Given 1 M solutions of acetic acid and sodium acetate, and distilled water, describe the preparation...

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Question

Given 1 M solutions of acetic acid and sodium acetate, and distilled water, describe the preparation...

Given 1 M solutions of acetic acid and sodium acetate, and distilled water, describe the preparation of 1 L of 0.1 M acetate buffer at pH = 5.4. The relevant pKa is 4.76.

I know how to solve this problem but i'm having a hard time converting the moles to liters (like the correct set up too use)

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Answer 1

Answer #1

given

pH = 5.4.

pKa is 4.76.

now

pH = pKa +log([A-]/[HA])

[A-] is concentration of base

[HA] is concentration of acid

so

5.4 = 4.76 + log([A-]/[HA])

log([A-]/[HA]) = 0.64

[A-]/[HA] = 4.37

1 L of 0.1 M acetate buffer

here

[A-] is CH3COO-

[HA] is CH3COOH

[CH3COOH] + [CH3COO-] = 0.1M

==>

[CH3COOH] = 0.1 - [CH3COO-]

[CH3COO-]/0.1 - [CH3COO-] = 4.37

solving this gives

[CH3COO-] = 0.08M

[CH3COOH] = 0.1 - 0.08 = 0.02M

1 L 0.1 M acetate buffer is prepared by 0.08 M CH3COO- and 0.02 M CH3COOH with volume of solution 1L

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Answer 2

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