b. A buffer solution consisting of equal parts base and conjugate acid is required. The buffer should have [B] = [HB*] = 0.0500 M with a volume of 500 mL. Describe two ways that you can prepare this buffer. The first should combine the base with the salt of the conjugate acid (figure out the volumes and masses you need and the appropriate concentrations to use). The second should add the appropriate amount of strong acid to the weak base to create the buffer (again, figure out the volumes and concentrations needed).
b. A buffer solution consisting of equal parts base and conjugate acid is required. The buffer should have [B] = [HB*] = 0.0500 M with a volume of 500 mL. Describe two ways that you can prepare this buffer. The first should combine the base with the salt of the conjugate acid (figure out the volumes and masses you need and the appropriate concentrations to use). The second should add the appropriate amount of strong acid to the weak base to create the buffer (again, figure out the volumes and concentrations needed).
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![b. A buffer solution consisting of equal parts base and conjugate acid is required. The buffer should have [B] = [HB*] =
0.0500 M with a volume of 500 mL. Describe two ways that you can prepare this buffer. The first should combine
the base with the salt of the conjugate acid (figure out the volumes and masses you need and the appropriate
concentrations to use). The second should add the appropriate amount of strong acid to the weak base to create
the buffer (again, figure out the volumes and concentrations needed).
c. Using the buffer from part b where [B] = [HB+] = 0.0500 M in 500 mL, find the pH of the buffer when:
8.0 mL of a 1.0 M HCI solution is added
i.
ii.
10.0 mL of a 0.650 M NaOH solution is added
d. How much of the 1.0 M HCI would need to be added to exceed the buffering capacity?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b0e7686-0c0d-4eba-ac81-54e736b47f2f%2F78d6e651-1f55-450a-8556-57fadacc575b%2Ful7r9nv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:b. A buffer solution consisting of equal parts base and conjugate acid is required. The buffer should have [B] = [HB*] =
0.0500 M with a volume of 500 mL. Describe two ways that you can prepare this buffer. The first should combine
the base with the salt of the conjugate acid (figure out the volumes and masses you need and the appropriate
concentrations to use). The second should add the appropriate amount of strong acid to the weak base to create
the buffer (again, figure out the volumes and concentrations needed).
c. Using the buffer from part b where [B] = [HB+] = 0.0500 M in 500 mL, find the pH of the buffer when:
8.0 mL of a 1.0 M HCI solution is added
i.
ii.
10.0 mL of a 0.650 M NaOH solution is added
d. How much of the 1.0 M HCI would need to be added to exceed the buffering capacity?
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