The solubility product

Let $x$ $\frac{mol}{L}$ be the number of moles of silver chloride dissolved in $1$ L of a $0.01$ M solution of $NaCl$. $x$ is the "solubility" of silver chloride in this solution. The dissolution of silver chloride $AgCl(s)$ $Ag^+(aq)$ $+$ $Cl^-(aq)$ supplies per L .......... mol Ag⁺ and .......... mol Cl^- Sodium chloride contributes per liter with .......... mol Cl^- in such a way that we finally have in the saturated solution: $[Ag^+]$ = ..........$\frac{mol}{L}$ $[Cl-]$ = ..........$\frac{mol}{L}$ The solubility product at $25^oC$ of AgCl, expressed in function of $x$, is therefore worth $K_s$ $= $ $[Ag^+][Cl^-]$ = .......... $\frac{mol^2}{L^2} $