Molecular interactions of alkanediols in methanol and in water: density and heat capacity measurements

Piekarski, Henryk; Pietrzak, A.

doi:10.1016/j.molliq.2004.08.025

Cited by 22 publications

(11 citation statements)

References 27 publications

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“…The method of determining these quantities on the base of the scaled particle theory (SPT) has been described in details in articles [19,20]. The values of DC p(cav) and DC p(int) calculated by us for the methanol-alkanediol and water-alkanediol mixtures have been presented and discussed in our recent article [15].…”

Section: Enthalpic Pair Interaction Coefficientsmentioning

confidence: 99%

“…Moreover, thanks to the molecular structure their interactions with other molecules are more diversified than those in which simpler molecules take part. The results of heat capacity measurements of alkanediol in methanol made it possible to determine the molar heat capacity of the interaction between alkanediol molecule and methanol, DC p(int) [15]. The comparison of the values of DC p(int) of diols in methanol with analogous data concerning aqueous systems has shown that the intermolecular solute-solvent interactions in water are stronger than those in methanol.…”

Section: Introductionmentioning

confidence: 99%

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Enthalpic interaction coefficients of NaI–alkanediol pairs in methanol and in water

Piekarski

Pietrzak

2011

J Therm Anal Calorim

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The dissolution enthalpies of NaI in the mixtures of methanol with 1,2-alkanediols (1,2-propanediol, 1,2-butanediol, 1,2-pentanediol) and with a,x-alkanediols (1,3-propanediol, 1,4-butanediol, 1,5-pentanediol), as well NaI in the mixtures of water with 1,3-propanediol and 1,2pentanediol, were determined at 298.15 K. The energetic effect of interactions between the investigated alkanediols and NaI in methanol and in water was calculated using the enthalpic pair interaction coefficients (h xy) model. These results along with the other data concerning the NaI-nonelectrolyte pairs taken from our earlier reports and from the literature were analyzed with respect to the effect of the non-electrolyte properties on the variations of the h xy values. The group contributions illustrating the interactions of NaI with selected functional groups in non-electrolyte (alkanediol and alkanol) molecules, namely: CH 2 and OH groups were calculated and discussed.

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Section: Enthalpic Pair Interaction Coefficientsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Enthalpic interaction coefficients of NaI–alkanediol pairs in methanol and in water

Piekarski

Pietrzak

2011

J Therm Anal Calorim

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“…I coh ð0Þ was determined as explained in the preceding section, the isothermal compressibility was interpolated from the values of the pure constituents, and the molar volumes and partial molar volumes were calculated from experimental density data. Densities for 1,2-pentanediol solution were as published by Piekarski & Pietrzak (2005), those for 1,5-pentanediol solutions were as published by Czechowski et al (1988) and densities of hexanediol solutions were measured by us. KBIs obtained for T = 298 K are displayed in Figs.…”

Section: Figurementioning

confidence: 99%

Small-angle neutron scattering study of aqueous solutions of pentanediol and hexanediol

et al. 2007

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Aqueous solutions of 1,2‐pentanediol, 1,5‐pentanediol, 1,2‐hexanediol and 1,6‐hexanediol have been studied by small‐angle neutron scattering over a wide range of concentrations and temperatures. The structure of the solutions on the mesoscopic length scale, corresponding to the intermolecular distances, was analysed with the help of the Kirkwood–Buff formalism. 1,2‐Hexanediol solutions exhibited a strong attractive diol–diol interaction, a weak diol–diol attraction was found for 1,6‐hexanediol and 1,2‐pentanediol, and an extremely weak diol–diol attraction was found in 1,5‐pentanediol solutions. The general tendencies are the following: aggregation is stronger as the length of the hydrophobic hydrocarbon chain increases and the 1,2‐diols exhibit much stronger attraction then the 1,‐diols. The temperature dependence of the aggregation is weak for the 1,2‐diols but strong for the 1,‐diols, indicating in the latter case the hydrophobic character of the interaction.

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“…Alkanediols and amides are used in a wide variety of end-use practical and theoretical applications [1][2][3][4][5][6][7][8][9][10][11][12][13][14][15]. In recent papers, we have reported thermophysical and spectroscopic studies for the mixtures of alkanediols (isomeric butanediols and a,x-alkanediols) with amides (N,Ndimethylformamide and pyrrolidin-2-one) [16][17][18].…”

Section: Introductionmentioning

confidence: 99%

Molecular interactions of α,ω-alkanediols in pyrrolidin-2-one: Thermophysical and spectroscopic measurements

Mehta

Ram

Bhasin

2008

The Journal of Chemical Thermodynamics

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Molecular interactions of alkanediols in methanol and in water: density and heat capacity measurements

Cited by 22 publications

References 27 publications

Enthalpic interaction coefficients of NaI–alkanediol pairs in methanol and in water

Enthalpic interaction coefficients of NaI–alkanediol pairs in methanol and in water

Small-angle neutron scattering study of aqueous solutions of pentanediol and hexanediol

Molecular interactions of α,ω-alkanediols in pyrrolidin-2-one: Thermophysical and spectroscopic measurements

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