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EDTA

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EDTA
EDTA
Chemical name EDTA
Other names EDTA
H4EDTA
Diaminoethanetetraacetic acid
Edetic acid
Edetate
Ethylenedinitrilotetraacetic acid
Versene
Chemical formula C10H16N2O8
Molecular mass 292.25 g/mol
CAS number [60-00-4]
Density 0.86 g/cm³
Melting point 237-245 °C (dec.)
SMILES OC(CN(CC(O)=O)C-

CN(CC(O)=O)CC(O)=O)=O

Hazards
MSDS External MSDS
Main hazards irritant
R/S statement R: 36
S: 26
RTECS number AH4025000
Disclaimer and references

EDTA is the acronym for the chemical compound ethylenediaminetetraacetic acid.

EDTA refers to the chelating agent that is widely used to sequester di- and trivalent metal ions such as magnesium ion in molecular biology.

EDTA features four carboxylic acid and two amine groups that can all bind to metals. EDTA forms specially strong complexes with Mn(II), Cu(II), Fe(III), and Co(III).[1]

Contents

Popular vs. chemical nomenclature

To describe EDTA and its various protonated forms, chemists use a more cumbersome but more precise acronym that distinguishes between EDTA4−, the conjugate base that is the ligand, and H4EDTA, the precursor to that ligand.

Coordination chemistry principles

In coordination chemistry, H4EDTA is a member of the aminocarboxylate family of ligands that includes imidodiacetic acid ("H2IDA") and nitrilotriacetic acid ("H3NTA"). More specialized relatives include N,N'-ethylenediaminediacetic acid ("H2EDDA") and 1,2-diaminocyclohexane-N,N,N',N'-tetraacetic acid ("H4CyDTA"). These ligands are all formally derived from the amino acid glycine.

H4EDTA forms highly stable coordination compounds that are soluble in water. In these complexes, the ligand is usually either hexa- or pentadentate, EDTA4− or HEDTA3−, respectively. Such complexes are chiral, and [Co(EDTA)] has been resolved into enantiomers.[2]

Metal-EDTA chelate
Metal-EDTA chelate

Research Applications of EDTA

In research and the laboratory, EDTA is also used for:

  • Scavenging metal ions such as magnesium (Mg).

In biochemistry and molecular biology, ion depletion is commonly used to inactivate metal-dependent enzymes such as DNAses and Proteases that can damage and degrate DNA or proteins respectively.

  • EDTA is used often in medical and laboratory equipment as an anticoagulant.

0.5 M EDTA Buffer Recipe Preparation

To make 0.5 M EDTA pH 8.0, you must mix the following.

For 1 liter add:

  • 186.1 g Na2EDTA.2H2O
  • 800 ml Milli-Q H2O

Adjust the pH to 8 with NaOH pellets (you will need about about 20 g) or NaOH solution.

The reason to adjust the pH is that the EDTA will not dissolve until the pH is about 8. Bring volume up to 1 L with double distilled water (ddH2O), put in vessel or container, and autoclave.

References

  1. Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  2. Kirchner, S. Barium (Ethylenediaminetetracetato) Cobalt(III) 4-Hydrate" Inorganic Syntheses, McGraw-Hill: New York, 1957; Vol. 5, pages 186-188.



See also

de:Ethylendiamintetraessigsäure es:EDTA fr:EDTA it:Acido etilendiamminotetraacetico he:EDTA nl:Ethyleendiaminetetra-acetaat ja:エチレンジアミン四酢酸 pl:EDTA pt:EDTA ru:Этилендиаминтетрауксусная кислота sv:EDTA zh:乙二胺四乙酸

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