| Uses |
- Nutritional supplements (iron enhancer); color former of fruit and vegetable; for example, the salted product used together with dried alum in eggplant can form stable complex salt with its pigment to prevent the discoloration caused by organic acids. However, it should be noted, for example, it will turn into black ink upon excess amount of iron. When the amount of alum is high, the meat of the pickled eggplant meat will become excessively solid. Formulation example: long eggplant 300 kg; edible salt 40kg; ferrous sulfate 100g; dried alum 500g. It can still be used as the color forming agent of black beans, sugar boiled beans and kelp. Food containing tannins, in order to avoid of causing blackening, should not be used. It can also be used for sterilization, deodorization and very weakly bactericidal.
- Legumes contained cryptochromic pigment is colorless upon reduction state while being oxidized into black upon oxidation in alkaline condition. Taking advantage of the reduction property of ferrous sulfate can achieve the purpose of color protection with the usage amount of 0.02% to 0.03%.
- If is used for the manufacturing of iron salt, iron oxide pigments, mordant, purifying agent, preservatives, disinfectants and medicine for anti-anemia drugs
|
| Toxicity | LD50: 279 to 558 mg/kg (rat, oral, calculated as Fe).
GRAS (FDA, § 182.5315, §184.1315, 2000);
ADI 0.8 mg Fe/kg (calculated in terms of Fe; FAO/WHO, 2001);
|
| Hazards & Safety Information | Category :Toxic substances
Toxicity classification: highly toxic
Acute Toxicity : Oral-Rat LD50 319 mg/kg; Oral-mouse LD50: 680 mg/kg
Flammability and Hazardous characteristics: Non-combustible with fire producing toxic iron-containing fumes
Storage and transportation characteristics Treasury: low temperature, ventilated, dry; store separately from food raw materials.
Fire extinguishing agent : water, carbon dioxide, dry powder, sand
Occupational Standard :TWA 1 mg (iron)/m3 |
| Description | Green vitriol, FeSO4.7H20, has been known since the thirteenth
century ; it crystallizes from solutions of iron or iron bases in dilute sulphuric acid. The
heptahydrate forms green monoclinic crystals of density 1·88, very soluble in water (296 g
litre-1 FeS04 at 25°C). By precipitating the aqueous solution with ethanol, heating the
heptahydrate to 140° in vacuo or by crystallizing it from 50 % sulphuric acid, the white monohydrate
is obtained. This can be further dehydrated to the white, amorphous FeSO4 by
heating to 300° in a current of hydrogen. At red heat the sulphate decomposes :
2FeS04 -> Fe203+S02+S03
A tetrahydrate, FeS04.4H20, crystallizes from aqueous solutions above 56°. |
| Chemical Properties | Greenish or yellow-brown crystals or
granules; odorless. Soluble in water with saline
taste; insoluble in alcohol. hygroscopic. |
| Chemical Properties | Ferrous sulfate is a greenish or yellowish solid
in fine or lumpy crystals. |
| Physical properties | White orthorhombic crystal; hygroscopic; density 3.65 g/cm3; soluble in water (26.6g/100g water at 20°C). The monohydrate is a yellowish-white monoclinic crystal; density 3.0 g/cm3; decomposes at 300°C; soluble in water. Heptahydrate is bluish-green monoclinic crystal; refractive index 1.47; hardness 2 Mohs; density 1.89g/cm上3; decomposes at about 60°C; very soluble in water; soluble in absolute methanol; slightly soluble in ethanol. |
| Occurrence | Iron(II) sulfate is probably the most important salt of iron, as well as the longest-known iron(II) compound. The compound is used as a mordant in dyeing; as a component of writing ink; in electroplating baths; in radiation dosimeters; in lithography and engraving; as a weed-killer; and in water purification. A major application of this compound is in the manufacture of other iron(II) salts including Prussian blue or ferric ferrocyanide. Iron(II) sulfate also is used as a reducing agent and an analytical reagent (in brown ring test for nitrate). |
| Uses | Ferrous Sulfate is a nutrient and dietary supplement that is a source
of iron. it is a white to grayish odorless powder. ferrous sulfate hep-
tahydrate contains approximately 20% iron, while ferrous sulfate
dried contains approximately 32% iron. it dissolves slowly in water
and has high bioavailability. it can cause discoloration and rancidity.
it is used for fortification of baking mixes. in the encapsulated form
it does not react with lipids in cereal flours. it is used in infant foods,
cereals, and pasta products. |
| Uses | Iron Supplement |
| Uses | Ferrous sulfate (FeSO4) is also known as iron sulfate or iron vitriol. It is used in the production
of various chemicals, such as sulfur dioxide and sulfuric acid. |
| Definition | Copperas: an off-whitesolid, FeSO4.H2O; monoclinic; r.d.2.970. There is also a heptahydrate,FeSO4.7H2O; blue-green monoclinic;r.d. 1.898; m.p. 64°C. The heptahydrateis the best known iron(II) saltand is sometimes called green vitriolor copperas. It is obtained by the actionof dilute sulphuric acid on ironin a reducing atmosphere. The anhydrouscompound is very hygroscopic.It decomposes at red heat to giveiron(III) oxide, sulphur trioxide, andsulphur dioxide. A solution of iron(II)sulphate is gradually oxidized on exposureto air, a basic iron(III) sulphatebeing deposited. |
| Production Methods | Iron(II) sulfate in industrial scale is mostly produced in the pickling process as a by-product of the steel industry. It is obtained when the surface of steel is cleaned with dilute sulfuric acid to remove metal impurities. In the laboratory iron(II) sulfate heptahydrate may be prepared by dissolving iron in dilute sulfuric acid in a reducing atmosphere, followed by crystallization:
Fe + H2SO4 → FeSO4 + H2
Alcohol may be added to the aqueous solution to speed up crystallization; iron(II) may otherwise oxidize to iron(III) during a slow crystallization process.
Iron(II) oxide or carbonate may be used instead of iron metal to prepare the heptahydrate.
. |
| Definition | A rusty-brown solid prepared by the action
of heat on iron(III) hydroxide or iron(II)
sulfate. It occurs in nature as the mineral
hematite. Industrially it is obtained by
roasting iron pyrites. Iron(III) oxide dissolves
in dilute acids to produce solutions
of iron(III) salts. It is stable at red heat, decomposes
around 1300°C to give triiron
tetroxide, and can be reduced to iron by
hydrogen at 1000°C. Iron(III) oxide is not
ionic in character but has a structure similar
to that of aluminum(III) oxide. |
| Hazard | Ingestion causes intestinal disorders. |
| Flammability and Explosibility | Nonflammable |
| Agricultural Uses | Copperas, also called green vitriol, is ferrous sulphate heptahydrate. It is an iron salt fertilizer, which is most effective in overcoming iron deficiency. |
| Agricultural Uses | Ferrous sulphate heptahydrate (FeSO4.7H2O), also called green vitriol or copperas, is a blue-green water-soluble crystal and is the best known ferrous salt. It is obtained by the action of dilute sulphuric acid on iron in a reducing atmosphere. The anhydrous compound is very hygroscopic. It gets oxidized gradually in an aqueous solution. On heating, the solid decomposes to give red ferric oxide, sulphur trioxide (SO3) and sulphur dioxide (SO2). |
| Clinical Use | Iron deficiency anaemia |
| Safety Profile | A human poison by
ingestion. Moderately toxic to humans by an
unspecified route. An experimental poison
by ingestion, intraduodenal, intraperitoneal,
intravenous, and subcutaneous routes.
Human systemic effects by ingestion:
aggression, somnolence, brain recorlng
changes, diarrhea, nausea or vomiting,
bleedmg from the stomach, coma.
Questionable carcinogen with experimental
tumorigenic data. Experimental teratogenic
and reproductive effects. Mutation data
reported. Potentially explosive reaction with
methyl isocyanoacetate at 25'. May igmte on
contact with arsenic trioxide + sodium
nitrate. When heated to decomposition it
emits toxic fumes of SOx. See also IRON COMPOUNDS. |
| Potential Exposure | It is used as a fertilizer, food or feed
additive; and in herbicides; process engraving; dyeing, and
water treatment. A byproduct of various chemical and
metal treating operations. |
| Veterinary Drugs and Treatments | While iron is a necessary trace element in all hemoglobin-utilizing
animals, the use of therapeutic dosages of ferrous sulfate (or other
oral iron) preparations in veterinary medicine is limited primarily
to the treatment of iron-deficiency anemias in dogs (usually due to
chronic blood loss), and as adjunctive therapy in cats when receiving
epoetin (erythropoietin) therapy. Injectable iron products are
usually used in the treatment of iron deficiency anemias associated
with newborn animals. |
| Drug interactions | Potentially hazardous interactions with other drugs
Antibacterials: reduced absorption of 4-quinolones
and tetracyclines.
Dimercaprol: avoid concomitant use.
Mycophenolate: may significantly reduce absorption
of mycophenolate. |
| Metabolism | Following absorption, the majority of iron is bound to
transferrin and transported to the bone marrow where
it is incorporated into haemoglobin. The remainder is
stored within ferritin or haemosiderin or is incorporated
into myoglobin with smaller amounts occurring in haemcontaining enzymes or in plasma bound to transferrin. Only very small amounts are excreted as the body
reabsorbs the iron after the haemoglobin has broken
down |
| Incompatibilities | Aqueous solution is acidic. Contact with
alkalies form iron. Keep away from alkalies, soluble carbo nates; gold and silver salts; lead acetate; lime water, potassium
iodide; potassium and sodium tartrate; sodium borate; tannin. |
