What `%` of the carbon in the `H_(2)CO_(3)-HCO_(3)^(-)` buffer should be in the form of `HCO_(3)^(-)` so as to have a neutral solution? `(K_(a)=4xx10^(-7))`

Options

A. `20%`
B. `40%`
C. `60%`
D. `80%`

Explanation

To solve the problem of determining what percentage of carbon in the `H2CO3-HCO3^(-)` buffer should be in the form of `HCO3^(-)` to achieve a neutral solution, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Relationship Between pH and pKa:**
The pH of a neutral solution is 7. The relationship between pH, pKa, and the concentrations of the acid and its conjugate base can be expressed using the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{HCO}_3^-]}{[\text{H}_2\text{CO}_3]}\right)
...