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(B) When hydrogen chloride gas $(HCl)$ is passed through a saturated solution of $NaCl$,it dissociates into its ions as: $NaCl \rightleftharpoons Na^{

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decreases

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(B) When hydrogen chloride gas $(HCl)$ is passed through a saturated solution of $NaCl$,it dissociates into its ions as: $NaCl \rightleftharpoons Na^{+} + Cl^{-}$ $HCl \rightleftharpoons H^{+} + Cl^{-}$ Due to the ionization of $HCl$,the concentration of $Cl^{-}$ ions increases significantly in the solution. According to Le Chatelier's principle,the increase in the concentration of the common ion $(Cl^{-})$ shifts the equilibrium of $NaCl$ dissociation to the left. This phenomenon is known as the common ion effect,which leads to a decrease in the solubility of $NaCl$,causing it to precipitate out.

On passing $HCl$ gas in a saturated solution of $NaCl$,the solubility of $NaCl$

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