Here's the net ionic equation:
2 MnO4�?/SUP> (aq) + 5 C2O42�?/SUP> (aq) + 16 H+ (aq) ––�?gt; 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l)
Putting in the K+ ions and using H2SO4 as the source of H+ ion, we have
2 KMnO4 (aq) + 5 K2C2O4 (aq) + 8 H2SO4 (aq) ––�?gt; 2 MnSO4 (aq) + 6 K2SO4 (aq) + 10 CO2 (g) + 8 H2O (l)
In acidic solution the oxalate ion would more realistically be in protonated form, H2C2O4. Here is the net ionic equation in this case:
2 MnO4�?/SUP> (aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ––�?gt; 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l)
Or again including the K+ ion and using H2SO4 as the acid, this equation becomes
2 KMnO4 (aq) + 5 H2C2O4 (aq) + 3 H2SO4 (aq) ––�?gt; 2 MnSO4 (aq) + K2SO4 (aq) + 10 CO2 (g) + 8 H2O (l)
For simplicity I assumed that both H+ ions from H2SO4 dissociate (if mainly only the first H+ ion dissociates, we would form hydrogen sulfate ion, HSO4�?/SUP>, and the reactions would be written accordingly. But the ratio of permanganate ion to oxalate ion would still be the same, 2 to 5.)
Also, the water of hydration in the formula of solid K2C2O4 can be omitted since in aqueous solution that water molecule is just another solvent molecule.
Steve
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