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LAB MANUAL
ENGINEERING CHEMISTRY (A10081)
R16 – JNTUH
I B.Tech (Common to all Branches)
Humanities and Basic sciences
MARRI EDUCATIONAL SOCIETY’S GROUP OF INSTITUTIONS
MARRI LAXMAN REDDYINSTITUTE OF TECHNOLOGY & MANAGEMENT
(Approved by AICTE, New Delhi & Affiliated JNTU Hyderabad)
Dundigal (v), Quthbullapur (M), R.R. (D), Hyderabad-500043, T.S
Website:www.mlritm.ac.in, Email:[email protected]
MARRI EDUCATIONAL SOCIETY’S GROUP OF INSTITUTIONS
MARRI LAXMAN REDDYINSTITUTE OF TECHNOLOGY & MANAGEMENT
(Approved by AICTE, New Delhi & Affiliated by JNTU Hyderabad)
CCeerrttiiffiiccaattee
This is to Certify that it is a bonafied record of Practical work done by
Sri/Kum. _____________________________________ bearing
the Roll No. ______________________ of ____________ Class
_______________________________________ Branch in the
____________________________ laboratory during the Academic
year ___________________ under our supervision.
Head of the Department Lecture In-Charge
External Examiner Internal Examiner
Index
S. No. List of Experiments Page No. Date Remarks
I Estimation of hardness of water by EDTA method
II Determination of viscosity of sample oil by Oswald’s
viscometer
III
Conductometric titration of strong acid vs. strong base
IV Conductometric titration of mixture of acid vs. strong base
V Potentiometric titration of strong acid vs. strong base
VI Estimation of manganese dioxide in pyrolusite
VII
Determination of the Percentage of Available Chlorine
present in Bleaching Powder sample
VIII
ESTIMATION OF FERROUS IRON BY
DICHROMETRY
IX To prepare phenol formaldehyde resin. (Bakelite)
X To prepare Urea formaldehyde
XI Estimation of cu by iodometry
XII Estimation of ferrous Iron by potentiometry
XIII Estimation of ferrous Iron in cement by colorometric
method
XIV Estimation of Ferrous iron by permanganometry
XV Estimation of Ferrous&Ferric ions in a given mixture by
dichrometry
XVI Determination of Salt concentration by Ion-exchange resin
XVII Estimation of Manganese in kmno4 by colorometric
method
Engineering Chemistry Laboratory Chemistry Lab Do’s & Don’ts
The chemistry laboratory must be a safe place in which to work and learn about chemistry. Most of
these involve just using common sense.
1. Wear a chemical-resistant apron.
2. Be familiar with your lab assignment before you come to lab. Follow all written and verbal
instructions carefully. Observe the safety alerts in the laboratory directions. If you do not
understand a direction or part of a procedure, ask the teacher before proceeding.
3. When entering the lab/classroom, do not touch any equipment, chemicals, or other materials
without being instructed to do so. Perform only those experiments authorized by the instructor.
4. No student may work in the laboratory without an instructor present. Work only with your lab
partner(s). Do not venture to other lab stations for any reason.
5. Do not wear bulky or dangling clothing.
6. Never eat or drink in the laboratory. Don't chew on the end of a pen which was lying on the lab
bench.
7. Wash acid, base, or any chemical spill off of yourself immediately with large amounts of water.
Notify your teacher of the spill.
8. Clean up spills immediately. If you spill a very reactive substance such as an acid or base, notify
the people in the area and then obtain assistance from your teacher. Acid spills should be
neutralized with baking soda, base spills with vinegar before cleaning them up.
9. If chemical substances get in your eye, wash the eye out for 15 minutes. Hold your eye open with
your fingers while washing it out.
10. When weighing never place chemicals directly on the balance pan. Never weigh a hot object.
11. Never smell anything in the laboratory unless your teacher tells you it is safe. Do not smell a
substance by putting your nose directly over the container and inhaling. Instead, waft the vapors
toward your nose by gently fanning the vapors toward yourself.
12. Do not directly touch any chemical with your hands. Never taste materials in the laboratory.
13. If you burn yourself on a hot object, immediately hold the burned area under cold water for 15
minutes. Inform your teacher.
14. Observe good housekeeping practices. Work areas should be kept clean and tidy at all times.
Only lab notebooks or lab handouts should be out on the table while performing an Experiment.
Books and book bags should not be on the lab table. Passageways need to be clear at all times.
15. Always replace lids or caps on bottles and jars.
16. If your Bunsen burner goes out, turn the gas off immediately.
17. Always add acid to water and stir the solution while adding the acid. Never add water to an acid.
18. Report all accidents to your teacher.
19. Absolutely no running, practical jokes, or horseplay is allowed in the Laboratory.
20. Thoroughly clean your laboratory work space at the end of the laboratory Session. Make sure that
all equipment is clean, and returned to its original place.
EXPERIMENT-I
ESTIMATION OF HARDNESS OF WATER BY EDTA METHOD
AIM: To estimate the total hardness, permanent hardness and temporary hardness of water by using
standard solution of EDTA
APPARATUS: Burette, pipette, Conical flask, Beakers, Standard flask, Burette stand and funnel etc..
CHEMICALS REQUIRED: Buffer sol
n, EDTA sol
n, Eriochrome black-T, Magnesium sulphate etc.
PRINCIPLE: Hard water which contains Ca
2+ andMg
2+ ions which forms wine red color complex with the
indicator
Ca2+
(or) Mg2+
+ EBT ———> Ca-EBT (or) Mg-EBT
(Wine red colour complex)
EDTA forms a colour less complex with the metal ions (Ca2+
andMg2+
)
Ca-EBT (or) Mg-EBT + EDTA———> Ca-EDTA (or) Mg-EDTA + EBT
(Wine red colour complex) (Colorless stable complex) (Blue)
When free ions are not available, EDTA extracts the metal from (ion) metal ion indicator
complex, there by releasing the free indicator.
PROCEDURE:
STEP-I
PREPARATION OF STANDARD SOLUTION OF MgSO4:
Weigh the approx 0.25gm of MgSO4 and transfer into 100ml standard flask through the
funnel and dissolve in minimum quantity of distilled water. Make up the solution up to the
mark with distilled water and shake the flask well for uniform concentration then calculate
the Molarity of MgSO4
M. Wt. of MgSO4 = 246.48gm
Molarity of MgSO4=0.01M
STEP-II
STANDARDISATION OF EDTA SOLUTION:
Pipette out 20ml of MgSO4 sol. into a clean conical flask. Add 2ml of buffer sol. and add
2 to 3 drops of EBT indicator and it gets wine red color sol. Take EDTA solution in a
burette after titrate with EDTA solution till wine red color changes to blue color. Note the
burette reading and repeat the titration to get concurrent values.
S. No Volume of
MgSO4 in ml
Burette Reading Volume of EDTA
consumed Initial Final
1 20
2 20
3 20
M1 = MgSO4 molarity M2 = EDTA molarity
V1 = volume of MgSO4 V2 = volume of EDTA consumed
M1V1 = M2V2
STEP-III
STANDARDISATION OF HARD WATER:
Pipette out 20ml of tap water into a 250ml conical flask add 2 ml of buffer sol. and add 2-
3drops of EBT indicator. Titrate the wine red color sol. with EDTA taken in burette, till a
blue color end point is obtained. Repeat the titration to get concurrent values.
S. No Volume of Hard
water in(ml)
Burette Reading Volume of EDTA
consumed Initial Final
1 20
2 20
3 20
M3 = molarity of hard water M2 = EDTA molarity
V3= volume of Hard water V2 = volume of EDTA consumed
M3V3 = M2V2
Total hardness= M3X100X1000
STEP-IV
STANDARDISATION OF PERMANENT HARDNESS OF WATER:
Pipette out 100ml of hard water sample into a beaker containing 250ml and boil the water
till volume reduces to 50ml (all the bicarbonates of Ca2+
, Mg2+
decomposes toCaCO3and
Mg(OH)2 respectively). Cool the solution and filter the water into beaker then pipette out
20ml of this cool water sample in to 250ml conical flask add 2ml of buffer sol. and 2-3
drops of EBT indicator. Titrate the wine red color solution with EDTA taken in the
burette, till a blue colored solution end point is obtained. Repeat the titration to get
concurrent values.
S. No Volume of Hard
water in (ml)
Burette Reading Volume of EDTA
consumed Initial Final
1 20
2 20
3 20
M4 = molarity of hard water M2 = EDTA molarity
V4 = volume of hard water V2 = volume of EDTA consumed
M4V4 = M2V2
Permenent hardness = M4X100X1000 = --------------PPM
RESULT:
1) Total Hardness in _______ PPM
2) Permanent Hardness in _______ PPM
3) Temporary hardness in _______ PPM
VIVA QUESTIONS:
1)What is EDTA and structure?
2)What is buffer solution?
3)What is Hardness?
4)Which hardness can be removed by boling?
5)What is the indicator?
EXPERIMENT - II
DETERMINATION OF VISCOSITY OF LIQUIDS BY OSWALD'S VISCOMETER
AIM: To determine the absolute viscosity of a liquid by using Oswald’s viscometer.
APPARATUS:
Oswald’s viscometer, stop watch, density bottle, rubber bulbs, Beakers, etc.
CHEMICALS REQUIRED:
Standard liquid (water), test liquid etc.
PRINCIPLE: (POISEUILLE'S PRINCIPLE)
If a liquid flows with in a uniform velocity at a rate of 'V'in 't' seconds through a capillary
tube of radius 'r' and length 1cm under a driving pressure 'p' dynes/ cm2. Then,
The co-efficient of viscosity is given as =
Viscosity of liquid in poise
P pressure head i.e. dynes/ cm2.
r radius of inner layer of capillary tube
L length of capillary tube
V volume of capillary tube
t flow time in seconds
The poiseulles law is applicable only to linear flow or stream line flow. For a given Oswald’s
viscometer the length, radius and volume of liquids are constants and at end are combined to
a single constant. The above equation can be written as
= k t P In this eq. P depends on
I. Density of liquid to be measured
II. Acceleration due to gravity
III. the difference due to gravity is constant Then
The viscosity of liquid may be expressed as
1= kt1
1 (viscosity Standard liquid (water))
2=kt2
2(viscosity of test liquid)
Relative viscosity
1/
2= t1
1/ t2
2
Units: (CGS) dynes-sec/cm2 or poise
= r4 t P/ 8VL
PROCEDURE:
Clean thoroughly and dry the Oswald’s viscometer, a definite volume of standard liquid is
allow to flow into 'A ' arm such that it raises above the values X and Y. The same procedure
is repeated with the test liquid and note the time by stop clock
CALCULATIONS:
S. No Standard liquid (t) Density(d)
TRIAL - I
TRIAL - II
Weight of empty density bottle (W1) = _________ gm
Weight of empty bottle + water (W2) = _________ gm
Weight of empty bottle +liquid (W3) = _________ gm
Density of water ( 1) = _______
Density of liquid ( 2) = _______
Viscosity Standard liquid ( 1) at 25oC= 1.0019cps
2= t2
2/ t1
1 x
1
RESULT:
Absolute viscosity of a given liquid (
2) = ________ cps
VIVA QUESTIONS:
1)What is viscocity?
2)What are the units of viscocity?
3)What are the apparatus are used to determine the viscocity?
4)What is lubricant?
5)What is formula of viscocity?
EXPERIMENT - III
CONDUCTOMETRIC TITRATION OF STRONG ACID VS STRONG BASE
AIM: To determine the strength of the strong acid by titration with strong base Conductometrically.
APPARATUS:
Conductivity Bridge, Conductivity cell, Burette, Beakers, Standard flask, pipette, Burette Stand
etc.
CHEMICALS REQUIRED: Sodium hydroxide, Hydrochloric acid
PRINCIPLE:
At first solution contain H+ and Cl
- ions. Since H
+ions posses greater mobility it follows that the
conductivity is mainly due to H+ ions. The addition of NaOH is represented by the equation.
H+ + Cl
- + Na
+ + OH
- ————> Na
++ Cl
- + H2O
As NaOH is added the H+ ions are removed. The conductivity decreases as Na
+ ions do not
process much mobility. As the neutralization point and solutions contains Na+ions and Cl
- ions
and will have minimum conductance value. If NaOH is further added this will add OH- ions and
so the conductivity increases.
PROCEDURE:
A standard solution of 0.2N NaOH is prepared. Similarly 0.1N HCl is prepared. 20 ml of HCl is
taken in a 100 ml beaker and to it 20 ml of distilled water is added and kept in a thermostat. The
conductivity cell is washed with distilled water and rinsed with acid soln. The cell is kept in acid
containing beaker and it is connected to the bridge. The conductivity of the soln is measured by
adjusting the reading. NaOH soln is taken into burette and add 1 ml of soln to acid, stirred well
and conductance is measured. Each time 1 ml of base is added to acid stirred well and the
conductance is measured. For every instance. Equal numbers of values are taken on either side of
the point of maximum. Repeat the procedure of addition of 1 ml NaOH and noting the
conductivity of the resulting solution. Take 20-25 readings
GRAPH:
CALCULATIONS:
S. No Volume of NaOH Observed conductance
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
FORMULA:
N1V1 = N2V2
RESULT:
The normality of strong acid (HCl) determined by titrating against a strong base (NaOH)
=________N
VIVA QUESTIONS:
1)What is conductance?
2)What is neutralization point?
3)What are the units of conductance?
4)Explain graph?
5)What is acid&Base?
EXPERIMENT - IV
CONDUCTOMETRIC TITRATION OF MIXTURE OF ACIDS VS STRONG BASE
AIM: To determine the strength of the mixture of acids by titration with strong base
Conductometrically.
APPARATUS:
Conductivity Bridge, Conductivity cell, Burette, Beakers, Standard flask, pipette, Burette Stand
etc.
CHEMICALS REQUIRED:
Sodium hydroxide (NaOH), Hydrochloric acid(HCl) and Acetic acid(CH3COOH) etc…
PRINCIPLE:
The conductivity of the solution is related to the mobility of ions which in turn related with the
size of the ions. When a mixture of acids like a strong acid (HCl) and weak acid (acetic acid) are
titrated against a strong base (NaOH), strong acid reacts first followed by a weak acid. When the
titration of strong acid and strong base are carried out, there is a decrease in conductivity as
highly mobilized hydrogen ions are replaced by sodium ions.
NaOH + HCl -------> NaCl + H2O
When the whole strong acid is consumed, base reacts with weak acid and conductivity increases
as unionized weak acid becomes the ionized salt.
CH3COOH + NaOH---------->. CH3COONa + H2O
After both the acids are consumed, there is a steep increase in conductivity which gives the end
point and this increase in conductivity is due to the fast moving hydroxyl ions from the base.
From this, amount of base consumed for acid and in turn, the amount of acids present is
calculated.
Let V1 and V2 ml be the volumes of alkaline corresponding beaker resp. Then V1 ml of NaOH
equivalent to HCl, (V2-V1)S ml of NaOH equivalent to CH3COOH
FORMULA:
N1V1 = N2V2
GRAPH:
PROCEDURE:
1) Fill the burette with standard 0.2N NaOH solution
2) Take the given mixture (25 ml of CH3COOH + 25 ml of HCl) in a small beaker and
titrate against NaOH Conducto metrically.
3) Add 1ml of NaOH from burette and stir well and note down the conductance of solution.
4) Repeat the determination by stirring well after each addition of 1ml of NaOH until add up
to 25-30 ml of NaOH.
5) Plot a graph between volume of NaOH Vs Conductance.
OBSERVATIONS AND CALCULATIONS:
S. No Volume of NaOH Observed conductance
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
The volume of NaOH corresponding to the first point of inflectionsis V1= X1 ml and that
corresponding to the second point of inflectionis V2 = X2 ml.
V2-V1=X3 ml
Hence the HCl and CH3COOH in their mixture of volume (50ml) consume respectively X1ml
and X3 ml
There fore
(a). Strength of HCL = X1ml x con. of NaOH
--------------------------- = ----------N
20ml
(b). Strength of CH3COOH = X3ml x con. of NaOH
--------------------------- = --------N
20ml
RESULT:
1) Strength of given HCl = _______________N
2) Strength of given CH3COOH = _____________N
VIVA QUESTIONS:
1)How many neutralization points are there in this experiment?
2)What is neutralization point?
3) What are the chemicals are used in this experiment?
4)Explain graph?
5)What are the examples of acid&bases?
EXPERIMENT – V
POTENTIOMETRIC TITRATION OF STRONG ACID VS STRONG BASE
AIM:
To determine the strength of the strong acid by titration with strong base Potentiometrically.
APPARATUS:
Potentiometer, Platinum electrode, Calomel electrode, Burette, Beakers, Standard flask,
pipette, Burette Stand etc.
CHEMICALS REQUIRED: Sodium hydroxide, Hydrochloric acid and Quinhydrone powder etc.
PRINCIPLE:
The cell will have certain emf depending upon pH value of the solution, on adding small
portions of alkali to an acid. The acid potential changes slowly at first since the change in
electrode depends on the fraction of hydrogen ions removed. After addition of certain amount
of alkali the titration of hydrogen ions removed by alkali increases, correspondingly there is a
rapid decrease in emf on addition of excess of alkali. The emf again shows a flow change. If
a graph is plotted by taking volume of alkali added on X- axis and change in emf by point of
intersection on Y-axis, a curve is obtained.
H+ + Cl
- + Na
+ + OH
- ————> Na
++ Cl
- + H2O
The cell can be represented as
H2, Pt/Acid soln // KCl aq / Calomel electrode
PROCEDURE:
Calibrate the instrument before starting the experiment. Approximately 0.1N HCl is
prepared and standard decinormal solution of NaOH is prepared. Exactly 20 ml of the acid
is pipette out into a clean 100ml of beaker and a pinch of Quinhydrone is added which acts
as indicator. Platinum electrode and calomel electrodes are dipped in the solution.
The alkali (NaOH) against which the acid is being titrated is taken in burette. The solution
is stirred well with a glass rod. The end reading is taken after adding definite amount of
alkali. Finally after knowing the range in which the end point can be located, the whole
experiment is repeatedly adding in steps of 1 ml in the end point.
GRAPH:
Two graphs are plotted of which one is between volume of alkali and observed emf and
other is between volume of alkali andE/V Sigmoid curve
CALCULATIONS:
S. No Volume of NaOH Observed EMF
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
FORMULA:
N1V1 = N2V2
EMF
Vol. of NaOH
RESULT:
The normality of strong acid (HCl) determined by titrating against a strong base (NaOH)
=________N
VIVA QUESTIONS:
1)What is EMF?
2)What are the electrodes are used in this experiment?
3)What is neutralization point?
4)What is the indicator electrode?
5)Explain graph?
EXPERIMENT-VI
ESTIMATION OF MANGANESE DIOXIDE IN PYROLUSITE
AIM: To estimate the amount of MnO2 present in the given sample of pyrolusite.
APPARATUS: Burette, pipette, conical flask, Standard flask, Burette, stand, Funnel and Beaker etc.
CHEMICALS REQUIRED:
Sodium Oxalate, Potassium permanganate, Sulphuric acid, pyrolusite sample and MnO2 ….
PRINCIPLE:
The MnO2 present in the pyrolusite sample is reduced by a known excess of standard Sodium
Oxalate solution and the uncreated oxalate is titrated against a standardized solution of
KMnO4, where KMnO4 acts as self indicator. Pale pink color is the end point of the titration.
MnO2 + Na2C2O4 + 2 H2SO4 --------> MnSO4 + Na2SO4 +2CO2 + 2H2O
(From pyrolusite)
Na2C2O4+KMnO4 +8H2SO4------->2MnSO4+K2SO4+5 Na2SO4+10CO2+8H2O
(Unreacted)
PROCEDURE:
1) PREPARATION OF STANDARD SODIUM OXALATE SOLUTION:
Weigh 0.67 gram of sodium oxalate into a clean 100 ml standard flask, dissolve in small
amount of water and make up the solution up to the mark with distilled water. Shake the
flask well for uniform concentration.
2) PREPARATION OF KMNO4 SOLUTION:
Dissolve 0.79 gram of KMnO4 into a 250 ml standard flask in little distilled water and
make up the solution up to the mark with distilled water. Shake the flask well for uniform
concentration.
3) PREPARATION OF 0.1N SULPHURIC ACID:
Dissolve 0.72 ml of concentrated H2SO4 slowly drop by drop in 100 ml of distilled water
(the acid must be added to water not water to acid)
4) STANDARDIZATION OF KMNO4 SOLUTION:
Rinse the burette with KMnO4 and fill the burette with KMnO4 up to zero mark, pipette
out 10ml of sodium oxalate into a clean 250 ml of conical flask and add 5 ml of 0.1N
H2So4 and keep the solution till fumes come out of the solution (70-80oC). Titrate the hot
solution with KMn04 till pale pink color is observed in the solution Repeat the solution to
get concurrent values. Let the titre value of the sample be X ml.
5) STANDARDIZATION OF PYROLUSITE SAMPLE:
Weigh out accurately about 0.20-0.25gm of sample into a 250 ml dry conical flask and
exactly 40 ml of sodium oxalate with the help of pipette and 40 ml of 0.1N H2SO4
solution. Put a small funnel in the neck of the flask and heat the solution on a small
flame. Till all the black particles of pyrolusite disappear in the conical flask. Now wash
the funnel and the side of the conical flask with little distilled water in to the flask and
titrate the unreacted oxalic acid present in hot solution with KMn04 solution taken in the
burette. Pale pink color is the end point of the titration. Let the titre value with unreacted
oxalic acid be Y ml.
Note: The titration of unreacted oxalic must be carried out in hot condition i.e. 60-70 oC.
6) STANDARDIZATION OF BLANK SOLUTION: Pipette out 40 ml of sodium oxalate solution into a 250 ml of conical flask and add 50 ml
of 0.1N H2SO4. Keep a small funnel in the neck of the flask and heat to 70-80oC, rinse
the funnel and neck of the flask with distilled water and titrate the hot solution with
KMn04 till pale pink colored end point is obtained the titre value z ml indicates the total
amount of potassium permanganate required for the complete reaction of the 40 ml of
sodium oxalate.
CALCULATIONS:
Weight of pyrolusite = ---------- gm
Normality of KMnO4 = 0.1N
Titre value of pyrolusite(Y) = ………….ml
Blank titre value (Z) = ………ml
Volume = Blank titre value (Z) – Titre value of pyrolusite(Y) (Eq. wt. of MnO2 =
43.46gm)
Amount of MnO2 present in sample= Volume X Normality of KMnO4 X Eq. wt. of MnO2 /
1000
% of MnO2 present in given sample = Amount of MnO2 X 100 / Wt. of sample
RESULT:
The amount of manganese dioxide present in given sample of pyrolusite is --------%
VIVA QUESTIONS:
1)What is pyrolusite?
2)What is self indicator in this in this experiment?
3)What is the mwt of KMNO4?
4)What is molarity?
5)What is Normality?
EXPERIMENT-VII
Determination of the Percentage of Available
Chlorine present in Bleaching Powder sample
Aim
Determine the percentage of available chlorine present in the given sample of bleaching
powder.
Theory
Bleaching powder is used as a bleaching agent and also as a disinfectant. The main constituent
of bleaching powder is calcium hypochlorite [Ca(OCl)2] which supplies chlorine [Cl2] with
dilute
acids.
So the available chlorine is defined as the percentage of chlorine made available by bleaching
powder when treated with dilute acids. The available chlorine present in bleaching powder
sample is
determined iodometricaliy by treating its solution with an excess of potassium iodide solution in
the
acidic medium.
The liberated iodine (I2) is treatedwith sodium thiosulphate (Na2S2O3) solution using freshly
prepared starch solution as indicator to be added near the end point.
Apparatus:
Digital Balance, Burette, Conical flask, Measuring flask, Funnel, Glass rod, Beakers
Reagents:
Bleaching powder, Standard sodium thiosulphate solution
10% Potassium iodide (KI)
dilute acetic acid, freshly prepared starch solution as indicator
Observations and Calculations:
S.No Volume of givenbleaching volume of sodium
thiosulphate
Initial Final
1
2
3
Concordant Volume of Na2S2O3 solution, V1 =………ml
Normality of standard Na2S2O3 solution,
Volume of standard Na2S2O3 solution, V1 = ……………ml
Volume of given bleaching powder solution , V2 = ………….....ml
Normality of given water sample, N2 can be calculated from the normality formula,
i.e., N1 x V1 = N2 x V2
Normality of given bleaching powder solution, N2 =
= ……………………N
Amount of available chlorine = = ………………..g/Lit
Amount of available chlorine present in 100 ml ofthe solution= ………………..g
The percentage of available chlorine present in the
given sample of bleaching powder (BP)= …………..%
Procedure:
………….g of bleaching powder is accurately weighed in a weighing bottle.It is transferred to a
clean beaker and is ground to a thin paste with water. The mixture allowed tosettle and the milky
supernatant liquid poured into a 100 ml standard flask. The residue in the beakeris ground with a
little more water and the operation repeated until the whole of the sample has beenquantitatively
transferred into the standard flask. Then the solution is made up to the volume.The flask is
shaken well for uniform concentration.
10 ml of the solution (use measuring flask) in a state of very fine suspension is taken into
a conical flask and add 10 ml of distilled water into it. Then add 10 ml of 10% potassium iodide
(KI)solution and 10 ml of dilute acetic acid. This solution [which contains liberated iodine (I2)]
titrateswith standard sodium thiosulphate solution (taken in the burette) until the dark brown
colour changesto pale yellow. To this add, 2 ml of freshlyprepared starch solution as indicator, so
the colour of thesolution turned into blue. Continue the titration till the disappearance of blue
colour of the solutionand note down the volume of the titrant used. The titration is repeated until
a concordant volume is
obtained.
Result:
The percentage of available chlorine present in the given sample of bleaching powder
is…………..%
VIVA QUESTIONS:
1)Give formula of bleaching powder?
2)What is chlorination?
3) What are the chemicals are used in this experiment?
4) What are the apparatus are used in this experiment?
5)What is available chlorine?
EXPERIMENT-VIII
ESTIMATION OF FERROUS IRON BY DICHROMETRY
AIM:
To estimate the amount of ferrous iron present of the whole solution with the help of standard
solution of potassium dichromate.
APPARATUS:
Beaker, burette, pipette, conical flask, volumetric flask.
CHEMICALS:
K2Cr2O7, diphenylamine, Conc.H2SO4,Distilled water.
THEROY AND PRINCIPLE:
Ferrous iron is oxidized to ferric iron by potassium dichromate in acid solution. The
completion of the oxidation of reaction is marked by the appearance of blue violet colorof the
diphenylamine which is used as an internal indicator.
The equivalent weight of iron is its atomic weight i.e.55.86 since one equivalent of potassium
dichromate oxidizes one equivalent of iron.
PROCEDURE:
1)Preparation of standard potassium dichromate:weigh out accurately about 0.49gms of
potassium dichromateinto a standard flask into a100 ml standard flask and dissolve the solid in a
small quantity of distilled water make up the resulting solution with distilled water up to themark
and shake the flask wellfor uniform concentration.
2)Preparation of acid mixture:
Mix up 100 ml of phosphoric with 300ml of concentrated H2S04in a reagent bottle and stopper
it.
3)Preparation of diphenylamine:
Dissolve 1gm of diphenylamine in 100ml of concentrated H2So4
4)Standardization of ferrous iron:Rinse the burette with K2Cr2O7solution and take
K2Cr2O7solution up to the zero of the burette. Pipette out 20ml of ferrous solution into a 250ml
conical flask, add 5ml of acid mixture and 2drops of diphenylamine indicator. Titrate the
resulting solution with potassium dichromate taken in the burette till blue violet coloris obtained
as end point. Repeat the titration to get concurrent values
CALCULATIONS AND OBSERVATIONS:
S.No Fe+2Solution(in ml ) Burette reading Volumek2cr2O7consumed.
Initial Final
Normality of K2Cr207(N) = Wt .of K2Cr207*10 / 49
Normality of ferrous iron(N2): N1V1 =N2V2
V1 = Volume of K2Cr207(Titrevalue ....ml)
N2= Normality of K2Cr207
V2= Volume of ferrous ironN2 =NIVI / V2 =
Titervalue* N1 / 20
RESULT:
Amount of ferrous iron present in the given solution =.................gms/100ml.
VIVA QUESTIONS:
1)What is the atomic no.of Fe?
2)What is molarity?
3) What are the chemicals are used in this experiment?
4) What are the apparatus are used in this experiment?
5)What is the mwt of Fe?
EXPERIMENT-IX
TO PREPARE PHENOL FORMALDEHYDE
AIM: - To prepare phenol formaldehyde resin. (Bakelite)
CHEMICALS USED: - Glacial acetic acid, 40% formaldehyde solution, Phenol, conc. H2SO4
.
APPARATUS REQUIRED: -Glass rod, beakers, funnel, measuring cylinder, dropper and filter
paper.
PRINCIPLE: - Phenol formaldehyde resins (PFs) are condensation polymers and are obtained b
condensing phenol with formaldehyde in the presence of an acidic or alkaline catalyst. They
were first prepared by Backeland, an American Chemist who gave them the name as Bakelite.
These are thermosetting polymers.
Uses:-
They are used for making moulded articles such as radio and TV parts, combs, fountain pen
barrels, phonograph records etc.
Preparation:- PFs are prepared by reaction of phenol with formaldehyde in the presence of
acidic or
basic catalyst. The process may be carried out as follows
A mixture of phenol and formaldehyde are allowed to react in the presence of a catalyst. The
process
involves formation of methylene bridges in ortho, para or both ortho and para positions. This
results
first in the formation of linear polymer (Called NOVALAC) and then in to cross-linked polymer
called phenol-formaldehyde resin or Bakelite
PROCEDURE: -
1. Place 5ml of glacial acetic acid and 2.5ml of 40% formaldehyde solution in a 500ml beaker
and add 2 grams of phenol.
2. Add few ml of conc. Sulphuric acid into the mixture carefully. With in 5 min. a large mass
of plastic is formed.
3. The residue obtained is washed several times with distilled water, and filtered product is
dried and yield is calculated.
RESULT: - The weight of the phenol formaldehyde resin is ___ g.
VIVA QUESTIONS:
1. Phenol formaldehyde is also called as.
2. What do you understand by resin?
3. Give main uses of the phenol formaldehyde resin.
4. What type of co-polymer is phenol formaldehyde resin?
5. Briefly describe the properties of phenolic resins
.
6. Write chemical equations for preparation of phenolic resins.
EXPERIMENT -X
To prepare urea formaldehyde resin. Apparatus required:-
Beaker, glass rod, funnel, filter paper and chemical balance.
Chemicals:-
Urea, formaldehyde sol., conc. H2SO4, distilled water.
Theory:-
Amino resins are condensation products obtained by the reaction of formaldehyde with nitrogen bearing
compounds such as aniline, amides for ex:- melamine formaldehyde, urea formaldehyde etc.
Urea formaldehyde is prepared by condensation reaction between urea and formaldehyde in
acidic or alkaline medium. The first product formed during the formation of resin is
monomethylol aand dimethylol ureas.
Urea Formaldehyde Monomethylol Dimethylol Urea. Polymerization can take place from mono
or dimethylol urea or possibly through both, with the formation of long chains.
Procedure:-
1.Place about 5 ml of 40% formaldehyde solution in 100 ml beaker.
2.Add about 2.5 g of urea with constant stirring till saturated solution is obtained.
3.Add a few drops of conc. H2SO4, with constant stirring.
4.A voluminous white solid mass appears in the beaker.
5.Wash the white solid with water and dry it in the folds of filter paper.
6.Weight the yield of product
Precautions:-
1.While adding concentrated H2SO4, it is better to stay little away from the beaker since the
reaction sometimes becomes vigorous.
2.The reaction mixture should be stirred continuously.
Observations:-
Mass of the beaker (W1) = ---------g.
Mass of the beaker with urea formaldehyde (W2) = --------g.
Therefore mass of
urea formaldehyde (W2 – W1) = --------g.
Result:-
The yield of urea formaldehyde = -------g
Properties:
1.They have good electricalinsulating properties .
2.They are resistant to oil, grease and weak acids.
3.They are hard, resist abrasion and scratching.
Uses:-
1.They are used adhesive applications for the production of plywood and laminating .
2.They are used for the manufacture of cation exchange resins.
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)What is polymer?
4)What is condensation?
5)What is polymerization?
Experiment-XI
ESTIMATION OF COPPER-
(IODOMETRY)
Aim: To estimate the amount of Copper present in the given solution using a standard solution
of Potassium Dichromate and Hypo as the link solution.
Apparatus: 100 ml standard flask,
Funnel, Burette,
Iodometric flask,
Conical Flask,
Pipette,
Simple balance with weights
Chemicals Required: K2Cr2O7, Hypo (Na2S2O3), KI, Conc.HCl, dil. Acetic acid, NaHCO3,
H2SO4, CuSO4, Ammonia solution, Starch & distilled water.
Principle: Any cupric salt in neutral medium when treated with Potassium Iodide forms a
white precipitate of cuprous iodide and iodine is set free quantitatively. The liberated
Iodine is treated against Hypo using starch as the indicator.
Chemical reactions:
CuSO4 + 2KI -------- CuI2 + K2 SO4
2CuI2 ----------- Cu2I2 + I2
I2 + 2Na2S2O3 +O2 -------- Na2S2O6 + 2NaI
2CuSO4 = I2 = Na2S2O3
Procedure:
1. Preparation of standard potassium dichromate: i. Weigh out accurately the given pure crystalline sample of potassium
dichromate and transfer into 100 ml standard (volumetric) flask provided
with a funnel.
ii. Dissolve the dichromate in a small quantity of distilled water, and make up to
the mark.
iii. The contents in the flask are shaken well for uniform concentration.
iv. Calculate the normality of potassium dichromate.
2. Preparation of hypo:
3. Prepation of KI:
4. Preparation of 2 N acetic acid:
5. Standardization of sodium thiosulphate: i. Rinse the burette and fill it up with hypo solution without any air bubbles.
ii. Note the burette reading. Take about 20 ml of 10%KI solution in a clean conical
flask and add 2 grams of sodium bicarbonate followed by 5 ml of concentrate
HCl gently rotate the flask for mixing the liquids.
iii. Rinse the pipette with a little of potassium dichromate solution and then transfer
20 ml of the same to the conical flask.
iv. Shake it well, stopper it, and keep it in dark place for 5 minutes. Titrate the
liberate iodine by running down hypo from the burette with constant stirring.
v. When the solution attains a pale yellow colour add 2 ml of freshly prepared
starch solution.
vi. The colour changes to blue.
vii. Continue the titration drop-wise till the colour changes from blue to light green
indicating the end point.
viii) Repeat the titration for concurrent values.
6. Startch indicator:
7. Estimation of copper: i. Make up the given solution of copper to 100 ml with distilled water and shake
well for uniform concentration.
ii. Pipette out 20 ml of this solution into a clean conical flask.
iii. Add few drops of ammonia when bluish white precipitate is obtained.
iv. Redissolve the precipitate in dilute acetic acid. Now add 10 ml of 5% KI,
when iodine is liberated giving a brown colour.
v. Titrate this solution against standard hypo solution till light yellow colour is
obtained.
vi. Now add 2 ml of starch solution and continue the titration till blue colour
changes to creamy white, which is the end point.
vii. Repeat the titration for concurrent values and calculate the amount of copper.
___________________________________________________________________________
Preparation of Standard solution: W1 = Weight of bottle + substance = ____________ gms
W2 = Weight of bottle = ____________ gms
Weight of substance = (W1-W2 ) = ____________ gms.
Normality of the solution = (W1-W2) X 10/Equivalent Weight =
= (W1-W2) X 10/49=
Volume consumed
Burette Reading Volume of
the
standard
K2Cr2O7
solution
(V1)
S.NO
Intial
final
20 ml 1
20 ml 2
20 ml 3
N1 = Normality of K2Cr2O7 solution =
V1 = Volume of K2Cr2O7 solution = 20ml
N2 = Normality of Hypo =?
V2 = Volume of Hypo =
N1 V1= N2 V2
N2 = N1 V1 / V2
N2 = Normality of Hypo =
Volume of consume (V4)
Burette Reading Volume of the Copper
solution (V3)
S.No
final Initial
20ml 1
20ml 2
20ml 3
V4=
N3 = Normality of the Copper solution =?
V3 = Volume of the Copper solution = 20ml
N4 = Normality of Hypo =?
V4 = Volume of Hypo =
N3 V3= N4 V4
Normality of the Copper solution = N3 = N4 V4 / V3
Amount of Copper present in the whole of the given solution (100 ml) = N3 X 63.54/10
Result: Amount of Copper present in the whole of the given solution (100 ml) = ______ gm.
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)Cu atomic number?
4)What is molarity?
5)What is Normality?
EXPERIMENT-XII
ESTIMATION OF OF FERROUS ION BY POTENTIOMETRY
AIM:
To estimate the amount of ferrous iron present in the given sample by potentiometry
CHEMICALS:Potassium dichromate,ferrous sulphate,calomel electrode,platinum electrode
PROCEDURE:
Prepare 0.1 N Potassiumdichromate solution solution by dissolving 4.9 gms of potassium
dichromate in 1000ml of distilled water.Take 25 ml of the ferrous solution in to the beaker ,add
25 ml 5 N H2SO4 and 50 ml of water.Fill the burette with potassium dichromate after rinsing the
burette with potassium dichromate.
Dip the satured calomel electrodeand bright platinum electrode.set the stirrer in motion and
measure the intial e.m.f.After each addition of potassium dichromate in 5 ml measure the emf of
the cell. Determination the end point.
TABLE:
S.NO volume of
Potassiumdichromate
EMF
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
V1=volume of potassium dichromate from the curve =x ml
N1=Normality of potassium dichromate=
V2=volume of ferrous sulphate=25 ml
N2=Normality of ferrous sulphate
V1N1=V2N2
N2=Normality of FeSo4=
RESULT:Amount of FeS04=N2X55.85= ------------- gm/l
VIVA QUESTIONS: 1) What are the chemicals are used in this experiment?
2) What are the apparatus are used in this experiment?
3) Fe atomic number?
4) Mwt of Feso4
EXPERIMENT-XIII
DETERMINATION OF FERROUS ION IN CEMENT BY COLOROMETRIC METHO
Aim:To estimate the amount of ferrous iron present in the given sample of cement by
colorometry using ammonium thio cynate as the reagent
Chemicals:cement,HCl,HNO3
Apparatus:Beakers,std flask,Watch glass, Colorometer
Procedure:Weigh out accurately about 0.1 g of the given cement sample into a clean 250 ml
beaker . Add about 5 ml water to moisten the sample .place a glass rod and a add concentrated
HCl through the walls of the glass. Stir the solution and cover with a watch glass. Remove the
watch glass and keep the beaker on a small flame and evaporate the solution to dry ness expel
the excess acid .take the beaker out of the flameml of distilled water to dissolve the contents
.Transfer the solution in to a 100 ml std flask .Wash the beaker twice with small portions of
distilled water .Shake the flask well for uniform concentration.
Development of colour:
Pipette out 10 ml of the solution prepared above ,in to 100 ml std flask,add 1 ml of concentrated
HNO3 from the a burettealso add 5 ml of 40% ammonium thiocynate from a burette. Make up
the solution up to the mark and shake well for uniform concentration. Measure the optical
density of the sample be X .Find out the concentration of iron calibration curve
Calculations:W1=Weight of the weighing bottle cement
W2=Weight of the weighing bottle
W1-W2=Weight of the cement sample
STANDARD VALUES FOR CALIBRATION CURVE : TABLE
S.No CONCENTRATION OF Fe+2
in mg
OD
1
2
3
4
5
6
7
8
9
RESULT:
Percentage of ferrous iron=yx10x100/W1-W2 In----------------------- mgs.
Y----Corres ponds to amount of ferrous iron from the calibration curve
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)Cement compostions
4)Mw t of HCl
EXPERIMENT-XIV
ESTIMATION OF FERROUS ION BY PERMANGANOMETRY
AIM:
To Prepare the standard solution of oxalic acid and estimation of iron by potassium
permanganate as an intermediate.
CHEMICALS: oxalic acid, potassium permanganate, concentrated sulphuric acid
PROCEDURE:
PREPARATION OF STANDARD OXALIC ACID SOLUTION:
Weigh out accurately 0.315 gms of oxalic acid crystals in to a 100 ml standard flask dissolve the
sample in little distilled water and make up the solution to the mark distilled water and shake the
flask well for uniform concentration.
PREPARATION OF POTASSIUM PERMANGANATE SOLUTION :
Dissolve 1.58 gms potassium permanganate in 1000 ml of distilled water and shake the flask
well for uniform concentration.
PREPARATION OF 2 N SULPHURIC ACID SOLUTION:
56 ml concentrated sulphuric acid is added drop by drop slowly to 1000 ml of water taken in a
beaker ,kept in a trough of water .Not directly added to water.
STANDARD ISATION OF POTASSIUM PERMANGANATE SOLUTION:
Pippette out 20 ml of the oxalic acid solution in to a 250 ml conical flask and add 20 ml of 2 N
sulphuric acid.Heat the solution till fumes come out of the solution and titrate the hot solution
with KMnO4 taken in a burette. Pale pink colour is the end point.Repeat the titration to get
concurrent values.Let the titre value be X ml
STANDARD ISATION OF Fe+2
SOLUTION
The Fe+2
Solution is given in a 100 ml standard flask .Make up the given Fe+2
solution up to
the mark with distilled water and shake the flask well for uniform concentration. Pippette out
20 ml of Fe+2
Solution in to a250 ml conical flask add 20 ml of 2 N sulphuric acid.Titrate the
resulting solution with KMnO4 taken in a burette. Pale pink colour is the end point.Repeat the
titration to get concurrent values. Let the titre value be Y ml.
Calculations:
Normality of oxalic acid N1= Wt of oxalic acid
63
N2=Normality of KMnO4 =>V1N1= V2N2
V1=Volume of oxalic acid
N1= Normality oxalic acid
V2= Volume of KMnO4=Y
N2=20X N1/titer value
V2N2= V3N3
N2= Normality of KMnO4
V2= Volume of KMnO4
V3= Volume of Fe+2
Solution
N3= V2N2 = Y X N2
V3 20
RESULT:
Amoun t of Fe+2
iron present in the given solution=N3XEquivalent weight of Fe+2
/10
=N3X55.85=---------------gms /100ml
10
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3) Mwt of KMno4
4)What is acid?
EXPERIMENT-XV
ESTIMATION OF FERROUS AND FERRIC IONS IN A GIVEN MIXTURE BY
DICHROMETRY
AIM:
To estimate the amount of ferrous and ferric ions in a given mixture by making use potassium
dichromate
CHEMICALS: potassium dichromate,Stannous chloride,Mercurous chloride,phenyl amine
PREPARATION OF SOLUTIONS:
STANDARD POTASSIUM DICHROMATE:
Weigh out accurately weighted 0.245 gm potassium dichromate in to a 100 ml standard
flask,dissolve in little amount of water and make up the solution with distilled water.Shake the
flask well for uniform concentration.
STANNOUS CHLORIDE SOLUTION:
Dissolve 150 gms of sncl2.2H2o in 100 ml concentrated HCl and dilute with water to 1 litre
MECURIC CHLORIDE SOLUTION:
Dissolve 60 gms of HgCl2 in hot water and dilute to 1 litre
ACID MIXTURE:
Dissolve 150 ml of concentrated H2SO4 and 50 ml of H3PO4 in a reagent bottle and stopper it.
PHENYL AMINE:
Dissolve 1 gm of di Phenyl amine in 100ml of concentrated H2SO4
PROCEDURE:
STANDARDISATION OF TOTAL IRON:
Make up the given mixture of Fe+2
and Fe+3
given in 100 ml standard flask up to the mark with
distilled water and shake the flask well for uniform concentration. Pippette out 20 ml of the iron
solution in to a conical flask ,Add 100 ml concentrated HCl and heat the solution to boling till
the colour of the solution changes yellow. Add stannous chloride drop by drop to the hot solution
till the yellow colour disappears. Cool the solution under tap and add 100 ml mercuric chloride
in one portion silky white ppt of mercurous is obtained. Add 5 ml of acid mixture and 3-4 drops
of diphenylamine indicator .Titrate the solution against standard potassium dichromate taken in a
burette till the green colour changes to blue violet. Repeat the titration to get concurrent values.
Let the titre value be x ml
STANDARDISATION OF FERROUS IRON:
Pippette out 20 ml of the total iron solution in to a250 ml conical flask,add 5 ml of acid mixture
and 2 drops of ofdi Phenyl amine indicator.Titre the resulting solution with potassium
dichromate taken in a burette till blue colour is obtained. Note the burette readings and repeat the
titration for concurrent values .Let the titre value be y ml
CALCULATIONS:
Normality of potassium dichromate N1=Weight of potassium dichromatex10/49
Normality of total iron =V1N1=V2N2
V1=Volume of dichromate
V2= Volume of dichromate consumed for total iron
N2= Normality of total iron
N1= Normality of dichromate
N2=V1N1/ V2= titre value be x ml XN1/20
Amount of total iron= N2X55.85= p gms /100 ml
10
Normality of ferrous iron Fe+2
= V1N1=V3N3
V1=Volume of dichromate
N1= Normality of dichromate
V3=Volume of Fe+2 solution
N3= Normality of Fe+2 solution
N3= V1N1= titre value be y ml XN1/20
V 3
Amount of Ferrous iron = N3X55.85= q gms /100ml
10
RESULT:
Amount of Ferrous iron =Amount of total iron-amount of Fe+2
= p-q gms
100
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)What is molarity?
4) What is Normality?
5)What is strong acid&base?
EXPERIMENT-XVI
DETERMINATION OF SALT CONCENTRATION BY –ION EXCHANGE RESIN
Aim:-
To determine the sodium sulphate salt concentrations by ion exchange resin
Chemicals:sodium nitrate,Resin beads,sodium hydroxide,silver nitrate,potassium chromate.
Procedure :
Weighout exactly 0.5gms air dried resin and transfer into a column with the help of small camel-
hair brush, through a funnel into the column add sufficient distilled water to cover the resin.
Adjust the level of outer tube, so that liquid un the column will drain 1 cm above resin beads.
Take 250ml separatory funnel with 100 ml of given NaN03 salt solution and run this solution at a
rete of 2 ml per minute. Collect the effluent in a 250 ml conical flask. When all the solution as
passed through the column titrate the effluent with standard 0.1 N sodium hydroxide using
phenlolphthalein as indicator. Pink color is the end point of the solution. Let the titre value be X
ml.
R-H +NaNO3-----------R-Na +HNO3
HNO3+NaOH---------------NaNO3+H2O
Take 1 gm anion –exchange in a coloumn and take 100 ml of the given sodium nitrate solution
into a separatory funnel and add slowly sodium nitrate solution at the rate of 2 ml per
minute.collect the effluent and titrate with 0.1 N silver nitrate solution using potassium chromate
as indicator. Let the titre value by Y ml
Calculations:
Normality of Na+ (N2)=V1N1=V2N2
V1=Volume of std.of NaOH(XML)
N1=Normality of std.NaOH
V2=Volume of Na+ effIuent
N2=V1N1 = X xN1
V2 100
N2=Normality of Na+ Effluent
Amount of Na+=N2x23=-------- gms/100ml
Normality of NO3-(N3)=V1N1=V3N3
V1=volume of std .AgNO3= yml
N1=Normality of std.AgNO3
V2=Volume of NO3-(Effluent)
N2=Normality of NO3 (effluent)
N3=V1N1 = YxN1
V2 100
RESULT:
Amount of No3- In the 100 ml of solution=N3x62= ----------------- gms
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)What is ion-exchange process?
4)What is indicator?
5)Write the strong acids&bases?
EXPERIMENT-XVII
ESTIMATION OF MANGANESE IN KMnO4 BY COLORIMETRIC METHOD
AIM:
To estimate the amount of manganese present in the given sample by colorimetry
CHEMICALS:
PROCEDURE:
The given potassium permanganate solution is diluted to 100 ml standard flask and shake the
flask well for uniform concentration. Measure the optical density of the test sample,let it be x.In
the same way prepare a set of 9 standards with KMnO4 and measure the optical density of these
samples and plot a graph with optical density on y axis and amount of KMnO4 on x axis
calculate the amount of KMnO4 from the curve in the following way.
CALCULATIONS:
Standard values for calibration curve
AMOUNT OF KMnO4 IN (MgS) OD
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
Optical density of of the test solution =X
Corresponding value of amount from curve=Y
RESULT:
Amount of KMnO4 present in the sample ----------------- Y mgs
Amount of Manganese in the given solution= 84x54.93
158
=-----------------mgs.
VIVA QUESTIONS:
1)What are the chemicals are used in this experiment?
2)What are the apparatus are used in this experiment?
3)Mn atomic number?
4) potassium permanganate formula?
5)What is OD?
