Question

a sample iron ore is dissolved in an acidic solution in which yhe iron is converted into fe2+. the solution formed the titrated with kmno4 which oxidies fe2+ to fe3+ while kmno- ions are reduced to mn2+. 92.95 ml of 0..02M of kmno4 is required for titration to reach the equivalent point.

a) balanced eq?

b) calculate the percentage of iron in the sample.

Answer 1

First let me suggest you find the caps key on your keyboard and use it. There is a big difference between Co, CO, and co. kmno4 doen't mean much to me.
I'll balance the redox part; you can finish.
5Fe^2+ + KMnO4 ==> 5Fe^3+ + Mn^2+
mols KMnO4 = M x L = ?
mols Fe = mols KMnO4 x 5
grams Fe = mols Fe x atomic mass Fe
%Fe = (grams Fe/grams sample)*100 = ?
It should be obvious that you didn't give a mass of the sample so you can't calculate percent Fe in the sample.

Post your work if you get stuck.

Post your work if you get stuck.