Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find the pH of a buffer composed of H2PO4−(aq) and HPO2−4(aq), which pKa value would you use in the Henderson–Hasselbalch equation? 1. p?a1=2.16 2. p?a2=7.21 3. p?a3=12.32 Calculate the pH of a buffer solution obtained by dissolving 21.021.0 g KH2PO4(s) and 39.0 g Na2HPO4(s) in water and then diluting to 1.00 L.
Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find the pH of a buffer composed of H2PO4−(aq) and HPO2−4(aq), which pKa value would you use in the Henderson–Hasselbalch equation? 1. p?a1=2.16 2. p?a2=7.21 3. p?a3=12.32 Calculate the pH of a buffer solution obtained by dissolving 21.021.0 g KH2PO4(s) and 39.0 g Na2HPO4(s) in water and then diluting to 1.00 L.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.60QE: Consider all acid-base indicators discussed in this chapter. Which of these indicators would be...
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Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M).
To find the pH of a buffer composed of H2PO4−(aq) and HPO2−4(aq), which pKa value would you use in the Henderson–Hasselbalch equation?
1. p?a1=2.16
2. p?a2=7.21
3. p?a3=12.32
Calculate the pH of a buffer solution obtained by dissolving 21.021.0 g KH2PO4(s) and 39.0 g Na2HPO4(s) in water and then diluting to 1.00 L.
pH=?
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