I know this question isn't about electrochemical, but the only acid and base section I could find was for 14A.
Somehow I got this question right on the midterm but don't know why or how.
It asks:
At pH 6 what is the net charge for acetic acid, CH3COOH (pKa=4.75)?
What is the concept behind this?
QD3 Midterm
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Re: QD3 Midterm
Since pH is higher than the pKa, the acid will dissociate into its conjugate base and H+, and so its conjugate base will have a charge of -1.
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Re: QD3 Midterm
At the pH of 6 you are assuming that the acetic acid dissolves into a higher concentration of it's conjugate base CHCH3COO- because the pKa (of acetic acid) =4.75 and the conjugate acid has a change of -1.
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Re: QD3 Midterm
You are assuming that acetic acid dissolved into CHCH3COO- and H+ due to the pH of 6.
Re: QD3 Midterm
Acetic acid will lose its proton/H+ because it’s an acid. Its conjugate base is CH3COO which makes its charge -1
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