III Sulfate

Submitted by Robert T. Claunch and Mark M. Jones Checked by Wayne C. WoLSEYf 

Pure anhydrous vanadium(III) sulfate can be prepared by the reduction of vanadium(V) oxide dissolved in sulfuric acid with elemental sulfur as the reducing agent.The procedure given below is an adaptation of this method. 

A 500-ml. three-necked, round-bottomed Pyrex flask is used as the reaction vessel. A glass or Teflon stirrer is inserted in the central opening and a water or air condenser 

If the length of reaction time is extended from 16 to 30 hours, larger particles of vanadium(III) sulfate are obtained which are much easier to handle. If the length of reaction time is decreased to 12 hours, a very fine powder is obtained which is very difficult to use. 

Vanadium is determined by ignition of the sulfate in air to vanadium(V) oxide. Sulfate is determined by dissolving a sample of the vanadium(III) sulfate in hot 3 N HNO3, adding about 1 ml. of 65 % hydrazine hydrate to reduce any vanadates which may have formed, and precipitating the sulfate as barium sulfate. Anal. Calcd. for V2(S04)s V, 26.12 SO4—, 73.88. Found V, 26.13 SO4 , 74.16. 

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IV) oxide sulfate (III) sulfate (III) sulfide Xenon difluoride hexafluoride tetrafluoride trioxide Ytterbium... 

III) nitrate 4-water (III) oxide (III) sulfate 8-water Yttrium chloride fluoride... 

Analytical and Test Methods. o-Nitrotoluene can be analyzed for purity and isomer content by infrared spectroscopy with an accuracy of about 1%. -Nitrotoluene content can be estimated by the decomposition of the isomeric toluene diazonium chlorides because the ortho and meta isomers decompose more readily than the para isomer. A colorimetric method for determining the content of the various isomers is based on the color which forms when the mononitrotoluenes are dissolved in sulfuric acid (45). From the absorption of the sulfuric acid solution at 436 and 305 nm, the ortho and para isomer content can be deterrnined, and the meta isomer can be obtained by difference. However, this and other colorimetric methods are subject to possible interferences from other aromatic nitro compounds. A titrimetric method, based on the reduction of the nitro group with titanium(III) sulfate or chloride, can be used to determine mononitrotoluenes (32). Chromatographic methods, eg, gas chromatography or high pressure Hquid chromatography, are well suited for the deterrnination of mononitrotoluenes as well as its individual isomers. Freezing points are used commonly as indicators of purity of the various isomers. 

Monosaccharides such as glucose and fmctose are the most suitable as starting materials. When starch is used, it is first hydrolyzed with oxahc acid or sulfuric acid into a monosaccharide, mainly glucose. It is then oxidized with nitric acid in an approximately 50% sulfuric acid solution at 63—85°C in the presence of a mixed catalyst of vanadium pentoxide and iron(III) sulfate. 

Tb allium (ITT) nitrate in nitric acid and thaHium(III) sulfate in sulfuric acid are also effective. 

Vanadium(IV) Oxysulfate. Vanadium(IV) oxysulfate pentahydrate (vanadyl sulfate), VOSO4 -5H20) is an ethereal blue sohd and is readily soluble in water. It forms from the reduction of V20 by SO2 in sulfuric acid solution. Vanadium(III) sulfate [13701 -70-7] ) is a powerful... 

Bismuth Trisulfate. Bismuth(III) sulfate [7787-68-0], Bi2(S0 3, is a colorless, very hygroscopic compound that decomposes above 405°C to yield bismuthyl salts and Bi202. The compound hydrolyzes slowly in cold water and rapidly in hot water to the yellow bismuthyl sulfate [12010-64-9], (Bi0)2S04. The normal sulfate is isomorphous with the sulfates of yttrium, lanthanum, and praseodymium. 

Indium (III) sulfate (5H2O) [17069-79-3] M 607.9, d 3.44. Dissolve in strong H2SO4 and slowly evaporate at ca 50°. Wash crystals with glacial AcOH and then heat in a furnace at a temperature of 450-500° for 6h. Sol in H2O is 5%. The pentahydrate is converted to an anhydrous hygroscopic powder on heating at 500° for 6h but heating above this temperature over N2 yields the oxide sulfate. Evaporation of neutral aqueous solutions provides basic sulfates. [J Am Chem Soc 55 1943 1933, 58 2126 1936.]... 

A 500-ml three-necked flask fitted with a mechanical stirrer and a nitrogen inlet and outlet is charged with 30 g (approx. 0.055 mole) of hydrated chromium (III) sulfate, 200 ml of distilled water, 7.5 g (0.12 g-atom) of mossy zinc, and 0.4 ml (5.4 g, 0.03 g-atom) of mercury. The flask is flushed with nitrogen for 30 minutes and a nitrogen atmosphere is maintained. The mixture is then heated to about 80° with stirring for 30 minutes to initiate reaction. Then the mixture is stirred at room temperature for an additional 30 hours, by which time the green mixture has been converted to a clear blue solution. Solutions prepared as above are about 0.55 M in chromium (II) and are indefinitely stable if protected from oxygen. 

Ammonium-ferrisulfat, n. ammonium iron(III). sulfate, ferric ammonium sulfate, -ferro-sulfat, n. ammonium iron(II) sulfate, ferrous ammonium sulfate, -jodat, n. ammonium iodate. -jodid, n. ammonium iodide, -platinchlorid, n. ammonium platinichloride (chloroplatinate). -rest, m. ammonium radical. rhodanid, -rhodantir, n. ammonium thiocyanate, -salpeter, m. ammonium nitrate, -salz, n. ammonium s t. -selfe,/. ammonia soap, -sulfhydrat, n. ammonium hydrosulfide, -sulfocyanid, n. ammonium thiocyanate, -verbindung,/. ammonium compound, -zinn-chlorid, n. ammonium chlorostannate, pink salt. 

Cero-. ceroua, cerium(III). -ion, n. ceroua ion, eerium(III) ion. -salz, n. eerous salt, cerium (III) salt, -sulfat, n. ceroua sulfate, cerium(III) sulfate. 

Chromi-nydroxyd, n. chromic hydroxide, chro-mium(III) hydroxide, -oxyd, n. chromic oxide, chromium(III) oxide, -rhodanwasser-stoffsMure, /. chromithiocyanic acid, thio-cyanatochromic(III) acid, -salz, n. chromic salt, chromium(III) salt, -suifat, n. chromic sulfate, chromium(III) sulfate, -suifocyan-saure, /. chromithiocyanic acid, thiocyana-tochromic(III) acid, -verbindung,/. chromic compound, chromium(III) compound. 

What volume of 0.2500 M cobalt(III) sulfate is required to react completely with... 

Basically, the oxidation of iron pyrite, FeS2, results in the production of iron(III) sulfate and sulfuric acid, H2SO4. However, two overall reaction stoichiometries are possible and each will yield a different acid generation capacity (e.g., Langmuir, 1997 Baird, 1995) ... 

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