Ksp Chemistry

Calculate the solubility (in grams per liter) of PbI$_2$ in water from the solubility product constant 1.4 x 10$^{-8}$.

Calculate the equilibrium concentration of Pb$^{2+}$, I$^-$, Na(\^+$, and NO$_3^-$when 100.0 mL of 0.0500 M Pb(NO$_3$)$_2## and 200.0 mL of 0.100 M NaI are mixed.

PbI$_2$ K$_{sp}$ = 1.4 x 10$^{-8}$

What is the molar solubility of Ag$_2$CrO$_4$ in 0.100 M AgNO$_3$? Compare this to the molar solubility of Ag$_2$CrO$_4$ in water, 1.3 x 10$^{-4}$ M

Ag$_2$CrO$_4$ K$_{sp}$ = 9.0 x 10$^{-12}$

The concentration of Mg(NO$_3$)$_2$ is 4 x 10$^{-4}$ M and the concentration of NaOH is 2 x 10$^{-4}$, do you expect Mg(OH)$_2$ to precipitate?

Mg(OH)$_2$ K$_{sp}$ = 8.9 x 10$^{-12}$