The conductivity of `0.001028 M` acetic acid is `4.95xx10^(-5) S cm^(-1)`. Calculate dissociation constant if `wedge_(m)^(@)` for acetic acid is `390.5 S cm^(2) mol ^(-1)`.

Explanation

To solve the problem, we need to calculate the dissociation constant (α) of acetic acid using the given conductivity and limiting molar conductivity. Here’s a step-by-step solution:

### Step 1: Understand the Given Data
- Conductivity (κ) of acetic acid solution = \(4.95 \times 10^{-5} \, \text{S cm}^{-1}\)
- Concentration (C) of acetic acid = \(0.001028 \, \text{M}\)
- Limiting molar conductivity (\( \Lambda_m^0 \)) of acetic acid = \(390.5 \, \text{S cm}^2 \text{mol}^{-1}\)

### Step 2: Calculate Molar Conductivity (Λm)
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