Organic chemistry

What is acetone used for?

Acetone structure and uses?

 

What is acetone used for ?

Acetone structure uses and facts :

Acetone structure uses and facts are listed here briefly by the way you can clear your doubts about it all.

Facts of acetone :

Here are some facts about acetone given below :

1.Acetone is a transparent , highly flammable and volatile liquid, used as a solvent and synthesis intermediate.

2.With the formula C 3 H 6 O, it gives off a characteristic odor, both acrid and aromatic .

3. Its double bond carbon-oxygen and the presence of carbon to hydrogen in the alpha position (α) give it a high reactivity to many products.

4.Stable under usual conditions, acetone can thus react strongly with powerful oxidizing agents such as chromic acid , hot nitric acid, potassium permanganate , hydrogen peroxide, somehalogenated hydrocarbons (trichloromethane, tribromomethane …) or in the presence of a strong base (for example sodium or potassium hydroxide ).

5. Not corrosive to metals , it attacks certain plastics .

6.Acetone may cause severe eye irritation , nausea, dizziness or drowsiness when inhaling high concentrations of vapors (above 10,000 ppm ).

Acetone: physical properties

  • Density: 0.788 g / ml at 20 ° C.
  • Molar mass : 58.08 g / mol.
  • Point of fusion : -94.7 ° C.
  • Boiling point: 56.29 ° C.
  • Point flash : -9.4 ° C.
  • Auto-ignition temperature: 465 ° C.
  • Evaporation rate (ether = 1): 1.9.
  • Lower explosion limit: 2.5% at 25 ° C.
  • Solubility: miscible with water, ethanol, diethyl ether, esters , benzene , dimethylformamide, chloroform, most oils.
Acetone structure uses and facts. Acetone is a chemical with the raw formula C3H6O.
Acetone structure

Uses of acetone:

Acetone is one of the most widely used organic solvents, which dissolves gums, resins, cellulose derivatives , greases, oils and rubbers . It is used in many formulations:

  • paint, varnish , lacquer;
  • paint stripper and thinner;
  • glue and adhesives;
  • ink, dyes and their thinners;
  • transport and storage of acetylene in compressed gas cylinders.

In the chemical industry, acetone is involved in many processes:

  • manufacture of pharmaceutical and cosmetic products (eg vitamin C , methamphetamine);
  • extraction of fats, oils and waxes;
  • purification of sugars and starches (precipitating agent);
  • paraffin purification;
  • cleaning and drying glassware in the laboratory;
  • cleaning and drying of electronic parts;
  • cooling medium in dry ice mixture ;
  • manufacture of Plexiglas ( polymethyl methacrylate );
  • manufacture of bisphenol A  ;
  • manufacture of explosive powders;
  • manufacture and spinning of cellulose acetate fibers (eg, paper glue, photographic film bases, synthetic fibers, rayon, artificial silk, viscose);
  • manufacture of resin objects reinforced with glass fibers.

Acetone and environment:

Various activities can release acetone into the atmosphere  :

  • exhaust gas ;
  • combustion of wood and waste ;
  • degradation of waste in landfills;
  • paper industry;
  • cigarette smoke.

Acetone can also emanate from particle board, carpets or certain coatings. It also comes from natural sources during forest fires or volcanic eruptions .

Acetone in biology:

Acetone is naturally produced and excreted in the body during metabolic processes, especially when food is insufficient (fasting, ketogenic diet ) or in diabetic pathologies  ( hypoglycemia ).

The body then degrades fatty acids in the form of ketone bodies. The excess acetone is manifested by a characteristic odor of the breath and a high concentration in the urine.

 If acetone builds up too much, it causes ketoacidosis, a toxic acidification of the blood that can lead to coma .

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