OH vs H

Moderators: Chem_Mod, Chem_Admin

Sophia Dinh 1D
Posts: 100
Joined: Thu Jul 25, 2019 12:15 am

OH vs H

Postby Sophia Dinh 1D » Fri Mar 13, 2020 2:26 am

Can you ever use H+ to balance the equation in a basic solution?

Hannah Romeo 1J
Posts: 58
Joined: Thu Jul 11, 2019 12:16 am

Re: OH vs H

Postby Hannah Romeo 1J » Fri Mar 13, 2020 4:36 am

No because H+ is only used in acidic solutions.

005324438
Posts: 51
Joined: Sat Aug 24, 2019 12:16 am

Re: OH vs H

Postby 005324438 » Fri Mar 13, 2020 10:32 am

H+ is used to balance acidic solutions, OH- is used to balance basic solutions. One can't be used for the other because there is no concentration to use, and that form of the reaction is highly unlikely to happen.

Asha Agarwal 1E
Posts: 51
Joined: Fri Aug 30, 2019 12:16 am

Re: OH vs H

Postby Asha Agarwal 1E » Fri Mar 13, 2020 10:36 am

You have to as balancing in a basic solution requires the same steps as balancing in an acidic solution, however, at the end you have to neutralize the H+ with OH- for a basic solution.

Pablo 1K
Posts: 118
Joined: Sat Feb 02, 2019 12:15 am

Re: OH vs H

Postby Pablo 1K » Fri Mar 13, 2020 10:47 am

No since fundamentally, H+ would make a solution more acidic and in a basic equation, you have more OH- so OH- would be utilized to balance only in basic solutions.

Suraj Doshi 2G
Posts: 100
Joined: Fri Aug 02, 2019 12:15 am

Re: OH vs H

Postby Suraj Doshi 2G » Fri Mar 13, 2020 10:50 am

We can't use H+ to balance an equation in basic solutions as adding H+ would decrease pH (Making the solution overall more acidic) and therefore messing up the equation. To balance an equation in basic solution we would have to use OH- and then add waters to the other side to balance everything out.

Simon Dionson 4I
Posts: 107
Joined: Sat Sep 14, 2019 12:17 am

Re: OH vs H

Postby Simon Dionson 4I » Sat Mar 14, 2020 12:15 am

I actually use H+ to help balance my basic equations, except an extra step would have to be taken.

When I have H+, I convert that to OH- by adding OH- to both sides. H+ and OH- neutralize to H2O so H+ never appears in my final equation

I learned this method in this video: https://www.youtube.com/watch?v=v5sDNmYCaqo

I recommend watching after 1 minute.

KnarGeghamyan1B
Posts: 102
Joined: Fri Aug 09, 2019 12:15 am

Re: OH vs H

Postby KnarGeghamyan1B » Sat Mar 14, 2020 1:15 am

If it's a basic solution, there's a trick that usually works. First balance the H+ by placing H2O on the opposite side, then balance the original side by adding twice the molecules of H2O, and finally add the doubles coefficient of OH to the other side to balance the additional atoms you added. The waters should reduce and you are left with no H+.

Madelyn Romberg 1H
Posts: 102
Joined: Tue Oct 02, 2018 12:16 am

Re: OH vs H

Postby Madelyn Romberg 1H » Sat Mar 14, 2020 10:07 am

In basic solutions, H+ is not readily available. To balance H, you add h20 to one side and then oh- to the other. This is essentially adding an H+ in a different manner.

KSong_1J
Posts: 101
Joined: Thu Jul 11, 2019 12:17 am

Re: OH vs H

Postby KSong_1J » Sat Mar 14, 2020 10:14 am

No, you would use OH- to balance basic solutions instead of H+. However, you do use H2O for balancing in both acidic and basic solutions

205291012
Posts: 50
Joined: Mon Nov 11, 2019 12:17 am

Re: OH vs H

Postby 205291012 » Sat Mar 14, 2020 3:59 pm

I would stick to balancing basic solutions with OH- and acidic with H+.

Nohemi Garcia 1L
Posts: 103
Joined: Fri Aug 02, 2019 12:15 am

Re: OH vs H

Postby Nohemi Garcia 1L » Sat Mar 14, 2020 4:03 pm

No, it's never used for balancing in an acidic solution.

ValerieChavarin 4F
Posts: 99
Joined: Wed Sep 18, 2019 12:18 am

Re: OH vs H

Postby ValerieChavarin 4F » Sun Mar 15, 2020 7:26 am

No, H+ is only used to balance a redox rxn in acidic conditions. In the case of a basic solution, you MUST use OH^-


Return to “Balancing Redox Reactions”

Who is online

Users browsing this forum: No registered users and 2 guests