Free Access Appendix C: Compiled Thermodynamic Dath Sources for Aqueous and Biochemical Systems: An Annotated Bibliography (1930-1983 Joseph F. Zemaitis Jr., Chem Solve, Inc.Search for more papers by this authorDiane M. Clark, OLI Systems, Inc.Search for more papers by this authorMarshall Rafal, OLI Systems, Inc.Search for more papers by this authorNoel C. Scrivner, E.I. duPont Nemours & Co., Inc.Search for more papers by this author Book Author(s):Joseph F. Zemaitis Jr., Chem Solve, Inc.Search for more papers by this authorDiane M. Clark, OLI Systems, Inc.Search for more papers by this authorMarshall Rafal, OLI Systems, Inc.Search for more papers by this authorNoel C. Scrivner, E.I. duPont Nemours & Co., Inc.Search for more papers by this author First published: 06 January 1986 https://doi.org/10.1002/9780470938416.app3 AboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onEmailFacebookTwitterLinked InRedditWechat Handbook of Aqueous Electrolyte Thermodynamics: Theory & Application RelatedInformation

Macroscopic sorption studies indicated that Pb sorption capacity was independent of pH over the pH range 5–7, while sorption as a function of reaction time up to two weeks for systems with no bulk precipitate phases showed continuous Pb uptake on dolomite. This could be due to diffusion of Pb into the micropores of dolomite as well as an increase in surface sites caused by particle size reduction during suspension mixing. Normalized XANES spectra for systems undersaturated with respect to Pb carbonate precipitates resembled the spectrum of Pb4(OH)4+4, suggesting that Pb is mainly coordinated to dolomite as an inner-sphere surface complex. On the other hand, the XANES spectrum for 10−3 M Pb at 1 atm CO2(g) in a 2 M Mg(NO3)2 background electrolyte solution resembled that of cerussite, while a sample at 5×10−4MPb in equilibrium with air and 2 M Mg(NO3)2 resembled that of hydrocerussite. EXAFS analyses of sorption samples in chloride solutions showed that there were only first-shell contributions under 1 atm CO2(g), while higher shell contributions from Ca/Mg were seen at 10−3.42 atm CO2(g). On the other hand, EXAFS samples prepared in nitrate solutions showed noticeable differences in speciation under different reaction conditions—from outer-sphere surface complexes at low Pb concentrations and pH, to inner-sphere surface complexes at moderate Pb concentrations and neutral pH, to the formation of Pb carbonate precipitates at the highest Pb loadings.

The reactions of acrylonitrile, crotonitrile, propionitrile, and a small set of related reaction products were investigated in high-temperature water. Hydrolysis of the cyano group yielded the corresponding amides, which underwent similar hydrolysis to yield the carboxylic acids. The conversion of acrylonitrile was more rapid than that of its saturated analogue propionitrile, as the unsaturated site of acrylonitrile provided a facile pathway for the formation of alcohols, amines, and ethers. Carbon-carbon bond cleavage pathways involving the hydration of the olefin moiety were also observed for acrylonitrile.

The partition or distribution of a solute between two immiscible solvents was first treated by Nernst (Bromberg, 1980). Generally the partition coefficient, which is the ratio of the concentrations of the solute in the two solvents, is a constant. The partition mechanism has been extended to describe the sorption of solutes on clay minerals and soil materials for systems in which no specific bonding was involved. It should be noted that two types of partition mechanisms have been proposed. Earlier, Greenland et al. (1962, 1965), Theng (1972), and Theng and Scharpenseel (1976) proposed that the linear sorption isotherm observed with clay minerals can be characterized by a partition of a solute between the bulk and intercrystalline water. Later, Chiou et al. (1979, 1983) proposed that the sorption of neutral organic chemicals is essentially a partition process between the soil organic matter and soil water. More recently, Lee et al. (1989), Smith et al. (1990), and Jaynes and Boyd ( 199 l) attributed this mechanism to the enhanced sorption of neutral organic molecules on soils and clays exchanged with organic cations with one or more long alkyl groups. Because clay minerals saturated with metal cations contain negligible amounts of organic matter, the sorption of neutral organic molecules on these clays only involves the partition mechanism proposed by the earlier investigators (Greenland et al . , 1962, 1965; Theng, 1972; Theng and Scharpenseel, 1976). Recently, Zhang et al. (1990a, 1990b, 1990c) have studied the sorption of several neutral organic molecules on montmorillonites saturated with different metal cations. Based on the partition mechanism, they have derived the following equation (Zhang et aL, 1990b),

Free Access Appendix B: Selected Thermodynamic Data Joseph F. Zemaitis Jr., Chem Solve, Inc.Search for more papers by this authorDiane M. Clark, OLI Systems, Inc.Search for more papers by this authorMarshall Rafal, OLI Systems, Inc.Search for more papers by this authorNoel C. Scrivner, E.I. duPont Nemours & Co., Inc.Search for more papers by this author Book Author(s):Joseph F. Zemaitis Jr., Chem Solve, Inc.Search for more papers by this authorDiane M. Clark, OLI Systems, Inc.Search for more papers by this authorMarshall Rafal, OLI Systems, Inc.Search for more papers by this authorNoel C. Scrivner, E.I. duPont Nemours & Co., Inc.Search for more papers by this author First published: 06 January 1986 https://doi.org/10.1002/9780470938416.app2 AboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onEmailFacebookTwitterLinked InRedditWechat Handbook of Aqueous Electrolyte Thermodynamics: Theory & Application RelatedInformation

This chapter contains sections titled: Identification of Complexing Electrolytes Phosphoric Acid Sulfuric Acid Zinc Chloride Ferric Chloride Cuprous Chloride Calcium Sulfate Sodium Sulfate Other Chloride Complexes Activity Coefficient Methods Summary Activity Coefficient Methods Cuprous Chloride