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Views: 0 Author: Site Editor Publish Time: 2026-08-06 Origin: Site
Ferrous carbonate — systematically named iron(II) carbonate with the chemical formula FeCO₃ — is an inorganic compound in which iron exists in its +2 oxidation state paired with a carbonate anion. It occurs naturally as the mineral siderite and is also produced synthetically for a wide range of industrial applications.
Unlike more common iron oxides (hematite Fe₂O₃, magnetite Fe₃O₄), ferrous carbonate is valued for its unique decomposition behavior, reactivity in acidic environments, and role as a precursor in the synthesis of other iron-based materials. It appears as a grayish-white to pale green-brown powder and is poorly soluble in water, which makes it suitable for controlled-release applications in industrial processes.
Key identifiers:
Property | Value |
Chemical formula | FeCO₃ |
CAS Number | 563-71-3 |
Molar mass | 115.85 g/mol |
Appearance | Gray-white to pale green-brown powder |
Density | 3.94 g/cm³ |
Solubility in water | 0.0067 g/100 mL (practically insoluble) |
Decomposition temperature | ~200 °C (decomposes to FeO + CO₂) |
Crystal structure | Trigonal (calcite-type) |
Ferrous carbonate serves diverse roles across multiple industrial sectors. Below is a comprehensive overview of its key non-medical applications.
1.Iron and Steel Production
Application | Description |
Direct-reduction feedstock | Siderite ore reduced with H₂ to produce sponge iron for electric arc furnaces |
Sinter feed additive | Blended with higher-grade ores to adjust burden chemistry in blast furnaces |
Green steel R&D | Hydrogen-based direct reduction of FeCO₃ as a low-carbon steelmaking pathway |
Ferrous carbonate is employed in industrial wastewater treatment as a source of ferrous ions. In moderately acidic conditions, it dissolves gradually, releasing Fe²⁺ that can:
● Precipitate phosphates and heavy metals through co-precipitation
● Act as a reducing agent for hexavalent chromium (Cr⁶⁺ → Cr³⁺) remediation
● Serve as a controlled iron source in Fenton-like advanced oxidation processes for organic pollutant degradation
Its low solubility provides a slow-release mechanism that avoids the rapid pH drop and overdosing risks associated with ferrous sulfate or ferrous chloride.
One of the earliest documented non-metallurgical uses of ferrous carbonate is in ceramics, where it serves as an iron source for coloration and magnetic property engineering.
Key applications in ceramics:
Ferrite manufacturing
● : US Patent US4657752A specifically describes ferrous carbonate as a precursor for iron ions in ceramics used in
computer memory cores
(soft magnetic ferrites)
Glaze colorant
● : When thermally decomposed in a glaze matrix, FeCO₃ yields iron oxides that produce a spectrum of colors — from celadon greens and amber browns in reduction firing to rust reds in oxidation — depending on kiln atmosphere and concentration
Clay body additive
● : Added to clay bodies to produce speckled or iron-rich effects in stoneware and brick
Glaze Atmosphere | FeCO₃-Derived Color Range |
Oxidation (electric kiln) | Amber, tan, rust, dark brown |
Reduction (gas/wood kiln) | Celadon green, blue-green, iron-red (high concentration) |
Salt/soda firing | Orange-peel browns with flashing effects |
Ferrous carbonate functions as an inorganic flame retardant in polymer formulations. Its flame-retardant mechanism is dual-action:
Endothermic decomposition: At approximately 200 °C, FeCO₃ absorbs heat as it decomposes, cooling the polymer matrix below its ignition threshold
CO₂ release: The evolved carbon dioxide dilutes flammable gases in the combustion zone and displaces oxygen
Unlike halogenated flame retardants, FeCO₃ produces low smoke and no toxic halogen gases during decomposition, making it attractive for applications where smoke toxicity is a concern — such as construction materials, transportation components, and electrical enclosures.
In the agricultural sector, ferrous carbonate is used as an iron source in animal feed premixes for livestock, poultry, and aquaculture. It provides bioavailable iron for:
● Hemoglobin synthesis in swine, cattle, and poultry
● Preventing iron-deficiency conditions in piglets
● Supporting growth rates in intensive farming operations
The carbonate form is preferred in certain formulations because its low solubility in neutral pH reduces unwanted oxidation of vitamins and other sensitive feed components during storage — unlike highly soluble ferrous sulfate, which can accelerate rancidity.
Note: This is an agricultural/feed application, distinct from human pharmaceutical use.
Thermally processed ferrous carbonate yields iron oxide pigments used in:
Construction materials: Coloring concrete pavers, roofing tiles, and architectural masonry
Coatings: Industrial paints, wood stains, and anti-corrosion primers
Plastics: Masterbatch colorants for PVC, polyethylene, and polypropylene
The key advantage of using FeCO₃ as a pigment precursor is that its decomposition can be controlled to produce specific iron oxide phases (red α-Fe₂O₃, black Fe₃O₄, or brown γ-Fe₂O₃) by adjusting calcination temperature and atmosphere.
Ferrous carbonate (FeCO₃) contains iron in the +2 oxidation state and is stable as a solid. Ferric carbonate (Fe₂(CO₃)₃), containing Fe³⁺, does not exist as a stable solid — attempts to prepare it from aqueous Fe³⁺ and carbonate ions invariably yield iron(III) hydroxide/oxide instead, due to the strong acidity of the Fe³⁺ ion in water.
Partially. FeCO₃ is typically not used directly as a pigment but rather as a precursor that is calcined (heated in air) to produce iron oxide pigments. The calcination temperature and atmosphere determine whether red (Fe₂O₃), black (Fe₃O₄), or brown (mixed-phase) pigments are obtained.
Pure FeCO₃ is paramagnetic at room temperature (weakly attracted to a magnetic field). It does not exhibit the strong ferromagnetism of magnetite (Fe₃O₄) or metallic iron. When thermally decomposed to Fe₃O₄ through controlled calcination, the resulting product becomes ferromagnetic.
As a slow-release iron source, FeCO₃ dissolves gradually in mildly acidic wastewater, providing Fe²⁺ ions for phosphate precipitation, heavy metal removal, and as a reductant for contaminants like hexavalent chromium. Its advantage over ferrous sulfate is the absence of sulfate ion addition and more controlled iron dosing.
Exact production figures are not aggregated across all forms (synthetic FeCO₃ vs. siderite ore). Siderite mining for iron ore runs in the millions of metric tons annually (concentrated in China), while synthetic ferrous carbonate production for chemical/industrial applications is estimated at several thousand to tens of thousands of metric tons per year globally.
Under most regulatory frameworks (USDOT, IMDG, IATA), technical-grade ferrous carbonate is not classified as dangerous goods for transport. Standard shipping practices apply, with the primary requirement being protection from moisture.
