Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, Ka2 = 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 pKa2 = 7.21 pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH,PO,(s) and 32.0 g of Na, HPO, (s) in water and then diluting to 1.00 L. pH =
Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, Ka2 = 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 pKa2 = 7.21 pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 16.0 g of KH,PO,(s) and 32.0 g of Na, HPO, (s) in water and then diluting to 1.00 L. pH =
Chemistry
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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
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![### pH Calculation of a Buffer Solution
**Phosphoric acid is a triprotic acid**, defined by its three dissociation constants:
- \( K_{a1} = 6.9 \times 10^{-3} \)
- \( K_{a2} = 6.2 \times 10^{-8} \)
- \( K_{a3} = 4.8 \times 10^{-13} \)
#### Determining the Correct \( \text{p}K_a \) for the Buffer Solution
To find the pH of a buffer that is composed of \( \text{H}_2\text{PO}_4^- \) (aq) and \( \text{HPO}_4^{2-} \) (aq), which \( \text{p}K_a \) value should be used in the Henderson-Hasselbalch equation? The options are:
- \( \text{p}K_{a1} = 2.16 \)
- \( \text{p}K_{a2} = 7.21 \)
- \( \text{p}K_{a3} = 12.32 \)
Since we are considering the buffer system involving \( \text{H}_2\text{PO}_4^- \) and \( \text{HPO}_4^{2-} \), the appropriate \( \text{p}K_a \) value to use is:
\[ \text{p}K_{a2} = 7.21 \]
#### Buffer Solution pH Calculation
To calculate the pH of a buffer solution obtained by:
- Dissolving **16.0 g of \( \text{KH}_2\text{PO}_4 \) (s)** and
- **32.0 g of \( \text{Na}_2\text{HPO}_4 \) (s)**
the mixture is then diluted to **1.00 L**.
Use the following open-ended form to determine the pH:
\[ \text{pH} = \]
[Include the Henderson-Hasselbalch equation and any necessary steps here to guide students through the calculation process.]
### Henderson-Hasselbalch Equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{A}^-]}{[\text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96b52401-77ae-42e3-bef0-cdd66c230602%2F6f20dfcc-4102-4a96-ad18-579b3a652806%2F7qgo546_processed.png&w=3840&q=75)
Transcribed Image Text:### pH Calculation of a Buffer Solution
**Phosphoric acid is a triprotic acid**, defined by its three dissociation constants:
- \( K_{a1} = 6.9 \times 10^{-3} \)
- \( K_{a2} = 6.2 \times 10^{-8} \)
- \( K_{a3} = 4.8 \times 10^{-13} \)
#### Determining the Correct \( \text{p}K_a \) for the Buffer Solution
To find the pH of a buffer that is composed of \( \text{H}_2\text{PO}_4^- \) (aq) and \( \text{HPO}_4^{2-} \) (aq), which \( \text{p}K_a \) value should be used in the Henderson-Hasselbalch equation? The options are:
- \( \text{p}K_{a1} = 2.16 \)
- \( \text{p}K_{a2} = 7.21 \)
- \( \text{p}K_{a3} = 12.32 \)
Since we are considering the buffer system involving \( \text{H}_2\text{PO}_4^- \) and \( \text{HPO}_4^{2-} \), the appropriate \( \text{p}K_a \) value to use is:
\[ \text{p}K_{a2} = 7.21 \]
#### Buffer Solution pH Calculation
To calculate the pH of a buffer solution obtained by:
- Dissolving **16.0 g of \( \text{KH}_2\text{PO}_4 \) (s)** and
- **32.0 g of \( \text{Na}_2\text{HPO}_4 \) (s)**
the mixture is then diluted to **1.00 L**.
Use the following open-ended form to determine the pH:
\[ \text{pH} = \]
[Include the Henderson-Hasselbalch equation and any necessary steps here to guide students through the calculation process.]
### Henderson-Hasselbalch Equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{A}^-]}{[\text{
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