The specific conductance of a 0.01 M solution of acetic acid at 298 K is `1.65 xx 10^(-4) "ohm"^(-1)cm^(-1)`. The molar conductance at infinite dilution for `H^(+)` ion and `CH_(3)COO^(-)` ion are 349.1 `"ohm"^(-1) cm^(2 )"mol"^(-1)` and 40.9 `"ohm"^(-1) cm^(2) "mol"^(-1)` respectively.
Calculate :
(i) Molar conductance of solution
(ii) Degree of dissociation of acetic acid
(iii) Dissociation constant for acetic acid.

Explanation

To solve the problem step by step, we will address each part of the question systematically.

### Given Data:
- Specific conductance (k) of 0.01 M acetic acid = \(1.65 \times 10^{-4} \, \Omega^{-1} \, \text{cm}^{-1}\)
- Molar conductance at infinite dilution for \(H^+\) = \(349.1 \, \Omega^{-1} \, \text{cm}^2 \, \text{mol}^{-1}\)
- Molar conductance at infinite dilution for \(CH_3COO^-\) = \(40.9 \, \Omega^{-1} \, \text{cm}^2 \, \text{mol}^{-1}\)

### (i) Molar Conductance of the Solution
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