The Thermodynamics of Aqueous Potassium Chloride Solutions from Electromotive Force Measurements

Harned, Herbert S.; Cook, Melvin A.

doi:10.1021/ja01286a038

Cited by 51 publications

(47 citation statements)

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“…No change in membrane morphology was observed after the membrane was compacted after the experiments. [19,20], high osmotic pressure and excellent performance as draw solution for forward osmosis fertigation application [5,6]. NaCl solution (5000 mg/L) has been used as model brackish water FS since the majority of solutes present in the brackish water consists of Na + and Clions.…”

Section: Membranes and Draw Solutionsmentioning

confidence: 99%

Performance comparison of thin-film composite forward osmosis membranes

Fam

Phuntsho

Lee

et al. 2013

Desalination and Water Treatment

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Forward osmosis (FO) is an emerging low-energy technology. Much effort was given on developing a new membrane material and engineering membrane structure to improve the performance of FO membranes. The performances of two newly developed polyamide based thin film composite (TFC) FO membranes were tested and compared with the commercially available cellulose triacetate (CTA) FO membrane. The intrinsic properties of the two TFC FO membranes determined in RO experiments indicate superior performance of the membranes. When tested in FO experiments, TFC membranes delivered consistent results, confirming their outstanding permeability and selectivity properties. The study shows that future studies on membrane fouling will be necessary to have a better understanding of membrane performance and to further optimize membrane properties.

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Section: Membranes and Draw Solutionsmentioning

confidence: 99%

Performance comparison of thin-film composite forward osmosis membranes

Fam

Phuntsho

Lee

et al. 2013

Desalination and Water Treatment

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“…Stokes [47] has calcula ted the activity of water in solutions of potassium chlorid e fron~ the electromotive-force data of H arned and Cook [48]. For molalities of po tassium chloride from 0 to 0.2 , -log -Jaw is 0.0072 m. The nonelectrolyte .…”

Section: Activity Coefficientsmentioning

confidence: 99%

Acidic dissociation constant of ammonium ion at 0 to 50 C, and the base strength of ammonia

Bates¹,

Pinching²

1949

J. RES. NATL. BUR. STAN.

187

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The acidic dissociation of many acids has been studied in detail, but weak bases have genera lly been neglected because of t he experimental difficulties encountered in the investigation of some of their buffer solutions by electromotiye-force methods. These difficulties may arise from volatility of the free base or the existence of extraneous electrode reactions such as the formation of ammine complexes at the s ilver-silver-chloride electrode. In th is study of ammonia, special saturators were used to prevent, insofar as possible, t he removal of ammonia from the solutions by the hydrogen gas. A co rrection was applied for the amou nt of diammine silver complex formed at the sil ver-silver-ch loride electrode, a nd t his silver ion was prevented by mechanical means from reaching the platinum electrodes.With these precautions, the acidic dissociation constant of ammonium ion at 0° to 50° C was determined f rom electromotive-force measurements on 19 b uffer solutions containing equal molalities of ammonia and ammonium chloride. The changes of free e nergy, heat content, entropy, and heat capacity that accompany the dissociation processes in the standard state were derived from the temperatu re coefficients of the acidic dissociation constant of ammonium ion and of the basic dissociation constant of ammonia. The activity coefficient o[ ammonium chloride in equ imolal buffer solutions at 25° C was calcu lated.

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“…In method II considered in ref , the constant parameter values obtained from method I were accepted for B , and a quadratic temperature dependence for parameter b 1 was determined mainly from the all amalgam cell data of Harned and Nims, and Harned and Cook for NaCl and KCl solutions, respectively. These electrochemical data cover the temperature range from (0 to 40) °C.…”

Section: Introductionmentioning

confidence: 99%

Traceable Thermodynamic Quantities for Dilute Aqueous Sodium Chloride Solutions at Temperatures from (0 to 80) °C. Part 1. Activity Coefficient, Osmotic Coefficient, and the Quantities Associated with the Partial Molar Enthalpy

Partanen

Vahteristo

2017

J. Chem. Eng. Data

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We present fully traceable two-parameter Hückel equations (with parameters B and b 1) for the activity coefficient of sodium chloride and for the osmotic coefficient of water in aqueous NaCl solutions at temperatures from (0 to 80) °C. These equations apply within experimental error to all thermodynamic data available for these solutions at least up a molality of 0.2 mol·kg–1. In our previous study (J. Chem. Eng. Data 2016, 61, 286–306), these equations were successfully tested against the literature results of electrochemical, isopiestic, and cryoscopic measurements usually in the temperature range from (0 to 25) °C. There, a constant value was employed for B, whereas a linear model with respect to the temperature was utilized for b 1. The linear model was determined from the values of b 1 at 0 °C and at 25 °C obtained from freezing-point depression data and from isopiestic and cell-potential difference data, respectively. In the present study, these two b 1 values are utilized alongside the constant value of parameter B but a new quadratic model is presented for the temperature dependence of b 1. The third data point required for this model is obtained from the direct vapor pressure measurements of Gibbard et al. (J. Chem. Eng. Data 1974, 19, 281–288) at 75 °C. The results obtained with this quadratic equation for b 1 agree well with the test results of the linear model in the previous paper (see the citation above) up to 25 °C. The most important new test results above that temperature are reported here. Our quadratic model has additionally been tested with all the high-precision calorimetric data available in the literature for NaCl solutions. In this first part (Part 1) of the study, the test results from the thermodynamic quantities associated with partial molar enthalpy are reported. In the forthcoming second part (Part 2) of the study, the results of the quantities associated with the heat capacity of NaCl solutions will be considered. In the tests of these two parts, all calculations dealing with calorimetric data are performed in a new way. Both the calorimetric data and the vapor pressure data (from both direct and isopiestic measurements) can be predicted using the new Hückel equations within experimental error in dilute NaCl solutions from (0 to 80) °C. For comparison, also other Hückel models are considered and at best these apply up to the molality of the saturated NaCl solution at various temperatures. Following the success of the new models, new values for the activity coefficients, osmotic coefficients, relative apparent molar enthalpies, and relative partial molar enthalpies for NaCl solutions at rounded molalities are reported at the end of this Article. We have good reasons to believe that the new values contain the most reliable ones available for the given thermodynamic quantities.

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The Thermodynamics of Aqueous Potassium Chloride Solutions from Electromotive Force Measurements

Cited by 51 publications

References 0 publications

Performance comparison of thin-film composite forward osmosis membranes

Performance comparison of thin-film composite forward osmosis membranes

Acidic dissociation constant of ammonium ion at 0 to 50 C, and the base strength of ammonia

Traceable Thermodynamic Quantities for Dilute Aqueous Sodium Chloride Solutions at Temperatures from (0 to 80) °C. Part 1. Activity Coefficient, Osmotic Coefficient, and the Quantities Associated with the Partial Molar Enthalpy

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