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Ferrous sulfate

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Ferrous sulfate

Template:Chembox ChEMBL
Iron(II) sulfate
Identifiers
PubChem 24393
ChemSpider 22804 YesY
UNII RIB00980VW YesY
EC number 231-753-5
ChEBI CHEBI:75832
RTECS number NO8500000
ATC code AA07
Jmol-3D images Image 1
Properties
Molecular formula FeSO4
Molar mass 151.908 g/mol (anhydrous)
169.92 g/mol (monohydrate)
278.05 g/mol (heptahydrate)
Appearance blue/green or white crystals
Odor odorless
Density 2.84 g/cm3 (anhydrous)
2.2 g/cm3 (pentahydrate)
1.898 g/cm3 (heptahydrate)
Melting point

70 °C (dehydration of heptahydrate)
400 °C (decomposes)

Solubility in water 25.6 g/100mL (anhydrous)
48.6 g/100 mL (heptahydrate) (50 °C)
Solubility negligible in alcohol
Refractive index (nD) 1.536 (pentahydrate)
1.478 (heptahydrate)
Hazards
EU Index 026-003-00-7 (anhydrous)
026-003-01-4 (heptahydrate)
EU classification Harmful (Xn)
Irritant (Xi)
R-phrases R22, R36/38
S-phrases (S2), S46
NFPA 704
0
1
0
Flash point Non-flammable
Thermochemistry
Std enthalpy of
formation
ΔfHo298
−929 kJ·mol−1[1]
Standard molar
entropy
So298
121 J·mol−1·K−1[1]
Related compounds
Other cations Cobalt(II) sulfate
Copper(II) sulfate
Manganese(II) sulfate
Nickel(II) sulfate
Related compounds Iron(III) sulfate
 N (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Iron(II) sulfate (Br.E. iron(II) sulphate) or ferrous sulfate is the chemical compound with the formula FeSO4. It is used medically to treat iron deficiency, and also for industrial applications. Known since ancient times as copperas and as green vitriol, the blue-green heptahydrate is the most common form of this material. All iron sulfates dissolve in water to give the same aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic.

Hydrates

Iron(II) sulfate can be found in various states of hydration, and several of these forms exist in nature.

  • FeSO4·H2O (mineral: szomolnokite, relatively rare)
  • FeSO4·4H2O (mineral: rozenite, white, relatively common, may be dehydratation product of melanterite)
  • FeSO4·5H2O (mineral: siderotil, relatively rare)
  • FeSO4·6H2O (mineral: ferrohexahydrite, relatively rare)
  • FeSO4·7H2O (mineral: melanterite, blue-green, relatively common)

At 90 °C, the heptahydrate loses water to form the colorless monohydrate. In its anhydrous, crystalline state, its standard enthalpy of formation is ΔfH°solid = -928.4 kJ·mol−1 and its standard molar entropy is S°solid = 107.5 J·K−1·mol−1. All mentioned mineral forms are connected with oxidation zones of Fe-bearing ore beds (pyrite, marcasite, chalcopyrite, etc.) and related environments (like coal fire sites). Many undergo rapid dehydration and sometimes oxidation.

Production and reactions

In the finishing of steel prior to plating or coating, the steel sheet or rod is passed through pickling baths of sulfuric acid. This treatment produces large quantities of iron(II) sulfate as a by-product.[2]

Fe + H2SO4 → FeSO4 + H2

Another source of large amounts results from the production of titanium dioxide from ilmenite via the sulfate process.

Ferrous sulfate is also prepared commercially by oxidation of pyrite:

2 FeS2 + 7 O2 + 2 H2O → 2 FeSO4 + 2 H2SO4

Reactions

On heating, iron(II) sulfate first loses its water of crystallization and the original green crystals are converted into a brown colored anhydrous solid. When further heated, the anhydrous material releases sulfur dioxide and white fumes of sulfur trioxide, leaving a reddish-brown iron(III) oxide. Decomposition of iron(II) sulfate begins at about 480 °C.

2 FeSO4 → Fe2O3 + SO2 + SO3

Like all iron(II) salts, iron(II) sulfate is a reducing agent. For example, it reduces nitric acid to nitrogen oxide and chlorine to chloride:

6 FeSO4 + 3 H2SO4 + 2 HNO3 → 3 Fe2(SO4)3 + 4 H2O + 2 NO
6 FeSO4 + 3 Cl2 → 2 Fe2(SO4)3 + 2 FeCl3


Upon exposure to air, it oxidizes to form a corrosive brown-yellow coating of basic ferric sulfate, which is an adduct of ferric oxide and ferric sulfate:

12 FeSO4 + 3 O2 → 4 Fe2(SO4)3 + 2 Fe2O3

Uses

Industrially, ferrous sulfate is mainly used as a precursor to other iron compounds. It is a reducing agent, mostly for the reduction of chromate in cement.

Nutritional supplement

Together with other iron compounds, ferrous sulfate is used to fortify foods and to treat iron-deficiency anemia. Constipation is a frequent and uncomfortable side effect associated with the administration of oral iron supplements. Stool softeners often are prescribed to prevent constipation.

Colorant

Ferrous sulfate was used in the manufacture of inks, most notably iron gall ink, which was used from the middle ages until the end of the eighteenth century. Chemical tests made on the Lachish letters [circa 588/6 BCE] showed the possible presence ... of iron (Torczyner, Lachish Letters, pp. 188-95). It is thought that oak galls and copperas may have been used in making the ink on those letters.[3] It also finds use in wool dyeing as a mordant. Harewood, a material used in marquetry and parquetry since the 17th century, is also made using ferrous sulfate.

Two different methods for the direct application of indigo dye were developed in England in the eighteenth century and remained in use well into the nineteenth century. One of these, known as china blue, involved iron(II) sulfate. After printing an insoluble form of indigo onto the fabric, the indigo was reduced to leuco-indigo in a sequence of baths of ferrous sulfate (with reoxidation to indigo in air between immersions). The china blue process could make sharp designs, but it could not produce the dark hues of other methods. Sometimes, it is included in canned black olives as an artificial colorant.

Ferrous sulfate can also be used to stain concrete and some limestones and sandstones a yellowish rust color.[4]

Woodworkers use ferrous sulfate solutions to color maple wood a silvery hue.

Other uses

In horticulture it is used for treating iron chlorosis.[5] Although not as rapid-acting as iron chelate, its effects are longer-lasting. It can be mixed with compost and dug into to the soil to create a store which can last for years.[6] It is also used as a lawn conditioner,[6] and moss killer.

In the second half of the 19th century, ferrous sulfate was also used as a photographic developer for collodion process images.

Ferrous sulfate is sometimes added to the cooling water flowing through the brass tubes of a turbine condenser. It forms a corrosion-resistant, protective coating on the inside of the tube.

It is used as a gold refining chemical to precipitate metallic gold from auric chloride solutions (gold that has been dissolved into solution with aqua regia).

It has been applied for the purification of water by flocculation and for phosphate removal in municipal and industrial sewage treatment plants to prevent eutrophication of surface water bodies.

It is used as a traditional method of treating wood panel on houses, either alone, dissolved in water, or as a component of water-based paint.

Green vitriol is also a useful reagent in the identification of mushrooms.[7]

See also

References

External links

  • How to Make Copperas (Iron Sulfate) from Pyrites
  • Template:Cite AmCyc
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