Iron is an element that is essential in the human diet. Some people need to take iron supplement tablets to ensure an adequate intake of iron. You will investigate the mass of iron in an iron supplement tablet by titrating a solution with potassium manganate(VII). FB 1 is an aqueous solution of iron supplement tablets made by dissolving 14 tablets in $$\(1.00 \mathrm{dm}^{3}\)$$ of solution. The iron in each tablet is iron(II) sulfate, $$\(\mathrm{FeSO}_{4} \bullet 7 \mathrm{H}_{2} \mathrm{O}\)$$. FB 2 is $$\(0.0100 \mathrm{~mol} \mathrm{dm}^{-3}\)$$ acidified aqueous potassium manganate(VII), $$\(\mathrm{KMnO}_{4}\)$$. FB 3 is dilute sulfuric acid, $$\(\mathrm{H}_{2} \mathrm{SO}_{4}\)$$. From your accurate titration results, calculate a suitable mean value to use in your calculations. Show clearly how you obtain the mean value. $$\(25.0 \mathrm{~cm}^{3}\)$$ of FB 1 required $$\(\mathrm{cm}^{3}\)$$ of FB 2.

Answer:

Knowledge points:

Solution: