@article {1258,
	title = {Fluctuation functions in aqueous NaCl and urea},
	journal = {Journal of Physical Chemistry B},
	volume = {109},
	number = {35},
	year = {2005},
	note = {ISI Document Delivery No.: 961UNTimes Cited: 4Cited Reference Count: 30},
	month = {Sep},
	pages = {16886-16890},
	type = {Article},
	abstract = {We earlier devised a set of fluctuation functions that provide relative qualitative differences of the amplitude (intensity) and the wavelength (extensity) of fluctuations in entropy and volume and the entropy-volume cross fluctuations. We discuss the mixing schemes in aqueous NaCl and urea using these fluctuation functions. Our earlier studies by using the second and third derivatives of Gibbs energy indicated that their effects on H2O are qualitatively different. An NaCl hydrates 7.5 molecules of H2O but leaves the bulk H2O away from the hydration shell unperturbed. Urea, on the other hand, connects onto the hydrogen bond network of H2O but retards the degree of fluctuation inherent in H2O. The behavior of the fluctuation functions calculated here are consistent with the above mixing schemes. Furthermore, urea was found to reduce the wavelength of fluctuation more strongly than NaCl.},
	keywords = {25-DEGREES-C, H2O, LIQUID WATER, MODEL, PARTIAL MOLAR FLUCTUATIONS, PERCOLATION, SODIUM-CHLORIDE, SYSTEMS, VOLUMETRIC PROPERTIES},
	isbn = {1520-6106},
	url = {<Go to ISI>://000231687400045},
	author = {Siu, D. and Koga,Yoshikata}
}
@article {4686,
	title = {Excess chemical potentials, excess partial molar enthalpies, entropies, volumes, and isobaric thermal expansivities of aqueous glycerol at 25 degrees C},
	journal = {Journal of Solution Chemistry},
	volume = {28},
	number = {10},
	year = {1999},
	note = {ISI Document Delivery No.: 247VPTimes Cited: 36Cited Reference Count: 27},
	month = {Oct},
	pages = {1137-1157},
	type = {Article},
	abstract = {The vapor pressures p the excess partial molar enthalpies of glycerol He,, the densities d and the thermal expansivities oc, of aqueous glycerol were measured at 25 degrees C. From the vapor pressure data, the excess chemical potential of H2O mu(W)(E) was calculated, assuming that the partial pressure of glycerol Poly is negligibly small. The excess chemical potential of glycerol mu(Gly)(E) was estimated by applying the Gibbs-Duhem relation and these data were used to calculate the excess partial molar entropies S-Gly(E). From the density data, the excess partial molar volumes of glycerol V-Gly(E) and from the thermal expansivity data, the normalized cross fluctuations (SV)Delta, introduced by us earlier, were evaluated. While the detailed manner in which glycerol modifies the molecular arrangement of H2O in its immediate vicinity is yet to be elucidated, the hydrogen bond probability in the bulk H2O away from solute molecules is reduced gradually as the glycerol composition increases to the point where putative presence of icelike patches is no longer possible. Thereupon, a qualitatively different mixing scheme seems to set in.},
	keywords = {2-BUTOXYETHANOL, aqueous glycerol, excess partial molar enthalpies and, fluctuations, MIXING SCHEME, MIXTURES, NONELECTROLYTES, normalized cross fluctuations, PERCOLATION, PRESSURES, TERT-BUTANOL, THERMAL EXPANSIVITIES, TRANSITION, vapor pressures, VOLUMES, WATER-RICH REGION},
	isbn = {0095-9782},
	url = {<Go to ISI>://000083241900003},
	author = {To, E. C. H. and Davies, J. V. and Tucker, M. and Westh, P. and Trandum, C. and Suh, K. S. H. and Koga,Yoshikata}
}
@article {4433,
	title = {How dilute is the Henry{\textquoteright}s law region? II},
	journal = {Journal of Physical Chemistry B},
	volume = {102},
	number = {25},
	year = {1998},
	note = {ISI Document Delivery No.: ZV967Times Cited: 13Cited Reference Count: 12},
	month = {Jun},
	pages = {4982-4987},
	type = {Article},
	abstract = {Vapor pressures for n-hexane-c-hexane were measured at extremely low concentrations of n-hexane. The vapor pressure data seemed to indicate within the experimental uncertainty that, in the range of the mole fraction of n-hexane x(nH) < 0.015, the solution obeys Henry{\textquoteright}s law. However, the excess partial molar enthalpy of n-hexane and c-hexane measured by a sensitive microcalorimeter showed that the Henry{\textquoteright}s law is not operative above x(nH) or x(cH) approximate to 2 x 10(-4), the lowest accessible for the calorimetry technique available at present. The excess partial molar enthalpies of the following solutes were also determined in aqueous solutions in an extremely dilute region. Within the experimental technique at our disposal, we could not locate a finite range of Henry{\textquoteright}s law. Thus, whether the solute-solute interaction becomes actually absent or whether such absence depends on the nature of the solvent (H2O or organic) cannot be addressed at present. For aqueous solutions, however, the lower limits of the mole fraction of a solute, above which the solutions behave as non-Henry-like, were found by an order of magnitude lower: 1 x 10(-5) for 2-butoxyethanol; 3 x 10(-5) for tert-butyl alcohol; 2 x 10(-5) for glycerol; 3 x 10(-5) for urea.},
	keywords = {H2O, PERCOLATION, TERT-BUTANOL MIXTURES, VAPOR-PRESSURES, WATER},
	isbn = {1089-5647},
	url = {<Go to ISI>://000074360300017},
	author = {Westh, P. and Haynes, C. A. and Koga,Yoshikata}
}
@article {4422,
	title = {Intermolecular interactions in tert-butyl alcohol dimethyl sulfoxide H2O: Chemical potentials, partial molar entropies and volumes},
	journal = {Journal of Physical Chemistry B},
	volume = {102},
	number = {26},
	year = {1998},
	note = {ISI Document Delivery No.: ZY137Times Cited: 13Cited Reference Count: 28},
	month = {Jun},
	pages = {5182-5195},
	type = {Article},
	abstract = {The excess chemical potentials, the excess partial molar entropies, and the partial molar volumes in tert-butyl alcohol (TBA)-dimethyl sulfoxide (DMSO)-H2O mixtures were determined. These data, together with previously published excess partial molar enthalpies (Fluid Phase Equilib. 1997, 136, 207) were used to evaluate intermolecular interactions. The TBA-TBA and TBA-DMSO, and DMSO-DMSO interactions were found to be crucially dependent on the composition. The net interaction in terms of chemical potential is very intricate. For example, net interactions of DMSO with a hydrophobic moiety (represented here by TEA) change from attractive to repulsive as the composition changes. This suggests that general discussions of the affinity of DMSO for nonpolar groups (or surfaces) are meaningful only by specifying the composition region. The interactions in terms of enthalpy and entropy are an order of magnitude larger and strongly compensating. Anomalous changes in the enthalpic/entropic interactions and hence qualitative changes in the mixing scheme of the solution, previously described in respective binary TBA-H2O and DMSO-H2O systems, are also apparent in this ternary system. II was found that as the mole fraction, x(D), of DMSO (third component) increases, the transition in mixing scheme occurred at a progressively lower value of x(B). The behavior of partial molar volume indicated that as x(B) increases, the initial increase in the partial molar volume of H2O on increasing x(D), reminiscent to "iceberg formation", diminished. This suggests that existing TEA molecules already made their contribution to the "iceberg formation". The DMSO-DMSO interaction in terms of volume also showed that the transition occurred at a smaller value of x(D) than that for x(B) = 0. The boundary between the two mixing schemes in the present ternary mixture was a straight line in the x(D)-x(B) field, suggesting that the effect of TEA and DMSO on H2O, causing the transition in the mixing scheme, is additive.},
	keywords = {AQUEOUS-SOLUTIONS, ENTHALPIES, HYDROPHOBIC INTERACTION, MIXING SCHEME, MIXTURES, NONELECTROLYTES, NONPOLAR SOLUTE PARTICLES, PERCOLATION, TRANSITION, WATER-RICH REGION},
	isbn = {1089-5647},
	url = {<Go to ISI>://000074590000026},
	author = {Trandum, C. and Westh, P. and Haynes, C. A. and Koga,Yoshikata}
}
