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CAS Number 60-00-4
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Linear Formula (HO2CCH2)2NCH2CH2N(CH2CO2H)2
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Molecular Weight 292.24
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Beilstein Registry Number 1716295
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EC Number 200-449-4
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MDL number MFCD00003541
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PubChem Substance ID 24894713
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eCl@ss 39030907
Synonym: (Ethylenedinitrilo)tetraacetic
acid, EDTA, Edathamil, Ethylenedinitrilotetraacetic acid
Properties
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Related Categories
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Antioxidants and Reducing
Agents for Protein Stabilization,Biochemicals and Reagents, Biological Buffers, Buffers A to Z, Calcium Chelators,
More...
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grade
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anhydrous
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InChI Key
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KCXVZYZYPLLWCC-UHFFFAOYSA-N
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product line
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BioUltra
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assay
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≥99% (titration)
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form
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powder
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mp
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250 °C (dec.)(lit.)
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solubility
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water: soluble0.4 g/L
at 20 °C
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Ethylenediaminetetraacetic
acid (EDTA), also
known by several other names, is a chemical used for both industrial
and medical purposes.
Detailed Description:
It is an aminopolycarboxylic
acid and a
colourless, water-soluble solid. Its conjugate base is ethylenediaminetetraacetate. It is widely used to dissolve limescale. Its usefulness arises because of its
role as a hexadentate ("six-toothed") ligand and chelating agent, i.e., its ability to
"sequester" metal ions such
as Ca2+ and Fe3+. After being bound by EDTA into a metal
complex, metal ions
remain in solution but exhibit diminished reactivity. EDTA is produced as
several salts, notably disodium EDTA and calcium disodium EDTA.
Uses
Industry
In industry, EDTA is mainly used to sequester metal
ions in aqueous solution. In the textile industry, it prevents metal ion
impurities from modifying colors of dyed products. In the pulp and paper
industry, EDTA inhibits the ability of metal ions, especially Mn2+,
from catalyzing 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 stabilizer to prevent
catalytic oxidative decoloration, which is catalyzed by metal ions.[3] In soft drinkscontaining ascorbic acid and sodium benzoate, EDTA mitigates formation
of benzene (a carcinogen).[4]
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 centers tend not to form precipitates or to interfere with
the action of the soaps and detergents. For similar reasons, cleaning
solutions often contain EDTA.
The solubilization of ferric ions, at or below near
neutral pH can be accomplished using EDTA. This property is useful in agricultureincluding hydroponics. However,
given the pH dependence of ligand formation, EDTA is not helpful for improving
Fe solubility in above neutral soils.[5] 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 oxidizing 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 ferric center is reduced to
its ferrous derivative, which can then be reoxidized by air. In similar
manner, nitrogen oxides are
removed from gas streams using [Fe(edta)]2−. The oxidizing
properties of [Fe(edta)]− are also exploited in photography,
where it is used to solubilize silver particles.[6]
EDTA was used in the 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 copper(II) as a retaining ion,
EDTA causes the lanthanides to migrate down the column of resin while
separating into bands of pure lanthanide. The lanthanides elute in order of
decreasing atomic number. Due to the expense of this method, relative to
counter-current solvent extraction, ion-exchange is now used only to obtain the
highest purities of lanthanide (typically greater than 4N, 99.99%).[citation needed]
Medicine
A specific salt of EDTA, known as sodium calcium
edetate, is used to bind metal ions in the practice of chelation therapy, e.g., for treating mercury and lead poisoning.[7] 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 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 (canals shaping) and facilitate
apical advancement of a file in a tight/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 complex [Cr(edta)]− is
administered intravenously and its filtration into the urine is monitored. This
method is useful for evaluating glomerular
filtration rate.[8]
EDTA is used extensively in the analysis of blood. It
is an anticoagulant for
blood samples for CBC/FBEs.
EDTA is a slime dispersant, and has been found to be
highly effective in reducing bacterial growth during implantation of intraocular lenses (IOLs).[9]
Alternative
medicine
Some alternative practitioners believe EDTA acts as an
antioxidant, preventing free radicals from injuring blood vessel walls,
therefore reducing atherosclerosis.[7] These ideas are as yet
unsupported by scientific studies, and seem to contradict some currently
accepted principles.[10] The U.S. FDA has
not approved it for the treatment of atherosclerosis.[11]
Cosmetics
In shampoos, cleaners, and other personal care
products, EDTA salts are used as a sequestering agent to improve their
stability in air.[12]
Laboratory
applications
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 or
proteins.[13] 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 specialized uses in the
biomedical laboratories, 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.[14] EDTA can also be used to test
for bioavailability of heavy metals in sediments. However, EDTA 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.
Packaging details
1 kg in
poly bottle
100, 500
g in poly bottle
PRICES
$229.34/KG OR $104.24/IB
For more information:
mobile: +2348039721941
contact person: emeaba uche
e-mail: emeabau@yahoo.com
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