Ka and Kb

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Angela Patel 2J
Posts: 110
Joined: Sat Aug 24, 2019 12:17 am

Ka and Kb

Postby Angela Patel 2J » Wed Jan 15, 2020 10:50 pm

Are Ka and Kb calculated differently?

nehashetty_2G
Posts: 102
Joined: Thu Jul 25, 2019 12:15 am

Re: Ka and Kb

Postby nehashetty_2G » Wed Jan 15, 2020 10:57 pm

No, the B versus the A subscript are just indicative of whether the reaction is an acid or base.

Matt Sanruk 2H
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Joined: Wed Sep 18, 2019 12:21 am

Re: Ka and Kb

Postby Matt Sanruk 2H » Wed Jan 15, 2020 11:03 pm

It is similar to the relationship between pOH and pH

Angela Patel 2J
Posts: 110
Joined: Sat Aug 24, 2019 12:17 am

Re: Ka and Kb

Postby Angela Patel 2J » Thu Jan 16, 2020 10:46 am

So Ka would be calculated for a compound by studying its equilibrium concentrations as if it were an acid, and Kb would be calculated for the conjugate base of that acid and its reaction is what I'm getting. Like the example with NH3 and NH4+ we did in lecture.

EvanWang
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Joined: Sat Sep 07, 2019 12:16 am

Re: Ka and Kb

Postby EvanWang » Thu Jan 16, 2020 11:27 am

KB and KA are calculated the same way. From what I gathered from the lecture, KB has to do with the equilibrium constant of bases and has [OH-] as a product. Conversely, KA has to do with the equilibrium constant of acids and has [H3O+] as a product. That's the extent to how much they differ.

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

Re: Ka and Kb

Postby Suraj Doshi 2G » Thu Jan 16, 2020 11:30 am

They are calculated similarily in that they both use the [products]/[reactants] ratio. The difference is that for Kb you need to have the [OH-] in the numerator and for Ka you need to have [H30+] in the numerator.


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