Isopropyl alcohol
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| Names | |||
|---|---|---|---|
| IUPAC name
isopropyl alcohol
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| Preferred IUPAC name
2-Propanol | |||
| Other names
Propan-2-ol; Isopropanol; Rubbing alcohol; sec-Propyl alcohol; s-Propanol; iPrOH; IPA
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| Identifiers | |||
3D model (JSmol)
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| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.000.601 | ||
| 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 | |||
| Solubility | miscible in benzene, chloroform, ethanol, ether, glycerin soluble in acetone insoluble in salt solutions | ||
| Acidity (pKa) | 16.5[1] | ||
Refractive index (nD)
|
1.3776 | ||
| Viscosity | 2.86 cP at 15 °C 1.96 cP at 25 °C[2] 1.77 cP at 30 °C[2] | ||
| 1.66 D (gas) | |||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
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Flammable | ||
| GHS labelling: | |||
 
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| Danger | |||
| H225, H319, H336 | |||
| P210, P261, P305+P351+P338 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | Open cup: 11.7 °C (53.1 °F) Closed cup: 13 °C (55 °F) | ||
| Explosive limits | 2–12.7% | ||
Threshold limit value (TLV)
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980 mg/m3 (TWA), 1225 mg/m3 (STEL) | ||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose)
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3600 mg/kg (oral, mouse) 12800 mg/kg (dermal, rabbit) LC50 = 53000 mg/m3 (inhalation, mouse) | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible)
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TWA 400 ppm (980 mg/m3)[3] | ||
REL (Recommended)
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TWA 400 ppm (980 mg/m3) ST 500 ppm (1225 mg/m3)[3] | ||
IDLH (Immediate danger)
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2000 ppm[3] | ||
| Related compounds | |||
| 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 2-propanol) is a chemical compound with the molecular formula C3H8O or C3H7OH or CH3CHOHCH3. It is a colorless, flammable chemical compound with a strong odor. It is the simplest example of a secondary alcohol, where the alcohol carbon atom is attached to two other carbon atoms sometimes shown as (CH3)2CHOH. It is a structural isomer of propanol.
Properties
Isopropyl alcohol is miscible in water, alcohol, ether and chloroform. It will dissolve ethyl cellulose, polyvinyl butyral, many oils, alkaloids, gums and natural resins.[4] It is insoluble in salt solutions. Unlike ethanol or methanol, isopropyl alcohol can be separated from aqueous solutions by adding a salt such as sodium chloride, sodium sulfate, or any of several other inorganic salts, since the alcohol is much less soluble in saline solutions than in salt-free water. The process is colloquially called salting out, and causes concentrated isopropyl alcohol to separate into a distinct layer.[5]
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.[5] It has a slightly bitter taste, and is not safe to drink.[5][6]
Isopropyl alcohol becomes increasingly viscous with decreasing temperature. At temperatures below −70 °C (−94 °F), isopropyl alcohol resembles maple syrup in viscosity.
Isopropyl alcohol has a maximum absorbance at 205 nm in an ultraviolet-visible spectrum.[7][8]
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.[9]
Production
In 1994, 1.5 million tonnes of isopropyl alcohol were produced in the United States, Europe, and Japan.[10] This compound is primarily produced by combining water and propene in a hydration reaction. It is also produced by hydrogenating acetone.[10][11]
There are two routes for the hydration process: indirect hydration via the sulfuric acid process, and direct hydration. The former process, which can use low-quality propene, predominates in the USA while the latter process, which requires high-purity propene, is more commonly used in Europe. These processes give predominantly isopropyl alcohol rather than 1-propanol because the addition of water or sulfuric acid to propene follows Markovnikov's rule.
Indirect hydration
The indirect process reacts propene with sulfuric acid to form a mixture of sulfate esters. Subsequent hydrolysis of these esters by steam produces isopropyl alcohol, which is distilled. Diisopropyl ether is a significant by-product of this process; it is recycled back to the process and hydrolyzed to give the desired product.[10]
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.[10]
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.[12] Pure (anhydrous) isopropyl alcohol is made by azeotropic distillation of the wet isopropyl alcohol using either diisopropyl ether or cyclohexane as azeotroping agents.[10]
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 coupled with excess acetone production, such as the cumene process.[10]
Uses
In 1990, 45 thousand tonnes 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 tonnes was consumed for household use and in personal care products. Isopropyl alcohol in particular is popular for pharmaceutical applications,[10] 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.[10]
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.[13]
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[14]). Isopropyl alcohol is used in keyboard, LCD and laptop cleaning, is sold commercially as a whiteboard cleaner, and is a strong but safer alternative to common household cleaning products.[which?] It is commonly used to clean prepared optical fibers just before splicing. It is used to clean LCD and glass computer monitor screens (at some risk to the anti-reflection coating on some screens[citation needed]), and used to give second-hand or worn non-vinyl phonograph records newer-looking sheen. It is effective at removing Hot-Melt Adhesive from a large variety of surfaces. It is effective at removing residual glue from some sticky labels although some other adhesives used on tapes and paper labels are resistant to it. It can also be used to remove stains[clarification needed] from most fabrics, wood, cotton, etc. In addition, it can also be used to clean paint or other oil-based products so that they may be reused, commonly known as "repainting." It is used as a wetting agent in the fountain solution used in lithographic printing, and often used as a solvent for French polishing shellac used in cabinet making.
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[15] and an ore flotation reagent.[16] 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.[10] This compound may serve as a chemical reagent in itself, by acting as a dihydrogen donor in transfer hydrogenation.
Medical
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.[17] Isopropyl alcohol is used as a water-drying aid for the prevention of otitis externa, better known as swimmer's ear.[18]
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 similar to ether as a solvent[19] or as an anesthetic by inhaling the fumes or orally. Early uses included using the solvent as general anesthetic for small mammals[20] 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 cold 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. Isopropyl alcohol is often sold in aerosol cans as a windshield de-icer. 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 into a 'pellet' after centrifuging the DNA. 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.[21] Isopropyl alcohol has also been reported to form peroxides, which may explode upon concentration.[22] Isopropyl alcohol is a skin irritant.[21]
Toxicology
Isopropyl alcohol and its metabolite, acetone, act as central nervous system (CNS) depressants. Symptoms of isopropyl alcohol poisoning include flushing, headache, dizziness, CNS depression, nausea, vomiting, anesthesia, and coma. Poisoning can occur from ingestion, inhalation, or absorption; therefore, well-ventilated areas and protective gloves are recommended. Around 15 g of isopropyl alcohol can have a toxic effect on a 70 kg human if left untreated.[23] However, it is not nearly as toxic as methanol or ethylene glycol. Isopropyl alcohol does not cause an anion gap acidosis (in which a lowered blood serum pH causes depletion of bicarbonate anion) unlike ethanol and methanol. Isopropyl alcohol does, however, produce an osmolal gap between the calculated and measured osmolalities of serum, as do the other alcohols. Overdoses may cause a fruity odor on the breath as a result of its metabolism to acetone, which is further metabolized to produce the nutrients acetate and glucose.[24] Isopropyl alcohol is oxidized to form acetone by alcohol dehydrogenase in the liver.
Isopropyl alcohol is denatured for certain uses, in which case the NFPA 704 rating is changed to 2,3,1.
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.[25]
References
- ^ 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. doi:10.1139/v79-444.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ 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).
- ^ 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.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ 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. and Loke, Richard A. (December 4, 2000). "Isopropyl Alcohol". Kirk‑Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc.
{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link) - ^ 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". Retrieved 2012-06-17.
- ^ "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. 2012-1-19. Retrieved 7/6/2012.
{{cite web}}: Check date values in:|accessdate=and|date=(help) - ^ Kolar, Wes (July 11, 2000). "Lab Safety Review: Danger! – Peroxides Present".
- ^ 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.
- ^ 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.
{{cite book}}: CS1 maint: multiple names: authors list (link)
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