Sodium chlorite is a salt-based chemical that also features the element chlorine. Sodium chlorite (NaClO2) is a chemical compound used in the manufacturing of paper. It has several practical uses and is very similar to sodium chlorate, a common food additive. Most people interact with sodium chlorite frequently but do not realize it, because the chemical is rarely interacted with in large portions. While not dangerous in small amounts, large doses of sodium chlorite can be dangerous.

Sodium chlorite(CAS.NO:7758-19-2) is the product of three elements: sodium (Na), chlorine (Cl) and oxygen. In each molecule, one sodium atom and one chlorine atom bind with two oxygen atoms. The chemical equation for this composition is NaClO2. It is found in solid form as a white powder and is also water-soluble. Under high heat, it can be explosive.

In its dried state, sodium chlorite (NaClO 2 ) is a white or light yellow-green solid. The greenish tint comes from trace amounts of CdO2 or iron, which are production residuals. Sodium chlorite has a molecular weight of 90.44 and decomposes at about 392°F (200°C). It is generally soluble in water, but its solubility increases as the temperature of the water rises. Sodium chlorite is a powerful oxidizer that will not explode on percussion. The anhydrous salt does not absorb water and is stable for up to ten years.
Sodium chlorite is used for a variety of applications. It is used as a disinfectant and purification chemical for water. It is also employed as a textile-bleaching and water anti-fouling agent. Additionally, it is used in the paper and electronics manufacturing industries as a bleaching agent.
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).
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.

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) and will also ignite if combined with a strong reducing agent.
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. A dose of 10-15 grams of sodium chlorate can be lethal.
While sodium chlorite is safe in low dosages, it can be harmful to your health if consumed in dosages larger than half a teaspoon. If this occurs, you should begin drinking water immediately and continue drinking to dilute the chemical. Call Poison Control for step-by-step guidance and, if needed, medical help. Health Science Spirit also recommends added half a teaspoon of soda bicarbonate with every glass drank. You can also consider inducing vomiting after drinking several glasses. Be aware that sodium chlorite can irritate the eyes and should not come in contact with them.