1. Uses
    Medical use  Colorant  Plant growth  Other uses 

2. Hydrates

3. Production and reactions
    Reactions 

4. See also

5. References

6. External links

It is on the World Health Organization's List of Essential Medicines, the most important medications needed in a basic health system.^[9]

Uses

Industrially, ferrous sulfate is mainly used as a precursor to other iron compounds. It is a reducing agent, and as such is useful for the reduction of chromate in cement to less toxic Cr(III) compounds. Historically ferrous sulfate was used in the textile industry for centuries as a dye fixative. It is used historically to blacken leather and as a constituent of ink.^[10] The preparation of sulfuric acid ('oil of vitriol') by the distillation of green vitriol (Iron(II) sulfate) has been known for at least 700 years.

Medical use

Together with other iron compounds, ferrous sulfate is used to fortify foods and to treat and prevent 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}}588–586 BCE) showed the possible presence of iron.^[11] It is thought that oak galls and copperas may have been used in making the ink on those letters.^[12] 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.^[13]

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

Plant growth

Iron (II) sulfate is sold as ferrous sulfate, a soil amendment^[14] for lowering the pH of a high alkaline soil so that plants can access the soil's nutrients.^[15]

In horticulture it is used for treating iron chlorosis.^[16] Although not as rapid-acting as ferric edta, its effects are longer-lasting. It can be mixed with compost and dug into the soil to create a store which can last for years.^[17] It is also used as a lawn conditioner,^[17] and moss killer.

Other uses

In the second half of the 1850s ferrous sulfate was used as a photographic developer for collodion process images.^[18]

Ferrous sulfate is sometimes added to the cooling water flowing through the brass tubes of turbine condensers to form a corrosion-resistant protective coating.

It is used in gold refining to precipitate metallic gold from auric chloride solutions (gold dissolved in solution with aqua regia).

It has been used in the purification of water by flocculation and for phosphate removal in municipal and industrial sewage treatment plants to prevent eutrophication of surface water bodies.{{Citation needed|reason=the flocculation article also lacks references|date=August 2008}}

It is used as a traditional method of treating wood panelling{{clarify|Houses are not "panelled", they are "sided" in wood|date=June 2016}} on houses, either alone, dissolved in water, or as a component of water-based paint.{{citation needed|date=June 2016}}

Green vitriol is also a useful reagent in the identification of mushrooms.^[19]

It is used as the iron catalyst component of Fenton's reagent.

In the early 19th century, chemist Friedrich Accum discovered that in England the dark beer porter often contained Iron(II) sulfate as a frothing agent.^[20]

Hydrates

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

• FeSO₄·H₂O (mineral: Szomolnokite,^[21] relatively rare)
• FeSO₄·4H₂O (mineral: Rozenite,^[22] white, relatively common, may be dehydratation product of melanterite)
• FeSO₄·5H₂O (mineral: Siderotil,^[23] relatively rare)
• FeSO₄·6H₂O (mineral: Ferrohexahydrite,^[24] relatively rare)
• FeSO₄·7H₂O (mineral: Melanterite,^[25] blue-green, relatively common)

The tetrahydrate is stabilized when the temperature of aqueous solutions reaches {{convert|56.6|C|F}}. At {{convert|64.8|C|F}} these solutions form both the tetrahydrate and monohydrate.^[26]

All mentioned mineral forms are connected with oxidation zones of iron-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.^[27]

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

Upon dissolving in water, ferrous sulfates form the metal aquo complex [Fe(H₂O)₆]²⁺, which is an almost colorless, paramagnetic ion.

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 {{convert|680|C|F}}.

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 monoxide 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 iron(III) oxide and iron(III) sulfate:

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

See also

• Iron(III) sulfate (ferric sulfate), the other common simple sulfate of iron.
• Copper(II) sulfate
• Ammonium iron(II) sulfate, also known as Mohr's salt, the common double salt of ammonium sulfate with iron(II) sulfate.
• Chalcanthum
• Ephraim Seehl known as an early manufacturer of green vitriol.^[28]

References

External links

• {{cite web |url=http://www.chemicalland21.com/industrialchem/inorganic/FERROUS%20SULFATE%20HEPTAHYDRATE.htm |title=Product Information |publisher=Chemical Land21 |date=January 10, 2007}}
• How to Make Copperas (Iron Sulfate) from Pyrites
• {{cite AmCyc |last=Hunt |first=T. Sterry |authorlink=T. Sterry Hunt |wstitle=Copperas |short=x}}

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