Solubility relationship

To understand why AgCl shows a more complex solubility relationship than that suggested by equation 8.2, we must recognize that Ag+ also forms a series of soluble chloro-complexes... 

K. Osseo-Asare, F. J. Arriagada, and J. H. Adair, "Solubility Relationships in the Coprecipitation Synthesis of Barium Titanate Heterogeneous Equihbria in the Ba—Ti—C2O4—H2O System," in G. L. Messing, E. R. Fuller, Jr., and Hans Hausin, eds.. Ceramic Powder Science Vol. 2,1987, pp. 47-53. 

AC)m is the mean eoneentration gradient, representing the deviation from equilibrium. Henee the rate is direetly related to eoeffieient K, whieh will generally inerease witli any inerease in mrbulenee sueh as inereased relative veloeity between the phases or agitation to the exposed surfaee area A and to the eoneentration differenee, whether it is a pressure or humidity differential or a solubility relationship. As a result ... 

F. W. Harris and L. H. Lannier, Structure-Solubility Relationships in Polymers, Academic, New York, 1987. 

Also in Structure-Solubility Relationships in Polymers, (eds.) Harris, F. W., Seymour, R. B., Academic Press, N. Y. 1977... 

The failure to identify the necessary authigenic silicate phases in sufficient quantities in marine sediments has led oceanographers to consider different approaches. The current models for seawater composition emphasize the dominant role played by the balance between the various inputs and outputs from the ocean. Mass balance calculations have become more important than solubility relationships in explaining oceanic chemistry. The difference between the equilibrium and mass balance points of view is not just a matter of mathematical and chemical formalism. In the equilibrium case, one would expect a very constant composition of the ocean and its sediments over geological time. In the other case, historical variations in the rates of input and removal should be reflected by changes in ocean composition and may be preserved in the sedimentary record. Models that emphasize the role of kinetic and material balance considerations are called kinetic models of seawater. This reasoning was pulled together by Broecker (1971) in a paper called "A kinetic model for the chemical composition of sea water."... 

Chiarini, A. Tartarini, A. Fini, A., pH-solubility relationship and partition coefficients for some anti-inflammatory arylaliphatic acids, Arch. Pharm. 317, 268-273 (1984). 

The zinc content of the overflow water from the densator-reactor is set by the pH-solubility relationship of zinc in water and results in a zinc content of 0.5 to 1 mg/L at pH = 10. Once the precipitated zinc is removed from the wastewater, the pH can be readjusted to a lower value. 

Liquid-liquid reactors. Examples of liquid-liquid reactions are the nitration and sulfonation of organic liquids. Much of the discussion for gas-liquid reactions also applies to liquid-liquid reactions. In liquid-liquid reactions, mass needs to be transferred between two immiscible liquids for the reaction to take place. However, rather than gas-and liquid-film resistance as shown in Figure 7.2, there are two liquid-film resistances. The reaction may occur in one phase or both phases simultaneously. Generally, the solubility relationships are such that the extent of the reactions in one of the phases is so small that it can be neglected. 

WI Higuchi, PK Lau, T Higuchi, JW Shell. Polymorphism and drug availability Solubility relationships in the methviorednisolone system. J Pharm Sci 52 150-153,... 

Also in Table 3.4 are some solubility relationships (including partition coefficients) and one transport property. In these cases, the molecule in question is interacting with other kinds, and the product vo-2ot is found to be of less importance. Instead, cr2ot, cr2, and a2 often appear in the equations, along with terms involving molecular size. 

Kamlet, M. J., Doherty, R. M., Abraham, M. H., Carr, P. W., Doherty, R. F., Raft, R. W. (1987) Linear solvation energy relationships. Important differences between aqueous solubility relationships for aliphatic and aromatic solutes. J. Phys. Chem. 91, 1996-2004. 

Sadiq, M. 1986. Solubility relationships of arsenic in calcareous soils and its uptake by com. Plant Soil 91 241-248. 

A very severe test of these virial-coefficient equations for the sea-water-related Na-K-Mg-Ca-Cl-S0,-H 0 system has been made by Harvie and Weare (37) who calculated tne solubility relationships for most of the solids which can arise from this complex system. There are 13 invariant points with four solids present in the system Na-K-Mg-Cl-SO - O and the predicted solution compositions in all 13 cases agree with the experimental values of Braitsch (38) substantially within the estimated error of measurement. In particular, Harvie and Weare found that fourth virial coefficients were not required even in the most concentrated solutions. They did make a few small adjustments in third virial coefficients which had not previously been measured accurately, but otherwise they used the previously published parameters. 

It is shown that the properties of fully ionized aqueous electrolyte systems can be represented by relatively simple equations over wide ranges of composition. There are only a few systems for which data are available over the full range to fused salt. A simple equation commonly used for nonelectrolytes fits the measured vapor pressure of water reasonably well and further refinements are clearly possible. Over the somewhat more limited composition range up to saturation of typical salts such as NaCl, the equations representing thermodynamic properties with a Debye-Hiickel term plus second and third virial coefficients are very successful and these coefficients are known for nearly 300 electrolytes at room temperature. These same equations effectively predict the properties of mixed electrolytes. A stringent test is offered by the calculation of the solubility relationships of the system Na-K-Mg-Ca-Cl-SO - O and the calculated results of Harvie and Weare show excellent agreement with experiment. 

Generalized computer techniques for calculating vapor-liquid equilibria and solubility relationships in electrolyte systems are not readily available in the metallurgical industry. 

The temperature-solubility relationship for solute and solvent is of prime importance in the selection of a crystalliser and, for solutions that yield appreciable amounts of crystals on cooling, either a simple cooling or a vacuum cooling unit is appropriate. An evaporating crystalliser would be used for solutions that change little in composition on cooling and... 

DuPont. Solubility Relationships of the Freon Fluorocarbon Compounds, Technical Bulletin B-7, (Wilmington. DE DuPont de Nemours, 1966). 

The amount of a solute that can be introduced into a solvent depends on its solubility, be it a gas (section 2.7.1), a solid nonelectrolyte (section 2.7.2), or an electrolyte (section 2.7.3). Ternary systems, which are the basic form of solvent extraction systems (a solute and two immiscible solvents), have then-own characteristic solubility relationships (section 2.8.1). 

The solubilities of aromatic compounds in the ionic liquid are dramatically higher than those of saturated compounds. Benzene has a solubility of 4.9mol/mol of ionic liquid, and thiophene has a solubility of 6.7mol/mol of ionic liquid. A dramatic steric effect was observed on the solubility of aromatics the alkyl-substituted aromatics showed reduced solubility. Although the solubility of hexene in the ionic liquid is considerably lower than that of the aromatics, it is still measurably higher than that of hexane. Similar structure-solubility relationships characteristic of organic molecules were observed with the ionic liquids [BMIM]BF4, [BMIM]PFg, and [EMIM]BF4 (Fig. 10) (27). 

Structure-solubility relationships can be used to predict the behavior of the hydrogenation reactions in an ionic liquid. For example ((S(S), the hydrogenation of aromatics in ionic liquids is much faster than that in the aqueous systems because of the higher solubilities of the aromatics in ionic liquids than in water. 

Equilibrium solubility This approach is considered a first attempt to characterize the true thermodynamic solubility of the compound. It is used to rank-order compounds and to extract a structure-solubility relationship within the chemical series. In this assay, compounds are usually equilibrated for 24 h before analysis. One can start from powder, but this is a quite labor-intensive step. In most cases one starts from DMSO stock solutions (usually 10 mM) because it is much more efficient from a compound logistics viewpoint. The solvent is then usually removed and the compound is dried before addition of the buffer medium [15, 16]. 

Solubility relationships revealed that methanol is the best solvent for the study of the reactions of [Ni(NiL2)2]Cl2 with alkyl halides. All the reactants of interest either react with methanol or undergo deleterious side reactions. Consequently, the relative rates of these processes had to be estimated in order to establish the feasibility of the study of interest and make any necessary corrections. 

However, these solubility relationships will change with Eh—e.g.9 as Eh becomes more positive, the Pu3+ line will be lower, while those for Pu(OH)3+ and Pu02+ will be raised. Also the presence of carbonate will raise the solubility line for Pu(IV) significantly. Nevertheless, in the neutral region of pH Figure 2 indicates that at the Eh used here, a typical environmental value, the solubility of plutonium in equilibrium with solid Pu(OH)4 is quite low. 

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