Measuring the isoelectric point of the edges of clay mineral particles. The case of montmorillonite

Abstract

The isoelectric point (IEP) of the edge surface of a montmorillonite sample was determined by using electrophoretic mobility measurements. This parameter, which is fundamental for the understanding of the charging behavior of clay mineral surfaces, was never measured so far because of the presence of permanent negative charges within the montmorillonite structure, charges that mask the electro- kinetic behavior of the edges. The strategy was to block or neutralize the structural charges with two di ff erent cations, methylene blue (MB + ) and tetraethylenepentaminecopper(II) ([Cu(tetren)] 2+ ), so that the charging behavior of the particles becomes that of the edge surfaces. Adsorption isotherms of MB + and [Cu(tetren)] 2+ at di ff erent ionic strengths (NaCl) were performed to establish the uptakes that neutralize the cation exchange capacity (CEC, 0.96 meq g − 1 ) of the sample. At high adsorptive concentrations, there was a superequivalent adsorption of MB + (adsorption exceeding the CEC) and an equivalent adsorption of [Cu(tetren)] 2+ (adsorption reaching the CEC). In both cases, structural charges were neutralized at uptakes very close to the CEC. Zeta potential ( ζ ) vs pH data at di ff erent ionic strengths of montmorillonite with adsorbed MB + allowed to estimate an upper limit of the edge ? s IEP, 5.3 ± 0.2. The same kind of data obtained with adsorbed [Cu(tetren)] 2+ provided a lower limit of the IEP, 4.0 ± 0.2. These values are in agreement with previously informed IEP and point of zero charge of pyrophyllite, which is structurally analogous to montmorillonite but carries no permanent charges. The importance of knowing the IEP of the edge surface of clay minerals is discussed. This value characterizes the intrinsic reactivity of edges, that is, the protonating capacity of edge groups in absence of any electric fi eld generated by structural charges. It also allows us to correct relative edge charge vs pH curves obtained by potentiometric titrations and to obtain the true edge charge vs pH curves at di ff erent electrolyte concentrations.