The solubility product for a salt of the type $AB$ is $4 \times 10^{-8}$. What is the molarity of its saturated solution?

What is the solubility product $(K_{sp})$ of a binary sparingly soluble salt $BA$ if a $100 \text{ mL}$ saturated solution of the salt contains $10^{-4} \text{ moles}$ at room temperature?

Which of the following pairs of ions when mixed in dilute solutions may give a precipitate?

Find the solubility in terms of $mol \ L^{-1}$ if the solubility product of silver bromide is $6.4 \times 10^{-13}$.

The solubility of $CdSO_{4}$ in water is $8.0 \times 10^{-4} \ mol \ L^{-1}$. Its solubility in $0.01 \ M \ H_{2}SO_{4}$ solution is $..... \ \times 10^{-6} \ mol \ L^{-1}$.
(Round off to the Nearest integer) (Assume that solubility is much less than $0.01 \ M$)

If the $[F^{-}] = 2.0 \times 10^{-5} \ M$ in water,how many grams of $CaCl_{2}$ must be added to initiate the precipitation of $CaF_{2}$? Given: $K_{sp}$ for $CaF_{2} = 1.7 \times 10^{-10}$ and the molar mass of $CaCl_{2} = 111 \ g \ mol^{-1}$. Assume the volume of the solution is $1 \ L$.