which is the correct formula of iron-containg compound:(a) or(b)?

Question

a compound has been isolated that can have either of two possible formulas:(a)k[fe(C2O4)2)(H2O)2 ]or (b)k3[fe(C2O4)3]. to fine which is correct,you dissolve a weighed sample of the compound in acid and then titratethe oxalate ion(C2O4 -2) that comes from the compound with potassium permanganate,kMnO4.the balanced net ionic equation for the titration
5C2O4-2+2MnO-4+16H+ gives 2Mn+2 +10CO2+8H2O

tyitration of 1.356 g of the compund requires 34.50ml of 0.108 M KMnO4.

Answer 1

(a) K[Fe(C2O4)2)(H2O)2 ]
- this is the correct one.

Answer 2

So basically, the choice is
a. two oxalates per molecule, or
b. three oxalates per molecule

A. You weigh out the 1.35 grams, calculate how many moles of oxalate if it is a, and how many moles of oxalate if it is b.

B. Now you do the titration, and use 34.5 ml of 0.108 M potassium permanganate. Calculate how many moles of permanganate were used.

C. Use the stoichiometry of the reaction you list for the titration to find how many moles of oxalate were present. Now compare this result with that from part A, and it should be much closer to either a or b.

D. Iron is involved in this reaction. Iron can also participate in redox reactions, and you are using a redox reaction to do the permanganate analysis for oxalate. Might there be an interference? Why or why not?