There are two types of electrolytes: strong and weak. Strong electrolytes usually undergo complete ionization, and therefore they have higher conductivity than weak electrolytes, which undergo only partial ionization. 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. Based on experimental data Friedrich Kohlrausch (around the year 1900) proposed the non-linear law for strong electrolytes:
where 
: Λ is the molar conductivity at infinite dilution (or limiting molar conductivity), which can be determined by extrapolation of Λ as a function of ,
: K is the Kohlrausch coefficient, which depends mainly on the stoichiometry of the specific salt in solution,
: α is the dissociation degree even for strong concentrated electrolytes,
: f is the lambda factor for concentrated solutions.
This law is valid for low electrolyte concentrations only; it fits into the Debye–Hückel–Onsager equation.
For weak electrolytes (i.e. incompletely dissociated electrolytes), however, the molar conductivity strongly depends on concentration: The more dilute a solution, the greater its molar conductivity, due to increased ionic dissociation. For example, acetic acid has a higher molar conductivity in dilute aqueous acetic acid than in concentrated acetic acid.