Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: MrEQ on December 05, 2021, 09:51:41 AM
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Hey,
I have a problem I'm struggling to solve. There's something fundamental I'm missing here.
The problem asks us to describe how to create a 500ml buffer with a pH of 2.4.
My first problem is that I don't know which compounds to use. I understand that there's some equation we can use whereby the ratio of the concentrations of the two compounds, [Compound1]/[Compound2] = [H+]/Ka.
An example in my book uses acetic acid and sodiumacetate, and demonstrates using HC2H3O2 and C2H3O2-.
If I want to use the same substances, could I do the following?
[HC2H3O2] / [C2H3O2-] = [H+] / Ka.
[H+] for a compound with pH=2.4 is 10-2.4. But what is Ka? Does it vary? The example uses 1.8*10-5, but I'm not sure if this is constant.
Am I on the right track here?
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Ka is an acid dissociation constant - different for every acid.
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My attempt involves Ka = [H+][C2H3O2-] / [HC2H3O2] = 1.8 * 10-5.
If I use this, I get the ratio 10-2.4 / 1.8 * 10-5 ≈ 221, but that seems like an unlikely ratio, right?
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No, the calculated ratio seems to be about right. But for a buffer you need an acid with pKa as close to the buffer pH as possible - that means at pH=2.4 acetic acid is out of the question.
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Thanks for the feedback! Good to know the calculation was somewhat right, albeit a dead end.
I guess I have to choose my compounds better. Any tips?
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Browse pKa tables, see which acids have pKa close to 2.4.