EDTA

Cas Numarası; 60-00-4

EC Number 200-573-9

Synonyms:
Ethylenediaminetetraacetic acid; edetic acid; Disodium EDTA; Edta disodium; 139-33-3; Disodium ethylenediaminetetraacetic acid; SCHEMBL33500; disodium ethylenediamine tetracetic acid; ethylenediaminetetraacetic acid disodium; disodium ethylene diaminetetraacetic acid
disodium ethylenediamine tetraacetic acid; 139D333; Ethylenediaminetetraacetic acid disodium salt solution, 0.01 M; Ethylenediaminetetraacetic acid disodium salt solution, 0.02 M; Ethylenediaminetetraacetic acid disodium salt solution, 0.05 M; Ethylenediaminetetraacetic acid disodium salt solution, 0.1 M; Ethylenediaminetetraacetic acid disodium salt solution, 2%, solution; Ethylenediaminetetraacetic acid disodium salt solution, for molecular biology, 0.5 M in H2O ; DNase, RNase, NICKase and protease, none detected; molecule; Ethylenediamine Tetraacetic Acid; Chelating Agent; Chelating Agent; 60-00-4; Na2; Na4;  Ethylenediaminetetraacetic Acid Trisodium Salt; Disodium EDTA; Isodium dihydrogen ethylenediaminetetraacetate; Edetic acid disodium salt; EDTA disodium salt; (Ethylenedinitrilo)tetraacetic acid disodium salt; Disodium Edetate; EDTA disodium salt; 139-33-3; Disodium EDTA; Ethylenediaminetetraacetic acid disodium salt; Edta disodium; Disodium ethylenediaminetetraacetate; EDTA 2Na; Disodium ethylenediaminetetraacetic acid; Disodium dihydrogen ethylenediaminetetraacetate; 6381-92-6;
ethylenediamine tetraacetic acid disodium salt; ETA Solution;Ethylenediaminetetraacetic acid disodium salt solution; EDTA 2Na Solution; SCHEMBL33501; AKOS015900960; AKOS016016390; CS-W019532; KS-0000058S; SC-65716; D3789; E0091; E0103; ethylenediamine tetra-acetic acid disodium salt; N-[2-[Bis(sodiooxycarbonylmethyl)amino]ethyl]iminobis(acetic acid); sodium 2,2'-(2-(bis(carboxymethyl)amino)ethylazanediyl)diacetate;
Disodium N,N'-1,2-ethanediylbis(N-(carboxymethyl)glycine); (Ethylenedinitrilo)-tetraacetic acid disodium salt; Cheladrate; Chelaplex III; Chelaton 3; Chelaton III; Chelest 200; Chelest B; Clewat N; Complexon III; DR-16133; Dinatrium ethylendiamintetraacetat [Czech]; Diso-Tate; Disodium (ethylenedinitrilo)tetraacetate; Disodium (ethylenedinitrilo)tetraacetic acid; Disodium diacid ethylenediaminetetraacetate; Disodium dihydrogen ethylenediaminetetraacetate; Disodium dihydrogen(ethylenedinitrilo)tetraacetate; Disodium edathamil; Disodium edetate; Disodium EDTA, anhydrous; Disodium ethylenediamine-N,N,N',N'-tetraacetate; Disodium ethylenediaminetetraacetate; Disodium ethylenediaminetetraacetic acid; Disodium salt of EDTA; Disodium sequestrene; Disodium tetracemate; Disodium versenate; Disodium versene; Dotite 2NA; E.D.T.A. disodique [French]; EDTA disodium; EDTA disodium salt; Edathamil disodium; Edetate disodium; Edetate sodium; Edetic acid disodium salt; Endrate disodium; Ethylenebis(iminodiacetic acid) disodium salt; Ethylenediaminetetraacetate, disodium salt; Ethylenediaminetetraacetic acid disodium salt; Ethylenediaminetetraacetic acid, disodium salt; F 1; F 1 (VAN); F 1 (complexon); Kiresuto B; Komplexon III; Mavacid ED 4; Metaquest B; N,N'-1,2-Ethanediylbis(N-(carboxymethyl)glycine) disodium salt; Perma Kleer 50 Crystals disodium salt; Perma Kleer Di Crystals; Selekton B 2; Sequestrene sodium 2; Sodium ethylenediaminetetraacetate; Sodium versenate; Tetracemate disodium; Titriplex III; Trilon BD; Triplex III; Veresene disodium salt; Versene NA; Versene Na2; Versonol 120; Zonon D; Ethylene diamine tetraacetic acid, disodium salt; Glycine, N,N'-1,2-ethanediylbis(N-(carboxymethyl)-, disodium salt; Glycine, N,N'-1,2-ethanediylbis(N-(carboxymethyl)-, sodium salt (1:2); Acetic acid, (ethylenedinitrilo)tetra-, disodium salt;

EDTA was thought to chemically soften the root canal dentin and dissolve the smear layer and increase dentin permeability. EDTA reacts with the calcium ions in dentin and forms soluble calcium chelates. For removing inorganic and organic material of smear layer, combined using EDTA and NaOCl is recommended. Ethylenediaminetetraacetic acid (EDTA) is a chelator of metal ions. It is a substituted diamine, which has antibacterial activity. EDTA removes the undesirable effects of ferric, cupric and manganic ions in bleaching. It prevents cellular division, chlorophyll synthesis and algal biomass production. EDTA is an inhibitor of metalloprotease. It has anticoagulant property. 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 catalysing the disproportionation of hydrogen peroxide, which is used in chlorine-free bleaching. In a similar manner, EDTA is added to some food as a preservative or stabiliser to prevent catalytic oxidative decolouration, which is catalysed by metal ions. 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+, Mg2+, as well as other metal ions. Once bound to EDTA, these metal centres tend not to form precipitates or to interfere with the action of the soaps and detergents. For similar reasons, cleaning solutions often contain EDTA. In a similar manner EDTA is used in the cement industry for the determination of free lime and free magnesia in cement and clinkers. 
The solubilisation of Fe3+ ions at or below near neutral pH can be accomplished using EDTA. This property is useful in agriculture including hydroponics. However, given the pH dependence of ligand formation, EDTA is not helpful for improving iron solubility in above neutral soils.[8] Otherwise, at near-neutral pH and above, iron(III) forms insoluble salts, which are less bioavailable to susceptible plant species. Aqueous [Fe(EDTA)]− is used for removing ("scrubbing") hydrogen sulfide from gas streams. This conversion is achieved by oxidising the hydrogen sulfide to elemental sulfur, which is non-volatile:
2 [Fe(EDTA)]− + H2S → 2 [Fe(EDTA)]2− + S + 2 H+
In this application, the iron(III) centre is reduced to its iron(II) derivative, which can then be reoxidised by air. In similar manner, nitrogen oxides are removed from gas streams using [Fe(edta)]2−. The oxidising properties of [Fe(edta)]− are also exploited in photography, where it is used to solubilise silver particles 
EDTA was used in 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 Cu2+ 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%).

Sodium calcium edetate, an EDTA derivative, is used to bind metal ions in the practice of chelation therapy, such as for treating mercury 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.
Dentists and endodontists use EDTA solutions to remove inorganic debris (smear layer) and lubricate the root canals in endodontics. This procedure helps prepare root canals for obturation. Furthermore, EDTA solutions with the addition of a surfactant loosen up calcifications 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.
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 chromium(III) complex [Cr(edta)]− (as radioactive chromium-51 (51Cr)) is administered intravenously and its filtration into the urine is monitored. This method is useful for evaluating glomerular filtration rate (GFR) in nuclear medicine. 
EDTA is used extensively in the analysis of blood. It is an anticoagulant for blood samples for CBC/FBCs, where the EDTA chelates the calcium present in the blood specimen, arresting the coagulation process and preserving blood cell morphology. Tubes containing EDTA are marked with lavender or pink tops. EDTA is also in tan top tubes for lead testing and can be used in royal blue top tubes for trace metal testing. 
EDTA is a slime dispersant, and has been found to be highly effective in reducing bacterial growth during implantation of intraocular lenses (IOLs). 

In shampoos, cleaners, and other personal care products, EDTA salts are used as a sequestering agent to improve their stability in air. 
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, proteins, and polysaccharides. EDTA also acts as a selective inhibitor against dNTP hydrolyzing enzymes (Taq polymerase, dUTPase, MutT), liver arginaseand horseradish peroxidase independently of metal ion 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 complexometric titrations and analysis of water hardness or as a 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 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. EDTA is also known to inhibit a range of metallopeptidases, the method of inhibition occurs via the chelation of the metal ion required for catalytic activity. EDTA can also be used to test for bioavailability of heavy metals in sediments. 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.
The compound was first described in 1935 by Ferdinand Münz, who prepared the compound from ethylenediamine and chloroacetic acid. Today, EDTA is mainly synthesised from ethylenediamine (1,2-diaminoethane), formaldehyde, and sodium cyanide. This route yields the tetrasodium EDTA, which is 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
This process is used to produce about 80,000 tonnes of EDTA each year. Impurities cogenerated by this route include glycine and nitrilotriacetic acid; they arise from reactions of the ammonia coproduct. 

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 H6EDTA2+ form predominates, whereas at very high pH or very basic condition, the fully deprotonated EDTA4− form is prevalent. In this article, the term EDTA is used to mean H4−xEDTAx−, whereas in its complexes EDTA4− stands for the tetraanion ligand.

In coordination chemistry, EDTA4− is a member of the aminopolycarboxylic 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 cobalt(III) anion [Co(EDTA)]− has been resolved into enantiomers. Many complexes of EDTA4− 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 iron(III) complex of EDTA is seven-coordinate. 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.
The pKa values of free EDTA are 0, 1.5 (deprotonation of the two amino groups), 2, 2.66, 6.16 and 10.24 (deprotonation of the four carboxyl groups) . 
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.[31]

The most important process for the elimination of EDTA from surface waters is direct photolysis at wavelengths below 400 nm. Depending on the light conditions, the photolysis half-lives of iron(III) EDTA in surface waters can range as low as 11.3 minutes up to more than 100 hours. 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 Mg2+ and Ca2+) are more persistent.
In many industrial wastewater treatment plants, EDTA elimination can be achieved at about 80% using microorganisms. Resulting byproducts are ED3A and 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. 
Several bacterial strains isolated from sewage treatment plants efficiently degrade EDTA. Specific strains include Agrobacterium radiobacter ATCC 55002 and the sub-branches of Proteobacteria like BNC1, BNC2, and strain DSM 9103. The three strains share similar properties of aerobic respiration and are classified as 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 while BNC1 and DSM 9103 are not capable of degrading iron(III) EDTA and are more suited for calcium, barium, magnesium and manganese(II) complexes. EDTA complexes require dissociation before degradation.

Interest in environmental safety has raised concerns about biodegradability of aminopolycarboxylates such as EDTA. These concerns incentivize the investigation of alternative aminopolycarboxylates. Candidate chelating agents include nitrilotriacetic acid (NTA), iminodisuccinic acid (IDS), polyaspartic acid, S,S-ethylenediamine-N,N′-disuccinic acid (EDDS), methylglycinediacetic acid (MGDA), and L-Glutamic acid N,N-diacetic acid, tetrasodium salt (GLDA). 
ommercially used since 1998, 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 Agrobacterium tumefaciens (BY6), which can be harvested on a large scale. The enzymes involved, IDS epimerase and C−N lyase, do not require any cofactors.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. he S,S isomer of EDTA, ethylenediamine-N,N′-disuccinic acid (EDDS) is readily biodegradable and exhibits a high rate biodegradation. 
he S,S isomer of EDTA, ethylenediamine-N,N′-disuccinic acid (EDDS) is readily biodegradable and exhibits a high rate biodegradation. 

It is one of the polyamino carboxylic acid types. More than one -COOH group is attached in the structure. It is in the group of polycarboxylic acids. They take the -NH2-linked amino attachment in their structure. Hence it is grouped as polyamino carboxylic acid. EDTA is the abbreviation for ethylenediamine tetraacetic acid. It is a colorless and crystalline solid. Cycle as a molecular biology class. And it is well suited for molecular biology applications. It has very good affinity for some metal ions. With this feature, it can make very good interlocking. As an anticoagulant agent, Ethylene Diamine Tetra Acetic Acid is the best chemical.
EDTA (Ethylenediamine Tetraacetic Acid) potassium and sodium salts are widely used in routine Hematology (blood science) determinations, as they do not damage the cellular components of blood.
Edta is used in the treatment of livestock for lead and heavy metal poisoning, as it forms stable complexes with most metal ions.
It is used as a component of household detergents, cosmetics, medicines and foodstuffs.
Its main function is to form complex structures by interacting with metal ions.
Cleaning agents are used in container pipes and nozzles in the aviation industry to prevent the precipitation of heavy metals that may cause sedimentation and coating. Edta is used in the manufacture of these cleaning agents.
Phosphates are balanced in alkaline degreasing fleets and are used for lumping of calcium soap.
Damage to metal surfaces by intensifying the cleaning effect. This application is carried out with edta.
It is used in milk and beverage production.
In the photochemicals industry, the combination of oxidation and fixation of metallic silver (complexation and removal of silver ions) is performed by applying Edta before bleaching.
It is used in textile coatings to crosslink cellulose molecules in the textile industry (to produce easy-care fabrics), to support oxidative bleaching processes and to prevent catalytic damage to fibers.
In the paper industry, bleaching agents are used to remove residual lignin from cellulose fibers. And the brightness is increased. Paper mills are also used. Heavy metals such as manganese can break down the peroxide if Hydrogen Peroxide, which is a bleach, is used. The reason for using Ethylene Diamine Tetra Acetic Acid is to create a chelated structure. Because ethylene diamine tetra acetic acid does not stick to paper like manganese, then all of the edta goes to the sewer as waste.

It is used in the metal plating industry for plating copper as a result of the precipitation of copper complex compounds on the wooden board by the catalytic reduction method. In this application, printed circuit boards are produced with the help of edta.It is used to prevent the formation of calcium and magnesium stones in water treatment systems. It is used as an additive in water treatment systems to prevent and clean internal deposits to the boilers of the water feeding the system.It is used in the production of Styrene Butadiene Elastomer produced by emulsion polymerization. The purpose of use here is to be a sequestering agent for Fe (II) / Fe (III) ions in the initiator system in production.It is used as a good cleaning agent in oil producing platforms. It should be added by continuous application in certain dosages. Edta is used to remove sulfur fumes in coal power plants and waste incineration plants. It has iron chelating properties by using 70% sorbitol together with sodium hydroxide for catalytic removal of hydrogen sulfide.
The biggest factor affecting the EDTA price is due to the prices of the raw material inputs used in its production.The price of this chemical also depends on the density of EDTA produced and the specification information.The higher the concentration, the higher the prices. Because the production cost is high. Due to the widening of the usage area of EDTA, the price increases. With a new major producer starting to produce EDTA, it will temporarily decrease but will soon reach the appropriate level.
Chemical substances are packaged in packages specified in international standards. These are sold by starting with the lowest packaging, to the largest packaging or by bulk method with tankers. These can be 1 gram packages, 1 ton big bind packaging, the lowest drum packaging, or unpackaged sales with tankers.
EDTA can be stored stable for months at 4 ° C as a 0.5 M stock solution at pH 8.5. It is kept in polyethylene, ie plastic containers, instead of glass bottles. This is because the Ethylene Diamine Tetra Acetic Acid in the glass bottle can react with the metal ions in the bottle structure over time. However, since there are no metal ions in plastic containers, it can be stored for a longer time in plastic containers.
Today, it is synthesized for industrial purposes by reacting ethylenediamine with formaldehyde and cyanide-containing compounds such as HCN or NaCN. First of all, sodium salt of EDTA is formed. It can then be acidified. Hydrochloric acid or sulfuric acid is added to acidify this sodium salt. One and two-step synthesis is used in the production of EDTA. In the 2-stage production process, this chemical with very high purity is produced. In the production process of Ethylenediamine Tetraacetic Acid, no separation is required in the one-step production process. Therefore, less equipment and less setup costs are required. In the process of ethylenediamine Tetraacetic Acid production, the EDTA salt was contaminated with the NTA salt in two stages.

Its melting point is 237 ° C.

Its boiling point is 100 ° C.

Its density is 0.86 g / cm3.

Storage temperature is 2-8 ° C.

The solubility of EDTA is 100 mg / mlt dissolved in 3M NaOH solution. But it dissolves 0.5 g / L (25 ° C) in water. So when we look at it, it is slightly soluble in water.

It has a crystal structure in appearance. It is almost white in color.

It is a stable chemical under normal conditions. Insoluble in copper, copper alloys, nickel, aluminum, strong oxidizing agents and strong bases. It is one of the polyamino carboxylic acid types. More than one -COOH group is attached in its structure. Therefore, it is in the polycarboxylic acid group. Since -NH2 is attached in its structure, they take the amino attachment. Hence it is grouped as polyamino carboxylic acid. EDTA is the abbreviation for ethylenediamine tetraacetic acid. It is a colorless and crystalline solid. It has been designated as the molecular biology class. And it is well suited for molecular biology applications. It has very good affinity for some metal ions. With this feature, it can make very good interlocking. As an anticoagulant agent, Ethylene Diamine Tetra Acetic Acid is the best chemical.
Ethylene diamine tetra acetic acid (EDTA) is an effective chelating agent and lubricant. EDTA was thought to chemically soften the root canal dentin and dissolve the smear layer and increase dentin permeability. EDTA reacts with the calcium ions in dentin and forms soluble calcium chelates. For removing inorganic and organic material of smear layer, combined using EDTA and NaOCl is recommended. In this article, the usage and efficacy of EDTA in endodontic therapy are discussed. The aim of this review is s to analyze the relevant literature on EDTA.

PRODUCT DESCRIPTION:
Characteristics: Trilon B is a white powder. It is soluble in water and polar solvents. It decomposes at 150-200 oC, slowly gives crystallization water and loses its color. Uses: It is a chelating agent used in various fields such as salad dressings, margarine, mayonnaise, processed fruit and vegetables, canned fish and soft drinks. It eliminates metal contamination caused by the machinery used in the production of foods and which are a part of modern food production technologies, and prevents bitterness and discoloration caused by contamination in advanced stages.
GENERAL INFORMATION ABOUT EDTA TYPES
The active substance in EDTA is EDTA, which is internationally expressed. It is an aminocarboxylic acid with 6 functional groups involved in EDTA complex reactions. Properties: EDTA is white powder. It is soluble in water and polar solvents. It decomposes at 150-200 oC, gradually gives crystallization water and loses its color. Complex formation: Its most important feature is their ability to form water-soluble complexes with Ca, Mg, Cu, Zn, Cd, Lead, manganese, iron, Al, mercury and other polyvalent metal ions over a wide range of pH. The complexation reaction is not affected much by temperature. The central metal ion is surrounded with more or less integrity by the ligand that prevents it from participating in typical chemical reactions. These kinds of complexes are particularly stable to alkaline environment and high temperature.

Chemical stability: EDTA varieties differ from inorganic complexing agents in their resistance to hydrolysis for a long period under pressure at 200 oC. EDTA grades are resistant to strong acids and alkalis. In chromic acid, it degrades slowly over prolonged periods with potassium permanganate and other oxidizing agents (except BVT). Chlorine donors are effective in the performance of all EDTA types. And they can degrade alkaline earth and heavy metal complexes. EDTA grades should be dissolved in stainless steel or glass containers or plastic-decorated shine-colored containers. Copper and security steel should not be used. Applications: Used in industrial processes involving metal ions that play a role in causing disarray. It is used to soften water and remove alkaline earth and heavy metal impurities. They are frequently added to cleaners and detergents for home and industrial use.

Precipitated metal powders and hydroxides can dissolve in Trilon B. Water softening: EDTA grades can be used to soften cooling and process water, but can corrode copper, zinc, Al and non-ferrous alloys. Metals that do not contain Fe should be inspected for corrosion. EDTA varieties are most effective in the neutral to alkaline pH range. Some hardness residue can be used at less than stoichiometric rates in undesirable applications. Trilon B variants can also be used to soften boiler feed water.
Laundry detergents: The most important feature of EDTA varieties is their high complexing capacity and resistance to hydrolysis. It is also important that the complex is stable in an alkaline environment at rising temperatures. The most important function of EDTA types in detergents is to stabilize perborate and percarbonate bleaching. As little as 0.5-0.1% is required to prevent trace amounts of heavy metals catalyzing decomposition.
Soap: EDTA can be added to bar soaps, toilet soaps, and shaving soaps to prevent discoloration and mold (rancidity, rancidity). (During production, metal parts may touch the soap due to equipment.) Trilon B can be added to soap bar after soaping, before shaping. EDTA powder: Soap bar: 0.1-0.2%; It should be added to liquid soap at a rate of approximately 1%.
Cleaners and degreasers: EDTA's solubility and resistance to hydrolysis make it useful in industrial and institutional cleaners and degreasers.
It prevents water-carrying residues from settling on the cleaned surface and prevents the formation of scale in pipes, nozzles and tanks. They also interact with surfactants that improve their detergency throughout the cleaning process. EDTA varieties are so soluble that they are used to replace all or some of the phosphates found in many formulations. EDTA varieties can be added to emulsions (including lubricant, brightener) to minimize the impact of water hardness and polyvalent metal ions.
Electroplating: EDTA salt is added to all types of alkaline degreasers to stabilize polyphosphates and to prevent lime soaps from clumping.
This extends the working time of degreasing baths.
EDTA powder is used in neutral and alkaline rust removal and scale removal (deposit removal) baths.

Photography: Complexing agents such as EDTA varieties are added to these developers to prevent precipitation if the developers used in photography were made with hard water.
Rubber: Used to bind iron ions in catalyst systems used in the polymerization of rubber.
Other applications: EDTA varieties are used in the chemical industry where metals must be separated or extracted. EDTA types are useful in radioactive decontamination processes. They are used to dissolve insoluble oxides or radioactive elements. The complex can be easily removed from hard surfaces or skin. The formulations are more meaty if they contain a surfactant.
EDTA varieties can be used in many bleaching, dyeing and finishing processes in textiles.
Safety: The increase in pH results in the separation of ammonia with a strong odor. EDTA can be removed from wastewater by biotic or abiotic processes.

CAS number: 60-00-4
PubChem: 6049
ChemSpider: 5826
UNII: 9G34HU7RV0
EC number: 200-449-4
UN number: 3077
DrugBank: DB00974
KEGG: D00052
MeSH: Edetic Acid
Chebi: 42191 CHEMBL858
RTECS number: AH4025000
ATC code: V03AB03
Beilstein Reference: 1716295
Gmelin Reference: 144943
Molecular formula: C10H16N2O8
Molar mass: 292.24 g mol-1
Appearance: Colorless crystals
Density: 860 mg ml-1 (20 ° C)
Log P: -0,836
Acid (pKa): 1,782
Basicity (PKB): 12,215
Other names: Ethylenediamine tetra acetic acid
View: White crystalline powder

Chemical Name: Ethylenediaminetetraacetic Acid

Chemical Formula: C10H16N2O8

Packaging shape: 25 Kg. in sacks

Definition and Usage Areas:

It behaves like a weak organic acid. Carboxylic acids donate hydrogen ions if there is a base to accept them. In this way, they react with both organic (eg, amines) and inorganic bases. Its reactions with bases, called "neutralizations", are accompanied by substantial amounts of heat. Neutralization between an acid and a base creates water plus a salt.

Carboxylic acids with six or fewer carbon atoms are freely or moderately soluble in water; Those with more than six carbons are poorly soluble in water. Soluble carboxylic acid dissociates from some water to obtain hydrogen ions. Many insoluble carboxylic acids react rapidly with aqueous solutions containing a chemical base and dissolve as neutralization forms a soluble salt. Carboxylic acids and liquid or molten carboxylic acids in aqueous solution can react with active metals to form gaseous hydrogen and a metal salt.

Carboxylic acids, like other acids, react with cyanide salts to form gaseous hydrogen cyanide. The reaction is slower for dry, solid carboxylic acids. Insoluble carboxylic acids react with cyanide solutions to cause the release of gaseous hydrogen cyanide. Flammable and / or toxic gases and heat are produced by the reaction of carboxylic acids with diazo compounds, dithiocarbamates, isocyanates, mercaptans, nitrites and sulfides.

Carboxylic acids react especially with sulfides, nitrites, thiosulfates (to give H2S and SO3), dithionites (SO2) in aqueous solution to produce flammable and / or toxic gases and heat. Their reaction with carbonates and bicarbonates produces a harmless gas (carbon dioxide) but still gives off heat. Like other organic compounds, carboxylic acids can be oxidized with strong oxidizing agents and reduced with strong reducing agents. These reactions generate heat. A wide variety of products are possible. Like other acids, carboxylic acids can initiate polymerization reactions; As with other acids, they usually catalyze (increase the speed) chemical reactions.

Usage areas : Because it is so good at displacing molecules in coordination complexes, EDTA can be used to prevent small amounts of unwanted metals from reacting and having detrimental effects on products.
EDTA serves to increase the resistance of the cosmetic product against molecules in the air.
Similarly, in personal care and skin care products, EDTA binds to free metal ions and acts as a purifying agent and persistent.
It fundamentally reduces the "hardness" (or the presence of metal cations) in tap water so that it can work to clean the shampoo and other ingredients in soap more effectively.
EDTA is used in laundry detergents to soften the water that comes into contact with it so that other active ingredients can clean it better.
In textiles, EDTA removes colorless metal ions from dyed fabrics to prevent discoloration and also removes the residues of industrial equipment (ie broilers) that must be used at high temperatures.
Generally, EDTA lowers the reactivity of a metal and prevents unwanted effects from its presence. EDTA is used in salt form, most likely disodium or calcium disodium EDTA.

SECURITY PRECAUTIONS
 Inhalation of dust, vapors will cause harm. It should not be swallowed. Harmful if swallowed. It is necessary to protect eyes and skin. Eye contact causes damage to the eyes. Areas in contact with the skin should be washed with plenty of water.

CAS Number 10378-23-1
 Linear Formula (NaOOCCH2)2NCH2CH2N(CH2COONa)2 · 2H2O 
Molecular Weight 416.20  Beilstein/REAXYS Number 3861753  
EC Number 200-573-9 
 MDL number MFCD00150026  P
PubChem Substance ID 24894629  N
ACRES NA.75
Biodegradable chelating agents
Aquapharm offers a biodegradable chelant GLDA which is a viable alternative to NTA and EDTA. Aquapharm GLDA is manufactured from renewable raw material which comes from a natural sustainable source. GLDA is classified as readily biodegradable as per OECD 301D tests. In trials, GLDA has proved to have an optimal balance between biodegradability, metal chelation and ease of use. It has uses in Industrial Cleaning, Food Processing, Personal Care, Kitchen Cleaning and Automatic Dishwashing amongst many others. GLDA is free from genetically modified raw materials and is not irritating to the skin or eyes.
Edta compound stands for Ethylenediamine tetraacetic acid 27%. Edta is a polyamino carboxylic acid compound. Its general formula is [CH2N (CH2CO2H) 2] 2. Edta was first defined by Ferdinand Munz. Munz achieved the discovery of EDTA 27% from ethylenediamine and chloracetic acid solutions. When looking at the chemical structure of EDTA, which is one of the polyamino carboxylic acid group, it has 2 amino 4 carboxyl ligands. EDTA shows high affinity for metal ions. It is used to chelate fertilizers. OTHER Usage Areas Biochemistry and molecular biology is used as an ion consumer against enzymes. E.D.T.A. in separation of metal ions used. As a preservative in the food industry, E.D.T.A. used. Water Softening in E.D.T.A. used. In the treatment of lead poisoning in medicine, E.D.T.A. used. E.D.T.A. in dentistry used. E.D.T.A. in blood analysis used. E.D.T.A. in shampoos, detergents, etc. used. E.D.T.A. used. E.D.T.A. in electrolysis process used. E.D.T.A. in degreasing baths used. E.D.T.A. in the photography industry used. E.D.T.A. in the rubber industry is used

IUPAC names
(EDTA)
(Ethylenedinitrilo)tetraacetic acid, EDTA, Edathamil, Ethylenedinitrilotetraacetic acid, Ethylenediaminetetraacetic acid, Diaminoethane-tetraacetic acid
2,2',2'',2'''-(1,2-Ethanediyldinitrilo)tetraacetic acid
2,2',2'',2'''-(1,2-ethanediyldinitrilo)tetrakisacetic acid
2,2',2'',2'''-(Ethane-1,2-diyldinitrilo)tetraacetic acid
2,2',2'',2'''-(ethane-1,2-diyldinitrilo)tetraacetic acid
2-({2-[Bis(carboxymethyl)amino]ethyl}(carboxymethyl)amino)acetic acid
2-({2-[bis(carboxymethyl)amino]ethyl}(carboxymethyl)amino)acetic acid
2-[2-(bis(carboxymethyl)amino)ethyl-(carboxymethyl)amino]acetic acid
2-[2-[bis(carboxymethyl)amino]ethyl-(carboxymethyl)amino]acetic acid
disodium 2-[2-[bis(carboxymethyl)amino]ethyl-(2-oxido-2-oxoethyl)amino]acetate dihydrate
Edetic Acid
Edetic acid
edetic acid
Edetic acid
Registration dossier
Registration dossier
Edetic acid(EDTA)
Edetic AcidEDTAH4EDTA
EDTA
EDTA
EDTA acid
EDTA; Edetic acid; Endrate ...
Ethylene Diamine Tetra Acetic Acid
Ethylenediamine tetraacetic acid
ethylenediamine-N,N-tetraacetic acid; (2,2',2'',2'''-(Ethane-1,2-diyldinitrilo)tetraacetic acid)
ETHYLENEDIAMINETETRAACETIC ACID
Ethylenediaminetetraacetic Acid
Ethylenediaminetetraacetic acid
ETHYLENEDIAMINETETRAACETIC ACID (EDTA)
Ethylenedinitrilotetraacetic acid
N,N,N',N'-tetracarbossimetil-1,2-diamminoetano
Trisodium nitrilotriacetate
{[2-(Bis-carboxymethyl-amino)-ethyl]-carboxymethyl-amino} acetic
{[2-(Bis-carboxymethyl-amino)-ethyl]-carboxymethyl-amino} acetic acid
{[2-(Bis-carboxymethyl-amino)-ethyl]-carboxymethyl-amino}acetic acid
Ácido 2-({2-[bis(carboximetil)amino]etil}(carboximetil)amino)acético

Trade names
Dabeersen H Farmacia
Dabeersen H Técnico
Dabeersen H4 HQ
Dissolvine Z
Dissolvine Z-S
Edetic Acid (EDTA)
EDTA
ethylene diamine tetraacetic acid
Trilon
Trilon BS
Versene
VERSENE* ACID CHELATING AGENT

Other names
Ethylenediaminetetraacetic acid

Chemical Properties
Tributyl phosphate is an odorless colorless to yellow liquid. The solubility of TBP is only 280 mg/L in water at 25°C. It is soluble in diethyl ether, benzene, carbon disulfide. It can be miscible with ethanol. It is stable, but it is incompatible with strong oxidizing agents.

Tributyl phosphate (TBP) is an organophosphorus compound widely used as a solvent in nuclear fuel reprocessing for the extraction of uranium and plutonium from other radionuclides.
The major uses of tributyl phosphate (TBP) in industry are as a flame retardant component of aircraft hydraulic fluid and as a solvent for rare earth extraction and purification. Minor uses of TBP include use as a defoamer additive in cement casings for oil wells, as an anti-air entrainment additive for coatings and floor finishes, as a solvent in nuclear fuel processing, and as a carrier for fluorescent dyes.
The microbial degradation of tributyl phosphate was carried out using Klebsiella pneumoniae S3 isolated from the soil. The solubilization behavior of TBP in aqueous solutions of L64-Pluronics was studied using light and small angle neutron scattering (SANS).
Uses
Tributyl phosphate (TBP) is a trialkyl phosphate that is the tributyl ester of phosphoric acid. TBP is a toxic organophosphorous compound widely used in many industrial applications, including significant usage in nuclear processing. TBP is a solvent and plasticizer for cellulose esters such as nitrocellulose and cellulose acetate. The major uses of TBP in industry are as a component of aircraft hydraulic fluid and as a solvent for extraction and purification of rare earth metals from their ores, such as uranium and plutonium. TBP is used also in mercerizing liquids, where it improves their wetting properties. TBP is also used as a heat exchange medium. TBP is used in some consumer products such as herbicides and water thinned paints and tinting bases.
Preparation
Tributyl phosphate is manufactured by reaction of phosphoryl chloride with n-butanol.
A 1-liter four-necked flask is fitted with an efficient condenser, an air-tight stirrer, a short-stemmed dropping funnel and a thermometer. Calcium chloride tubes are attached to the top of dropping funnel and the reflux condenser. 137 ml (111 g) of dry n-butyl alcohol, 132.5 ml (130 g) of dry pyridine and 140 ml of dry benzene are placed in the flask, which is stirred and cooled in an ice-salt mixture until the temperature falls to – 5° C. 40.5 ml (76.5 g) of freshly redistilled (b.p. 106-107° C) phosphorus oxychloride are dropwise added from the funnel at such a rate that the temperature does not rise above 10° C. When all phosphorus oxychloride has been added the reaction mixture is gently refluxed for 2 hours and cooled to room temperature. 250 ml of water are added in order to dissolve the pyridine hydrochloride, the benzene layer is separated, washed several times with water until the washings are neutral, and dried over anhydrous sodium or magnesium sulfate. The benzene is removed by evaporation and crude tributyl phosphate is purified by distillation in a vacuum. The fraction boiling at 160-162°/15 mm or 138-140°/6 mm is collected yielding 95 g of pure tributyl phosphate.
Potential Exposure
The industrial application of this chemical is responsible for occupational exposure and environmental pollution. Exposure to TBP can be from ingestion, inhalation, or skin or eye contact. This exposure will most often happen from occupational use of hydraulic fluid. If TBP is released to the environment, it will bind tightly to dust particles in the air. Unbound TBP will break down in air. It will move slowly through soil because it will bind with soil particles. It may volatilize slowly from moist soil and water surfaces. It may build up in aquatic organisms. It will be broken down in water by microbes.
Description
On decomposition, TBP releases COx, toxic fumes of phosphoric acid, phosphorus oxides, and/or phosphine. TBP is incompatible with strong oxidising agents and alkalis. The major uses of TBP in industry are as a component of aircraft hydraulic fluid and as a solvent for rare earth extraction and purification. Minor uses of TBP include use as a defoamer additive in cement casings for oil wells, an anti-air entrainment additive for coatings and floor finishes, as well as a carrier for fluorescent dyes. The major uses of TBP comprise over 80% of the volume produced.
Chemical Properties
Stable, colorless liquid; odorless. Miscible with most solvents and diluents; soluble in water. Combustible.
Physical properties
Clear, colorless to pale yellow, odorless, slightly flammable, oily liquid
Uses
Tributyl phosphate is used as a plasticizer for cellulose esters, vinyl resins, and lacquers; and in making fireretardants, biocides, defoamers, and catalysts.
Uses
Plasticizer for cellulose esters, lacquers, plastics, and vinyl resins.
Uses
Tributyl phosphate is used as an antifoaming agent; plasticizer for cellulose esters, lacquers, plastic, and vinyl resins; component in hydraulic fluids for aircraft control systems.
Definition
ChEBI: A trialkyl phosphate that is the tributyl ester of phosphoric acid.
Production Methods
Prepared by the reaction of phosphorus oxychloride with butyl alcohol.
Air & Water Reactions
Water insoluble. Reacts slowly with water under basic conditions.
Reactivity Profile
Tributyl phosphate is incompatible with strong oxidizing agents and strong bases. Attacks some forms of plastics and rubber .
Health Hazard
Tributyl phosphate is a neurotoxic compound and an irritant. The toxic effects are characteristic of organic phosphates. It inhibits cholinesterase activity and causes paralysis. Inaddition,itcancausedepressionofthecentralnervoussystem,aswellasirritationofthe skin,eyes,andrespiratorypassage.Inhalation toxicity data in the literature are inconsistent.
The oral toxicity in rats was low; the LD50 value was reported as 1189 mg/kg (NIOSH 1986).
The pure liquid instilled into rabbits’ eyes caused severe irritation but no permanent damage. The irritation effect on the skin is mild.
Tributyl phosphate exhibited teratogenic effects in rats. There is no report on its carcinogenicity..
Fire Hazard
Special Hazards of Combustion Products: Toxic fumes of PO x
Industrial uses
1. As an antifoaming agent.
2. As a plasticizer for cellulose esters, lacquers, plastics, and vinyl resins.
3. As a complexing agent in the extraction of heavy metals, especially for the extraction of metal ions from solutions of reactor products in nuclear fuel reprocessing.
4. As an aircraft hydraulic fluid.
5. As a heat exchange medium and dielectric.
6. As a pigment-grinding agent.
Safety Profile
Poison by intraperitoneal and intravenous routes. Moderately toxic by ingestion, inhalation, and subcutaneous routes. Experimental reproductive effects. A skin, eye, and mucous membrane irritant. Combustible when exposed to heat or flame. To fight fire, use CO2, dry chemical, fog, mist. When heated to decomposition it emits toxic fumes of POx.
Carcinogenicity
Environmental Fate
Biological. Indigenous microbes in Mississippi River water degraded tributyl phosphate to carbon dioxide. After 4 wk, 90.8% of the theoretical carbon dioxide had evolved (Saeger et al., 1979).
Chemical/Physical. Complete hydrolysis yields 1-butanol and phosphoric acid via the intermediates dibutyl phosphate and monobutyl phosphate (Thomas and Macaskie, 1996).
Purification Methods
The main contaminants in commercial samples are organic pyrophosphates, monoand dibutyl phosphates and butanol. It is purified by washing successively with 0.2M HNO3 (three times), 0.2M NaOH (three times) and water (three times), then fractionally distilled under vacuum. [Yoshida J Inorg Nucl Chem 24 1257 1962.] It has also been purified via its uranyl nitrate addition compound, obtained by saturating the crude phosphate with uranyl nitrate. This compound is crystallised three times from n-hexane by cooling to -40o, and then decomposed by washing with Na2CO3 and water. Hexane is removed by steam distillation; the water is then evaporated under reduced pressure, and the residue is distilled under reduced pressure. [Siddall & Dukes J Am Chem Soc 81 790 1959.] Alternatively, wash it with water, then with 1% NaOH or 5% Na2CO3 for several hours, then finally with water. Dry it under reduced pressure and fractionate it carefully under vacuum. It is a stable colourless oil, sparingly soluble in H2O (1mL dissolves in 165mL of H2O), but freely miscible in organic solvents. [Kuivila & Masterton J Am Chem Soc 74 4953 1952, Cox & Westheimer J Am Chem Soc 80 5441 1958, 31P NMR: Van Wazer J Am Chem Soc 78 5715 1956, Fertig et al. J Chem Soc 1488 1957, Beilstein 1 IV 1531.]
Waste Disposal
Tributyl phosphate is dissolved in a combustible solvent and is burned in a chemical incinerator equipped with an afterburner and scrubber.
Ethylenediaminetetraacetic acid (EDTA) is an aminopolycarboxylic acid with the formula [CH2N(CH2CO2H)2]2. This white, water-soluble solid is widely used to bind to iron and calcium ions. It binds these ions as a hexadentate ("six-toothed") chelating agent. EDTA is produced as several salts, notably disodium EDTA, sodium calcium edetate, and tetrasodium EDTA.[4]
Uses
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 catalysing the disproportionation of hydrogen peroxide, which is used in chlorine-free bleaching. In a similar manner, EDTA is added to some food as a preservative or stabiliser to prevent catalytic oxidative decolouration, which is catalysed by metal ions. 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+, Mg2+, as well as other metal ions. Once bound to EDTA, these metal centres tend not to form precipitates or to interfere with the action of the soaps and detergents. For similar reasons, cleaning solutions often contain EDTA. In a similar manner EDTA is used in the cement industry for the determination of free lime and free magnesia in cement and clinkers. 
The solubilisation of Fe3+ ions at or below near neutral pH can be accomplished using EDTA. This property is useful in agriculture including hydroponics. However, given the pH dependence of ligand formation, EDTA is not helpful for improving iron solubility in above neutral soils.[8] Otherwise, at near-neutral pH and above, iron(III) forms insoluble salts, which are less bioavailable to susceptible plant species. Aqueous [Fe(EDTA)]− is used for removing ("scrubbing") hydrogen sulfide from gas streams. This conversion is achieved by oxidising the hydrogen sulfide to elemental sulfur, which is non-volatile:
2 [Fe(EDTA)]− + H2S → 2 [Fe(EDTA)]2− + S + 2 H+
In this application, the iron(III) centre is reduced to its iron(II) derivative, which can then be reoxidised by air. In similar manner, nitrogen oxides are removed from gas streams using [Fe(edta)]2−. The oxidising properties of [Fe(edta)]− are also exploited in photography, where it is used to solubilise silver particles.[4]
EDTA was used in separation of the lanthanide metals by ion-exchange chromatography. Perfected by F. H. Spedding et al. in 1954,[citation needed] the method relies on the steady increase in stability constant of the lanthanide EDTA complexes with atomic number. Using sulfonated polystyrene beads and Cu2+ 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%). 
Synthesis
The compound was first described in 1935 by Ferdinand Münz, who prepared the compound from ethylenediamine and chloroacetic acid.[23] Today, EDTA is mainly synthesised from ethylenediamine (1,2-diaminoethane), formaldehyde, and sodium cyanide. This route yields the tetrasodium EDTA, which is 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
This process is used to produce about 80,000 tonnes of EDTA each year. Impurities cogenerated by this route include glycine and nitrilotriacetic acid; they arise from reactions of the ammonia coproduct. 
Nomenclature
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 H6EDTA2+ form predominates, whereas at very high pH or very basic condition, the fully deprotonated EDTA4− form is prevalent. In this article, the term EDTA is used to mean H4−xEDTAx−, whereas in its complexes EDTA4− stands for the tetraanion ligand.
Coordination chemistry principles

Metal–EDTA chelate as found in Co(III) complexes.
Structure of [Fe(EDTA)(H2O)]−, showing that the EDTA4− ligand does not fully encapsulate Fe(III), which is seven-coordinate. 
In coordination chemistry, EDTA4− is a member of the aminopolycarboxylic 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 cobalt(III) anion [Co(EDTA)]− has been resolved into enantiomers. Many complexes of EDTA4− 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 iron(III) complex of EDTA is seven-coordinate. 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.
The pKa values of free EDTA are 0, 1.5 (deprotonation of the two amino groups), 2, 2.66, 6.16 and 10.24 (deprotonation of the four carboxyl groups) . 
Environmental fate
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. 
The most important process for the elimination of EDTA from surface waters is direct photolysis at wavelengths below 400 nm. Depending on the light conditions, the photolysis half-lives of iron(III) EDTA in surface waters can range as low as 11.3 minutes up to more than 100 hours.[33] 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 Mg2+ and Ca2+) are more persistent.
Biodegradation
In many industrial wastewater treatment plants, EDTA elimination can be achieved at about 80% using microorganisms. Resulting byproducts are ED3A and 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. 
Several bacterial strains isolated from sewage treatment plants efficiently degrade EDTA. Specific strains include Agrobacterium radiobacter ATCC 55002 and the sub-branches of Proteobacteria like BNC1, BNC2,[37] and strain DSM 9103. The three strains share similar properties of aerobic respiration and are classified as 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) EDTAwhile BNC1 and DSM 9103 are not capable of degrading iron(III) EDTA and are more suited for calcium, barium, magnesium and manganese(II) complexes. 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. Candidate chelating agents include nitrilotriacetic acid (NTA), iminodisuccinic acid (IDS), polyaspartic acid, S,S-ethylenediamine-N,N′-disuccinic acid (EDDS), methylglycinediacetic acid (MGDA), and L-Glutamic acid N,N-diacetic acid, tetrasodium salt (GLDA). 
Iminodisuccinic acid (IDS)
Commercially used since 1998, 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 Agrobacterium tumefaciens (BY6), which can be harvested on a large scale. The enzymes involved, IDS epimerase and C−N lyase, do not require any cofactors. 
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. 
S,S-Ethylenediamine-N,N′-disuccinic acid (EDDS)
The S,S isomer of EDTA, ethylenediamine-N,N′-disuccinic acid (EDDS) is readily biodegradable and exhibits a high rate biodegradation. 
Methylglycinediacetic acid (MGDA)
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. MGDA has been shown to be an effective chelating agent, with a capacity for mobilization comparable with that of Nitrilotriacetic acid (NTA), with application to water for industrial use and for the removal of calcium oxalate from urine from patients with kidney stones.[44]
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 (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. 
EDTA has also been measured in non-alcoholic beverages using high performance liquid chromatography (HPLC) at a level of 2.0 μg/mL. 
In popular culture
•    In the movie Blade (1998), EDTA is used as a weapon to kill vampires, exploding when in contact with vampire blood.