If the solubility product $(K_{sp})$ 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 product of $BaSO_4$ is $1 \times 10^{-10}$ at $298 \ K$. The solubility of $BaSO_4$ in $0.1 \ M \ K_2SO_4 \ (aq)$ solution is $......... \times 10^{-9} \ g \ L^{-1}$ (nearest integer). Given: Molar mass of $BaSO_4$ is $233 \ g \ mol^{-1}$.

The solubility product of a sparingly soluble salt $AX_2$ is $3.2 \times 10^{-8}$. What is its solubility (in $mol \ dm^{-3}$)?

For the precipitation reaction of $Ag^{+}$ ions with $NaCl$,which of the following statements is correct?

The molar solubility of $Zn(OH)_{2}$ in $0.1 \, M \, NaOH$ solution is $x \times 10^{-18} \, M$. The value of $x$ is ...... . (Nearest integer)
(Given : The solubility product of $Zn(OH)_{2}$ is $2 \times 10^{-20}$)

Solubility product of a salt $AB$ is $1 \times 10^{-8}$ in a solution in which the concentration of $A^{+}$ ions is $10^{-3} \ M$. The salt will precipitate when the concentration of $B^{-}$ ions is kept