This article may require cleanup to meet Wikipedia's quality standards. Please improve this article if you can. (April 2009)

This article does not cite any references or sources. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. (February 2007)

The standard enthalpy change of neutralisation is the change in enthalpy that occurs when an acid and base undergo a neutralisation reaction to form one mole of water under standard conditions (298 K and 1 atm), i.e. react to produce water and a salt. It is a special case of the standard enthalpy change of reaction.

Equations for working out standard enthalpy of neutralisation:

 q=cm∆t 

Where q is the heat energy liberated in KJ . m is the mass or volume of the solution, usually volume of water in Kg. c is the specific thermal capacity of water normally 4.18. ∆T is the temperature change of the reaction between an acid and a base.

From this the standard enthalpy change (∆h) can be calculated by dividing the negative of q by the moles of the limiting reactant, usually moles of H⁺ ions.

Standard enthalpy change of neutralization=-57.3 kJ/mol

∆h=-q/n in kJmol^-1

 the standard enthalpy of mineral acids is far greater than that of organic acids. this is because strong acids ionise completely and yet organic acids ionise partially. 

This chemistry article is a stub. You can help Wikipedia by expanding it. v • d • e

..................