Neutralisation Enthalpy Overview
Neutralisation enthalpy refers to the heat change that occurs when an acid reacts with a base to form water and a salt. For strong acids and strong bases, this process is exothermic, meaning it releases heat.
Neutralisation of Strong Acid and Strong Base
- The typical neutralisation reaction involves a strong acid (like HCl) and a strong base (like NaOH).
- The reaction can be represented as:
- HCl + NaOH → NaCl + H2O
Enthalpy Value
- The enthalpy change for the neutralisation of a strong acid with a strong base is approximately -57.1 kcal per mole of water produced.
- This value can vary slightly depending on the specific acid and base used but remains relatively consistent for strong acid-base reactions.
Factors Affecting Neutralisation Enthalpy
- Concentration: The concentration of the acid and base can influence the heat released. Higher concentrations typically lead to more significant heat production.
- Temperature: Initial temperature can affect the enthalpy change. Reactions at higher temperatures may exhibit slightly different enthalpy values.
Practical Implications
- Understanding neutralisation enthalpy is crucial in various applications, such as titrations in analytical chemistry and in industrial processes.
- Safety measures should be taken during experiments due to the exothermic nature of the reaction, which can lead to vigorous reactions if not properly controlled.
In summary, the neutralisation enthalpy for strong acids and bases is a significant concept in thermochemistry, providing insights into the energy changes during acid-base reactions.

-1364.286cal/mol