The acid dissociation constants of H2S and HS− are 10−7 and 10−13 respectively. The pH of 0.1M H2S aqueous solution will be ______

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The acid dissociation constants of $H_{2} S$ and $H S^{-}$ are $10^{- 7}$ and $10^{- 13}$ respectively. The $p H$ of 0.1M $H_{2} S$ aqueous solution will be _______

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answer is 4.

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Detailed Solution

As $K_{a_{2}} < < K_{a_{1}}$ , $H^{+}$ are mainly obtained from the first dissociation , second dissociation constant is extremely low when compare to first, therefore we can neglect ${K_{a_{2}}}_{}$ for calculation
$H_{2} S ⇌ H^{+} + H S^{-}$ for which
$[H^{+}] = \sqrt{K C} = \sqrt{10^{- 7} \times 10^{- 1}} = 10^{- 4} p H = 4$