A solution is a mixture of two or more substances that is homogeneous. Solid, liquid, and gaseous solutions are the three types of solutions. A solution’s concentration is expressed in terms of mole fraction, molarity, molality, and percentages.
Download Class 12 Chemistry Worksheet on Chapter 2 Solutions Set 3 PDF
CBSE Class 12 Chemistry Chapter 2 Solutions Worksheet – Set 3
Q-1: Which of the following statements is correct for the Van’t Hoff factor?
- In the case of dissociation, it is less than one.
- In the case of association, it is more than one..
- It is never greater than one.
- In the case of association, it is less than one.
Q-2: Which pair will not show positive deviation from Raoult’s law?
a) Methanol and chloroform
b) Methanol and cyclopentane
c) Ethanol and cyclohexane
d) Toluene and benzene
Q-3: 0.5% KCl solution has depression in freezing point of 0.24 K. Calculate the degree of dissociation of KCl.
Given: Kf(water) = 1.86 K kg/mol
Q-4: 0.01 mmoles, 1L H2SO4 solution is given. 50% of this solution is taken out and 500 mL water is added to make 1L solution. Further,0.01 mmoles of H2SO4 is added to this solution. Find out the final moles of H2SO4 in terms of 10-3 mmoles.
Q-5: Which of the following is incorrect for an ideal solution?
a) Raoult’s law is obeyed for the entire concentration range and temperatures.
b) ΔHmix=0
c) ΔVmix=0
d) ΔSmix=0
Q-6: How is the maximum boiling azeotrope formed? Give an example
Q-7: Henry’s law constant for two gases are 22.5 and 50.5 atm, which gas is more
soluble ?
Q-8: In 450 g of water,15 g of an unknown molecular material is dissolved. At -0.34oC, the resulting solution freezes. What is the material’s molar mass?
Q-9: What effect does temperature have on the solubility of gases in liquids as temperature rises?
Q-10: Which statement is correct for the 0.1M solution of NaCl and Na2SO4 ?
a) Same boiling point but different freezing point.
b) Osmotic pressure of NaCl will be more than Na2SO4.
c) Osmotic pressure of Na2SO4 will be more than NaCl.
d) Osmotic pressure of Na2SO4 will be less than NaCl.
Q-11: Choose the correct statement about a liquid’s vapour pressure from the options below:
a) It increases linearly with temperature
b) It decreases with temperature non linearly
c) It increases with temperature non linearly
d) It increases with temperature linearly
Q-12: At 300 K, the vapour pressure of water is 12.3 Kpa. Determine the vapour pressure of a one-molal solution of a nonvolatile solute in it.
Q-13: Define Raoult’s law for a binary solution containing a nonvolatile solute.
Q-14: Determine the boiling point of a solution made by combining 15.00 g of NaCl with 250 g of water. (Kb = 0.512 K kg mol-1 and NaCl molar mass = 58.44 g mol-1)
Q-15: Which of the following is an example of a liquid solution?
a) Chloroform mixed with nitrogen gas
b) Oxygen dissolved in water
c) Amalgam of mercury with sodium
d) All of the above
Q-16: What is the mole fraction unit used for?
Q-17: Select the correct statement(s) from the following.
a) The freezing point of water is an exothermic process.
b) Addition of any substance to water lowers its freezing point
c) At freezing point or below it, the freezing of both solute and solvent occurs
d) In freezing, ΔSsolvent<ΔSsolution
Q-18: At 25oC, an osmotic pressure of 0.335 tonne is obtained by dissolving 8.95 mg of a gene fragment in 35.0 ml of water. Determine the molar mass of the gene fragment assuming it is a non electrolyte.
Q-19: Mass percent, ppm, mole fraction, and molality are temperature independent, whereas molarity is temperature dependent. Why?
Q-20: Manali is where Neha’s grandmother lives. There is a lot of snow in front of the house in the winter. She requested that Neha clear the snow. To clear the snow, Sneha added NaCl.
a) Why does Sneha do so ?
b) What is the value in Sneha’s thinking ?
c) Define molal freezing point depression constant, Kf .
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