15275-07-7

Basic information

• Product Name: Fe(III)-EDTA
• Synonyms: ethylenediaminetetraacetatoferrate(1-)
• CAS NO: 15275-07-7
• Molecular Formula: C10H12FeN2O8-
• Molecular Weight: 344.05588
• EINECS: 241-171-3
• Mol File: 15275-07-7.mol
• Article Data: 8

Chemical Properties

• Boiling Point: 614.2 °C at 760 mmHg
• Flash Point: 325.2 °C
• Appearance: /
• Vapor Pressure: 1.15E-16mmHg at 25°C
• CAS DataBase Reference: Fe(III)-EDTA(CAS DataBase Reference)
• NIST Chemistry Reference: Fe(III)-EDTA(15275-07-7)
• EPA Substance Registry System: Fe(III)-EDTA(15275-07-7)

Safety Data

• Hazardous Substances Data: 15275-07-7(Hazardous Substances Data)

Usage

Hazard

A poison.

InChI:InChI=1/C10H16N2O8.Fe/c13-7(14)3-11(4-8(15)16)1-2-12(5-9(17)18)6-10(19)20;/h1-6H2,(H,13,14)(H,15,16)(H,17,18)(H,19,20);/q;+3/p-4

Upstream product

• 64-02-8 disodium ethylenediamine tetraacetic acid 
• 15651-72-6 iron(II) ethylenediaminetetraacetic acid 
• 60-00-4 ethylenediaminetetraacetic acid 
• 94706-21-5 iron N-{2-((o-hydroxyphenyl)glycino)-ethyl}salicylideneamine 
• 150-43-6 ethylenediaminetetraacetate 
• 13479-49-7 tris(1,10-phenanthroline)iron(III) 
• 32446-51-8 Dipotassium EDTA 
• 64-02-8 ethylene diamine tetraacetic acid tetrasodium salt 
• 1120563-88-3 {Fe(ethylenediaminetetraacatate)(H₂O)}^(2-) 

Downstream Products

• 16043-45-1 titanium(IV) 
• 7439-89-6 iron(II) 

Relevant articles and documents

Coordination Chemistry of Microbial Iron Transport Compounds. 21. Kinetics and Mechanism of Iron Exchange in Hydroxamate Siderophore Complexes

The kinetics of iron exchange and iron removal from two siderophore complexes have been examined, using 55Fe labeling techniques and UV-vis spectrophotometric methods, respectively.Iron exchange between the ferric complexes of ferrioxamine B (FeHDFO+) and ferrichrome A (FeDFC3-), two trihydroxamate siderophores from microbial cultures, is extremely slow; under conditions where there is a 5percent excess of H4DFO+ per FeHDFO+, the half-time for exchange for equimolar concentrations (4.0 mM) of the two complexes at 25 deg C and pH 7.4 is approximately 220 h.The kinetic reveal an apparent first-order dependence of the rate on each of the competing metal complexes, with the exchange proceeding through a chain reaction involving free ligand.Furthermore, pH dependence studies demonstrate that the exchange rate is accelerated as a function of increasing hydrogen ion concentration.Kinetics of iron removal from ferrioxamine B with use of ethylenediaminetetraacetic acid (EDTA) show first-order dependence on the concentrations of the iron complex and hydrogen ion at 25 deg C, with a pseudo-first-order rate constant of 4.8*10-5 s-1 at pH 5.4.Variation of the initial rate with EDTA concentration shows saturation kinetics at high ligand concentrations.The results are interpreted in terms of a two-step mechanism involving: (1) protonation of the ferrioxamine B complex and (2) subsequent bimolecular reaction with EDTA.Results of kinetic studies of the reverse process are consistent with the known equilibrium constants and microscopic reversibility.The reaction is first-order in the FeEDTA complex and desferrioxamine B.Although essentially no pH dependence is observed for this reverse process between pH 4 and 6, the reaction rate varies inversely with hydrogen ion concentration above pH 6.This is explained by consideration of the acid-base equilibria associated with the reactants, which give rise to multiple pathway for product formation.Specifically, the deprotonated form of the ferric-EDTA complex, Fe(OH)EDTA2-, displays faster reaction kinetics with desferrioxamine B than does its conjugate acid form.A comparison of observed rate constants for the forward and reverse processes with known equilibrium constants shows good agreement.The postulated mechanisms for siderophore mediated microbial iron transport are evaluared in terms of the rates of iron exchange observed in these experiments.

Influence of the polyamino carboxylate chelating ligand (L) on the kinetics and mechanism of the formation of FeII(L)NO in the system FeII(L)/NO/HONO/NO2- in aqueous solution

FeII(L) reacts with NO, HONO, and NO2- to produce FeII(L)NO for L = diethylenetriaminepentaacetate, ethylenediaminetetraacetate, N-(hydroxyethyl)ethylenediaminetriacetate, nitrilotriacetate, ethylenediaminediacetate, and water. The reaction with HONO and NO2- occurs in two parallel paths of different order with respect to the reaction components. The systematic variation of the nature of L enables an investigation of the role of labile coordination sites on the Fe(II) center during such reactions. The parallel reactions are characterized by the rate law -d[FeII(L)]/dt = kA[HONO]2 + kB[FeII(L)][HONO], and the contribution of each path depends on the nature of L, pH, and total nitrite concentration. The kinetic data support the formation of a reactive intermediate, most probably N2O3 (kA path), and the reduction of HONO by FeII(L) to NO (kB path). The observed reactions and reactivity patterns strongly depend on the availability of labile coordinated solvent molecules on FeII(L), as governed by the nature of the ligand L. The results of this study are discussed in reference to the available literture data and in comparison to the kinetics of oxidation of these complexes by molecular oxygen.

Coordination compounds of titanium(IV) with furoylphenylhydroxylamine and 1,8-dihydroxynaphthalene

Complex compounds of titanium(IV) with furoylphenylhydroxylamine and 1,8-dihydroxynaphthalene, isolated preparatively from solutions with pH 5-6, 3-1, and also 1 and 11 M HCI were studied by the IR spectroscopic method. Their composition was established, and the probable structure of the coordination compounds was suggested.