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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 ...
Electrical conductivity of water samples is used as an indicator of how salt-free, ion-free, or impurity-free the sample is; the purer the water, the lower the conductivity (the higher the resistivity). Conductivity measurements in water are often reported as specific conductance, relative to the conductivity of pure water at 25 °C.
An electrolyte is a substance that conducts electricity through the movement of ions, but not through the movement of electrons. [ 1 ] [ 2 ] [ 3 ] This includes most soluble salts , acids , and bases , dissolved in a polar solvent like water.
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]
The term standard in SHE requires a supply of hydrogen gas bubbled through the electrolyte at a pressure of 1 atm and an acidic electrolyte with H + activity equal to 1 (usually assumed to be [H +] = 1 mol/liter, i.e. pH = 0). The SHE electrode can be connected to any other electrode by a salt bridge and an external circuit to form a cell.
Conductometry is a measurement of electrolytic conductivity to monitor a progress of chemical reaction. Conductometry has notable application in analytical chemistry, where conductometric titration is a standard technique.
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An aqueous electrolyte can considerably raise conductivity. The electrolyte disassociates into cations and anions; the anions rush towards the anode and neutralize the buildup of positively charged H + there; similarly, the cations rush towards the cathode and neutralize the buildup of negatively charged OH − there.