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Basic redox reactions

Posted: Tue Feb 26, 2019 6:20 pm
by Maayan Epstein 14B
How do you balance the H+ in a cell when it is basic?
I don't understand how to convert H+ into OH- and balance from there (what order of steps should I take?)

Thank you!

Re: Basic redox reactions

Posted: Tue Feb 26, 2019 6:35 pm
by Tarika Gujral 1K
First balance O with H2O.
Then balance H — add h2o equal to the number of hydrogens and for every h2o, add an oh- on opposite side

So if you have 4 extra hydrogens on one side, add four h2o on opposite side to balance, and add 4 oh- on the original side

Re: Basic redox reactions

Posted: Tue Feb 26, 2019 7:14 pm
by Nicole Lee 4E
In basic redox reactions, you don't balance with H+. You balance with OH-

Re: Basic redox reactions

Posted: Wed Feb 27, 2019 5:49 pm
by Cameron_Greenberg_3C
A basic redox problem will not have H+ ions present. Balancing hydrogens is instead done with H2O and OH-. If the left side of the equation needs, for example, two more hydrogens to be balanced, instead add 2 H2O to the left side and 2 OH- on the right side, resulting in a net gain of only two hydrogens on the left side. H+ is only in acidic redox problems.