Using the symbol $\text{HZ}$ to stand for a Brønsted-Lowry acid, write equations to show $\text{NH}_3 +$ and $\text{CH}_3\text{OH} +$ acting as Brønsted-Lowry bases.
Using the symbol $\text{B}^-$ to stand for a Brønsted-Lowry base, write equations to show $\text{NH}_3 +$ and $\text{CH}_3\text{OH} +$ acting as Brønsted-Lowry acids.
State briefly what is meant by a reaction that is reversible.
State briefly what is meant by dynamic equilibrium in a reaction mixture.
Explain what the term buffer solution means.
Explain how the action of a buffer solution depends on a reversible reaction involving a Brønsted-Lowry acid such as $\text{HZ}$ and a Brønsted-Lowry base such as $\text{Z}^-$.
Propanoic acid, $\text{CH}_3\text{CH}_2\text{CO}_2\text{H}$, is a weak acid with $K_a = 1.34 \times 10^{-5}\,\text{mol dm}^{-3}$. Calculate the $\text{pH}$ of a $0.500\,\text{mol dm}^{-3}$ solution of propanoic acid.
Write an equation for the reaction of sodium hydroxide with propanoic acid.
Calculate the concentrations of propanoic acid and sodium propanoate in buffer solution $F$.
Calculate the $\text{pH}$ of buffer solution $F$.
Phenyl propanoate cannot be prepared directly from propanoic acid and phenol. In the reaction scheme shown, identify the intermediate $G$, the reagent $H$ and the by-product $J$.