Apparent Molar Volumes of Aqueous Solutions of Lithium Pentaborate from 283.15 to 363.15 K and 101.325 kPa: An Experimental and Theoretical Study

Zhao, Kaiyu; Li, Long; Guo, Yafei; Meng, Lingzong; Li, Mingli; Duo, Ji; Deng, Tianlong

doi:10.1021/acs.jced.8b00814

Cited by 11 publications

(7 citation statements)

References 13 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…The relationship between the apparent molar volume and the molality of maltitol can be correlated with the following equation. 16,17 = +…”

Section: Resultsmentioning

confidence: 99%

“…The relationship between the apparent molar volume and the molality of maltitol can be correlated with the following equation. , where m a is the molality of maltitol in solution, V φ 0 is the limiting partial molar volume, which reflects the solute–solvent interaction, and S v is the fitting parameter. The limiting partial molar volume and fitting parameter obtained by the least-square method are listed in Table .…”

Section: Resultsmentioning

confidence: 99%

See 1 more Smart Citation

Volumetric and Viscometric Properties of Maltitol in Glycylglycine Aqueous Solutions at T = 293.15–333.15 K

Shi

Zhu

et al. 2020

J. Chem. Eng. Data

View full text Add to dashboard Cite

The densities and viscosities of maltitol in glycylglycine aqueous solutions were measured at T = 293. 15, 303.15, 313.15, 323.15, and 333.15 K and at atmospheric pressure. Furthermore, the apparent molar volume (V φ ), the limiting partial molar volume (V φ 0 ), the limiting partial molar volume of transfer (Δ tr V φ 0 ), the viscosity B coefficient, and the active free energies per mole of the solvent and solute (Δμ 1 0≠ and Δμ 2 0≠ ) were obtained from the experimental densities and viscosities. Moreover, the limiting partial molar volume of transfer was analyzed based on the cosphere overlap model, and the active free energies were also discussed according to the transition-state theory. The results indicate that the ion−hydrophilic interaction between the maltitol and glycylglycine molecules occupies a dominant position in the solution, and maltitol tends to act as a structural maker in the glycylglycine aqueous solution.

show abstract

“…The relationship between the apparent molar volume and the molality of maltitol can be correlated with the following equation. 16,17 = +…”

Section: Resultsmentioning

confidence: 99%

Section: Resultsmentioning

confidence: 99%

Volumetric and Viscometric Properties of Maltitol in Glycylglycine Aqueous Solutions at T = 293.15–333.15 K

Shi

Zhu

et al. 2020

J. Chem. Eng. Data

View full text Add to dashboard Cite

show abstract

“…It can be seen that the apparent molar volumes of YCl 3 aqueous solutions increased with the increase of molality at the constant temperature. With the increasing temperature, the apparent molar volumes increase when the temperature is varied within 283.15-308.15 K, and the variation tendency is opposite when the temperature is higher than 308.15 K. It can be concluded that the ionic association of yttrium and chlorine ions is strong at low temperatures [20].…”

Section: Apparent Molar Volumesmentioning

confidence: 90%

Volumetric Properties for the Aqueous Solution of Yttrium Trichloride at Temperatures from 283.15 to 363.15 K and Ambient Pressure

Jiang

Liu³

et al. 2021

Journal of Chemistry

Self Cite

View full text Add to dashboard Cite

To effectively develop the rare earth elements resources from the geothermal waters, it is essential to understand the volumetric properties of the aqueous solution system to establish the relative thermodynamic model. In this study, densities of YCl3 (aq) at the molalities of 0.08837–1.60639 mol·kg−1 from 283.15 K to 363.15 K at 5 K intervals and ambient pressure were measured experimentally by an Anton Paar digital vibrating-tube densimeter. Based on experimental data, the volumetric properties including apparent molar volume (Vϕ) and the coefficient of thermal expansion of the solution (α) of the binary systems (YCl3 + H2O) were derived. The 3D diagram (mi, T, Vϕ) of apparent molar volumes against temperature and molality was plotted. On the basis of the Pitzer ion-interaction model of electrolyte, the Pitzer single-salt parameters ( β MX 0 v , β MX 1 v , and C MX v ) for YCl3 and temperature-dependence equation F(i, p, T) = a1 + a2ln(T/298.15) + a3(T-298.15) + a4/(620-T) + a5(T-227) as well as their coefficients ai (i = 1–5) in the binary system were obtained for the first time. The values of Pitzer single-salt parameters of YCl3 agree well with the calculated values corresponding to the temperature-dependence equations, indicating that single-salt parameters and temperature-dependent formula obtained in this work are reliable.

show abstract

“…Vibrating-tube density meters were used in most experimental investigations of the density of dilute aqueous solutions of 1-butanol and 1-pentanol reported in the published literature, and very impressive uncertainties were claimed (≤ 0.005 kg·m –3 ). However, it should also be noted that in other recent studies in which vibrating-tube density meters were used, more conservative standard uncertainty estimates have been reported (0.1 to 2.0 kg·m –3 ). ,− Pycnometers − have also been used to determine the density of dilute aqueous solutions of 1-butanol and 1-pentanol, with reported uncertainties ranging from 0.01 to 5 kg·m –3 .…”

Section: Introductionmentioning

confidence: 99%

Densities of Dilute Aqueous Solutions of 1-Butanol and 1-Pentanol at Atmospheric Pressure and Temperatures in the Range of 283.15 to 353.15 K

2021

View full text Add to dashboard Cite

Mass densities of dilute aqueous solutions of 1-butanol and 1pentanol (with alcohol concentrations between 0.07 to 0.7 and 0.006 to 0.06 mol• kg −1 , respectively) were determined at atmospheric pressure and temperatures in the range of 283.15 to 353.15 K using a custom-built volume dilatometer. The dilatometer was first calibrated using water, and it was then benchmarked using water and aqueous solutions of ethanol. Evaporation in the experiments with water and the alcohol solutions was prevented by adding a small amount of oil (about 0.2 mL) over the liquid surface that was exposed to the ambient air. The density data complement and extend those available in the published literature. They also show that at alcohol concentrations less than 0.01 mol•kg −1 , the density of such solutions may be reasonably assumed to be the same as that of water or calculated using the idealsolution assumption. For solutions with higher alcohol concentrations, however, the aforementioned assumptions are inappropriate, as they lead to density values that differ from the data presented in this paper by amounts that exceed the expanded uncertainty of the underlying measurements.

show abstract

Apparent Molar Volumes of Aqueous Solutions of Lithium Pentaborate from 283.15 to 363.15 K and 101.325 kPa: An Experimental and Theoretical Study

Cited by 11 publications

References 13 publications

Volumetric and Viscometric Properties of Maltitol in Glycylglycine Aqueous Solutions at T = 293.15–333.15 K

Volumetric and Viscometric Properties of Maltitol in Glycylglycine Aqueous Solutions at T = 293.15–333.15 K

Volumetric Properties for the Aqueous Solution of Yttrium Trichloride at Temperatures from 283.15 to 363.15 K and Ambient Pressure

Densities of Dilute Aqueous Solutions of 1-Butanol and 1-Pentanol at Atmospheric Pressure and Temperatures in the Range of 283.15 to 353.15 K

Contact Info

Product

Resources

About