posted by june .
1)If 36 mL of KMnO4 solution are required to oxidize 25 mL of 0.02932 M NaC204 solution, what is the concentration of the solution?
2)A Certain brand of iron supplement contains FeSO4-7H2O with miscellaneous binders and fillers. Suppose 22.93 mL of the KMn04 solution used in question one above are needed to oxidize Fe2+ to Fe3+ in a 0.4927 g pill. What is the mass % of FeSO4-7H2O(MM 278.03 g mol) in the pill?
1. Write the equation and balance it. I think 2 KMnO4 requires 5 Na2C24(note your typo).
moles KMnO4 = M x L = ??
Using the coefficients in the balanced equation, convert moles KMnO4 to moles Na2C2O4.
Now, M Na2C2O4 = moles Na2C2O4/L Na2C2O4.
2. Same thing for Fe sample. However, instead of M of Fe at the end, convert moles to grams FeSO4.7H2O, then
% = (mass FeSO4.7H2O/mass sample)*100 =xx
Post your work if you get stuck.