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(D) The given equilibrium is: $H_2S \rightleftharpoons H^{+} + HS^{-}$.When dilute $HCl$ is added,it provides $H^{+}$ ions to the solution $(HCl \righ

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The concentration of $HS^{-}$ will decrease

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(D) The given equilibrium is: $H_2S \rightleftharpoons H^{+} + HS^{-}$.When dilute $HCl$ is added,it provides $H^{+}$ ions to the solution $(HCl \rightarrow H^{+} + Cl^{-})$.According to Le Chatelier's principle,the increase in the concentration of $H^{+}$ ions shifts the equilibrium to the left side to counteract the change.As a result,the concentration of $HS^{-}$ decreases and the concentration of undissociated $H_2S$ increases.Therefore,the correct option is $D$.

The following equilibrium exists in an aqueous solution of hydrogen sulphide: $H_2S \rightleftharpoons H^{+} + HS^{-}$. If dilute $HCl$ is added to an aqueous solution of $H_2S$ without any change in temperature,what happens?

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