Ammonia, ${\mathrm{NH}}_3$ , is a weak base. It has a ${\mathrm{pK}}_{\mathrm{b}}$ value of $4.75$.

Calculate the pH of a $1.00\times {10}^{-2} \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous solution of ammonia at $298 \mathrm{K}$.

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.

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.

Distinguish between the terms strong and weak acid and state the equations used to show the dissociation of acids ${\mathrm{HNO}}_3$ and $\mathrm{HCN}$ in aqueous solution.

Ammonia can be converted into nitric acid, ${\mathrm{HNO}}_3\left(\mathrm{aq}\right)$, and hydrocyanic acid, $\mathrm{HCN}\left(\mathrm{aq}\right)$. The ${\mathrm{pK}}_{\mathrm{a}}$ of hydrocyanic acid is $9.21$.

Deduce the expression for the ionization constant, ${\mathrm{K}}_{\mathrm{a}}$, of hydrocyanic acid and calculate its value from the ${\mathrm{pK}}_{\mathrm{a}}$ value given.

Ammonia can be converted into nitric acid, ${\mathrm{HNO}}_3\left(\mathrm{aq}\right)$, and hydrocyanic acid, $\mathrm{HCN}\left(\mathrm{aq}\right)$. The ${\mathrm{pK}}_{\mathrm{a}}$ of hydrocyanic acid is $9.21$.

Calculate the $\left[{\mathrm{H}}^{+}\right]$ and the $\mathrm{pH}$ of an aqueous solution of hydrocyanic acid of concentration $0.108 \mathrm{mol} {\mathrm{dm}}^{-3}$. State one assumption made in arriving at your answer.

$0.100 \mathrm{mol}$ of ammonia, ${\mathrm{NH}}_3$, was dissolved in water to make $1.00 {\mathrm{dm}}^3$ of solution. This solution has a hydroxide ion concentration of $1.28\times {10}^{-3} \mathrm{mol} {\mathrm{dm}}^{-3}$. Determine the $\mathrm{pH}$ of the solution.

$0.100 \mathrm{mol}$ of ammonia, ${\mathrm{NH}}_3$, was dissolved in water to make $1.00 {\mathrm{dm}}^3$ of solution. This solution has a hydroxide ion concentration of $1.28\times {10}^{-3} \mathrm{mol} {\mathrm{dm}}^{-3}$. Calculate the base dissociation constant, ${\mathrm{K}}_{\mathrm{b}}$, for ammonia.