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Lime

Base Information Edit
  • Chemical Name:Lime
  • CAS No.:1305-78-8
  • Deprecated CAS:104624-96-6,245321-52-2,60873-85-0
  • Molecular Formula:CaO
  • Molecular Weight:56.08
  • Hs Code.:28259019
  • European Community (EC) Number:277-225-8
  • UNII:C7X2M0VVNH
  • DSSTox Substance ID:DTXSID5029631
  • Mol file:1305-78-8.mol
Lime

Synonyms:calciumoxide;calcium;oxygen(2-);Lime oxide;73018-51-6;MFCD00010911;calcium oxid;LIME [HSDB];CALCIUM OXIDE [MI];CALCIUM OXIDE [FCC];CALCIUM OXIDE [JAN];CALCIUM OXIDE [INCI];LIME [USP MONOGRAPH];CALCIUM OXIDE [MART.];CALCIUM OXIDE [WHO-DD];DTXSID5029631;BRPQOXSCLDDYGP-UHFFFAOYSA-N;LIME (CALCIUM OXIDE) [II];EINECS 277-225-8;AKOS032949954;ETHYLBIS(2-BROMOETHYL)CARBAMATE;FT-0604488;1,6-Octadien-3-ol, 3,7-dimethyl-, acid isomerized;1,6-Octadien-3-ol, 3,7-dimethyl-, acid-isomerized

Suppliers and Price of Lime
Supply Marketing:Edit
Business phase:
The product has achieved commercial mass production*data from LookChem market partment
Manufacturers and distributors:
  • Manufacture/Brand
  • Chemicals and raw materials
  • Packaging
  • price
  • TRC
  • Calcium oxide
  • 50g
  • $ 85.00
  • Strem Chemicals
  • Calcium oxide (99.95%-Ca)
  • 50g
  • $ 95.00
  • Strem Chemicals
  • Calcium oxide, 98%
  • 1kg
  • $ 115.00
  • Strem Chemicals
  • Calcium oxide nanopowder, min. 99.9%, 30-200 nm
  • 10g
  • $ 75.00
  • Strem Chemicals
  • Calcium oxide, 98%
  • 250g
  • $ 39.00
  • Strem Chemicals
  • Calcium oxide (99.95%-Ca)
  • 10g
  • $ 25.00
  • Strem Chemicals
  • Calcium oxide nanopowder, min. 99.9%, 30-200 nm
  • 50g
  • $ 299.00
  • Sigma-Aldrich
  • Calcium oxide from marble small lumps ~3-20 mm
  • 1021099025
  • $ 1680.00
  • Sigma-Aldrich
  • Calcium oxide from marble small lumps ~3-20 mm
  • 25 kg
  • $ 1609.50
  • Sigma-Aldrich
  • Calcium oxide anhydrous, powder, ≥99.99% trace metals basis
  • 5g
  • $ 252.00
Total 269 raw suppliers
Chemical Property of Lime Edit
Chemical Property:
  • Appearance/Colour:white to grey solid 
  • Melting Point:2570 °C 
  • Refractive Index:1.83 
  • Boiling Point:2850 °C 
  • Flash Point:2850°C 
  • PSA:17.07000 
  • Density:3.3 g/mL at 25 °C(lit.) 
  • LogP:-0.11880 
  • Storage Temp.:Store at RT. 
  • Sensitive.:Air & Moisture Sensitive 
  • Solubility.:1.65g/l Risk of violent reaction. 
  • Water Solubility.:REACTS 
  • Hydrogen Bond Donor Count:0
  • Hydrogen Bond Acceptor Count:1
  • Rotatable Bond Count:0
  • Exact Mass:55.9575055
  • Heavy Atom Count:2
  • Complexity:0
Purity/Quality:

99% *data from raw suppliers

Calcium oxide *data from reagent suppliers

Safty Information:
  • Pictogram(s): CorrosiveC,IrritantXi 
  • Hazard Codes:C,Xi 
  • Statements: 34-41-37/38 
  • Safety Statements: 26-36/37/39-45-25-39 
MSDS Files:

SDS file from LookChem

Total 1 MSDS from other Authors

Useful:
  • Chemical Classes:UVCB
  • Canonical SMILES:[O-2].[Ca+2]
  • Uses 1.? Calcium oxide can be used in the manufacture of calcium carbide, soda ash, bleaching powder, used as building materials, refractoriness’, desiccant and soil conditioner and calcium fertilizer 2.? It can be used as an analysis reagent and flux agent for manufacturing fluorescence powder. 3.? It can be used in the manufacture of calcium carbide, soda ash, bleaching powder, also used for leather, waste water purification 4.? Calcium oxide can be used as building materials, metallurgical flux agent and the major raw materials for the manufacturing of calcium hydroxide and a variety of calcium compounds. It is also the inexpensive alkali in the chemical industry. It is widely used in pesticides, paper, food, petrochemical, leather, waste water purification and so on. It can also be used for the drying of the laboratory ammonia and alcohol dehydration. 5.? Use as drug carriers. 6.? Uses as analysis reagents; Calcium oxide can be applied to steel, pesticides, pharmaceuticals, non-ferrous metals, fertilizers, leather and manufacturing of calcium hydroxide, drying of laboratory ammonia, carbon dioxide absorbent and alcohol dehydration. The major uses of lime are metallurgy, flue gas desulfurization, construction, mining, papermaking, and water treatment. About one third of calcium oxide production in the United States is used for metallurgical processes, principally in the iron and steel industry. Calcium oxide is used to remove impurities during the refining of iron ore. Calcium oxide combines with compounds such as silicates, phosphates, and sulfates contained in iron ores to form slag. Lime is also used for purification in other metal refining and to control pH in mining processes such as leaching and precipitation. The calcium oxide is also used in remediation of mine wastes to recover cyanides and to neutralize acid mine drainage. In bricks, plaster, mortar, stucco and other building and construction materials; manufacture of steel, aluminum, magnesium, and flotation of non-ferrous ores; manufacture of glass, paper, Na2CO3 (Solvay process), Ca salts and many other industrial chemicals; dehairing hides; clarification of cane and beet sugar juices; in fungicides, insecticides, drilling fluids, lubricants; water and sewage treatment; in laboratory to absorb CO2 (the combination with NaOH is known as soda-lime, q.v.). Calcium Oxide is a general food additive consisting of white granules or powder of poor water solubility. it is obtained by heating limestone (calcium carbonate) in a furnace. it is also termed lime or quicklime. it is used as an anticaking agent, firming agent, and nutritive supple- ment in applications such as grain products and soft candy.
  • Production method Calcium carbonate calcination first apply calcium carbonate for reaction with hydrochloric acid to generate calcium chloride, followed by addition of ammonia for neutralization, standing for precipitation and filtration, followed by adding sodium bicarbonate for reaction to generate calcium carbonate precipitate. It is further subject to centrifugal separation dehydration, drying and calcination, followed by crushing and screening to obtain the finished product of medicinal calcium oxide. Its reaction is: CaCO3 + 2HCl → CaCl2 + CO2 + H2O CaCl2 + 2NH3? H2O? Ca (OH) 2 + 2NH4Cl Ca (OH) 2 + NaHCO3 → CaCO3 + NaOH + H2O CaCO3 [△]→CaO + CO2 ?. Limestone calcination method: crush the coarse limestone to 150 mm, and screen for the fine residue below 30 to 50 mm. Anthracite or coke required a particle size to be below 50 mm, which contains not too much low melting point ash content. The amount of anthracite or coke is 7.5% to 8.5% of that of limestone by weight. The selected limestone and fuel are timely and quantitatively supplied from the kiln crown to the kiln, further calcinated at 900~1200 ℃ and then lead to the finished product after cooling. In the calcination process, carbon dioxide is produced as by-product. Its reaction equation is: CaCO3 [△]→CaO + CO2 .
  • Description Calcium oxide (CaO, CAS Reg. No. 1305-78-8) is also known as lime, quick lime, burnt lime, or calx. Lime does not occur naturally since it reacts so readily with water (to form hydrated lime) and carbon dioxide (to form limestone). It is produced from calcium carbonate, limestone, or oyster shells by calcination at temperatures of 1,700-2,450℃. Calcium Oxide is a solid with a very high affinity for water - it will react with water in the air, or in your skin or anywhere it can and form calcium hydroxide. This reaction is exothermic so it releases a lot of heat while it is reacting - there fore as well as being corrosive and causing significant skin irritation, calcium oxide's reaction with water can also cause burns. Calcium hydroxide is basically hydrated calcium oxide. It is alkali so can be corrosive. In solution it makes limewater. CaO is not found pure in nature but rather is contained in various abundant minerals (i.e. calcite, aragonite, limestone, marble) but vary greatly in their purity (impurities usually include magnesia, iron, alumina, silica, sulfur). Of these iron and sulfur are most troublesome (i.e. where clarity is important in glass). Lime minerals vary in the degree of crystallization and cohesion of the crystalline mass and the homogeneity of the matrix. Calcium oxide is the principle flux in medium and high temperature glazes, beginning its action (within the glaze) around 1100C. It must be used with care in high-fire bodies because its active fluxing action can produce a body that is too volatile (melting if slightly overfired). Lime, or calcium oxide, is a principle ingredient in the production of Portland cement, the basis for most mortars and concrete. Hydrated or ‘slaked’ lime is the chemical calcium hydroxide. This chemical is also used in mortars. Both types of lime are strong bases and are also used in food production (calcium hydroxide is commonly used in making corn tortillas), petroleum refining and sewage treatment. In the household it is used by aquarium hobbyists to add bioavailable calcium to fish tanks. It is also found in hair relaxers.
  • Physical properties Calcium oxide is a white caustic crystalline alkali substance that goes by the common name lime. The term lime is used both generically for several calcium compounds and with adjectives to qualify different forms of lime. This entry equates lime, also called quicklime or burnt lime, with the compound calcium oxide. Hydrated lime, made by combining lime with water, is calcium hydroxide and is often referred to as slaked lime (Ca(OH)2). Dolomite limes contain magnesium as well as calcium. Limestone is the compound calcium carbonate. The term lime comes from the Old English word l?m for a sticky substance and denotes lime’s traditional use to produce mortar. Calx was the Latin word for lime and was used to name the element calcium.
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