Abstract:Densities of aqueous mixtures of KCI with NaBr are reported at Ionic strengths of 0.5, 1, 2, 3, and 4 mol kg'1 and at 298.15 K from pure KCI to pure NaBr solutions. The excess volumes of mixing, which are negative, can be fitted to Friedman's equation. Mixing experiments at equlmolal concentration and Ionic strengths 1 and 4 mol kg'1 were also conducted at 278.15 and 318.15 K. The results Indicate weak temperature dependence of the excess volumes. The densities of these mixtures can be estimated accurately wi… Show more
“…The mixing rule for the segment energy for K + −other cation interaction is u αβ = u βα = ( u α u β ) 1/2 (1 − k αβ ), where k αβ is the adjustable binary interaction parameter. 5 Predicted and experimental osmotic coefficients for KCl (1) + NaBr (2) and NaNO 3 (1) + KNO 3 (2) solutions at 298.15 K: symbols, experimental data listed in Table ; solid curves, predicted with k αβ ; dashed curves, predicted with k αβ = 1. 6 Predicted and experimental densities for NaCl (1) + KCl (2) and KCl (1) + NaBr (2) solutions at 298.15 K: symbols, experimental data; , solid curves, predicted. 7 Predicted and experimental densities for KCl (1) + CaCl 2 (2) and KCl (1) + MgCl 2 (2) solutions at 298.15 K: symbols, experimental data; , solid curves, predicted.…”
SAFT2 with individual-ion parameters, referred to as ion-based SAFT2, is used to represent the properties of
aqueous electrolyte solutions. A new set of parameters for 5 cations (Li+, Na+, K+, Ca2+, and Mg2+) and 6
anions (Cl-, Br-, I-, NO3
-, SO4
2-,and HCO3
-) is obtained from the fitting of the experimental mean ionic
activity coefficients and liquid densities of 24 aqueous single-salt solutions at 298.15 K. The ion parameters
are universal and transferable to different salts containing the same ion. Because of the peculiar segment
energy of K+, a mixing rule with a binary interaction parameter for the segment energy describing the short-range interactions between K+ and other cations is needed. The binary interaction parameter is derived from
the osmotic coefficients of chloride solutions. The predictions of the osmotic coefficients, vapor pressures,
and liquid densities of single- and multiple-salt solutions including seawater (brine) are found to agree with
experimental data.
“…The mixing rule for the segment energy for K + −other cation interaction is u αβ = u βα = ( u α u β ) 1/2 (1 − k αβ ), where k αβ is the adjustable binary interaction parameter. 5 Predicted and experimental osmotic coefficients for KCl (1) + NaBr (2) and NaNO 3 (1) + KNO 3 (2) solutions at 298.15 K: symbols, experimental data listed in Table ; solid curves, predicted with k αβ ; dashed curves, predicted with k αβ = 1. 6 Predicted and experimental densities for NaCl (1) + KCl (2) and KCl (1) + NaBr (2) solutions at 298.15 K: symbols, experimental data; , solid curves, predicted. 7 Predicted and experimental densities for KCl (1) + CaCl 2 (2) and KCl (1) + MgCl 2 (2) solutions at 298.15 K: symbols, experimental data; , solid curves, predicted.…”
SAFT2 with individual-ion parameters, referred to as ion-based SAFT2, is used to represent the properties of
aqueous electrolyte solutions. A new set of parameters for 5 cations (Li+, Na+, K+, Ca2+, and Mg2+) and 6
anions (Cl-, Br-, I-, NO3
-, SO4
2-,and HCO3
-) is obtained from the fitting of the experimental mean ionic
activity coefficients and liquid densities of 24 aqueous single-salt solutions at 298.15 K. The ion parameters
are universal and transferable to different salts containing the same ion. Because of the peculiar segment
energy of K+, a mixing rule with a binary interaction parameter for the segment energy describing the short-range interactions between K+ and other cations is needed. The binary interaction parameter is derived from
the osmotic coefficients of chloride solutions. The predictions of the osmotic coefficients, vapor pressures,
and liquid densities of single- and multiple-salt solutions including seawater (brine) are found to agree with
experimental data.
“…The ∆U values when combined with the densities F of the solutions can yield adiabatic compressibilities β of the mixture by β ) U -2 F -1 . The densities of these mixtures were taken from our earlier work (Kumar, 1986(Kumar, , 1989b at the desired y 2 using the appropriate interpolation function.…”
Section: Resultsmentioning
confidence: 99%
“…Though the experimental volume data on aqueous mixed electrolyte systems have been collected (Kumar et al, 1982;Kumar and Atkinson, 1983;Kumar, 1988;Kumar, 1989a;Kumar, 1989b) with a view to analyze the specific interaction theory of Pitzer (1973), compressibility data for the concentrated mixtures are scarce in the literature. As a part of our research plan we had published the densities and resultant molal volumes for the aqueous KCl + CaCl 2 and KCl + MgCl 2 systems up to an ionic strength of 4.5 mol kg -1 (Kumar, 1986;Kumar, 1989a).…”
The experimental sound velocities of mixtures composed of KCl + CaCl 2 + water and KCl + MgCl 2 + water are reported at 298.15 K at several ionic strengths in the full mixture composition range. These sound velocities, in conjunction with the earlier published densities, have been employed to estimate the mean apparent molal compressibilities of the mixtures. These mean apparent molal compressibilities of the mixtures have been analyzed by the Pitzer equations without and with binary interaction parameters. The calculated properties with the help of binary interaction parameters show good agreement with those obtained from the experiments. The excess compressibilities examined in light of the Friedman equation have been correlated with excess volumes and enthalpies.
“…The general equation for the excess Gibbs energy of a multi-component electrolyte solution proposed by P1TZER 6,7 is (8) ~ mZ = ~. malZa{: ~_.,mc{Zc{ (9) Cl C where ~O,ca ~la and Cca are temperature-and pressuredependent PITZER parameters reported in the literature. 607 Substituting Eqs (6) and (7) …”
Section: ) Imentioning
confidence: 99%
“…PITZER equation has been tested on the volumetric properties of some mixed aqueous electrolyte solutions at various concentrations. KUMAR 8,9 have recently shown the applicability of PITZER equation in predicting the apparent molar volumes of aqueous electrolyte solutions, in which the ternary mixing terms have not been considered. It is noticed that the values of the mixing parameters greatly depend on the chosen data.…”
In order to obtain the exact information of atomic number density in the ternary system of HNO3-UO2(NO3)z-H20, the densities were measured with an Anton-Paar DMA60/602 digital density meter thermostated at 298.15+0.01 K. The apparent molal volumes for the systems were calculated from the experimental data. The present measured apparent molar volumes have been fitted to the Pitzer ion-interaction model, which provides an adequate representation of the experimental data for mixed aqueous electrolyte solutions up to 6.2 mol/kg ionic strength. This fit yields O r. and ~z, which are the first derivatives with respect to pressure of the mixing interaction parameters for the excess free energy. With the mixing parameters 0 z, and ~v, the densities and apparent molar volumes of the ternary system studied in this work can be calculated with good accuracy, as shown by the standard deviations.
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