Balancing Redox Reactions

[Renee Grange 1I]

When do we need to cancel H+ with OH- when balancing redox reactions?

[Long Luong 2H]

When balancing redox reactions under basic conditions.

[J Medina 2I]

What are basic conditions?

[Michelle Song 1I]

What are basic conditions?

Conditions where the pH is above 7

[Sam McNeill 1E]

I think the question will specify what the conditions are, and for basic conditions you use the exact same steps as acidic condition, but at the end balance out H+ with OH-.

[Brianna Becerra 1B]

This is done under basic conditions. In order to balance the oxygen, you add needed H20 to the necessary side. This often result in a surplus of Hydrogen on one side causing H20 to be added to the other side, along with OH- in order to cancel out the added oxygen. It differs from acidic conditions as you follow the first step of adding H20 to the necessary side, however on the other side to balance the Hydrogen, you can add H+.

[charleejohnson1L]

you can cancel the H+ and OH- ions when you're combining your redox half reactions and making the final full reaction equation. after you're done balancing the two, you flip one of them, most of the time you flip the oxidation half reaction, and then some things will cancel and some won't. you add H+ when the redox reaction takes place in an acidic solution, and OH- when the redox takes place in a basic solution. I hope this helps. :)

[ABombino_2J]

Only cancel the H+ with OH- when it says to balance the equation in basic solution.