PRODUCTS

ACETIC ACID

Acetic Acid is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Acetic Acid is used as a food preservative and food additive (known as E260).
Acetic Acid is also used in some household cleaning products to remove lime scale.

CAS Number: 64-19-7
EC Number: 200-580-7
E number: E260 (preservatives)
Molecular Formula: C2H4O2 / CH3COOH

SYNONYMS:
Acetic acid (aqueous), Ethanoic acid, Glacial acetic acid, Methanecarboxylic acid, Ethanoic acid, vinegar, ethylic acid, vinegar acid, methanecarboxylic acid, TCLP extraction fluid 2, shotgun, glacial acetic acid, glacial ethanoic acid, Ethanoic acid, Ethylic acid, Glacial acetic acid, Methanecarboxylic acid, Vinegar acid, CH3COOH, Acetasol, Acide acetique, Acido acetico, Azijnzuur, Essigsaeure, Octowy kwas, Acetic acid, glacial, Kyselina octova, UN 2789, Aci-jel, Shotgun, Ethanoic acid monomer, NSC 132953, Acetic acid, Ethanoic acid, Vinegar (when dilute), Hydrogen acetate, Methanecarboxylic acid, Ethylic acid, Ethanoic acid, Ethylic acid, Glacial acetic acid, Methanecarboxylic acid, Vinegar acid, CH3COOH, Acetasol, Acide acetique, Acido acetico, Azijnzuur, Essigsaeure, Octowy kwas, Acetic acid, glacial, Kyselina octova, UN 2789, Aci-jel, Shotgun, Ethanoic acid monomer, NSC 132953, Ethanoic acid, vinegar, ethylic acid, vinegar acid, methanecarboxylic acid, TCLP extraction fluid 2, shotgun, glacial acetic acid, glacial ethanoic acid, Ethanoic acid, Ethylic acid, Glacial acetic acid, Methanecarboxylic acid, Vinegar acid, CH3COOH, Acetasol, Acide acetique, Acido acetico, Azijnzuur, Essigsaeure, Octowy kwas, Acetic acid, glacial, Kyselina octova, UN 2789, Aci-jel, Shotgun, Ethanoic acid monomer, NSC 132953, BDBM50074329, FA 2:0, LMFA01010002, NSC132953, NSC406306, 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, USEPA/OPP Pesticide Code: 044001, Acetic acid USP 99.5-100.5%, NCGC00255303-01, Acetic acid 1000 microg/mL in Methanol, Acetic acid SAJ first grade >=99.0%, 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, NS00002089, 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, InChI=1/C2H4O2/c1-2(3)4/h1H3(H,3,4), 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, Acetic acid puriss. meets analytical specification of Ph. Eur. BP USP FCC 99.8-100.5%, acetic-acid, Glacial acetate, acetic cid, actic acid, UNII-Q40Q9N063P, acetic -acid, Distilled vinegar, Methanecarboxylate, Acetic acid glacial [USP:JAN], Acetasol (TN), Acetic acid glacial for LC-MS, Vinegar (Salt/Mix), HOOCCH3, 546-67-8, Acetic acid LC/MS Grade, ACETIC ACID [II], ACETIC ACID [MI], Acetic acid ACS reagent, 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 glacial (USP), 4-02-00-00094 (Beilstein Handbook Reference), 77671-22-8, Glacial acetic acid (JP17), UN 2790 (Salt/Mix), ACETIC ACID [WHO-DD], ACETIC ACID [WHO-IP], ACETICUM ACIDUM [HPUS], GTPL1058, Acetic Acid Glacial HPLC Grade, Acetic acid analytical standard, Acetic acid Glacial USP grade, Acetic acid puriss. >=80%, Acetic acid 99.8% anhydrous, Acetic acid AR >=99.8%, Acetic acid LR >=99.5%, Acetic acid extra pure 99.8%, Acetic acid 99.5-100.0%, Acetic acid Glacial ACS Reagent, STR00276, Acetic acid puriss. 99-100%, Tox21_301453, Acetic acid glacial >=99.85%, acetic acid, ethanoic acid, 64-19-7, Ethylic acid, Vinegar acid, Acetic acid glacial, Glacial acetic acid, Acetic acid glacial, Methanecarboxylic acid, Acetasol, Essigsaeure, Acide acetique, Pyroligneous acid, Vinegar, Azijnzuur, Aceticum acidum, Acido acetico, Octowy kwas, Aci-jel, HOAc, ethoic acid, Kyselina octova, Orthoacetic acid, AcOH, Ethanoic acid monomer, Acetic, Caswell No. 003, Otic Tridesilon, MeCOOH, Acetic acid-17O2, Otic Domeboro, Acidum aceticum glaciale, Acidum aceticum, CH3-COOH, acetic acid-, CH3CO2H, UN2789, UN2790, EPA Pesticide Chemical Code 044001, NSC 132953, NSC-132953, NSC-406306, BRN 0506007, Acetic acid diluted, INS NO.260, Acetic acid [JAN], DTXSID5024394, MeCO2H, CHEBI:15366, AI3-02394, CH3COOH, INS-260, Q40Q9N063P, E-260, 10.Methanecarboxylic acid, CHEMBL539, NSC-111201, NSC-112209, NSC-115870, NSC-127175, Acetic acid-2-13C,d4, INS No. 260, DTXCID304394, E 260, Acetic-13C2 acid (8CI,9CI), Ethanoat, Shotgun, MFCD00036152, Acetic acid of a concentration of more than 10 per cent by weight of acetic acid, 285977-76-6, 68475-71-8, C2:0, acetyl alcohol, Orlex, Vosol, ACETIC-1-13C-2-D3 ACID-1 H (D), WLN: QV1, ACETIC ACID (MART.), ACETIC ACID [MART.], Acetic acid >=99.7%, 57745-60-5, 63459-47-2, FEMA Number 2006, ACETIC-13C2-2-D3 ACID, 97 ATOM % 13C, 97 ATOM % D, Acetic acid ACS reagent >=99.7%, ACY, HSDB 40, CCRIS 5952, 79562-15-5, methane carboxylic acid, EINECS 200-580-7, Acetic acid 0.25% in plastic container, Essigsaure, Ethylate, acetic acid, Acetic acid, Ethanoic acid, Vinegar (when dilute), Hydrogen acetate, Methanecarboxylic acid, Ethylic acid, acetic acid, ethanoic acid, 64-19-7, Acetic acid glacial, Ethylic acid, Vinegar acid, Glacial acetic acid, Acetic acid, glacial, Methanecarboxylic acid, Essigsaeure, Acide acetique, Pyroligneous acid, Vinegar, Azijnzuur, Aceticum acidum, Acido acetico, Octowy kwas, Aci-jel, HOAc, ethoic acid

Acetic acid /əˈsiːtɪk/, 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.

Acetic Acid has been used, as a component of vinegar, throughout history from at least the third century BC.
Acetic acid is the second simplest carboxylic acid (after formic acid).
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 as of 2023 is about 17.88 million metric tonnes per year (t/a).
Most of the world's acetic acid is produced via the carbonylation of methanol.

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 registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 000 tonnes per annum.
Acetic acid is an organic chemical substance, it is a colourless liquid with a very distinctive odour.

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).

Synthesis of acetic acid from methanol and carbon monoxide.
Pure acetic acid, often called glacial acetic acid, is a corrosive, colourless liquid (boiling point 117.9 °C [244.2 °F]; melting point 16.6 °C [61.9 °F]) that is completely miscible with water.

Acetic Acid can also be obtained through the food industry by the acetic fermentation process of ethanol, or more commonly explained, through alcoholic fermentation and with the distillation of wood.
Vinegar is a hygroscopic substance, i.e. Acetic Acid can absorb moisture from its surroundings.

Therefore, when Acetic Acid is mixed with water, there is a very significant reduction in its volume.
On the other hand, when acetic acid 100 % is exposed to low temperatures, the surface, also known as acetic essence, crystallises and forms ice-like crystals at the top.

Due to the chemical structure of this material, Acetic Acid has a very high boiling point.
Furthermore, it is worth noting that acetic acid, being a carboxylic acid, has the ability to dissociate, but only slightly, as it is a weak acid [FC1] .
Moreover, thanks to this ability to dissociate, Acetic Acid conducts electricity effectively.

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 its 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 it.
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 or ethanoic acid is a colourless liquid organic compound with the molecular formula CH3COOH.
When acetic acid is dissolved in water, it is termed glacial acetic acid.
Vinegar is no less than 4 per cent acetic acid by volume, aside from water, allowing acetic acid to be the main ingredient of vinegar.

Acetic Acid is produced primarily as a precursor to polyvinyl acetate and cellulose acetate, in addition to household vinegar.
Acetic Acid is a weak acid since the solution dissociates only slightly.
But concentrated acetic acid is corrosive and can damage the flesh.

The second simplest carboxylic acid is acetic acid (after formic acid).
Acetic Acid consists of a methyl group to which a carboxyl group is bound.
Acetic Acid is an important chemical reagent and industrial chemical which is mainly useful for the manufacture of photographic film cellulose acetate, wood glue polyvinyl acetate, and synthetic fibres and fabrics.

USES and APPLICATIONS of ACETIC ACID:
Acetic Acid is an important chemical reagent and industrial chemical across various fields, 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.
Acetic Acid is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.

Acetic Acid is approved in the EEA and/or Switzerland for use in biocidal products more favourable for the environment, human or animal health.
Acetic Acid is an authorised food additive.

Acetic Acid is used in the following products: coating products, washing & cleaning products, air care products, lubricants and greases, fillers, putties, plasters, modelling clay, anti-freeze products, fertilisers, plant protection products, finger paints, biocides (e.g. disinfectants, pest control products), welding & soldering products and textile treatment products and dyes.

Other release to the environment of Acetic Acid is likely to occur from: outdoor use, indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners) and indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters).

Release to the environment of Acetic Acid can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Acetic Acid is used for the manufacture of: chemicals.

Other release to the environment of Acetic Acid is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment) and outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials).

Acetic Acid can be found in products with material based on: paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper), leather (e.g. gloves, shoes, purses, furniture), fabrics, textiles and apparel (e.g. clothing, mattress, curtains or carpets, textile toys) and wood (e.g. floors, furniture, toys).

Acetic Acid is used in the following products: laboratory chemicals, pH regulators and water treatment products, water treatment chemicals, plant protection products and washing & cleaning products.
Acetic Acid is used in the following areas: formulation of mixtures and/or re-packaging.

Other release to the environment of Acetic Acid is likely to occur from: outdoor use and indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners).
Acetic Acid is used in the following products: coating products, perfumes and fragrances, paper chemicals and dyes, textile treatment products and dyes, metal surface treatment products, non-metal-surface treatment products and polymers.

Release to the environment of Acetic Acid can occur from industrial use: formulation of mixtures, formulation in materials, manufacturing of the substance, in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, for thermoplastic manufacture, as processing aid, of substances in closed systems with minimal release and in the production of articles.

As chemical distributors, the purposes for which this type of acid is processed are varied.
As mentioned above, Acetic Acid can be found in many grocery shops as white vinegar.
In such products, acetic acid cannot be found in its pure form, but only in small quantities.

Acetic Acid is also present in foods such as canned and pickled foods, cheese and dairy products, sauces or prepared salads.
Acetic Acid is also commonly used in the pharmaceutical, cosmetic and industrial industries both to produce other substances and to regulate their properties, especially with regards to their pH.

Due to its strong odour, one of its other main uses is in cosmetics as a regulator in the aroma of fragrances, i.e. Acetic Acid achieves a balance between sweet smells in particular.
In the textile industry, Acetic Acid is used to dye fabrics and produce fabrics such as viscose or latex.

In the chemical industry, acetic acid is used in the production of cleaning products and, in the pharmaceutical industry, in supplements and some medicines, as it is capable of stabilising blood pressure and reducing blood sugar levels.
Acetic Acid is also a common ingredient in ointments.

Acetic acid is the main component of vinegar, which contains 4 to 18% acetic acid.
Acetic Acid is used as a food preservative and food additive (known as E260).
Large quantities of acetic acid are used to make products such as ink for textile printing, dyes, photographic chemicals, pesticides, pharmaceuticals, rubber and plastics.

Acetic Acid is also used in some household cleaning products to remove lime scale.
Acetic Acid is used in the following products: laboratory chemicals, pH regulators and water treatment products, oil and gas exploration or production products, water treatment chemicals, washing & cleaning products, polymers and coating products.

Acetic Acid is used in the following areas: mining and formulation of mixtures and/or re-packaging.
Acetic Acid is used for the manufacture of: chemicals, textile, leather or fur, wood and wood products and pulp, paper and paper products.
Release to the environment of Acetic Acid can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates) and manufacturing of the substance.

Release to the environment of Acetic Acid can occur from industrial use: manufacturing of the substance, in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), formulation of mixtures, formulation in materials, in the production of articles, as processing aid, for thermoplastic manufacture, as processing aid and of substances in closed systems with minimal release.

Acetic Acid (CH3COOH), 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 it occurs naturally in body fluids and in plant juices.
One of its most common uses is in the composition of vinegar, although Acetic Acid is also used in cosmetics and pharmaceuticals, in the food, textile and chemical industries.

On an industrial level, acetic acid is produced through the carbonylation of methanol and is used as a raw material for the production of different compounds.
Acetic Acid is a very important organic compound in the day-to-day lives of humans.

Acetic acid is used as an antiseptic due to its antibacterial qualities
The manufacture of rayon fiber involves the use of Acetic Acid.
Medically, acetic acid has been employed to treat cancer by its direct injection into the tumour.

Being the major constituent of vinegar, Acetic Acid finds use in the pickling of many vegetables.
The manufacture of rubber involves the use of Acetic Acid.
Acetic Acid is also used in the manufacture of various perfumes.

When two molecules of acetic acid undergo a condensation reaction together, the product formed is acetic anhydride.
Acetic acid is used in a number of topical medical preparations, including the destruction of warts, in eardrops, as an expectorant, liniment and astringent.

Acetic Acid is used in the manufacture of a number of chemical compounds, plastics, pharmaceuticals, dyes, insecticides, photographic chemicals, vitamins, antibiotics, cosmetics and hormones.

Acetic Acid is used as an antimicrobial agent, latex coagulant and oil-well acidifier.
Acetic Acid is used in textile printing, as a preservative in foods and as a solvent for gums, resins and volatile oils.
Acetic Acid is widely used in the production of VAM (vinyl acetate monomer).

-Vinyl acetate monomer uses of Acetic Acid:
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.[49]

-Ester production uses of Acetic Acid:
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:
CH3COO−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 it 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 uses of Acetic Acid:
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, its 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.

-Acetic Acid is used 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.
It then can be titrated using a solution in glacial acetic acid of a very strong acid, such as perchloric acid.

-Medical use of Acetic acid
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.
Acetic 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.

-Uses of Acetic Acid:
The chemical reagent for the processing of chemical compounds is acetic acid.
In the production of vinyl acetate monomer, acetic anhydride, and ester production, the use of acetic acid is important.

*Vinyl Acetate Monomer:
Vinyl acetate monomer (VAM) processing is the main application of acetic acid.
Vinyl acetate undergoes polymerization to produce polyvinyl acetate or other polymers, which are components of paints and adhesives.

The reaction consists of ethylene and acetic acid with oxygen over a palladium catalyst.
2CH3COOH+2C2H4+O2→2CH3CO2CH=CH2+2H2O
Wood glue also utilizes vinyl acetate polymers.

*Acetic Anhydride:
Acetic anhydride is the result of the condensation of two acetic acid molecules.
Significant use is the worldwide processing of acetic anhydride, utilizing about 25 per cent to 30 per cent of global acetic acid production.

The key method includes acetic acid dehydration to give ketene at 700-750 °C.
CH3CO2H→CH2=C=O+H2O
CH3CO2H+CH2=C=O→CH3CO2O

It is great for general disinfection and fighting mould and mildew since acetic acid kills fungi and bacteria.
Acetic Acid is useful in a range of traditional and green cleaning materials, such as mould and mildew cleaners, floor cleaners, sprays for cleaning and dusting, and roof cleaners, either as vinegar or as an element.

The acetyl group is in use widely in the biochemistry field.
Products made from acetic acid are an effective metabolizer of carbohydrates and fats when bound to coenzyme A.

As a treatment for otitis externa, Acetic Acid is the best and most effective drug in a health system on the World Health Organization’s List of Essential Medicines.

ACETIC ACID AS A SOLVENT:
In its liquid state, Acetic Acid is a hydrophile (readily dissolves in water) and also a polar, protic solvent.
A mixture of acetic acid and water is, in this manner, similar to a mixture of ethanol and water.

Acetic acid also forms miscible mixtures with hexane, chloroform, and several oils.
However, Acetic Acid does not form miscible mixtures with long-chain alkanes (such as octane).

The desirable solvent properties of acetic acid, along with its ability to form miscible mixtures with both polar and non-polar compounds, make it a very important industrial solvent.
Acetic Acid is widely used in the industrial preparation of dimethyl terephthalate (DMT).

FOODS, ACETIC ACID:
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 industrial uses, but it is by far the oldest and best-known application.

ACETIC ACID IN EVERYDAY LIFE:
Acetic Acid is found in many everyday products as described above, such as food, cleaning products and cosmetics, among others.
Of all of them, vinegar is one of the most important ones, as Acetic Acid has different uses, such as for cooking or cleaning.
Acetic Acid is an infallible product when it comes to dealing with stubborn stains such as dog urine, rust or other dirt.

REACTIONS OF ACETIC ACID:
Organic chemistry
Acetic acid undergoes the typical chemical reactions of a carboxylic acid.
Upon treatment with a standard base, it converts to metal acetate and water.

With strong bases (e.g., organolithium reagents), it 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.

Containers lined with glass, stainless steel or polyethylene are also used for this purpose.
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 its malodorous vapours.

CHEMICAL PROPERTIES OF ACETIC ACID:
The chemical reactions undergone by acetic acid are similar to those of other carboxylic acids.
When heated to temperatures above 440oC, Acetic Acid undergoes decomposition to yield either methane and carbon dioxide or water and ethenone, as described by the following chemical equations.

CH3COOH + Heat → CO2 + CH4
CH3COOH + Heat → H2C=C=O + H2O

Some metals such as magnesium, zinc, and iron undergo corrosion when exposed to acetic acid.
These reactions result in the formation of acetate salts.

2CH3COOH + Mg → Mg(CH3COO)2 (magnesium acetate) + H2
The reaction between ethanoic acid and magnesium results in the formation of magnesium acetate and hydrogen gas, as described by the chemical equation provided above.

OTHER REACTIONS OF ACETIC ACID:
Acetic acid reacts with alkalis and forms acetate salts, as described below.
CH3COOH + KOH → CH3COOK + H2O

This compound also forms acetate salts by reacting with carbonates (along with carbon dioxide and water).
Examples of such reactions include:

2CH3COOH + Na2CO3 (sodium carbonate) → 2CH3COONa + CO2 + H2O
CH3COOH + NaHCO3 (sodium bicarbonate) → CH3COONa + CO2 + H2O
The reaction between PCl5 and ethanoic acid results in the formation of ethanoyl chloride.

RELATED COMPOUNDS OF ACETIC ACID:
*Related carboxylic acids
*Formic acid
*Propionic acid
*Acetaldehyde
*Acetamide
*Acetic anhydride
*Chloroacetic acid
*Acetyl chloride
*Glycolic acid
*Ethyl acetate
*Potassium acetate
*Sodium acetate
*Thioacetic acid

OTHER DERIVATIVES OF ACETIC ACID:
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.

HOW ACETIC ACID GETS INTO THE ENVIRONMENT:
Acetic acid can enter the environment from discharge and emissions from industries.
The burning of plastics or rubber, and exhaust fumes from vehicles may also release acetic acid into the environment.
When released into soil it evaporates into the air where Acetic Acid is broken down naturally by sunlight.
Levels of acetic acid in the environment would be expected to be low.

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's 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

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

Dimers also occur in the liquid phase in dilute solutions with non-hydrogen-bonding solvents, and to 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, it dissolves not only polar compounds such as inorganic salts and sugars, but also non-polar compounds such as oils as well as polar solutes.

It 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 it 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 in aqueous solution.
The acetyl group, formally derived from acetic acid, is fundamental to all forms of life.

Typically, it is bound to coenzyme A by acetyl-CoA synthetase enzymes, where it 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.

Most of the acetate generated in cells for use in acetyl-CoA is synthesized directly from ethanol or pyruvate.
However, the artificial triglyceride triacetin (glycerine triacetate) is a common food additive and is found in cosmetics and topical medicines; this additive is metabolized to glycerol and acetic acid in the body.

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 it appears to serve as a mild antibacterial agent

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 it 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.[34][35] Since then, the global production has increased from 10.7 Mt/a in 2010 to 17.88 Mt/a in 2023.

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 metal carbonyl catalyst is needed for the carbonylation (step 2).

CH3OH + HI → CH3I + H2O
CH3I + CO → CH3COI
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.

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 in plants using rhodium catalysis.

*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.

Similar conditions and catalysts 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
It is thought to be competitive with methanol carbonylation for smaller plants (100–250 kt/a), depending on the local price of ethylene.

*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, it remains more cost-effective to produce vinegar using Acetobacter, rather than using Clostridium and concentrating it.
As a result, although acetogenic bacteria have been known since 1940, their industrial use is confined to a few niche applications.

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 solid ice-like crystals that form with agitation, slightly below room temperature at 16.6 °C (61.9 °F).

Acetic acid can never be truly water-free in an atmosphere that contains water, so the presence of 0.1% water in glacial acetic acid lowers its melting point by 0.2 °C.

A common symbol for acetic acid is AcOH (or HOAc), where Ac is the pseudoelement symbol representing the acetyl group CH3−C(=O)−; the conjugate base, acetate (CH3COO−), is thus represented as AcO−.
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.

(The symbol Ac for the acetyl functional group is not to be confused with the symbol Ac for the element actinium; context prevents confusion among organic chemists).
To better reflect its 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).
The carboxymethyl functional group derived from removing one hydrogen from the methyl group of acetic acid has the chemical formula −CH2−C(=O)−OH.

PHYSICAL PROPERTIES OF ACETIC ACID:
Acetic acid is a colourless liquid; with a strong vinegar-like odour.
Acetic Acid is flammable, and at temperatures warmer than 39°C, explosive vapour/air mixtures may be formed.
Acetic acid is considered a volatile organic compound by the National Pollutant Inventory.
Specific Gravity: 1.049 @ 25°C
Melting Point: 16.7°C
Boiling Point: 118°C
Vapour pressure: 1.5 kPa @ 20°C

CHEMICAL PROPERTIES OF ACETIC ACID:
Acetic acid is hygroscopic, meaning that it tends to absorb moisture.
Acetic Acid mixes with ethyl alcohol, glycerol, ether, carbon tetrachloride and water and reacts with oxidants and bases.
Concentrated acetic acid is corrosive and attacks many metals forming flammable or explosive gases.
Acetic Acid can also attack some forms of plastic, rubber and coatings.

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.

glass beaker of crystallised acetic acid
Crystallised acetic acid

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.
The first commercial methanol carbonylation process, which used a cobalt catalyst, was developed by German chemical company BASF in 1963.

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, BP Chemicals commercialised the Cativa catalyst ([Ir(CO)2I2]−), which is promoted by iridium for greater efficiency.
Known as the Cativa process, the iridium-catalyzed production of glacial acetic acid is greener, 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.
It 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.

ACETIC ACID DEHYDRATION:
Dehydration of acetic acid is one of the most important industrial uses of AD in the manufacture of aromatic acids such as terephthalic acid (TA), which involves a high purity of acetic acid.

Two major parts are used in the manufacturing process: oxidation (where p-xylene is catalytically oxidized to produce crude TA) and PTA purification.
Acetic acid, present as a solvent in the oxidation reactor but also helpful to the reaction itself, must be isolated from the oxidation-produced water.

For the effective and economical operation of a TA facility, the recovery and storage of the acetic acid solvent are important.
At high water temperatures, water, and acetic acid show a pinch point, make recovering the pure acid very difficult.

Two absorbers (low and high pressure) and an acid dehydration column consist of a traditional acetic acid recovery unit in a PTA phase.
Tall columns of 70–80 trays require the separation of acetic acid and water by traditional distillation.

N-butyl acetate, which exhibits minimal miscibility with water and forms a heterogeneous azeotrope (b.p. 90.23°C), which is a typical azeotropic agent.
With all the water being fed to the dehydration column, n-Butyl acetate is added in appropriate amounts to form an azeotrope.

On condensation, the heterogeneous azeotrope forms two phases; an organic layer containing almost pure n-butyl acetate and an aqueous layer phase containing almost pure water.

The organic phase is recycled back to the column of dehydration, while the aqueous phase is fed to a column of stripping.
The amount of acetic acid lost in the aqueous discharge is cut by approximately 40 per cent as AD results in a cleaner separation.

PROPERTIES OF ACETIC ACID:
Acetic acid is a smooth, colourless liquid with a 1 ppm visible, unpleasant vinegar odour.
The melting point of Acetic Acid is 16.73 ° C and the usual 117.9 ° C boiling point.
At 20°C, the density of pure acetic acid is 1.0491.

It is highly hygroscopic acetic acid.
Acetic Acid is possible to link the purity of the water solutions to their freezing point.
In carboxylic acids such as acetic acid, the hydrogen centre in the carboxyl group −COOH can differentiate from the molecule by ionization:

Due to this proton H+1 release, acetic acid has an acidic character.
Acetic acid is a weak monoprotic acid.

Acetic Acid has a pK value of 4.76 in an aqueous solution.
Acetate CH3COO−1 is the conjugate base.

For polar and non-polar solvents such as acid, chloroform, and hexane, Acetic Acid is miscible.
The molecules form chains in solid acetic acid, with hydrogen bonds interconnecting individual molecules.
Dimers can be found in the vapour at 120 °C.

In the liquid form, dimers often exist in dilute solutions in non-hydrogen-bonding solvents and, to a certain degree, in pure acetic acid; but are interacted with by solvents that bind to hydrogen.
Acetic acid is normally completely ionized to acetate at physiological phis.

Acetic Acid is central to the metabolism of carbohydrates and fats when bound to coenzyme A.
Acetic acid does not exist in natural triglycerides, unlike longer-chain carboxylic acids (fatty acids).

STRUCTURE OF ACETIC ACID:
Acetic Acid can be observed in the solid-state of acetic acid that there is a chain of molecules wherein individual molecules are connected to each other via hydrogen bonds.
Dimers of ethanoic acid in Acetic Acid's vapour phase can be found at temperatures approximating to 120o

Even in the liquid phase of Acetic Acid, its dimers can be found when it is present in a dilute solution.
These dimers are adversely affected by solvents that promote hydrogen bonding.

The structure of acetic acid is given by CH3(C=O)OH, or CH3CO2H
Structurally, Acetic Acid is the second simplest carboxylic acid (the simplest being formic acid, HCOOH), and is essentially a methyl group with a carboxyl functional group attached to it.

PREPARATION OF ACETIC ACID:
Acetic acid is produced industrially via the carbonylation of methanol.
Acetic Acid equations for the three steps involved in this process are provided below.

CH3OH (methanol) + HI (hydrogen iodide) → CH3I (methyl iodide intermediate) + H2O
CH3I + CO (carbon monoxide) → CH3COI (acetyl iodide)
CH3COI + H2O → CH3COOH (acetic acid) + HI

Here, a methyl iodide intermediate is generated from the reaction between methanol and hydrogen iodide.
This intermediate is then reacted with carbon monoxide and the resulting compound is treated with water to afford the acetic acid product.
It is important to note that a metal carbonyl complex must be used as a catalyst for step 2 of this process.

PHYSICAL and CHEMICAL PROPERTIES of ACETIC ACID:
Molecular Weight: 60.05 g/mol
XLogP3-AA: -0.2
Hydrogen Bond Donor Count: 1
Hydrogen Bond Acceptor Count: 2
Rotatable Bond Count: 0
Exact Mass: 60.021129366 Da
Monoisotopic Mass: 60.021129366 Da
Topological Polar Surface Area: 37.3 Å²
Heavy Atom Count: 4
Formal Charge: 0

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

Appearance: Colorless clear liquid (estimated)
Assay: 95.00 to 100.00
Titration: (99.5% - 100.5% with NaOH) (99.7 % with NaOH)
Heavy Metals: <10.00 ppm
Food Chemicals Codex Listed: Yes
Specific Gravity: 1.04700 to 1.05900 @ 25.00 °C
Pounds per Gallon - (estimated): 8.712 to 8.812
Refractive Index: 1.36600 to 1.37600 @ 20.00 °C
Melting Point: 16.60 to 16.70 °C @ 760.00 mm Hg

Boiling Point: 117.00 to 118.00 °C @ 760.00 mm Hg
Boiling Point: 48.00 to 49.00 °C @ 50.00 mm Hg
Vapor Pressure: 15.700000 mmHg @ 25.00 °C
Vapor Density: 2.07 (Air = 1)
Flash Point: 104.00 °F TCC (40.00 °C)
logP (o/w): -0.170
Shelf Life: 36.00 month(s) or longer if stored properly
Storage: Store in a cool, dry place in tightly sealed containers,
protected from heat and light

Soluble in:
Alcohol
Water, 4.759e+005 mg/L @ 25 °C (estimated)
Water, 1.00E+06 mg/L @ 25 °C (experimental)
Similar Items: Pseudoacetic acid, methane dicarboxylic acid
Molecular Weight: 60.05 g/mol
XLogP3-AA: -0.2
Hydrogen Bond Donor Count: 1
Hydrogen Bond Acceptor Count: 2
Rotatable Bond Count: 0
Exact Mass: 60.021129366 g/mol

Monoisotopic Mass: 60.021129366 g/mol
Topological Polar Surface Area: 37.3 Å²
Heavy Atom Count: 4
Formal Charge: 0
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
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
Vapor pressure: 1.54653947 kPa (20 °C); 11.6 mmHg (20 °C)
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; 1.22 cP

Dipole moment: 1.74 D
Thermochemistry
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
Physical state: Liquid
Color: Colorless
Odor: Stinging

Melting point/freezing point: Melting point/range: 16.2 °C - lit.
Initial boiling point and boiling range: 117 - 118 °C - lit.
Flammability (solid, gas): No data available
Upper/lower flammability or explosive limits:
Upper explosion limit: 19.9% (V),
Lower explosion limit: 4% (V)
Flash point: 39 °C - closed cup
Autoignition temperature: 463 °C
Decomposition temperature: Distillable in an undecomposed state at normal pressure.
pH: 2.5 at 50 g/L at 20 °C

Viscosity:
Kinematic viscosity: 1.17 mm2/s at 20 °C
Dynamic viscosity: 1.05 mPa•s at 25 °C
Water solubility: 602.9 g/L at 25 °C at 1.013 hPa - completely soluble
Partition coefficient (n-octanol/water): log Pow: -0.17 at 25 °C -
Bioaccumulation is not expected.
Vapor pressure: 20.79 hPa at 25 °C
Density: 1.049 g/cm3 at 25 °C - lit.
Relative vapor density: 2.07
Surface tension: 28.8 mN/m at 10.0 °C

CAS number: 64-19-7
Molecular formula: C2H4O2
Molecular weight: 60.052 g/mol
Density: 1.1 ± 0.1 g/cm3
Boiling point: 117.1 ± 3.0 °C at 760 mmHg
Melting point: 16.2 °C (lit.)
Flash point: 40.0 ± 0.0 °C
EC index number: 607-002-00-6
EC number: 200-580-7
Hill Formula: C₂H₄O₂
Chemical formula: CH₃COOH
Molar Mass: 60.05 g/mol

HS Code: 2915 21 00
Boiling point: 116 - 118 °C (1013 hPa)
Density: 1.04 g/cm3 (25 °C)
Explosion limit: 4 - 19.9% (V)
Flash point: 39 °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
Boiling point: 244°F
Molecular weight: 60.1

Freezing point/melting point: 62°F
Vapor pressure: 11 mmHg
Flash point: 103°F
Specific gravity: 1.05
Ionization potential: 10.66 eV
Lower explosive limit (LEL): 4.0%
Upper explosive limit (UEL): 19.9% at 200°F
NFPA health rating: 3
NFPA fire rating: 2
NFPA reactivity rating: 0
Alternative CAS RN: -
MDL Number: MFCD00036152
Storage Temperature: +20°C

Flash point: 40 °C (104 °F; 313 K)
Autoignition temperature: 427 °C (801 °F; 700 K)
Explosive limits: 4–16%
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
Vapor pressure: 1.54653947 kPa (20 °C)
11.6 mmHg (20 °C)
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
1.22 cP
Dipole moment: 1.74 D
Thermochemistry
Heat capacity (C): 123.1 J/(K⋅mol)
Std molar entropy (S⦵298): 158.0 J/(K⋅mol)
Std enthalpy of formation (ΔfH⦵298): −483.88–483.16 kJ/mol
Std enthalpy of combustion (ΔcH⦵298): −875.50–874.82 kJ/mol

FIRST AID MEASURES of ACETIC ACID:
-Description of first-aid measures:
*General advice:
First aiders need to protect themselves.
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
Call in physician.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
Call a physician immediately.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Immediately call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Make victim drink water.
Do not attempt to neutralise.
-Indication of any immediate medical attention and special treatment needed:
No data available

ACCIDENTAL RELEASE MEASURES of ACETIC ACID:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up with liquid-absorbent and neutralising material.
Dispose of properly.
Clean up affected area.

FIRE FIGHTING MEASURES of ACETIC ACID:
-Extinguishing media:
*Suitable extinguishing media:
Water
Foam
Carbon dioxide (CO2)
Dry powder
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Remove container from danger zone and cool with water.
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of ACETIC ACID:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Tightly fitting safety goggles
*Skin protection:
Full contact:
Material: butyl-rubber
Minimum layer thickness: 0,7 mm
Break through time: 480 min
Splash contact:
Material: Latex gloves
Minimum layer thickness: 0,6 mm
Break through time: 30 min
*Body Protection:
Flame retardant antistatic protective clothing.
*Respiratory protection:
Recommended Filter type: filter E-(P2)
-Control of environmental exposure:
Do not let product enter drains.

HANDLING and STORAGE of ACETIC ACID:
-Precautions for safe handling:
*Advice on protection against fire and explosion:
Take precautionary measures against static discharge.
*Hygiene measures:
Wash hands and face after working with substance.
-Conditions for safe storage, including any incompatibilities
*Storage conditions:
Keep container tightly closed in a dry and well-ventilated place.
Moisture sensitive.

STABILITY and REACTIVITY of ACETIC ACID:
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature).
-Incompatible materials:
No data available