Cupric chlorid nitrate

Effect on the reaction of copper(II) from salts—cupric chloride, nitrate, acetate, and sulfate. 

CUPRIC CHLORATE CUPRIC CHLORIDE CUPRIC NITRATE CUPRIC OXALATE CUPRIC SULFATE... 

Aluminium sulphate Ammonium bifluoride Ammonium bisulphite Ammonium bromide Ammonium persulphate Antimony trichloride Beryllium chloride Cadmium chloride Calcium hypochlorite Copper nitrate Copper sulphate Cupric chloride Cuprous chloride Ferric chloride Ferric nitrate... 

The reaction shows a first-order dependence on substrate concentration but, except at very low concentration, is zero-order with respect to oxidant moreover, the zero-order rate coefficient is the same as that observed with oxidations by iodine, cupric chloride and silver nitrate. The reaction is acid-catalysed. The oxidation is completely analogous to the halogenation of ketones and involves a slow tautomeric equilibrium followed by rapid oxidation, viz. 

Most corrosion processes in copper and copper alloys generally start at the surface layer of the metal or alloy. When exposed to the atmosphere at ambient temperature, the surface reacts with oxygen, water, carbon dioxide, and air pollutants in buried objects the surface layer reacts with the components of the soil and with soil pollutants. In either case it gradually acquires a more or less thick patina under which the metallic core of an object may remain substantially unchanged. At particular sites, however, the corrosion processes may penetrate beyond the surface, and buried objects in particular may become severely corroded. At times, only extremely small remains of the original metal or alloy may be left underneath the corrosion layers. Very small amounts of active ions in the soil, such as chloride and nitrate under moist conditions, for example, may result, first in the corrosion of the surface layer and eventually, of the entire object. The process usually starts when surface atoms of the metal react with, say, chloride ions in the groundwater and form compounds of copper and chlorine, mainly cuprous chloride, cupric chloride, and/or hydrated cupric chloride. 

Other Methods of Preparation.—Ethyl 2-(D-ara6i no-tetrahydroxybutyl)-5-methyl-4-furoate has been prepared by heating D-glucose plus ethyl acetoacetate in aqueous alcohol without a catalyst,1 or from the same reagents (1 g. and 0.5 ml., respectively) in 0.5 ml. of 96% ethanol plus 1.5 ml. of water at room temperature in the presence of ferric chloride, zinc chloride (with small quantities of hydrochloric acid or of sodium hydroxide), cupric chloride, ferric sulfate, zinc sulfate, aluminum chloride, nickel chloride, or cobalt nitrate.18... 

Arsine reacts with cupric chloride solution to give cupric arsenide. Oxidation with stannic chloride, SnCR, forms hydrogen diarsenide, AS4H2. It reacts with dilute silver nitrate solution forming metallic silver. 

Hydrofluoric acid like water is an associated liquid, and even the gas, as we shall soon see, is associated. It has the power of uniting with fluorides. It also seems to be an ionizing solvent for a soln. of potassium fluoride in liquid hydrogen fluoride is an excellent conductor it also possesses marked solvent powers. According to E. C. Franklin,7 the liquid readily dissolves potassium fluoride, ehloride, and sulphate sodium fluoride, bromide, nitrate, chlorate, and bromate acetamide and urea. The solvent action is not so marked with barium fluoride, cupric chloride, and silver cyanide while calcium and lead fluorides copper sulphate and nitrate ferric chloride, mercuric oxide, and magnesium metal, are virtually insoluble in this menstruum. Glass also is not affected by the liquid if moisture be absent. The liquid scarcely acts on most of the metals or non-metals at ordinary temp., though it does act on the alkali metals at ordinary temp., much the same as does water, with the simultaneous production of flame. 

Even the comparatively unreactive phenoxazine and phenothiazine systems undergo halogenation and nitration with ease and it is normal to prepare monosubstituted derivatives by stepwise procedures rather than by direct electrophilic attack. Indeed, the nitration of phenoxazine is uncontrollable and even N-acylphenoxazines afford a mixture of di- and tetra-nitro products (03CB475). Similarly phenothiazine and nitric acid produce a complex mixture of nitrated sulfoxides and sulfones. Chlorine in DMSO at 40 °C reacts with phenothiazine to yield 3,7-dichlorophenothiazine, whereas cupric chloride gives the 1,7-isomer (76JPR353). Direct bromination of phenoxazine produces a mixture of 3-bromo- and 3,7-dibromo-phenoxazines, while thionyl chloride affords the 1,3,7,9-tetrachloro derivative (60ZOB1893). 

Cupric arsenate, Cu3(As04)2.—The arsenate occurs as pentahydrate under the name trichalcite. The tetrdhydrate is produced by heating cupric nitrate with calcium arsenate, or copper with a solution of arsenic acid,1 and also by the interaction of cupric chloride and silver arsenate.2 Concentration at 70° C. of a solution of cupric carbonate in excess of arsenic acid yields pale-blue leaflets of the formula CuHAsO 4,H20.3 Other acidic salts,4 and also basic salts,5 are known. 

Silver subchloride, AgaCl.—When silver subfluoride is heated with phosphorus trichloride at 140° C., silver subchloride is formed.8 It is also a product of the interaction of silver nitrate and cuprous chloride, of a colloidal solution of silver and chlorine-water,9 and of silver-foil and weak oxidizers such as cupric chloride. 

In alkaline solution oxidation of ferrous iron is fairly rapid,8 but certain acids retard the reaction. Ferrous sulphate, for example, in the presence of free sulphuric acid, is very stable in air. Concentrated hydrochloric acid assists the oxidation, as also do traces of certain substances, such as platinic and cupric chlorides, palladium nitrate, etc.9... 

The rates of reaction of hypophosphorous acid with iodine bromine ", chlorine ", iodine chlorides , iodate , selenious and tel-lurous acids, silver nitrate , cupric chloride and mercuric chloride" (all forming phosphorous acid or phosphites) have been measured, and the results of the earlier work summarized clearly" . All the data are consistent with the hypothesis that there is prior transformation to some reactive form (I). This form (I) does not discriminate very effectively between different oxidants and thus the oxidation steps are presumed to have rates close to the diffusion-controlled limit. The rates of formation of I deduced in these studies are close enough to the rates of deuterium and tritium exchange for the residual difference to represent an isotope effect. Mitchell wrote the formula H5PO3 for I. Others have supposed it to be a tautomer e.g. HPO(OH)2. Both the isotopic exchange results and the oxidation studies require that its formation and decomposition be subject to acid catalysis. For the general mechanism... 

A silver (or copper) catalyst suitable for the oxidation of methanol may also be prepared by heating silver or copper cyanide or a mixture of these in the presence of air to the point where puffing occurs. By incorporating a fervo- or ferri-cyanide, e.g., bismuth ferro-cyanide, bismuth ferri-cyanide, calcium cerium ferro-cyanide, cerium cobalt ferro-cyanide, vanadium or molybdenum ferro-cyanide with the starting material, an activated product may be obtained. The silver or copper cyanides are prepared by precipitating a soluble cyanide with silver nitrate or cupric chloride respectively.30... 

ACETIC ACID, COBALT(II) SALT (71-48-7) Co(CjH30j)i 4HOH Noncombustible solid. Solution in water is basic (pH 6.8 to >7.0) reacts with acids. Some cobalt compounds react with oxidizers, acetylene. Cobalt is a known animal carcinogen. ACETIC ACID, CUPRIC SALT (142-71-2) Cu(C2H302)i H20 Noncombustible solid. Solution in water is basic reacts with acids. Incompatible with acetylides, hydrazine, nitromethane, mercurous chloride nitrates, sodium hypobromite. Thermal decomposition releases fumes of copper, acetic acid, and carbon oxides. 

CUPRIC DIACETATE (142-71-2) Cu(CjH30i)j Hj0 Noncombustible solid. Solution in water is basic reacts with acids. Incompatible with acetylides, hydrazine, nitromethane, mercurous chloride nitrates, sodium hypobromite. Thermal decomposition releases fiimes of copper, acetic acid, and carbon oxides. 

Nugatory attempts to render the metal active by the addition of cupric chloride, sodium sulphite, alcohol, ferrous chloride, ferric chloride, colloidal platinum, chromic acid, potassium nitrite prolonged contact with metallic platinum variation of temp, between 0 and 50° previous treatment of the metal with chromic acid or potassium permanganate fusion with potassium nitrate heating on charcoal with sodium phosphate to give the metal a phosphorus content melting in the electric oven in an atm. of coal-gas using the metal as anode have all been made. 

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