Partial molar volumes, isentropic compressibilities, and partial molar expansibilities of N-Methylglycine and d-Glucose in aqueous environments at temperatures between (298.15 and 323.15) K

Gheorghe, Ioana L.; Stoicescu, C.; Sîrbu, Florinela

doi:10.1016/j.molliq.2016.02.033

Cited by 45 publications

(7 citation statements)

References 50 publications

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“…The increase of V̅ i ∞ with temperature is an effect of decrease in volume of the solute solvation sphere due to intensification of the heat motion. The limiting partial molar volume of the solute can be expressed as a sum of two contributions: − where V m,(int) is the intrinsic molar volume of the solvent which does not change under solvation and is almost constant within the temperature range studied; V m,(s–s) is the varying volume of the solvation sphere when one mole of the solute interacts with the solvent, this value characterizes the solute solvation; V b is the molar volume of pure solvent; N is the solvation number, i.e., the number of solute molecules within the solute solvation sphere, where the solvent molar volume V h has another numerical value. Therefore, the increase of the limiting partial molar volumes of water and formamide, V̅ i ∞ , with temperature growth can be caused only by the V m,(s–s) decrease, which is connected with ability of these two solutes to interact with H-bond network of the solvent.…”

Section: Discussionmentioning

confidence: 99%

Densities and Molar Isobaric Thermal Expansions of the Water + Formamide Mixture over the Temperature Range from 274.15 to 333.15 K at Atmospheric Pressure

Egorov

Makarov

2017

J. Chem. Eng. Data

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The density of the {water (1) + formamide (2)} mixture has been measured over the whole composition range at temperatures from 274.15 to 333.15 K at atmospheric pressure using the vibration densimeter. The volumetric parameters of the mixture, such as the excess molar volume, molar isobaric thermal expansions, and apparent and partial molar volumes of water and formamide, as well as their limiting values, have been calculated. It was shown that the mixture formation resulted in the volume decrease at all temperatures, and the largest absolute value of the excess molar volume corresponded to the mixture composition of 2H 2 O-FA. The limiting partial molar volumes of water and formamide increased with the temperature rise. At a temperature of about 323 K the limiting partial molar volume of water became larger than its own molar volume.

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Section: Discussionmentioning

confidence: 99%

Densities and Molar Isobaric Thermal Expansions of the Water + Formamide Mixture over the Temperature Range from 274.15 to 333.15 K at Atmospheric Pressure

Egorov

Makarov

2017

J. Chem. Eng. Data

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“…From Table S2 in the Supporting Information, it could be seen that apparent molar volume increases with the increasing of the molality of the ILs; also, it increases with increase of the temperature. As stated by Gheorghe et al (2016) and Dubey et al (2019), these values could suggest the presence of strong intermolecular forces between ILs and alcohol molecules. 32,33 Finally, apparent molar isentropic compressibility (κ ø ) is expressed by using eq 7…”

Section: T H I S C O N T E N T Imentioning

confidence: 61%

“…As stated by Gheorghe et al (2016) and Dubey et al (2019), these values could suggest the presence of strong intermolecular forces between ILs and alcohol molecules. 32,33 Finally, apparent molar isentropic compressibility (κ ø ) is expressed by using eq 7…”

Section: T H I S C O N T E N T Imentioning

confidence: 61%

Liquid Densities and Speed of Sound for Ionic Liquid (2-HEAA and 2-HDEAA) + Alcohol (1-Propanol and 2-Propanol) Mixtures at T = (293.15–323.15 K) and Atmospheric Pressure

et al. 2019

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Liquid–liquid equilibrium data are widely used in many industrial sectors. For this reason, it is important to know thermodynamics binary mixture data to better understand molecular interactions between components. This work reports experimental density (ρ) and speed of sound (υ) data for 2-hydroxyethanolamine acetate + 1-propanol, 2-hydroxyethanolamine acetate + 2-propanol, 2-hydroxydiethanolamine acetate + 1-propanol, and 2-hydroxydiethanolamine acetate + 2-propanol binary mixtures, over a wide composition range, between 293.15 and 323.15 K, and at atmospheric pressure (101.3 kPa). For this purpose, a vibrating tube densitometer was used to perform density and speed of sound experimental measurements. From these data, important derivative properties have been calculated, such as isentropic compressibility (κs), apparent molar isentropic compressibility (κø), excess molar volumes (V m E), and apparent molar volume (V Ø).

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“…For this to be the case, the behaviors of glucose and other carbohydrate osmolytes in solution would have to be similar to the same special case as anhydrous salts, such as MgSO 4 , in which | V̅ solvated – V̅ solid | < V̅ solid , that is, they have a negative volume in aqueous solution. A negative partial molar volume effect that caused contraction of the polar phase could account for smaller sized w 0 equivalent RMs and constant sized loaded RMs; however, this is inconsistent with the behavior of glucose both in pure water − and aqueous solutions. ,− This would require the negative excess partial molar volume of glucose to change from −5 to −105%, purely through the change in environment from bulk to confined aqueous solution. Thus, excess partial molar volume cannot account for the sizes we observe.…”

Section: Resultsmentioning

confidence: 99%

Sweet Confinement: Glucose and Carbohydrate Osmolytes in Reverse Micelles

et al. 2018

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The research presented here reports the surprising observation that adding glucose and other carbohydrate osmolytes to the polar phase of water-containing reverse micelles causes the particles to shrink. This apparent change in reverse micelle size is attributed to two factors: an increase in the surface area per surfactant molecule induced by the presence of carbohydrate and changes in the particle shape eccentricity. The studies reported here not only focus on glucose but also explore other carbohydrate osmolytes, specifically ethylene glycol, glycerol, erythritol, xylitol, sorbitol, myo-inositol, and trehalose, in the nanoconfined environments of reverse micelles. Through two-dimensional proton nuclear Overhauser enhancement nuclear magnetic resonance spectroscopy, the osmolytes were determined to reside solvated in the aqueous interior of the reverse micelles. This paper reports the loading limit of carbohydrates into AOT [sodium bis(2-ethylhexyl)sulfosuccinate] reverse micelles, demonstrates the location of the carbohydrates in the reverse micelles, and shows an unexpected effect where the carbohydrates add to the reverse micelle volume without causing an apparent increase in the reverse micelle diameter.

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Partial molar volumes, isentropic compressibilities, and partial molar expansibilities of N-Methylglycine and d-Glucose in aqueous environments at temperatures between (298.15 and 323.15) K

Cited by 45 publications

References 50 publications

Densities and Molar Isobaric Thermal Expansions of the Water + Formamide Mixture over the Temperature Range from 274.15 to 333.15 K at Atmospheric Pressure

Densities and Molar Isobaric Thermal Expansions of the Water + Formamide Mixture over the Temperature Range from 274.15 to 333.15 K at Atmospheric Pressure

Liquid Densities and Speed of Sound for Ionic Liquid (2-HEAA and 2-HDEAA) + Alcohol (1-Propanol and 2-Propanol) Mixtures at T = (293.15–323.15 K) and Atmospheric Pressure

Sweet Confinement: Glucose and Carbohydrate Osmolytes in Reverse Micelles

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