Find out the solubility of $Ni(OH)_2$ in $0.1 \ M \ NaOH$.
Given that the solubility product constant $(K_{sp})$ of $Ni(OH)_2$ is $2 \times 10^{-15}$.

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,the relationship between the solubilities of these can be correctly represented as

The solubility of $AgCl$ at $20 \, ^oC$ is $1.435 \times 10^{-3} \, g/L$. The solubility product $(K_{sp})$ of $AgCl$ 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 $233 \ g \ mol^{-1}$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$BaSO_3 \downarrow + SO_2 + H_2O \longrightarrow Ba(HSO_3)_2$

Solubility (in molarity) of sparingly soluble salts $MX, MX_2$ and $MX_3$ in water are same. The order of $K_{sp}$ of $MX, MX_2$ and $MX_3$ is