Express the relationship between $K_{sp}$ and solubility $(S)$ for the salt $Ca_3(PO_4)_2$.

The solubility product of a salt $AB$ is $1 \times 10^{-8}$ in a solution in which the concentration of $A$ is $10^{-3} \ M$. The salt will precipitate when the concentration of $B$ becomes more than:

$0.08 \ g$ of $CaF_2$ is dissolved in $2.90 \ L$ of water to form a saturated solution at $298 \ K$. Calculate the solubility product constant $(K_{sp})$ of $CaF_2$. (Molar mass of $CaF_2 = 78.08 \ g/mol$)

Assign $A, B, C, D$ from the given type of reaction.
$FeS \downarrow + 2HCl \longrightarrow FeCl_2 + H_2S \uparrow$

The solubility product of $CaCO_3$ is $5 \times 10^{-9}$. Its solubility is equal to .......

If the $pH$ of a saturated solution of $Ba(OH)_2$ is $12$,what is the value of its solubility product constant $K_{sp}$?