The solubility product of a sparingly soluble salt is defined as the product of the ionic concentrations in a:

Calculate the solubility in $\text{mol dm}^{-3}$ of a sparingly soluble salt $BA$ at $293 \text{ K}$ if its solubility product constant $(K_{sp})$ is $8.56 \times 10^{-5}$ at the same temperature.

The $K_{sp}$ for $AgBr$ at $25 \, ^\circ C$ is $4.9 \times 10^{-13}$. How much $AgBr$ (in grams) will dissolve in $20 \, L$ of its saturated solution? (Molecular weight of $AgBr = 188$)

In qualitative analysis,the metals of group $I$ can be separated from other ions by precipitating them as chloride salts. $A$ solution initially contains $Ag^{+}$ and $Pb^{2+}$ at a concentration of $0.10 \, M$. Aqueous $HCl$ is added to this solution until the $Cl^{-}$ concentration is $0.10 \, M$. What will the concentrations of $Ag^{+}$ and $Pb^{2+}$ be at equilibrium? ($K_{sp}$ for $AgCl = 1.8 \times 10^{-10}$,$K_{sp}$ for $PbCl_2 = 1.7 \times 10^{-5}$)

Solubility product constants $(K_{sp})$ of silver salts are given as $AgCl = 2 \times 10^{-10}$,$AgBr = 5 \times 10^{-13}$,$Ag_2CO_3 = 8 \times 10^{-12}$,and $AgI = 8 \times 10^{-17}$. Which salt shows the highest solubility?

Assign $A, B, C, D$ from the given type of reaction.
$AlCl_3 + 3NaOH \longrightarrow Al(OH)_3 \downarrow + 3NaCl$