IB Chemistry HL 3.1.12 Hl Salt Hydrolysis Questions

Use real HL exam questions to write salt-ion hydrolysis equations, classify salt solutions and calculate pH at hydrolysis-driven equilibria.

Exam points

Write the ion–water hydrolysis equation for a conjugate acid or base and identify the ion producing H₃O⁺ or OH⁻.
Predict whether a salt solution is acidic, basic or neutral from the strengths of its parent acid and base, including comparisons among salt solutions.
Calculate or deduce the pH of a hydrolysing salt solution or titration-equivalence mixture using the relevant Ka, Kb and concentration data.

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Study 3.1.12 (HL)—Salt hydrolysis conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

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Phenylethene (styrene) is produced from ethylbenzene in a gas-phase equilibrium.

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Benzoic acid is a weak acid. The graph shows how the pH changes during the titration of a $10.0 \mathrm{~cm}^{3}$ aqueous solution of benzoic acid with aqueous sodium hydroxide.

Explain, with reference to acid-base equilibria, why the sodium benzoate solution formed has a pH>7.

«benzoate ion» hydrolysis/reaction with water AND forms $\mathrm{OH}^{-}$ OR
$\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \quad$

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IB Chemistry HL 3.1.12 Hl Salt Hydrolysis Questions question 1