The ionization constant of HF is `3.2xx10^(-4)`. Calculate the degree of dissociation of HF in its 0.02 M solution. Calculate the concentration of all the species present `(H_(3)O^(+), F^(-) and HF)` in the solution and its pH .

Explanation

To solve the problem, we need to calculate the degree of dissociation of HF in a 0.02 M solution, the concentrations of all species present (H₃O⁺, F⁻, and HF), and the pH of the solution.

### Step-by-Step Solution:

1. **Write the Ionization Reaction:**
The ionization of HF in water can be represented as:
\[
\text{HF} \rightleftharpoons \text{H}_3\text{O}^+ + \text{F}^-
...