The solubility of sparingly soluble salt $AB_2$ is $1.0 \times 10^{-4} \ mol \ dm^{-3}$. What is its solubility product?

At $20 \, ^\circ C$,the concentration of $Ag^+$ ions in a saturated solution of $Ag_2CrO_4$ is $1.5 \times 10^{-4} \, M$. The solubility product $(K_{sp})$ of $Ag_2CrO_4$ at $20 \, ^\circ C$ is:

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

$MY$ 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?

Assign $A, B, C, D$ from the given type of reaction.
$Ca(OH)_2 + 2HF \longrightarrow CaF_2 \downarrow + 2H_2O$