2gAcids, bases and salt preparations

Syllabus objectives

• 2.34know the general rules for predicting the solubility of ionic compounds in water: • common sodium, potassium and ammonium compounds are soluble • all nitrates are soluble • common chlorides are soluble, except those of silver and lead(II) • common sulfates are soluble, except for those of barium, calcium and lead(II) • common carbonates are insoluble, except for those of sodium, potassium and ammonium • common hydroxides are insoluble except for those of sodium, potassium and calcium (calcium hydroxide is slightly soluble).
• 2.35understand acids and bases in terms of proton transfer
• 2.36understand that an acid is a proton donor and a base is a proton acceptor
• 2.37describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, bases and metal carbonates (excluding the reactions between nitric acid and metals) to form salts
• 2.38know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in water
• 2.39describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactant
• 2.40describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an acid and alkaliSeparate Chemistry only
• 2.41describe an experiment to prepare a pure, dry sample of an insoluble salt, starting from two soluble reactantsSeparate Chemistry only
• 2.42practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxidePractical
• 2.43practical: prepare a sample of pure, dry lead(II) sulfateSeparate Chemistry onlyPractical