Calculate the mass of impure iron used in the experiment if the beaker has a mass of $36.53\,\text{g}$ and the beaker plus impure iron has a mass of $38.31\,\text{g}$.
Give a test and observation to identify hydrogen gas produced in the reaction $\text{Fe}(s) + 2\text{H}^+(aq) \rightarrow \text{Fe}^{2+}(aq) + \text{H}_2(g)$.
Suggest how the student makes sure that no $\text{Fe}^{2+}(aq)$ is left on the filter paper.
Suggest how the student should make sure that every drop of filtrate is transferred from the conical flask to the volumetric flask.
Name the piece of apparatus used to transfer $25.0\,\text{cm}^3$ of solution P into the conical flask.
Identify the solution used to wash out the burette before it is filled with solution Q.
Use the diagrams to fill in the table and calculate the average volume of Q.
Calculate the number of moles of potassium manganate(VII) in the average volume of $0.0100\,\text{mol dm}^{-3}$ solution Q.
One mole of potassium manganate(VII) reacts with five moles of $\text{Fe}^{2+}(aq)$. Calculate the number of moles of $\text{Fe}^{2+}(aq)$ in $25.0\,\text{cm}^3$ of P.
Calculate the number of moles of $\text{Fe}^{2+}(aq)$ in $500\,\text{cm}^3$ of P.
Calculate the mass of iron in $500\,\text{cm}^3$ of P. [$A_r(\text{Fe}) = 56$]
Use your answers to (a) and (k) to calculate the percentage by mass of iron in the impure iron.