|Preferred IUPAC name
3D model (JSmol)
|Molar mass||g·mol−1 60.096|
|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|
Refractive index (nD)
|Viscosity||2.86 cP at 15 °C
1.96 cP at 25 °C
1.77 cP at 30 °C
|1.66 D (gas)|
|Safety data sheet||See: data page
|GHS signal word||Danger|
|H225, H319, H336|
|P210, P261, P305+351+338|
|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)|
|980 mg/m3 (TWA), 1225 mg/m3 (STEL)|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|12800 mg/kg (dermal, rabbit)
3600 mg/kg (oral, mouse)
5045 mg/kg (oral, rat)
6410 mg/kg (oral, rabbit)
LC50 (median concentration)
|53000 mg/m3 (inhalation, mouse)
12,000 ppm (rat, 8 hr)
LCLo (lowest published)
|16,000 ppm (rat, 4 hr)
12,800 ppm (mouse, 3 hr)
|US health exposure limits (NIOSH):|
|TWA 400 ppm (980 mg/m3)|
|TWA 400 ppm (980 mg/m3) ST 500 ppm (1225 mg/m3)|
IDLH (Immediate danger)
|1-Propanol, ethanol, 2-butanol|
|Supplementary data page|
|Refractive index (n),
Dielectric constant (εr), etc.
|UV, IR, NMR, MS|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Isopropyl alcohol (IUPAC name propan-2-ol; commonly called isopropanol or 2-propanol) is a compound with the chemical formula CH3CHOHCH3. 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 and ethyl methyl ether.
It is used in the manufacture of a wide variety of industrial and household chemicals, and is a common ingredient in chemicals such as antiseptics, disinfectants and detergents.
Isopropyl alcohol is miscible in water, ethanol, ether, and chloroform. It will dissolve ethyl cellulose, polyvinyl butyral, many oils, alkaloids, gums and natural resins. 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.
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. It has a slightly bitter taste, and is not safe to drink.
Isopropyl alcohol becomes increasingly viscous with decreasing temperature and will freeze at −89 °C (−128 °F).
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.
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 I for the preparation of cordite, a smokeless, low explosive propellant.
In 1994, 1.5 million tonnes of isopropyl alcohol were produced in the United States, Europe, and Japan.
It is primarily produced by combining water and propene in a hydration reaction or by hydrogenating acetone.
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. Pure (anhydrous) isopropyl alcohol is made by azeotropic distillation of the wet isopropyl alcohol using either diisopropyl ether or cyclohexane as azeotroping agents.
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.
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. 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.
In 1990, 45,000 metric tonnes of isopropyl alcohol were used in the United States, mostly as a solvent for coatings or for industrial processes. In that year, 5400 metric tons were used for household purposes and in personal care products. Isopropyl alcohol is popular in particular for pharmaceutical applications, due to its low toxicity. 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.
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.
Examples of this application include cleaning eyeglasses, 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).
Isopropyl alcohol is esterified to give isopropyl acetate, another solvent. It reacts with carbon disulfide and sodium hydroxide to give sodium isopropylxanthate, an herbicide and an ore flotation reagent. 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. This compound may serve as a chemical reagent in itself, by acting as a dihydrogen donor in transfer hydrogenation.
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 for isopropyl alcohol. A 75% v/v solution in water may be used as a hand sanitizer. Isopropyl alcohol is used as a water-drying aid for the prevention of otitis externa, better known as swimmer’s ear.
Early uses as an anesthetic
Although isopropyl alcohol can be used for anesthesia, its many negative attributes or drawbacks prohibit this use. Isopropyl alcohol can also be used similarly to ether as a solvent or as an anesthetic by inhaling the fumes or orally. Early uses included using the solvent as general anesthetic for small mammals 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.
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.
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.
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. Distillation of isopropyl alcohol over magnesium has been reported to form peroxides, which may explode upon concentration. Isopropyl alcohol is a skin irritant.  Wearing protective gloves is recommended.
Isopropyl alcohol and its metabolite, acetone, act as central nervous system (CNS) depressants. Poisoning can occur from ingestion, inhalation, or skin absorption. Symptoms of isopropyl alcohol poisoning include flushing, headache, dizziness, CNS depression, nausea, vomiting, anesthesia, hypothermia, low blood pressure, shock, respiratory depression, and coma. Overdoses may cause a fruity odor on the breath as a result of its metabolism to acetone.
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.
Isopropyl alcohol is oxidized to form acetone by alcohol dehydrogenase in the liver, and has a biological half-life in humans between 2.5 and 8.0 hours. 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.
- “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.
- “Isopropanol_msds”. chemsrc.com.
- 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.
- Yaws, C.L. (1999). Chemical Properties Handbook. McGraw-Hill. ISBN 978-0-07-073401-2.
- “NIOSH Pocket Guide to Chemical Hazards #0359”. National Institute for Occupational Safety and Health (NIOSH).
- “Isopropyl alcohol”. Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- “PubChem – Isopropanol”. Retrieved February 10, 2019.
- Doolittle, Arthur K. (1954). The Technology of Solvents and Plasticizers. New York: John Wiley & Sons, Inc. p. 628.
- 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. 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.
- Wittcoff, M.M. Green ; H.A. (2003). Organic chemistry principles and industrial practice (1. ed., 1. reprint. ed.). Weinheim: Wiley-VCH. p. 4. ISBN 978-3-527-30289-5.
- Papa, A. J., “Propanols”, Ullmann’s Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a22_173
- 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 978-0471238966.
- CRC Handbook of Chemistry and Physics, 44th ed. pp 2143–2184
- Market Study Soviet. Ceresana. April 2012
- Arctic Silver thermal compound. arcticsilver.com
- “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). Medical 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.
- “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.
- García-Gavín, Juan; Lissens, Ruth; Timmermans, Ann; Goossens, An (2011-06-17). “Allergic contact dermatitis caused by isopropyl alcohol: a missed allergen?”. Contact Dermatitis. 65 (2): 101–106. doi:10.1111/j.1600-0536.2011.01936.x. ISSN 0105-1873. PMID 21679194.
- McInnes, A (1973-02-10). “Skin reaction to isopropyl alcohol”. British Medical Journal. 1 (5849): 357. ISSN 0007-1447. PMC 1588210. PMID 4265463.
- 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.
- 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.
- CDC – NIOSH Pocket Guide to Chemical Hazards – Isopropyl alcohol
- Environmental Health Criteria 103: 2-Propanol