Multiple Choice Questions (MCQs) for JEE Chemistry: Solutions
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Multiple Choice Questions
(a) Na2SO4
(b) Al2(SO4)3
(c) Al(NO3)3
(d) NaCl
Show Answer & Explanation
Answer: (a) Na2SO4
Explanation:
1. \( Hg_2Cl_2 \to Hg_2^{2+}+2Cl^- \) gives 3 ions, so i = 3.
2. \( Na_2SO_4\to2Na^++SO_4^{2-} \) also gives 3 ions.
Teacher's Note:
1. Count the ions for each salt: NaCl 2, Na2SO4 3, Al(NO3)3 4, Al2(SO4)3 5.
(a) 0.186 °C
(b) 1.86 °C
(c) 3.72 °C
(d) 0.372 °C
Show Answer & Explanation
Answer: (d) 0.372 °C
Explanation:
1. Molality \( = \dfrac{0.02}{0.1\ \text{kg}} = 0.2 \).
2. \( \Delta T_f = 1.86\times0.2 = 0.372 \) °C.
Teacher's Note:
1. Molality uses the mass of the solvent in kilograms.
(a) -0.372 °C
(b) -0.186 °C
(c) -0.72 °C
(d) -0.54 °C
Show Answer & Explanation
Answer: (b) -0.186 °C
Explanation:
1. Moles of glucose \( = 18/180 = 0.1 \), so \( m = 0.1 \).
2. \( \Delta T_f = 1.86\times0.1 = 0.186 \), so the freezing point is \( -0.186 \) °C.
Teacher's Note:
1. The freezing point is 0 °C minus the depression.
(a) 96.01 g mol⁻¹
(b) 179.79 g mol⁻¹
(c) 207.8 g mol⁻¹
(d) 209.6 g mol⁻¹
Show Answer & Explanation
Answer: (a) 96.01 g mol⁻¹
Explanation:
1. \( \Delta T_f = 273.15-271.94 = 1.21 \) K.
2. \( M = \dfrac{K_f\times w\times1000}{\Delta T_f\times W} = \dfrac{1.86\times1.25\times1000}{1.21\times20} \approx 96 \) g/mol.
Teacher's Note:
1. Use the freezing point of pure water as 273.15 K to find the depression.
(a) sugar beet will lose water from its cells
(b) sugar beet will neither absorb nor lose water
(c) sugar beet will absorb water from the solution
(d) sugar beet will dissolve in the solution
Show Answer & Explanation
Answer: (a) sugar beet will lose water from its cells
Explanation:
1. The NaCl solution is hypertonic compared with the cell sap.
2. Water leaves the cells by osmosis through the cell membrane, so the slice shrinks.
Teacher's Note:
1. Water moves from lower solute concentration to higher solute concentration through a semipermeable membrane.
(a) solute molecules occurs from lower concentration to higher concentration
(b) solute molecules occurs from higher concentration to lower concentration
(c) solvent molecules occurs from lower concentration to higher concentration of the solution
(d) solvent molecules occurs from higher concentration to lower concentration of the solution
Show Answer & Explanation
Answer: (c) solvent molecules occurs from lower concentration to higher concentration of the solution
Explanation:
1. Osmosis is the net flow of solvent through a semipermeable membrane.
2. The solvent moves from the dilute solution (or pure solvent) towards the more concentrated solution.
Teacher's Note:
1. The solute cannot pass through the semipermeable membrane. Only the solvent flows.
(a) inversely proportional to the concentration
(b) directly proportional to the square root of the concentration
(c) directly proportional to the square of the concentration
(d) directly proportional to the concentration
Show Answer & Explanation
Answer: (d) directly proportional to the concentration
Explanation:
1. \( \pi = CRT \), so at constant T, \( \pi\propto C \).
Teacher's Note:
1. This is van't Hoff's law, which is analogous to Boyle's and Charles's laws for gases.
(a) Barium oxalate
(b) Nickel phosphate
(c) Copper ferrocyanide
(d) Calcium sulphate
Show Answer & Explanation
Answer: (c) Copper ferrocyanide
Explanation:
1. Copper ferrocyanide, Cu2[Fe(CN)6], is a gelatinous precipitate that allows water but not solutes to pass.
Teacher's Note:
1. Copper ferrocyanide is the membrane used in the Morse and Frazer experiments on osmotic pressure.
Assertion (A): The molality of the solution does not change with change in temperature.
Reason (R): The molality is expressed in units of moles per 1000 mL of solution.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Molality is moles of solute per 1000 g of solvent. It involves only masses, so it does not change with temperature: A is true.
2. The reason is false, as molality is per 1000 g of solvent, not per 1000 mL of solution.
Teacher's Note:
1. Molarity (per litre of solution) changes with temperature. Molality does not.
Assertion (A): The sum of the mole fractions of all the components is unity.
Reason (R): Mole fraction is a temperature dependent mode of concentration.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Mole fractions \( x_i = n_i/\sum n \), so their sum is always 1: A is true.
2. Mole fraction involves only the number of moles, so it is independent of temperature: R is false.
Teacher's Note:
1. Concentration terms that use only masses or moles do not depend on temperature.
Assertion (A): A solution which contains one gram equivalent of solute per litre of the solution is called a normal solution.
Reason (R): A normal solution means a solution in which the solute does not associate or dissociate.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. By definition, a normal solution has 1 gram equivalent per litre: A is true.
2. The reason is wrong. Normality has no relation to association or dissociation of the solute.
Teacher's Note:
1. Normality is equivalents per litre. It is not about whether the solute splits up.
Assertion (A): The molarity and normality of a solution of sodium carbonate are the same.
Reason (R): Normality is the product of molarity and valency factor.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (d) A is false, but R is true.
Explanation:
1. Na2CO3 has a valency factor of 2, so its normality is twice its molarity. The assertion is false.
2. The reason is true: N = M × n-factor.
Teacher's Note:
1. The normality equals the molarity only when the valency factor is 1.
Assertion (A): Ideal solutions are those which obey Raoult's law at all temperatures and concentrations.
Reason (R): A very dilute solution can be treated as an ideal solution.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. By definition an ideal solution obeys Raoult's law over the whole range: A is true.
2. A very dilute solution of non-ideal liquids approaches Raoult's law, so R is true. However, this is not the reason for the definition of ideal solutions.
Teacher's Note:
1. Dilute solutions approximate ideal behaviour, but the definition of an ideal solution does not depend on that fact.
Assertion (A): Cooking time is reduced in pressure cookers.
Reason (R): The boiling point inside the pressure cooker is raised.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. Under increased pressure, water boils at a higher temperature, so food is cooked at a higher temperature.
2. That is why the cooking time is reduced. R correctly explains A.
Teacher's Note:
1. Boiling point rises with external pressure, and higher temperature speeds up cooking.
Assertion (A): In a positive deviation of non-ideal solutions, the attraction between solute and solvent is less than the attraction between solute-solute and solvent-solvent.
Reason (R): In a negative deviation of non-ideal solutions, the attraction between solute and solvent is more than the attraction between solute-solute and solvent-solvent.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. Positive deviation arises when A-B attractions are weaker than A-A and B-B: A is true.
2. Negative deviation arises when A-B attractions are stronger: R is true.
3. R describes the opposite case, so it does not explain A.
Teacher's Note:
1. Both statements are correct but describe different cases.
Assertion (A): Isotonic solutions do not show the net phenomenon of osmosis.
Reason (R): Isotonic solutions have equal osmotic pressure at constant temperature.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. Isotonic solutions have equal osmotic pressures, so there is no net flow of solvent between them.
2. R is true and explains A.
Teacher's Note:
1. Net osmosis occurs only when the two sides have different osmotic pressures.
Assertion (A): When benzoic acid is dissolved in benzene, its van't Hoff factor is less than one.
Reason (R): In benzene, benzoic acid has a tendency to form dimers.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. Dimerisation reduces the number of particles, so i is about 0.5, which is less than 1: A is true.
2. R is true and is the cause of A.
Teacher's Note:
1. Association in a non-polar solvent gives i less than 1.
Assertion (A): Non-ideal solutions form azeotropic mixtures.
Reason (R): The boiling point of an azeotropic mixture is only higher than the boiling points of both the components.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Solutions with large positive or negative deviations form azeotropes: A is true.
2. An azeotrope may have a boiling point lower (positive deviation) or higher (negative deviation) than the components. The word 'only' makes R false.
Teacher's Note:
1. Minimum-boiling and maximum-boiling azeotropes both exist.
Assertion (A): The van't Hoff factor is always more than or equal to one.
Reason (R): The van't Hoff factor is the ratio of the observed colligative property to the calculated colligative property.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (d) A is false, but R is true.
Explanation:
1. For association i is less than 1, so A is false.
2. R is true: \( i = \dfrac{\text{observed colligative property}}{\text{calculated colligative property}} \).
Teacher's Note:
1. In case of association, the number of particles decreases, so i is below 1.
Assertion (A): An azeotropic mixture cannot be separated by fractional distillation.
Reason (R): Azeotropic mixtures are constant boiling mixtures.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. An azeotrope boils at a constant temperature and the vapour has the same composition as the liquid.
2. So it cannot be separated by fractional distillation: R explains A.
Teacher's Note:
1. Fractional distillation needs a difference between vapour and liquid compositions.
Assertion (A): ΔH(mix) and ΔV(mix) for the preparation of an ideal solution are zero.
Reason (R): The A-B interaction in an ideal solution is the same as between A-A and B-B in the two liquids before mixing.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. If the A-B interactions are equal to the A-A and B-B interactions, no heat is absorbed or released and the volume is additive.
2. So A is true and R explains it.
Teacher's Note:
1. Equal intermolecular forces are the key property of an ideal solution.
Assertion (A): A 0.1 M solution of NaCl has a lower freezing point than a 0.1 M urea solution.
Reason (R): The van't Hoff factor (number of particles) for NaCl is more than for urea.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. NaCl gives 2 ions and urea gives 1 particle, so the NaCl solution has twice as many particles.
2. A larger depression means a lower freezing point: A is true, and R explains it.
Teacher's Note:
1. The depression in freezing point depends on the number of particles.
Assertion (A): At high altitude, cooking food is difficult.
Reason (R): Water boils at a high temperature at high altitude.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. The atmospheric pressure is lower at high altitude, so water boils at a lower temperature and food takes longer to cook: A is true.
2. R is false, since water boils at a lower temperature.
Teacher's Note:
1. The boiling point of water falls as the external pressure falls.
Assertion (A): After adding a non-volatile solute, the freezing point of the solvent is depressed.
Reason (R): The vapour pressure of the solvent decreases and becomes equal to that of the solid solvent at a temperature lower than the freezing point of the pure solvent.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. Freezing occurs when the vapour pressure of the liquid equals that of the solid.
2. Since the solution has a lower vapour pressure, this match happens at a lower temperature. R explains A.
Teacher's Note:
1. Lower vapour pressure of the solution shifts the intersection with the solid's curve to a lower temperature.
Assertion (A): On increasing pressure, the solubility of gases in a liquid solvent increases.
Reason (R): The dissolution of gases in a liquid is exothermic.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. By Henry's law, solubility is proportional to the pressure: A is true.
2. Dissolution of gases in liquids is exothermic, so R is true.
3. But the exothermic nature explains the effect of temperature, not of pressure, so R does not explain A.
Teacher's Note:
1. Exothermic dissolution means solubility decreases on heating, which is a separate fact from the effect of pressure.
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FAQs
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