calcium carbonate

calcium carbonate

Mesh 1200 Mesh 800 Mesh 400 Mesh 3500 Mesh 2500 Morvarid Bandar Pol Calcium Carbonate (CaCO3) Calcium carbonate is one of the minerals we can supply out of all of places in Iran. MBP uses this good quality of calcium carbonate to produce high quality of CaCO3 powder and sizing. We are one of the premium calcium carbonate supplier in Bandar Abbas Iran and dedicated to establishing long term business relationships with our customers from a range of manufacturing industries. Our proven success and years of experience enables us to provide the best quality and services to our customers. We are committed to developing more value added solutions for our customers and ensure a high quality, consistent and reliable source of calcium carbonate products. Calcium carbonate is biologically safe and inexpensive, therefore, it is widely used as a white colored filler in many fields of industries. On a base of calcium carbonate supply, we deliver "Delicacy", "Safety" and "Health" to you. We give the highest priority to "Safety" in supplying seasonings, conditioning agents and enrichments. Our products contribute to the reduction of negative factors in "picking", "distribution" and "storage". We help you in your efforts to grow high value-added. Calcium Carbonate Calcium carbonate, or CaCO3, comprises more than 4% of the earths crust and is found throughout the world. Its 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 recrystallized under conditions of high temperature and pressure 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 latter 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. Our Capabilities Calcium Carbonate storage private area more than 7 hectares in Shahid Rajaee port Bandar Abbas Hormozgan province. Calcium Carbonate port services such as marble chips loading and unloading vessels, barges, landing crafts, marble chips loading/unloading in containers. Calcium Carbonate land transportation with using modern trucks. Calcium Carbonate stevedoring. Calcium Carbonate port handling. Calcium Carbonate clearing, shipping agencies, ship chartering. Calcium Carbonate land transportation with using modern trucks. Accept customers valuable marble chips order with any method of the delivery. We are one of the biggest high quality calcium carbonate supplier and exporter company in Bandar Abbas Iran. Supplying, exporting calcium carbonate from Bandar Abbas Iran to any ports of India, Philippines, Malaysia, Singapore, Vietnam, Sri Lanka, Indonesia, Qatar, Bahrain, Kuwait, UAE, China, Tanzania, Mozambique, Djibouti, Kenya, and east African countries. Morvarid Bandar Pol Marble Chips Types Powdered calcium carbonate Sized calcium carbonate Calcium carbonate meshes up to 3500 Uses of Calcium Carbonate As interesting as calcium carbonate may be in nature, its impact and value to our everyday life are truly extraordinary. Paper, Plastics, Paints, and Coatings Calcium carbonate is the most widely used mineral in the paper, plastics, paints and coatings industries both as a filler and due to its special white color - as a coating pigment. In the paper industry it is valued worldwide for its high brightness and light scattering characteristics, and is used as an inexpensive filler to make bright opaque paper. Filler is used at the wet-end of paper making machines, and calcium carbonate filler allows for the paper to be bright and smooth. As an extender, calcium carbonate can represent as much as 30% by weight in paints. Calcium carbonate also is used widely as a filler in adhesives, and sealants. Personal Health and Food Production Calcium carbonate is used widely as an effective dietary calcium supplement, antacid, phosphate binder, or base material for medicinal tablets. It also is found on many grocery store shelves in products such as baking powder, toothpaste, dry-mix dessert mixes, dough, and wine. Calcium carbonate is the active ingredient in agricultural lime, and is used in animal feed. Calcium carbonate also benefits the environment through water and waste treatment. Building Materials and Construction Calcium carbonate is critical to the construction industry, both as a building material in its own right (e.g. marble), and as an ingredient of cement. It contributes to the making of mortar used in bonding bricks, concrete blocks, stones, roofing shingles, rubber compounds, and tiles. Calcium carbonate decomposes to form carbon dioxide and lime, an important material in making steel, glass, and paper. Because of its antacid properties, calcium carbonate is used in industrial settings to neutralize acidic conditions in both soil and water. Calcium carbonate is used in the purification and separation of iron from its ore. It is often used in swimming pools for maintaining the alkalinity of water and countervailing acidic properties of the disinfectant. As it is heavy, calcium carbonate increases the density of drilling fluids and helps in controlling the down hole pressure. Hence it is widely used in the oil industry. It is also added to drilling fluids as a formation bridging and filter-cake sealing agent. Calcium carbonate is also used in industries like paint, plastic, rubber, ceramic, cement, glass, steel, oil refining, and in biorock creation for mariculture of sea organisms. The decomposition of calcium carbonate gives carbon dioxide and lime, which is of use in the glass, steel, and paper industries. Calcium carbonate is the most preferred mineral in the paper industry, used for filling and coating paper. It is used as a filler in sealants and adhesives. Calcium carbonate is also used in the production of mortar which is utilized for making concrete blocks, bonding bricks, rubber compounds, tiles, etc. Calcium carbonate is used in the construction of buildings, roads, and other engineering works. It is used in the construction industry as a building material as well as a component of cement. It is also used in the production of baking powder, dry-mix dessert mixes, dough, wine, etc., and as a part of animal feed. Calcium carbonate crystals (calcite) have a double refraction property due to which they find applications in optics. In case of whitewashing, calcium hydroxide reacts with carbon dioxide in air to form calcium carbonate, which forms a thin layer on the walls, giving them a gloss. Calcium carbonate is a primary component of garden lime, also known as agricultural lime, which is used for neutralizing acidic soil and to enhance soil quality. Garden lime when added to soil, acts as a rich source of calcium for plants and increases the pH and water-retaining capacity of acidic soils. It is a rich source of calcium, and is beneficial for the crops. Also, it enhances the consumption of essential plant nutrients like nitrogen, phosphorus, and potassium in acidic soils. An experiment conducted by Ken Simmons has proved that calcium carbonate helps neutralize the effects of harmful acid rains in a river water ecosystem. Ground calcium carbonate (GCC) acts as a reagent in flue-gas desulfurization applications by eliminating sulfur dioxide emissions from coal and other fossil fuels. It also helps neutralize acidic water from the mines and in the treatment of drinking as well as waste water. The paste of calcium carbonate and deionized water is used to clean the tarnish on silver. It is a food additive (designated E170) and bears the INS number 170. It is also used as a food preservative. Calcium carbonate is also utilized as a color retainer for organic apples and other foods. It acts like a firming agent for many canned or bottled vegetable products. It is used as blackboard chalk. Finely ground calcium carbonate (GCC) is used for the preparation of microporous films in baby diapers. Calcium carbonate is used in homeopathy, in the production of toothpaste, and as an inert substance in tablets. Health Benefits Calcium supplements that contain calcium carbonate are prescribed by doctors as a remedy for diarrhea or as an antacid. A combination of calcium carbonate and magnesium helps to reduce diarrhea among people who suffer from irritable bowel syndrome (IBS). It has gastric antacid qualities and is used as a medication for symptoms like heartburn and stomach upset caused by acidity. It is also used to treat GERD and Peptic ulcers. It is used as a dietary supplement as it is rich in calcium, and can be of help in the treatment of hyperphosphatemia. Calcium supplements (in the form of calcium carbonate) are effective in treating certain ailments related to calcium deficiency like bone loss and osteoporosis. Calcium supplements help control high blood pressure during pregnancy. They are used in managing premenstrual syndrome symptoms. It helps maintain the overall pH balance of the body. Calcium carbonate crystals are referred to as calcite. The calcite crystal generally is considered a rhombohedron because of its cleavage properties. Cleavage is what causes crystals to angle where the bonding forces are weak and are apt to break into planes. Calcite is unique in that its cleavage takes three distinct directions. There are more than 300 forms of calcite crystals. Calcite crystals also come in many different colors, but usually are white or transparent. Another important property of the calcite crystal is its property of double refraction. Double refraction occurs when a ray of light travels through a medium and is split into two different beams, one traveling slowly, one traveling fast. The two different beams are bent at two different angles of refraction. As a result of this property a person looking through calcite sees two images. This property of double refraction is a feature valuable to a number of optical applications. Calcium and Water Calcium is naturally present in water. It may dissolve from rocks such as limestone, marble, calcite, dolomite, gypsum, fluorite and apatite. Calcium is a determinant of water hardness, because it can be found in water as Ca2+ ions. Magnesium is the other hardness determinant. Calcium is present in various construction materials, such as cement, brick lime and concrete. It is present in batteries, and is applied in plaster as calcium sulphate. The metal is applying for zirconium and thorium production. In steel industries calcium is applied as a blotter, and is added to aluminum, copper and lead alloys. Calcium can extract Sulphur dioxide from industrial exhaust, and neutralize sulphuric acids before discharge. Other examples of calcium applications are calcium hypo chloride as bleach and for disinfection, calcium phosphate in glass and porcelain industries, calcium polysulphide and hydroxide as flocculants in wastewater treatment, and calcium fluoride as turbidity agent in enamel industries, in UV-spectroscopy, and as a raw material for fluid acid production. Calcium may also be applied for removal of carbon and Sulphur from iron and iron alloys, and for dewatering oil. Limestone is applied as a paper filler, causing paper to color whiter, and in plastics to improve stability. Calcium often positively affects soil quality and various compounds are applied as a fertilizer. For example, CaCl2- or Ca(NO)3 solutions are applied in horticulture. Calcium oxide is a dehydrating molluscicide. Calcium is a dietary requirement for all organisms apart from some insects and bacteria. Calcium carbonate is a building stone of skeletons of most marine organisms, and eye lenses. Calcium phosphate is required for bone structure and teeth structure of terrestrial organisms. Plants mainly contain calcium oxalate. Calcium storage in plants is about 1% of dry mass. Calcium is largely responsible for water hardness, and may negatively influence toxicity of other compounds. Elements such as copper, lead and zinc are much more toxic in soft water. In limed soils calcium may immobilize iron. This may cause iron shortages, even when plenty of iron is present in the soil. Water hardness influences aquatic organisms concerning metal toxicity. In softer water membrane permeability in the gills is increased. Calcium also competes with other ions for binding spots in the gills. Consequently, hard water better protects fishes from direct metal uptake. pH values of 4.5-4.9 may harm salmon eggs and grown salmons, when the calcium, sodium and chlorine content is low. Various calcium compounds may be toxic. The LD50 of rats for calcium arsenite is 20 mg/ kg body weight. Calcium carbide forms flammable ethyn when it comes in contact with water and is therefore considered hazardous. Some environmental effects of water hardness include hardening of domestic equipment, because high temperatures cause carbonate hardness. This may dramatically decrease the lifespan of equipment, and causes an increase of domestic waste. Calcium carbonate interacts with detergents and cleansing agents. Complex formation causes a decrease in detergent efficiency, resulting in requirement for increased detergent application and softener purchases (see also magnesium and water). Softening is often carried out by means of ion exchangers. These must be regenerates with kitchen salt, and therefore burden wastewater. There are six stable calcium isotopes. Today, we know of eight instable calcium isotopes. 45Ca is highly radioactive and toxic. Calcium carbonate geology Calcium carbonate is normally found as a white mineral (calcite) which occurs naturally in chalks, limestones and marbles. Some of these rocks were formed by inorganic processes, but many are of organic origin being composed of the remains of countless sea organisms. Most are limestones, a general term used for a rock possessing varying proportions of calcite and dolomite with small amounts of iron-bearing carbonates. Dolomite is a double carbonate of calcium and magnesium, with the formula CaMg(CO3)2. Limestones are usually clear or white. However, with impurities, they can take on a variety of colors, commonly white, tan or grey. The most common crystal arrangement for naturally-occurring calcium carbonates is the hexagonal form of calcite. Less common is aragonite, which has a discrete or clustered needle, orthorhombic crystal structure. Aragonite is formed in a narrow range of physio-chemical conditions, typically in thermal springs although mollusc shells and pearls are made of aragonite. Geology Carbonate is found frequently in geologic settings and constitute an enormous carbon reservoir. Calcium carbonate occurs as aragonite, calcite and dolomite. 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 sediment 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 carbonate compensation depth (CCD) is the point in the ocean where the rate of precipitation of calcium carbonate is balanced by the rate of dissolution due to the conditions present. Deep in the ocean, the temperature drops and pressure increases. Calcium carbonate is unusual in that its solubility increases with decreasing temperature. Increasing pressure also increases the solubility of calcium carbonate. The carbonate compensation depth can range from 46 km below sea level. Calcium carbonate can preserve fossils through permineralization. Most of the vertebrate fossils of the Two Medicine Formationa geologic formation known for its duck-billed dinosaur eggs are preserved by CaCO3 permineralization. This type of preservation preserves high levels of detail, even down to the microscopic level. However, it also leaves specimens vulnerable to weathering when exposed to the surface.

difference between calcium carbonate and calcium oxide | compare the difference between similar terms

difference between calcium carbonate and calcium oxide | compare the difference between similar terms

The key difference between calcium carbonate and calcium oxide is that calcium carbonate tends to undergo decomposition upon heating to high temperatures, whereas calcium oxide is very stable towards heat treatment.

Calcium carbonate is a carbonate of calcium that has the chemical formula CaCO3. This compound naturally occurs aslimestone, chalk,calcite, etc. Therefore, it is a common substance in rocks. Ex: calcite or aragonite (Limestone contains both these forms). Calcium carbonate occurs as white hexagonal crystals or powder, and it is odourless.

Moreover, Calcium carbonate has a chalky taste. The molar mass of this compound is 100 g/mol, and the melting point is 1,339 C (for the calcite form). However, it has no boiling point because this compound decomposes at high temperatures. We can get this compound by mining the calcium-bearing minerals. But this form is not pure. We can obtain a pure form using a pure quarried source such as marble. When calcium carbonate reacts with acids, it forms CO2gas. When it reacts with water, it forms calcium hydroxide. In addition to these, it can undergo thermal decomposition, releasing CO2gas.

Calcium oxide is an inorganic compound having the chemical formula CaO. It is also named quicklime or burnt lime. We can describe this substance as a white, caustic, alkaline, and crystalline compound. It is odourless as well.

Concerning the preparation of calcium oxide, this substance is usually manufactured by the thermal decomposition of limestone or seashells containing calcium carbonate in a lime kiln. In this preparation process, we need to heat the reactants to above 625 Celsius degree temperature. This heat treatment is called calcination. This process releases molecular carbon dioxide, which leaves quicklime. Since quicklime is not stable, it can spontaneously react with carbon dioxide when cooled, and after a sufficient time, it will completely convert back to calcium carbonate. Therefore, we need to slack it with water to set it as lime plaster or lime mortar.

When considering the uses of calcium oxide, the major use is in the basic oxygen steelmaking process, where it can neutralize the acidic oxides, silicone oxide, aluminum oxide and ferric oxide, producing a molten slag. Another important application of calcium oxide is using it in the production of aerated concrete blocks having varying densities.

Calcium carbonate is a carbonate of calcium that has the chemical formula CaCO3, while Calcium oxide is an inorganic compound having the chemical formula CaO. The key difference between calcium carbonate and calcium oxide is that calcium carbonate tends to undergo decomposition upon heating to high temperatures, whereas calcium oxide is very stable towards heat treatment.

Calcium carbonate and calcium oxide are important inorganic compounds of calcium metal. The key difference between calcium carbonate and calcium oxide is that calcium carbonate tends to undergo decomposition upon heating to high temperatures, whereas calcium oxide is very stable towards heat treatment.

Madhu is a graduate in Biological Sciences with BSc (Honours) Degree and currently persuing a Masters Degree in Industrial and Environmental Chemistry. With a mind rooted firmly to basic principals of chemistry and passion for ever evolving field of industrial chemistry, she is keenly interested to be a true companion for those who seek knowledge in the subject of chemistry.

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