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ACETIC ACID

Acetic acid is an aliphatic organic acid.
Acetic acid is a hygroscopic, corrosive liquid with a vinegar-like odor.
Acetic acid can be synthesized by oxidizing acetaldehyde in the presence of manganese or cobalt salts.

CAS Number: 64-19-7
EC Number: 200-580-7
Chemical Formula: CH3COOH
Molar Mass: 60.05 g/mol

Synonyms: acetic acid, ethanoic acid, 64-19-7, Glacial acetic acid, Ethylic acid, Vinegar acid, Acetic acid, glacial, Acetic acid glacial, Methanecarboxylic acid, Acetasol, Essigsaeure, Acide acetique, Vinegar, Aci-jel, Azijnzuur, Aceticum acidum, Acido acetico, Kyselina octova, Octowy kwas, Pyroligneous acid, HOAc, Azijnzuur [Dutch], Ethanoic acid monomer, acetyl alcohol, Essigsaeure [German], ethoic acid, Caswell No. 003, Otic Tridesilon, Octowy kwas [Polish], Otic Domeboro, Acetic acid (natural), Acide acetique [French], Acido acetico [Italian], FEMA No. 2006, Kyselina octova [Czech], AcOH, acetic acid-, ethanoate, UN2789, UN2790, MeCOOH, EPA Pesticide Chemical Code 044001, NSC 132953, BRN 0506007, Acetic acid, diluted, Acetic acid [JAN], AI3-02394, CH3COOH, Acidum aceticum glaciale, CH3-COOH, CH3CO2H, 10.Methanecarboxylic acid, CHEMBL539, NSC-132953, NSC-406306, INS NO.260, E-260, CHEBI:15366, INS-260, Q40Q9N063P, Ethanoat, Shotgun, MFCD00036152, Acetic acid, of a concentration of more than 10 per cent, by weight, of acetic acid, NSC-111201, NSC-112209, NSC-115870, NSC-127175, 68475-71-8, C2:0, Orlex, Vosol, WLN: QV1, Acetic acid, >=99.7%, FEMA Number 2006, Acetic acid, ACS reagent, >=99.7%, ACY, HSDB 40, CCRIS 5952, 63459-47-2, methane carboxylic acid, EINECS 200-580-7, Acetic acid 0.25% in plastic container, Ethylate, acetic aicd, acetic-acid, Acidum aceticum, Glacial acetate, acetic cid, actic acid, UNII-Q40Q9N063P, acetic -acid, Distilled vinegar, Methanecarboxylate, Acetic acid, glacial [USP:JAN], Nat. Acetic Acid, Acetasol (TN), Acetic acid,glacial, Acetic Acid Natural, Vinegar (Salt/Mix), MeCO2H, Undiluted Acetic Acid, 77671-22-8, Oxytocin identification, 3,3'-(1,4-phenylene)dipropiolic acid, HOOCCH3, Acetic Acid (Recovered), 546-67-8, Acetic acid LC/MS Grade, E 260, ACETIC ACID [II], ACETIC ACID [MI], Acetic acid, ACS reagent, Acetic acid-[13C,d3], bmse000191, bmse000817, bmse000857, Otic Domeboro (Salt/Mix), EC 200-580-7, Acetic acid (JP17/NF), ACETIC ACID [FHFI], ACETIC ACID [INCI], Acetic Acid [for LC-MS], ACETIC ACID [VANDF], NCIOpen2_000659, NCIOpen2_000682, ACETIC ACID [MART.], Acetic acid, glacial (USP), 4-02-00-00094 (Beilstein Handbook Reference), Glacial acetic acid (JP17), UN 2790 (Salt/Mix), ACETIC ACID [WHO-DD], ACETIC ACID [WHO-IP], ACETICUM ACIDUM [HPUS], INS No. 260, GTPL1058, Acetic Acid Glacial HPLC Grade, Acetic acid, analytical standard, Acetic acid, Glacial USP grade, DTXSID5024394, Acetic acid, puriss., >=80%, Acetic acid, 99.8%, anhydrous, Acetic acid, AR, >=99.8%, Acetic acid, LR, >=99.5%, Acetic Acid, Glacial Reagent ACS, Acetic acid, extra pure, 99.8%, Acetic acid, 99.5-100.0%, Acetic acid, Glacial, ACS Reagent, STR00276, ZINC5224164, Acetic acid, puriss., 99-100%, Tox21_301453, Acetic acid, glacial, >=99.85%, BDBM50074329, LMFA01010002, NSC132953, NSC406306, STL264240, Acetic acid, Environmental Grade Plus, Acetic acid, for HPLC, >=99.8%, AKOS000268789, ACIDUM ACETICUM [WHO-IP LATIN], DB03166, UN 2789, Acetic acid, >=99.5%, FCC, FG, Acetic acid, natural, >=99.5%, FG, Acetic acid, ReagentPlus(R), >=99%, CAS-64-19-7, Acetic acid, USP, 99.5-100.5%, NCGC00255303-01, Acetic acid 1000 microg/mL in Methanol, Acetic acid, SAJ first grade, >=99.0%, DB-085748, Acetic acid 1000 microg/mL in Acetonitrile, Acetic acid, >=99.99% trace metals basis, Acetic acid, JIS special grade, >=99.7%, Acetic acid, purified by double-distillation, FT-0621735, FT-0621743, FT-0621764, FT-0661109, FT-0661110, Acetic acid, UV HPLC spectroscopic, 99.9%, EN300-18074, Acetic acid, Vetec(TM) reagent grade, >=99%, Bifido Selective Supplement B, for microbiology, C00033, D00010, ORLEX HC COMPONENT ACETIC ACID, GLACIAL, Q47512, VOSOL HC COMPONENT ACETIC ACID, GLACIAL, Acetic acid, glacial, electronic grade, 99.7%, TRIDESILON COMPONENT ACETIC ACID, GLACIAL, A834671, ACETASOL HC COMPONENT ACETIC ACID, GLACIAL, Acetic acid, >=99.7%, SAJ super special grade, ACETIC ACID, GLACIAL COMPONENT OF BOROFAIR, ACETIC ACID, GLACIAL COMPONENT OF ORLEX HC, ACETIC ACID, GLACIAL COMPONENT OF VOSOL HC, SR-01000944354, ACETIC ACID, GLACIAL COMPONENT OF TRIDESILON, SR-01000944354-1, ACETIC ACID, GLACIAL COMPONENT OF ACETASOL HC, Glacial acetic acid, meets USP testing specifications, Acetic acid, >=99.7%, suitable for amino acid analysis, Acetic acid, >=99.7%, for titration in non-aqueous medium, Acetic acid, for luminescence, BioUltra, >=99.5% (GC), Acetic acid, p.a., ACS reagent, reag. ISO, reag. Ph. Eur., 99.8%, Acetic acid, semiconductor grade MOS PURANAL(TM) (Honeywell 17926), Glacial acetic acid, United States Pharmacopeia (USP) Reference Standard, Acetic acid, puriss. p.a., ACS reagent, reag. ISO, reag. Ph. Eur., >=99.8%, Glacial Acetic Acid, Pharmaceutical Secondary Standard; Certified Reference Material, 158461-04-2, Acetic acid, puriss., meets analytical specification of Ph. Eur., BP, USP, FCC, 99.8-100.5%, 200-580-7 [EINECS], 64-19-7 [RN], Acetic acid [ACD/Index Name] [ACD/IUPAC Name] [Wiki], Acid, Acetic, Acide acétique [French] [ACD/IUPAC Name], Acido acetico [Italian], AcOH [Formula], ättiksyra [Swedish], azido azetikoa [Basque], azijnzuur [Dutch], Essigsäure [German] [ACD/IUPAC Name], Ethanoic acid, etikkahappo [Finnish], Glacial acetic acid, HOAc [Formula], kwas octowy [Polish], Kyselina octova [Czech], MFCD00036152 [MDL number], MFCD00198163 [MDL number], QV1 [WLN], (2H3)Acetic (2H)acid, 10.Methanecarboxylic acid, 109945-04-2 [RN], 1112-02-3 [RN], 120416-14-0 [RN], 147416-04-4 [RN], 149748-09-4 [RN], 159037-04-4 [RN], 1794892-02-6 [RN], 2-Mercapto-5-chlor-benzoxazol-7-sulfonsure, Kaliumsalz, 3913-68-6 [RN], 42204-14-8 [RN], 498-63-5 [RN], 55511-07-4 [RN], 88-32-4 [RN], AA, Acetic acid (glacial)missing, Acetic acid 1 mol/L, Acetic Acid, Glacialmissing, Acetic Acid, GlenDry, anhydrous, Acetic acid-C,C,C-d3, Acetic Acid-d4, Acetic acidmissing, Acetic-2,2,2-d3 Acid, acetol, C2:0, Essigsaeure, Ethylic acid, Glacial Acetic, hydron [Wiki], MeCO2H [Formula], MeCOOH [Formula], Methanecarboxylic acid, Methanecarboxylic Acid, Acetic Acid, methyl carboxylic acid, MFCD00036287 [MDL number], missing, Pyroacetic acid, STR00276, Vinegar

Acetic acid is utilized for synthesizing acetic anhydride, cellulose acetate and acetic esters.
Acetic acid impact on the degradation of historic paper has been analyzed.

Acetic acid is a clear, colorless, organic liquid with a pungent odor similar to household vinegar.
Acetic acid is used as a raw material and solvent in the production of other chemical products, in oil and gas production, and in the food and pharmaceutical industries.

Acetic acid is an important bulk chemical that is currently produced via methanol carbonylation using fossil based CO.
Synthesis of acetic acid from the renewable and cheap CO2 is of great importance, but state of the art routes encounter difficulties, especially in reaction selectivity and activity.

Acetic acid, CH3COOH, is a corrosive organic acid having a sharp odor, burning taste, and pernicious blistering properties.
Acetic acid is found in ocean water, oilfield brines, rain, and at trace concentrations in many plant and animal liquids, and has a place in organic processes comparable to sulfuric acid in the mineral chemical industries.

Acetic acid is central to all biological energy pathways. Fermentation of fruit and vegetable juices yields 2–12% acetic acid solutions, usually called vinegar.
Uses include the manufacture of vinyl acetate and acetic anhydride. Vinyl acetate is used to make latex emulsion resins for paints and adhesives.

Acetic anhydride is used in making cellulose acetate fibers and cellulosic plastics.
About half of the world production comes from methanol carbonylation and about one-third from acetaldehyde oxidation.

Glacial acetic acid is dangerous, but Acetic acid precise toxic dose is not known for humans.
Vinegar, on the other hand, which is dilute acetic acid, has been used in foods and beverages since ancient times.

Acetic acid is an organic compound with the formula CH3COOH.
Acetic acid is a carboxylic acid consisting of a methyl group that is attached to a carboxyl functional group.

The systematic IUPAC name of acetic acid is ethanoic acid and Acetic acid chemical formula can also be written as C2H4O2.
Vinegar is a solution of acetic acid in water and contains between 5% to 20% ethanoic acid by volume.
The pungent smell and the sour taste is characteristic of the acetic acid present in Acetic acid.

An undiluted solution of acetic acid is commonly referred to as glacial acetic acid.
Acetic acid forms crystals which appear like ice at temperatures below 16.6oC.

Acetic acid has a wide range of applications as a polar, protic solvent.
In the field of analytical chemistry, glacial acetic acid is widely used in order to estimate substances that are weakly alkaline.

Acetic acid, systematically named ethanoic acid, is an organic compound with the chemical formula CH3COOH.
Acetic acid is a colorless liquid that, when undiluted, is also called glacial acetic acid.
Acetic acid has a distinctive sour taste and purgent smell.

Besides Acetic acid production as household vinegar, Acetic acid is mainly used as a precursor to polyvinylacetate and cellulose acetate.
Although Acetic acid is classified as a weak acid, concentrated acetic acid is corrosive and can attack the skin.

Acetic acid is also known as ethanoic acid, ethylic acid, vinegar acid, and methane carboxylic acid; Acetic acid has the chemical formula of CH3COOH.
Acetic acid is a byproduct of fermentation, and gives vinegar Acetic acid characteristic odor.

Vinegar is about 4-6% acetic acid in water.
More concentrated solutions can be found in laboratory use, and pure acetic acid containing only traces of water is known as glacial acetic acid.

Acetic acid is the 33rd highest volume chemical produced in the United States.
Acetic acid is used in the manufacture of acetic anhydride, cellulose acetate, vinyl acetate monomer, acetic esters, chloracetic acid, plastics, dyes, insecticides, photographic chemicals, and rubber.

Other commercial uses include the manufacture of vitamins, antibiotics, hormones, and organic chemicals, and as a food additive.
Typical concentrations of acetic acid occurring naturally in foods are 700 to 1,200 milligrams/kilogram (mg/kg) in wines, up to 860 mg/kg in aged cheeses, and 2.8 mg/kg in fresh orange juice.

Acetic acid (CH3COOH), also called ethanoic acid, the most important of the carboxylic acids.
A dilute (approximately 5 percent by volume) solution of acetic acid produced by fermentation and oxidation of natural carbohydrates is called vinegar; a salt, ester, or acylal of acetic acid is called acetate.
Industrially, acetic acid is used in the preparation of metal acetates, used in some printing processes; vinyl acetate, employed in the production of plastics; cellulose acetate, used in making photographic films and textiles; and volatile organic esters (such as ethyl and butyl acetates), widely used as solvents for resins, paints, and lacquers.Biologically, acetic acid is an important metabolic intermediate, and Acetic acid occurs naturally in body fluids and in plant juices.

Acetic acid has been prepared on an industrial scale by air oxidation of acetaldehyde, by oxidation of ethanol (ethyl alcohol), and by oxidation of butane and butene.
Today acetic acid is manufactured by a process developed by the chemical company Monsanto in the 1960s; it involves a rhodium-iodine catalyzed carbonylation of methanol (methyl alcohol).

Acetic Acid is a synthetic carboxylic acid with antibacterial and antifungal properties.
Although Acetic acid mechanism of action is not fully known, undissociated acetic acid may enhance lipid solubility allowing increased fatty acid accumulation on the cell membrane or in other cell wall structures.
Acetic acid, as a weak acid, can inhibit carbohydrate metabolism resulting in subsequent death of the organism.

Acetic acid is one of the simplest carboxylic acids.
Acetic acid is an important chemical reagent and industrial chemical that is used in the production of plastic soft drink bottles, photographic film; and polyvinyl acetate for wood glue, as well as many synthetic fibres and fabrics.

Acetic acid can be very corrosive, depending on the concentration.
Acetic acid is one ingredient of cigarette.

In households diluted acetic acid is often used as a cleaning agent.
In the food industry acetic acid is used as an acidity regulator.

The acetyl group, derived from acetic acid, is fundamental to the biochemistry of virtually all forms of life.
When bound to coenzyme A Acetic acid is central to the metabolism of carbohydrates and fats.

However, the concentration of free acetic acid in cells is kept at a low level to avoid disrupting the control of the pH of the cell contents.
Acetic acid is produced and excreted by certain bacteria, notably 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 some other foods spoil.
Acetic acid is also a component of the vaginal lubrication of humans and other primates, where Acetic acid appears to serve as a mild antibacterial agent.

Acetic acid is a simple monocarboxylic acid containing two carbons.
Acetic acid has a role as a protic solvent, a food acidity regulator, an antimicrobial food preservative and a Daphnia magna metabolite.
Acetic acid is a conjugate acid of an acetate.

Acetic acid, systematically named ethanoic acid /ˌɛθəˈnoʊɪk/, is an acidic, colourless liquid and organic compound with the chemical formula CH3COOH (also written as CH3CO2H, C2H4O2, or HC2H3O2).
Vinegar is at least 4% acetic acid by volume, making acetic acid the main component of vinegar apart from water and other trace elements.

Acetic acid is the second simplest carboxylic acid (after formic acid).
Acetic acid is an important chemical reagent and industrial chemical, used primarily in the production of cellulose acetate for photographic film, polyvinyl acetate for wood glue, and synthetic fibres and fabrics.

In households, diluted acetic acid is often used in descaling agents.
In the food industry, acetic acid is controlled by the food additive code E260 as an acidity regulator and as a condiment.

In biochemistry, the acetyl group, derived from acetic acid, is fundamental to all forms of life.
When bound to coenzyme A, Acetic acid is central to the metabolism of carbohydrates and fats.

The global demand for acetic acid is about 6.5 million metric tons per year (t/a), of which approximately 1.5 t/a is met by recycling; the remainder is manufactured from methanol.
Vinegar is mostly dilute acetic acid, often produced by fermentation and subsequent oxidation of ethanol.

Benefits of Acetic acid:
One of the most common ways consumers may come into contact with acetic acid is in the form of household vinegar, which is naturally made from fermentable sources such as wine, potatoes, apples, grapes, berries and grains.
Vinegar is a clear solution generally containing about 5 percent acetic acid and 95 percent water.

Vinegar is used as a food ingredient and can also be an ingredient in personal care products, household cleaners, pet shampoos and many other products for the home:

Food Preparation:
Vinegar is a common food ingredient, often used as a brine in pickling liquids, vinaigrettes, marinades and other salad dressings.
Vinegar also can be used in food preparation to help control Salmonella contamination in meat and poultry products.

Cleaning:
Vinegar can be used throughout the home as a window cleaner, to clean automatic coffee makers and dishes, as a rinsing agent for dishwashers, and to clean bathroom tile and grout.
Vinegar can also be used to clean food-related tools and equipment because Acetic acid generally does not leave behind a harmful residue and requires less rinsing.

Gardening:
In concentrations of 10 to 20 percent, acetic acid can be used as a weed killer on gardens and lawns.
When used as an herbicide, the acetic acid can kill weeds that have emerged from the soil, but does not affect the roots of the weed, so they can regrow.

Applications of Acetic acid:

Acetic acid (AcOH) can be used as:
A reaction solvent in many organic reactions such as bromination, hydrolysis, solvolysis, reductions, and hydrogenations.
A reagent in the protonolysis of organometallic compounds.

An acetylating agent for the acetylation of electron-rich aromatic compounds.
A catalyst to synthesize di(indolyl)methanes by the condensation reaction of indole and aromatic aldehydes.
A solvent system to prepare 3,4-dihydropyrimidin-2(1H)-one derivative via Biginelli reaction of aromatic aldehydes, 1,3-dicarbonyl compounds, and urea in the presence of a boric acid catalyst.

Acetic acid can also be used in the following:
Manganese(III) acetate/AcOH catalytic system is used in the conversion of alkenes to lactones.
Iron salts/AcOH is used to oxidize 2-methylnaphthalene to 2-methyl-1-naphthol in the presence of H2O2.

When acetic acid is at 99.5 percent concentration, Acetic acid is referred to as glacial acetic acid.
Glacial acetic acid has a variety of uses, including as a raw material and solvent in the production of other chemical products.

Industrial applications for glacial acetic acid include:

Vinyl Acetate, cellulose fibers and plastics:
Acetic acid is used to make many chemicals, including vinyl acetate, acetic anhydride and acetate esters.
Vinyl acetate is used to make polyvinyl acetate, a polymer used in paints, adhesives, plastics and textile finishes.

Acetic anhydride is used in the manufacture of cellulose acetate fibers and plastics used for photographic film, clothing and coatings.
Acetic acid is also used in the chemical reaction to produce purified terephthalic acid (PTA), which is used to manufacture the PET plastic resin used in synthetic fibers, food containers, beverage bottles and plastic films.

Solvents:
Acetic acid is a hydrophilic solvent, similar to ethanol.
Acetic acid dissolves compounds such as oils, sulfur and iodine and mixes with water, chloroform and hexane.

Acidizing oil and gas:
Acetic acid can help reduce metal corrosion and scale build-up in oil and gas well applications.
Acetic acid is also used in oil well stimulation to improve flow and increase production of oil and gas.
Pharmaceuticals and vitamins: The pharmaceutical industry uses acetic acid in the manufacture of vitamins, antibiotics, hormones and other products.

Food Processing:
Acetic acid is commonly used as a cleaning and disinfecting product in food processing plants.

Other uses:
Salts of acetic acid and various rubber and photographic chemicals are made from acetic acid.
Acetic acid and its sodium salt are commonly used as a food preservative.

Other Applications:
Adhesives/sealants-B&C
Agriculture intermediates
Apparel
Architectural coatings
Automotive protective coatings
Building materials
Commerical printing inks
Construction chemicals
Decorative interiors
Fertilizer
Food ingredients
Food preservatives
Formulators
Hard surface care
Industrial cleaners
Institutional cleaners
Intermediates
Oil or gas processing
Other-food chemicals
Other-transportation
Packaging components non food contact
Paints & coatings
Pharmaceutical chemicals
Process additives
Refining
Specialty chemicals
Starting material
Water treatment industrial

Uses of Acetic acid:
Acetic acid is a chemical reagent for the production of chemical compounds.
The largest single use of acetic acid is in the production of vinyl acetate monomer, closely followed by acetic anhydride and ester production.
The volume of acetic acid used in vinegar is comparatively small.

Acetic acid is used to manufacture acetic anhydride and other organic chemicals used in the plastic, pharmaceutical, dye, insecticide, textile, rubber, and photographic industries.
Acetic acid is used in photography (stop bath).

Acetic acid is used as a wet etchant in semiconductor manufacturing at standard concentrations of 36% or 99.5%.
Acetic acid is used in the bating and tanning stages of leather production.

Acetic acid is used in organic syntheses.
Permitted for use as an inert ingredient in non-food pesticide products.

Vinegar is a liquid consisting mainly of acetic acid (CH3COOH) and water.
The acetic acid is produced by the fermentation of ethanol by acetic acid bacteria.

Acetic acid is used as a laboratory reagent in chemical and biochemical analysis, in field testing of lead fumes, vinyl chloride determination, uric acid in urine, aniline vapors, and separation of gases.
Acetic acid is used in miscellaneous applications for etching compounds for engraving.

Acetic acid is deliming agent during leather tanning, solvent for organic compounds, and oil well acidizer.
Acetic acid is used in chemical industry as an acidifying and neutralizing agent.

Acetic acid is used in canning industries as an additive or flavorant for pickles, fish, meat, candy, and glazes used in textile and dye industries as dye catalysts, textile finishing, dye after-treatment, and production of nylon and acrylic fibers.
Acetic acid is constituent of photographic fixing baths, hardeners, hypotest solutions, and constituent of microfilm cements.

Acetic acid gives vinegar its sour taste and pungent smell.
Acetic acid is an important chemical reagent and industrial chemical, used in the plastic, pharmaceutical, dye, insecticide, textile, rubber, and photographic industries.

Water-free acetic acid (glacial acetic acid) is used in the production of certain fragrances.
Acetic acid is used to treat infections in the ear canal.

Consumer Uses:
Agricultural chemicals (non-pesticidal)
Catalyst
Cleaning agent
Dye
Fixing agent (mordant)
Intermediate
Intermediates
Laboratory chemicals
Monomers
Paint additives and coating additives not described by other categories
Photosensitive chemicals
Plasticizers
Processing aids, not otherwise listed
Softener and conditioner
Solvent

Industry Uses:
Agricultural chemicals (non-pesticidal)
Catalyst
Chemical reaction regulator
Cleaning agent
Corrosion inhibitor
Defoamer
Dye
Etching agent
Finishing agents
Functional fluids (open systems)
Intermediate
Intermediates
Laboratory chemicals
Lubricants and lubricant additives
Lubricating agent
Oxidizing/reducing agents
Paint additives and coating additives not described by other categories
Process regulators
Processing aids not otherwise specified
Processing aids, not otherwise listed
Processing aids, specific to petroleum production
Solubility enhancer
Solvent
Solvents (which become part of product formulation or mixture)
Surface active agents
pH regulating agent

Industrial Processes with risk of exposure:
Semiconductor Manufacturing
Textiles (Fiber & Fabric Manufacturing)
Leather Tanning and Processing
Photographic Processing
Textiles (Printing, Dyeing, or Finishing)
Burning Natural Polymers
Burning Synthetic Polymers

Activities with risk of exposure:
Sculpturing plastics
Textile arts
Smoking cigarettes
Applying metallic patinas
Burning biomass fuel for cooking and heating

Vinyl Acetate Monomer:
The primary use of acetic acid is the production of vinyl acetate monomer (VAM).
In 2008, this application was estimated to consume a third of the world's production of acetic acid.
The reaction consists of ethylene and acetic acid with oxygen over a palladium catalyst, conducted in the gas phase.

2 H3C−COOH + 2 C2H4 + O2 → 2 H3C−CO−O−CH=CH2 + 2 H2O

Vinyl acetate can be polymerised to polyvinyl acetate or other polymers, which are components in paints and adhesives.

Ester Production:
The major esters of acetic acid are commonly used as solvents for inks, paints and coatings.
The esters include ethyl acetate, n-butyl acetate, isobutyl acetate, and propyl acetate.

They are typically produced by catalyzed reaction from acetic acid and the corresponding alcohol:
H3COO−H + HO−R → CH3COO−R + H2O, R = general alkyl group

For example, acetic acid and ethanol gives ethyl acetate and water.
CH3COO−H + HO−CH2CH3 → CH3COO−CH2CH3 + H2O

Most acetate esters, however, are produced from acetaldehyde using the Tishchenko reaction.
In addition, ether acetates are used as solvents for nitrocellulose, acrylic lacquers, varnish removers, and wood stains.

First, glycol monoethers are produced from ethylene oxide or propylene oxide with alcohol, which are then esterified with acetic acid.
The three major products are ethylene glycol monoethyl ether acetate (EEA), ethylene glycol monobutyl ether acetate (EBA), and propylene glycol monomethyl ether acetate (PMA, more commonly known as PGMEA in semiconductor manufacturing processes, where Acetic acid is used as a resist solvent).

This application consumes about 15% to 20% of worldwide acetic acid.
Ether acetates, for example EEA, have been shown to be harmful to human reproduction.

Acetic Anhydride:
The product of the condensation of two molecules of acetic acid is acetic anhydride.
The worldwide production of acetic anhydride is a major application, and uses approximately 25% to 30% of the global production of acetic acid.
The main process involves dehydration of acetic acid to give ketene at 700–750 °C.

Ketene is thereafter reacted with acetic acid to obtain the anhydride:
CH3CO2H → CH2=C=O + H2O
CH3CO2H + CH2=C=O → (CH3CO)2O

Acetic anhydride is an acetylation agent.
As such, Acetic acid major application is for cellulose acetate, a synthetic textile also used for photographic film.
Acetic anhydride is also a reagent for the production of heroin and other compounds.

Use as Solvent:
As a polar protic solvent, acetic acid is frequently used for recrystallization to purify organic compounds.
Acetic acid is used as a solvent in the production of terephthalic acid (TPA), the raw material for polyethylene terephthalate (PET).
In 2006, about 20% of acetic acid was used for TPA production.

Acetic acid is often used as a solvent for reactions involving carbocations, such as Friedel-Crafts alkylation.
For example, one stage in the commercial manufacture of synthetic camphor involves a Wagner-Meerwein rearrangement of camphene to isobornyl acetate.
Here acetic acid acts both as a solvent and as a nucleophile to trap the rearranged carbocation.

Glacial acetic acid is used in analytical chemistry for the estimation of weakly alkaline substances such as organic amides.
Glacial acetic acid is a much weaker base than water, so the amide behaves as a strong base in this medium.
Acetic acid then can be titrated using a solution in glacial acetic acid of a very strong acid, such as perchloric acid.

Medical Use:
Acetic acid injection into a tumor has been used to treat cancer since the 1800s.

Acetic acid is used as part of cervical cancer screening in many areas in the developing world.
The acid is applied to the cervix and if an area of white appears after about a minute the test is positive.

Acetic acid is an effective antiseptic when used as a 1% solution, with broad spectrum of activity against streptococci, staphylococci, pseudomonas, enterococci and others.
Acetic acid may be used to treat skin infections caused by pseudomonas strains resistant to typical antibiotics.

While diluted acetic acid is used in iontophoresis, no high quality evidence supports this treatment for rotator cuff disease.

As a treatment for otitis externa, Acetic acid is on the World Health Organization's List of Essential Medicines.

Foods:
Acetic acid has 349 kcal (1,460 kJ) per 100 g.
Vinegar is typically no less than 4% acetic acid by mass.

Legal limits on acetic acid content vary by jurisdiction.
Vinegar is used directly as a condiment, and in the pickling of vegetables and other foods.

Table vinegar tends to be more diluted (4% to 8% acetic acid), while commercial food pickling employs solutions that are more concentrated.
The proportion of acetic acid used worldwide as vinegar is not as large as commercial uses, but is by far the oldest and best-known application.

Properties of Acetic acid:

Acidity:
The hydrogen centre in the carboxyl group (−COOH) in carboxylic acids such as acetic acid can separate from the molecule by ionization:
CH3COOH ⇌ CH3CO−2 + H+

Because of this release of the proton (H+), acetic acid has acidic character.
Acetic acid is a weak monoprotic acid.

In aqueous solution, Acetic acid has a pKa value of 4.76.
Acetic acid 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.
However, in very dilute (< 10−6 M) solution acetic acid is >90% dissociated.

Structure:
In solid acetic acid, the molecules form chains, individual molecules being interconnected by hydrogen bonds.
In the vapour at 120 °C (248 °F), dimers can be detected.

Dimers also occur in the liquid phase in dilute solutions in non-hydrogen-bonding solvents, and a certain extent in pure acetic acid, but are disrupted by hydrogen-bonding solvents.
The dissociation enthalpy of the dimer is estimated at 65.0–66.0 kJ/mol, and the dissociation entropy at 154–157 J mol−1 K−1.
Other carboxylic acids engage in similar intermolecular hydrogen bonding interactions.

Solvent Properties:
Liquid acetic acid is a hydrophilic (polar) protic solvent, similar to ethanol and water.
With a relative static permittivity (dielectric constant) of 6.2, Acetic acid dissolves not only polar compounds such as inorganic salts and sugars, but also non-polar compounds such as oils as well as polar solutes.

Acetic acid is miscible with polar and non-polar solvents such as water, chloroform, and hexane.
With higher alkanes (starting with octane), acetic acid is not miscible at all compositions, and solubility of acetic acid in alkanes declines with longer n-alkanes.
The solvent and miscibility properties of acetic acid make Acetic acid a useful industrial chemical, for example, as a solvent in the production of dimethyl terephthalate.

Biochemistry:
At physiological pHs, acetic acid is usually fully ionised to acetate.

The acetyl group, formally derived from acetic acid, is fundamental to all forms of life.
When bound to coenzyme A, Acetic acid is central to the metabolism of carbohydrates and fats.

Unlike longer-chain carboxylic acids (the fatty acids), acetic acid does not occur in natural triglycerides.
However, the artificial triglyceride triacetin (glycerine triacetate) is a common food additive and is found in cosmetics and topical medicines.

Acetic acid is produced and excreted by acetic acid bacteria, notably the genus Acetobacter 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.
Acetic acid is also a component of the vaginal lubrication of humans and other primates, where Acetic acid appears to serve as a mild antibacterial agent.

Nomenclature of Acetic acid:
The trivial name "acetic acid" is the most commonly used and preferred IUPAC name.
The systematic name "ethanoic acid", a valid IUPAC name, is constructed according to the substitutive nomenclature.
The name "acetic acid" derives from the Latin word for vinegar, "acetum", which is related to the word "acid" itself.

"Glacial acetic acid" is a name for water-free (anhydrous) acetic acid.
Similar to the German name "Eisessig" ("ice vinegar"), 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 Acetic acids melting point by 0.2 °C).

A common symbol for acetic acid is AcOH, where Ac is the pseudoelement symbol representing the acetyl group CH3−C(=O)−.
The conjugate base, acetate (CH3COO−), is thus represented as AcO−. (The symbol Ac for the acetyl functional group is not to be confused with the symbol Ac for the element actinium; the context prevents confusion among organic chemists).

To better reflect Acetic acid structure, acetic acid is often written as CH3−C(O)OH, CH3−C(=O)OH, CH3COOH, and CH3CO2H.
In the context of acid–base reactions, the abbreviation HAc is sometimes used, where Ac in this case is a symbol for acetate (rather than acetyl).

Acetate is the ion resulting from loss of H+ from acetic acid.
The name "acetate" can also refer to a salt containing this anion, or an ester of acetic acid.

Production of Acetic acid:
Acetic acid is produced industrially both synthetically and by bacterial fermentation.
About 75% of acetic acid made for use in the chemical industry is made by the carbonylation of methanol, explained below.

The biological route accounts for only about 10% of world production, but Acetic acid remains important for the production of vinegar because many food purity laws require vinegar used in foods to be of biological origin.
Other processes are methyl formate isomerization, conversion of syngas to acetic acid, and gas phase oxidation of ethylene and ethanol.

Acetic acid can be purified via fractional freezing using an ice bath.
The water and other impurities will remain liquid while the acetic acid will precipitate out.

As of 2003–2005, total worldwide production of virgin acetic acid was estimated at 5 Mt/a (million tonnes per year), approximately half of which was produced in the United States.
European production was approximately 1 Mt/a and declining, while Japanese production was 0.7 Mt/a.

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, a slowing in this increase in production is predicted.

The two biggest producers of virgin acetic acid are Celanese and BP Chemicals.
Other major producers include Millennium Chemicals, Sterling Chemicals, Samsung, Eastman, and Svensk Etanolkemi [sv].

Methanol Carbonylation:
Most acetic acid is produced by methanol carbonylation.
In this process, methanol and carbon monoxide react to produce acetic acid according to the equation.

The process involves iodomethane as an intermediate, and occurs in three steps.
A catalyst, metal carbonyl, is needed for the carbonylation (step 2).

1- CH3OH + HI → CH3I + H2O
2- CH3I + CO → CH3COI
3- CH3COI + H2O → CH3COOH + HI

Two related processes exist for the carbonylation of methanol: the rhodium-catalyzed Monsanto process, and the iridium-catalyzed Cativa process.
The latter process is greener and more efficient and has largely supplanted the former process, often in the same production plants.
Catalytic amounts of water are used in both processes, but the Cativa process requires less, so the water-gas shift reaction is suppressed, and fewer by-products are formed.

By altering the process conditions, acetic anhydride may also be produced on the same plant using the rhodium catalysts.

Acetaldehyde Oxidation:
Prior to the commercialization of the Monsanto process, most acetic acid was produced by oxidation of acetaldehyde.
This remains the second-most-important manufacturing method, although Acetic acid is usually not competitive with the carbonylation of methanol.

The acetaldehyde can be produced by hydration of acetylene.
This was the dominant technology in the early 1900s.

Light naphtha components are readily oxidized by oxygen or even air to give peroxides, which decompose to produce acetic acid according to the chemical equation, illustrated with butane:
2 C4H10 + 5 O2 → 4 CH3CO2H + 2 H2O

Such oxidations require metal catalyst, such as the naphthenate salts of manganese, cobalt, and chromium.

The typical reaction is conducted at temperatures and pressures designed to be as hot as possible while still keeping the butane a liquid.
Typical reaction conditions are 150 °C (302 °F) and 55 atm.

Side-products may also form, including butanone, ethyl acetate, formic acid, and propionic acid.
These side-products are also commercially valuable, and the reaction conditions may be altered to produce more of them where needed.
However, the separation of acetic acid from these by-products adds to the cost of the process.

Under similar conditions and using similar catalysts as are used for butane oxidation, the oxygen in air to produce acetic acid can oxidize acetaldehyde.

2 CH3CHO + O2 → 2 CH3CO2H

Using modern catalysts, this reaction can have an acetic acid yield greater than 95%.
The major side-products are ethyl acetate, formic acid, and formaldehyde, all of which have lower boiling points than acetic acid and are readily separated by distillation.

Ethylene Oxidation:
Acetaldehyde may be prepared from ethylene via the Wacker process, and then oxidised as above.

In more recent times, chemical company Showa Denko, which opened an ethylene oxidation plant in Ōita, Japan, in 1997, commercialised a cheaper single-stage conversion of ethylene to acetic acid.
The process is catalyzed by a palladium metal catalyst supported on a heteropoly acid such as silicotungstic acid.

A similar process uses the same metal catalyst on silicotungstic acid and silica:
C2H4 + O2 → CH3CO2H

Acetic acid is thought to be competitive with methanol carbonylation for smaller plants (100–250 kt/a), depending on the local price of ethylene.
The approach will be based on utilizing a novel selective photocatalytic oxidation technology for the selective oxidation of ethylene and ethane to acetic acid.
Unlike traditional oxidation catalysts, the selective oxidation process will use UV light to produce acetic acid at ambient temperatures and pressure.

Oxidative Fermentation:
For most of human history, acetic acid bacteria of the genus Acetobacter have made acetic acid, in the form of vinegar.
Given sufficient oxygen, these bacteria can produce vinegar from a variety of alcoholic foodstuffs.
Commonly used feeds include apple cider, wine, and fermented grain, malt, rice, or potato mashes.

The overall chemical reaction facilitated by these bacteria is:
C2H5OH + O2 → CH3COOH + H2O

A dilute alcohol solution inoculated with Acetobacter and kept in a warm, airy place will become vinegar over the course of a few months.
Industrial vinegar-making methods accelerate this process by improving the supply of oxygen to the bacteria.

The first batches of vinegar produced by fermentation probably followed errors in the winemaking process.
If must is fermented at too high a temperature, acetobacter will overwhelm the yeast naturally occurring on the grapes.

As the demand for vinegar for culinary, medical, and sanitary purposes increased, vintners quickly learned to use other organic materials to produce vinegar in the hot summer months before the grapes were ripe and ready for processing into wine.
This method was slow, however, and not always successful, as the vintners did not understand the process.

One of the first modern commercial processes was the "fast method" or "German method", first practised in Germany in 1823.
In this process, fermentation takes place in a tower packed with wood shavings or charcoal.

The alcohol-containing feed is trickled into the top of the tower, and fresh air supplied from the bottom by either natural or forced convection.
The improved air supply in this process cut the time to prepare vinegar from months to weeks.

Nowadays, most vinegar is made in submerged tank culture, first described in 1949 by Otto Hromatka and Heinrich Ebner.
In this method, alcohol is fermented to vinegar in a continuously stirred tank, and oxygen is supplied by bubbling air through the solution.
Using modern applications of this method, vinegar of 15% acetic acid can be prepared in only 24 hours in batch process, even 20% in 60-hour fed-batch process.

Anaerobic Fermentation:
Species of anaerobic bacteria, including members of the genus Clostridium or Acetobacterium can convert sugars to acetic acid directly without creating ethanol as an intermediate.

The overall chemical reaction conducted by these bacteria may be represented as:
C6H12O6 → 3 CH3COOH

These acetogenic bacteria produce acetic acid from one-carbon compounds, including methanol, carbon monoxide, or a mixture of carbon dioxide and hydrogen:
2 CO2 + 4 H2 → CH3COOH + 2 H2O

This ability of Clostridium to metabolize sugars directly, or to produce acetic acid from less costly inputs, suggests that these bacteria could produce acetic acid more efficiently than ethanol-oxidizers like Acetobacter.
However, Clostridium bacteria are less acid-tolerant than Acetobacter.

Even the most acid-tolerant Clostridium strains can produce vinegar in concentrations of only a few per cent, compared to Acetobacter strains that can produce vinegar in concentrations up to 20%.
At present, Acetic acid remains more cost-effective to produce vinegar using Acetobacter, rather than using Clostridium and concentrating Acetic acid.
As a result, although acetogenic bacteria have been known since 1940, their industrial use is confined to a few niche applications.

General Manufacturing Information of Acetic acid:

Industry Processing Sectors:
Agriculture, Forestry, Fishing and Hunting
All Other Basic Inorganic Chemical Manufacturing
All Other Basic Organic Chemical Manufacturing
All Other Chemical Product and Preparation Manufacturing
Computer and Electronic Product Manufacturing
Explosives Manufacturing
Fabricated Metal Product Manufacturing
Food, beverage, and tobacco product manufacturing
Non-metallic Mineral Product Manufacturing (includes clay, glass, cement, concrete, lime, gypsum, and other non-metallic mineral product manufacturing)
Not Known or Reasonably Ascertainable
Oil and Gas Drilling, Extraction, and Support activities
Other (requires additional information)
Paper Manufacturing
Pesticide, Fertilizer, and Other Agricultural Chemical Manufacturing
Petrochemical Manufacturing
Petroleum Lubricating Oil and Grease Manufacturing
Petroleum Refineries
Pharmaceutical and Medicine Manufacturing
Photographic Film, Paper, Plate, and Chemical Manufacturing
Plastics Material and Resin Manufacturing
Plastics Product Manufacturing
Services
Soap, Cleaning Compound, and Toilet Preparation Manufacturing
Synthetic Dye and Pigment Manufacturing
Textiles, apparel, and leather manufacturing
Transportation Equipment Manufacturing
Wholesale and Retail Trade

Reactions of Acetic acid:

Organic Chemistry:
Acetic acid undergoes the typical chemical reactions of a carboxylic acid.
Upon treatment with a standard base, Acetic acid converts to metal acetate and water.

With strong bases (e.g., organolithium reagents), Acetic acid can be doubly deprotonated to give LiCH2COOLi.
Reduction of acetic acid gives ethanol.

The OH group is the main site of reaction, as illustrated by the conversion of acetic acid to acetyl chloride.
Other substitution derivatives include acetic anhydride; this anhydride is produced by loss of water from two molecules of acetic acid.
Esters of acetic acid can likewise be formed via Fischer esterification, and amides can be formed.

When heated above 440 °C (824 °F), acetic acid decomposes to produce carbon dioxide and methane, or to produce ketene and water:
CH3COOH → CH4 + CO2
CH3COOH → CH2=C=O + H2O

Reactions With Inorganic Compounds:
Acetic acid is mildly corrosive to metals including iron, magnesium, and zinc, forming hydrogen gas and salts called acetates:
Mg + 2 CH3COOH → (CH3COO)2Mg + H2

Because aluminium forms a passivating acid-resistant film of aluminium oxide, aluminium tanks are used to transport acetic acid.

Metal acetates can also be prepared from acetic acid and an appropriate base, as in the popular "baking soda + vinegar" reaction giving off sodium acetate:
NaHCO3 + CH3COOH → CH3COONa + CO2 + H2O

A colour reaction for salts of acetic acid is iron(III) chloride solution, which results in a deeply red colour that disappears after acidification.
A more sensitive test uses lanthanum nitrate with iodine and ammonia to give a blue solution.
Acetates when heated with arsenic trioxide form cacodyl oxide, which can be detected by Acetic acid malodorous vapours.

Other Derivatives:
Organic or inorganic salts are produced from acetic acid. Some commercially significant derivatives:
Sodium acetate, used in the textile industry and as a food preservative (E262).

Copper(II) acetate, used as a pigment and a fungicide.
Aluminium acetate and iron(II) acetate—used as mordants for dyes.
Palladium(II) acetate, used as a catalyst for organic coupling reactions such as the Heck reaction.

Halogenated acetic acids are produced from acetic acid. Some commercially significant derivatives:
Chloroacetic acid (monochloroacetic acid, MCA), dichloroacetic acid (considered a by-product), and trichloroacetic acid.

MCA is used in the manufacture of indigo dye.
Bromoacetic acid, which is esterified to produce the reagent ethyl bromoacetate.

Trifluoroacetic acid, which is a common reagent in organic synthesis.
Amounts of acetic acid used in these other applications together account for another 5–10% of acetic acid use worldwide.

History of Acetic acid:
Vinegar was known early in civilization as the natural result of exposure of beer and wine to air, because acetic acid-producing bacteria are present globally.
The use of acetic acid in alchemy extends into the third century BC, when the Greek philosopher Theophrastus described how vinegar acted on metals to produce pigments useful in art, including white lead (lead carbonate) and verdigris, a green mixture of copper salts including copper(II) acetate.

Ancient Romans boiled soured wine to produce a highly sweet syrup called sapa.
Sapa that was produced in lead pots was rich in lead acetate, a sweet substance also called sugar of lead or sugar of Saturn, which contributed to lead poisoning among the Roman aristocracy.

In the 16th-century German alchemist Andreas Libavius described the production of acetone from the dry distillation of lead acetate, ketonic decarboxylation.
The presence of water in vinegar has such a profound effect on acetic acid's properties that for centuries chemists believed that glacial acetic acid and the acid found in vinegar were two different substances.
French chemist Pierre Adet proved them identical.

In 1845 German chemist Hermann Kolbe synthesised acetic acid from inorganic compounds for the first time.
This reaction sequence consisted of chlorination of carbon disulfide to carbon tetrachloride, followed by pyrolysis to tetrachloroethylene and aqueous chlorination to trichloroacetic acid, and concluded with electrolytic reduction to acetic acid.

By 1910, most glacial acetic acid was obtained from the pyroligneous liquor, a product of the distillation of wood.
The acetic acid was isolated by treatment with milk of lime, and the resulting calcium acetate was then acidified with sulfuric acid to recover acetic acid.
At that time, Germany was producing 10,000 tons of glacial acetic acid, around 30% of which was used for the manufacture of indigo dye.

Because both methanol and carbon monoxide are commodity raw materials, methanol carbonylation long appeared to be attractive precursors to acetic acid.
Henri Dreyfus at British Celanese developed a methanol carbonylation pilot plant as early as 1925.

However, a lack of practical materials that could contain the corrosive reaction mixture at the high pressures needed (200 atm or more) discouraged commercialization of these routes.
In 1968, a rhodium-based catalyst (cis−[Rh(CO)2I2]−) was discovered that could operate efficiently at lower pressure with almost no by-products.

US chemical company Monsanto Company built the first plant using this catalyst in 1970, and rhodium-catalyzed methanol carbonylation became the dominant method of acetic acid production (see Monsanto process).
In the late 1990s, the chemicals company BP Chemicals commercialised the Cativa catalyst ([Ir(CO)2I2]−), which is promoted by iridium for greater efficiency.
This iridium-catalyzed Cativa process is greener and more efficient and has largely supplanted the Monsanto process, often in the same production plants.

Interstellar Medium:
Interstellar acetic acid was discovered in 1996 by a team led by David Mehringer using the former Berkeley-Illinois-Maryland Association array at the Hat Creek Radio Observatory and the former Millimeter Array located at the Owens Valley Radio Observatory.
Acetic acid was first detected in the Sagittarius B2 North molecular cloud (also known as the Sgr B2 Large Molecule Heimat source).
Acetic acid has the distinction of being the first molecule discovered in the interstellar medium using solely radio interferometers; in all previous ISM molecular discoveries made in the millimetre and centimetre wavelength regimes, single dish radio telescopes were at least partly responsible for the detections.

Human Metabolite Information of Acetic acid:

Tissue Locations:
Kidney
Liver

Cellular Locations:
Cytoplasm
Extracellular
Golgi apparatus
Mitochondria

Handling and Storage of Acetic acid:

Nonfire Spill Response:
ELIMINATE all ignition sources (no smoking, flares, sparks or flames) from immediate area.
All equipment used when handling the product must be grounded.

Do not touch or walk through spilled material.
Stop leak if you can do Acetic acid without risk.

Prevent entry into waterways, sewers, basements or confined areas.
A vapor-suppressing foam may be used to reduce vapors.

Absorb with earth, sand or other non-combustible material.
For hydrazine, absorb with DRY sand or inert absorbent (vermiculite or absorbent pads).
Use clean, non-sparking tools to collect absorbed material.

LARGE SPILL:
Dike far ahead of liquid spill for later disposal.
Water spray may reduce vapor, but may not prevent ignition in closed spaces.

ELIMINATE all ignition sources (no smoking, flares, sparks or flames) from immediate area.
Do not touch damaged containers or spilled material unless wearing appropriate protective clothing.

Stop leak if you can do Acetic acid without risk.
Prevent entry into waterways, sewers, basements or confined areas.

Absorb or cover with dry earth, sand or other non-combustible material and transfer to containers.
DO NOT GET WATER INSIDE CONTAINERS.

Neutralizing Agents for Acids and Caustics:
Dilute with water, rinse with dilute sodium bicarbonate or lime solution.

Safe Storage:
Separated from food and feedstuffs, strong oxidants, strong acids and strong bases.
Store only in original container.

Keep in a well-ventilated room.
Store in an area without drain or sewer access.

Storage Conditions:
Store in a dry, well-ventilated place.
Separate from oxidizing materials and alkaline substances.

Separate from food and feedstuffs.
Keep in a well-ventilated room.

Quantities greater than 1 liter should be stored in tightly sealed metal containers in areas separate from oxidizers.

Health Effects and Safety of Acetic acid:
Concentrated acetic acid is corrosive to skin.
These burns or blisters may not appear until hours after exposure.

Prolonged inhalation exposure (eight hours) to acetic acid vapours at 10 ppm can produce some irritation of eyes, nose, and throat; at 100 ppm marked lung irritation and possible damage to lungs, eyes, and skin may 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.

In 12 workers exposed for two or more years to acetic acid airborne average concentration of 51 ppm (estimated), produced 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.

Unacclimatised 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 five workers exposed for seven 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).

The hazards of solutions of acetic acid depend on the concentration.

Concentrated acetic acid can be ignited only with difficulty at standard temperature and pressure, but becomes a flammable risk in temperatures greater than 39 °C (102 °F), and can form explosive mixtures with air at higher temperatures (explosive limits: 5.4–16%).

First Aid Measures of Acetic acid:

EYES:
First check the victim for contact lenses and remove if present.
Flush victim's eyes with water or normal saline solution for 20 to 30 minutes while simultaneously calling a hospital or poison control center.

Do not put any ointments, oils, or medication in the victim's eyes without specific instructions from a physician.
IMMEDIATELY transport the victim after flushing eyes to a hospital even if no symptoms (such as redness or irritation) develop.

SKIN:
IMMEDIATELY flood affected skin with water while removing and isolating all contaminated clothing.
Gently wash all affected skin areas thoroughly with soap and water.

IMMEDIATELY call a hospital or poison control center even if no symptoms (such as redness or irritation) develop.
IMMEDIATELY transport the victim to a hospital for treatment after washing the affected areas.

INHALATION:
IMMEDIATELY leave the contaminated area; take deep breaths of fresh air.
If symptoms (such as wheezing, coughing, shortness of breath, or burning in the mouth, throat, or chest) develop, call a physician and be prepared to transport the victim to a hospital.

Provide proper respiratory protection to rescuers entering an unknown atmosphere.
Whenever possible, Self-Contained Breathing Apparatus (SCBA) should be used.
If not available, use a level of protection greater than or equal to that advised under Protective Clothing.

INGESTION:
DO NOT INDUCE VOMITING.
Corrosive chemicals will destroy the membranes of the mouth, throat, and esophagus and, in addition, have a high risk of being aspirated into the victim's lungs during vomiting which increases the medical problems.

If the victim is conscious and not convulsing, give 1 or 2 glasses of water to dilute the chemical and IMMEDIATELY call a hospital or poison control center.
IMMEDIATELY transport the victim to a hospital.

If the victim is convulsing or unconscious, do not give anything by mouth, ensure that the victim's airway is open and lay the victim on his/her side with the head lower than the body.
DO NOT INDUCE VOMITING.
Transport the victim IMMEDIATELY to a hospital.

Fire Fighting
Some of these materials may react violently with water.

SMALL FIRE:
Dry chemical, CO2, water spray or alcohol-resistant foam.

LARGE FIRE:
Water spray, fog or alcohol-resistant foam.
If Acetic acid can be done safely, move undamaged containers away from the area around the fire.

Dike runoff from fire control for later disposal.
Do not get water inside containers.

FIRE INVOLVING TANKS OR CAR/TRAILER LOADS:
Fight fire from maximum distance or use unmanned master stream devices or monitor nozzles.

Cool containers with flooding quantities of water until well after fire is out.
Withdraw immediately in case of rising sound from venting safety devices or discoloration of tank.

ALWAYS stay away from tanks engulfed in fire.
For massive fire, use unmanned master stream devices or monitor nozzles.
If this is impossible, withdraw from area and let fire burn.

Identifiers of Acetic acid:
CAS Number: 64-19-7
3DMet: B00009
Abbreviations: AcOH
Beilstein Reference: 506007
ChEBI: CHEBI:15366
ChEMBL: ChEMBL539
ChemSpider: 171
DrugBank: DB03166
ECHA InfoCard: 100.000.528
EC Number: 200-580-7
E number: E260 (preservatives)
Gmelin Reference: 1380
IUPHAR/BPS: 1058
KEGG:
C00033
D00010
MeSH: Acetic+acid
PubChem CID: 176
RTECS number: AF1225000
UNII: Q40Q9N063P
UN number: 2789
CompTox Dashboard (EPA): DTXSID5024394
InChI: InChI=1S/C2H4O2/c1-2(3)4/h1H3,(H,3,4)
Key: QTBSBXVTEAMEQO-UHFFFAOYSA-N
SMILES: CC(O)=O

Synonym(s): Glacial acetic acid
Linear Formula: CH3CO2H
CAS Number: 64-19-7
Molecular Weight: 60.05
Beilstein: 506007
EC Number: 200-580-7
MDL number: MFCD00036152
PubChem Substance ID: 329770889
NACRES: NA.21

CAS number: 64-19-7
EC index number: 607-002-00-6
EC number: 200-580-7
Grade: ACS
Hill Formula: C₂H₄O₂
Chemical formula: CH₃COOH
Molar Mass: 60.05 g/mol
HS Code: 2915 21 00

Properties of Acetic acid:
Vapor density: 2.07 (vs air)
Quality Level: 200
Assay: ≥99%
Form: liquid
Autoignition temp.: 800 °F
expl. lim.:
16 %, 92 °F
4 %, 59 °F

Refractive index: n20/D 1.371 (lit.)
pH: 2.5 (20 °C, 50 g/L)
bp: 117-118 °C (lit.)
mp: 16.2 °C (lit.)

Solubility:
Alcohol: miscible(lit.)
Carbon disulfide: insoluble(lit.)
Glycerol: miscible(lit.)
Water: miscible(lit.)

Density: 1.049 g/mL at 25 °C (lit.)
Storage temp.: room temp
SMILES string: CC(O)=O
InChI: 1S/C2H4O2/c1-2(3)4/h1H3,(H,3,4)
InChI key: QTBSBXVTEAMEQO-UHFFFAOYSA-N

Boiling point: 116 - 118 °C (1013 hPa)
Density: 1.04 g/cm3 (25 °C)
Explosion limit: 4 - 19.9 %(V)
Flash point: 40 °C
Ignition temperature: 485 °C
Melting Point: 16.64 °C
pH value: 2.5 (50 g/l, H₂O, 20 °C)
Vapor pressure: 20.79 hPa (25 °C)
Viscosity kinematic: 1.17 mm2/s (20 °C)
Solubility: 602.9 g/l soluble

CAS: 64-19-7
Molecular Formula: C2H4O2
Molecular Weight (g/mol): 60.052
InChI Key: QTBSBXVTEAMEQO-UHFFFAOYSA-NShow Less
PubChem CID: 176
ChEBI: CHEBI:15366
IUPAC Name: acetic acid
SMILES: CC(=O)O

Chemical formula: CH3COOH
Molar mass: 60.052 g·mol−1
Appearance: Colourless liquid
Odor: Heavily vinegar-like
Density: 1.049 g/cm3 (liquid); 1.27 g/cm3 (solid)
Melting point: 16 to 17 °C; 61 to 62 °F; 289 to 290 K
Boiling point: 118 to 119 °C; 244 to 246 °F; 391 to 392 K
Solubility in water: Miscible
log P: -0.28[4]
Vapor pressure: 11.6 mmHg (20 °C)[5]
Acidity (pKa): 4.756
Conjugate base: Acetate
Magnetic susceptibility (χ): -31.54·10−6 cm3/mol
Refractive index (nD): 1.371 (VD = 18.19)
Viscosity: 1.22 mPa s
Dipole moment: 1.74 D

Molecular Weight: 60.05
XLogP3-AA: -0.2
Hydrogen Bond Donor Count: 1
Hydrogen Bond Acceptor Count: 2
Rotatable Bond Count: 0
Exact Mass: 60.021129366
Monoisotopic Mass: 60.021129366
Topological Polar Surface Area: 37.3 Å²
Heavy Atom Count: 4
Complexity: 31
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 1
Compound Is Canonicalized: Yes

Specifications of Acetic acid:
Assay (acidimetric): ≥ 99.7 %
Color: ≤ 10 Hazen
Titratable base: ≤ 0.0004 meq/g
Acetic anhydride: ≤ 100 ppm
Chloride (Cl): ≤ 1 ppm
Heavy metals (as Pb): ≤ 0.5 ppm
Sulfate (SO₄): ≤ 1 ppm
Fe (Iron): ≤ 0.2 ppm
Substances reducing potassium dichromate: passes test
Substances reducing potassium permanganate: passes test
Evaporation residue: ≤ 10 ppm
Dilution test: passes test

Linear Formula: CH3CO2H
Solubility Information: Solubility in water: completely soluble.
Formula Weight: 60.05
Percent Purity: 80% (vol.)
Quantity: 5 L
Flash Point: >60°C
Chemical Name or Material: Acetic acid

Thermochemistry of Acetic acid:
Heat capacity (C): 123.1 J K−1 mol−1
Std molar entropy (S⦵298): 158.0 J K−1 mol−1
Std enthalpy of formation (ΔfH⦵298): -483.88–483.16 kJ/mol
Std enthalpy of combustion (ΔcH⦵298): -875.50–874.82 kJ/mol

Pharmacology of Acetic acid:
ATC code: G01AD02 (WHO) S02AA10 (WHO)

Related compounds of Acetic acid:
Acetaldehyde
Acetamide
Acetic anhydride
Chloroacetic acid
Acetyl chloride
Glycolic acid
Ethyl acetate
Potassium acetate
Sodium acetate
Thioacetic acid

Related carboxylic acids:
Formic acid
Propionic acid

Names of Acetic acid:

Preferred IUPAC name:
Acetic acid

Systematic IUPAC name:
Ethanoic acid

Other names:
Vinegar (when dilute)
Hydrogen acetate
Methanecarboxylic acid
Ethylic acid