what is the concentration of Hg2 in equilibrium with 0.10M Cl- in a solution of KCl containing excess undissolved Hg2Cl2(s)

[Hg₂²⁺] = 1.3 × 10⁻¹⁶ M

Explanation:

Step 1: Given data

[Cl⁻]: 0.10 M

Solubility product constant of Hg₂Cl₂ at 25 °C (Ksp): 1.3 × 10⁻¹⁸

Step 2: Write the reaction for the solution of mercury (I) chloride

Hg₂Cl₂(s) ⇄ Hg₂²⁺(aq) + 2 Cl⁻(aq)

Step 3: Use the solubility product constant to calculate [Hg₂²⁺]

Ksp = 1.3 × 10⁻¹⁸ = [Hg₂²⁺].[Cl⁻]² = [Hg₂²⁺].(0.10)²

[Hg₂²⁺] = 1.3 × 10⁻¹⁶ M

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