The graph below shows the titration curve of $25{\mathrm{cm}}^3$ of $0.100 \mathrm{mol} {\mathrm{dm}}^{-3}$ of hydrochloric acid with sodium hydroxide, of $0.100 \mathrm{mol} {\mathrm{dm}}^{-3}$concentration. The indicator methyl orange was used to determine the equivalence point. Methyl orange has a pH range of $3.1–4.4$.

If the hydrochloric acid was replaced by ethanoic acid of the same volume and concentration, which property of the titration would remain the same?

When the following $1.0 \mathrm{mol} {\mathrm{dm}}^3$ aqueous solutions are arranged in order of increasing pH, which is the correct order?

I Ammonium chloride

II Ammonium ethanoate

III Sodium ethanoate

Predict and explain, using equations where appropriate, whether the following solution is acidic, alkaline, or neutral.

$0.1 \mathrm{mol} {\mathrm{dm}}^{-3}{ \mathrm{FeCl}}_3\left(\mathrm{aq}\right)$

Predict and explain, using equations where appropriate, whether the following solution is acidic, alkaline, or neutral.

$0.1 \mathrm{mol} {\mathrm{dm}}^{-3}{ \mathrm{NaNO}}_3\left(\mathrm{aq}\right)$

Predict and explain, using equations where appropriate, whether the following solutions are acidic, alkaline, or neutral.

$0.1 \mathrm{mol} {\mathrm{dm}}^{-3}{ \mathrm{Na}}_2{\mathrm{CO}}_3\left(\mathrm{aq}\right)$

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.

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