Chemistry
posted by Matthias on .
This is a question I am presently doing right now which I found in my homework. I am quite sure that in (a) I have to use the Hasselbach equation though I am not sure how to work it out. If anyone knows any of the answers, and how you got to them, please feel free to share. Any help is greatly appreciated :)
CH3COO (aq) + H2O (l) <==> CH3COOH (aq) + OH (aq)
A 0.01mol dm^3 solution has a pH of 8.87
a. Calculate [H+] and [OH] in the solution
b. Find [CH3COOH] in the solution.
c. Calculate the acid dissociation constant of CH3COOH.
Thanks! :)

a.
pH = 8.87
8.87 = log(H^+)
Solve for (H^+), then
pH + pOH = pKw = 14
You know pH and pKw, solve for pOH and
pOH = log(OH^) which lets you solve for OH.
b.
This is a hydrolysis problem.
You know OH^ from part a. That = (CH3COOH).
c.
Kb for CH3COO^ = (Kw/Ka for CH3COOH)
(Kw/Ka) = (CH3COOH)(OH^)/(CH3COO^)
You know Kw, CH3COOH, OH, and CH3COO^(hat's 0.01 in the problem), solve for Ka.