Balancing Redox EQs

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SarahCoufal_1k
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Balancing Redox EQs

Postby SarahCoufal_1k » Sun Feb 23, 2020 6:26 pm

In the examples in discussion for balancing redox equations it seems like you first add H2Os to balance Oxygens. Can you then add either OH-s or H+s depending on the EQ, or is one preferred over the other?

nehashetty_2G
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Re: Balancing Redox EQs

Postby nehashetty_2G » Sun Feb 23, 2020 6:26 pm

It depends on if the reaction is occurring in an acidic or basic solution. If it is an acidic solution you use H+ and if it is a basic solution you use OH-

Louise Lin 2B
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Re: Balancing Redox EQs

Postby Louise Lin 2B » Sun Feb 23, 2020 6:33 pm

the reaction depends on the molecules involved; if acidic, use H+ and if acidic, use OH-

Andrew F 2L
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Re: Balancing Redox EQs

Postby Andrew F 2L » Sun Feb 23, 2020 7:18 pm

Also to note, for both acidic and basic solutions you can also add water alongside either H+ or OH- depending on the type of solution! This will help to balance Oxygen molecules first!

Anna Chen 1K
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Re: Balancing Redox EQs

Postby Anna Chen 1K » Sun Feb 23, 2020 7:22 pm

If it is an acidic solution, you add H+; if it is a basic solution, you add OH-.

William Francis 2E
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Re: Balancing Redox EQs

Postby William Francis 2E » Sun Feb 23, 2020 7:34 pm

First, you should balance the species being oxidized or reduced in the half reaction. Then, add water to balance oxygen. Then, add H+ to balance hydrogen in acidic solutions. If the reaction is in a basic solution, you add OH- to one side of the half reaction and H2O to the other side to balance hydrogen. This is described in Toolbox 6K.1 on page 538 of the textbook.

Owen-Koetters-4I
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Re: Balancing Redox EQs

Postby Owen-Koetters-4I » Sun Feb 23, 2020 7:35 pm

it depends on the solution. If it is an acidic solution use H+ and if it is a basic solution use OH-

SarahCoufal_1k
Posts: 102
Joined: Thu Jul 25, 2019 12:17 am

Re: Balancing Redox EQs

Postby SarahCoufal_1k » Sun Feb 23, 2020 11:12 pm

William Francis 2E wrote:First, you should balance the species being oxidized or reduced in the half reaction. Then, add water to balance oxygen. Then, add H+ to balance hydrogen in acidic solutions. If the reaction is in a basic solution, you add OH- to one side of the half reaction and H2O to the other side to balance hydrogen. This is described in Toolbox 6K.1 on page 538 of the textbook.


thank you!!

Joanne Lee 1J
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Re: Balancing Redox EQs

Postby Joanne Lee 1J » Mon Feb 24, 2020 12:28 pm

It depends on the solution; if it is acidic add H+ and if basic then add OH-.

charleejohnson1L
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Re: Balancing Redox EQs

Postby charleejohnson1L » Mon Feb 24, 2020 1:11 pm

the biggest thing that helped me with this was like, explicitly realizing that you can only add what's in the reaction to your equations. so like in acidic solution, the only things in the solution except for your redox reaction is water and hydrogen ions and in a basic solution, the only things in the solutions except for your redox reaction is water and hydroxide ions. I hope this helps :)

Aarushi Solanki 4F
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Re: Balancing Redox EQs

Postby Aarushi Solanki 4F » Mon Feb 24, 2020 2:23 pm

If it's an acidic solution, you add H+ ions to balance the H's. If it's a basic solution, you add H2O and OH- ions to opposite sides to the equation in equal moles to balance the H's.


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