[toadesque]

I have to determine the exact normality of KMnO4. According to my lab handout, the approximate N is .1.

I did titrations and got the following data:

Mass of KMnO4: 0.82 g
Equivalents of KMnO4: 0.025 (really not sure if it's correct though)
Volume of solution (H2O): 0.025 mL
Volume of KMnO4 used in titration: 19 mL

I don't know if this is needed but here is the reaction for oxalate ion.

C2O4 (2-) (aq) => 2CO2 + 2 e-

I got 0.4 for my answer but it seems so wrong. I think the equivalent i used is wrong.

[Borek]

What is reaction equation?

[toadesque]

My lab handout says that the # of equivalents of each reactant is the same. So if I know one side, I should know the other?

I'm not sure what the reaction equation is.

But the overall reaction with the permanganate ion is

5 C2O4 (2-) + 2 MnO4 (-) + 16 H+ => 10 CO2 + 2 Mn (2+) + H2O

If that's it, how do I determine the equivalent #?

[toadesque]

This question kinda deals with the same thing as well. I have to find out the mass of Fe (2+) from my unknown sample.  The mass of the unknown is .5125 g. Volume of KMnO4 is 10.95 mL.

So I still have to know the equivalents of Fe (2+) and then I can go forward to do:

# of equivalents = (grams of substance / GEW substance).

I guess in order to do that I need the reaction equation again...

Fe (2+) => Fe (3+) + 1 e-

When that happens with the reduction of permangnate reaction it's two half reactions:

5 Fe (2+) + MnO4 (-) + 8 H (+) => 5 Fe(3+) + Mn(2+) + 4 H2O