PRODUCTS

CALCIUM CARBONATE

CAS NO.: 471-34-1
EC/LIST NO.: 207-439-9

Calcium carbonate is a chemical compound with the formula CaCO3.
Calcium carbonate is a common substance found in rocks as the minerals calcite and aragonite (most notably as limestone, which is a type of sedimentary rock consisting mainly of calcite) and is the main component of eggshells, gastropod shells, shellfish skeletons and pearls.
Calcium carbonate is the active ingredient in agricultural lime and is created when calcium ions in hard water react with carbonate ions to create limescale.
Calcium carbonate has medical use as a calcium supplement or as an antacid, but excessive consumption can be hazardous and cause hypercalcemia and digestive issues.

Calcium carbonate shares the typical properties of other carbonates.
Notably it

reacts with acids, releasing carbon dioxide (technically speaking, carbonic acid, but that disintegrates quickly to CO2 and H2O):

CaCO3(s) + 2 H+(aq) → Ca2+(aq) + CO2(g) + H2O(l)

releases carbon dioxide upon heating, called a thermal decomposition reaction, or calcination (to above 840 °C in the case of CaCO3), to form calcium oxide, commonly called quicklime, with reaction enthalpy 178 kJ/mol:

CaCO3(s) → CaO(s) + CO2(g)

Calcium carbonate reacts with water that is saturated with carbon dioxide to form the soluble calcium bicarbonate.

CaCO3(s) + CO2(g) + H2O(l) → Ca(HCO3)2(aq)

This reaction is important in the erosion of carbonate rock, forming caverns, and leads to hard water in many regions.

An unusual form of calcium carbonate is the hexahydrate, ikaite, CaCO3·6H2O.
Ikaite is stable only below 8 °C.

The vast majority of calcium carbonate used in industry is extracted by mining or quarrying.
Pure calcium carbonate (such as for food or pharmaceutical use), can be produced from a pure quarried source (usually marble).

Alternatively, calcium carbonate is prepared from calcium oxide.
Water is added to give calcium hydroxide then carbon dioxide is passed through this solution to precipitate the desired calcium carbonate, referred to in the industry as precipitated calcium carbonate (PCC):

CaO + H2O → Ca(OH)2
Ca(OH)2 + CO2 → CaCO3↓ + H2O

The thermodynamically stable form of CaCO3 under normal conditions is hexagonal β-CaCO3 (the mineral calcite).
Other forms can be prepared, the denser (2.83 g/cm3) orthorhombic λ-CaCO3 (the mineral aragonite) and hexagonal μ-CaCO3, occurring as the mineral vaterite.
The aragonite form can be prepared by precipitation at temperatures above 85 °C; the vaterite form can be prepared by precipitation at 60 °C.
Calcite contains calcium atoms coordinated by six oxygen atoms; in aragonite they are coordinated by nine oxygen atoms.
The vaterite structure is not fully understood.
Magnesium carbonate (MgCO3) has the calcite structure, whereas strontium carbonate and barium carbonate (SrCO3 and BaCO3) adopt the aragonite structure, reflecting their larger ionic radii.

Carbonate is found frequently in geologic settings and constitutes an enormous carbon reservoir.
Calcium carbonate occurs as aragonite, calcite and dolomite as significant constituents of the calcium cycle.
The carbonate minerals form the rock types: limestone, chalk, marble, travertine, tufa, and others.

In warm, clear tropical waters corals are more abundant than towards the poles where the waters are cold.
Calcium carbonate contributors, including plankton (such as coccoliths and planktic foraminifera), coralline algae, sponges, brachiopods, echinoderms, bryozoa and mollusks, are typically found in shallow water environments where sunlight and filterable food are more abundant.
Cold-water carbonates do exist at higher latitudes but have a very slow growth rate.
The calcification processes are changed by ocean acidification.

Where the oceanic crust is subducted under a continental plate sediments will be carried down to warmer zones in the asthenosphere and lithosphere.
Under these conditions calcium carbonate decomposes to produce carbon dioxide which, along with other gases, give rise to explosive volcanic eruptions.

The main use of calcium carbonate is in the construction industry, either as a building material, or limestone aggregate for road building, as an ingredient of cement, or as the starting material for the preparation of builders' lime by burning in a kiln.
However, because of weathering mainly caused by acid rain, calcium carbonate (in limestone form) is no longer used for building purposes on its own, but only as a raw primary substance for building materials.

Calcium carbonate is also used in the purification of iron from iron ore in a blast furnace.
The carbonate is calcined in situ to give calcium oxide, which forms a slag with various impurities present, and separates from the purified iron.

In the oil industry, calcium carbonate is added to drilling fluids as a formation-bridging and filtercake-sealing agent; it is also a weighting material which increases the density of drilling fluids to control the downhole pressure.
Calcium carbonate is added to swimming pools, as a pH corrector for maintaining alkalinity and offsetting the acidic properties of the disinfectant agent.

Calcium carbonate is also used as a raw material in the refining of sugar from sugar beet; it is calcined in a kiln with anthracite to produce calcium oxide and carbon dioxide.
This burnt lime is then slaked in fresh water to produce a calcium hydroxide suspension for the precipitation of impurities in raw juice during carbonatation.

Calcium carbonate in the form of chalk has traditionally been a major component of blackboard chalk.
However, modern manufactured chalk is mostly gypsum, hydrated calcium sulfate CaSO4·2H2O.
Calcium carbonate is a main source for growing biorock.
Precipitated calcium carbonate (PCC), pre-dispersed in slurry form, is a common filler material for latex gloves with the aim of achieving maximum saving in material and production costs.

Fine ground calcium carbonate (GCC) is an essential ingredient in the microporous film used in diapers and some building films, as the pores are nucleated around the calcium carbonate particles during the manufacture of the film by biaxial stretching.
GCC and PCC are used as a filler in paper because they are cheaper than wood fiber.
In terms of market volume, GCC are the most important types of fillers currently used.
Printing and writing paper can contain 10–20% calcium carbonate.
In North America, calcium carbonate has begun to replace kaolin in the production of glossy paper. Europe has been practicing this as alkaline papermaking or acid-free papermaking for some decades.
PCC used for paper filling and paper coatings is precipitated and prepared in a variety of shapes and sizes having characteristic narrow particle size distributions and equivalent spherical diameters of 0.4 to 3 micrometers.

Calcium carbonate is widely used as an extender in paints, in particular matte emulsion paint where typically 30% by weight of the paint is either chalk or marble.
Calcium carbonate is also a popular filler in plastics.
Some typical examples include around 15 to 20% loading of chalk in unplasticized polyvinyl chloride (uPVC) drainpipes, 5% to 15% loading of stearate-coated chalk or marble in uPVC window profile.
PVC cables can use calcium carbonate at loadings of up to 70 phr (parts per hundred parts of resin) to improve mechanical properties (tensile strength and elongation) and electrical properties (volume resistivity).
Polypropylene compounds are often filled with calcium carbonate to increase rigidity, a requirement that becomes important at high usage temperatures.
Here the percentage is often 20–40%. It also routinely used as a filler in thermosetting resins (sheet and bulk molding compounds) and has also been mixed with ABS, and other ingredients, to form some types of compression molded "clay" poker chips.
Precipitated calcium carbonate, made by dropping calcium oxide into water, is used by itself or with additives as a white paint, known as whitewashing.

Calcium carbonate is added to a wide range of trade and do it yourself adhesives, sealants, and decorating fillers.
Ceramic tile adhesives typically contain 70% to 80% limestone.
Decorating crack fillers contain similar levels of marble or dolomite.
Calcium carbonate is also mixed with putty in setting stained glass windows, and as a resist to prevent glass from sticking to kiln shelves when firing glazes and paints at high temperature.

In ceramic glaze applications, calcium carbonate is known as whiting, and is a common ingredient for many glazes in its white powdered form.
When a glaze containing this material is fired in a kiln, the whiting acts as a flux material in the glaze.
Ground calcium carbonate is an abrasive (both as scouring powder and as an ingredient of household scouring creams), in particular in its calcite form, which has the relatively low hardness level of 3 on the Mohs scale, and will therefore not scratch glass and most other ceramics, enamel, bronze, iron, and steel, and have a moderate effect on softer metals like aluminium and copper.
A paste made from calcium carbonate and deionized water can be used to clean tarnish on silver.

Calcium carbonate appears as white, odorless powder or colorless crystals.
Practically insoluble in water.
Occurs extensive in rocks world-wide.
Ground calcium carbonate (CAS: 1317-65-3) results directly from the mining of limestone.
The extraction process keeps the carbonate very close to its original state of purity and delivers a finely ground product either in dry or slurry form.
Precipitated calcium carbonate (CAS: 471-34-1) is produced industrially by the decomposition of limestone to calcium oxide followed by subsequent recarbonization or as a by-product of the Solvay process (which is used to make sodium carbonate).
Precipitated calcium carbonate is purer than ground calcium carbonate and has different (and tailorable) handling properties.

Calcium Carbonate is the carbonic salt of calcium (CaCO3).
Calcium carbonate is used therapeutically as a phosphate buffer in hemodialysis, as an antacid in gastric hyperacidity for temporary relief of indigestion and heartburn, and as a calcium supplement for preventing and treating osteoporosis. (NCI04)

Calcium carbonate is a calcium salt with formula CCaO3.
Calcium carbonate has a role as an antacid, a food colouring, a food firming agent and a fertilizer.
Calcium carbonate is a calcium salt, a carbonate salt and a one-carbon compound.

Calcium carbonate, or CaCO3, comprises more than 4% of the earth’s crust and is found throughout the world.
Calcium carbonate most common natural forms are chalk, limestone, and marble, produced by the sedimentation of the shells of small fossilized snails, shellfish, and coral over millions of years.
Although all three forms are identical in chemical terms, they differ in many other respects, including purity, whiteness, thickness and homogeneity.
Calcium carbonate is one of the most useful and versatile materials known to man.

Many of us encounter calcium carbonate for the first time in the school classroom, where we use blackboard chalk.
Chalk has been used as a writing tool for over 10,000 years and is a fine, microcrystalline material.
As limestone, calcium carbonate is a biogenic rock, and is more compacted than chalk.
As marble, calcium carbonate is a coarse-crystalline, metamorphic rock, which is formed when chalk or limestone is recrystallised under conditions of high temperature and pressure.
Large deposits of marble are found in North America and in Europe; e.g., in Carrara, Italy, the home of the pure white "statuario" from which Michelangelo created his sculptures.

Calcium carbonate, as it is used for industrial purposes, is extracted by mining or quarrying.
Pure calcium carbonate can be produced from marble, or it can be prepared by passing carbon dioxide into a solution of calcium hydroxide.
In the later case calcium carbonate is derived from the mixture, forming a grade of product called "precipitated calcium carbonate,” or PCC.
PCC has a very fine and controlled particle size, on the order of 2 microns in diameter, particularly useful in production of paper.
The other primary type of industrial product is "ground calcium carbonate,” or GCC.
GCC, as the name implies, involves crushing and processing limestone to create a powdery-like form graded by size and other properties for many different industrial and pharmaceutical applications.

A study of calcium carbonate provides important lessons about the history of the earth, since chalk, limestone and marble trace their origin to shallow water.
Thus, observation that large amounts of chalk deposits of the same age are found on many continents led to the discovery that there existed a period in which there was shallow water world-wide where shelled organisms thrived.
Some offer this as proof for the Biblical flood.
Nature returns the favor as calcium carbonate solutions from current deposits provide living organisms today with the material they need to grow their protective shells and skeletons.
Eggshells, for example, are composed of approximately 95% calcium carbonate.

Calcium carbonate causes a unique reaction with acids.
Upon contact with an acid - no matter the strength - it produces carbon dioxide.
This provides geologists with a reliable test to identify calcium carbonate.
This same phenomenon is important to the formation of caves.
Acidic rain water runs off and goes underground where it dissolves the calcium carbonate limestone.
The calcium carbonate water runs down and eventually reaches an air-filled cavity underground where the carbon dioxide can be released.
When it is released, the calcium carbonate crystallizes again.
Stalactite and stalagmite formations are created when water containing calcium carbonate drips, leaving some mineral at the source of the drip at the roof of the cave and some where it falls.
This is an extremely long process, and often takes place over many thousands of years.

As interesting as calcium carbonate may be in nature, its impact and value to our everyday life are truly extraordinary.

This medication is used to treat symptoms caused by too much stomach acid such as heartburn, upset stomach, or indigestion.
Calcium carbonate is an antacid that works by lowering the amount of acid in the stomach.Check the ingredients on the label even if you have used the product before.
The manufacturer may have changed the ingredients.
Also, products with similar names may contain different ingredients meant for different purposes.
Taking the wrong product could harm you.

Calcium carbonate (CaCO3) is the most widely used filler in polymer formulations.
As a filler, calcium carbonate allows cost reduction and improved mechanical properties.
Calcium carbonate is found in sedimentary rocks (chalk, limestone), marbles and minerals (dolomite).
Some typical properties are: density 2.7-2.9 g/cm3; pH of water suspension 9; particle size 0.2-30 μm; oil absorption 13–21 g/100 g; specific surface area 5–24 m2/g.
Depending on their origin and history of formation, and their impurities, the calcium carbonates have different properties.
Three major technological processes are used in the production of calcium carbonate fillers: milling, precipitation, and coating.
However, most calcium carbonate fillers are processed by milling using a dry or wet method.
Dry milling provides ultra-fine calcium carbonate grades (particle size about 0.6 μm).
Natural milled calcium carbonates are added to decrease cost in rubber base adhesives.

Calcium is a mineral that is found naturally in foods.
Calcium is necessary for many normal functions of the body, especially bone formation and maintenance.

Calcium carbonate is used to prevent or to treat a calcium deficiency.

There are many brands and forms of calcium carbonate available.
Not all brands are listed on this leaflet.

Calcium carbonate may also be used for purposes not listed in this medication guide

Calcium is a mineral that is found naturally in foods.
Calcium is necessary for many normal functions of the body, especially bone formation and maintenance.

Calcium carbonate is used to prevent or to treat a calcium deficiency.

There are many brands and forms of calcium carbonate available.
Not all brands are listed on this leaflet.

Calcium carbonate may also be used for purposes not listed in this medication guide.

Most calcium carbonate deposits are made up of the remains of marine organisms that have sedimented to the bottom of a shallow sea.
These organisms, such as crustaceans, algae and coral, absorb calcium carbonate from the water and use it to form their skeletons and shells.
When they die, their remains form sedimentary deposits on sea-beds which build up over time to form rock.

Calcium Carbonate is an exceptional mineral.
The chemical formula CaCO3 covers a raw material, which is widespread throughout nature, whether dissolved in rivers and oceans, in molten form as “cold” carbonatite-lava, or solid as a mineral in the form of stalactites, stalagmites or as the major constituent of whole mountain ranges.
Plants and animals need calcium carbonate to form their skeletons and shells.
In fact, when considering our lives, modern mankind could hardly imagine existing without calcium carbonate.
Almost every product in our daily lives either contains calcium carbonate or has some association with the mineral during its production.
The Earth’s crust contains more than 4% calcium carbonate.
As a result, the three calcium carbonate minerals – calcite, aragonite and vaterite – are among the most important rock-forming minerals.
Rocks are not the only calcium carbonate deposits in nature, most stretches of water and countless plants and animals contain huge amounts of calcium carbonate.
The link between these natural resources is the calcium carbonate cycle.
Plants and animals absorb calcium carbonate from water – where it exists, in most cases, in the dissolved form of calcium hydrogen carbonate Ca(HCO3)2 – and use it to build up their skeletons and shells.
After their death, crustacea, coccoliths, algae and corals form sedimentary deposits on sea-beds, thus the rock forming process is put in motion.
The first stage is the sedimentation process from which chalk and limestone originate.
Chalk is a poorly compacted sedimentary calcium carbonate rock, whose diagenesis is incomplete.
When the sedimentation process is completed this results in the formation of limestone.
If the sedimentation process takes place in magnesium containing water a dolomitisation may occur.
Part of the calcium ions in the crystal lattice are replaced by magnesium ions, a fact that leads to the formation of dolomite CaMg[CO3]2.
Marble is a metamorphic rock, which is the result of a recrystallisation process of limestone, under conditions of high pressure and temperature.
The carbonate rocks, chalk, limestone, dolomite and marble rocks are subject to erosion, under the influence of wind, temperature and water they dissolve, and the cycle may start again.
Calcium carbonate rocks are spread throughout the world, which is why they have been among the most widely used Calcium Carbonate raw materials for more than 5000 years.
Long ago, the Egyptians built their pyramids with limestone, and today we still use hundred of millions of tonnes of calcium carbonate in the building industry alone.
However, although the deposits are plentiful, only a few are of sufficiently high quality to be worked and even a fewer number of deposits will provide raw materials for industrial and agricultural uses other than the construction and roads building industry.
Only if the purity, degree of whiteness, thickness and homogeneity are acceptable is commercial extraction worthwhile.
After quarrying, further treatment is required to process natural calcium carbonates of the highest quality, known generically as Ground Calcium Carbonate (GCC).
Precipitated Calcium Carbonate (PCC) is a synthetic calcium carbonate produced industrially by means of a recarbonisation process.
Both GCC or PCC can be used in a wide range of applications.
For each end use there exists a tailor-made product, where fineness and particle size distribution are optimally balanced to meet the technical demands of that particular requirement.

Calcium carbonate is an inorganic salt used as an antacid.
Calcium carbonate is a basic compound that acts by neutralizing hydrochloric acid in gastric secretions.
Subsequent increases in pH may inhibit the action of pepsin.
An increase in bicarbonate ions and prostaglandins may also confer cytoprotective effects.
Calcium carbonate may also be used as a nutritional supplement or to treat hypocalcemia.

Density   : 2.8 g/cm3
Melting Point   : 825 °C (decomposition)
pH value   : 8.0 (H₂O) (slurry)
Bulk density   : 300 - 1400 kg/m3
Solubility   : 0.017 g/l

Assay (complexometric)   : ≥ 99.0 %
Substances insoluble in hydrochloric acid   : ≤ 0.005 %
Chloride (Cl)   :≤ 0.02 %
Sulfate (SO₄)   : ≤ 0.01 %
Total nitrogen (N)   : ≤ 0.01 %
Heavy metals (as Pb)   : ≤ 0.001 %
Ba (Barium)   : ≤ 0.02 %
Fe (Iron)   : ≤ 0.001 %
K (Potassium)   : ≤ 0.002 %
Mg (Magnesium)   : ≤ 0.02 %
Na (Sodium)   : ≤ 0.005 %
Sr (Strontium)   : ≤ 0.02 %

CALCIUM CARBONATE (KAL see um KAR bon ate) is a calcium salt.
Calcium carbonate is used as an antacid to relieve the symptoms of indigestion and heartburn.
Calcium carbonate is also used to prevent osteoporosis, as a calcium supplement, and to treat high phosphate levels in patients with kidney disease.

This medicine may be used for other purposes; ask your health care provider or pharmacist if you have questions.

Calcium carbonate accounts for more than 4% of the earth's crust.
As a result, the three minerals – calcite, aragonite and vaterite – are among the most important rock-forming minerals.
Rocks are not the only deposits in nature – almost all stretches of water and countless plants and animals contain huge amounts of calcium carbonate as well.
These natural resources are linked by the calcium carbonate cycle.

Plants and animals absorb calcium carbonate in water, where it usually exists dissolved in the form of calcium hydrogen carbonate Ca(HCO3)2, and use it to build up their skeletons and shells.
After their death, mussels, coccoliths, algae and corals form sedimentary deposits on sea beds and the rock-forming process is set in motion.

The first stage is the sedimentation process, from which chalk and limestone originate.
Chalk is a poorly compacted sedimentary calcium carbonate rock whose diagenesis is incomplete.

A completed sedimentation process results in the formation of limestone.
If the sedimentation process takes place in water containing magnesium, dolomitization may occur.
Part of the calcium ions in the crystal lattice are replaced by magnesium ions, leading to the formation of dolomite (CaMg(CO3)2).

Marble is a metamorphic rock resulting from the recrystallization of limestone under high pressure and temperature.
Whether chalk, limestone, dolomite or marble, all carbonate rocks are subject to erosion.
These dissolve under the influence of wind, temperature and water, and the cycle is ready to start anew.

The first stage is the sedimentation process, from which chalk and limestone originate.
Chalk is a poorly compacted sedimentary calcium carbonate rock whose diagenesis is incomplete.

Calcium supplements are generally made with one of two sources of elemental calcium: either calcium carbonate or calcium citrate.
Calcium carbonate, the form of calcium found in Caltrate, is the most concentrated form and is commonly found in food and drug stores.

Most formulas supply calcium in the form of calcium carbonate.
Calcium carbonate, which is found in Caltrate +++, is more concentrated, allowing for smaller or fewer tablets.

Calcium can make it difficult for the body to absorb certain medications.
Calcium products bind to quinolone (for example, ciprofloxacin) and tetracycline (for example, Sumycin) antibiotics in the intestine and can prevent their absorption into the body.
To prevent this interaction, doses of quinolone and tetracycline antibiotics should be separated by three or more hours from doses of calcium.

Calcium carbonate-containing products reduce acidity in the stomach.
The reduction of acid decreases the absorption of iron from the intestine.
Therefore, doses of calcium and iron should be separated by a several hours.

Calcium carbonate is one of the most abundant minerals on Earth and accounts for about 4% of the Crust.
Calcium carbonate can be found in nature three principal rock types: chalk, limestone and marble.

Calcium carbonate can also be produced synthetically in the form of Precipitated Calcium Carbonate (PCC).
The transformation process consists in decarbonating limestone to separate CaO and CO2, and then recombining these elements in a chemical reactor.
The final product has the same chemical composition as GCC, but with different properties in terms of particle size distribution, particle shape, and even higher purity.

Calcium carbonate is composed of three elements which are of particular importance for all organic and inorganic material on our planet: carbon, oxygen and calcium.
Calcium carbonate (CaCO3) is a white solid, is non-toxic and odourless.

Calcium carbonate, CaCO3, is one of the most common compounds on Earth, making up about 7% of Earth’s crust.
Calcium carbonate occurs in a wide variety of mineral forms, including limestone, marble, travertine, and chalk.
Calcium carbonate also occurs combined with magnesium as the mineral dolomite, CaMg (CO3)2.
Stalactites and stalagmites in caves are made of calcium carbonate, as are a variety of animal products, notably coral, seashells, eggshells, and pearls.

Calcium carbonate has two major crystalline forms—two different geometric arrangements of the calcium ions and carbonate ions that make up the compound—aragonite and calcite.
All calcium carbonate minerals are conglomerations of various-sized crystals of these two forms, packed together in different ways and containing various impurities.
The large, transparent crystals known as Iceland spar, however, are pure calcite.

Calcium carbonate is an important ingredient of many household products.
Calcium carbonate is used as a whitening agent in paints, soaps, art products, paper, polishes, putty products and cement.
Calcium carbonate is used as a filler and whitener in many cosmetic products including mouth washes, creams, pastes, powders and lotions.
Calcium carbonate is widely present naturally and as an additive in food and beverage production for dietary calcium, for adjustment of pH and as a stabilizer.
Calcium carbonate is also widely used as a calcium source in animal feeds.
Calcium carbonate is used in fertilizers and soil conditioners and in many industrial processes.
Calcium carbonate is also widely used in medications, as an antacid as a bulking agent and whitener.
Calcium carbonate is also used in water treatment to reduce acidity and to increase alkalinity of naturally acid waters.

Three types of calcium carbonate-containing rock are excavated and used by industry.
They are limestone, chalk and dolomite.
Limestone and chalk are both forms of calcium carbonate and dolomite is a mixture of calcium and magnesium carbonates.
All have impurities such as clay but some rocks are over 97% pure.
Limestone and other products derived from it are used extensively in the construction industry and to neutralise acidic compounds in a variety of contexts.

The calcium carbonate used was prepared by precipitation from calcium hydrate solution with carbon dioxide.
The saturated calcium carbonate solution was prepared by washing the precipitated salt with an abundance of conductance water, after which it was dissolved in conductance water free of carbon dioxide.
After the solution had been allowed to

Calcium carbonate is commonly found in antacids (for heartburn) and some dietary supplements.
Calcium carbonate overdose occurs when someone takes more than the normal or recommended amount of a product containing this substance.
This can be by accident or on purpose.

Calcium carbonate is also referred to as chalk, this dense, white powdery mineral is a common addition to the madder dye bath to deepen shades and is one of the principle minerals that create hard water.
Calcium carbonate may also be used with weld extract to bring out the bright, rich yellow shades.

Calcium carbonate is a fine, white powder consisting essentially of precipitated calcium carbonate (CaCO3) prepared either by grinding naturally occurring limestone or synthetically, by precipitation.

IUPAC NAME :

aquakal

Cacium carbonate

CaCO3

CaCO3_Co-registrant

CaCO3_Co-registrant_Sibelco

calcio carbonato

calcio carbonato precipitato

CALCIUM CARBONATE

Calcium Carbonate

Calcium carbonate

calcium carbonate

Calcium Carbonate

Calcium carbonate

calcium carbonate

Calcium carbonate (precipitated)

calcium carbonate precipitated

calcium carbonate.

Calcium Carbonate: Scoralite ®

calcium carnbonate

Calciumcarbonaat

CALCIUMCARBONAT

Calciumcarbonat

calciumcarbonate

SYNONYMS:

Calcium carbonate
1317-65-3 [RN]
207-439-9 [EINECS]
Calcii carbonas
Calcium Carbonate (AS)
Calcium monocarbonate
Calciumcarbonat [German]
Carbonate de calcium [French]
Carbonic acid calcium salt (1:1)
Carbonic acid, calcium salt (1:1)