URGENT HELP NEEDED :( MEDALS WILL BE GIVEN :)

[(5Fe2+) + (MnO4-) + (8H+)]
--
[(5Fe3+) + (Mn2+) + (4H2O)]

(titrating with KMnO4)

Knowing the volume of KMnO4 needed to oxidise Fe2+ by tirations, how do I calculate the initial concentration of Fe2+ ions?

Question

URGENT HELP NEEDED :(   MEDALS WILL BE GIVEN :)

[(5Fe2+) + (MnO4-) + (8H+)] 
--> 
[(5Fe3+) + (Mn2+) + (4H2O)]

(titrating with KMnO4)

Knowing the volume of KMnO4 needed to oxidise Fe2+ by tirations, how do I calculate the initial concentration of Fe2+ ions?

aaronq · Answer

use stoichiometry. the amount of moles of $\sf Fe^{2+}$oxidized is 5 times that of $\sf KMnO_4$ used.