Application of the Specific Ion Interaction Theory (SIT) for the ionic products of aqueous electrolyte solutions of very high concentrations

The Bronsted-Guggenheim-Scatchard Specific Ion Interaction Theory (SIT) has been employed for the pK(w) values of highly concentrated aqueous solutions of NaCl (I-m <= 6.00 mol kg(-1)), KCl (I-m <= 4.57 mol kg(-1)), CsCI (I-m <= 10.02 mol kg(-1)), KBr (I-m <= 4.71 mol kg(-1)), KI (I-m <= 6.96 mol kg(-1)), NaClO4 (I-m <= 13.66 mol kg(-1)), (CH3)(4)NCI (I-m <= 12.82 mol kg(-1)) and NaCF3SO3 (I-m <= 6.41 mol kg(-1)) at 25 degrees C. No systematic deviation from linearity was observed at very high ionic strengths (in some cases up to 10 mol kg(-1)). The intercept of the SIT plots, pK(w)(0) (even with the inclusion of data points at the highest ionic strength) was found to be 14.00 +/- 0.04. Systematic downward deviation from linearity can only be identified in the I(m) >6 mol kg(-1) range for NaClO4 and (CH3)4NCI containing systems (i.e., background electrolytes that are thought to be inert or non-interacting). Delta epsilon values obtained as the sum of epsilon(OH-,M+) and epsilon(H+,A(-)) calculated from the osmotic coefficients of HA and MOH solutions are always somewhat larger than those determined from the linear sections of our SIT plots for the given MA salt. The specific ion interaction coefficient e(OH-,(CH3)4N') has been estimated and, as expected for a non-complexing cation, it was found to be significantly larger, than those obtained for the other alkaline metal ions studied. On the basis of these results, it is possible that linear SIT behavior holds for equilibria other than the autoprotolysis of water, up to very high, i.e., hydrometallurgically relevant ionic strengths. (C) 2008 Elsevier B.V. All rights reserved.