Neutralisation — H⁺ meets OH⁻

4 minAS Level7.2.7

AI-drafted, independently checked · not yet teacher-reviewed

By the end of this lesson

By the end you can write the ionic equation for neutralisation, explain why ΔH_neut for strong acid + strong base is –57 kJ mol⁻¹, and predict the pH of the resulting solution.

The heart of neutralisation

Neutralisation is one reaction at its core: $\text{H}^+(\text{aq}) + \text{OH}^-(\text{aq}) \rightarrow \text{H}_2\text{O(l)}$

Everything else (spectator ions, salts, enthalpy) is just packaging around this.

Worked example: Molecular, ionic, and net ionic

Write the three equations for HCl + NaOH.

Have a go first?

Neutralisation equations

Short answerQuestion 1 · Apply

Write the net ionic equation for the reaction between H₂SO₄(aq) and NaOH(aq). Use H+ for H⁺, OH- for OH⁻, H2O for H₂O.

Short answerQuestion 2 · Apply

Write the net ionic equation for the reaction between CH₃COOH(aq) and NaOH(aq). CH₃COOH is a weak acid (write it as CH3COOH). Use OH- for OH⁻, H2O for H₂O, CH3COO- for CH₃COO⁻.

Answer the 2 questions above to continue.

Previous lessonStrong vs weak acids — it's about dissociation Next lessonSalts — the neutralisation products