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Seller Store backyard-science-2000
(775) 99.2%,
Location: Salt Lick, Kentucky
Ships to: US,
Item: 334593494056
All returns accepted:ReturnsNotAccepted
Backyard Science 2000:Backyard Science 2000
Volume/Quantity:100g
EPA Registration Number:7782-63-0
Common Name:Ferric Sulfate
Custom Bundle:No
1.1:1.1
MPN:BYS-FERR.SULF.100.G-2K
Country/Region of Manufacture:United States
Modified Item:No
Preferred IUPAC Name:Ferrous Sulfate Heptahydrate
Intended Use/Discipline:Biological Laboratory,Physical Laboratory
California Prop 65 Warning:N/A
Ferrous Sulfate Heptahydrate, 100g, FeSO4 7H2O, 98% purity. AKA: Iron II Sulfate About: The hydrated form is used medically to treat iron deficiency, and also for industrial applications. Known since ancient times as copperas and as green vitriol (vitriol is an archaic name for sulfate), the blue-green heptahydrate (hydrate with 7 molecules of water) is the most common form of this material. All the iron(II) sulfates dissolve in water to give the same aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic. The name copperas dates from times when the copper(II) sulfate was known as blue copperas, and perhaps in analogy, iron(II) and zinc sulfate were known respectively as green and white copperas. It is on the World Health Organization’s List of Essential Medicines. In 2020, it was the 116th most commonly prescribed medication in the United States, with more than 5 million prescriptions(this is not a prescription medication!!!!). 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 iron gall ink. 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. Iron(II) sulfate is sold as ferrous sulfate, a soil amendment for lowering the pH of a high alkaline soil so that plants can access the soil’s nutrients. In horticulture it is used for treating iron chlorosis. 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. Ferrous sulfate can be used as a lawn conditioner. It can also be used to eliminate silvery thread moss in golf course putting greens. Ferrous sulfate can be used to stain concrete and some limestones and sandstones a yellowish rust color. Woodworkers use ferrous sulfate solutions to color maple wood a silvery hue. Green vitriol is also a useful reagent in the identification of mushrooms. 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 18th century. Chemical tests made on the Lachish letters (c.588586 BCE) showed the possible presence of iron. It is thought that oak galls and copperas may have been used in making the ink on those letters. 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 18th century and remained in use well into the 19th 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. In the second half of the 1850s ferrous sulfate was used as a photographic developer for collodion process images. 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. 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 It can be produced by displacement of metals less reactive than Iron from solutions of their sulfate: CuSO4 + Fe FeSO4 + Cu 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 white anhydrous solid. When further heated, the anhydrous material decomposes into sulfur dioxide and sulfur trioxide, leaving a reddish-brown iron(III) oxide. Thermolysis of iron(II) sulfate begins at about 680 C (1,256 F). Fe_2O_3 + SO_2 + SO_3 Like other 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 Its mild reducing power is of value in organic synthesis. It is used as the iron catalyst component of Fenton’s reagent. Ferrous sulfate can be detected by the cerimetric method, which is the official method of the Indian Pharmacopoeia. This method includes the use of ferroin solution showing a red to light green colour change during titration. Will come in vacuum sealed bags. These bags will be labeled, then bubble wrapped and shipped via USPS First Class Mail with Tracking. I wrote 98% purity because there are some small dots of decomposed product. This is just a tiny bit of decomposition that came from the supplier. It can be filtered out when the material is dissolved in solution. Everything should be filtered after it’s dissolved anyways. It could probably be labeled as >99%, but I’d rather label it a bit lower to grab your attention to get you to read this. This won’t hurt anything at all for 99% of the reactions that can be done with this materials. If it is extremely complicated and requires many, many specific conditions to be met for the reaction, then you’ll want to purify. But dissolving and filtering will do that anyways. So this material is perfectly fine for almost any reaction. If it ruins your reaction let me know and we’ll do something about it. For sure! Shipped via USPS First Class Mail.
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