The solubility product of sparingly soluble salt $AX_{2}$ is $3.2 \times 10^{-11}$. Its solubility (in $mol / L$) is

$K_{sp}$ for $Cr(OH)_3$ is $1.6 \times 10^{-30}$. What is the molar solubility of this salt in water?

At $310 \, K$,the solubility of $CaF_{2}$ in water is $2.34 \times 10^{-3} \, g / 100 \, mL$. The solubility product of $CaF_{2}$ is $x \times 10^{-8} \, (mol / L)^{3}$. Find the value of $x$. (Given molar mass: $CaF_{2} = 78 \, g \, mol^{-1}$)

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?

Which of the following has maximum solubility at low $pH$?

The solubility product of lead bromide is $8 \times 10^{-5}$. If the salt is $80\%$ dissociated in a saturated solution,find the solubility of the salt.