Chloramine
From Wikipedia, the free encyclopedia
| Chloramine | |
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| Systematic name | Chloroazane |
| Other names | Monochloramine Chloramide |
| Molecular formula | NH2Cl |
| Molar mass | 51.48 g/mol |
| CAS number | [10599-90-3] |
| Appearance | colorless |
| Density | ? g/cm3 |
| Solubility (water) | Soluble |
| Melting point | −66 °C |
| Boiling point | ? °C |
| Related compounds | Dichloramine Nitrogen trichloride |
| Disclaimer and references | |
Chloramine (monochloramine) is chemical compound with the formula NH2Cl. Although it is important, NH2Cl is invariably used as very dilute solutions where it is used as disinfectant.
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[edit] Synthesis and chemical reactions
NH2Cl is a highly unstable compound in concentrated form, much less as a pure liquid. Pure NH2Cl decomposes violently above −40 °C.[1] NH2Cl is, however, quite stable in dilute solution, and this considerable stability is the basis of its applications.
NH2Cl is prepared by the chemical reaction of ammonia and sodium hypochlorite (chlorine bleach) under mildly alkaline conditions:
- NH3 + HOCl → NH2Cl + H2O
The synthesis is conducted in dilute solution. In this reaction HOCl undergoes attack by the nucleophile NH3. At lower pH's, further chlorination occurs.
The above syntheses are useful but do not deliver NH2Cl in pure form. The pure compound can be prepared by contacting fluoroamine with calcium chloride:
- NH2F + CaCl2 → NH2Cl + CaClF
NH2Cl is a key intermediate in the traditional synthesis of hydrazine.
[edit] Uses in water treatment
NH2Cl is commonly used in low concentrations as a disinfectant in municipal water systems as an alternative to chlorination. This application is increasing. Chlorine (sometimes referred to as Free Chlorine) is being displaced by chloramine, which is much more stable and does not dissipate from the water before it reaches consumers. NH2Cl also exhibits less tendency to convert organic materials into chlorocarbons such as chloroform and carbon tetrachloride. Such compounds have been identified as carcinogens and in 1979 the U.S. EPA began regulating their levels in U.S. drinking water. Furthermore, water treated with chloramine lacks the distinct chlorine odour of the gaseous treatment and so has improved taste.
Chloramine in tap water gives a greenish cast to the water in bulk, versus the normally bluish cast to pure water or water containing only free chlorine disinfectant. This greenish color may be observed by filling a white polyethylene bucket with chloraminated tap water and comparing it to chloramine-free water such as distilled water or a sample from a swimming pool.
Chloramine can be removed from tap water by treatment with superchlorination (10 ppm or more of free chlorine, such as from a dose of sodium hypochlorite bleach or pool sanitizer) while maintaining a pH of about 7 (such as from a dose of muriatic acid). Hypochlorous acid from the free chlorine strips the ammonia from the chloramine, and the ammonia outgasses from the surface of the bulk water. This process takes about 24 hours for normal tap water concentrations of a few ppm of chloramine. Residual free chlorine can then be removed by exposure to bright sunlight for about 4 hours.
[edit] Situations where NH2Cl should be removed
Aquarium owners must remove the chloramine from their tap water because it is toxic to fish. Aging the water for a few days removes chlorine but not the more stable chloramine, which can be neutralised using products available at pet stores.
Many animals are sensitive to chloramine and it must be removed from water given to many animals in zoos.
Chloramine must also be removed from the water prior to use in kidney dialysis machines, as it would come in contact with the bloodstream across a permeable membrane. However, since chloramine is neutralized by the digestive process, kidney dialysis patients can still safely drink chloramine-treated water.
Home brewers use reducing agents such as sodium metabisulfite to remove chloramine from brewing liquor as it, unlike chlorine, cannot be removed by boiling.
[edit] Other chloramines
Dichloramine (NHCl2) and nitrogen trichloride (NCl3) can be produced by lowering the pH and adjusting the molar ratios of the reactants to favor their formation.
[edit] Safety
NH2Cl is toxic.
[edit] References
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
