If the solubility product constant $(K_{sp})$ of $Ni(OH)_2$ is $1.9 \times 10^{-15}$,the molar solubility of $Ni(OH)_2$ in $1.0 \ M \ NaOH$ is:

The solubility of $AgBr$ is $7.1 \times 10^{-7} \ mol \ dm^{-3}$. Calculate its solubility product at the same temperature.

Which of the following is most soluble in water?

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 solubility of $AgCl$ is $1.435 \times 10^{-5} \ g \ L^{-1}$ at $30^{\circ} C$. Calculate its solubility product $(K_{sp})$. (Molar mass of $AgCl = 143.5 \ g \ mol^{-1}$)

The solubility product of $BaSO_4$ at $25 \, ^\circ C$ is $1.0 \times 10^{-9}$. What will be the concentration of $H_2SO_4$ required to precipitate $BaSO_4$ from a $0.01 \, M$ solution of $Ba^{2+}$ ions?