Iron(II) gluconate hydrate comes as a solid, usually greenish-grey in its powder or crystalline form. Chemically, it holds the formula C12H22FeO14·xH2O. As a source of iron, it shows up in food supplements, pharmaceutical tablets, and even as an additive in some livestock feeds. The material comes in different forms—dense powder, solid flakes, crystals, and sometimes as a pressed pellet or tablet. Iron(II) gluconate displays a density close to 1.8 grams per cubic centimeter, though the presence of water in the hydrate influences the exact value. It dissolves in water easily, making it helpful for liquid formulations and solutions needed for clinical or industrial use. Color comes from the iron itself, giving this chemical its recognized tint among common iron supplements. HS Code for international shipping and customs clears as 29181600, directly tying the substance to both global trade standards and chemical identity.
Unlike heavy metals that risk toxicity even at low concentrations, the iron within gluconate hydrate stabilizes due to its organic acid pairing. This chelation process changes things—absorption in the body goes up and causes less stomach upset versus raw iron salts. Its molecular weight ranges (446–482 g/mol) based on hydration level, which matters during production runs and precise dosing calculations. The hydrated form resists caking and lump formation in storage, and the powder flows with minimal dust generation. Iron(II) gluconate hydrate feels slippery under fingertips, almost like talc, but it drops as solid pearls or crystals when humidity in storage exceeds optimal range. Anyone working with large-scale batching quickly notices the sweet metallic smell, a sign of volatility at certain temperatures, which seldom sticks to packaging but can affect neighboring goods during warehousing.
Many pharmaceutical and food brands demand raw iron(II) gluconate that is high-purity, usually above 98%. Particle size has to stay consistent; large flakes and uniform pearls allow better metering in automatic filling machines, but fine powder still works in custom compounding. Density sits in a range, but as water leaves during dehydration, the granules sometimes become harder, leading lab technicians to screen and sift by mesh. Solutions of iron(II) gluconate hydrate keep well in closed containers—dark glass or food-grade plastic shields against UV, which can speed breakdown and lower shelf life. Most labs use distilled water when preparing stock solutions because minerals and chlorine in regular tap water alter solubility and can leave behind precipitate. Manufacturers record lot numbers and weight down to the kilogram, tracking solution volumes accurately down to the liter, especially in large-run liquid fortification.
Handling iron(II) gluconate hydrate feels routine for most operators, but health and safety sheets still matter. Swallowing large doses accidentally or inhaling bulk powder may cause stomach pain or mild irritation, particularly for people with sensitive airways. The substance has no major record of explosive or flammable risk, but fine powder in bulk storage can trigger minor dust clouds—good ventilation and sturdy masks help. Long storage without airtight seals leads to moisture absorption; the material clumps and weighs down bags, sometimes inviting mold on the exterior packaging if conditions stay damp. Old product loses its greenish color, greying out—an easy way to tell it's overdue for restocking. Many plants store iron(II) gluconate hydrate in drum containers off the ground, away from acids, alkalis, or other metals that could react and change its structure. Disposal rarely causes trouble since the compound breaks down with water, but bulk spills should always go for professional recovery, especially if animals or water sources stand nearby.
Pharmaceutical companies rely on iron(II) gluconate hydrate for its gentle absorption and stable nutritional content. Food processors use it in breakfast cereals, fortified cereals, and beverages to boost iron levels without the harsh aftertaste that comes from inorganic salts. Livestock feed manufacturers press iron(II) gluconate hydrate into multinutrient blocks, especially in areas where soil runs iron-poor and animals develop deficiency. Many industrial processes pick iron(II) gluconate hydrate over other chemicals because the product stores well, travels long distances without degradation, and counts as a safer raw material in bulk chemical synthesis. For medical labs, the compound serves as a control in blood and plasma testing due to its reliable molecular structure—nothing in the hydrated compound surprises a trained analyst.
Every iron(II) gluconate hydrate batch starts with iron salts, usually iron(II) sulfate, alongside gluconic acid derived from glucose fermentation. Producers carefully purify each input, since unwanted metals or leftover reactants cut into product quality and hurt downstream manufacturing. Some regions source local sugar beets or cane for the gluconate portion, making the process both renewable and cost-stable. As with most fine chemicals, large producers keep close record of storage temperatures and atmospheric moisture since humid storerooms turn raw crystals to mush, sometimes ruining an entire run. Raw material price swings influence supply, with iron’s cost fluctuating less than high-grade gluconic acid. In the end, economic stability for iron(II) gluconate hydrate pivots on both robust chemical sourcing and careful quality checks at every production step.
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