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(D) The solubility of a sparingly soluble salt like $AgCl$ decreases in the presence of a common ion due to the common ion effect,which shifts the equ

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$BaCl_2 \ (0.3 \ M)$

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(D) The solubility of a sparingly soluble salt like $AgCl$ decreases in the presence of a common ion due to the common ion effect,which shifts the equilibrium $AgCl(s) ightleftharpoons Ag^+(aq) + Cl^-(aq)$ to the left.Calculate the concentration of the common ion ($Ag^+$ or $Cl^-$) in each solution:$1$. $AgNO_3 \ (0.1 \ M) 	o [Ag^+] = 0.1 \ M$$2$. $H_2O \ (l) 	o [Ag^+] = 0, [Cl^-] = 0$$3$. $NaCl \ (0.4 \ M) 	o [Cl^-] = 0.4 \ M$$4$. $BaCl_2 \ (0.3 \ M) 	o [Cl^-] = 2 	imes 0.3 = 0.6 \ M$Since the solubility is inversely proportional to the concentration of the common ion,the solubility is minimum where the common ion concentration is maximum.Comparing the concentrations: $0.6 \ M > 0.4 \ M > 0.1 \ M > 0$.Therefore,the solubility of $AgCl$ is minimum in $0.3 \ M \ BaCl_2$.

The solubility of $AgCl$ is minimum in

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