Calculate the mass of V used in the experiment.
What is the colour of the solution in the conical flask before the acid is added and at the end-point?
Use the diagrams to fill in the titration table and determine the mean volume of $0.100\,\text{mol dm}^{-3}$ hydrochloric acid used.
Calculate the number of moles of hydrochloric acid in the average volume of $0.100\,\text{mol dm}^{-3}$ hydrochloric acid from (c).
Using the equation $\text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O}$ and your answer from (d), determine the number of moles of sodium hydroxide in $25.0\,\text{cm}^3$ of W.
Using your answer from (e), calculate the number of moles of sodium hydroxide in $250\,\text{cm}^3$ of W.
Calculate the number of moles of sodium hydroxide in $50\,\text{cm}^3$ of $1.00\,\text{mol dm}^{-3}$ sodium hydroxide.
By subtracting your answer in (f) from your answer in (g), calculate how many moles of sodium hydroxide reacted with the original sample of the organic acid, V.
One mole of V reacts with two moles of sodium hydroxide. Deduce the number of moles of V in the sample.
Using your answers from (a) and (i), calculate the relative molecular mass of the acid V.
The acid V contains two carboxylic acid groups and has the molecular formula $\text{HO}_2\text{C}_x\text{H}_y\text{CO}_2\text{H}$. Deduce the values of $x$ and $y$ in the molecular formula.
Give the structure of the ester produced when V reacts with two molecules of ethanol under suitable conditions.