Bleach
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A bleach is a chemical that removes color or whitens, often via oxidation. Common chemical bleaches include household "chlorine bleach", a solution of approximately 3-6% sodium hypochlorite (NaOCl), and "oxygen bleach", which contains hydrogen peroxide or a peroxide-releasing compound such as sodium perborate or sodium percarbonate. To bleach something is to apply bleach, sometimes as a preliminary step in the process of dyeing. Bleaching powder is calcium hypochlorite.
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[edit] Other types of bleaches
Chlorine dioxide is used for the bleaching of wood pulp, fats and oils, cellulose, flour, textiles, beeswax, skin, and in a number of other industries.
In the food industry, some organic peroxides (benzoyl peroxide, etc.) and other agents (e.g. bromates) are used as flour bleaching and maturing agents.
Peracetic acid, ozone and hydrogen peroxide and oxygen are used in bleaching sequences in the pulp industry to produce totally chlorine free (TCF) paper.
Not all bleaches are hazardous and have a oxidizing nature. Sodium dithionite is used as a powerful reducing agent in some bleaching formulas. It is commonly used to bleach wood pulp used to make newsprint.
[edit] Hazards
Since bleaches are strong oxidizing agents, they can be quite hazardous, especially when reacted with other common household chemicals.
Mixing sodium hypochlorite with acids like vinegar or drain cleaners containing sodium bisulfate (sodium hydrogen sulfate), or even lemon juice can release chlorine. Hypochlorite and chlorine are in equilibrium in water, the position of the equilibrium is pH dependant and low pH (acidic) favors chlorine,[1]
Cl2 + H2O 
H+ + Cl- + HClO
Chlorine is a respiratory irritant that attacks mucous membranes and burns the skin. As little as 3.5 ppm can be detected as an odor, and 1000 ppm is likely to be fatal after a few deep breaths. Exposure to chlorine has been limited to 0.5 ppm (8-hour time-weighted average—40 hour week) by OSHA in the U.S.[2]
Sodium hypochlorite and ammonia react to form a number of products, depending on the temperature, concentration, and how they are mixed. [3]. The main reaction is chlorination of ammonia, first giving chloramine (NH2Cl), then NHCl2 and finally nitrogen trichloride (NCl3). These materials are very irritating to eyes and lungs and are toxic above certain concentrations.
NH3 + NaOCl --> NaOH + NH2Cl
NH2Cl + NaOCl --> NaOH + NHCl2
NHCl2 + NaOCl --> NaOH + NCl3
Additional reactions produce hydrazine, in a variation of the Olin Raschig process.
NH3 + NH2Cl + NaOH --> N2H4 + NaCl + H2O
The hydrazine generated can further react with the monochloramine in an exothermic reaction:[1]
2 NH2Cl + N2H4 --> 2 NH4Cl + N2
Industrial bleaching agents can also be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines, persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under detectable levels.[4] However, respiratory risk from chlorine and highly toxic chlorinated byproducts still
[edit] Chemistry
The process of bleaching can be summarised in the following set of chemical reaction:
Cl2(aq) + H2O(l) H+(aq) + Cl-(aq) + HClO(aq)
The H+ ion of the hypochlorous acid then dissolves into solution, and so the final result is effectively:
Cl2(aq) + H2O(l) 2H+(aq) + Cl-(aq) + ClO-(aq)
[edit] Mechanism of bleach action
Color in most dyes and pigments is produced by molecules, such as beta carotene, which contain chromophores. Chemical bleaches work in one of two ways:
- An oxidizing bleach works by breaking the chemical bonds that make up the chromophore. This changes the molecule into a different substance that either does not contain a chromophore, or contains a chromophore that does not absorb visible light.
- A reducing bleach works by converting double bonds in the chromophore into single bonds. This eliminates the ability of the chromophore to absorb visible light.[5]
Sunlight acts as a bleach through a process leading to similar results: high energy photons of light, often in the violet or ultraviolet range, can disrupt the bonds in the chromophore, rendering the resulting substance colorless. Extended exposure often leads to massive discoloration usually reducing the colors to white and typically very faded blue spectrums.[6]
[edit] See also
[edit] References
- ^ a b Cotton, F.A; G. Wilkinson (1972). Advanced Inorganic Chemistry. John Wiley and Sons Inc. ISBN 0-471-17560-9.
- ^ Occupational Safety & Health Administration (2007). and peroxide/recognition.html OSHA -- Chlorine. OSHA. Retrieved on 2007-08-26.
- ^ Rizk-Ouaini, Rosette & Ferriol, Michel; Gazet, Josette; Saugier-Cohen Adad, Marie Therese (1986), “Oxidation reaction of ammonia with sodium hypochlorite. Production and degradation reactions of chloramines.”, Bulletin de la Societe Chimique de France 4: 512–21
- ^ ECF: The Sustainable Technology. Alliance for Environmental Technology. Retrieved on 2007-09-19.
- ^ Field, Simon Q (2006). Ingredients -- Bleach. Science Toys. Retrieved on 2006-03-02.
- ^ Bloomfield, Louis A (2006). Sunlight. How Things Work Home Page. Retrieved on 2006-03-02.
[edit] Further reading
- Bodkins, Dr. Bailey. Bleach. Philadelphia: Virginia Printing Press, 1995.
- Trotman, E.R. Textile Scouring and Bleaching. London: Charles Griffin & Co., 1968. ISBN 0852640676.
- Book in numerical format Knew you that?
[edit] External links
