Enthalpy of Neutralisation
| Formula / Notation | ΔH°_neut: H⁺(aq)+OH⁻(aq)→H₂O; strong/strong: −57.1 kJ/mol |
|---|---|
| Also Known As | Heat of neutralisation, ΔH_neut, neutralisation enthalpy |
What is Enthalpy of Neutralisation?
The heat released when one mole of water is formed by the reaction of an acid with a base under standard conditions. For strong acid-strong base reactions, this value is approximately -57 kJ/mol. Weaker acids or bases give less negative values due to incomplete dissociation.
Formula & Notation
Other Names / Synonyms: Heat of neutralisation, ΔH_neut, neutralisation enthalpy
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
The heat released when one mole of water is formed by the reaction of an acid with a base under standard conditions. For strong acid-strong base reactions, this value is approximately -57 kJ/mol. Weaker acids or bases give less negative values due to incomplete dissociation.
Enthalpies of neutralisation are used in thermochemical calculations, in calorimetric analysis, in understanding acid strength differences, and in industrial neutralisation process design (heat management in large-scale acid-base reactions).
Concentrated acid-base neutralisations are highly exothermic and can cause boiling and splattering if mixed too quickly. Industrial neutralisation must use controlled addition rates, adequate cooling, and appropriate PPE.
The formula or notation for Enthalpy of Neutralisation is: ΔH°_neut: H⁺(aq)+OH⁻(aq)→H₂O; strong/strong: −57.1 kJ/mol