The `pK_(a)` of a weak acid, `HA`, is `4.80`. The `pK_(b)` of a weak base, `BOH`, is `4.78`. The `pH` of an aqueous solution of the corresponding salt, `BA`, will be:

Options

A. 8.58
B. 4.79
C. 7.01
D. 9.22

Explanation

To find the pH of an aqueous solution of the corresponding salt BA formed from the weak acid HA and the weak base BOH, we can use the formula:

\[ \text{pH} = 7 + \frac{pK_a - pK_b}{2} \]

### Step-by-Step Solution:

1. **Identify the given values**:
- \( pK_a = 4.80 \)
- \( pK_b = 4.78 \)

2. **Substitute the values into the formula**:
\[ \text{pH} = 7 + \frac{4.80 - 4.78}{2} \]

3. **Calculate the difference between \( pK_a \) and \( pK_b \)**:
\[ 4.80 - 4.78 = 0.02 \]

4. **Divide the difference by 2**:
\[ \frac{0.02}{2} = 0.01 \]

5. **Add this value to 7**:
\[ \text{pH} = 7 + 0.01 = 7.01 \]

### Final Answer:
The pH of the aqueous solution of the corresponding salt BA is **7.01**.

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