Isopropyl alcohol: Difference between revisions
Sternenmeer (talk | contribs) deleted sentence about Sarin because the introductory paragraph is not about specific chemicals manufactured out of isopropanyl |
Enthusiast01 (talk | contribs) Undid revision 837237559 by Sternenmeer (talk)it’s important to note that it is not just a benign chemical |
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'''Isopropyl alcohol''' ([[International Union of Pure and Applied Chemistry|IUPAC]] name '''propan-2-ol'''; commonly called '''isopropanol''') is a [[chemical compound|compound]] with the [[chemical formula]] C<sub>3</sub>H<sub>8</sub>O. It is a [[Transparency and translucency|colorless]], [[Flammability|flammable]] chemical compound with a strong [[odor]]. As an [[isopropyl]] group linked to a [[hydroxyl]] group, it is the simplest example of a [[Alcohol#Systematic names|secondary alcohol]], where the [[alcohol]] carbon atom is attached to two other carbon atoms. It is a [[structural isomer]] of [[1-Propanol|1-propanol]]. It is manufactured for a wide variety of industrial and household uses, and is a common ingredient in chemicals such as [[antiseptic]]s, disinfectants and detergents. |
'''Isopropyl alcohol''' ([[International Union of Pure and Applied Chemistry|IUPAC]] name '''propan-2-ol'''; commonly called '''isopropanol''') is a [[chemical compound|compound]] with the [[chemical formula]] C<sub>3</sub>H<sub>8</sub>O. It is a [[Transparency and translucency|colorless]], [[Flammability|flammable]] chemical compound with a strong [[odor]]. As an [[isopropyl]] group linked to a [[hydroxyl]] group, it is the simplest example of a [[Alcohol#Systematic names|secondary alcohol]], where the [[alcohol]] carbon atom is attached to two other carbon atoms. It is a [[structural isomer]] of [[1-Propanol|1-propanol]]. It is manufactured for a wide variety of industrial and household uses, and is a common ingredient in chemicals such as [[antiseptic]]s, disinfectants and detergents. Isopropanol can also be used in the manufacture of [[sarin]], a toxic [[nerve agent]].<ref name=jp190418>[http://www.jpost.com/Middle-East/Belgium-companies-sold-deadly-chemicals-to-Assad-in-violation-of-sanctions-551224 Belgium companies sold deadly chemicals to Assad in violation of sanctions]</ref> |
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==Properties== |
==Properties== |
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Revision as of 21:25, 19 April 2018
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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Propan-2-ol[2] | |||
| Other names | |||
| Identifiers | |||
3D model (JSmol)
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| 635639 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.000.601 | ||
| 1464 | |||
| KEGG | |||
PubChem CID
|
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| RTECS number |
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| UNII | |||
| UN number | 1219 | ||
CompTox Dashboard (EPA)
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| Properties | |||
| C3H8O | |||
| Molar mass | 60.096 g·mol−1 | ||
| Appearance | Colorless liquid | ||
| Density | 0.786 g/cm3 (20 °C) | ||
| Melting point | −89 °C (−128 °F; 184 K) | ||
| Boiling point | 82.6 °C (180.7 °F; 355.8 K) | ||
| Miscible with water | |||
| Solubility | Miscible with benzene, chloroform, ethanol, ether, glycerin; soluble in acetone | ||
| Acidity (pKa) | 16.5[3] | ||
| -45.794·10−6 cm3/mol | |||
Refractive index (nD)
|
1.3776 | ||
| Viscosity | 2.86 cP at 15 °C 1.96 cP at 25 °C[4] 1.77 cP at 30 °C[4] | ||
| 1.66 D (gas) | |||
| Pharmacology | |||
| D08AX05 (WHO) | |||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
|
Flammable | ||
| GHS labelling: | |||
 
| |||
| Danger | |||
| H225, H319, H336 | |||
| P210, P261, P305+P351+P338 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | Open cup: 11.7 °C (53.1 °F; 284.8 K) Closed cup: 13 °C (55 °F) | ||
| 399 °C (750 °F; 672 K) | |||
| Explosive limits | 2–12.7% | ||
Threshold limit value (TLV)
|
980 mg/m3 (TWA), 1225 mg/m3 (STEL) | ||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose)
|
12800 mg/kg (dermal, rabbit)[citation needed] 3600 mg/kg (oral, mouse) 5045 mg/kg (oral, rat) 6410 mg/kg (oral, rabbit)[6] | ||
LC50 (median concentration)
|
53000 mg/m3 (inhalation, mouse)[citation needed] 12,000 ppm (rat, 8 hr)[6] | ||
LCLo (lowest published)
|
16,000 ppm (rat, 4 hr) 12,800 ppm (mouse, 3 hr)[6] | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible)
|
TWA 400 ppm (980 mg/m3)[5] | ||
REL (Recommended)
|
TWA 400 ppm (980 mg/m3) ST 500 ppm (1225 mg/m3)[5] | ||
IDLH (Immediate danger)
|
2000 ppm[5] | ||
| Safety data sheet (SDS) | External MSDS | ||
| Related compounds | |||
Related alcohols
|
1-Propanol, ethanol, 2-butanol | ||
| Supplementary data page | |||
| Isopropyl alcohol (data page) | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Isopropyl alcohol (IUPAC name propan-2-ol; commonly called isopropanol) is a compound with the chemical formula C3H8O. It is a colorless, flammable chemical compound with a strong odor. As an isopropyl group linked to a hydroxyl group, it is the simplest example of a secondary alcohol, where the alcohol carbon atom is attached to two other carbon atoms. It is a structural isomer of 1-propanol. It is manufactured for a wide variety of industrial and household uses, and is a common ingredient in chemicals such as antiseptics, disinfectants and detergents. Isopropanol can also be used in the manufacture of sarin, a toxic nerve agent.[7]
Properties
Isopropyl alcohol, synonymous with 2-propanol, sec-propyl alcohol, IPA, isopropanol, or rubbing alcohol is miscible in water, ethanol, ether, and chloroform. It will dissolve ethyl cellulose, polyvinyl butyral, many oils, alkaloids, gums and natural resins.[8] Unlike ethanol or methanol, isopropyl alcohol is not miscible with salt solutions and can be separated from aqueous solutions by adding a salt such as sodium chloride. The process is colloquially called salting out, and causes concentrated isopropyl alcohol to separate into a distinct layer.[9]
Isopropyl alcohol forms an azeotrope with water, which gives a boiling point of 80.37 °C (176.67 °F) and a composition of 87.7 wt% (91 vol%) isopropyl alcohol. Water-isopropyl alcohol mixtures have depressed melting points.[9] It has a slightly bitter taste, and is not safe to drink.[9][10]
Isopropyl alcohol becomes increasingly viscous with decreasing temperature and will freeze at −89 °C (−128 °F).
Isopropyl alcohol has a maximum absorbance at 205 nm in an ultraviolet-visible spectrum.[11][12]
Reactions
Isopropyl alcohol can be oxidized to acetone, which is the corresponding ketone. This can be achieved using oxidizing agents such as chromic acid, or by dehydrogenation of isopropyl alcohol over a heated copper catalyst:
- (CH3)2CHOH → (CH3)2CO + H2
Isopropyl alcohol is often used as both solvent and hydride source in the Meerwein-Ponndorf-Verley reduction and other transfer hydrogenation reactions. Isopropyl alcohol may be converted to 2-bromopropane using phosphorus tribromide, or dehydrated to propene by heating with sulfuric acid.
Like most alcohols, isopropyl alcohol reacts with active metals such as potassium to form alkoxides that can be called isopropoxides. The reaction with aluminium (initiated by a trace of mercury) is used to prepare the catalyst aluminium isopropoxide.[13]
Production
In 1994, 1.5 million tonnes of isopropyl alcohol were produced in the United States, Europe, and Japan.[14] It is primarily produced by combining water and propene in a hydration reaction or by hydrogenating acetone.[14][15] There are two routes for the hydration process and both processes require that the isopropyl alcohol be separated from water and other by-products by distillation. Isopropyl alcohol and water form an azeotrope and simple distillation gives a material that is 87.9% by weight isopropyl alcohol and 12.1% by weight water.[16] Pure (anhydrous) isopropyl alcohol is made by azeotropic distillation of the wet isopropyl alcohol using either diisopropyl ether or cyclohexane as azeotroping agents.[14]
Indirect hydration
Indirect hydration reacts propene with sulfuric acid to form a mixture of sulfate esters. This process can use low-quality propene, and is predominant in the USA. These processes give primarily isopropyl alcohol rather than 1-propanol, because adding water or sulfuric acid to propene follows Markovnikov's rule. Subsequent hydrolysis of these esters by steam produces isopropyl alcohol, by distillation. Diisopropyl ether is a significant by-product of this process; it is recycled back to the process and hydrolyzed to give the desired product.[14]
Direct hydration
Direct hydration reacts propene and water, either in gas phase or in liquid phase, at high pressures in the presence of solid or supported acidic catalysts. Higher-purity propylene (> 90%) tends to be required for this type of process.[14] Direct hydration is more commonly used in Europe.
Hydrogenation of acetone
Crude acetone is hydrogenated in the liquid phase over Raney nickel or a mixture of copper and chromium oxide to give isopropyl alcohol. This process is useful, when it is coupled with excess acetone production, such as the cumene process.[14]
Uses
In 1990, 45 thousand metric tons of isopropyl alcohol were used in the United States. The vast majority of isopropyl alcohol was used as a solvent for coatings or for industrial processes. In that year, 5.4 thousand metric tons were consumed for household use and in personal care products. Isopropyl alcohol in particular is popular for pharmaceutical applications,[14] it is presumed due to the low toxicity of any residues. Some isopropyl alcohol is used as a chemical intermediate. Isopropyl alcohol may be converted to acetone, but the cumene process is more significant. It is also used as a gasoline additive.[14]
Solvent
Isopropyl alcohol dissolves a wide range of non-polar compounds. It also evaporates quickly, leaves nearly zero oil traces, compared to ethanol, and is relatively non-toxic, compared to alternative solvents. Thus, it is used widely as a solvent and as a cleaning fluid, especially for dissolving oils. Together with ethanol, n-butanol, and methanol, it belongs to the group of alcohol solvents, about 6.4 million tonnes of which were utilized worldwide in 2011.[17]
Examples of this application include cleaning electronic devices such as contact pins (like those on ROM cartridges), magnetic tape and disk heads (such as those in audio and video tape recorders and floppy disk drives), the lenses of lasers in optical disc drives (e.g., CD, DVD) and removing thermal paste from heatsinks and IC packages (such as CPUs[18]).
Intermediate
Isopropyl alcohol is esterified to give isopropyl acetate, another solvent. It reacts with carbon disulfide and sodium hydroxide to give sodium isopropylxanthate, a herbicide[19] and an ore flotation reagent.[20] Isopropyl alcohol reacts with titanium tetrachloride and aluminium metal to give titanium and aluminium isopropoxides, respectively, the former a catalyst, and the latter a chemical reagent.[14] This compound may serve as a chemical reagent in itself, by acting as a dihydrogen donor in transfer hydrogenation.
Medical
Rubbing alcohol, hand sanitizer, and disinfecting pads typically contain a 60–70% solution of isopropyl alcohol in water. Water is required to open up membrane pores of bacteria, which acts as a gateway inside for isopropyl. A 75% v/v solution in water may be used as a hand sanitizer.[21] Isopropyl alcohol is used as a water-drying aid for the prevention of otitis externa, better known as swimmer’s ear.[22]
Early uses as an anesthetic
Although isopropyl alcohol can be technically used for anesthesia, its many negative drawbacks prohibit this use. Isopropyl alcohol can also be used similarly to ether as a solvent[23] or as an anesthetic by inhaling the fumes or orally. Early uses included using the solvent as general anesthetic for small mammals[24] and rodents by scientists and some veterinarians. However, it was soon discontinued, as many complications arose, including respiratory irritation, internal bleeding, and visual and hearing problems. In rare cases, respiratory failure leading to death in animals was observed.
Automotive
Isopropyl alcohol is a major ingredient in "gas dryer" fuel additives. In significant quantities water is a problem in fuel tanks as it separates from the gasoline and can freeze in the supply lines at low temperatures. Alcohol does not remove water from gasoline; rather, the alcohol solubilizes water in gasoline. Once soluble, water does not pose the same risk as insoluble water, as it will no longer accumulate in the supply lines and freeze, but will be consumed along with the fuel itself. Isopropyl alcohol is often sold in aerosol cans as a windshield or door lock deicer. Isopropyl alcohol is also used to remove brake fluid traces from hydraulic braking systems, so that the brake fluid (usually DOT 3, DOT 4, or mineral oil) does not contaminate the brake pads, which would result in poor braking.
Laboratory
As a biological specimen preservative, isopropyl alcohol provides a comparatively non-toxic alternative to formaldehyde and other synthetic preservatives. Isopropyl alcohol solutions of 70–99% are used to preserve specimens.
Isopropyl alcohol is often used in DNA extraction. It is added to a DNA solution in order to precipitate the DNA which then forms a pellet after centrifugation. This is possible because DNA is insoluble in isopropyl alcohol.
Safety
Isopropyl alcohol vapor is denser than air and is flammable, with a flammability range of between 2 and 12.7% in air. It should be kept away from heat and open flame.[25] Distillation of isopropyl alcohol over magnesium has been reported to form peroxides, which may explode upon concentration.[26][27] Isopropyl alcohol is a skin irritant.[25]
Toxicology
Isopropyl alcohol and its metabolite, acetone, act as central nervous system (CNS) depressants,[28] and around 15 g of isopropyl alcohol can have a toxic effect on a 70-kg human if left untreated.[29] Poisoning can occur from ingestion, inhalation, or skin absorption. Symptoms of isopropyl alcohol poisoning include flushing, headache, dizziness, CNS depression, nausea, vomiting, anesthesia, hypothermia, hypotension, shock, respiratory depression, and coma.[28] Overdoses may cause a fruity odor on the breath as a result of its metabolism to acetone.[30] Isopropyl alcohol does not cause an anion gap acidosis but it produces an osmolal gap between the calculated and measured osmolalities of serum, as do the other alcohols.[28]
Isopropyl alcohol is oxidized to form acetone by alcohol dehydrogenase in the liver,[28] and has a biological half-life in humans between 2.5 and 8.0 hours.[28] Unlike methanol or ethylene glycol poisoning, the metabolites of isopropyl alcohol are less toxic, and treatment is largely supportive. Furthermore, there is no indication for the use of fomepizole, an alcohol dehydrogenase inhibitor, unless co-ingestion with methanol or ethylene glycol is suspected.[31]
Isopropyl alcohol is denatured for certain uses, in which case the NFPA 704 rating[clarification needed] is changed to 2,3,1.[citation needed]
History
In 1920, Standard Oil first produced isopropyl alcohol by hydrating propene. Its major use at the time was not rubbing alcohol but for oxidation to acetone, whose first major use was in World War One for the preparation of the smokeless propellant, cordite.[32]
References
- ^ "Alcohols Rule C-201.1". Nomenclature of Organic Chemistry (The IUPAC 'Blue Book'), Sections A, B, C, D, E, F, and H. Oxford: Pergamon Press. 1979.
Designations such as isopropanol, sec-butanol, and tert-butanol are incorrect because there are no hydrocarbons isopropane, sec-butane, and tert-butane to which the suffix "-ol" can be added; such names should be abandoned. Isopropyl alcohol, sec-butyl alcohol, and tert-butyl alcohol are, however, permissible (see Rule C-201.3) because the radicals isopropyl, sec-butyl, and tert-butyl do exist.
- ^ Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 631. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
- ^ Reeve, W.; Erikson, C.M.; Aluotto, P.F. (1979). "A new method for the determination of the relative acidities of alcohols in alcoholic solutions. The nucleophilicities and competitive reactivities of alkoxides and phenoxides". Can. J. Chem. 57 (20): 2747–2754. doi:10.1139/v79-444.
- ^ a b Yaws, C.L. (1999). Chemical Properties Handbook. McGraw-Hill. ISBN 0-07-073401-1.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0359". National Institute for Occupational Safety and Health (NIOSH).
- ^ a b c "Isopropyl alcohol". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ Belgium companies sold deadly chemicals to Assad in violation of sanctions
- ^ Doolittle, Arthur K. (1954). The Technology of Solvents and Plasticizers. New York: John Wiley & Sons, Inc. p. 628.
- ^ a b c The Merck Index (10th ed.). Rahway, NJ: Merck & Co. 1983. p. 749.
- ^ Logsden, John E.; Loke, Richard A (1999). "Propyl Alcohols". In Jacqueline I., Kroschwitz (ed.). Kirk-Othmer Concise Encylclopedia of Chemical Technology, (4th ed.). New York: John Wiley & Sons, Inc. pp. 1654–1656. ISBN 978-0471419617.
- ^ "Isopropyl Alcohol, UltimAR, Suitable for Liquid Chromatography, Extract/Conc, UV-Spectrophotometry". VWR International. Retrieved 25 August 2014.
- ^ "UV Cutoff" (PDF). University of Toronto. Retrieved 25 August 2014.
- ^ Young, W.; Hartung, W.; Crossley, F. (1936). "Reduction of Aldehydes with Aluminum Isopropoxide". J. Am. Chem. Soc. 58: 100–2. doi:10.1021/ja01292a033.
- ^ a b c d e f g h i Papa, A. J. "Propanols". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_173. ISBN 978-3527306732.
- ^ Logsdon, John E.; Loke, Richard A. (December 4, 2000). "Isopropyl Alcohol". Kirk-Othmer Encyclopedia of Chemical Technology. Kirk‑Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. doi:10.1002/0471238961.0919151612150719.a01. ISBN 0471238961.
- ^ CRC Handbook of Chemistry and Physics, 44th ed. pp 2143–2184
- ^ Market Study Solvents, Ceresana, published Apr 2012
- ^ Arctic Silver thermal compound. arcticsilver.com
- ^ "proxan-sodium". alanwood.net.
- ^ "Sodium Isopropyl Xanthate, SIPX, Xanthate". 3DChem.com. Retrieved 2012-06-17.
- ^ "Guide to Local Production: WHO-recommended Handrub Formulations" (PDF). World Health Organization. August 2009.
- ^ Otitis Externa (Swimmers Ear). Medial College of Wisconsin
- ^ Burlage, Henry M.; Welch, H; Price, CW (2006). "Pharmaceutical applications of isopropyl alcohol II. Solubilities of local anesthetics". Journal of the American Pharmaceutical Association. 36 (1): 17–9. doi:10.1002/jps.3030360105. PMID 20285822.
- ^ Society for Experimental Biology and Medicine (1922). Proceedings of the Society for Experimental Biology and Medicine, Volume 19. p. 85.
- ^ a b "Isopropanol". Sigma-Aldrich. 19 January 2012. Retrieved 6 July 2012.
- ^ Mirafzal, Gholam A; Baumgarten, Henry E (1988). "Control of peroxidizable compounds: An addendum". Journal of Chemical Education. 65 (9): A226. Bibcode:1988JChEd..65A.226M. doi:10.1021/ed065pA226.
- ^ "Chemical safety: peroxide formation in 2-propanol". Chemical & Engineering News. 94 (31): 2. August 1, 2016.
- ^ a b c d e Slaughter RJ, Mason RW, Beasley DM, Vale JA, Schep LJ (2014). "Isopropanol poisoning". Clinical Toxicology. 52 (5): 470–8. doi:10.3109/15563650.2014.914527. PMID 24815348.
- ^ Calculated from TDLO listed at Oxford University MSDS, assuming weight of 70 kg
- ^ Kalapos, MP (2003). "On the mammalian acetone metabolism: from chemistry to clinical implications". Biochimica et Biophysica Acta. 1621 (2): 122–39. doi:10.1016/S0304-4165(03)00051-5. PMID 12726989.
- ^ "Isopropyl alcohol poisoning". www.uptodate.com. Retrieved 2017-10-10.
- ^ Wittcoff, M.M. Green ; H.A. (2003). Organic chemistry principles and industrial practice (1. ed., 1. reprint. ed.). Weinheim: Wiley-VCH. p. 4. ISBN 3-527-30289-1.
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