Studies on molecular interactions of oxalic acid and its salts in co-aqueous solutions of 1,3-dioxolane by volumetric and viscometric measurements at T=(298.15, 308.15, and 318.15) K

Roy, Mahendra Nath; Bhattacharjee, Arijit; Das, Rajesh Kumar

doi:10.1016/j.molliq.2010.07.003

Cited by 2 publications

(11 citation statements)

References 21 publications

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“…It was interesting to analyze experimental viscosity data on the basis of transition state theory of relative viscosity, using the following expression: where B is the viscosity coefficient obtained from eq , Δμ 2 o≠ is the ionic activation energy at infinite dilution, and V 1 o is the partial molar volumes of the solvent at infinite dilution calculated from our previous work . Experimental density values used for this calculation at 298.15 K and from our previous work are presented in Table .…”

Section: Resultsmentioning

confidence: 99%

“…It can be seen that Δμ 1 o≠ is practically constant at all compositions and temperatures, implying that Δμ 2 o≠ depends mainly on the viscosity coefficient B and the V 2 o – V 1 o term in eq . According to Feakins et al, if Δμ 2 o≠ > Δμ 1 o≠ the coefficient B will be positive for electrolyte solutions. This indicates stronger ion–solvent interactions and suggests a weakening of the intermolecular forces in the solvent structure.…”

Section: Resultsmentioning

confidence: 99%

“…1,2 Earlier, viscosity was mainly investigated in diluted solutions in the range of validity of the Debye−Huckel law 3 providing valuable information in diluted solutions regarding ion−dipole interactions. 4,5 Since concentrated solutions are widely used in many industrial areas, further studies of the viscosity in the wide electrolyte concentration range in different solvents is justified.…”

Section: Introductionmentioning

confidence: 99%

“…It was interesting to analyze experimental viscosity data on the basis of transition state theory of relative viscosity, 5 using the following expression:…”

Section: Introductionmentioning

confidence: 99%

“…One of the key transport properties of the electrolyte solution for many applications in new technological processes is viscosity. Thus, knowledge of an accurate viscosity together with the influences of temperature, pressure, and composition is of a great importance for the engineering community. , Earlier, viscosity was mainly investigated in diluted solutions in the range of validity of the Debye–Hückel law providing valuable information in diluted solutions regarding ion–dipole interactions. , Since concentrated solutions are widely used in many industrial areas, further studies of the viscosity in the wide electrolyte concentration range in different solvents is justified.…”

Section: Introductionmentioning

confidence: 99%

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Viscosity of Ammonium Nitrate + Formamide Mixtures

2014

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In this work the viscosity of NH 4 NO 3 + formamide solutions in a wide concentration range up to 0.3703 ammonium nitrate mole and in the temperature range from (298.15 to 348.15) K was determined. The validity of Jones−Dole and Goldsack−Franchetto's equations were checked and applied to describe the viscosity dependence on concentration. The equation for the viscosity dependence on both the ammonium nitrate mole fraction and temperature is also presented in this paper.

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Section: Resultsmentioning

confidence: 99%

Section: Resultsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

“…It was interesting to analyze experimental viscosity data on the basis of transition state theory of relative viscosity, 5 using the following expression:…”

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 3 more Smart Citations

Viscosity of Ammonium Nitrate + Formamide Mixtures

2014

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Densities and Volumetric Properties of Water + 1,3-Dioxolane Mixtures at Temperatures of (274.15 to 323.15) K and Ambient Pressure

Egorov

2023

J. Chem. Eng. Data

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The densities of the binary mixture {water (1) + 1,3-dioxolane (2)} were measured using a vibration density meter over the entire range of compositions in the temperature range from (274.15 to 333.15) K at atmospheric pressure. The excess molar volumes, molar isobaric temperature expansions of the mixture, and apparent and partial molar volumes of water and 1,3-dioxolane, including their limiting values, were calculated. The obtained results were compared with the literature data and with those having similar properties of aqueous mixtures of other simple cyclic ethers: oxolane and 1,4-dioxane. The formation of the water + 1,3-dioxolane mixture was shown to be accompanied by a volume decrease at all temperatures. The addition of ether to water led to a negative shift in the temperature corresponding to the maximum mixture density. The concentration dependencies of the partial molar volumes of 1,3-dioxolane were characterized by the absence of a minimum at low concentrations of cyclic ether in the mixture. The limiting partial molar volumes of water and 1,3-dioxolane were smaller than the respective molar volumes and increased as the temperature increased. The temperature coefficient of the limiting molar isobaric expansion of water in 1,3-dioxolane was positive, which indicated that the temperature increase made the solvate shell larger. The negative temperature coefficient of the limiting molar isobaric expansion of 1,3-dioxolane indicates the destruction of the water structure in the immediate environment of the cyclic ether molecule.

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Studies on molecular interactions of oxalic acid and its salts in co-aqueous solutions of 1,3-dioxolane by volumetric and viscometric measurements at T=(298.15, 308.15, and 318.15) K

Cited by 2 publications

References 21 publications

Viscosity of Ammonium Nitrate + Formamide Mixtures

Viscosity of Ammonium Nitrate + Formamide Mixtures

Densities and Volumetric Properties of Water + 1,3-Dioxolane Mixtures at Temperatures of (274.15 to 323.15) K and Ambient Pressure

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