Comprehension Enthalpy of neutralization is defined as the enthalpy change when 1 mole of an aci...
0Comprehension Enthalpy of neutralization is defined as the enthalpy change when 1 mole of an acid/a base is completely neutralized by a base/an acid in dilute solution.
For strong acid and strong base, neutralizations net chemical change is
\[
\mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\ell) ; \Delta_{\mathrm{r}} \mathrm{H}^{\mathrm{o}}=-55.84 \mathrm{~kJ} / \mathrm{mol}
\]
\( \Delta \mathrm{H}_{\text {ionization }}^{\mathrm{o}} \) of aqueous solution of strong acid and strong base is zero.
When a dilute solution of a weak acid or base is neutralized, the enthalpy of neutralization is some what less because of the absorption of heat in the ionization of the weak acid or weak base, for a weak acid/ weak base
\[
\Delta \mathrm{H}_{\text {neutralization }}^{\mathrm{o}}=\Delta \mathrm{H}_{\text {ionization }}^{\mathrm{o}}+\Delta_{\mathrm{r}} \mathrm{H}^{\circ}\left(\mathrm{H}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}\right)
\]
If enthalpy of neutralization of \( \mathrm{CH}_{3} \mathrm{COOH} \) by \( \mathrm{NaOH} \) is \( -49.86 \mathrm{~kJ} / \mathrm{mol} \), then enthalpy of ionization of \( \mathrm{CH}_{3} \mathrm{COOH} \) is:
(a) \( 5.98 \mathrm{~kJ} / \mathrm{mol} \)
(b) \( -5.98 \mathrm{~kJ} / \mathrm{mol} \)
(c) \( 105.7 \mathrm{~kJ} / \mathrm{mol} \)
(d) None of these
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