A saturated solution of a sparingly soluble salt  ${\text{MCI}}_2$ has a vapour pressure of 31.78mm of Hg at ${\text{30}}^{\text{0}}\text{C.}$ While pure water exert a pressure of 31.82mm og Hg at the same temperature. Calculate the solubility product of the compound at this temp. is approximately  ${\text{x\hspace{0.17em}×\hspace{0.17em}10}}^{\text{-5}}{\text{mol}}^{\text{3}}{\text{L}}^{\text{-3}}$.  Find the value of x. (Rounding to nearest integer value)