Henderson Hasselbalch's equation

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Alexis Cooke 4G
Posts: 6
Joined: Fri Sep 25, 2015 3:00 am

Henderson Hasselbalch's equation

Postby Alexis Cooke 4G » Sat Dec 05, 2015 1:28 pm

I know that you can always use Henderson Hasselbalch's equation when doing buffer problems, but when is it acceptable to use in a titration problem? (i.e. strong acid-strong base, strong acid-weak base, etc.)

Matt Jacobs 3H
Posts: 32
Joined: Fri Sep 25, 2015 3:00 am

Re: Henderson Hasselbalch's equation

Postby Matt Jacobs 3H » Sat Dec 05, 2015 1:39 pm

You can always use the Henderson-Hasselbalch when a buffer problem shows up in a titration calculation, i.e. when you know the concentration of a weak acid and it's conjugate base, or the concentration of a weak base and its conjugate acid. You usually have the Pka already, or you can find it by taking the -log of the Ka value. Then you can find your pH. This will save a lot more time than drawing out another I.C.E. table and trying to find the concentration of H3O+ or -OH.

Aliya Habib 1L
Posts: 20
Joined: Fri Sep 25, 2015 3:00 am

Re: Henderson Hasselbalch's equation

Postby Aliya Habib 1L » Sat Dec 05, 2015 8:16 pm

From my discussion notes if the Percent Dissociation is less than 5% then you can use it. Or you can use the equation whenever x is negligible (when is disappears).


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