If I am given that an unknown sample containing iron(II)ion is .949 g and it requires 31.28 ml of .01192 M KMnO4 to titrate the sample to a pink end- point....
How can i calculate the moles of MnO4 ion consumed and the moles of of Fe^(2+) in the sample? Thanks
mols KMnO4 consumed = M x L.
Convert mols KMnO4 to mols Fe by using the coefficients in the balanced redox equation between Fe(II) and KMnO4.
Then g Fe = mols Fe x molar mass Fe.
Finally, %Fe = [mass Fe/mass sample]*100
Post your work if you get stuck.