The solubility of water in low-dielectric solvents

1976 ◽  
Vol 54 (24) ◽  
pp. 3909-3916 ◽  
Author(s):  
Jitka Kirchnerová ◽  
Genille C. B. Cave
Keyword(s):  
Formation Constants ◽  
Solvent Interaction ◽  
Low Dielectric ◽  
Polar Species ◽  
Nonpolar Solvents ◽  
Water Solvent ◽  
Species Formation ◽  
Dispersion Component ◽  
Benzene Toluene ◽  
Polar Interactions

The solubility of water has been measured in several low-dielectric solvents at 25 °C, and the values in the nonpolar solvents are treated by using a modification of the Scatchard–Hildebrand equation. The water–solvent interaction parameter in this equation is represented by a new relationship involving the separate contributions due to dispersion and polar interactions. A new method is given for calculation of the dispersion component of the solubility parameter of a polar species. Formation constants are reported for 1:1 water–solvent complexes in carbon tetrachloride, benzene, toluene, and p-xylene.

Enthalpies of interaction of nitrogen base solutes with organic solvents

1985 ◽  
Vol 63 (9) ◽  
pp. 2540-2544 ◽  
Author(s):  
W. Kirk Stephenson ◽  
Richard Fuchs
Keyword(s):  
Hydrogen Bond ◽  
Organic Solvents ◽  
Butyl Alcohol ◽  
Hydrogen Bond Donor ◽  
Butyl Ether ◽  
Hydrogen Bond Acceptor ◽  
Nitrogen Base ◽  
Benzene Toluene ◽  
Polar Interactions ◽  
S Model

Heats of solution of triethylamine, aniline, pyridine, and model compounds (3-ethylpentane, benzene) in 17 organic solvents (n-heptane, cyclohexane, carbon tetrachloride, 1,2-dichloroethane, α,α,α-trifluorotoluene, triethylamine, butyl ether, ethyl acetate, dimethylformamide, dimethyl sulfoxide, benzene, toluene, mesitylene, t-butyl alcohol, 1-octanol, methanol, 2,2,2-trifluoroethanol) have been combined with solute heats of vaporization to give enthalpies of transfer from vapor to solvent (ΔH(v → s)). Differences between solute and model values (ΔΔH(v → s) = ΔH(v → s) (solute) – ΔH(v → s) (model)) were used to evaluate nitrogen base solute–solvent polar interactions. Correlations of ΔΔH(v → s) with Taft–Kamlet solvatochromic parameters (π*, α, β) have been determined.Aniline was found to be a better hydrogen bond donor acid than hydrogen bond acceptor base. Nevertheless, alcohols donate H-bonds to aniline. Triethylamine and pyridine are stronger HBA bases than aniline. The π* (dipolarity–polarizability) parameter of aniline (as a solute) is calculated to be 1.10.

scholarly journals Influence of amino acid additives on solution behaviour of L-alanine

2018 ◽  
Vol 20 (1) ◽  
pp. 23
Author(s):  
Muhamad Fitri Othman ◽  
Nornizar Anuar ◽  
Noor Fitrah Abu Bakar ◽  
Norazah Abdul Rahman
Keyword(s):  
Amino Acid ◽  
Chemical Engineering ◽  
Gravimetric Method ◽  
Side Chain ◽  
Water Molecules ◽  
Solvent Interaction ◽  
Engineering Research ◽  
Water Solvent ◽  
Solution Behaviour ◽  
The Ideal

<p>The solubility experiment of L-alanine solution was performed in a 250ml jacketed glass crystallizer without and with amino acid additives at temperature from 15<sup>o</sup>C to 75<sup>o</sup>C by means of gravimetric method. On the whole, L-leucine additive significantly altered the solubility of L-alanine and Glycine additive caused an erratic pattern on the solubility data of L-alanine. The hydrophobic methyl side chain of L-leucine additives is believed to contribute to the formation of water clathrate in the solution which affected the interaction of L-alanine molecules in water solvent and thus modified the solubility of L-alanine. Finally, thermodynamic data analysis of L-alanine solution was extensively assessed. The negative deviation of L-alanine from the ideal solution is as a result of high solute-solvent interaction, which is due to the hydrophobicity and clathrate phenomenon of the water molecules in the solution.</p><p>Chemical Engineering Research Bulletin 20(2018) 23-29</p>

Solvent structure effects on solvated electron reactions with ions in 2-butanol/water mixed solvents

1991 ◽  
Vol 69 (5) ◽  
pp. 884-892 ◽  
Author(s):  
Sedigallage A. Peiris ◽  
Gordon R. Freeman
Keyword(s):  
Rate Constant ◽  
Pure Water ◽  
Mixed Solvents ◽  
Reaction Rates ◽  
Bimolecular Reaction ◽  
Activation Energies ◽  
Solvated Electron ◽  
Polar Species ◽  
Water Solvent ◽  
Alcohol Water

The Smoluchowski–Debye–Stokes–Einstein equation for the rate constant k2 of a bimolecular reaction between charged or polar species[Formula: see text]was used to evaluate effects of bulk solvent properties on reaction rates of solvated electrons with [Formula: see text] and [Formula: see text] in 2-butanol/water mixed solvents. To explain detailed effects it was necessary to consider more specific behavior of the solvent. Rate constants k2, activation energies E2, and pre-exponential factors A2 of these reactions vary with the composition of 2-butanol/water mixtures. The values of E2 were in general similar to activation energies of ionic conductance EΛ0 of the solutions, except for much higher values of E2 of [Formula: see text] in alcohol-rich solvents and of [Formula: see text] in pure water solvent. The solvent apparently participates chemically in the [Formula: see text] reaction, and the [Formula: see text] reaction is multistep. Rate constant and conductance measurements of thallium acetate solutions in 2-butanol containing zero and 10 mol% water were complicated by the formation of ion clusters larger than pairs. Key words: alcohol/water mixed solvents, ions, reaction kinetics, solvated kinetics, solvated electron, solvent effects.

Association and hydration of alcohols in low-dielectric solvents. II. tert-Butyl alcohol and cyclohexanol

1976 ◽  
Vol 54 (24) ◽  
pp. 3929-3943
Author(s):  
Jitka Kirchnerová ◽  
Genille C. B. Cave
Keyword(s):  
Carbon Tetrachloride ◽  
Formation Constants ◽  
Butyl Alcohol ◽  
Mathematical Treatment ◽  
Tert Butyl ◽  
Low Dielectric ◽  
Tert Butyl Alcohol

Formulae and thermodynamic formation constants of the aggregates of tert-butyl alcohol and of cyclohexanol and their hydrates in six low-dielectric solvents have been deduced by using an iterative mathematical treatment of distribution and isopiestic data. The solvents were cyclohexane, carbon tetrachloride, p-xylene, benzene, chlorobenzene, and o-dichlorobenzene. These results and those previously obtained for n-butanol in the same six solvents are discussed in a qualitative way.

scholarly journals The Formation Constants of Some Metal Thiobenzoato- and Thioacetato-Complexes in Dioxane-Water Solvent

1972 ◽  
Vol 45 (1) ◽  
pp. 282-283 ◽  
Author(s):  
Akira Ouchi ◽  
Toshio Takeuchi ◽  
Yoshiaki Takahashi ◽  
Mitsuhisa Nakatani
Keyword(s):  
Formation Constants ◽  
Water Solvent

scholarly journals Oxovanadium(IV) Coordination Compounds with Kojic Acid Derivatives in Aqueous Solution

Molecules ◽  
2019 ◽  
Vol 24 (20) ◽  
pp. 3768
Author(s):  
Silvia Berto ◽  
Eugenio Alladio ◽  
Pier Giuseppe Daniele ◽  
Enzo Laurenti ◽  
Andrea Bono ◽  
...  
Keyword(s):  
Coordination Compounds ◽  
Kojic Acid ◽  
Formation Constants ◽  
Coordination Shell ◽  
Metal Species ◽  
Multivariate Curve Resolution ◽  
Chemical Systems ◽  
Insulin Mimetic ◽  
Species Formation ◽  
Rats And Mice

Hydroxypyrone derivatives have a good bioavailability in rats and mice and have been used in drug development. Moreover, they show chelating properties towards vanadyl cation that could be used in insulin-mimetic compound development. In this work, the formation of coordination compounds of oxovanadium(IV) with four kojic acid (5-hydroxy-2-(hydroxymethyl)-4-pyrone) derivatives was studied. The synthetized studied ligands (S2, S3, S4, and SC) have two or three kojic acid units linked through diamines or tris(2-aminoethyl)amine chains, respectively. The chemical systems were studied by potentiometry (25 °C, ionic strength 0.1 mol L−1 with KCl), and UV-visible and EPR spectroscopy. The experimental data were analyzed by a thermodynamic and a chemometric (Multivariate Curve Resolution–Alternating Least Squares) approach. Chemical coordination models were proposed, together with the species formation constants and the pure estimated UV-vis and EPR spectra. In all systems, the coordination of the oxovanadium(IV) starts already under acidic conditions (the cation is totally bound at pH higher than 3–4) and the metal species remain stable even at pH 8. Ligands S3, S4, and SC form three coordination species. Two of them are probably due to the successive insertion of the kojate units in the coordination shell, whereas the third is most likely a hydrolytic species.

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