Aqueous electrolytes at high temperatures: Comparison of experiment with simulation and continuum models

Wood, Robert H.; Carter, Richard W.; Quint, Jacques R.; Majer, Vladimı́r; Thompson, Peter T.; Boccio, John R.

doi:10.1016/0021-9614(94)90002-7

Cited by 39 publications

(52 citation statements)

References 67 publications

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“…This is a consequence of the high compressibility and lower dielectric constant of the solvent which increase electrostriction and the degree of ion-pairing, respectively, as was documented in previous communications. (16,26,32) It is of interest to compare the present data with those of related salts. Figures 4 and 5 compare the volumetric behaviour of MgCl 2 (aq) with three other electrolyte solutions having a common ion: a 1-1 electrolyte NaCl(aq), (24) a 2:1 electrolyte CaCl 2 (aq), (33) a 2:2 electrolyte MgSO 4 (aq), (34) and with a typical 1:2 electrolyte Na 2 SO 4 (aq) (17) consisting of different ions.…”

Section: Resultsmentioning

confidence: 86%

Volumes of MgCl2(aq) at temperatures from 298 K to 623 K and pressures up to 30 MPa

Obšil

Majer

Hefter

et al. 1997

The Journal of Chemical Thermodynamics

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Section: Resultsmentioning

confidence: 86%

Volumes of MgCl2(aq) at temperatures from 298 K to 623 K and pressures up to 30 MPa

Obšil

Majer

Hefter

et al. 1997

The Journal of Chemical Thermodynamics

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“…Many of their results have been cited by Wood et al (73). Other measurements have been reported for (H+, C1-) to 140°C by Tremaine et al (39), for [Na+, OH-] to 250°C by Simonson et al (74), and for hydrolyzed and unhydrolyzed solutions of aluminum chloride by Conti et al (75).…”

Section: Experimental and Calculation Methodsmentioning

confidence: 87%

Standard state heat capacities of aqueous electrolytes and some related undissociated species

Hepler¹,

Hovey²

1996

Can. J. Chem.

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Uses of heat capacities of solutions of electrolytes are reviewed, with a particular emphasis on the standard state partial molar heat capacities and their applications to calculations of the effects of temperature on equilibrium constants, electrode potentials, enthalpies, and entropies. Methods of obtaining these standard partial molar heat capacities are summarized, followed by comparisons of values obtained in different ways. Many of the "best" such heat capacities are collected and then used as the basis for establishing single-ion heat capacities based on the convention that c p O (~+ ) = 0, followed by illustrations of the convenient use of these quantities. Finally, there is brief discussion of theoretical analysis of these standard partial molar heat capacities in relation to ion-solvent interactions.Key words: heat capacities, electrolytes; aqueous solutions, heat capacities; thermodynamics, electrolytes.RCsumC : On prksente une revue de l'utilisation des capacitCs calorifiques de solutions d'Clectrolytes en insistant d'une faqon particuliere sur les capacites calorifiques molaires partielles dans 1'Ctat standard et leurs applications aux calculs des effets de la temperature sur les constantes d'equilibre, les potentiels d'klectrode, les enthalpies et les entropies. On rksume les methodes d'obtenir ces capacites calorifiques molaires partielles standard et on prksente ensuite un comparaison des diverses valeurs obtenues d'aprks les diverses manieres. Plusieurs des ccmeilleuresa propriCtCs, comme les capacitks calorifiques, ont CtC rassemblCes et ont ensuite Ct C utilisees comme base pour I'Ctablissement des capacitks calorifiques d'un seul ion en se basant sur la convention que c,' (H+) = 0; elles sont suivies par des illustrations sur l'utilisation commode de ces quantitks. Enfin, on presente une breve discussion de I'analyse thiorique de ces capacitks calorifiques molaires partielles standard en relation avec les interactions ion-solvant.

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“…The non-Born terms arise predominantly from configurational hydration effects. (15,16) At low temperature, where configurational effects dominate, the non-Born terms for lanthanides lie in two groups in which the contributions for La(ClO 4 ) 3 …”

Section: Standard Partial Molar Propertiesmentioning

confidence: 99%

“…The standard partial molar heat capacity is traditionally divided into five contributions: (15,16,51,52) C°p ,2 = C°p ,gas + DC°p ,std states + DC°p ,I + DC°p ,II + DC°p ,Born ,…”

Section: Hydration Effectsmentioning

confidence: 99%

“…(14) Thus, the values for C°p ,2 and V°2 of aqueous ions at high temperatures are determined primarily by their size and charge. (15,16) Accurate measurements of C p,f,2 and V f,2 for the aqueous lanthanide perchlorates near ambient conditions are needed to further our understanding of the solvation of trivalent cations under conditions where configurational hydration effects are important.…”

Section: Introductionmentioning

confidence: 99%

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The thermodynamics of aqueous trivalent rare earth elements. Apparent molar heat capacities and volumes of Nd(ClO4)3(aq), Eu(ClO4)3(aq), Er(ClO4)3(aq), and Yb(ClO4)3(aq) from the temperatures 283 K to 328 K

Xiao

Tremaine

1997

The Journal of Chemical Thermodynamics

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Aqueous electrolytes at high temperatures: Comparison of experiment with simulation and continuum models

Cited by 39 publications

References 67 publications

Volumes of MgCl2(aq) at temperatures from 298 K to 623 K and pressures up to 30 MPa

Volumes of MgCl2(aq) at temperatures from 298 K to 623 K and pressures up to 30 MPa

Standard state heat capacities of aqueous electrolytes and some related undissociated species

The thermodynamics of aqueous trivalent rare earth elements. Apparent molar heat capacities and volumes of Nd(ClO4)3(aq), Eu(ClO4)3(aq), Er(ClO4)3(aq), and Yb(ClO4)3(aq) from the temperatures 283 K to 328 K

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