Valency of ions

As is derived from Equation (8), can be adjusted by changing the dielectric constant and/or the viscosity of the medium, but also C- As mentioned before, the zeta potential is mainly influenced by the distribution of charges at the capillary wall. All alterations resulting in a change of the charge distribution at the capillary wall like changes in the pH, ionic strength, valence of ions in the buffer electrolyte, etc., can be applied to adjust the velocity of the EOF. 

Examination of Figure 1-12 provides some clue to qualitatively gauge the interface reaction rate for reactions in water. Figure 1-12 shows that, for mineral with low solubility and high bond strength (characterized by (z+z )max, where z+ and z are valences of ions to be dissociated), the overall dissolution rate is controlled by interface reaction otherwise, it is controlled by mass transport. Because diffusivities of common cations and anions in water do not differ much (by less than a factor of 10 Table l-3a), when the overall reaction rate is controlled by interface reaction, it means that interface reaction is slow when the overall reaction rate is controlled by mass transport, the interface reaction rate is rapid. Therefore, from Figure 1-12, we may conclude that the interface reaction rate increases with mineral solubility and decreases with bond strength (z+z )max to be dissociated. 

For solutions of electrolytes the standard state is derived from an analogous hypothetical state of the ideal solution it will be shown later that when indicating the concentration of such a solution even the valences of ions formed on the dissociation should be considered. )... 

We see from equation (1) that, in very dilute solutions of a strong electrolyte, the activity coefficient is determined only by the concentration and valence of ions, the specific nature of the ions having no appreciable influence. 

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