Disodium EDTA-Copper ●
TL;DR. This ingredient is primarily a chelating and metal-complexing agent, used to bind free metal ions and help stabilize formulas against discoloration, odor shift, and oxidation. It may also contribute a trace-metal conditioning or color-related role depending on the product type.
What does Disodium EDTA-Copper do in a cosmetic formula?
This ingredient is primarily a chelating and metal-complexing agent, used to bind free metal ions and help stabilize formulas against discoloration, odor shift, and oxidation. It may also contribute a trace-metal conditioning or color-related role depending on the product type.
Is Disodium EDTA-Copper clean?
From a clean-beauty perspective, it has friction because its aminopolycarboxylate chelator backbone is commonly restricted by stricter retailer and brand standards due to poor biodegradation and aquatic persistence concerns. Skin irritation at typical cosmetic levels is usually low, so the concern is more environmental and standards-based than routine topical tolerance.
Is Disodium EDTA-Copper sustainable?
It is typically synthetic and derived from petrochemical feedstocks, with the metal component supplied through conventional mineral supply chains. The chelator portion is not readily biodegradable and can remain active in wastewater, where it may increase mobility of metals.
Is Disodium EDTA-Copper COSMOS-approved?
It is not permitted under COSMOS-natural or COSMOS-organic because this class of persistent synthetic chelators does not fit the standard’s allowed chemistry. Its fit with Green Chemistry is weak, mainly due to nonrenewable feedstocks, limited biodegradability, and persistence after use.
How does Disodium EDTA-Copper work chemically?
The molecule is a coordination complex in which a hexadentate aminopolycarboxylate ligand wraps a divalent transition-metal ion, with alkali counterions improving water compatibility. Typical use levels are low, often around 0.01 to 0.2% for stabilization, and performance is strongest in water-based systems where pH keeps the carboxylate groups ionized and available for metal binding.
Last updated 2026-05-13