The ionisation constant of `HF` is `3.2 xx 10^(-4)`.
a. Calculate the degree of dissociation of HF present in its 1M solution.
b. Calculate the concentration of all species present `(H_(3)O^(o+),F^(Θ)` and `HF`) in the solution.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understanding the Ionization of HF
Hydrofluoric acid (HF) ionizes in water according to the following equilibrium reaction:
\[ \text{HF} \rightleftharpoons \text{H}^+ + \text{F}^- \]

### Step 2: Setting Up the Initial Concentrations
Given that the initial concentration of HF (\(C_0\)) is 1 M, we can set up the initial concentrations:
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