ChemistryCode 9701
Brønsted–Lowry theory of acids and bases
What this topic asks you to be able to do
- give the name and formula of each typical acid, limited to hydrochloric acid, HCl, sulfuric acid, H2SO4, nitric acid, HNO3, ethanoic acid, CH3COOH
- recall the name and formula of each typical alkali, limited to sodium hydroxide, NaOH, potassium hydroxide, KOH, ammonia, NH3
- describe how the Brønsted–Lowry theory defines an acid and a base
- outline how strong acids and strong bases dissociate fully in aqueous solution, while weak acids and weak bases dissociate partially
- appreciate that water has a pH of 7, that acid solutions have a pH below 7 and that alkaline solutions have a pH above 7
- account for, in qualitative terms, how strong and weak acids differ in behaviour, including their reactions with a reactive metal and their pH values measured using a pH meter, universal indicator or conductivity
- appreciate that neutralisation takes place when H+(aq) and OH–(aq) combine to give H2O(l)
- understand that neutralisation reactions produce salts
- sketch the pH titration curves for each pairing of a strong or weak acid with a strong or weak alkali
- select a suitable indicator for an acid–alkali titration from appropriate data (pKa values do not feature)