In class 12 chemistry, molar conductivity refers to the conductivity of an electrolyte solution at a specific concentration, measured between two electrodes with a known distance. It is denoted by the symbol Λ (lambda) and has units of siemens per meter squared per mole (S m² mol⁻¹).

Molar conductivity is a measure of the ability of an electrolyte solution to conduct electricity. It depends on the concentration of the electrolyte and provides information about the extent to which ions in the solution contribute to the overall conductivity.

Molar conductivity can be determined experimentally by measuring the conductivity of the electrolyte solution at different concentrations. The molar conductivity (Λ) is calculated using the equation:

Λ = κ / C

where κ is the conductivity of the solution in siemens per meter (S m⁻¹), and C is the concentration of the electrolyte in moles per cubic meter (mol m⁻³).

The molar conductivity of an electrolyte solution is influenced by factors such as the nature and charge of the ions, temperature, and solvent used. It can provide insights into the behavior and properties of electrolytes, including the degree of dissociation or ionization of the electrolyte in solution.

Molar conductivity is commonly used in studying electrolytic conductivity, determining the strength of electrolytes, understanding the conductance behavior of solutions, and characterizing the transport of ions in various applications such as electrochemistry and chemical kinetics.