@article {911,
	title = {"Icebergs" or no "Icebergs" in aqueous alcohols?: Composition-dependent mixing schemes},
	journal = {Journal of Physical Chemistry A},
	volume = {108},
	number = {17},
	year = {2004},
	note = {ISI Document Delivery No.: 814TNTimes Cited: 22Cited Reference Count: 38},
	month = {Apr},
	pages = {3873-3877},
	type = {Article},
	abstract = {The classical concept of "iceberg formation" is modified by our recent thermodynamic studies. The local enhancement of the hydrogen-bond network of H2O in the immediate vicinity of small nonelectrolyte solutes (i.e., the "iceberg formation") is still correct. However, the hydrogen-bond probability of bulk H2O away from solutes is reduced progressively, as the solute composition increases. When the hydrogen-bond probability of bulk H2O is reduced to the bond percolation threshold of the hexagonal ice connectivity, the hydrogen-bond percolation is lost and a qualitatively different mixing scheme sets in, whereby the solution consists of two kinds of clusters. In the solute-rich region, solute molecules form Clusters of its own kind. Thus, the "iceberg, formation" is basically correct within a narrow range in the H2O-rich region for small nonelectrolyte solutes. Thus, reference made to the "iceberg" concept in recent literatures should be clarified in terms of the concentration range and the size of solute in question.},
	keywords = {2-BUTOXYETHANOL, BUTANOL, fluctuations, hydration, HYDROPHOBIC SURFACES, MIXTURES, PARTIAL MOLAR VOLUMES, TERT-BUTYL ALCOHOL, WATER-RICH REGION, X-RAY-SCATTERING},
	isbn = {1089-5639},
	url = {<Go to ISI>://000220997100023},
	author = {Koga,Yoshikata and Nishikawa, K. and Westh, P.}
}
@article {656,
	title = {Excess partial molar entropy of alkane-mono-ols in aqueous solutions 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: 9Cited Reference Count: 21},
	month = {Feb},
	pages = {150-155},
	type = {Article},
	abstract = {In the preceding paper, we reported the values of model-free chemical potentials for aqueous methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, and 1-hexanol at 25degreesC over the entire compositional region. Using alcohol excess partial molar enthalpies, H-AL(E), determined earlier in this laboratory (Can. J. Chem. 74, 713 (1996)), we have calculated excess partial molar entropies for the alcohols, S-AL(E), where AL stands for an alcohol. We then calculated, numerically, the entropic interaction, S-AL-AL(E) = N(partial derivativeS(AL)(E)/partial derivativen(AL))(p,T,nW), where n(AL) is the amount of AL, n(W) is the amount of H2O, and N is the total amount of solution. S-AL-AL(E) signifies the effect of addition of AL upon the entropic situation of existing AL in solution. Using these quantities, the mixing schemes in aqueous alcohols have been studied. The earlier conclusions, which used H-AL(E) and H-AL-AL(E) alone, are confirmed. Furthermore, the order of the relative hydrophobic nature of alcohols is established from the behaviour of S-AL-AL(E) and of H-AL-AL(E) as methanol < ethanol < 2-propanol < 1-propanol.},
	keywords = {2-BUTOXYETHANOL, ALCOHOL, aqueous alcohols, BUTANOL, ENTHALPIES, entropic interaction, excess partial molar entropies, hydrophobicity ranking, MIXING SCHEME, MIXING SCHEMES, MIXTURES, NONELECTROLYTES, TRANSITION, VOLUMES, WATER-RICH REGION},
	isbn = {0008-4042},
	url = {<Go to ISI>://000181376800004},
	author = {Koga,Yoshikata and Westh, P. and Nishikawa, K.}
}
@article {3721,
	title = {Mixing schemes in aqueous solutions of nonelectrolytes: A thermodynamic approach},
	journal = {Journal of Physical Chemistry},
	volume = {100},
	number = {13},
	year = {1996},
	note = {ISI Document Delivery No.: UC398Times Cited: 92Cited Reference Count: 77},
	month = {Mar},
	pages = {5172-5181},
	type = {Article},
	abstract = {Thermodynamic studies were carried out on aqueous solutions of some nonelectrolytes. The quantities proportional to the second derivatives of Gibbs energy were measured directly and in small increments in mole fraction or temperature. Therefore, we were able to differentiate once more with respect to mole fraction or temperature. Generally, the higher the order of the derivative, the more detailed the information it contains. Using these second and third derivatives, an attempt was made at elucidating the mixing schemes, the way in which solute and solvent H2O molecules mix with each other. For the following nonelectrolytes studied so far, 2-butoxyethanol, tert-butyl alcohol, 2-butanone, isobutyric acid, and dimethyl sulfoxide, there are separate regions in the single-phase domain of the temperature-mole fraction field, in each of which the mixing scheme is qualitatively different from those of the other regions. The details of each mixing scheme were elucidated from the behavior of the second and third derivatives of Gibbs energy. In the water-rich region (I), the effect of a solute was suggested to enhance the hydrogen bonds of H2O in the vicinity of the solute but to diminish the hydrogen bond probability of the bulk H2O away from the solute. When the hydrogen bond probability at a certain region of bulk water decreases to that of the percolation threshold, this mixing scheme is no longer operative, and mixing scheme II sets in. The transition from the mixing scheme of region I to that in region (II) was found to accompany anomalies in the third derivatives of Gibbs energy, in contrast to the normal phase transitions which are associated with anomalies in the second derivatives of Gibbs energy. In the intermediate region (II), it was suggested that the solution consists of two kinds of clusters rich in each component. In the solute-rich region (III), at least for the 2-butoxyethanol and dimethyl sulfoxide cases, the clusters of purely solute molecules exist and H2O molecules are {\textquoteright}{\textquoteright}adsorbed{\textquoteright}{\textquoteright} on the surfaces of such clusters.},
	keywords = {2-BUTOXYETHANOL WATER, BUTANOL, CORRELATION LENGTH, HEAT-CAPACITIES, KIRKWOOD-BUFF PARAMETERS, LOCAL-STRUCTURE, MIXTURES, PARTIAL MOLAR ENTHALPIES, TERT-BUTYL ALCOHOL, WATER-RICH REGION, X-RAY-SCATTERING},
	isbn = {0022-3654},
	url = {<Go to ISI>://A1996UC39800006},
	author = {Koga,Yoshikata}
}
@article {2851,
	title = {EXCESS PARTIAL MOLAR ENTHALPIES AND FREE-ENERGIES IN METHANOL ISOBUTANOL MIXTURES AT 20-DEGREES-C - THE EFFECT OF SIZE DIFFERENCE},
	journal = {Thermochimica Acta},
	volume = {230},
	year = {1993},
	note = {ISI Document Delivery No.: MW430Times Cited: 0Cited Reference Count: 10},
	month = {Dec},
	pages = {39-53},
	type = {Article},
	abstract = {The excess partial molar enthalpies, H(m)E(i), and free energies, G(m)E(i), (where i is methanol or isobutanol) were determined at 20.00-degrees-C in methanol-isobutanol mixtures. The Bhatia-March approach (J. Phys. F, 5 (1975) 1100), taking into account the size difference between the components within the framework of the conformational solution theory, was applied to explain the composition dependence of H(m)E(i) and G(m)E(i). It was reasonably successful : however, it did not seem to work for the other isomeric butanol and methanol mixtures.},
	keywords = {25 DEGREES C, ALLOYS, BUTANOL, CONCENTRATION FLUCTUATIONS, NA-CS, SYSTEMS, WATER},
	isbn = {0040-6031},
	url = {<Go to ISI>://A1993MW43000004},
	author = {Lai, J. T. W. and Kam, J. S. C. and Lau, F. W. and Beach, L. J. and Koga,Yoshikata}
}
