Ferric phosphate

• CAT Number: M120592
• CAS Number: 10045-86-0
• Molecular Formula: FePO4
• Molecular Weight: 150.82
• Purity: ≥95%
• Synonyms: Iron(III) phosphate; Iron orthophosphate.
• Storage: Room Temperature
• IUPAC Name: iron(3+);phosphate
• InChI: InChI=1S/Fe.H3O4P/c;1-5(2,3)4/h;(H3,1,2,3,4)/q+3;/p-3
• InChIKey: WBJZTOZJJYAKHQ-UHFFFAOYSA-K
• SMILES: [O-]P(=O)([O-])[O-].[Fe+3]

Iron phosphate (Cat No.:M120592), also known as iron orthophosphate, has a wide range of applications, including catalysts, additives, and electrode materials. As a catalyst, nanoscale iron phosphate can be used as a catalyst, which has remarkable effect in dehydrogenation and oxidation, and can realize selective oxidation catalysis, showing its potential application in the field of organic synthesis. As an additive, iron phosphate can be used as cement additive and iron strengthening agent, especially for bread and feed additive.

Reference

[1]. Bioresour Technol. 2021 Mar;323:124622. doi: 10.1016/j.biortech.2020.124622. Epub 2020 Dec 28.
Effects of ferric-phosphate forms on phosphorus release and the performance of anaerobic fermentation of waste activated sludge.
Zhang Z(1), Ping Q(1), Gao D(1), Vanrolleghem PA(2), Li Y(3).
Author information: (1)State Key Laboratory of Pollution Control and Resource Reuse, College of Environmental Science and Engineering, Tongji University, Shanghai 200092, China. (2)Modeleau, Département de génie civil et de génie des eaux, Université Laval, 1065 av. de la Médecine, Québec, QC G1V 0A6, Canada. (3)State Key Laboratory of Pollution Control and Resource Reuse, College of Environmental Science and Engineering, Tongji University, Shanghai 200092, China; Shanghai Institute of Pollution Control and Ecological Security, Shanghai 200092, China. Electronic address: .
Five ferric-phosphate (Fe(III)Ps) with amorphous or crystalline structures were added to waste activated sludge (WAS) for anaerobic fermentation, aiming to investigate effects of Fe(III)Ps forms on phosphorus (P) release and the performance of WAS fermentation. The results revealed that the Fe(III) reduction rate of hexagonal-FePO4 was faster than that of monoclinic-FePO4·2H2O, thanks to its lower crystal field stabilization energy. FePO4·nH2O was reduced to vivianite and part of the phosphate was released as orthophosphate (PO4-P). Giniite (Fe5(PO4)4(OH)3·2H2O) as an iron hydroxyphosphate was transformed to βFe(III)Fe(II)(PO4)O-like compounds without PO4-P release. In addition, Fe(III)Ps had an adverse effect on the anaerobic fermentation of WAS. The specific hydrolysis rate constant and volatile fatty acids (VFAs) yield decreased by 38.4% and 41.9%, respectively, for the sludge sample with amorphous-FePO4·3H2O, which dropped the most. This study provides new insights into various forms of Fe(III)Ps performance during anaerobic fermentation and is beneficial to enhancing P recovery efficiency.
DOI: 10.1016/j.biortech.2020.124622 PMID: 33421830 [Indexed for MEDLINE]

[2]. ChemistryOpen. 2015 Jun;4(3):274-7. doi: 10.1002/open.201402112. Epub 2015 Jan 12.
Ferric Phosphate Hydroxide Microstructures Affect Their Magnetic Properties.
Zhao J(1), Zhang Y(1), Run Z(1), Li P(1), Guo Q(1), Pang H(2).
Author information: (1)College of Chemistry and Chemical Engineering, Anyang Normal University Anyang, Henan, 455002, P. R. China. (2)College of Chemistry and Chemical Engineering, Anyang Normal University Anyang, Henan, 455002, P. R. China ; State Key Laboratory of Coordination Chemistry, Nanjing University Nanjing, Jiangsu, 210093, P. R. China.
Uniformly sized and shape-controlled nanoparticles are important due to their applications in catalysis, electrochemistry, ion exchange, molecular adsorption, and electronics. Several ferric phosphate hydroxide (Fe4(OH)3(PO4)3) microstructures were successfully prepared under hydrothermal conditions. Using controlled variations in the reaction conditions, such as reaction time, temperature, and amount of hexadecyltrimethylammonium bromide (CTAB), the crystals can be grown as almost perfect hyperbranched microcrystals at 180 °C (without CTAB) or relatively monodisperse particles at 220 °C (with CTAB). The large hyperbranched structure of Fe4(OH)3(PO4)3 with a size of ∼19 μm forms with the "fractal growth rule" and shows many branches. More importantly, the magnetic properties of these materials are directly correlated to their size and micro/nanostructure morphology. Interestingly, the blocking temperature (T B) shows a dependence on size and shape, and a smaller size resulted in a lower T B. These crystals are good examples that prove that physical and chemical properties of nano/microstructured materials are related to their structures, and the precise control of the morphology of such functional materials could allow for the control of their performance.
DOI: 10.1002/open.201402112 PMCID: PMC4522176 PMID: 26246988

[3]. Chemosphere. 2019 May;223:551-559. doi: 10.1016/j.chemosphere.2019.02.070. Epub 2019 Feb 15.
Simultaneous adsorption of As(III), Cd(II) and Pb(II) by hybrid bio-nanocomposites of nano hydroxy ferric phosphate and hydroxy ferric sulfate particles coating on Aspergillus niger.
Liao Q(1), Tu G(2), Yang Z(1), Wang H(3), He L(2), Tang J(2), Yang W(4).
Author information: (1)Institute of Environmental Science and Engineering, School of Metallurgy and Environment, Central South University, 410083, Changsha, China; National Engineering Research Center for Heavy Metals Pollution Control and Treatment, 410083, Changsha, China. (2)Institute of Environmental Science and Engineering, School of Metallurgy and Environment, Central South University, 410083, Changsha, China. (3)Institute of Environmental Science and Engineering, School of Metallurgy and Environment, Central South University, 410083, Changsha, China; National Engineering Research Center for Heavy Metals Pollution Control and Treatment, 410083, Changsha, China; Water Pollution Control Technology Key Lab of Hunan Province, 410083, Changsha, China. (4)Institute of Environmental Science and Engineering, School of Metallurgy and Environment, Central South University, 410083, Changsha, China; National Engineering Research Center for Heavy Metals Pollution Control and Treatment, 410083, Changsha, China; Water Pollution Control Technology Key Lab of Hunan Province, 410083, Changsha, China. Electronic address: .
To develop an efficient, convenient and cost-effective method to simultaneously remove pollution of As(III), Cd(II) and Pb(II) in wastewater, a strategy to fabricate hybrid bio-nanocomposites ((n-HFP + n-HFS)@An) of nano hydroxy ferric phosphate (n-HFP) and hydroxy ferric sulfate (n-HFS) particles coating on Aspergillus niger was applied. The scanning electron microscope and energy dispersive spectrum analyses showed that (n-HFP + n-HFS)@An composites had been successfully developed which well solved the self-agglomeration problem of the nano particles. Comparing to the bulk nanoparticles, the adsorption rates of the (n-HFP + n-HFS)@An composites for the three metals were promoted 145.34, 28.98 and 25.18% and reached 76.84, 73.62 and 94.31%, respectively. Similarly, the adsorption capacities for As(III), Cd(II), and Pb(II) were 162.00, 205.83 and 730.79 mg/g, respectively. Moreover, the pseudo-second-order kinetic model was more relevant to the adsorption on the three metals by (n-HFP + n-HFS)@An, and adsorbing As(III) was fitted to the Freundlich isotherm model, while the adsorption on Cd(II) or Pb(II) was related to the Langmuir isotherm model. In addition, the adsorption of Cd(II) and Pb(II) was associated with transformation of hydroxyl groups and precipitation with phosphate. As(III) was adsorbed through exchange between AsO2- and SO42- in the (n-HFP + n-HFS)@An composites.
DOI: 10.1016/j.chemosphere.2019.02.070 PMID: 30797164 [Indexed for MEDLINE]

[4]. Nutrients. 2017 Apr 4;9(4):359. doi: 10.3390/nu9040359.
Mechanisms of Iron Uptake from Ferric Phosphate Nanoparticles in Human Intestinal Caco-2 Cells.
Perfecto A(1), Elgy C(2), Valsami-Jones E(3), Sharp P(4), Hilty F(5), Fairweather-Tait S(6).
Author information: (1)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . . (2)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . . (3)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . . (4)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . . (5)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . . (6)1Norwich Medical School, University of East Anglia, Norwich, Norfolk NR4 7UQ, UK; of Geography, Earth and Environmental Sciences, University of Birmingham, Edgbaston, Birmingham B15 2TT, UK; (C.E.); (E.V.-J.)3Diabetes and Nutritional Sciences Division, King's College London, London SE1 9NH, UK; of Food, Nutrition, and Health, ETH, Schmelzbergstrasse 9, 8092 Zürich, Switzerland; . .
Food fortification programs to reduce iron deficiency anemia require bioavailable forms of iron that do not cause adverse organoleptic effects. Rodent studies show that nano-sized ferric phosphate (NP-FePO4) is as bioavailable as ferrous sulfate, but there is controversy over the mechanism of absorption. We undertook in vitro studies to examine this using a Caco-2 cell model and simulated gastrointestinal (GI) digestion. Supernatant iron concentrations increased inversely with pH, and iron uptake into Caco-2 cells was 2-3 fold higher when NP-FePO4 was digested at pH 1 compared to pH 2. The size and distribution of NP-FePO4 particles during GI digestion was examined using transmission electron microscopy. The d50 of the particle distribution was 413 nm. Using disc centrifugal sedimentation, a high degree of agglomeration in NP-FePO4 following simulated GI digestion was observed, with only 20% of the particles ≤1000 nm. In Caco-2 cells, divalent metal transporter-1 (DMT1) and endocytosis inhibitors demonstrated that NP-FePO4 was mainly absorbed via DMT1. Small particles may be absorbed by clathrin-mediated endocytosis and micropinocytosis. These findings should be considered when assessing the potential of iron nanoparticles for food fortification.
DOI: 10.3390/nu9040359 PMCID: PMC5409698 PMID: 28375175 [Indexed for MEDLINE]

[5]. J Inorg Biochem. 2017 Mar;168:107-113. doi: 10.1016/j.jinorgbio.2016.12.010. Epub 2016 Dec 11.
Citrate and albumin facilitate transferrin iron loading in the presence of phosphate.
Matias C(1), Belnap DW(1), Smith MT(1), Stewart MG(1), Torres IF(1), Gross AJ(2), Watt RK(3).
Author information: (1)Department of Chemistry and Biochemistry, Brigham Young University, Provo, UT 84602, United States; College of Dental Medicine, Roseman University of Health Sciences, South Jordan, UT 84095, United States. (2)Department of Chemistry and Biochemistry, Brigham Young University, Provo, UT 84602, United States; College of Dental Medicine, Roseman University of Health Sciences, South Jordan, UT 84095, United States. Electronic address: . (3)Department of Chemistry and Biochemistry, Brigham Young University, Provo, UT 84602, United States; College of Dental Medicine, Roseman University of Health Sciences, South Jordan, UT 84095, United States. Electronic address: .
Labile plasma iron (LPI) is redox active, exchangeable iron that catalyzes the formation of reactive oxygen species. Serum transferrin binds iron in a non-exchangeable form and delivers iron to cells. In several inflammatory diseases serum LPI increases but the reason LPI forms is unknown. This work evaluates possible pathways leading to LPI and examines potential mediators of apo transferrin iron loading to prevent LPI. Previously phosphate was shown to inhibit iron loading into apo transferrin by competitively binding free Fe3+. The reaction of Fe3+ with phosphate produced a soluble ferric phosphate complex. In this study we evaluate iron loading into transferrin under physiologically relevant phosphate conditions to evaluate the roles of citrate and albumin in mediating iron delivery into apo transferrin. We report that preformed Fe3+-citrate was loaded into apo transferrin and was not inhibited by phosphate. A competition study evaluated reactions when Fe3+ was added to a solution with citrate, phosphate and apo transferrin. The results showed citrate marginally improved the delivery of Fe3+ to apo transferrin. Studies adding Fe3+ to a solution with phosphate, albumin and apo transferrin showed that albumin improved Fe3+ loading into apo transferrin. The most efficient Fe3+ loading into apo transferrin in a phosphate solution occurred when both citrate and albumin were present at physiological concentrations. Citrate and albumin overcame phosphate inhibition and loaded apo transferrin equal to the control of Fe3+ added to apo transferrin. Our results suggest a physiologically important role for albumin and citrate for apo transferrin iron loading.
DOI: 10.1016/j.jinorgbio.2016.12.010 PMID: 28110161 [Indexed for MEDLINE]