Chloralkali Process
Procedures
There are two production methods in use. While the mercury cell method produces chlorine free sodium hydroxide the use of several tonnes of mercury leads to serious environmental problems. In normal production cycle a few hundred pounds of mercury per year are emitted which accumulate in the environment. Additionally, the chlorine and sodium hydroxide produced via the mercury-cell chloralkali process are themselves contaminated with trace amounts of mercury. The membrane and diaphragm method use no mercury, but the sodium hydroxide contains chlorine which has to be removed.
Membrane cell
Basic membrane cell used in the electrolysis of brine.
The most common chloralkali process involves the electrolysis of aqueous sodium chloride (a brine) in a membrane cell.
Saturated brine is passed into the first chamber of the cell where the chloride ions are oxidised at the anode to chlorine:
2Cl Cl2 + 2e
At the cathode, hydrogen in the water is reduced to hydrogen gas, releasing hydroxide ions into the solution:
2H2O + 2e H2 + 2OH
The non-permeable ion exchange membrane at the center of the cell allows the sodium ions (Na+) to pass to the second chamber where they react with the hydroxide ions to produce caustic soda (NaOH). The overall reaction for the electrolysis of brine is thus:
2NaCl + 2H2O Cl2 + H2 + 2NaOH
A membrane cell is used to prevent the reaction between the chlorine and hydroxide ions. If this reaction were to occur the chlorine would be disproportionated to form chloride and hypochlorite ions:
Cl2 + 2OH Cl + ClO + H2O
At higher temperatures, 333K, chlorate can be formed:
3Cl2 + 6OH 5Cl + ClO3 + 3H2O
Because of the corrosive nature of the chlorine produced, the anode has to be made from a non-reactive metal such as titanium, whereas the cathode can be made from Nickel.
In the membrane cell, the anode and cathode are separated by an ion-permeable membrane. Saturated brine is fed to the compartment with the anode (the anolyte). A DC current is passed through the cell and the NaCl splits into its constituent components. The membrane passes Na+ ions to the cathode compartment (catholyte), where it forms sodium hydroxide in solution. The membrane allows only positive ions to pass through to prevent the chlorine from mixing with the sodium hydroxide. The chloride ions are oxidised to chlorine gas at the anode, which is collected, purified and stored. Hydrogen gas and Hydroxide ions are formed at the cathode.
Diaphragm cell
Main article: Manufacture of Sodium hydroxide by Nelson’s process
In the diaphragm cell process, there are two compartments separated by a permeable diaphragm, often made of asbestos fibers. Brine is introduced into the anode compartment and flows into the cathode compartment. Similarly to the Membrane Cell, chloride ions are oxidized at the anode to produce chlorine, and at the cathode, water is split into caustic soda and hydrogen. The diaphragm prevents the reaction of the caustic soda with the chlorine. A diluted caustic brine leaves the cell. The caustic soda must usually be concentrated to 50% and the salt removed. This is done using an evaporative process with about three tonnes of steam per tonne of caustic soda. The salt separated from the caustic brine can be used to saturate diluted brine. The chlorine contains oxygen and must often be purified by liquefaction and evaporation.
Mercury cell
Main article: Castner-Kellner process
In the mercury-cell process, also known as the Castner-Kellner process, a saturated brine solution floats on top of the cathode which is a thin layer of mercury. Chlorine is produced at the anode, and sodium is produced at the cathode where it forms a sodium-mercury amalgam with the mercury. The amalgam is continuously drawn out of the cell and reacted with water which decomposes the amalgam into sodium hydroxide and mercury. The mercury is recycled into the electrolytic cell. Mercury cells are being phased out due to concerns about mercury poisoning from mercury cell pollution such as occurred in Canada (see Ontario Minamata disease) and Japan (see Minamata disease).
Manufacturer Associations
The interests of chloralkali product manufacturers are represented at regional, national and international levels by associations such as Euro Chlor and The World Chlorine Council.
In the Laboratory
Electrolysis can be done with two beakers, one containing a brine and one containing pure water. A salt bridge can be make of a length of bent hose (don’t use metal pipe) to connect the two beakers. Plug the ends with tissue or cloth. Put any electrode in the solution that you want to produce sodium hydroxide and hydrogen with. Put an electrode made from a carbon rod (or a pencil lead) into the solution that you want to produce the chlorine gas. If you want the hydrochloric and hypochlorous acid from the chlorine dissolution, put its electrode in the pure water solution. If you want the sodium hydroxide and hydrogen gas, put its electrode into the pure water solution. Connect the “any” electrode to the negative terminal of a 12 volt power supply.
See also
Gas diffusion electrode
External links
Chloralkali Electrolysis (Archived 2009-10-31)
Encyclopedia article
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Articles related to electrolysis
Principles of electrolysis
Electrochemical cell Electrolytic process Faraday’s laws of electrolysis Half cell High-temperature electrolysis High pressure electrolysis Regenerative fuel cell Solid oxide electrolyser cell Unitized regenerative fuel cell Standard electrode potential
Electrolytic processes
Betts electrolytic process Castner process Castner-Kellner process Chloralkali process Downs cell Electrolysis of water Electrowinning Hall-Hroult process Hofmann voltameter Kolbe electrolysis
Materials produced by electrolysis
Aluminium (extraction) Calcium metal Chlorine Copper Electrolysed water Fluorine Hydrogen Lithium metal Magnesium Potassium metal Sodium metal Sodium hydroxide Zinc
See also
Electrochemistry Gas cracker Standard electrode potential (data page)
Categories: Chemical processes | Unit processes | Electrolysis
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