Osmotic Coefficients and Mean Activity Coefficients of Uni-univalent Electrolytes in Water at 25°C

Abstract

This paper gives values for the osmotic coefficients and mean activity coefficients of uni-univalent electrolytes in aqueous solutions at 25 °C. The values are expressed on the molality or weight basis. The data available in the literature have been corrected to the presently accepted scales of atomic weights (1969) and temperature (IPST 1968) and, where necessary, to the absolute electrical units of 1969 and the fundamental constants of 1963. The selected values of osmotic coefficients and mean activity coefficients for individual electrolytes have been made internally consistent thermodynamically. In some cases estimated values are given; in other cases, references only are given when the data are sparse or unsuited to critical evaluation. Values of the osmotic coefficients and mean activity coefficients of 79 compounds are given together with the standard deviation, variance, and normalized standard deviation of their fit to equations which express these quantities as functions of electrolyte concentration. Finally, literature references are given to data on 51 additional uni-univalent electrolytes.

Gas/Aerosol Distribution of Formic and Acetic Acids

“…For CH,COONa, the behavior of the three methods is similar to that for HCOONa. The Pitzer method agrees well with the new data, although its parameters were obtained from the old data (Hamer and Wu 1972) that were measured for ionic strength up to only 3.5 m. For CH,COOK, the experimental data are only available at low ionic strengths, and all the three methods perform well. At high ionic strengths, however, the Pitzer method behaves quite differently from the Bromley and K-M methods.…”

“…Values of the parameters B and q for the Bromley and K-M methods have been refitted to both b~r o m Kim and Frederick (1988). Hamer and Wu's (1972) and Bonner's experimental data for ionic strength up to 14.7 m. In spite of using new fitting parameters (i.e., B and q ) for the Bromley and K-M methods, there is some disagreement between predicted and measured values of the activity coefficient. The Pitzer method, whose parameters were obtained by fitting Hamer and Wu's (1972) experimental data for ionic strength only up to 3.5 m, starts to depart from the measured activity coefficients at an ionic strength of about 7 m. At high ionic strength the Bromley and K-M methods behave similarly for HCOONa, whereas the Pitzer method predicts a considerably lower value of the activity coefficient.…”

Chemical characteristics of inorganic ammonium salts in PM<sub>2.5</sub> in the atmosphere of Beijing (China)

“…A comparison between µmol m −3 amount of NH ). The measured concentration product K mn in units of ppb 2 was determined using the measured data for 24-h sampling time while the theoretical equilibrium constant K n in units of ppb 2 was calculated according to the method in Stelson and Seinfeld (1982a), when the ambient relative humidity (RH) is less than relative humidity of deliquescence (RHD) at any absolute temperature (T ) recorded in Kelvin (Hammer and Wu, 1972):…”

Some Aspects on the Problem of Individual Activity Coefficients of Single-ion Species of Aqueous Strong Electrolytes

“…The values are β NaOH =-2.2415168, β KOH =-1.5256335 and the values for the slopes (b 3 +b 4 ) NaOH =0.457198, (b 3 +b 4 ) KOH =0.519862, respectively. The γ ± values of NaOH solutions and KOH solutions were taken from the book by (Robinson & Stokes, 1959/65) and the paper by (Hamer & Wu 1972). The mean activity coefficients for the ionic strength 10 -3 mol/kg in Eq.…”