Answer:
Solubility of silver chromate = [tex]0.7937\times10^{-4}\;mol/L[/tex]
Explanation:
Given,
[tex]Ag_2CrO_4\leftrightharpoons2Ag^{+}\;+\;CrO4^{2-}[/tex]
Solubility product (Ksp) = 2 x 10-12
at equilibrium, [tex][Ag^{+}][/tex] = 2x, [tex][CrO4^{2-}][/tex] = x
[tex]Ksp=[Ag^{+}]^{2}[CrO_4^{2-}]\\2\times10^{-12}=(2x)^{2}(x)\\2\times10^{-12}=(4x)^{3}\\(x)^{3} = \frac{2\times10^{-12}}{4}\\\\\sqrt[3]{5\times10^{-13}}[/tex]
[tex]x=\sqrt[3]{0.5\times10^{-12}} =0.7937\times10^{-4}\;mol/L[/tex]
