**Phosphoric acid is a triprotic acid** \((K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, \text{and } K_{a3} = 4.8 \times 10^{-13})\).**To find the pH of a buffer composed of \(H_2PO_4^-\)(aq) and \(HPO_4^{2-}\)(aq), which \(pK_a\) value should be used in the Henderson–Hasselbalch equation?**- \(pK_{a1} = 2.16\)- \(pK_{a2} = 7.21\)- \(pK_{a3} = 12.32\)**Calculate the pH of a buffer solution obtained by dissolving 18.0 g of \(KH_2PO_4\)(s) and 34.0 g of \(Na_2HPO_4\)(s) in water and then diluting to 1.00 L.**\[ \text{pH} = \] [Text Box]

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Answered: Phosphoric acid is a triprotic acid…

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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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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