Sodium chlorite

Sodium chlorite

Names
IUPAC name Sodium chlorite
Other names Chlorous acid, sodium salt Textone
Identifiers
CAS Number	7758-19-2 Y 49658-21-1 (trihydrate) N
3D model (Jmol)	Interactive image
ChEBI	CHEBI:78667 N
ChemSpider	22860 Y
ECHA InfoCard	100.028.942
EC Number	231-836-6
KEGG	C19523 N
PubChem	23668197
RTECS number	VZ4800000
UNII	G538EBV4VF Y
UN number	1496
InChI InChI=1S/ClHO2.Na/c2-1-3;/h(H,2,3);/q;+1/p-1 Y Key: UKLNMMHNWFDKNT-UHFFFAOYSA-M Y InChI=1/ClHO2.Na/c2-1-3;/h(H,2,3);/q;+1/p-1 Key: UKLNMMHNWFDKNT-REWHXWOFAT
SMILES [Na+].[O-]Cl=O
Properties
Chemical formula	NaClO2
Molar mass	90.442 g/mol (anhydrous) 144.487 g/mol (trihydrate)
Appearance	white solid
Odor	odorless
Density	2.468 g/cm3, solid
Melting point	anhydrous decomposes at 180–200 °C trihydrate decomposes at 38 °C
Solubility in water	75.8 g/100 mL (25 °C) 122 g/100 mL (60 °C)
Solubility	slightly soluble in methanol, ethanol
Acidity (pKa)	10-11
Structure
Crystal structure	monoclinic
Thermochemistry
Std enthalpy of formation (ΔfHo298)	-307.0 kJ/mol
Pharmacology
ATC code	D03AX11 (WHO)
Hazards
Safety data sheet	ICSC 1045
NFPA 704	0 1 1 OX
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	350 mg/kg (rat, oral)
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 otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Sodium chlorite (NaClO₂) is a chemical compound used in the manufacturing of paper and as a disinfectant.

Use

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 of municipal water treatment plants after conversion to chlorine dioxide.^[1]:2 An advantage in this application, as compared to the more commonly used chlorine, is that trihalomethanes (such as chloroform) are not produced from organic contaminants.^[1]:25,33 Chlorine dioxide generated from sodium chlorite is approved by FDA under some conditions for disinfecting water used to wash fruits, vegetables, and poultry.^[2]

Sodium chlorite, NaClO₂, sometimes in combination with zinc chloride, also finds application as a component in therapeutic rinses, mouthwashes,^[3][4] toothpastes and gels, mouth sprays,^[5] as preservative in eye drops,^[6] and in contact lens cleaning solution under the trade name Purite.

Under the brand name Oxine it is used for sanitizing air ducts and HVAC/R systems and animal containment areas (walls, floors, and other surfaces).

Neuraltus Pharmaceuticals is investigating a drug that they refer to as NP001 for treatment of amyotrophic lateral sclerosis. Some people with ALS have concluded that NP001 is a formulation of sodium chlorite, and are ordering the chemical and self-dosing outside of any scientific study. Preliminary results suggest that this sodium chlorite treatment is less effective than NP001.^[7] One seller of “Miracle Mineral Solution” (a mixture of sodium chlorite and water also known as "MMS") was recently convicted in the United States for marketing a toxic chemical as a miracle cure, as sodium chlorite cannot be legally sold for human consumption in the country.^[8]

Chemical reagent

In organic synthesis, sodium chlorite is frequently used as a reagent in the Pinnick oxidation for the oxidation of aldehydes to carboxylic acids. The reaction is usually performed in monosodium phosphate buffered solution in the presence of a chlorine scavenger (usually 2-methyl-2-butene).^[9]

Recently, sodium chlorite has been used as an oxidizing agent to convert alkyl furans to the corresponding 4-oxo-2-alkenoic acids in a simple one pot synthesis.^[10]

Acidified sodium chlorite

Mixing sodium chlorite solution with a weak food-grade acid solution (commonly citric acid), both stable, produces short-lived acidified sodium chlorite (ASC) which has potent decontaminating properties. Upon mixing the main active ingredient, chlorous acid is produced in equilibrium with chlorite anion. The proportion varies with pH, temperature, and other factors, ranging from approximately 5–35% chlorous acid with 65–95% chlorite; more acidic solutions result in a higher proportion of chlorous acid. Chlorous acid breaks down to chlorine dioxide which in turn breaks down to chlorite anion and ultimately chloride anion. ASC is used for sanitation of the hard surfaces which come in contact with food and as a wash or rinse for a variety of foods including red meat, poultry, seafood, fruits and vegetables. Because the oxo-chlorine compounds are unstable when properly prepared, there should be no measurable residue on food if treated appropriately.^[11][12] ASC also is used as a teat dip for control of mastitis in dairy cattle.^[13]

Army

The U.S. Army Natick Soldier Research, Development, and Engineering Center produced a portable "no power required" method of generating chlorine dioxide, known as ClO₂, gas, described as one of the best biocides available for combating contaminants, which range from benign microbes and food pathogens to Category A Bioterror agents. In the weeks after the 9/11 attacks when terrorists sent anthrax in letters to public officials, hazardous materials teams used ClO₂ to decontaminate the Hart Senate Office Building, and the Brentwood Postal Facility.^[14]

Safety

Sodium chlorite, like many oxidizing agents, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture. The chemical is highly stable in pure form and does not explode on percussive impact (unless organic contaminants are present, e.g. a greasy hammer striking the chemical on an anvil)^[15] and will also ignite if combined with a strong reducing agent.

Toxicity

Sodium chlorite is a strong oxidant and can therefore be expected to cause clinical symptoms similar to the well known sodium chlorate: methemoglobinemia, hemolysis, renal failure.^[16] A dose of 10-15 grams of sodium chlorate can be lethal.^[17] Methemoglobemia had been demonstrated in rats and cats,^[18] and recent studies by the EMEA have confirmed that the clinical symptomatology is very similar to the one caused by sodium chlorate in rats, mice, rabbits, and green monkeys.^[19]

There is only one human case in the medical literature of chlorite poisoning.^[20] It seems to confirm that the toxicity is equal to sodium chlorate. From the analogy with sodium chlorate, even small amounts of about 1 gram can be expected to cause nausea, vomiting and even life-threatening hemolysis in Glucose-6-Phosphate Dehydrogenase deficient persons.

The EPA has set a maximum contaminant level of 1 milligram of chlorite per liter (1 mg/L) in drinking water.^[21]

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 explosive (only at concentrations greater than 10% in atmosphere) chlorine dioxide, ClO₂ is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent (for example, sodium sulfite, 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.

General 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

References

External links

• International Chemical Safety Card 1045