14634-91-4

Basic information

• Product Name: FERROIN
• Synonyms: (TRIS)-1,10-PHENANTHROLINE IRON (II) SULFATE;O-PHENANTHROLINE FERROUS SULFATE;O-PHENANTHROLINE FERROUS SULFATE COMPLEX;PHENANTHROLINE FERROUS SULFATE;1,10-Phenanthroline iron(II) sulfate complex;tris(1,10-phenanthroline-N1,N10)iron sulphate;FERROIN INDICATOR, 0.1 WT. % SOLUTION IN WATER;FERROIN SOLUTION 100 ML
• CAS NO: 14634-91-4
• Molecular Formula: C₃₆H₂₄FeN₆*O₄S
• Molecular Weight: 692.52
• EINECS: 238-676-6
• Product Categories: Organometallics;Classes of Metal Compounds;Fe (Iron) Compounds;Transition Metal Compounds
• Mol File: 14634-91-4.mol
• Article Data: 16

Chemical Properties

• Boiling Point: 365.1°Cat760mmHg
• Flash Point: 164.8°C
• Appearance: Dark red/Liquid
• Density: 0.999 g/mL at 25 °C
• Storage Temp.: Amber Vial, Refrigerator, Under inert atmosphere
• Solubility: Water
• Stability: Light Sensitive
• CAS DataBase Reference: FERROIN(CAS DataBase Reference)
• NIST Chemistry Reference: FERROIN(14634-91-4)
• EPA Substance Registry System: FERROIN(14634-91-4)

Safety Data

• Hazard Codes: N
• Statements: 52/53-51/53
• Safety Statements: 24/25-61
• TSCA: Yes
• Hazardous Substances Data: 14634-91-4(Hazardous Substances Data)

Usage

Description

FERROIN, also known as Ferroin Sulfate, is a dark red liquid that serves as a metal catalyst. It is predominantly utilized in the synthesis of dyes, where it facilitates green oxidative degradation. This characteristic makes it a valuable component in the production of dyes and their associated metabolites.

Uses

Used in Dye Synthesis Industry:
FERROIN is used as a metal catalyst for dye synthesis, specifically in the green oxidative degradation process. Its application reason is to enhance the efficiency and effectiveness of dye production, leading to the creation of dyes and their metabolites with improved properties and reduced environmental impact.

InChI:InChI=1/C12H8N2.Fe.H2O4S/c1-3-9-5-6-10-4-2-8-14-12(10)11(9)13-7-1;;1-5(2,3)4/h1-8H;;(H2,1,2,3,4)/q;+2;/p-2

Synthetic route

1,10-Phenanthroline (66-71-7) + Ammonium iron sulfate → ferroin (14634-91-4)

Conditions	Yield
In ethanol; water in situ react.;
In methanol; water not isolated;

ferrous(II) sulfate heptahydrate + 1,10-Phenanthroline (66-71-7) → ferroin (14634-91-4)

Conditions	Yield
In water FeSO4 and phenanthroline reacted in a 1:3 stoichiometric relationship;
In water added excess of FeSO4*7H2O; not isolated; investigated by Photoelectron Emission Spectroscopy;
In water

1,10-Phenanthroline (66-71-7) + ferrous ammonium sulphate → ferroin (14634-91-4)

Conditions	Yield
In not given

1,10-Phenanthroline (66-71-7) + iron(II) (7439-89-6) → ferroin (14634-91-4)

Conditions	Yield
In water 1,10-phenanthroline added in 1,10-phenanthroline:Fe ratio of ca. 3:1 todeaerated Fe(2+) soln.;

1,10-Phenanthroline (66-71-7) + iron(II) sulfate → ferroin (14634-91-4)

Conditions	Yield
FeS:1,10-phenanthroline, molar ratio 1:3;
In water Prepn. by dissolving stoich. amts. of starting compds. in pure H2O.;
In sulfuric acid stoichiometric amounts; filtered;
In not given
In water

tris(1,10-phenanthroline)iron(II) perchlorate → ferroin (14634-91-4)

Conditions	Yield
With Na2SO4 In water addn of pptd. educt to water contg. anion exchange resin (equilibrated with Na2SO4); not isolated, spectrophotometric control;

ferroin (14634-91-4) → dicyanobis(1,10-phenanthroline)iron(II) (14768-11-7, 30872-77-6, 80875-80-5, 15334-30-2, 15362-08-0)

Conditions	Yield
With potassium cyanide In water Fe salt aq. soln. heating nearly boiling, aq. KCN adding at once, stirring, cooling to room temp., dark violet crystals collecting, drying in vacuo; identified by IR, UV spectra;	90%

ferroin (14634-91-4) + Na2[Ni(maleonitriledithiolate)2] → Fe(C12H8N2)3(2+)*Ni(S2C2(CN)2)2(2-) = [Fe(C12H8N2)3][Ni(S2C2(CN)2)2] (176735-71-0)

Conditions	Yield
In methanol; water byproducts: Na2SO4; stirring (20 min); filtration, washing (water/ethanol), drying in air; elem. anal.;	50%

ferroin (14634-91-4) + 1,3-benzenedisulfonic acid disodium salt (831-59-4) → tris(1,10-phenanthroline)iron(II), m-benzenedisulfonate salt

Conditions	Yield
With water In water recrystd. twice from water, air-dried at room temp., water of crystn. determined by Karl-Fischer method;

ferroin (14634-91-4) + disodium 2,6-naphthalenedisulfonate (1655-45-4) → tris(1,10-phenanthroline)iron(II), 2,6-naphthalenedisulfonate salt

Conditions	Yield
With water In water recrystd. twice from water, air-dried at room temp., water of crystn. determined by Karl-Fischer method;

ferroin (14634-91-4) + 2,7-naphthalenedisulfonic acid, sodium salt (1655-35-2, 51770-81-1) → tris(1,10-phenanthroline)iron(II), 2,7-naphthalenedisulfonate salt

Conditions	Yield
With water In water recrystd. twice from water, air-dried at room temp., then dried in a silica gel desiccator, water of crystn. determined by Karl-Fischer method;

ferroin (14634-91-4) + o-Benzenedisulfonic acid dipotassium salt (5710-54-3) → tris(1,10-phenanthroline)iron(II), o-benzenedisulfonate salt

Conditions	Yield
With water In water recrystd. twice from water, air-dried at room temp., water of crystn. determined by Karl-Fischer method;

ferroin (14634-91-4) + water (7732-18-5) + sodium chloride (7647-14-5) → iron(II) triphenanthrolinechloride 99 hydrate

Conditions	Yield
In water pptn. of an iron(II) tirphenanthrolinesulfate-soln. with NaCl;; crystn.;;

hydrogenchloride (7647-01-0) + ferroin (14634-91-4) + water (7732-18-5) → iron(II) triphenanthrolinechloride 99 hydrate

Conditions	Yield
In water pptn. of an iron(II) tirphenanthrolinesulfate-soln. with HCl;; crystn.;;

ferroin (14634-91-4) → tris(1,10-phenanthroline)iron(III) (13479-49-7)

Conditions	Yield
With sodium bromate; sulfuric acid In sulfuric acid Oxidn. of starting compd. in NaBrO3 and H2SO4.;
With NaBrO3 In sulfuric acid aq. H2SO4;

ferroin (14634-91-4) → 2Fe(C12H8N2)3(3+)*3SO4(2-)=(Fe(C12H8N2)3)2(SO4)3

Conditions	Yield
With cerium (IV) sulfate; sulfuric acid In water Kinetics; at 25°C; investigated by stopped-flow method;
With potassium sulfate; dipotassium peroxodisulfate In water at 34.502℃; Kinetics; Temperature;

ferroin (14634-91-4) → tris(1,10-phenantholine)iron(III) perchlorate

Conditions	Yield
With lead dioxide In water treatment of aq. acidic ferroin soln. with PbO2 (Can. J. Chem., 1988, 55, 2763-2767); elem. anal.;

ferroin (14634-91-4) → Fe(1,10-phenanthroline)2(C12H10N2O)(1+)

Conditions	Yield
With NaOH In methanol; water Kinetics; 0.033-0.167 M NaOH, 0.081-0.593 mole fraction of MeOH, I=0.167, 298.1 K; not isolated, reaction followed by UV/VIS spectroscopy;
With NaOH In water; acetone Kinetics; 0.0033-0.0167 M NaOH, 0.047-0.328 mole fraction of Me2CO, I=0.0167, 298.1 K; not isolated, reaction followed by UV/VIS spectroscopy;
With NaOH In water Kinetics; 0.0033-0.167 M NaOH, I=0.0167-0.167, 298.1 K; not isolated, reaction followed by UV/VIS spectroscopy;

ferroin (14634-91-4) + potassium bromide (7558-02-3) → {Fe(C12H8N2)3}(2+)*2Br(1-)*7H2O={Fe(C12H8N2)3}Br2*7H2O

Conditions	Yield
In not given

disodium pentacarbonylchromium + ferroin (14634-91-4) → {Fe(phan)3}{(CO)5CrH}

Conditions	Yield
With water hydrolysis under addn. of (Fe(phan)3)SO4;;
With sodium hydroxide careful addn. of aq. NaOH to Cr complex with cooling; addn. of Fe complex;;
In water

ferroin (14634-91-4) + K2[UO2(1-ethoxycarbonyl-1-cyanoethylene-2,2-dithiolate)2] → Fe(C12H8N2)3(2+)*UO2(C12H10N2O4S4)(2-)=UO2(FeC48H34N8O4S4)

Conditions	Yield
In methanol; water (open atmosphere); stirring (30 min, room temp.), standing (1 h); filtration, washing (water-ethanol, ethanol, diethyl ether), drying (vac.), recrystn. (nitromethane-ether); elem. anal.;

ferroin (14634-91-4) + K2[bis-(1-ethoxy carbonyl-1-cyanoethylene-2,2-dithiolato)dioxouranate(VI)] → tris(1,10-phenanthroline)iron(II) bis(1-ethoxycarbonyl-1-cyanoethylene-2,2-dithiolato)dioxouranate(VI) (261161-84-6)

Conditions	Yield
In not given soln./suspn. of uranyl compound (generated in situ) reacted with iron complex (1:1 molar ratio) (according to N. Singh et al. (1999), Indian J. Chem., vol. 38A, p. 997);

dihydrogen hexachloroplatinate(IV) hexahydrate + ferroin (14634-91-4) → [Fe(1,10-phenanthroline)3][PtCl6]

Conditions	Yield
In ethanol; water at 20℃; for 5h;

Upstream product

• 66-71-7 1,10-Phenanthroline 
• 7439-89-6 iron(II) 
• 14586-54-0 tris(1,10-phenanthroline)iron(II) perchlorate 

Downstream Products

• 14768-11-7 dicyanobis(1,10-phenanthroline)iron(II) 

Relevant articles and documents

Tracer diffusion of the tris(1,10-phenanthroline)iron(II) cation in aqueous salt solutions. Effect of hydrophobic interactions

Tracer diffusion coefficients for the Fe(phen)2+3 ion (phen = 1,10-phenanthroline) have been measured in aqueous solutions containing Ni(phen)3SO4, Bu4NBr, MgSO4, and NaBr, respectively, at 298.2 K.The diffusion coefficient-viscosity

Temperature Dependence of Hydrophobic Ion Association of Tris(1,10-phenanthroline)iron(II) Ion with Arenedisulfonate Ions in Water

The ion-association constants(K) of (Fe(phen)3)2+ with o- and m-benzenedisulfonate, 2,6- and 2,7-naphthalenedisulfonate ions, determined by conductivity measurements at 0-50 deg C, were considerably larger than the electrostatic prediction: K(2

A Completely Inorganic BZ-Type Oscillator in a Closed Homogeneous System

In a batch reactor, an absolutely homogeneous inorganic Belousov-Zhabotinskii (BZ)-type oscillator has been designed in the system of BrO3--H2PO2--Mn 2+-Fe(Phen)32+-H2SO4. The oscillations of both [Br-] and [Mn3+]/[Mn2+] as well as [Fe(phen)33+]/[Fe(phen)32+] were observed by monitoring the changes of either the potential on a bromide electrode or the absorbance at the maximum absorbance wavelength for Mn3+ and Fe(phen)33+, respectively. Both of those two metallic ions are essential in the present system to give rise to the oscillations; their roles in the oscillation are discussed. It is found that Mn2+ can not be replaced by other substances, while Fe(phen)32+ can be replaced by either N2 flow or acetone. However, it can not be replaced by other metallic ions, including Mn2+ and Ce3+. Those results suggest that Mn2+ is the real oscillating catalyst for an autocatalytic formation of HBrO2 and Fe(phen)32+ is a catalyst for the catalytic reduction of Br2 by H2PO2- to remove any excess Br2 produced during the oscillations.

Anomalously Slow Electron Transfer at Ordered Graphite Electrodes: Influence of Electronic Factors and Reactive Sites

Electron-transfer rates for 17 inorganic redox systems plus methyl viologen were determined on highly ordered pyrolytic graphite (HOPG) and glassy carbon (GC).Provided the HOPG defect density is low, the electron-transfer rates of all systems are much slower on the basal plane of HOPG than on GC.The slow rates on HOPG show a trend with the homogenous self-exchange rate constants, but in all cases the HOPG rate constants are substantially lower than that calculated via Marcus theory from self-exchange rates.The low HOPG rates do not exhibit any trends with redox system charge or E1/2, as might be expected in the presence of double-layer or hydrophobic effects.The results are consistent with the semimetal properties of HOPG, which have been invoked to explain its low interfacial capacitance.Both the density of electronic states (DOS) and carrier density for HOPG are much lower than those for metals.By analogy to theories developed for electron transfer at semiconductor electrodes, the rate dependsd on an effectively bimolecular reaction between the redox system and carriers in the electrode.The low DOS and carrier density of HOPG leads to low electron-transfer rates compared to those of metals, or to those predicted from exchange rates.Disorder in the graphite increases electron-tranfer rates and the DOS, thus yielding much faster rates on both GC and defective HOPG.For the 14 outer-sphere systems studied here, this electronic factor is much more important than any interaction with specific surface sites present at defects.The evidence indicates that, for Fe(CN)6-3/-4, Euaq+2/+3, Feaq+2/+3, and Vaq+2/+3, specific surface interactions provide inner-sphere routes which have a large effect on the observed rate constant.

Direct Synthesis of Intermetallic Platinum-Alloy Nanoparticles Highly Loaded on Carbon Supports for Efficient Electrocatalysis

Compared to nanostructured platinum (Pt) catalysts, ordered Pt-based intermetallic nanoparticles supported on a carbon substrate exhibit much enhanced catalytic performance, especially in fuel cell electrocatalysis. However, direct synthesis of homogeneous intermetallic alloy nanocatalysts on carbonaceous supports with high loading is still challenging. Herein, we report a novel synthetic strategy to directly produce highly dispersed MPt alloy nanoparticles (M = Fe, Co, or Ni) on various carbon supports with high catalyst loading. Importantly, a unique bimetallic compound, composed of [M(bpy)3]2+ cation (bpy = 2,2′-bipyridine) and [PtCl6]2- anion, evenly decomposes on carbon surface and forms uniformly sized intermetallic nanoparticles with a nitrogen-doped carbon protection layer. The excellent oxygen reduction reaction (ORR) activity and stability of the representative reduced graphene oxide (rGO)-supported L10-FePt catalyst (37 wt %-FePt/rGO), exhibiting 18.8 times higher specific activity than commercial Pt/C catalyst without degradation over 20a ?000 cycles, well demonstrate the effectiveness of our synthetic approach toward uniformly alloyed nanoparticles with high homogeneity.

Boron cluster anions [BnHn]2- (n = 10, 12) in reactions of iron(II) and iron(III) complexation with 2, 2?-bipyridyl and 1, 10-phenanthroline

Complexation of FeII and FeIII with azaheterocyclic ligands L (L = phen or bipy) were studied in the presence and in the absence of boron cluster anions [BnHn]2- (n = 10, 12). The reactions were carried out in air at room temperature in organic solvents and/or water. In all the solvents used, well known [FeL3]An (An = 2Cl- or SO42-) ferrous complexes were formed from FeII salts. Composition of ferric complexes with L ligands depends on the nature of solvent: either dinuclear oxo-iron(III) chlorides [L2ClFeIII-O-FeIIIL2Cl]Cl 2 or ferric ferrates(III) [FeIIIL2Cl 2][FeIIICl4], or [FeIIIL 2Cl2][FeIIICl4L] were isolated from FeIII salts. Introduction of the closo-borate anions to a Fe 3+(or Fe2+)/L/solv. mixture stabilizes ferrous cationic complexes [FeL3]2+ in all the solvents used: only ferrous [FeL3][BnHn] (n = 10, 12) complexes were isolated from all the reaction mixtures in the presence of boron cluster anions. Copyright