Cobaltic salts nitrate

Ammonium tetrathiocyanatomercurate(II)-cobalt sulphate test This test is similar to that described under reaction 8, except that a minute amount of a dilute solution of a cobalt salt (nitrate, sulphate or acetate) is added. Coprecipitation of the cobalt tetrathiocyanatomercurate(II) yields a blue precipitate composed of mixed crystals of Zn[Hg(SCN)4] + Co[Hg(SCN)4], Iron(II) salts give a red colouration but this can be eliminated by the addition of a little alkali fluoride (colourless [FeF6]3- ions are formed). Copper salts should be absent. 

A fermentation such as that of Pseudomonas dentrificans typicaby requires 3—6 days. A submerged culture is employed with glucose, comsteep Hquor and/or yeast extract, and a cobalt source (nitrate or chloride). Other minerals may be required for optimal growth. pH control at 6—7 is usuaby required and is achieved by ammonium or calcium salts. Under most conditions, adequate 5,6-dimethylben2imida2ole is produced in the fermentation. However, in some circumstances, supplementation maybe required. 

Cobalt(Il) dicobalt(Ill) tetroxide [1308-06-17, Co O, is a black cubic crystalline material containing about 72% cobalt. It is prepared by oxidation of cobalt metal at temperatures below 900°C or by pyrolysis in air of cobalt salts, usually the nitrate or chloride. The mixed valence oxide is insoluble in water and organic solvents and only partially soluble in mineral acids. Complete solubiUty can be effected by dissolution in acids under reducing conditions. It is used in enamels, semiconductors, and grinding wheels. Both oxides adsorb molecular oxygen at room temperatures. 

Kobalto-. cobaltous, cobalto-, cobalt(II). -chlorid, n. cobaltous chloride, cobalt(II) chloride, -cyanwasserstoff, m., -cyanwasser-stoffs ure, /. cobaltocyanic acid, -nitrat, n. cobaltous nitrate, cobalt(II) nitrate, -oxyd, n. cobaltous oxide, cobalt (II) oxide, -salz, n. cobaltous salt, cobalt(IJ) salt, -sulfat, n. cobaltous sulfate, cobalt(II) sulfate, -sulfid, n. cobaltous sulfide, cobalt (II) sulfide, -verbindung, /. cobaltous compound. cobalt(II) compound. 

Subcategory A encompasses the manufacture of all batteries in which cadmium is the reactive anode material. Cadmium anode batteries currently manufactured are based on nickel-cadmium, silver-cadmium, and mercury-cadmium couples (Table 32.1). The manufacture of cadmium anode batteries uses various raw materials, which comprises cadmium or cadmium salts (mainly nitrates and oxides) to produce cell cathodes nickel powder and either nickel or nickel-plated steel screen to make the electrode support structures nylon and polypropylene, for use in manufacturing the cell separators and either sodium or potassium hydroxide, for use as process chemicals and as the cell electrolyte. Cobalt salts may be added to some electrodes. Batteries of this subcategory are predominantly rechargeable and find application in calculators, cell phones, laptops, and other portable electronic devices, in addition to a variety of industrial applications.1-4 A typical example is the nickel-cadmium battery described below. 

Evaporation by heating a filtrate from precipitation of potassium cobaltinitrite caused it to turn purple and explode violently [1]. This was attributed to interaction of nitrite, nitrate, acetic acid and residual cobalt with formation of fulminic or methylnitrolic acids or their cobalt salts, all of which are explosive [2], Mixtures containing nitrates, nitrites and organic materials are potentially dangerous, especially in presence of acidic materials and heavy metals. A later publication confirms the suggestion of formation of nitro- or nitrito-cobaltate(III) [3],... 

In the complex [Co(NH3)6]Cl3, the cation is [Co(NH3)6]3+, and it is named first. The coordinated ammonia molecules are named as ammine, with the number of them being indicated by the prefix hexa. Therefore, the name for the compound is hexaamminecobalt(III) chloride. There are no spaces in the name of the cation. [Co(NH3)5C1]C12 has five NH3 molecules and one CN coordinated to Co3+. Following the rules just listed leads to the name pentaamminechlorocobalt(III) chloride. Potassium hexacyanoferrate(III) is K3[Fe(CN)6j. Reinecke s salt, NH4[Cr(NCS)4(NH3)2], would be named as ammonium diamminetetrathiocyanatochro mate (III). In Magnus s green salt, [Pt(NH3)4][PtCl4], both cation and anion are complexes. The name of the complex is tetraammineplatinum(II) tetrachloroplatinate(II). The compound [Co(en)3](N03)3 is named as tris(ethylenediamine)cobalt(III) nitrate. 

Complexes of butyl vinyl sulfoxide and iron, chromium and cobalt (III) nitrates were found to be unstable, the ferric salt (the least stable) exploding even as a 40 mol% solution in benzene. It is considered that other vinyl sulfoxide ligands will behave similarly. 

Nitrato-pentammino-cobaltic Nitrate, [Co(NH3)5N03](N03)2. —If an aqueous ammoniacal solution of eobaltous nitrate be oxidised by means of air and then heated with excess of ammonium nitrate, the nitrato-salt is formed. It is more easily prepared by dissolving eobaltous carbonate in warm dilute nitric acid and then warming the mixture with concentrated aqueous ammonia. Iodine is thereafter added, one atom for every atom of cobalt in solution, and the whole warmed until the iodine dissolves and a precipitate of hexammino-cobaltic iodido-nitrate is formed. It is filtered and the residue washed W ith dilute aqueous ammonia. The filtrate is treated with nitric acid, and the precipitate of aquo-pentammino-nitrate is converted into the nitrato-salt by heating with more nitric acid. The change from aquo-1 JOrgensen, J. prakt. Chem., 1881, 23, 227. 

The dithionate, [Rh(NH3)5N03]S206.H20, is precipitated from a saturated solution of the nitrate or chloride on the addition of a solution of sodium dithionate. It crystallises in white silky needles resembling the corresponding cobalt salt, and is insoluble in water. 

Synonym Gamma-Chloropropylene Oxide 3-Chloro-1,2-Propylene Oxide Chlorosulfonic Acid Chlorothene Chiorotoluene, Alpha Alpha-Chlorotoluene Omega-Chlorotoluene Chlorotrifluoroethylene Chlorotrimethylsilane Chlorsulfonic Acid Clilorylen Clip Chromic Acid Chromic Anhydride Chromic Oxide Chromium (VI) Dioxychloride Chromium Oxychloride Chromium Trioxide Chromyl Chloride Cianurina Citric Acid Citric Acid, Diammonium Salt Clarified Oil Clorox Cc Ral Coal Tar Oil Cobalt Acetate Cobalt Acetate Tetrahydrate Cobalt (II) Acetate Cobalt Chloride Cobalt (II) Chloride Cobaltous Acetate Cobaltous Chloride Cobaltous Chloride Dihydrate Cobaltous Chloride Hexahydrate Cobaltous Nitrate Cobaltous Nitrate Hexahydrate Cobaltous Sulfate Heptahydrate Cobalt Nitrate Cobalt (II) Nitrate Cobalt Sulfate Compound Name Epichlorohydrin Epichlorohydrin Chlorosulfonic Acid Trichloroethane Benzyl Chloride Benzyl Chloride Benzyl Chloride Trifluorochloroethylene Trimethylchlorosilane Chlorosulfonic Acid Trichloroethylene Cumene Hydroperoxide Chromic Anhydride Chromic Anhydride Chromic Anhydride Chromyl Chloride Chromyl Chloride Chromic Anhydride Chromyl Chloride Mercuric Cyanide Citric Acid Ammonium Citrate Oil Clarified Sodium Hypochlorite Coumaphos Oil Coal Tar Cobalt Acetate Cobalt Acetate Cobalt Acetate Cobalt Chloride Cobalt Chloride Cobalt Acetate Cobalt Chloride Cobalt Chloride Cobalt Chloride Cobalt Nitrate Cobalt Nitrate Cobalt Sulfate Cobalt Nitrate Cobalt Nitrate Cobalt Sulfate... 

Saturating the electrolyte with iron(lll) hydroxide (e.g., by addition of aqueous solutions of ferric nitrate) and simultaneously adding cobaltous salts leads to in situ formation of a mixed Fe(llI)/Co(ll)/Co(IIl) deposit, which exhibits catalytic activity comparable to that of Fe304 shown by the current voltage curve in Fig. 11. Such mixed oxidic catalyst coatings are composed of very small oxide crystals, which evidently are dissolved upon current interruption due to dissociative oxide dissolution. The transfer of dissolved metal ions to the cathode followed by cathodic deposition of the metal, however, can be completely prohibited, if the potential of the cathode due to optimal electrocatalysis of cathodic hydrogen evolution proceeds with an over-... 

The increase in the rate of decomposition under the influence of added Cr203 and K2Cr207 is shown on Figs. 171 and 172 respectively.lt has been found that an increase of the rate occurred only at temperatures near to the melting point of the samples. Guiochon [17] also found that cobalt salts increase the rate of thermolysis of ammonium nitrate. Other mineral salts (of manganese, nickel and copper) have a similar but much weaker action. A large number of salts of other metals are without any noticeable action. 

A mixture of 0.05 mole of a cobalt salt (14.5g of the nitrate or 12g of the chloride—both 6-hydrate) and 21g of potassium thiocyanate are heated in 30ml of water until solution is complete. The dark blue liquid is cooled in ice until crystallization of potassium nitrate or chloride is complete and then suction-filtered. The residue is washed repeatedly with 10ml portions of ethyl acetate until it is... 

Compounds containing the cation [Co(NH3)6NO]++ are obtained when aqueous cobalt(II) salt solutions containing ammonia are saturated with nitrogen(II) oxide.1 These compounds are either black or pink, depending upon the conditions used in their preparation. The black chloride and iodate are formed in the absence of air,2-4 whereas many members of the pink series are obtained in the presence of air.2-4 The method of preparation for the black chloride described here is a composite of those recommended by various authors1-5 and gives a product of considerable stability. The same reaction, using cobalt(II) nitrate, when run in the presence of air and at room temperature, may be used for the preparation of the pink nitrate. This may be converted into the pink chloride by treatment with concentrated hydrochloric acid.3... 

A solution of 300 g. of cobalt (II) nitrate 6-hydrate (1.03 mols) in 150 ml. of water is thoroughly mixed with a solution of 450 g. of ammonium carbonate (4.68 mols) in 450 ml. of water and 750 ml. of concentrated aqueous ammonia (sp. gr. 0.90, 28% NH3). A stream of air is bubbled slowly through the mixture for 24 hours. After the mixture has been cooled in an ice-salt bath overnight, the product is collected on a filter, washed with not more than 50 ml. of ice-... 

Ten grams of carbonatopentamminecobalt(III) nitrate (0.036 mol) is suspended in 25 ml. of water, and 20 ml. of colorless nitric acid (1 1 concentrated acid and water) is added with stirring. When the evolution of carbon dioxide has stopped (10 minutes), 100 ml. of methanol is added, the aquopentammine cobalt (III) nitrate is collected on a filter, and washed with alcohol and ether. This salt is heated at 100° for 18 hours (until 1 mol of water is lost), yielding 10 g. (83 %) of the desired material. Anal. Calcd. for [Co(NH3) 6-N03](N03)2 NHs, 25.8. Found NH3, 25.6. 

Classical methods for the synthesis of frans-dinitro-bis(ethylenediamine)cobalt(III) nitrate involve conversion of the cis isomer by heat1 or action of sodium nitrite on frans-chloronitrobis(othylenediamine)cobalt(III) nitrate.2 These methods involve isolation of intermediate coordination compounds and consequently are subject to low yields, based upon original cobalt(II) salt. The following procedure for the preparation of the trans compound gives an 84% yield it depends upon oxidation of cobalt(II) to cobalt(III) in the presence of sodium nitrite, ethylene-diamine, and nitric acid. 

A vigorous stream of air i drawn or passed through the solution. The yellow precipitate after a few minutes, and the reaction is complete in about 20 minutes. The mixture is cooled in an ice-salt bath and filtered. The yellow crystalline solid is recrystallized from boiling water, washed with alcohol and ether, and air-dried. The yield of rans-dinitrobis (ethylenediamine) cobalt (111) nitrate is 11.2 g. (84%, based on cobalt(II) nitrate 6-hydrate). Anal. Calcd. for [Coen2(N02)2]N03 Co, 17.7 N, 29.44. Found Co, 17.5 N, 29.52. 

Cobalt Sesquioxide, Co203, results when cobalt nitrate is gently heated to 180° C.4 It is a black, amorphous powder, of density 518. Hydrogen begins to reduce it at 182° C.5 It may be regarded as the cobalt salt of cobaltous acid, namely, cobaltous cobaltile, CoCo03. 

At 55° C. nickel nitrate has nearly the same solubility as the corresponding cobalt salt. 

The synthesis of pentaammine(carbonato)cobalt(III) salts is readily accomplished by an air-oxidation method starting with cobalt(II) nitrate and ammonium carbonate in aqueous ammonia.1 However, a suitable general method for making other types of monodentate amino(carbonato) metal salts is not available in the literature. The air-oxidation technique can be applied only to complexes where the ligands are all ammonia molecules or where the central metal ion is cobalt. 

Triphenyl phosphite (15.5 g., 0.050 mole) is added to a solution of cobalt(II) nitrate hexahydrate (2.91 g., 0.010 mole) in ethanol (60 ml.). Sodium tetrahydroborate (1.0 g.) is dissolved in warm ethanol (25 ml.) and the solution cooled rapidly to room temperature. The sodium tetrahydroborate solution is added dropwise over a period of 10 minutes to the well-stirred cobalt nitrate solution. The purple color of the cobalt(II) salt rapidly discharges, and a pale yellow precipitate deposits. After stirring for a further 10 minutes the product is filtered off, washed with ethanol, and dried in vacuo. Yield is 11.0 g. (85%). The product may be further purified by dissolving in the minimum volume of benzene and reprecipitating by drop-wise addition of methanol. Anal. Calcd. for C72H61C0O12P4 C, 66.48 H, 4.74 P, 9.52. Found C, 66.60 H, 4.47 P, 9.21%. The tri-p-tolyl phosphite complex can be prepared (85% yield) by an analogous route. Anal. Calcd. for C84H85C0O12P4 C, 68.64 H, 5.84. Found C, 68.74 H, 5.92%. 

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