Relationship with solubility

The basic relationships between solubility and pH can be derived for any given equilibrium model. The model refers to a set of equilibrium equations and the associated equilibrium quotients. In a saturated solution, three additional equations need to be considered, along with the ionization Eqs. (2a)-(2d), which describe the equilibria between the dissolved acid, base or ampholyte in solutions containing a suspension of the (usually crystaUine) solid form of the compounds ... 

In general, if S is the solubility (in g-moles liter-1) of a sparingly soluble salt having the formulae B in pure water, one has [B+] = % S and [A-] = y S, assuming complete dissociation. Therefore, Ksp = [B+]x A F= (x S)x (y S)y = xx yY Sx+r. This is the general expression showing the relationship between solubility and the solubility product. It is known that solubility varies with temperature, and so does the solubility product. 

Weissenbom PK, Pugh RJ (1996) Surface tension of aqueous solutions of electrolytes relationship with hydration, oxygen solubility, and bubble coalescence. J Colloid Interface Sci 184 550-553... 

Working co-operatively with others, we have found some indication that certain alilphatic linkages between aromatic nucleii are involved in the rapid dissolution of coal. The absolute aliphatic hydrogen content as determined by P. Solomon using FTIR (22) shows a very good linear relationship with conversion of coal in 3 minutes to pyridine soluble materials (Figure 14a). 

Liposome partitioning of ionizable drugs can be determined by titration, and has been correlated with human absorption [102-104]. A new absorption potential parameter has been suggested, as calculated from liposome distribution data and the solubility-dose ratio, which shows an excellent sigmoidal relationship with human passive intestinal absorption (Eq. 2) [102, 103]. 

Bruggeman, W. A., van der Steen, J., Hutzinger, O. (1982) Reversed-phase thin-layer chromatography of polynuclear aromatic hydrocarbons and chlorinated biphenyls. Relationship with hydrophobicity as measured by aqueous solubility and octanol-water partition coefficient. J. Chromatogr. 238, 335-346. 

How can a saturated solution of one ionic compound react with another ionic compound to form another precipitate What is the relationship between solubility and the K value of a saturated solution ... 

Cal, K. Aqueous solubility of liquid monoterpenes at 293 K and relationship with calculated log P value. Yakugaku Zasshi, 126(4) 307-309, 2006. 

Solvent dyes are really intermediate between dyes and pigments being insoluble in water but soluble in solvents, especially hydrocarbons. Structurally many solvent dyes bear a close similarity and relationship with disperse dyes. The Colour Index has an issne on Solvent Dyes, where several hundred dyes are described, unfortunately many of the strnctnres remain confldential. The structures of the disclosed dyes range from very simple monoazo dyes, e.g. Cl Solvent Yellow 14 (2.78) to the higher performing anthraquinones, e.g. Cl Solvent Yellow 163 (2.79) and Blue 36 (2.80), quinophthalones... 

Torgersen and Toledo (15) assessed the relationship between solubility and water absorption of WPC, peanut protein, single cell protein (SCP), and chicken preen gland protein and characteristics in a comminuted meat system containing the various protein additives. Protein additives with high water absorption capacities were correlated with more viscous raw mixtures and with less fat and water released on cooking. Simple system determination of water absorption capacity at 90°C rather than at 78.5°C was the better predictor of water and fat retention in the food system studied. 

A method of prediction of the salt effect of vapor-liquid equilibrium relationships in the methanol-ethyl acetate-calcium chloride system at atmospheric pressure is described. From the determined solubilities it is assumed that methanol forms a preferential solvate of CaCl296CH OH. The preferential solvation number was calculated from the observed values of the salt effect in 14 systems, as a result of which the solvation number showed a linear relationship with respect to the concentration of solvent. With the use of the linear relation the salt effect can be determined from the solvation number of pure solvent and the vapor-liquid equilibrium relations obtained without adding a salt. 

Similarities between reversal of charge spectra for colloids with solubility sequences of salts in bulk solution have been indicated (7, 37)— for example, for salts possessing different cations but the same anion, the solubility sequence of the phosphates is K+ > Na+ > Li+, while it is the reverse for the sulfates (7, 30). In view of this similarity, it is natural to introduce this fact as another possible link to explain the reversal of the specific cation effect in tt-A isotherms, though the precise relationship to monolayers is not clear at this time. 

These values are summarized in Figure 2 and compared with our results on the soluble fractions from depolymerization. Van Krevelen (9) reported aromatic hydrogen values ranging from 23 to 54% for coals containing 76 to 89% carbon. Aromatic hydrogen content varies directly with rank. Brown (i) obtained values of 19-42% for a series of vitrains and showed a similar relationship with rank displaced toward lower aromatic values. Ladner and Stacey (5) analyzed two additional coals using the procedure developed by Brown, and the results fit Brown s correlation. 

The octanol/water coefficient (log P) is the standard molecular descriptor used to provide the chemical property of the hydrophobicity of a molecule. Compounds with high partition coefficients usually have very low aqueous solubility. This will decrease the chance of attack by hydroxyl radicals and lead to a lower rate constant. Nevertheless, the linear relationships with log P do not reproduce similar trends of several chemical classes such as alkane and phenol. They could be either positive or negative linear relationships. Alkene (R2 < 0.67), benzene (R2 < 0.78), carboxylic acid (R2 < 0.74), and halide (R2 < 0.55) classes do not provide significant correlations. 

Therefore, the mole fraction ideal solubility of a crystalline solute in a saturated ideal solution is a function of three experimental parameters the melting point, the molar enthalpy of fusion, and the solution temperature. Equation 2.15 can be expressed as a linear relationship with respect to the inverse of the solution temperature ... 

For a weakly acidic compound at pHc pKa (e.g., by 2 units), the solubility is practically independent of pH and remains constant pKa, the solubility increases exponentially with pH, where the excess solid phase in equilibrium with the saturated solution is the free acid. At certain pH value, the log-linear relationship of solubility with pH abruptly ends, and the solubility plots enter a nearly constant range, where the excess solid phase is the salt. The pH value where the log-linear relationship ends and near constant solubility starts is the pH of maximum solubility pHmax- Forcompounds containing bothacidicand basic functional groups, the solubility of zwitterion (internal salt pair) at the isoelectric point is typically the lowest over the entire pH range. 

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