Define what is meant by the enthalpy change of neutralisation, $\Delta H_{\text{neut}}$.
Use equation 1 to work out the amount, in mol, of $\text{H}_2\text{SO}_4\text{(aq)}$ neutralised in the experiment.
Calculate the theoretical maximum temperature of the mixture in this experiment. Assume that the enthalpy change of neutralisation, $\Delta H_{\text{neut}}$, of $\text{NaOH(aq)}$ and $\text{H}_2\text{SO}_4\text{(aq)}$ is $-57.1\,\text{kJ mol}^{-1}$, full dissociation of $\text{H}_2\text{SO}_4\text{(aq)}$ occurs, the specific heat capacity of the final solution is $4.18\,\text{J g}^{-1}\text{K}^{-1}$, $1.00\,\text{cm}^3$ of the final solution has a mass of $1.00\,\text{g}$, there is no heat loss to the surroundings, and the experiment takes place at constant pressure. Show your working.
Complete the equation for the reaction: $\text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \;\;\;\;\;\;\;\;$
Suggest why the value of $\Delta H_{\text{neut}}$ for the weak acid, $\text{CH}_3\text{COOH}$, reacting with $\text{NaOH}$ is different from the value found using the strong acid, $\text{HCl}$. Assume the results are obtained under the same conditions.