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 products of three sparingly soluble salts $AB$,$A_2B$ and $AB_3$ are respectively $4.0 \times 10^{-20}$,$3.2 \times 10^{-11}$ and $2.7 \times 10^{-31}$. The increasing order of their solubility is

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ba(AcO)_2 + K_2CrO_4 \longrightarrow BaCrO_4 \downarrow + 2AcOK$

The solubility product of silver chloride at $298 \ K$ is $1.8 \times 10^{-10}$. The solubility of $AgCl$ in $0.2 \ M \ NaCl$ solution will be ............

$A$ $1.0 \ L$ of aqueous solution contains $1 \times 10^{-8} \ M \ NaBr$,$1 \times 10^{-8} \ M \ NaCl$ and $1 \times 10^{-8} \ M \ NaI$. To this solution,$1 \times 10^{-10} \ M$ aqueous $AgNO_3$ solution is added dropwise. The order of precipitation of $AgX$ $(X = Cl, Br, I)$ is:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$

When equal volumes of $Ca^{2+}$ and $F^{-}$ solutions are mixed,in which of the solutions precipitation will not occur? $(K_{sp} \text{ of } CaF_2 = 1.6 \times 10^{-10})$