Difference between revisions of "Acetone"
(→Relevant Sciencemadness threads)
|Line 185:||Line 185:|
Revision as of 23:43, 6 May 2017
Sample of acetone
Acetone chemical structure
| IUPAC name
| Preferred IUPAC name
| Other names
Spirit of Saturn
|Molar mass||58.08 g/mol|
|Appearance||Colorless volatile liquid|
|Odor||Pungent, irritating, floral|
|Melting point||−94.7 °C (−138.5 °F; 178.5 K)|
|Boiling point||56.05 °C (132.89 °F; 329.20 K)|
|Solubility|| Miscible with almost all organic solvents|
Immiscible with perfluorocarbons
|Vapor pressure|| 9.39 kPa (0 °C)|
30.6 kPa (25 °C)
374 kPa (100 °C)
2.8 MPa (200 °C)
Std enthalpy of
|−250.03 - −248.77 kJ/mol|
|Safety data sheet||Sigma-Aldrich|
|Flash point||−20 °C (−4 °F; 253 K)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
| 5,800 mg/kg (rat, oral)|
3,000 mg/kg (mouse, oral)
5,340 mg/kg (rabbit, oral)
LC50 (Median concentration)
|20,702 ppm (rat, 8 hr)|
|Methyl ethyl ketone|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Acetone, also known as propanone or dimethyl ketone (chemical formula (CH3)2CO) is a popular solvent and useful chemical for lots of organic chemistry, being the simplest ketone.
Acetone is highly flammable and will burn in air releasing carbon dioxide and water vapors.
It will react with halogens to form halogenated organic compounds, i.e. iodoacetone. Acetone reacts very exothermically with halogens dissolved in basic solutions to give a haloform of the said halogen, process known as haloform reaction. One example is with household bleach and other hypochlorites to form chloroform.
Acetone is a clear liquid with very low viscosity that is miscible in water, that boils at 56°C and freezes between −95 to −93 °C. It has a sharp, somewhat sweet, and floral aroma similar to other ketones. It is also miscible in benzene, chloroform, ethanol, diethyl ether and methanol.
Acetone can be found at hardware stores as paint thinners or nail polish remover, either pure or mixed with other organic substances (usually esters). Distillation may be required to purify the acetone.
Most technical-grade acetone tends to be fairly pure and has very little if any water. If you want it more pure, you can distill it again.
- 2 Na(CH3COO) → Na2CO3 + (CH3)2CO
- Ca(CH3COO)2 → CaCO3 + (CH3)2CO
Because this reaction occurs at around 400-500°C, temperature above the boiling and autoignition temperature of acetone, it must be performed in an oxygen free chamber (carbon dioxide rich or only atmosphere is sufficient) and because the acetone results as vapors, it must be condensed.
- Methyl methacrylate synthesis
- Acetone peroxide synthesis
- Chloroform synthesis
- Organic extractions
- Make ethenone
Skin contact with acetone is not recommended, as prolonged exposure can cause defatting of the skin. Acetone's low boiling point of requires work in a ventilated area. While acetone is volatile and while its fumes are not particularly toxic, they can be irritating in large amounts. Acetone however is among the least toxic solvents, and as many studies have shown there are no long term risks in case of repeated exposure.
The main danger of acetone comes from its flammability. Its vapors have a flash point much below room temperature, so air/acetone mixtures can explode or burst into flames easily, even from static shocks.
At 486°C acetone will self-ignite.
Acetone is best stored in closed bottles, away from any source of heat.
Acetone can be safely burned. Traces of acetone can be released in open air. Strongly diluted acetone solutions can be poured down the drain, but do not release large amounts.