If the solubility product of $BaSO_4$ is $1.5 \times 10^{-9}$ in water,its solubility in moles per litre is

The solubility product of $AgCl$ is $1.8 \times 10^{-10}$. Mixing equal volumes of which of the following solutions will result in the precipitation of $AgCl$?

Find the solubility of $PbI_2$ if its solubility product is $7.0 \times 10^{-9}$.

The solubility product of silver bromide $(AgBr)$ is $5.0 \times 10^{-13}$. What is the minimum amount of potassium bromide $(KBr)$ that must be added to $1 \ L$ of $0.05 \ M$ silver nitrate $(AgNO_3)$ solution to initiate the precipitation of $AgBr$? (Molar mass of $KBr = 120 \ g \ mol^{-1}$)

$Mg(OH)_2$ is precipitated when $NaOH$ is added to a solution of $Mg^{2+}$. If the final concentration of $Mg^{2+}$ is $10^{-10} \ M$,the concentration of $OH^{-} \ (M)$ in the solution is (Given: Solubility product for $Mg(OH)_2 = 5.6 \times 10^{-12}$)

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