Table of contents

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

Given the molar solubility of Ag2SO3 in pure water is 1.55×10⁻⁵ M, what is the solubility product constant (Ksp) for Ag2SO3?

2.40×10⁻¹⁵

1.48×10⁻¹⁴

6.20×10⁻¹⁶

3.72×10⁻¹⁰

Verified step by step guidance

Start by writing the dissociation equation for Ag2SO3 in water: Ag2SO3(s) ⇌ 2Ag⁺(aq) + SO3²⁻(aq).

Identify the stoichiometry of the dissociation: 1 mole of Ag2SO3 produces 2 moles of Ag⁺ and 1 mole of SO3²⁻.

Let the molar solubility of Ag2SO3 be 's'. Therefore, [Ag⁺] = 2s and [SO3²⁻] = s.

Substitute the molar solubility value into the expressions: [Ag⁺] = 2 × 1.55×10⁻⁵ M and [SO3²⁻] = 1.55×10⁻⁵ M.

Calculate the solubility product constant (Ksp) using the expression Ksp = [Ag⁺]²[SO3²⁻]. Substitute the concentrations to find Ksp.

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