Okay so I have a question about this equivalent mass/Normality stuff Since i'm really bad at Gchem I decided to start from the beginning with Schaums College Gchem and it's pretty good. Anyway, I got to the normality stuff, specifically question 13.12 in the Schaum text, and I think somethings not registering. So if someone would like to help it would be really great if you did. The question states... Calculate the mass (g) of FeSO4 that will be oxidized by 24.0mL of .250 N KMn04 in a solution acidified with sulfuric acid. The unbalanced equation for the reaction is below. The statement of normality of KMnO4 is with respect to the reaction (Mn changes from +7 to +2 during this reaction). MnO4- + Fe2+ + H+ ----> Fe3+ + Mn2+ + H20 So in the beginning of the solution they solve for the Equivalent mass of FeSO4 (this I understand), Fe is oxidized with one electron therefore it equals molar mass/ oxidation change = 152/1 Here is where I get messed up They set the equation up like this Number of eq KMnO4 = number of eq FeSO4 (volume KMnO4) x (normality KMnO4) = (mass FeSO4)/(equivalent mass FeSO4) Maybe I don't understand the concept of equivalence but how are these two things equal to each other. can someone explain please? by the way the answer is w=.912g FeSO4 if someone was wondering.