This definitions covers Key Definitions within Neutralisation Reactions for GCSE Chemistry. Revise Neutralisation Reactions in Chemical Changes for GCSE Chemistry with 20 exam-style questions and 20 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 6 of 13 in this topic. Make sure you can use the exact wording confidently, because definition marks are often lost through vague language.
📖 Key Definitions
Neutralisation: The reaction between an acid and a base (or alkali) to form a salt and water. The H⁺ ions from the acid react with the OH⁻ ions from the alkali: H⁺ + OH⁻ → H₂O.
Salt: An ionic compound formed when the H⁺ ions of an acid are replaced by metal ions (or ammonium ions). The name of the salt comes from the acid and the base used.
Base: A substance that neutralises an acid to form a salt and water. Bases include metal oxides, metal hydroxides, and metal carbonates.
Ionic equation for neutralisation: H⁺(aq) + OH⁻(aq) → H₂O(l) — this is the same for ALL acid-alkali neutralisations, regardless of which specific acid or alkali is used.
Practice questions for Neutralisation Reactions
Which word equation correctly represents a neutralisation reaction?
Explain why the ionic equation for any strong acid-alkali neutralisation is always H⁺(aq) + OH⁻(aq) → H₂O(l).