At 298 K the solubility of silver chloride in water is 0.00188 g/L. What is its `K_(sp)` ?

Explanation

Given solubility of AgCl in water at 298 K = 0.00188 gL = `1.88 xx 10^(-3)gL^(-1)`
Molar mass = `143.5 g mol^(-1)`
`therefore` Solubility of AgCl (in mol `L^(-1)`) `= (1.88 xx 10^(-3))/(143.5) mol L^(-1) = 1.315 xx 10^(-5)` mol `L^(-1)`
`AgCl (s) overset(aq)hArr Ag^(+)(aq) + Cl^(-)(aq) K_(sp) = [Ag^(+)][Cl^(-)] = 1.315 xx 10^(-5) xx 1.315 xx 10^(-5) = 1.728 xx 10^(-10)`