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Conductivity or specific conductance of an electrolyte solution is a measure of its ability to conduct electricity. The SI unit of conductivity is siemens per meter (S/m). Conductivity measurements are used routinely in many industrial and environmental applications as a fast, inexpensive and reliable way of measuring the ionic content in a ...
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.
[3] Normally, glass frits, a porous material, cover the ends of the tube or the electrolyte is often gelified with agar-agar to help prevent the intermixing of fluids that might otherwise occur. [3] The conductivity of a glass tube bridge primarily depends on the concentration of the electrolyte solution. At concentrations below saturation, an ...
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.
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.
A supporting electrolyte, in electrochemistry, according to an IUPAC definition, [1] is an electrolyte containing chemical species that are not electroactive (within the range of potentials used) and which has an ionic strength and conductivity much larger than those due to the electroactive species added to the electrolyte.
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The cation of the indicator electrolyte should not move faster than the cation whose transport number is to be determined, and it should have same anion as the principle electrolyte. Besides the principal electrolyte (e.g., HCl) is kept light so that it floats on indicator electrolyte.