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UPCET / UPSEE Reactions in Aqueous Solution — practice questions — page 2

Explore 121 free Reactions in Aqueous Solution questions in UPCET / UPSEE Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Reactions in Aqueous Solution questions and exercises with answers

Showing questions 31–60 of 121.

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 →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 →

Worked practice questions

Raoult's law for a solution of two volatile liquids states that the partial pressure of component 1 is:

  1. p₁ = p₁⁰ × x₂
  2. p₁ = p₁⁰ × x₁
  3. p₁ = p₁⁰ + x₁
  4. p₁ = p₁⁰ / x₁
Show answer and solution

Correct answer: B. p₁ = p₁⁰ × x₁

**Raoult's law (volatile components):** p_i = p_i⁰ × x_i. The partial pressure is directly proportional to the mole fraction in solution the proportionality constant is the vapour pressure of the *pure* component.

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For a binary solution of volatile liquids, the total vapour pressure can be written as:

  1. p_total = (p₁⁰ + p₂⁰) / 2
  2. p_total = p₁⁰ + (p₂⁰ − p₁⁰) × x₂
  3. p_total = p₁⁰ × p₂⁰
  4. p_total = p₁⁰ + p₂⁰
Show answer and solution

Correct answer: B. p_total = p₁⁰ + (p₂⁰ − p₁⁰) × x₂

p_total = x₁ p₁⁰ + x₂ p₂⁰. Substituting x₁ = (1 − x₂) gives **p_total = p₁⁰ + (p₂⁰ − p₁⁰) x₂** — linear in x₂.

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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:

  1. (p₁⁰ − p₁)/p₁⁰ = x₂
  2. (p₁⁰ − p₁)/p₁⁰ = n₁/n₂
  3. (p₁⁰ − p₁)/p₁⁰ = x₁/x₂
  4. (p₁⁰ − p₁)/p₁⁰ = x₁
Show answer and solution

Correct answer: A. (p₁⁰ − p₁)/p₁⁰ = x₂

**Relative lowering of VP = mole fraction of solute (x₂)**. **From Raoult's law:** p₁ = x₁ p₁⁰; Δp/p⁰ = 1 − x₁ = x₂. This is a colligative property.

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