68391-67-3

Basic information

• Product Name: iron(2+) [(carboxylatomethyl)(carboxymethyl)amino]acetate
• CAS NO: 68391-67-3
• Molecular Formula: C₆H₇FeNO₆
• Molecular Weight: 244.9679
• Mol File: 68391-67-3.mol
• Article Data: 1

Chemical Properties

• Boiling Point: 498.2°C at 760 mmHg
• Flash Point: 255.1°C
• Vapor Pressure: 2.78E-11mmHg at 25°C
• CAS DataBase Reference: iron(2+) [(carboxylatomethyl)(carboxymethyl)amino]acetate(CAS DataBase Reference)
• NIST Chemistry Reference: iron(2+) [(carboxylatomethyl)(carboxymethyl)amino]acetate(68391-67-3)
• EPA Substance Registry System: iron(2+) [(carboxylatomethyl)(carboxymethyl)amino]acetate(68391-67-3)

Safety Data

• Hazardous Substances Data: 68391-67-3(Hazardous Substances Data)

Upstream product

• 139-13-9 nitrilotriacetic acid 

Downstream Products

• 16448-54-7 ferric nitrilotriacetate 

Relevant articles and documents

Reactions of FeIInta and FeIIedda with Hydrogen Peroxide

Reactions of ferrous nitrilotriacetate (nta) and ethylenediamine-N,N'-diacetate (edda) complexes with hydrogen peroxide at neutral pH in the presence of formate lead to transient intermediates characterized by absorptions near 280 and 400 nm as previously observed for hedta as a ligand.The decomposition of hydrogen peroxide by FeIIInta and-edda leads to ligand destruction, which is not inhibited by formate.During this process a reactive intermediate is scavenged by ABTS at concentrations of the latter that are much higher than expected if the hydroxyl radical were the reactive intermediate.This intermediate is not scavenged by the bromide ion.These stopped-flow and steady-state experiments give evidence for the following reactions (HL = nta, edda): (a) HLFeII + H2O2 -> HLFe(H2O2), (b) HLFe(H2O2) + HLFeII + 2H+ -> 2HLFeIII + 2H2O, (c) HLFe(H2O2) + HCO2- -> L.FeII + CO2.- + 2H2O, (d) HLFe(H2O2) + H+ -> L+FeII + 2H2O, (e) HLFe(H2O2) + ABTS + 2H+ -> HLFeIII + ABTS.+ + 2H2O.Reactions b-e are ascribed to a compound designated as HLFe(H2O2) in reaction a, which might be a hypervalent iron complex HLFeIV(OH-)2 but not a hydroxyl radical.The ability of the HLFe(H2O2) complex to oxidize ethanol but not bromide suggests a one-electron reduction potential greater than E0'(CH3.CHOH,H+/CH3CH2OH) = 1.2 V at pH 7 and smaller than E0(Br2.-/2Br- = 1.63 V.