Ferrous sulfate CAS 7720-78-7
Introduction：Basic information about Ferrous sulfate CAS 7720-78-7, including its chemical name, molecular formula, synonyms, physicochemical properties, and safety information, etc.
Ferrous sulfate Basic informationChemical and Physical Properties Uses Toxicity Hazards & Safety Information
| Product Name: | Ferrous sulfate |
| Synonyms: | Iron(Ⅱ) sulfate;ferric potassium alum;potassium ferric sulfate;FERROUS SULFATE;FERROIN SOLUTION;FERROUS SULPHATE;IRON(II) SULFATE;COPPERAS |
| CAS: | 7720-78-7 |
| MF: | FeO4S |
| MW: | 151.91 |
| EINECS: | 231-753-5 |
| Product Categories: | INORGANIC & ORGANIC CHEMICALS;Inorganics;Industry grade;Food Additives;7720-78-7 |
| Mol File: | 7720-78-7.mol |
Ferrous sulfate Chemical Properties
| Melting point | decomposes at 671℃ [JAN85] |
| density | 3.650 |
| vapor pressure | 0Pa at 20℃ |
| storage temp. | Store at +15°C to +25°C. |
| solubility | Water (Slightly) |
| form | white orthorhombic crystals |
| color | white orthorhombic crystals, crystalline; hygroscopic |
| PH | 2.5 (20°C, 50g/L in H2O) |
| Odor | at 100.00?%. odorless |
| Water Solubility | g/100g solution H2O: 13.6 (0°C), 22.8 (25°C), 24.0 (100°C); solid phase, FeSO4 · 7H2O (0°C, 25°C), FeSO4 ·H2O (100°C) [KRU93] |
| Dielectric constant | 14.2（14℃） |
| Cosmetics Ingredients Functions | ASTRINGENT |
| InChI | InChI=1S/Fe.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 |
| InChIKey | BAUYGSIQEAFULO-UHFFFAOYSA-L |
| SMILES | [Fe+2].S([O-])([O-])(=O)=O |
| CAS DataBase Reference | 7720-78-7(CAS DataBase Reference) |
| NIST Chemistry Reference | Ferrous sulfate(7720-78-7) |
| EPA Substance Registry System | Ferrous sulfate (7720-78-7) |
Safety Information
| Risk Statements | 25 |
| Safety Statements | 45 |
| WGK Germany | WGK 2 |
| TSCA | TSCA listed |
| HS Code | 28332910 |
| Storage Class | 12 - Non Combustible Liquids |
| Hazard Classifications | Aquatic Chronic 3 |
| Hazardous Substances Data | 7720-78-7(Hazardous Substances Data) |
| Toxicity | LD50 oral in rat: 319mg/kg |
| Chemical and Physical Properties | Ferrous sulfate, also known as Ferrous sulphate or green vitriol, is a sulphate of ferrous iron with the chemical formula FeSO₄. It appears as a dull blue-green monoclinic crystalline powder or granules. Odourless, it possesses a salty, astringent taste. It deliquesces in dry air and readily oxidises to form brownish-yellow basic ferric sulphate in humid conditions. A 10% aqueous solution exhibits acidity towards litmus (pH approximately 3.7). Upon heating to 70–73°C, it loses three molecules of water; at 80–123°C, it loses six molecules of water; and above 156°C, it transforms into basic ferric sulphate. It is readily soluble in water (1g/1.5ml at 25°C or 1g/0.5ml in boiling water) but insoluble in ethanol. Green vitriol refers to its heptahydrate form, FeSO₄·7H₂O, which contains 19% iron (Fe). The pure substance forms green crystals. Upon exposure to air, it gradually oxidises to form basic ferric sulphate, appearing yellowish-brown. It dissolves in water, yielding an acidic aqueous solution. Ferrous sulphate exhibits strong acidity and is highly corrosive. It is generally soluble in water; when chlorides are present in the solution, a brownish precipitate forms, also known as iron sulphate rust. The crystalline hydrate of ferrous sulphate at room temperature is the heptahydrate (i.e., ferrous sulphate heptahydrate). The heptahydrate is a blue-green monoclinic crystal that loses six molecules of water of hydration at 64–90°C and is completely dehydrated at 300°C, undergoing partial decomposition simultaneously. It is corrosive, deliquescent in dry air, and readily oxidised by moist air. It is soluble in water (48 g/100 mL) and methanol, and slightly soluble in ethanol. |
| Uses |
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| Toxicity | LD50: 279 to 558 mg/kg (rat, oral, calculated as Fe). GRAS (FDA, § 182.5315, §184.1315, 2000); ADI 0.8 mg Fe/kg (calculated in terms of Fe; FAO/WHO, 2001); |
| Hazards & Safety Information | Category :Toxic substances Toxicity classification: highly toxic Acute Toxicity : Oral-Rat LD50 319 mg/kg; Oral-mouse LD50: 680 mg/kg Flammability and Hazardous characteristics: Non-combustible with fire producing toxic iron-containing fumes Storage and transportation characteristics Treasury: low temperature, ventilated, dry; store separately from food raw materials. Fire extinguishing agent : water, carbon dioxide, dry powder, sand Occupational Standard :TWA 1 mg (iron)/m3 |
| Description | Green vitriol (FeSO₄·7H₂O) has been known since the thirteenth century; it crystallizes from solutions of iron or iron bases in dilute sulfuric acid. The heptahydrate forms green monoclinic crystals with a density of 1.88 and is very soluble in water (296 g L⁻¹ FeSO₄ at 25 °C). The white monohydrate is obtained by precipitating the aqueous solution with ethanol, heating the heptahydrate to 140 °C in vacuo, or crystallizing it from 50% sulfuric acid. This can be further dehydrated to white, amorphous FeSO₄ by heating to 300 °C in a stream of hydrogen. At red heat, the sulfate decomposes: 2FeSO₄ → Fe₂O₃ + SO₂ + SO₃ A tetrahydrate (FeSO₄·4H₂O) crystallizes from aqueous solutions above 56 °C. |
| Chemical Properties | Ferrous sulfate is a greenish or yellowish solid in fine or lumpy crystals. It is odorless, soluble in water (with a saline taste), insoluble in alcohol, and hygroscopic. |
| 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/cm3; 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). |
| Uses | Ferrous sulfate (FeSO4) is also known as iron sulfate or iron vitriol. It is used in the productionof various chemicals, such as sulfur dioxide and sulfuric acid. |
| Uses | Iron Supplement |
| Uses | Ferrous Sulfate is a nutrient and dietary supplement that is a source of iron. it is a white to grayish odorless powder. ferrous sulfate hep-tahydrate contains approximately 20% iron, while ferrous sulfate dried contains approximately 32% iron. it dissolves slowly in water and has high bioavailability. it can cause discoloration and rancidity. it is used for fortification of baking mixes. in the encapsulated form it does not react with lipids in cereal flours. it is used in infant foods, cereals, and pasta products. |
| Definition | A rusty-brown solid prepared by the actionof heat on iron(III) hydroxide or iron(II)sulfate. It occurs in nature as the mineralhematite. Industrially it is obtained byroasting iron pyrites. Iron(III) oxide dissolvesin dilute acids to produce solutionsof iron(III) salts. It is stable at red heat, decomposesaround 1300°C to give triirontetroxide, and can be reduced to iron byhydrogen at 1000°C. Iron(III) oxide is notionic in character but has a structure similarto 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. |
| Hazard | Ingestion causes intestinal disorders. |
| Flammability and Explosibility | Non flammable |
| 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 |
| Safety Profile | A human poison by ingestion. Moderately toxic to humans by an unspecified route. An experimental poison by ingestion, intraduodenal, intraperitoneal, intravenous, and subcutaneous routes. Human systemic effects by ingestion: aggression, somnolence, brain recorlng changes, diarrhea, nausea or vomiting, bleedmg from the stomach, coma. Questionable carcinogen with experimental tumorigenic data. Experimental teratogenic and reproductive effects. Mutation data reported. Potentially explosive reaction with methyl isocyanoacetate at 25'. May igmte on contact with arsenic trioxide + sodium nitrate. When heated to decomposition it emits toxic fumes of SOx. See also IRON COMPOUNDS. |
| Potential Exposure | It is used as a fertilizer, food or feedadditive; and in herbicides; process engraving; dyeing, andwater treatment. A byproduct of various chemical andmetal treating operations. |
| Veterinary Drugs and Treatments | While iron is a necessary trace element in all hemoglobin-utilizinganimals, the use of therapeutic dosages of ferrous sulfate (or otheroral iron) preparations in veterinary medicine is limited primarilyto the treatment of iron-deficiency anemias in dogs (usually due tochronic blood loss), and as adjunctive therapy in cats when receivingepoetin (erythropoietin) therapy. Injectable iron products areusually used in the treatment of iron deficiency anemias associatedwith 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. |
| First aid | If this chemical gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts theskin, remove contaminated clothing and wash immediatelywith soap and water. Seek medical attention immediately. Ifthis chemical has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR ifheart action has stopped. Transfer promptly to a medicalfacility. When this chemical has been swallowed, get medical attention. Give large quantities of water and inducevomiting. Do not make an unconscious person vomit.Note to physician: Gastric lavage with large amounts of 5%sodium phosphate or water. Follow this with a large amountof 1% sodium bicarbonate over a 3-h period.Note to physician: For severe poisoning do not use BAL[British Anti-Lewisite, dimercaprol, dithiopropanol(C3H8OS2)] as it is contraindicated or ineffective in poisoning from iron. |
| 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. |
| Incompatibilities | Aqueous solution is acidic. Contact withalkalies form iron. Keep away from alkalies, soluble carbo nates; gold and silver salts; lead acetate; lime water, potassiumiodide; potassium and sodium tartrate; sodium borate; tannin. |
Ferrous sulfate Preparation Products And Raw materials
| Raw materials | Sulfuric acid-->Iron-->AMMONIUM PENTABORATE-->CERIUM(III) CHLORIDE HEPTAHYDRATE |
| Preparation Products | Iron oxide-->Prussian Blue-->Gentamicin sulfate-->Pigment Yellow 42-->Potassium ferrocyanide trihyrate-->Sodium ferrocyanide-->Foliar-fertilizer-->Triiron tetraoxide-->FE2O3 AS BROWN PIGMENT-->High temperature shift calalyst-->Desulfurizer-->Kanamycin sulfate-->Naphthenate drier-->Ammonium iron(II) sulfate-->Ferric chrome lignin sulfonate-->Iron naphthenate-->Quinhydrone-->Iron Oxide Green |
