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|Other names||EDTA, Y, H4EDTA, Diaminoethanetetraacetic acid, Edetic acid, Edetate, Ethylenedinitrilotetraacetic acid, Versene, Ethylene diamine tetraacetic acid, ethylenediaminetetraacetate, 2-[2-(Bis(carboxymethyl)amino) ethyl-(carboxymethyl)amino]acetic acid|
|Molar mass||292.24 g mol−1|
237–245 °C (dec.)
|Acidity (pKa)||pK1=0.0 (CO2H) (µ=1.0)
pK2=1.5 (CO2H) (µ=0.1)
pK3=2.00 (CO2H) (µ=0.1)
pK4=2.69 (CO2H) (µ=0.1)
pK5=6.13 (NH+) (µ=0.1)
pK6=10.37 (NH+) (µ=0.1)
| Y (what is this?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
EDTA is a widely used initialism for the chemical compound ethylenediaminetetraacetic acid (which has many other names, see Table). EDTA is a polyamino carboxylic acid with the formula [CH2N(CH2CO2H)2]2. This colourless, water-soluble solid is widely used to dissolve scale. Its usefulness arises because of its role as a chelating agent, i.e. its ability to "sequester" metal ions such as Ca2+ and Fe3+. After being bound by EDTA, metal ions remain in solution but exhibit diminished reactivity. EDTA is produced as several salts, notably disodium EDTA and calcium disodium EDTA.
The compound was first described in 1935 by Ferdinand Munz, who prepared the compound from ethylenediamine and chloroacetic acid. Today, EDTA is mainly synthesised from ethylenediamine (1,2-diaminoethane), formaldehyde (methanal), and sodium cyanide. This route yields the sodium salt, which can be converted in a subsequent step into the acid forms:
- H2NCH2CH2NH2 + 4 CH2O + 4 NaCN + 4 H2O → (NaO2CCH2)2NCH2CH2N(CH2CO2Na)2 + 4 NH3
- (NaO2CCH2)2NCH2CH2N(CH2CO2Na)2 + 4 HCl → (HO2CCH2)2NCH2CH2N(CH2CO2H)2 + 4 NaCl
To describe EDTA and its various protonated forms, chemists distinguish between EDTA4−, the conjugate base that is the ligand, and H4EDTA, the precursor to that ligand. At very low pH (very acidic conditions) the fully protonated H6Y2+ forms predominates (where Y denotes EDTA), whereas at very high pH or very basic condition, the fully deprotonated Y4− form is prevalent. In this article, the term EDTA is used to mean H4-xEDTAx-, whereas in its complexes edta4- stands for the tetra-deprotonated ligand.
 Coordination chemistry principles
In coordination chemistry, EDTA4- is a member of the polyamino carboxylic acid family of ligands. EDTA4- usually binds to a metal cation through its two amines and four carboxylates. Many of the resulting coordination compounds adopt octahedral geometry. Although of little consequence for its applications, these octahedral complexes are chiral. The anion [Co(edta)]− has been resolved into enantiomers. Many complexes of EDTA4- adopt more complex structures due to (i) the formation of an additional bond to water, i.e. seven-coordinate complexes, or (ii) the displacement of one carboxylate arm by water. Early work on the development of EDTA was undertaken by Gerold Schwarzenbach in the 1940s. EDTA forms especially strong complexes with Mn(II), Cu(II), Fe(III), Pb (II) and Co(III).
Several features of EDTA's complexes are relevant to its applications. First, because of its high denticity, this ligand has a high affinity for metal cations:
- [Fe(H2O)6]3+ + H4EDTA [Fe(EDTA)]- + 6 H2O + 4 H+ (Keq = 1025.1)
Written in this way, the equilibrium quotient shows that metal ions compete with protons for binding to EDTA. Because metal ions are extensively enveloped by EDTA, their catalytic properties are often suppressed. Finally, since complexes of EDTA4- are anionic, they tend to be highly soluble in water. For this reason, EDTA is able to dissolve deposits of metal oxides and carbonates.
In industry, EDTA is mainly used to sequester metal ions in aqueous solution. In the textile industry, it prevents metal ion impurities from modifying colours of dyed products. In the pulp and paper industry, EDTA inhibits the ability of metal ions, especially Mn2+, from catalyzing the disproportionation of hydrogen peroxide, which is used in "chlorine-free bleaching." In similar manner, EDTA is added to some food as a preservative or stabilizer to prevent catalytic oxidative decolouration, which is catalyzed by metal ions. In personal care products, it is added to cosmetics to improve their stability toward air. In Soft drinks containing ascorbic acid and sodium benzoate, EDTA mitigates formation of benzene (a carcinogen).
The reduction of water hardness in laundry applications and the dissolution of scale in boilers both rely on EDTA and related complexants to bind Ca2+ and Mg2+ ions as well as other metal ions. Once bound to EDTA, these metal centers tend not to form precipitates or to interfere with the action of the detergents. For similar reasons, cleaning solutions often contain EDTA.
The solubilization of ferric ions near neutral pH is accomplished using EDTA. This property is useful in agriculture including hydroponics, especially in calcareous soils. Otherwise, at near-neutral pH, iron(III) forms insoluble salts, which are less bioavailable. Aqueous [Fe(edta)]- is used for removing ("scrubbing") hydrogen sulfide from gas streams. This conversion is achieved by oxidizing the hydrogen sulfur to elemental sulfur, which is non-volatile:
- 2 [Fe(edta)]- + H2S → 2 [Fe(edta)]2- + S + 2 H+
In this application, the ferric center is reduced to its ferrous derivative, which can then be reoxidized by air. In similar manner, nitrogen oxides are removed from gas streams using [Fe(edta)]2-. The oxidizing properties of [Fe(edta)]- are also exploited in photography, where it is used to solubilize silver particles.
EDTA was an most important chelating agents used in the separation of the lanthanide metals by ion-exchange chromatography. Perfected by F.H. Spedding et al. in 1954, the method relies on the steady increase in stability constant of the lanthanide EDTA complexes with atomic number. Using sulfonated polystyrene beads and copper(II) as a retaining ion, EDTA causes the lanthanides to migrate down the column of resin while separating into bands of pure lanthanide. The lanthanides elute in order of decreasing atomic number. Due to the expense of this method, relative to counter-current solvent extraction, ion-exchange is now used only to obtain the highest purities of lanthanide (typically greater than 4N, 99.99%).
EDTA is used to bind metal ions in chelation therapy, e.g., for mercury (performs poorly) and lead poisoning. It is used in a similar manner to remove excess iron from the body. This therapy is used to treat the complication of repeated blood transfusions, as would be applied to treat thalassaemia. EDTA acts as a powerful antioxidant to prevent free radicals from injuring blood vessel walls. 
Dentists use EDTA solutions to remove inorganic debris (smear layer) and prepare root canals for obturation. It serves as a preservative (usually to enhance the action of another preservative such as benzalkonium chloride or thiomersal) in ocular preparations and eyedrops. In evaluating kidney function, the complex [Cr(edta)]- is administered intravenously and its filtration into the urine is monitored. This method is useful for evaluating glomerular filtration rate.
EDTA is used extensively in the analysis of blood. It is an anticoagulant for blood samples for CBC/FBEs (complete blood count also known as full blood examination). Laboratory studies also suggest that EDTA chelation may prevent collection of platelets on the lining of the vessel [such as arteries] (which can otherwise lead to formation of blood clots, which itself is associated with atheromatous plaque formation or rupture, and thereby ultimately disrupts blood flow). These ideas are theoretical, and have so far been proven ineffective; however a major clinical study of the effects of EDTA on coronary arteries is currently (2008) proceeding. EDTA played a role in the O.J. Simpson trial when the defense alleged that one of the blood samples collected from Simpson's estate was found to contain traces of the compound.
 Laboratory applications
In the laboratory, EDTA is widely used for scavenging metal ions: In biochemistry and molecular biology, ion depletion is commonly used to deactivate metal-dependent enzymes, either as an assay for their reactivity or to suppress damage to DNA or proteins. In analytical chemistry, EDTA is used in complexometric titrations and analysis of water hardness or as a masking agent to sequester metal ions that would interfere with the analyses. EDTA is added to some buffer solutions.
EDTA finds many specialized uses in the biomedical laboratories, such as in veterinary ophthalmology as an anticollagenase to prevent the worsening of corneal ulcers in animals. In tissue culture EDTA is used as a chelating agent that binds to calcium and prevents joining of cadherins between cells, preventing clumping of cells grown in liquid suspension, or detaching adherent cells for passaging.
In Histopathology, EDTA can be used as a decalcifying agent making it possible to cut sections using a microtome once the tissue sample is demineralised
 Toxicity and environmental considerations
EDTA is in such widespread use that it has emerged as a persistent organic pollutant. Its degradation entails conversion to ethylenediaminetriacetic acid, which then cyclizes. Alternative, more readily degradable chelating agents are being developed such as ethylenediamine-N,N'-disuccinic acid.
EDTA exhibits low acute toxicity with LD50 (rat) of 2.0 – 2.2 g/kg. It has been found to be both cytotoxic and weakly genotoxic in laboratory animals. Oral exposures have been noted to cause reproductive and developmental effects. The same study by Lanigan also found that both dermal exposure to EDTA in most cosmetic formulations and inhalation exposure to EDTA in aerosolized cosmetic formulations would produce systemic effects below those seen to be toxic in oral dosing studies.
 Methods of detection and analysis
The most sensitive method of detecting and measuring EDTA in biological samples is selected-reaction-monitoring capillary-electrophoresis mass-spectrometry (abbreviation SRM-CE/MS) which has a detection limit of 7.3 ng/mL in human plasma and a quantitation limit of 15 ng/mL. This method works with sample volumes as small as ~7-8 nL.
 See also
 Notes & References
- ^ Harris, D.C. "Quantitative Chemical Analysis", 7th ed., W. H. Freeman and Compagny, New York, 2007
- ^ F. Munz "Polyamino carboxylic acids to I. G. Farbenindustrie, DE 718 981, 1935; US 2 130 505, 1938.
- ^ Synthesis of EDTA
- ^ a b c J. Roger Hart "Ethylenediaminetetraacetic Acid and Related Chelating Agents" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.
- ^ Kirchner, S. Barium (Ethylenediaminetetracetato) Cobalt(III) 4-Hydrate" Inorganic Syntheses, 1957, Volume 5, pages 186-188.
- ^ Edta - Motm
- ^ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
- ^ Furia T (1964). "EDTA in Foods — A technical review". Food Technology 18 (12): 1874–1882.
- ^ a b c Lanigan RS and Yamarik TA (2002). "Final report on the safety assessment of EDTA, calcium disodium EDTA, diammonium EDTA, dipotassium EDTA, disodium EDTA, TEA-EDTA, tetrasodium EDTA, tripotassium EDTA, trisodium EDTA, HEDTA, and trisodium HEDTA". Int J Toxicol. 21 Suppl 2: 95–142. http://www.ncbi.nlm.nih.gov/sites/entrez?cmd=Retrieve&db=PubMed&list_uids=12396676&dopt=AbstractPlus. Retrieved 2008-01-28.
- ^ US Food and Drug Administration: Center for Food Safety and Applied Nutrition Questions and Answers on the Occurrence of Benzene in Soft Drinks and Other Beverages
- ^ Ruth DeBusk et al. (2002). "Ethylenediaminetetraacetic acid (EDTA)". http://www.umm.edu/altmed/articles/ethylenediaminetetraacetic-acid-000302.htm. Retrieved 2007-07-25.
- ^ http://www.umm.edu/altmed/articles/ethylenediaminetetraacetic-acid-000302.htm
- ^ http://www.oralchelation.net/data/EDTA/data14e.htm
- ^ See "les conservateurs en opthalmologie" Doctors Patrice Vo Tan & Yves lachkar, Librarie Médicale Théa.
- ^ http://www.quackwatch.org/01QuackeryRelatedTopics/chelationimp.html
- ^ http://www.clinicaltrials.gov/ct/show/NCT00044213?order=2
- ^ http://query.nytimes.com/gst/fullpage.html?sec=health&res=990CE4DD1F3DF935A15754C0A963958260
- ^ Zhiwen Yuan, Jeanne M. VanBriesen "The Formation of Intermediates in EDTA and NTA Biodegradation" Environmental Engineering Science 2006, volume 23, pp. 533-544. doi:10.1089/ees.2006.23.533
- ^ a b Robin L. Sheppard, and Jack Henion (1997). "Determining EDTA in Blood" ([dead link] – Scholar search). Analytical Chemistry 69: 477A–480A. http://pubs.acs.org/hotartcl/ac/97/aug/det.html. Retrieved 2007-07-25.
- ^ S. Loyaux-Lawniczak, J. Douch, and P. Behra (1999). "Optimisation of the analytical detection of EDTA by HPLC in natural waters". Fresenius' J. Anal. Chem. 364 (8): 727–731. doi:10.1007/s002160051422. http://cat.inist.fr/?aModele=afficheN&cpsidt=1898737. Retrieved 2007-07-25.
- ^ Carolina E. Cagnassoa, Laura B. López, Viviana G. Rodríguez and Mirta E. Valencia (May 2006). "Development and validation of a method for the determination of EDTA in non-alcoholic drinks by HPLC". Journal of Food Composition and Analysis 20 (3-4): 248. doi:10.1016/j.jfca.2006.05.008.
- Lanigan RS, Yamarik TA (2002). "Final report on the safety assessment of EDTA, calcium disodium EDTA, diammonium EDTA, dipotassium EDTA, disodium EDTA, TEA-EDTA, tetrasodium EDTA, tripotassium EDTA, trisodium EDTA, HEDTA, and trisodium HEDTA". Int. J. Toxicol. 21 Suppl 2: 95–142. doi:10.1080/10915810290096522. PMID 12396676.
- pH-Spectrum of EDTA complexes
- EDTA: Molecule of the Month
- EDTA Determination of Total Water Hardness
- 507 references regarding oral EDTA
- EDTA: the chelating agent under environmental scrutiny, Química Nova, Nov.-Dec., 2003 (text version)
- EDTA: the chelating agent under environmental scrutiny, Química Nova, Nov.-Dec., 2003 (PDF version)