PRODUCTS

CALCIUMCHLORIDE

Calciumchloride is used in the setting bath to activate the sodium alginate.
Calciumchloride for use in spherification and molecular gastronomy.
Calciumchloride is a salt of calcium and chlorine.

CAS Number: 10043-52-4
22691-02-7 (monohydrate)
10035-04-8 (dihydrate)
25094-02-4 (tetrahydrate)
7774-34-7 (hexahydrate)
EC Number: 233-140-8
E number: E509 (acidity regulators, ...)
Chemical formula: CaCl2
Molar mass: 110.98 g·mol−1

SYNONYMS:
Calcium chloride, Neutral calcium chloride, calcium(II) chloride, calcium dichloride (1:2), E509, 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, CaCl2H4O2, Calcium Chloride, Dihydrate, Calcium Dichloride.

Calciumchloride is an inorganic compound, a salt with the chemical formula CaCl2.
Calciumchloride is a white crystalline solid at room temperature, and it is highly soluble in water.
Calciumchloride can be created by neutralising hydrochloric acid with calcium hydroxide.

Calciumchloride is an ionic compound of calcium and chlorine.
Calciumchloride is highly soluble in water and it is deliquescent.
Calciumchloride is a salt that is solid at room temperature, and it behaves as a typical ionic halide.

Calciumchloride is the ionic compound of calcium and chlorine and has a wide variety of uses in many food, industrial and agricultural applications.
Calciumchloride 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, Calciumchloride is used as a desiccant.
Calciumchloride was sprayed on this road to prevent weathering, giving it a wet appearance even in dry weather.
The second largest application of Calciumchloride exploits its hygroscopic nature and the tackiness of its hydrates; Calciumchloride is highly hygroscopic and its hydration is an exothermic process.

A concentrated solution keeps a liquid layer on the surface of dirt roads, which suppresses the formation of dust.
Calciumchloride keeps the finer dust particles on the road, providing a cushioning layer.
If these are allowed to blow away, the large aggregate begins to shift around and the road breaks down.

Using Calciumchloride reduces the need for grading by as much as 50% and the need for fill-in materials as much as 80%
Calciumchloride is one of the most versatile chemicals with endless applications.
Add a small amount of Calciumchloride to each jar of pickles or sauerkraut.

Calciumchloride is designated generally recognized as safe (GRAS) by the U.S. Food and Drug Administration.
Because of its hygroscopic nature, anhydrous Calciumchloride must be kept in tightly-sealed air-tight containers.
Calciumchloride is a crystalline salt that is highly soluble in water.

We use Calciumchloride in some of our laundry products to improve their viscosity and stability.
Calciumchloride can be produced by reacting hydrochloric acid with calcium hydroxide (slaked lime).
Calciumchloride can also be derived from limestone and brine (as by-product of the Solvay process, which produces soda ash from brine).

Calciumchloride is highly hygroscopic, which means it readily absorbs water, and its uses range from de-icing road surfaces, to applications in medicine and food technologies such as ‘self-heating’ meal kits.
Calciumchloride is an ionic compound of calcium and chlorine.

Calciumchloride is highly soluble in water and it is deliquescent.
Calciumchloride is a salt that is solid at room temperature, and it behaves as a typical ionic halide.
Calciumchloride is an inorganic compound, a salt with the chemical formula CaCl2.

Calciumchloride is a white coloured crystalline solid at room temperature, and it is highly soluble in water.
Calciumchloride can be created by neutralising hydrochloric acid with calcium hydroxide.
Calciumchloride is an inorganic compound – a salt with the chemical formula CaCl2.

Calciumchloride is also known as calcium chlorine.
Calciumchloride is a composition of calcium and chloride and is mostly contains two water molecules.
Calciumchloride absorbs moisture intensively and is known as desalting substances.

In much of the world, Calciumchloride is derived from limestone as a by-product of the Solvay process. calcium chlorine can also be obtained from brine purification.
Calciumchloride is not hazardous to the environment but classified as H319 according to GHS (causes serious eye irritation).

Calciumchloride is using in two major fields, food and industrial grades.
CaCl2 is an ionic compound with chemical name Calciumchloride.
It is also called Calciumchloride anhydrous or Calcium dichloride.

Calciumchloride is an ionic compound of chlorine and calcium.
At room temperature, Calciumchloride is a crystalline solid white in colour.
Calciumchloride is highly soluble in water and hence is hygroscopic in nature.

Calciumchloride is odourless and has a very high enthalpy change of solution.
Calciumchloride is widely used for dust control and de-icing.
Calciumchloride is prepared as by the following;

By reacting calcium carbonate and hydrochloric acid or
Directly from limestone, but a large amount is also produced as a by-product of the Solvay process.
Calciumchloride was discovered in the 15th century but received little attention or study until the latter part of the 18th century.

All of the early work was done with laboratory-prepared samples since it was not produced on a commercial scale until after the ammonia-soda process for the manufacture of soda ash was in operation.
It was actually considered a waste product until its uses were discovered.

A crystalline, white substance, soluble in water, Calciumchloride is the chloride salt of calcium, a bivalent metallic element with many crucial biological roles.
Calcium is a major constituent of the skeleton but plays many roles as an intracellular and plasma ion as well.

Calciumchloride is a type of inorganic salt that comprises about 0.1% of the ocean, is harmless to the human body and is used as a food additive.
Calciumchloride is an inorganic, white crystalline salts which is highly soluble in water.
Calciumchloride can be created by neutralising hydrochloric acid with calcium hydroxide or as a by-product from the Solvay process to generating Sodium

Carbonate from the reaction of Sodium Chloride brine with Calcium Carbonate.
Calciumchloride is a white to off-white solid. Sinks and mixes with water.
Calcium dichloride is a calcium salt, an inorganic chloride and an inorganic calcium salt.

Calciumchloride has a role as a fertilizer.
Calciumchloride is an ionic compound of calcium and chlorine.
Calciumchloride is highly soluble in water and it is deliquescent.

Calciumchloride is a salt that is solid at room temperature, and it behaves as a typical ionic halide.
Calciumchloride has several common applications such as brine for refrigeration plants, ice and dust control on roads, and in cement.
Calciumchloride can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process.

Because of its hygroscopic nature, Calciumchloride must be kept in tightly-sealed containers.
Chemical formula of Calciumchloride is the salt form of calcium and chlorine.
Hygroscopic is an ionic chemical that is solid at room temperature and should be kept in anhydrous Calciumchloride, air-tight containers due to its hygroscopic structure.

The solubility of water is exothermic.
Low freezing point and high usage area are widespread.
Calciumchloride is soluble in water and alcohol.

Calciumchloride serves as source of calcium ion in solution.
Calciumchloride causes precipitation due to insoluble calcium compounds.
Calciumchloride is a crystalline, white substance, soluble in water. Calciumchloride is the chloride salt of calcium, a bivalent metallic element with many crucial biological roles.

Calcium is a major constituent of the skeleton but plays many roles as an intracellular and plasma ion as well.
In medicine, Calciumchloride is also used as a 10% solution in injection, for calcium replenishment. (NCI04)
Calciumchloride is a small molecule drug with a maximum clinical trial phase of IV (across all indications) and is indicated for hypocalcemia and has 7 investigational indications.

Calciumchloride is hygroscopic, which means it attracts moisture from its environment.
This quality makes Calciumchloride a good chemical to use for suppressing dust on gravel roads and other byways.
Calciumchloride is a common ingredient in sports drinks.

When it dissolves in water, it splits into positive calcium ions and negative chlorine ones, and because the Calciumchloride formula includes two chloride ions, it creates a more powerful electrolyte than sodium chloride, which has only one.
The ability of Calciumchloride to completely dissociate into its component ions gives the compound a salty taste, and it could be a substitute for table salt were it not so hygroscopic.

However, its propensity to absorb water causes intestinal problems and abdominal pain if you ingest Calciumchloride in large amounts.
Calciumchloride is an inorganic compound, a salt with the chemical formula CaCl 2 .

Calciumchloride is a white colored crystalline solid at room temperature, highly soluble in water.
Calciumchloride can be created by neutralizing hydrochloric acid with calcium hydroxide.

USES and APPLICATIONS of CALCIUMCHLORIDE:
Calciumchloride is used to prevent ice formation and therefore used in deicing.
Calciumchloride is used in the production of activated charcoal.
Calciumchloride is used as a sterilant for male animals.

Calciumchloride is used in heating pads and self-heating cans.
Calciumchloride is used to correct the mineral deficiencies in brewing beer
Calciumchloride is used as an electrolyte in sports drinks

In laboratories, the drying tubes are usually packed with Calciumchloride.
As it is moisture absorbent, Calciumchloride is used as a dust collector in construction sites.
Calciumchloride is used as an additive material in the plastic industry

Calciumchloride is used as an additive in fire powders.
Calciumchloride is used melting ice on roads (does not harm the environment like regular salt)
Concrete/Cement: Calciumchloride provides durability and strength to the concrete by drying it quickly, especially in cold weather.

In purification: Calciumchloride is used in reducing high fluoride levels in drinking water.
Calciumchloride is used also in the treatment of wastewater from industrial facilities such as oil refineries and aluminum factories.
Oil Exploration/Drilling: Calciumchloride is used extensively.

Calciumchloride is used in sports drinks.
Calciumchloride is used in canned foods (especially pickles).
Calciumchloride is used in some chocolate products.

Calciumchloride is used in milk, cheese (as a calcium additive).
Calciumchloride is used in brewing (as an enzyme).
Calciumchloride is used in ice cream: As a freezer.

Calciumchloride is used in animal feed: In dairy cattle, to reduce milk fever and prevent disease.
Calciumchloride is used in providing calcium to plants.
Calciumchloride is used in reducing sodium levels in soil.

Calciumchloride is used extending the shelf life of fruits and vegetables at harvest time.
Some uses of Calciumchloride in the food industry include: the acceleration of coagulation in the cheese manufacturing process, the production of beer and soft drinks, increasing the firmness and shelf life of fruit, meat tenderization, and sodium content reduction.

Industrial applications include dust binding/control, winter road maintenance services and de-icing, construction materials (cement and concrete acceleration), agricultural nutrients, and oil and gas exploration.

In water treatment, Calciumchloride is used for nanofiltration, flocculation, and precipitation of fluorides, sulfates, and phosphates.
Calciumchloride has several common applications such as brine for refrigeration plants, ice and dust control on roads, and in cement.
Calciumchloride can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process.

Because of its hygroscopic nature, Calciumchloride must be kept in tightly-sealed containers.
Calciumchloride 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, Calciumchloride is used as a desiccant.
Calciumchloride is used in concrete mixes to accelerate the initial setting, but chloride ions lead to corrosion of steel rebar, so it 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, Calciumchloride is used to increase the density of solids-free brines.

Calciumchloride is also used to provide inhibition of swelling clays in the water phase of invert emulsion drilling fluids.
Calciumchloride (CaCl2) 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.

Calciumchloride is also used in the production of activated charcoal.
Calciumchloride can be used to precipitate fluoride ions from water as insoluble CaF2.
Calciumchloride is also an ingredient used in ceramic slipware.

Calciumchloride suspends clay particles so that they float within the solution, making it easier to use in a variety of slipcasting techniques.
Calciumchloride solution is used immediately after preparation to prevent potential alterations in its chemical composition.

Besides that, Calciumchloride is highly hygroscopic, meaning it readily absorbs moisture from the air.
If the solution is left standing, Calciumchloride can absorb additional water vapor, leading to dilution and a decrease in the intended concentration.

Prolonged standing may lead to the precipitation of calcium hydroxide or other insoluble calcium compounds, reducing the availability of calcium ions in the solution and reducing the effectiveness of the solution as a calcium source for plants.
Nutrient solutions can become a medium for microbial growth if stored for extended periods.

Microbial contamination may alter the composition of the solution and potentially introduce pathogens to the plants.
When dissolved in water, Calciumchloride can undergo hydrolysis, especially over time, which can lead to the formation of small amounts of hydrochloric acid and calcium hydroxide:
Ca+2+2H2O ⇌ Ca(OH)2+2H+

This reaction can lower the pH of the solution, making it more acidic.
Acidic solutions may harm plant tissues and disrupt nutrient uptake.
Calciumchloride dihydrate (20 percent by weight) dissolved in ethanol (95 percent ABV) has been used as a sterilant for male animals.

The solution is injected into the testes of the animal.
Within one month, necrosis of testicular tissue results in sterilization.
Calciumchloride is used to treat or prevent low calcium levels.

Calciumchloride is used to protect the heart from high potassium levels.
Calciumchloride is used to protect the heart and lungs from high magnesium levels.
Calciumchloride may be given to you for other reasons.

Key applications of Calciumchloride: Beverage processing, Food additive, Water treatment, De-icer, Pulp and paper, Agricultural, Personal care, Cosmetic products, Industries, Pulp & Paper, Pharma, Energy Services, Cleaning, CASE & Construction, Polymers, Mining,
Beauty & Personal Care, Water Treatment, Food & Nutrition, Animal Nutrition, Agriculture, Lubricants, Chemical Processing, and Rubber.

Main uses of Calciumchloride: Antifreezing, de-icing, dehumidifying, dust-control, waste liquid treatment, etc.
Calciumchloride is used for antifreezing, de-icing, brine for refrigerators, dust-resistant agents for road surfaces or sports arenas, water waste treatment, etc.

In medicine, Calciumchloride is also used as a 10% solution in injection, for calcium replenishment.
Calciumchloride is used in many applications.
Calciumchloride food grade is used as food ingredient in the food industry (a.o. cheese production).

While other grades are used in the oil and gas industry, in fertilisers or animal feed and in road maintenance.
Calciumchloride is used as a sequestrant and firming agent.
Calciumchloride is one of the primary ingredients in direct spherification.

Calciumchloride is used in the setting bath to activate the sodium alginate.
Calciumchloride for use in spherification and molecular gastronomy.
Calciumchloride is a salt of calcium and chlorine.

Due to it's extremely salty taste, Calciumchloride should not be used in reverse spherification.
Calciumchloride has several common applications such as brine for refrigeration plants, ice and dust control on roads, and in cement.
Calciumchloride can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process.

Because of its hygroscopic nature, Calciumchloride must be kept in tightly-sealed containers.
Food: In this sector, Calciumchloride is used as an additive in canned foods, milk and cheese products, as an enzyme in the beer sector, as a freezer in the freezing sector and as an additive in animal feed.

Agriculture: In the agricultural sector, Calciumchloride is used to reduce the calcium deficiency of plants, to decrease the sodium level in the soil and to extend the shelf life of the products.
Construction-Building: Calciumchloride is used as a dust catcher in constructions due to its moisture-absorbing property.

Chemistry: In the chemical industry, Calciumchloride is used in the drying (removal of water) of many organic compounds, such as saturated olefylic and aromatic hydrocarbons, alkyl halides and esters, and their aqueous solutions.
Calciumchloride is used to treat or prevent low calcium levels.

Calciumchloride is used as an additive material in the plastics industry and fire dusts.
Calciumchloride used to replenish calcium levels, as an acid-producing diuretic, and as an antidote for magnesium poisoning.

-CaCl2 Uses on Roads and Highways
Like sodium chloride, Calciumchloride lowers the melting point of ice, so one of its most common uses is for road deicing.
Calciumchloride works at much lower temperatures — minus 20°F vs. 20°F for rock salt — because it actually releases heat in an exothermic reaction when it dissolves.

Calciumchloride costs more per pound than rock salt, but you need less of it to do the same amount of deicing.
Deicing products often contain both sodium chloride and Calciumchloride.

-what is the main use of Calciumchloride
Calciumchloride is often used for de-icing or dust control on gravel roads, in food or as the absorbing agent in desiccants.
In much of the world, Calciumchloride is derived from limestone as a by-product of the Solvay process.
Calciumchloride can also be obtained from brine purification.

-Uses of Calciumchloride
When a no chemist thinks of salt, NaCl (sodium chloride) comes instantly to mind, but for a chemist, many other compounds also fit the bill, and
Calciumchloride is one of them.
The CaCl2 compound name is Calciumchloride.

Like table salt, it’s a white crystal at room temperature, but Calciumchloride has properties that clearly set it apart.
Calciumchloride can be obtained by refining soda ash, natural brine, or limestone.

Calciumchloride dissolves readily in water and will actually turn to liquid if left long enough in a humid environment.
Common uses include deicing roads, accelerating the set time of concrete, controlling humidity, and improving the taste of beer.

-De-icing and freezing-point depression uses of Calciumchloride:
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 Calciumchloride.
Calciumchloride is relatively harmless to plants and soil.

As a de-icing agent, Calciumchloride is much more effective at lower temperatures than sodium chloride.
When distributed for this use, Calciumchloride 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.

Calciumchloride is also used in domestic and industrial chemical air dehumidifiers.
Calciumchloride is used in domestic and industrial chemical air dehumidifiers.

-Calciumchloride uses in the Food Industry
Calciumchloride is safe to consume and is a common food additive. Calciumchloride adds firmness to cheese, tofu, and canned fruits and vegetables, and it provides a way to enhance the salty taste of pickles without adding extra sodium.
Brewers add Calciumchloride to the water they use to make beer to lower the pH and add alkalinity, which improves the taste.

-Areas of Use:
Calciumchloride chloride and production, the water-soluble aquo complex [Ca (lH 2 O) 6 ] 2+ .
In this way, these solutions are sources of "free" calcium and free chloride ions.

This explanation is illustrated by the reaction of these solutions with phosphate sources to give a solid precipitate of calcium phosphate:
3 CaC2 + 2 PO3-
4 Ca → 3 (PO 4 ) 2 + 6 Cl -

Calciumchloride exhibits a very high enthalpy change, indicated by the considerable temperature increase accompanying dissolution of the anhydrous salt in water.
This property forms the basis of Calciumchloride's largest-scale application.

Molten Calciumchloride can be electrolyzed to yield calcium metal and chlorine gas.
CaC 2 , Ca + Cl → 2

-Drilling Fluid Additive uses of Calciumchloride:
Onshore and offshore oil and gas producers rely heavily on custom-formulated clear brine fluids containing Calciumchloride for all types of drilling and completion applications.

These fluids are used in oilfield completion and workover operations to reduce water activity and create osmotic forces to prevent absorption of water by shales.

The divalent calcium ion inhibits clay swelling, dispersion and migration.
Water containing high concentrations of Calciumchloride can be used as a kill fluid in production wells, especially those containing heavy concentrations of carbon dioxide.

-Oil and petrochemical industry uses of Calciumchloride:
The moisture absorption property of Calcium Chlorine helps petrochemical industry to remove water from hydrocarbons.
Calciumchloride is also useful for drying materials such as Ethane, Butane, Propane, Diesel Fuels etc.

The other common application for Calciumchloride is controlling pressure in industrial solutions.
In addition to above usage, Calciumchloride can act as swelling agents in drilling mud.

-Deicing and preventing road freezing uses of Calciumchloride:
Calciumchloride is used to prevent water freezing, especially on road surfaces, due to its ability to reduce the freezing point.

During the dissolution of Calciumchloride, significant heat is released, and this heat helps to melt the ice on the road surface.
It works better at low temperatures than other deicing agents such as Potassium Chloride and Urea, Magnesium chloride.

Calciumchloride melts a larger volume of ice at lower temperatures than other deicing.
Calciumchloride also increases the melting rate at low temperatures.

This type of chloride is naturally liquid and retains Calciumchloride's affinity for returning to the liquid state.
The use of this inorganic material will be very effective in places with high humidity.

-Calciumchloride in Food industry:
The importance of Calcium in the body has led to the widespread use of Calciumchloride in the production of various foods.
This inorganic chemical, Calciumchloride, is used to increase the strength of fruits and vegetables during the cooking process.

Calciumchloride is Widely used in production of cheeses, canned fruits and vegetables, energy drinks and etc. as a flavoring and additive.
Calciumchloride reacts with the pectin in fruits and prevents these products from becoming too soft during canning.

In the preparation and production of cheese, Calciumchloride causes the cheese to harden and form.
Calciumchloride in milk affects coagulation and clotting time.

-Calciumchloride usage in Concrete industry:
Calciumchloride has an accelerating role in making concrete.
Mixture of Calciumchloride with concrete and water and then sand and cement can make quick-setting concretes.

In this method, instead of using quick-setting cement, ordinary cement with Calciumchloride Can be replaced Concrete made with this method is more resistant to erosion.
But these concretes are more vulnerable to sulfate attack and concrete drop increases by about 10 to 15 percent.

The worst disadvantage of this method is corrosion effect on steel structures.
The use of Calciumchloride is allowed only in non-steel concretes and its consumption is limited to 2% by weight of cement.

-Water Treatment uses of Calciumchloride:
Calciumchloride is used in wastewater treatment applications to remove undesired impurities.

The petroleum, metal working, laundry, textile and food processing industries add Calciumchloride to oily waste streams to cause oil droplets to float to the surface where they can be removed by skimming.

When Calciumchloride is added to water containing fluorides, silicates, phosphates, sulfates, and heavy metals, it reacts with the contaminants to form highly insoluble salts, which precipitate, settle and can then be removed from the bottom of the stream.

-Agriculture industry uses of Calciumchloride:
Calciumchloride fertilizer is one of the fertilizers that compensates for the lack of Calcium in the soil and is widely used in agriculture.
Calcium is one of the most important nutrients for plant growth.

This fertilizer helps to absorb nutrients, increase plant resistance, create stronger cell walls and better transfer of phosphorus in the plant.
Calciumchloride can also improve soil properties and regulate the amount of sodium in the soil.

-Using Calciumchloride in Construction
Because Calciumchloride absorbs water so well, and it generates heat when doing so, cement workers add it to concrete to accelerate the cure rate at low temperatures.

The addition of a 2 percent concentration creates the same cure rate at 50°F as plain concrete has at 70°F.
Kits for testing the moisture content of concrete slabs typically contain Calciumchloride in a container.

Because Calciumchloride absorbs off-gassing water vapor from the slab, the test consists of weighing the container, leaving it on the slab for a prescribed period, weighing it again, and recording the gain in weight.

-Uses of Calciumchloride:
The environment influences pool water–from leaves swirling down, to the swimmers, to airborne dust particles.
All this affects the quality of the water, thus the need for constant cleaning and filtration.

In addition, the water should have a proper balance of acidity, alkalinity, and calcium hardness.
Calciumchloride maintains calcium hardness.

-Uses of Calciumchloride in Hard and Soft Water:
Hard water is water oversaturated with calcium and magnesium.
This excess calcium settles on the pool surfaces creating rough spots.

It looks like a crystallized, whitish scale and feels like a rough spot.
Soft water is low in calcium carbonate–it is undersaturated.

Here the water becomes corrosive in its attempt to obtain the calcium.
It pits pool surfaces and corrodes pipes and fixtures.

*Correcting Pool Balance with Calciumchloride
You can correct both hard and soft water conditions.

If the pool water is undersaturated, then add Calciumchloride to bring the level in balance.
If the pool water is hard then you have to reduce the amount of Calciumchloride in the water to balance it.

MEDICAL USE OF CALCIUMCHLORIDE:
Calciumchloride infusions may be used as an intravenous therapy to prevent hypocalcemia.
Calciumchloride is a highly soluble calcium salt.
Hexahydrate Calciumchloride (CaCl2·6H2O) has solubility in water of 811 g/L at 25 °C.

Calciumchloridewhen taken orally completely dissociates into calcium ions (Ca2+) in the gastrointestinal tract, resulting in readily bioavailable calcium.
The high concentration of calcium ions facilitates efficient absorption in the small intestine.

However, the use of Calciumchloride as a source of calcium taken orally is less common compared to other calcium salts because of potential adverse effects such as gastrointestinal irritation and discomfort.
When tasted, Calciumchloride exhibits a distinctive bitter flavor alongside its salty taste.

The bitterness is attributable to the calcium ions and their interaction with human taste receptors: certain members of the TAS2R family of bitter taste receptors respond to calcium ions; the bitter perception of calcium is thought to be a protective mechanism to avoid ingestion of toxic substances, as many poisonous compounds taste bitter.

While chloride ions (Cl⁻) primarily contribute to saltiness, at higher concentrations, they can enhance the bitter sensation.
The combination of calcium and chloride ions intensifies the overall bitterness.
At lower concentrations, Calciumchloride may taste predominantly salty.

The salty taste arises from the electrolyte nature of the compound, similar to sodium chloride (table salt).
As the concentration increases, the bitter taste becomes more pronounced: the increased presence of calcium ions enhances the activation of bitterness receptors

FOOD USES OF CALCIUMCHLORIDE:
In the food industry, Calciumchloride is frequently employed as a firming agent in canned vegetables, particularly for canned tomatoes and cucumber pickles.
Calciumchloride is also used in firming soybean curds into tofu and in producing a caviar substitute from vegetable or fruit juices.

Calciumchloride 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, Calciumchloride is frequently added to sliced apples to maintain texture.
In brewing beer, Calciumchloride is sometimes used to correct mineral deficiencies in the brewing water.
Calciumchloride 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.
Calciumchloride is added before the coagulant.

Calciumchloride 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.
The average intake of Calciumchloride as food additives has been estimated to be 160–345 mg/day.

Calciumchloride is permitted as a food additive in the European Union for use as a sequestrant and firming agent with the E number E509.
Calciumchloride is considered as generally recognized as safe (GRAS) by the U.S. Food and Drug Administration.
Calciumchloride's use in organic crop production is generally prohibited under the US National Organic Program.

The elemental calcium content in Calciumchloride hexahydrate (CaCl2·6H2O) is approximately 18.2%.
This means that for every gram of Calciumchloride hexahydrate, there are about 182 milligrams of elemental calcium.

For anhydrous Calciumchloride (CaCl2), the elemental calcium content is slightly higher, around 36.1% (for every gram of anhydrous Calciumchloride there are about 361 milligrams of elemental calcium).

Calciumchloride has a very salty taste and can cause mouth and throat irritation at high concentrations, so it is typically not the first choice for long-term oral supplementation (as a calcium supplement).

Calciumchloride, characterized by its low molecular weight and high water solubility, readily breaks down into calcium and chloride ions when exposed to water.
These ions are efficiently absorbed from the intestine.

However, caution should be exercised when handling Calciumchloride, for it has the potential to release heat energy upon dissolution in water.
This release of heat can lead to trauma and burns in the mouth, throat, esophagus, and stomach.

In fact, there have been reported cases of stomach necrosis resulting from burns caused by accidental ingestions of big amounts of undissolved Calciumchloride.

The extremely salty taste of Calciumchloride is used to flavor pickles without increasing the food's sodium content.
Calciumchloride is used to prevent cork spot and bitter pit on apples by spraying on the tree during the late growing season.

CALCIUMCHLORIDE STRUCTURE:
Calciumchloride molecules feature two ionic bonds between the single calcium cation and the two chloride anions.
The structure of Calciumchloride molecules is illustrated below.
Calciumchloride can be noted that the calcium cation holds a charge of magnitude +2 and each chloride anion holds a charge of magnitude -1.
Calciumchloride is, therefore, electrically neutral.

PREPARATION OF CALCIUMCHLORIDE:
The steps listed below can be followed in order to prepare Calciumchloride:

Step 1:
Take a beaker.
Wear gloves and place limestones in it until the beaker is filled up by a quarter of its total volume.

Step 2:
Add approximately 1/4th of a beaker of HCl (hydrochloric acid) to the limestones.

Step 3:
As the HCl dissolves the limestone it starts to bubble.
Mix the contents in the beaker gently and take care that the reaction completes.
Add a little limestone if all the limestones dissolve in it completely.

Step 4:
Filter off the solids by pouring the solution through the filter paper as soon as the solution stops bubbling.

Step 5:
Heat the second beaker which contains the Calciumchloride solution.
Solid Calciumchloride is the solid left after the water evaporates.

CALCIUMCHLORIDE SOLUTIONS:
Calciumchloride is highly soluble in water, because of its high solubility it is used to obtain solutions having relatively high densities.
For example, densities as high as 1430kg/m3 are achieved at 208oC and 1570kg/m3 at 808oC.

The oil and gas drilling industries frequently exploit these high densities when completing or reworking wells.
Density or specific gravity can also be used to determine the molal concentration, c of Calciumchloride in water.

The densities of Calciumchloride solution at various values and different temperatures have been identified.
Densities and apparent molar volumes of aqueous Calciumchloride solutions at temperatures from 323K to 600K and at pressure up to 40MPa have also been reported.

Viscosity is an important property of Calciumchloride solutions in terms of engineering design and in application of such solutions to flow through porous media.

Data and equations for estimating viscosity of Calciumchloride solutions over the temperature range of 20-508oC are available.
Numerous studies on the thermodynamics of Calciumchloride solutions were published in the 1980s.

Many of these were oriented toward verifying and expanding the Pitzer equations for determination of activity coefficients and other parameters in electrolyte solutions of high ionic strength.

Calciumchloride is produced in commercial amounts using many procedures: refining of natural brines, reaction of calcium hydroxide with ammonium chloride in Solvay soda ash production and reaction of hydrochloric acid with calcium carbonate.

A property possessed by some substances of absorbing moisture from the air on exposure.
Anhydrous Calciumchloride, which possesses this property, is widely used as a drying agent.

PRODUCTION AND REACTIONS OF CALCIUMCHLORIDE:
Calciumchloride can be produced directly from limestone.
Another production path can be obtained as a high by-product by the solvent method.

PURIFICATION OF CALCIUMCHLORIDE:
While Calciumchloride is used to reduce the high fluoride level in drinking water, it is widely used in the treatment of waste water in industrial plants such as oil refineries and aluminum factories.

CALCIUMCHLORIDE FOR HUMIDITY CONTROL:
Calciumchloride is more than just hygroscopic; it is deliquescent, which means it can absorb enough moisture to turn to liquid brine at room temperature.
Calciumchloride’s the most common ingredient in moisture absorbers available at big box stores for controlling humidity in drawers and closets.
You often find Calciumchloride combined with baking soda, which is a deodorizer.

Dehumidifying with Calciumchloride is not without its hazards.
Calciumchloride is corrosive and promotes rust, so it should not be used around metals.

Moreover, prolonged exposure can cause respiratory issues and lung damage.
Silica gel is a safer desiccant and is often used instead of Calciumchloride.

PROPERTIES OF CALCIUMCHLORIDE:
Calciumchloride 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−
Calciumchloride 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 Calciumchloride's largest-scale application.
Aqueous solutions of Calciumchloride tend to be slightly acidic due to the influence of the chloride ions on the hydrogen ion concentration in water.

The slight acidity of Calciumchloride 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.

Molten Calciumchloride can be electrolysed to give calcium metal and chlorine gas:
CaCl2 → Ca + Cl2

HISTORY OF CALCIUMCHLORIDE:
Calciumchloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century.
It was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum) because Calciumchloride 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.) it was called "muriate of lime" (Latin: murias calcis, calcaria muriatica).

FEATURES OF CALCIUMCHLORIDE:
Calciumchloride is highly absorbent, highly deliquescent and can easily be dissolved in water.
When dissolved into water, Calciumchloride creates a large amount of solution heat and greatly lowers the freezing point of water, with strong antifreezing and de-icing effects.
Reaction） CaCO3 + 2HCl > CaCl2 Calcium chlorid + H2O + CO2

OCCURRENCE OF CALCIUMCHLORIDE:
Calciumchloride occurs as the rare evaporite minerals sinjarite (dihydrate) and antarcticite (hexahydrate).
Another natural hydrate known is ghiaraite – a tetrahydrate.
The related minerals chlorocalcite (potassium Calciumchloride, KCaCl3) and tachyhydrite (calcium magnesium chloride, Ca Mg2Cl6·12H2O) are also very rare.
The same is true for rorisite, CaClF (Calciumchloride fluoride).

HOW TO USE CALCIUMCHLORIDE IN POOLS:
The proper way to perform the addition of Calciumchloride is to add a little at a time.
Wait for Calciumchloride to dissolve, (about four hours) and then test the water.
Add more only if needed.

Thus, you do not oversaturate the water.
There are three ways of reducing the amount of Calciumchloride. You can dilute the pool water with fresh water, or add sequestering agents that keep the calcium in suspension.

In extreme cases, you may have to drain the pool completely.
The recommended hardness range is 200-400 ppm.
Test weekly for the hardness level.

ABSORPTION EFFICIENCY OF CALCIUMCHLORIDE:
A desiccant’s absorption capacity greatly depends on the following factors:
*Moisture available (high temperature and high relative humidity).
*The higher – the more absorption
*Duration of the test
*The longer – the more absorption
*The below diagrams illustrate absorption in different conditions, absorption from AbsorGel and ‘traditional’ desiccants like clay, silica and Calciumchloride 77-94%.
Both diagrams are based on climate chamber tests and should not be used for ‘real condition’ dimensioning.

WHY CALCIUMCHLORIDE?
Calciumchloride is highly effective, and one of the most hygroscopic materials, when it comes to absorbing moisture from the surrounding air.
Calciumchloride is an inorganic compound – a salt with the chemical formula CaCl2.
Calciumchloride is white flakes or pellets at room temperature, and is highly soluble in water.

Calciumchloride desiccants work well over a temperature range from freezing point up to 80 °C or more.
Calciumchloride is the active compound in all Absortech products.

Calciumchloride is often used for de-icing or dust control on gravel roads, in food or as the absorbing agent in desiccants.
In much of the world, Calciumchloride is derived from limestone as a by-product of the Solvay process.

Calciumchloride can also be obtained from brine purification.
Calciumchloride is not hazardous to the environment but classified as H319 according to GHS (causes serious eye irritation).

Calciumchloride is available in different concentrations and is often specified as 74-77% or 94-97% depending on the purity level.
The higher the concentration, the better the absorption capacity.
Meaning a desiccant with 94-97% Calciumchloride has the ability to absorb more moisture than 74-77% CaCl2.

Absortech uses Calciumchloride as the absorbing agent in our desiccants due to its high efficiency compared to other types of desiccants, such as silica gel and clay desiccants.

*Superior by nature
Calciumchloride absorbs moisture from the air effectively.
Calciumchloride can attract several times its own weight in water, dissolving into a liquid brine if the air is humid enough and the temperature is high enough.
The liquid brine is either trapped inside a collector or mixed with a modified starch and thereby formed as a gel inside its packaging.

*Absorption capacity
Calciumchloride desiccant absorbs more moisture when the relative humidity (RH) of the surrounding air is higher.
And Calciumchloride's absorption increases exponentially as RH rises, which is a remarkable result compared to other desiccants like silica gel and clay.

*The sustainable option
Other desiccants may include toxic substances.
For example, silica gel with indicators, can include the toxic substance cobalt.

Whereas Calciumchloride is a natural product with no negative affect on the environment.
But the main environmental advantage of using Calciumchloride desiccants compared to other types of desiccants is, of course, that these desiccants are much more efficient and thereby the amount and weight of desiccants used for the same protection is much lower.

By choosing the most efficient desiccants, huge savings can be made on plastic, transport and the CO2 footprint as a result.
And cutting down on CO2 is one of the most important challenges that we have for the future.

LABORATORY AND RELATED DRYING OPERATIONS OF CALCIUMCHLORIDE:
Drying tubes are frequently packed with Calciumchloride.
Kelp is dried with Calciumchloride for use in producing sodium carbonate.

Anhydrous Calciumchloride has been approved by the FDA as a packaging aid to ensure dryness (CPG 7117.02).
The hydrated salt can be dried for re-use but will dissolve in its own water of hydration if heated quickly and form a hard amalgamated solid when cooled.

Metal reduction flux
Similarly, Calciumchloride is used as a flux and electrolyte in the FFC Cambridge electrolysis process for titanium production, where it ensures the proper exchange of calcium and oxygen ions between the electrodes.

PREPARATION OF CALCIUMCHLORIDE:
In much of the world, Calciumchloride 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 Calciumchloride 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.

PHYSICAL and CHEMICAL PROPERTIES of CALCIUMCHLORIDE:
Water Solubility: 21.4 mg/mL
logP: 1.08
logP: -0.65
logS: -0.71
pKa (Strongest Acidic): 15.7
pKa (Strongest Basic): -1.8
Physiological Charge: 0
Hydrogen Acceptor Count: 1
Hydrogen Donor Count: 1
Polar Surface Area: 25.3 Å²

Rotatable Bond Count: 0
Refractivity: 3.7 m³·mol⁻¹
Polarizability: 1.51 Å³
Number of Rings: 0
Bioavailability: 1
Rule of Five: Yes
Ghose Filter: No
Veber's Rule: Yes
MDDR-like Rule: No

CAS Number: 10043-52-4, 22691-02-7 (monohydrate)
10035-04-8 (dihydrate) 25094-02-4 (tetrahydrate)
7774-34-7 (hexahydrate)
PubChem: 24854
ChemSpider: 23237
UNII: OFM21057LP
EC Number: 233-140-8
DrugBank: DB01164
Chebi: 3312
CHEMBL1200668
RTECS Number: EV9800000

ATC Code: A12AA07, B05XA07, G04BA03
Molecular Formula: CaCl₂
Molar Mass: 110.98 g/mol (anhydrous) 128.999 g/mol (monohydrate)
147.014 g/mol (dihydrate) 183.045 g/mol (tetrahydrate)
219.08 g/mol (hexahydrate)
Appearance: White powder
Density: 2.15 g/cm³ (anhydrous) 1.835 g/cm³ (dihydrate)
1.83 g/cm³ (tetrahydrate) 1.71 g/cm³ (hexahydrate)
Melting Point: 772°C (anhydrous) 260°C (monohydrate)
176°C (dihydrate) 45.5°C (tetrahydrate) 30°C (hexahydrate)

Boiling Point: 1935°C (anhydrous)
Solubility in Water: 74.5 g/100 mL (20°C) 59.5 g/100 mL (0°C)
Solubility: Soluble in acetone, acetic acid
Acid (pKa): 8-9 (anhydrous) 6.5-8.0 (hexahydrate)
Refractive Index (nD): 1.52
Chemical Formula: CaCl₂
Molar Mass: 110.98 g·mol⁻¹
Appearance: White hygroscopic powder
Odor: Odorless

Density:
2.15 g/cm³ (anhydrous)
2.24 g/cm³ (monohydrate)
1.85 g/cm³ (dihydrate)
1.83 g/cm³ (tetrahydrate)
1.71 g/cm³ (hexahydrate)
Melting Point: 772–775 °C (1,422–1,427 °F; 1,045–1,048 K) anhydrous
260 °C (500 °F; 533 K) monohydrate, decomposes
175 °C (347 °F; 448 K) dihydrate, decomposes
45.5 °C (113.9 °F; 318.6 K) tetrahydrate, decomposes
30 °C (86 °F; 303 K) hexahydrate, decomposes

Boiling Point: 1,935 °C (3,515 °F; 2,208 K) anhydrous
Solubility in Water:
Anhydrous: 74.5 g/100 mL (20 °C)
Hexahydrate:
49.4 g/100 mL (−25 °C)
59.5 g/100 mL (0 °C)
65 g/100 mL (10 °C)
81.1 g/100 mL (25 °C)
102.2 g/100 mL (30.2 °C)

α-Tetrahydrate:
90.8 g/100 mL (20 °C)
114.4 g/100 mL (40 °C)
Dihydrate:
134.5 g/100 mL (60 °C)
152.4 g/100 mL (100 °C)
Solubility:
Soluble in acetic acid, alcohols
Insoluble in liquid ammonia, dimethyl sulfoxide (DMSO), ethyl acetate

Solubility in Ethanol:
18.3 g/100 g (0 °C)
25.8 g/100 g (20 °C)
35.3 g/100 g (40 °C)
56.2 g/100 g (70 °C)
Solubility in Methanol:
21.8 g/100 g (0 °C)
29.2 g/100 g (20 °C)
38.5 g/100 g (40 °C)

Solubility in Acetone: 0.1 g/kg (20 °C)
Solubility in Pyridine: 16.6 g/kg
Acidity (pKa):
8–9 (anhydrous)
6.5–8.0 (hexahydrate)
Magnetic Susceptibility (χ): −5.47·10⁻⁵ cm³/mol
Refractive Index (nD): 1.52
Viscosity:
3.34 cP (787 °C)
1.44 cP (967 °C)

Structure
Crystal Structure:
Orthorhombic (rutile, anhydrous), oP6
Tetragonal (anhydrous, > 217 °C), oP6
Trigonal (hexahydrate)
Space Group:
Pnnm, No. 58 (anhydrous)
P42/mnm, No. 136 (anhydrous, >217 °C)
Point Group:
2/m 2/m 2/m (anhydrous)
4/m 2/m 2/m (anhydrous, >217 °C)

Lattice Constant:
a = 6.259 Å, b = 6.444 Å, c = 4.17 Å (anhydrous, 17 °C)
α = 90°, β = 90°, γ = 90°
Coordination Geometry: Octahedral at Ca²⁺ centres (anhydrous)
Thermochemistry
Heat Capacity (C):
72.89 J/(mol·K) (anhydrous)
106.23 J/(mol·K) (monohydrate)
172.92 J/(mol·K) (dihydrate)
251.17 J/(mol·K) (tetrahydrate)
300.7 J/(mol·K) (hexahydrate)
Std Molar Entropy (S⦵298): 108.4 J/(mol·K)

Std Enthalpy of Formation (ΔfH⦵298):
−795.42 kJ/mol (anhydrous)
−1110.98 kJ/mol (monohydrate)
−1403.98 kJ/mol (dihydrate)
−2009.99 kJ/mol (tetrahydrate)
−2608.01 kJ/mol (hexahydrate)
Gibbs Free Energy (ΔfG⦵): −748.81 kJ/mol
Molecular Weight: 110.98 g/mol

Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 2
Rotatable Bond Count: 0
Exact Mass: 109.9002962 Da
Monoisotopic Mass: 109.9002962 Da
Topological Polar Surface Area: 0 Å²
Heavy Atom Count: 3
Formal Charge: 0
Complexity: 0
Isotope Atom Count: 0

Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 3
Compound Is Canonicalized: Yes
Physical State: Powder
Color: White
Odor: Odorless

Melting Point/Freezing Point:
Melting Point: 775 °C at 1.013 hPa
Initial Boiling Point and Boiling Range: 1,935 °C at 1.013 hPa
Flammability (Solid, Gas): The product is not flammable.
Upper/Lower Flammability or Explosive Limits: No data available
Flash Point: No data available
Autoignition Temperature: No data available
Decomposition Temperature: No data available
pH: 8 - 10

Viscosity:
Viscosity, Kinematic: No data available
Viscosity, Dynamic: No data available
Water Solubility: 745 g/l at 20 °C - Soluble
Partition Coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor Pressure: 0.01 hPa at 20 °C
Density: 2.15 g/cm³ at 25 °C
Relative Density: No data available
Relative Vapor Density: No data available
Particle Characteristics: No data available
Explosive Properties: No data available
Oxidizing Properties: None
Other Safety Information: No data available

FIRST AID MEASURES of CALCIUMCHLORIDE:
-Description of first-aid measures
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with
water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed.
No data available

ACCIDENTAL RELEASE MEASURES of CALCIUMCHLORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.

FIRE FIGHTING MEASURES of CALCIUMCHLORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Carbon dioxide (CO2)
Foam
Dry powder
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of CALCIUMCHLORIDE:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter A
-Control of environmental exposure:
Do not let product enter drains.

HANDLING and STORAGE of CALCIUMCHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.

STABILITY and REACTIVITY of CALCIUMCHLORIDE:
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Possibility of hazardous reactions:
No data available