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Topic: Calculating the pH of a Buffer Solution  (Read 2747 times)

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Offline jakebvt

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Calculating the pH of a Buffer Solution
« on: March 31, 2015, 09:25:33 AM »
Calculate the pH of a buffer solution that is 0.100 M in HC2H3O2 and 0.100 M in NaC2H3O2
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Offline sjb

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Re: Calculating the pH of a Buffer Solution
« Reply #1 on: March 31, 2015, 09:38:52 AM »
Quote from: jakebvt on March 31, 2015, 09:25:33 AM
Calculate the pH of a buffer solution that is 0.100 M in CH3CO2H and 0.100 M in CH3CO2Na

Do you know any equations that may help? Please make an effort to solve the question.
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Offline jakebvt

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Re: Calculating the pH of a Buffer Solution
« Reply #2 on: March 31, 2015, 10:22:15 AM »
I think you're supposed to make an ICE table or something.
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Offline Babcock_Hall

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Re: Calculating the pH of a Buffer Solution
« Reply #3 on: March 31, 2015, 10:55:42 AM »
An ICE table is appropriate when a reaction has occurred.  Can you define what a buffer is for us?
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Offline Borek

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Re: Calculating the pH of a Buffer Solution
« Reply #4 on: March 31, 2015, 11:58:54 AM »
Quote from: jakebvt on March 31, 2015, 10:22:15 AM
I think you're supposed to make an ICE table or something.

Try.

While that wouldn't be my favorite approach, if done correctly it should definitely lead to a correct answer.
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Offline emk4630

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Re: Calculating the pH of a Buffer Solution
« Reply #5 on: April 07, 2015, 10:28:59 PM »
i could be wrong because im only in AP chem but you could use the henderson smallbach equation because they are conjugate acid bases in solution.
pH=pKa + log.1/.1
or just pH=pKa
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Offline Borek

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Re: Calculating the pH of a Buffer Solution
« Reply #6 on: April 08, 2015, 03:56:48 AM »
Definitely Henderson-Hasselbalch equation is the simplest approach. But it is not the only one, and trying to find the answer with the ICE table (http://www.chembuddy.com/?left=buffers&right=with-ICE-table) has some educational value.
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