The ionisation constant os dimethylamine is `5.4xx10^(-4)`. Calculate its degree of ionization in its `0.02M` solution. What percentage of dimethylamine is ionized if the solution is also `0.1 M` in `NaOH`?

Explanation

To solve the problem, we need to calculate the degree of ionization of dimethylamine in a 0.02 M solution and then determine the percentage of dimethylamine that is ionized when the solution is also 0.1 M in NaOH.

### Step 1: Write the ionization equation for dimethylamine
Dimethylamine (C2H7N) ionizes in water as follows:
\[ \text{C}_2\text{H}_7\text{N} + \text{H}_2\text{O} \rightleftharpoons \text{C}_2\text{H}_7\text{NH}^+ + \text{OH}^- \]

### Step 2: Set up the expression for the ionization constant (K)
The ionization constant (K) is given by:
...