Viscosity of the Aqueous Ca(NO₃)₂ Solutions at Temperatures from 298 to 573 K and at Pressures up to 40 MPa

Abstract

Dynamic viscosities of seven (0.3207, 0.6771, 1.5235, 2.0310, 2.6118, 3.2810, and 4.0628) mol‚kg -1 and kinematic viscosities of two (4.9861 and 6.0941) mol‚kg -1 aqueous Ca(NO 3 ) 2 solutions have been measured in the liquid phase with a capillary flow technique. Measurements were made at six isobars (0.1, 5, 10, 20, 30, and 40) MPa. The range of temperatures was from (298 to 573) K. The total uncertainty of viscosity, pressure, temperature, and concentration measurements were estimated to be less than 1.5%, 0.05%, 15 mK, and 0.014%, respectively. The reliability and accuracy of the experimental method was confirmed with measurements on pure water for five selected isobars (1, 10, 20, 40, and 50) MPa and at temperatures between (294.5 and 597.6) K. The experimental and calculated values from International Association for the Properties of Water and Steam formulation for the viscosity of pure water show excellent agreement within their experimental uncertainty (average absolute deviation, AAD ) 0.27%). A correlation equation for viscosity of solutions was obtained as a function of temperature and pressure for each measured composition by a least-squares method from the experimental data. The AAD between measured and calculated values from this correlation equation for the viscosity was 0.6 %. The measured values of viscosity at atmospheric pressure were directly compared with the data reported in the literature by other authors.

Thermal Conductivity and Viscosity of Aqueous K2SO4 Solutions at Temperatures from 298 to 575 K and at Pressures up to 30 MPa

“…The main objective of the paper is to provide new accurate experimental thermal conductivity and viscosity data for binary H 2 O + K 2 SO 4 solutions at high temperatures (up to 575 K) and high pressures (up to 30 MPa) for compositions up to 0.782 mol·kg −1 using coaxial-cylinder (steady-state) and capillary-flow techniques, respectively, which have been previously used for accurate measurements on other systems at high temperatures and high pressures [29][30][31][32][33][34][35][36][37][38][39][40][41][42][43][44][45][46][47]. The present results expand considerably the temperature, pressure, and concentration ranges for which thermal conductivity and viscosity data for aqueous K 2 SO 4 solutions are available.…”

“…This work is a part of a continuing program on the transport properties (thermal conductivity and viscosity) of electrolytes in aqueous solutions at high temperatures and high pressures. In previous studies [29][30][31][32][33][34][35][36][37][38][39][40][41][42][43][44][45][46][47] we measured the thermal conductivity and viscosity of 30 aqueous salt solutions at high temperatures (up to 573.15 K) and high pressures (up to 100 MPa) using coaxial-cylinder, parallel-plate, and capillary-flow techniques.…”

Viscosity

“…It should be stressed, however, that the conclusions derived here are only based on a preliminary comparison, and should be viewed accordingly. Below the discrepancies between different datasets were examined statistically in terms of the absolute H 2 O+Ca(NO 3 ) 2 : Two datasets were found (Zeynalova et al, 1991;Abdulagatov et al, 2004). The agreement between these data sets at atmospheric pressure and at temperatures from 298 to 348 K is within 0.1%, while at 373 K…”

“…To extend the validity of Equation (6.41) to higher concentrations, Jones and Talley (1933), Kaminsky (1955Kaminsky ( , 1956Kaminsky ( , 1957, Feakins and Lawrence (1966), Robertson and Tyrrell (1969), Desnoyers et al (1969), Desnoyers and Perron (1972), Abdulagatov et al (2004Abdulagatov et al ( , 2005 and Abdulagatov and Azizov, 2006a,b), added a quadratic term Dc 2 (extended Jones-Dole equation), as η η 0 2 1 = + + + A c Bc Dc .…”

“…It was proposed that the new term in Equation (6.42) accounted for solute-solvent and solute-solute structural interactions at high concentrations (Stokes and Mills, 1965;Desnoyers and Perron, 1972) such as: long-range Coulombic forces; high term hydrodynamic effects; and effects arising from changes in solute-solvent interactions due to concentration changes. Finally, Abdulagatov et al (2004Abdulagatov et al ( , 2005,b) included one further term, Fc 2.5 , as and thus increased the validity of the equation up to saturated concentration. Grimes et al (1979) and Kestin and Shankland (1984b) omitted the square-root term owing to its small magnitude, and proposed an equation of the form (6.45) Grimes et al (1979) and Kestin and Shankland (1984b) employed successfully the aforementioned equation to describe the behavior of the systems H 2 O + NaCl and H 2 O + KCl.…”