Isotope effects in aqueous systems. 13. The hydrophobic interaction. Some thermodynamic properties of benzene/water and toluene/water solutions and their isotope effects

Partial molar volumes of organic solutes in water. X. Benzene and toluene at temperatures from (298 to 573) K and at pressures up to 30 MPa

“…Here the deviations are larger than those for benzene but the agreement is within the estimated uncertainties. [17]; s, Sakurai [18]; M, Masterton [19]; Â, Shahidi [20]; Ã, Makhatadze [21]; }, Dutta-Choudhury [22]. The values at 298.15 K selected by Cabani et al [23] and Lepori and Gianni [24] are identical with our data.…”

“…The data set used for a comparison include the experimental data [18][19][20][21][22]25] as well as the data selected by some authors [17,23,24]. Since the dependence of partial molar volume on pressure at lower temperatures is moderate (see the discussion below) our data at 0.49 MPa and 0.47 MPa can be compared with data at 0.1 MPa taken from the literature.…”

“…The values at 298.15 K selected by Cabani et al [23] and Lepori and Gianni [24] are identical with our data. [17]: s, Sakurai [18]; M, Lepori [24]; Â, Shahidi [20]; Ã, Makhatadze [21]; }, Dutta-Choudhury [22]. Sawamura et al [15] reported the V 0 m;2 ðT ; pÞ surface for toluene evaluated from pressure dependence of solubility in the range from about 273 K up to 320 K. According to SawamuraÕs data the derivative ðoV 0 m;2 =opÞ T at low pressures is positive in the range from T % 273 K to T % 300 K with ðoV 0 m;2 =opÞ T ¼ 0 (maximum of V 0 m;2 ) at higher pressures (about 50 MPa) and the V 0 m;2 ðpÞ dependence has a concave FIGURE 6.…”

Infinite dilution activity coefficients for benzene and toluene in water and in aqueous solutions of the protein denaturants urea and guanidine hydrochloride

“…For both benzene and toluene, starting from the freezing temperature of water, the limiting activity coefficient rises with increasing temperature, passes through a rather flat maximum at a temperature slightly below room temperature, and then continuously decreases with increasing temperature. For each of the two solutes, we fitted this temperature dependence to the following equation originating from the assumption of temperature independent heat capacity of solution: (27) , Bittrich et al; (28) •, Dutta et al; (29) · , Sanemasa et al; (30) , Sanemasa et al; (31) ·, Brown and Wasik; (32) , Bradley et al; (33) ♦ · , Pierotti and Labastre; (34) ♦, Bohon and Claussen; (26) ×, Anderson and Prausnitz. (35) The error bars correspond to the standard errors.…”

Comments on H/D Isotope Effects on Polarizabilities of Small Molecules. Correlation with Virial Coefficient, Molar Volume, and Electronic Second Moment Isotope Effects

“…The Sutherland po tential is crude, but in first approxim ation it suffices to estimate virial coefficient isotope effects using the dif ference formalism. With Aa/a calculated as in the sec tion above, and with Aa/a estimated from mean square amplitudes for the gas phase molecules follow ing Bartell and Roskos [32], or for more massive molecules from AV/V [6,29,30,[32][33][34][35][36][37] not too far from the triple point, the VCIE's reported in Table 7 were calculated. The table compares calculated and experimental VCIE's for those four hydro/deuterocarbons [4,5] where comparison with experiment is pos sible, and gives a calculated VCIE for one other com pound.…”