Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K₁2 = 6.2 x 10-8, and K₁3 = 4.8 × 10-13). To find the pH of a buffer composed of H₂PO4 (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? PKa1 = 2.16 pK₁2 = 7.21 OPK₁3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH₂PO4(s) and 30.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH =
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K₁2 = 6.2 x 10-8, and K₁3 = 4.8 × 10-13). To find the pH of a buffer composed of H₂PO4 (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? PKa1 = 2.16 pK₁2 = 7.21 OPK₁3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH₂PO4(s) and 30.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH =
General Chemistry - Standalone book (MindTap Course List)
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.141QP: Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid,...
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![Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and K₁3 = 4.8 × 10-¹3).
To find the pH of a buffer composed of H₂PO (aq) and HPO2 (aq), which pKa value should be used in the
Henderson-Hasselbalch equation?
O PKal = 2.16
O pK₁2 = 7.21
a2
O pk₂3 = 12.32
a3
Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH₂PO4(s) and 30.0 g of Na₂HPO4(s) in water and then
diluting to 1.00 L.
pH =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa50e57d1-2bd6-427e-801e-187552a1e482%2F6a2b498b-1de8-45c5-a89d-942f38a5bd5a%2F253mg2ch_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and K₁3 = 4.8 × 10-¹3).
To find the pH of a buffer composed of H₂PO (aq) and HPO2 (aq), which pKa value should be used in the
Henderson-Hasselbalch equation?
O PKal = 2.16
O pK₁2 = 7.21
a2
O pk₂3 = 12.32
a3
Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH₂PO4(s) and 30.0 g of Na₂HPO4(s) in water and then
diluting to 1.00 L.
pH =
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