If you make a buffer with acetic acid and sodium acetate in equimolar amounts, w

Question

If you make a buffer with acetic acid and sodium acetate in equimolar amounts, what happens to the pH when the concentration is adjusted so that there is 10x as much sodium acetate as acetic acid. (Consider what you learned in Parts 1 and 2 of the experiment about which ions are present in water and whether or not these ions undergo hydrolysis.)

a. Not enough information is given to predict the pH change.

b.The pH of the new solution will be the same as that of the original solution.

c. The pH of the new solution will be higher than the original solution.

d. The pH of the new solution will be lower than the original solution. (I originally answered this one but this is wrong)

Explanation / Answer

For equimolar amounts:

pH = 4.75 + log(Acetate/acetic acid)

is Acetate/acetic acid) = 1

then

pH = 4.75 + 0

10x acetate than acid...

so ratio is 1:10

then

pH = pKa + log(Acetate/Acetic acid)

is ratio is 10:1

pH = 4.75 + log(10/1)

so

pH = 4.75+ log(10) = 5.75

Then, the pH is clearly increasing

choose C

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