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Calculate the ratio of "acetic / acetate" concentrations that must exist in a buffer solution of...

Calculate the ratio of "acetic / acetate" concentrations that must exist in a buffer solution of pH = 5.00. Deduce the pH change that will occur if one liter of the previous solution, which is 0.10 M in acetic, is added 50 ml of 1.00 M HCl.
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Answer #2

Ka of acetic acid = 1.80 x 10-5

pKa of acetic acid = -log(Ka) = -log(1.80 x 10-5) = 4.74

According to Henderson-Hasselbach equation,

pH = pKa + log([conjugate base] / [acid])

where [conjugate base] = concentration of conjugate base = concentration of acetate

[acid] = concentration of acid = concentration of acetic acid

pKa = 4.74

pH = 5.00

substituting the values,

5.00 = 4.74 + log([acetate] / [acetic acid])

log([acetate] / [acetic acid]) = 5.00 - 4.74 = 0.26

[acetate] / [acetic acid] = 100.26

[acetate] / [acetic acid] = 1.80

answered by: anonymous
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