In practice the molar ionic conductivities are calculated from the measured ion transport numbers and the total molar conductivity.
3.
For example, acetic acid has a higher molar conductivity in dilute aqueous acetic acid than in concentrated acetic acid.
4.
From the ionic molar conductivities of cations and anions, ionic radii can be calculated using the concept of Stokes radius.
5.
Kohlrausch showed for weak ( incompletely dissociated ) electrolytes that the more dilute a solution, the greater its molar conductivity due to increased ionic dissociation.
6.
For strong electrolytes, such as salts, strong acids and strong bases, the molar conductivity depends only " weakly " on concentration.
7.
Friedrich Kohlrausch's researches in 1875-79 established that to a high accuracy in dilute solutions, molar conductivity is composed of individual contributions of ions.
8.
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.
9.
At zero concentration, the limiting ion transport numbers may be expressed in terms of the limiting molar conductivities of the cation ( \ lambda _ 0 ^ + ), anion ( \ lambda _ 0 ^-) and electrolyte ( \ Lambda _ 0 ):
10.
For multivalent ions, it is usual to consider the conductivity divided by the equivalent ion concentration in terms of equivalents per litre, where 1 equivalent is the quantity of ions which have the same amount of electric charge as 1 mol of a monovalent ion : 1 / 2 mol Ca 2 +, 1 / 2 mol SO 4 2, 1 / 3 mol Al 3 +, 1 / 4 mol Fe ( CN ) 6 4, etc . This quotient can be called the " equivalent conductivity ", although IUPAC has recommended that use of this term be discontinued and the term molar conductivity be used for the values of conductivity divided by equivalent concentration.
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