The value of the enthalpy of neutralization o | vedclass

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(A) The enthalpy of neutralization is defined as the heat evolved when $1 \ gram \ equivalent$ of an acid is neutralized by $1 \ gram \ equivalent$ of

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Both acid and base are strong.

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(A) The enthalpy of neutralization is defined as the heat evolved when $1 \ gram \ equivalent$ of an acid is neutralized by $1 \ gram \ equivalent$ of a base in dilute solution. For strong acids and strong bases,the enthalpy of neutralization is constant at approximately $-57.1 \ kJ \ mol^{-1}$ because it represents the heat of formation of water from $H^+$ and $OH^-$ ions $(H^+ + OH^- \rightarrow H_2O)$. If either the acid or the base is weak,some energy is consumed in the dissociation of the weak electrolyte,making the enthalpy of neutralization less than $-57.1 \ kJ \ mol^{-1}$. Therefore,the value is most significant and constant when both the acid and the base are strong.

$H-H$ 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 value of the enthalpy of neutralization of an acid and a base is significant only when $......$

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