Potentiometric study of aluminium-fluoride complexation equilibria and definition of the thermodynamic model

Complexation constants of the Al3+/F- system were determined at different ionic strengths in a NaClO4 (1.0, 2.0 and 3.0 mol . dm(-3) ) ionic medium by means of a potentiometry using two electrode systems: an ion fluoride selective electrode as well as a glass electrode. All the experimentation was performed at 25 C. The main species in the complexation equilibria were determined as AlF2+, AlF2+, AlF30, AlF4-, AlF52- and AlF63-. The differences found in the complexation constants for the ionic strength considered were explained by the different behavior of the interaction parameters for the AlFn3-n species. These parameters were calculated using the Modified Bromley's Methodology (MBM). The corresponding thermodynamic quantities were also determined. From all the results obtained, it can be concluded that pH, fluoride concentration and ionic strength influenced the distribution of the fluoride- aluminium complexes.