A $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ ammonia solution is placed in a flask and titrated with a $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ hydrochloric acid solution.

When half the ammonia has been neutralized (the half-equivalence point), the pH of the solution is $9.25$. Deduce the relationship between $\left[{\mathrm{NH}}_3\right]$ and $\left[{\mathrm{NH}}_4^{+}\right]$ at the half equivalence point.

A $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ ammonia solution is placed in a flask and titrated with a $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ hydrochloric acid solution.

Determine ${\mathrm{pK}}_{\mathrm{b}}$ and ${\mathrm{K}}_{\mathrm{b}}$ for ammonia based on the pH at the half-equivalence point.

A $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ ammonia solution is placed in a flask and titrated with a $0.10 \mathrm{mol} {\mathrm{dm}}^{-3}$ hydrochloric acid solution.

Describe the significance of the halfequivalence point in terms of its effectiveness as a buffer.

The equilibrium reached when ethanoic acid is added to water can be represented by the following equation:

${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{l}\right)+{\mathrm{H}}_2\mathrm{O}\left(1\right)\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COO}}^{-}\left(\mathrm{aq}\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(\mathrm{aq}\right)$

Define the terms Brønsted–Lowry acid and Lewis base, and identify two examples of each of these species in the equation.

Deduce the two acids and their conjugate bases in the following reaction:

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{NH}}_3\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{OH}}^{-}\left(\mathrm{aq}\right)+{\mathrm{NH}}_4^{+}\left(\mathrm{aq}\right)$