Chemistry · Unit 3 · Chemical equilibrium systems · Chemical equilibrium

Apply Le Châtelier’s principle to explain how buffer solutions respond to the addition of hydrogen ions and hydroxide ions. Chem istry 2025 v1.3 Dissociation constants

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Question 1

A buffer solution contains ethanoic acid \(\text{CH}_3\text{COOH}(aq)\) and sodium ethanoate \(\text{CH}_3\text{COONa}(aq)\). Which statement correctly describes how this buffer resists a change in pH when a small amount of hydrochloric acid is added?

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Apply Le Châtelier’s principle to determine the effect changes of temperature, concentration of chemicals, pressure and the addition of a catalyst have on the position of equili brium and on the value of the equilibrium constant. Equilibrium constants

Calculate dissociation constants (Ka, Kb, and Kw), pKa, pKb, and the concentrations of reactants and products. (Formula: 𝐾a = [H3O+][A−] [HA]; 𝐾b = [BH+][OH−] [B]; 𝐾𝑤 = 𝐾a × 𝐾b)

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