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In particular, this reaction occurs in sodium hypochlorite solutions at high temperatures, forming sodium chlorate and sodium chloride: [22] [23] 3 NaOCl(aq) → 2 NaCl(aq) + NaClO 3 (aq) This reaction is exploited in the industrial production of sodium chlorate. An alternative decomposition of hypochlorite produces oxygen instead: 2 OCl − ...
Inorganic chloramines are produced by the reaction of ammonia and hypochlorous acid or chlorine. An urban legend claims that mixing household bleach (aqueous sodium hypochlorite) with ammonia-based cleaners releases chlorine gas or mustard gas; in reality, the gas produced by the reaction is a mixture of inorganic chloramines.
Hypochlorite salts are formed by the reaction between chlorine and alkali and alkaline earth metal hydroxides. The reaction is performed at close to room temperature to suppress the formation of chlorates. This process is widely used for the industrial production of sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(ClO) 2).
The Olin Raschig process is a chemical process for the production of hydrazine.The main steps in this process, patented by German chemist Friedrich Raschig in 1906 and one of three reactions named after him, are the formation of monochloramine from ammonia and hypochlorite, and the subsequent reaction of monochloramine with ammonia towards hydrazine. [1]
In dilute aqueous solution, chloramine is prepared by the reaction of ammonia with sodium hypochlorite: [5] NH 3 + NaOCl → NH 2 Cl + NaOH. This reaction is also the first step of the Olin Raschig process for hydrazine synthesis. The reaction has to be carried out in a slightly alkaline medium (pH 8.5–11).
When acids are added to aqueous salts of hypochlorous acid (such as sodium hypochlorite in commercial bleach solution), the resultant reaction is driven to the left, and chlorine gas is formed. Thus, the formation of stable hypochlorite bleaches is facilitated by dissolving chlorine gas into basic water solutions, such as sodium hydroxide.
Sodium hypochlorite solution, 3–6%, (common household bleach) is typically diluted for safe use when disinfecting surfaces and when used to treat drinking water. [31] [32] A weak solution of 2% household bleach in warm water is typical for sanitizing smooth surfaces before the brewing of beer or wine. [citation needed]
For example, the label of a household bleach product may specify "5% sodium hypochlorite by weight." That would mean that 1 kilogram of the product contains 0.05 × 1000 g = 50 g of NaClO. A typical oxidation reaction is the conversion of iodide I − to elemental iodine I 2. The relevant reactions are NaClO + 2 H + + 2 I − → NaCl + H 2 O ...