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Ethylenediamine tetraacetic acid, also called EDTA acid, is an aminopolycarboxylic acid with the formula [CH2N(CH2CO2H)2]2.
Ethylenediamine tetraacetic acid is thus used to dissolve Fe- and Ca-containing scale as well as to deliver iron ions under conditions where its oxides are insoluble.
Ethylenediamine tetraacetic acid is available as several salts, notably disodium EDTA, sodium calcium edetate, and tetrasodium EDTA, but these all function similarly.
CAS Number: 60-00-4
Molecular Formula: C10H16N2O8
Molecular Weight: 292.24
EINECS Number: 200-449-4
Synonyms: EDTA, Edetic acid, Ethylenediaminetetraacetic acid, 60-00-4, Edathamil, Sequestrol, Havidote, Titriplex, EDTA acid, Versene acid, Cheelox, Gluma cleanser, Sequestrene aa, Sequestric acid, Warkeelate acid, Komplexon ii, Tetrine acid, Quastal Special, Metaquest A, Trilon bw, Titriplex II, Hamp-ene acid, Cheelox BF acid, Trilon BS, Celon A, Celon ATH, Chelest 3A, Questex 4H, (Ethylenedinitrilo)tetraacetic acid, Chemcolox 340, Acide edetique, Acido edetico, Universne acid, EDTA (chelating agent), Dissolvine E, Vinkeil 100, Nullapon B acid, Nullapon bf acid, Nervanaid B acid, Perma kleer 50 acid, Clewat TAA, Ethylenedinitrilotetraacetic acid, Acidum edeticum, Caswell No. 438, ICRF 185, Ethylenebisiminodiacetic acid, Ethylenediamine-N,N,N',N'-tetraacetic acid, SEQ 100, YD 30, CCRIS 946, Ethylenebis(iminodiacetic acid), HSDB 809, Acide ethylenediaminetetracetique, ETHYLENEDIAMINE TETRAACETIC ACID, Acide edetique [INN-French], Acido edetico [INN-Spanish], Acidum edeticum [INN-Latin], Acetic acid, (ethylenedinitrilo)tetra-, EPA Pesticide Chemical Code 039101, Kyselina ethylendiamintetraoctova, Tricon bw, Acid, Edetic, AI3-17181, H4edta, 3,6-Diazaoctanedioic acid, 3,6-bis(carboxymethyl)-, EINECS 200-449-4, UNII-9G34HU7RV0, BRN 1716295, 9G34HU7RV0, Acetic acid, 2,2',2'',2'''-(1,2-ethanediyldinitrilo)tetrakis-, DTXSID6022977, N,N'-1,2-Ethanediylbis(N-(carboxymethyl)glycine), CHEBI:42191, N,N'-1,2-Ethane diylbis-(N-(carboxymethyl)glycine), {[-(BIS-CARBOXYMETHYL-AMINO)-ETHYL]-CARBOXYMETHYL-AMINO}-ACETIC ACID, ethylenediamine tetracetic acid, DTXCID902977, (ethylenedinitrilo)tetraacetic acid, ion(4-), EC 200-449-4, (ethane-1,2-diyldinitrilo)tetraacetic acid, ([2-(Bis-carboxymethyl-amino)-ethyl]-carboxymethyl-amino)-acetic acid, (ethylenedinitrilo)tetra-aceticaci, (Ethylenedintrilo)tetraacetic acid, {[2-(Bis-carboxymethyl-amino)-ethyl]-carboxymethyl-amino}-acetic acid, 2,2’,2’’,2’’’-(1,2-ethanediyldinitrilo)tetrakis-aceticaci, 3,6-bis(carboxymethyl)-6-diazaoctanedioicacid, 3,6-Diazaoctanedioic acid, 3,6-bis(carboxymethyl)-, Acetic acid, (ethylenedinitrilo)tetra-
Ethylenediamine tetraacetic acid is a synthetic, amino acid–like compound that acts as a powerful chelating agent, meaning it has the ability to bind to and form stable complexes with metal ions, especially heavy metals such as lead, mercury, cadmium, and calcium.
Because of this property, Ethylenediamine tetraacetic acid is widely used in various industrial, medical, pharmaceutical, and laboratory settings to control, remove, or neutralize metal ions that might otherwise cause harm or interfere with chemical processes.
Ethylenediamine tetraacetic acid consists of a central ethylenediamine molecule connected to four acetic acid groups, which together provide multiple sites for binding to metal ions, forming a cage-like structure that traps the metal and prevents it from reacting with other substances.
This makes Ethylenediamine tetraacetic acid particularly useful in situations where trace metals could catalyze unwanted chemical reactions or degrade products, such as in food, cosmetics, or pharmaceuticals.
Ethylenediamine tetraacetic acid is a common polydentate ligand.
In Ethylenediamine tetraacetic acid, the hydrogen atoms are easily removed in solution to produce anionic EDTA4-.
In its anionic form Ethylenediamine tetraacetic acid has six binding atoms, two nitrogen and four oxygen.
Ethylenediamine tetraacetic acid binds to a metal ion at the six binding sites, wrapping itself around the metal ion, forming a very stable complex.
The strong grasp of Ethylenediamine tetraacetic acid on the metal ion is analogous to a crab or lobster clamping down on an object with its claw, hence the name chelation.
Ethylenediamine tetraacetic acid is such an effective chelating agent because it can deactivate a metal at up to six sites.
In many industrial wastewater treatment plants, Ethylenediamine tetraacetic acid elimination can be achieved at about 80% using microorganisms.
Resulting byproducts are Ethylenediamine tetraacetic acid 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 Ethylenediamine tetraacetic acid.
Specific strains include Agrobacterium radiobacter ATCC 55002 and the sub-branches of Pseudomonadota 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–Ethylenediamine tetraacetic acid complexes through several enzymatic pathways.
Agrobacterium radiobacter only degrades Fe(III) Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid complexes require dissociation before degradation.
Interest in environmental safety has raised concerns about biodegradability of aminopolycarboxylates such as Ethylenediamine tetraacetic acid.
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).
Ethylenediamine tetraacetic acid is a kind of metal chelating agent (binds to bivalent and trivalent metal cations, including calcium).
Ethylenediamine tetraacetic acid has antibacterial, anti-inflammatory, antioxidant, anti-hypercalcemia and anticoagulant activities.
Ethylenediamine tetraacetic acid decreases the metal ion-catalyzed oxidative damage to proteins, and allows maintenance of reducing environment during protein purification.
Ethylenediamine tetraacetic acid can alleviate the liver fibrosis.
Ethylenediamine tetraacetic acid can be used for coronary artery disease and neural system disease research.
Ethylenediamine tetraacetic acid is sometimes used in a process known as chelation therapy, which involves injecting or infusing the compound into the bloodstream to help remove toxic metals—such as lead or arsenic—from the body.
Ethylenediamine tetraacetic acid is also used in certain blood collection tubes and anticoagulants to prevent blood from clotting, as Ethylenediamine tetraacetic acid can bind calcium, a mineral essential for the clotting process.
This study investigates the use of photo-Fenton processes catalyzed by Ethylenediamine tetraacetic acid under neutral pH conditions, optimizing reaction parameters for environmental applications.
This white, slightly water-soluble solid is widely used to bind to iron (Fe2+/Fe3+) and calcium ions (Ca2+), forming water-soluble complexes even at neutral pH.
Mixtures of chelating agents to enhance photo-Fenton process at natural pH: Influence of wastewater matrix on micropollutant removal and bacterial inactivation.
Research shows how Ethylenediamine tetraacetic acid, when used in combination with other chelators, enhances the efficiency of the photo-Fenton process at natural pH levels for water treatment, focusing on micropollutant degradation and pathogen inactivation.
Ethylenediamine tetraacetic acid is the salt resulting from the neutralization of ethylenediaminetetraacetic acid with four equivalents of sodium hydroxide (or an equivalent sodium base).
Ethylenediamine tetraacetic acid is a white solid that is highly soluble in water.
Commercial samples are often hydrated, e.g. Na4EDTA.4H2O.
The properties of solutions produced from the anhydrous and hydrated forms are the same, provided they are at the same pH.
Ethylenediamine tetraacetic acid is used as a source of the chelating agent EDTA4-.
When dissolved in neutral water, it converts partially to H2EDTA2-.
Ethylenediamine tetraacetic acid is produced commercially via the intermediacy of tetrasodium EDTA.
Ethylenediamine tetraacetic acid is also known as Dissolvine E-39.
Ethylenediamine tetraacetic acid is a salt of edetic acid.
It has been known at least since 1954.
Ethylenediamine tetraacetic acid is sometimes used as a chelating agent.
The assignee on 5% of patents at the USPTO containing the substance is the firm Procter and Gamble.
Ethylenediamine tetraacetic acid is used most notably in cosmetics and hair and skin care products.
Ethylenediamine tetraacetic acid has been used to aid in formulation of a removal product for rust, corrosion, and scale from ferrous metal, copper, brass, and other surfaces.
At a concentration of 6%, Ethylenediamine tetraacetic acid is the main active ingredient in some types of engine coolant system flushes.
Ethylenediamine tetraacetic acid, Sodium Salt (EDTA) is a colorless, crystalline solid, used as an industrial chelating agent, food preservative and in medicine to chelate lead, copper, etc. in metal poisoning to prevent coagulation of blood.
Ethylenediamine tetraacetic acid and its salts (such as disodium EDTA or tetrasodium EDTA) are added to shampoos, soaps, creams, and lotions to improve product stability and effectiveness by binding metal ions that may be present in water or raw ingredients, which could otherwise cause changes in color, odor, or texture over time.
Melting point: 250 °C (dec.) (lit.)
Boiling point: 434.18 °C (rough estimate)
Bulk density: 600 kg/m³
Density: 1.46 g/cm³ at 20 °C
Vapor pressure: <0.013 hPa (20 °C)
Refractive index: n20/D 1.363
Flash point: >400 °C DIN 51758
Storage temp.: 2–8 °C
Solubility: 3 M NaOH: 100 mg/mL
Form: Crystalline
pKa: pKa 2 (Uncertain), 10.26 (Uncertain)
Color: White to almost white
Odor: Odorless
pH Range: 2.5 at 10 g/L at 23 °C
pH: 2.5 (10 g/L, H₂O, 23 °C) (slurry)
Water solubility: 0.5 g/L (25 °C)
λmax: λ: 280 nm Amax: ≤0.25
Decomposition: 240 °C
Merck: 14,3517
BRN: 1716295
Stability: Stable. Incompatible with copper, copper alloys, nickel, aluminium, strong oxidizing agents, strong bases
LogP: –0.836 (est)
Ethylenediamine tetraacetic acid is a colorless crystalline solid. Ethylenediaminetetraacetic acid is slightly soluble in water.
The primary hazard is the threat to the environment.
Immediate steps should be taken to limit its spread to the environment.
Ethylenediamine tetraacetic acid is used in chemical analysis, to make detergents and cleaning compounds, and for many other uses.
Ethylenediamine tetraacetic acid is generally considered safe when used appropriately and in controlled amounts, it can pose risks if used improperly, particularly in high doses or over prolonged periods.
Potential side effects of medical chelation therapy may include kidney stress, mineral imbalances, or allergic reactions.
For these reasons, its medical use is typically limited to specific, diagnosed cases of metal poisoning and carried out under professional supervision.
Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid is a highly versatile and widely used chemical compound valued for its ability to bind metal ions, making it essential in diverse fields ranging from medicine and cosmetics to industrial chemistry and environmental science.
Ethylenediamine tetraacetic acid is commonly used in buffer solutions, detergents, and cleaning agents to neutralize metal ions and enhance the performance of certain reactions or processes.
Ethylenediamine tetraacetic acid also plays a role in water treatment, where it helps prevent the buildup of mineral deposits in pipes, boilers, or cooling systems by binding to calcium and magnesium ions found in hard water.
Ethylenediamine tetraacetic acid was first synthesized in the early 1930s by the German chemist Ferdinand Münz working for I. G. Farben.
Münz, who was looking for a substitute for citric acid to use with dye solutions in the textile industry, was the first to patent a process for Ethylenediamine tetraacetic acid synthesis in Germany in 1935.
Münz subsequently applied for United States patents in 1936 and 1937, his method involved reacting monochloroacetic acid (C2H3ClO2) and ethylene diamine (C2H8N2).
Concurrent with Münz’s work, Frederick C. Bersworth in the United States synthesized Ethylenediamine tetraacetic acid using different methods that gave greater yields and made EDTA’s commercial production economically viable.
Bersworth syntheses involved reacting formaldehyde, amines, and hydrogen cyanide. Bersworth and Münz obtained patents for Ethylenediamine tetraacetic acid production in the 1940s.
Ethylenediamine tetraacetic acid may be prepared by the condensation of ethylenediamine with sodium monochloroacetate in the presence of sodium carbonate.
An aqueous solution of the reactants is heated to about 90°C for 10 hours, then cooled, and hydrochloric acid is added to precipitate the edetic acid.
Ethylenediamine tetraacetic acid may also be prepared by the reaction of ethylenediamine with hydrogen cyanide and formaldehyde with subsequent hydrolysis of the tetranitrile, or under alkaline conditions with continuous extraction of ammonia.
Behaves as a weak organic acid carboxylic acids donate hydrogen ions if a base is present to accept them.
They react in this way with all bases, both organic (for example, the amines) and inorganic.
Their reactions with bases, called "neutralizations", are accompanied by the evolution of substantial amounts of heat.
Neutralization between an acid and a base produces water plus a salt.
Ethylenediamine tetraacetic acid with six or fewer carbon atoms are freely or moderately soluble in water, those with more than six carbons are slightly soluble in water.
Soluble carboxylic acid dissociate to an extent in water to yield hydrogen ions.
The pH of solutions of carboxylic acids is therefore less than 7.0.
Many insoluble carboxylic acids react rapidly with aqueous solutions containing a chemical base and dissolve as the neutralization generates a soluble salt.
Ethylenediamine tetraacetic acid in aqueous solution and liquid or molten carboxylic acids can react with active metals to form gaseous hydrogen and a metal salt.
Such reactions occur in principle for solid Ethylenediamine tetraacetic acid as well, but are slow if the solid acid remains dry.
Even "insoluble" carboxylic acids may absorb enough water from the air and dissolve sufficiently in Ethylenediaminetetraacetic acid to corrode or dissolve iron, steel, and aluminum parts and containers.
Ethylenediamine tetraacetic acid, like other acids, react with cyanide salts to generate gaseous hydrogen cyanide.
The reaction is slower for dry, solid carboxylic acids. Insoluble carboxylic acids react with solutions of cyanides to cause the release of gaseous hydrogen cyanide.
Flammable and/or toxic gases and heat are generated by the reaction of carboxylic acids with diazo compounds, dithiocarbamates, isocyanates, mercaptans, nitrides, and sulfides.
Ethylenediamine tetraacetic acid, especially in aqueous solution, also react with sulfites, nitrites, thiosulfates (to give H2S and SO3), dithionites (SO2), to generate flammable and/or toxic gases and heat.
Their reaction with carbonates and bicarbonates generates a harmless gas (carbon dioxide) but still heat.
Like other organic compounds, carboxylic acids can be oxidized by strong oxidizing agents and reduced by strong reducing agents.
These reactions generate heat.
A wide variety of products is possible like other acids, carboxylic acids may initiate polymerization reactions, like other acids, they often catalyze (increase the rate of) chemical reactions
If Ethylenediamine tetraacetic acid gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids.
If Ethylenediamine tetraacetic acid contacts theskin, remove contaminated clothing and wash immediatelywith soap and water.
If Ethylenediamine tetraacetic acid has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if heart action has stopped.
When Ethylenediamine tetraacetic acid has been swallowed, get medical attention. Give large quantities of water and inducevomiting.
Storage Of Ethylenediamine tetraacetic acid:
Although Ethylenediamine tetraacetic acid is fairly stable in the solid state, edetate salts are more stable than the free acid, which decarboxylates if heated above 150°C.
Disodium edetate dihydrate loses water of crystallization when heated to 120°C.
Edetate calcium disodium is slightly hygroscopic and should be protected from moisture.
Aqueous solutions of Ethylenediamine tetraacetic acid or edetate salts may be sterilized by autoclaving, and should be stored in an alkali-free container.
Ethylenediamine tetraacetic acid and edetates should be stored in well-closed containers in a cool, dry place.
Uses Of Ethylenediamine tetraacetic acid:
Ethylenediamine tetraacetic acid, also known as editic acid, is a colorless crystalline substance widely used to chelate metal ions.
Ethylenediamine tetraacetic acid is marketed in its salt forms such as sodium Ethylenediaminetetraacetic Acid (EDTA) or calcium EDTA.
Ethylenediamine tetraacetic acid hasindustrial and medical uses as a chelating agent.
Much of its utility is related to the fact that metals and metal compounds are important catalysts in numerous reactions.
By chelatingmetals, Ethylenediamine tetraacetic acid prevents the metal from catalyzing reactions, thereby limiting degradation, oxidation,and other undesirable reactions.
The major industries using Ethylenediamine tetraacetic acid and other chelatingagents are paper and pulp, cleaning products, chemicals, agriculture, and water treatment.
The paper and pulp industry is the major user of Ethylenediamine tetraacetic acid, where it is used to stabilize bleachesby sequestering metals that catalyze the degradation of bleaches.
Ethylenediamine tetraacetic acid’s ability to stabilizebleaches also makes them useful in laundry detergents and various other cleaning products.
In addition to improving bleaching effi ciency, Ethylenediamine tetraacetic acid use in detergents and cleansers alsosoftens hard water by tying up divalent metal ions responsible for water hardness, primarilyCa2+ and Mg2+.
Its softening ability helps Ethylenediamine tetraacetic acid reduce scale formation and improves foamingproperties in cleaning formulations.
Ethylenediamine tetraacetic acid is applied in general water treatment to softenwater, helping to prevent scale and corrosion.
Ethylenediamine tetraacetic acid has low toxicity and is used in the foodand beverage industry.
Foods naturally contain small traces of metals and small quantities areadded during food processing.
Ethylenediamine tetraacetic acid is used with foods to preserve color and preserve flavor,prevent odors, maintain nutrient content, and extend shelf life.
When used in beverages, Ethylenediamine tetraacetic acid preserves color and stabilizes other ingredients such as citric acid and benzoates.
In thechemical industry, Ethylenediamine tetraacetic acid is used to control metal catalytic processes during reactions.
Ethylenediamine tetraacetic acid salts are used in agriculture to provide metal micronutrients in fertilizers.
Ethylenediamine tetraacetic acid is a powerful chelating agent, EDTA forms stable complexes with most metal ions.
Ethylenediamine tetraacetic acid is used in treatment of lead and heavy metal poisoning of farm a nimals.
Ethylenediamine tetraacetic acid is helps boost a formulation’s preservative system and is also a chelating agent.
Ethylenediamine tetraacetic acid is a sequestrant and chelating agent that functions in water but not in fats and oils.
Ethylenediamine tetraacetic acid is used to control the reaction of trace metals with some organic and inorganic components to prevent deterioration of color, texture, and development of precipitates, as well as to prevent oxidation which results in rancidity.
The reactive sites of the metal ions are blocked, which prevents their normal reactions.
The most common interfering metal ions in food products are iron and copper.
Ethylenediamine tetraacetic acid can be used in combination with the antioxidants bht and propyl gallate.
It is used in margarine, mayonnaise, and spreads to prevent the vegetable oil from going rancid.
Ethylenediamine tetraacetic acid is used in canned corn prior to retorting to prevent discoloration caused by trace quantities of copper, iron, and chromium.
Ethylenediamine tetraacetic acid also inhibits copper-catalyzed oxidation of ascorbic acid.
Ethylenediamine tetraacetic acid occurs as disodium calcium and disodium dihydrogen.
Its use is approved in specified foods, with an average usage level being in the range of 100–300 ppm.
Ethylenediamine tetraacetic acid and edetate salts are used in pharmaceutical formulations, cosmetics, and foods as chelating agents.
They form stable water-soluble complexes (chelates) with alkaline earth and heavy metal ions.
The chelated form has few of the properties of the free ion, and for this reason chelating agents are often described as ‘removing’ ions from solution, this process is also called sequestering.
The stability of the metal–edetate complex depends on the metal ion involved and also on the pH.
The calcium chelate is relatively weak and will preferentially chelate heavy metals, such as iron, copper, and lead, with the release of calcium ions.
For this reason, edetate calcium disodium is used therapeutically in cases of lead poisoning.
Ethylenediamine tetraacetic acid and edetates are primarily used as antioxidant synergists, sequestering trace amounts of metal ions, particularly copper, iron, and manganese, that might otherwise catalyze autoxidation reactions.
Ethylenediamine tetraacetic acid and edetates may be used alone or in combination with true antioxidants, the usual concentration employed being in the range 0.005–0.1% w/v.
Edetates have been used to stabilize ascorbic acid, corticosteroids, epinephrine, folic acid, formaldehyde, gums and resins, hyaluronidase, hydrogen peroxide, oxytetracycline, penicillin, salicylic acid, and unsaturated fatty acids.
Essential oils may be washed with a 2% w/v solution of edetate to remove trace metal impurities.
Ethylenediamine tetraacetic acid and edetates possess some antimicrobial activity but are most frequently used in combination with other antimicrobial preservatives owing to their synergistic effects.
Many solutions used for the cleaning, storage, and wetting of contact lenses contain disodium edetate.
Typically, edetic acid and edetates are used in concentrations of 0.01–0.1% w/v as antimicrobial preservative synergists.
Ethylenediamine tetraacetic acid and disodium edetate may also be used as water softeners since they will chelate the calcium and magnesium ions present in hard water, edetate calcium disodium is not effective.
Many cosmetic and toiletry products, e.g. soaps, contain edetic acid as a water softener.
Ethylenediamine tetraacetic acid is short for ethylenediamhetetraacetic acid, an amino polycarboxylic acid.
It is a tetraprotic acid and is represented as H4Y with four carboxyl groups and two nitrogen atoms acting as ligand sites.
Thus the compound is a hexadentate ligand.
Ligands include ions such as Cl-, NO2-and CN- or neutral molecules like NH3 and H2O, which possess a lone pair of electrons that can be shared with a metal cation in coordinate covalent bonds.
The water solubility of Ethylenediamine tetraacetic acid is very low and, therefore, its di-sodium salt Na2H2Y.2H2O is commonly used in titrations.
The Y4- forms very stable, one-to-one complexes with practically every metal ion in the Periodic Table.
The reactions are carried out in a neutral or alkaline medium as the complex decomposes in acidic medium.
Ethylenediamine tetraacetic acid metal complexes, such as NaFeEDTA, MnEDTA, ZnEDTA and CuEDTA are used as fertilizers and foliar sprays.
Ethylenediamine tetraacetic acid is an anticoagulant, majorly used in preventing clotting of blood samples.
Ethylenediamine tetraacetic acid may trigger aggregation of platelets resulting in pseudothrombocytopenia.
Ethylenediamine tetraacetic acid along with tetracycline imparts serves as root conditioning agent and provides relief in gum infection.
Ethylenediamine tetraacetic acid-tetracycline therapy decreases coronary artery calcium levels in atherosclerosis.
Ethylenediamine tetraacetic acid administration is effective in slowing down the progression of chronic kidney disease.
Ethylenediamine tetraacetic acid is widely used in industry.
Ethylenediamine tetraacetic acid also has applications in food preservation, medicine, cosmetics, water softening, in laboratories, and other fields.
Ethylenediamine tetraacetic acid is mainly used to 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, Ethylenediamine tetraacetic acid inhibits the ability of metal ions, especially Mn2+, from catalysing the disproportionation of hydrogen peroxide, which is used in chlorine-free bleaching.
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 a similar manner, nitrogen oxides are removed from gas streams using [Fe(EDTA)]2−
Sodium calcium edetate, an Ethylenediamine tetraacetic acid derivative, is used to bind metal ions in the practice of chelation therapy, such as for treating mercury and lead poisoning.
Ethylenediamine tetraacetic acid 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.
In the laboratory, Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid also acts as a selective inhibitor against dNTP hydrolyzing enzymes liver arginase and horseradish peroxidase independently of metal ion chelation.
These findings urge the rethinking of the utilisation of Ethylenediamine tetraacetic acid as a biochemically inactive metal ion scavenger in enzymatic experiments.
In analytical chemistry, Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid 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, Ethylenediamine tetraacetic acid 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, Ethylenediamine tetraacetic acid can be used as a decalcifying agent making it possible to cut sections using a microtome once the tissue sample is demineralised.
Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid is in such widespread use that questions have been raised whether it is a persistent organic pollutant.
While Ethylenediamine tetraacetic acid 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.
Ethylenediamine tetraacetic acid mainly occurs abiotically in the presence of sunlight.
The most important process for the elimination of Ethylenediamine tetraacetic acid from surface waters is direct photolysis at wavelengths below 400 nm.
Depending on the light conditions, the photolysis half-lives of iron(III) Ethylenediamine tetraacetic acid in surface waters can range from as low as 11.3 minutes up to more than 100 hours.
Degradation of FeEDTA, but not Ethylenediamine tetraacetic acid 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.
Safety Profile Of Ethylenediamine tetraacetic acid:
Ethylenediamine tetraacetic acid exhibits low acute toxicity with LD50 (rat) of 2.0 g/kg to 2.2 g/kg.
Ethylenediamine tetraacetic acid has been found to be both cytotoxic and weakly genotoxic in laboratory animals.
Oral exposures have been noted to cause reproductive and developmental effects.
The same study also found that both dermal exposure to Ethylenediamine tetraacetic acid in most cosmetic formulations and inhalation exposure to EDTA in aerosolised cosmetic formulations would produce exposure levels below those seen to be toxic in oral dosing studies.
Ethylenediamine tetraacetic acid, especially in its pure form or concentrated solutions, can cause mild to moderate irritation to the skin, eyes, and respiratory system upon direct contact or inhalation.
If it comes into contact with the eyes, it may cause redness, tearing, and a burning sensation, while skin exposure can lead to dryness, itching, or rash.
Inhalation of dust or aerosolized particles may irritate the nasal passages, throat, or lungs, resulting in coughing or shortness of breath, particularly in poorly ventilated environments.
Repeated or prolonged exposure to Ethylenediamine tetraacetic acid or its salts (such as disodium EDTA or tetrasodium EDTA) may lead to skin sensitization or allergic reactions in some individuals.
These may include contact dermatitis, inflammation, or allergic rashes, especially for people with sensitive skin or a history of allergies to cosmetic or cleaning products.
While Ethylenediamine tetraacetic acid is used in very small amounts in food and pharmaceutical products as a stabilizer or preservative, accidental or intentional ingestion of large amounts can be harmful.
In high doses, Ethylenediamine tetraacetic acid can bind to essential minerals like calcium, magnesium, iron, and zinc in the body, leading to mineral deficiencies, electrolyte imbalances, and, in extreme cases, kidney dysfunction or cardiac complications due to low calcium levels (hypocalcemia).
Poison by intraperitoneal route experimental teratogenic and reproductive effects.
Mutation data reported a general-purpose chelaung and complexing agent when heated to decomposition it emits toxic fumes of NOx.
Ethylenediamine tetraacetic acid and edetates are widely used in topical, oral, and parenteral pharmaceutical formulations.
They are also extensively used in cosmetics and food products.
Ethylenediamine tetraacetic acid is generally regarded as an essentially nontoxic and nonirritant material, although it has been associated with doserelated bronchoconstriction when used as a preservative in nebulizer solutions.
Ethylenediamine tetraacetic acid has therefore been recommended that nebulizer solutions for bronchodilation should not contain edetic acid.
Edetates, particularly Ethylenediamine tetraacetic acid and edetate calcium disodium, are used in a greater number and variety of pharmaceutical formulations than the free acid.
Disodium edetate, trisodium edetate, and edetic acid readily chelate calcium and can, in large doses, cause calcium depletion (hypocalcemia) if used over an extended period or if administered too rapidly by intravenous infusion.
If used in preparations for the mouth, they can also leach calcium from the teeth.
In contrast, Ethylenediamine tetraacetic acid does not chelate calcium.
Ethylenediamine tetraacetic acid is nephrotoxic and should be used with caution in patients with renal impairment.
