@article {2474,
	title = {Spectrum of Excess Partial Molar Absorptivity. I. Near Infrared Spectroscopic Study of Aqueous Acetonitrile and Acetone},
	journal = {Journal of Physical Chemistry B},
	volume = {113},
	number = {35},
	year = {2009},
	note = {ISI Document Delivery No.: 487EETimes Cited: 4Cited Reference Count: 22Koga, Yoshikata Sebe, Fumie Minami, Takamasa Otake, Keiko Saitow, Ken-ichi Nishikawa, Keiko},
	month = {Sep},
	pages = {11928-11935},
	type = {Article},
	abstract = {We study the mixing schemes or the molecular processes occurring in aqueous acetonitrile (ACN) and acetone (ACT) by near-infrared spectroscopy (NIR). Both solutions (any other aqueous solutions) are not free from strong and complex intermolecular interactions. To tackle such a many-body problem, we first use the concept of the excess molar absorptivity, epsilon(E), which is a function of solute mole fraction in addition to that of wavenumber, nu. The plots of F E calculated from NIR spectra for both aqueous solutions against nu showed two clearly separated bands at 5020 and 5230 cm(-1); the former showed negative and the latter positive peaks. At zero and unity mole fractions of solute, epsilon(E) is identically zero independent of v. Similar to the thermodynamic excess functions, both negative and positive bands grow in size from zero to the minimum (or the maximum) and back to zero, as the mole fraction varies from 0 to 1. Since the negative band{\textquoteright}s nu-locus coincides with the NIR spectrum of ice, and the positive with that of liquid H2O, we suggest that on addition of solute the "ice-likeness" decreases and the "liquid-likeness" increases, reminiscent of the two-mixture model for liquid H2O. The modes of these variations, however, are qualitatively different between ACN-H2O and ACT-H2O. The former ACN is known to,let as a hydrophobe and ACT as a hydrophile from Our previous thermodynamic studies. To see the difference more clearly, we introduced and calculated the excess partial molar absorptivity of ACN and ACT, epsilon(E)(N), and epsilon(E,)(T) respectively. The mole fraction dependences of epsilon(E)(N) and epsilon(E)(T) show qualitatively different behavior and are consistent with the detailed mixing schemes elucidated by our earlier differential thermodynamic studies. Furthermore, we found in the H2O-rich region that the effect of hydrophobic ACN is acted on the negative band at 5020 cm(-1), while that of hydrophilic ACT is on the positive high-energy band. Thus, the present method of analysis adds more detailed insight into the difference between a hydrophobe and a hydrophile in their effects on H2O.},
	keywords = {2-DIMENSIONAL CORRELATION SPECTROSCOPY, 25-DEGREES-C, CHEMICAL-POTENTIALS, ENTHALPIES, ENTROPIES, HYDROGEN-BONDS, MIXTURES, NON-ELECTROLYTES, TEMPERATURE, WATER},
	isbn = {1520-6106},
	url = {<Go to ISI>://000269252700016},
	author = {Koga,Yoshikata and Sebe, F. and Minami, T. and Otake, K. and Saitow, K. and Nishikawa, K.}
}
@article {634,
	title = {Chemical potential and concentration fluctuation in some aqueous alkane-mono-ols at 25 degrees C},
	journal = {Canadian Journal of Chemistry-Revue Canadienne De Chimie},
	volume = {81},
	number = {2},
	year = {2003},
	note = {ISI Document Delivery No.: 652JVTimes Cited: 14Cited Reference Count: 40},
	month = {Feb},
	pages = {141-149},
	type = {Article},
	abstract = {Vapour pressures of binary aqueous solutions of methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, and 1-hexanol were measured at 25.00(o)C in small compositional increments over the entire compositional range. Without resorting to any fitting function, the partial pressures were calculated numerically by methods based on the Gibbs-Duhem relation. When the system had an azeotrope, near which the numerical methods caused large errors, a graphical readjustment was applied such that the concentration fluctuation, S-XX(0) = RT(1 - x(AL))/(partial derivativemu (E)(AL)/partial derivativex(AL)), connected smoothly across the azeotrope. Values of S-XX(0) from scattering experiments were also used as a guide for the readjustment procedure. Hence, we report here chemical potential data free from any model or any fitting function.},
	keywords = {1-PROPANOL, 2-PROPANOL, aqueous mono-ols, BUTANOL MIXTURES, CONCENTRATION FLUCTUATIONS, ENTROPIES, KIRKWOOD-BUFF PARAMETERS, mixing, PARTIAL MOLAR ENTHALPIES, partial pressures by the Boissonnas method, SCHEMES, TERT-BUTYL ALCOHOL, WATER-RICH REGION, X-RAY-SCATTERING},
	isbn = {0008-4042},
	url = {<Go to ISI>://000181376800003},
	author = {Hu, J. H. and Haynes, C. A. and Wu, A. H. Y. and Cheung, C. M. W. and Chen, M. M. and Yee, E. G. M. and Ichioka, T. and Nishikawa, K. and Westh, P. and Koga,Yoshikata}
}
@article {709,
	title = {Excess chemical potentials and partial molar enthalpies in aqueous 1,2-and 1,3-propanediols at 25 degrees C},
	journal = {Journal of Solution Chemistry},
	volume = {32},
	number = {2},
	year = {2003},
	note = {ISI Document Delivery No.: 661CMTimes Cited: 4Cited Reference Count: 24},
	month = {Feb},
	pages = {137-153},
	type = {Article},
	abstract = {Excess chemical potentials and excess partial molar enthalpies of 1,2- and 1,3-propanediols ( abbreviated as 12P and 13P), mu(i)(E), and H-i(E) ( i = 12P or 13P) were determined in the respective binary aqueous solutions at 25degreesC. For both systems, the values of mu(i)(E) are almost zero, within +/-0.4 kJ-mol(-1). However, the excess partial molar enthalpies, H-i(E) show a sharp mole fraction dependence in the water-rich region. Thus, the systems are highly nonideal, in spite of almost zero mu(i)(E). Namely, the enthalpy-entropy compensation is almost complete. From the slopes of the HE i against the respective mole fraction x(i) we obtain the enthalpic interaction functions between solutes, H-i-i(E), ( i = 12P or 13P). Using these quantities and comparing them with the equivalent quantities for binary aqueous solutions of 1-propanol ( 1P), 2-propanol (2P), glycerol (Gly), and dimethyl sulfoxide ( DMSO), we conclude that there are three composition regions in each of which mixing schemes are qualitatively different. Mixing Schemes II and III, operative in the intermediate and the solute-rich regions, seem similar in all the binary aqueous solutions mentioned above. Mixing Scheme I in the water-rich region is different from solute to solute. 12P shows a behavior similar to that of DMSO, which is somewhat different from typical hydrophobic solute, 1P or 2P. 13P, on the other hand, is less hydrophobic than 12P, and shows a behavior closer to glycerol, which shows hydrophilic behavior.},
	keywords = {2-and 1, 3-propanediols, ALCOHOL, chemical potentials, ENERGIES, ENTHALPIES, ENTROPIES, H2O, interaction functions, MIXING SCHEMES, mixing schemes in aqueous 1, MOLECULAR-ORGANIZATION, NONELECTROLYTES, partial molar, TERT-BUTANOL MIXTURES, VOLUMES, WATER-RICH REGION},
	isbn = {0095-9782},
	url = {<Go to ISI>://000181873700003},
	author = {Parsons, M. T. and Lau, F. W. and Yee, E. G. M. and Koga,Yoshikata}
}
@article {421,
	title = {Mixing schemes in ternary aqueous solutions - Thermodynamic approach},
	journal = {Journal of Thermal Analysis and Calorimetry},
	volume = {69},
	number = {3},
	year = {2002},
	note = {ISI Document Delivery No.: 604BRTimes Cited: 8Cited Reference Count: 282nd International Symposium on the New Frontiers of Thermal Studies of MaterialsNOV 25-27, 2001SUZUKAKEDAI, JAPAN},
	pages = {705-716},
	type = {Proceedings Paper},
	abstract = {The enthalpic interaction functions introduced by us earlier were evaluated in some ternary aqueous solutions. They are determined purely experimentally without resorting to any model system. From them, the pair interaction coefficients based on the virial expansion were evaluated, which will serve for a future theoretical development based on the McMillan-Mayer theory of solution. Secondly, our new methodology of using the mole fraction dependence of the enthalpic interaction function as a probe to elucidate the effect of a third component on the molecular organization is introduced. The conclusions for selected third components in ternary aqueous 1-propanol are reviewed.},
	keywords = {25-DEGREES-C, effect of selected solutes on the molecular organization of H2O, enthalpic interaction functions, ENTROPIES, EXCESS CHEMICAL-POTENTIALS, H2O, MOLECULAR-ORGANIZATION, pair interaction coefficients, PARTIAL MOLAR ENTHALPIES, ternary aqueous solutions, TERT-BUTANOL, TETRAMETHYL UREA, the, VOLUMES, WATER},
	isbn = {1418-2874},
	url = {<Go to ISI>://000178596200002},
	author = {Koga,Yoshikata}
}
@article {5094,
	title = {Additive effect of 1-propanol and 2-propanol on molecular organization of H2O in the water-rich region: Excess chemical potential, partial molar enthalpy and volume of 1-propanol in 1-propanol-2-propanol-H2O at 25 degrees C},
	journal = {Bulletin of the Chemical Society of Japan},
	volume = {74},
	number = {5},
	year = {2001},
	note = {ISI Document Delivery No.: 443WKTimes Cited: 16Cited Reference Count: 25},
	month = {May},
	pages = {809-816},
	type = {Article},
	abstract = {Excess chemical potential, mu (E)(1P), partial molar enthalpy, H-1P(E) and volume of 1-propanol, V-1P(E), were determined as a function of mole fraction of l-propanol, rip, in mixed solvents of aqueous 2-propanol with various initial mole fraction of 2-propanol, x(2P)(0). The 1-propanol-1-propanol interaction functions, H-1P-1P(E) equivalent to N(partial derivativeH(1P)(E)/partial derivativen(1P)), and V-1P-1P(E) equivalent to N(partial derivativeV(1P)(E)/ partial derivativen(1P)), were evaluated by graphical differentiation. The rip-dependence of all these quantities indicates that l-propanol and 2-propanol modify the molecular organization of H2O in the same and additive manner in the water-rich region. The additive effect of 1-propanol and that of 2-propanol are in the ratio of (0.07/0.08).},
	keywords = {25-DEGREES-C, AQUEOUS 2-BUTOXYETHANOL, ENTROPIES, fluctuations, INTERMOLECULAR INTERACTIONS, LYSOZYME, MIXING SCHEMES, MIXTURES, TERT-BUTANOL},
	isbn = {0009-2673},
	url = {<Go to ISI>://000169365200004},
	author = {Hu, J. H. and Chiang, W. M. D. and Westh, P. and Chen, D. H. C. and Haynes, C. A. and Koga,Yoshikata}
}
@article {5032,
	title = {Excess partial molar enthalpy of 1-propanol in 1-propanol-acetone (or tetramethyl urea)-H2O at 25 degrees C: effect of acetone (or tetramethyl urea) on H2O},
	journal = {Fluid Phase Equilibria},
	volume = {189},
	number = {1-2},
	year = {2001},
	note = {ISI Document Delivery No.: 495HBTimes Cited: 6Cited Reference Count: 11},
	month = {Oct},
	pages = {31-38},
	type = {Article},
	abstract = {Excess partial molar enthalpies of 1-propanol, H-1P(E), were measured at 25 degreesC in ternary 1-propanol-acetone (or tetramethyl urea)-H2O, with various initial compositions of acetone (or tetramethyl urea). They were determined accurately and in small increments in mole fraction of 1-propanol. It was therefore, possible to take a derivative of H-1P(E) with respect to the amount of 1-propanol, n(1P), H-1P-1P(E) = N (partial derivativeH(1P)(E)/partial derivativen(1P)). The changes in the mole fraction dependence of H-1P(E) and hence, H-1P-1P(E) caused by adding a third component, acetone or tetramethyl urea, were compared with the results of analogous earlier studies with urea and 2-propanol as a third component. The effects of acetone and tetramethyl urea were found qualitatively the same. The CH3- group in each compound works as a typical hydrophobic moiety and enhances the hydrogen bond network of H2O in the immediate vicinity of solute molecule ("iceberg formation") with concomitant reduction of the hydrogen bond probability of H2O. The C=O group on the other hand, seems to reduce the degree of fluctuation in the hydrogen bond strength in the bulk H2O away from the solute. (C) 2001 Elsevier Science B.V. All rights reserved.},
	keywords = {1-PROPANOL, 1-propanol-1-propanol enthalpic interaction, 1-propanol-acetone (or tetramethyl urea)-H2O, acetone or tetramethyl urea on H2O, CHEMICAL-POTENTIALS, effect of, ENTROPIES, fluctuations, partial molar enthalpy of, TERT-BUTANOL},
	isbn = {0378-3812},
	url = {<Go to ISI>://000172333200003},
	author = {Chen, D. H. C. and Liu, A. P. C. and Koga,Yoshikata}
}
@article {5159,
	title = {A thermodynamic study of 1-propanol-glycerol-H2O at 25 degrees C: Effect of glycerol on molecular organization of H2O},
	journal = {Journal of Solution Chemistry},
	volume = {30},
	number = {11},
	year = {2001},
	note = {ISI Document Delivery No.: 514HPTimes Cited: 29Cited Reference Count: 36},
	month = {Nov},
	pages = {1007-1028},
	type = {Article},
	abstract = {The excess chemical potential, partial molar enthalpy, and volume of 1-propanol were determined in ternary mixtures of 1-propanol-glycerol-H2O at 25degreesC. The mole fraction dependence of all these thermodynamic functions was used to elucidate the effect of glycerol on the molecular organization of H2O. The glycerol molecules do not exert a hydrophobic effect on H2O. Rather, the hydroxyl groups of glycerol, perhaps by forming clusters via its alkyl backbone with hydroxyl groups pointing outward, interact with H2O so as to reduce the characteristics of liquid H2O. The global hydrogen bond probability and, hence, the percolation nature of the hydrogen bond network is reduced. In addition, the degree of fluctuation inherent in liquid H2O is reduced by glycerol perhaps by participating in the hydrogen bond network via OH groups. At infinite dilution, the pair interaction coefficients in enthalpy were evaluated and these data suggest a possibility that the interaction is mediated through H2O.},
	keywords = {1-propanol-glycerol-H2O, AQUEOUS-SOLUTIONS, CHEMICAL-POTENTIALS, effect of glycerol on H2O, enthalpy of 1-propanol, ENTROPIES, excess chemical potential, fluctuations, interactions, INTERMOLECULAR, INTERMOLECULAR INTERACTIONS, MIXING SCHEMES, partial molar, PARTIAL MOLAR ENTHALPIES, partial molar volume of 1-propanol, TERT-BUTANOL, VOLUMES, WATER},
	isbn = {0095-9782},
	url = {<Go to ISI>://000173433400005},
	author = {Parsons, M. T. and Westh, P. and Davies, J. V. and Trandum, C. and To, E. C. H. and Chiang, W. M. and Yee, E. G. M. and Koga,Yoshikata}
}
@article {3830,
	title = {Excess partial molar enthalpies of alkane-mono-ols in aqueous solutions},
	journal = {Canadian Journal of Chemistry-Revue Canadienne De Chimie},
	volume = {74},
	number = {5},
	year = {1996},
	note = {ISI Document Delivery No.: UP791Times Cited: 50Cited Reference Count: 29},
	month = {May},
	pages = {713-721},
	type = {Article},
	abstract = {Excess partial molar enthalpies, H-A(E), of methanol, ethanol, and 1- and 2-propanols in aqueous solutions were measured directly, accurately, and in small increments in mole fraction at 25 degrees C. From these data, the solute-solute enthalpic interactions, H-AA(E) = N(partial derivative H-A(E)/partial derivative n(A)), were evaluated for each alcohol. These data indicate that three distinctively different mixing schemes, I, II, and III exist, as was the case for aqueous 2-butoxyethanol previously studied in our laboratory. The transition from mixing scheme I to II appears to take place gradually within a small composition range. As the hydrophobic moiety becomes smaller from 2-butoxyethanol to methanol, the locus of the transition moves to a higher value in mole fraction of the alcohol. At the same time, the range of transition becomes wider and the solute-solute enthalpic interaction weaker.},
	keywords = {1-PROPANOL, 2-BUTOXYETHANOL, 2-PROPANOL, 25-DEGREES-C, BUTYL ALCOHOL-SOLUTIONS, CONCENTRATION FLUCTUATIONS, enthalpic interaction, ENTROPIES, ETHANOL, excess partial molar enthalpies in aqueous solutions, FREE-ENERGIES, METHANOL, MIXING SCHEME, TERT-BUTANOL MIXTURES, TRANSITION, transition of, WATER-RICH REGION},
	isbn = {0008-4042},
	url = {<Go to ISI>://A1996UP79100011},
	author = {Tanaka, S. H. and Yoshihara, H. I. and Ho, A. W. C. and Lau, F. W. and Westh, P. and Koga,Yoshikata}
}
@article {3412,
	title = {EXCESS PARTIAL MOLAR ENTHALPIES, ENTROPIES, GIBBS ENERGIES, AND VOLUMES IN AQUEOUS DIMETHYLSULFOXIDE},
	journal = {Journal of Solution Chemistry},
	volume = {24},
	number = {1},
	year = {1995},
	note = {ISI Document Delivery No.: QF279Times Cited: 60Cited Reference Count: 20},
	month = {Jan},
	pages = {89-102},
	type = {Article},
	abstract = {The excess partial molar enthalpies, the vapor pressures, and the densities of dimethylsulfoxide (DMSO) - H2O mixtures were measured and the excess partial molar Gibbs energies and the partial molar volumes were calculated for DMSO and for H2O. The values of the excess partial molar Gibbs energies for both DMSO and H2O are negative over the entire composition range. The results for the water-rich region indicated that the presence of DMSO enhances the hydrogen bond network of H2O. Unlike monohydric alcohols, however, the solute-solute interaction is repulsive in terms of the Gibbs energy. This was a result of the fact that the repulsion among solutes in terms of enthalpy surpassed the attraction in terms of entropy. The data in the DMSO-rich region suggest that DMSO molecules form clusters which protect H2O molecules from exposure to the nonpolar alkyl groups of DMSO.},
	keywords = {2-BUTOXYETHANOL, 25-DEGREES-C, AQUEOUS DIMETHYLSULFOXIDE, DIMETHYL-SULFOXIDE, ENTROPIES, excess partial molar enthalpies, GIBBS ENERGIES AND VOLUMES, HEAT-CAPACITIES, LIQUID-MIXTURES, MIXING SCHEME, RANGE, SOLUTE-SOLUTE INTERACTION, TRANSITION, WATER-RICH REGION},
	isbn = {0095-9782},
	url = {<Go to ISI>://A1995QF27900007},
	author = {Lai, J. T. W. and Lau, F. W. and Robb, D. and Westh, P. and Nielsen, G. and Trandum, C. and Hvidt, A. and Koga,Yoshikata}
}
