Oxidation using hypochlorite

The conversion in high yield of aromatic compounds to arene oxides using hypochlorite and phase transfer catalysts. S. Krishnan, D. G. Kuhn, H. F. Fonouni and G. A. Hamilton, Abstracts of the American Chemical Society Meeting, Chicago, August 1977... 

Other strong base reactions such as Michael additions, aldol condensations, Wittig reactions, Darzens condensations, carbene reactions Oxidations using hypochlorite, hydrogen peroxide, oxygen, permanganate Epoxidations... 

Chlorine dioxide is usually used in aqueous solution. It is a weaker oxidant than hypochlorite. Unlike chlorine it does not react with water to form hypochlorite or with amines to form A/-chloro compounds. Thus chlorine dioxide is easily removed from solutions by passing air through the solution or its headspace. Chlorine dioxide solutions decompose by equation 12 ... 

Oxidation under moderate conditions (83) yields soUd products referred to as oxyceUuloses. This general term describes various products that must be qualified by indicating the oxidant employed. Among oxidants used are periodate, dinitrogen tetroxide, and sodium hypochlorite. CeUulose is particularly susceptible to oxidation under alkaline conditions. 

It was not their reactivity but their chemical inertness that was the true surprise when diazirines were discovered in 1960. Thus they are in marked contrast to the known linear diazo compounds which are characterized by the multiplicity of their reactions. For example, cycloadditions were never observed with the diazirines. Especially surprising is the inertness of diazirines towards electrophiles. Strong oxidants used in their synthesis like dichromate, bromine, chlorine or hypochlorite are without action on diazirines. Diazirine formation may even proceed by oxidative dealkylation of a diaziridine nitrogen in (186) without destruction of the diazirine ring (75ZOR2221). The diazirine ring is inert towards ozone simple diazirines are decomposed only by more than 80% sulfuric acid (B-67MI50800). 

Raschig s industrial oxidation of NH3 to N2H4 using hypochlorite. 

Ordinary alkenes (without an allylic OH group) have been enantioselectively epoxidized with sodium hypochlorite (commercial bleach) and an optically active manganese-complex catalyst. Variations of this oxidation use a manganese-salen complex with various oxidizing agents, in what is called the Jacobsen-Katsuki... 

Chlorine is used to make laundry bleach, such as Clorox, by dissolving chlorine in sodium hydroxide to give a weak solution of sodium hypochlorite. Sodium hypochlorite slowly releases an active form of oxygen, which reacts with many forms of soil and dirt to destroy them by oxidation. Sodium hypochlorite also rapidly destroys bacteria, viruses, and molds. 

Oxidations Using Oxoammonium Ions. Another oxidation procedure uses an oxoammonium ion, usually derived from the stable nitroxide tetramethylpiperidine nitroxide, TEMPO, as the active reagent.31 It is regenerated in a catalytic cycle using hypochlorite ion32 or NCS33 as the stoichiometric oxidant. These reactions involve an intermediate adduct of the alcohol and the oxoammonium ion. 

For producing bromates, oxidation with hypochlorite as shown here is a useful reaction ... 

Chemical oxidation using ozone, hydrogen peroxide, potassium permanganate or sodium hypochlorite (in the case of relatively low concentrations)... 

Oxidation using ozone, potassium permanganate, hydrogen peroxide or sodium hypochlorite... 

Sodium hypochlorite NaOCl is a strong oxidizer used in swimming pools, and when diluted to 5.25%, it is known as the laundry bleach Clorox. 

The oxidation of aryl diazoates with oxidants like hypochlorite, permanganate and ferri-cyanide anion has seen some limited use for the synthesis of nitramines. This method finds use for the synthesis of arylnitramines where aromatic ring nitration is not required and so excludes the use of standard nitrating agents. 

The hypochlorite ion may be identified most distinctly by ion chromatography. Its concentration in the aqueous solution combined as CIO and molecular CI2 (which is partly formed when hypochlorite is dissolved in water) can be measured by iodometric titration. A measured volume of sodium hypochlorite solution is added to a small volume of an acidified solution of potassium iodide (in excess). Iodine liberated is titrated with a standard solution of sodium thiosulfate or phenyl arsine oxide using starch as indicator. Blue color of starch solution decolorizes at the end point. 

Elemental composition Na 15.34%, I 84.66%. Aqueous solution is analyzed for sodium by AA or ICP and for iodide ion by ion chromatography or leuko-crystal violent colorimetry (See Iodine). Alternatively, in an acidified solution of sodium hypochlorite, a measured amount of sodium iodide is titrated against a standard solution of sodium thiosulfate or phenyl arsine oxide using starch indicator to detect the end point. 

Among oxidizers used have been sodium hypochlorite, potassium permanganate, and hydrogen peroxide. Bisulfite is commonly used in the wet milling of corn (maize) and in processing wines, fruit juices, jams, and dried fruits. 

Although NaI04 or KI04 are the secondary oxidants used in the vast majority of cases in which alcohols are oxidized with catalytic Ru04, the employment of sodium hypochlorite (NaOCl),31 sodium bromate (NaBrOj )32 or Cl+, electrolytic-ally generated by oxidation of chloride ion,33 have also been reported. 

Care is necessary in using hypochlorite solutions to destroy cyanide wastes by oxidation to cyanates. This reaction goes readily, even at high pH, but the secondary oxidation of cyanate to nitrogen and carbon dioxide is very pH dependent. This is slow at pH 11 but runs away at 10—10.3, with subsequent sudden release of nitrogen... 

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