Hypochlorites are the salts of hypochlorous acid. Common examples include sodium hypochlorite (chlorine bleach or bleaching agent) and calcium hypochlorite (bleaching powder). Hypochlorites are frequently quite unstable — for example, sodium hypochlorite is not available as a solid, since removal of the water from NaClO solution converts it to a mixture of sodium chloride and sodium chlorate. Heating of NaClO solution also causes this reaction. Hypochlorites decompose in sunlight, giving chlorides and oxygen.
Due to their low stability, hypochlorites are very strong oxidizing agents. They react with many organic and inorganic compounds. Reaction with organic compounds is very exothermic and may cause ignition, so hypochlorites should be handled with care. They can oxidize manganese compounds, converting them to permanganates.
Strength of oxidation
Hypochlorite is the strongest oxidizer of the generalized chlorates. It is also the least stable.Stability
Many hypochlorite compounds exist only in solution, and are nonexistent in a pure form, as is hypochlorous acid (HClO) itself.Besides oxidizing almost any reducing agent, hypochlorite is unstable with respect to disproportionation (that is, it will oxidize itself); hypochlorite will often degrade to some mixture of chloride and other chlorates, especially if not kept cool.
This article is licensed under the GNU Free Documentation License.
Last updated on Tuesday September 23, 2008 at 17:06:44 PDT (GMT -0700)
View this article at Wikipedia.org - Edit this article at Wikipedia.org - Donate to the Wikimedia Foundation
|
|
|
|
|
|
|
|
|
|
|
Copyright © 2009, Dictionary.com, LLC. All rights reserved.
