Chapter 17.4, Problem 1CP

Interpretation Introduction

Interpretation:

The molar solubility of $\text{Al}{\left(\text{OH}\right)}_{\text{3}}$ is to be calculated using $K_{\text{sp}}$ value.

Concept introduction:

The amount of solute dissolved in a given volume of solvent to form a saturated solution at a given temperature is termed as solubility of the solute in the solvent at that temperature. Number of moles of solute dissolved in per litre of solution is called molar solubility.

The solubility product of the sparingly soluble salt is given as the product of the concentration of ions raise to the power equal to the number of times the ion occurs in the equation after the dissociation of electrolyte.

The presence of common ions in the solution decreases the solubility of a given compound.

For a general reaction: $\text{AB}\left(s\right)\rightleftharpoons {\text{A}}^{+}\left(aq\right)+{\text{B}}^{-}\left(aq\right)$

The solubility product can be calculated by the expression as: $K_{\text{sp}}{\text{= [A}}^{\text{+}}{\text{][B}}^{-}\text{]}$

Here, $K_{\text{sp}}$ is the solubility product constant and $sp$ stands for solubility product.