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Phosphate Buffer [Conjugate Base] [Weak Acid] pH pH after NaOH was added 6.2 7.2 8.2

Phosphate Buffer [Conjugate Base] [Weak Acid] pH pH after NaOH was added 6.2 7.2 8.2

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...
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The data shows from the first pic and the table for Case 1 and 2 is the answer that needs to be filled out.

B. Factors affecting buffer capacity You will be considering the buffer system, phosphate buffer H:PO, ========== HPO. + Or more appropriately written as: H;PO. + H,0 HPO. + H,O 1. Effect of concentration of buffer (your instructor will tell you which of the two cases and corresponding concentrations you will prepare). CASE1. Using 0.1 M phosphate buffer, pH 7.2, prepare 25ml each of the buffer solutions with the following concentrations at pH 7.2: 1. 0.005 M 2. 0.05 M 3. 0.10 M CASE 2. Using 0.1 Macetate buffer, pH 4.7, prepare 25 ml each of the buffer solutions with the following concentrations at pH 4.7: Record the pH of each of the buffer solutions. Add 2 ml of 0.1 M N2OH to each of the 25 ml buffer samples assigned to your group. Record the pH of each buffer solution after the addition of alkali. Account for the magnitude of the change in pH. 2. Effect of the ratio of the conjugate base to the weak acid. CASE 1. From the Henderson-Hasselbach equation, calculate the ratio of dihydrogen phosphate (H;PO.) and monohydrogen phosphate (HPO.") components required to produce buffer solution with 1. рH6.2 2. pH 7.2 3. рH8.2 CASE 2. From the Henderson-Hasselbach equation, calculate the ratio of acetic acid and acetate required to produce buffer solution with Page 6of 10 Vision: Mission: A globally competitive univenity for science, technology, and environmental conservation. Development of a highly competitive human resource, cutting-edge scientific knouledge and insovative technologies for suitainable communities and environment. TP-IMD-04 For instructional purposes only • 1" Semester SY 2020-2021 1. рH 3.7 2. pH 4.7 3. рH 5.7 Using the stock solution provided to you, make 25 ml of each of the buffer solutions assigned to you. Measure and record the pH of each of the buffer solutions. Add 2 ml of 0.1 M NAOH to each of the 25 ml buffer solutions. Record the pH of each buffer solution after addition of alkali. Account for the magnitude of pH shift in each with reference to the direction of pH shift.
Transcribed Image Text:B. Factors affecting buffer capacity You will be considering the buffer system, phosphate buffer H:PO, ========== HPO. + Or more appropriately written as: H;PO. + H,0 HPO. + H,O 1. Effect of concentration of buffer (your instructor will tell you which of the two cases and corresponding concentrations you will prepare). CASE1. Using 0.1 M phosphate buffer, pH 7.2, prepare 25ml each of the buffer solutions with the following concentrations at pH 7.2: 1. 0.005 M 2. 0.05 M 3. 0.10 M CASE 2. Using 0.1 Macetate buffer, pH 4.7, prepare 25 ml each of the buffer solutions with the following concentrations at pH 4.7: Record the pH of each of the buffer solutions. Add 2 ml of 0.1 M N2OH to each of the 25 ml buffer samples assigned to your group. Record the pH of each buffer solution after the addition of alkali. Account for the magnitude of the change in pH. 2. Effect of the ratio of the conjugate base to the weak acid. CASE 1. From the Henderson-Hasselbach equation, calculate the ratio of dihydrogen phosphate (H;PO.) and monohydrogen phosphate (HPO.") components required to produce buffer solution with 1. рH6.2 2. pH 7.2 3. рH8.2 CASE 2. From the Henderson-Hasselbach equation, calculate the ratio of acetic acid and acetate required to produce buffer solution with Page 6of 10 Vision: Mission: A globally competitive univenity for science, technology, and environmental conservation. Development of a highly competitive human resource, cutting-edge scientific knouledge and insovative technologies for suitainable communities and environment. TP-IMD-04 For instructional purposes only • 1" Semester SY 2020-2021 1. рH 3.7 2. pH 4.7 3. рH 5.7 Using the stock solution provided to you, make 25 ml of each of the buffer solutions assigned to you. Measure and record the pH of each of the buffer solutions. Add 2 ml of 0.1 M NAOH to each of the 25 ml buffer solutions. Record the pH of each buffer solution after addition of alkali. Account for the magnitude of pH shift in each with reference to the direction of pH shift.
Effect of the ratio of the conjugate base to weak acid Effect of the ratio of the conjugate base to the weak acid. CASE 1. From the Henderson-Hasselbach equation, calculate the ratio of dihydrogen phosphate (H2P04-) and monohydrogen phosphate (HPO4-2) components required to produce buffer solution with 1. pH 6.2 2. pH 7.2 3. pH 8.2 Phosphate Buffer [Conjugate Base] [Weak Acid] pH pH after NaOH was added 6.2 7.2 8.2 Discussion: Acetate Buffer CASE 2. From the Henderson-Hasselbach equation, calculate the ratio of acetic acid and acetate required to produce buffer solution with [Conjugate Base] [Weak Acid] pH pH after NaOH was added 3.7 4.7 5.7 Discussion:
Transcribed Image Text:Effect of the ratio of the conjugate base to weak acid Effect of the ratio of the conjugate base to the weak acid. CASE 1. From the Henderson-Hasselbach equation, calculate the ratio of dihydrogen phosphate (H2P04-) and monohydrogen phosphate (HPO4-2) components required to produce buffer solution with 1. pH 6.2 2. pH 7.2 3. pH 8.2 Phosphate Buffer [Conjugate Base] [Weak Acid] pH pH after NaOH was added 6.2 7.2 8.2 Discussion: Acetate Buffer CASE 2. From the Henderson-Hasselbach equation, calculate the ratio of acetic acid and acetate required to produce buffer solution with [Conjugate Base] [Weak Acid] pH pH after NaOH was added 3.7 4.7 5.7 Discussion:
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