Measurements and Correlations of the Solid–Liquid Equilibrium of RbCl/CsCl + [Cnmim]Cl (n = 2, 4, 6, 8) + H2O Ternary Systems at T = (288.15, 298.15, and 308.15) K

Tang, Jing; Li, Shu-Ni; Zhai, Quan‐Guo; Jiang, Yucheng

doi:10.1021/je4007986

Cited by 21 publications

(9 citation statements)

References 33 publications

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“…The comparison of the solubilities, densities, and refractive indices of the four salts NaCl/KCl/RbCl/CsCl in pure water are in good agreement with the literature values ,,,− (Tables S1–S3 and Figures S1–S3). The experimental values of solubility, density, and refractive index of all the saturated solutions of the NMP + NaCl/KCl/RbCl/CsCl + H 2 O ternary system are listed in Table and graphically shown in Figures – .…”

Section: Results and Discussionsupporting

confidence: 88%

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K

Qiu

Cao

et al. 2021

J. Chem. Eng. Data

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In this paper, the solid–liquid equilibrium of N-methylpyrrolidone (NMP) + MCl (M = Na, K, Rb, and Cs) + H2O ternary systems was investigated at three temperatures (T = 288.2, 298.2, and 308.2 K). The isothermal solubility, density, and refractive index of the saturated ternary systems were obtained. At the same temperature, as the NMP content in the mixed solvent increases, the solubility of the salt decreases significantly, and the density change trend is consistent with the solubility. However, as the NMP content in the mixed solvent increases, the refractive index increases. As the experimental temperature increases, the solubility and density increase, while the refractive index decreases. Moreover, the semi-empirical four-parameter equation was used to fit the experimental data.

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Section: Results and Discussionsupporting

confidence: 88%

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K

Qiu

Cao

et al. 2021

J. Chem. Eng. Data

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“…It was also noted that the refractive index increased with increasing mass fraction of 1-ethyl-3methylimidazolium chloride. Similar behavior was observed by Tang et al (2014), who observed that the index of refraction increased with the mass fraction of the ionic liquid. It can be seen that the electrical conductivity increased with increasing mass fraction of 1-ethyl-3methylimidazolium chloride due to the increase in the amount of ions present in the aqueous solution (Xu et al, 2015).…”

Section: Density Refractive Index and Electrical Conductivity Of Thesupporting

confidence: 86%

Thermophysical Properties of 1-Ethyl-3-Methylimidazolium Chloride Solution From 293.15 to 323.15 K

Gandolfi

Gonçalves

Pimentel

et al. 2019

Braz. J. Chem. Eng.

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Aqueous systems composed of ionic liquid make up a new alternative for use in processes involving the separation of biomolecules. The objective of this experiment was to obtain the thermo-physical properties of density, refractive index, electrical conductivity, molar volume, thermal expansion coefficient and apparent specific volume of the ionic liquid 1-ethyl-3-methylimidazolium chloride. The thermo-physical properties of aqueous solutions of this ionic liquid were measured as a function of the mass fraction w = (0.05, 0.125, 0.2, 0.275 and 0.35), temperature T = (293.15, 303.15, 313.15 and 323.15) K and pH = (7.5, 8.0 and 8.5). Models representing the combined effects between variables were fit since they are required for industrial applications where the physical parameters must be accurately calculated. Models representing the combined effects of the variables temperature, mass fraction and pH values of ionic liquid were adjusted and presented good fit.

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“…The measured values of density for binary ([Emim][Cl] + H 2 O) system and ternary ([Emim][Cl] + LiCl + H 2 O), ([Emim][Cl] + LiBr + H 2 O), and ([Emim][Cl] + LiNO 3 + H 2 O) mixtures at different concentrations of [Emim][Cl] and (LiCl, LiBr and LiNO 3 ), and at different temperatures are given in Suppporting Information Tables S1 to S4. Figure shows the comparison of measured densities for ([Emim][Cl] + H 2 O) binary system in this work and literature at T = 298.15 K. Both data show linear dependence to molality of ionic liquid with same intercepts but different slopes. This discrepancy in slopes may come from differences in purities of used ionic liquid and also little differences in densities due to pressure.…”

Section: Resultsmentioning

confidence: 59%

“…S1 to S4. Figure 1 shows the comparison of measured densities for ([Emim][Cl] + H 2 O) binary system in this work and literature 14 at T = 298.15 K. Both data show linear dependence to molality of ionic liquid with same intercepts but different slopes. This discrepancy in slopes may come from differences in purities of used ionic liquid and also little differences in densities due to pressure.…”

Section: Methodsmentioning

confidence: 64%

Study of Apparent Molar Volumes for Ionic Liquid, 1-Ethyl-3-methyl Imidazolium Chloride in Aqueous Lithium Nitrate, Lithium Bromide, and Lithium Chloride Solutions at Temperatures (298.15 to 318.15) K

Rafiee

Frouzesh

2015

J. Chem. Eng. Data

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The densities of ternary systems ([Emim][Cl]+ LiCl + H 2 O), ([Emim][Cl] + LiBr + H 2 O), and ([Emim][Cl]+ LiNO 3 + H 2 O) and also binary system ([Emim][Cl] + H 2 O) were measured at T = (298.15 to 318.15) K using a vibrating U-tube densimeter. On the basis of experimental density data, the apparent molar volumes, V φ , were computed. The values of apparent molar volumes for binary system were correlated to Redlich−Meyer and Pitzer equations and for ternary systems were correlated to Redlich−Meyer equation and apparent molar volumes at infinite dilution, V φ 0 , are also calculated. Our results showed a negative transfer volume of [EmimCl] from water to the aqueous LiCl, LiBr, and LiNO 3 solutions, which decrease by enhancing the salt mass fraction. The solute−solvent interactions and structure making or breaking ability of [Emim][Cl] have been discussed in details. The results of second derivative of limiting apparent molar volumes showed that the studied ionic liquid in this work acts as a structure maker.

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Measurements and Correlations of the Solid–Liquid Equilibrium of RbCl/CsCl + [C_nmim]Cl (n = 2, 4, 6, 8) + H₂O Ternary Systems at T = (288.15, 298.15, and 308.15) K

Cited by 21 publications

References 33 publications

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K

Thermophysical Properties of 1-Ethyl-3-Methylimidazolium Chloride Solution From 293.15 to 323.15 K

Study of Apparent Molar Volumes for Ionic Liquid, 1-Ethyl-3-methyl Imidazolium Chloride in Aqueous Lithium Nitrate, Lithium Bromide, and Lithium Chloride Solutions at Temperatures (298.15 to 318.15) K

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Measurements and Correlations of the Solid–Liquid Equilibrium of RbCl/CsCl + [Cnmim]Cl (n = 2, 4, 6, 8) + H2O Ternary Systems at T = (288.15, 298.15, and 308.15) K

Cited by 21 publications

References 33 publications

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H2O Systems at 288.2, 298.2, and 308.2 K

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H2O Systems at 288.2, 298.2, and 308.2 K

Thermophysical Properties of 1-Ethyl-3-Methylimidazolium Chloride Solution From 293.15 to 323.15 K

Study of Apparent Molar Volumes for Ionic Liquid, 1-Ethyl-3-methyl Imidazolium Chloride in Aqueous Lithium Nitrate, Lithium Bromide, and Lithium Chloride Solutions at Temperatures (298.15 to 318.15) K

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Measurements and Correlations of the Solid–Liquid Equilibrium of RbCl/CsCl + [C_nmim]Cl (n = 2, 4, 6, 8) + H₂O Ternary Systems at T = (288.15, 298.15, and 308.15) K

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K

Phase Behavior of N-Methylpyrrolidone + MCl (M = Na, K, Rb, Cs) + H₂O Systems at 288.2, 298.2, and 308.2 K