Solubility Product Questions

The solubility product of a salt having general formula ${\text{MX}}_2$, in water is $4\times 10^{-12}$. The concentration of ${\text{M}}^{2+}$ ions in the aqueous solution of the salt is:

If the solubility product constant $K_{sp}$ of ${\text{AgIO}}_3$ at a given temperature is $1.0\times 10^{-8}$, what is the mass of ${\text{AgIO}}_3$ contained in $100\text{mL}$ of its saturated solution? (Molar mass of ${\text{AgIO}}_3=283\text{g/mol}$)

The molar solubility product of a salt ${\text{A}}_2{\text{B}}_3$ is $K_{sp}$. The solubility '$s$ ' is given in terms of $K_{sp}$ by the relation:

Solid $\text{Ba}({\text{NO}}_3{)}_2$ is gradually dissolved in a $1.0\times 10^{-4}\text{M}$ ${\text{Na}}_2{\text{CO}}_3$ solution. At what concentration of ${\text{Ba}}^{2+}$ will a precipitate begin to form? ($K_{sp}$ for ${\text{BaCO}}_3=5.1\times 10^{-9}$).

Solubility product of silver bromide is $5.0\times 10^{-13}$. The quantity of potassium bromide (molar mass taken as $120{\text{g mol}}^{-1}$) to be added to $1\text{litre}$ of $0.05\text{M}$ solution of silver nitrate to start the precipitation of $\text{AgBr}$ is: