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What is the concentration of ${CN}^{-}$ ions in a solution with 0.1 M HCl and 0.01 M HCN where $K_{a}$ of HCN is $10^{- 6} ?$

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10^{- 4} M

10^{- 5} M

10^{- 6} M

10^{- 7} M

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detailed solution

Correct option is D

HCl is a strong acid and completely dissociates in water. Therefore, the concentration of HCl, H⁺ and Cl^- is the same, 0.1 M.

HCN is a weak acid and partially dissociates.

$HCN ⇌ H^{+} + {CN}^{-}$

K_a expression of HCN:

$K_{a} = \frac{[H^{+}] [{CN}^{-}]}{[HCN]} 10^{- 6} = \frac{[0.1] [{CN}^{-}]}{[0.01]} [{CN}^{-}] = 10^{- 7}$

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What is the concentration of CN- ions in a solution with 0.1 M HCl and 0.01 M HCN where Ka of HCN is 10-6?

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What is the concentration of ${CN}^{-}$ ions in a solution with 0.1 M HCl and 0.01 M HCN where $K_{a}$ of HCN is $10^{- 6} ?$