| Identification | More | [Name]
Ferric oxide | [CAS]
1309-37-1 | [Synonyms]
IRON(III) OXIDE DIHYDRATE
11554red
anchredstandard
anhydrousironoxide
anhydrousoxideofiron
armenianbole
bauxiteresidue
blackoxideofiron
blendedredoxidesofiron
burntislandred
burntsienna
c.i.pigmentred101
c.i.pigmentred101and102
c.i.pigmentred102
calcotonered
caputmortuum
colcothar
colloidalferricoxide
crocusmartisadstringens
deanox | [EINECS(EC#)]
215-168-2 | [Molecular Formula]
Fe2O3 | [MDL Number]
MFCD00748135 | [Molecular Weight]
159.69 | [MOL File]
1309-37-1.mol |
| Chemical Properties | Back Directory | [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.
| [Appearance]
Hematite is a noncombustible, black to black red or brick-red mineral (iron ore) composed mainly of
ferric oxide, Fe2O3. Ferric oxide | [Melting point ]
1538°C | [density ]
5.24 | [Fp ]
>230 °F
| [storage temp. ]
2-8°C | [solubility ]
It is soluble In Warm Hydrochloric Acid, Slightly Soluble in Sulfuric Acid. | [form ]
pieces
| [color ]
black | [Specific Gravity]
5.1～5.2 | [PH]
3.7±0.3 | [Stability:]
Stable. | [Water Solubility ]
INSOLUBLE | [Merck ]
14,4028 | [Exposure limits]
ACGIH: TWA 5 mg/m3
OSHA: TWA 10 mg/m3; TWA 15 mg/m3; TWA 5 mg/m3
NIOSH: IDLH 2500 mg/m3; TWA 5 mg/m3 | [Uses]
Ferric Oxide is a nutrient and dietary supplement that is a source of
iron. | [CAS DataBase Reference]
1309-37-1(CAS DataBase Reference) | [IARC]
3 (Vol. 1, Sup 7) 1987 | [NIST Chemistry Reference]
Iron(iii) oxide(1309-37-1) | [EPA Substance Registry System]
1309-37-1(EPA Substance) |
| Safety Data | Back Directory | [Hazard Codes ]
Xi,F | [Risk Statements ]
R36/37/38:Irritating to eyes, respiratory system and skin . | [Safety Statements ]
S26:In case of contact with eyes, rinse immediately with plenty of water and seek medical advice . | [WGK Germany ]
-
| [RTECS ]
NO7400000
| [TSCA ]
Yes | [HS Code ]
28211000 | [Hazardous Substances Data]
1309-37-1(Hazardous Substances Data) | [IDLA]
2,500 mg Fe/m3 |
| Hazard Information | Back Directory | [Hazard]
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. | [First aid]
If this chemical gets into the eyes, remove any
contact lenses at once and irrigate immediately for at least
15 minutes, occasionally lifting upper and lower lids. Seek
medical attention immediately. If this chemical contacts the
skin, remove contaminated clothing and wash immediately
with soap and water. Seek medical attention immediately.
If this chemical has been inhaled, remove from exposure,
begin rescue breathing (using universal precautions, includ ing resuscitation mask) if breathing has stopped and CPR if
heart action has stopped. Transfer promptly to a medical
facility. When this chemical has been swallowed, get medi cal attention. Give large quantities of water and induce
vomiting. Do not make an unconscious person vomit.
| [Incompatibilities]
Contact with hydrogen peroxide, ethyl ene oxide, calcium hypochlorite will cause explosion.
Violent reaction with powdered aluminum; hydrazine,
hydrogen trisulfide. | [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. | [Flammability and Explosibility]
Nonflammable | [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 | [storage]
Color Code- Green: General storage may be used.Prior to working with this chemical you should be trainedonits proper handling and storage. Store in tightly closedcontainers in a cool, well-ventilatedarea. .Where possible,automatically transfer material from other storage contain-ers to process containers A regulated, marked area shouldbe established where this chemical is handled, used, orstored in compliance with OSHA Standard 1910.1045. | [Properties and Applications]
|
TEST ITEMS
|
SPECIFICATION
|
|
APPEARANCE
|
DARK RED POWDER
|
|
SHADE
|
CLOSE TO STANDARD
|
|
CONTENT OF
Fe
2
O
3
|
96% min
|
|
pH VALUE
|
3-7
|
|
OIL ABSORPTION
|
15-25%
|
|
RESIDUE ON 320 MESH
|
0.3% max
|
|
WATER SOLUBLE
|
0.3% max
|
|
VOLATITE 105 °C
|
1.0% max
|
|
TINTING STRENGTH
|
98-102 %
|
|
| Questions And Answer | Back Directory | [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.
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