Sodium chlorite

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Sodium chlorite
Image:Sodium chlorite.jpg
General
Systematic name	Sodium chlorite
Other names	Sodium chlorate(III)
Molecular formula	NaClO2
Molar mass	90.44 g/mol
Appearance	white solid
CAS number	[7758-19-2]
Properties
Density and phase	2.5 g/cm3, solid
Solubility in water	39 g/100 ml (17 °C)
Melting point	180–200 °C decomp.
Structure
Coordination geometry	?
Crystal structure	?
Hazards
MSDS	External MSDS
EU classification	not listed
NFPA 704	0 1 1 OX
Flash point	non flammable
RTECS number	VZ4800000
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Related compounds
Other anions	Sodium chloride Sodium hypochlorite Sodium chlorate Sodium perchlorate
Other cations	Potassium chlorite Barium chlorite
Related compounds	Chlorine dioxide Chlorous acid
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references

Sodium chlorite is a chemical compound used in the manufacture of paper.

Contents 1 Manufacture 2 Usage 3 References: 4 External links

[edit] Manufacture

The free acid, chlorous acid, HClO₂, is only stable at low concentrations. Since it cannot be concentrated, it is not a commercial product. However, the corresponding sodium salt, sodium chlorite, NaClO₂ is stable and inexpensive enough to be commercially available. The corresponding salts of heavy metals (Ag⁺, Hg⁺, Tl⁺, Pb²⁺, and also Cu²⁺ and NH₄⁺) decompose explosively with heat or shock.

Sodium chlorite is derived indirectly from sodium chlorate, NaClO₃. First, the explosively unstable gas chlorine dioxide, ClO₂ 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, H₂O₂ yielding sodium chlorite.

[edit] 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, NaClO₂ also finds application as a component in therapeutic rinses, mouthwashes, toothpastes and gels, mouth sprays chewing gums and lozenges, and also in contact lens cleaning solution under the trade name purite.

In organic synthesis, sodium chlorite is frequently used for the oxidation of aldehydes to carboxylic acids. The reaction is usually performed in the presence of a chlorine scavenger.

Sodium chlorite, like many oxidizing agents, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture.

[edit] References:

• "Chemistry of the Elements", N.N. Greenwood and A. Earnshaw, Pergamon Press, 1984.
• "Kirk-Othmer Concise Encyclopedia of Chemistry", Martin Grayson, Editor, John Wiley & Sons, Inc., 1985

[edit] External links

• International Chemical Safety Card 1045