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.

Explain why the pH of the ammonia solution is less than $13$.

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 ${\mathrm{NH}}_3 \left(\mathrm{aq}\right)$.

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.