Chapter 16, Problem 43PE

Interpretation Introduction

Interpretation:

Moles of $\text{AgBr}$ dissolved in $\text{0}\text{.10 }M\text{ NaBr}$ has to be calculated.

Concept Introduction:

Concentration of solution is expressed in terms of molarity. It is the ratio of moles of solute to the volume of solution in litres. The expression used to determine the concentration of solution is as follows:

  $\text{Concentration of solution}=\frac{\text{moles of solute}}{\text{volume of solution}\left(\text{L}\right)}$

Equilibrium constant used for the partially soluble salt in water is termed as solubility product constant $K_{\text{sp}}$. Consider solubility of $\text{AB}$ in water and equilibrium equation of $\text{AB}$ is as follows:

  $\text{AB}\left(s\right)\rightleftharpoons {\text{A}}^{+}\left(aq\right)+{\text{B}}^{-}\left(aq\right)$

The expression for $K_{\text{sp}}$ is as follows:

  $K_{\text{sp}}=\frac{\left[{\text{A}}^{+}\right]\left[{\text{B}}^{-}\right]}{\left[\text{AB}\left(s\right)\right]}$

Generally the concentration of solid is taken as constant. Therefore the expression for $K_{\text{sp}}$ of $\text{AB}$ is as follows:

  $K_{\text{sp}}=\left[{\text{A}}^{+}\right]\left[{\text{B}}^{-}\right]$