Entropy is a measure of the disorder of a system.
The enthalpy change of solution, ΔH°sol, of the Group 2 sulfates becomes more endothermic down the group.
An aqueous solution of sodium hydroxide has a pH of 13.25 at 298 K.
The Ka for ethanoic acid is 1.75 × 10⁻⁵ mol dm⁻³ at 298 K.
Titration curves for two different acid-base reactions, M and N, are shown.
[Figure showing two titration curves: reaction M (strong acid-strong base) and reaction N (weak acid-strong base)]

Q: What topic does this question test?

This question tests Equilibria in A-Level Chemistry (syllabus code 9701). It is worth 19 marks.

Q: Which exam paper is this question from?

This question appeared in the Cambridge A-Level Chemistry Oct/Nov 2018 examination, Paper 4 Variant 1 (9701_w18_qp_41.pdf).

Question

Entropy is a measure of the disorder of a system.
The enthalpy change of solution, ΔH°sol, of the Group 2 sulfates becomes more endothermic down the group.
An aqueous solution of sodium hydroxide has a pH of 13.25 at 298 K.
The Ka for ethanoic acid is 1.75 × 10⁻⁵ mol dm⁻³ at 298 K.
Titration curves for two different acid-base reactions, M and N, are shown.
[Figure showing two titration curves: reaction M (strong acid-strong base) and reaction N (weak acid-strong base)]

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