Reverse Schreinemakers Method for Experimental Analysis of Mixed-Solvent Electrolyte Systems

The solubility of disodium terephthalate in aqueous sodium hydroxide and in aqueous sodium hydroxide–ethylene glycol mixtures was determined experimentally by temperature analysis, gravimetry and titration. The experimental results were compared with existing literature data and the phase diagrams were determined from −25 to 70 °C. The solubility of disodium terephthalate has no considerable dependence on temperature. The freezing points of disodium terephthalate solutions vary with composition like any other solution. The solubility and freezing points decrease with increasing concentrations of ethylene glycol. Disodium terephthalate is salted out by the addition of sodium hydroxide.

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“…The interpretation of the experiments is very similar to previous work by Fosbøl et al 30 2.4. Uncertainty and Deviation.…”

Section: Gravimetric Experimentssupporting

confidence: 90%

Solubility and Freezing Points of Disodium Terephthalate in Water–Ethylene Glycol Mixtures

et al. 2021

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“…σ is the standard deviation. The results of the RS method was calculated from equations of Fosbøl et al 4,14 . wi is the weight percent of component i.…”

Section: Resultsmentioning

confidence: 99%

Solubility of NaHCO₃ in Systems of Aqueous Glycols (Monoethylene Glycol, Diethylene Glycol, Triethylene Glycol, and Tetraethylene Glycol): The Role of Solvation

et al. 2020

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The solubility and density of NaHCO3 in the systems: monoethylene glycol (MEG)-water, diethylene glycol (DEG)-water, triethylene glycol (TEG)-water, and tetraethylene glycol (TeEG)water have been measured over the entire concentration range from pure water to pure glycol.Experimental measurements have been conducted at the temperatures 5, 20, 40, and 60 °C, and at atmospheric pressure.The solubility of NaHCO3 in all glycol mixtures were increasing with increasing temperatures.Solubility is largest in aqueous MEG and decreases with the higher molecular weights of glycol 2 used. Local minima were observed in all systems in the concentration range 80 to 90 wt% glycol, salt-free. On a mole fraction scale, minima were found at x(glycol, salt-free)=0.5. There is a clear tendency that two solvate mechanisms exist with a 1:1 solvation relation. One type of solvation is formed in NaHCO3-water, and a second type is formed in NaHCO3-glycol.The density results showed a linearly increase up to a glycol concentration ≈ 80 wt%. Above 80 wt% the density seemed to form a minima similar to the solubility phase diagrams.

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“…After equilibration, the supernatant was removed by a quick pipet and diluted to determine the concentration, so that the solubility of each substance in the saturated solution was calculated. The Schreinemakers method 21 combined with XRD was used to identify the crystalline solid phase composition corresponding to the saturated liquid phase at the dissolution equilibrium.…”

Section: Methodsmentioning

confidence: 99%

Experiment and Calculation of Solid–Liquid Phase Equilibria in the Ternary System SrCl₂–SrBr₂–H₂O at T = 273, 298, and 323 K

Zhang

Zhao

et al. 2020

J. Chem. Eng. Data

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This work describes the solid−liquid phase equilibria in the ternary system SrCl 2 −SrBr 2 −H 2 O at T = 273, 298, and 323 K based on the method of isothermal dissolution equilibrium. Since saturated liquid phases and humid residue compositions for a series of synthetic brines were determined simultaneously, the measured equilibrium tie lines were constructed. At the same time, the corresponding equilibrium solid phases were identified by using the Schreinemakers' method supplemented with X-ray powder diffraction. The experimental phase diagrams of the system SrCl 2 −SrBr 2 −H 2 O at T = 273, 298, and 323 K were established according to the theory of phase diagram for water salt system. It is found that the type of the system is classified as completely solid solution type due to formation of solid solution Sr(Cl, Br) 2 •6H 2 O. The phase diagrams of the ternary system SrCl 2 −SrBr 2 −H 2 O at 273, 298, and 323 K are constituted of one univariant solubility curve and one solid crystalline phase region corresponding to Sr(Cl, Br) 2 •6H 2 O, without any invariant point. The Pitzer equation was selected to calculate the solubility data in the ternary system SrCl 2 −SrBr 2 −H 2 O at T = 273, 298, and 323 K. The solubility modeling approach achieved good agreement with experimental solubility data.

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Reverse Schreinemakers Method for Experimental Analysis of Mixed-Solvent Electrolyte Systems

Cited by 36 publications

References 20 publications

Solubility and Freezing Points of Disodium Terephthalate in Water–Ethylene Glycol Mixtures

Solubility and Freezing Points of Disodium Terephthalate in Water–Ethylene Glycol Mixtures

Solubility of NaHCO₃ in Systems of Aqueous Glycols (Monoethylene Glycol, Diethylene Glycol, Triethylene Glycol, and Tetraethylene Glycol): The Role of Solvation

Experiment and Calculation of Solid–Liquid Phase Equilibria in the Ternary System SrCl₂–SrBr₂–H₂O at T = 273, 298, and 323 K

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Reverse Schreinemakers Method for Experimental Analysis of Mixed-Solvent Electrolyte Systems

Cited by 36 publications

References 20 publications

Solubility and Freezing Points of Disodium Terephthalate in Water–Ethylene Glycol Mixtures

Solubility and Freezing Points of Disodium Terephthalate in Water–Ethylene Glycol Mixtures

Solubility of NaHCO3 in Systems of Aqueous Glycols (Monoethylene Glycol, Diethylene Glycol, Triethylene Glycol, and Tetraethylene Glycol): The Role of Solvation

Experiment and Calculation of Solid–Liquid Phase Equilibria in the Ternary System SrCl2–SrBr2–H2O at T = 273, 298, and 323 K

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Product

Resources

About

Solubility of NaHCO₃ in Systems of Aqueous Glycols (Monoethylene Glycol, Diethylene Glycol, Triethylene Glycol, and Tetraethylene Glycol): The Role of Solvation

Experiment and Calculation of Solid–Liquid Phase Equilibria in the Ternary System SrCl₂–SrBr₂–H₂O at T = 273, 298, and 323 K