Heat capacity of aqueous CaCl2 from 306 to 603 K at 17.5 MPa

The standard state thermodynamic properties for completely ionized hydrochloric acid and ionization of water up to 523 K

“…The hydrogen ion is a unique +1 cation, and at high temperatures, the rapid decrease of the solvent dielectric constant with temperature is known to favor formation of ion pairs (or undissociated species) [13,14] even for some solutes which are strong electrolytes at room temperature (e.g., aqueous HCl [15]). Under these conditions, extrapolation of results from other laboratories at finite concentrations (m > 0.05) to infinite dilution for determination of standard state values is not accurate for many species and cannot be guided by strong electrolyte models.…”

The System CaCl2–H2O: Thermodynamic Modeling and Flow Calorimetry Experiments at Elevated Temperatures and Pressures

“…Data for specific enthalpies of the CaCl 2 –H 2 O system are uncommon; however, indirect enthalpy measurements are possible with the enthalpy of dilution , or heat capacity. ,,, The specific volume correlation can be used to directly determine the specific enthalpy for a given condition using thermodynamic relations shown in eq , …”

“…The fit to ambient temperature data is limited; as with the specific volume correlations, high concentrations of CaCl 2 at room temperature produce a T * that is well below the freezing point of water. There are a total of five data sets, including this study; ,,,, only two of these , feature data above 373 K.…”

“…In this paper, a series of correlations are developed that allow for accurate prediction of key thermodynamic and phase properties of CaCl 2 –H 2 O solutions, namely, ( T , P , w ) behavior along the critical curve, vapor–liquid equilibria at supercritical temperatures, and density, enthalpy, and heat capacity correlations across a broad region of the ( T , P , w ) phase space. In addition, heat capacity data for CaCl 2 –H 2 O have been furnished for high temperatures and pressures, allowing for more accurate determination of specific enthalpies in regions that were previously unavailable. − …”

High dilution calorimetric determination of the standard state thermodynamic differences between the properties of H+(aq) and Na+(aq) up to 598.15K

“…For example, the chloride complexes of most transition metal ions become much stronger at temperature of 573 K [5]. The analysis of CaCl 2 ðaqÞ data [6] has shown that at temperatures above 500 K, there is significant ion association between Ca 2þ ðaqÞ and Cl À ðaqÞ ions.…”