a solid, the solid in small quantity is filled in a .......
a. fusion tube
b. capillary tube with one sealed end.
c. Thiele’s tube containing paraffin liquid.
d. capillary tube with both open end.
3. Melting point is a criteria of purify of a organic solid because
a. a pure liquid boil sharply at a definite temperature.
b. a pure solid melts sharply at a definite temperature.
c. a pure solid melts at some higher temperature than its melting point.
d. a pure liquid boils at some lower temperature than its boiling point
4. The melting point of oxalic acid is
a. 80 0C
b. 101 0C
c. 110 0C
d. 122 0C
5. In the determination of melting point, Thiele’s tube is filled with paraffin oil because
a. paraffin oil has high boiling point
b. paraffin oil is chemically highly reactive
c. paraffin oil undergo decomposition
d. paraffin oil react solid quickly.
6. The temperature in 0C is converted into Kelvin by addition of
a. 0
b. 100
c. 273
d. 373
Short answer questions
1. Define melting point.
Ans
2. What is criteria of purity of solid substances?
Ans.
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79
Date:
/
/
Experiment No. 18
Aim: To determine the boiling point of an organic compound.
Apparatus: Thiele’s tube, retort stand with clamps thermometer, capillary tube, fusion tube,
thread, burner, etc.
Chemicals: Given organic liquid compound, liquid paraffin.
Theory: Boiling point of a liquid, is the temperature at which vapor pressure of a liquid is equal
to the external atmospheric pressure. (Boiling point changes with change in external pressure.)
Procedure:
1. Fill small quantity of given organic liquid in a fusion tube.
2. Take a capillary tube seal its one end by mean of heating and place it in a fusion tube inverted
(sealed end upward and open end dipped in the liquid.)
3. Tie the fusion tube near the bulb of the thermometer by thread.
4. Now, suspend the thermometer tied with fusion tube in Thiele’s tube containing liquid paraffin
such that it should not touch the sides of the Thiele’s tube and organic liquid in fusion tube
should be completely dipped in paraffin. Precaution should be taken such that paraffin should
not be enterd in fusion tube.
5. Heat gently the side arm with waving fl ame.
6. Stop the heating, when bubbles start coming out from the open end of the capillary tube.
7. Record the temperature when continues bubbling in fusion tube is stop and liquid rises in the
capillary.
Fig. 18.1 Determination of boiling point
Observation: Boiling point of given organic compound = ------- 0C
= (...........0C+ 273) K = ------ K
Note: Minimum two different oraginc liquid compounds should be taken for this experiment.
Table:
Sr. No.
1
2
Compounds
Acetone
Acetic acid
Boiling Point (0C)
56
118
3
4
Aniline
Ethyl alcohol
184
78
80
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The boiling point of a liquid is the temperature at which
a. vapor pressure of liquid is higher than external pressure
b. vapor pressure of liquid is lower than external pressure
c. vapor pressure of liquid is equal to the external pressure
d. the external pressure is equal to atmospheric pressure
2. The boiling point of acetone in Kelvin is ------a. 273 K
c. 329 K
b. 356 K
d. 423 K
3. Which of the following apparatus is use for the determination of temperature?
a. Thermometer
c. Speedometer
b. Barometer
d. Colorimeter
4. In which of the following stage, boiling point of organic liquid is to be recorded?
a. At the time of heating Thiele’s tube
b. Continuous stream of bubbles start coming
c. Last bubble is given out and liquid raise in capillary
d. When first bubble comes out of capillary
Short answer questions
1. Define the term boiling point.
Ans
2. What is criteria of purity of liquid substances?
Ans
3. Draw neat label diagram of determination of boiling point of liquid.
Ans:
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81
Experiment No. 19
Date:
/
/
Aim: To prepare pure crystals of copper sulfate (CuSO4.5H2O) or benzoic acid C6H5-COOH from
a given impure sample.
Theory: Generally the substance is more soluble at higher temperature in a given solvent.
In chemistry, recrystallization is a technique use to purify chemicals. By dissolving both impurities
and a compound in an appropriate solvent, either the desired compound or impurities can be
removed from the solution, leaving the other behind with filter paper.
Apparatus: Glass beakers, glass rod, funnel, filter paper, evaporating dish, wire gauze, tripod
stand, Bunsen burner, etc.
Procedure:
1. 5 gm of an impure sample of copper sulfate or benzoic acid is dissolved at high temperature in
minimum quantity of water.
2. The solution is heated to get the saturated solution. This hot solution is filtered to remove
insoluble impurities, evaporate this solution in evaporating dish.
3. The filtrate is allowed to cool slowly to room temperature when fine crystals of pure substance
are formed.
4. These crystals are removed from the mother liquor by filtration and washed with the same
solvent to remove adhered impurities. Theses crystals are then dried.
Step1
Step2
evaporating
dish
solvent
impure
solid
stir to dissolve
solid
The solution is heated to
evaporate most of the solvent
Fig. 19.1 Simple crystallization process.
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82
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. At which temperature generally the substance is more soluble in a given solvent?
a. Very very low
c. Very low
b. At room temperature
d. Higher temperature.
2. The stage at which crystal starts to appear on glass rod is called ----------.
a. boiling point
c. melting point
b. point of crystallization
d. triple point
3. Which solution is to be prepared for crystallization?
a. Unsaturated
c. Supersaturated
b. Saturated
d. Fused mass of impure substance
4. What is the Color of prismatic copper sulfate crystals?
a. Red
b. Blue
c. Pink
d. Green
5. What is the Color of crystals of benzoic acid?
a. Black
b. Yellow
c. White
d. Brown
Short answer questions
1. How does cooling rate affect crystal size?
Ans.
2. Which type of solvent is used for crystallization?
Ans
3. Write the names of observed Color of saturated solutions of copper sulfate and benzoic
acid in water at high temperature.
Ans
4. Write the names of apparatus used during filtration process.
Ans
5. What is filtrate?
Ans
6. Arrange the following steps involved in crystallization in proper sequence.
a. Filtration b. Dissolution c. Drying d. Crystallization e. Solvent selection.
Ans
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83
Date:
/
/
Activity 1
Aim: To prepare 100 mL of 0.1 M standard solution of oxalic acid.
Theory: The molecular formula of oxalic acid is H C O .2H O. Its molar mass is 126 g/mol.
2
2
4
2
1000 mL of 1M solution of oxalic acid contains 126 g of H2C2O4.2H2O
Hence 100 mL of0solution of oxalic acid will contains
100 mL u0u126 g
=
= 1.26 g of oxalic acid.
1000 mL u0
Apparatus: 100 mL volumetric fl ask, beaker, glass rod etc.
Chemicals: Oxalic acid, distilled water.
Procedure:
1. Wight accurately 1.26 g of oxalic acid. Transfer it to a beaker and add little distilled water. Stir
it well with the help of glass rod.
2. Transfer the solution from beaker to volumetric fl ask, using conical funnel and glass rod
properly (Take care to prevent loss of even a single drop of solution).
3. Wash the beaker twice / thrice with distilled water and transfer the washing to the volumetric
fl ask.
4. Dilute the solution by adding distilled water up to the mark on the volumetric fl ask to make the
volume 100 mL. (See that the volume marking appears tangential to the meniscus of the final
solution)
Fig. Activity 1.1 Volumetric flask.
Conclusion: -------------------------------------------------------------------------------------------------Remark and sign of teacher: ..................................................................................................
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84
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. A solution whose concentration is accurately known is called----a. dilute solution
b. concentrated solution
c. standard solution
d. colloidal solution
2. The molar mass of oxalic acid is
a. 126 u
b. 126 g / mol
c. 12.6 u
d. 12.6 g / mol
3. To prepare standard 1M solution of oxalic acid.
a. 0.126 g of oxalic acid is dissolved in 1 L of solution.
b. 1.26 g of oxalic acid is dissolved in 1 L of solution.
c. 12.6 g of oxalic acid is dissolved in 1 L of solution.
d. 126 g of oxalic acid is dissolved in 1 L of solution.
4. To prepare 100 mL of standard 0.1M oxalic acid solution.
a. 0.63 g of oxalic acid is dissolved in 100 ml of distilled water.
b. 1.26 g of oxalic acid is dissolved in 100 ml of distilled water.
c. 12.6 g of oxalic acid is dissolved in 1000 ml of distilled water.
d. 126 g of oxalic acid is dissolved in 100 ml of distilled water
Short answer questions
1. Calculate the amount of oxalic acid required to prepare 1000 mL 0.1 M standard solution
of oxalic acid
Ans.
.
2. Calculate the molar mass of oxalic acid. (C = 12, O = 16, H = 1)
Ans.
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85
Date:
/
/
Activity 2
Aim: To determine pH of different fruit juices by using universal indicator or pH paper.
Apparatus: Test tubes, droppers, glass rod, beakers, etc.
Chemicals: Different fruit juices, pH paper or universal indicator.
Procedure:
1. Take 5 ml of given different fruit juices in separate A, B, C, D marked test tubes.
2. Put pH paper or add 2 drops of universal indicator in each test tube and shake it well.
3. Observe the color of pH paper or solution developed in each test tube.
4. Determine the pH of each solution by comparing the colors with the standard pH color strips.
5. Find out nature of given fruit juices on the basis of pH values.
Acidic
Neutral
Red Orange Yellow
Green
Alkaline
Blue
Indigo
Violet
Fig. Activity 2.1 pH scale
Observation table and Conclusion :
Sr.
No.
Juice sample
Color of pH paper or solution of
universal indicator
pH
Nature
1
....................(A)
................................................
..........
.............
2
....................(B)
................................................
..........
.............
3
....................(C)
...............................................
..........
.............
4
.....................(D)
...............................................
...........
.............
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86
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. In a 5 mL solution of lemon juice add 2 drops of universal indicator, the color of solution
becomes red-orange, the pH of solution is ...............
a. ! 7
c. equal to 7
b. 7
d. between 7 to 14
2. The pH of grape juice is about 3.3, the nature of grape juice is ...............
a. Acidic
c. neutral
b. alkaline
d. acidic as well as alkaline
3. When a strip of pH paper is dipped in a solution of orange juice, the color of pH paper become
orange the pH of solution is ...............
a. ! 7
c. equal to 7
b. 7
d. between 7 to 14
Short answer questions
1. What is the pH of pure water?
Ans
2. On mixing any two fruit juices, would pH remains same or differ? Verify your answer
experimentally.
Ans
3. What is the pH range of universal indicator?
Ans
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87
Date:
/
/
Activity 3
Aim: Calibration of pipette by burette.
Apparatus: Burette (25 mL), pipette (10 mL), beaker (100 mL), etc.
Chemicals: Distilled water
Procedure:
1. Take a 25 mL burette and fixed it on burette stand.
2. Fill the burette with distilled water upto10 mL mark with lower meniscus.
3. Now pipette out 10 mL of distilled water and add it to the burette.
4. Observe the level of water in the burette, if it is zero then that pipette is calibrated.
5. If the level of the water in the burette is not zero or more than zero, then take another pipette
for calibration.
6. Continue this process till pipette is calibrated.
Pipette
Stopcock
Fig. Activity 3.1 (a) Burette
(25 mL capacity)
Fig. Activity 3.1 (b) Pipette
(10 mL capacity)
Conclusion: The pipette is ----------------------------------------------------------------------------------.
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88
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The minimum volume of solution is measured by burette is
a. 0.01 mL
c. 1.0 mL
b. 0.1 mL
d. 10.0 mL
2. The capacity of pipette used by you in this activity is ...............
a. 0.01 L
c. 1 L
b. 0.1 L
d. 10 L
3. The Least count of the burette is ...............
a. 1 mL
c. 0.01 mL
b. 0.1 mL
d. 0.001 mL
4. A student added 10 mL distilled water in burette already having 5 mL of distilled water by
calibrated pipette. What is correct burette reading in burette?
a. 5 mL
c. 15 mL
b. 10 mL
d. 25 mL
Short answer questions
1. Arrange the following step in proper sequence
a. Burette fix on a burette stand
b. Observed the level of water in burette
c. Take 25 mL burette
d. Take 10 mL of distilled water by pipette
e. Add 10 mL water from pipette to the burette
f. Fill the burette upto 10 mL with water
Ans
.
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89
Date:
/
/
Activity 4
Aim: To obtain pure water from impure water containing ink by simple distillation method.
Apparatus: Distilling fl ask, water condenser, thermometer, retort stand with clamps, Bunsen
burner, a receiver (fl ask), etc.
Chemical: Impure water containing ink.
Theory: Distillation method is generally used to purify a volatile liquid from a non volatile
substance dissolved in it, or from a liquids which are less readily volatile than the liquid to be
purified.
A pure liquid under constant pressure boils at a constant temperature and hence distillation of
a liquid forms a method of purifying it. This method is useful however only when the liquid does
not decompose on boiling.
The method consists of heating the liquid substance in a fl ask known as the distilling fl ask
(fig. 4.1). The fl ask is heated directly on a wire gauze by a Bunsen burner or indirectly in a water/
oil bath. The liquid boils and forms vapors, leaving behind the impurities in the distilling fl ask.
The vapors of the liquid is then cooled in a water condenser, where it condenses to reproduce the
liquid in a pure form. The liquid collects is a fl ask known as the receiver.
The distilling fl ask is normally a round bottom fl ask with a side tube (arm). A cork carrying a
thermometer through it is fitted to the distilling fl ask so that the bulb of the thermometer is in level
with the side tube. The side tube is connected to the water condenser by another cork (adapter).
Cold water is circulated through the condenser in a direction opposite to the fl ow of the vapor of
the liquid substance. This cold water keeps the condenser cool and provides a cool surface for the
vapors to condense.
The temperature at which vapors start to condense in liquid and remains constant, is nothing
but the boiling point of water. This temperature in the thermometer remains constant till all distillate
will collect into receiver.
Thermometer
Condenser
Clamp
Retort
stand
Vapors
Distilling Flask
water out
Burner
cold water in
Receiving Flask
Distillate
Fig. Activity 4.1 Simple distillation
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Procedure:
1. Pour impure water containing ink into the distilling fl ask by means of a funnel with a long
stem. Seal the mouth of the distilling fl ask with rubber cork having a hole at the center in
which thermometer is fitted. Add some pieces of porcelain to avoid bumping.
2. Now heat the fl ask carefully by means of a Bunsen burner. The solution begins to boil after
some time.
3. The water vapors formed passes into the condenser through the side tube of the distilling
fl ask.
4. The vapors are cooled and condensed to drops of water which collect into the receiver.
5. The pure water obtained is distilled water (distillate) having no ink contain.
6. Impurities (ink) remains behind in distilling fl ask.
Conclusion/ Result: The pure water is obtained from the impure water.
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. The boiling point of pure water is ..............
a. 100 K
b. 273 K
c. 373 K
d. 273 0C
2. Impure organic liquid having soluble impurities can be purified by a ..............
a. crystallization
c. simple distillation
b. fractional crystallization
d. fractional distillation
3. Which of the following statement is correct about simple distillation ..............
a. process to convert impure liquid into pure form.
b. process to convert pure liquid into impure liquid.
c. process to convert impure solid in pure form.
d. process to separate mixture of two different impure liquid.
Short answer questions
1. Define simple distillation method?
Ans
2. What is the role of water condenser in simple distillation method?
Ans
3. What is the role of bumping stone in simple distillation method?
Ans
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Date:
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Activity 5
Aim: To detect the presence of adulterant in given food samples.
Theory: The substance which lowers or degrades the quality of food material is called adulterant.
Sr.
No.
Name of food material
Common Adulterant
1
Powdered Sugar
Baking soda
2
Turmeric powder
Metanil yellow color
3
Tea powder
Exhausted tea leaves dried and artificially Colored
4
Chili powder
Brick powder
5
Edible oil
Argemone oil
Chemicals: Given food samples, dil. HCl, conc. HCl, etc.
Apparatus: Test tubes, test tube stand, etc.
Procedure:
Sr.
Name of
Test
Observation
No.
Food
1 Powdered Sample of sugar + Effervescence
sugar
dil. HCl
No effervescence
2
3
4
5
Turmeric
powder
Tea
powder
Chili
powder
Edible oil
Sample of
turmeric powder +
few drops of conc.
HCl
Sprinkle the
sample of tea
powder on a wet
filter paper
Violet color
No violet color
Yellow or red
colored spot appears
Inference
Sugar sample is adulterated
Sugar sample is
not adulterated / Pure
Turmeric powder sample
is adulterated
Turmeric powder sample is
not adulterated / Pure
Tea sample is adulterated
No yellow or red
spot appears
Tea sample is
not adulterated / Pure
Sprinkle chili
powder on the
surface of water
Brick powder settled
at the bottom of test
tube
No brick powder
settled at the bottom
of test tube
Chili powder sample is
adulterated
5 ml sample of
edible oil + 5 ml
of conc. HCl and
shake.
Yellow or orange
yellow color appears
in lower acid layer
Edible oil sample is
adulterated
Chili powder sample is
not adulterated / Pure
Edible oil sample is
No yellow or orange
yellow color appears in not adulterated / Pure
lower acid layer
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Conclusion: The given food materialsSr.
No.
Name of food
material
1
Powdered sugar
2
Turmeric powder
3
Chili powder
4
Tea powder
5
Edible oil
Pure / adulterated
MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. Turmeric powder is adulterated with ……….............color.
a. yellow
c. saffron
b. metanil yellow
d. indigo red
2. When a small quantity of dil. HCl is added to a sample of powdered sugar effervescence of CO2
are observed. The sugar sample is ……….........
a. adulterated with brick powder
b. not adulterated (Pure)
c. adulterated with baking soda
d. adulterated by metanil yellow
3. Now a days chili powder is adulterated with ……….........
a. saw dust
c. brick powder
b. red color
d. yellow color
4. When 5 mL of concentrated HCl is added to 5 mL sample of edible oil, lower layer of acid
becomes yellow, orange yellow or crimson colored indicates.
a. edible oil sample is pure.
b. eible oil sample is adulterated with conc. nitric acid.
c. edible oil sample is adulterated with argemone oil.
d. edible oil sample is adulterated with conc. sulphuric acid?
Short answer questions
Q1. What do you meant by adulteration in food materials?
Ans
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Date:
Activity 6
/
/
Aim: To determine pH of HCl solution of various concentrations by using pH paper or universal
indicator.
Apparatus: Test tubes, test tube stand.
Chemicals: 0.1M, 0.01M, 0.001M HCl solution, pH paper or universal indicator.
Theory: pH = -log10[H+]
For Acidic solution, pH 7, Basic solution pH ! 7,and neutral solution pH = 7.
The value of pH changes with change in concentration of HCl.
Procedure:
1. Take 5 ml each of 0.1 M, 0.01 M, 0.001 M HCl solutions in separate test tubes marked A, B,
C.
2. Add 2 drops of universal indicator in each test tube or put piece of pH paper in each test tube.
3. Observe the Color of solution or pH paper and record pH of each solution.
Acidic
Neutral
Alkaline
Red Orange Yellow
Green
Blue
Indigo
Violet
Fig. Activity 6.1 pH range
Note: Student has to prepare 0.01M and 0.001M HCl solution from the given 0.1M HCl solution.
Observation Table/ Conclusion:
Sr.
No.
Solutions
Concentration of
solutions
Color of pH paper or
solution
pH
1
A
........................
........................
.............
2
B
........................
........................
.............
3
C
........................
........................
.............
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MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. If nature of the solution is acidic, then its pH value is --a. ! 7
c. equal to 7
b. 7
d. in between 7 to 14
2. Which of the following indicator have different pH range is -a. phenolphthalein indicator
c. methyl orange indicator
b. acid-base indicator
d. universal indicator
+
3. The negative log of H ions concentration to the base 10, is known as --a. pH
c. pKa
b. pOH
d. pKb
4. The Color of universal indicator in strongly acidic solution is ---a. red
c. oranges
b. violet
d. blue
+
5. If concentration of H ions increase, the values of the pH of the solution will be ----a. decrease
c. increase
b. remain constant
d. first increases then decreases
Short answer questions
Q1. What do you meant by pH of the solution?
Ans
Q2. If the concentration of given solution of HCl is 0.01M. Calculate the pH of the solution.
Ans.....................................................................................................................................................
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Date:
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Activity 7
Aim: To determine pH of NaOH solution of various concentrations by using pH paper or universal
indicator.
Apparatus: Test tubes, test tube stand.
Chemicals: 0.1 M NaOH, 0.01 M NaOH, 0.001 M NaOH solutions, pH paper or universal
indicator.
Theory: pOH = -log10[OH-]; pH = 14- pOH
For Acidic solution pH 7, Basic solution pH ! 7, Neutral solution pH = 7.
The value of pH changes with change in concentration of NaOH.
Procedure:
1. Take 5 ml each of 0.1M, 0.01M, 0.001M NaOH solutions in separate test tubes marked A, B,
C.
2. Add 2 drops of universal indicator in each test tube or put piece of pH paper in each test tube.
3. Observe the Colors of solution or pH paper and record pH of each solution.
Acidic
Neutral
Red Orange Yellow
Alkaline
Green
Blue
Indigo
Violet
Fig. Activity 7.1 pH range
Note: Student has to prepare 0.01M and 0.001M NAOH from the given 0.1M NaOH solution.
Observation Table/ Conclusion:
Sr.
No.
1
Solutions
A
Concentration of
solutions
........................
Color of pH paper
or solution
............................
pH
.............
2
B
........................
............................
.............
3
C
........................
............................
.............
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MCQ
Select [3] or underline the most appropriate answer from given alternatives of each sub
question.
1. If nature of the solution is alkaline is then its pH values is .......
a. ! 7
c. Equal to 7
b. 7
d. In between 7 to 14
2. Which of the following indicator have different pH range is .......
a. Phenolphthalein indicator
c. Methyl orange indicator
b. Acid-base indicator
d. Universal indicator
3. The negative logarithm to the base 10 of OH- ions concentration is known as .......
a. pH
c. pKa
b. pOH
d. pKb
4. The color of universal indicator in strongly basic solution is .......
a. red
c. orange
b. violet
d. blue
3. If concentration of OH- ions increase, the values of the pH of the solution will be .......
a. decrease
c. increase
b. remain constant
d. first increases then decreases
Short answer questions
1. What is pOH of the solution?
Ans
2. If the concentration of given solution of KOH is 0.01M. Calculate the pOH and pH of the
solution.
Ans
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NOTES /CALCULATIONS /ROUGH WORK
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100
101
102
103
104
105
106
Exam. Seat No.
Roll No.
Maharashtra State Bureau of Textbook Production and
Curriculum Research, Pune-04
Certificate
Laboratory journal for Chemistry
This is to certify that Shri/Miss .......................................................................
has satisfactory carried out the required practical work prescribed by Maharashtra
State Bureau of Textbook Production and Curriculum Research, Pune-04 for first
year jr. college science course Roll No. ------------ in subject Chemistry and that
this journal his/her bonafide work in year 20... - 20 ... .
No of experements performed
Subject Teacher
No of activities performed
Examiner
Stamp
107
Principal
108
CHEMISTRY PRACTICAL NOTEBOOK STANDARD XI
(agm`Zemó àmË`{jH$ Zm|Xdhr B`Îmm 11 dr)
< 59.00