The precipitate of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ is obtained when equal volumes of the following are mixed:

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

The solubility product of $BaSO_4$ is $1.3 \times 10^{-9}$. The solubility of this salt in pure water will be

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?

The solubility product constant $K_{sp}$ of $Mg(OH)_2$ is $9.0 \times 10^{-12}.$ If a solution is $0.010 \ M$ with respect to $Mg^{2+}$ ion,what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg(OH)_2$?

Solubility product $(K_{sp})$ of the salts $MX$,$MX_2$,and $M_3X$ at temperature $T$ are $4 \times 10^{-8}$,$3.2 \times 10^{-14}$,and $2.7 \times 10^{-15}$ respectively. The solubilities of these salts at temperature $T$ are in the order: