516-03-0

Basic information

• Product Name: Ferrous oxalate
• Synonyms: OXALIC ACID IRON (II) SALT;Ethanedioicacid,iron(2+)salt(1:1);ethanedioicacid,iron(2+)salt(1:1)[qr];ethanedioicacid,iron(2++)salt(1:1);ferrox[qr];iron(2+)oxalate[qr];iron(ii)oxalate[qr];ironoxalate[fec2o4][qr]
• CAS NO: 516-03-0
• Molecular Formula: C₂O₄*Fe
• Molecular Weight: 143.86
• EINECS: 208-217-4
• Product Categories: other
• Mol File: 516-03-0.mol
• Article Data: 1

Chemical Properties

• Melting Point: 190°C
• Boiling Point: 365.1 °C at 760 mmHg
• Flash Point: 188.8 °C
• Appearance: Odorless yellow solid
• Density: 2.30
• Vapor Pressure: 0.038Pa at 25℃
• Storage Temp.: Inert atmosphere,Room Temperature
• Solubility: Soluble in acids
• Water Solubility: Slightly soluble
• Sensitive: Hygroscopic
• CAS DataBase Reference: Ferrous oxalate(CAS DataBase Reference)
• NIST Chemistry Reference: Ferrous oxalate(516-03-0)
• EPA Substance Registry System: Ferrous oxalate(516-03-0)

Safety Data

• RIDADR: UN3288
• TSCA: Yes
• HazardClass: 6.1
• PackingGroup: III
• Hazardous Substances Data: 516-03-0(Hazardous Substances Data)

Usage

Description

Ferrous oxalate, or iron (II) oxalate, is a chemical compound consisting of one iron (II) ion (Fe2+) and one oxalate ion (C2O42-). It has the chemical formula FeC2O4. Iron(II) oxalate is more commonly encountered as the dihydrate, FeC2O4·2H2O . Its crystal structure consists of chains of oxalatebridged iron atoms, capped by water molecules. When heated, it dehydrates and decomposes into carbon dioxide, carbon monoxide, iron oxides and pyrophoric black iron.

Chemical Properties

Pale-yellow, crystalline powder; odorless. Soluble in acids; insoluble in water.

Uses

Different sources of media describe the Uses of 516-03-0 differently. You can refer to the following data:
1. Used as a photographic developer, glass tint, decorative glass colorant, and pigment in plastics, paints, and lacquers.
2. Photographic developer, pigment in glass, plastics, paints.

General Description

Odorless yellow solid. Insoluble in water and denser in water. Sinks in water.

Air & Water Reactions

Insoluble in water.

Reactivity Profile

Inorganic reducing agents, such as Ferrous oxalate, react with oxidizing agents to generate heat and products that may be flammable, combustible, or otherwise reactive.

Hazard

Toxic. Evolves carbon monoxide on heating.

Health Hazard

Inhalation of dust may cause irritation of nose and throat. Ingestion causes burning pain in throat and stomach; mucous membranes turn white; can also cause vomiting, weak pulse, collapse, and death. Dust irritates eyes and may irritate skin on prolonged contact.

Fire Hazard

Special Hazards of Combustion Products: Iron fume or iron oxide fume may form in fire.

Flammability and Explosibility

Notclassified

InChI:InChI=1/C2H2O4.Fe/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2/p-2

Synthetic route

tin(II) chloride dihdyrate (10025-69-1) + iron(III) oxalate pentahydrate → tin(IV) chloride tetrahydrate + Sn(2+)*C2O4(2-)*3H2O=SnC2O4*3H2O + FeC2O4, α (516-03-0)

Conditions	Yield
In neat (no solvent, solid phase) Solid state reaction in hydrogen or helium atmosphere.; Gas chromatography, Moessbauer spectroscopy.;

iron(III) oxalate pentahydrate → FeC2O4, α (516-03-0) + carbon dioxide (124-38-9) + water (7732-18-5)

Conditions	Yield
In neat (no solvent, solid phase) Solid state reaction in hydrogen or helium atmosphere.; Gas chromatography, Moessbauer spectroscopy.;

Upstream product

• 10025-69-1 tin(II) chloride dihdyrate 

Relevant articles and documents

Studies on solid state redox reaction of iron(III) oxalate by gas chromatography

The solid state redox reaction of iron (III) oxalate with sodium nitrate and tin(II) chloride was investigated in hydrogen atmosphere and helium atmosphere by use of a non-isothermal technique. The evolved gases (EG) formed during the reaction were directly detected by gas chromatography, and the solid products were also identified by XRD, Moessbauer spectra and IR. The results show that the solid state redox reaction can go to completion because electron transfer is much easier than mass diffusion along the boundaries of the reactant. The releasing of crystal and coordination water during the redox reaction also facilitates completion of the reaction. The mechanism of the solid state reaction is also discussed.