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| Cerium(IV) sulfate | |
|---|---|
| Name | Cerium(IV) sulfate |
| IUPACName | Cerium(IV) sulfate |
| OtherNames | Ceric sulfate |
| ChemicalFormula | Ce(SO4)2 |
| MolarMass | 332.23 g·mol−1 |
| Appearance | yellow-green crystalline solid (hydrate) |
| Density | 2.99 g·cm−3 (anhydrous, calc.) |
| MeltingPoint | decomposes before melting |
| Solubility | soluble in water (varies with hydration) |
| CASNumber | 10294-32-7 |
Cerium(IV) sulfate is an inorganic salt composed of cerium in the +4 oxidation state coordinated to sulfate anions. It is a strong inorganic oxidant found in hydrated crystalline forms used in redox chemistry and analytical procedures. The compound sits at the intersection of lanthanide coordination chemistry, industrial oxidation processes, and classical wet-chemical analysis.
Cerium(IV) sulfate exhibits strong oxidizing behavior characteristic of tetravalent lanthanide salts, with redox potentials comparable to reagents used historically in classical titrimetry and in synthetic oxidative transformations; this reactivity parallels that of reagents familiar to practitioners at institutions such as University of Cambridge, Massachusetts Institute of Technology, Max Planck Society, California Institute of Technology, and Stanford University. The salt exists in multiple hydrated states whose acid–base equilibria and hydrolysis behavior are affected by media familiar from work at Brookhaven National Laboratory, Lawrence Berkeley National Laboratory, Argonne National Laboratory, Oak Ridge National Laboratory, and Los Alamos National Laboratory. In aqueous solution, Ce(IV) can undergo redox cycling with Ce(III), a property exploited in methods developed at Harvard University, Yale University, Princeton University, Columbia University, and University of Chicago. Coordination to sulfate produces inner-sphere and outer-sphere complexes analyzed in studies associated with Royal Society of Chemistry, American Chemical Society, Deutsche Forschungsgemeinschaft, National Science Foundation, and European Research Council.
Typical laboratory preparation routes mirror those reported in method collections maintained at National Institute of Standards and Technology, American Society for Testing and Materials, Royal Society, Institut Pasteur, and CNRS repositories: oxidation of cerium(III) salts with strong oxidants followed by sulfate metathesis. Industrial and academic syntheses use oxidants and acids traced in literature from BASF, Dow Chemical Company, DuPont, Johnson Matthey, and AkzoNobel-type processes. Electrochemical oxidation of Ce(III) sulfate at boron-doped diamond or platinum electrodes, techniques refined at Imperial College London, ETH Zurich, Tokyo Institute of Technology, Seoul National University, and Tsinghua University, gives Ce(IV) sulfate under controlled potential. Crystallization from sulfuric acid has been optimized in workflows reported by research groups at University of Oxford, University of Melbourne, McGill University, Peking University, and University of Toronto.
The solid-state arrangements of Ce(IV) sulfate are built from CeO8-type polyhedra and sulfate tetrahedra, motifs that echo coordination paradigms investigated at Bell Labs, Rutherford Appleton Laboratory, CERN, National Renewable Energy Laboratory, and Scripps Research. Ce–O bond metrics and sulfate bridging patterns are resolved by single-crystal X-ray diffraction and neutron studies carried out at facilities like Diamond Light Source, European Synchrotron Radiation Facility, ISIS Neutron and Muon Source, Advanced Photon Source, and Spallation Neutron Source. Bonding combines predominantly ionic character with covalent contributions from 4f–O interactions, a theme central to discussions at Los Alamos National Laboratory, Argonne National Laboratory, Oak Ridge National Laboratory, Lawrence Livermore National Laboratory, and Brookhaven National Laboratory. Hydration leads to hydrogen-bonded networks analogous to structures cataloged by International Union of Crystallography, Cambridge Crystallographic Data Centre, American Crystallographic Association, European Crystallographic Committee, and Japanese Society of Coordination Chemistry.
Hydrated cerium(IV) sulfate typically appears as yellow to yellow-green crystals whose color and solubility vary with hydration and acid concentration, observations reported by laboratories at University of California, Berkeley, University of Illinois Urbana-Champaign, University of Wisconsin–Madison, Utrecht University, and KU Leuven. The compound decomposes on heating to release oxygen and form lower-valent cerium oxides (CeO2, Ce2O3), pathways characterized in thermal analyses undertaken at National Institute for Materials Science, Fraunhofer Society, Paul Scherrer Institute, Korean Advanced Institute of Science and Technology, and Indian Institute of Science. Magnetic susceptibility and spectroscopic fingerprints (UV–Vis, Raman, infrared) arise from Ce(IV) electronic structure and sulfate vibrations, data compiled by groups at Swiss Federal Institute of Technology Lausanne, Wuhan University, University of Barcelona, University of São Paulo, and University of Copenhagen.
Cerium(IV) sulfate is applied as an oxidant in organic and inorganic syntheses, electrochemical studies, and classical volumetric analyses such as cerimetry, usages documented in manuals produced by Sigma-Aldrich, Merck Group, Fisher Scientific, VWR International, and Tokyo Chemical Industry. It serves as a precursor in preparation of cerium oxide catalysts and materials used in automotive catalysis and solid-oxide fuel cells, domains advanced by Toyota Motor Corporation, General Motors, Bosch, Shell, and Hitachi. In analytical chemistry it functions in redox titrations and as a reagent in oxidative digestion protocols applied in laboratories at Food and Drug Administration, Environmental Protection Agency, World Health Organization, Centers for Disease Control and Prevention, and European Medicines Agency.
As a strong oxidizer and an acidic salt, cerium(IV) sulfate requires handling practices consistent with guidance from Occupational Safety and Health Administration, National Institute for Occupational Safety and Health, European Chemicals Agency, Health and Safety Executive, and Safe Work Australia. Protective measures align with protocols published by American Chemical Society Committee on Chemical Safety, International Labour Organization, United Nations Environment Programme, World Health Organization, and Red Cross training materials. Storage must avoid reducing agents and organic combustibles; spill and waste management follow procedures used by Johnson & Johnson, Pfizer, GlaxoSmithKline, Novartis, and Roche industrial safety departments.
Quantitative determination of Ce(IV) sulfate and its redox activity employs titrimetry against ferrous standards and spectrophotometric assays calibrated with standards traceable to National Institute of Standards and Technology, International Organization for Standardization, American National Standards Institute, European Committee for Standardization, and Japanese Industrial Standards. Kinetic and mechanistic studies of Ce(IV)-mediated oxidations, including one-electron and two-electron pathways, are examined in research originating from Stanford University School of Engineering, Massachusetts General Hospital, Max Planck Institute for Coal Research, Weizmann Institute of Science, and Salk Institute for Biological Studies. Complexation and speciation analyses use ion chromatography, mass spectrometry, and synchrotron techniques maintained at Thermo Fisher Scientific, Agilent Technologies, Bruker Corporation, Shimadzu Corporation, and Waters Corporation.
Category:Cerium compounds