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Redox Concepts, Cathode and Anode of Electrochemical Cells, Note:…

- - - - To balance the equation multiply the half equations so that the electrons lost and gained match
- - - - Set up:
        
        2 half-cells with metal strips
        
        Metal strips of the 2 metals involved
        
        Electrolyte in each half cell consisting of metals (e.g. sulfate solutions)
        
        Salt bridge between both half cells to maintain equilibrium
        
        Voltmeter to allow the flow of electrons from anode
        
        Application: Standard Electrode potentials of the substances can be calculated by substracting the e naught of the reducing agent (at anode) with that of the oxidising agent (at cathode)
  - - - Set-up:
        
        One electrolyte
        
        Two inert electrodes (usually)
        
        DC Battery (power supply)
        
        Application: Electrolysis of various substances
        
        Reactions that occur at the cathode and anode are determined by the E naught values of the substances, the concentrations of the ions and the type of electrodes used (active or inert)
- - - - Series of redox reactions take place involving the addition of Manganese, Iodide ions and sodium thiosulfate. 1 mole of O2: 4 mole of thiosulfate
        
        Application: calculates the Biochemical oxygen demand of waterbody
    - - Oxidising agents reacted with iodine to form iodide ions, colour change is observed
      - Application: calculating sodium hypochlorite content in bleach
    - - Iron is oxidised
        
        Application: content of iron tablets can be found