Acid-Base Chemistry structured questions · SEC G3 Pure Chemistry

Learning objectives

• describe the meanings of the terms acid and alkali in terms of the ions they produce in aqueous solution and their effects on Universal Indicator
• describe neutrality and relative acidity and alkalinity, in terms of — relative H+ and OH– ion concentrations,
• describe neutrality and relative acidity and alkalinity, in terms of — colour in Universal Indicator, and
• describe neutrality and relative acidity and alkalinity, in terms of — the pH scale (calculation of pH from hydrogen ion concentration is not required)
• describe qualitatively the difference between strong and weak acids in terms of the extent of ionisation
• describe the characteristic properties of acids as in reactions with metals, bases and carbonates to form salts
• describe the reaction between hydrogen ions and hydroxide ions to produce water, H+ + OH– → H2O, as neutralisation
• describe the importance of controlling the pH in soils and how excess acidity can be treated using calcium hydroxide
• describe the characteristic properties of bases in reactions with acids and with ammonium salts
• classify oxides as acidic, basic, amphoteric or neutral based on metallic/non-metallic character.
• describe the techniques used in the preparation, separation and purification of salts as examples of some of the techniques specified in Section 1.2(a) (methods for preparation should include precipitation and titration together with reactions of acids with metals, insoluble bases and insoluble carbonates)
• describe the general rules of solubility for common salts to include nitrates, chlorides (including those of silver and lead), sulfates (including those of barium, calcium and lead), carbonates, hydroxides, salts of Group 1 cations and ammonium salts
• suggest a method of preparing a given salt from suitable starting materials, given appropriate information.
• describe the use of nitrogen, from air, and hydrogen, from the cracking of crude oil, in the manufacture of ammonia
• state that some chemical reactions are reversible, e.g. manufacture of ammonia
• interpret data relating to the conditions used in industry for processes involving reversible reactions, e.g. manufacture of ammonia by the Haber Process (knowledge of Le Chatelier’s Principle is not required).