[xstrae]

Can someone give me a clue on how to start this problem?
How many ml of 0.05M KMnO4 solution are required to oxidise 2.0g of FeSO4 in a dilute acid solution?
How do you determine the equation in such a case? I know the standard reaction of KMnO4 with H2SO4 but how do u put in FeSO4 in this?

[Borek]

Only thing that can be not obvious is the permanganate part. Generally speaking it gets reduced to MnO₄^2- in alkailic solution, to MnO₂ in neutral, and to Mn²⁺ in acidic.

http://www.chembuddy.com/?left=balancing-stoichiometry&right=half-reactions-method

Otherwise - as usual - start with the reaction equation