How many moles of oxalic acid (C2H2O4) is oxidised by one mole of potassium manganate (KMnO4), in an acidic medium?
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Answers
Explanation:
We had a titration of oxalic acid vs. potassium permanganate for an experiment in which we used concentrated H2SO4.
Actually, the reaction requires an acidic medium i.e. H+ is involved as a reactant... I suppose the H+ released by the oxalic acid would be enough since you are studying the rate of the reaction though I am not sure.
The balanced ionic equation is: 2MnO4−+5H2C2O4+6H+⟶2Mn2++10CO2+8H2O
As you can see, H+ is involved as a reactant and that is why you might have read that conc.H2SO4 is necessary.
Answer:
1 mole
Reduction Half reaction:- MnO4– + 8H+ + 5e– → Mn2+ + 4H2O
Oxidation Half reaction:- C2H42- → 2CO2 + 2e–
Overall Ionic reaction:- 2MnO4– + 16H+ + 5C2H42- → 2Mn2+ + 10CO2 + 8H2O
This titration cannot be carried out in the presence of acids like nitric acid or hydrochloric acid because itself is an oxidising agent. So hydrochloric acid chemically reacts with KMnO4 solution forming chlorine which is also
an oxidising agent.
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