4. Use the following steps to determine how to make 600 mL of a 0.1M acetate buffer, pH 5.0, using 0.1M acetic acid and 0.1M sodium acetate. a. Consider the Henderson-Hasselbalch equation. pH=pKa + log [base] [acid] Using the desired pH (5.0) and pKą of acetic acid, use the Henderson Hasselbach equation to determine a ratio of [base] [acid] required for this buffer. (For example, your answer should look something like this: [base] [acid] = 2.3 Note that this is NOT the ratio you will obtain - it is just an example) b. Given the example above, we can set [acid] = x and [base] =2.3x. Remember that the concentration of acid and base should equal the desired molarity, which 0.1. Based on this, a second equation can be obtained - given the example above, the equation would. be x + 2.3x = 0.1. Use this to solve for x, which represents the concentration of acid. ([acid]), and for [base].

4. Use the following steps to determine how to make 600 mL of a 0.1M acetate buffer, pH 5.0, using 0.1M acetic acid and 0.1M sodium acetate. a. Consider the Henderson-Hasselbalch equation. pH=pKa + log [base] [acid] Using the desired pH (5.0) and pKą of acetic acid, use the Henderson Hasselbach equation to determine a ratio of [base] [acid] required for this buffer. (For example, your answer should look something like this: [base] [acid] = 2.3 Note that this is NOT the ratio you will obtain - it is just an example) b. Given the example above, we can set [acid] = x and [base] =2.3x. Remember that the concentration of acid and base should equal the desired molarity, which 0.1. Based on this, a second equation can be obtained - given the example above, the equation would. be x + 2.3x = 0.1. Use this to solve for x, which represents the concentration of acid. ([acid]), and for [base].

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 14Q: Consider the following pH curves for 100.0 mL of two different acids with the same initial...

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Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.) a. Calculate the pH of this solution. b. Calculate the pH after 0.10 mole of HCl has been added to the original solution. Assume no volume change on addition of HCl. c. Calculate the pH after 0.20 mole of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.
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2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
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