Which of the following has the minimum solubility in water?

The solubility products of three sparingly soluble salts $AB$,$A_2B$ and $AB_3$ are respectively $4.0 \times 10^{-20}$,$3.2 \times 10^{-11}$ and $2.7 \times 10^{-31}$. The increasing order of their solubility is

The values of $\Delta G_f^o$ (in $kJ \ mol^{-1}$) for $Mg(OH)_2$ at $25 \ ^oC$ are given below. Calculate the solubility product constant $(K_{sp})$.
$Mg^{2+}_{(aq)} = -456.0; OH^{-}_{(aq)} = -157.3; Mg(OH)_{2(s)} = -833.9$

What is the molar solubility of $Mn(OH)_2$ $(K_{sp} = 4.5 \times 10^{-14})$ in a buffer solution containing equal moles of $NH_4^+$ and $NH_3$ $(K_b = 1.8 \times 10^{-5})$?

The molar solubility of a sparingly soluble salt $MX_4$ is $s \ mol \ L^{-1}$. If the solubility product is $K_{sp}$,then $s$ in terms of $K_{sp}$ is:

The solubility product constants of $Ag_2CrO_4$ and $AgBr$ are $32x$ and $4y$ respectively at $298 \text{ K}$. The value of $(\frac{\text{molarity of } Ag_2CrO_4}{\text{molarity of } AgBr})$ can be expressed as :