Design a buffer that has a pH of 7.76 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pka HC₂04 C₂04²- 6.4 x 10-5 4.19 H₂PO4 HPO4²- 6.2 x 10-8 7.21 HCO3 CO3²- 4.8 x 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base =
Design a buffer that has a pH of 7.76 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pka HC₂04 C₂04²- 6.4 x 10-5 4.19 H₂PO4 HPO4²- 6.2 x 10-8 7.21 HCO3 CO3²- 4.8 x 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base =
Chemistry
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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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![**Designing a Buffer Solution**
To design a buffer with a pH of 7.76 using one of the weak acid/conjugate base systems shown below, consider the following data:
| Weak Acid | Conjugate Base | \( K_a \) | \( pK_a \) |
|-----------|----------------|-----------|-----------|
| \( \text{HC}_2\text{O}_4^- \) | \( \text{C}_2\text{O}_4^{2-} \) | \( 6.4 \times 10^{-5} \) | \( 4.19 \) |
| \( \text{H}_2\text{PO}_4^- \) | \( \text{HPO}_4^{2-} \) | \( 6.2 \times 10^{-8} \) | \( 7.21 \) |
| \( \text{HCO}_3^- \) | \( \text{CO}_3^{2-} \) | \( 4.8 \times 10^{-11} \) | \( 10.32 \) |
**Problem Statement:**
Calculate how many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base.
**Buffer Preparation:**
- **Grams of potassium salt of weak acid:**
- \[ \text{Enter value} \]
- **Grams of potassium salt of conjugate base:**
- \[ \text{Enter value} \]
To solve this problem, you need to:
1. **Select the appropriate acid/base pair:** Choose the weak acid and its conjugate base that has a \( pK_a \) value close to your target pH for the buffer.
2. **Use the Henderson-Hasselbalch equation:** This equation relates the pH of the buffer to the \( pK_a \) and the concentrations of the acid and its conjugate base.
\[ \text{pH} = pK_a + \log\left( \frac{[\text{base}]}{[\text{acid}]} \right) \]
3. **Determine the ratio of the conjugate base to the acid:** Using the desired pH and the chosen](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6ab0bbaf-7c6a-41d9-a28d-d2a0ce6f8c93%2F518390e7-354b-4c29-a027-0d1a5da04359%2Fwyn2ii_processed.png&w=3840&q=75)
Transcribed Image Text:**Designing a Buffer Solution**
To design a buffer with a pH of 7.76 using one of the weak acid/conjugate base systems shown below, consider the following data:
| Weak Acid | Conjugate Base | \( K_a \) | \( pK_a \) |
|-----------|----------------|-----------|-----------|
| \( \text{HC}_2\text{O}_4^- \) | \( \text{C}_2\text{O}_4^{2-} \) | \( 6.4 \times 10^{-5} \) | \( 4.19 \) |
| \( \text{H}_2\text{PO}_4^- \) | \( \text{HPO}_4^{2-} \) | \( 6.2 \times 10^{-8} \) | \( 7.21 \) |
| \( \text{HCO}_3^- \) | \( \text{CO}_3^{2-} \) | \( 4.8 \times 10^{-11} \) | \( 10.32 \) |
**Problem Statement:**
Calculate how many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base.
**Buffer Preparation:**
- **Grams of potassium salt of weak acid:**
- \[ \text{Enter value} \]
- **Grams of potassium salt of conjugate base:**
- \[ \text{Enter value} \]
To solve this problem, you need to:
1. **Select the appropriate acid/base pair:** Choose the weak acid and its conjugate base that has a \( pK_a \) value close to your target pH for the buffer.
2. **Use the Henderson-Hasselbalch equation:** This equation relates the pH of the buffer to the \( pK_a \) and the concentrations of the acid and its conjugate base.
\[ \text{pH} = pK_a + \log\left( \frac{[\text{base}]}{[\text{acid}]} \right) \]
3. **Determine the ratio of the conjugate base to the acid:** Using the desired pH and the chosen
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