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탄산칼슘 구조식 이미지
카스 번호:
Calcium carbonate
포뮬러 무게:
MOL 파일:

탄산칼슘 속성

825 °C
끓는 점
800 °C
2.93 g/mL at 25 °C(lit.)
저장 조건
Store at RT.
5 M HCl: 0.1 M at 20 °C, clear, colorless
물리적 상태
random crystals
White-beige to slightly beige-gray
Specific Gravity
9.5-10.5 (100g/l, H2O, 20℃)(slurry)
최대 파장(λmax)
λ: 260 nm Amax: ≤0.09
λ: 280 nm Amax: ≤0.06
Solubility Product Constant (Ksp)
pKsp: 8.54
Stable. Incompatible with acids, fluorine, ammonium salts, alum.
CAS 데이터베이스
471-34-1(CAS DataBase Reference)
Carbonic acid calcium salt (1:1)(471-34-1)


위험품 표기 Xi
위험 카페고리 넘버 37/38-41-36/38-36
안전지침서 26-36/37/39-37/39-37
WGK 독일 -
RTECS 번호 FF9335000
HS 번호 28365000
유해 물질 데이터 471-34-1(Hazardous Substances Data)
독성 LD50 orally in Rabbit: 6450 mg/kg LD50 dermal Rat > 2000 mg/kg

탄산칼슘 MSDS


탄산칼슘 C화학적 특성, 용도, 생산


칼슘의 탄산염이다. 화학식은 CaCO3. 상온에서 흰색의 고체. 산을 만나면 이산화탄소를 내놓으면서 반응한다든가, 열을 가하면 이산화탄소를 내놓으면서 산화물로 분해되는 점 등 일반적인 탄산염의 특성을 갖고 있다.매우 흔하게 볼 수 있는 성분이다. 각종 암석에 흔하게 들어 있고, 생명체에서도 흔히 볼 수 있다. 방해석이나 아라고나이트는 순수한 탄산칼슘으로 이루어졌고, 석회석, 백악, 대리석 등에도 탄산칼슘이 많다.


탄산칼슘은 값도 싸고 무게도 가벼워서 이런 저런 용도로 널리 쓰인다. 건축재료로 많이 사용된다. 도로를 까는 데 쓰이는 아스팔트에 충진재로서 추가된다. 미세한 가루로 만든 탄산칼슘은 콘크리트의 충진재로 들어간다. 예전에는 탄산칼슘이 많은 석회암을 이용해서 석상 등을 만들기도 했지만, 요즘은 산성비 때문에 석회암을 건축 재료로 직접적으로 사용하지는 않는다. 산성비에 포함된 산이 탄산칼슘을 녹이기 때문이다. 용광로에서 철을 정련할 때 사용된다. 탄산칼슘에서 나온 칼슘 산화물이 철광석의 각종 불순물과 결합해서 찌꺼기로 떨어져 나가기 때문이다. 탈황 처리, 불소 제거에 사용된다. 유리 제조에 사용되어 점도를 조절한다. 타일용 접착제의 주성분이다. 마감용 실런트에도 들어간다. 각종 제품에서 충진재로 사용된다. 제지 공정에서 종이에 첨가된다. 최대 20%를 차지하기도 한다. 페인트나 플라스틱류에도 충진재로 첨가된다. 농업용 석회의 주 성분이다. 비료용은 아니고, 땅이 산성화한 것을 중화시키는 용도의 토양 개선제로 사용된다. 분필의 주재료로도 사용된다. 대표적으로는 문교 탄산칼슘 분필. 탄산칼슘은 의약품이나 식품첨가물로도 사용된다.


석회석 ·대리석으로서 시멘트의 주원료, 산화칼슘의 원료, 제철 ·건축재료 등의 각종 중화제로서 사용된다. 또, 호분은 백색 안료 ·수성도료에, 침강 탄산칼슘은 안료 ·도료 ·치약 등에 사용되며, 고무에도 보강제로서 배합된다.


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
calcium carbonate block

화학적 성질

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.

화학적 성질

Calcium carbonate occurs as an odorless and tasteless white powder or crystals.

물리적 성질

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.

물리적 성질

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.


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.


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.


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.


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.

생산 방법

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.


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.

생산 방법

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.

제조 방법

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.

화학 반응

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


Cal-Sup (3M Pharmaceuticals); Children’s Mylanta Upset Stomach Relief (Johnson & Johnson-Merck Consumer); Chooz (Schering- Plough HealthCare); Mylanta Soothing Lozenges (Johnson & Johnson-Merck Consumer).


Calcium carbonate (CaCO3) is a naturally occurring white solid that is sparingly soluble in water. It is most commonly used to neutralize soil acidity to the required level in a process called liming.
The major sources of calcium carbonate are calcitic limestone, dolomitic limestone, marl, chalk and marble. Calcium carbonate is made by passing carbon dioxide (CO2) into limewater. Pure calcium carbonate is assumed to have a 100% neutralizing value. The values of other liming materials are measured against the neutralizing value of pure calcium carbonate. Calcium carbonate, on heating, decomposes to give calcium oxide (quick lime) and carbon dioxide.
Limestone, which consists mainly of calcium carbonate, is called calcitic limestone or high calcium limestone. Limestone containing more than 10% magnesium carbonate is called dolomitic limestone or dolomite. These forms contain about 12% magnesium. Agricultural dolomitic limestone is a fine, grey to white powder of a double carbonate of calcium and magnesium with 12.8% magnesium and 17% calcium. The double carbonate is much less soluble in water than the individual carbonates.

Pharmaceutical Applications

Calcium carbonate, employed as a pharmaceutical excipient, is mainly used in solid-dosage forms as a diluent. It is also used as a base for medicated dental preparations, as a buffering agent, and as a dissolution aid in dispersible tablets. Calcium carbonate is used as a bulking agent in tablet sugar-coating processes and as an opacifier in tablet film-coating.
Calcium carbonate is also used as a food additive and therapeutically as an antacid and calcium supplement.

Pharmaceutical Applications

Calcium carbonate (CaCO3) can be found in clinical applications such as antacids, but not that an excessive intake can be hazardous.
A variety of calcium salts are used for clinical application, including calcium carbonate, calcium chloride, calcium phosphate, calcium lactate, calcium aspartate and calcium gluconate. Calcium carbonate is the most common and least expensive calcium supplement. It can be difficult to digest and may cause gas in some people because of the reaction of stomach HCl with the carbonate and the subsequent production of CO2.
Calcium carbonate is recommended to be taken with food, and the absorption rate in the intestine depends on the pH levels. Taking magnesium salts with it can help prevent constipation. Calcium carbonate consists of 40% Ca2+, which means that 1000 mg of the salt contains around 400 mg of Ca2+. Often, labels will only indicate the amount of Ca2+ present in each tablet and not the amount of calcium carbonate.


Calcium carbonate is mainly used in oral pharmaceutical formulations and is generally regarded as a nontoxic material. However, calcium carbonate administered orally may cause constipation and flatulence. Consumption of large quantities (4–60 g daily) may also result in hypercalcemia or renal impairment. Therapeutically, oral doses of up to about 1.5 g are employed as an antacid. In the treatment of hyperphosphatemia in patients with chronic renal failure, oral daily doses of 2.5–17 g have been used. Calcium carbonate may interfere with the absorption of other drugs from the gastrointestinal tract if administered concomitantly.
LD50 (rat, oral): 6.45 g/kg


Calcium carbonate is stable and should be stored in a well-closed container in a cool, dry place.

비 호환성

Incompatible with acids and ammonium salts.

Regulatory Status

GRAS listed. Accepted for use as a food additive in Europe. Included in the FDA Inactive Ingredients Database (buccal chewing gum, oral capsules and tablets; otic solutions; respiratory inhalation solutions). Included in nonparenteral medicines licensed in the UK. Included in the Canadian List of Acceptable Non-medicinal Ingredients.

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