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:

How many grams of $CaC_2O_4$ (molecular mass $= 128$) on dissolving in one litre distilled water will give a saturated solution (in $g$)? $[K_{sp}(CaC_2O_4) = 2.5 \times 10^{-9} \ mol^2 \ L^{-2}]$

If the solubility product of $Ni(OH)_2$ is $4.0 \times 10^{-15}$,the solubility (in $mol \ L^{-1}$) is

If the concentration of $CrO_4^{2-}$ ions in a saturated solution of silver chromate is $2 \times 10^{-4} \ M$,the solubility product of silver chromate 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:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$

The $K_{sp}$ expression for $Ca_3(PO_4)_2$ is: