Chlorine oxide 8-hydrate

Mercury(II) oxide Chlorine, hydrazine hydrate, hydrogen peroxide, hypophosphorous acid, magnesium, phosphorus, sulfur, butadiene, hydrocarbons, methanethiol... 

A salt of this composition was obtained by dehydration of the 6-hydrate.67 It melts at 210°C, with the evolution of chlorine oxides. 

SYNS ALCIDE ANTHIUM DIOXIDE CHLORINE DIOXIDE, not hydrated pOTl CHLORINE OXIDE CHLORINE(TV) OXIDE CHLORINE PEROXIDE CHLOROPEROXYL CHLORYL RADICAL DOXCIDE 50... 

Excellent reviews of CO hydrogenation, chlorination, nitration, sulfo-chlorination, oxidation, dehydrogenation, extractive distillation, hydration, synthetic lubricants, etc. 

Removal of iron(II) and manganese(II) ions by oxidation of the bivalent ions with air, or if necessary, with chlorine and separation of the oxide hydrates formed. Dissolved carbon dioxide also expelled during air oxidation... 

The zinc salt solutions, which currently mainly come from zinc and copper smelters, contain impurities which have to be completely removed prior to use, because all heavy metals form colored sulfides. For the purification step the solution is oxidized with chlorine (pH 4), which precipitates most of the iron and manganese as the oxide-hydrate and part of the cobalt, nickel and cadmium present as their hydroxides. In the second step, the elements nobler than zinc (Ni, Co, Cd, In, Tl, Pb, Cu, Ag) are precipitated as their metals by adding zinc dust and the metals returned to the copper smelters for noble metal extraction. After purification the solutions are adjusted to a particular zinc content. Mixtures of zinc sulfate and zinc chloride solutions are used for manufacturing lithopone types with more than 30% ZnS. 

Chlorine is applied as chlorine gas, powdered calcium hypochlorite (Ca(OCl)2), or liquid sodium hypochlorite (NaOCl bleach). Chlorine reacts with the organic (natural organic matter, NOM) or inorganic (bromide ion, Br ) precursors in the water to form chlorine disinfection by-products (CBPs), including trihalomethanes (THMs), haloacetic acids (HAAs), haloacetonitriles (HANs), haloketones, chloral hydrate, and chloropicrin. Humic and fulvic acids are the predominant NOMs. When bromine exists, the chlorine oxidizes it to hypobromous acid/ hypobromite ion (HOBr/OBr ) to form bromo THMs (bromodichloromethane, BDCM, and di-bromochloromethane, DBCM), HAAs, and HANs. 

The Diels-Alder reaction was utilized to construct bicyclo [2.2 1]heptane or bicyclo[2 2 l]heptene structures The reaction of isopropylidenecyclopentadiene with maleic anhydride produced the endo and exo configurational isomers of 8-isopropylidenebicyclo[2.2.1] hept-2-ene-5,6-dicarboxylic anhydride Similar reactions were applied to unsubstituted and l-(methoxycarbonyl)cyclopentadienes to give the corresponding anhydrides The anhydrides were reduced to alcohols, which were then allowed to react with thionyl chloride or tosyl chloride to give cyclic sulfites or tosylates Reaction of the tosylates with lithium chloride gave chlorinated compounds Hydration of the double bonds of the chlorinated compounds was accomplished by hydroboration-oxidation Diol 31 thus obtained was converted to 5,6-bis(chloromethyl)-7-isopropylidene-bicyclo[2 2 1] heptan-2-one [33] by chromium trioxide oxidation of the secondary hydroxyl group followed by dehydration at the C-7 substituent. 

CHLORINE DIOXIDE or CHLORINE DIOXIDE, HYDRATE, FROZEN (10049-04-4 70377-94-5) ClOj-xHiO ClOj (gas) A self-reactive and explosive oxidizing gas. 

On the other hand, a gas that is already largely free of such impurities as Og and chlorine oxides is produced by the reaction of hydrated manganese dioxide with pure hydrochloric acid. For this preparation, see method n below. 

Earlier studies made Mosander suspect that cerium oxide obtained from cerite contains a foreign substance. He attempted to separate it by shaking cerium oxide hydrate with water, introducing chlorine gas to transform cerium oxydul into cerium oxide and the unknown substance into chlorure. Insoluble yellow cerium oxide was precipitated in the operation. From the filtrate he again precipitated the solute with potassium hydrate, shook the suspension and again introduced chlorine gas. Further cerium oxide was precipitated and the rest was dissolved. He repeated this operation several times, in this manner he succeeded to separate the total amount of cerium oxide and obtain a chlorure from which potassium hydrate precipitated a hydrate that did not turn yellow in air and when treated with chlorine, was completely soluble in water. Thus the separation was terminated, and the oxide which is not further oxidized by chlorine gas was termed lanthanum oxide, as generally known. 

Only one halide - the white bismuth chloride oxide q.v) - appears to have been used significantly as a pigment. However, Salter (1869) describes a purple compound (bismuth purple) prepared by passing chlorine through a bismuth oxide hydrate suspension in aqueous potash the precise composition is unknown. 

A problem with sodium hypochlorite is its ability to chlorinate some compounds to form volatile reaction products. Ammonia and alkylamines, for example, can be chlorinated to form chloramines. The problem can be avoided by removing alkaline nitrogen compounds from the gas stream with an acid wash prior to the sodium hypochlorite scrubber. An alternative approach described by Valentin (1990) is the use of a catalyst in the scrubber liquid to promote oxidation. Hydrated nickelic oxide, which is formed in solution from nickel sulfate and sodium hypochlorite at a pH of 9 to lO.S, is recommended. A nickel concentration of 50-75 ppm is said to be effective, making removal of up to 95% of the odorous compounds possible in a single stage. 

Antimony oxide, hydrated alumina, halogenated hydrocarbons Petroleum oils (aromatic and napthenic), esters, chlorinated paraffins, polymeric polyesters... 

CCls CHO. A colourless oily liquid with a pungent odour b.p. 98°C. Manut actured by the action of chlorine on ethanol it is also made by the chlorination of ethanal. When allowed to stand, it changes slowly to a white solid. Addition compounds are formed with water see chloral hydrate), ammonia, sodium hydrogen sulphite, alcohols, and some amines and amides. Oxidized by nitric acid to tri-chloroethanoic acid. Decomposed by alkalis to chloroform and a methanoate a convenient method of obtaining pure CHCI3. It is used for the manufacture of DDT. It is also used as a hypnotic. 

Examples include luminescence from anthracene crystals subjected to alternating electric current (159), luminescence from electron recombination with the carbazole free radical produced by photolysis of potassium carba2ole in a fro2en glass matrix (160), reactions of free radicals with solvated electrons (155), and reduction of mtheiiium(III)tris(bipyridyl) with the hydrated electron (161). Other examples include the oxidation of aromatic radical anions with such oxidants as chlorine or ben2oyl peroxide (162,163), and the reduction of 9,10-dichloro-9,10-diphenyl-9,10-dihydroanthracene with the 9,10-diphenylanthracene radical anion (162,164). Many other examples of electron-transfer chemiluminescence have been reported (156,165). 

Tin does not react directly with nitrogen, hydrogen, carbon dioxide, or gaseous ammonia. Sulfur dioxide, when moist, attacks tin. Chlorine, bromine, and iodine readily react with tin with fluorine, the action is slow at room temperature. The halogen acids attack tin, particularly when hot and concentrated. Hot sulfuric acid dissolves tin, especially in the presence of oxidizers. Although cold nitric acid attacks tin only slowly, hot concentrated nitric acid converts it to an insoluble hydrated stannic oxide. Sulfurous, chlorosulfuric, and pyrosulfiiric acids react rapidly with tin. Phosphoric acid dissolves tin less readily than the other mineral acids. Organic acids such as lactic, citric, tartaric, and oxaUc attack tin slowly in the presence of air or oxidizing substances. 

The action of hydrogen peroxide on freshly precipitated hydrated Ti(IV) oxide or the hydrolysis of a peroxide compound such as K2[Ti(02)(S0 2] yields, after drying, a yellow soHd, stable below 0°C, of composition TiO 2H2O. There is one peroxo group per titanium, but the precise stmcture is not known. The yellow soHd loses oxygen and water when heated and Hberates chlorine from hydrochloric acid. When freshly prepared, it is stable in acid or alkah, giving peroxy salts. 

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