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.

Estimate the pH at the equivalence point for the titration of hydrochloric acid with ammonia and explain your reasoning.

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.

State the equation for the reaction of ammonia with water and write the ${\mathrm{K}}_{\mathrm{b}}$ expression for ${\mathrm{NH}}_3 \left(\mathrm{aq}\right)$.

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:

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

Explain why the following reaction can also be described as an acid–base reaction.

${\mathrm{F}}^{-}\left(\mathrm{g}\right)+{\mathrm{BF}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{BF}}_4^{-}\left(\mathrm{s}\right)$