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Acetone - 100ml
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Acetone is the organic compound with the formula (CH3)2CO. This colorless, mobile, flammable liquid is the simplest example of the ketones. Acetone is miscible with water and serves as an important solvent in its own right, typically as the solvent of choice for cleaning purposes in the laboratory. About 5.1 million tonnes were produced worldwide in 2009, mainly for use as a solvent and production of methyl methacrylate and bisphenol A.[2][3] Familiar household uses of acetone are as the active ingredient in nail polish remover and as paint thinner. It is a common building block in organic chemistry.
Acetone is naturally produced and disposed of in the human body as a result of normal metabolic processes. Reproductive toxicity tests show that it has low potential to cause reproductive problems. In fact, the body naturally increases the level of acetone in pregnant women, nursing mothers and children because their higher energy requirements lead to higher levels of acetone production. Ketogenic diets that increase acetone in the body are used to reduce epileptic attacks in infants and children who suffer from recalcitrant refractory epilepsy.USES:
About a third of the world's acetone is used as a solvent, and a quarter is consumed as a precursor to methyl methacrylate.[2] This application begins with the initial conversion of acetone to acetone cyanohydrin:
(CH3)2CO + HCN → (CH3)2C(OH)CN
In a subsequent step, the nitrile is hydrolyzed to the unsaturated amide, which is esterified:
(CH3)2C(OH)CN + CH3OH → CH2=(CH3)CCO2CH3 + NH3
The third major use of acetone (about 20%)[2] entails its condensation with phenol to give bisphenol A:
(CH3)2CO + 2 C6H5OH → (CH3)2C(C6H4OH)2 + H2O
Bisphenol A is a component of many polymers such as polycarbonates, polyurethanes, and epoxy resins.
As a solvent:
Acetone is a good solvent for most plastics and synthetic fibers including those used in laboratory bottles made of polystyrene, polycarbonate and some types of polypropylene.[5] It is ideal for thinning fiberglass resin, cleaning fiberglass tools and dissolving two-part epoxies and superglue before hardening. It is used as a volatile component of some paints and varnishes. As a heavy-duty degreaser, it is useful in the preparation of metal prior to painting; it also thins polyester resins, vinyl and adhesives.
Many millions of kilograms of acetone are consumed in the production of the solvents methyl isobutyl alcohol and methyl isobutyl ketone. These products arise via an initial aldol condensation to give diacetone alcohol.[3]
2 (CH3)2CO → (CH3)2C(OH)CH2C(O)CH3
Acetone is used as a solvent by the pharmaceutical industry and as a denaturation agent in denatured alcohol.[6] Acetone is also present as an excipient in some pharmaceutical products.[7]
Storage of acetylene
Although flammable itself, acetone is also used extensively as a solvent for the safe transporting and storing of acetylene, which cannot be safely pressurized as a pure compound. Vessels containing a porous material are first filled with acetone followed by acetylene, which dissolves into the acetone. One liter of acetone can dissolve around 250 liters of acetylene.[8][9]
Medical and cosmetic uses:
Acetone is used in a variety of general medical and cosmetic applications and is also listed as a component in food additives and food packaging.
Acetone is commonly used in the skin rejuvenation process in medical offices and medical spas. Since the days of ancient Egypt, people have been using chemexfoliation methods, also known as chemical peeling, to rejuvenate skin. Common agents used today for chemical peels are salicylic acid, glycolic acid, 30% salicylic acid in ethanol, and trichloroacetic acid (TCA). Prior to chemexfoliation, the skin should be cleaned properly and excess fat removed. This process is known as defatting. Acetone, Septisol, or a combination of these agents is commonly used in this process.
Laboratory uses:
In the laboratory, acetone is used as a polar aprotic solvent in a variety of organic reactions, such as SN2 reactions. The use of acetone solvent is also critical for the Jones oxidation. It is a common solvent for rinsing laboratory glassware because of its low cost and volatility, however, it does not form an azeotrope with water (see azeotrope (data)).[10] Despite its common use as a supposed drying agent, it is not effective except by bulk displacement and dilution. Acetone can be cooled with dry ice to −78 °C without freezing; acetone/dry ice baths are commonly used to conduct reactions at low temperatures. Acetone is fluorescent under ultraviolet light, and its vapor may be used as a fluorescent tracer in fluid flow experiments.[11]
Domestic and other niche uses:
Acetone is often the primary component in cleaning agents such as nail polish remover. Ethyl acetate, another organic solvent, is sometimes used as well. Acetone is a component of superglue remover and it easily removes residues from glass and porcelain.
It can be used as an artistic agent; when rubbed on the back of a laser print or photocopy placed face-down on another surface and burnished firmly, the toner of the image transfers to the destination surface.
Make-up artists use acetone to remove skin adhesive from the netting of wigs and moustaches by immersing the item in an acetone bath, then removing the softened glue residue with a stiff brush.
NOTE:
The information contained herein is believed to be accurate and is offered in good faith for the user's consideration and investigation. No warranty is expressed or implied regarding the completeness or accuracy of this information, whether originating from chem Kit Depot LLC. or from an alternate source. Users of this material should satisfy themselves by independent investigation of current scientific and medical information that this material may be safely handled.
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