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19 Nov 2019

You want to make 150 mL of 0.20 M acetic buffer with pH= 4.5. You are given a stock of 1.0 M acetic acid and a bottle of solid sodium acetate salt (MW= 82 g/mol). The formula for this dissociation of acetic acid is shown here.
CH3COOH <----> CH3COO- + H pKa= 4.75

1. What is the ratio of [A]/ [HA] when your buffer pH = 4.75?

2. Determine the concentrations of weak acid and conjugate base in the buffer.

3. How many mL of 1.0 M acetic acid will you need?

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Collen VonLv2

30 Mar 2019

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Related questions

A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acid-conjugate base or weak base-conjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH?

0.01 M acetic acid/0.01 M sodium acetate

0.1 M acetic acid/0.1 M sodium acetate

1.0 M acetic acid/1.0 M sodium acetate

magentamammoth658

A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acid–conjugate base or weak base–conjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH?

0.01 M acetic acid/0.01 M sodium acetate

0.1 M acetic acid/0.1 M sodium acetate

1.0 M acetic acid/1.0 M sodium acetate

pucehamster19

CH₃COOH <-------> CH₃COO^- + H⁺

Prepared 200 ml of 0.1 M sodium acetate solution using acetic acid (1.74M, 11.493 mL) and sodium acetate (1.641g).

Prepated 200 mL of 0.1 M acetic acid solution using the stock 1.74M acetic acid solution (11.494 mL).

testing buffer capacity of solutions

Used teh acetic acid and sodium acetate soltuions containing the volumes below:

	1	2	3	4	5	6	7
Acetic Acid	18 mL	15 mL	12 mL	9 mL	6 mL	3 mL	0 mL
Acetate	0 mL	3 mL	6 mL	9 ml	12 mL	15 mL	18 mL
Buffer pH	3.27	4.14	4.45	4.73	5.01	5.39	7.41
pH with HCl	2.65	3.63	4.22	4.51	4.79	5.13	5.69
pH with NaOH	4.04	4.43	4.74	4.96	5.35	6.09	11.54

From the inital pH and ratio of weak acid to base, calculate the pK_a of acetic acid using teh Henderson-Hasselbalch equation for all the effective buffering solutions and average th?e values. How does this compare to the actual pK_a of acetic acid of 4.76? (Please show step-by-step process)

What is the observed effective pH buffering range for inital acetate buffers?

Which mixtures of acetate buffer resist pH changes to BOTH HCl and NaOH? How did you decide? Which would be the best buffer solution against added acid and base? Why?

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