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| EGTA | |
|---|---|
| Name | EGTA |
| IUPAC name | 2,2′,2′′,2′′′-(ethane-1,2-diyldiimino)tetraacetic acid |
| Other names | Ethylene glycol-bis(β-aminoethyl ether)-N,N,N',N'-tetraacetic acid |
| Formula | C14H20N2O10 |
| Molar mass | 380.31 g·mol−1 |
| Appearance | white crystalline powder |
| Solubility | soluble in water |
EGTA is a synthetic aminopolycarboxylic acid used primarily as a selective calcium chelator in biochemical, physiological, and industrial contexts. Developed alongside related ligands, EGTA is notable for its high affinity for calcium relative to magnesium, enabling controlled modulation of divalent cation concentrations in studies ranging from Electrophysiology to Signal transduction. Widely employed in biochemistry laboratories, EGTA interfaces with techniques and institutions across contemporary life sciences.
EGTA is a tetracarboxylate derivative of an ethylenediamine backbone bearing two ether-linked ethanol arms; its systematic name is 2,2′,2′′,2′′′-(ethane-1,2-diyldiimino)tetraacetic acid. The molecule contains four carboxylate groups and two tertiary amine centers, producing multiple protonation states that depend on pH and ionic strength; pKa values are typically reported in the context of buffers employed in Physiology and Biochemistry protocols. EGTA forms octa- or heptadentate coordination geometries with divalent cations, giving rise to thermodynamic stability constants used in calculations similar to those for EDTA and BAPTA. Physical properties such as aqueous solubility and UV absorbance influence its use in assays conducted in facilities like university laboratories and research centers associated with institutions such as Harvard University, Max Planck Society, and National Institutes of Health.
Commercial EGTA is produced via multistep organic syntheses beginning from Ethylenediamine and haloacetic acid derivatives or glycols under controlled conditions. Methods include alkylation of amine precursors, ether formation with Ethylene oxide or substituted alcohols, and subsequent carboxymethylation to install the tetraacetic acid moieties; reactions are carried out in industrial and academic settings comparable to synthesis routes for other chelators used by companies such as Sigma-Aldrich and industrial chemistry groups at BASF or Dow Chemical Company. Purification strategies employ recrystallization, ion-exchange chromatography, and quality control by NMR, MS, and HPLC—techniques common at laboratories affiliated with centers like Lawrence Berkeley National Laboratory and European Molecular Biology Laboratory.
EGTA chelation relies on electron donation from carboxylate oxygens and tertiary amine nitrogens to coordinate divalent cations; binding equilibria are governed by coordination number, ionic radius, and hydration energy. Thermodynamic selectivity favors Ca2+ over Mg2+ due to the larger ionic radius and lower dehydration penalty of Ca2+, paralleling selectivity considerations in natural chelators such as Calmodulin and synthetic ligands like BAPTA. Binding constants (log K) are used in computational models alongside variables from standards like the IUPAC and tabulations from groups including NIST to predict free ion concentrations in buffered systems used in experiments at institutions like Cold Spring Harbor Laboratory and Salk Institute.
EGTA is used to buffer free Ca2+ in experiments spanning patch-clamp electrophysiology, Calcium imaging, Muscle physiology, and studies of Synaptic transmission. It appears in protocols for isolating organelles in cell biology studies conducted at centers such as Johns Hopkins University and University of Cambridge, and in biochemical assays probing enzymes like Protein kinase C and Calpain. EGTA is favored where discrimination between Ca2+ and Mg2+ is required, complementing other reagents including EDTA, EGTA-AM derivatives for cell-permeant delivery, and calcium indicators like Fura-2 and Fluo-4. EGTA is also employed in industrial water treatment scenarios and materials research conducted in collaboration with laboratories at MIT and Caltech.
As a chelating agent, EGTA perturbs cellular Ca2+ homeostasis and can inhibit Ca2+-dependent processes such as Muscle contraction, Neurotransmitter release, and Exocytosis. In vitro exposure is routinely controlled; in vivo uses are limited and require oversight by institutional review boards and animal care committees like those at Wellcome Trust–funded facilities and NIH-funded programs. Safety data sheets advise standard precautions—eye and skin protection, ventilation, and proper disposal—consistent with chemical hygiene practices followed at research institutions including University of California, San Francisco and Yale University. Toxicology assessments draw on studies published in journals associated with publishers like Nature Publishing Group and Elsevier.
EGTA released to the environment undergoes dilution, biodegradation, and complexation with metal ions; persistence and mobility depend on local conditions monitored by agencies such as the Environmental Protection Agency and the European Chemicals Agency. Because EGTA can mobilize heavy metals, its environmental management is addressed in regulatory frameworks and guidance documents used by industrial partners including WHO-aligned programs and regional authorities in the European Union and United States. Disposal and wastewater treatment practices follow standards from organizations like OECD and waste management protocols at municipal facilities and research campuses.
Category:Chelating agents Category:Organic compounds