Investigating K3Fe(C2O4)3.3H2O Synthesis

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SUMMARY

The synthesis of K3Fe(C2O4)3.3H2O involves two main steps: first, the reaction of Iron(II) ammonium sulfate (Fe(NH4)2(SO4)2.6H2O) with oxalic acid dihydrate to produce Iron(II) oxalate precipitate, followed by oxidation of this precipitate using hydrogen peroxide (H2O2) and potassium oxalate (K2C2O4). The discussion raises a critical observation regarding gas evolution during the second step, suggesting that carbon dioxide (CO2) is released due to the oxidation of oxalate, rather than oxygen. This indicates a need for clarity in the chemical equations provided in lab resources, particularly concerning the oxidation of oxalate and gas release.

PREREQUISITES
  • Understanding of chemical synthesis processes
  • Knowledge of redox reactions, specifically involving iron and oxalate
  • Familiarity with the properties and reactions of hydrogen peroxide
  • Basic grasp of stoichiometry in chemical equations
NEXT STEPS
  • Research the mechanism of Iron(II) to Iron(III) oxidation reactions
  • Investigate the role of hydrogen peroxide in organic oxidation reactions
  • Learn about the decomposition of oxalate in redox reactions
  • Examine the gas evolution in chemical reactions and its implications
USEFUL FOR

Chemistry students, laboratory technicians, and educators involved in chemical synthesis and redox reaction studies will benefit from this discussion.

z89
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Actually this is a part of homework. I've found the answer, but I have some problems.

The lab I did in previous lesson is the preparation of K3Fe(C2O4)3.3H2O from Fe(NH4)2(SO4)2.6H2O

In the first step, Iron(II) ammonium sulphate was reacted with oxalic acid dihydrate to form Iron(II) oxalate precipitate.

In the second step, Iron(II) oxalate was oxidized to potassium trioxalatoferrate(III) K3Fe(C2O4)3 by addition of H2O2 and K2C2O4.

In fact, I found link(s) talking about the lab

http://www.chem.umass.edu/genchem/chem112/112_Experiment_1.htm

but I was a bit doubt about the equation mentioned. I observed that there was bubbles formed/gas evolving in step 2. I believed that this is not oxygen, since Fe2+ is oxidized to Fe3+ in this process, H2O2(O: -1 in ON) cannot be oxidized to O2(O: 0) in the same time.
Therefore, it should be CO2, which was oxidized from oxalate, am I right?

And then, why the equation did not mention the oxidization of oxalate... even the release of gas

of course, this problem didn't affect the calculation process. I am just curious ..
Thanks.
 
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I've known iron salts to catalytically decompose hydrogen peroxide into water and oxygen. Was the peroxide present in excess?
 
yes, thanks for your reminder:biggrin:

but, is the reaction between oxalate and H2O2 favourable?
 

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