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(C) The solubility of a sparingly soluble salt like $AgCl$ decreases in the presence of a common ion due to the common ion effect.$AgCl(s) \rightlefth

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$0.01 \ M \ CaCl_2$

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(C) The solubility of a sparingly soluble salt like $AgCl$ decreases in the presence of a common ion due to the common ion effect.$AgCl(s) ightleftharpoons Ag^+(aq) + Cl^-(aq)$$K_{sp} = [Ag^+][Cl^-]$Comparing the concentration of common ions:$(A)$ $0.001 \ M \ AgNO_3$ provides $0.001 \ M \ Ag^+$.$(B)$ Pure water has no common ions.$(C)$ $0.01 \ M \ CaCl_2$ provides $2 	imes 0.01 = 0.02 \ M \ Cl^-$.$(D)$ $0.01 \ M \ NaCl$ provides $0.01 \ M \ Cl^-$.Since $0.01 \ M \ CaCl_2$ provides the highest concentration of common ion $(Cl^-)$,the equilibrium shifts furthest to the left,resulting in the minimum solubility of $AgCl$.

Solubility of $AgCl$ will be minimum in

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