For strong acid and strong base neutralisatio | vedclass

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(A) The enthalpy of neutralisation for a strong acid and strong base is given by: $H^{+} + OH^{-} \longrightarrow H_2O; \Delta_r H^{\circ} = -55.84 \

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$5.98 \ kJ \ mol^{-1}$

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(A) The enthalpy of neutralisation for a strong acid and strong base is given by: $H^{+} + OH^{-} \longrightarrow H_2O; \Delta_r H^{\circ} = -55.84 \ kJ \ mol^{-1}$.For the weak acid $CH_3COOH$,the neutralisation reaction is: $CH_3COOH + OH^{-} \longrightarrow CH_3COO^{-} + H_2O; \Delta_r H = -49.86 \ kJ \ mol^{-1}$.The enthalpy of ionisation $(\Delta H_i)$ is the energy required to dissociate the weak acid: $CH_3COOH \longrightarrow CH_3COO^{-} + H^{+}; \Delta H_i = ?$.This can be calculated as: $\Delta H_i = \Delta H_{	ext{neutralisation(weak)}} - \Delta H_{	ext{neutralisation(strong)}}$.$\Delta H_i = -49.86 - (-55.84) = 5.98 \ kJ \ mol^{-1}$.

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