General Chemistry 2: Solubility Product

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$^{-8}$

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$^{-12}$

What is the solubility of AgCl in 0.020 M NaCN?

AgCl K$_{sp}$ = 1.8 x 10$^{-10}$

Ag(CN)$_2^-$ K$_{f}$ = 5.6 x 10$^{18}$

0.25 moles of AgNO$_3$ are dissolved in 1 L of 0.60 M NaCN and 1 mole of NaCl is added. Will AgCl precipitate?

AgCl K$_{sp}$ = 1.8 x 10$^{-10}$

Ag(CN)$_2^-$ K$_{f}$ = 5.6 x 10$^{18}$

How many moles of Mg(OH)$_2$ can be dissolved in a 1 L solution that already contains 0.52 moles Mg$^{2+}$.

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