The enthalpy of dilution and thermodynamics of Na2CO3(aq) and NaHCO3(aq) fromT = 298 K toT = 523.15 K and pressure of 40 MPa |
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| Institution: | 1. School of Chemistry, Physics and Mechanical Engineering, Science and Engineering Faculty, Queensland University of Technology, GPO Box 2434, Brisbane, Queensland 4001, Australia;2. Geology Department, Federal University of Minas Gerais, Belo Horizonte, MG 31270-901, Brazil;3. Geology Department, School of Mines, Federal University of Ouro Preto, Campus Morro do Cruzeiro, Ouro Preto, MG 35400-00, Brazil;1. Department of Physical Chemistry, Chemical Faculty, Gdańsk University of Technology, 80-233 Gdańsk, Poland;2. Department of Analytical Chemistry, Chemical Faculty, Gdańsk University of Technology, 80-233 Gdańsk, Poland;1. Laboratorio de Termodinámica de Soluciones, Departamento de Química, Universidad de Los Andes, Cr. 1 No. 18 A-10, Bogotá, Colombia;2. Institut für Physikalische und Theoretische Chemie, Universität Regensburg, D-93040 Regensburg, Germany;1. Los Alamos National Laboratory, P.O. Box 1663, M.S. J535, Los Alamos, NM 87545, United States;2. Department of Earth and Planetary Sciences, McGill University, 3450 University Street, Montreal H3A 0E8, Canada;1. College of Food and Bioengineering, Henan Key Laboratory of Cold Chain Food Quality and Safety Control, Zhengzhou University of Light Industry, Zhengzhou 450000, PR China;2. School of Light Industry and Engineering, Qi Lu University of Technology (Shandong Academy of Sciences), Jinan 250353, PR China |
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| Abstract: | Molar enthalpies of dilution ΔdilHmofNa2CO3(aq) were measured from molality m = 1.45 mol · kg − 1to m = 0.008 mol · kg − 1at seven temperatures from T = 298 K toT = 523 K at the pressure p = 7 MPa, and at four temperatures fromT = 371 K to T = 523 K at the pressurep = 40 MPa. Molar enthalpies of dilutionΔdilHm of NaHCO3(aq) were measured fromm = 0.98 mol · kg − 1tom = 0.007 mol · kg − 1at the same temperatures and pressures. Hydrolysis and ionization equilibria contribute substantially to the measured enthalpies under many of the conditions of this study. Explicit consideration of these reactions, using thermodynamic quantities from previous studies, facilitates a quantitative representation of apparent molar enthalpies, activity coefficients, and osmotic coefficients with the Pitzer ion-interaction treatment over the ranges of temperature, pressure, and molality of the experiments. |
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