By G.H. Bolt, M.G.M. Bruggenwert

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2). *2 -0 by convention G, is put at zero for the &-ion at unit tctivity in water, which convention is then used as a reference for the calculation of G i for all other ions. 1 kcal/mole yielding the well-known value of the dissociation constant for water of at 25OC and 1bar pressure. 33) 26 where the activity of H20g) is assumed to be unity, which is justifiable for dilute solutions. 8 kcal/mole. ,), is a type of relationship frequently encountered in chapter 6. e. A13+)in terms of the pH, a parameter that can be determined experimentally in a relatively easy manner.

Mole. The ionic species present in the system are then A13+, H+,C1-, OH-. 36) where [Cl-] = lo-,, as it remains in solution. 36) in x (replacing activities by concentrations because of the low value of the ionic strength). x = lo-, + 10-lo/x. As x is close to unity, the last term is obviously negligible, thus one finds, after multiplying with lo4 : 0 . 48 x x lod6 Thus about one half micromole of gibbsite has dissolved. e. 986 x lo-,. Referring to chapter 6 it is pointed out that in reality the above calculation does not entirely apply to this system,as Al3+-ionswill form an association complex with OH--ions.

Aq = in aqueous solution at unit activity (cf. 2). *2 -0 by convention G, is put at zero for the &-ion at unit tctivity in water, which convention is then used as a reference for the calculation of G i for all other ions. 1 kcal/mole yielding the well-known value of the dissociation constant for water of at 25OC and 1bar pressure. 33) 26 where the activity of H20g) is assumed to be unity, which is justifiable for dilute solutions. 8 kcal/mole. ,), is a type of relationship frequently encountered in chapter 6.

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