EDTA Disodium Dihydrate, (EDTA-2Na)

Description

Quick Detail:
Ethylenediaminetetraacetic acid (EDTA) is a chelating agent produced as a series of salts. A chelating agent is a material that tightly binds or captures metal ions.
Salts of EDTA are typically sold as an aqueous solution for controlling / binding metal ions over a broad pH range in aqueous (water-based) systems.2 Salts of EDTA typically exist as a light amber liquid and some have a slight amine odor. Some salts are sold as dry powders.
Occupational exposure is dependent upon the conditions under which salts of EDTA are used. Under fire conditions, salts of EDTA can decompose and the smoke may contain toxic and/or irritating compounds.
Based on currently available information, there is no indication of harmful effects of EDTA due to long-term exposure to low concentrations found in the environment.
Description:
EDTA is an aminopolycarboxylic salt. The various salts of EDTA typically exist as clear to amber liquids. Some have a slight amine odor. They can be used as chelating agents over a broad pH range in aqueous systems. Some salts are produced as dry powders and crystals. These salts are water soluble, but insoluble in acid and organic liquids
Chelating agents bind or capture trace amounts of iron, copper, manganese, calcium and other metals that occur naturally in many materials. Such naturally occurring metals can cause foods to degrade, chemical degradation, discoloration, scaling, instability, rancidity, ineffective cleaning performance and other problems
Applications:
1) Agriculture – to stabilize formulations and to provide micronutrients to fertilizers
2) Cleaning products – to remove hard water scale, soap film, and inorganic scales in a wide variety of cleaning products and formulations, including hard surface cleaners, institutional cleaners, laundry detergents, liquid soaps, germicidal and anti-bacterial cleansing preparations, and vehicle cleaners
3) Metalworking – for surface preparation, metal cleaning, metal plating, and in metalworking fluids
4) Oil field applications – in the drilling, production, and recovery of oil
5) Personal care products – to increase effectiveness and improve stability of bar and solid soaps; bath preparations; creams, oils, and ointments; hair preparations, shampoos and almost every type of personal care formulation
6) Polymerization – for suspension, emulsion, and solution polymers, both in polymerization reactions and for finished polymer stabilization
7) Photography – as a bleach in photographic film processing
8) Pulp and paper – to maximize bleaching efficiency during pulping, prevent brightness reversion, and protect bleach potency
9) Scale removal and prevention – to clean calcium and other types of scale from boilers, evaporators, heat exchangers, filter cloths, and glass-lined kettles
*0) Textiles – in all phases of textile processing, particularly the scouring, dyeing and color stripping stages
*1) Water treatment – to control water hardness and scale-forming calcium and magnesium ions; to prevent scale formation
*2) Consumer products – in food and pharmaceutical applications
Specifications:
CAS Number: ********6
Chemical Formula: C*0H*4N2NA2O8. 2H2O
Molecular Weight: **2.*4
Appearance: white crystalline powder
Assay: *9% min.
PH value (1% water solution): 4~6
Chelate value(CaCO3mg/g): **0
Iron [Fe]: 0.*1% max.
Heavy metals [Pb]: 0.**5% max.
 
Competitive Advantage:
Metal chelation is important because it makes metal ions more available for uptake by plants. Positively charged metal ions, such as Zn, Mn, Cu and Fe, readily react with negatively charged hydroxide ions (OH-), making them unavailable to plants. OH- ions are abundant in alkaline or neutral soils and soil-less medias.
The ligand coats the metal ion, protecting it from the surrounding OH- ions. The complex can then be easily absorbed by the plant, where it is being degraded and consumed as micronutrients.
The strength of the chemical bond between the ligand and the metal ion depends on the type of ligand, the type of ion and the pH. The stronger the bond, the more stable the metallic ion and each chelate has a characteristic "stability diagram".
 
Here are examples for stability diagrams for a Copper chelate and a Zinc chelate. It is obvious that in specific pH levels, the complexes are not stable, i.e. the ligand tends to separate from the metal ion.