@article {2302,
	title = {Experimental determination of the third derivative of G. I. Enthalpic interaction},
	journal = {Journal of Chemical Physics},
	volume = {129},
	number = {21},
	year = {2008},
	note = {ISI Document Delivery No.: 379XWTimes Cited: 2Cited Reference Count: 19Westh, Peter Inaba, Akira Koga, Yoshikata},
	month = {Dec},
	pages = {4},
	type = {Article},
	abstract = {The solute (i)-solute interaction in terms of enthalpy, H-i-i(E)=N(partial derivative H-2(E)/partial derivative n(i)(2))=(1-x(i))(partial derivative H-2(E)/partial derivative n(i)partial derivative x(i)), the third derivative of G, was experimentally determined using a Thermal Activity Monitor isothermal titration calorimeter for aqueous solutions of 2-butoxyethanol (BE) and 1-propanol (1P). This was done using both calorimetric reference and sample vessels actively. We simultaneously titrate small and exactly equal amounts of solute i (=BE or 1P) into both cells which contain the binary mixtures at an average mole fraction, x(i), which differs by a small amount Delta x(i). The appropriate amount of titrant delta n(i) was chosen so that the quotient (delta H-E/delta n(i)) can be approximated as (partial derivative H-E/partial derivative n(i)), and so that the scatter of the results is reasonable. delta H-E is the thermal response from an individual cell on titration, and we measure directly the difference in the thermal response between the two cells, Delta(delta H-E). The resulting quotient, Delta(delta H-E)/delta n(i)/Delta x(i), can be approximated as (partial derivative H-2(E)/partial derivative n(i)partial derivative x(i)) and hence provides a direct experimental avenue for the enthalpy interaction function. We varied the value of Delta x(i) to seek its appropriate size. Since H-E contains the first derivative of G with respect to T, the result is the third derivative quantity. Thus we present here a third derivative quantity directly determined experimentally for the first time.},
	keywords = {AQUEOUS-SOLUTIONS, calorimetry, DYNAMICS, enthalpy, fluctuations, H2O, HOFMEISTER SERIES, LIQUID MIXTURES, MOLECULAR-ORGANIZATION, organic compounds, SOLVATION, WATER},
	isbn = {0021-9606},
	url = {<Go to ISI>://000261430900001},
	author = {Westh, P. and Inaba, A. and Koga,Yoshikata}
}
@article {1523,
	title = {Kirkwood-Buff integrals of aqueous alcohol binary mixtures},
	journal = {Journal of Chemical Physics},
	volume = {124},
	number = {12},
	year = {2006},
	note = {ISI Document Delivery No.: 028CPTimes Cited: 16Cited Reference Count: 32},
	month = {Mar},
	pages = {9},
	type = {Article},
	abstract = {The Kirkwood-Buff integrals of some binary aqueous alcohol mixtures are computed from the available vapor pressure measurements and compared with previous results as well as small angle neutron scattering experiments. The emphasis of the present report is on accuracy of the results that can be achieved by these two different types of measurements. This seems to be needed, mainly in view of the discrepancies between the various published results, as shown herein. It is argued that agreement in peak positions is more important than that in magnitude. In general, very good agreement is obtained by both methods, and sources of disagreements are discussed. The issue of the computer simulations of aqueous systems and the problematics related to correlations, microheterogeneity, and consequently the Kirkwood-Buff integrals are equally discussed herein.},
	keywords = {25-DEGREES-C, fluctuations, FORCE-FIELD, LIQUID-MIXTURES, MIXING SCHEME, PARAMETERS, PARTICLE NUMBER, TERT-BUTYL ALCOHOL, WATER MIXTURES, X-RAY-SCATTERING},
	isbn = {0021-9606},
	url = {<Go to ISI>://000236464000052},
	author = {Perera, A. and Sokolic, F. and Almasy, L. and Koga,Yoshikata}
}
@article {1350,
	title = {Single molecule force spectroscopy reveals a weakly populated microstate of the FnIII domains of tenascin},
	journal = {Journal of Molecular Biology},
	volume = {361},
	number = {2},
	year = {2006},
	note = {ISI Document Delivery No.: 074WPTimes Cited: 8Cited Reference Count: 48Cao, Y. Li, Hongbin},
	month = {Aug},
	pages = {372-381},
	type = {Article},
	abstract = {The native states of proteins exist as an ensemble of conformationally similar microstates. The fluctuations among different microstates are of great importance for the functions and structural stability of proteins. Here, we demonstrate that single molecule atomic force microscopy (AFM) can be used to directly probe the existence of multiple folded microstates. We used the AFM to repeatedly stretch and relax a recombinant tenascin fragment TNfnALL to allow the fibronectin type III (FnIII) domains to undergo repeated unfolding/refolding cycles. In addition to the native state, we discovered that some FnIII domains can refold from the unfolded state into a previously unrecognized microstate, N* state. This novel state is conformationally similar to the native state, but mechanically less stable. The native state unfolds at similar to 120 pN, while the N* state unfolds at similar to 50 pN. These two distinct populations of microstates constitute the ensemble of the folded states for some FnIII domains. An unfolded FnIII domain can fold into either one of the two microstates via two distinct folding routes. These results reveal the dynamic and heterogeneous picture of the folded ensemble for some FnIII domains of tenascin, which may carry important implications for the mechanical functions of tenascins in vivo. (c) 2006 Elsevier Ltd. All rights reserved.},
	keywords = {DYNAMICS, fluctuations, FnIII domains, HYDROGEN-EXCHANGE, IMMUNOGLOBULIN, MECHANICAL STABILITY, mechanical unfolding, microscopy, MODULES, PROTEIN-STRUCTURE, scanning probe, single-molecule force spectroscopy, tenascin, TITIN, UNFOLDING PATHWAYS},
	isbn = {0022-2836},
	url = {<Go to ISI>://000239842800014},
	author = {Cao, Y. and Li, H. B.}
}
@article {1202,
	title = {Effect of an "ionic liquid" cation, 1-butyl-3-methylimidazolium, on the molecular organization of H2O},
	journal = {Journal of Physical Chemistry B},
	volume = {109},
	number = {18},
	year = {2005},
	note = {ISI Document Delivery No.: 924MMTimes Cited: 46Cited Reference Count: 46},
	month = {May},
	pages = {9014-9019},
	type = {Article},
	abstract = {The excess partial molar enthalpy of 1-propanol (1P), H-1P(E), was measured at 28 \&DEG; C in the ternary mixture of 1P-1-butyl-3-methylimidazolium chloride ([bmim]Cl)-H2O in the H2O-rich composition range. From these data we evaluated what we call the 1P-1P enthalpic interaction function, H-1P-1P(E). Its changes induced by addition of (bmim]Cl of the pattern of H-1P-1P(E) were used as a probe to elucidate the effect of [bmim]Cl on the molecular organization of H2O. It was found that the effect of Cl- was not conspicuous within this methodology, and the observed dependence is predominantly due to the hydration of [bmim](+). The changes in the \&chi;(1P)-dependence of H-1P-1P(E) were compared with those brought about by temperature increase, or by the addition of fructose or glycerol. It was found that the effect of [bmim](+) is similar to that of fructose or increased temperature. We speculate that in the H2O-rich composition region a number of H2O molecules are attracted to the delocalized positive charge of the imidazolium ring and the bulk of H2O is influenced in such a manner that the global hydrogen bond probability is reduced.},
	keywords = {25-DEGREES-C, ALKANE-MONO-OLS, AQUEOUS-SOLUTIONS, fluctuations, HEXAFLUOROPHOSPHATE, MIXING SCHEMES, PARTIAL MOLAR ENTHALPIES, SOLVENTS, TERT-BUTANOL MIXTURES, WATER SOLUTIONS},
	isbn = {1520-6106},
	url = {<Go to ISI>://000228982900071},
	author = {Miki, K. and Westh, P. and Nishikawa, K. and Koga,Yoshikata}
}
@article {1227,
	title = {Hydration number of glycine in aqueous solution: An experimental estimate},
	journal = {Journal of Chemical Physics},
	volume = {123},
	number = {23},
	year = {2005},
	note = {ISI Document Delivery No.: 996ADTimes Cited: 6Cited Reference Count: 31},
	month = {Dec},
	pages = {6},
	type = {Article},
	abstract = {An experimental estimate of hydration number, N-H, of glycine in aqueous solution is given by using the calorimetric methodology developed by us earlier, which is briefly reviewed. We found N-H to be 7 +/- 0.6 for glycine presumably in the zwitter ion form, 10 +/- 1 for sodium glycinate, and 5 +/- 0.4 for glycine hydrochloride. Both glycine and sodium glycinate seem to work purely as a hydration center without altering the nature of the bulk H2O away from the hydration shell. Glycine hydrochloride, in addition to the role of hydration center, seems also to act as a typical hydrophilic species such as polyols, urea, or polyethylene glycols. Hence, the effect of the latter on H2O is of a long range, like other hydrophilic species. (c) 2005 American Institute of Physics.},
	keywords = {25-DEGREES-C, fluctuations, H2O, INTRAMOLECULAR PROTON-TRANSFER, MIXING SCHEMES, MOLECULAR-ORGANIZATION, NONELECTROLYTES, PARTIAL MOLAR ENTHALPIES, TAUTOMERIZATION, WATER},
	isbn = {0021-9606},
	url = {<Go to ISI>://000234145900026},
	author = {Parsons, M. T. and Koga,Yoshikata}
}
@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 {912,
	title = {Toward understanding the Hofmeister series. 1. Effects of sodium salts of some anions on the molecular organization of H2O},
	journal = {Journal of Physical Chemistry A},
	volume = {108},
	number = {40},
	year = {2004},
	note = {ISI Document Delivery No.: 858TGTimes Cited: 18Cited Reference Count: 28},
	month = {Oct},
	pages = {8533-8541},
	type = {Article},
	abstract = {We studied a detailed thermodynamic behavior of 1-propanol (abbreviated as 1P) in mixed solvents of aqueous Na2SO4, NaOOCCH3, and NaClO4, and NaSCN. We measured the excess partial molar enthalpy of 1P, H-1P(E), in these mixed solvents at various initial salt concentrations. We then evaluated what we call the enthalpic interaction, H-1P-1P(E) = (partial derivativeH(1P)(E)/partial derivativen(1P)), where n(1P) is the amount of 1P. The composition dependence of H-1P-1P(E) changes in a characteristic manner on addition of a specific salt. This induced change in the behavior of H-1P-1P(E) is used to elucidate the effect of the salt on the molecular organization of H2O. Na+ ion seems to hydrate a number less than seven or eight molecules of H2O, leaving the bulk H2O outside the hydration shell unperturbed. SO42- also hydrates a number less than 26 H2O molecules with a concomitant increase in the degree of fluctuation of the bulk H2O. Na2SO4 as a whole hydrates the total of 26 H2O. CH3COO- ion modifies H2O in a similar manner as an alcohol. Cl- ion hydrates a number less than seven or eight H2O molecules leaving the bulk H2O in the same state as in pure H2O. NaCl as a whole hydrates the total of seven or eight molecules of H2O. ClO4- and SCN- participate in hydrogen bonding with the hydrogen bond network of H2O keeping its connectivity intact. However, they reduce the degree of fluctuation inherent in liquid H2O. Thus, each ion has its own unique manner of modifying H2O, except that ClO4- and SCN- modify H2O in almost the same way. Therefore, it seems fair to state that the phenomenological net result manifested as the Hofmeister series is due to multifacetted factors working in the holistic manner, and a single or a small number of parameters is not sufficient to explain its effect.},
	keywords = {1-PROPANOL, 25-DEGREES-C, ALKANE-MONO-OLS, AQUEOUS-SOLUTIONS, fluctuations, MIXING SCHEMES, PARTIAL MOLAR ENTHALPIES, THERMODYNAMIC APPROACH, WATER},
	isbn = {1089-5639},
	url = {<Go to ISI>://000224214100050},
	author = {Koga,Yoshikata and Westh, P. and Davies, J. V. and Miki, K. and Nishikawa, K. and Katayanagi, H.}
}
@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 {4949,
	title = {Mixing scheme of aqueous butan-1-ol in the water-rich region at 25 degrees C: Excess chemical potential, partial molar enthalpy, entropy and volume, heat capacity compressibility and thermal expansivity},
	journal = {Physical Chemistry Chemical Physics},
	volume = {2},
	number = {3},
	year = {2000},
	note = {ISI Document Delivery No.: 286KDTimes Cited: 15Cited Reference Count: 20},
	month = {Feb},
	pages = {355-359},
	type = {Article},
	abstract = {We determined excess chemical potential, partial molar enthalpy, entropy and volume, heat capacity, isothermal compressibility and thermal expansivity for aqueous butan-1-ol in the water-rich region up to the phase separation boundary at 25 degrees C. The latter three response functions were used to calculate the mean-square fluctuation densities, which signifies the amplitude, or the intensity, of fluctuations in volume, entropy or cross (entropy-volume) fluctuations. Furthermore, we calculated the (mean-square) normalized fluctuations that are indicative of the wavelength, or the extensity, as well as the amplitude of respective fluctuations. The behaviour of these thermodynamic quantities were compared with those obtained earlier in this laboratory for aqueous methanol, ethanol, propan-1-ol, tert-butanol (tert-butyl alcohol), and 2-butoxyethanol. We conclude that in the water-rich region of aqueous butan-1-ol, mixing scheme I is operative as in other alcohols, whereby butan-1-ol molecules enhance the hydrogen bond network of H2O in their immediate vicinities with concomitant reduction of hydrogen bond probability in the bulk H2O away from solutes. However, before reaching the phase separation boundary there was no signature indicative of the transition of mixing scheme observed in other aqueous alcohols. Thus, in aqueous butan-1-ol phase separation occurs directly from mixing scheme I, without going through mixing scheme II, which we argued earlier to be a preparation stage for phase separation for the other alcohols.},
	keywords = {2-BUTOXYETHANOL, fluctuations, ISOTHERMAL COMPRESSIBILITIES, MIXTURES},
	isbn = {1463-9076},
	url = {<Go to ISI>://000085442300008},
	author = {Tamura, K. and Hu, J. H. and Trandum, C. and Westh, P. and Haynes, C. A. and Koga,Yoshikata}
}
@article {4889,
	title = {A thermodynamic study of aqueous acetonitrile: excess chemical potentials, partial molar enthalpies, entropies and volumes, and fluctuations},
	journal = {Canadian Journal of Chemistry-Revue Canadienne De Chimie},
	volume = {78},
	number = {12},
	year = {2000},
	note = {ISI Document Delivery No.: 385LGTimes Cited: 9Cited Reference Count: 24},
	month = {Dec},
	pages = {1553-1560},
	type = {Article},
	abstract = {We measured vapour pressures of aqueous acetonitrile (abbreviated as ACN) at 6, 20, and 37 degreesC, from which excess chemical potentials of ACN (mu (E)(ACN)) were calculated. We also determined excess partial molar enthalpies of ACN (H-ACN(E)) at 6, 20, 30, 37, and 45 degreesC. From these data, excess partial molar entropies of ACN (S-ACN(E)) were calculated at 6, 20, and 37 degreesC. Using density data by Benson{\textquoteright}s group, excess partial molar volumes of ACN (V-ACN(E)) were evaluated. The response function data by the same group were also used to evaluate amplitude and wavelength of mean-square fluctuations in terms of volume, entropy, and cross between volume and entropy. All the above quantities and their dependence on the mol fraction of solute, i.e., the effect of additional solute on the above quantities were used to study the effect of acetonitrile on the molecular organization of H2O. It was found that acetonitrile works as a stronger structure-making solute than methanol. Rather its effect on H2O is about the same as that of propan-1-ol.},
	keywords = {2-BUTOXYETHANOL, 25-DEGREES-C, aqueous acetonitrile, BUTYL ALCOHOL, fluctuations, FREE-ENERGIES, interaction functions, MIXING SCHEMES, MIXTURES, NON-ELECTROLYTES, TERT-BUTANOL, VAPOR-PRESSURES, WATER-RICH REGION},
	isbn = {0008-4042},
	url = {<Go to ISI>://000166005500003},
	author = {Nikolova, P. V. and Duff, S. J. B. and Westh, P. and Haynes, C. A. and Kasahara, Y. and Nishikawa, K. 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 {4613,
	title = {Excess partial molar enthalpy of 1-propanol in 1-propanol-NaCl-H2O at 25 degrees C: The effect of NaCl on molecular organization of H2O},
	journal = {Journal of Physical Chemistry B},
	volume = {103},
	number = {15},
	year = {1999},
	note = {ISI Document Delivery No.: 189YNTimes Cited: 23Cited Reference Count: 26},
	month = {Apr},
	pages = {2981-2983},
	type = {Article},
	abstract = {Excess partial molar enthalpies of l-propanol, H-1p(E), in 1-propanol-NaCl-H2O were measured directly, accurately, and in small increments in mole fraction of 1-propanol, x(1P), at 25 degrees C in the range x(NaCl) < 0.04 x(NaCl) is the mole fraction of NaCl. The enthalpic interaction function, H-1P-1P(E), between l-propanol molecules was then evaluated. H-1P-1P(E) is a convenient, model-free measure for the intermolecular interaction in terms of enthalpy. The behavior of these thermodynamic quantities was compared with that of the binary 1-propanol-H2O. Based on the knowledge accumulated in our laboratory on the binary aqueous l-propanol, the effect of NaCl on H2O became apparent. Our tentative conclusions are that (1) a NaCl molecule "binds" to seven or eight molecules of H2O on dissolving into H2O, and (2) the reminder of bulk H2O away from solute NaCl is not affected and stays almost the same as pure H2O.},
	keywords = {2-BUTOXYETHANOL, AQUEOUS SODIUM-CHLORIDE, CLUSTERS, EQUILIBRIUM, fluctuations, INTERMOLECULAR INTERACTIONS, LYSOZYME, SPECTROSCOPY, vibrational, VOLUMES, WATER},
	isbn = {1089-5647},
	url = {<Go to ISI>://000079934100023},
	author = {Matsuo, H. and To, E. C. H. and Wong, D. C. Y. and Sawamura, S. and Taniguchi, Y. and Koga,Yoshikata}
}
@article {4420,
	title = {Interactions in 1-propanol-urea-H2O: Chemical potentials, partial molar enthalpies, and entropies at 25 degrees C},
	journal = {Journal of Physical Chemistry B},
	volume = {102},
	number = {52},
	year = {1998},
	note = {ISI Document Delivery No.: 153MQTimes Cited: 27Cited Reference Count: 31},
	month = {Dec},
	pages = {10958-10965},
	type = {Article},
	abstract = {The excess partial molar enthalpies of I-propanol were determined in aqueous urea solutions. The total vapor pressures of 1-propanol-urea-H2O were also measured. The numerical analysis applied in a previous paper (J. Phys. Chem. B 1998, 102, 5182) was used to calculate partial pressures and, hence, the excess chemical potentials of each component. Thus, the excess partial molar entropies of l-propanol were obtained. From these partial molar quantities, the interaction functions between a pair of solute molecules were calculated following the method developed by us ( J. Phys. Chern. B 1996, 100, 5172). All these data seem to indicate that urea molecules lock into the hydrogen bond network of H2O, keep the connectivity of hydrogen bond intact, but reduce the degree of fluctuation that is characteristic of liquid water. I-Propanol molecules modify the hydrogen bond network in the same manner with or without urea, and hence the same amount of 1-propanol is required to break down the connectivity, i.e., the loss of hydrogen bond percolation. However, the H2O-mediated interaction between l-propanol solutes is weakened since the hydrogen bond fluctuation responsible for such an interaction is reduced by the presence of urea.},
	keywords = {AQUEOUS-SOLUTIONS, fluctuations, INTERMOLECULAR INTERACTIONS, KIRKWOOD-BUFF PARAMETERS, MIXING SCHEMES, MIXTURES, TERT-BUTYL ALCOHOL, UREA, WATER-RICH REGION, X-RAY-SCATTERING},
	isbn = {1089-5647},
	url = {<Go to ISI>://000077837200040},
	author = {To, E. C. H. and Hu, J. H. and Haynes, C. A. and Koga,Yoshikata}
}
@article {4106,
	title = {Nematic-isotropic phase coexistence in a Lebwohl-Lasher model binary liquid crystal mixture},
	journal = {Chemical Physics Letters},
	volume = {281},
	number = {1-3},
	year = {1997},
	note = {ISI Document Delivery No.: YP239Times Cited: 12Cited Reference Count: 31},
	month = {Dec},
	pages = {207-211},
	type = {Article},
	abstract = {Monte Carlo computer simulations were used to investigate the phase behaviour of a Lebwohl-Lasher binary liquid-crystal mixture. A finite-size scaling analysis confirmed the first-order nature of the transition. The calculated nematic-isotopic phase coexistence region and the orientational order parameters for the two species along the phase boundary for a sample system were found to deviate significantly from those predicted by a mean-field theory. Increasing the difference between the isotropic components of the pair-potential of the two species resulted in a broadening of the coexistence region. (C) 1997 Elsevier Science B.V.},
	keywords = {1ST-ORDER MELTING TRANSITION, ANISOTROPIC SYSTEMS, BEHAVIOR, COMPUTER-SIMULATION, fluctuations, LATTICE, LIPID BILAYERS, MONTE-CARLO, POTTS-MODEL},
	isbn = {0009-2614},
	url = {<Go to ISI>://000071256600031},
	author = {Polson, J. M. and Burnell, E. E.}
}
@article {3846,
	title = {Characteristics of an inductively coupled argon plasma operating with organic aerosols .4. Noise power spectra},
	journal = {Journal of Analytical Atomic Spectrometry},
	volume = {11},
	number = {11},
	year = {1996},
	note = {ISI Document Delivery No.: VT965Times Cited: 3Cited Reference Count: 31},
	month = {Nov},
	pages = {1011-1018},
	type = {Article},
	abstract = {With the use of noise power spectra it is shown that the vortex shedding frequency depends on the solvent and the solvent plasma load, and modulates both the plasma boundary and analyte plume of the discharge.},
	keywords = {ATOMIC EMISSION-SPECTROMETRY, DROPLETS, FLOW TORCH, fluctuations, INDUCTIVELY COUPLED ARGON PLASMA, jet, LOAD, MASS-SPECTROMETER, noise power spectra, ORGANIC SOLVENT, SOLVENT, SOLVENT PLASMA LOAD},
	isbn = {0267-9477},
	url = {<Go to ISI>://A1996VT96500002},
	author = {Weir, D. G. and Blades, M. W.}
}
@article {3196,
	title = {CHARACTERISTICS OF AN INDUCTIVELY-COUPLED ARGON PLASMA OPERATING WITH ORGANIC AEROSOLS .1. SPECTRAL AND SPATIAL OBSERVATIONS},
	journal = {Journal of Analytical Atomic Spectrometry},
	volume = {9},
	number = {12},
	year = {1994},
	note = {ISI Document Delivery No.: PY149Times Cited: 33Cited Reference Count: 27},
	month = {Dec},
	pages = {1311-1322},
	type = {Article},
	abstract = {The effect of solvent and solvent load on the background spectra and visual features obtained from an inductively coupled argon plasma have been recorded. An experimental system for making these measurements is described. The solvents studied were water, methanol and chloroform, at solvent loads corresponding to the maximum and minimum obtainable. The most conspicuous features observed were emission atomic carbon, diatomic carbon and cyanide. A thermal pinch created by the introduction of organic solvents and a recirculation eddy at the base of the torch have been characterized.},
	keywords = {ATOMIC EMISSION-SPECTROMETRY, DROPLETS, DYNAMICS, fluctuations, GAS-FLOW, INDUCTIVELY COUPLED ARGON PLASMA, LOAD, ORGANIC SOLVENT, SAMPLE INTRODUCTION, SOLVENT PLASMA LOAD, THERMAL PINCH},
	isbn = {0267-9477},
	url = {<Go to ISI>://A1994PY14900002},
	author = {Weir, D. G. and Blades, M. W.}
}
@article {3007,
	title = {EXCESS PARTIAL MOLAR VOLUMES AND THERMAL EXPANSIVITIES IN THE WATER-RICH REGION OF AQUEOUS 2-BUTANONE},
	journal = {Journal of Solution Chemistry},
	volume = {23},
	number = {2},
	year = {1994},
	note = {ISI Document Delivery No.: NB508Times Cited: 8Cited Reference Count: 22Symposium in Honor of Donald Patterson on His 65th Birthday, at the 76th Congress of the Canadian-Society-for-ChemistryMAY 31-JUN 03, 1993SHERBROOKE, CANADACANADIAN SOC CHEM},
	month = {Feb},
	pages = {339-349},
	type = {Proceedings Paper},
	abstract = {Excess partial molar volumes of 2-butanone V(m)E(B) and thermal expansivities alpha(p) were measured in the water-rich region of aqueous 2-butanone. The composition derivatives of both quantities showed anomalies at about X(B) = 0.033 (x(B) is the mole fraction of B). (partial derivative V(m)E(B)/partial derivative n(B))p,T,nW showed a step anomaly, while (partial derivative alpha(p)/partial derivatives n(B))p,T,nw exhibited a peak anomaly. The compositions at which these anomalies occurred match those of the step anomalies observed earlier in (partial derivative H(m)E(B)/partial derivative n(B))p,T,nW and (partial derivative S(m)E(B)/partial derivative n(B))p,T,nW in aqueous 2-butanone. These results are discussed in comparison with those obtained previously for aqueous 2-butoxyethanol.},
	keywords = {2-BUTANONE, 2-BUTOXYETHANOL, 25-DEGREES-C, ANOMALIES IN 3RD DERIVATIVES, AQUEOUS, DERIVATIVES, ENTHALPIES, EXCESS PARTIAL MOLAR VOLUMES, fluctuations, FREE-ENERGIES, HEAT-CAPACITIES, MIXING SCHEME, OF GIBBS FREE ENERGY, TERT-BUTANOL MIXTURES, THERMAL EXPANSIVITIES, TRANSITION, TRANSITION OF MIXING SCHEME},
	isbn = {0095-9782},
	url = {<Go to ISI>://A1994NB50800016},
	author = {Davies, J. V. and Fooks, R. and Koga,Yoshikata}
}
