The solubility of ${\mathrm{CaF}}_2$ in water at $18°\mathrm{C}$ is $2.04\times {10}^{-4} \mathrm{mol}/\mathrm{L}$. Calculate ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{CaF}}_2$ and its solubility in $0.01 \mathrm{M}$ $\mathrm{NaF}$ solution.

Will a precipitate of silver sulphate be formed if the solutions of $1 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$ and $0.02 \mathrm{M} {\mathrm{AgNO}}_3$ are mixed in equal volumes?

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{Ag}}_2{\mathrm{SO}}_4\right)=2\times {10}^{-5}$.

Will a precipitate of ${\mathrm{CaSO}}_4$ be formed if equal volumes of $0.02 \mathrm{M} {\mathrm{CaCl}}_2$ and $0.0004 \mathrm{M} {\mathrm{Na}}_2{\mathrm{SO}}_4$ are mixed?

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaSO}}_4\right)=2.4\times {10}^{-5}$.

Will a precipitate of ${\mathrm{CaSO}}_4$ be formed if equal volumes of $0.08 \mathrm{M} {\mathrm{CaCl}}_2$ and $0.02 \mathrm{M} {\mathrm{Na}}_2{\mathrm{SO}}_4$ are mixed?

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaSO}}_4\right)=2.4\times {10}^{-5}$.

A solution containing $0.01 \mathrm{mol}/\mathrm{L}$ of ${\mathrm{CaCl}}_2$ and $0.01 \mathrm{mol}/\mathrm{L}$ of ${\mathrm{SrCl}}_2$ is slowly added to a $0.01 \mathrm{N}$ solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$. Which substance begins to precipitate first?

(a) ${\mathrm{SrSO}}_4$ 

(b) ${\mathrm{CaSO}}_4$

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{SrSO}}_4\right) = 3.2\times {10}^{-7}; {\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaSO}}_4\right) = 1.3\times {10}^{-4}$.

If the solubility product of silver oxalate is $1\times {10}^{-11}$, what will be the weight of ${\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4$ (in grams) in $2.5 \mathrm{L}$ of a saturated solution?

Answer correct up to four places of decimal.

Find the solubility of ${\mathrm{CaF}}_2$ in $0.05 \mathrm{M}$ solution of ${\mathrm{CaCl}}_2$ and water. How many times is the solubility in the second case greater than in the first?

${\mathrm{K}}_{\mathrm{sp}}\left({\mathrm{CaF}}_2\right)=4\times {10}^{-11}$