Silvery Calcium Carbonate CaCO3 Powder For YCOB Crystals , BZT Ceramics

Calcium Carbonate (CaCO₃): For Ca₃(VO₄)₂, YCOB Crystals, BZT Ceramics, CaF₂ Transparent Ceramics

White fine crystalline powder, odorless and tasteless. Exists in amorphous and crystalline forms. Crystalline types include orthorhombic (anhydrous CaCO₃ as colorless orthorhombic crystals) and hexagonal systems (hexahydrate CaCO₃ as colorless monoclinic crystals [10]), presenting as columnar or rhombic shapes with a density of 2.93 g/cm³. Melting point: 1339°C (decomposes at 825–896.6°C); under 10.7 MPa, melts at 1289°C. Slightly soluble in alcohol, soluble in ammonium chloride solution, and nearly insoluble in water.

Our high-purity calcium carbonate is produced using conventional raw materials purified via ion extraction technology to remove impurities. We are currently the only known domestic enterprise capable of mass-producing high-purity calcium carbonate.

Applications

1. For calcium vanadate (Ca₃(VO₄)₂) crystal growth
2. For yttrium calcium oxyborate (YCOB) crystals
3. For barium zirconate titanate (BCZT)-based transparent ceramics
4. For calcium fluoride (CaF₂)-based transparent ceramics
5. For calcium carbonate chewable tablets

Product Series

Health and Safety Information

Packaging Specifications

• Standard packaging: 50 kg/drum, 500 kg/pallet, ton bags
• Sample packaging: 500 g/bag, 1 kg/bottle

About Calcium Carbonate

Calcium carbonate consists of calcium ions and carbonate ions bonded ionically, while the carbonate group is formed by covalent carbon-oxygen bonds. The carbonate group adopts sp² hybridization, with the central carbon atom having three σ orbitals and one p orbital. According to the VSEPR model (AY3 type), its ideal geometry is a planar triangle, with three C-O bonds arranged trigonally. Additionally, it features a 4-orbital, 6-electron p-p π bond.

Chemical Properties

1.Decomposes into calcium oxide and carbon dioxide at 825–896.6°C (industrial CO₂ production):
CaCO₃ → CaO + CO₂↑

2.Reacts with dilute acids (e.g., acetic acid, hydrochloric acid, nitric acid) to effervesce and dissolve, releasing CO₂ (exothermic). Example (laboratory CO₂ production):
CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂↑

3.In water saturated with CO₂, forms soluble calcium bicarbonate. Reacts with carbonic acid (rainwater) similarly. Turbid limewater clears upon CO₂ introduction due to:
CaCO₃ + H₂CO₃ → Ca(HCO₃)₂
or
CaCO₃ + CO₂ + H₂O → Ca(HCO₃)₂

4.Anhydrous CaCO₃ converts to calcite when heated to 1000K.