The dissolution kinetics of alumina in aqueous solution was studied in batch and continuous systems. Data were correlated by the kinetic equation C(t) = 1 -exp(-kt"). The parameter k was a function of temperature and acid concentration, while the parameter a remained constant.The temperature variation of k was accurately represented by an Arrhenius-type equation with a temperature coefficient, 18,200 kJ / kmol. The data obtained in batch experiments were free of mass transport and mixing effects. Adsorption-desorption equilibrium of hydrogen ion at the alumina surface was observed. The results supported postulated reactions reported in the literature for alumina dissolution. The basic features of the mechanism include hydration of the aluminum oxide surface, hydrogen ion adsorption followed by reaction to form a positively charged surface species [AI(OH),+ 1, formation of stable surface species [AIOOH and (AI(OH),), SO,], and desorption of products.
IntroductionThe interaction of alumina with acids is encountered in the preparation and regeneration of certain types of catalysts. For example, in studies of the preparation of Pt/AI,O, catalysts, the interaction of hexachloroplatinic acid with alumina supports, and the influence of adding inorganic acids as coingredients to hexachloroplatinic acid impregnating solution have been investigated (Maatman et al., 1971;Santacesaria et al., 1977;Shyr and Ernst, 1980). Methods have been proposed for the removal of nickel and vanadium from contaminated Co/Mo/Al,O, hydrodesulfurization catalysts (Hernandez, 1982; Ganguli, 1984;Myerson and Ernst, 1985). Each of these processes employs a t least one step in which the catalyst is contacted with an acidic solution.One purpose of this work was to examine the dissolution of alumina in aqueous acid solutions. Such data may aid in the further development of catalyst preparation and catalyst regeneration procedures.Often dissolution processes can be described by mass transfer theories (Nernst, 1904), which predict that the instantaneous dissolution rate varies in proportion to a driving force-usually a difference between dissolved species concentration at the solid surface and that in the bulk solution. The rate follows an equation of the form:(1) dc/dt = ~" u * ( c , -C) which, for constant a*, has the solution:Several authors, including Hulbert and Huff (1970) and Kabai (1973), have found that Eq. 2 often does not adequately describe dissolution processes involving metals and metal oxides. Kabai grouped dissolution processes into three basic classifications. In type I, the initial rate of dissolution is finite. Type I processes would include those described by Eq. 2. Type I1 dissolution exhibits an initial rate approaching zero, or an induction period (Diggle, 1973). As the process proceeds, the rate increases and rises to a maximum until equilibrium, or a decreasing amount of undissolved solid, slows the rate. In Type I11 dissolution, the initial rate is infinite. The rate continually decreases with increasing time (Kabai, 1973).Hu...