Standard enthalpy change of neutralisation
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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 = mcΔT
Where:
- Q is the heat energy liberated
- m is the mass of the solution.
- c is the specific heat capacity of the solution.
- ∆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.
The standard enthalpy change of neutralisation for a strong acid and base is -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.
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