## Basic and Acidic Conditions

Ryan_K_1K
Posts: 51
Joined: Wed Nov 14, 2018 12:18 am

### Basic and Acidic Conditions

What is the difference between balancing a half-reaction "under basic conditions" and balancing one "under acidic conditions?"

JonathanS 1H
Posts: 101
Joined: Thu Jul 11, 2019 12:17 am

### Re: Basic and Acidic Conditions

Under acidic conditions, we use the H+ ions while balancing the equation. Under basic conditions, we use the H+ initially, but balance the charge with H20 and OH- in order to have the reaction in a basic environment.

Alex Tchekanov Dis 2k
Posts: 118
Joined: Sat Aug 24, 2019 12:16 am

### Re: Basic and Acidic Conditions

The way I was taught was to solve both the same way as if under acid conditions and then for the basic conditions after you've solved it then you add an equivalent amount of OH- to both sides as there are H+. Thus, when you have for example 6OH- and 6H+ on one side it will create 6H20.

Ashley Nguyen 2L
Posts: 103
Joined: Sat Aug 17, 2019 12:18 am
Been upvoted: 1 time

### Re: Basic and Acidic Conditions

When balancing a reaction in an acidic solution, balance the equations by using H3O+ and H2O. If in a basic solution, balance by using OH- and H2O. Everything else will remain the same.

Posts: 74
Joined: Fri Sep 28, 2018 12:29 am

### Re: Basic and Acidic Conditions

It makes sense to balance the H+ by adding OH- because we are in basic conditions. By leaving the H+ ions we are saying the solution is acidic

Elizabeth Bowen 1J
Posts: 53
Joined: Wed Nov 14, 2018 12:20 am

### Re: Basic and Acidic Conditions

Yes, do what the other responses have said. What I've been told is that it's good not to think of Basic and Acidic Conditions as being too different, the procedure is exactly the same except for that one extra step.