The use of potassium chloride and tris(hydroxymethyl)aminomethane as standard substances for solution calorimetry

Determination of the energy equivalent of a water solution calorimeter with a standard substance

We have summarized results of many experimental investigations of the thermodynamics of ionization of H2O(liq.) from 0–300°C and from 1.0 atm to nearly 8000 atm. Results of these investigations (equilibrium constants, enthalpies of ionization, heat capacities, partial molal volumes, and compressibilities) have been used for a number of thermodynamic calculations. It is particularly noteworthy that it is possible to use thermal data from 0–145°C with an equilibrium constant for 25°C in calculating reasonably accurate equilibrium constants for temperatures as high as 300°C. Similarly, it is possible to use volumetric data that refer to 1.0 atm in calculating useful equilibrium constants that apply for pressures as high as 2000 atm.

Thermodynamics of ionization of water over wide ranges of temperature and pressure

Thermodynamics for ionization of water at temperatures from 278.15 K to 393.15 K and at the pressure 0.35 MPa: apparent molar volumes of aqueous KCl, KOH, and NaOH and apparent molar heat capacities of aqueous HCl, KCl, KOH, and NaOH☆

Thermodynamics of ionization of water at temperatures 278.15⩽⩽⩽T / K⩽⩽⩽ 393.15 and at the pressurep = 0.35 MPa: apparent molar volumes and apparent molar heat capacities of aqueous solutions of potassium and sodium nitrates and nitric acid

G.L. Kimball

Papers

Calorimetric determination of the heat of reaction of solid tris(hydroxymethyl)aminomethane with 0.1 M HCl solutions at 10, 25 and 40°c

Calorimetric Determination of the Heat of Ionization of Water at 10° and 40°C*