[kevinkevin]

  I'm very uneasy with this reaction because of the acetate ion on the product side.
 
  HClO + HC2H3O2--> Cl2 + H2O + C2H3O2-

  So what I see here is that if I were to do this reaction to completion and then evaporated all the water I would be left with acetate ions.  I don't get it, how could I have acetate ions!  Also will some of the chlorine gas that is produced in this reaction dissolve in the water to produce HCl and more HClO.  I am a bit perplexed by this equation and would love some insight.  Thanks!

  I also thought that equations had to have charged balanced as well as mass.  But since I have been working with basic quantum mechanics math lately and have used equations to solve for electron energies that have been dealing with He+ ions and Li2+ I can easily see why only beginning level chemistry knowledge can easily mislead me.   

[sjb]

  I'm very uneasy with this reaction because of the acetate ion on the product side.
 
  HClO + HC2H3O2--> Cl2 + H2O + C2H3O2-

True enough, but this isn't balanced, there is one chlorine on the left and two on the right...

[kevinkevin]

 Oops your right. 
     
   2HClO + 2HC2H3O2 --> Cl2 + 2H2O + 2C2H3O2-

[Borek]

This equation won't be balanced as it is. As long as you have only negatively charged ions and only on one side of the equation, it is obvious it can't be balanced. Charge must be balanced as well.

[kevinkevin]

  That is exactly what I thought.  But I have seen this equation multiple times so that is why i'm confused.

[Hunter2]

Don't think so. In this equation only hypochlorite is reduced to chlorine. But nothing is oxidized. Beside the missing charges something else is wrong.

[kevinkevin]

  So is there a reaction at all?  Can this equation be modified to be correct?