Aqueous solutions of strong electrolytes

E. A. Guggenheim, Specific Thermodynamic Properties of Aqueous Solutions of Strong Electrolytes , Phil. Mag., 19, 588-643 (1935). 

G. Jones and M. Dole, The viscosity of aqueous solutions of strong electrolytes with spedal reference to barium chloride,... 

Ionic melts possess electrical conductivities roughly a factor ten larger than those of concentrated aqueous solutions of strong electrolytes (ionophores). 

Guggenheim G. A. (1935) The specific thermodynamic properties of aqueous solutions of strong electrolytes. Phil. Mag. 19, 588-643. 

Concentrations of ions in aqueous solutions of strong electrolytes can be calculated directly from the molarity of the strong electrolyte, as the following example illustrates. 

The evidence just given, which is typical of that obtained from all recent measurements, shows that the Onsager equation is valid for very dilute aqueous solutions of strong electrolytes. This fact is important as it lends additional and strong support to the correctness and utility of the interionic attraction theory. As has already been emphasized Onsager s equation is a limiting equation and deviations from it, even for completely dissociated electrolytes, are to be expected as the concentration is increased. 

In the intervening ten years, has there been developed a more accurate way (or ways) to describe activity coefficients in complex, concentrated aqueous solutions of strong electrolytes ... 

In early experiments (60) the results of electrolyte noise measurements were best described by relation 10 if the dimensionless parameter a was assumed to be proportional to the electrolyte concentration and was taken to be equal to 10 for 1-M aqueous solutions of strong electrolytes. 

In polarography as we shall see later, the solutions used are usually aqueous solutions of strong electrolytes and in these cases the ohmic drop is negligible. If we ignore this factor then ... 

Gupta and Heidemann (1990) used a modified UNIFAC model to predict the effects of temperature and pH on the solubility of amino acids in water. They also made a similar approach to the modelling of the solubility of several antibiotic substances in mixed non-aqueous solvents. Macedo, Skovborg and Rasmussen (1990) used a modified UNIFAC model to calculate phase equilibria for aqueous solutions of strong electrolytes. 

Jones G, Dole M (1929) The viscosity of aqueous solutions of strong electrolytes with special reference to barium chloride. J Am Chem Soc 51 2950-2964 Kalidas C, Hefter GT, Marcus Y (2000) Gibbs eneigies of transfer of cations from water to aqueous organic solvents. Chem Rev 100 819-852... 

M4. Meissner, H.P. and C.L. Kusik. "Vapor Pressures of Water Over Aqueous Solutions of Strong Electrolytes", Ind. Eng. Chem. Proc. Des. Dev., 12, 112... 

The first to report the concentration dependence of halide ion quadrupole relaxation in aqueous solutions of strong electrolytes were Itoh and Yamagata [247]. Their and later studies have shown that whereas the change in relaxation with concentration may depend greatly on the cation present, the relaxation rate at low concentrations is independent of cation. For aqueous solutions of alkali halides, the concentration dependence of the anion quadrupole relaxation rate is in most cases weak below ca. 1 M. Consequently the relaxation rate in the... 

On the whole, one finds that the existing interpretations of the non-ideal behavior of solutions are fairly complicated and that there is no simple, meaningful and unified explanation of the properties of dilute and concentrated solutions. Therefore, the present author decided to interpret directly, without presupposed models, the actual experimental data as such rather than their deviations from ideality (or complete dissociation) represented by formal coefficients like 9 and V. Attention is paid here mainly to aqueous solutions of strong electrolytes, since these are considered anomalous (15). Extensive work on univalent and multivalent electrolytes has shown (8,9a-i) that when allowance is made for the solvation of solutes, Arrhenius theory of partial dissociation of electrolytes explains the properties of dilute as well as concentrated solutions. This finding is in conformity with the increasing evidence for ion association of recent years mentioned above. 

Kaminsky, M. 1957. The concentration and temperature dependence of the viscosity of aqueous solutions of strong electrolytes. III. KCl, K2SO4, MgCl2, BeS04, and MgS04 solutions. Zeitschriftfuer Physikalische Chemie. 12 206. 

Jones, G. Dole, M. (1929). The transference number of barium chloride as a function of the concentration. Journal of the American Chemical Society, 51, (1929), 1073-1091 Kaminsky M. (1957). The concentration and temperature dependence of the viscosity of aqueous solutions of strong electrolytes. III. KCl, K2SC>4, MgC12, BeS04, and MgS04 solutions. Zeitschrift filer Physikalische Chemie, 12, (1957), 206-231 Kaneko, S. Kono, Y. Kobayashi, H. Ishikawa, H. Utsuki, K. (2009). Nonaqueous electrolyte solution, gel electrolyte, and secondary lithium battery using the electrolyte solution and the gel electrolyte. Jpn. Kokai Tokkyo Koho (2009), ]P 2009140641 A 20090625... 

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