Tests of equations for the electrical conductance of electrolyte mixtures:Measurements of association of NaCl (Aq) and Na2SO4 (Aq) at high temperatures
Av. Sharygin et al., Tests of equations for the electrical conductance of electrolyte mixtures:Measurements of association of NaCl (Aq) and Na2SO4 (Aq) at high temperatures, J PHYS CH B, 105(1), 2001, pp. 229-237
A review of requirements for equations to calculate the conductivity of a m
ixture of ions in low dielectric constant solvents (i.e., water at high tem
peratures) shows that there are conceptual difficulties with all current eq
uations. To explore whether these difficulties limit our ability to predict
mixtures, four models for the activity coefficients, two models for the co
nductivity of a single strong electrolyte, and an equation for the change i
n equivalent conductivity on mixing single strong electrolytes were chosen.
These equations were then tested on the theoretical equation of Turq et al
. (J. Phys. Chem. 1995, 99, 822-827) for three ion mixtures. Next the equat
ions were tested on a single 1-1 electrolyte, NaCl (aq) at 652.6 K and 22.7
5 MPa measured by Gruskiewicz and Wood (J. Phys. Chem. B 1997, 101, 61549-6
559) and new measurements at 623.9 K and 19.79 MPa. Then it was tested with
new measurements on Na2SO4 tag) from 300 to 574 K because, in water at hig
h temperatures, this salt produces a solution containing six different ions
(Na+, SO42-, NaSO4-, HSO4-, H+, OH-). The equations were able to reproduce
the experimental data. Values of equilibrium constants, K, for the dissoci
ation of NaCl and NaSO4- and equivalent conductances A, derived by a least-
squares fit agreed with reported data determined by other methods, showing
that conductivity measurements can yield accurate equilibrium constants in
complex mixtures of ions. The values of K and A, were not very sensitive to
changes in (Ij the single electrolyte conductance equation, (2) assumed va
lues of A, for minor species, or (3) equilibrium constants for minor reacti
ons. Uncertainty in the activity coefficient model was the largest contribu
tor to uncertainty in K and A,. This method should allow rapid and accurate
measurements of the equilibrium constant for any reaction, which changes t
he number of ions in solution. The equilibrium constants for many reactions
of this type are unknown in water at high temperatures.