What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.6?Note that the concentration, pH value, or both may differ from that in the first question.%3DStrategy1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A–/[HA].2. Use the mole fraction of acetate to calculate the concentration of acetate.3. Calculate the concentration of acetic acid.Step 1: The ratio of base to acid is lacetate][acetic acid]= 0.69. That is, there are 0.69 molecules of acetate for each molecule ofacetic acid.Step 2: Use the mole fraction of acetate to calculate the concentration of acetate.[acetate] =

We would use Henderson Hasselbalch equation to calculate the concentration of acetate.

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.6? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A-1/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1: The ratio of base to acid is [acetate] [acetic acid] 0.69. That is, there are 0.69 molecules of acetate for each molecule of acetic acid. Step 2: Use the mole fraction of acetate to calculate the concentration of acetate. [acetate] = %3D M

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.6? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A-1/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1: The ratio of base to acid is [acetate] [acetic acid] 0.69. That is, there are 0.69 molecules of acetate for each molecule of acetic acid. Step 2: Use the mole fraction of acetate to calculate the concentration of acetate. [acetate] = %3D M

Chemistry

10th Edition

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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Question

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.6?
Note that the concentration, pH value, or both may differ from that in the first question.
%3D
Strategy
1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A–/[HA].
2. Use the mole fraction of acetate to calculate the concentration of acetate.
3. Calculate the concentration of acetic acid.
Step 1: The ratio of base to acid is lacetate]
[acetic acid]
= 0.69. That is, there are 0.69 molecules of acetate for each molecule of
acetic acid.
Step 2: Use the mole fraction of acetate to calculate the concentration of acetate.
[acetate] =

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