Thermodynamic Properties of the NaBr+H2O System

Abstract

Equations that described the thermodynamic properties of the NaBr + H 2 0 system were obtained from a fit to experimental results for this system. The experimental results included in the fit spanned the range of temperature of approximately 260 to 623 K and the range of pressure from the vapor pressure of the solution to 150 MPa. New equations and/or values for the fonowing properties are given in the present work: 1) the change in chemical poten.tial with respect to temperature and pressure for NaBr(cr), valid from 200 to 900 K, 2) ~fG~and .6.fH~for formation from the elements for NaBr(cr) for 298.15 K and 0.1 MPa, 3) A.fG~ and Ad/rit from the elements, as well as S~ and C;, m, all for 298.15 K, 0.1 MPa for NaBr-2H 2 0(cr), 4) the change in chemical potential for both NaBr and H20 in NaBr(aq) as a function of temperature, pressure, and molality, valid from 260 to 600 K and from the vapor pressure of the solution to 150 MPa.

Measurement and PC-SAFT modeling of solid-liquid equilibrium of deep eutectic solvents of quaternary ammonium chlorides and carboxylic acids

“…Moreover, in order to achieve the given accuracy, a calibration curve was built using at least six aqueous solutions of LiCl or NaBr at different salt molalities and results were compared to those recommended by Refs. [29] and [30], respectively. Quaternary ammonium solutions were prepared at room temperature by mixing salts and water at the desired composition.…”

Aqueous solutions of the mono- and di-hydrogenphosphate salts of sodium and potassium at elevated temperatures. Isopiestic results

“…In the case of the dihydrogenphosphates, neither the standard ion-interaction model nor the simple expedient of allowing α 1 to be an adjustable parameter proved sufficient to give an acceptable fit. Archer, (21) in deriving a model for the available results for NaBr (aq), introduced a variation of the standard ion-interaction model which he subsequently used in his model for NaCl (aq) (15) and also in a revised model for NaBr (aq). (22) Archer's revision consists of allowing the third virial coefficient, C φ in equation (2), to be dependent on ionic strength in a manner analogous to Pitzer's original assumption (16) for the ionic strength dependence of the second virial coefficient {B φ in equation (2)}.…”

“…(14,21,22) Archer used the third virial coefficient for the excess Gibbs free energy in all of his equations, regardless of the property involved, whereas Pitzer used distinct, but related, third virial coefficients for, as an example, the osmotic and activity coefficients. (15) This difference results in some minor variations in coefficients of the third virial term when comparing Archer's equation with those of Pitzer.…”

Aqueous electrolyte solution modelling: Some limitations of the Pitzer equations

“…A key reason for this gain in popularity is that the increased number of parameters permit more accurate reproduction of available data over wider concentration ranges than the standard form. One of the most popular of the extended forms is due to Archer (1991), who introduced ionic-strength dependence into the third virial coefficient . Other extensions have increased the number of virial terms (Ananthaswamy and Atkinson, 1985) or introduced a temperature-dependent α 1 parameter (Holmes et al, 1997).…”