Strong electrolytes are hypothesized to dissociate completely in solution. The conductivity of a solution of a strong electrolyte at low concentration follows Kohlrausch's Law
where  is known as the limiting molar conductivity,  is an empirical constant and  is the electrolyte concentration. (Limiting here means "at the limit of the infinite dilution".) In effect, the observed conductivity of a strong electrolyte becomes directly proportional to concentration, at sufficiently low concentrations i.e. when
As the concentration is increased however, the conductivity no longer rises in proportion.
Moreover, Kohlrausch also found that the limiting conductivity of an electrolyte;
:  and  are the limiting molar conductivities of the individual ions.
The following table gives values for the limiting molar conductivities for some selected ions.
An interpretation of these results was based on the theory of Debye and Hückel, yielding the Debye–Hückel–Onsager theory:
where  and  are constants that depend only on known quantities such as temperature, the charges on the ions and the dielectric constant and viscosity of the solvent. As the name suggests, this is an extension of the Debye–Hückel theory, due to Onsager. It is very successful for solutions at low concentration.