Cadmium acetate carbonate

Cadmium Acetate. Cadmium acetate [543-90-8], Cd(CH3COO)2 vdLO, can exist as the anhydrous salt (n = 0) mp 256°C, d = 2.341 g/mL or as one of a series of hydrates (n = 1-3). The anhydrous material may be prepared by treating cadmium nitrate with acetic anhydride or by very careful heating and drying the dihydrate at 130°C. The cadmium acetate dihydrate [5743-044], d = 2.01 g/mL, is obtained by dissolving cadmium metal or its oxide, hydroxide, or carbonate in acetic acid and crystallizing. Cadmium acetate monohydrate [543-90-8] may be obtained from the dihydrate by careful drying. All acetates are very soluble in water and alcohols. 

Peng er a/.6 "71 have proposed the use of greener Cd sources such as cadmium oxide, carbonate and acetate instead of the dimethylcadmium. These workers suggest that the size distribution of the nanocrystals is improved by the use of hexadecylamine, a long-chain phosphonic acid or a carboxylic acid. The method can be extended to prepare CdS nanoparticles by the use of tri-n-octylphosphine sulfide (TOP-S) and hexyl or telradecyl phosphonic acid in mixture with TOPO-TOP. Hyeon and coworkers71 have prepared nanocrystals of several metal sulfides such as CdS, ZnS, PbS, and MnS with different shapes and sizes by the thermolysis of metal-oleylamine complexes in the presence of S and oleylamine (Fig. 7). 

Cadmium carbonate suspension (freshly precipitated). To 20 ml of 0 5m cadmium acetate add 20 ml of 0 5m sodium carbonate solution. Allow the precipitate to settle and wash 4-5 times with water by decantation. 

Peng et al. [328-331] have proposed the use of greener Cd sources such as cadmium oxide, carbonate or acetate instead of the pyrophoric... 

Procedure. Boil the fibre in 30 per cent sulphuric acid and trap the carbon disulphide set free in a U-tube (Fig. 40) filled with a 1 per cent ethanolic solution of diethylamine. Trap the hydrogen sulphide in a tube containing cadmium acetate solution, incorporated between the sulphuric acid and sample and the trapping U-tube. Determine the diethyldithiocarbamate formed polarographically, using the anodic wave of the mercury salt formation, as in the determination of carbon disulphide given in Chapter VI. 

In a second method air (500 litres) is drawn at 33.3 litres per minute through a glass-fibre pad treated with cadmium acetate and sodium sulphide. The pad is then removed for determination of mercury. The active carbon or the cadmium sulphide pad is ignited in the apparatus of Sargeant et al, the absorbent replacing the iodised carbon and the mineral wool being omitted. The color produced on selenium sulphide test paper is compared with a color chart. Both methods are applicable to the determination of ethylmercury dicyanidiamide, The first method only, is applicable to diethylmercury. 

Cadmium is a transition metal in group IIB of the periodic table of elements. The metal is bluish-white to silver-white. At room temperature, it has a hexagonal close-packed crystal structure. Eight stable isotopes are known to be present in natui . The atomic weight of cadmium is 112.4 and the atomic number 48. The density at 25°C is 8.6 g/cm the melting point 321°C and the boiling point 765°C. The most common oxidation state is +2. " The most important compounds are cadmium acetate, cadmium sulfide, cadmium sulfoselenide, cadmium stearate, cadmium oxide, cadmium carbonate, cadmium sulfate, and cadmium chloride. The acetate, chloride, and sulfate are soluble in water, whereas the oxide and sulfide are almost insoluble. ... 

Carbonate is measured by evolution of carbon dioxide on treating the sample with sulfuric acid. The gas train should iaclude a silver acetate absorber to remove hydrogen sulfide, a magnesium perchlorate drying unit, and a CO2-absorption bulb. Sulfide is determined by distilling hydrogen sulfide from an acidified slurry of the sample iato an ammoniacal cadmium chloride solution, and titrating the precipitated cadmium sulfide iodimetrically. 

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. 

Dimethyl ketals and enol ethers are stable to the conditions of oxime formation (hydroxylamine acetate or hydroxylamine hydrochloride-pyridine). Thioketals and hemithioketals are cleaved to the parent ketones by cadmium carbonate and mercuric chloride. Desulfurization of thioketals with Raney nickel leads to the corresponding methylene compounds, while thioenol ethers give the corresponding olefin. In contrast, desulfurization of hemithioketals regenerates the parent ketone. ... 

Codeposition of silver vapor with perfluoroalkyl iodides at -196 °C provides an alternative route to nonsolvated primary perfluoroalkylsilvers [272] Phosphine complexes of trifluaromethylsilver are formed from the reaction of trimethyl-phosphme, silver acetate, and bis(trifluoromethyl)cadmium glyme [755] The per-fluoroalkylsilver compounds react with halogens [270], carbon dioxide [274], allyl halides [270, 274], mineral acids and water [275], and nitrosyl chloride [276] to give the expected products Oxidation with dioxygen gives ketones [270] or acyl halides [270] Sulfur reacts via insertion of sulfur into the carbon-silver bond [270] (equation 188)... 

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