Limiting molar conductivity for CH3COOH cannot be determined experimentally due to the presence of an equilibrium reaction. This is because CH3COOH is a weak acid that undergoes partial ionization in aqueous solutions, resulting in the formation of both ions and undissociated molecules.

Equilibrium Reaction

The equilibrium reaction for CH3COOH can be represented as follows:

CH3COOH + H2O ⇌ CH3COO- + H3O+

This means that the concentration of both ions and undissociated molecules are present in the solution, and it is impossible to separate the contribution of each species to the overall conductivity.

Kohlrausch's Law

Kohlrausch's law states that the limiting molar conductivity of an electrolyte can be determined by measuring the conductance of a solution of the electrolyte at different dilutions and extrapolating the conductance to infinite dilution. However, this law is applicable only to strong electrolytes that undergo complete ionization in aqueous solutions.

Conclusion

In the case of CH3COOH, since it is a weak acid and undergoes partial ionization, the limiting molar conductivity cannot be determined experimentally using Kohlrausch's law. Instead, theoretical calculations and modeling can be used to estimate the limiting molar conductivity of CH3COOH.

See--

CH3COOH = acitic acid


Acetic acid is a weak acid. Hence its molar conductivity can be measured.

According to Kohlaraush Law, the plot of molar conductivity versus square root is a steep curve which can't be extrapolated to get the value of molar conductivity at infinite dilution.

Also, the ionization is increased with dilution which leads to increase in molar conductivity as infinite dilution can't reache