Sulfates thiosulfate, reaction with

C. Cyclobutanone (Note 16). The residue consisting of oxaspiro-pentane (35%) and dichloromethane (about 200 ml.) is added dropwise at room temperature to a magnetically stirred solution containing about 5-10 mg. of lithium iodide in 50 ml. of dichloromethane (Notes 17, 18), at such a rate as to maintain gentle reflux of the solvent. At the end of the addition when the reaction mixture returns to room temperature, the transformation into cyclobutanone is complete. The dichloromethane solution is washed with 20 ml. of saturated aqueous sodium thiosulfate and with 20 ml. of water. After drying over magnesium sulfate and concentration by distillation of the solvent through a 15-cm., helix-packed, vacuum-insulated column, the residual liquid consists of cyclobutanone (95%) and of 3-buten-2-one and 2-methylpropenal... 

Iron frequently has been postulated to be an important electron acceptor for oxidation of sulfide (58, 84,119, 142, 152). Experimental and theoretical studies have demonstrated that Fe(III) will oxidize pyrite (153-157). Reductive dissolution of iron oxides by sulfide also is well documented. Progressive depletion of iron oxides often is coincident with increases in iron sulfides in marine sediments (94, 158, 159). Low concentrations of sulfide even in zones of rapid sulfide formation were attributed to reactions with iron oxides (94). Pyzik and Sommer (160) and Rickard (161) studied the kinetics of goethite reduction by sulfide thiosulfate and elemental S were the oxidized S species identified. Recent investigations of reductive dissolution of hematite and lepidocrocite found polysulfides, thiosulfate, sulfite, and sulfate as end products (162, 163). 

Sulfinic acid amides are obtained in the reaction of sulfinic acids with amines in the presence of DCC." In the reaction of sulfuric acid with alcohols, thioalcohols and amines in the presence of DCC, the respective sulfates, thiosulfates and amides are obtained." The reaction of H3PO4 with DCC, followed by alcohol affords (R0)2P(0)H." ... 

The reaction of a strong solution of aqueous ammonia with the sulfide concentrate in a strongly agitated pressure vessel at a temperature between 160 and 190°F under an oxygen partial pressure of about 10 psi, either as pure oxygen or as compressed air, fulfills the optimal conditions for the above requirements. The iron present in the concentrate is oxidized to hydrated ferric oxide which, together with the silicates is insoluble in aqueous ammonia. The copper, nickel, and cobalt form their amines, while the sulfides are oxidized to sulfates, thiosulfates, and polythionates. 

The sulfate group can be transferred to other nucleophilic atoms, such as nitrogen or sulfur, resulting in the formation of sulfamates (RR — N — SO3) and thiosulfates (R — S — SO3), respectively, rather than sulfates. The sulfotrans-ferases (STs) that catalyse the sulfonation of drugs, hormones and neurotransmitters in animals, like those in plants that catalyse similar reactions with flavonols as... 

It is well established that most of the known anaerobic prokaryotes perform oxidative phosphorylation without O2. Depending on the species and the metabolic conditions, these bacteria may use a large variety of inorganic (e.g., nitrate, nitrite, sulfate, thiosulfate, elemental sulfm, polysulfide sulfur) or organic compounds (e.g., fumarate, dimethylsulfoxide, trimethylamine-A -oxide, vinyl- or arylchlorides) as terminal electron acceptor instead of oxygen. The redox reactions with these acceptors are catalyzed by membrane-integrated electron transport chains and are coupled to the generation of an electrochemical proton potential (Ap) across the membrane. Oxidative phosphorylation in the absence of O2 is also termed anaerobic respiration . Oxidative phosphorylation with elemental sulfur is called sulfm respiration . Oxidative phosphorylation with polysulfide sulfur is called polysulfide respiration . 

As a result, there are several possible reactions with chlorine. As pH increases, the product of the reaction may be dithionite or sulfate, with or without colloidal sulfur. The stoichiometry shows that the efficiency of thiosulfate as a chlorine scavenger depends strongly on the reaction regime ... 

The complex between zirconium and alizarine red S (sodium 3,4-dihydroxy-9,10-dioxo-2-anthracene sulfonate. Figure 6.2) gives red-brown color in acid solution if alizarine red S is in excess and violet color if the zirconium is in excess. The complex is decolorized by fluoride ions. Phosphate, arsenate, sulfate, thiosulfate, and oxalate as well as organic hydroxy acids interfere with this reaction. 

The absorption reactions are those of H2S and HCN combining with ammonia to form ammonium bisulfide and ammonium cyanide, followed by the oxidation of the ammonium bisulfide by the naphthoquinone (NQ) to form elemental sulfur and the naphthohydro-quinone (H2NQ). The reactions with oxygen take place in the regenerator and lead to the formation of NQ, thiocyanate, thiosulfate, and sulfate. Part of the elemental sulfur reacts with the available NH4CN in the oxidizer to produce NH4SCN. 

Increasing occurrence of secondary reactions, with oxidation of thiosulfate to sulfate and sulfuric acid... 

The catalyst can also be sulfated at lower temperature by a complex series of reactions with sulfur dioxide, and the catalyst can contain up to 3% of combined sulfur under normal operating conditions. It has been snggested that sulfur dioxide is strongly chemisorbed by snrface hydroxyl gronps to give a sulfite intermediate. This reacts with sulfur vapor to give a thiosulfate intermediate that reacts, in tnm, with a neighboring hydroxyl to form snlfate. This does not necessarily deactivate the catalyst. 

A mixture of 17 g of the methiodide and 32 ml of a 40 % aqueous potassium hydroxide solution is heated with stirring in a flask fitted with a condenser. The heating bath should be kept at 125-130°, and the heating should be continued for 5 hours. The cooled reaction mixture is then diluted with 30 ml of water and washed twice with 25-ml portions of ether. The aqueous layer is cautiously acidified in the cold with concentrated hydrochloric acid to a pH of about 2 and then extracted five times with 25-ml portions of ether. The combined extracts are washed twice with 10% sodium thiosulfate solution and are dried (magnesium sulfate). Removal of the solvent followed by distillation affords about 3 g of 4-cyclooctene-l-carboxylic acid, bp 125-12671-1 mm. The product may solidify and may be recrystallized by dissolution in a minimum amount of pentane followed by cooling in a Dry-Ice bath. After rapid filtration, the collected solid has mp 34-35°. 

It is decompd even by weak acids with evolution of brown fumes of nitrous anhydride (Ref 1) KN02 detonates violently when heated in the presence of thiosulfates or cyanides. Ref 1 states that when mixed with K cyanide, the mixt burns, and at 450°, it explds violently. Ref 6 details instances of molten KN02 being violently decompd by boron, and of a wgorous reaction attended by flame caused by the addition of a 0 little amm sulfate to fused KNOa... 

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