Calculate the mass of mixture used in the experiment.
Suggest how the student ensures that no iron(II) sulfate is left on the filter paper.
Suggest how the student should ensure that all the aqueous iron(II) sulfate is moved from the conical flask to the volumetric flask.
Name the additional piece of apparatus used alongside the pipette.
State the colour change seen in the conical flask at the end-point of the titration.
Use the diagrams to fill in the table and calculate the average volume of T.
Calculate the number of moles of potassium manganate(VII) in the average volume of T used in the titration.
Calculate the number of moles of $\text{FeSO}_4$ in $20.0\,\text{cm}^3$ of R.
Calculate the number of moles of $\text{FeSO}_4$ present in $500\,\text{cm}^3$ of R.
Calculate the mass of $\text{FeSO}_4$ contained in $500\,\text{cm}^3$ of R. $[M_r:\text{FeSO}_4, 152]$
Use your answers to (a) and (j) to find the percentage by mass of $\text{FeSO}_4$ in the mixture.