The student measures a volume with the wrong apparatus. Identify the incorrect apparatus and suggest a more precise alternative.
Explain why the mixture in the volumetric flask is shaken at step 5.
Explain the purpose of the indicator in step 9.
Calculate the mass of citric acid put into the beaker.
Calculate the number of moles of citric acid put into the beaker. Give your answer to three significant figures. $[M_r\text{ citric acid} = 192]$
Calculate the concentration, in $\text{mol dm}^{-3}$, of the citric acid solution in the volumetric flask.
Use the diagrams to fill in the values for titration 1 in the results table shown.
Complete the table by ticking the most reliable titration results. Explain why these values have been ticked.
Use the most reliable titration results to work out the mean volume of $\text{NaOH(aq)}$ used.
Use your result from (f) to calculate the number of moles of citric acid present in $25.0\text{ cm}^3$ of solution P.
Calculate the number of moles of $\text{NaOH}$ that react with the citric acid in $25.0\text{ cm}^3$ of solution P, using $\text{C}_6\text{H}_8\text{O}_7 + 3\text{NaOH} \rightarrow \text{Na}_3\text{C}_6\text{H}_5\text{O}_7 + 3\text{H}_2\text{O}$.
Calculate the concentration, in $\text{mol dm}^{-3}$, of $\text{NaOH(aq)}$.
Use the equation $2\text{NaOH(aq)} + \text{FeSO}_4\text{(aq)} \rightarrow \text{Na}_2\text{SO}_4\text{(aq)} + \text{Fe(OH)}_2\text{(s)}$ together with your answer from (l) to work out the number of moles of $\text{Fe(OH)}_2\text{(s)}$ formed.
State the colour seen for the precipitate.