The solubility product

The maximum amount of silver chloride that dissolves in 1 L of water at $25^oC$ is $1.27 \cdot 10^{-5}\;mol$ . The .......... of $AgCl$ (not to be confused with the product of solubility!) is therefore worth $1.27 \cdot 10^{-5}\frac{mol}{L}$ This dissolution is immediately followed by dissociation into ions. $AgCl(s)$ $Ag^+(aq)$ $+$ $Cl^-(aq)$ In $1$ L of a .......... solution of $AgCl$ in equilibrium with solid non dissolved $AgCl$, we find therefore .......... mol $Ag^+$ and .......... mol $Cl^-$. So, the solubility product at $25^oC$ of $AgCl$ is $K_s$ $=$ $[Ag^+][Cl^-]$ = .......... $\frac{mol^2}{L^2}$