Ascorbic acid

This article is about the molecular aspects of ascorbic acid. For information about its role in nutrition, see Vitamin C.

Template:Chembox ECNumberTemplate:Chembox E numberTemplate:Chembox AppearanceTemplate:Chembox DensityTemplate:Chembox MeltingPtTemplate:Chembox SolubilityInWaterTemplate:Chembox SolubilityTemplate:Chembox SolubilityTemplate:Chembox SolubilityTemplate:Chembox SolubilityTemplate:Chembox pKaTemplate:Chembox NFPATemplate:Chembox Lethal amounts (set)

L-Ascorbic acid

File:L-Ascorbic acid.svg
Names
IUPAC name (5R)-[(1S)-1,2-Dihydroxyethyl]-3,4-dihydroxyfuran-2(5H)-one
Other names Vitamin C
Identifiers
CAS Number	50-81-7 N
3D model (JSmol)	Interactive image Interactive image
ChEBI	CHEBI:29073 N
ChEMBL	ChEMBL196 N
ChemSpider	10189562 N
ECHA InfoCard
KEGG	D00018 Y
PubChem CID	5785
UNII	PQ6CK8PD0R Y
InChI InChI=1S/C6H8O6/c7-1-2(8)5-3(9)4(10)6(11)12-5/h2,5,7-10H,1H2/t2-,5+/m0/s1 N Key: CIWBSHSKHKDKBQ-JLAZNSOCSA-N N
SMILES OC=1C(OC(=O)C=1O)[C@@H](O)CO C([C@@H]([C@@H]1C(=C(C(=O)O1)O)O)O)O
Properties
Chemical formula	C6H8O6
Molar mass	176.12 g·mol−1
Hazards
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

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Editor-In-Chief: C. Michael Gibson, M.S., M.D. [1]

Overview

Ascorbic acid is a naturally occurring organic compound with antioxidant properties. It is a white solid, but impure samples can appear yellowish. It dissolves well in water to give mildly acidic solutions. Ascorbic acid is one form ("vitamer") of vitamin C. It was originally called L-hexuronic acid, but, when it was found to have vitamin C activity in animals ("vitamin C" being defined as a vitamin activity, not then a specific substance), the suggestion was made to rename it. The new name, ascorbic acid, is derived from a- (meaning "no") and scorbutus (scurvy), the disease caused by a deficiency of vitamin C. Because it is derived from glucose, many animals are able to produce it, but humans require it as part of their nutrition. Other vertebrates which lack the ability to produce ascorbic acid include some primates, guinea pigs, teleost fishes, bats, and some birds, all of which require it as a dietary micronutrient (that is, in vitamin form).

History

From the middle of the 18th century, it was noted that lemon and lime juice could help prevent sailors from getting scurvy. At first, it was supposed that the acid properties were responsible for this benefit; however, it soon became clear that other dietary acids, such as vinegar, had no such benefits. In 1907, two Norwegian physicians reported an essential disease-preventing compound in foods that was distinct from the one that prevented beriberi. These physicians were investigating dietary-deficiency diseases using the new animal model of guinea pigs, which are susceptible to scurvy. The newly discovered food-factor was eventually called vitamin C.

From 1928 to 1932, the Hungarian research team led by Albert Szent-Györgyi, as well as that of the American researcher Charles Glen King, identified the antiscorbutic factor as a particular single chemical substance. At the Mayo clinic, Szent-Györgyi had isolated the chemical hexuronic acid from animal adrenal glands. He suspected it to be the antiscorbutic factor but could not prove it without a biological assay. This assay was finally conducted at the University of Pittsburgh in the laboratory of King, which had been working on the problem for years, using guinea pigs. In late 1931, King's lab obtained adrenal hexuronic acid indirectly from Szent-Györgyi and, using their animal model, proved that it is vitamin C, by early 1932.

This was the last of the compound from animal sources, but, later that year, Szent-Györgyi's group discovered that paprika pepper, a common spice in the Hungarian diet, is a rich source of hexuronic acid. He sent some of the now-more-available chemical to Walter Norman Haworth, a British sugar chemist. In 1933, working with the then-Assistant Director of Research (later Sir) Edmund Hirst and their research teams, Haworth deduced the correct structure and optical-isomeric nature of vitamin C, and in 1934 reported the first synthesis of the vitamin. In honor of the compound's antiscorbutic properties, Haworth and Szent-Györgyi now proposed the new name of "a-scorbic acid" for the compound. It was named L-ascorbic acid by Haworth and Szent-Györgyi when its structure was finally proven by synthesis.

In 1937, the Nobel Prize for chemistry was awarded to Haworth for his work in determining the structure of ascorbic acid — shared with Paul Karrer, who received his award for work on vitamins — and the prize for Physiology or Medicine that year went to Albert Szent-Györgyi for his studies of the biological functions of L-ascorbic acid.

The American physician Fred R. Klenner, M.D. promoted vitamin C as a cure for many diseases in the 1950s by elevating the dosages greatly to as much as tens of grams vitamin C daily orally and by injection. From 1967 on, Nobel prize winner Linus Pauling recommended high doses of ascorbic acid as a prevention against cold and cancer; he took 18 grams daily.

Acidity

Canonical structures for the ascorbate anion

Ascorbic acid is classed as a reductone. The ascorbate anion is stabilized by electron delocalization, as shown above in terms of resonance between two canonical forms. For this reason, ascorbic acid is much more acidic than would be expected if the compound contained only isolated hydroxyl groups.

Antioxidant mechanism

File:L-Semidehydroascorbinsäure.svg

Semidehydroascorbate acid radical

Template:Citation needed sectionThe ascorbate ion is the predominant species at typical biological pH values. It is a mild reducing agent and antioxidant. It is oxidized with loss of one electron to form a radical cation and then with loss of a second electron to form dehydroascorbic acid. It typically reacts with oxidants of the reactive oxygen species, such as the hydroxyl radical. Such radicals are damaging to animals and plants at the molecular level due to their possible interaction with nucleic acids, proteins, and lipids. Sometimes these radicals initiate chain reactions. Ascorbate can terminate these chain radical reactions by electron transfer. Ascorbic acid is special because it can transfer a single electron, owing to the resonance-stabilized nature of its own radical ion called, semidehydroascorbate. The net reaction is:

RO • + C₆H₇O₆⁻ → RO- + C₆H₇O₆^• → → ROH + C₆H₆O₆

The oxidized forms of ascorbate are relatively unreactive and do not cause cellular damage.

However, being a good electron donor, excess ascorbate in the presence of free metal ions can not only promote but also initiate free radical reactions, thus making it a potentially dangerous pro-oxidative compound in certain metabolic contexts.

Reactions

Nucleophilic attack of ascorbic enol on proton to give 1,3-diketone

Food chemistry

Ascorbic acid and its sodium, potassium, and calcium salts are commonly used as antioxidant food additives. These compounds are water-soluble and, thus, cannot protect fats from oxidation: For this purpose, the fat-soluble esters of ascorbic acid with long-chain fatty acids (ascorbyl palmitate or ascorbyl stearate) can be used as food antioxidants. Eighty percent of the world's supply of ascorbic acid is produced in China.

The relevant European food additive E numbers are:

1. E300 ascorbic acid (approved for use as a food additive in the EU USA and Australia and New Zealand)
2. E301 sodium ascorbate (approved for use as a food additive in the EU USA and Australia and New Zealand)
3. E302 calcium ascorbate (approved for use as a food additive in the EU USA and Australia and New Zealand)
4. E303 potassium ascorbate
5. E304 fatty acid esters of ascorbic acid (i) ascorbyl palmitate (ii) ascorbyl stearate.

It creates volatile compounds when mixed with glucose and amino acids in 90 °C.

It is a cofactor in tyrosine oxidation.

Niche, non-food uses

• Ascorbic acid is easily oxidized and so is used as a reductant in photographic developer solutions (among others) and as a preservative.
• In fluorescence microscopy and related fluorescence-based techniques, ascorbic acid can be used as an antioxidant to increase fluorescent signal and chemically retard dye photobleaching.
• It is also commonly used to remove dissolved metal stains, such as iron, from fiberglass swimming pool surfaces.
• In plastic manufacturing, ascorbic acid can be used to assemble molecular chains more quickly and with less waste than traditional synthesis methods.
• Heroin users are known to use ascorbic acid as a means to convert heroin base to a water-soluble salt so that it can be injected.
• As justified by its reaction with iodine, it is used to negate the effects of iodine tablets in water purification. It reacts with the sterilized water, removing the taste, color, and smell of the iodine. This is why it is often sold as a second set of tablets in most sporting goods stores as Portable Aqua-Neutralizing Tablets, along with the potassium iodide tablets.
• Intravenous high-dose ascorbate is being used as a chemotherapeutic and biological response modifying agent. Currently it is still under clinical trials.

Biosynthesis

Main article: Vitamin C

Ascorbic acid is found in plants and animals where it is produced from glucose. Animals must either produce it or digest it, otherwise a lack of vitamin C may cause scurvy, which may eventually lead to death. Reptiles and older orders of birds make ascorbic acid in their kidneys. Recent orders of birds and most mammals make ascorbic acid in their liver where the enzyme L-gulonolactone oxidase is required to convert glucose to ascorbic acid. Humans, other higher primates, guinea pigs and most bats require dietary L-gulonolactone oxidase because the enzyme catalysing the last step in the biosynthesis is highly mutated and non-functional, therefore, unable to make ascorbic acid. Synthesis and signalling properties are still under investigation.

Animal ascorbic acid biosynthesis pathway

The biosynthesis of ascorbic acid starts with the formation of UDP-glucuronic acid. UDP-glucuronic acid is formed when UDP-glucose undergoes two oxidations catalyzed by the enzyme UDP-glucose 6-dehydrogenase. UDP-glucose 6-dehydrogenase uses the co-factor NAD⁺ as the electron acceptor. The transferase UDP-glucuronate pyrophosphorylase removes a UMP and glucuronokinase, with the cofactor ADP, removes the final phosphate leading to D-glucuronic acid. The aldehyde group of this is reduced to a primary alcohol using the enzyme glucuronate reductase and the cofactor NADPH, yielding L-gulonic acid. This is followed by lactone formation with the hydrolase gluconolactonase between the carbonyl on C1 and hydroxyl group on the C4. L-Gulonolactone then reacts with oxygen, catalyzed by the enzyme L-gulonolactone oxidase (which is nonfunctional in humans and other primates) and the cofactor FAD+. This reaction produces 2-oxogulonolactone, which spontaneously undergoes enolization to form ascorbic acid.

Plant ascorbic acid biosynthesis pathway

There are many different biosynthesis pathways for ascorbic acid in plants. Most of these pathways are derived from products found in glycolysis and other pathways. For example, one pathway goes through the plant cell wall polymers. The plant ascorbic acid biosynthesis pathway most principal seems to be L-galactose. L-Galactose reacts with the enzyme L-galactose dehydrogenase, whereby the lactone ring opens and forms again but with between the carbonyl on C1 and hydroxyl group on the C4, resulting in L-galactonolactone. L-Galactonolactone then reacts with the mitochondrial flavoenzyme L-galactonolactone dehydrogenase. to produce ascorbic acid. L-Ascorbic acid has a negative feedback on L-galactose dehydrogenase in spinach. Ascorbic acid efflux by embryo of dicots plants is a well-established mechanism of iron reduction, and a step obligatory for iron uptake.

Yeasts do not make L-ascorbic acid but rather a similar antioxidant known as D-erythroascorbic acid.

Industrial preparation

Ascorbic acid is prepared in industry from glucose in a method based on the historical Reichstein process. In the first of a five-step process, glucose is catalytically hydrogenated to sorbitol, which is then oxidized by the microorganism Acetobacter suboxydans to sorbose. Only one of the six hydroxy groups is oxidized by this enzymatic reaction. From this point, two routes are available. Treatment of the product with acetone in the presence of an acid catalyst converts four of the remaining hydroxyl groups to acetals. The unprotected hydroxyl group is oxidized to the carboxylic acid by reaction with the catalytic oxidant TEMPO (regenerated by sodium hypochlorite — bleaching solution). Historically, industrial preparation via the Reichstein process used potassium permanganate as the bleaching solution. Acid-catalyzed hydrolysis of this product performs the dual function of removing the two acetal groups and ring-closing lactonization. This step yields ascorbic acid. Each of the five steps has a yield larger than 90%.

A more biotechnological process, first developed in China in the 1960s, but further developed in the 1990s, bypasses the use of acetone-protecting groups. A second genetically-modified microbe species, such as mutant Erwinia, among others, oxidises sorbose into 2-ketogluconic acid (2-KGA), which can then undergo ring-closing lactonization via dehydration. This method is used in the predominant process used by the ascorbic acid industry in China, which supplies 80% of world's ascorbic acid. American and Chinese researchers are competing to engineer a mutant that can carry out a one-pot fermentation directly from glucose to 2-KGA, bypassing both the need for a second fermentation and the need to reduce glucose to sorbitol.

There exists a D-ascorbic acid, which does not occur in nature but can be synthesized artificially. It has identical antioxidant properties to L-ascorbic acid yet has far less vitamin C activity (although not quite zero). This fact is taken as evidence that the antioxidant properties of ascorbic acid are only a small part of its effective vitamin activity. To be specific, L-ascorbate is known to participate in many specific enzyme reactions that require the correct enantiomer (L-ascorbate and not D-ascorbate). L-Ascorbic acid has a specific rotation of <math>\textstyle[\alpha]_D^{20} = +23</math>°.

The outdated, but historically-important industrial synthesis of ascorbic acid from glucose via the Reichstein process.

Determination

The traditional way to analyze the ascorbic acid content is the process of titration with an oxidizing agent, and several procedures have been developed, mainly relying on iodometry. Iodine is used in the presence of a starch indicator. Iodine is reduced by ascorbic acid, and, when all the ascorbic acid has reacted, the iodine is then in excess, forming a blue-black complex with the starch indicator. This indicates the end-point of the titration. As an alternative, ascorbic acid can be treated with iodine in excess, followed by back titration with sodium thiosulfate using starch as an indicator. The preceding iodometric method has been revised to exploit reaction of ascorbic acid with iodate and iodide in acid solution. Electrolyzing the solution of potassium iodide produces iodine, which reacts with ascorbic acid. The end of process is determined by potentiometric titration in a manner similar to Karl Fischer titration. The amount of ascorbic acid can be calculated by Faraday's law.

An uncommon oxidising agent is N-bromosuccinimide, (NBS). In this titration, the NBS oxidizes the ascorbic acid in the presence of potassium iodide and starch. When the NBS is in excess (i.e., the reaction is complete), the NBS liberates the iodine from the potassium iodide, which then forms the blue-black complex with starch, indicating the end-point of the titration.

Compendial status

• British Pharmacopoeia
• Japanese Pharmacopoeia

See also

• Colour retention agent
• Erythorbic acid: a diastereomer of ascorbic acid.
• Mineral ascorbates: salts of ascorbic acid
• Acids in wine

Further reading

• Clayden; Greeves; Warren; Wothers (2001), Organic Chemistry, Oxford University Press, ISBN 0-19-850346-6.
• Davies, Michael B.; Austin, John; Partridge, David A., Vitamin C: Its Chemistry and Biochemistry, Royal Society of Chemistry, ISBN 0-85186-333-7.
• Coultate, T. P., Food: The Chemistry of Its Components (3rd ed.), Royal Society of Chemistry, ISBN 0-85404-513-9.
• Gruenwald, J.; Brendler, T.; Jaenicke, C., eds. (2004), PDR for Herbal Medicines (3rd ed.), Montvale, New Jersey: Thomson PDR.
• McMurry, John (2008), Organic Chemistry (7e ed.), Thomson Learning, ISBN 978-0-495-11628-8.

External links

• Template:ICSC

Editor-In-Chief: C. Michael Gibson, M.S., M.D. [2]; Associate Editor(s)-in-Chief:

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References

• IPCS Poisons Information Monograph (PIM) 046
• Interactive 3D-structure of vitamin C with details on the x-ray structure