Which of the following equations represents the solubility product $(K_{sp})$ of $As_2S_3$?

The solubility of silver chromate is $1.992 \times 10^{-2} \ g/L$. The molar mass of $Ag_2CrO_4$ is $332 \ g/mol$. What is the molar concentration of $Ag^{+}$ in a saturated solution of $Ag_2CrO_4$?

If the $[F^{-}] = 2.0 \times 10^{-5} \ M$ in water,how many grams of $CaCl_{2}$ must be added to initiate the precipitation of $CaF_{2}$? Given: $K_{sp}$ for $CaF_{2} = 1.7 \times 10^{-10}$ and the molar mass of $CaCl_{2} = 111 \ g \ mol^{-1}$. Assume the volume of the solution is $1 \ L$.

Solubility product expression of salt $MX_4$ which is sparingly soluble with a solubility $(S)$ can be given as

The volume of water required to dissolve $0.1 \ g$ $PbCl_2$ to get a saturated solution (in $mL$) is (Given $K_{sp}(PbCl_2) = 3.2 \times 10^{-8}$; Atomic mass of $Pb = 207 \ u$, $Cl = 35.5 \ u$)

The $pH$ of a saturated solution of $Ba(OH)_2$ is $12$. What is the value of the solubility product $(K_{sp})$ of $Ba(OH)_2$?