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Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and HPO¾¯(aq), which pKą value should be used in the Henderson-Hasselbalch equation? pKal = 2.16 PK₁2 = 7.21 pK₁3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH₂PO4(s) and 28.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH = = 6.9 × 10-³, K₁2 = 6.2 × 10-8, and K₁3 = 4.8 × 10-¹3). 7.4 Incorrect

Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and HPO¾¯(aq), which pKą value should be used in the Henderson-Hasselbalch equation? pKal = 2.16 PK₁2 = 7.21 pK₁3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH₂PO4(s) and 28.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH = = 6.9 × 10-³, K₁2 = 6.2 × 10-8, and K₁3 = 4.8 × 10-¹3). 7.4 Incorrect

Chemistry
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
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Phosphoric acid is a triprotic acid (?a1= 6.9×10^−3, ?a2= 6.2×10^−8, and ?a3= 4.8×10^−13).
To find the pH of a buffer composed of H2PO−4(aq) and HPO2−4(aq), which p?a value should be used in the Henderson–Hasselbalch equation?
p?a1 = 2.16
p?a2 = 7.21
p?a3 = 12.32
Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH2PO4(s) and 28.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
### Understanding Buffer Solutions with Phosphoric Acid Phosphoric acid is a triprotic acid. The acid dissociation constants (Ka) for phosphoric acid are: - \( K_{a1} = 6.9 \times 10^{-3} \) - \( K_{a2} = 6.2 \times 10^{-8} \) - \( K_{a3} = 4.8 \times 10^{-13} \) ### Using the Henderson-Hasselbalch Equation **Question:** To find the pH of a buffer composed of \( \text{H}_2\text{PO}_4^- \) (aq) and \( \text{HPO}_4^{2-} \) (aq), which \( \text{pKa} \) value should be used in the Henderson-Hasselbalch equation? - \(\bigcirc\) \( \text{pKa}_1 = 2.16 \) - \(\bigcirc\) \( \text{pKa}_2 = 7.21 \) - \(\bigcirc\) \( \text{pKa}_3 = 12.32 \) **Answer:** - \( \mathbf{\bigcirc} \) \( \text{pKa}_2 = 7.21 \) ### Calculating the pH of a Buffer Solution **Problem:** Calculate the pH of a buffer solution obtained by dissolving 11.0 g of \( \text{KH}_2\text{PO}_4 \) (s) and 28.0 g of \( \text{Na}_2\text{HPO}_4 \) (s) in water and then diluting to 1.00 L. ### Input: - **pH** = **7.4** (Enter this value in the provided textbox) **Result:** - A red box appears around the answer with the text “Incorrect” below it, indicating that the provided pH value is incorrect. This exercise demonstrates the application of the Henderson-Hasselbalch equation in calculating the pH of buffer solutions and understanding the appropriate \( \text{pKa} \) values to use based on the components of the buffer system.
Transcribed Image Text:### Understanding Buffer Solutions with Phosphoric Acid Phosphoric acid is a triprotic acid. The acid dissociation constants (Ka) for phosphoric acid are: - \( K_{a1} = 6.9 \times 10^{-3} \) - \( K_{a2} = 6.2 \times 10^{-8} \) - \( K_{a3} = 4.8 \times 10^{-13} \) ### Using the Henderson-Hasselbalch Equation **Question:** To find the pH of a buffer composed of \( \text{H}_2\text{PO}_4^- \) (aq) and \( \text{HPO}_4^{2-} \) (aq), which \( \text{pKa} \) value should be used in the Henderson-Hasselbalch equation? - \(\bigcirc\) \( \text{pKa}_1 = 2.16 \) - \(\bigcirc\) \( \text{pKa}_2 = 7.21 \) - \(\bigcirc\) \( \text{pKa}_3 = 12.32 \) **Answer:** - \( \mathbf{\bigcirc} \) \( \text{pKa}_2 = 7.21 \) ### Calculating the pH of a Buffer Solution **Problem:** Calculate the pH of a buffer solution obtained by dissolving 11.0 g of \( \text{KH}_2\text{PO}_4 \) (s) and 28.0 g of \( \text{Na}_2\text{HPO}_4 \) (s) in water and then diluting to 1.00 L. ### Input: - **pH** = **7.4** (Enter this value in the provided textbox) **Result:** - A red box appears around the answer with the text “Incorrect” below it, indicating that the provided pH value is incorrect. This exercise demonstrates the application of the Henderson-Hasselbalch equation in calculating the pH of buffer solutions and understanding the appropriate \( \text{pKa} \) values to use based on the components of the buffer system.
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