Ferric basic sulfate

Iron sulfate (see also Ferric, ferrous sulfate) - 237, 244, 376, 380, 385, 389, 409,830, 868 Iron sulfate, basic - 823 Iron sulfide - 620 Iron tersulfate - 830 Iron vitriol (see Ferrous sulfate)... 

Alkali metal haHdes can be volatile at incineration temperatures. Rapid quenching of volatile salts results in the formation of a submicrometer aerosol which must be removed or else exhaust stack opacity is likely to exceed allowed limits. Sulfates have low volatiHty and should end up in the ash. Alkaline earths also form basic oxides. Calcium is the most common and sulfates are formed ahead of haHdes. Calcium carbonate is not stable at incineration temperatures (see Calcium compounds). Transition metals are more likely to form an oxide ash. Iron (qv), for example, forms ferric oxide in preference to haHdes, sulfates, or carbonates. SiHca and alumina form complexes with the basic oxides, eg, alkaH metals, alkaline earths, and some transition-metal oxidation states, in the ash. 

Ferric sulfate (XH2O) [10028-22-5] M 399.9 + XH2O. Dissolve in the minimum volume of dilute aqueous H2SO4 and allow to evaporate at room temp until crystals start to form. Do not concentrate by boiling off the H2O as basic salts will be formed. Various hydrates are formed the—common ones are the dodeca and none hydrates which are violet in colour. The anhydrous salt is colourless and very hygroscopic but dissolves in H2O slowly unless ferrous sulfate is added. 

In the jarosite process, the precipitation of iron occurs from acidic sulfate solutions as one of a group of basic ferric sulfates known as jarosites. The conditions for the precipitation of iron in the specific form of jarosite require a solution pH of about 1.5 and a temperature of about 95 °C. The reaction may simplifiedly be represented as ... 

Fersona A process for stabilizing the calcium sulfite/sulfate waste from FGD processes, so that it may be used for landfill. The waste is mixed with ferric sulfate waste from another process (e.g., metallurgical leaching) to form sparingly soluble basic sodium ferric sulfates. Developed in the 1970s at the Battelle Columbus Laboratories, OH, under contract with Industrial Resources. See also Sintema. 

Like ferric nitrate, antimony sulfate is decomposed by water, various basic salts being formed, the simplest of which has the formula (SbOLSCL. The normal salt is stable only in rather concentrated sulfuric acid. Since this latter solvent has almost no vapor pressure at ordinary temperatures, the moist salt cannot be dried by evaporation of the solvent. It cannot be dried on absorbent paper, since the oily liquid rapidly carbonizes it. In such a case, it is best to take advantage of the drying qualities of unglazed earthenware (porous plate), such as the biscuit which forms the body of dishes. Owing to the fine pores which this material contains, liquids are sucked up by it by capillary attraction, and it is not acted upon by most reagents. 

Small Quantities or Solutions. Wear eye protection, laboratory coat, and nitrile rubber gloves. In the fume hood, add the sodium cyanide to a solution of 1% sodium hydroxide (about 50 mL/g of cyanide). Household bleach (about 70 mL/g of cyanide) is slowly added to the basic cyanide solution while stirring. When addition of the bleach is complete, the solution can be tested for the presence of cyanide using the Prussian blue test To 1 mL of the solution to be tested, add 2 drops of a freshly prepared 5% aqueous ferrous sulfate solution. Boil this mixture for at least 60 seconds, cool to room temperature, and then add 2 drops of 1% ferric chloride solution. The resulting mixture is made acid to litmus with 6 M hydrochloric acid (prepared by adding concentrated acid to an equal volume of cold water). If cyanide is present, a deep blue precipitate will form. (Concentrations of cyanide greater than 1 ppm can be detected.) If the test is positive, add more bleach to the cyanide solution, and repeat the test. Continue until no Prussian blue precipitate is formed. Wash the solution into the drain.4 6... 

Ferrous Sulfate occurs as pale, blue-green crystals or granules that are efflorescent in dry air. In moist air, it oxidizes readily to form a brown-yellow, basic ferric sulfate. A 1 10 aqueous solution has a PH of about 3.7. One gram dissolves in 1.5... 

Other investigators (14, T3) contend that the bacteria biologically oxidize the ferrous to the ferric state as sulfate, which in turn attacks the metal sulfides ores, resulting in both the dissolution of the metal and the oxidation of the sulfide. In the process the ferric iron reduces back to the ferrous state. An increase in the pH causes the basic ferric sulfate to precipitate (self-buffering action) with corresponding release of sulfuric acid. This has the cumulative effect of increasing the acidity of the mine water. 

The nickel in solution in the slurry is completely precipitated without liquids-solids separation with metallic powered iron at about 150°C under a pressure of 150 psig. The precipitated nickel contains occluded basic ferric sulfates which are decomposed by calcining at 950°C to produce a mixture of metallic nickel, metallic iron, and iron oxides. Melting of this mixture with a slag is calculated to yield a ferro-nickel containing more than 55% nickel. 

Cellulose acetate phthalate is incompatible with ferrous sulfate, ferric chloride, silver nitrate, sodium citrate, aluminum sulfate, calcium chloride, mercuric chloride, barium nitrate, basic lead acetate, and strong oxidizing agents such as strong alkalis and acids. 

Wet chemical qualttative analysis Catalyst samples analyzed directly after the reactor experiment only showed the presence of ferrous ions. The catalysts samples after exposure for a week to air revealed also the presence of ferric ions. This indicates that the iron sulfate fomied in the reactor is indeed an iron(II) sulfate, which can easily be convened into basic irofi(III) sulfate salts in wet air. 

The effect of added hydrochloric acid concentration was studied in order to determine whether or not the acid had any effect on pyrite and ash removal, sulfate-to-sulfur ratio, final heat content, and possible chlorination of the coal. Coal has many basic ash constituents, so increased ash removal was expected, as well as some suppression of the sulfate-to-sulfur ratio because the reaction that results in sulfate formation also yields eight moles of hydrogen ion per mole of sulfate (common ion effect). Added acid was studied in the range of 0.0 to 1.2M (0.0, 0.1, 0.3, and 1.2M) hydrochloric acid in 0.9M ferric chloride. Duplicate runs were made at each concentration with all four coals for a total of 32 runs. The results showed no definite trends (except one-uide infra) even when the data were smoothed via computer regression analysis. Apparently the concentration range was not broad enough to have any substantial effect on the production of sulfate or to cause the removal of additional ash over that which is removed at the pH of IM ferric chloride ( pH 2). 

Hydrous manganese oxides and amorphous iron oxides were prepared in the laboratory according to the methods described by Oakley et al 3). The addition of manganese sulfate solution to a slightly basic potassium permanganate solution produces a suspension of hydrous MnO. A suspension of Fe(0H)2 is produced by simply adjusting a ferric nitrate solution to a pH of 8.0 with a dilute sodium hydroxide solution. Both suspensions were washed repeatedly with seawater and stored in seawater for several days. 

Matijevic, E., Sapieszko, R.S.. and Melville. J.B., Ferric hydrous oxide sols. 1. Monodispersed basic iron(III) sulfate particles. J. Colloid Interf. Sci.. 50, 567, 1975. 

Typical basic pigments include basic lead carbonate, basic lead sulfate, red lead, and zinc oxide. The soaps formed when these materials Interact, for example, with linseed oil, are oxidized in the presence of water and oxygen to form mono- and dibasic straight chain Cy to Cg acids. Materials of this type (e.g., sodium and calcium azelate and pelargonate) are known to inhibit corrosion. Inhibition is associated with formation of complex ferric salts that reinforce the oxide film. Lead salts act at lower concentration than the sodium or calcium salts (3, 41). 

Ferric Subsulfate Solution, Basic ferric sulfate soln Monsel s soln. Approx Fe4(OH)2(SO >s. Prepn from FeSOj and HNO, U.S.D. 25th ed., p 574. 

It forms green, efflorescent, oblique rhombic prisms, quite soluble in HaO, insoluble in alcohol. It loses 6 Aq at 100° (212° P.) (Ferr. sulf. exsiccatus, TT. S.) and the last Aq at about 300° (572° F.). At a red heat it is decomposed into FeaOa SOa and SOa. By exposure to air it Is gradually converted into a basic ferric sulfate, (Fea)(S04)s,5Fea0a. 

Of the many basic ferric sulfates, the only one of medical interest is monsel s salt, 5(Fea)(SO))s-f4FejO, which exists in the Iiiq. ferri subsulfatis (TJ. S.) and Liq. fer. persulfatis (Br.). Its solution is decolorized, and forms a white deposit with excess of HaSOi. 

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