Carbon chloride

An alloy of sodium and potassium (NaK) is used as a heat-transfer medium. Many potassium salts are of utmost importance, including the hydroxide, nitrate, carbonate, chloride, chlorate, bromide, iodide, cyanide, sulfate, chromate, and dichromate. 

Rubidium metal alloys with the other alkaU metals, the alkaline-earth metals, antimony, bismuth, gold, and mercury. Rubidium forms double haUde salts with antimony, bismuth, cadmium, cobalt, copper, iron, lead, manganese, mercury, nickel, thorium, and 2iac. These complexes are generally water iasoluble and not hygroscopic. The soluble mbidium compounds are acetate, bromide, carbonate, chloride, chromate, fluoride, formate, hydroxide, iodide. 

The more soluble forms of barium such as the carbonate, chloride, acetate, sulfide, oxide, and nitrate, tend to be more acutely toxic (50). Mean lethal doses for ingested barium chloride were 300—500 mg/kg in rats and 7—29 mg/kg in mice (47). 

Assay, wt % Acetate tetrahydrate Carbonate Chloride hexahydrate Hydroxide Nitrate Mixed oxide Sulfate hexahydrate Sulfate feed grade... 

The hydroxyl ions migrate inward, attracted by the positive charge that is produced by the ferrous ion generated near the corroding surface (Fig. 3.4). Other anions such as carbonate, chloride, and sulfate also concentrate beneath the shell. Carbonate may react with ferrous ions to form siderite (FeCOa) as in Reaction 3.4 (Fig. 3.7) ... 

Chlorkohlen-oxyd, n. carbonyl chloride, -oxyd-ather, m. ethyl chloroformate. -saure, /. chlorocarbonic acid (chloroformic acid, CICOOH). -sMureamtd, n. chlorocarbonyl amide (carbamyl chloride, H2NCOCI). -stoff, m. carbon chloride, carbon tetrachloride (sometimes with the adj. vierfach). 

Cupri-. cupric, copper(II). -azetst, n. cupric acetate, copper(II) acetate, -carbonat, n. cupric carbonate, copper(II) carbonate, -chlorid, n. cupric chloride, copper(II) chloride. -hydroxyd, n. cupric hydroxide, cop-per(II) hydroxide. -ion, n. cupric ion, copper(II) ion. -ozalat, n. cupric oxalate, copper(II) oxalate, -oxyd, n. cupric oxide, copper(II) oxide. -salz, n. cupric salt, copper(II) salt, -suifat, n. cupric sulfate. copper(II) sulfate, -sulfid, n. cupric sulfide, copper(II) sulfide, -verbihdung, /. cupric compound, copper(II) compound, -wein-saure, /. cupritartaric acid. 

Bicarbonate. Carbonate Chloride.. . Hydrate.. . Hypochlorite. Oxide. Sulfale. . . Sulfate. . . Nitrate. . . I hofl >hate... 

Lead usually has excellent resistance to seawater owing to the formation of a passive film of basic carbonate and carbonate-chloride double salts , which should be compared with its behaviour in solutions of alkali chlorides (see salts p. 4 87). 

Anode processes yield gaseous chlorine, fluorine, carbon chloride or fluoride. In the case of melts containing dissolved tantalum oxide, carbon oxides (mostly carbon dioxide) are formed on the graphite anode [28,37]. 

The co-precipitation technique starts with an aqueous solution of nitrates, carbonates, chlorides, oxychlorides, etc., which is added to a pH-controlled solution of NH4OH, allowing the hydroxides to precipitate immediately. This method requires water-soluble precursors and insoluble hydroxides as a final product. The hydroxides are filtered and rinsed with water when chlorides are employed as starting materials and chlorine is not desired in the final product. After drying the filtrate, it is calcined and sintered. This method is being applied very successfully for oxygen-ion conducting zirconia ceramics [30],... 

Chlorhexidine base is not readily soluble in water therefore the freely soluble salts, acetate, gluconate and hydrochloride, are used in formulation. Chlorhexidine exhibits the greatest antibacterial activity at pH 7-8 where it exists exclusively as a di-cation. The cationic nature of the compound results in activity being reduced by anionic compounds including soap and many anions due to the formation of insoluble salts. Anions to be wary of include bicarbonate, borate, carbonate, chloride, citrate and phosphate with due attention being paid to the presence of hard water. Deionized or distilled water should preferably be used for dilution purposes. Reduction in activity will also occur in the presence of blood, pus and other organic matter. 

Total dissolved solids Carbonate Chloride Nitrate Phosphate Sulphate ... 

Chlorination of oleic acid dissolved in carbon chloride was tested in a flow reactor at 12.8 C with the tabulated results (Roper, Chem Eng Sci 2 27, 1953). Chlorine (A) and oleic acid (B) were dissolved separately in CC14 and mixed in the liquid phase at the inlet to the reactor. Concentrations are gmol/liter and time is in seconds. Check a second order mechanism. 

Synonyms AI3-04705 Benzinoform Carbona Carbon chloride Carbon tet Caswell No. 164 CCRIS 123 EINECS 200-262-8 ENT 4705 ENT 27164 EPA pesticide chemical code 016501 Fasciolin Flukoids Freon 10 Halon 1040 Methane tetrachloride Necatorina Necatorine NSC 87063 Perchloromethane R 10 RCRA waste number U211 Tetrachloormetaan Tetrachloro-carbon Tetrachloromethane Tetrafinol Tetraform Tetrasol UN 1846 Univerm Vermo-estricid. 

Synonyms AI3-01719 AIDS-17533 Amatin Anticarie BRN 1912585 Bunt-cure Bunt-no-more Caswell No. 477 CCRIS 325 Co-op hexa EINECS 204-273-9 ENT 1719 EPA pesticide chemical code 061001 Granox Granox NM HCB HCBz Hexa C.B. Julen s carbon chloride Julian s carbon chloride Julin s carbon chloride Julin s chloride No bunt No bunt 40 No bunt 80 No bunt liquid NSC 9243 Pentachlorophenyl chloride Perchlorobenzene Phenyl perchloryl RCRA waste number U127 Sanocid Sanocide Smut-go Snieciotox UN 2729 Voronit C. 

Carbona, see Carbon tetrachloride Carbon bichloride, see Tetrachloroethylene Carbon bisulfide, see Carbon disulfide Carbon bisulphide, see Carbon disulfide Carbon chloride, see Carbon tetrachloride Carbon dichloride, see Tetrachloroethylene Carbon disulphide, see Carbon disulfide Carbon hexachloride, see Hexachloroethane Carbon monobrotnide trifluoride, see Bromotrifluoromethane... 

Photolytic. Low et al. (1991) reported that the photooxidation of a saturated solution of atrazine by UV light in the presence of titanium dioxide resulted in the formation of ammonium, carbonate, chloride, and nitrate ions. Evgenidou and Fytianos (2002) also studied the photodegradation of atrazine using UV light (X >290 nm) in distilled water (pH 7.1, conductivity 456 mS/cm, dissolved oxygen 8.0 mg/L, total organic carbon 0.8 mg/L), lake water (pH 8.7,... 

To disrupt the carbon-chloride bond at position 5 of the substrate anion-radical, population of this bond with an unpaired electron should be increased. However, if a spin density at carboncarrying chlorine is too great, the initial chlorine-containing anion-radicals dimerize instead of cleaving the chloride ion. Thus, in the isomeric 6-chloro-27/,3//-benzo[b]thiophenedione-2,3 anion-radical, unpaired electron density at C-6 is five times greater than at C-5, and the dimerization proceeds much more rapidly than the cleavage of carbon-chlorine bond (Alberti et al. 1981). 

The carbon content of MSW cannot be converted into C02 entirely, and due to incomplete combustion, minor amounts of CO and soot particles are found in the flue gases. The particulate carbon is known to be involved in the formation of volatile and toxic compounds especially poly-chlorodibenzo-dioxins and -furanes. Tests in the fully working incinerator plants revealed the presence of particulate carbon, chlorides, and Cu compounds as catalysts in the fly ash (see also Table 3). 

FIGURE 2.13 (a) X-ray scattering factors for hydrogen, carbon, chloride and ferrous ions (b) the neutron scattering cross sections for several elements, as a function of sinOA. 

The Preparation of a Chloride by the Action of Sulfur or Carbon Chloride upon an Oxide.—An interesting reaction, which is not a double decomposition in the usual sense, takes place when a volatile chloride of a nonmetallic element is conducted over a hot oxide or a salt of any oxygen acid. An example of such reaction is shown in the equation... 

The dissociation energies for the highlighted (by pointing arrows) carbon—chloride bonds are significantly lower than that of a normal secondary C—Cl... 

Borgford, and J. B. Ealy, "Name That Precipitate," Chemical Demonstrations, A Sourcebook for Teachers, Vol. 2 (American Chemical Society, Washington, DC, 1988), pp. 121-123. Blue, brown, red, white, and yellow precipitates are formed when solutions containing +2 cations of mercury, nickel, lead, and barium are mixed with solutions containing carbonate, chloride, iodide, and sulfate anions. Students are asked to name and determine the formula of each precipitate and to write an ionic equation for each reaction. 

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