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Ethylenediaminetetraacetic acid (EDTA), also called EDTA acid, is an aminopolycarboxylic acid with the formula [CH 2 N(CH 2 CO 2 H) 2] 2. This white, slightly water-soluble solid is widely used to bind to iron (Fe 2+ /Fe 3+) and calcium ions (Ca 2+), forming water-soluble complexes even at neutral pH. It is thus used to dissolve Fe- and Ca ...
The prevalence of pseudothrombocytopenia in K2-EDTA reported in different studies ranges from 0.03 to 0.27 percent in outpatients, [3] which accounts for 15 to 30 percent of all cases of isolated thrombocytopenia. Tests can mistake small clumps of platelets for leukocytes, thus showing a pseudoleukocytosis in blood counts. [4] Platelet ...
In addition, test tubes used for laboratory blood tests will have chemicals added to stop blood clotting. Besides heparin, most of these chemicals bind calcium ions, preventing the coagulation proteins from using them. Ethylenediaminetetraacetic acid (EDTA) strongly and irreversibly chelates (binds) calcium ions, preventing blood from clotting.
The test tubes in which blood is collected may contain one or more of several additives. In general, tests requiring whole blood call for blood samples collected in test tubes containing some form of the anticoagulant EDTA. EDTA chelates calcium to prevent clotting. EDTA is preferred for hematology tests because it does minimum damage to cell ...
Tetrasodium EDTA is the salt resulting from the neutralization of ethylenediaminetetraacetic acid with four equivalents of sodium hydroxide (or an equivalent sodium base). It is a white solid that is highly soluble in water. Commercial samples are often hydrated, e.g. Na 4 EDTA. 4H 2 O. The properties of solutions produced from the anhydrous ...
The plastic tube version, known as Vacutainer PLUS, was developed at B-D in the early 1990s by E. Vogler, D. Montgomery and G. Harper amongst others of the Surface Science Group as US patents 5344611, 5326535, 5320812, 5257633 and 5246666. [17] Vacutainers are widely used in phlebotomy in developed countries due to safety and ease of use.
TAE buffer is commonly prepared as a 50× stock solution for laboratory use. A 50× stock solution can be prepared by dissolving 242 g Tris base in water, adding 57.1 ml glacial acetic acid, and 100 ml of 500 mM EDTA (pH 8.0) solution, and bringing the final volume up to 1 litre.
EDTA forms an octahedral complex with most 2+ metal cations, M 2+, in aqueous solution. The main reason that EDTA is used so extensively in the standardization of metal cation solutions is that the formation constant for most metal cation-EDTA complexes is very high, meaning that the equilibrium for the reaction: M 2+ + H 4 Y → MH 2 Y + 2H +