What is the concentration of $Ba^{2+}$ when $BaF_2$ $(K_{sp} = 1.0 \times 10^{-6})$ begins to precipitate from a solution that is $0.30 \, M \ F^{-}$?

For the precipitation reaction of $Ag^{+}$ ions with $NaCl$,which of the following statements is correct?

An aqueous solution contains $SCN^{-}$,$Br^{-}$,$I^{-}$,and $Cl^{-}$ ions. When $AgNO_3$ is added to the solution,which of these will precipitate first? Given: $K_{sp}(AgCl) = 1.2 \times 10^{-10}$,$K_{sp}(AgI) = 1.7 \times 10^{-16}$,$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,$K_{sp}(AgBr) = 3.5 \times 10^{-13}$.

$MY$ and $NY_3$,two nearly insoluble salts,have the same $K_{sp}$ values of $6.2 \times 10^{-13}$ at room temperature. Which statement would be true in regard to $MY$ and $NY_3$?

Which of the following is the correct relationship between solubility $(S)$ and solubility product $(K_{sp})$ for silver oxalate?

Explain the difference between ionic product and solubility product. Explain the condition for the precipitation of a sparingly soluble salt.