Basic information Physical Properties Occurrence and Uses Preparation Reactions Safety Supplier Related
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Ferric oxide

Basic information Physical Properties Occurrence and Uses Preparation Reactions Safety Supplier Related

Ferric oxide Basic information

Product Name:
Ferric oxide
Synonyms:
  • Ferric oxide(II,III), magnetic nanoparticles solution
  • Ferric(III) oxide
  • Iron(III) oxide, 99% trace metals basis
  • Iron(III) oxide, 99.9% trace metals basis
  • Iron(III) oxide, 98% trace metals basis
  • Iron(III) oxide, 99.95% trace metals basis
  • Iron(III) oxide, 99.99% trace metals basis
  • Iron(lll) oxide
CAS:
1309-37-1
MF:
Fe2O3
MW:
159.69
EINECS:
215-168-2
Product Categories:
  • Inorganics
  • metal oxide
Mol File:
1309-37-1.mol
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Ferric oxide Chemical Properties

Melting point:
1538°C
Density 
5.24
Flash point:
>230 °F
storage temp. 
2-8°C
solubility 
It is soluble In Warm Hydrochloric Acid, Slightly Soluble in Sulfuric Acid.
form 
pieces
Specific Gravity
5.1~5.2
color 
black
PH
3.7±0.3
Water Solubility 
INSOLUBLE
Merck 
14,4028
Stability:
Stable.
CAS DataBase Reference
1309-37-1(CAS DataBase Reference)
NIST Chemistry Reference
Iron(iii) oxide(1309-37-1)
IARC
3 (Vol. 1, Sup 7) 1987
EPA Substance Registry System
Ferric oxide (1309-37-1)
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Safety Information

Hazard Codes 
Xi,F
Risk Statements 
36/37/38-11
Safety Statements 
26-16
RIDADR 
UN 1376
WGK Germany 
-
RTECS 
NO7400000
TSCA 
Yes
HS Code 
28211000
Hazardous Substances Data
1309-37-1(Hazardous Substances Data)

MSDS

  • Language:English Provider:ALFA
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Ferric oxide Usage And Synthesis

Physical Properties

Reddish-brown hexagonal crystal; refractive index 2.91; density 5.25g/cm3; Moh’s hardness 6.0; melts at 1565°C; insoluble in water; dissolves in acids.

Occurrence and Uses

Ferric oxide occurs in nature as the mineral hematite. It is the principal ore of iron from which the metal and its alloys are produced. Also, this oxide occurs in the mineral, limonite, 2Fe2O3•3H2O. An important application of this compound involves producing red, orange, and yellow pigments. Other applications are in coatings for metals, steel and rubber; in ceramics; and as a catalyst for oxidation reactions.

Preparation

Ferric oxide is prepared as a reddish-brown hydrated precipitate by treating an aqueous solution of an iron(III) salt with caustic soda:
2FeCl3 + 6NaOH → Fe2O3•3H2O + 6NaCl
It also is obtained by thermal decomposition of iron(II) sulfate or the brown oxide hydroxide:
2FeSO4 → Fe2O3 + SO2 + SO3
2FeO(OH) → Fe2O3 + H2O
The oxide is prepared in industrial scale by first precipitating iron(II) hydroxide Fe(OH)2 by treating aqueous solutions of iron(II) sulfate and caustic soda. The Fe(OH)2 is then oxidized to iron(III) hydroxide by aeration. The latter is dehydrated by heating:
Fe2+ (aq) + OH¯ (aq) → Fe(OH)2(s) → 2Fe(OH)3 → Fe2O3 + 3H2O
It also is produced by ignition of iron(III) oxalate and iron carbonyls:
2Fe2(C2O4)3 +3O2 → 2Fe2O3 + 12CO

Reactions

Ferric oxide decomposes to its elements when heated at elevated temperatures:
2Fe2O3 → 4Fe + 3O2
The oxide is reduced by most reducing agents. Reaction with carbon monoxide at elevated temperatures (that occurs in the blast furnace) gives metallic iron. The overall reaction is mildly exothermic (ΔHrxn –113.4 kcal/mol):
2 Fe2O3 + 6CO → 4Fe + 6CO2
It also is reduced by powdered aluminum at elevated temperatures, forming aluminum oxide and metallic iron:
Fe2O3 + 2Al → Al2O3 + 2Fe
The reaction is highly exothermic and becomes self-sustaining after ignition.
When heated with sand in an electric furnace, iron(III) oxide forms ferrosilicon alloy. When heated in a vacuum at 1,000°C, it forms triiron tetroxide, Fe3O4.

Description

Iron oxides are produced synthetically and consist essentially of anhydrous and/or hydrated iron oxides. The range of hues includesyellows, reds, browns and blacks. Food quality iron oxides are primarily distinguished from technical grades by the comparatively low levels of contamination by other metals. This is achieved by the selection and control of the source of iron and/or by the extent of chemical purification during the manufacturing process. Iron oxides have been used to color confectionery, fillings and decorations for pastry products, cheese products, fish paste, pet foods, cosmetics and pharmaceutical products.

Chemical Properties

Hematite is a noncombustible, black to black red or brick-red mineral (iron ore) composed mainly of ferric oxide, Fe2O3. Ferric oxide

Occurrence

Iron(III) oxide occurs in nature as the mineral hematite. It is the principal ore of iron from which the metal and its alloys are produced. Also, this oxide occurs in the mineral, limonite, 2Fe2O3?3H2O. An important application of this compound involves producing red, orange, and yellow pigments. Other applications are in coatings for metals, steel and rubber; in ceramics; and as a catalyst for oxidation reactions.

Uses

Red iron oxide (Fe2O3) is an inorganic pigment of either natural or synthetic origin. It is a low chroma red with excellent durability and low cost. Synthetic pigment is made by heating iron sulfate with quicklime in a furnace. The second preparatory technique involves calcining iron sulfate in the presence of air at high temperatures. Natural and oxides of iron are mined either as the mineral hematite (Fe2O3) or as hematite in its hydrated form.

Uses

As pigment for rubber, paints, paper, linoleum, ceramics, glass; in paint for ironwork, ship hulls; as polishing agent for glass, precious metals, diamonds; in electrical resistors and semiconductors; in magnets, magnetic tapes; as catalyst; colloidal solutions as stain for polysaccharides.

Uses

Ferric Oxide is a nutrient and dietary supplement that is a source of iron.

Definition

A high-grade red pigment used as a polishing agent for glass, jewelry, etc. (2) A cosmetic prepared from dried flowers of the saf- flower.

Definition

A black solid prepared by passing either steam or carbon dioxide over redhot iron. It may also be prepared by passing steam over heated iron(II) sulfide. Triiron tetroxide occurs in nature as the mineral magnetite. It is insoluble in water but will dissolve in acids to give a mixture of iron(II) and iron(III) salts in the ratio 1:2. Generally it is chemically unreactive; it is, however, a fairly good conductor of electricity.

Preparation

Iron(III) oxide is prepared as a reddish-brown hydrated precipitate by treating an aqueous solution of an iron(III) salt with caustic soda:
2FeCl3 + 6NaOH → Fe2O3?3H2O + 6NaCl
It also is obtained by thermal decomposition of iron(II) sulfate or the brown oxide hydroxide:
2FeSO4 → Fe2O3 + SO2 + SO3
2FeO(OH) → Fe2O3 + H2O
The oxide is prepared in industrial scale by first precipitating iron(II) hydroxide Fe(OH)2 by treating aqueous solutions of iron(II) sulfate and caustic soda. The Fe(OH)2 is then oxidized to iron(III) hydroxide by aeration. The latter is dehydrated by heating:
Fe2+ (aq) + OHˉ (aq) → Fe(OH)2(s) → 2Fe(OH)3 → Fe2O3 + 3H2O
It also is produced by ignition of iron(III) oxalate and iron carbonyls:
2Fe2(C2O4)3 +3O2 → 2Fe2O3 + 12CO
.

Hazard

Pneumoconiosis. Questionable carcinogen.

Potential Exposure

Hematite; as an iron ore composed mainly of ferric oxide, is a major source of iron and is used as a pigment for rubber, paints, paper, linoleum, ceramics, dental restoratives; and as a polishing agent for glass and pre cious metals. It is also used in electrical resistors, semiconduc tors, magnets, and as a catalyst. Human exposure to hematite from underground hematite mining is principally through inhalation and/or ingestion of dusts. No estimates are available concerning the number of underground miners exposed.

Carcinogenicity

Welders are typically exposed to a complex mixture of dust and fume of metallic oxides, as well as irritant gases, and are subject to mixeddust pneumoconiosis with possible loss of pulmonary function; this should not be confused with benign pneumoconiosis caused by iron oxide.1 Although an increased incidence of lung cancer has been observed among hematite miners exposed to iron oxide, presumably owing to concomitant radon gas exposure, there is no evidence that iron oxide alone is carcinogenic to man or animals.6

Incompatibilities

Contact with hydrogen peroxide, ethyl ene oxide, calcium hypochlorite will cause explosion. Violent reaction with powdered aluminum; hydrazine, hydrogen trisulfide.

Ferric oxide Supplier

Shanghai Yunfu Nano Technology Co., Ltd Gold
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J & K SCIENTIFIC LTD.
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010-82848833- ;010-82848833-
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Meryer (Shanghai) Chemical Technology Co., Ltd.
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21-61259100-
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Alfa Aesar
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400-610-6006; 021-67582000
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saleschina@alfa-asia.com
BeiJing Hwrk Chemicals Limted
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0757-86311057-
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