Redox titration calculation
An experiment was carried out to find the value of n in hydrated iron(II) ethanedioate, FeC2O4nH2O.
1.71 g of the compound was dissolved in deionised water and made up to 250 cm3 solution in a
volumetric flask. When 25.0 cm3 of this solution was acidified using an excess of dilute sulfuric acid, it
was found to react with 28.50 cm3 of 0.0200 mol dm-3 potassium manganate(VII).
a) Deduce the number of moles of MnO4
– that react with one mole of FeC2O4nH2O. Remember that both
the Fe2+ and C2O4
2– ions react.
b) Find the relative formula mass of hydrated iron(II) ethanedioate and the value of n.
Can anyone explain how to form the redox equation?
1.71 g of the compound was dissolved in deionised water and made up to 250 cm3 solution in a
volumetric flask. When 25.0 cm3 of this solution was acidified using an excess of dilute sulfuric acid, it
was found to react with 28.50 cm3 of 0.0200 mol dm-3 potassium manganate(VII).
a) Deduce the number of moles of MnO4
– that react with one mole of FeC2O4nH2O. Remember that both
the Fe2+ and C2O4
2– ions react.
b) Find the relative formula mass of hydrated iron(II) ethanedioate and the value of n.
Can anyone explain how to form the redox equation?
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