Why was the aqueous sodium hydroxide left for a few minutes before the first portion of sulfuric acid was added?
What kind of reaction is indicated by the temperature rise?
Why does the temperature start to fall after $25.0\,\text{cm}^3$ of sulfuric acid has been added?
Plot temperature against the volume of sulfuric acid added, then find the intersection point.
From your graph, what volume of sulfuric acid is needed to react with all the aqueous sodium hydroxide?
What temperature does the mixture reach when this volume of sulfuric acid has been added?
Write the equation for the reaction of sulfuric acid with aqueous sodium hydroxide.
From your equation in (f)(i) and your answer to (e)(i), calculate the concentration of the sulfuric acid used.
Calculate the largest temperature change.
Calculate the total volume of liquid in the beaker when the temperature reaches its maximum.
Use the formula $\Delta H = \dfrac{\text{volume in (g)(ii)} \times 4.2 \times \text{temperature change in (g)(i)}}{1000 \times \text{moles of aqueous sodium hydroxide used}}$ to work out the enthalpy change, $\Delta H$, for the reaction.
Describe how the student can prepare pure dry crystals of sodium sulfate from the solution.