ANSWER NUMBER FOUR ONLY A study of vaccines suggest that a higher pH, preferably near 7, is necessary for the faster formation of the antibodies. Because of this, a chemist proposed using a citric acid buffer. They were tasked to prepare a 500.0 mL, 0.25 M pH 5.00 buffer from 1.20M citric acid (H3C6H5O7; pKa1 = 3.13, pKa2 = 4.76, pKa3 = 6.40) and 0.90 M NaOH. Note: When adding a strong acid/base to a weak base/acid, the strong acid/base is fully consumed. What is the acid component and base component of the buffer solution? What are the moles of each component in the buffer solution? Calculate the amounts of reagents needed to prepare the buffer solution. What will be the pH of the buffer upon addition of 0.75 mL 2.00 M HNO3? What will be the pH of the buffer upon addition of 2.30 mL of 1.75 M NaOH?
ANSWER NUMBER FOUR ONLY A study of vaccines suggest that a higher pH, preferably near 7, is necessary for the faster formation of the antibodies. Because of this, a chemist proposed using a citric acid buffer. They were tasked to prepare a 500.0 mL, 0.25 M pH 5.00 buffer from 1.20M citric acid (H3C6H5O7; pKa1 = 3.13, pKa2 = 4.76, pKa3 = 6.40) and 0.90 M NaOH. Note: When adding a strong acid/base to a weak base/acid, the strong acid/base is fully consumed. What is the acid component and base component of the buffer solution? What are the moles of each component in the buffer solution? Calculate the amounts of reagents needed to prepare the buffer solution. What will be the pH of the buffer upon addition of 0.75 mL 2.00 M HNO3? What will be the pH of the buffer upon addition of 2.30 mL of 1.75 M NaOH?
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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ANSWER NUMBER FOUR ONLY
A study of vaccines suggest that a higher pH, preferably near 7, is necessary for the faster formation of the antibodies. Because of this, a chemist proposed using a citric acid buffer. They were tasked to prepare a 500.0 mL, 0.25 M pH 5.00 buffer from 1.20M citric acid (H3C6H5O7; pKa1 = 3.13, pKa2 = 4.76, pKa3 = 6.40) and 0.90 M NaOH. Note: When adding a strong acid/base to a weak base/acid, the strong acid/base is fully consumed.
- What is the acid component and base component of the buffer solution?
- What are the moles of each component in the buffer solution?
- Calculate the amounts of reagents needed to prepare the buffer solution.
- What will be the pH of the buffer upon addition of 0.75 mL 2.00 M HNO3? What will be the pH of the buffer upon addition of 2.30 mL of 1.75 M NaOH?
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