Key Definitions
Part of Neutralisation Reactions · GCSE GCSE Chemistry revision
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.
Topic position
Section 6 of 13
Practice
20 questions
Recall
20 flashcards
📖 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.
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Read this section alongside the surrounding pages in Neutralisation Reactions. That gives you the full topic sequence instead of a single isolated revision point.
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).
Quick Recall Flashcards
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