Common Ion Effect

What are the concentrations of the ionic species in a saturated solution of Ag$_2$CrO$_4$

K$_{sp}$ = 1.1 x 10$^{-12}$

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$^{-8}$

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$^{-12}$

A solution contains 1.0 x 10$^{-4}$ M Cu$^+$ and 2.0 x 10$^{-3}$ M Pb$^{2+}$. When I$^{-}$ is added, which will precipitate first? How much I$^-$ is needed to cause a precipitate to form?When CuI is added to PbI$_2$

CuI K$_{sp}$ = 5.3 x 10$^{-12}$

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