In which of the following solutions will the solubility of $Ag_2CO_3$ $(K_{sp} = 8 \times 10^{-12})$ be maximum at $30 \, ^\circ C$?

If the solubility product $(K_{sp})$ of $Ni(OH)_2$ is $1.9 \times 10^{-15}$, the molar solubility of $Ni(OH)_2$ in $1.0 \ M \ NaOH$ is:

In an aqueous solution,$SCN^-$,$Br^-$,$I^-$,and $Cl^-$ are present. Which will get precipitated first when $AgNO_3$ is added to the solution? Given that:
$K_{sp}(AgCl) = 1.2 \times 10^{-10}$,
$K_{sp}(AgI) = 1.7 \times 10^{-16}$,
$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,
$K_{sp}(AgBr) = 3.5 \times 10^{-13}$

At $298 \, K$,the solubility product $(K_{sp})$ of $M_2SO_4$ (where $M^+$ is a monovalent metal ion) is $1.2 \times 10^{-5}$. What is the maximum concentration of $M^+$ ions in a saturated solution of this salt at $298 \, K$?

Which of the following is the correct relationship between solubility $(S)$ and solubility product $(K_{sp})$ for silver oxalate?

The $K_{sp}$ of $PbI_2$ is $1.4 \times 10^{-8}$. The molar mass of $PbI_2$ is $461 \ g \ mol^{-1}$. The molar mass of $Pb(NO_3)_2$ is $331.9 \ g \ mol^{-1}$. Find the solubility of $PbI_2$ in: $(a)$ $500 \ mL$ of water,$(b)$ $500 \ mL$ of $0.10 \ M \ KI$ solution,$(c)$ What is the weight of $PbI_2$ soluble in $500 \ mL$ of solution containing $1.33 \ g$ of $Pb(NO_3)_2$?