fluorosulfonic acid
fluorosulfonic acid
CAS: 7789-21-1
Molecular Formula: FHO3S
fluorosulfonic acid - Names and Identifiers
| Name | fluorosulfonic acid |
| Synonyms | HSO3F fluorosulfonic fluosulfuricacid FLUOSULFONIC ACID Fluorosulforic Acid FLUOROSULFONIC ACID FLUOROSULFURIC ACID fluorosulfonic acid Fluorosulphonic acid fluorosulphuric acid sulfurofluoridic acid monofluorosulfuricacid fluorosulfuricacid(hso3f) |
| CAS | 7789-21-1 |
| EINECS | 232-149-4 |
| InChI | InChI=1/FHO3S/c1-5(2,3)4/h(H,2,3,4) |
fluorosulfonic acid - Physico-chemical Properties
| Molecular Formula | FHO3S |
| Molar Mass | 100.07 |
| Density | 1.726g/mLat 25°C(lit.) |
| Melting Point | −87.3°C(lit.) |
| Boling Point | 165.5°C(lit.) |
| Water Solubility | hydrolyzes violently in H2O; reddish?brown color in acetone [MER06] |
| Vapor Presure | 2.5 mm Hg ( 25 °C) |
| Vapor Density | 3.5 (vs air) |
| Appearance | colorless liquid |
| Merck | 13,4206 |
| pKa | -6.29±0.15(Predicted) |
| Storage Condition | 2-8°C |
| Stability | Stable. May corrode glass. Incompatible with many metals, bases. |
| Refractive Index | 1.392 |
| Use | Polymerization, degradation and foreign body formation of inactive alkanes in superacid |
fluorosulfonic acid - Risk and Safety
| Risk Codes | R20 - Harmful by inhalation R35 - Causes severe burns |
| Safety Description | S26 - In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. S45 - In case of accident or if you feel unwell, seek medical advice immediately (show the label whenever possible.) |
| UN IDs | UN 1777 8/PG 1 |
| WGK Germany | 1 |
| RTECS | LP0715000 |
| Hazard Note | Corrosive/Toxic |
| Hazard Class | 8 |
| Packing Group | I |
fluorosulfonic acid - Reference Information
| EPA chemical substance information | information provided by: ofmpeb.epa.gov (external link) |
| important acidic solvent | fluorosulfonic acid is an important acidic solvent, acid is stronger than perchloric acid, is the strongest in simple acid, chemical formula HSO3F, molecular weight 100.07, Colorless fuming liquid, melting point -87.3 ℃, boiling point 165.5 ℃, relative density of 1.74315. The thermal stability of pure fluorosulfonic acid is high, and it is still stable when heated to 900 ° C., and the impurity sulfur makes it completely decomposed at the boiling point. Smoke is produced in moist air. Can dissolve sulfur, lead, mercury, tin. Dissolved in nitrobenzene, soluble in water and explosive reaction with water, also soluble in alkali. At room temperature does not react with sulfur, carbon, selenium, tellurium, lead, etc., but can react with tin to generate gas, slightly able to attack Mercury. Can quickly damage the rubber, Cork, fire paint. The pure product does not corrode the glass. Sulfur, lead, tin and mercury are strongly eroded by heating. It reacts with benzene and chloroform to generate hydrogen fluoride, and reacts with ether to release a large amount of heat and foam to generate ethyl ester. With sodium chloride to the role of its sodium salt. The dried hydrogen fluoride is reacted with sulfur trioxide or with concentrated sulfuric acid to obtain a fluorosulfonic acid product. purposes: fluorosulfonic acid can be used as a fluorinating agent in organic and inorganic synthesis, and is a catalyst for alkyl substitution, acylation, hydrofluorination and polymerization. |
| Super acid | Super acid usually acid or acidic medium with acid strength exceeding 100% sulfuric acid, such as fluorosulfonic acid (HSO3F) is an important acidic solvent, the acid in addition to sulfuric acid (H2S2O7), than any of the pure acid to be strong. When antimony pentafluoride (SbF5) or a mixture of antimony pentafluoride and sulfur trioxide is added to the fluorosulfonic acid, a more acidic solvent can be obtained. Super acid has a strong protonation ability, high acidity, generally 106 to 1010 times stronger than inorganic acid. If the acidity function H0 is used to measure the acidity of super acid, it can be said that the acidity function H0<-11.9 of the acidic system is super acid, because H0 of 100% sulfuric acid is -11.9. So perchloric acid (H0 -13.0), chlorosulfonic acid (H0 -13.8), pyrosulfuric acid (H0 -14.4), fluorosulfonic acid (H0 -15.1), hydrogen fluoride (H0 is − 15.1) and the like are all superacids. Super Acids are mostly inorganic acids. According to the state, can be divided into liquid super acid and solid super acid. According to the composition, it can be divided into proton acid, Lewis acid and conjugated proton-Lewis acid. HF,HClO4,HSO3Cl,HSO3F and HSO3CF3, etc., are protic superacids. SbF5,AsF5,TaF5 and NbF5 are all Lewis super acids, and SbF5 is the strongest Lewis acid known at present. H2SO4 · SO3(H2S2O7), H2SO4 · B(OH)3,HSO3F · SbF5, HSO3F · SO3 and other systems consisting of a proton acid and a Lewis acid are proton-Lewis superacids. Fluorosulfonic acid containing 90mol% of SbF5 mixed acid, H0 -27, is currently the highest acidity of the acid, is the most widely used super acid, also known as the acid. Super acid has a high strength of acid and high dielectric constant, can make the non electrolyte electrolyte, can make the weak base protonation. Therefore, super acid has a wide range of applications in chemical research and chemical production. The super acid can produce a stable solution of alkane positive carbon ions, can also produce many halogen positive ions, and can even obtain stable crystalline salts of these ions. Especially as a good catalyst, super acid can make some difficult to carry out the reaction can be carried out under mild conditions, in organic synthesis has been widely used. Liquid super acid can be used as a catalyst for saturated hydrocarbon cracking, re-polymerization, isomerization and alkylation, and solid super acid is used as a catalyst for n-hexane isomerization, low molecular weight polymerization and the like in petrochemical industry. |
| Use | polymerization and degradation of inactive alkanes in superacid, foreign body reaction |
| production method | 1. Fluorosulfonic acid can be formed by reacting potassium fluorohydride with fuming sulfuric acid. Add 40ml of fuming sulfuric acid (containing about 60% of SO3) to a platinum or aluminum dish cooled with an ice-salt cold bath, 20g of dried and pulverized potassium fluorohydride KHF2 was slowly added to fuming sulfuric acid with stirring. This can form a viscous mass, some smoke in the air. This was followed by slow heating to 100 °c to drive off excess SO3 and HF. The product was placed in a Jena glass distillation unit with a mill tip, gradually heated to 250 ° C., and HSO3F was distilled off. After the second distillation, the fluorosulfonic acid obtained was already very pure. Fluorosulfonic acid can be formed by the reaction of chlorosulfonic acid with hydrogen fluoride. A silver distillation flask with a silver dropping funnel was used as a reaction flask, which was cooled in an ice-salt bath, and 50g of anhydrous HF was distilled from the gas outlet tube of the reaction flask into the reaction flask, the end of the outlet tube is then connected to a steel drying tube, which is filled with KF in order to absorb HF entrained in the gas. HSO3Cl was added to the reaction flask from the dropping funnel, and the reaction started immediately, and HCl gas was uniformly evolved. After completion of the reaction, a flow of dry air was introduced into the reaction flask, and the temperature was slowly increased to 110 ° C. To blow off excess HF and residual HCl. The remaining material in the reaction flask was chlorine-free HSO3F. Completely pure fluorosulfonic acid can be stored in sealed glass ampoules or in aluminum containers. |
| category | corrosive article |
| flammability hazard characteristics | exposure to air and heating smoke release toxic gases; Exposure to H porogen is flammable; toxic fluoride and phosphorus oxide fumes from combustion |
| storage and transportation characteristics | The warehouse was ventilated and dried at low temperature, separate storage of bases |
| extinguishing agent | Sand, carbon dioxide; No water |
| Occupational Standard | TWA 2.5 mg (fluorine)/m3 |
| toxic substance data | information provided by: pubchem.ncbi.nlm.nih.gov (external link) |
Last Update：2024-04-09 19:05:15
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