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88. Chem 2001 Electrochemistry chemistry and Electricity. The quantity of electrons that flow from a reactionis proportional to the quantity of analyte that reacts. The electric force http://www.chem.lsu.edu/lucid/limbach/2001_f98/electrochem/electrochemistry.html

Electrochemistry Outline Basic Concepts Review Chemistry and Electricity Galvanic Cells Salt Bridge Line Notation Standard Potentials The Nernst Equation Electrodes Reference Electrodes Silver-Silver Chloride Reference Electrode Calomel Reference Electrode Indicator Electrodes Ion Selective Electrodes Polarography Cyclic Voltammetry Supplementary Reading Material from Harris, Quantitative Chemical Analysis , 4th Ed.: Chapters 14, 15, 18 Supplementary Reading Material from Harris, Exploring Chemical Analysis , 1st Ed.: Chapters 13, 14 Basic Concepts Oxidation Numbers oxidation number or ( oxidation state ) in a simple binary ionic compound is the number of electrons gained or lost by an atom of that element when it forms a compound. In the cases of single-atom ions it corresponds to the actual charge on the ion. General Rules to Determine the Oxidation Number of an Element The oxidation number is in any neutral substance that contains atoms of only one element. The oxidation number is equal to the charge on the ion for ions that contain only a single atom. The oxidation number of hydrogen is +1 when it is combined with a more electronegative element.

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99. Tutorial #11 Tutorial 11 Electrochemistry. eg What is the reduction potential forthe hydrogen electrode in a solution having a pH of 4.00? The http://www.carleton.ca/~rburk/chem1000/tutorials/tut11-01.htm

Tutorial #11 Electrochemistry e.g. What is the reduction potential for the hydrogen electrode in a solution having a pH of 4.00? The half reaction is 2 H (aq) + 2 e H 2(g, 1 atm) If pH = 4.00, then [H M. For this reaction, Q = p / [H Thus, E = E o - RT/nF ln(Q) = 0.00 V - 8.314(298)/(2)(96500) ln(10 = -0.24 V The lesson to learn here is that the Nernst equation applies to half reactions as well as to complete REDOX reactions! Electrolytic Cells These cells have E cell e.g. for the reaction using the two half-reactions: Fe + 2 e Fe E = -0.440 V 2 Ag 2 Ag + 2 e E = -0.800 V overall: Fe + 2 Ag Fe + 2 Ag E cell = -1.240 V To make this reaction occur, we must apply a potential of at least -1.240 V. The potential must be applied so that electrons are being supplied to the electrode where reduction is occuring. This is always the cathode, and in this case it is the iron electrode. Predicting the reactions at the electrodes In an eletrolytic cell, there is usually more than one species that could be oxidized at the anode, and more than one species that could be reduced at the cathode. Not only are hte obvious species present (e.g. metals and metal ions), but there is also a solvent (usually water) and some other ions, many of which are oxidizable or reducible. You need a rule to predict what happens at each electrode - perhaps the metal ion you are trying to reduce will not get reduced! The rule is: the reaction with the more positive half-reaction potential will occur preferentially

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