kas 152p/252p session 2021-2022 - galgotiacollege.edu

ENGINEERING CHEMISTRY LAB

ACADEMIC CONTENT

KAS 152P/252P

SESSION: 2021-2022

Galgotia College of Engineering & Technology

Greater Noida

Vision of Institute:

To be a leading educational institution recognized for excellence in engineering education

& research producing globally competent and socially responsible technocrats.

Mission of Institute:

• To provide state of art infrastructural facilities that support achieving academic excellence.

• To provide a work environment that is conducive for professional growth of faculty & staff.

• To collaborate with industry for achieving excellence in research, consultancy and

entrepreneurship development.

DEPARTMENT OF APPLIED SCIENCES

VISION OF DEPARTMENT

To be a center of excellence in education in the field of physics, chemistry, mathematics and

other related interdisciplinary sciences with ethical and social values.

MISSION OF DEPARTMENT

1. To provide quality education by providing state of the art facility

2. To educate the students by giving them a blend of knowledge of applied and

interdisciplinary sciences.

3. To make students conscious of ethical and social values in pursuing their

education and profession.

KAS 152P/ KAS 252P : ENGINEERING CHEMISTRY PRACTICALS(B.TECH IST Year)As per AKTU Syllabus

0L:0T:2P 1 Credit

LIST OF EXPERIMENTS

1. Determination of alkalinity in the given water sample.

2. Determination of temporary and permanent hardness in water sample using EDTA.

3. Determination of iron content in the given solution of Mohr‟s salt.

4. Determination of viscosity of given liquid.

5. Determination of surface tension of given liquid.

6. Determination of chloride content in water sample.

7. Determination of available chlorine in bleaching powder.

8. Determination of pH by pH-metric titration.

9. Preparation of Phenol-formaldehyde and Urea-formaldehyde resin.

10. Determination of Cell constant and conductance of a solution.

11. Determination of rate constant of hydrolysis of esters.

12. Verification of Beer"s law.

List of Experiments: Any ten experiments with virtual link

SN Lab Practical Virtual Lab Link

1

Determination of alkalinity in the

given water sample.

https://vlab.amrita.edu/?sub=2&brch=193&sim=15

48&cnt=1

2

Determination of temporary and permanent hardness in water sample using EDTA.

http://vlabs.iitb.ac.in/vlabs- dev/labs/nitk_labs/Environmental_Engineering_1/l abs/determination-of-hardness-nitk/simulation.html

3

Determination of iron content in the given solution by Mohr’s method.

https://vlab.amrita.edu/?sub=2&brch=193&sim=35 2&cnt=1

4

Determination of viscosity of given liquid.

http://vlab.amrita.edu/?sub=3&brch=190&sim=339 &cnt=1

5

Determination of surface tension of given liquid.

https://amrita.olabs.edu.in/?sub=1&brch=5&sim=2 24&cnt=7

6

Determination of chloride content in water sample.

http://vlabs.iitb.ac.in/vlabs- dev/labs/nitk_labs/Environmental_Engineering_1/l abs/determination-of-hardness-nitk/index.html

7

Determination of available chlorine in bleaching powder.

Proposed in E bootathon 04

8

Determination of pH by pH-metric titration.

https://vlab.amrita.edu/?sub=2&brch=193&sim=35

2&cnt=1

9

Preparation of Phenol-formaldehyde and Urea-formaldehyde resin.

Experiment has been developed in E bootathon 01 and

is in the process of hosting. The link will be available soon

10

Determination of Cell constant and conductance of a solution.

http://vlab.amrita.edu/?sub=3&brch=193&sim=575

&cnt=1

11

Determination of rate constant of hydrolysis of esters.

Proposed in E bootathon 04

12

Verification of Beer’s law. http://vlab.amrita.edu/?sub=3&brch=206&sim=569

&cnt=975

http://vlabs.iitb.ac.in/vlabs-





KAS 152P/ KAS 252P : ENGINEERING CHEMISTRY PRACTICALS (B.TECH 1stYear)

List of Experiments to be Conducted CO Wise

CO1 Estimate different impurities present in water sample.

1.Determination of alkalinity in the given water sample.

2. Determination of temporary and permanent hardness in water sample using EDTA.

3. Determination of chloride content in water sample.

CO2 Determine molecular properties such as surface tension, viscosity, pH, conductance and

concentration of solution

4. Determination of viscosity of given liquid.

5. Determination of surface tension of given liquid.

6.Determination of pH by pH-metric titration.

7. Verification of Beer"s law.

CO3 Identify iron concentration and percentage of available chlorine in supplied sample using titration methods.

8.Determination of available chlorine in bleaching powder.

9. Determination of iron content in the given solution of Mohr’s salt.

PO1 Engineering knowledge: Ability to apply the knowledge of mathematics, science,

engineering fundamentals and an engineering specialization to solve complex Mechanical Engineering problems.

PO2 Problem analysis: Ability to identify, formulate, research literature, and analyze complex Mechanical Engineering problems reaching substantiated conclusions using first principles of mathematics, natural sciences, and engineering sciences.

PO3 Design/development of solutions: Ability to design solutions for complex mechanical engineering problems and design system components or processes that meet the specified

needs with appropriate consideration for the public health and safety, and the cultural, societal, and environmental considerations.

PO4 Conduct investigations of complex problems: Ability to design & perform experiments of complex mechanical systems, analyze and interpret data to provide valid conclusions.

PO5 Modern tool usage: Ability to create, select, and apply appropriate techniques, resources, and modern engineering and IT tools including prediction and modeling to complex mechanical engineering problems/ activities with an understanding of the limitations.

PO6 The engineer and society: Ability to Apply reasoning informed by the contextual

knowledge to assess societal, health, safety, legal, and cultural issues and the consequent responsibilities relevant to the professional engineering practice.

PO7 Environment and sustainability: Ability to understand the impact of the professional engineering solutions in societal and environmental contexts, and demonstrate the knowledge of, and need for sustainable development.

PO8 Ethics: Ability to understand, commit to and apply professional ethics, responsibilities and norms to engineering practice.

PO9 Individual and team work: Ability to function effectively as an individual, and as a member or leader in diverse teams, in multidisciplinary settings.

PO10 Communication: Ability to communicate effectively on complex engineering activities

with the engineering community and with society at large, such as, being able to comprehend and write effective reports and design documentation, make effective presentations, and give and receive clear instructions.

PO11 Project management and finance: Ability to demonstrate knowledge and understanding of the engineering and management principles and apply these to one’s own work, as a member and leader in a team, to manage projects and in multidisciplinary environments.

PO12 Life-long learning: Recognize the need for, and have the preparation and ability to

engage in independent and life-long learning in the broadest context of technological change.

Course Outcomes (CO) : Engineering Chemistry Lab (KAS-152P/252P)

Course Name: Chemistry Lab (KAS-152P/252P), Year of study: 2021-2022

Course

outcome Statement (On completion of this course, the student will be able to - )

KAS-152P/252P.1

Estimate different impurities present in water sample. (K4)

KAS-152P/252P.2

Determine molecular properties such as surface tension, viscosity, pH, conductance and concentration of solution. (K2)

KAS-152P/252P.3

Identify iron concentration and percentage of available chlorine in supplied sample using titration methods. (K2)

CO-PO Mapping

Chemistry Lab (KAS-152P/252P)

CO / POs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PO11 PO12

CO1 3 2 - - - 3

2 3 3 - -

-

CO2 3 2 - - - - - 3 3 - - -

CO3 3 2 -

- - 2

2 3 3 - - -

KAS-152P/252P.3 3 2 -

- - 2.5

2 3 3 - - -

GALGOTIAS COLLEGE OF ENGINEERING AND TECHNOLOGY

1, Knowledge Park-II, Greater Noida, U.P.

Applied Sciences Department(Chemistry)

Session 2021-2022

List of Relevant sources of Engineering Chemistry Lab

https://nptel.ac.in/courses/122101001

www.vpkbiet.org/pdf/FE/Lab_Manual_Chem.pdf

https://www.hach.com/wah

https://www.bvrit.ac.in/...Lab...engineering_chemistry/Engineering%20Chemistry.pdf


http://vlabs.iitb.ac.in/vlabs- dev/labs/nitk_labs/Environmental_Engineering_1/l abs/determination-of-hardness-nitk/simulation.html



https://amrita.olabs.edu.in/?sub=1&brch=5&sim=2 24&cnt=7

http://vlabs.iitb.ac.in/vlabs- dev/labs/nitk_labs/Environmental_Engineering_1/l abs/determination-of-

hardness-nitk/index.html




http://www.vpkbiet.org/pdf/FE/Lab_Manual_Chem.pdf

https://www.hach.com/wah

https://www.bvrit.ac.in/...Lab...engineering_chemistry/Engineering%20Chemistry.pdf







GREATER NOIDA

List of Equipment/Instrument in Engineering Chemistry Lab

S. No.

Name of

Instrument/E

quipment

Specification Model/Make Status of

Working

1 Digital Balance 0.1g-600g Denwar

working

2 Analytical Balance .001g-100g Sunshine

working

3 Colorimeter Digital 400-700nm Elico/LabMED

working

4

Conductivity

metre 0-1000ms Decibel

working

5

p H meter

Digital p H 0-14 Decibel/Bench

working

6 Heating Mantle 0-500 Degree Centigrade Paras

working

7 Fridge 175 Litre LG

working

8 Muffle Furnace 0-1200 Degree Centigrade Jindal

working

9 Oven 0-300 Degree Centigrade Jindal

working

10

Double Distillation

Water Assembly 0-5litre Borosil

working

11 Stopwatch milliseconds to minutes

working


1, Knowledge Park-II, Greater Noida, U.P.

Applied Sciences Department(Chemistry)

LAYOUT OF LAB

Galgotias College of Engineering and Technology

Department of AS(Chemistry)

LAB Plan : B. Tech. - …I/II… Semester : 2021-22

Name of Subject with Code: ENGINEERING CHEMISTRY LAB (KAS152P/KAS252P)

Faculty Name:

Exp. No.

CO Experiment to be conducted

Remarks

if any

1. CO 1

Determination of temporary and permanent hardness in water sample

using EDTA as standard solution.

2. CO 1

Determination of alkalinity in the given water sample.

3. CO 1

Determination of Chloride content in water sample

4. CO 3

Determination of available chlorine in bleaching powder.

5. CO 3

Determination of iron content in the given water sample of Mohr’s salt

solution..

6. CO 2 Determination of Viscosity of given liquid.

7. CO 2

Determination of iron concentration in sample of water by colorimetric

method. The method involves the use of KCNS as a colour developing

agent and the measurements are carried out at λmax 480nm.

8. CO 2 Determination of pH by pH- metric titration.

9. CO 2 Determination of Surface tension of given liquid.

10. CO2 Preparation of Phenol-formaldehyde and Urea-formaldehyde resin.

ENGG CHEMISTRY

LAB

MANUAL

EXPERIMENT NO.1

CO1 Estimate different impurities present in water sample

Object To determine the constituents and amount of alkalinity of the supplied water

sample .

Requirements HCl (N/10), Phenolphthalein (Ph), Methyl Orange (MO), Water sample,

Burette, Pipette, Conical Flask, Beaker, Funnel

Principle Alkalinity of water sample is mainly due to the presence of various hydroxides,

carbonates and bicarbonates. Following possibilities may arise with respect to

the constituents causing alkalinity in water:

❖ due to −OH only

❖ due to −2

3CO only

❖ due to −

3HCO only

❖ due to −OH and −2

3CO

❖ due to −2

3CO and −

3HCO

Note: −OH and −

3HCO cannot exist together as they react to produce −2

3CO

ions.

OHCOOHHCO 2

2

33 +→+ −−−

These can be estimated separately by titration against standardised acid using

phenolphthalein (pH range: 8.2 – 10.0) and methyl orange (pH range: 3.2 – 4.4)

as indicators.

(a) OHOHH 2→+ −+

(b) −+− →+ 33 COHHCO 2

(c) OHCOHHCO 223 +→+ +−

Titration of the water sample against a standardised acid to Ph end point marks

the completion of reactions (a) and (b) only. The amount of acid used thus

corresponds to −OH and one-half of the normal −2

3CO present.

On the other hand, titration of the water sample against a standardised acid to

MO end point marks the completion of reactions (a), (b) and (c). Hence, the

P M

Observations

Calculations

amount of acid used after the phenolphthalein end point corresponds to one-

half of normal carbonate plus all the bicarbonates while the total amount of

acid used represent the total alkalinity.

End point With Ph as indicator – pink to colourless

With MO as indicator – yellowish to reddish

Procedure ▪ Pipette out 25mL of the water sample in a clean titration flask.

▪ Add 2 drops of phenolphthalein indicator and titrate against standardised HCl with

constant shaking until the pink colour just disappears.

▪ Note the burette reading, which corresponds to Ph end point (P).

▪ Then to the same solution, add 2-3 drops of methyl orange indicator and continue

titration until a colour change from yellow to pink takes place.

▪ Note the burette reading as methyl orange end point (M).

▪ Repeat the procedure for the other samples

S.No.

Volume of

water sample

taken / mL

Burette reading / mL P (in mL) =

V1 – IR

M (in mL) =

V2 –IR Initial (IR) Final (V1) Final (V2)

1 25

2 25

3 25

Depending upon the P and M values, different cases of alkalinity due to individual ions are presented in the table below

S.No. Alkalinity −OH / ppm −2

3CO / ppm −

3HCO / ppm

1 P = 0 Nil Nil M

2 M = 0 P Nil Nil

3 P = M Nil 2P or 2M Nil

4 P <1/2 M Nil 2P M-2P

5 P >1/2 M 2P-M 2(M-P) Nil

For the case, P < 1/2M so −2

3CO and −

3HCO are present.

Note: Alkalinity has to be reported in terms of CaCO3

For −

3HCO

N −

3HCO X V −

3HCO = NHCl X VHCl

N −

3HCO x 25 = 0.1N X (M-2P)

Alkalinity due to −

3HCO ions = 1000503

−HCON mg/L (≡ ppm)

For −2

3CO

HClHClCOCOVNVN = −− 2

323

N −2

3CO X 25 = 0.1N X 2P

Alkalinity due to −2

3CO ions = N −2

3CO x 50 x 1000 mg/L (≡ ppm)

Total alkalinity = Alkalinity due to −

3HCO + Alkalinity due to −2

3CO

For the case, P >1/2 M so −2

3CO and −OH are present.

For −OH

N −OH X V −OH = NHCl X VHCl

N −OH X 25 = 0.1N X (2P-M)

Alkalinity due to ions = N −OH x 50 x 1000 mg/L (≡ ppm)

For −2

3CO

HClHClCOCOVNVN = −− 2

323

N −2

3CO X 25 = 0.1N X 2(M-P)

Alkalinity due to −2

3CO ions = N −2

3CO x 50 x 1000 mg/L (≡ ppm)

Total alkalinity = Alkalinity due to−OH + Alkalinity due to −2

3CO

Result The total alkalinity of given water sample is ….. mg/L.

Precautions 1. Add only phenolphthalein indicator initially.

2. If no pink colour is generated with phenolphthalein, add methyl orange at the

start.

3. End point should be noted carefully since two indicators are used

simultaneously.

Experiment No. 2


OBJECT: To determine the total hardness of given water sample by using (EDTA)Na2 as

standard solution by complexometry.

REQUIREMENTS: Conical flask, burette, pipette, beaker, measuring flask, M/100 of

(EDTA)Na2 solution, buffer solution of pH 10, Eriochrome black –T indicator, standard hard

water (1 gm./lit.) and supplied water sample.

THEORY: Temporary hardness of water is due to the presence of soluble salts of bicarbonates

of calcium and magnesium, while the permanent hardness of water is due to the presence of

sulphates, chlorides, nitrates etc. of calcium, magnesium and other heavy metals. Temporary

hardness of water can be removed by boiling of water while permanent hardness can not be

removed by boiling.

EDTA( Ethylenediaminetetraceticacid) is a complexing agent, which is widely used due to its

strong complexing agent, which is widely used due to its strong complexing action and

commercial availability.EDTA is a tetraprotic acid,because of its limited solubility, it is not used

directly. (EDTA)Na2 is used which in auueous solution ionize to give two Na+ ions and a

strong chelating agent. The indicator used is [Sodium-1-(1-hydroxy-2-naphthylazo)-6-nitro-2-

naphthol-4-sulphonate] commonly known as Eriochrome Black-T (EBT). EBT has two

ionisable phenolic hydrogen atoms and for simplicity it is represented as Na+H2In-.

END POINT: Wine red to blue.

PROCEDURE: Take 25ml. of hard water sample in a conical flask. Add 2ml of buffer

solution and 2drops of Eriochrome black-T indicator, the colour of the solution turns wine red.

Now titrate the solution against (EDTA)Na2. So that the colour changes from wine red to

blue. Repeat the titration for two concordant readings.

OBSERVATION:

S.No. Vol.of unknown solution

taken (mL)

Burette reading (mL) Vol.of(EDTA)Na2

used Initial Final

1.

2.

3.

25

25

25

V2(mL)

CALCULATION:

M1V1 = M2V2

(SAMPLE) (EDTA)Na2

M1 X 25 = 1/100 X V2

M1 = 1/100 X V2 / 25

Strength of water simple = M1 X 100 g/L

= 1/100 X V2 / 25 X 100 X 1000 mg/L

= V2 / 25 X 1000 mg/L

RESULT: The total hardness of given water sample is……………………ppm.

PRECAUTIONS:

1) The glass wares should be properly rinsed with distilled water .

2) The reaction mixture should be shaken properly.

3) The amount of indicator should be same in all titrations.

EXPERIMENT NO. 3

CO3 Identify iron concentration and percentage of available chlorine in supplied sample

using titration methods.

Object To determine the iron (II) content in the supplied sample Mohr’s salt solution

by volumetric analysis against standard potassium dichromate solution using

potassium ferricyanide (K3[Fe(CN)6]) as an external indicator.

Requirement

s

Standard potassium dichromate (K2Cr2O7) solution (N/20), potassium

ferricyanide indicator, Mohr’s salt solution, conical flask, glass rod, glazes tile

Principle Ferrous ions are the active constituents of the Mohr’s salt solution. Potassium

dichromate solution in acidic medium is a strong oxidizing agent which

converts ferrous ions into ferric ions. The end point can be determined by using

potassium ferricyanide as an external indicator.

After the reaction is completed, ferrous ions are completely oxidized to ferric

ions. As a result, when checked using an external indicator, no coloration will

be produced.

O3OH4 )(SOCr SOKSOH4 OCrK 23424242722 +++→+

OH7 )(SOFe3)(SOCr SOKFeSO6SOH7 OCrK

3O}H )(SOFeOSOH FeSO{2

234234242442722

2342424

+++→++

+→++

Reaction between external indicator and FeSO4

42263463 SOK3 ][Fe(CN)FeFeSO3 ][Fe(CN)K +→+

End point No change in yellow colour of the indicator.

Procedure

1. 10 mL of the sample solution was pipetted out in a conical flask.

2. 10 drops of indicator (Potassium ferricyanide) was placed on a glazed

tile.

3. The initial reading of the burette was noted down (upper meniscus of the

K2Cr2O7 solution).

4. The sample solution was titrated against K2Cr2O7 solution. After the

addition of 5 drops K2Cr2O7 solution the reaction mixture was mixed

well.

5. A drop from the reaction mixture was placed on the drop of indicator.

The blue colour developed.

6. Step 4 & 5 was repeated after adding……mL K2Cr2O7 solution the

colour of indicator remains yellow.

7. The procedure was repeated till concordant readings were obtained.

Results Ferrous content in the sample provided = …….. g/L

Precautions 4. All reagents should be freshly prepared.

5. The glass apparatus should be washed with chromic acid and then with

distilled water.

6. After every titration wash the conical flask with distilled water.

7. Potassium dichromate acts as an oxidizing agent in acidic medium

therefore add dilute H2SO4 in the Mohr’s salt solution.

Ferrous ferricyanide

(greenish-blue)

(yellow)

Observations

Calculations N1 V1 = N2 V2

N1 × 10 = N2 V2

Strength of iron in sample solution = N1 × 56 g/L

S.No. Volume of sample

taken in mL

Burette reading in mL Volume of K2Cr2O7

solution used in mL Initial Final

1 10

2 10

3 10

EXPERIMENT NO. 4


concentration of solution.

Object: To determine the viscosity of the given liquid at room temperature by Ostwald’s Viscometer.

Apparatus: Ostwald’s Viscometer, beaker, R.D. bottle, Stop watch

Theory: The property of resistance to flow when a stress is applied to a liquid is called “Viscosity”. It is

produced by the shearing effect of moving one layer of the fluid past another. When a liquid is in the laminar

flow through a tube the layer close to the surface of the tube is almost stationary and the layer at the axis of the

tube moves faster than any other layer. A slow moving layer exerts a friction on its nearest layer. The

measurement of the viscosity coefficient (η) of the given liquid by Ostwald’s Viscometer is based on Poiseuille’s

equation,

η = π𝑟4 Pt

8Vl

Where V is the volume of the liquid of viscosity coefficient η which flows in time t through a capillary tube of

radius 𝑟 and length l under a pressure head of P.

𝑃 = ℎ𝑑𝑔

Where h = height, d= density and g = acceleration due to gravity.

If equal volume of two liquids are allowed to flow through the same capillary under the identical conditions,

η1

η2 =

𝜋𝑟4hd1g t1

8Vl×

8Vl

𝜋𝑟4hd2g t2

η1

η2=

𝑑1

𝑑2×

𝑡1

𝑡2

where , d1 = density of Solvent

d2 = density of given solution

η1 = viscosity of solvent

η2 = viscosity of given solution

t1 = time flow of solvent

t2 = time flow of given solution

Procedure:

1) Clean the Ostwald’s viscometer first with chromic acid and then wash thoroughly with distilled

water.

2) A sufficient volume of solvent is introduced in bulb B so that the bent portion of tube and

half or a little more than a half of bulb B is filled up.

3) Clamp the viscometer in quite vertical position.

4) Through upper arm of bulb A, suck up solvent until it rises above the upper mark C and allow it to

flow under its own weight.

5) The time of flow of solvent from C to D is continued by starting the stop watch as the Meniscus just

reaches upper mark C and stopping the watch as the meniscus just passes the lower mark D.

6) Take at least three reading for solvent .

7) Now clean the viscometer and dry it.

8) Repeat the whole procedure for the given solution.

9) The density of given solution can be calculated by R.D. bottle.

Observation Table:

S.No.

Solvent

Given Solution

Flow time between

C& D

Mean (t1) Flow time between

C& D

Mean (t2)

1.

2.

3.

4.

Room temperature = ----------0C

Density measurement of liquid:

Mass of empty R.D. bottle (w1) = ---------------gm

Mass of R.D. bottle with solvent(w2) = ---------------gm

Mass of R.D. bottle with solution (w3) = ---------------gm

Mass of solvent (w2- w1) = ---------------gm

Mass of solutions (w3- w1) = ---------------gm

Calculation:

Density of solvent at the room temperature = --------------gm/cm3

The viscosity of solvent at the room temperature = -------------- poise

Density of liquid (d2 ) = Mass of solution (w3 − w1)

Mass of solvent (w2 − w1)× d1

.

η1

η2=

𝑑1

𝑑2×

𝑡1

𝑡2

η2 = 𝑑2

𝑑1

𝑡2

𝑡1× η1

Result: The viscosity of the given solution at the room temperature is --------------poise.

Precautions:

1. The viscometer must be cleaned and dried properly before use.

2. The viscometer should be kept in a vertical position.

3. The flow time should be noted carefully.

4. Formation of air bubbles in the viscometer should be avoided.

EXPERIMENT NO.5



Object To determine the surface tension of the given liquid at room temperature by

stalagmometer.

Requirements Stalagmometer, Distilled Water, Unknown liquid, Clamp stand, Specific

gravity bottle etc.

Principle The surface tension of the given liquid is determined at the room temperature

by using stalagmometer. The numbers of drops for the same volume of distilled

water and the given liquid are counted and let these be as n1 and n2

respectively. Now if d1 and d2 are densities of water and given liquid at the

room temperature as determined separately by using specific gravity bottle ,

then the surface-tension y2 of the given liquid can be calculated by using the

simplified relationship as: ρ1/ ρ2 = n2/n1 . d1/d2

Procedure 1. Cleaned the stalagmometer and specific gravity bottle thoroughly first with

chromic acid solution and wash finally with distilled Water and then dry.

2. By immersing lower end in a beaker containing distilled water, suck up

water until it rises above the mark C.

3. Now allow the liquid drops to fall and count it.

4. Clean the stalagmometer and dry it. Fill it with liquid it rises above the upper

mark C and count the number of drops as before.

5. Clean and dry the specific gravity bottle and measure the density of liquid.

Observation-

Room Temperature = -----------0C.

Density of water at room temp. (d1) = -------- gm/cm3

Surface tension of water at room temp. (y1) = 72.14 dynes/cm

S. No. Water Given Liquid

No. of drops Mean (n1) No. of drops Mean (n2)

1.

2.

3.

Calculation :

Measurement of Density of Solution

1. Weight of empty specific gravity bottle = w1 gm

2. Weight of bottle + water = w2 gm

3. Weight of bottle + Some volume of liquid = w3 gm

Density of the given liquid (d2) = (w3 – w1/ w2 – w1) X d1

Also, ρ 1/ ρ 2 = n2/n1 . d2/d1.

ρ 2 = ρ 1 . n1/n2 . d2/d1.

Where ρ1 = surface tension of water at room temperature.

Substituting the values of ρ1, n1, n2, d1 and d2 the surface- tension of the given liquid at room

temperature thus becomes known.

Result: The surface tension of liquid at room temperature is ------------ (dynes/cm).

Precautions: 1. The stalagmometerr and specific gravity bottle should be cleaned properly

and dried before use.

2. Fit the stalagmometer vertically.

3. The rate of the fall of drops should be adjusted in a way of having interval of

at last 2-3 seconds in successive drops. The number of drops per minute must be

in between 15-20.

4. The drops should fall from the tip of the stalagamometer under their own

weight rather than pushing them by force.

5. Wash and dry the stalagmometer after use.

EXPERIMENT NO. 6


Object To determine the chloride content in supplied water sample by Mohr’s method.

Requirements Burette, Pipette, Conical Flask, Beaker, Funnel AgNO3 (N/100), Water

sample, Potassium chromate indicator.

Principle Mohr’s method is used to determine chloride content in water sample. In this

method a slightly alkaline solution is titrated against standard silver nitrate

solution using potassium chromate as an indicator. As the titration proceeds,

the chloride ions present react with AgNO3 forming white precipitate of AgCl.

The extra drop of AgNO3 reacts with indicator forming red silver chromate.

The change of colour from bright yellow to faint but distinct reddish brown

colour marks the end point.

NaCl + AgNO3 → AgCl + NaNO3

White ppt.

2AgNO3 + K2CrO4 → Ag2CrO4 + 2KNO3

Reddish brown

Reddish colour disappears if solution contains high concentration of chloride

ions.

Ag2CrO4 + 2Cl- → 2AgCl + CrO4 - -

In this method a slightly alkaline solution is used because in acidic medium

Ag2CrO4 gets dissolved where as in basic medium AgOH gets formed.

End point bright yellow colour to reddish brown colour

Procedure ▪ Filled the burette with AgNO3 Solution.

▪ Initial reading of the burette is noted down.

▪ 10mL of the water sample was pipetted out in a clean conical flask.

▪ Added 2 drops of potassium chromate indicator and titrated against standard

AgNO3 with constant shaking until a colour change from yellow to reddish

brown colour marks the end point.

▪ Noted the volume of the AgNO3 from the burette reading.

▪ Repeated the titration for concordant readings.

▪ Repeated the titration for blank correction.

Result The chloride content in given water sample =….. mg/L.

Precautions 8. The apparatus should be washed with distilled water.

9. The reaction mixture should be properly shaken during titration.

10. End point should be noted carefully.

Observations

Table for sample solution

Calculations

S.No. Volume of water

sample taken / mL

Burette reading / mL Volume of AgNO3

V2 (mL) Initial Final

1 10

2 10

3 10

Chloride content determination :

N1 V1 = N2 V2

(Sample ) (AgNO3 )

N1 x 25 = N2 x V2

N1 = N2 x V2/ 10

So strength of chloride ions = N1 x 35.5 g/ L

= N1 x 35.5 x 1000 mg/ L

EXPERIMENT NO. 7


using titration methods

Object To determine the percentage of available chlorine in the given sample of bleaching

powder (Iodometrically)

Requirements Potassium Iodide (KI), Bleaching powder, glacial Acetic acid (CH3COOH), (N/20)

Sodium Thiosulphate (hypo) solution, Starch solution (freshly prepared), Burette,

Pipette, Measuring flask

Principle The available chlorine is the amount of chlorine liberated by the action of mineral

acids on bleaching powder. It is generally expressed in terms of % by mass of

bleaching powder.

Commercial bleaching powder is a mixture of calcium hypochlorite (CaOCl2), basic

calcium chloride (CaCl2.Ca(OH)2) and some free calcium hydroxide. The active part

of the bleaching powder is calcium hypochlorite, responsible for disinfection and

bleaching action.

When a (dilute) mineral acid reacts with bleaching powder then free chlorine is

liberated. This liberated Cl2 reacts with KI to release free I2. Free I2 liberated is

titrated against a standard hypo solution using freshly prepared starch solution as

indicator.

222332 ClOHCOO)Ca(CHCOOHCH2CaOCl ++→+

22 IKCl2KI2Cl +→+

][KIKI(excess)I 32 +

6423222 OSNaNaI2OSNa2I +→+

Sodium tetrathionate

AdductstarchI2 →+ (starch – iodide complex)

End point Blue to colourless

Procedure • 25 mL of the standard solution was taken in a conical flask.

• Added 1 mL of KI solution and about half a test tube of acetic acid (glacial)

acetic acid.

• The liberated iodine was titrated against hypo solution till a light yellow colour

persists.

• Now 5 drops of freshly prepared starch solution is added, then a blue colour

appears.

• Now the solution is titrated against hypo till colour disappears.

• The titration is repeated to get concordant readings and noted down the total

volume of hypo used.

Observations

Strength of bleaching powder taken (w) = 5 g/L

Calculations

1g equivalent of available Chlorine ≈ 1g equivalent of hypo solution

N1 V1 = N2 V2

N1 × 25 = N2 V2

N1 = N2V2 / 25

Amount of chlorine = N1 × 35.5 g/L

% available chlorine = (N1 × 35.5 × 100)/w

S.No. Volume of sample taken /

mL

Burette reading / mL Volume of hypo

solution

consumed / mL Initial Final

1 25

2 25

3 25

Results

The available chlorine in the given sample of bleaching powder = %

Precautions

All reagents should be freshly prepared

1. The glass apparatus should be washed with chromic acid and then with

distilled water

2. Same amount of starch indicator must be used in all titrations

3. The end point of titration should be carefully observed.

Experiment No. 8

CO 2 Determine molecular properties such as surface tension, viscosity, pH,

conductance and concentration of solution

Object To determine the strength of given solutions pH-metrically.

Requirements pH meter, glass electrode, stirrer, beaker, burette

Principle pH of a solution is defined as the negative logarithm of

hydrogen ion concentration

pH = - log[ +H ]

When an alkali is added to an acid solution, pH of the solution increases slowly

but at the vicinity of equivalence point

the rate of change of pH is very rapid.

From the sharp change in the curve we

can find the Equivalence point from

which the strength can be calculated by

normality equation:

alkalialkaliacidacid VNVN =

Neutralization point pH = 7

Procedure

▪ The pH meter was calibrated against buffer solutions of known pH (4, 7 and

9.2).

▪ The glass electrode was washed with distilled water and dried.

▪ 25 mL of HCl solution was taken in a 100 mL beaker and pH of the solution

was noted.

▪ Now 0.5mL of given NaOH from the burette was added to the beaker, stirred

well and pH noted.

NaOH solution from the burette was added in installments till pH of solution

reached ~12.

▪ A graph was plotted between pH value (on Y-axis) and volume of NaOH

added (in mL) on x-axis. With the help of it, the volume of alkali used to

neutralize the given acid solution (at pH=7) was determined.

Result The strength of given acid solution is ……… g/L

The strength of given basic solution is……..g/L

Precautions

1. Temperature knob of pH meter should be adjusted to the room temperature.

2. After addition of acid, solution should be properly stirred

3. The pH should be first standardized by taking the buffer of a known pH

4. The activation of electrode should be done before 24 h.

Observations

Volume of HCl taken = 25 mL

Vol. of NaOH added (mL)

pH

Calculations

For acid pH=-log[H]+

[H+]=1/antilog(pH)

[H+] mol/L which is equivalent to normality of acid(HCl)

For base

alkalialkaliacidacid VNVN =

Nalkali =Nacid x Vacid /Valkali

Strength of HCl solution = 5.36N acid g/L

Strength of NaOH solution = Nalkali x 40 g/L

EXPERIMENT NO. 9

Object: To prepare the Bakelite (Phenol-formaldehyde) and Urea formaldehyde resin.

EXPERIMENT NO. 9(a)

Object: To prepare the Bakelite (Phenol-formaldehyde) Resin

Reagents/ Apparatus: Phenol, 40% formaldehyde solution,conc. HCl, glacial acetic acid, glass

rod, glass funnel, beaker,filter paper etc.

Theory: Bakelite is a copolymer formed by the polymerization of phenol and formaldehyde. It is

thermosetting in nature and is also known as PF-resin.

PF- resin is prepared by the condensation of phenol (P) and formaldehyde (F) in presence of

acid catalyst. Phenol first react with ortho and para hydroxy methyl phenol.

Ortho- hydroxy methyl phenol undergoes poly condensation with phenol to form linear chain

polymer known as novolac which is converted into hard infusible, cross- linked, solid bakelite

on reaction with formaldehyde.

EXPERIMENT NO. 9(b)

Object: To prepare the Urea-formaldehyde Resin.

Reagents/ Apparatus:

Urea ,formaldehyde solution,conc.H2SO4,Distilled water,glass rod, glass funnel, beaker,filter

paper etc.

Theory: Urea Formaldehyde resin is prepared by condensation reaction between Urea and

Formaldehyde in acidic or alkaline medium.

Procedure:

(i) Place about 5 ml of 40% Formaldehyde in 100ml beaker.

(ii) Add about 2.5 gm Urea with constant stirring till saturated solution obtained.

(iii) Add a few drops of conc. H2SO4 with constant stirring.

(iv) White solid mass appears in beaker.

(v) Wash white solid with water and dry it in the folds of filter paper.

(vi) Weight the yield of product.

Observations:

Mass of beaker(W1)……….gm

Mass of beaker with Urea Formaldehyde(W2)……….gm

Therefore Mass of Urea Formaldehyde(W2-W1)……….gm

Result:The yield of Urea formaldehyde is……..gm.

Properties:

(1) They have good electrical insulating properties.

(2) They are resistant to oil,grease and weak acids.

(3) They have good adhesive properties.

Uses:

(1) They are used for manufacture of cation exchange resins.

(2) They are used in manufacture of electrical switches,Plugs.

(3) They are used as adhesive application for the production of plywood and laminating.

Precautions:

(1) Keep yourself away from the beaker during the addition of conc. H2SO4 as the

reaction some times tends to become vigorous. (2) Reaction mixture should be stirred continuously.

EXPERIMENT NO.10

CO 2 Determine molecular properties such as surface tension, viscosity, pH, conductance and


Object

To determine cell constant and conductance of a solution.

Requirements KCl(solid),0.1N acetic acid solution,conductivity cell,conductometre, Wash

bottle 1 Thermometer .

Principle Measurement of conductance is one of the best ways for checking and

monitoring the purity of water. The conductance G is defined as the reciprocal

of resistance R, i.e., Resistance is measured in ohm (a) and conductance in

siemens (S). The conductivity meter in fact measures the conductance, and

displays the reading converted into conductivity.

Cell constant This is the ratio of the distance (d) between the electrodes to the

area (a) of the electrodes.

K = d/a K = cell constant (cm-1)

a = effective area of the electrodes (cm2)

d = distance between the electrodes (cm)

Conductance (G) is defined as the reciprocal of the electrical resistance (R) of a

solution between two electrodes. G = 1/R (S) The conductivity meter in fact

measures the conductance, and displays the reading converted into

conductivity.

Procedure:

Part 1 Determination of cell constant of the conductivity cell

1. Prepare 0.1NKCl by dissolving 0.745 g of it in 100mL of solution.

2. Rinse the conductivity cell and a beaker first with distilled water and then with a small

quantity of 0.1NKCl solution.

3. Place the conductivity cell(clamped vertical) in the beaker and fill it with sufficient

quantity of 0.1NKCl solution.

4. Standardize the conductometre using built in standard conductance.

5. Connect the terminals of the conductivity cell to the conductometre and determine the

conductance of the KCl solution,using this value obtain the cell constant of the

conductivity cell.

Calculation:

Conductance of 0.1N KCl solution =_________S

Specific Conductance of 0.1N KCl =_________S cm -1 (given

by examiner}

Cell Constant = Specific conductance = …… cm-1

Measured conductance

Part II Determination of the conductance of the various concentrations of acetic

acid solution.

Procedure:

1. Prepare the different dilutions of acetic acid solutions in 100cm3 measuring flasks as

follows: 0.05N acetic acid: 50cm3 0.1N acetic acid and dilute it to 100cm3

0.025N acetic acid: 50cm3 0.05N acetic acid and dilute it to 100cm3



2. Rinse the conductivity cell and a 500cm3 of beaker with distilled water and then

with 0.1N acetic acid solution.

3. Take about 25cm3 to 30 cm3 of 0.1 N acetic acid in the beaker and dip the cell into it.

Determine the conductance of this solution.

4. Determine the conductance of remaining concentrations of acetic acid solution as per

step 2 and 3.

Observation:

Cell Constant =…….. cm-1

S. No Concentration /Strength( Conductance C0(S)

1. 0.1N

2. 0.05N

3. 0.025N

4. 0.0125N

5. 0.00625N

Specific conductance of Solution:

K = Cell constant x Conductance

Result : 1) The Cell Constant = …….. cm-1

2) The specific conductance of the various concentrations of solution = ……….

Precautions 1. The conductivity cell, when not in use, should be kept in distilled water

to prevent drying of the platinum electrodes.

2. In case of fouling of the conductivity cell electrode plates, clean them b

keeping in dilute K2Cr2O7 containing H2SO4 solution (i.e. dilute

chromic acid) for 24 hours and then washing with running water

followed by with distilled water.

EXPERIMENT NO.11

Object To determine rate constant of hydrolysis of esters.

.

Requirements Ethyl acetate, HCl(0.5M),0.1M NaOH, ice water, Burette, Pipette, Conical

Flask,,stop watch, stopwatch,thermometer and thermostat etc.

Principle

Hydrolysis of ester is quite slow and reversible.But acid and alkalies catalyze

this reaction.Hydrolysis of ethylacetate in presence of acid HCl takes place as:

It is a Pseudo first order reaction(the concentration of H2O is high and it

remains almost constant).The reaction rate depends only on the concentration

of ester

CH3COOC2H5(aq) +H2O → CH3COOH(aq) +C2H5OH …….. (1)

Rate =k[CH3COOC2H5] …….. (2)

For first order reaction

K = 2.303 log C0

t C0-x

………. (3)

Where C0 = initial concentration of the ester

C0-x =Concentration of the ester at a time

Mix known amounts of ester and the mineral acid and withdraw equal volumes

of reaction mixture at definite intervals into vessels containing ice cold

water.The ice cold water is added to decrease the rate of the reaction.The

reaction mixture so withdrawn is titrated against standardized alkali using

phenolphthalein as the indicator.The end point is the appearance of pink colour

which does not disappear within ten seconds.From the titre values at various

time intervals, the rate constant is calculated using the procedure.

The reaction mixture withdrawn each time contains a definite amount of

hydrochloric acid and also acetic acid formed due to hydrolysis.Each titre value

represents the volume of sodium hydroxide solution required to neutralize both

these acids.

Vα = is proportional to the amount of hydrochloric acid,and acetic acid present

in a definite volume of reaction mixture after the completion of the reaction.

Vt = is proportional to the amount of hydrochloric acid,and acetic acid present

in a definite volume of reaction mixture after a time t.

Vα –V0 is proportional to the amount of acetic acid formed when hydrolysis is

complete or it is proportional to the initial concentration of ester(C0)

i.e (Vα –V0) is proportional to C0 ……….(4)

log (Vα–Vt) = log(Vα–V0) – kt/2.303

…….(7)

Procedure:

1.Transfer 50mL of 0.5M hydrochloric acid in a 250 mL conical flask.

2.Pipette out 5ml of ethyl acetate in a test tube and keep both the conical flask and the test tube

in thermostat for about five minutes.

3.Transfer the ester to the conical flask containing hydrochloric acid and immediately start the

stop watch.

4.After complete transfer,shake the mixture in the conical flask.

5.Immediately pipette out 5ml of the mixture into a 100mL conical flask containing 25mL of ice -

cold water.Add a drop of phenolphthalein and titrate the resultant solution against 0.1 M sodium

hydroxide solution.The end point is the appearance of light pink colour.

6. The first titre value represents V0.Repeat the process after interval of 10 minutes upto 30min

or 1 hour.Each of thr titre values from second onwards constitute Vt.

7.After taking 3 or 4 readings,pipette out 10 mL of a mixture into a 100mL conical flask and

close it with a cork. Heat the conical flask on a water bath at 500C for about 30 minutes,then cool

the conical flask to room temperature and titrate 5 mL of this mixture against0.1M sodium

hydroxide solution using phenolphthalein as indicator. The last titre value represents the infinite

reading(Vα).

Observation:

S.No. Time(t)seconds

Burette reading / mL

log( Vα–Vt)

Initial Final

Volume of

NaOH

solution used

(mL)

1 25

2 25

3 25

Calculations:

(a) Using Eq.

K = 2.303 log (Vα –V0)

t (Vα–Vt)

Five values of k are calculated and entered below:

(1) k =…….s-1

(2) k =…….s-1

(3) k =…….s-1

(4) k =…….s-1

(5) k =…….s-1

Average k = ……. s-1

(b) k is calculated from log(Vα–Vt) against t plot(Graph) using eq 7

K= -2.303xslope = ……… s-1

Result

(1)The Rate constant k by calculation =………s-1.

(2)The Rate constant k by graphical method =………s-1

Precautions 1. The temperature of the bath should be maintained constant within

+_0.50C.The rate of reaction is very sensitive to temperature changeEnd

point should be noted carefully since two indicators are used

simultaneously.

2. As ethyl acetate are flammable so avoid contact,do not breathe their

vapours

EXPERIMENT NO. 12

CO 2 Determine molecular properties such as surface tension, viscosity, pH, conductance and


Object: To determine the iron concentration in a given water sample by colorimeter method

using KCNS as colour developing agent.

Reagents/Apparatus: Stock solution of Ammonium Fe(III) sulphate, KCNS, conc.HNO3,

distilled water, test tubes, beaker, pipette, burette, spectrophotometer etc.

Theory: According to Lambert’s -Beer law “ The decrease in intensity of the incident light is

proportional to the length of thickness of the absorbing medium and the concentration of

the solution.”

log I0/ I = A= εCl

I0 = intensity of incident light, I = intensity of transmitted light,

A = Absorbance, l = thickness of medium,

C = Concentration of the solution, and ε = molar absorption coefficient.

For a particular substance, ε and l are constants, therefore absorbance is directly

proportional to the concentration.

A α C

Now a graph is plotted between absorbance and different concentration of a number of

solutions of known iron concentrations. From this graph the concentration of iron in unknown

solution can be determined by drawing a perpendicular on X-axis with respect to its absorbance

shown on Y-axis.

Fe(III) reacts with thiocyanate to give intense red colored compounds, depending upon the

concentration of thiocyanate solution. Fe(II) does not give this reaction. At high concentrations

of thiocyanate, generally [Fe(SCN)6]3-complex is formed, which increases the intensity and the

stability of color. So, in colorimetric method, a large excess of thiocyanate should be used. Also,

strong acids(HCl or HNO3) should be used to prevent the hydrolysis of Fe(III) ions.

Fe(III) + nCNS- → [Fe(SCN)n]3-

Where n = 1,2……..6.

Procedure:

1. Take different volumes (between 0 to 2.5mL) of the stock solution of iron (III) provided in six different test tubes. (As listed in table below)

2. Add 1mL conc.HNO3 and 0.5mL KCNS to each test tube. 3. Make the volume upto 10 mL by adding distilled water and mix properly.

Test tube No. 1 2 3 4 5 6

Fe(III)solution (mL) 0 0.5 1.0 1.5 2.0 2.5

Conc. HNO3 (mL) 1 1 1 1 1 1

KCNS (mL) 0.5 0.5 0.5 0.5 0.5 0.5

Distilled water (mL) 8.5 8.0 7.5 7.0 6.5 6.0

4. Make the separate test tube of unknown concentration of iron (III) in

the same manner.

5. Note the absorbance of all the solutions by spectrometer at 480 nm.

Observation Table: 1mL = 0.05 mg/L

Solution No. 1 2 3 4 5 6 unknown

concentration (mg/L) 0

Absorbance 0

Now a graph is plotted between absorbance and different concentration of a number of solutions

of known iron concentrations. From this graph the concentration of iron in unknown solution can

be determined by drawing a perpendicular on X-axis with respect to its absorbance shown on Y-

axis.

Result: The concentration of iron (III) in the given sample is…... mg/L.

Precautions:

1. Always use dilute solutions for obtaining calibration curve. 2. Cuvette should be cleaned and wiped properly.

3. Leave no finger marks on cuvette.

0 0.025 0.05 0.075 0.1 0.125 0.15

Concentration (mg/L)

Ab

so

rban

ce


Greater Noida

Chemistry Lab

SAFETY MEASURES

1. Fire Extinguisher and sand bucket is installed in the lab for any fire

hazard

2. First Aid Box is available in the Lab

3. Safe storage space are demarcated for Chemicals

4. Safe storage space for Glassware is marked.

5. Routine and Regular check is conducted for Gas pipeline.

6. Lab is equipped with proper exhaust system.

7. List of Do’s and Don’t are displayed in the Lab.

8. Gloves and Apron are available in lab.

9. Emergency Exit is properly displayed.

11. Lab has arrangement for proper disposable of hazardous and other

chemicals.


Greater Noida

Chemistry Lab

Personal and General Laboratory Safety

1. Never eat, drink, or smoke while working in the laboratory.

2. Read labels carefully.

3. Do not use any equipment unless you are trained and approved as a user by your supervisor.

4. Wear safety glasses or face shields when working with hazardous materials and/or

equipment.

5. Wear gloves when using any hazardous or toxic agent.

6. Clothing: When handling dangerous substances, wear gloves, laboratory coats, and safety

shield or glasses. Shorts and sandals should not be worn in the lab at any time. Shoes are

required when working in the machine shops.

7. If you have long hair or loose clothes, make sure it is tied back or confined.

8. Keep the work area clear of all materials except those needed for your work. Coats should be

hung in the hall or placed in a locker. Extra books, purses, etc. should be kept away from

equipment, that requires air flow or ventilation to prevent overheating.

9. Disposal - Students are responsible for the proper disposal of used material if any in

appropriate containers.

10. Equipment Failure - If a piece of equipment fails while being used, report it immediately to

your lab assistant or tutor. Never try to fix the problem yourself because you could harm

yourself and others.

11. Never pipette anything by mouth.

12. Clean up your work area before leaving.

13. Wash hands before leaving the lab and before eating.

ENGINEERING

CHEMISTRY LAB

VIVA QUESTIONS

Constituents and Alkalinity of Water Samples

Viva Questions

CO 1 Estimate different impurities present in water sample.

1. What do you understand by strength and normality of solution?

2. What is alkalinity?

3. Name the chemical species which are responsible for alkalinity in water.

4. Which indicator(s) is used in this titration?

5. Why hydroxide and bicarbonate alkalinity cannot be present together?

6. What colour does phenolphthalein gives with hydroxides and carbonates in the solution?

7. What colour does methyl orange gives with alkali and bicarbonates?

HARDNESS BY Na2(EDTA)

Viva Questions

CO 1 Estimate different impurities present in water sample.

1. Write the name of substances which imparts hardness to water.

2. What are the different units of hardness?

3. Why it is convenient to express to the units of hardness as CaCO3?

4. Why buffer solution is added into titrating mixture?

5. Name the substances which produce temporary and permanent hardness towater.

6. List the methods of removal of temporary and permanent hardness?

7. Give the full name of EDTA and write its formula.

Ferrous Content in Water Sample

(External Indicator method)

Viva Questions



1. What is the formula of F.A.S.?

2. Why sulphuric acid is added while preparing standard F.A.S.?

3. What is the equivalent weight of F.A.S.?

4. Why Mohr’s salt is considered a primary standard?

5. What is the oxidation state of Cr in K2Cr2O7?

6. What is the oxidation state of Fe in K4 [Fe (CN)6]?

7. Why you are using potassium ferricyanide indicator externally?

Viscosity of the given liquid by Ostwald’s Viscometer

Viva Questions



Q1. What do you understand by viscosity?

Q2. How is viscosity related to temperature? Q3. What is the significance of viscosity.

Q4. What is Poiseuille’s equation?.

Q5. What are the units of viscosity?

Q6. Write the name of the apparatus required for viscosity measurement. Q7. How is viscosity related to density?

Surface tension of Liquid

Viva Questions



Q.1 Define surface tension.

Q.2 What is the unit of surface tension?

Q.3 What are application of surface tension?

Q.4 What is the effect of temperature on surface tension?

Q.5 Name the apparatus used to determine the surface tension of liquid.

Q.6 What are the forces responsible for surface tension?

Q.7 Write the equation to determine surface tension by liquid drop method..

Chloride Ion Determination by Mohr’s Method

Viva Questions

CO 1 Estimate different impurities present in water sample

Q.1 Why we prepare fresh silver nitrate solution?

Q.2 WhyAgNO3 solution is kept in brown bottle.

Q.3 What are primary standards

Q.4 Which indicator is used in this titration?

Q.5 Why is necessary to maintain the pH near 7-8?

Q.6 What is the significance of Cl- ion determination?

Q.7 Which method is used in this titration?

Available Cl2 in Bleaching Powder

Viva Questions



Q 1.What do you understand by available chlorine? Write equation.

Q 2.Which indicator is used for the titration?

Q 3.What is hypo solution? Write its reaction with iodine.

Q 4.What is function of KI in the experiment?

Q 5.What is the importance to measure the available chlorine?

Q 6.What is the reason for the appearance of blue colour when starch is added to iodine solution?

Q 7.Why always freshly prepared starch should be used in the titration?

pH metric titration

Viva Questions



1. Define pH.

2. What is pH of pure water?

3. Define reference electrode?

4. What is the effect of temperature on pH?

5. What do you understand by buffer solution?

6. Which electrodes are used in pH-metric titration?

7. What is the effect of dilution on pH of an acidic solution?

Bakelite and Urea Formaldehyde Preparation

Viva Questions

Q.1What are thermosetting polymers?

Q.2 What are thermoplastic polymers?

Q.3 Write the monomers of Bakelite and Urea Formaldehyde Resin.

Q.4 Write few uses of Bakelite and Urea Formaldehyde Resin

.Q.5 What is the difference between addition and condensation polymers.

Q.6 Why thermosetting resins can’t be reused and reshaped?

Q.7 Bakelite is an example of thermoplastic polymer.(T/F)

Cell Constant and Conductance of Solution

Viva Questions

CO2 Determine molecular properties such as surface tension, viscosity, pH, conductance

and concentration of solution.

Q.1 Define the term conductance.

Q.2 What is the effect of temperature on conductivity of electrolytic solution.

Q.3 Define cell constant.

Q.4 What is the unit of conductance.

Q.5 What is the difference between metallic conduction and Electrolytic conduction.

Q.6 Define Specific conductance?

Q.7 What is the effect of dilution on conductance ?

Rate constant of hydrolysis of Ester

Viva Questions



Q.1 What is the rate of reaction?

Q.2 Name the factors which affects rate of reaction.

Q.3 What is rate constant of a reaction?

Q.4 Write equation for a first order reaction.

Q.5 Write the medicinal uses of esters.

Q.6 Define pseudo first order reaction.

Q.7 What is the unit of first order reaction.

COLORIMETER

Viva Questions



1. Define Beer-Lambert’s law.

2. What do you understand by colorimetry?

3. Give the reaction involved in the blood red coloured complex formation?

4. What is transmittance?

5. How is a filter selected in colorimeter?

6. What is calibration curve?

7. Define λmax and give the wavelength at which measurements are carried out?

SAMPLE QUIZ

GALGOTIAS COLLEGE OF ENGINEERING & TECHNOLOGY 1, Knowledge Park-II, Greater Noida

B.Tech. Second Semester 2018-2019 KAS-202, Engineering Chemistry Laboratory Quiz

Answer all Questions. Put mark by choosing the correct answer Faculty Name : Branch: Time: 202 minutes Name of student : Roll. No.: Date: CO1. Estimate various impurities present in water sample(9)

1. When P<1/2M, which alkaline ions present in water sample (a) OH_ (b) CO3

_ (c) HCO3-& CO3

_ (d) OH_ & CO3 _

2. Which standard solution is used in the determination of hardness of water sample? (a) N/10 HCl (b) N/20 NaOH (c) M/100 (EDTA)Na2 (d) none 3. Which two alkaline ions does not exist together (a) HCO3

-& CO3 _ (b) OH- & CO3

_ (c) HCO3-& OH- (d) None

4. Which standard solution is used in the determination of chloride content by Mohr’s method? (a) N/10 HCl (b) N/20 K2CrO4 (c) M/100 (EDTA)Na2 (d) N/100 AgNO3 5. What is the colour of phenolphthalein indicator? (a) colourless (b) pink (c) orange (d) yellow 6. Hardness can be calculated in terms of (a) MgCO3 equivalent (b) CaCO3 equivalent (c) CaSO4 equivalent (d) none 7. Which salt is responsible for permanent hardness? (a) CaSO4 (b) Ca (HCO3)2 (c) Mg (HCO3)2 (d) none 8. What colour does Methyl orange give with bicarbonates in the solution? (a) Orange (b) pink (c) colourless (d) yellow 9. 8.0-10.0 is the pH range for which indicator

(a) Phenolphthalein (b) EBT (c) Methyl orange (d) none CO2. Determine molecular properties such as surface tension, viscosity, pH, conductance and concentration of solution.(4)

10. Which type of apparatus used in viscosity measurement? (a) Ostwald viscometer (b) stalagmometer (c) Pipette (d) specific gravity bottle 11. The force present between similar molecules is known as (a) cohesive force (b) adhesive force (c) vander wall force (d) none of these 12. What is the unit of viscosity? (a) Kg/L (b) poise (c) gm/L (d) dynes/cm 13. Which apparatus is used for the determination of density of liquids? a) Ostwald viscometer (b) stalagmometer (c) Pipette (d) specific gravity bottle CO3. Identify iron concentration and percentage of available chlorine in supplied sample using titration methods.(7)

14. What is the colour of potassium ferricyanide indicator? (a) Red (b) pink (c) yellow (d) orange 15. End point in iodometric titration by titrating iodine content in iodide salt with hypo solution is

(a) Blue to colourless (b) wine red to blue (c) pink to colourless (d) red to blue 16. Which salt of Potassium is used in iodometric titration? (a) KI (b) KIO3 (c) KClO3 (d) none 17. What colour obtained when starch added in the solution of iodized salt (a) Red (b) pink (c) colourless (d) blue 18. Which gas get liberated when conc. Sulphuric acid is added to a solution of iodized salt (a) I2 gas (b) Cl2 gas (c) H2 gas (d) CO2 gas 19.What is the oxidation state of Fe in K3Fe(CN)6 (a) +2 (b) +3 (c) +4 (d) none 20.What is the colour of Ferrous ferricyanide.

(a) Red (b) pink (c) colourless (d) blue

P

1

1

1


B.Tech.

RAS-152, Engineering Chemistry Laboratory Quiz

First Semester 2017-2018 Answer all Questions. Put mark by choosing the correct answer

Faculty Name : Branch: Name of student : Date: Roll. No. : Time: 201 minutes 1. What is the oxidation state of Cr in K2Cr2O7?

(a) +2 (b) +3 (c) +6 (d) +4

2. What is the colour of starch indicator? (a) Red (b) pink (c) colourless (d) orange 3. What is the unit of viscosity? a) ppm (b) Poise (c) mg/L (d) Dynes/m2 4. Which standard solution is used in the determination of alkalinity of water sample? (a) N/10 HCl (b) N/20 NaOH (c) (EDTA)Na2 (d) none 5. Buffer solution is added into titrating mixture: (a) to alter pH (b)to maintain pH (c )both a and b (d) none 6. What colour obtained when starch added in the solution of iodized salt (a) Red (b) pink (c) colourless (d) blue 7. 3.4 - 4.3 is the pH range for which indicator (a) Phenolphthalein (b) EBT (c) Methyl orange (d) none 8. When density is increases the viscosity of liquids get

(a) Increases (b) decreases (c) no effect (d) none 9. What colour does phenolphthalein gives with carbonates and hydroxides in the solution? (a) Orange (b) pink (c) colourless (d) yellow 10. What is the chemical formula of Bleaching Powder?

(a) CaCl2 (b) CaOCl2 (c) Ca (OH)2 (d) CaCO3

11. Name the colour developing agent in Colorimetric method

(a) KNCS (b) Starch (c) KCNS (d) Phenolphthalein

12. When P>1/2M, which alkaline ions present in water sample (a) OH_ (b) CO3

_ (c) HCO3-& CO3

_ (d) OH_ & CO3 _

13. Which indicator is used in determination of ferrous content?

(a) K3[Fe(CN)6] (b) EBT (c) Starch (d) K2CrO4

14. The end point for the chloride content determination is formation of

(a) Reddish brown precipitate (b) brown precipitate (c) yellow precipitate (d) white

precipitate

15. Which standard solution is used in the determination of chloride content of water sample? (a) N/10 HCl (b) N/20 NaOH (c) (EDTA)Na2 (d) AgNO3 16. What is the chemical formula of Mohr’s salt

(a)FeSO4. (NH4)2SO4.6H2O (b) (NH4 )2SO4.6H2O (c) FeSO4.6H2O (d)None 17. Hardness can be calculated in terms of (a) CaCO3 equivalent (b) MgCO3 equivalent (c) CaSO4 equivalent (d) none 18. Which indicator is used in iodometric titration?

(a) Methyl Orange (b) Starch (c) Potassium permanganate (d) EBT

19. Potassium ferricyanide (K3[Fe(CN)6]) is used as an:

P

1

1

1

(a) Internal indicator (b) External indicator (c) Self indicator (d) none

20. Lambert’s Beer Law: (a) C=A.ε.l (b) A= ε.c.l (c) l= ε.c.A (d) none


B.Tech. 2017

RAS-252, Engineering Chemistry Laboratory

Second Semester QUIZ

Answer all Questions. Put mark by choosing the correct answer Faculty Name : Branch: Name of student : Date: Roll. No. : Time: 202 minutes 1. What is the colour of starch indicator? (a) red (b) pink (c) colourless (d) orange 2. Which gas get liberated when conc. Sulphuric acid is added to a solution of iodized salt (a) I2 gas (b) Cl2 gas (c) H2 gas (d) CO2 gas 3. Which salt of Potassium is used in iodometric titration (a) KI (b) KIO3 (c) KClO3 (d) none 4. Which type of apparatus used in viscosity measurement? (a) Ostwald viscometer (b) stalagmometer (c) Pipette (d) specific gravity bottle 5. Hardness can be calculated in terms of (a) MgCO3 equivalent (b) CaCO3 equivalent (c) CaSO4 equivalent (d) none 6. What colour obtained when starch added in the solution of iodized salt (a) red (b) pink (c) colourless (d) blue 7. 8.0-10.0 is the pH range for which indicator (a) Phenolphthalein (b) EBT (c) Methyl orange (d) none 8. Which salt is responsible for permanent hardnees (a) CaSO4 (b) Ca(HCO3)2 (c) Mg(HCO3)2 (d) none 9. What colour does Methyl orange gives with bicarbonates and carbonates in the solution (a) orange (b) pink (c) colourless (d) yellow 10. Lambert’s Beer Law: (a) C=A.ε.l (b) A= ε.c.l (c) l= ε.c.A (d) none 11. End point in iodometric titration by titrating iodine content in iodide salt with hypo solution is

(a) blue to colourless (b) wine red to blue (c) pink to colourless (d) red to blue 12. What is the unit of viscosity? (a) Kg/L (b) poise (c) gm/L (d) dynes/cm 13. Which apparatus is used for the determination of density of liquids a) Ostwald viscometer (b) stalagmometer (c) Pipette (d) specific gravity bottle 14. Name the colour developing agent in Colorimetric method

(a) KNCS (b) Starch (c) KCNS (d) Phenolphthalein

15. When P<1/2M, which alkaline ions present in water sample (a) OH_ (b) CO3

_ (c) HCO3-& CO3

_ (d) OH_ & CO3 _

16. Which standard solution is used in the determination of hardness of water sample (a) N/10 HCl (b) N/20 NaOH (c)M/100 (EDTA)Na2 (d) none 17.Which two alkaline ions does not exist together (a) HCO3

-& CO3 _ (b) OH- & CO3

_ (c ) HCO3-& OH- (d) None

18. What colour does phenolphthalein gives with bicarbonates in the solution? (a) colourless (b) pink (c) orange (d) yellow 19. Which standard solution is used in the determination of chloride content by Mohr ’s method? (a) N/10 HCl (b) N/20 K2CrO4 (c) M/100 (EDTA)Na2 (d) N/100 AgNO3

P

1

1

1

20. What colour does phenolphthalein gives with bicarbonates in the solution (a) colourless (b) pink (c) orange (d) yellow

Lecture No. CO Kx

Unit No. Topic

Date Planned (to be generated as per first time-table)

(YYYY - MM - DD)

Link of Video Lecture (Uploaded to MS Stream through FYStudyMat login, prior to conduct of classes)

Remarks, if any

0 Introduction to OBE, Vision, Mission, PO, CO, Syllabus etc https://web.microsoftstream.com/video/1d276158-773d-4249-8b46-b162c50647c7

https://web.microsoftstream.com/video/6148b9f2-b75b-4b8c-af29-17ade59e63f8 A(Demo)https://web.microsoftstream.com/video/5135defb-e4a8-4a41-b3a8-b8fff930aee3 B(ppt recording)https://web.microsoftstream.com/video/ec30e573-77d6-45f4-8773-32a442191e0f A(Demo)https://web.microsoftstream.com/video/c8242620-944c-43e5-b23b-b6493a8dee94 B(ppt recording)https://web.microsoftstream.com/video/10e1615a-27bc-4412-8647-c3d0cbd2e2bc A(Demo)https://web.microsoftstream.com/video/0bbd5d7b-bea7-4561-b1e8-283a726365f8 B(ppt recording)https://web.microsoftstream.com/video/d66d72df-d982-494d-9986-e82cc2802eba A(Demo)https://web.microsoftstream.com/video/ee1891d3-702b-4051-a628-055696a440b3 B(ppt recording)https://web.microsoftstream.com/video/687b3a31-329a-4945-a8b0-b01a931975f7 A(Demo)https://web.microsoftstream.com/video/c06fdedd-d35f-4325-a74b-133321721f2d B(ppt recording)https://web.microsoftstream.com/video/8861850d-62e8-40b3-8e3a-2d080e31824a A(Demo)https://web.microsoftstream.com/video/6d9ee755-bebc-407a-935a-9c3619acce74 B(ppt recording)https://web.microsoftstream.com/video/bf746206-fed3-453a-847a-7ebacf7bdbd8 A(Demo)https://web.microsoftstream.com/video/b2995726-f95c-4e88-8c6f-9d1fa053c376 B(ppt recording)https://web.microsoftstream.com/video/734f8f87-5989-449a-a81e-674c31eb6cbf A(Demo)https://web.microsoftstream.com/video/650f3727-71d6-46ca-abb1-b0783ea0b1ad B(ppt recording)

Galgotias College of Engineering and Technology, Greater Noida

Teaching / Lecture / Lesson Plan (Engg Chemistry Lab) : B. Tech. – I Sem : 2021-22Subject Name with Code : Engineering Chemistry Lab (KAS152P) ## Teaching Pedagogy : Students’ Centric

Determination of temporary and permanent hardness in water sample using EDTA

CO1 K41

Determination of alkalinity in the given water sample.

K4CO12

7

4 CO3 K2 Determination of available chlorine in bleaching powder.

Determination of chloride content in water sample

K4CO13

Determination of iron content in the given solution of Mohr‟s salt

K2CO3

CO2

Determination of viscosity of given liquid.K2CO2

Determination of surface tension of given liquid.

K2

5

CO28 Verification of Beer"s law. K2

6

Lecture No. CO Kx

Unit No. Topic

Date Planned (to be generated as per first time-table)

(YYYY - MM - DD)

Link of Video Lecture (Uploaded to MS Stream through FYStudyMat login, prior to conduct of classes)

Remarks, if any

Teaching / Lecture / Lesson Plan (Engg Chemistry Lab) : B. Tech. – I Sem : 2021-22Subject Name with Code : Engineering Chemistry Lab (KAS152P) ## Teaching Pedagogy : Students’ Centric

https://web.microsoftstream.com/video/954f6d7a-8d6c-4e1e-a7a0-09e908668f56 A(Demo)https://web.microsoftstream.com/video/c635ca9c-e858-447c-b481-ae2c0f8c62f3 B(ppt recording)

Determination of pH by pH-metric titration.K2CO29

kas 152p/252p session 2021-2022 - galgotiacollege.edu

Documents