Calculate the degree of ionization of a weak acid with Ka = 10⁻⁴ and initial concentration C = 0.01 M. Also, analyze the provided neutralization reaction based on Brønsted-Lowry theory.

To calculate the degree of ionization ($\alpha$) for a weak acid, we can use the approximation $\alpha = \sqrt{\frac{K_a}{C}}$, where $K_a$ is the acid dissociation constant and $C$ is the initial concentration of the acid.

The given hypothetical neutralization reaction is:

Let's analyze each statement based on Brønsted-Lowry acid-base theory:

• A Brønsted-Lowry acid donates protons ($\text{H}^+$).
• A Brønsted-Lowry base accepts protons ($\text{H}^+$).
• A conjugate acid is formed when a base accepts a proton.
• A conjugate base is formed when an acid donates a proton.

In the reaction:

• $\text{H}_2\text{X}$ donates protons to $\text{BOH}$ (specifically, its $\text{OH}^-$ part). Thus, $\text{H}_2\text{X}$ acts as an acid.
• $\text{BOH}$ (or $\text{OH}^-$ from $\text{BOH}$) accepts protons from $\text{H}_2\text{X}$. Thus, $\text{BOH}$ acts as a base.
• When $\text{H}_2\text{X}$ donates protons, its conjugate base is $\text{X}^{2-}$ (which forms $\text{B}_2\text{X}$ with $\text{B}^+$).
• When $\text{OH}^-$ accepts a proton, its conjugate acid is $\text{H}_2\text{O}$.

Now, let's evaluate each statement:

• I. $\text{B}_2\text{X}$ is conjugate acid. $\text{B}_2\text{X}$ is a salt formed from the cation $\text{B}^+$ and the