<P> 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 . </P> <P> The limiting molar conductivity can be decomposed into contributions from the different ions (Kohlrausch's law of independent migration of ions): </P> <Dl> <Dd> Λ m ∘ = Σ i ν i λ i (\ displaystyle \ Lambda _ (\ mathrm (m)) ^ (\ circ) = \ Sigma _ (i) \ nu _ (i) \ lambda _ (i)) </Dd> </Dl> <Dd> Λ m ∘ = Σ i ν i λ i (\ displaystyle \ Lambda _ (\ mathrm (m)) ^ (\ circ) = \ Sigma _ (i) \ nu _ (i) \ lambda _ (i)) </Dd>

Define conductivity and molar conductivity for the solution of an electrolyte