[murmelburmel]

(Basic medium!) My idea so far:

SO₃^2- + H₂O₂  SO₄^2- + H₂O

Oxidation: SO3^2- + 2OH^-  SO4^2- + H2O +2e^-

Reduction: H2O2 H2O
...and here is the problem. I don't get the two sides balanced with OH^- and H2O. Probably something really simple I'm missing but just can't figure it out.

[Babcock_Hall]

You have not clearly stated what the question is and how much information you were given; therefore, it is difficult to tell what the question is vs. what is your work.  Your reduction half-cell does not show any electrons.

[murmelburmel]

Sorry, I thought it was clear from the headline. The task is letting SO3 react with H2O2. We are not given a product. I thought SO4 and H2O would be the most likely so that's what I went with. I didn't add electrons because I learned to do those last. The problem is I don't get the atoms equal on both sides. Is H2O even right as the product of that reduction?

[sjb]

Is SO₃ sulfite (sulfate(IV) if you must) or sulfur trioxide? You use both which might be where the confusion is arising? As it is SO₃^2- + H₂O₂  SO₄^2- + H₂O is balanced....

[AWK]

https://www.wikiwand.com/en/Peroxymonosulfuric_acid

[murmelburmel]

Is SO₃ sulfite (sulfate(IV) if you must) or sulfur trioxide? You use both which might be where the confusion is arising? As it is SO₃^2- + H₂O₂  SO₄^2- + H₂O is balanced....

Thank you. It's all supposed to be sulfite, just left the charge out when replying (which yes, it looks confusing reading it again).

What about the problem with the reduction part? Any idea why I can't get the atoms balanced on both sides?