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Calciumdichloride is an inorganic compound, a salt with the chemical formula CaCl2.
Calciumdichloride is a white crystalline solid at room temperature, and it is highly soluble in water.
Calciumdichloride can be created by neutralising hydrochloric acid with calcium hydroxide.
CAS: 10043-52-4
MF: CaCl2
MW: 110.98
EINECS: 233-140-8
Synonyms
PELADOW(R) SNOW AND ICE MELT;Calcium chloride,aqueous solution;Calcium chloride,medicinal;Additive Screening Solution 21/Fluka kit no 78374, Calcium chloride solution;calcium chloride anhydrus for technical;calcium chloride anhydrous for food;CACL2 (CALCIUM CHLORIDE);CalciuM chloride, 96%, for biocheMistry, anhydrous;10043-52-4;Calcium chloride anhydrous;Calcium dichloride;Dowflake;Liquidow;Peladow;CaCl2;Bovikalc;Calcium chloride (CaCl2);Calcium Chloride, Anhydrous;Intergravin-orales;Cacl2 (anhydrous);Calcium(2+) chloride;CHEBI:3312;Calcarea muriatica;INS NO.509;Calcium-45 chloride;DTXSID5020235;INS-509;NSC-759598;DTXCID30235;OFM21057LP;E-509;Calcium(II) chloride;Calcio cloruro;Calcium Choride;Conclyte-Ca;CaCl;856 - Pickles;E509;[CaCl2];Calcium chloride, Prilled;Calcium chloride ultra dry;CALCIUM CHLORIDE [MI];CALCIUM CHLORIDE 10%;CALCIUM CHLORIDE HYDRATES;CHEMBL1200668;CALCIUM CHLORIDE [WHO-DD];Calcium chloride anhydrous, powder;Tox21_202585;AKOS024437435;DB01164;USEPA/OPP Pesticide Code: 075605;CALCIUM CHLORIDE ANHYDROUS [HSDB];NCGC00260134-01;CAS-10043-52-4;NS00093589;C08130;Q208451;Calcium chloride, anhydrous, dessicant, ACS grade, granular
Calciumdichloride is commonly encountered as a hydrated solid with generic formula CaCl2·nH2O, where n = 0, 1, 2, 4, and 6.
These compounds are mainly used for de-icing and dust control.
Because the anhydrous salt is hygroscopic and deliquescent, Calciumdichloride is used as a desiccant.
Calciumdichloride is usedas road salt for melting snow, a drying agent in desiccators,for dehydrating organic liquids and gases, in refrigerationbrines and antifreeze, as a dust-proofing agent, food additive, concrete hardening accelerator, and others.
Incompatibilities: The solution in water is a weak base.
Reacts with zinc in presence of moisture, forming highly526 Calcium chlorideflammable hydrogen gas.
Dissolves violently in waterwith generation of much heat.
Incompatible with water,bromine trifluoride; 2-furan, percarboxylic acid.
Mayattack some building materials and metals in the presenceof moisture.
Calciumdichloride may be found in nature as the mineral tachhydrite, CaCl2-2MgCl2-12H2O.
Calciumdichloride also is found in other minerals.
Calciumdichloride's concentration in sea water is about 0.15%.
Calciumdichloride has several industrial applications.
The major applications of this compound are in deicing of roads, dust control, imparting stability to roads and buildings, and to improve traction in tractor tires.
Calciumdichloride is mixed with ice to make freezing mixtures.
Hexahydrate mixed with crushed ice can lower the temperature of the cooling bath to below -50°C.
Calciumdichloride also is used as a desiccant for dehydrating gases and liquids.
Calciumdichloride is added to cement in various proportions to manufacture different types of concrete.
Other uses are in adhesives, to lower gel temperatures, and as a calcium source in liquid feed supplements for dairy cattle.
Also, Calciumdichloride is used to control particle size development and reduce coalescence in plastics.
calcium chloride: A white deliquescentcompound, CaCl2, which issoluble in water; r.d. 2.15; m.p.782°C; b.p. >1600°C.
There are anumber of hydrated forms, includingthe monohydrate, CaCl2.H2O, the dihydrate,CaCl2.2H2O (r.d. 0.84), andthe hexahydrate, CaCl2.6H2O (trigonal;r.d. 1.71; the hexahydrate loses4H2O at 30°C and the remaining2H2O at 200°C).
Large quantities of itare formed as a byproduct of theSolvay process and it can be preparedby dissolving calcium carbonateor calcium oxide in hydrochloricacid.
Crystals of the anhydrous saltcan only be obtained if the hydratedsalt is heated in a stream of hydrogenchloride.
Solid Calciumdichloride isused in mines and on roads to reducedust problems, whilst the molten saltis the electrolyte in the extraction ofcalcium.
An aqueous solution of calciumchloride is used in refrigerationplants.
Calciumdichloride is a water soluble ionic crystal with a high enthalpy change of solution.
Calciumdichloride is majorly derived from limestone and is a by-product of the Solvay process.
Calciumdichloride is an anhydrous salt that has a hygroscopic nature and can be used as a desiccant.
History
Calciumdichloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century.
Calciumdichloride was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum) because it was synthesized during the distillation of ammonium chloride with lime and was nonvolatile (while the former appeared to sublime); in more modern times (18th-19th cc.) Calciumdichloride was called "muriate of lime" (Latin: murias calcis, calcaria muriatica).
Calciumdichloride Chemical Properties
Melting point: 772 °C (lit.)
Boiling point: 1935 °C/1 atm (lit.)
Density: 1.086 g/mL at 20 °C
Vapor pressure: 0.01 mm Hg ( 20 °C)
Refractive index: n20/D 1.358
Fp: >1600°C
Storage temp.: Store at +5°C to +30°C.
Solubility H2O: soluble
Form: powder
Color: White to gray
Specific Gravity: 2.15
Odor: Odorless
Flame Color: Redish
PH: 8-10 (100g/l, H2O, 20℃)
Water Solubility: 740 g/L (20 ºC)
Sensitive: Hygroscopic
λmax λ: 260 nm Amax: 0.04
λ: 280 nm Amax: 0.02
Crystal Structure: CaCl2 type
crystal system: Nogata
Merck: 14,1659
Calciumdichloride, CaC12, is colorless deliquescent solid that is soluble in water and ethanol.
Calciumdichloride is formed from the reaction of calcium carbonate and hydrochloric acid or calcium hydroxide and ammonium chloride.
Calciumdichloride is used in medicine, as an antifreeze, and as a coagulant.
Calciumdichloride, CaC12, is colorless deliquescent solid that is soluble in water and ethanol.
Calciumdichloride is formed from the reaction of calcium carbonate and hydrochloric acid or calcium hydroxide and ammonium chloride.
Calciumdichloride is used in medicine, as an antifreeze, and as a coagulant.
Calciumdichloride occurs as a white or colorless crystalline powder, granules, or crystalline mass, and is hygroscopic (deliquescent).
Calciumdichloride dissolves in water, producing chloride and the aquo complex [Ca(H2O)6]2+. In this way, these solutions are sources of "free" calcium and free chloride ions.
This description is illustrated by the fact that these solutions react with phosphate sources to give a solid precipitate of calcium phosphate:
3 CaCl2 + 2 PO3−4 → Ca3(PO4)2 + 6 Cl−
Calciumdichloride has a very high enthalpy change of solution, indicated by considerable temperature rise accompanying dissolution of the anhydrous salt in water.
This property is the basis for its largest-scale application.
Aqueous solutions of Calciumdichloride tend to be slightly acidic due to the influence of the chloride ions on the hydrogen ion concentration in water.
The slight acidity of Calciumdichloride solutions is primarily due to the increased ionic strength of the solution, which can influence the activity of hydrogen ions and lower the pH slightly.
Physical properties
White crystal, powder or flake; highly hygroscopic; the compound and its solutions absorb moisture from the air at various rates depending on Calciumdichloride concentrations, relative humidity and vapor pressure of water in the air, temperature, surface area of exposed material, and the rate of air circulation; at 40% and 95% relative humidity and 25°C, one gram anhydrous calcium chloride may absorb about 1.4 g and 17 g water, respectively.
Uses
Calciumdichloride has many uses.
Calciumdichloride is used as a drying agent and to melt ice and snow on highways, to control dust, to thaw building materials (sand, gravel, concrete, and so on).
Calciumdichloride is also used in various food and pharmaceutical industries and as a fungicide.
Calciumdichloride is one of the most versatile of the basic chemicals.
Calciumdichloride has several common applications such as brine for refrigeration plants, ice and dust control on roads, and in concrete.
The anhydrous salt is also widely used as a desiccant, where Calciumdichloride will absorb so much water that it will eventually dissolve in its own crystal lattice water (water of hydration).
Calciumdichloride can be produced directly from limestone, but large amounts are also produced as a by-product of the “Solvay Process” (which is a process to produce soda ash from brine).
Calciumdichloride is also commonly used as an additive in swimming pool water as it increases the “calcium hardness” value for the water.
Other industrial applications include use as an additive in plastics, as a drainage aid for wastewater treatment, as an additive in fire extinguishers, as an additive in control scaffolding in blast furnaces, and as a thinner in “fabric softeners”.
Calciumchloride is commonly used as an “electrolyte” and has an extremely salty taste, as found in sports drinks and other beverages such as Nestle bottled water.
Calciumdichloride can also be used as a preservative to maintain firmness in canned vegetables or in higher concentrations in pickles to give a salty taste while not increasing the food’s sodium content.
Calciumdichloride is even found in snack foods, including Cadbury chocolate bars.
In brewing beer, calciumchloride is sometimes used to correct mineral deficiencies in the brewing water.
Calciumdichloride affects flavor and chemical reactions during the brewing process, and it can also affect yeast function during fermentation.
Calciumdichloride can be injected as intravenous therapy for the treatment of “hypocalcemia” (low serum calcium).
Calciumdichloride can be used for insect bites or stings (such as Black Widow spider bites), sensitivity reactions, particularly when characterized by “urticaria” (hives).
Obtained as a by-product in the manufacture of potassium chlorate.
The white crystals, soluble in water and alcohol, are deliquescent and must be kept in a well-stoppered bottle.
Calciumdichloride was used in iodized collodion formulas and in collodion emulsions.
Calciumdichloride was also an important desiccating substance used in tin calcium tubes designed to store presensitized platinum papers.
For the treatment of hypocalcemia in those conditions requiring a prompt increase in blood plasma calcium levels, for the treatment of magnesium intoxication due to overdosage of magnesium sulfate, and used to combat the deleterious effects of hyperkalemi
Calciumchloride is highly hygroscopic and is often used as a desiccant.
calciumchloride is an astringent.
Calciumdichloride also helps improve the reaction among certain ingredients used in cosmetic formulations.
This inorganic salt is no longer commonly used in skin care products and is being replaced with potassium chloride.
CalciumChloride is a general purpose food additive, the anhydrous form being readily soluble in water with a solubility of 59 g in 100 ml of water at 0°c.
Calciumdichloride dissolves with the liberation of heat. it also exists as calcium chloride dihydrate, being very soluble in water with a solubility of 97 g in 100 ml at 0°c.
Calciumdichloride is used as a firming agent for canned tomatoes, potatoes, and apple slices.
in evaporated milk, Calciumdichloride is used at levels not more than 0.1% to adjust the salt balance so as to prevent coagulation of milk during sterilization.
Calciumdichloride is used with disodium edta to protect the flavor in pickles and as a source of calcium ions for reaction with alginates to form gels.
By depressing the freezing point of water, calciumchloride is used to prevent ice formation and is used to de-ice.
This application consumes the greatest amount of calcium chloride.
Calciumdichloride is relatively harmless to plants and soil.
As a de-icing agent, Calciumdichloride is much more effective at lower temperatures than sodium chloride. When distributed for this use, it usually takes the form of small, white spheres a few millimeters in diameter, called prills.
Solutions of calciumchloride can prevent freezing at temperatures as low as −52 °C (−62 °F), making it ideal for filling agricultural implement tires as a liquid ballast, aiding traction in cold climates.
Calciumdichloride is also used in domestic and industrial chemical air dehumidifiers.
Calciumchloride is used in concrete mixes to accelerate the initial setting, but chloride ions lead to corrosion of steel rebar, so Calciumdichloride should not be used in reinforced concrete.
The anhydrous form of calciumchloride may also be used for this purpose and can provide a measure of the moisture in concrete.
Calciumchloride is included as an additive in plastics and in fire extinguishers, in blast furnaces as an additive to control scaffolding (clumping and adhesion of materials that prevent the furnace charge from descending), and in fabric softener as a thinner.
The exothermic dissolution of calciumchloride is used in self-heating cans and heating pads.
Calciumchloride is used as a water hardener in the maintenance of hot tub water, as insufficiently hard water can lead to corrosion and foaming.
In the oil industry, calcium chloride is used to increase the density of solids-free brines.
Calciumdichloride is also used to provide inhibition of swelling clays in the water phase of invert emulsion drilling fluids.
Calciumdichloride acts as flux material, decreasing the melting point, in the Davy process for the industrial production of sodium metal through the electrolysis of molten NaCl.
Calciumdichloride is also used in the production of activated charcoal.
Calciumdichloride can be used to precipitate fluoride ions from water as insoluble CaF2.
Calciumdichloride is also an ingredient used in ceramic slipware.
Calciumdichloride suspends clay particles so that they float within the solution, making it easier to use in a variety of slipcasting techniques.
Pharmaceutical Applications
The main applications of Calciumdichloride as an excipient relate to its dehydrating properties and, therefore, it has been used as an antimicrobial preservative, as a desiccant, and as an astringent in eye lotions.
Therapeutically, Calciumdichloride injection 10% (as the dihydrate form) is used to treat hypocalcemia.
Food
In the food industry, calciumchloride is frequently employed as a firming agent in canned vegetables, particularly for canned tomatoes and cucumber pickles.
Calciumdichloride is also used in firming soybean curds into tofu and in producing a caviar substitute from vegetable or fruit juices.
Calciumdichloride is also used to enhance the texture of various other products, such as whole apples, whole hot peppers, whole and sliced strawberries, diced tomatoes, and whole peaches.
The firming effect of calciumchloride can be attributed to several mechanisms:
Complexation, since calcium ions form complexes with pectin, a polysaccharide found in the cell wall and middle lamella of plant tissues.
Membrane stabilization, since calcium ions contribute to the stabilization of the cell membrane.
Turgor pressure regulation, since calcium ions influence cell turgor pressure, which is the pressure exerted by the cell contents against the cell wall.
Calciumchloride's freezing-point depression properties are used to slow the freezing of the caramel in caramel-filled chocolate bars.
Also, Calciumdichloride is frequently added to sliced apples to maintain texture.
In brewing beer, calcium chloride is sometimes used to correct mineral deficiencies in the brewing water.
Calciumdichloride affects flavor and chemical reactions during the brewing process, and can also affect yeast function during fermentation.
In cheesemaking, calciumchloride is sometimes added to processed (pasteurized/homogenized) milk to restore the natural balance between calcium and protein in casein.
Calciumdichloride is added before the coagulant.
Calcium chloride is also commonly used as an "electrolyte" in sports drinks and other beverages; as a food additive used in conjunction with other inorganic salts it adds taste to bottled water.
Preparation
Calciumdichloride is obtained as a by-product in the manufacture of sodium carbonate (soda ash) by ammonia-soda (Solvay) process.
The process involves the reaction of sodium chloride with calcium carbonate and ammonia.
Calciumdichloride is currently produced in bulk amounts by evaporation of natural underground brines.
In the laboratory, Calciumdichloride can be prepared by treating limestone with hydrochloric acid followed by evaporation of solution to obtain crystals.
The crystals are dehydrated to obtain anhydrous salt.
Calcium oxide or hydroxide may be used instead of carbonate.
In much of the world, Calciumdichloride is derived from limestone as a by-product of the Solvay process, which follows the net reaction below:
2 NaCl + CaCO3 → Na2CO3 + CaCl2
North American consumption in 2002 was 1,529,000 tonnes (3.37 billion pounds).
In the US, most Calciumdichloride is obtained by purification from brine.
As with most bulk commodity salt products, trace amounts of other cations from the alkali metals and alkaline earth metals (groups 1 and 2) and other anions from the halogens (group 17) typically occur.
Reactivity Profile
Bromine trifluoride rapidly attacks the following salts: barium chloride, cadmium chloride, Calciumdichloride, cesium chloride, lithium chloride, silver chloride, rubidium chloride, potassium bromide, potassium chloride, potassium iodide, rhodium tetrabromide, sodium bromide, sodium chloride, and sodium iodide.
Long term exposure of Calciumdichloride solution upon a zinc coated galvanized iron vessel caused slow evolution of hydrogen which ignited and exploded.
