Effects of pH and phosphate on CeO2 nanoparticle dissolution

Chemosphere

Volumn 119, Issue , 2015, Pages 1365-1371

  Dahle, Jessica T ^a   Livi, Ken ^b   Arai, Yuji ^c  

^a CLEMSON UNIVERSITY   (United States)

^b JOHNS HOPKINS UNIVERSITY   (United States)

^c UNIVERSITY OF ILLINOIS AT URBANA CHAMPAIGN   (United States)

Author keywords

CeO2; Cerium nanoparticle; Cerium oxide; Dissolution; Nanoparticle; Phosphate sorption

Indexed keywords

DISSOLUTION; HEALTH RISKS; NANOPARTICLES; PARTICLE SIZE; SOLUBILITY;

AQUATIC ENVIRONMENTS; CEO2; CEO2 NANOPARTICLES; ENGINEERED NANOPARTICLES; FATE AND TRANSPORT; NANOTECHNOLOGY INDUSTRY; PHOSPHATE SORPTION; ZETA POTENTIAL MEASUREMENTS;

CERIUM OXIDE;

CERIUM OXIDE; LIGAND; NANOPARTICLE; PHOSPHATE; CERIC OXIDE; CERIUM; METAL NANOPARTICLE; POLLUTANT;

AQUATIC ENVIRONMENT; DISSOLUTION; ENVIRONMENTAL FATE; ION EXCHANGE; NANOTECHNOLOGY; PH; PHOSPHATE; POLLUTANT TRANSPORT; SORPTION;

ADSORPTION; AQUATIC ENVIRONMENT; ARTICLE; ATOMIC EMISSION SPECTROMETRY; COMPLEX FORMATION; DISSOLUTION; NANOTECHNOLOGY; PARTICLE SIZE; PH; SOLUBILITY; SURFACE PROPERTY; TRANSMISSION ELECTRON MICROSCOPY; ZETA POTENTIAL; CHEMISTRY; DRUG EFFECTS; FOURIER ANALYSIS; POLLUTANT; TIME; ULTRASTRUCTURE;

ADSORPTION; CERIUM; ENVIRONMENTAL POLLUTANTS; FOURIER ANALYSIS; HYDROGEN-ION CONCENTRATION; METAL NANOPARTICLES; MICROSCOPY, ELECTRON, TRANSMISSION; PARTICLE SIZE; PHOSPHATES; SOLUBILITY; TIME FACTORS;

EID: 84919776285     PISSN: 00456535     EISSN: 18791298     Source Type: Journal    
DOI: 10.1016/j.chemosphere.2014.02.027     Document Type: Article

References (39)

1. 2 catalyst used for total oxidation of toluene. Int. J. Chem. React. Eng. 2011, 9:A45.
2. Abreu R.D., Morais C.A. Purification of rare earth elements from monazite sulphuric acid leach liquor and the production of high-purity ceric oxide. Miner. Eng. 2010, 23:536-540.
3. Agrawal A., Sekhar K.C., Pandey L.P. Spectrophotometric determination of Ce(IV) using O-Phenylenediamine Lenediamine in steels. Bull. Mater. Sci. 1994, 17:1467-1471.
4. Berg J.M., Romoser A., Banerjee N., Zebda R., Sayes C.M. The relationship between pH and zeta potential of similar to 30 nm metal oxide nanoparticle suspensions relevant to in vitro toxicological evaluations. Nanotoxicology 2009, 3:276-283.
5. Biber M.V., Afonso M.D., Stumm W. The Coordination chemistry of weathering. 4. Inhibition of the dissolution of oxide minerals. Geochim. Cosmochim. Ac 1994, 58:1999-2010.
6. Bjerrum J., Sillen L.G. Stability Constants of Metal Complexes, Part II, The Chemical Society 1958, Burlington House, London.
7. Clever H.L., Johnston F.J. J. Phys. Chem. Ref. Data 1980, 9:751.
8. Clever H.L., Johnson S.A., Derrick M.E. Stability Constants of Metal Complexes, Part II, 14, The Chemical Society 1985, Burlington House, London.
9. Clever H.L., Johnson S.A., Derrick M.E. Stability Constants of Metal Complexes, Part II, 21, The Chemical Society 1992, Burlington House, London.
10. 2 nanoparticles in soils. Environ. Sci. Technol. 2011, 45:2777-2782.
11. De S.K. Adsorption of phosphate ion by hydrous ferric, chromic, and aluminium oxides. Part I With inorganic materials added. Kolloid-Zeitschrift 1961, 179:134-140.
12. 2. J. Colloid Interf. Sci. 1994, 167(2):352-357.
13. 2, ZnO, Ag, CNT, Fullerenes) for different regions. Environ. Sci. Technol. 2009, 43:9216-9222.
14. Gustaffson J.P. VisualMinteq, division of land and water resources 2007, Royal Institute of Technology, Stockholm, SWE.
15. He Z.L., Baligar V.C., Martens D.C., Ritchey K.D. Determination of soluble phosphorus in the presence of organic ligands or fluoride. Soil Sci. Soc. Am. J. 1998, 62:1538-1541.
16. Hedrick, J. B., 2004. Rare Earths. Minerals Yearbook. vol 1. Metals and Minerals U.S. Geological Survey, US Department of the Interior, Reston, VA.
17. Hedrick J.B., Sinha S.P. Cerium-based polishing compounds-discovery to manufacture. J. Alloys Comp. 1994, 207:377-382.
18. Hsu P.H., Rennie D.A. Reactions of phosphate in aluminium systems. Part I. Adsorption of phosphate by X-ray amorphous aluminium hydroxide. Can. J. Soil Sci. 1962, 42:197-209.
19. 2 nanoparticles. Nanotechnology 2006, 17:5983-5987.
20. Hunter R.J. Zeta Potential in Colloid Science: Principles and Applications 1988, Academic Press, New York.
21. IUPAC. Solubility Data Project: Solubility Data Series. International Union of Pure and Applied Chemistry. Pergamon Press, Oxford, 1979-1992.
22. Jakupec M.A., Unfried P., Keppler B.K. Pharmacological properties of cerium compounds. Reviews of Physiology Biochemistry and Pharmacology 2005, 101-111. Springer Berlin Heidelberg. S.G. Amara, E. Bamberg, R. Jahn, W.J. Lederer, A. Miyajima, H. Murer, S. Offermanns, G. Schultz, G. Schweiger (Eds.).
23. Kilbourn B. Cerium and Cerium Compounds. Kirk-Othmer Encyclopedia of Chemical Technology 2003, John Wiley and Sons Inc., New York (NY).
24. Limbach L.K., Bereiter R., Mueller E., Krebs R., Gaelli R., Stark W.J. Removal of oxide nanoparticles in a model wastewater treatment plant: Influence of agglomeration and surfactants on clearing efficiency. Environ. Sci. Technol. 2008, 42:5828-5833.
25. Marcus Y. J. Phys. Chem. Ref. Data 9 1980, AIP Publishing LLC, Melville, NY.
26. Muljadi D., Posner A.M., Quirk J.P. The mechanisms of phosphate adsorption: adsorption by kaolinite, gibbsite and pseudoboehmite. J. Soil Sci 1966, 17.
27. Ogata F., Tominaga H., Yabutani H., Kawasaki N. Phosphate adsorption ability of granular gibbsite and cerium hydroxide. J. Oleo Sci. 2011, 60:133-138.
28. Patil S., Kuiry S.C., Seal S., Vanfleet R. Synthesis of nanocrys-talline ceria particles for high temperature oxidation resistant coating. J. Nanopart. Res. 2002, 4:433-438.
29. Patnaik P. Handbook of Inorganic Chemicals 2003, McGraw-Hill.
30. Pelletier D.A., Suresh A.K., Holton G.A., McKeown C., Wang W., Gu B., Mortensen N.P., Allison D.P., Joy D.C., Allison M.R., Brown S.D., Phelps T.J., Doktycz M.J. Effects of engineered cerium oxide nanoparticles on bacterial growth and viability. Appl. Environ. Microbiol. 2010, 76(24):7981-7989.
31. Rakicioglu Y., Akseli A. New fluorimetric reagents, sodium pyrophosphate, sodium trimetaphosphate, and sodium tetrametaphosphate, for the determination of cerium(III). J. Fluoresc. 1998, 8:45-52.
32. Recillas S., García A., González E., Casals E., Puntes V., Sánchez A., Font X. Preliminary study of phosphate adsorption onto cerium oxide nanoparticles for use in water purification; nanoparticles synthesis and characterization. Water Sci. Technol. 2012, 66:503-509.
33. Rubasinghege G., Kye P.K., Scherer M.M., Grassian V.H. Proton-promoted dissolution of α-FeOOH nanorods and microrods: size dependence, anion effects (carbonate and phosphate), aggregation and surface adsorption. J. Colloid Interface. Sci. 2012, 385:15-23.
34. Schwertmann U. Solubility and dissolution of iron-oxides. Plant Soil 1991, 130:1-25.
35. Sposito G. Surface Chemistry of Soils 1984, Oxford University Press, New York.
36. Stumm W. Reactivity at the mineral-water interface: dissolution and inhibition. Colloid Surfaces A 1997, 120:143-166.
37. Torrent J., Barron V., Schwertmann U. Phosphate adsorption and desorption by goethite differing in crystal morphology. Soil Sci. Soc. Am. J. 1990, 54:1007-1012.
38. van Loef E.V.D., Dorenbos P., van Eijk C.W.E., Kramer K., Gudel H.U. High-energy-resolution scintillator: Ce(3+) activated LaBr(3). Appl. Phys. Lett. 2001, 79:1573-1575.
39. Winkler H., Reinhardt K. Cerium Mischmetal, Cerium Alloys, and Cerium Compounds. Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim, Germany, pp. 285-300.