Chapter 18.4, Problem 18.10AFP

Interpretation Introduction

Interpretation:

The equilibrium values has to be calculated for the $\left[{\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}\right]\text{, }\left[{\text{HC}}_{\text{2}}{\text{O}}_4^{-}\right]\text{, and }\left[{\text{C}}_{\text{2}}{\text{O}}_4^{2-}\right]$ and $\text{pH}$ of the solution has to be calculated for $\text{0}{\text{.150 M H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}$.

Concept introduction:

An equilibrium constant $\left(K\right)$ is the ratio of concentration of products and reactants raised to appropriate stoichiometric coefficient at equlibrium.

For the general acid HA,

  $\text{HA}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)\rightleftharpoons {\text{H}}_{\text{3}}{\text{O}}^{+}\left(\text{aq}\right)+{\text{A}}^{-}\left(\text{aq}\right)$

The relative strength of an acid and base in water can be also expressed quantitatively with an equilibrium constant as follows:

  $K_a=\frac{\left[{\text{H}}_{\text{3}}{\text{O}}^{+}\right]\left[{\text{A}}^{-}\right]}{\left[\text{HA}\right]}$                                                                                                   $\left(1\right)$

An equilibrium constant $\left(K\right)$ with subscript $a$ indicate that it is an equilibrium constant of an acid in water.