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(D) The solubility of a salt is governed by its solubility product constant $(K_{sp})$.When $HCl$ is added to a saturated solution of $NaCl$,the conce

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The ionic product of $NaCl$ exceeds its solubility product.

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(D) The solubility of a salt is governed by its solubility product constant $(K_{sp})$.When $HCl$ is added to a saturated solution of $NaCl$,the concentration of $Cl^-$ ions increases significantly due to the common ion effect.According to the solubility equilibrium $NaCl(s) \rightleftharpoons Na^+(aq) + Cl^-(aq)$,the ionic product $Q = [Na^+][Cl^-]$ increases.When the ionic product $Q$ exceeds the solubility product $K_{sp}$,the equilibrium shifts to the left,causing the precipitation of $NaCl$.

When $HCl$ is added to a saturated solution of $NaCl$,pure $NaCl$ precipitates because:

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