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 that solution.
The dissolution of silver chloride
$AgCl(s)$ 
$Ag^+(aq)$ $+$ $Cl^-(aq)$
produces per liter .......... mol $Ag^+$ and .......... mol $Cl^-$
The sodium chloride contributes per liter with .......... mol $Cl^-$ so that finally we have in the saturated solution :
$[Ag^+]$ = ..........$\frac{mol}{L}$
$[Cl^-]$ = ..........$\frac{mol}{L}$
The solubility product at $25^oC$ of $AgCl$, expressed in terms of $x$, is therefore equal to $K_s$ $=$ $[Ag^+][Cl^-]$ = .......... $\frac{mol^2}{L^2} $
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