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(C) The dissolution of $NaCl$ is represented as: $NaCl_{(s)} ⇌ Na^+_{(aq)} + Cl^-_{(aq)}$.When $HCl$ gas is passed through the solution,it dissociates

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Ionic product of $NaCl$ becomes greater than its ${K_{sp}}$

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(C) The dissolution of $NaCl$ is represented as: $NaCl_{(s)} ⇌ Na^+_{(aq)} + Cl^-_{(aq)}$.When $HCl$ gas is passed through the solution,it dissociates as: $HCl_{(g)} ⇌ H^+_{(aq)} + Cl^-_{(aq)}$.This increases the concentration of $Cl^-$ ions in the solution (Common Ion Effect).According to Le Chatelier's principle,the equilibrium shifts to the left,and the ionic product $[Na^+][Cl^-]$ exceeds the solubility product constant ${K_{sp}}$ of $NaCl$,causing precipitation.

At equilibrium,if $HCl$ gas is passed through a saturated solution of $NaCl$,$NaCl$ gets precipitated because:

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