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Iron III sulfate

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. [Pg.457]

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. [Pg.21]

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) ... [Pg.406]

Ammonium iron(III) sulfate dodecahydrate Clark, R. E. D., private comm., 1973... [Pg.1644]

Na2S04 sodium sulfate Fe2(S04)3 iron(III) sulfate or ferric sulfate... [Pg.93]

Iron(II) sulfate reacts with concentrated sulfuric acid to form iron(III) sulfate and sulfur dioxide ... [Pg.437]

The compound is oxidized by moist air forming basic iron(III) sulfate. Aqueous solutions exposed to air also undergo oxidation the reaction, however, is very slow. The rate of oxidation increases with temperature and the pH. In alkaline medium, the oxidation is much faster. In solution, it also is oxidized to Fe + by radiations from radioactive substances. This reaction is utilized to measure the radiation dose in dosimeter solutions. [Pg.437]

Even in the absence of an oxidizing agent, concentrated sulfuric acid alone can convert iron(II) sulfate to iron(III) sulfate ... [Pg.438]

Iron(III) sulfate readily forms alums with many isomorphous compounds by mixing equimolar amounts of both the salts in aqueous solutions followed by crystaUization ... [Pg.438]

Iron(III) sulfate may be reduced to +2 oxidation state of the metal in solution in the presence of common reducing agents. For example, reaction with zinc in sulfuric acid can produce iron(II) sulfate. The molecular equation is as follows ... [Pg.439]

Oxidation with the iron(III) sulfate from ilmenite digestion (see Section 2.1.3.1) [2.21], followed by crystallization of the iron(II) sulfate... [Pg.50]

See other pages where Iron III sulfate is mentioned: [Pg.378]    [Pg.526]    [Pg.438]    [Pg.438]    [Pg.438]    [Pg.444]    [Pg.1084]    [Pg.96]    [Pg.95]    [Pg.19]    [Pg.1550]    [Pg.1550]    [Pg.141]    [Pg.234]    [Pg.23]    [Pg.457]    [Pg.647]    [Pg.42]    [Pg.58]    [Pg.82]    [Pg.493]    [Pg.249]    [Pg.230]    [Pg.45]    [Pg.437]    [Pg.437]    [Pg.438]    [Pg.438]    [Pg.126]    [Pg.170]    [Pg.89]    [Pg.91]   
See also in sourсe #XX -- [ Pg.19 , Pg.393 ]

See also in sourсe #XX -- [ Pg.28 , Pg.148 ]



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