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

Explanation

To solve the problem step by step, we will follow these steps:

### Step 1: Write the ionization equation for HF
The ionization of hydrofluoric acid (HF) in water can be represented as:
\[ \text{HF} \rightleftharpoons \text{H}^+ + \text{F}^- \]

### Step 2: Set up the equilibrium expression
Let the initial concentration of HF be \( C = 0.02 \, \text{M} \). If \( \alpha \) is the degree of ionization, then at equilibrium:
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