Sulfate sources

Amide-Based Sulfonic Acids. The most important amide-based sulfonic acids are the alkenylarnidoalkanesulfoiiic acids. These materials have been extensively described ia the Hterature. A variety of examples are given ia Table 5. Acrylarnidoalkanesulfoiiic acids are typically prepared usiag technology originally disclosed by Lubrizol Corporation ia 1970 (80). The chemistry iavolves an initial reaction of an olefin, which contains at least one aHyhc proton, with an acyl hydrogen sulfate source, to produce a sulfonated intermediate. This intermediate subsequendy reacts with water, acrylonitrile, and sulfuric acid. 

This global average burden of anthropogenic sulfate aerosol can be estimated by considering the entire atmospheric volume as a box. Because the lifetime of sulfate aerosol is short, the sum of all sulfate sources, Q, and its lifetime in the box, f, along with the area of the earth, determine B ... 

Characteristics often ascribed to MVT deposits include temperatures generally <200°C and deposition from externally derived fluids, possibly basinal brines. Sulfur isotope valnes from MVT deposits suggest two major sulfide reservoirs, one between -5 and +15%c and one greater than +20%c (Seal 2006). Both sulfide reservoirs can be related, however, to a common sea water sulfate source that has undergone different sulfur fractionation processes. Reduction of sulfate occurs either bacterially or by abiotic thermochemical reduction. High 5 S-values should reflect minimal fractionations associated with thermochemical reduction of sea water sulfate (Jones et al. 1996). 

RAW MATERIAL Rhodapex ES-2 CHEMICAL DESCRIPTION Sodium laureth (2) sulfate SOURCE Rhone... 

To experimentally validate the Gitterman model, we prepared an artificial seawater sample that had the composition of seawater s liquid partially frozen down to — 23 °C (Marion et al. 1999). To this sample we added an excess of mirabilite crystals to ensure an adequate sulfate source. The sample was then placed in a — 26 °C temperature-controlled bath and allowed to equilibrate with periodic sampling and analyses over a 12-week period. The precipitation of hydrohalite between — 23 °C and — 26 °C (Fig. 3.16) led to an initial decrease in the sodium molality. Magnesium, on the other hand, was conserved in the solution phase, as ice formed and hydrohalite precipi-... 

Sulfur isotopic measurements can shed light on the origin of sulfur in coal. The 34S/32S ratio depends on the source of sulfur and the geologic processes involved during coal formation. For example, isotopic compositions are different for the two principal sources of sulfur in coal 1) the sulfur preserved from the precursor plant material, and 2) the sulfur derived from the bacterial reduction of dissolved sulfate in ambient waters. Plant assimilation of sulfur results in a slight depletion of 34S (4-4.5%c) relative to the 834S in the dissolved sulfate source (102.103). In contrast, the dissimilatory bacterial reduction of sulfate results in a large isotopic fractionation sulfide sulfur can be depleted as much as 60%o in the heavy isotope (89.104-106). 

Note The following steps describe a specific method of filtering, weighing and mounting the sample. The instructor may provide alternate instructions for preparing the barium sulfate source appropriate for the available counting facilities. 

For this reason Pb has been used as a tracer of the precipitation fate of S04. Turekian et al. (1989) used the S04 / Pb ratio in aerosols and the flux of °Pb measured in bucket collections to determine the SO flux across the Pacific Ocean. Further, they showed that the S04 / Pb in aerosols from regions of high biological productivity was higher than for normal relatively unpolluted air (Table 3) indicating a sulfate source from the oxidation of dimethyl sulfide (DMS). The measured flux of DMS from the oceans at the equator matched the biogenic flux determined from the °Pb calculation (Table 4). (Actually, as we shall see below, this concordance is probably due to an underestimate of sulfate flux and an overestimate of the fraction of DMS oxidized to sulfate.)... 

Yang W., Spencer R. J., and Krouse H. R. (1997) Stable isotope composition of waters and sulfate species therein, Death Valley, CaUfomia, USA impUcations for inflow and sulfate sources, and arid basin cUmate. Earth Planet. Sci. Lett. 147, 69-82. 

Archean rocks occurred between 2.4-2.0 Ga, consistent with a shift from an 02-free early atmosphere in which SO2 photochemistry could dominate among seawater sulfate sources to an 02-rich later atmosphere in which oxidative weathering of sulfide minerals predominated over photochemistry as the major source of seawater sulfate. Sulfur isotope heterogeneities... 

By w eighing the uranium oxide samples and barium sulfate sources to the nearest 0.05 mg the error was 0.1fo or less. 

Seven portions of natural uranium as the oxide UgOg were irradiated, processed chemically after the addition of barium carrier, and the barium sulfate sources counted for 4 min (approximately 50,(KK) counts). The coefficient of variation on a single result was found to be 0.53% of which 0.44% was due to statistical variations in the count rate. 

Bao, H., Jenkins, K.A., Khachaturyan, M. Chong Diaz, G. (2004) Different sulfate sources and their post-depositional migration in Atacama soils. Earth and Planetary Science Letters 224, 577-587. 

Example 3. Add twelve (12) cubic centimeters of a five (5) per cent, glue solution to three (3) liters of twenty (20) per cent, ammonia solution, then add further one (1) liter of sodium hypochlorite solution containing about seventy (70) grams of active chlorin, and then heat up the mixture finally driving off the excess of ammonia. The residue contains hydrazin which can be conveniently isolated by evaporating the residue and precipitating the hydrazin in the form of its sulfate. Source Raschig 1909... 

CHEMICAL DESCRIPTION Alcohol ether sulfate SOURCE Stepan... 

FIGURE 17.17 CCN closure study carried out during July 2003 in the Pacific Ocean marine boundary layer off the coast of Monterey, California. A CCN counter on board an aircraft measured activation of the boundary layer aerosol at 3 supersaturations data for 0.1% supersaturation are shown here. Panels (a) and (b) show data when the airmasses sampled were of marine and continental origins, respectively. The predicted CCN concentrations are based on the assumption that the aerosol was pure ammonium sulfate. Source California Institute of Technology... 

The amount of desorbed H2S and SO2 molecules during the TPR treatment corresponds to about 1.5 monolayer of recovered Ce02 sites. From these rough calculations we can thus conclude that only a part of the available sulfate source was released as H2S/SO2. This is supported by the findings of Diwell (4) and Beck (7), who state that the reaction only involves the surface region of the washcoat. The XPS results verifies the role of the surface. It was foimd that a residual sulfiir concentration of 0.9 % remained after the TPR sequence, thus deriving from bulk sulfate species, simultaneously as the oxidation state of Ce was strongly influenced, as shown in fig. 4. 

Tang, E J., and E. M. Gartner (1987). Influence of sulfate source on Portland cement hydration . PCE R D Serial No. 1876, Construction Technology Laboratories, Inc., Skokie, Illinois, U.S. 

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