Design a buffer that has a pH of 4.66 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pka CH3NH₂ 4.2x 10-4 CH3NH3+ 2.4x10-11 10.62 C6H1503N 5.9x107 1.7x10-8 7.77 C5H5N 1.5x109 C5H5NH+ 6.7x10-6 5.17 C6H1503NH+ How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =

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### Designing a Buffer Solution

To design a buffer with a pH of 4.66 using one of the weak base/conjugate acid systems listed below, follow the instructions provided.

#### Weak Base/Conjugate Acid Systems
| Weak Base      | \( K_b \)     | Conjugate Acid | \( K_a \)         | \( pK_a \)  |
|----------------|---------------|----------------|-------------------|------------|
| \( \text{CH}_3\text{NH}_2 \)   | \( 4.2 \times 10^{-4} \) | \( \text{CH}_3\text{NH}_3^+ \) | \( 2.4 \times 10^{-11} \) | 10.62      |
| \( \text{C}_6\text{H}_{15}\text{O}_3\text{N} \) | \( 5.9 \times 10^{-7} \) | \( \text{C}_6\text{H}_{15}\text{O}_3\text{NH}^+ \) | \( 1.7 \times 10^{-8} \)  | 7.77       |
| \( \text{C}_5\text{H}_5\text{N} \) | \( 1.5 \times 10^{-9} \) | \( \text{C}_5\text{H}_5\text{NH}^+ \) | \( 6.7 \times 10^{-6} \)  | 5.17       |

#### Buffer Composition Calculation
Determine the number of grams of the chloride salt of the conjugate acid and the number of grams of the weak base required to produce 1.00 L of a buffer solution that is 1.00 M in the weak base.

- **Grams of chloride salt of conjugate acid**: [_______]
- **Grams of weak base**: [_______]

These calculations involve using the Henderson-Hasselbalch equation and appropriate conversion between the amounts of substances and mass.

#### Explanation of Values
- \( pK_a \): The negative logarithm of the acid dissociation constant (\( K_a \)), which indicates the strength of the conjugate acid.
- \( K_b \): The base dissociation constant, representing the strength of the weak base
Transcribed Image Text:### Designing a Buffer Solution To design a buffer with a pH of 4.66 using one of the weak base/conjugate acid systems listed below, follow the instructions provided. #### Weak Base/Conjugate Acid Systems | Weak Base | \( K_b \) | Conjugate Acid | \( K_a \) | \( pK_a \) | |----------------|---------------|----------------|-------------------|------------| | \( \text{CH}_3\text{NH}_2 \) | \( 4.2 \times 10^{-4} \) | \( \text{CH}_3\text{NH}_3^+ \) | \( 2.4 \times 10^{-11} \) | 10.62 | | \( \text{C}_6\text{H}_{15}\text{O}_3\text{N} \) | \( 5.9 \times 10^{-7} \) | \( \text{C}_6\text{H}_{15}\text{O}_3\text{NH}^+ \) | \( 1.7 \times 10^{-8} \) | 7.77 | | \( \text{C}_5\text{H}_5\text{N} \) | \( 1.5 \times 10^{-9} \) | \( \text{C}_5\text{H}_5\text{NH}^+ \) | \( 6.7 \times 10^{-6} \) | 5.17 | #### Buffer Composition Calculation Determine the number of grams of the chloride salt of the conjugate acid and the number of grams of the weak base required to produce 1.00 L of a buffer solution that is 1.00 M in the weak base. - **Grams of chloride salt of conjugate acid**: [_______] - **Grams of weak base**: [_______] These calculations involve using the Henderson-Hasselbalch equation and appropriate conversion between the amounts of substances and mass. #### Explanation of Values - \( pK_a \): The negative logarithm of the acid dissociation constant (\( K_a \)), which indicates the strength of the conjugate acid. - \( K_b \): The base dissociation constant, representing the strength of the weak base
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