What is the Calcium carbonate?

Calcium carbonate is White powder, while it's Molecular Formula is CaCO3. White powder Made by adding soluble carbonate to a calcium salt solution.The white powder or crystals are soluble in acid but not in water.Calcium carbonate was used to neutralize gold toning baths andas a fine abrasive added to water and alcohol for cleaning glassplates before they were coated with photographic binders.

What is the CAS number for Calcium carbonate?

The CAS number of Calcium carbonate is 471-34-1.

What is Calcium carbonate (471-34-1) used for?

Calcium carbonate occurs in nature as limestone in various forms, such as marble, chalk, and coral. It is probably the most widely-used raw material in the chemical industry. It has numerous applications, primarily to produce cement, mortars, plasters, refractories, and glass as building materials. It also is used to produce quicklime, hydrated lime and a number of calcium compounds. It is produced either as powdered or precipitated calcium carbonate. The latter consists of finer particles of greater purity and more uniform size. They also have many important commercial applications. Various grades of precipitated calcium carbonate are used in several products, such as textiles, papers, paints, plastics, adhesives, sealants, and cosmetics.calcium carbonate blockInChI:InChI=1/CH2O3.Ca.2H/c2-1(3)4;;;/h(H2,2,3,4);;;/p-2/rCH2O3.CaH2/c2-1(3)4;/h(H2,2,3,4);1H2/p-2

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Calcium carbonate

Product Name: Calcium carbonate
CasNo: 471-34-1
Purity:
Appearance: White powder

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CasNo： 471-34-1

Molecular Formula： CaCO₃

Appearance： White powder

Offer Chemical Raw Material Calcium carbonate 471-34-1 In Stock

Molecular Formula:CaCO3
Molecular Weight:100.09
Appearance/Colour:White powder
Melting Point:825 °C
Refractive Index:1.6583
Boiling Point:333.6oC at 760mmHg
Flash Point:197oC
PSA：63.19000
Density:2.93 g/mL at 25 °C(lit.)
LogP:-2.44700

Calcium carbonate(Cas 471-34-1) Usage

Description	Calcium carbonate (CaCO3) is a naturally occurring compound found in limestone, marble, and chalk. It’s produced mainly through the calcination of limestone to yield calcium oxide (CaO), which is then carbonated by adding CO2. This process can be controlled to achieve specific crystal sizes for various applications. Calcium carbonate is widely used in industries such as agriculture for soil neutralization, in pharmaceuticals as an antacid, and as a filler in products like paper and plastics. Additionally, its polymorphs, including calcite and aragonite, exhibit different properties suitable for diverse applications, from biomaterials to targeted drug delivery systems.
Industrial Applications	An essential component of cement and concrete, and used as a limestone aggregate in construction. Used in the production of paper, plastics, rubber, paints, and coatings to improve texture and whiteness.
Agricultural Uses	Used to neutralize soil acidity (liming) and improve soil structure.
Pharmaceutical Applications	A dietary supplement for preventing or treating calcium deficiency. Commonly used to relieve heartburn and indigestion.
Food Industry	Acts as a calcium fortifier and is used as a preservative or colorant (E170).
Environmental Applications	Used to soften water and remove impurities.

InChI:InChI=1/CH2O3.Ca.2H/c2-1(3)4;;;/h(H2,2,3,4);;;/p-2/rCH2O3.CaH2/c2-1(3)4;/h(H2,2,3,4);1H2/p-2

471-34-1 Relevant articles

The formation and transformation mechanism of calcium carbonate in water

Takeshi Ogino , Toshio Suzuki , Kiyoshi Sawada

, Geochimica et Cosmochimica Acta Volume 51, Issue 10 , October 1987, Pages 2757-2767

Highly supersaturated solutions of Ca2+ and CO2−3 ions rapidly precipitate amorphous calcium carbonate, ACC, the logarithmic thermodynamic solubility product of which is about −6.0 at 25°C. The ACC initially formed is transformed to a mixture of several crystalline calcium carbonate polymorphs within several minutes.

The mechanism of the thermal decomposition of calcium carbonate

A.W.D. Hills

, Chemical Engineering Science Volume 23, Issue 4 , June 1968, Pages 297-320

The decomposition of single sintered spheres of calcium carbonate has been investigated using a thermo-balance, modified to allow the simultaneous measurement of the temperature and weight of a decomposing sample. It has been shown that the decomposition reaction takes place on a definite boundary between the undecomposed carbonate, and the layer of porous lime formed outside it.

A hydrated crystalline calcium carbonate phase: Calcium carbonate hemihydrate

Z Zou, WJEM Habraken, G Matveeva, ACS Jensen

, Critical Reviews in Toxicology Volume 43, 2013 - Issue 4

It is proposed that Mg2+ ions in solution inhibit the dehydration of ACC and control the hydration level of the crystalline phases. The discovery of this hydrated crystalline calcium carbonate phase emphasizes the importance of amorphous precursors and Mg2+ in controlling the crystallization pathways of calcium carbonate.

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