Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO; (aq), which pKa value should be used in the Henderson-Hasselbalch equation? pKal = 2.16 O pKa2 = 7.21 pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH,PO,(s) and 25.0 g of Na, HPO, (s) in water and then diluting to 1.00 L. pH =
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO; (aq), which pKa value should be used in the Henderson-Hasselbalch equation? pKal = 2.16 O pKa2 = 7.21 pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH,PO,(s) and 25.0 g of Na, HPO, (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
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Chapter1: Chemical Foundations
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![Phosphoric acid is a triprotic acid (Kal
= 6.9 x 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13).
To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in the
Henderson-Hasselbalch equation?
O pKal = 2.16
pK22 = 7.21
O pKa3
= 12.32
Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO,(s) and 25.0 g of Na, HPO,(s) in water and then
diluting to 1.00 L.
pH =
II](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F214a1152-ccda-43e7-9936-4a2ae323f75a%2Ff0f9c121-b3e9-437b-8f9d-fc097421e296%2F7i5e0mt_processed.png&w=3840&q=75)
Transcribed Image Text:Phosphoric acid is a triprotic acid (Kal
= 6.9 x 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13).
To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in the
Henderson-Hasselbalch equation?
O pKal = 2.16
pK22 = 7.21
O pKa3
= 12.32
Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO,(s) and 25.0 g of Na, HPO,(s) in water and then
diluting to 1.00 L.
pH =
II
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