1. Here is the part of the equation you need to work the problem. You can fill in all the rest of it.
MnO4^- + 5Fe^2+ ==> 5Fe^3+ + Mn^2+
2. mols KMnO4 = M x L = ?
mols Fe = 5 x mols KMnO4
grams Fe = mols Fe x atomic mass Fe = ?
%Fe in sample = (grams Fe/grams sample)*100 = ?
Post yuour work if you get stuck.
A sample of 1.55g of iron ore is dissolved in a acid solution in which the iron is converted into Fe2+. The solution formed is then titrated with KMnO4 which oxidises Fe2+ to Fe3+ while the MnO4- ions are reduced to Mn2+ ions. 92.95 mL of 0.020M KMnO4 is required for titration to reach the equivalent point.
a) Write the balanced equation for the titration.
b) Calculate the percentage of iron in the sample.
5 answers
Where is the KMnO4 in the chemical equation?
Why Fe2+ and Fe3+ become 5Fe2+ and 5Fe3+
5.6
The answer is 33.49%
1 answer