FERROUS SULFATE

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).

The Uses of FERROUS SULFATE

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.

The Uses of FERROUS SULFATE

Iron Supplement

The Uses of FERROUS SULFATE

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.

Background

Iron deficiency anemia is a large public health concern worldwide, especially in young children, infants, and women of childbearing age. This type of anemia occurs when iron intake, iron stores, and iron loss do not adequately support the formation of erythrocytes, also known as red blood cells.
Ferrous sulfate is a synthetic agent used in the treatment of iron deficiency. It is the gold standard of oral iron therapy in the UK and many other countries.

Indications

Ferrous sulfate is used for the prevention and treatment of iron deficiency anemia in adults and children.

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.

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.
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Hazard

Ingestion causes intestinal disorders.

Flammability and Explosibility

Non flammable

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).

Pharmacokinetics

Ferrous sulfate replenishes iron, an essential component in hemoglobin, myoglobin, and various enzymes. It replaces the iron that is usually found in hemoglobin and myoglobin. Iron participates in oxygen transport and storage, electron transport and energy metabolism, antioxidant and beneficial pro-oxidant functions, oxygen sensing, tissue proliferation and growth, as well as DNA replication and repair.

Clinical Use

Iron deficiency anaemia

Side Effects

Iron is toxic to the gastrointestinal system, cardiovascular system, in addition to central nervous system. The most early reported effects following the excess ingestion of iron include nausea, flatulence, abdominal pain, diarrhea, constipation, and black/tarry stools. Symptoms of overdose in the later stages include bluish lips, fingernails, and palms, drowsiness, tachycardia, seizures, metabolic acidosis, hepatic injury, and cardiovascular dysfunction. Sequelae of iron sulfate overdose include intestinal obstruction, pyloric stenosis, and gastric scarring.

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.

First aid

If this chemical gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts theskin, remove contaminated clothing and wash immediatelywith soap and water. Seek medical attention immediately. Ifthis chemical has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR ifheart action has stopped. Transfer promptly to a medicalfacility. When this chemical has been swallowed, get medical attention. Give large quantities of water and inducevomiting. Do not make an unconscious person vomit.Note to physician: Gastric lavage with large amounts of 5%sodium phosphate or water. Follow this with a large amountof 1% sodium bicarbonate over a 3-h period.Note to physician: For severe poisoning do not use BAL[British Anti-Lewisite, dimercaprol, dithiopropanol(C3H8OS2)] as it is contraindicated or ineffective in poisoning from iron.

Absorption

Approximately 5 – 10% of dietary iron is absorbed, and this absorption rate increases to up to 30% in iron deficiency states. Oral iron supplements are absorbed up to 60% via active and passive transport processes. Gastrointestinal absorption of iron occurs via strict regulation by the enterocyte and duodenal cytochrome and ferric reductase enzymes. The hormone hepcidin heavily regulates iron absorption and distribution throughout the body.
The median time to maximum serum concentration (Tmax) is generally 4 hours after administration. Between 2-8 hours post administration, average serum iron concentrations fluctuate by 20%, according to one study. Bioavailability of iron depends on whether it is administered in a film coated tablet or enteric coated tablet. One pharmacokinetic study in healthy volunteers revealed a 30% bioavailability for enteric coated tablets. The AUC of enteric coated tablets varied between a lower limit of -46.93 to 5.25 μmolxh/l. Cmax is higher for film coated tablets, ranging from 3.4 to 22.1 μmol/h/l.

Metabolism

The metabolism of iron is complex. Normally, iron exists in the ferrous (Fe2+) or ferric (Fe3+) state, but since Fe2+ is oxidized to Fe3+, which hydrolyzes to insoluble iron(III)hydroxides in neutral aqueous solutions, iron binds to plasma proteins and is either transported or stored throughout the body.
There are three proteins that serve to regulate the storage and transport of ingested iron. The first protein , transferrin, transports iron in both the plasma and extracellular fluid. Ceruloplasmin in the plasma and hephaestin on the enterocyte participate in the oxidation and binding of iron to transferrin. The main role of transferrin is the chelation of iron to prevent the production of reactive oxygen species, while facilitating its transport into cells. The transferrin receptor, located on many cells that require iron, binds the transferrin complex and internalizes this complex. Ferritin is a protein that stores iron, making it readily available for body requirements.

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

Toxicity

The toxicity of ferrous sulfate in humans depends on the amount of iron ingested. Up to 20 mg/kg of elemental iron is not toxic, 20-60 mg/kg has mild toxicity, and more than 60 mg/kg can lead to severe symptoms and morbidity.

storage

Color Code—Green: General storage may beused. Prior to working with this chemical you should betrained on its proper handling and storage. Store in tightlyclosed containers in a cool, well-ventilated area away fromalkalis.

Shipping

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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.