The relationship between solubility $(S)$ and solubility product $(K_{sp})$ for a salt of type $A_x B_y$ is given by:

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 $KBr = 120 \ g \ mol^{-1}$)

$PbCl_2$ has a maximum concentration of $1.0 \times 10^{-3} \ M$ in its saturated aqueous solution at $25 \ ^oC$. Its solubility in a $0.1 \ M \ NaCl$ solution will be:

Select the ion exchange reaction,which proceeds in the forward direction in an aqueous medium.

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M \ Na_2CO_3$ solution. At which concentration of $Ba^{2+}$,precipitate of $BaCO_3$ begins to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

What is the solubility product $(K_{sp})$ of calcium phosphate in pure water? $[S = \text{molar solubility}]$