The heat of neutralisation of one equivalent | vedclass

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(D) The heat of neutralisation is defined as the enthalpy change when $1 	ext{ equivalent}$ of an acid is neutralised by $1 	ext{ equivalent}$ of a

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Both the acid and base are weak

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(D) The heat of neutralisation is defined as the enthalpy change when $1 	ext{ equivalent}$ of an acid is neutralised by $1 	ext{ equivalent}$ of a base. For strong acids and strong bases,the reaction is simply $H^+ (aq) + OH^- (aq) ightarrow H_2O (l)$,which releases approximately $-57.1 	ext{ kJ/mol}$. When either the acid or the base is weak,some energy is consumed in the dissociation of the weak electrolyte. When both the acid and the base are weak,the energy required for the dissociation of both the weak acid and the weak base is significant,resulting in the minimum net heat of neutralisation.

$H-H$ bond energy	$431.37 \text{ kJ mol}^{-1}$
$C=C$ bond energy	$606.10 \text{ kJ mol}^{-1}$
$C-C$ bond energy	$336.49 \text{ kJ mol}^{-1}$
$C-H$ bond energy	$410.50 \text{ kJ mol}^{-1}$

The heat of neutralisation of one equivalent of an acid by one equivalent of a base is minimum when:

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