Experiment and correlation of osmotic coefficient for aqueous solution of carboxylic acids using NRTL nonrandom factor model

Pirouzi, Ali; Nosrati, Masoud; Haghtalab, Ali; Vasheghani‐Farahani, Ebrahim

doi:10.1016/j.fluid.2012.05.002

Cited by 11 publications

(20 citation statements)

References 18 publications

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“…The second work concerns the study of Pirouzi et al 21 about experimental and correlation of osmotic coefficients for aqueous solutions of carboxylic acids, especially propionic acid. The experimental measurements are based on the isopiestic method at 298 K, which consists of the equilibrium between a sample container and a standard container (NaCl solutions in this study) by transferring water molecules from a container to the other.…”

Section: ■ Results and Discussionmentioning

confidence: 99%

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

et al. 2016

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Solid−liquid phase diagram of the system water/ propionic acid was achieved using two methods, the differential scanning calorimetry and a synthetic method. The liquidus curve is a simple eutectic diagram (89 wt % at 243 K) with an "S-shaped" form due to an inflection point (occurring at around 30% in weight of propionic acid), characteristic of a metastable liquid−liquid phase separation. The experimental data were modeled using experimental activity coefficients of the same system reported in the literature. The results are coherent, although the working temperature domains are different. The obtained phase diagram shows that ice is in equilibrium with the solution in a large composition domain; this is favorable for our further application of freeze wastewater treatment.

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Section: ■ Results and Discussionmentioning

confidence: 99%

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

et al. 2016

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“…The most prevalent systematic experimental methods used to determine the thermodynamic properties are the hygrometric method, isopiestic vapor pressure, − and electromotive force (EMF) measurement. − Among the various experimental techniques, the potentiometric method, due to its advantages such as accuracy, continuous determination, rapidity, stability, and possibility of measurement in more diluted concentrations, could be considered as an attractive alternative approach and efficient for the thermodynamic investigation of such electrolyte systems …”

Section: Introductionmentioning

confidence: 99%

Quaternary System Thermodynamic Investigation in a Mixed Solvent: NaCl + KCl + N,N-Dimethylformamide + H₂O

Masumi

Salamat-Ahangari

2021

J. Chem. Eng. Data

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This article focuses on measuring and modeling activity coefficients and some thermodynamic properties of the quaternary system (NaCl + KCl + N,N-dimethylformamide (DMF) + H 2 O) using a potentiometric technique at (298.15 ± 0.05) K. By employing ion-selective electrodes (Na + -ISE, Cl − -ISE), experimental results were collated for the four series of the mixed electrolyte systems in various ionic strengths for the investigated quaternary system. The electrochemical measurements were carried out over total ionic strengths range from 0.0249 up to about 3.8223 mol•kg −1 in mixed N,N-dimethylformamide + H 2 O solvents, with various solvent mass percents (wt % = 0.0, 0.10, 0.20, and 0.30) at 298.15 ± 0.05 K. Experimental data were modeled on the basis of the Pitzer approach, and the two and three particles mixing ionic interaction parameters (θ NaK and ψ NaKCl ) estimated for the quaternary electrolyte systems under investigation. Finally, using the optimized parameters (θ NaK and ψ NaKCl ), the thermodynamic properties of electrolyte systems, such as activity coefficients of the constituent's electrolyte, osmotic coefficients, and the excess Gibbs free energy, were determined for each mass percent of DMF in water for mixtures of sodium and potassium salts with common anion chloride. The resultant activity coefficients demonstrate a decreasing trend upon decreasing dielectric constants and as the mixed solvent medium growing dense and viscous.

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“…The results of Apelblat et al were adjusted by the authors for the effects of dissociation, and therefore the osmotic coefficients tend to unity at infinite dilution, unlike those of Levien, for example, which have not been adjusted. The most consistent measurements, which have only slight scatter and show expected behavior at low molalities, are those of Apelblat et al, Levien, and Pirouzi et al The osmotic coefficients of Apelblat et al are lower than those of the other two studies at moderate and high concentrations. Fits of the data of Levien from 1 to 5 mol kg –1 yield λ H 3 Citr,H 3 Citr = 0.0738 ± 0.0007 and 0.0760 ± 0.0004 from 1 to 8 mol kg –1 .…”

Section: Model Developmentmentioning

confidence: 65%

“…These are summarized in Table S1 of the Supporting Information. Other relevant measurements include water activities of aqueous H 3 Citr and of liquid–liquid phase equilibrium (both of which yield the Pitzer model self-interaction parameter of the acid) by Kirsch et al, Maffia and Meirelles, Apelblat et al, Peng and Chan, Pirouzi et al, Levien, and also unpublished work from the Ph.D thesis of M. J. Carlo . Water activities of Na 3 Citr solutions have also been measured by Salabat et al, Sadeghi, and Kazemi et al Note, however, that none of these studies of water activities provide any information regarding the concentrations of the individual species in solution (i.e., only those of the total acid and the total salt).…”

Section: Model Developmentmentioning

confidence: 99%

Ion Interaction Models and Measurements of Eu³⁺ Complexation: HEDTA in Aqueous Solutions at 25 °C Containing 1:1 Na⁺ Salts and Citrate pH Buffer

Clegg

Zalupski

Dutech

2016

Ind. Eng. Chem. Res.

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In the TALSPEAK liquid–liquid distribution process, dissolved lanthanides can be separated from actinides using a complexing agent such as N-(2-hydroxyethyl)ethylenediamine-N,N′,N′-triacetic acid (HEDTA, CAS Reg. No. 150-39-0) in a low pH buffered aqueous phase in contact with an organic phase containing a suitable extractant. This study focuses on the chemical speciation of HEDTA, citrate pH buffer, and Eu3+ in aqueous solutions of 1:1 Na+ salts (mainly NaNO3) as a function of ionic strength and pH. New measurements of stoichiometric protonation constants of HEDTA, and the HEDTA complex of Eu3+, in aqueous NaNO3 are reported for ionic strengths from 0.5 to 4.0 M at 25 °C. A Pitzer activity coefficient model of the aqueous mixture has been developed based upon these measurements, available osmotic and activity coefficient data, and stoichiometric equilibrium constants in different 1:1 electrolyte media over a range of ionic strengths. This enables the HEDTA and buffer speciation, and complexation of Eu3+ by both HEDTA and citrate, to be calculated for different solution compositions and pH values. The model of the citrate buffer, which is based on an extensive range of data for NaCl and NaNO3 media, should also be useful in other practical applications.

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Experiment and correlation of osmotic coefficient for aqueous solution of carboxylic acids using NRTL nonrandom factor model

Cited by 11 publications

References 18 publications

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

Quaternary System Thermodynamic Investigation in a Mixed Solvent: NaCl + KCl + N,N-Dimethylformamide + H₂O

Ion Interaction Models and Measurements of Eu³⁺ Complexation: HEDTA in Aqueous Solutions at 25 °C Containing 1:1 Na⁺ Salts and Citrate pH Buffer

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Experiment and correlation of osmotic coefficient for aqueous solution of carboxylic acids using NRTL nonrandom factor model

Cited by 11 publications

References 18 publications

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

Determination of the Solid–Liquid Phase Diagram of the Binary System Propionic Acid/Water

Quaternary System Thermodynamic Investigation in a Mixed Solvent: NaCl + KCl + N,N-Dimethylformamide + H2O

Ion Interaction Models and Measurements of Eu3+ Complexation: HEDTA in Aqueous Solutions at 25 °C Containing 1:1 Na+ Salts and Citrate pH Buffer

Contact Info

Product

Resources

About

Quaternary System Thermodynamic Investigation in a Mixed Solvent: NaCl + KCl + N,N-Dimethylformamide + H₂O

Ion Interaction Models and Measurements of Eu³⁺ Complexation: HEDTA in Aqueous Solutions at 25 °C Containing 1:1 Na⁺ Salts and Citrate pH Buffer