Phosphoric acid is a triprotic acid ($K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, K_{a3} = 4.8 \times 10^{-13}$). 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 10.0 g of $KH_2PO_4 (s)$ and 25.0 g of $Na_2HPO_4 (s)$ in water and then diluting to 1.00 L. pH = \_\_\_\_

Phosphoric acid is a triprotic acid ($K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, K_{a3} = 4.8 \times 10^{-13}$). 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 10.0 g of $KH_2PO_4 (s)$ and 25.0 g of $Na_2HPO_4 (s)$ in water and then diluting to 1.00 L. pH = \_\_\_\_

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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