The dissociation constants for acetic acid and HCN at 25°C are 1.5 × 10⁻⁵ and 4.5 × 10⁻¹⁰ respectively. The equilibrium constant for the equilibrium CN⁻ + CH₃COOH ⇌ HCN + CH₃COO⁻ would be:

Question

Accepted Answer

3.0 × 10⁴. The equilibrium constant for the given reaction is the ratio of the dissociation constant of acetic acid (Ka of CH₃COOH) to that of HCN (Ka of HCN). Thus, K = (1.5 × 10⁻⁵) / (4.5 × 10⁻¹⁰) = 3.0 × 10⁴.

The dissociation constants for acetic acid and HCN at 25°C are 1.5 × 10⁻⁵ and 4.5 × 10⁻¹⁰ respectively. The equilibrium constant for the equilibrium CN⁻ + CH₃COOH ⇌ HCN + CH₃COO⁻ would be:

Solution

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