Question

What is the relationship between degree of dissociation and molar conductivity?

Answer 1

We need to remember that the molar conductivity of an electrolyte is defined as its conductivity divided by its molar concentration. There are two types of electrolytes: strong and weak. Strong electrolytes usually undergo complete ionization, due to which they have higher conductivity than weak electrolytes, which leads only to partial ionization.

Complete answer:
For strong electrolytes, such as salts, strong acids and strong bases, the molar conductivity depends only weakly on concentration. On dilution there is a regular increase in the molar conductivity of strong electrolyte, due to the decrease in solute–solute interaction. Molar conductivity measures the efficiency with which a given electrolyte conducts electricity in solution. With the increase of degree of dissociation, the molar conductivity of both weak and strong electrolytes increases.
$\alpha = \dfrac{{({\lambda _m})\infty }}{{({\lambda _m})c}} = \dfrac{{{\lambda _{}}}}{{{\lambda _o}}}$
Molar conductivity can be expressed in the following term given below:
${\Lambda _m}\; = {\text{ }}\dfrac{K}{C}$
Where $K$ is the specific conductivity and $C$is the concentration in mole per litre.
In general, the molar conductivity of an electrolytic solution is the conductance of the volume of the solution containing a unit mole of electrolyte that is placed between two electrodes of unit area cross-section or at a distance of one-centimeter apart.
The unit of molar conductivity is$S \cdot {m^2} \cdot mo{l^{ - 1}}$.

Note:
We need to know that the degree of association is classified as the fraction of the total number of molecules that are connected or combined, resulting in a larger molecule being created. The degree of dissociation is the phenomenon of producing free ions carrying current, which at a given concentration is dissociated from the fraction of solute.