Copper Citrate stands out in the field of inorganic salts, mainly because its unique combination of copper and citrate ions brings together the stability of a coordinated compound and the reactivity needed in many industries. It takes the form of a solid in ordinary conditions, coming out as pale blue-green flakes, fine powder, or crystalline granules. Someone who works with raw materials on a routine basis will notice the distinct color and faint metallic scent that often hints at its copper content. Unlike common copper salts such as copper sulfate, copper citrate tends to dissolve in water to a lesser degree, but its solubility still supports its use in liquid formulations when agitation increases. The structure relies on copper(II) ions bonded with three citrate molecules—a configuration that influences its physical and chemical behavior. Its HS Code generally falls under 2918.15, a code applied to carboxylic acid derivatives containing inorganic elements, making import and regulatory tracking more predictable for global suppliers.
Copper Citrate is characterized by a molecular formula of C6H5CuO7 and a molecular weight of approximately 293.65 g/mol. In my experience handling chemical samples in a laboratory, observing its appearance reveals a texture that shifts from granular or pearly solid to a smoother, sometimes floury powder after grinding. The density measures in the range of 1.8 to 2.1 g/cm³, reflecting a material that settles well and stores compactly in bulk containers. This density also offers clues on how to handle large shipments and informs the safest stacking practices in a warehouse. Copper citrate remains stable under normal atmospheric conditions, but like many copper-containing chemicals, it oxidizes slowly if left exposed to moisture and air, eventually forming a bluish patina on surfaces. Chemical stability keeps it from decomposing during short-term storage or transport, yet it breaks down in strong acids or bases—a fact any process engineer knows when planning for compatibility in formulations.
A look at the molecular architecture reveals that each copper ion in the citric acid backbone forms bonds through both carboxylate and hydroxyl oxygen atoms. This multi-point attachment gives the compound more resistance against dissociation than other, less tightly coordinated copper salts. For chemists, this means that copper citrate will rarely shed its metal ion in neutral or weakly acidic solutions, though strong acids or intense heat can readily cleave the bonds. Crystalline forms grow with characteristic blue-green luster under a microscope, showing off the ordered arrangement—fascinating evidence of ion pairing that opens up possibilities for imaging or analytical studies. Granular as well as powder forms both retain the same underlying chemistry, letting users switch between them based on their tools without worrying about performance shifts.
The market recognizes copper citrate in multiple forms. Powder dominates in laboratories, with researchers preferring the easy measurement and mixing for analytical or testing needs. Crystalline and pearl forms get picked out by manufacturers who care about consistent dissolution in batch processes—they flow well, limiting clumping that slows industrial production. Dense flakes make sense in settings with frequent manual handling, like crafts or educational kits. These varieties roll out from reactors as solid particles, sometimes compressed or re-processed to reach a particular grain size or density. With a general bulk density falling within 1.9 g/cm³, storage always requires dry, cool spaces to keep hydration and caking at bay, a lesson learned the hard way by anyone who has returned to a poorly kept bag of chemicals.
Handling copper citrate means respect for its dual nature: useful but not entirely benign. While not the most toxic copper compound, it draws attention for being both an irritant and a possible environmental hazard at large concentrations. On skin, direct contact may cause redness or slight itching after prolonged exposure, making gloves a regular companion. Inhalation of dust can irritate the throat or provoke short-term respiratory discomfort, especially in poorly ventilated workspaces—a situation all too familiar in older labs. Ingestion by accident, though unlikely under proper protocols, brings up issues common to most copper salts, such as nausea or mild gastrointestinal upset. From an environmental view, discharge into water supplies or soils runs the risk of disrupting copper-sensitive microorganisms, impacting natural cycles.
Industrial and laboratory users need to watch for the hazards attached to large-scale handling. As a raw material, copper citrate participates in chemical syntheses across biomedical, agricultural, and chemical supply industries, acting as a specialist copper source. Its safety documentation lists it as non-flammable, with only limited reactivity under standard use, but it does react unpredictably with strong oxidizers or concentrated acids, which means any chemical inventory system must place it away from incompatible materials. The safety data extends to proper waste treatment—dilution and neutralization before environmental release, and sealed, labeled containers during disposal routines. With a growing focus on environmental, health, and safety compliance, keeping up with standards from agencies like OSHA or the European Chemicals Agency becomes a matter of daily practice.
Commonly, copper citrate features as a micronutrient in feedstock, dietary supplements, and some plant fertilizers, where its controlled copper release helps address deficiency without the harshness of simpler copper salts. Experienced manufacturers know that the solid, powder, and crystal versions differ slightly in dissolution time, so solutions might involve gentle stirring, moderate heating, or acidification to reach full solubility. In the realm of chemical synthesis, copper citrate’s stability aids in forming complex reagents and catalysts, letting chemists build intricate molecules or trigger reactions at lower temperatures than with metallic copper. From a personal perspective, choosing the right form of copper citrate ensures smoother experiments and more reliable industrial yields—something clear to anyone who’s had to repeat a failed batch.
On the logistics side, the HS Code for copper citrate—usually 2918.15—streams it through customs faster and with less regulatory confusion than less distinct materials. Accurate documentation cuts delays, keeps inventories flowing, and reduces penalties. This is particularly noteworthy in international transactions where missing codes can trigger costly holdups. Knowledge about the code, proper packing, and correct labeling supports both compliance and high safety standards, reflecting the strong need for expertise in every part of the supply chain.
Working with copper citrate means balancing its virtues against its hazards, knowing both its technical profile and how daily routines adapt to handle it safely. Its place in science and manufacturing rests on a dependable set of properties, a versatile chemistry, and responsible stewardship from everyone—from warehouse to laboratory bench. Understanding its specifications, forms, and safe handling rules goes far beyond paperwork; it keeps operations running smoothly and supports the growing culture of safety and compliance in modern industry.
