Let $x$ $\frac{mol}{L}$ be the solubility of silver chloride ( = molarity in a saturated solution of the pure salt)
The dissolution of the pure salt is immediately followed by a dissociation to ions:
$AgCl(s)$ 
$Ag^+(aq)$ + $Cl^-(aq)$
The solubility product at $25^oC$ of $AgCl$, expessed in terms of $x$, is therefore equal to $K_s=[Ag^+][Cl^-]$ = .......... $\frac{mol^2}{L^2} $
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