View source for Chemistry:Ethylenediaminetetraacetic acid


{{chembox
|Verifiedfields = changed
|Watchedfields = changed
|verifiedrevid = 408562373
|ImageFile = EDTA.svg
|ImageFile_Ref = {{chemboximage|correct|??}}
|ImageName = Skeletal formula of ethylenediaminetetraacetic acid
|IUPACName = ''N'',''N''′-(Ethane-1,2-diyl)bis[''N''-(carboxymethyl)glycine]<ref name=iupac2013 />
|SystematicName = 2,2′,2′′,2′′′-(Ethane-1,2-diyldinitrilo)tetraacetic acid<ref name=iupac2013>{{cite book | title =  Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book) | publisher = [[Organization:Royal Society of Chemistry|The Royal Society of Chemistry]] | date = 2014 | location = Cambridge | pages = 79, 123, 586, 754 | isbn = 978-0-85404-182-4 }}</ref>
|OtherNames = {{Anchor|Names}} {{unbulleted list|EthyleneDiamineTetraAcetic acid|Diaminoethane-tetraacetic acid|Edetic acid ([[Chemistry:Conjugate acid|conjugate base]] edetate) ([[Medicine:International nonproprietary name|INN]], USAN)|Versene}}
|Section1 = {{Chembox Identifiers
|Abbreviations = EDTA, H<sub>4</sub>EDTA
|CASNo = 60-00-4
|CASNo_Ref = {{cascite|correct|CAS}}
|CASNo_Comment = (free acid)
|CASNo2_Ref = {{cascite|correct|CAS}}
|CASNo2 = 6381-92-6 
|CASNo2_Comment = (dihydrate disodium salt) <!--also verified against the Chemical Abstracts Service list -->
|PubChem = 6049
|ChemSpiderID = 5826
|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
|DrugBank = DB00974
|DrugBank_Ref = {{drugbankcite|correct|drugbank}}
|UNII = 9G34HU7RV0
|UNII_Ref = {{fdacite|correct|FDA}}
|UNII1_Ref = {{fdacite|correct|FDA}}
|UNII1 = 7FLD91C86K
|UNII1_Comment = (dihydrate disodium salt)
|EINECS = 200-449-4
|UNNumber = 3077
|KEGG = D00052
|KEGG_Ref = {{keggcite|correct|kegg}}
|MeSHName = Edetic+Acid
|ChEBI = 4735
|ChEBI_Ref = {{ebicite|correct|EBI}}
|ChEMBL = 858
|ChEMBL_Ref = {{ebicite|correct|EBI}}
|RTECS = AH4025000
|Beilstein = 1716295
|Gmelin = 144943
|SMILES = OC(=O)CN(CCN(CC(O)=O)CC(O)=O)CC(O)=O
|StdInChI = 1S/C10H16N2O8/c13-7(14)3-11(4-8(15)16)1-2-12(5-9(17)18)6-10(19)20/h1-6H2,(H,13,14)(H,15,16)(H,17,18)(H,19,20)
|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
|StdInChIKey = KCXVZYZYPLLWCC-UHFFFAOYSA-N
|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
}}
|Section2 = {{Chembox Properties
|C=10 | H=16 | N=2 | O=8
|Appearance = Colourless crystals
|Density = 0.860 g&nbsp;cm<sup>−3</sup> (at 20&nbsp;°C)
|LogP = −0.836
|pKa = 2.0, 2.7, 6.16, 10.26<ref>[https://onlinelibrary.wiley.com/doi/abs/10.1002/9780470110195.ch10 Raaflaub, J. (1956) ''Methods Biochem. Anal.'' 3, 301–324.]</ref>
| pKb = <!-- see text -->
}}
|Section3 = {{Chembox Thermochemistry
|DeltaHf = −1765.4 to −1758.0 kJ&nbsp;mol<sup>−1</sup>
|DeltaHc = −4461.7 to −4454.5 kJ&nbsp;mol<sup>−1</sup>
}}
|Section4 = {{Chembox Pharmacology
|AdminRoutes = {{unbulleted list|Intramuscular|Intravenous}}
|ATCCode_prefix = S01
|ATCCode_suffix = XA05
|ATC_Supplemental = {{ATC|V03|AB03}} (salt)
}}
|Section5 = {{Chembox Hazards
|GHSPictograms = {{gHS exclamation mark}}
|GHSSignalWord = '''WARNING'''
|HPhrases = {{h-phrases|319}}
|PPhrases = {{p-phrases|305+351+338}}
|NFPA-H = 1
|NFPA-F = 0
|NFPA-R = 0
|LD50 = 1000 mg/kg (oral, rat)<ref>[https://chem.nlm.nih.gov/chemidplus/rn/62-33-9 Substance Name: Sodium calcium edetate]. NIH.gov</ref>
}}
|Section6 = {{Chembox Related
|OtherFunction_label = alkanoic acids
|OtherFunction = {{unbulleted list|[[Chemistry:Daminozide|Daminozide]]|[[Chemistry:Octopine|Octopine]]}}
|OtherCompounds = {{unbulleted list|[[Chemistry:Triethylenetetramine|Triethylenetetramine]]|[[Chemistry:Tetraacetylethylenediamine|Tetraacetylethylenediamine]]|[[Chemistry:PMDTA|PMDTA]]|[[Chemistry:Bis-tris propane|Bis-tris propane]]}}
}}
}}

'''Ethylenediaminetetraacetic acid''' ('''EDTA'''), also called '''EDTA acid''' after its own abbreviation, is an [[Chemistry:Aminopolycarboxylic acid|aminopolycarboxylic acid]] with the formula [CH<sub>2</sub>N(CH<sub>2</sub>CO<sub>2</sub>H)<sub>2</sub>]<sub>2</sub>. This white, water-insoluble solid is widely used to bind to iron (Fe<sup>2+</sup>/Fe<sup>3+</sup>) and calcium ions (Ca<sup>2+</sup>), forming water-soluble [[Chemistry:Coordination complex|complexes]] even at neutral pH.  It is thus used to dissolve Fe- and Ca-containing scale as well as to deliver iron ions under conditions where its oxides are insoluble.  EDTA is available as several salts, notably '''disodium EDTA''', [[Chemistry:Sodium calcium edetate|sodium calcium edetate]], and [[Chemistry:Tetrasodium EDTA|tetrasodium EDTA]], but these all function similarly.<ref name="Ullmann" />

==Uses==
=== Textiles and paper ===
In industry, EDTA is mainly used to [[Chemistry:Sequestrant|sequester]] (bind or confine) 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 [[Chemistry:Manganese|Mn<sup>2+</sup>]], from catalysing the [[Biology:Disproportionation|disproportionation]] of [[Chemistry:Hydrogen peroxide|hydrogen peroxide]], which is used in chlorine-free bleaching.

=== Food ===
In a similar manner, EDTA is added to some food as a [[Chemistry:Preservative|preservative]] or stabiliser to prevent catalytic oxidative decolouration, which is catalysed by metal ions.<ref name="furia1964">{{cite journal | last=Furia | first=T. | title=EDTA in Foods – A technical review | journal=Food Technology | volume=18 | issue=12 | pages=1874–1882 | year=1964}}</ref>

=== Water softener ===
The reduction of water hardness in laundry applications and the dissolution of scale in boilers both rely on EDTA and related [[Chemistry:Complex|complexants]] to bind [[Chemistry:Calcium|Ca<sup>2+</sup>]], [[Chemistry:Magnesium|Mg<sup>2+</sup>]], as well as other metal ions. Once bound to EDTA, these metal complexes are less likely to form precipitates or to interfere with the action of the [[Chemistry:Soap|soap]]s and detergents.{{Cn|date=June 2022}} For similar reasons, cleaning solutions often contain EDTA.  In a similar manner EDTA is used in the cement industry for the determination of free [[Earth:Limestone|lime]] and free [[Chemistry:Magnesium oxide|magnesia]] in cement  and clinkers.<ref name="Cement Chemistry, H. F. W. Taylor">{{Cite book |last=Taylor |first=H. F. W. |year=1990 |title=Cement Chemistry |publisher=Academic Press |isbn=978-0-12-683900-5}}</ref>{{page needed|date=October 2017}}

The solubilisation of [[Chemistry:Iron|Fe<sup>3+</sup>]] ions at or below near neutral [[Chemistry:PH|pH]] can be accomplished using EDTA.  This property is useful in [[Earth:Agriculture|agriculture]] including hydroponics. However, given the pH dependence of ligand formation, EDTA is not helpful for improving iron solubility in above neutral soils.<ref>{{Cite journal | doi = 10.2136/sssaj1969.03615995003300010024x| title = Reactions of EDTA Complexes of Fe, Zn, Mn, and Cu with Soils| journal = Soil Science Society of America Journal| volume = 33| issue = 1| page = 86| year = 1969| last1 = Norvell | first1 = W. A.| last2 = Lindsay | first2 = W. L.| bibcode = 1969SSASJ..33...86N}}</ref>  Otherwise, at near-neutral pH and above, iron(III) forms insoluble salts, which are less [[Chemistry:Bioavailability|bioavailable]] to susceptible plant species. 

=== Scrubbing ===
Aqueous [Fe(EDTA)]<sup>−</sup> is used for removing ("scrubbing") [[Chemistry:Hydrogen sulfide|hydrogen sulfide]] from gas streams.  This conversion is achieved by oxidising the hydrogen sulfide to elemental sulfur, which is non-volatile:
:2&nbsp;[Fe(EDTA)]<sup>−</sup>  +  [[Chemistry:Hydrogen sulfide|H<sub>2</sub>S]]  →  2&nbsp;[Fe(EDTA)]<sup>2−</sup>  +  [[Chemistry:Sulfur|S]]  +  2&nbsp;H<sup>+</sup>
In this application, the iron(III) centre is [[Chemistry:Redox|reduced]] to its iron(II) derivative, which can then be reoxidised by air.  In similar manner, [[Chemistry:Nitrogen oxide|nitrogen oxide]]s are removed from gas streams using [Fe(EDTA)]<sup>2−</sup>. 

The oxidising properties of [Fe(EDTA)]<sup>−</sup> are also exploited in [[Photography|photography]], where it is used to solubilise [[Chemistry:Silver|silver]] particles.<ref name="Ullmann" />

=== Ion-exchange chromatography ===
EDTA was used in separation of the lanthanide metals by ion-exchange chromatography.  Perfected by F.&nbsp;H. Spedding ''et al''. in 1954, the method relies on the steady increase in [[Chemistry:Stability constants of complexes|stability constant]] of the lanthanide EDTA complexes with [[Physics:Atomic number|atomic number]].<ref>{{Cite tech report |last1=Powell |first1=J. E. |last2=Spedding |first2=F. H. |date=1956 |title=Basic Principles Involved in the Macro-Separation of Adjacent Rare Earths from Each Other by Means of Ion Exchange |publisher=Iowa State College |doi=10.2172/4289324 |doi-access=free |s2cid=93195586 |osti=4289324 |osti-access=free}}</ref> Using [[Chemistry:Sulfonate|sulfonate]]d [[Chemistry:Polystyrene|polystyrene]] beads and [[Chemistry:Copper|Cu<sup>2+</sup>]] as a retaining ion, EDTA causes the lanthanides to migrate down the column of resin while separating into bands of pure lanthanides. The lanthanides elute in order of decreasing atomic number. Due to the expense of this method, relative to countercurrent solvent extraction, ion exchange is now used only to obtain the highest purities of lanthanides (typically greater than 99.99%).{{Citation needed|date=June 2009}}

===Medicine===
[[Chemistry:Sodium calcium edetate|Sodium calcium edetate]], an EDTA derivative, is used to bind metal ions in the practice of [[Unsolved:Chelation therapy|chelation therapy]], such as for treating [[Medicine:Mercury poisoning|mercury]] and [[Medicine:Lead poisoning|lead poisoning]].<ref name=r1>{{cite web | last = DeBusk | first = Ruth | title = Ethylenediaminetetraacetic acid (EDTA) | year = 2002 | url=http://www.umm.edu/altmed/articles/ethylenediaminetetraacetic-acid-000302.htm | archive-url=https://web.archive.org/web/20070504081119/http://www.umm.edu/altmed/articles/ethylenediaminetetraacetic-acid-000302.htm| archive-date=2007-05-04 | publisher=University of Maryland Medical Center|display-authors=0}}</ref> It is used in a similar manner to remove excess [[Chemistry:Iron|iron]] from the body. This therapy is used to treat the complication of repeated [[Medicine:Blood transfusion|blood transfusion]]s, as would be applied to treat thalassaemia.

==== Dentistry ====
Dentists and endodontists use EDTA solutions to remove inorganic debris ([[Medicine:Smear layer|smear layer]]) and lubricate the [[Medicine:Root canal|root canal]]s in endodontics.  This procedure helps prepare root canals for [[Engineering:Obturation|obturation]].  Furthermore, EDTA solutions with the addition of a [[Biology:Surfactant|surfactant]] loosen up [[Biology:Calcification|calcification]]s inside a root canal and allow instrumentation (canal shaping) and facilitate apical advancement of a file in a tight or calcified root canal towards the apex.

==== Eyedrops ====
It serves as a [[Chemistry:Preservative|preservative]] (usually to enhance the action of another preservative such as [[Chemistry:Benzalkonium chloride|benzalkonium chloride]] or [[Chemistry:Thiomersal|thiomersal]]) in ocular preparations and eyedrops.

==== Analysis ====
In [[Medicine:Medical diagnosis|medical diagnosis]] and organ function tests (here, kidney function test), the [[Chemistry:Chromium|chromium(III)]] complex [Cr(EDTA)]<sup>−</sup> (as radioactive [[Physics:Chromium-51|chromium-51]] (<sup>51</sup>Cr)) is administered intravenously and its filtration into the [[Biology:Urine|urine]] is monitored. This method is useful for evaluating [[Medicine:Renal function#Measurement with radioactive tracers|glomerular filtration rate]] (GFR) in [[Medicine:Nuclear medicine|nuclear medicine]].<ref>{{cite journal|last1=Soveri|first1=Inga|last2=Berg|first2=Ulla B.|last3=Björk|first3=Jonas|last4=Elinder|first4=Carl-Gustaf|last5=Grubb|first5=Anders|last6=Mejare|first6=Ingegerd|last7=Sterner|first7=Gunnar|last8=Bäck|first8=Sten-Erik|title=Measuring GFR: A Systematic Review|journal=American Journal of Kidney Diseases|date=September 2014|volume=64|issue=3|pages=411–424|doi=10.1053/j.ajkd.2014.04.010|pmid=24840668}}</ref>

EDTA is used extensively in the analysis of blood.  It is an [[Medicine:Anticoagulant|anticoagulant]] for blood samples for [[Medicine:Complete blood count|CBC/FBC]]s, where the EDTA chelates the calcium present in the blood specimen, arresting the coagulation process and preserving blood cell morphology.<ref>{{cite journal |pmid=17484616 |year=2007 |last1=Banfi |first1=G |title=The role of ethylenediamine tetraacetic acid (EDTA) as in vitro anticoagulant for diagnostic purposes |journal=Clinical Chemistry and Laboratory Medicine |volume=45 |issue=5 |pages=565–76 |last2=Salvagno |first2=G. L |last3=Lippi |first3=G |doi=10.1515/CCLM.2007.110 |s2cid=23824484 }}</ref> Tubes containing EDTA are marked with [[Lavender (color)|lavender]] (purple) or pink tops.<ref name="mi">{{cite web |title=ORDER OF DRAW FOR MULTIPLE TUBE COLLECTIONS |url=http://mlabs.umich.edu/files/pdfs/PRC%20-%20Order_Draw_Multiple.pdf |publisher=Michigan Medicine Laboratories |date=2019-09-15 |access-date=2020-03-27 |archive-date=2019-11-26 |archive-url=https://web.archive.org/web/20191126160736/http://mlabs.umich.edu/files/pdfs/PRC%20-%20Order_Draw_Multiple.pdf }}</ref> EDTA is also in tan top tubes for lead testing and can be used in royal blue top tubes for trace metal testing.<ref name="mi" />

EDTA is a slime dispersant, and has been found to be highly effective in reducing bacterial growth during implantation of [[Biology:Intraocular lens|intraocular lens]]es (IOLs).<ref>{{Cite journal | doi = 10.1093/jac/dkn533| pmid = 19147522| title = Impact of slime dispersants and anti-adhesives on in vitro biofilm formation of Staphylococcus epidermidis on intraocular lenses and on antibiotic activities| journal = Journal of Antimicrobial Chemotherapy| volume = 63| issue = 3| pages = 480–4| year = 2009| last1 = Kadry | first1 = A. A.| last2 = Fouda | first2 = S. I.| last3 = Shibl | first3 = A. M.| last4 = Abu El-Asrar | first4 = A. A.| doi-access = }}</ref>

===Alternative medicine===
Some [[Medicine:Alternative medicine|alternative practitioners]] believe EDTA acts as an [[Biology:Antioxidant|antioxidant]],  preventing [[Biology:Free radical|free radical]]s from injuring [[Biology:Blood vessel|blood vessel]] walls, therefore reducing [[Medicine:Atherosclerosis|atherosclerosis]].<ref>{{Cite journal |  pmc=1282574| doi = 10.1186/1471-2261-5-32| pmid = 19147522| title = EDTA chelation therapy for cardiovascular disease: a systematic review| journal = BMC Cardiovasc Disord| volume = 5| issue = 32| year = 2005| last1 = Seely | first1 = D. M.| last2 = Wu | first2 = P.| last3 = Mills | first3 = E. J.| pages = 480–484| doi-access = free}}</ref> These ideas are unsupported by scientific studies, and seem to contradict some currently accepted principles.<ref>{{cite web|url=http://www.quackwatch.org/01QuackeryRelatedTopics/chelationimp.html|title=EDTA Chelation Therapy for Atherosclerosis And Degenerative Diseases: Implausibility and Paradoxical Oxidant Effects|last1=Green|first1=Saul|first2=Wallace|last2=Sampson|date= December 14, 2002|work=Quackwatch|access-date=16 December 2009}}</ref> The [[Organization:Food and Drug Administration|U.S. FDA]] has not approved it for the treatment of atherosclerosis.<ref>{{cite web|url=https://www.fda.gov/Drugs/DrugSafety/PostmarketDrugSafetyInformationforPatientsandProviders/ucm113738.htm|title=Postmarket Drug Safety Information for Patients and Providers – Questions and Answers on Edetate Disodium (marketed as Endrate and generic products)|work=U.S. Food and Drug Administration}}</ref>

===Cosmetics===
In [[Medicine:Shampoo|shampoo]]s, cleaners, and other personal care products, EDTA salts are used as a sequestering agent to improve their stability in air.<ref name="lanigan2002" />

===Laboratory applications===
In the laboratory, EDTA is widely used for scavenging metal ions: In [[Biology:Biochemistry|biochemistry]] and [[Biology:Molecular biology|molecular biology]], ion depletion is commonly used to deactivate metal-dependent enzymes, either as an assay for their reactivity or to suppress damage to [[Biology:DNA|DNA]], [[Biology:Protein|protein]]s, and [[Chemistry:Polysaccharide|polysaccharide]]s.<ref>{{cite journal |title=A novel nuclease activity that is activated by Ca<sup>2+</sup> chelated to EGTA |last1=Domínguez |first1=K. |last2=Ward |first2=W. S. |journal=[[Medicine:Systems Biology in Reproductive Medicine|Systems Biology in Reproductive Medicine]] |date=December 2009 |volume=55 |issue=5–6|doi=10.3109/19396360903234052 |pmid=19938954 |pages=193–199|pmc=2865586 }}</ref> EDTA also acts as a selective [[Biology:Enzyme inhibitor|inhibitor]] against dNTP hydrolyzing enzymes ([[Biology:Taq polymerase|Taq polymerase]], [[Biology:DUTP diphosphatase|dUTPase]], MutT),<ref>{{Cite journal|last1=Lopata|first1=Anna|last2=Jójárt|first2=Balázs|last3=Surányi|first3=Éva V.|last4=Takács|first4=Enikő|last5=Bezúr|first5=László|last6=Leveles|first6=Ibolya|last7=Bendes|first7=Ábris Á|last8=Viskolcz|first8=Béla|last9=Vértessy|first9=Beáta G.|last10=Tóth|first10=Judit|date=October 2019|title=Beyond Chelation: EDTA Tightly Binds Taq DNA Polymerase, MutT and dUTPase and Directly Inhibits dNTPase Activity|journal=Biomolecules|volume=9|issue=10|page=621|doi=10.3390/biom9100621|pmid=31627475|pmc=6843921|doi-access=free}}</ref> liver [[Biology:Arginase|arginase]]<ref>{{Cite journal|last1=Carvajal|first1=Nelson|last2=Orellana|first2=María S|last3=Bórquez|first3=Jessica|last4=Uribe|first4=Elena|last5=López|first5=Vasthi|last6=Salas|first6=Mónica|date=2004-08-01|title=Non-chelating inhibition of the H101N variant of human liver arginase by EDTA|journal=Journal of Inorganic Biochemistry|volume=98|issue=8|pages=1465–1469|doi=10.1016/j.jinorgbio.2004.05.005|pmid=15271525|issn=0162-0134}}</ref> and [[Biology:Horseradish peroxidase|horseradish peroxidase]]<ref>{{Cite journal|last1=Bhattacharyya|first1=D K|last2=Adak|first2=S|last3=Bandyopadhyay|first3=U|last4=Banerjee|first4=R K|date=1994-03-01|title=Mechanism of inhibition of horseradish peroxidase-catalysed iodide oxidation by EDTA.|journal=Biochemical Journal|volume=298|issue=Pt 2|pages=281–288|issn=0264-6021|pmc=1137937|pmid=8135732|doi=10.1042/bj2980281}}</ref> independently of metal ion [[Chemistry:Chelation|chelation]]. These findings urge the rethinking of the utilisation of EDTA as a biochemically inactive metal ion scavenger in enzymatic experiments. In analytical chemistry, EDTA is used in [[Chemistry:Complexometric titration|complexometric titration]]s and analysis of water hardness or as a [[Chemistry:Masking agent|masking agent]] to sequester metal ions that would interfere with the analyses.

EDTA finds many specialised uses in the biomedical labs, such as in veterinary [[Medicine:Ophthalmology|ophthalmology]] as an [[Biology:Collagenase|anticollagenase]] to prevent the worsening of [[Medicine:Corneal ulcers in animals|corneal ulcers in animals]]. In [[Biology:Tissue culture|tissue culture]] EDTA is used as a chelating agent that binds to [[Chemistry:Calcium|calcium]] and prevents joining of cadherins between cells, preventing clumping of cells grown in liquid suspension, or detaching adherent cells for passaging. In [[Medicine:Histopathology|histopathology]], EDTA can be used as a decalcifying agent making it possible to cut sections using a [[Biology:Microtome|microtome]] once the tissue sample is demineralised.

EDTA is also known to inhibit a range of [[Biology:Metalloproteinase|metallopeptidases]], the method of inhibition occurs via the [[Chemistry:Chelation|chelation]] of the metal ion required for catalytic activity.<ref>{{Cite book| pmid = 7674923| year = 1995| last1 = Auld| first1 = D. S.| chapter = Removal and replacement of metal ions in metallopeptidases| title = Proteolytic Enzymes: Aspartic and Metallo Peptidases| series = Methods in Enzymology| volume = 248| pages = 228–242 | doi = 10.1016/0076-6879(95)48016-1 | isbn = 978-0-12-182149-4}}</ref> EDTA can also be used to test for [[Chemistry:Bioavailability|bioavailability]] of heavy metals in [[Earth:Sediment|sediment]]s. However, it may ''influence'' the bioavailability of metals in solution, which may pose concerns regarding its effects in the environment, especially given its widespread uses and applications.

EDTA is also used to remove crud (corroded metals) from fuel rods in nuclear reactors.<ref>{{cite journal |url=https://www.sciencedirect.com/science/article/pii/B9780124058972000203 |first1=Gregory |last1=Choppin |first2=Jan-Olov |last2=Liljenzin |first3=Jan |last3=Rydberg |first4=Christian |last4=Ekberg |date=2013 |title=Chapter 20 - Nuclear Power Reactors |journal=Radiochemistry and Nuclear Chemistry |edition=Fourth  |pages=655–684 |doi=10.1016/B978-0-12-405897-2.00020-3|isbn=978-0-12-405897-2 }}</ref>

==Side effects==
EDTA exhibits low acute toxicity with {{LD50}} (rat) of 2.0&nbsp;g/kg to 2.2&nbsp;g/kg.<ref name="Ullmann"/> It has been found to be both [[Biology:Cytotoxicity|cytotoxic]] and weakly [[Biology:Genotoxicity|genotoxic]] in laboratory animals.  Oral exposures have been noted to cause reproductive and developmental effects.<ref name="lanigan2002">{{cite journal|last1=Lanigan |first1=R. S. |last2=Yamarik |first2=T. A. | title=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 | journal=International Journal of Toxicology |volume='''21''' Suppl. 2 |pages=95–142 |year=2002 |pmid=12396676|doi=10.1080/10915810290096522 | issue=5|s2cid=83388249 }}</ref> The same study<ref name="lanigan2002" /> also found that both dermal exposure to EDTA in most cosmetic formulations and inhalation exposure to EDTA in [[Chemistry:Aerosol|aerosol]]ised cosmetic formulations would produce exposure levels below those seen to be toxic in oral dosing studies.

==Synthesis==

The compound was first described in 1935 by Ferdinand Münz,<ref>{{cite journal |last=Paolieri |first=Matteo |date=December 2017 |title= Ferdinand Münz: EDTA and 40 years of inventions |url=https://www.researchgate.net/publication/321552574 |journal=Bull. Hist. Chem. |publisher=ACS | volume=42 |issue=2 |pages=133–140}}</ref> who prepared the compound from [[Chemistry:Ethylenediamine|ethylenediamine]] and [[Chemistry:Chloroacetic acid|chloroacetic acid]].<ref>{{cite patent|inventor-last=Münz|inventor-first=Ferdinand|inventor-link=Ferdinand_Münz|pubdate=1938-09-20|title=Polyamino carboxylic acids and process of making same|assign1=General Aniline Works Ltd.|country=US|number=2130505}}. Also {{cite patent|inventor-last=Münz|inventor-first=Ferdinand|assign1=I. G. Farbenindustrie|country=DE|number=718981|pubdate=1938-09-20|title=Verfahren zum Unschädlichmachen der Härtebildner des Wassers [Process for rendering the hardness components of water harmless]|inventor-link=Ferdinand_Münz}}</ref> Today, EDTA is mainly synthesised from [[Chemistry:Ethylenediamine|ethylenediamine]] (1,2-diaminoethane), [[Physics:Formaldehyde|formaldehyde]], and [[Chemistry:Sodium cyanide|sodium cyanide]].<ref>{{cite web|url=http://www.chm.bris.ac.uk/motm/edta/synthesis_of_edta.htm|title=Industrial Synthesis of EDTA|publisher=University of Bristol}}</ref> This route yields the tetrasodium EDTA, which is converted in a subsequent step into the acid forms:

:H<sub>2</sub>NCH<sub>2</sub>CH<sub>2</sub>NH<sub>2</sub>  +  4&nbsp;[[Physics:Formaldehyde|CH<sub>2</sub>O]]  +  4&nbsp;[[Chemistry:Sodium cyanide|NaCN]]  +  4&nbsp;H<sub>2</sub>O   →  (NaO<sub>2</sub>CCH<sub>2</sub>)<sub>2</sub>NCH<sub>2</sub>CH<sub>2</sub>N(CH<sub>2</sub>CO<sub>2</sub>Na)<sub>2</sub>  +  4&nbsp;[[Chemistry:Ammonia|NH<sub>3</sub>]]

:(NaO<sub>2</sub>CCH<sub>2</sub>)<sub>2</sub>NCH<sub>2</sub>CH<sub>2</sub>N(CH<sub>2</sub>CO<sub>2</sub>Na)<sub>2</sub>  +  4&nbsp;[[Chemistry:Hydrochloric acid|HCl]]  →  (HO<sub>2</sub>CCH<sub>2</sub>)<sub>2</sub>NCH<sub>2</sub>CH<sub>2</sub>N(CH<sub>2</sub>CO<sub>2</sub>H)<sub>2</sub>  +  4&nbsp;[[Chemistry:Sodium chloride|NaCl]]

This process is used to produce about 80,000&nbsp;tonnes of EDTA each year. Impurities cogenerated by this route include [[Chemistry:Glycine|glycine]] and [[Chemistry:Nitrilotriacetic acid|nitrilotriacetic acid]]; they arise from reactions of the [[Chemistry:Ammonia|ammonia]] coproduct.<ref name="Ullmann">{{Ullmann|last=Hart|first=J. Roger|date=2005|title=Ethylenediaminetetraacetic Acid and Related Chelating Agents|doi=10.1002/14356007.a10_095}}</ref>

==Nomenclature==
To describe EDTA and its various [[Chemistry:Protonation|protonated forms]], chemists distinguish between EDTA<sup>4−</sup>, the conjugate base that is the [[Chemistry:Ligand|ligand]], and H<sub>4</sub>EDTA, the [[Biology:Precursor|precursor]] to that ligand. At very low pH (very acidic conditions) the fully protonated H<sub>6</sub>EDTA<sup>2+</sup> form predominates, whereas at very high pH or very basic condition, the fully deprotonated EDTA<sup>4−</sup> form is prevalent. In this article, the term EDTA is used to mean H<sub>4−''x''</sub>EDTA<sup>''x''−</sup>, whereas in its complexes EDTA<sup>4−</sup> stands for the tetraanion ligand.

==Coordination chemistry principles==
[[Image:Metal-EDTA.svg|thumb|Metal–EDTA chelate as found in Co(III) complexes]]
[[File:SFEDTD01.png|thumb|Structure of [Fe(EDTA)(H<sub>2</sub>O)]<sup>−</sup>, showing that the EDTA<sup>4−</sup> ligand does not fully encapsulate [[Chemistry:Iron|Fe(III)]], which is seven-coordinate<ref>{{cite journal|last1=Solans |first1=X. |last2=Font Altaba |first2=M. |last3=García Oricain |first3=J.|title=Crystal Structures of Ethylenediaminetetraacetato Metal Complexes. V. Structures Containing the [Fe(C<sub>10</sub>H<sub>12</sub>N<sub>2</sub>O<sub>8</sub>)(H<sub>2</sub>O)]<sup>−</sup> Anion|journal=Acta Crystallographica Section C|year=1984|volume=40|issue=4 |pages=635–638|doi=10.1107/S0108270184005151}}</ref>]]
In [[Chemistry:Coordination complex|coordination chemistry]], EDTA<sup>4−</sup> is a member of the [[Chemistry:Aminopolycarboxylic acid|aminopolycarboxylic acid]] family of ligands.  EDTA<sup>4−</sup> usually binds to a metal cation through its two amines and four carboxylates, i.e., it is a hexadentate ("six-toothed") chelating agent.  Many of the resulting [[Chemistry:Complex|coordination compound]]s adopt octahedral geometry.  Although of little consequence for its applications, these octahedral complexes are [[Biology:Chirality|chiral]].  The [[Chemistry:Cobalt|cobalt(III)]] anion [Co(EDTA)]<sup>−</sup> has been resolved into [[Chemistry:Enantiomer|enantiomer]]s.<ref>{{Cite book | last1 = Kirchner | first1 = S. | last2 = Gyarfas | first2 = Eleonora C. | chapter = Barium (Ethylenediaminetetraacetato)cobaltate(III) 4‐Hydrate | year = 1957 | title = Inorganic Syntheses | volume = 5 | pages = 186–188 | doi = 10.1002/9780470132364.ch52 | isbn = 978-0-470-13236-4 }}</ref>  Many complexes of EDTA<sup>4−</sup> adopt more complex structures due to either the formation of an additional bond to water, ''i.e.'' seven-coordinate complexes, or the displacement of one carboxylate arm by water. The [[Chemistry:Iron|iron(III)]] [[Chemistry:Ferric EDTA|complex]] of EDTA is seven-coordinate.<ref>{{cite journal | last1 = López Alcalá | first1 = J. M. | last2 = Puerta Vizcaíno | first2 = M. C. | last3 = González Vílchez | first3 = F. | last4 = Duesler | first4 = E. N. | last5 = Tapscott | first5 = R. E. | year = 1984 | title = A redetermination of sodium aqua[ethylenediaminetetraacetato(4−)]ferrate(III) dihydrate, Na[Fe(C<sub>10</sub>H<sub>12</sub>N<sub>2</sub>O<sub>8</sub>)(H<sub>2</sub>O)]·2H<sub>2</sub>O| journal = Acta Crystallogr C | volume = 40 | issue = 6 | pages = 939–941 | doi = 10.1107/S0108270184006338 | doi-access =  }}</ref>  Early work on the development of EDTA was undertaken by Gerold Schwarzenbach in the 1940s.<ref>{{cite web|last=Sinex |first=Scott A. |url=http://www.chm.bris.ac.uk/motm/edta/edtah.htm |title=EDTA – A Molecule with a Complex Story |publisher=University of Bristol}}</ref>  EDTA forms especially strong complexes with [[Chemistry:Manganese|Mn(II)]], [[Chemistry:Copper|Cu(II)]], Fe(III), [[Chemistry:Lead|Pb(II)]] and Co(III).<ref>{{cite book | last1 = Holleman | first1 = A. F. |last2=Wiberg |first2=E. | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | year = 2001 | isbn = 978-0-12-352651-9}}</ref>{{page needed|date=March 2018}}

Several features of EDTA's complexes are relevant to its applications.  First, because of its high [[Chemistry:Denticity|denticity]], this ligand has a high affinity for metal cations:

:[Fe(H<sub>2</sub>O)<sub>6</sub>]<sup>3+</sup>  +  H<sub>4</sub>EDTA  {{eqm}} [Fe(EDTA)]<sup>−</sup>  +  6&nbsp;H<sub>2</sub>O  +  4&nbsp;H<sup>+</sup>  {{pad|2em}}[[Chemistry:Equilibrium constant|''K''<sub>eq</sub>]] = 10<sup>25.1</sup>

Written in this way, the [[Chemistry:Stability constants of complexes|equilibrium quotient]] shows that metal ions compete with protons for binding to EDTA.  Because metal ions are extensively enveloped by EDTA, their [[Chemistry:Catalysis|catalytic properties]] are often suppressed.  Finally, since complexes of EDTA<sup>4−</sup> are anionic, they tend to be highly soluble in water.  For this reason, EDTA is able to dissolve deposits of metal oxides and [[Chemistry:Carbonate|carbonate]]s.

The [[Chemistry:Acid dissociation constant|p''K''<sub>a</sub> values]] of free EDTA are 0, 1.5, 2, 2.66 ([[Chemistry:Deprotonation|deprotonation]] of the four carboxyl groups) and 6.16, 10.24 (deprotonation of the two amino groups).<ref name="Latscha">Hans Peter Latscha: ''Analytische Chemie.'' Springer-Verlag, 2013, {{ISBN|978-3-642-18493-2}}, p.&nbsp;303.</ref>

==Environmental concerns==

===Abiotic degradation===
EDTA is in such widespread use that questions have been raised whether it is a persistent organic pollutant. While EDTA serves many positive functions in different industrial, pharmaceutical and other avenues, the longevity of EDTA can pose serious issues in the environment.  The degradation of EDTA is slow.  It mainly occurs abiotically in the presence of sunlight.<ref name=Bucheli>{{citation|last1=Bucheli-Witschel |first1=M. |last2=Egli |first2=T. | journal= FEMS Microbiology Reviews| title=DAB: Environmental Fate and Microbial Degradation of Aminopolycarboxylic Acids| volume=25| issue= 1| pages=69–106| year=2001| doi=10.1111/j.1574-6976.2001.tb00572.x| pmid= 11152941 | doi-access=free}}</ref>

The most important process for the elimination of EDTA from surface waters is direct photolysis at wavelengths below 400&nbsp;nm.<ref>{{Cite thesis |last= Kari |first= F. G.|title= Umweltverhalten von Ethylenediaminetetraacetate (EDTA) under spezieller Berucksuchtigung des photochemischen Ab-baus.|type=PhD |year= 1994 |publisher= Swiss Federal Institute of Technology}}</ref> Depending on the light conditions, the photolysis [[Physics:Half-life|half-lives]] of iron(III) EDTA in surface waters can range as low as 11.3 minutes up to more than 100 hours.<ref>{{cite journal |last1= Frank|first1= R.|last2= Rau|first2=H. |year=1989 |title= Photochemical transformation in aqueous solution and possible environmental fate of Ethylenediaminetetraacetatic acid (EDTA)|journal= Ecotoxicology and Environmental Safety |volume= 19 |issue= 1|pages=55–63 |doi=10.1016/0147-6513(90)90078-j|pmid= 2107071}}</ref> Degradation of FeEDTA, but not EDTA itself, produces iron complexes of the triacetate (ED3A), diacetate (EDDA), and monoacetate (EDMA) – 92% of EDDA and EDMA biodegrades in 20 hours while ED3A displays significantly higher resistance.  Many environmentally-abundant EDTA species (such as [[Chemistry:Magnesium|Mg<sup>2+</sup>]] and [[Chemistry:Calcium|Ca<sup>2+</sup>]]) are more persistent.

===Biodegradation===
In many [[Earth:Industrial wastewater treatment|industrial wastewater treatment]] plants, EDTA elimination can be achieved at about 80% using microorganisms.<ref>{{cite journal |last1= Kaluza|first1= U.|last2= Klingelhofer|first2=P. |first3 = Taeger |last3=K. |year=1998 |title= Microbial degradation of EDTA in an industrial wastewater treatment plant |journal= Water Research |volume= 32 |issue= 9|pages=2843–2845 |doi=10.1016/S0043-1354(98)00048-7}}</ref> Resulting byproducts are ED3A and [[Chemistry:Iminodiacetic acid|iminodiacetic acid]] (IDA) – suggesting that both the backbone and acetyl groups were attacked. Some microorganisms have even been discovered to form nitrates out of EDTA, but they function optimally at moderately alkaline conditions of pH 9.0–9.5.<ref>{{cite journal |last1= VanGinkel|first1= C. G. |last2= Vandenbroucke|first2=K. L. |first3 = Troo |last3=C. A. |year=1997 |title= Biological removal of EDTA in conventional activated-sludge plants operated under alkaline conditions |journal= Bioresource Technology |volume= 32 |issue= 2–3 |pages=2843–2845 |doi=10.1016/S0960-8524(96)00158-7}}</ref>

Several bacterial strains isolated from sewage treatment plants efficiently degrade EDTA. Specific strains include ''Agrobacterium radiobacter'' ATCC 55002<ref>{{cite journal |last1= Lauff|first1= J. J. |last2= Steele|first2=D. B. |last3 = Coogan |first3=L. A. |last4 = Breitfeller |first4=J. M.|year=1990 |title= Degradation of the ferric chelate of EDTA by a pure culture of an ''Agrobacterium'' sp. |pmid=16348340|pmc=184952 |journal= Applied and Environmental Microbiology |volume= 56 |pages=3346–3353 |issue=11|doi= 10.1128/AEM.56.11.3346-3353.1990 |bibcode= 1990ApEnM..56.3346L }}</ref> and the sub-branches of [[Biology:Pseudomonadota|Pseudomonadota]] like BNC1, BNC2,<ref name="Nortemannl 1992 671–676">{{cite journal |last= Nortemannl|first= B |year=1992 |title= Total degradation of EDTA by mixed culturesand a bacterial isolate |journal= Applied and Environmental Microbiology |volume= 58 |pages=671–676 |issue=2|doi= 10.1128/AEM.58.2.671-676.1992 |pmid= 16348653 |pmc= 195300 |bibcode= 1992ApEnM..58..671N }}</ref> and strain DSM 9103.<ref>{{cite speech |title=Degradation of EDTA by a bacterial isolate. Poster presented at the 45th Annual Meeting of the Swiss Society for Microbiology |last1=Witschel |first1=M. |last2=Weilemann |first2=H.-U. |last3=Egli |first3=T. |year=1995 |location= Lugano, Switzerland}}</ref> The three strains share similar properties of aerobic respiration and are classified as [[Biology:Gram-negative bacteria|gram-negative bacteria]]. Unlike photolysis, the chelated species is not exclusive to iron(III) in order to be degraded. Rather, each strain uniquely consumes varying metal–EDTA complexes through several enzymatic pathways. Agrobacterium radiobacter only degrades Fe(III) EDTA<ref name="Nortemannl 1992 671–676"/> while BNC1 and DSM 9103 are not capable of degrading iron(III) EDTA and are more suited for [[Chemistry:Calcium|calcium]], [[Chemistry:Barium|barium]], [[Chemistry:Magnesium|magnesium]] and [[Chemistry:Manganese|manganese(II)]] complexes.<ref>{{cite journal |last1= Hennekenl|first1= L. |last2=Nortemann |first2=B. |last3 = Hempel |first3=D. C. |year=1995 |title= Influence of physiological conditions on EDTA degradation |journal= Applied and Environmental Microbiology |volume= 44 |issue= 1–2 |pages=190–197 |doi=10.1007/bf00164501|s2cid= 30072817 }}</ref> EDTA complexes require dissociation before degradation.

==Alternatives to EDTA==
Interest in environmental safety has raised concerns about biodegradability of aminopolycarboxylates such as EDTA. These concerns incentivize the investigation of alternative aminopolycarboxylates.<ref name=Bucheli/> Candidate chelating agents include [[Chemistry:Nitrilotriacetic acid|nitrilotriacetic acid]] (NTA), iminodisuccinic acid (IDS), [[Chemistry:Polyaspartic acid|polyaspartic acid]], [[Chemistry:EDDS|''S,S''-ethylenediamine-''N'',''N''′-disuccinic acid (EDDS)]], methylglycinediacetic acid (MGDA), and <small>L</small>-Glutamic acid ''N'',''N''-diacetic acid, tetrasodium salt (GLDA).<ref>{{cite journal|doi=10.1021/es0348750|pmid=14968886|title=Extraction of Heavy Metals from Soils Using Biodegradable Chelating Agents|journal=Environmental Science & Technology|volume=38|issue=3|pages=937–944|year=2004|last1=Tandy|first1=Susan|last2=Bossart|first2=Karin|last3=Mueller|first3=Roland|last4=Ritschel|first4=Jens|last5=Hauser|first5=Lukas|last6=Schulin|first6=Rainer|last7=Nowack|first7=Bernd|bibcode=2004EnST...38..937T}}</ref>

===Iminodisuccinic acid (IDS)===
Commercially used since 1998, [[Chemistry:Tetrasodium iminodisuccinate|iminodisuccinic acid]] (IDS) biodegrades by about 80% after only 7 days. IDS binds to calcium exceptionally well and forms stable compounds with other heavy metal ions. In addition to having a lower toxicity after chelation, IDS is degraded by ''[[Biology:Agrobacterium tumefaciens|Agrobacterium tumefaciens]]'' (BY6), which can be harvested on a large scale. The enzymes involved, IDS epimerase and C−N [[Biology:Lyase|lyase]], do not require any [[Biology:Cofactor (biochemistry)|cofactors]].<ref>{{citation|last1=Cokesa |first1=Z. |last2=Knackmuss |first2=H. |last3=Rieger |first3=P. | journal= Applied and Environmental Microbiology| title=Biodegradation of All Stereoisomers of the EDTA Substitute Iminodisuccinate by Agrobacterium Tumefaciens BY6 Requires an Epimerase and a Stereoselective C−N Lyase| volume=70| issue= 7| pages=3941–3947| year=2004| doi=10.1128/aem.70.7.3941-3947.2004| pmid= 15240267| pmc= 444814 |bibcode=2004ApEnM..70.3941C }}</ref>

===Polyaspartic acid===
[[Chemistry:Polyaspartic acid|Polyaspartic acid]], like IDS, binds to calcium and other heavy metal ions.  It has many practical applications including corrosion inhibitors, wastewater additives, and agricultural polymers. A Polyaspartic acid-based laundry detergent was the first laundry detergent in the world to receive the EU flower ecolabel.<ref name ="Roweton 1997" >{{Ullmann|chapter=Polyaspartates and Polysuccinimide |author=Thomas Klein |author2=Ralf-Johann Moritz |author3=René Graupner |year= 2008|doi=10.1002/14356007.l21_l01}}</ref> Calcium binding ability of polyaspartic acid has been exploited for targeting of drug-loaded nanocarriers to bone.<ref>{{Cite journal|last1=Adelnia|first1=Hossein|last2=Tran|first2=Huong D.N.|last3=Little|first3=Peter J.|last4=Blakey|first4=Idriss|last5=Ta|first5=Hang T.|date=2021-06-14|title=Poly(aspartic acid) in Biomedical Applications: From Polymerization, Modification, Properties, Degradation, and Biocompatibility to Applications|journal=ACS Biomaterials Science & Engineering|volume=7|issue=6|pages=2083–2105|doi=10.1021/acsbiomaterials.1c00150|pmid=33797239|hdl=10072/404497 |s2cid=232761877|hdl-access=free}}</ref> Preparation of [[Chemistry:Hydrogel|hydrogel]]s based on polyaspartic acid, in a variety of physical forms ranging from [[Chemistry:Fiber|fiber]] to [[Physics:Particle|particle]], can potentially enable facile separation of the chelated ions from a solution.<ref>{{Cite journal|last1=Adelnia|first1=Hossein|last2=Blakey|first2=Idriss|last3=Little|first3=Peter J.|last4=Ta|first4=Hang T.|date=2019|title=Hydrogels Based on Poly(aspartic acid): Synthesis and Applications|journal=Frontiers in Chemistry|volume=7|page=755|language=English|doi=10.3389/fchem.2019.00755|pmid=31799235|pmc=6861526|bibcode=2019FrCh....7..755A|issn=2296-2646|doi-access=free}}</ref> Therefore, despite being weaker than EDTA, polyaspartic acid can still be regarded as a viable alternative due to these features as well as [[Chemistry:Biocompatibility|biocompatibility]], and biodegradability.<ref>{{Cite journal|last1=Hasson|first1=David|last2=Shemer|first2=Hilla|last3=Sher|first3=Alexander|date=2011-06-15|title=State of the Art of Friendly "Green" Scale Control Inhibitors: A Review Article|journal=Industrial & Engineering Chemistry Research|volume=50|issue=12|pages=7601–7607|doi=10.1021/ie200370v|issn=0888-5885}}</ref>

===''S'',''S''-Ethylenediamine-''N'',''N''′-disuccinic acid (EDDS)===
A [[Chemistry:Structural isomer|structural isomer]] of EDTA, [[Chemistry:EDDS|ethylenediamine-''N'',''N''′-disuccinic acid]] (EDDS) is readily biodegradable at high rate in its ''S'',''S'' form.<ref>{{cite journal |author1=Tandy, S. |author2=Ammann, A. |author3=Schulin, R. |author4=Nowack, B. |year=2006 |title=Biodegredation and speciation of residual SS-ethylenediaminedisuccinic acid (EDDS) in soil solution left after soil washing |journal=Environmental Pollution |volume=142 |issue=2 |pages=191–199 |doi=10.1016/j.envpol.2005.10.013 |pmid=16338042}}</ref>

===Methylglycinediacetic acid (MGDA)===
[[Chemistry:Trisodium dicarboxymethyl alaninate|Trisodium dicarboxymethyl alaninate]], also known as methylglycinediacetic acid (MGDA), has a high rate of biodegradation at over 68%, but unlike many other chelating agents can degrade without the assistance of adapted bacteria. Additionally, unlike EDDS or IDS, MGDA can withstand higher temperatures while maintaining a high stability as well as the entire pH range.{{Citation needed|date=December 2019|reason=removed citation to predatory publisher content}}  MGDA has been shown to be an effective chelating agent, with a capacity for mobilization comparable with that of [[Chemistry:Nitrilotriacetic acid|nitrilotriacetic acid]] (NTA), with application to water for industrial use and for the removal of [[Chemistry:Calcium oxalate|calcium oxalate]] from urine from patients with kidney stones.<ref>{{cite journal |last1=Bretti |first1=Clemente |last2=Cigala |first2=Rosalia Maria |last3=De Stefano |first3=Concetta |last4=Lando |first4=Gabriele |last5=Sammartano |first5=Silvio |title=Thermodynamic solution properties of a biodegradable chelant (MGDA) and its interaction with the major constituents of natural fluids |journal=Fluid Phase Equilibria |date=2017 |volume=434 |pages=63–73 |doi=10.1016/j.fluid.2016.11.027}}</ref>

==Methods of detection and analysis==
The most sensitive method of detecting and measuring EDTA in biological samples is selected reaction monitoring [[Physics:Capillary electrophoresis|capillary electrophoresis]] mass spectrometry (SRM-CE/MS), which has a [[Chemistry:Detection limit|detection limit]] of 7.3&nbsp;ng/mL in human plasma and a [[Chemistry:Detection limit|quantitation limit]] of 15&nbsp;ng/mL.<ref name="sheppard">{{Cite journal | doi = 10.1021/ac971726p| pmid = 9253241| title = Peer Reviewed: Determining EDTA in Blood| journal = Analytical Chemistry| volume = 69| issue = 15| pages = 477A–480A| year = 1997| last1 = Sheppard | first1 = R. L. | last2 = Henion | first2 = J. }}</ref> This method works with sample volumes as small as 7–8&nbsp;nL.<ref name="sheppard" />

EDTA has also been measured in non-alcoholic beverages using [[High-performance liquid chromatography|high performance liquid chromatography]] (HPLC) at a level of 2.0&nbsp;μg/mL.<ref>{{Cite journal | doi = 10.1007/s002160051422| title = Optimisation of the analytical detection of EDTA by HPLC in natural waters| journal = Fresenius' Journal of Analytical Chemistry| volume = 364| issue = 8| page = 727| year = 1999| last1 = Loyaux-Lawniczak | first1 = S. | last2 = Douch | first2 = J. | last3 = Behra | first3 = P.| s2cid = 95648833}}</ref><ref>{{Cite journal | doi = 10.1016/j.jfca.2006.05.008| title = Development and validation of a method for the determination of EDTA in non-alcoholic drinks by HPLC| journal = Journal of Food Composition and Analysis| volume = 20| issue = 3–4| page = 248| year = 2007| last1 = Cagnasso | first1 = C. E. | last2 = López | first2 = L. B. | last3 = Rodríguez | first3 = V. G. | last4 = Valencia | first4 = M. E. }}</ref>

== In popular culture ==

In the movie ''Blade'' (1998), EDTA is used as a weapon to kill vampires, exploding when in contact with vampire blood.<ref>{{cite web |title=Blade (1998) |website=Internet Movie Database ([[Social:IMDb|IMDb]])|url=https://imdb.com/title/tt0120611/goofs/#:~:text=when%20a,grenade |access-date=2022-11-14}}</ref>

==References==
{{reflist|30em}}

==External links==
* [http://www.chm.bris.ac.uk/motm/edta/edtah.htm EDTA: Molecule of the Month]
* [https://web.archive.org/web/20061029103725/http://www.chem.utk.edu/~chem319/Experiments/Exp6.pdf EDTA Determination of Total Water Hardness]
*{{cite journal |doi=10.1590/S0100-40422003000600020 |title=EDTA: The chelating agent under environmental scrutiny |journal=Química Nova |volume=26 |issue=6 |pages=901–905 |year=2003 |last1=Oviedo |first1=Claudia |last2=Rodríguez |first2=Jaime |doi-access=free }}

{{Antidotes}}
{{antithrombotics}}
{{Chelating agents}}
{{Endodontology}}
{{Consumer Food Safety}}

{{DEFAULTSORT:Ethylenediaminetetraacetic Acid}}
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[[Category:Antidotes]]
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