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 (Kα) for acetic acid using the given conductivity and limiting molar conductivity. Let's break down the steps:

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

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