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| [[File:Voltametro a rame.png|thumb|200px|Copper coulometer]]
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| The '''copper coulometer''' is a one application for the [[copper-copper(II) sulfate electrode]]. Such a [[coulometry|coulometer]] consists of two identical copper electrodes immersed in slightly acidic [[buffer solution|pH-buffered]] solution of [[copper(II) sulfate]]. Passing of [[current (electricity)|current]] through the element leads to the anodic [[solvation|dissolution]] of the metal on [[anode]] and simultaneous [[deposition (chemistry)|deposition]] of [[copper]] ions on the [[cathode]]. These reactions have 100% efficiency over a wide range of current density.
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| The amount of [[electric charge]] (quantity of electricity) passed through the cell can easily be determined by measuring the change in mass of either electrode and calculating:
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| :<math>Q = \frac{2\Delta m F}{63.546}</math>, | |
| where:
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| *Q is the quantity of electricity (coulombs)
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| *<math>\Delta m</math> is the mass transported (gm)
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| *the factor 2 is due to the transport of [[divalent]] ions
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| *F is the [[Faraday constant]] (96485.3383 coulombs per mole)
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| *63.546 is the [[atomic weight]] of copper (as grams per mole)
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| Although this apparatus is interesting from a theoretical and historical point of view, present-day electronic measurement of time and electrical current provide in their multiplication the amount of passed [[coulomb]]s much easier, with greater precision, and in a shorter period of time than is possible by weighing the electrodes.
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| ==See also==
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| *[[Mercury coulometer]]
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| *[[Coulometry]]
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| == References ==
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| <references/> | |
| {{unreferenced|date=October 2008}}
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| [[Category:Physical chemistry]]
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| [[Category:Electroanalytical chemistry devices]]
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| [[Category:Copper|Coulometer]]
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| [[Category:Coulometers]]
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| {{physical-chemistry-stub}}
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