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NEET UG Unit 3B1: Solutions and Concentrations — practice questions

Explore 28 free Unit 3B1: Solutions and Concentrations questions in NEET UG 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 1–28 of 28.

'Like dissolves like' implies that:Read the answer and worked solution →If dissolution of a solid in a liquid is endothermic (Δ_sol H > 0), the solubility will:Read the answer and worked solution →Solubility of gases in liquids generally:Read the answer and worked solution →To increase the solubility of CO₂ in soft drinks, manufacturers:Read the answer and worked solution →Raoult's law for a solution of two volatile liquids states that the partial pressure of component 1 is:Read the answer and worked solution →For a binary solution of volatile liquids, the total vapour pressure can be written as:Read the answer and worked solution →Raoult's law in its general form, for the solvent in a solution of a non-volatile solute, gives the relative lowering of vapour pressure as:Read the answer and worked solution →For an ideal solution, both the enthalpy of mixing and the volume of mixing are:Read the answer and worked solution →Which of the following is an example of a near-ideal solution?Read the answer and worked solution →Solutions showing large **positive deviation** from Raoult's law form which type of azeotrope?Read the answer and worked solution →Ethanol–water mixture, on fractional distillation, gives an azeotrope at approximately:Read the answer and worked solution →HNO₃–water mixture forms a *maximum* boiling azeotrope at composition:Read the answer and worked solution →Which of the following is NOT a colligative property?Read the answer and worked solution →The four colligative properties all originate from:Read the answer and worked solution →Elevation of boiling point (ΔT_b) is related to molality (m) by:Read the answer and worked solution →For water, K_b = 0.52 K kg mol⁻¹. What is the boiling point of a solution of 18 g glucose (M = 180) in 1 kg water?Read the answer and worked solution →Depression of freezing point (ΔT_f) is given by:Read the answer and worked solution →45 g of ethylene glycol (M = 62) is dissolved in 600 g of water. K_f(water) = 1.86 K kg mol⁻¹. The depression in freezing point is approximately:Read the answer and worked solution →The osmotic pressure (Π) of a dilute solution is given by:Read the answer and worked solution →Two solutions are termed *isotonic* if they:Read the answer and worked solution →Blood cells placed in a hypertonic solution (e.g., > 0.9% NaCl) will:Read the answer and worked solution →Why do wilted flowers revive when placed in fresh water?Read the answer and worked solution →The van't Hoff factor (i) for a solute that completely dissociates into n particles is:Read the answer and worked solution →For benzoic acid dimerising in benzene (2 CH₃COOH ⇌ (CH₃COOH)₂), the van't Hoff factor approaches:Read the answer and worked solution →Inclusion of the van't Hoff factor modifies the boiling point elevation formula to:Read the answer and worked solution →Experimentally, a solute is found to have a molar mass *lower* than its formula mass. This indicates the solute is:Read the answer and worked solution →In an antifreeze formulation, 35% (v/v) ethylene glycol in water lowers the freezing point of water to about:Read the answer and worked solution →A student states: 'More the pressure of a gas over a liquid, more gas is dissolved.' This statement is an application ofRead the answer and worked solution →

Worked practice questions

'Like dissolves like' implies that:

  1. Solubility depends only on temperature
  2. Polar solutes dissolve in polar solvents and non-polar in non-polar
  3. Polar solutes dissolve in non-polar solvents
  4. All solutes dissolve in water
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Correct answer: B. Polar solutes dissolve in polar solvents and non-polar in non-polar

Solutes dissolve well in solvents with **similar intermolecular interactions**: polar–polar (NaCl in water) and non-polar–non-polar (naphthalene in benzene).

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If dissolution of a solid in a liquid is endothermic (Δ_sol H > 0), the solubility will:

  1. Remain unchanged with temperature
  2. First increase, then decrease
  3. Increase with rise in temperature
  4. Decrease with rise in temperature
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Correct answer: C. Increase with rise in temperature

By Le Chatelier: heating an endothermic equilibrium shifts it forward → **solubility increases** with T. (Exothermic dissolution → solubility decreases with T.)

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Solubility of gases in liquids generally:

  1. Increases with both temperature and pressure
  2. Decreases with temperature, increases with pressure
  3. Increases with temperature, decreases with pressure
  4. Is independent of temperature and pressure
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Correct answer: B. Decreases with temperature, increases with pressure

Gas dissolution is exothermic → solubility **falls with T** (why aquatic life prefers cold water). Higher pressure → more gas particles striking surface → **solubility rises with P** (Henry's law).

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