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JEE Advanced Unit 3B1: Solutions and Concentrations — practice questions — page 2

Explore 46 free Unit 3B1: Solutions and Concentrations questions in JEE Advanced Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Unit 3B1: Solutions and Concentrations questions and exercises with answers

Showing questions 31–46 of 46.

For dilute solutions, lowering of vapor pressure of solvent ΔP / P°_A =Read the answer and worked solution →Elevation in boiling point ΔT_b for solution of non-volatile solute:Read the answer and worked solution →Depression in freezing point ΔT_f for non-electrolyte solute:Read the answer and worked solution →Osmotic pressure π for dilute solution:Read the answer and worked solution →For NaCl in water (assumes complete dissociation), van't Hoff factor i =Read the answer and worked solution →For 0.1 M urea in water, freezing point depression (K_f = 1.86):Read the answer and worked solution →Mass percent of solute = (mass of solute / mass of solution) × 100. For 5 g NaCl in 95 g water:Read the answer and worked solution →Two volatile liquids A (P°_A = 100) and B (P°_B = 200) form ideal solution. For x_A = 0.4, total vapor pressure:Read the answer and worked solution →Osmotic pressure of 0.01 M sucrose solution at 27°C (R = 0.0821 L atm/mol K):Read the answer and worked solution →For solution of urea (M_w = 60 g/mol) with 6 g in 100 g water, molality:Read the answer and worked solution →For 0.1 M acetic acid (Ka = 1.8 × 10⁻⁵), van't Hoff factor i is:Read the answer and worked solution →For salt CaCl₂ (assume full dissociation), i =Read the answer and worked solution →For a 1 m glucose aqueous solution (i = 1), boiling point:Read the answer and worked solution →Freezing-point depression and elevation are colligative properties: depend on:Read the answer and worked solution →Adsorption isotherm:Read the answer and worked solution →Hydrogenation of vegetable oils to make margarine uses catalyst:Read the answer and worked solution →

Worked practice questions

For dilute solutions, lowering of vapor pressure of solvent ΔP / P°_A =

  1. Volume change
  2. x_solute (mole fraction of solute) — colligative
  3. Mass of solute
  4. Always 1
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Correct answer: B. x_solute (mole fraction of solute) — colligative

ΔP / P°_A = x_B (solute mole fraction) by Raoult's law. **Colligative:** depends only on number of solute particles, not their nature.

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Elevation in boiling point ΔT_b for solution of non-volatile solute:

  1. Independent of m
  2. K_b × M
  3. K_b × x
  4. K_b × m (K_b = ebullioscopic constant, m = molality)
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Correct answer: D. K_b × m (K_b = ebullioscopic constant, m = molality)

ΔT_b = K_b × m. K_b is solvent-specific molal elevation constant. e.g., for water K_b = 0.52 K kg/mol. Used to determine molar mass from BP measurement.

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Depression in freezing point ΔT_f for non-electrolyte solute:

  1. K_f × M
  2. -K_f
  3. Always positive equal to K_b
  4. K_f × m (K_f = cryoscopic constant)
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Correct answer: D. K_f × m (K_f = cryoscopic constant)

ΔT_f = K_f × m. K_f for water = 1.86 K kg/mol. Why salt is spread on icy roads (depresses freezing point of water below 0°C). Also used to determine molar masses.

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