What is the redox equation you are trying to find the half reactions for?
Your entire question is confusing because of the "it might be this, but" and "or it might be this, but..."
If you can clean up the question I can help.
The correct final equation, which you have written as the last step is correct (if you put the charges on).
2H2O + Zn + 2OH^- ==>Zn(OH)4^-2 + H2
In that total redox equation, one half cell is
Zn ==> Zn^+2 + 2e and the other is
2OH^- + 2e + 2H2O ==> H2 + 4OH^-
my question is about whether I have to add water or just H to firstly balance the second half reaction
which one is correct for a basic solution reaction ?
thanks a lot
Oh I see you answered that, So , it is incorrect to add 2H to balance H2 in a basic solution... ?
Although all the first steps are the same as used in acidic solution?
In basic solution you add OH^- and not H^+. Either will work; e.g., if adding H^+, then you balance the H^+ added with OH^- and it all comes out in the wash.
However, answer on the worksheet or not, I don't buy that the half cell is
2e + 2H2O ==> H2 + 2OH^-
You didn't say what redox equation you are trying to balance. This one comes from
Zn + OH^- --> Zn(OH)4^-2 + H2 and the two half cells are
Zn ==> Zn^+2 + 2e and
OH^- + ....etc.
The point I'm trying to make is that the H2 gas comes from the base (the OH^- in the initial equation) and not from the H2O which is added as a result of the reaction.
thanks a lot
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