Lawrie Ryan and Roger Norris Solutions for Chapter: Equilibria, Exercise 16: Questions

Suggest a suitable indicator to find the end-points of the reactions between: $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ nitric acid and $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous ammonia.

Suggest a suitable indicator to find the end-points of the reactions between: $2.00 \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous sodium hydroxide and $1.00 \mathrm{mol} {\mathrm{dm}}^{-3}$ sulphuric acid.

Suggest a suitable indicator to find the end-points of the reactions between $0.00500 \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous potassium hydroxide and $0.00500 \mathrm{mol} {\mathrm{dm}}^{-3}$ butanoic acid.

Suggest why phenolphthalein would not be a suitable indicator to use to find the end-point when $0.0100 \mathrm{mol} {\mathrm{dm}}^{-3}$ hydrochloric acid is titrated against $0.0100 \mathrm{mol} {\mathrm{dm}}^{-3}$ urea, a weak base.

The sketch graph (Figure $8.23$) shows the change in $\mathrm{pH}$ when an acid and an alkali react with one being added slowly to the other. Both acid and alkali have a concentration $0.1 \mathrm{mol} {\mathrm{dm}}^{-3}$. Which one of these statements is correct?