On the surface tension and Zeta potential of electrolyte solutions

The distribution of ions in the vicinity of the air/water interface is still a matter of strong debate, with numerous calculations and experiments providing contradictory results, even regarding the preference of simple ions (such as H⁺ and OH^-) for interfacial or bulk water. When short range interactions between ions and the interface are assumed independent of bulk concentrations, if they are compatible with the surface tension data, they underpredict the experimental Zeta potentials by orders of magnitude. If they are compatible with Zeta potential data, they are in strong disagreement with surface tension experiments. It is suggested that these observations might be a result of the relatively low number of interfacial water molecules available to hydrate the ions and the competition between various ions for adsorption sites. Therefore, whereas at low bulk concentrations, the Structure-Breaking ions prefer the interface, at sufficiently large bulk concentrations the surface adsorptions of these ions become saturated, and their interfacial concentrations may become lower than in the bulk. Consequently, the total interactions of ions with the interface can be strongly attractive at low bulk concentrations, and less attractive (or even repulsive), at high concentrations. To model this effect, the interactions between ions and interface are taken into account via modified Langmuir adsorption expressions for OH^- and Cl^-, while the H⁺ ions are considered to be attached to any interfacial water molecule, even if the latter participate in the hydration of anions. The simple model of adsorption employed here is in agreement with both experiments on Zeta potential and on surface tension, and might reveal the conditions under which a given ion exhibits propensity for either the air/water interface, or for bulk water.