- #1

alr1014

- 7

- 1

## Homework Statement

You need to produce a buffer solution that has a pH of 5.70. You already have a solution that contains 0.0200 moles of acetic acid. Using the Henderson-Hasselbalch equation calculate the moles of sodium acetate needed to create a buffer with the desired pH? The Ka of acetic acid is 1.8 × 10^-5.

## Homework Equations

pKa = -log (Ka)

pH= pKa + log (base / acid)

## The Attempt at a Solution

pKa= -log (1.8 × 10^-5) = 4.74

5.70 = 4.74 + log (base/acid)

Unfortunately, I have been staring at this problem for about an hour and am unsure how to find the concentration of the acid to discover the consent ration of the base. I am not sure how to proceed since the problem does not give a volume to find the molarity.

Any help with this would be greatly appreciated!