The solubility in water of a sparingly soluble salt $AB_2$ is $1.0 \times 10^{-5} \ mol \ L^{-1}$. Its solubility product constant will be

The solubility product of $PbS$ is $3.4 \times 10^{-28}$. If $[Pb^{2+}] = 1 \times 10^{-2} \ mol/L$,what concentration of $[S^{2-}]$ is required to precipitate $PbS$?

The solubility product of silver bromide $(AgBr)$ is $5.0 \times 10^{-13}$. What is the minimum amount of potassium bromide $(KBr)$ that must be added to $1 \ L$ of $0.05 \ M$ silver nitrate $(AgNO_3)$ solution to initiate the precipitation of $AgBr$? (Molar mass of $KBr = 120 \ g \ mol^{-1}$)

If the concentration of sodium ions in a saturated solution of $Na_2SO_4$ is $10^{-5} \ mol/L$,find the solubility product $(K_{sp})$.

Determine the solubilities of silver chromate,barium chromate,ferric hydroxide,lead chloride,and mercurous iodide at $298 \, K$ from their solubility product constants. Determine also the molarities of individual ions. (Given $K_{sp}$ values: $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$,$BaCrO_{4} = 1.2 \times 10^{-10}$,$Fe(OH)_{3} = 1.0 \times 10^{-38}$,$PbCl_{2} = 1.6 \times 10^{-5}$,$Hg_{2}I_{2} = 4.5 \times 10^{-29}$)

The solubility product of a sparingly soluble salt $BA$ is $6.4 \times 10^{-13}$. Calculate its solubility in $\text{g dm}^{-3}$. The molar mass of the salt is $190 \text{ g mol}^{-1}$.