Everything about Chlorite totally explained
:
This discusses some chlorine compounds. Chlorite is also a type of mineral; see chlorite group.
The
chlorite ion is ClO
2−. A
chlorite (compound) is a compound that contains this group,
with
chlorine in
oxidation state +3. Chlorites are also known as
salts of
chlorous acid.
Oxidation states
Chlorine can assume oxidation states of −1, +1, +3, +5, or +7 corresponding to the anions Cl
−, ClO
−, ClO
2−, ClO
3−, or ClO
4−, respectively (known as chloride, hypochlorite, chlorite, chlorate, and perchlorate.)
Some chlorite compounds
Manufacture
The free acid,
chlorous acid, HClO
2, is only stable at low concentrations. Since it can't be concentrated, it isn't a commercial product. However, the corresponding sodium salt,
sodium chlorite, NaClO
2 is stable and inexpensive enough to be commercially available. The corresponding salts of heavy metals (Ag
+, Hg
+, Tl
+, Pb
2+, and also Cu
2+ and NH
4+) decompose explosively with heat or shock.
Sodium chlorite is derived indirectly from
sodium chlorate, NaClO
3. First, the explosively unstable gas
chlorine dioxide, ClO
2 is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent (for example, sodium chloride, sulfur dioxide, or hydrochloric acid). The
chlorine dioxide is then absorbed into an alkaline solution and reduced with
hydrogen peroxide, H
2O
2 yielding
sodium chlorite.
Usage
The main application of
sodium chlorite is the generation of chlorine dioxide for bleaching and stripping of textiles, pulp, and paper. It is also used for disinfection in a few municipal water treatment plants after conversion to
chlorine dioxide. An advantage in this application, as compared to the more commonly used chlorine, is that trihalomethanes are not produced from organic contaminants.
Sodium chlorite, NaClO
2 also finds application as a component of contact lens cleaning solution under the trade name purite.
Sodium chlorite, like many oxidizers, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture.
Further Information
Get more info on 'Chlorite'.
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