[Vileblood]

A solution containing 0.1244 g of K2C2O4 was acidified changing the C2O4(2- charge) ions to H2C2O4. The solution was then titrated with 13.93 ml of a KMnO4 solution to reach a faint pink endpoint. In this reaction, the MnO4(-) gets reduced to Mn(2+) and the H2C2O4 gets oxidixed to CO2.
a. write the net ionic equation
b. calculate the molarity of the KMnO4 solution
c. explain why the solution turned pink at the end point of the titration

I'm so confused as to where to even begin with this, but is this the correct balanced equation? K2C2O4 + HMnO4 > KMnO4 + H2C2O4?

[Vileblood]

actually, would it be K2C2O4 + 2HMnO4 > 2KMnO4 + H2C2O4

[sjb]

No, whilst the equation you have written represents the neutralisation at the start, you are told that MnO₄^-  Mn²⁺; and that H₂C₂O₄  CO₂. Can you balance these half equations?