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

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 1–30 of 46.

Molarity M is defined as:Read the answer and worked solution →Molality m is defined as:Read the answer and worked solution →Mole fraction x_A is:Read the answer and worked solution →Raoult's law for an ideal solution (one component A in solvent S) is:Read the answer and worked solution →Colligative properties depend on:Read the answer and worked solution →What is the molarity of a solution containing 5.85 g of NaCl (M.W. = 58.5) in 250 mL of solution?Read the answer and worked solution →Boiling point elevation: ΔT_b = K_b × m. For 1 molal aqueous urea (K_b = 0.52 K kg/mol), ΔT_b equals:Read the answer and worked solution →Freezing point depression: ΔT_f = K_f × m. For 0.5 molal NaCl (assume full dissociation, K_f = 1.86), the depression is:Read the answer and worked solution →Vapour pressure of pure water at 25°C is 23.8 mm Hg. The vapour pressure of a solution with 18 g glucose (M.W. = 180) in 90 g water:Read the answer and worked solution →Osmotic pressure π = nRT/V (or CRT for molarity C). What is π for 0.1 M sugar solution at 27°C (R = 0.0821)?Read the answer and worked solution →The van't Hoff factor i for a strong electrolyte like CaCl2 (full dissociation) is:Read the answer and worked solution →In ideal solutions, ΔH_mix is:Read the answer and worked solution →Mass percentage (w/w) of a solution: 12 g sugar in 100 g of solution is:Read the answer and worked solution →Two solutions are isotonic if:Read the answer and worked solution →Maximum boiling azeotropes are formed by mixtures with:Read the answer and worked solution →Molality of a solution does not depend on:Read the answer and worked solution →For 0.5 m solutions of NaCl, KCl, and BaCl2, which gives largest ΔT_f?Read the answer and worked solution →Osmotic pressure of 0.1 M Glucose at 27°C is π_g. For 0.1 M NaCl at same T, the osmotic pressure is approximately:Read the answer and worked solution →The pKa of a weak acid HA is 4.75. Find pH of an equimolar mixture of HA and A⁻:Read the answer and worked solution →Solubility of N2 in water at 25°C is 6.8 × 10⁻⁴ mol/L at 1 atm partial pressure. By Henry's law, at 5 atm partial pressure of N2:Read the answer and worked solution →Two solutions A (0.1 M urea, π_A) and B (0.1 M NaCl, π_B). Water flows by osmosis:Read the answer and worked solution →A solution boils at 100.5°C (water at 100). If K_b = 0.52, molality is:Read the answer and worked solution →Mole fraction of solute in 18% glucose (180 g/mol) by mass in water:Read the answer and worked solution →Vapour pressure of pure water is 100 (arbitrary units). Add 1 mole non-volatile solute to 9 moles water. New vapour pressure is:Read the answer and worked solution →A solution is:Read the answer and worked solution →Mole fraction of solute x_B in a binary solution:Read the answer and worked solution →Molarity M is defined as:Read the answer and worked solution →Molality m is defined as:Read the answer and worked solution →Henry's law states partial pressure of a gas above liquid is proportional to:Read the answer and worked solution →Raoult's law for ideal solution states vapor pressure of solvent:Read the answer and worked solution →

Worked practice questions

Molarity M is defined as:

  1. Moles of solute per kg of solvent
  2. Volume of solute per litre
  3. Mass of solute per litre
  4. Moles of solute per litre of SOLUTION
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Correct answer: D. Moles of solute per litre of SOLUTION

Molarity (M) = moles of solute / litres of solution. *Note: this is per litre of SOLUTION, not solvent (different from molality).*

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Molality m is defined as:

  1. Mass of solute per total mass
  2. Mole fraction
  3. Moles solute per litre of solution
  4. Moles solute per kilogram of SOLVENT
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Correct answer: D. Moles solute per kilogram of SOLVENT

Molality (m) = moles of solute / kg of solvent. Used for colligative property calculations because, unlike molarity, it does not depend on temperature.

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Mole fraction x_A is:

  1. n_A / (n_A + n_B)
  2. Concentration
  3. mass_A / total mass
  4. n_A / V
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Correct answer: A. n_A / (n_A + n_B)

Mole fraction x_A = moles of A / total moles in solution. Dimensionless, sums to 1 over all components.

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