Chlorine Characteristics

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Chlorine Characteristics ( chlorine-characteristics )

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Copyright © Tarek Kakhia. All rights reserved. http://tarek.kakhia.org Addition of chlorine to water gives both hydro chloric acid HCl and hypo chlorous acid : Cl2 + H2O = HClO + HCl 2 . Production Using Electrolysis Solutions of hypo chlorites can be produced by electrolysis of an aqueous chloride solution. Chlorine gas is produced at the anode, while hydrogen forms at the cathode. Some of the chlorine gas produced will dissolve forming hypochlorite ions through the above reaction. The geometry of the cell is critical to ensure that as much of the chlorine as possible dissolves, rather than simply bubbling out of the cell. At the anode : 2 Cl- ---> Cl 2 (g) + 2e- At the cathode : 2H+ + 2e- ---> H2 (g) It can be seen that over time, the electrolyte will become increasingly basic. There are a number of potential hazards and challenges associated with this process. It should not be attempted by untrained persons.  The electrochemical environment of the cell is highly corrosive, particularly at the anode. Few materials are suitable as an anode electrolyte. Graphite can be used, but will degrade quickly ( which also results in contamination of the cell with finely divided carbon particles ). Graphite supported lead dioxide electrodes have been reported to be more effective.  If the reaction conditions are not controlled, the produced hypochlorite can react with the hydroxide ions to form chlorate ions. These can additionally be electrochemically oxidized to perchlorate ions ( within the same cell ) .  Hypochlorite is a powerful oxidizing agent, and will attack the dyes used in pH paper and damage pH sensors, making measurement and control of the conditions difficult. 34

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