Chemical Properties
Ferrous sulfate is a greenish or yellowish solid
in fine or lumpy crystals.
Chemical Properties
Greenish or yellow-brown crystals or
granules; odorless. Soluble in water with saline
taste; insoluble in alcohol. hygroscopic.
Hazard
Ingestion causes intestinal disorders.
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.
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 immedi ately with soap and water. Seek medical attention immedi ately. If this chemical has been inhaled, remove from
exposure, begin rescue breathing (using universal precau tions, including 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 medical attention. Give large quanti ties of water and induce vomiting. Do not make an uncon scious person vomit.
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.
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°.
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).
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.
.
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
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
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.
