Studies on the Hydrolysis of Metal Ions. XI. The Aluminium Ion, Al3+.

Brosset, Cyrill; Biedermann, George; Sillén, Lars Gunnar; Sørensen, Nils Andreas

doi:10.3891/acta.chem.scand.08-1917

Cited by 151 publications

(58 citation statements)

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“…The best quantitative evidence for this conclusion is furnished by the precise measurements of Kubota (5) and Nazarenko and Nevskaya (6). At increasing A1 concentrations the formation of polynuclear hydroxo-complexes are called upon to explain the experimental data (2)(3)(4)(7)(8)(9). Unfortunately, no general consensus of opinion exists as to the exact identity and number of such polymeric species in solution.…”

Section: Introductionmentioning

confidence: 99%

Hydrolysis-precipitation studies of aluminum (III) solutions. I. Titration of acidified aluminum nitrate solutions

Vermeulen

Geus

Stol

et al. 1975

Journal of Colloid and Interface Science

110

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Acidified aluminum nitrate solutions were fitrated with alkali (NaOH or KOH) over a temperature range of 24°C to 90°C. A homogeneous distribution of added base was achieved by: (i) in situ decomposition of urea (90°C); and (ii) a novel method involving injection through a capillary submerged in the agitated salt solution.The experimental pH curves are characterized by two plateaus (or platforms) separated by a steep jump in pH. These characteristic features were not previously observed in continuous titration experiments. This is especially true of the second platform, which begins at an OH/A1 ratio larger than 2.5. Stable colloidal solutions or gels are formed on traversing this plateau. The hydrolysis-precipitation behavior was also followed by light scattering and x-ray diffraction measurements.A qualitative picture of the neutralization process is developed.

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Section: Introductionmentioning

confidence: 99%

Hydrolysis-precipitation studies of aluminum (III) solutions. I. Titration of acidified aluminum nitrate solutions

Vermeulen

Geus

Stol

et al. 1975

Journal of Colloid and Interface Science

110

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“…The distributions of aqueous mononuclear aluminium and iron species in water are well known through constants of ligand protonation, metal complex formation, metal hydrolysis and the ionic product of water. The stability constants of many aluminium oxo-hydroxy polynuclear ions (Al n m þ ) are also known (Flaten, 1994;Brosset et al, 1954;Baes and Mesmer, 1976;Ö hman and Forsling, 1981;Ö hman, 1988;Sincero and Sincero, 2003). For the most part these values have been determined by potentiometric titrations.…”

Section: Introductionmentioning

confidence: 99%

Colloidal surfaces and oligomeric species generated by water treatment chemicals

Rämö

Sarpola

Hellman

et al. 2008

Chemical Speciation & Bioavailability

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Properties of water treatment chemicals were investigated by a novel combination of analytical methods. Oligomer distribution, total surface charge, zeta potential and conductivity were evaluated in simulated systems containing highly and moderately basic polyaluminium chlorides, aluminium sulfate (alum), ferric chloride and ferric sulfate. Species were quantified on the basis of mass spectrometric results. Polyaluminium chemicals gave rise to an intensive and completely cationic distribution of mainly Al 13 -based oligomers and high surface charges. Both cationic distribution and charge decreased with increase of pH and increased with concentration of the chemical. The other chemicals produced a wider oligomeric distribution of smaller species, including anions. The dimeric form was typical for iron. In the case of the sulfate-containing chemicals, sulfate was present in the majority of oligomers and zeta potentials were stable. For the chemicals without sulfate, pH values needed to be high enough to provide high zeta values. The results can be utilized in the improvement of coagulation and flocculation mechanisms aimed at the removal of bacteria, viruses and other micro organisms, as well as at humic and mineral particles. In addition, semi quantitative information about oligomeric species may be helpful in breaking down cell membranes to support disinfection.

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“…The mechanisms of intercalation, however, have not been clear, primarily because of the controversy over the nature of OH-AI polymers. Brosset et al (1954), followed by Hsu and others, first proposed that the OH-AI polymers have a hexagonal-ring structure resembling fragments of AI(OH)3 crystals (Hsu, 1989). Many recent studies (Akitt et al, 1972;Akitt and Farthing, 1978;Bottero et al, 1980;Bertsch et al, 1986aBertsch et al, , 1986b) favored the Alia Keggin structure for the OH-A1 polymers in solution, originally proposed by Johansson (1963).…”

Section: Introductionmentioning

confidence: 99%

Reaction of OH-Al Polymers with Smectites and Vermiculites

Hsu¹

1992

Clays and clay miner.

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Abstract--Five montmorillonites, one hectorite, and two vermiculites were treated with OH-AI solutions containing rapid-and slow-reacting polymers of similar concentrations. With all smectites, both rapidand slow-reacting OH-A1 polymers were much more preferentially adsorbed than monomeric species. Relatively slow-reacting OH-AI polymers were more preferentially adsorbed than rapid-reacting ones. The average basicity of the adsorbed A1 was 2.46, which was close to that of the OH-AI polymers in the original solution. The OH-AI polymers that enter the interlayer resemble those in original solutions.With vermiculites, the solution concentration of rapid-reacting OH-A1 polymers was much reduced after reaction. The average basicity of the adsorbed A1 was 1.99, which was considerably lower than that in the original solution. It is postulated that OH-AI polymers break to monomeric Al ions and then enter the clay. The monomeric Al species that enter the clay interlayers hydrolyze and polymerize in situ and become fixed. The H ~ ions released from hydrolysis convert the rapid-reacting OH-AI polymers to monomeric Al in solution. Limited amounts of slow-reacting polymers were adsorbed because of their resistance to acid depolymerization.

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Studies on the Hydrolysis of Metal Ions. XI. The Aluminium Ion, Al3+.

Cited by 151 publications

References 0 publications

Hydrolysis-precipitation studies of aluminum (III) solutions. I. Titration of acidified aluminum nitrate solutions

Hydrolysis-precipitation studies of aluminum (III) solutions. I. Titration of acidified aluminum nitrate solutions

Colloidal surfaces and oligomeric species generated by water treatment chemicals

Reaction of OH-Al Polymers with Smectites and Vermiculites

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