![]() 5.3 Reactions with other common productsĬhemistry Stability of the solid Īnhydrous sodium hypochlorite can be prepared but, like many hypochlorites, it is highly unstable and decomposes explosively on heating or friction.1.3 Decomposition to chlorate or oxygen.1.2 Equilibria and stability of solutions.With excess ammonia and sodium hydroxide, hydrazine may be generated. A common urban legend states that mixing bleach with ammonia also releases chlorine, but in reality the two chemicals react differently, producing chloramines and/or nitrogen trichloride. ![]() In particular, mixing liquid bleach with other cleaning products, such as acids found in limescale-removing products, will produce chlorine gas, which was used as a poison gas in World War I. ![]() Its corrosive properties, common availability, and reaction products make it a significant safety risk. Sodium hypochlorite is the oldest and still most important chlorine-based bleach. In solution, the compound is unstable and easily decomposes, liberating chlorine, which is the active principle of such products. Sodium hypochlorite is most often encountered as a pale greenish-yellow dilute solution referred to as liquid bleach, which is a household chemical widely used (since the 18th century) as a disinfectant or a bleaching agent. It can be crystallized as a pentahydrate NaOCl♵ HĢO, a pale greenish-yellow solid which is not explosive and is stable if kept refrigerated. The anhydrous compound is unstable and may decompose explosively. It may also be viewed as the sodium salt of hypochlorous acid. Sodium hypochlorite (commonly known in a dilute solution as bleach) is a chemical compound with the formula NaOCl or NaClO, comprising a sodium cation ( Na +
0 Comments
Leave a Reply. |
Details
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |