Iron (II) sulfate (English English: iron (II) sulfate ) or iron sulfate indicates various salts of the formula FeSO 4 Ã, Â · x H 2 O. These compounds exist most often as heptahydrate ( x Ã, = Ã, 7 ) but is known for some values ​​ x . Hydrated forms are used medically to treat iron deficiency, and also for industrial applications. Known since ancient times as copperas and as green vitriol , blue-green heptahydrate is the most common form of this material. All iron (II) sulfates dissolve in water to give the same aquo complexes [Fe (H 2 O) 6 ] 2 , which has a geometry octralral molecules and are paramagnetic. The name Copperas comes from an age when copper (II) sulfate is known as blue copper, and possibly in analogy, iron (II) and zinc sulfate are known respectively as green and white copper.
It's in the List of Essential Medicines of the World Health Organization, the most important drugs needed in basic health systems.
Video Iron(II) sulfate
Usage
Industrially, iron sulfate is primarily used as a precursor for other iron compounds. It is a reducing agent, and is thus useful for the reduction of chromate in cement into less toxic Cr (III) compounds. Historically, iron sulfate has been used in the textile industry for centuries as a dye. It is used historically to discolor the skin and as an ink constituent. The preparation of sulfuric acid ('vitriol' oil) by vitriol green distillation (Iron (II) sulfate) has been known for at least 700 years.
Medical use
Together with other iron compounds, iron sulfate is used to fortify food and to treat and prevent iron deficiency anemia. Constipation is a frequent and uncomfortable side effect associated with oral iron supplementation. Dirt softeners are often prescribed to prevent constipation.
Colorant
Ferrous sulfate is used in the manufacture of inks, especially iron inks, which were used from the mid to late 18th century. Chemical tests performed on the Lakhis ( c. 588-586Ã, BCE) indicate the possibility of iron. It is thought that galls oak and copperas may have been used in making the ink on the letters. He also finds use in dyeing wool as a mordant. Harewood, a material used in marquetry and parquet since the 17th century, was also made using iron sulphate.
Two different methods for direct application of indigo dye were developed in England in the eighteenth century and remained in good use until the nineteenth century. One of them, known as china blue , involves iron (II) sulfate. After printing the indigo-insoluble shape into the fabric, indigo is reduced to leuco -indigo in the bath sulfate bath sequence (by reoxidation to indigo in air between dyeing). The Chinese blue process can create sharp designs, but can not produce dark colors from other methods.
Sometimes, it is included in a canned black olive as an artificial coloring.
Ferrous sulfate can also be used to stain the concrete and some claystone and yellowish rust sandstones.
Carpenters use a solution of iron sulfate to dye maple wood with silvery colors.
Plant growth
Iron (II) sulfate is sold as iron sulphate, an amendment of soil to lower the pH of high alkaline so that the plant can access soil nutrients.
In horticulture is used to treat iron chlorosis. Although not fast acting as iron edta, the effect is more durable. Can be mixed with compost and dug into the ground to create a store that can last for years. It is also used as a grass conditioner, and a moss killer.
Other uses
In the second half of the 1850s iron sulphate was used as a photographic developer for collodion process images.
Ferrous sulfate is sometimes added to the cooling water flowing through the turbine condenser brass tube to form a corrosion-resistant protective coating.
It is used in the purification of gold to precipitate metallic gold from auric chloride solution (gold dissolved in solution with aqua regia).
It has been used in water purification by flocculation and for phosphate removal at municipal and industrial waste mills to prevent eutrophication of surface water bodies.
It is used as a traditional method of treating wood panels in homes, either alone, dissolved in water, or as a component of water-based paint.
Green vitriol is also a useful reagent in the identification of fungi.
Maps Iron(II) sulfate
Hydrate
Iron (II) sulfate can be found in various hydration states, and some of these forms exist in nature.
- FeSO 4 Ã, Â · H 2 O (minerals: Szomolnokite, relatively rare)
- FeSO 4 O (minerals: Rozenite, white, relatively common, possibly melanterite dehydratation product)
- FeSO 4 Ã, Â · 5H 2 O (minerals: Siderotil, relatively rare)
- FeSO 4 Ã, Â · 6H 2 O (minerals: Ferrohexahydrite, relatively rare)
- FeSO 4 Ã, Â · 7H 2 O (minerals: Melanterite, blue-green, relatively common)
Tetrahydrate is stabilized when the aqueous solution temperature reaches 56.6 Â ° C (133.9 Â ° F). At 64.8 Â ° C (148.6 Â ° F) this solution forms both the tetrahydrate and the monohydrate.
All the mineralized forms mentioned are related to the oxidation zones of iron ore beds (pyrite, marcasite, chalcopyrite, etc.) and related environments (such as coal fire sites). Many have rapid dehydration and sometimes oxidation.
Production and reaction
In the steel finish prior to coating or coating, sheets or steel rods are passed through the acid sulphate acid bath. This treatment produces large amounts of iron (II) sulfate as a by-product.
- Fe H 2 SO 4 -> FeSO 4 H 2
Other sources of large quantities result from the production of titanium dioxide from ilmenite through the sulphate process.
Ferrous sulfate is also commercially prepared with pyrite oxidation:
- 2 FeS 2 2a, 2 <2 2 2 -> 2Ã, FeSO 4 2Ã, H 2 SO 4
Reactions
After dissolving in water, the iron sulfate forms a metal aquo complex [Fe (H 2 O) 6 ] 2 , which is almost colorless, a paramagnetic ion.
In heating, the first iron (II) sulfate loses the water of crystallization and the original green crystal is converted to a brown anhydrous solid. When heated further, the anhydrous material releases sulfur dioxide and white smoke from sulfur trioxide, leaving a reddish-brown (III) oxide iron. The decomposition of iron (II) sulphate starts at about 680 ° C (1.256 ° F).
- 2 FeSO 4 -> Fe 2 O 3 SO 2 SO 3
Like all iron (II) salts, iron (II) sulfate is the reducing agent. For example, reducing nitric acid to nitrogen monoxide and chlorine to chloride:
- 6Ã, FeSO 4 3Ã, H 2 SO 4 2 HNO 3 -> 3 Fe 2 (SO 4 ) 3 4Ã, H 2 O 2 NOTHING
- 6Ã, FeSO 4 3Ã, Cl 2 -> 2Ã, Fe 2 (SO 4 ) < sub> 3 2Ã, FeCl 3
After exposure to air, it oxidizes to form a corrosive brown-yellow layer of "base iron sulfate", which is an adduct of iron (III) oxide and iron (III) sulfate:
- 12Ã, FeSO 4 3Ã, 2 -> 4Ã, Fe 2 (SO 4 ) 3 2Ã, Fe 2 O 3
See also
- Iron (III) sulphate (iron sulphate), other common common sulfate of iron.
- Copper (II) sulfate Ammonium iron (II) sulfate, also known as Mohr's salt, is a common double salt of ammonium sulfate with iron (II) sulfate.
- Chalcanthum
- Ephraim Seehl is known as the earliest manufacturer of green vitriol.
References
External links
Source of the article : Wikipedia
0 Comments