An iron deficiency can be treated with iron tablets. A chemist wants to determine the percentage by mass of iron(II) ions (Fe2+\text{Fe}^{2+}Fe2+) in a brand of iron tablets.
She uses the following method:
The table below shows her experimental results:
| Measurement | Value |
|---|---|
| Mass of iron tablet | 0.350 g0.350\text{ g}0.350 g |
| Concentration of KMnO4\text{KMnO}_4KMnO4 solution | 0.0150 mol/dm30.0150\text{ mol/dm}^30.0150 mol/dm3 |
| Volume of KMnO4\text{KMnO}_4KMnO4 solution added | 22.40 cm322.40\text{ cm}^322.40 cm3 |
Calculate the amount, in moles, of KMnO4\text{KMnO}_4KMnO4 in 22.40 cm322.40\text{ cm}^322.40 cm3 of 0.0150 mol/dm30.0150\text{ mol/dm}^30.0150 mol/dm3 potassium permanganate solution.
In the titration, 1 mol1\text{ mol}1 mol of KMnO4\text{KMnO}_4KMnO4 reacts with 5 mol5\text{ mol}5 mol of Fe2+\text{Fe}^{2+}Fe2+. Calculate the amount, in moles, of Fe2+\text{Fe}^{2+}Fe2+ in the iron tablet.
Calculate the mass, in grams, of Fe2+\text{Fe}^{2+}Fe2+ in the iron tablet. [Ar of Fe=56.0A_{\text{r}}\text{ of Fe} = 56.0Ar of Fe=56.0]
Calculate the percentage by mass of Fe2+\text{Fe}^{2+}Fe2+ in the iron tablet.
