In a saturated solution of an electrolyte,the product of the concentrations of its ions is constant at a constant temperature. This constant for the electrolyte is known as:

If $K_{sp}$ is the solubility product of $Al(OH)_3$,its solubility is expressed by the formula:

$A$ sparingly soluble salt having general formula $A_{x}B_{y}$ and molar solubility $S$ is in equilibrium with its saturated solution. Derive a relationship between solubility and the solubility product for such salt.

Which of the following formulas can be used to calculate the solubility of $Ag_2CO_3$?

When equal volumes of $Ca^{2+}$ and $F^{-}$ solutions are mixed,in which of the solutions precipitation will not occur? $(K_{sp} \text{ of } CaF_2 = 1.6 \times 10^{-10})$

The values of $K_{sp}$ of $CaCO_{3}$ and $CaC_{2}O_{4}$ are $4.7 \times 10^{-9}$ and $1.3 \times 10^{-9}$ respectively at $25 \, ^oC$. If the mixture of these two is washed with water,what is the concentration of $Ca^{2+}$ ions in water $\dots \times 10^{-5} \, M$?