At 298K , the solubility of silver chloride in water is 1.434$\times$10^-3 g L^-1. the value of -log K_sp for silver chloride is ____.

Solubility is given in gL^-1 should be converted to mole L^-1
$$\begin{gathered} \begin{array}{l}\text{ Solubility }=\frac{1.434\times {10}^{-3}}{143.4}\text{ mole }/\mathrm{L}\\ {10}^{-5}\mathrm{mol}/\mathrm{lit}\\ {\mathrm{k}}_{\mathrm{sp}}=\left[{\mathrm{Ag}}^{+}\right]\left[{\mathrm{C\ell }}^{-}\right]\\ ={10}^{-5}\times {10}^{-5} \\ \begin{array}{l}={10}^{-10}{\text{ mole }}^2/{\text{ litre }}^2\\ -\log {\mathrm{K}}_{\mathrm{sp}}=10\\ \end{array}\end{array} \end{gathered}$$