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Arsenic chloride reactions

When heated in air at 800°C AS4S4 vapors begin to dissociate to AS2S2 which then ignites to form arsenic oxides. Ignition in chlorine produces arsenic chloride. Reaction with fluorine forms arsenic trifluoride. It is stable in water and also in the air at ambient temperatures. It does not react with hot concentrated HCl but is decomposed by nitric acid. It forms thioarsenite ion, AsS3 and elemental arsenic when warmed with caustic soda solution. Similar reaction occurs with sodium sulfide. [Pg.68]

Nitrophenylarsonic acid has been prepared by heating p-nitrobenzenediazonium chloride with arsenious acid in hydrochloric acid, by the action of -nitrobenzenediazonium chloride on sodium arsenite, by the action of sodium arsenite on sodium -nitrobenzeneisodiazo oxide, by the diazotization of -nitro-aniline in acetic acid in the presence of arsenic chloride and cuprous chloride, and by the reaction of -nitrobenzenediazonium borofluoride with sodium arsenite in the presence of cuprous chloride. ... [Pg.62]

In 1869 Bettendorff recorded 1 the formation of a voluminous brown precipitate when stannous chloride was added to a solution of arsenious oxide, or of magnesium ammonium arsenate, in hydrochloric acid. The precipitate proved to be arsenic (96 to 99 per cent.) with traces of tin which were irremovable. The speed of precipitation depends upon the amount of arsenic present and the temperature. With solutions containing little arsenic, Bettendorff observed, on warming, a yellow colour before the precipitate appeared, but he was unable to prove that the colour was due to arsenic. The reaction involved may be represented thus—... [Pg.28]

Inorganic arsenic complexes based on oxygen ligands is scarce. Simple esters of arsenic acid, As(0)(0R)3 (R = Me, Ft, n-Pr, n-Bu, CeHn) have tetragonal structures. Reaction of the diol ligand 2,4-dimethyl-2,4-pentanediol with AsCfr affords an arsenic chloride complex in which the As atom is part of a six-membered ring (37). ... [Pg.240]

Pope and Turner have also determined the optimum conditions for carrying out this reaction. They recommend heating the triphenyl arsine in an open vessel to 350° C. and then allowing the arsenic chloride to enter from a tap-funnel terminating in a capillary tube. [Pg.307]

American Method. The process used by the Americans at Edgewood Arsenal for the manufacture of phenarsazine chloride is based on the reaction of diphenylamine with arsenic chloride ... [Pg.321]

The dihalides, RgShHaLg, may be obtained by heating mercury diphenyl with antimony trichloride at a high temperature in an autoclave, or as by-products in the preparation of triarylstibmes by the Fittig reaction. Halogens also add on directly to triarylstibines, gi nng the dihalides, and in the case of chlorine, the following chlorides may replace the free element in the preparation copper, iron, thallium, phosphorus or arsenic chloride. [Pg.199]

That report mentioned the reaction of arsenic chloride and acetylene and a tarry very poisonous substance that was produced. We now know this to be Lewisite oxide, or Ml oxide, one of the concerns at the AUES owing to its toxicity and stable nature. Capt. Lewis continues ... [Pg.197]

To a mixture of 0.1 mol aromatic amine, 10 g sulfuric acid, and 28 g arsenous chloride (AsCls) in 250 mL absolute alcohol cooled at 0°C was added an equivalent amount of saturated aqueous solution of sodium nitrite, using starch-iodide paper to protect the end point. Then, and not before, 1 g cuprous bromide was added to the mixture, and the resulting mixture was stirred vigorously. The solution was warmed to 60° C until no more nitrogen was evolved, then the reaction mixture was steam distillated to afford the corresponding arsonic acid, which can be further purified via recrystallization. [Pg.225]

Colloidal Silver Halides. — Hydrosols of silver chloride, bromide, and iodide were prepared by Lottermoser and E. v. Meyer 1[ by treating colloidal silver with the corresponding halogen. They were very sensitive to electrolytes. Another theoretically interesting method has also been worked out by Lottermoser. 11 It is based on the effect of silver nitrate on the silver halides. By this method have been prepared colloidal solutions of silver chloride, bromide, iodide, cyanide, ferro and ferricyanides, phosphate and arsenate. The reaction is particularly interesting because it can be followed by measurement. It may be carried out in two ways. Either a measured amount of silver nitrate is treated Avith dilute solutions of the alkali halides, or silver nitrate from a buret is added to a known amount of the halide. In the first there must be an excess of the silver ion and in the second an excess of the halide ion in order to obtain a hydrosol. If too much of the lesser constituent is added precipitation results. [Pg.179]

Poisons for the nickel catalyst are sulfur, arsenic, chlorides or other halogens, phosphates. and copper or lead. A 15 percent nickel catalyst is poisoned at 775°C, should the gas contain 0.005 percent sulfur. This is equivalent to reaction of all the nickel on the surface of the crystallites 1 micron in diameter. For lower operating temperatures, the amount required for poisoning is even lower. When using naphtha as a feedstock, 0.5 ppm of sulfur (w/w) in the naphtha is the maximum allowed concentration for operation at 775°C. [Pg.1076]

Lewisite is reduced to elementary arsenic by reaction with ammonia up at temperatures of 1000-1100 C. Besides elementary arsenic, the products are non-toxic compounds, such as methane, nitrogen, and ammonium chloride. [Pg.85]

The success of the Bart reaction when applied to nuclear- substituted anilines is often much affected by the pH of the reaction-mixture. Furthermore, the yields obtained from some m-substituted anilines, which under the normal conditions are usually low, arc considerably increased by the modifications introduced by Scheller, and by Doak, in which the diazotisation is carried out in ethanolic solution followed by reaction with arsenic trichloride in the presence of a cuprous chloride or bromide catalyst. [Pg.312]

Bromide ndIodide. The spectrophotometric determination of trace bromide concentration is based on the bromide catalysis of iodine oxidation to iodate by permanganate in acidic solution. Iodide can also be measured spectrophotometricaHy by selective oxidation to iodine by potassium peroxymonosulfate (KHSO ). The iodine reacts with colorless leucocrystal violet to produce the highly colored leucocrystal violet dye. Greater than 200 mg/L of chloride interferes with the color development. Trace concentrations of iodide are determined by its abiUty to cataly2e ceric ion reduction by arsenous acid. The reduction reaction is stopped at a specific time by the addition of ferrous ammonium sulfate. The ferrous ion is oxidi2ed to ferric ion, which then reacts with thiocyanate to produce a deep red complex. [Pg.232]

Arsenic trichloride (arsenic(III) chloride), AsQ. is the most common and important haUde of arsenic. It may be formed by spontaneous combination of the elements and, in addition, by the following reactions (/) chlorine with arsenic trioxide (2) sulfur monochloride, 82(11, or a mixture of S2CI2 chlorine, with arsenic trioxide and (J) arsenic trioxide with concentrated hydrochloric acid or with a mixture of sulfuric acid and a chloride. [Pg.333]

Caution Because tellurium compounds have toxic effects similar to those of arsenic compounds care should be taken not to bring tellurium tetrachloride and its reaction products into contact with the skin. Avoid breathing fumes and dust of tellurium compounds. In addition, hydrogen chloride is evolved in Step A, and pyrophoric Raney nickel is used in Step B. Therefore all manipulations described in this procedure must be carried out in an efficient fume hood. [Pg.18]


See other pages where Arsenic chloride reactions is mentioned: [Pg.86]    [Pg.72]    [Pg.345]    [Pg.628]    [Pg.851]    [Pg.996]    [Pg.1003]    [Pg.1005]    [Pg.31]    [Pg.515]    [Pg.86]    [Pg.303]    [Pg.121]    [Pg.167]    [Pg.167]    [Pg.44]    [Pg.71]    [Pg.108]    [Pg.3288]    [Pg.195]    [Pg.205]    [Pg.830]    [Pg.334]    [Pg.336]    [Pg.339]    [Pg.222]    [Pg.149]    [Pg.356]    [Pg.48]    [Pg.316]   
See also in sourсe #XX -- [ Pg.3 , Pg.252 ]




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