Design a buffer that has a pH of 3.76 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

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### Designing a Buffer System with pH 3.76

**Objective:**
Design a buffer that has a pH of 3.76 using one of the weak acid/conjugate base systems shown below.

#### Buffer Systems:
The table shows three potential weak acid/conjugate base systems, their dissociation constants (Kₐ), and their pKₐ values:

| Weak Acid | Conjugate Base | Kₐ | pKₐ |
| --------- | -------------- | --- | --- |
| HC₂O₄⁻ | C₂O₄²⁻ | 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 |

**Problem:**
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?

**Required Calculations:**
- grams of potassium salt of the weak acid = ____
- grams of potassium salt of the conjugate base = ____

### Understanding the Table and Problem

The table contains valuable information about different buffer systems that can potentially be used to create a buffer solution with the desired pH. Here's a breakdown of the columns:
- **Weak Acid:** The chemical formula of the weak acid.
- **Conjugate Base:** The chemical formula of the conjugate base that pairs with the weak acid.
- **Kₐ (Acid Dissociation Constant):** A numeric value representing the strength of the weak acid in water.
- **pKₐ:** The negative logarithm of the Kₐ value, giving a more intuitive measure of acid strength.

### Choosing the Appropriate Buffer System

To choose the correct buffer system, compare the desired pH (3.76) with the pKₐ values of the acids. The most effective buffer will have a pKₐ close to the desired pH. In this case:
- HC₂O₄⁻ has a pKₐ of 4.19, which is close
Transcribed Image Text:### Designing a Buffer System with pH 3.76 **Objective:** Design a buffer that has a pH of 3.76 using one of the weak acid/conjugate base systems shown below. #### Buffer Systems: The table shows three potential weak acid/conjugate base systems, their dissociation constants (Kₐ), and their pKₐ values: | Weak Acid | Conjugate Base | Kₐ | pKₐ | | --------- | -------------- | --- | --- | | HC₂O₄⁻ | C₂O₄²⁻ | 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 | **Problem:** 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? **Required Calculations:** - grams of potassium salt of the weak acid = ____ - grams of potassium salt of the conjugate base = ____ ### Understanding the Table and Problem The table contains valuable information about different buffer systems that can potentially be used to create a buffer solution with the desired pH. Here's a breakdown of the columns: - **Weak Acid:** The chemical formula of the weak acid. - **Conjugate Base:** The chemical formula of the conjugate base that pairs with the weak acid. - **Kₐ (Acid Dissociation Constant):** A numeric value representing the strength of the weak acid in water. - **pKₐ:** The negative logarithm of the Kₐ value, giving a more intuitive measure of acid strength. ### Choosing the Appropriate Buffer System To choose the correct buffer system, compare the desired pH (3.76) with the pKₐ values of the acids. The most effective buffer will have a pKₐ close to the desired pH. In this case: - HC₂O₄⁻ has a pKₐ of 4.19, which is close
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