The full ionic equation shows all the ions present:
H⁺(aq) + Cl⁻(aq) + Na⁺(aq) + OH⁻(aq) → Na⁺(aq) + Cl⁻(aq) + H₂O(l)
The ionic equation removes spectator ions (ions unchanged):
H⁺(aq) + OH⁻(aq) → H₂O(l)
This equation is the same for ALL neutralisation reactions between an acid and an alkali. It shows that neutralisation is fundamentally about H⁺ and OH⁻ combining to form water.
This higher tier covers Higher Tier: Ionic Equations 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 8 of 13 in this topic. This section is most useful once the core foundation idea is secure, because it adds the detail that pushes answers higher.
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).