Oxidation calcium hypochlorite

Carbon, activated Calcium hypochlorite, oxidizing agents... 

The reaction below shows how calcium hypochlorite oxidizes dissolved manganese and converts it to manganese oxide, an insoluble solid ... 

Chlorine is the basis for the most commonly used bleaches, for example the solution of sodium hypochlorite, which is so ubiquitous that many people just call it bleach, and calcium hypochlorite. Oxidizing bleaching agents that do not contain chlorine are often based on peroxides, such as hydrogen peroxide, sodium percarbonate, and sodium perborate. 

Two oxidants commonly used are chlorine and potassium permanganate. The Roe chlorine number, the uptake of gaseous chlorine by a known weight of unbleached pulp (ie. Technical Association of the Pulp and Paper Industry (TAPPl) Standard Method T202 ts-66) has been superseded by the simpler hypo number (ie, TAPPl Official Test Method T253 om-86), eg, chlorine consumption in treatment of the pulp with acidified sodium or calcium hypochlorite. 

Thiol spills are handled ia the same manner that all chemical spills are handled, with the added requirement that the odor be eliminated as rapidly as possible. In general, the leak should be stopped, the spill should be contained, and then the odor should be reduced. The odor can be reduced by sprayiag the spill area with sodium hypochlorite (3% solution), calcium hypochlorite solution (3%), or hydrogen peroxide (3—10% solution). The use of higher concentrations of oxidant gives strongly exothermic reactions, which iacrease the amount of thiol ia the vapor, as well as pose a safety ha2ard. The apphcation of an adsorbent prior to addition of the oxidant can be quite helpful and add to the ease of cleanup. 

Potassium peroxymonosulfate, introduced in the late 1980s, is finding increasing use as an auxiUary oxidant for shock treatment and oxidation of chloramines. Sodium peroxydisulfate is also being sold for shock treatment, however, it is less reactive than peroxymonosulfate. Mixtures of sodium peroxydisulfate and calcium hypochlorite can be used for shock treatment (28). Disadvantages of peroxymonosulfate and peroxydisulfate are they do not provide a disinfectant residual and peroxymonosulfate oxidizes urea and chloramines to nitrate ion, which is a nutrient for algae. 

Dichlorides and e2thers are the main by-products in this reaction. Treatment with base produces propylene oxide. Specialty epoxides, eg, butylene oxide, are also produced on an industrial scale by means of HOCl generated from calcium hypochlorite and acetic acid followed by dehydrohalogenation with base. 

Oxidizing bleaches kill microbes by reacting with cell membranes and cell proteins. The most widely used is sodium hypochlorite for household and hospital uses, and calcium hypochlorite for drinking water and swimming pool disinfecting. 

Primary and secondary amines and amides are first chlorinated at nitrogen by the chlorine released by the gradually decomposing calcium hypochlorite. Excess chlorine gas is then selectively reduced in the TLC layer by gaseous formaldehyde. The reactive chloramines produced in the chromatogram zones then oxidize iodide to iodine, which reacts with the starch to yield an intense blue iodine-starch inclusion complex. 

This oxide catalyses the violent or even explosive decomposition of hydrogen peroxide. This reaction explains the numerous accidents mentioned involving the contact of hydrogen peroxide with rusted iron. Two accidents of this nature dealt with mixtures of hydrogen peroxide with ammonia and an alkaline hydroxide The detonations took place after a period of induction of respectively several hours and four minutes. Iron (III) oxide also catalyses the explosive decomposition of calcium hypochlorite. 

Stability Unstable in air. Protect from water or moisture. Store away horn heat or ignition sources and sulfur compounds. Reacts with sulfur and sulfur compounds, producing highly toxic VX or VX-like compounds. It completely dissolves polymethylmethacrylate. It is incompatible with calcium hypochlorite (HTH), many chlorinated hydrocarbons, selenium, selenium compounds, moisture, oxidants, and carbon tetrachloride. 

Calcium oxide Carbon, activated Chlorates Water Calcium hypochlorite Ammonium salts, acids, metal powders, sulphur, finely-divided organics or combustibles... 

See Dinitrogen oxide or Halogens, both above Oxygen, below Calcium hypochlorite Acetylene Nitric acid Acetylene, Mercury(II) salts Nitrogen oxide Dienes, Oxygen Ozone Acetylene... 

Sodium 1,3-dichloro-1,3,5 -triazine-2,4-dione-6-oxide See Sodium l,3-dichloro-l,3,5-triazine-2,4-dione-6-oxide Calcium hypochlorite... 

Sodium chlorite reacts very violently with organic compounds of divalent sulfur, or with free sulfur (which may ignite), even in presence of water. Contact of the chlorite with rubber vulcanised with sulfur or a divalent sulfur compound should therefore be avoided [1]. Application of factorial design techniques to experimental planning gave specific conditions for the safe oxidation of organic sulfides to sulfoxides using sodium chlorite or calcium hypochlorite [2],... 

Although solutions of sodium hypochlorite are useful oxidizing agents, the solid is not very stable. Calcium hypochlorite is used in bleaches, swimming pool treatments, and so forth. The decomposition of OC1- is catalyzed by compounds containing transition metals. 

Diamond occurring in the blue ground of volcanic pipes as well as freshly pulverized diamond show hydrophobic behavior. This is used in its isolation by flotation. Diamond found in sediments is hydrophilic, however. According to Plaksin and Alekseev (154), hydrophobic diamond turns slowly hydrophilic on storing with exposure to air. Hofmann (155) reported that fine particle size diamond forms stable suspensions in dilute ammonia after treatment with calcium hypochlorite. It seems rather obvious that formation of surface oxides is responsible for the hydrophilic properties. 

Oxidizers may not themselves be combustible, but they may provide reaction pathways to accelerate the oxidation of other combustible materials. Combustible solids and liquids should be segregated from oxidizers. Certain oxidizers undergo dangerous reactions with specific noncombustible materials. Some oxidizers, such as calcium hypochlorite, decompose upon heating or contamination and self-react with violent heat output. Oxidizers include nitrates, nitric acid, nitrites, inorganic peroxides, chlorates, chlorites, dichromates, hypochlorites, perchlorates, permanganates, persulfates and the halogens. 

Table 6.2 shows the important applications of sodium hydroxide. Direct applications can be further broken down into pulp and paper (24%), soaps and detergents (10%), alumina (6%), petroleum (7%), textiles (5%), water treatment (5%), and miscellaneous (43%). Organic chemicals manufactured with sodium hydroxide are propylene oxide (23%), polycarbonate (5%), ethyleneamines (3%), epoxy resins (3%), and miscellaneous (66%). Inorganic chemicals manufactured are sodium and calcium hypochlorite (24%), sodium cyanide (10%), sulfur compounds (14%), and miscellaneous (52%). As you can see from the number of applications listed, and still the high percentages of miscellaneous uses, sodium hydroxide has a very diverse use profile. It is the chief industrial alkali. 

After the crude pulp is obtained from the alkaline sulfate process, it must be bleached in stages with elemental chlorine, extracted with sodium hydroxide, and oxidized with calcium hypochlorite, chlorine dioxide, and... 

Calcium hypochlorite is an oxidizing agent. It undergoes vigorous to violent reactions with reducing agents and organics. In aqueous solution, it dissociates to calcium and hypochlorite ions. The hypochlorite ions form hypochlor-ous acid and molecular chlorine, which coexist in equilibrium. 

The hypochlorous acid oxidizes the cell walls and kills bacteria. Solid calcium hypochlorite, Ca(OCl)2, and liquid solutions of sodium hypochlorite, NaOCl, can be used to generate hypochlorous acid in place of chlorine gas, for example, in chlorinating swimming pools. The hypochlorite ion generated from Ca(OCl)2 and NaOCl forms an equilibrium with water represented by the equation ... 

Potassium chlorate Potassium chloride, Bleach (Calcium hypochlorite) Low explosive, lED filler, Black powder weapon propellant, Oxidizer... 

Many classical oxidations are frequently performed in aqueous media, using oxidants such as potassium permanganate, sodium periodate, or sodium or calcium hypochlorite (Hudlicky, 1990). Cyclohexene can now be oxidized directly to colorless crystalline adipic acid with aqueous 30 percent hydrogen peroxide under organic solvent-and halide-free conditions, as discussed earlier (Sato et al., 1998) (see fig. 6.1). 

Calcium Arsenate Calcium Phosphate Calcium Carbide Calcium Chlorate Calcium Chloride Calcium Chloride Calcium Chloride Calcium Chromate Calcium Chromate Calcium Chromate Calcium Cyanide Calcium Peroxide Calcium Fluoride Calcium Hydroxide Calcium Hypochlorite Calcium Phosphate Calcium, Metallic Calcium Nitrate Calcium Nitrate Calcium Oxide Calcium Peroxide Calcium Phosphate Calcium Phosphate Calcium Phosphide Calcium Resinate Calcium Resinate Calcium Resinate Calcium Phosphate Mercuric Chloride Mercurous Chloride... 

CALCIUM HYPOCHLORITE HTH, HTH Dry Chlorine, Sentry Oxidizing Material, II 2 0 2 oxy... 

Sodium hypochlorites (and calcium hypochlorite s) disinfection property is due to its ability to form hypochlorous acid, HOC1. The hypochlorous acid oxidizes the cell walls and kills bacteria. Sodium hypochlorite generates hypochlorous acid according to the reaction NaOCl( H2offi —> HOCl + NaOH(Ml. The hypochlorite ion generated from NaOCl exists... 

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