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The molar conductivity of an electrolyte solution is defined as its conductivity divided by its molar concentration. [1] [2] =, where: κ is the measured conductivity (formerly known as specific conductance), [3] c is the molar concentration of the electrolyte.
The conductivity of a solution of a strong electrolyte at low concentration follows Kohlrausch's Law = where Λ 0 m is known as the limiting molar conductivity, K is an empirical constant and c is the electrolyte concentration. (Limiting here means "at the limit of the infinite dilution".)
In practice the molar ionic conductivities are calculated from the measured ion transport numbers and the total molar conductivity. For the cation + = + +, and similarly for the anion. In solutions, where ionic complexation or associaltion are important, two different transport/transference numbers can be defined.
The Ostwald law of dilution provides a satisfactory description of the concentration dependence of the conductivity of weak electrolytes like CH 3 COOH and NH 4 OH. [3] [4] The variation of molar conductivity is essentially due to the incomplete dissociation of weak electrolytes into ions.
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Condosity is a comparative measurement of electrical conductivity of a solution. The condosity of any given solution is defined as the molar concentration of a sodium chloride (NaCl) solution that has the same specific electrical conductance as the solution under test. [1] [2] [3]
SYDNEY (Reuters) -The remaining five members of the "Bali Nine" Australian drug ring have returned from Indonesia after diplomatic efforts between the countries this month to strike a repatriation ...