Asked by amirah
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.
a) balanced eq?
b) calculate the percentage of iron in the sample.
Answers
Answered by
DrBob222
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.
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.
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