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Home > Articles > EDTA Full Form: (Ethylenediamine Tetraacetic Acid), Definition, Uses, Acid or Base and Side Effects
Updated on 05th June, 2024 , 7 min read
EDTA Full Form is Ethylenediamine tetraacetic acid. EDTA is a popular chemical that is known by multiple names. It is comprehensively used in medicinal and industrial applications. Ferdinand Munz was the first to synthesize this chemical in 1935. It is a colorless, crystalline, slightly soluble organic molecule utilized in biology and inorganic chemistry. It is a chelating agent. It's also something with a claw-like structure that we use to grab and stick to other molecules. It is a metal ion-binding chemical that contains calcium, magnesium, lead, and iron. It is a polyprotic acid that chelates calcium and other metal ions. It is made up of four carboxylic acid groups and two amine groups with lone-pair electrons. In this article, we will look into the full form of EDTA, its structure, properties, applications, and significance in various fields.
EDTA Full Form in Medical: EDTA stands for Ethylenediamine Tetraacetic Acid. It is a synthetic compound that belongs to the class of polyamino carboxylic acids. EDTA is a chelating agent, which means it can bind with metal ions and form stable complexes. |
EDTA, which stands for Ethylenediaminetetraacetic Acid, is a synthetic organic compound widely used for its chelating properties. It is a complex molecule with the ability to bind to metal ions and form stable complexes. The term "chelate" comes from the Greek word "chele," which means claw, and refers to the way EDTA's structure wraps around metal ions, resembling a claw-like grasp.
EDTA is a hexadentate ligand, meaning it has six sites in its molecule where it can form bonds with metal ions. These bonds are formed through coordination chemistry, where the electron pairs in EDTA's functional groups form bonds with the metal ions.
EDTA is a weak acid. EDTA (ethylenediamine tetraacetic acid) has four carboxyl and two amine groups and can act as an electron donor or a Lewis base. EDTA is a hexadentate ligand because it can theoretically give six lone pairs of electrons to metal cations to create coordinate covalent connections.
EDTA has a complex molecular structure that contributes to its unique properties. Its chemical formula is C10H16N2O8, and it consists of four carboxylic acid groups and two amine groups, making it an octadentate ligand. The structure allows EDTA to form strong coordination complexes with metal ions through its lone pair electrons.
EDTA, a prescribed pharmaceutical, finds its way into the body through intramuscular or intravenous routes. Consequently, several applications can be categorized for both intravenous and intramuscular uses:
It is an artificially produced compound extensively utilized in the medical field both as an anticoagulant and a chelating agent. Similar to any pharmaceutical, EDTA has the potential to induce adverse reactions in certain individuals. The nature of EDTA's side effects can be influenced by factors such as dosage, frequency of administration, and the individual's overall health condition.
Several commonly encountered side effects associated with this chemical include:
Furthermore, there are certain infrequent side effects linked to EDTA, encompassing:
It's important to note that the manifestation of these side effects can vary depending on individual responses to EDTA, making it crucial for medical practitioners to consider these factors while prescribing and administering the compound.
Ferdinand Münz] initially characterized the chemical in 1935, after preparing it from ethylenediamine and chloroacetic acid.[25] Today, EDTA is primarily made from ethylenediamine (1,2-diaminoethane), formaldehyde, and sodium cyanide.[26] This process produces tetrasodium EDTA, which is then transformed 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 technique is used to create around 80,000 tons of EDTA each year. Impurities produced by this technique include glycine and nitrilotriacetic acid, which result from reactions with the ammonia coproduct.
Chemists distinguish between EDTA4−, the conjugate base that serves as the ligand, and H4EDTA, the precursor of the ligand. At low pH (acidic conditions), the fully protonated H6EDTA2+ form prevails, while at high pH (basic conditions), the fully deprotonated EDTA4− form is found. In this article, the term EDTA is used to mean H4−xEDTAx−, whereas in its complexes EDTA4− stands for the tetraanion ligand.
1.Abiotic degradation: EDTA is so widely used that some have questioned whether it is a persistent organic pollution. While EDTA has many beneficial applications in various industries, pharmaceuticals, and other fields, its long-term use can cause major environmental problems. The breakdown of EDTA is gradual. It primarily grows abiotically in the presence of sunshine.
2.Biodegradation: In many industrial wastewater treatment plants, microbes can eliminate EDTA by up to 80%. The resulting byproducts are ED3A and iminodiacetic acid (IDA), indicating that both the backbone and acetyl groups were attacked. Some microbes have even been discovered to generate nitrates out of EDTA; however, they function optimally at moderately alkaline circumstances of pH 9.0-9.5.
The most sensitive technology for detecting and quantifying EDTA in biological samples is selective reaction monitoring capillary electrophoresis mass spectrometry (SRM-CE/MS), with a detection limit of 7.3 ng/mL in human plasma and a quantitation limit of 15 ng/mL. This approach is effective with sample quantities as tiny as 7-8 nL. HPLC was used to evaluate EDTA levels in non-alcoholic beverages at 2.0 μg/mL.
The possible diseases that can be caused by consuming EDTA are:
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By - Nikita Parmar 2024-09-06 10:59:22 , 6 min readThe full form of EDTA is Ethylenediaminetetraacetic Acid.
EDTA is used in medicine for chelation therapy, treating heavy metal poisoning, and as an anticoagulant in blood collection tubes.
EDTA is water-soluble, pH-sensitive, and can form stable complexes with metal ions, making it useful in various applications.
EDTA's structure allows it to bind with metal ions by forming coordinate covalent bonds, leading to stable complexes.
Common side effects include nausea, vomiting, headache, and dizziness. Rare side effects include asthma, hives, kidney damage, and seizures.
EDTA is used as a preservative to prevent oxidation and color deterioration in food and beverages.
EDTA is essential in complexometric titration, a method to determine metal ion concentrations accurately.
Ethylenediaminetetraacetic acid (EDTA) has been a popular anticoagulant since the early 1950s, and it offers several advantages over other anticoagulants. It prevents clotting by eliminating or chelating calcium from the bloodstream.
Ethylenediaminetetraacetic acid (EDTA) is the full form of EDTA. Formula is [CH2N(CH2CO2H)2]2.
Some persons may experience an allergic reaction to EDTA. It can have manageable to non-manageable side effects.