Topic: Buffer solution (Read 3539 times)

suomi · « **on:** September 10, 2011, 05:30:33 PM »

Can anybody help me with this problem? Thanks!

Given 0.1 M solutions of acetic acid and acetate, describe the preparation of 1 L of 0.1 M acetate buffer at a pH of 5.4.

Arkcon · « **Reply #1 on:** September 10, 2011, 07:56:59 PM »

Are you aware of any formulas that you can use to relate concentration to pH for a particular chemical?

suomi · « **Reply #2 on:** September 10, 2011, 11:40:49 PM »

First I thought, I could use the Handelson-Hasselbalch equation, which is

pH= pKa + log (A^-/HAc).

The pKa value of an acetate is 4.76, and the pH should be 5.4.

Since pH= -log[H⁺], I did 10^-5.4 = 3.981*10^-6.

I plugged all those three values in the HH equation, but then I didn't know how I should relate 0.1M of the buffer.

Other equation I thought about was C= n/V, but I am just stuck in the problem and can't see the big picture...

Borek · « **Reply #3 on:** September 11, 2011, 04:18:56 AM »

So far so good.

0.1M buffer means sum of concentrations of acetic acid and acetate is 0.1M.

Topic: Buffer solution (Read 3539 times)

suomi

Buffer solution

Arkcon

Re: Buffer solution

suomi

Re: Buffer solution

Borek

Re: Buffer solution

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