[Nasbah bm]

i have a question.
how to determine percentage oxidation of a sample of partially oxidized FeSO4.7H2O, provided 0.02 KMnO4?

[Borek]

You have to show your attempts at solving the question to receive help. This is a forum policy.

It would also not hurt to list the problem with all data you have and with the information about procedure. As of now there is not enough information to help you without making guesses about what what it is all about.

Definitely start with the reaction equation.

[Nasbah bm]

firstly thanks for replying
KMnO4 Molarity is .02 and of FeSO4 is 0.1
volum of both = 10 ml

2KMnO4+8H2SO4+10FeSO4.7H2O==K2SO4+2MnSO4+5Fe2(SO4)3+78H2O

so     5 Fe2+ + MnO4- + 8 H+ → 5 Fe3++ Mn2+ + 4 H2O

so fe+2 is oxidized to fe+3
after that I have no clue
should I be comparing masses of iron in reactant and product?? and get %???

[Dan]

Your English and formatting are atrocious.

Write properly, capitalise your elemental symbols correctly and use subscript/superscript.

e.g. KMnO₄^- not kmno4-

These are Forum Rules, which you agreed to follow before posting.

[Nasbah bm]

Sir you are right but I am unable to write my question in that formte but however i will try to follow this formte, to which i agreed to follow before posting

[Borek]

i will try to follow this formte

About post formatting...

[Nasbah bm]

thanks Chembuddy that was really helpful!