7. Acids, bases and salts
- Syllabus
- 0620–2026–2027
- Section
- 7
- Level
- —
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Topic 7.1
7.1 The characteristic properties of acids and bases
Objectives in this topic
7.1.1—Characteristic properties of acids in
- Describe characteristic properties of acids in terms of their reactions with: (a) metals (b) bases (c) carbonates
7.1.2—Acids in terms of their effect on: (a)
- Describe acids in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange
7.1.3—Bases are oxides or hydroxides of
- State: bases are oxides or hydroxides of metals and that alkalis are soluble bases
7.1.4—Characteristic properties of bases in
- Describe characteristic properties of bases in terms of their reactions with: (a) acids (b) ammonium salts
7.1.5—Alkalis in terms of their effect on
- Describe alkalis in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange
7.1.6—Aqueous solutions of acids contain H+
- State: aqueous solutions of acids contain H+ ions and aqueous solutions of alkalis contain OH– ions
7.1.7—To compare hydrogen ion concentration
- Describe how to compare hydrogen ion concentration, neutrality, relative acidity and relative alkalinity in terms of colour and pH using universal indicator paper
7.1.8—Neutralisation reaction between an
- Describe neutralisation reaction between an acid and an alkali to produce water, H+ (aq) + OH– (aq) → H2O (l)
7.1.9—Acids as proton donors and bases as
- Define acids as proton donors and bases as proton acceptors
7.1.10—Strong acid as an acid that is
- Define a strong acid as an acid that is completely dissociated in aqueous solution and a weak acid as an acid that is partially dissociated in aqueous solution
7.1.11—Hydrochloric acid is a strong acid, as
- State: hydrochloric acid is a strong acid, as shown by the symbol equation, HCl (aq) → H+(aq) + Cl –(aq)
7.1.12—Ethanoic acid is a weak acid, as shown
- State: ethanoic acid is a weak acid, as shown by the symbol equation, CH3COOH(aq) ⇌ H+(aq) + CH3COO–(aq)
Topic 7.2
7.2 Oxides
Objectives in this topic
7.2.1—Classify oxides as acidic
- Classify oxides as acidic, including SO 2 and CO2, or basic, including CuO and CaO, related to metallic and non-metallic character
7.2.2—Amphoteric oxides as oxides that react
- Describe amphoteric oxides as oxides that react with acids and with bases to produce a salt and water
7.2.3—Classify Al 2O3 and ZnO as amphoteric
- Classify Al 2O3 and ZnO as amphoteric oxides
Topic 7.3
7.3 Preparation of salts
Objectives in this topic
7.3.1—Preparation, separation and
- Describe preparation, separation and purification of soluble salts by reaction of an acid with: (a) an alkali by titration (b) excess metal (c) excess insoluble base (d) excess insoluble carbonate
7.3.2—Salt solubility rules: soluble
- Describe salt solubility rules: soluble sodium/potassium/ammonium salts and nitrates; chlorides except lead/silver; sulfates except barium/calcium/lead; insoluble carbonates except sodium/potassium/ammonium; insoluble hydroxides except sodium/potassium/ammonium/calcium (partial)
7.3.3—Hydrated substance as a substance that
- Define a hydrated substance as a substance that is chemically combined with water and an anhydrous substance as a substance containing no water
7.3.4—Preparation of insoluble salts by
- Describe preparation of insoluble salts by precipitation
7.3.5—Term water of crystallisation as the
- Define the term water of crystallisation as the water molecules present in hydrated crystals, including CuSO4•5H2O and CoCl2•6H2O