In chemistry and thermodynamics, the enthalpy of neutralization is the change in enthalpy that occurs when one equivalent of an acid and a base undergo a neutralization reaction to form water and a salt. It is a special case of the enthalpy of reaction. It is defined as the energy released with the formation of 1 mole of water.When a reaction is carried out under standard conditions at the temperature of 298 K (25 degrees Celsius) and 1 atm of pressure and one mole of water is formed, the heat released by the reaction is called the standard enthalpy of neutralization .
The heat released during a reaction is
Q=mcp\DeltaT
where is the mass of the solution, is the specific heat capacity of the solution, and is the temperature change observed during the reaction. From this, the standard enthalpy change is obtained by division with the amount of substance (in moles) involved.
\DeltaH=-
| Q | |
| n |
For weak acids or bases, the heat of neutralization is pH-dependent. In the absence of any added mineral acid or alkali, some heat is required for complete dissociation. The total heat evolved during neutralization will be smaller.
e.g. at 25°C
The heat of ionization for this reaction is equal to (–12 + 57.3) = 45.3 kJ/mol at 25 °C.[2]