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These conditions provide an environment in which Kohlrausch reactions determine the molar conductivity.
From its definition, the molar conductivity is given by:
The following table gives values for limiting molar conductivities for selected ions.
Molar conductivity is a scientific term.
The molar conductivity of an electrolyte is a measure of how well it conducts electricity in solution.
The symbol for molar conductivity is Λ, or Λm.
Molar conductivity has the SI unit S m mol.
Friedrich Kohlrausch established that to a high accuracy in dilute solutions, molar conductivity is composed of individual contributions of ions.
The limiting molar conductivity can be decomposed into contributions from the different ions (law of independent migration of ions):
Kohlrausch showed for weak (incompletely dissociated) electrolytes that the more dilute a solution, the greater its molar conductivity due to increased ionic dissociation.
Molar conductivity is defined as the conductivity of an electrolyte solution divided by the molar concentration of the electrolyte, and so measures the efficiency with which a given electrolyte conducts electricity in solution.
For strong electrolytes, such as salts, strong acids and strong bases, molar conductivity is only weakly dependent on concentration and, to a good approximation, fits into the Debye - Huckel - Onsager equation :
After taking this into account, together with the specific requirements of moving ions, such as viscosity and electrophoretic effects, Onsager was able to derive a theoretical expression to account for the empirical relation known as Kohlrausch's Law, for the molar conductivity, Λ.
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