The dissociation constants for acetic acid and HCN at 25oC are 1.5 $ \times $ 10$-$5 and 4.5 $ \times $ 10$-$10 respectively. The equilibrium constant for the equilibrium CN$-$ + CH3COOH $\rightleftharpoons$ HCN + CH3COO$-$ would be

Question

The dissociation constants for acetic acid and HCN at 25^oC are 1.5 $ \times $ 10^$-$5 and 4.5 $ \times $ 10^$-$10 respectively. The equilibrium constant for the equilibrium
CN^$-$ + CH₃COOH $\rightleftharpoons$ HCN + CH₃COO^$-$ would be

3.0 $ \times $ 10^$-$5

3.0 $ \times $ 10^$-$4

3.0 $ \times $ 10⁴

3.0 $ \times $ 10⁵

Solution

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