When equal volumes of following solution are mixed, precipitation of AgCl ?

$\left({\mathrm{K}}_{\mathrm{sp}} = 1.8 \times {10}^{-10}\right)$ will occur only with

 Ionic product is greater than solubility product constant precipitation occurs

${\mathrm{K}}_{\mathrm{sp}} = 1.8 \times {10}^{-10}$

$$\begin{gathered} \left[{\mathrm{Ag}}^{+}\right] \left[{\mathrm{Cl}}^{-}\right] = {10}^{-4} \times {10}^{-4}={10}^{-8} \\ \therefore {\mathrm{K}}_{\mathrm{sp}} \mathrm{of} \mathrm{AgCl} < \left[{\mathrm{Ag}}^{+}\right] \left[{\mathrm{Cl}}^{-}\right] \end{gathered}$$