Question Bank
Unit I
1. Define – Transport number, following electrolyte, ionic mobility, mass defect, binding
energy, nucleons, nuclear isotopes, isobars, nuclear binding energy per nucleons, packing
fraction, viscosity, surface tension, parachor value, liquid crystal, surface energy, ideal
fluid, fluidity
2. Explain Moving boundary method with suitable diagram.
3. Explain variation of transport number with velocity of the ions.
4. State and explain Hittorf’s rule with the help of velocities of ions of electrolyte.
5. Explain how the concentration of the electrolyte changes in the anode and cathode
compartments during electrolysis.
6. Explain the various factors affecting transport number of the electrolyte.
7. Describe the relationship between ionic conductance and ionic mobility.
8. Explain the classification of nucleus on the basis of stability.
9. How do you establish nuclear stability on the basis of – neutron proton ratio, odd – even
combination of proton and neutron, magic number, binding energy.
10. Define mass defect and binding energy. How do they affect the nuclear stability?
11. Define mass defect. How it is calculated?
12. Define nuclear binding energy per nucleons. How it is calculated?
13. Explain the following – Absorbed dose, External dose, Effective dose, Equivalent dose,
Biological Dose, Q-factor.
14. Explain different types of radiations emitted by radioactive nucleus.
15. What are the different types of units of radioactivity? Give relationship between them.
16. Give the different types of units of radiation doses with units and symbol.
17. Explain the term viscosity. What are the factors on which the viscosity of a liquid
depends?
18. How is the viscosity of the liquid experimentally determined?
19. Explain the term surface tension with the help of suitable examples.
20. How is the surface tension measured with the help of stalagmometer?
21. What is parachor? How is it used for the structural determination?
22. Give different types of applications of dynamic surface tension.
23. What are liquid crystals? Give its classification.
24. Discuss the applications of liquid crystals.
25. What are the thermotroic and lyotropic crystals?
26. Explain the structure of Nematic, Smectic and cholesteric liquid crystals.
Solve the following.
1. Calculate transport number of chloride ion in 1N KCl was determined by moving boundary
method, with BaCl2 as the following electrolyte. A current 0.0142 amperes was passed
through the solution for 1675 seconds. In the same time interval, the boundary swept a
volume of 0.1205 ml. [Given F = 96500 Coulombs].
2. In a solution of 0.1 N sodium sulphate, transport number of sodium ion is 0.383. If a suitable
boundary is made in a uniform glass tube 18 mm in a diameter, and if a current of 0.02
amperes is passed through the solution for 5 minutes. Calculate the distance travelled by
boundary in the same time interval.
3. The ionic conductance of K+ and HO- ions at infinite dilution are 73.5 x 10-4 and 198.6 x 104 Sm2 gm per equivalent respectively. Calculate the transport number of the two ions at same
conditions.
4. Calculate the mass defect of 235U. Given actual mass of U-235 = 235.0439 amu; A = 235; Z
= 92; Mass of proton = 1.00727 amu; Mass of neutron = 1.00866 amu and mass of electron =
0.00055 amu.
5. Calculate binding energy per nucleon for deuterium nucleus if the experimentally measured
mass of deuterium atom is 2.014102 amu. Given - Mass of proton = 1.00727 amu; Mass of
neutron = 1.00866 amu and mass of electron = 0.00055 amu.
6. Calculate the binding energy and binding energy per nucleon for 38Sr87 nucleus if the
experimentally measured mass of 87Sr nucleus is 86.908877 amu. Given - Mass of proton =
1.00727 amu; Mass of neutron = 1.00866 amu and mass of electron = 0.00055 amu.
7. Calculate the binding energy and binding energy per nucleon for 16S29 nucleus if the
experimentally measured mass of 29S nucleus is 28.996610 amu. Given - Mass of proton =
1.00727 amu; Mass of neutron = 1.00866 amu and mass of electron = 0.00055 amu.
8. At 293K water formed 30 drops while flowing through the capillary of a stalagmometer and
an organic liquid forms 49 drops. Calculate the surface tension of organic liquid if the
densities of water and organic liquid are 0.998 and 0.851 kg per lit respectively at 293K and
the surface tension of the water at the same temperature is 0.0728 N per m.
9. Calculate the number of drops formed by organic liquid having density 0.854 kg per lit and
surface tension 0.051 N per m; if water formed 30 drops with stalagmometer. Given densities of water is 0.998 and the surface tension of the water at the same temperature is
0.0728 N per m.
10. Water and the given liquid takes 100 seconds and 35 seconds respectively to flow between
the two marks of an Ostwald’s viscometer. Calculate the viscosity of the liquid, it its density
is 0.85 g per ml. Given - Viscosity of water is 0.0106 poise and density is 0.997 g per ml.
11. At 200C water with viscosity of 0.01 poise and density of 0.997 g per ml takes 1.8 minutes to
flow through a viscometer. Find the time required by an organic liquid to flow through the
same viscometer, given its density to be 0.896 g per ml and its viscosity to be 0.0059 poise.
Unit II
1. Define the following – Homogeneous system, phase, component of system, amplitude,
wavelength, frequency, wave number, radiant power, transmittance, percentage
transmittance, Absorbance, Intensity of light, monochromatic light, Molar extinction
coefficient, photometer.
2. Explain decomposition of solid CaCO3 in close vessel is example of two component system.
3. State and explain Raoult’s law with phase diagram.
4. Explain - Diethy ether + Acetone system shows positive deviation in Raoult’s law with the
help of phase diagram.
5. Explain - Chloroform + Acetone system shows negative deviation in Raoult’s law with the
help of phase diagram.
6. What is critical solution temperature? Explain phase diagram of phenol – water system.
7. What is critical solution temperature? Explain phase diagram of triethylamine – water
system.
8. What is critical solution temperature? Explain phase diagram of nicotine – water system.
9. Define absorbance. State and explain Lambert law.
10. Define absorbance. State and explain Beer’s law.
11. Define absorbance. State and explain Lambert - Beer’s law.
12. What major deviations in Lambert - Beer’s law? Explain chemical deviations with the help of
two examples.
13. What are the major deviations in Lambert - Beer’s law? Give the limitations of Lambert Beer’s law.
14. Explain the important characteristics of spectrophotometric and photometric methods.
15. Explain the standard calibration curve method of photometric titration.
16. Explain the principle, construction and working single beam spectrophotometer.
17. Explain the principle, construction and working double beam spectrophotometer.
18. State Lambert - Beer’s law. Draw different types of photometric titration curves.
19. Explain different types of applications of photometric titrations.
20. What are the different types advantageous and limitations of photometric titration.
Numerical problems:
1. Liquid A (mol. Wt. 46) and liquid B (mol. Wt. 18) form an ideal solution. At 200C the vapor
pressure of liquid A and pure liquid B are 5.865 x 104 N per m2 and 2.333 x 103 N per m2
respectively. Calculate the vapor pressure of the solution A in B containing 20% of A in B.
2. A 40% solution of Liquid A in liquid B behaves ideally. The vapor pressure of the pure
component A is 0.5 bar and that of B is 0.3 bar. Calculate the partial vapor pressure of A and
B in solution.
3. Liquids A and B form an ideal solution obeying Raoult’s law. At 500C, the total vapor
pressure of a solution containing 1 mole of A and 2 mole of B is 3.999 x 104 Nm-2. When 1
more mole of A is added to the solution, the total vapor pressure is increases to 5.332 x 104
Nm-2. Calculate the vapor pressure of the components.
4. At 250C the vapor pressure of pure CCl4 and SiCl4 are 1.532 x 104 Nm-2 and 3.177 x 104 Nm2
respectively. By assuming the mixture behaves ideally, calculate – (a) the total vapor
pressure of mixture containing one part by weight of CCl4 and three part of SiCl4, and (b)
mole fraction of each component in the vapor phase. Given – mol. Wt. of CCl4 = 154 and
mol. wt. of SiCl4.
5. The vapor pressures of pure benzene and toluene at 400C are 2.453 x 104 Nm-2 and 7.364 x
103 Nm-2 respectively. Calculate the partial pressures of benzene and toluene, the total vapor
pressure of the solution and the mole fraction of benzene in vapor above the solution which
has 0.40 mole fraction of benzene. Assume that the solution is ideal.
6. Calculate the energy, wave number and frequency associated with quantum of infra red
radiation of λ = 1240 nm. Given c = 3 x 108 ms-1, h = 6.625 x 10-34 Js.
7. Calculate the energy, wavelength, and frequency with radiation of wave number 1.4 x 10 5 m1
. Given c = 3 x 108 ms-1, h = 6.625 x 10-34 Js.
8. A solution of a substance with molar absorptivity 9500 gives an absorbance of 0.7 using a
cell having path length 1 cm. Calculate the concentration and the percentage transmittance of
the solution. What is absorbance when concentration of the solution becomes half?
9. A solution of concentration of 5 x 10-5 M has absorbance of 0.75 in a cell of 1 cm length.
Calculate the absorptivity and transmittance of this solution. What is concentration to
maintain the absorbance constant when length of solution becomes double?
10. A 2.3 x 10-4 M solution of a substance has a transmittance of 0.508 for λ = 525 nm when
placed in a cuvette of 1 cm path length. Calculate the absorbance if the concentration is
doubled.
Unit III
1. Explain the following performance characteristics of an analytical method – precision,
accuracy, error, sensitivity, selectivity, detection limit, linear dynamic range, robustness,
ruggedness, limit of quantification, absolute error, relative error, systematic error, bias,
Instrumental error, method error, personal error, random error, constant error,
proportional error, mean, mode, median, sample, population of analysis, correlation
coefficient, population mean, sample mean, deviation, population standard deviation,
sample standard deviation, relative deviation, relative standard deviation, sample
variance, range of analysis, precipitation titration, argentometric titration, adsorption
indicator.
2. Explain the importance of signal to noise ration and sensitivity in analytical methods.
3. Explain systematic error and its types.
4. Explain different steps used to minimize the error of analysis.
5. Explain precipitation titration curve of 50.00 ml of 0.05 M NaCl with 0.10 M AgNO3.
Given Ksp of AgCl = 1.2 x 10-10.
6. Draw the titration curve for the titration of – 25 ml of 0.2 M NaCl against 0.1 M AgNO3.
Given Ksp of AgCl = 1.2 x 10-10.
7. Draw the titration curve for the titration of – 25 ml of 0.2 M KI against 0.1 M AgNO3.
Given Ksp of AgI = 1.7 x 10-16.
8. What is precipitation titration? Explain different titration used to determine equivalence
point of silver nitrate titration.
9. What is precipitation titration? Explain Volhard method used for the estimation of
chlorine content.
10. What is precipitation titration? Explain Mohr titration used for the estimation of chlorine
content.
11. What is precipitation titration? Explain Fajans titration used for the estimation of chlorine
content.
12. What is adsorption indicator? Explain the theory of adsorption indicator in detail.
13. Write a note on fluorescein indicator.
14. What are the limitations of adsorption indicator?
Numerical Problems:
1. Calculate the deviation, absolute error and relative error for the measurement, if in the
determination of the chloride content of a water sample 100 ml required 1.8 ml of 0.1 M
silver nitrate and the expected value of the chloride content is 70 ppm.
2. Calculate the deviation, absolute error and relative error for the measurement, if in the
determination of the sulphate content of a water sample 100 ml required 1.8 ml of 0.1 M
barium chloride and the expected value of the chloride content is 65 ppm.
3. Calculate the mean and standard deviation for the following set of results. 10.28, 10.24,
10.25, 10.25, and 10.30.
4. Six samples of chloride were analyzed. The values of chloride content obtained in ppm
are as follows – 2.06, 2.16, 2.12, 1.93, 1.89 and 1.95. Calculate – Mean, mode, median,
deviation, average deviation, relative average deviation, range, standard deviation,
variance, relative standard deviation, coefficient of variation.
5. The results obtained in ten replicate determination of the chromium content (in %) in the
sample of steel are as follows: 4.88, 4.92, 4.86, 4.85, 4.71, 4.86, 4.87, 4.87, 4.84, and
4.99. Calculate all the measures of central tendency and dispersion.
6. Compare precision of the following set of results.
% paracetamol per tablet
24.67, 25.34, 25.11, 24.98, 24.57, 25.17
% paracetamol per tablet
50.35, 50.45, 51.05, 51.12, 50.81, 51.02