[Purplepiscean]

The redox reaction: ClO3^2- (aq) + Cl ^- (aq) --> Cl2 (g) + ClO2 (aq) is to be balanced in acid solution using the ion-electron method.
Note: There is an oxidation and a reduction.
Pick pairs where there is a change in oxidation number.

Ps: Not only do I not know how to do this method, but also, I'm really confused about the ClO3^-2!?!?!?! Is there such an ionic compound? I thought it was only ClO3^- but my assignment says otherwise!!! Please help...any help is greatly appreciated!!!! Thank you in advance!!!
Also, what is the oxidation on ClO2?

[Purplepiscean]

Anybody?

[Borek]

I don't think it can be balanced with ClO₃^2-. It can be done starting with ClO₃^-.

[Purplepiscean]

Ok, that's what I thought...so then how do I proceed from there?
I'm unsure of how what the oxidation states of ClO2 is...I don't understand which half-reaction would be an reduction reaction and which half-reaction would be an oxidation reaction and how?
I'm really confused about how to answer which substance is reduced and which substance is oxidized...


Edit: Smileys removed. You do not need to finish your post with 14 smileys.

[AWK]

The redox reaction: ClO3^- (aq) + Cl ^- (aq) --> Cl2 (g) + ClO2 (aq) is to be balanced in acid solution using the ion-electron method.

Yoy should split this reaction into 2 separate reactions:
KClO3 + HCl = KCl + H2O + Cl2
KClO3 + HCl = KCl + H2O + ClO2
balance both reactions, then form linear combinations of both balanced reaction.
For ionic reaction omit spectacor ion (K⁺)

[Borek]

I'm unsure of how what the oxidation states of ClO2 is...I don't understand which half-reaction would be an reduction reaction and which half-reaction would be an oxidation reaction and how?

You don't need to assign oxidation numbers to use half reaction method. Apparently Cl^- -> Cl₂ is an oxidation, so for the reduction you are left with ClO₃^- -> ClO₂.

[Purplepiscean]

    I figured it out yesterday!!! I kept overlooking the simple things!!! THANK YOU SO MUCH FOR YOUR HELP Borek!!!!