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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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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