What is solubility product? Calculate the solubility of $A_{2} X_{3}$ in pure water, assuming that neither kind of ion reacts with water. The solubility product of $A_{2} X_{3}$ ksp $= 1.1 \times 10^{- 23}$ .

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Solution

The solubility product, $K s p$ , applies in situations where salts do not fully dissolve in a solvent. The solvent is generally water. A substance's solubility product is the mathematical product of its dissolved ion concentrations raised to the power of their stoichiometric coefficients.
Applying law of solubility products
$K_{S P} = {[A^{3 +}]}^{2} {[X^{2 -}]}^{3} ⇢ (1)$
$1.1 \times 1 0^{- 23} = (2 S)^{2} (3 S)^{3}$
$1.1 \times 1 0^{- 23} = (108 S)^{5}$
$(S)^{5} = 1 \times 1 0^{- 25}$
$(S) = (1 \times 1 0^{- 25})^{\frac{1}{5}}$
$S = 1 \times 1 0^{- 5} m o l^{- 1}$

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