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Problem: Titration of an acidic solution of Na2C2O4 with KMnO4(aq). The balanced chemical equation for this reaction is: 16 H+(aq) + 2 MnO4-(aq) + 5 C2O42-(aq)  →  2 Mn2+(aq) + 8 H2O(l) + 10 CO2(g) Which species is the reducing agent?

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Problem Details

Titration of an acidic solution of Na2C2O4 with KMnO4(aq).

Photographs show a reaction of MnO4- with C2O42 -. a) A beaker contains a colorless solution of C2O42- (aqueous).  MnO4- (aqueous), which appears purple, is slowly added to the beaker.  The purple color of MnO4- disappears immediately as the reaction with C2O42- occurs. b) The solution in the beaker appears entirely purple. The purple color of MnO4- remains because C2O42- is completely consumed.

The balanced chemical equation for this reaction is:

16 H+(aq) + 2 MnO4-(aq) + 5 C2O42-(aq)  →  2 Mn2+(aq) + 8 H2O(l) + 10 CO2(g)

Which species is the reducing agent?

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Our tutors have indicated that to solve this problem you will need to apply the Redox Reactions concept. If you need more Redox Reactions practice, you can also practice Redox Reactions practice problems.