Acetic acid
(systematically named ethanoic acid,
also methanecarboxylic acid)
Chemical formula : C2H4O2 (also
written as CH3CO2H or CH3-COOH).
(O = 53,29 %, C = 40 %, H = 6,71 %)
Molar mass = 60,052 ± 0,0025 g·mol-1
Glacial acetic acid is a trivial name for water-free
(anhydrous) acetic acid, the name comes from
the ice-like crystals that form slightly below room temperature at
16.6 °C (61.9 °F)
[the presence of 0.1% water lowers its melting
point by 0.2 °C]. It ispresent in the vinegar
naturally, he gives his sour taste and pungent smell
(detectable from 1 ppm22).
Acetic acid is one of the simplest carboxylic acids
(as examples: methanoïc acid, formic acid,
-secreted by certain ants, propanoïc acid, propionic
acid, butanoïc acid, etc.).. It is an important chemical
reagent and industrial chemical, mainly used in the production of
cellulose acetate for photographic film and polyvinyl acetate for
wood glue, as well as synthetic fibers and fabrics.
The hydrogen center in the carboxyl group (-COOH) in carboxylic acids
such as acetic acid can separate from the molecule by ionization:
Because of this release of the proton (H+), acetic acid has acidic
character. Acetic acid is a weak monoprotic acid. In aqueous
solution, it has a pKa value of 4.76. Its conjugate base is acetate
(CH3COO-). A 1.0 M solution (about the
concentration of domestic vinegar) has a pH of 2.4, indicating
that merely 0.4% of the acetic acid molecules are dissociated.
Acetic acid is also present in the environment. Many plants contain
and can thus identify as volatile issue. The thermal degradation of
the wood product. It is found in many foods as an added ingredient or
as a natural component. Human activity can also be a source of acetic
acid emission in the atmosphere, including, among others, the vehicle
exhaust and combustion plants, plastics and other waste.
Acetic acid is produced and excreted by acetic acid bacteria, notable
ones being the Acetobacter genus and Clostridium
acetobutylicum. These bacteria are found universally in
foodstuffs, water, and soil, and acetic acid is produced naturally as
fruits and other foods spoil.
Production.
Industrially, it is produced in 75% acetic acid for the chemical
industry acid by carbonylation of methanol. Also by oxidation
of acetaldehyde or by liquid phase oxidation of n-butane
C4H10, or it is recovered in the production of
cellulose acetate or polyvinyl alcohol (CH2-CHOH) n. It can be
prepared from ethylene (Wacker or Showa Denko
processes). Acetic acid may be produced synthetically or by
bacterial fermentation. Today, the biological method is no longer
about 10% of production, but it remains important for the production
of vinegar, because in most countries the law provides that the
vinegar for food must be of biological origin.
As of 20032005, total worldwide production of virgin acetic
acid was estimated at 5 Mt/a (million tonnes per
year), approximately half of which was then produced in the
United States. European production stood at approximately 1 Mt/a and
was declining, and 0.7 Mt/a were produced in Japan. Another 1.5 Mt
were recycled each year, bringing the total world market to 6.5
Mt/a.
Since then the global production has increased to 10.7 Mt/a
(in 2010), and further, however, slowing
increase in production is predicted.[
Main features :
Pure acetic acid is a colorless, flammable, hygroscopic liquid,
and very poor conductor.
These properties of the solvent and miscibility of the acid form is
widely used in the chemical industry.
It is corrosive to many metals, including iron, magnesium and zinc.
It forms dihydrogen and metal salts called acetates. The aluminum
shape in contact with a thin layer of oxygen relatively resistant
aluminum oxide, which covers its surface: aluminum tanks are often
used to carry acetic acid.
|
|
|
|
|
|
|
|
|
|
|
|
In water treatment, it is used by injection in the form of water
diluted reagent (diluted to 5% by volume solutions, from 75%
acid).
NOTE:
Impurities that can be detected in acetic acid solutions depend on
the process used to produce glacial acetic acid.
It can detect small amounts of acetaldehyde, acetic anhydride, formic
acid, diacetyl, methyl acetate, ethyl acetoacetate, iron, mercury,
iodine, bromine and chlorides.
A formulation for water treatment.
Reaction mechanism of calcium bicarbonates (simplified
equations):
With 1 mg / l (or 1 g/m3) CH3COOH added, there is
(10/120) = 0.08 °f lower TAC
(alkalinity), and it is formed 0.74 mg of free
CO2, and 0.98 mg of CH3COO-acetate.
Storage.
Choosing a type of container must comply with the code of flammable
and combustible liquids, the maximum capacity of containers and
portable tanks for flammable or combustible liquids are different
depending on the type of container.
A store (link) in an airtight container kept closed, wearing a clear
identification of its contents, placed in a cool, dry,
well-ventilated area, away from bases and other incompatible
materials.
Store in a place with cement floor resistant to corrosion. Reservoirs
and tanks corrosive liquid must be equipped with an overfill
device.
Usually stored in stainless steel containers or high-density
polyethylene and polypropylene.
Uses :
Health effects and safety.
Concentrated acetic acid is corrosive to skin and must,
therefore, be handled with appropriate care, since it can cause skin
burns, permanent eye damage, and irritation to the mucous membranes.
These burns or blisters may not appear until hours after exposure.
Latex gloves offer no protection, so specially resistant gloves, such
as those made of nitrile rubber, are worn when handling the compound.
Concentrated acetic acid can be ignited with difficulty in the
laboratory. It becomes a flammable risk if the ambient temperature
exceeds 39 °C (102 °F), and can form explosive mixtures
with air above this temperature (explosive limits: 5.416%).
Acetic acid is a strong eye, skin, and mucous membrane irritant.
Prolonged skin contact with glacial acetic acid may result in tissue
destruction.
Inhalation exposure (8 hours) to acetic acid vapours at 10 ppm could
produce some irritation of eyes, nose, and throat; at 100 ppm marked
lung irritation and possible damage to lungs, eyes, and skin might
result. Vapour concentrations of 1,000 ppm cause marked irritation of
eyes, nose and upper respiratory tract and cannot be tolerated. These
predictions were based on animal experiments and industrial
exposure.
Skin sensitization to acetic acid is rare, but has occurred. It has
been reported that, 12 workers exposed for two or more years to an
estimated mean acetic acid airborne concentration of 51 ppm, there
were symptoms of conjunctive irritation, upper respiratory tract
irritation, and hyperkeratotic dermatitis. Exposure to 50 ppm or more
is intolerable to most persons and results in intensive lacrimation
and irritation of the eyes, nose, and throat, with pharyngeal oedema
and chronic bronchitis. Un acclimatized humans experience extreme eye
and nasal irritation at concentrations in excess of 25 ppm, and
conjunctivitis from concentrations below 10 ppm has been reported. In
a study of 5 workers exposed for 7 to 12 years to concentrations of
80 to 200 ppm at peaks, the principal findings were blackening and
hyperkeratosis of the skin of the hands, conjunctivitis (but no
corneal damage), bronchitis and pharyngitis, and erosion of the
exposed teeth (incisors and canines).
Toxicological profile (French) - Acide nitrique
(FT
24) par l'Institut national de recherche et de
sécurité (INRS).