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You have a 100.0-ml buffer solution that is 1.0M acetic acid (K, = 1.77 x 10-5). and 2.OM sodium acetate. Use this to answer the next 3 questions. 4. What is the pH of the buffer prepared? a. 4.75 b. 4.50 c. 9.50 d. 5.05 Based on the description of the buffer which of the following is true? a. It has a greater resistance to changes in pH from the addition of acids than bases. b. It has a greater resistance to changes in pH from the addition of bases than acids. C. It has an equal resistance to changes in pH from the addition of acids or bases. d. It is not a buffer because acetic acid is a strong acid 0.0mL of 6.0M HCl is added to the solution what is the resulting pH. a. 4.75

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Answer:

1. d. 5,05

2. a. It has a greater resistance to changes in pH from the addition of acids than bases.

3. The addition of 0.0mL of 6.0M HCl will not change the pH.

Explanation:

To know the pH of the buffer you need to use Henderson-Hasselbalch formula:

pH = pka + logā‚ā‚€ [tex]\frac{[A^-]}{[HA]}[/tex]

Where pka is -logā‚ā‚€ K,. Thus, pka = 4,75

[Aā»] is concentration of acetate: 2,0 M

[HA] is acetic acid concentration: 1,0 M

Thus, pH of this buffer is: 5,05

The range of work in a buffer is pka Ā± 1. As the buffer has a pH higher than pka -more basic- will has a greater resistance to changes in pH from the addition of acids than bases.

The addition of 0.0mL of 6.0M HCl will not change the pH.

I hope it helps!

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