In an experiment, you get about 0.3g K 3 [Fe(C 2 O 4 ) 3 ].3H 2 O, and dissolve

Question

In an experiment, you get about 0.3g K3[Fe(C2O4)3].3H2O, and dissolve it in about 20ml of 3M H2SO4 solution, then you add about 20ml of distilled water to it.

Next, you fill your buret with 0.02M KMnO4 and heat the solution of K3[Fe(C2O4)3].3H2O you just prepared. Titrate the hot solution using the buret, you added the MnO4- solution dropwise from the buret until you get a permanent pink color. Save the solution from the titration because you will use it for the analysis for iron.

Question: What is the oxidation state of iron in your solution after you have completed the analysis for C2O42- ?

Please explain and show the answer. Thanks

Explanation / Answer

K3[Fe(C2O4)3].3H2O is neutral.

Let the oxidation state of Fe is x.

K = +1

C2O4 = -2

3*(+1) + x + 3*(-2) = 0

+3 + x - 6 = 0

x - 3 = 0

x = +3

So, the oxidation state of Fe is +3.

The permanganate reacts with the oxalate, not the iron, so the iron remains at 3+ throughout.

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