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EC number: 239-018-0 | CAS number: 14940-41-1
- Life Cycle description
- Uses advised against
- Endpoint summary
- Appearance / physical state / colour
- Melting point / freezing point
- Boiling point
- Density
- Particle size distribution (Granulometry)
- Vapour pressure
- Partition coefficient
- Water solubility
- Solubility in organic solvents / fat solubility
- Surface tension
- Flash point
- Auto flammability
- Flammability
- Explosiveness
- Oxidising properties
- Oxidation reduction potential
- Stability in organic solvents and identity of relevant degradation products
- Storage stability and reactivity towards container material
- Stability: thermal, sunlight, metals
- pH
- Dissociation constant
- Viscosity
- Additional physico-chemical information
- Additional physico-chemical properties of nanomaterials
- Nanomaterial agglomeration / aggregation
- Nanomaterial crystalline phase
- Nanomaterial crystallite and grain size
- Nanomaterial aspect ratio / shape
- Nanomaterial specific surface area
- Nanomaterial Zeta potential
- Nanomaterial surface chemistry
- Nanomaterial dustiness
- Nanomaterial porosity
- Nanomaterial pour density
- Nanomaterial photocatalytic activity
- Nanomaterial radical formation potential
- Nanomaterial catalytic activity
- Endpoint summary
- Stability
- Biodegradation
- Bioaccumulation
- Transport and distribution
- Environmental data
- Additional information on environmental fate and behaviour
- Ecotoxicological Summary
- Aquatic toxicity
- Endpoint summary
- Short-term toxicity to fish
- Long-term toxicity to fish
- Short-term toxicity to aquatic invertebrates
- Long-term toxicity to aquatic invertebrates
- Toxicity to aquatic algae and cyanobacteria
- Toxicity to aquatic plants other than algae
- Toxicity to microorganisms
- Endocrine disrupter testing in aquatic vertebrates – in vivo
- Toxicity to other aquatic organisms
- Sediment toxicity
- Terrestrial toxicity
- Biological effects monitoring
- Biotransformation and kinetics
- Additional ecotoxological information
- Toxicological Summary
- Toxicokinetics, metabolism and distribution
- Acute Toxicity
- Irritation / corrosion
- Sensitisation
- Repeated dose toxicity
- Genetic toxicity
- Carcinogenicity
- Toxicity to reproduction
- Specific investigations
- Exposure related observations in humans
- Toxic effects on livestock and pets
- Additional toxicological data
Endpoint summary
Administrative data
Description of key information
Additional information
Triiron bis(orthophosphate) (CAS 14940-41-1) is an inorganic phosphate substance. Biotic degradation is therefore not relevant for the substance. Furthermore abiotic degradation processes like photolysis in air, water and soil are not likely. In water, soil and biological systems, dissolved Triiron bis(orthophosphate) dissociates to orthophosphate and ferrous ion (Fe2+).
“Redox transformation of iron, as well as dissolution and precipitation and thus mobilization and redistribution, are caused by chemical and to a significant extent by microbial processes (see attachment Fig. 1) (Kappler A. and Straub K. L. 2005).”
Transformations of iron by microorganisms are often much faster than the respective chemical reactions. They occur in most soils and sediments, both in freshwater and marine environments (Thamdrup 2000; Straub et al. 2001; Cornell and Schwertmann 2003).
The iron transport and distribution depend on pH, Eh (redox) and the presence or absence of other dissolved constituents which form with FE(II) or FE(III) dissolved complexes, colloids or poorly soluble mineral phases (Boyd and Ellwood 2010; Konhauser et al. 2011a; Radic et al. 2011; Raiswell 2011). With increasing Eh and pH the amount if iron dissolved in groundwaters, rivers and seawater decreases (see attachment Fig. 2) (Kendall 2012).
Ferric iron (Fe3+) is the stable form in oxygenated waters, which forms at neutral pH highly insoluble oxides and hydroxides (Wang 1998; Simpson 2002; Zhang 1999). In anoxic waters ferrous iron (Fe2+) is stable. As dissolved ion it occurs usually in many freshwater systems. Insoluble salts will be formed in the presences of high carbonate, sulphide and orthophosphate levels (Stumm, W. and Morgan, J. J. 1981).
Orthophosphate is available for biological metabolism without further breakdown. Besides of chemical precipitation phosphate can be biologically removed from waste water. Biological phosphate removal process is relies upon microorganisms to uptake phosphate into their cells either via anaerobic or anaerobic pathways, which is subsequently removed from the STP process as a result of sludge wasting.
References:
Boyd PW, Ellwood MJ (2010) The biogeochemical cycle of iron in the ocean. Nature Geoscience 3, 675–682.
Cornell R. M. and Schwertmann U. (2003).The iron Oxides: Structures, Properties, Reactions, Occurrences and Uses. Wiley-VCH, Weinheim
Kappler A. and Straub K.L. (2005). Geomicrobiological Cycling of Iron. Reviews in Mineralogy & Geochemistry, Vol. 59, pp 85-108
Konhauser KO, Kappler A, Roden EE (2011) Iron in microbial metabolisms. Elements 7, 89–93.
Kendall B., Anbar A.D., Kappler A. and Konhauser K.O. (2012). The global iron cycle. In book: Fundamentals of Geobiology, Blackwell Publishing Ltd., chapter 6, 65-92
Radic A, Lacan F, Murray JW (2011) Iron isotopes in the seawater of the equatorial Pacific Ocean: new constraints for the oceanic iron cycle. Earth and Planetary Science Letters 306, 1–10.
Raiswell R (2011) Iron transport from the continents to the open ocean: the aging-rejuvenation cycle. Elements 7, 101–106.
Simpson, S.L., Rochford, L. and Birch, G.F. (2002) Geochemical influences on metal partitioning in contaminated estuarine sediments. Marine and Freshwater Research, 53, 9-17 (cited in: Xing W. and Liu G. (2011))
Straub K. L., Benz M., Schink B. (2001).Iron metabolism in anoxic environments at near neutral pH. FEMS Microbiol Ecol 34: 181-186
Stumm, W. and Morgan, J. J. (1981). Aquatic Chemistry. Wiley: New York
Thamdrup B. (2000). Bacterial manganese and iron reduction in aquatic sediments. In: Advances in microbial ecology. Schink B. (ed) Kluwer Academic/ Plenum Publishers, New York, p 41-84
Wang, S.M. and Dou, H.S. (1998). Chinese Lake Notes. Science, Press: Beijing. (In Chinese) (cited in: Xing W. and Liu G. (2011))
Xing W. and Liu G. (2011) IRON BIOGEOCHEMISTRY AND IST ENVIRONMENTAL IMPACTS IN FRESHWATER LAKES. Fresenius Environmental Bulletin, Vol 20, No. 6, 1339-1345.
Zhang, X.H. (1999) Iron cycle and transformation in drinking water source. Water and wastewater, 25, 18-22. (In Chinese) (cited in: Xing W. and Liu G. (2011))
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