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Lecture 2 - RedOx Titration.pptx - Oxidation-Reduction...

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Oxidation-Reduction Titration Assoc. Prof. Dr. A.K.M. Shafiqul Islam Department of Chemical Engineering Technology (Industrial Chemical Process) University Malaysia Perlis
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Oxidation Reduction Reaction Reactions of metals or any other organic compounds with oxygen to give oxides are labeled as oxidation. The removal of oxygen from metal oxides to give the metals in their elemental forms is labeled as reduction. In other words, oxidation is addition of oxygen and removal of hydrogen whereas reduction is addition of hydrogen and removal of oxygen.
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Chemical reaction Reduction-Oxidation reaction commonly known as RedOx reaction Ox 1 + Red 2 ⇌ Red 1 + Ox 2 Chemical reaction based oxidation and reduction reaction is known as RedOx reaction Fe 2+ + Ce 4+ → Fe 3+ + Ce 3+ (1)
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There are two kinds of electro chemical cells, galvanic or electrolytic. In galvanic cells, the chemical reaction occurs spontaneously to produce electrical energy. In a electrolytic cell, electrical energy is used to force the non spontaneous chemical reaction. Galvanic cells are of importance in our further discussion as we will be discussing the spontaneous chemical reaction to produce electrical energy. Electrochemical Cells
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If a solution containing Fe 2+ is mixed with another solution containing Ce 4+ , there will be a redox reaction situation due to their tendency of transfer electrons. If we consider that these two solution are kept in separate beaker and connected by salt bridge and a platinum wire that will become a galvanic cell. If we connect a voltmeter between two electrode, the potential difference of two electrode can be directly measured. The Fe 2+ is being oxidised at the platinum wire (the anode): Fe 2+ → Fe 3+ + e - The electron thus produced will flow through the wire to the other beaker where the Ce 4+ is reduced (at the cathode). Ce 4+ + e - → Ce 3+
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The reaction involve electron transfer Fe 2+ → Fe 3+ + e - (2) Ce 4+ + e - → Ce 3+ (3) Equation (2) & (3) are called half reactions No half reaction can occur by itself There must be an electron donner (reducing agent) and an electron accepter (oxidizing agent) Fe 2+ is the reducing agent and Ce 3+ is the oxidizing agent
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Before we start the discussion of the oxidation reduction titration curve construction, we should understand the Nernst equation which was introduced by German scientist, Wlater Nernst in 1889.
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