Complete the table using the diagrams. Tick $(\checkmark)$ the best titration results. Use those results to calculate the average volume of $\text{H}_2\text{SO}_4\text{(aq)}$ needed to neutralise the $\text{NaOH(aq)}$.
Calculate the number of moles of $\text{NaOH}$ in $10.0\,\text{cm}^3$ of $0.100\,\text{mol dm}^{-3}$ $\text{NaOH(aq)}$.
The reaction equation between $\text{NaOH}$ and $\text{H}_2\text{SO}_4$ is shown. $2\text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O}$ Calculate the number of moles of $\text{H}_2\text{SO}_4$ that react with $10.0\,\text{cm}^3$ of $0.100\,\text{mol dm}^{-3}$ $\text{NaOH(aq)}$.
Calculate the concentration of the $\text{H}_2\text{SO}_4\text{(aq)}$ in $\text{mol dm}^{-3}$. Give your answer to three significant figures.