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1 Gram

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Purity: 95%~99%
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Appearance:White-beige to slightly beige-gray
Application:Active calcium carbonate is mainly used as reinforcing agent for rubber and plastics, which can improve the tensile strength and abrasion resistance of products, and make foaming rubber foam evenly
PackAge:customer demand
ProductionCapacity:10|Kilogram|Week
Storage:Store at RT.
Transportation:by sea or by air

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Calcium carbonate Basic information

Uses

Product Name:	Calcium carbonate
Synonyms:	whiton1500;whiton450;whitonb;whitonh;whitonp10;whitonp30;whitonp50;whitons
CAS:	471-34-1
MF:	CCaO3
MW:	100.0869
EINECS:	207-439-9
Product Categories:	Inorganics;Chemical Synthesis;Analytical Reagents for General Use;C-D, Puriss p.a.;Puriss p.a.;ACS GradeMetal and Ceramic Science;Calcium SaltsChemical Synthesis;Essential Chemicals;Routine Reagents;AlphabeticalChemical Synthesis;Biological Buffers;BioUltra Buffers;API's;Inorganic Bases;ACS Grade;Chemical Synthesis;Essential Chemicals;Inorganic Salts;Materials Science;Metal and Ceramic Science;Research Essentials;Solutions and Reagents;Synthetic Reagents;Food additive;Calcium carbonate ada@tuskwei.com whatsapp;8618031153937;Pharmacopoeial Organics;Pharmacopoeia (USP);Pharmacopoeia A-ZPharmacopoeia (USP);Companion Products and ReagentsChemical Synthesis;-;Inorganic Bases;Insect Platform;Serum-free Media;Synthetic Reagents;CA - CGCertified Reference Materials (CRMs);Alphabetic;Application CRMs;C;Titrimetry;Titrimetry CRMs;TitrimetryAnalytical Standards;Calcium Salts;Metal and Ceramic Science;Salts;metal carbonate;#N/A
Mol File:	471-34-1.mol

Calcium carbonate Chemical Properties

Melting point	825 °C
density	2.93 g/mL at 25 °C(lit.)
refractive index	1.6583
storage temp.	Store at RT.
solubility	5 M HCl: 0.1 M at 20 °C, clear, colorless
form	random crystals
color	White-beige to slightly beige-gray
Specific Gravity	2.93
PH	9.5-10.5 (100g/l, H2O, 20℃)(slurry)
Water Solubility	Insoluble
λmax	λ: 260 nm Amax: ≤0.09 λ: 280 nm Amax: ≤0.06
Merck	14,1657
BRN	8008338
Solubility Product Constant (Ksp)	pKsp: 8.54
Stability:	Stable. Incompatible with acids, fluorine, ammonium salts, alum.
InChIKey	VTYYLEPIZMXCLO-UHFFFAOYSA-L
CAS DataBase Reference	471-34-1(CAS DataBase Reference)
EPA Substance Registry System	Carbonic acid calcium salt (1:1)(471-34-1)

Safety Information

Hazard Codes	Xi
Risk Statements	37/38-41-36/38-36
Safety Statements	26-36/37/39-37/39-37
WGK Germany	-
RTECS	FF9335000
TSCA	Yes
HS Code	28365000
Hazardous Substances Data	471-34-1(Hazardous Substances Data)
Toxicity	LD50 orally in Rabbit: 6450 mg/kg LD50 dermal Rat > 2000 mg/kg

MSDS Information

Provider	Language
Limestone	English
SigmaAldrich	English
ACROS	English
ALFA	English

Calcium carbonate Usage And Synthesis

Uses	Calcium carbonate (CaCO3) can be in the form of an odorless crystal or powder and is one of calcium’s most stable compounds, better known in its natural state as limestone, marble, chalk, calcite, oyster shells, and the minerals marl and travertine. Calcium carbonate is the source of lime and is used as a “filler” for many products, including paints, plastics, and foods (bread), and as an antacid.
Description	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 block
Chemical Properties	Calcium carbonate occurs in two forms—hexagonal crystal known as calcite, and orthorhombic form, aragonite. Calcite decomposes on heating at 825°C, aragonite melts at 1,339°C (at 102.5 atm). Density 2.71 g/cm3 (calcite), 2.83 g/cm3 (aragonite); insoluble in water (15mg/L at 25°C); Ksp 4.8x10–9 ; soluble in dilute mineral acids.
Chemical Properties	Calcium carbonate occurs as an odorless and tasteless white powder or crystals.
Physical properties	Calcium carbonate is a naturally occurring compound found in organisms and throughout the earth’s crust. After quartz, calcium carbonate, primarily in the form of calcite, is the most common mineral found in the crust. Geologically, calcium carbonate exists in several mineral forms: calcite, aragonite, and vaterite. Calcite is the most common calcium carbonate mineral, whereas vaterite is a very rare form. The different mineral forms of calcium carbonate are based on their crystalline structure. The form of calcium carbonate depends on the conditions at its formation such as temperature and pressure.
Physical properties	Calcium carbonate has the molecular formula of CaCO₃and the molecular weight of 100.0924 g/mol. It is a common substance found in rock in all parts of the world, and is the main component of the shells of many marine organisms such as snails and conches. It is the main ingredient in eggshells of birds and pearls obtained from oysters. Calcium carbonate is the active ingredient in “limestone” used as “agricultural lime” and is the principal cause of “hard water” since most subterranean streams used for fresh water come from wells where underground water flows through limestone beds which are eroded due to its passage. Calcium carbonate occurs in nature as limestone in various forms, such as marble, chalk, and coral.
Uses	Humans primarily use calcium carbonate as a primary source of calcium to combat osteoporosis. Most limestone is used today as construction material. In addition to its use as a construction material, calcium carbonate is also used in numerous industrial processes. Two forms commonly used are ground calcium carbonate (gcc) and precipitated calcium carbonate (pcc). Calcium carbonate is used widely in papermaking as filler and coating pigment to whiten paper. Calcium carbonate is used in place of more expensive optical brightening agents in paper and as a fill to replace more expensive wood pulp fiber; it also helps control the pH in an alkaline range. The second most common industrial use of calcium carbonate (after papermaking) representing the largest use of gcc is in the production of plastics. It is used in the production of polyvinyl chloride (PVC), thermoset polyesters, and polyolefins. Calcium carbonate can be used to replace resins that are more expensive. Similar to its use in the paper industry, it is used as an optical brightener and whitening agent. It also is used to increase strength and absorb heat during exothermic processes. Calcium carbonate is also used in the production of polyethylene and polypropylene. It is an additive to paints and coatings for several purposes including particle size distribution, opacity control, weather resistance, pH control, and anticorrosion. Calcium carbonate is used to buff er acidic soils. Calcium carbonate has also been used to mitigate the effects of acid precipitation on water bodies. Another environmental application of calcium carbonate is for gas desulfurization in scrubbers used to reduce sulfur emissions from air pollution sources.
Uses	Calcium Carbonate is the calcium salt of carbonic acid which is used as an anticaking agent and dough strengthener. it is available in varying particle sizes ranging from coarse to fine powder. it is practically insoluble in water and alcohol, but the presence of any ammonium salt or carbon dioxide increases its solubility while the presence of any alkali hydroxide reduces its solubility. it has a ph of 9–9.5. it is the primary source of lime (calcium oxide) which is made by heating limestone in a furnace. calcium carbonate is used as a filler in baking powder, for calcium enrichment, as a mild buffering agent in doughs, as a source of calcium ions in dry mix desserts, and as a neutralizer in antacids. it is also termed limestone.
Uses	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 and as a fine abrasive added to water and alcohol for cleaning glass plates before they were coated with photographic binders.
Uses	Calcium carbonate 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 is also used to produce quicklime, hydrated lime and a number of calcium compounds.
Production Methods	Calcium carbonate is obtained from natural limestone deposits. The purified compound, known as precipitated calcium carbonate, is synthesized from limestone. Limestone is calcined to calcium oxide and carbon dioxide in a kiln. The products are recombined after purification. Calcium oxide is hydrated with water to give a slurry called milk of lime, which is then carbonated by bubbling CO2 through it. The reactions involved in the process are as follows: CaCO3 CaO + CO2 CaO + H2O Ca(OH)2 Ca(OH)2+ CO2→CaCO3+ H2O The crystal sizes required for various commercial applications may be controlled by temperature, pH, concentrations, and mixing rate. Calcium carbonate also may be precipitated by mixing solutions of calcium chloride and sodium carbonate.
Preparation	Calcium carbonate may also be produced by mixing solutions of calcium chloride and sodium carbonate. In some cases, the presence of sodium is objectionable so that the ammonium carbonate salt is preferable.
Production Methods	Calcium carbonate is prepared by double decomposition of calcium chloride and sodium bicarbonate in aqueous solution. Density and fineness are governed by the concentrations of the solutions. Calcium carbonate is also obtained from the naturally occurring minerals aragonite, calcite, and vaterite.
Definition	calcium carbonate: A white solid,CaCO₃, which is only sparingly solublein water. Calcium carbonatedecomposes on heating to give calciumoxide (quicklime) and carbondioxide. It occurs naturally as theminerals calcite (rhombohedral; r.d.2.71) and aragonite (rhombic; r.d.2.93). Rocks containing calcium carbonatedissolve slowly in acidifiedrainwater (containing dissolved CO₂)to cause temporary hardness. In thelaboratory, calcium carbonate is precipitatedfrom limewater by carbondioxide. Calcium carbonate is used inmaking lime (calcium oxide) and isthe main raw material for theSolvay process.
Reactions	Calcium carbonate decomposes to calcium oxide and CO2 on heating. Treatment with dilute mineral acids produces corresponding calcium salts with liberation of CO2: CaCO3+ 2HCl →CaCl2+ H2O + CO2 In the presence of CO2 it dissolves in water with the formation of bicarbonate: CaCO3+ H2O + CO2→Ca2++ 2HCO3 ¯ It is reduced to calcium carbide when heated with coke or anthracite in an electric furnace: 2CaCO3+ 5C→(high temperature)→2CaC2+ 3CO2

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