Calculating The Degree of ionization: The molar conductance of an infinitely dilute solution `NH_(4)Cl` is `150 S cm^(2) mol^(-1)` and the limiting ionic conductacnes of `Cl^(-)` and `OH^(-)` ions are `76` and `198 S cm^(2) mol^(-1)` respectively. If the molar conductivity of a `0.01 M` solution of `NH_(4)OH` is ` 9.6 S cm^(2) mol^(-1)`, what will be its degree of ionization
Strategy: At any concentration `C`, if `alpha` is the degree of ionization then it can be approximented to the ratio of molar conductivity `Lambda_(m)^(c)` at the concentration `C` to limiting molar conducting, `Lambda_(m)^(0)`. We are given `Lambda_(m)^(c)` but we need to find `Lambda_(m)^(0)`.

Explanation

To calculate the degree of ionization of a 0.01 M solution of \( NH_4OH \), we will follow these steps:

### Step 1: Determine the limiting molar conductivity of \( NH_4^+ \)

Using Kohlrausch's law, we can find the molar conductivity of \( NH_4^+ \) from the given data about \( NH_4Cl \):
\[ \Lambda_m^{0}(NH_4^+) = \Lambda_m^{0}(NH_4Cl) - \Lambda_m^{0}(Cl^-) \]
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