# Titration calculations

Patients suffering from iron deficiency are often prescribed tablets containing hydrated iron(II) sulphate, FeSO4.7H2O.

[Molar mass FeSO4.7H2O = 278 g mol–1 )

Some tablets, of total mass 6.00 g, were dissolved in distilled water and made up to 200 cm3 in a volumetric flask. 25.0 cm3 portions of this solution were titrated against a 0.0200 mol dm–3 solution of acidified potassium manganate(VII). The mean titre was 20.10 cm3.

The Fe(II) is oxidized to Fe(III) during the titration

1. What is the mean number of moles of potassium manganate(VII) used in the titration
1. MnO4 – is reduced to Mn2+ in the titration. Find the mole ratio of MnO4 – : Fe2+ in this titration, either by combining two half-equations or using changes in oxidation no.
1. Hence find the moles of Fe2+ in each 25.0 cm3 portion used
1. Hence find the moles of Fe2+ in the 200 cm3 portion solution in the volumetric flask

1. Hence find the mass of FeSO4.7H2O in the 200 cm3 solution in the volumetric flask
1. Calculate the percentage of hydrated iron(II) sulphate in the tablets.

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