SURFACE COMPLEXATION MODELING GIBBSITE -- CONTENTS -- FOREWORD -- PREFACE -- 1 ALUMINUM OXIDES AND HYDROXIDES UNDER ENVIRONMENTAL CONDITIONS -- 1.1 INTRODUCTION -- 1.2 OCCURRENCE OF ALUMINUM OXIDES AND HYDROXIDES IN THE SUBSURFACE -- 1.3 OCCURRENCE OF ALUMINUM OXIDES AND HYDROXIDES IN SURFACE WATER -- 1.4 USE OF ALUMINUM HYDROXIDE IN WATER TREATMENT -- 1.5 SUMMARY -- 2 FORMATION AND PROPERTIES OF GIBBSITE AND CLOSELY RELATED MINERALS -- 2.1 Al POLYMERIZATION MODELS -- 2.1.1 The "Core-Links" Model -- 2.1.2 The "Cage-Like" (Keggin-Al13 Structure) Model -- 2.1.3 The "Continuous" Model -- 2.2 FORMATION OF GIBBSITE AND OTHER Al HYDROXIDES AND OXYHYDROXIDES -- 2.3 ALUMINUM HYDROXIDE POLYMORPHS: STRUCTURE AND NOMENCLATURE -- 2.4 GIBBSITE -- 2.4.1 Kinetics of Precipitation and Crystal Growth -- 2.4.2 Structure -- 2.4.3 Common Techniques of Synthesis -- 2.4.4 Synthesized Gibbsite and Differences from Natural Gibbsite -- 2.5 BAYERITE -- 2.5.1 Kinetics of Precipitation and Crystal Growth -- 2.5.2 Structure -- 2.5.3 Differences from Gibbsite -- 2.5.4 Synthesized Bayerite and Transformation to Gibbsite -- 2.6 NORDSTRANDITE -- 2.7 DOYLEITE -- 2.8 OTHER FORMS OF ALUMINUM OXIDES AND OXYHYDROXIDES -- 2.8.1 Corundum (α-Al2O3) -- 2.8.2 Boehmite (γ-AlOOH) -- 2.8.3 Diaspore (α-AlOOH) -- 2.9 OTHER FORMS MANUFACTURED UNDER HIGH TEMPERATURE AND PRESSURE -- 3 TYPES OF AVAILABLE DATA -- 3.1 GIBBSITE STRUCTURE VERIFICATION -- 3.2 PHYSICAL-CHEMICAL PROPERTIES -- 3.2.1 Specific Surface Area -- 3.2.2 Surface Site Characterization -- 3.2.2.1 Hydroxyl Surface Sites -- 3.2.2.2 Surface Site Density -- 3.3 ACID-BASE TITRATION DATA -- 3.4 CATION AND ANION SORPTION DATA -- 3.5 SPECTROSCOPIC DATA FOR SORPTION ON GIBBSITE -- 3.6 PROTON RELEASE/UPTAKE DATA -- 3.7 ELECTROKINETIC DATA -- 3.8 SUMMARY -- 4 DATA COMPILATION AND TREATMENT METHODS -- 4.1 COLLECTION OF DATA.

4.2 ASSESSMENT OF DATA QUALITY -- 4.2.1 Solid-Preparation Method -- 4.2.2 Type of Reaction Vessel -- 4.2.3 Nature of Background Electrolyte -- 4.2.4 Sorption Kinetics -- 4.2.4.1 Proton Sorption Kinetics -- 4.2.4.2 Cation and Anion Sorption Kinetics -- 4.2.5 Method of Solid-Liquid Separation -- 4.2.6 CO2 Exclusion -- 4.2.7 Experimental Temperature -- 4.3 COMPILATION OF SURFACE PROPERTIES -- 4.4 EXTRACTION OF EQUILIBRIUM SORPTION CONSTANTS -- 4.4.1 Solution Activity Coefficients -- 4.4.2 FITEQL -- 4.4.3 Data Grouping -- 4.4.4 Selection of Surface Species -- 4.4.5 Selection of Best Estimates -- 4.5 OPTIMAL-FIT SIMULATIONS -- 4.6 PRESENTATION OF RESULTS -- 5 SURFACE PROPERTIES OF GIBBSITE -- 5.1 SURFACE AREA -- 5.2 SITE DENSITY -- 5.3 POINT OF ZERO CHARGE -- 5.4 SURFACE ACID-BASE CHEMISTRY -- 5.5 EFFECTS OF DISSOLUTION ON GIBBSITE SURFACE ACID-BASE CHEMISTRY -- 5.6 SUMMARY -- 6 CATION SORPTION ON GIBBSITE -- 6.1 MODELING METHODOLOGY AND REACTIONS -- 6.2 AVAILABLE SPECTROSCOPIC DATA AND USE IN MODELING -- 6.2.1 Copper -- 6.2.2 Lead -- 6.2.3 Cobalt -- 6.2.4 Cadmium -- 6.2.5 Manganese -- 6.2.6 Iron(II) -- 6.2.7 Calcium -- 6.2.8 Zinc -- 6.2.9 Mercury -- 6.2.10 Uranium -- 6.2.11 Thorium -- 6.3 COPPER -- 6.4 LEAD -- 6.5 COBALT -- 6.6 CADMIUM -- 6.7 MANGANESE -- 6.8 IRON (II) -- 6.9 CALCIUM -- 6.10 ZINC -- 6.11 MERCURY -- 6.12 URANIUM -- 6.13 THORIUM -- 7 ANION SORPTION ON GIBBSITE -- 7.1 MODELING METHODOLOGY AND REACTIONS -- 7.2 AVAILABLE SPECTROSCOPIC DATA AND USE IN MODELING -- 7.2.1 Phosphate -- 7.2.2 Arsenate -- 7.2.3 Arsenite -- 7.2.4 Molybdate -- 7.2.5 Selenate -- 7.2.6 Chromate -- 7.2.7 Borate -- 7.2.8 Sulfate -- 7.2.9 Fluoride -- 7.2.10 Silicate -- 7.3 PHOSPHATE -- 7.4 ARSENATE -- 7.5 ARSENITE -- 7.6 MOLYBDATE -- 7.7 SELENATE -- 7.8 CHROMATE -- 7.9 BORATE -- 7.10 SULFATE -- 7.11 FLUORIDE -- 7.12 SILICATE -- 8 COHERENCE AND EXTRAPOLATION OF THE RESULTS.

8.1 CATION SORPTION ON GIBBSITE -- 8.2 ANION SORPTION ON GIBBSITE -- 8.3 COMPARISON OF GIBBSITE SURFACE-COMPLEXATION CONSTANTS WITH THOSE OF GOETHITE, HYDROUS FERRIC OXIDE, AND HYDROUS MANGANESE OXIDE -- 8.4 SUMMARY -- REFERENCES -- APPENDIX A: SUMMARY OF EXPERIMENTAL DETAILS -- AUTHOR INDEX -- SUBJECT INDEX.