The correct representation for the solubility product of $SnS_2$ is:

The solubility of calcium carbonate $(CaCO_3)$ at $298 \ K$ is $6.4 \times 10^{-5} \ mol \ dm^{-3}$. Calculate the value of solubility product $(K_{sp})$ at the same temperature.

At $20 \, ^\circ C$,the $Ag^+$ ion concentration in a saturated solution of $Ag_2CrO_4$ is $1.5 \times 10^{-4} \, mol/L$. At $20 \, ^\circ C$,the solubility product of $Ag_2CrO_4$ would be:

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 $KBr = 120 \ g \ mol^{-1}$)

For a sparingly soluble,strong electrolyte salt,the following equilibrium is established in a saturated solution:
$AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO_{3(aq)}^-$
At a certain temperature,the solubility product of $AgIO_3$ is $K_{sp} = 1.0 \times 10^{-8}$. The molar mass of $AgIO_3$ is $283 \ g \ mol^{-1}$. What is the mass of $AgIO_3$ in $100 \ mL$ of its saturated solution?

The $pH$ at which $Mg(OH)_2$ $[K_{sp} = 1 \times 10^{-11}]$ begins to precipitate from a solution containing $0.10 \ M$ $Mg^{2+}$ ions is . . . . . .