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Browsing through the chronicles of chemistry, calcium chloride dihydrate started gaining attention around the 19th century. Early industrialists used it to melt ice off streets before winter’s grip could snarl transport and shut down daily life. By the time folks figured out how to extract it efficiently from brine and limestone, manufacturers realized its benefits stretched far beyond just de-icing roads. Technological leaps tied to the chemical industry in Europe and North America helped turn this simple compound into a multi-purpose commodity. Now, you’ll find its fingerprints on water treatment, construction, food preservation, and even across science labs and hospitals. Each chapter of its story shows how responding to real problems—like urban safety, agricultural yield, and fresh food storage—has kept calcium chloride dihydrate in the picture.
At the most basic level, calcium chloride dihydrate shows up as a white, crystalline substance that’s straightforward to store and transport. It absorbs water from the air, which makes it useful as a drying agent for a long list of practical jobs. Food manufacturers lean on it to keep pickles crisp or cheese intact, while the construction sector depends on it to set concrete and control dust. Chemists keep it close by in the laboratory since it’s a reliable reagent that doesn’t break the bank. Its relatively low cost and wide availability mean it doesn’t stay stuck in a single industry. As demand for durable infrastructure, shelf-stable foods, and dependable industrial agents remains high, calcium chloride dihydrate keeps finding new uses.
This compound, CaCl2·2H2O in chemical terms, stands out for being highly soluble in water—just a handful of crystals can turn a dry glass of water bracingly salty. When humidity spikes, it pulls moisture straight out of the air, clumping together and sometimes even forming puddles if left open long enough. With a melting point below 100°C, it won’t survive open flames, but it won’t catch fire either. Scientists appreciate how calcium chloride dihydrate reacts consistently in lab settings: it increases the boiling point of water, it doesn’t fuss with most common substances, and although it carries a salty flavor, it stays relatively neutral in complicated mixtures.
Anyone who's bought bulk chemicals knows labeling matters. Genuine calcium chloride dihydrate products list purity—usually above 99% for lab or food grades. Labels display CAS number (10035-04-8), proper chemical names, and manufacturer identifiers. SHipping regulations require clear hazard signs and usage instructions, matching GHS pictograms so handlers know what to expect: irritation risks, proper storage, and emergency actions. Since global commerce brings different rules together, clear and accurate technical documentation helps folks avoid confusion. Technical sheets detail storage temperature, recommended containers (plastic, glass, or steel for most uses), and even batch tracking for traceability.
Industrial production of calcium chloride dihydrate usually starts with hydrochloric acid and limestone, which react to form calcium chloride, then the mixture is evaporated to produce the dihydrate crystals. In some parts of the world, natural brine or salt deposits play a starring role, bypassing the acid route for a more sustainable approach. Different factories tweak heat and concentration to fine-tune crystal size or purity, which matters if you’re making de-icing pellets versus crisping agents for packaged greens. Equipment built to handle corrosive and humid environments lines up at these facilities, turning basic minerals into widely-used chemicals by way of careful monitoring.
Ask any seasoned chemist: calcium chloride dihydrate reacts as a strong electrolyte in water, splitting into calcium and chloride ions. Its strong affinity for water leads to rapid hydration and dehydration cycles, providing a tool for moisture removal or chemical drying. Introduce it to carbonates and you’ll see bubbling carbon dioxide; mix it with certain alkalis and you might precipitate calcium carbonate or hydroxides. These predictable reactions let it serve as a buffer in labs, a drying agent in chemistry, or a reactant for industrial syntheses. For folks wanting tailored products, further modifications combine it with stabilizers, anti-caking agents, or acids that swap out one property for another.
You’ll find it under several names: calcium chloride dihydrate, CaCl2·2H2O, E509 (in the food industry), or simply dihydrate if context makes it clear. Some suppliers call it “ice melt,” “de-icing salt,” or “concrete accelerator.” Scientific communities usually stick with the chemical name to avoid confusion, especially since each hydrate level—anhydrous, dihydrate, hexahydrate—delivers different properties for handling and storage. For customers, synonyms can cause headaches, but reading the label and knowing the use case clears up most issues.
People handling calcium chloride dihydrate wear gloves and safety goggles, even though the compound doesn’t burn or explode. It irritates skin and eyes, and even in small amounts can dry out or corrode. Workers rely on ventilation and well-sealed storage to minimize dust and moisture problems. Safety data sheets warn about accidental ingestion, which can cause stomach problems, and suggest rinsing exposed eyes or skin with lots of water. Facility managers trust spill kits and neutralizing agents to keep accidents in check, often running annual drills and updating training whenever new regulations drop. Proper labeling, up-to-date first aid guidance, and regular inspections go a long way toward preventing serious mishaps.
Calcium chloride dihydrate shows up in more places than most people notice. Road crews spread it to cut down on winter ice slicks. Construction firms add it to concrete mixes—especially in cold climates—to get the material curing faster and more reliably. Farmers work it into soil amendments and livestock feed, counting on the extra calcium to boost yields and animal health. Food processors favor it for cheese, bottled vegetables, and sports drinks as a firming or stabilizing agent. In swimming pools, facility managers use it to keep calcium hardness within safe ranges to protect tiles and pipes. Lab technicians depend on its drying power to keep reagents free from unwanted moisture. Hospitals and clinics trust its stability and purity for making saline solutions and other medical supplies. It’s even found a niche in oil and gas drilling as a brine additive.
Research around calcium chloride dihydrate never stands still. Material scientists, for example, are looking for ways it might shore up roads in floods and landslides. Medical researchers use it to refine drug delivery and dialysis fluids, seeking less irritation or better uptake. Climate adaptation efforts experiment with blending it into gritting and dust control formulas that work even as weather patterns change. Food technologists pay close attention to texture and flavor tweaks, especially for plant-based alternatives. Chemical engineers scrutinize its performance in water softening and recycling, setting out to lower costs while cleaning up waste streams. Each advance draws on studies and trials, comparing results to known standards and pushing boundaries for everything from household safety to industrial application.
With widespread use, scientists keep a close watch on toxicity. Animal studies show high doses irritate digestive systems and lungs, supporting advice to keep dust and powder away from faces and food. Regulatory agencies, including the FDA and EPA, set exposure limits and recommend safe handling. Toxicologists run chronic studies to see if any long-term exposure risks sneak up, but so far standard doses in food and water pose little risk to humans. Environmental research tracks runoff, especially in areas with heavy de-icing or agriculture, to ensure no harm to groundwater or soil. Transparency and public awareness about toxicity depend on regular reviews, clearly published results, and careful monitoring at every stage—production, transport, and end use.
The run on calcium chloride dihydrate shows no sign of slowing. Urban planners in cold climates keep stocking up for road treatment, while new markets in dust suppression and building repair pick up steam every year. Food processing looks for safer, more effective firming agents as plant-based foods expand, and technology firms weigh it against other candidates for battery cooling and heat storage. Environmental responsibility points research toward less energy-intensive production or innovative recycling methods out of brine and industrial runoff. Researchers see an opening for greener manufacturing and recovery processes, especially as climate pressures reshape industries and regulations. With no shortage of practical problems still waiting for a fix, calcium chloride dihydrate stands ready to be part of the answer.
Calcium chloride dihydrate stands out in many households and industries. People often see it in winter, tossed onto sidewalks and driveways. It melts ice far better than table salt, helping to keep people upright and cars moving. That same knack for drawing in moisture turns it into a useful product in damp basements. A few scattered pellets help keep corners dry and mildew at bay. Farmers and growers lean on it too. Calcium keeps fruits and vegetables firm, so a solution containing this compound goes onto produce after harvest. Tomatoes and apples arrive firmer and last longer on store shelves. Cheese makers use it during the cheese-making process to help milk curdle just right.
Construction projects take hits from the weather all the time. Calcium chloride dihydrate shortens the wait when a contractor wants to pour concrete, especially on cold days. It speeds up hardening, letting workers push forward without long delays. Crews patching roads in dry spots use it to keep down the dust that comes off the ground. A fine mist sprayed over gravel or dirt roads cuts airborne particles, making neighborhoods cleaner and limiting asthma triggers for nearby families. Even oilfield operators use it to stabilize soil, fighting the shifting ground that can throw equipment off balance.
Water companies add calcium chloride dihydrate to the treatment process. It boosts calcium levels in drinking water, which helps counteract the effect of softening agents that lower mineral content. This keeps pipes safe from corrosion and also supports public health. Many people don’t get enough calcium in their diets, and tap water can supply a steady, overlooked source. After struggling with muscle cramps as a runner, I noticed fewer issues in areas with higher-mineral water. Doctors sometimes recommend this compound through intravenous fluids for patients with dangerously low calcium levels. It keeps muscles and nerves working smoothly, so emergencies in the ER move toward safety, not risk.
Labs and factories use calcium chloride dihydrate for more than just the end product. Chemists rely on its moisture-loving nature during experiments to trap water or dry gases. It serves as a reagent during reactions, helping push things along, whether researchers test soil samples or prepare medicines. Without it, some steps take longer, cost more, or simply don’t work as well. Food-packaging companies put packets of it in boxes to prevent soggy cookies and crackers from losing their crunch. Shoppers may not notice these tiny bags, but they save money and waste in the long run by protecting products from spoilage.
Relying heavily on any chemical raises questions about safety and the environment. Some runoff can damage local waterways and harm plants or aquatic life. I’ve seen grass near busy roads suffer after heavy salting in winter. Manufacturers and municipal workers can look to smarter application practices—using only what’s needed and switching to sand in sensitive spots. Homeowners can sweep up leftover pellets at winter’s end to keep gardens alive. Choosing well means less waste and longer-lasting benefits for the community.
Calcium chloride dihydrate pops up in road de-icing, food preservation, even in concrete work. I’ve pulled bags of it from hardware store shelves, spilled it on my own workbench, and talked shop with people using it in pools or aquariums. It feels basic, not mysterious or sinister. That comfort makes it easy to overlook: what’s actually in the bag, and is it safe on our skin, near our eyes, or left around the garage?
Anyone who’s ever gotten a powdery handful of calcium chloride will remember an itchy spot or even a mild burn. This stuff draws water out of whatever it touches. Dry skin gets prickly, cut skin stings. I’ve seen redness where I brushed it off. Nothing dramatic, not like a strong acid, but ignoring gloves isn’t wise. Eyes need protection too. Like most salts, even a tiny bit in your eye will lead to tears and some pain.
In my years helping out at swim clubs, I heard a few complaints after a loader spilled calcium chloride while opening a bag. Nobody went to the ER, but we learned that rinsing thoroughly under running water beats toughing it out.
Some calcium chloride ends up in food, especially cheese and bottled water. The food-grade form meets strict purity standards, and small amounts pass through us without harm. That said, scooping from a bag labeled “industrial” into a kitchen could go wrong: grit, unknown additives, or higher dust levels qualify as risk.
Dust from big applications – think construction or treating icy roads – carries more risk for the lungs. Breathing in clouds of fine powder over time can irritate airways. I’ve used a simple mask when pouring it on driveways; a solid precaution, especially if wind kicks up clouds.
Once calcium chloride dissolves, it spreads fast and changes the local chemistry in soil and water. Runoff finds its way into streams, where too much salt can harm aquatic life or crops. My experience with local gardening shows stunted growth near driveways treated year after year. It takes neighbors working together to manage how much goes down, or runoff control improves.
Spilling dry calcium chloride on the garage floor usually leads to sweep-up and rinsing. Still, disposal matters. Flushing it into storm drains shifts the problem downstream. Bag up dry remnants, use a lot of water for diluting dissolved spills, and avoid dumping near vegetable beds or flower patches.
Good gloves, eye protection, and fresh air matter more than heavy-duty hazmat suits. Keep bags taped up, label containers, avoid mixing old chemical leftovers. It’s smart to show kids or new helpers the “what not to touch, what not to breathe” talk. Simple routines make the difference: rinse skin, wash clothes if dust settles, check local guides before large disposal.
A quick read of the safety sheet (the SDS) reveals the same advice: don’t be reckless, but don’t fear it. Common sense and a bit of local knowledge keep encounters with calcium chloride dihydrate boring instead of newsworthy.
Calcium chloride dihydrate pops up in a bunch of places—on icy roads in winter, in labs, even in medicine cabinets. Folks sometimes squint at the label and wonder about what’s actually inside that white, grainy stuff. I’ve held a bag of the crystals in my hand, tossed it across slick concrete on cold mornings, and watched it eat away at ice faster than anything else. What’s doing the work? It all comes back to chemistry—the formula that tells the story of every atom.
This compound goes by the formula CaCl₂·2H₂O. That little “dot” and the water molecules on the end matter more than most people realize. The “CaCl₂” gives you calcium chloride itself: one calcium atom paired with two chlorine atoms. Add the “·2H₂O” and you’ve got dihydrate—meaning every molecule of calcium chloride cozies up with two water molecules.
Some of my chemistry teachers liked to say those water molecules are “trapped” inside, woven into the atomic structure. You can see the difference if you heat it—steam rolls off, and the powder left behind turns crumbly and dry. It’s not just dusty trivia. That bit of water changes how the chemical handles moisture, how it dissolves, and even its weight. If you need accurate results for lab work or a batch of homemade pickling salt, using the wrong hydrate version can mess up your measurements by a mile.
It’s not just scientists and de-icing crews who should care about chemical formulas. Say you’re running a small business making cheese. The softness and taste hang on calcium chloride—add the wrong type and you’ll taste the difference. The extra water in the dihydrate version actually makes it dissolve quicker and more smoothly in milk. You won’t catch it clumping at the bottom like the anhydrous form. For folks making homemade tofu or pickling cucumbers, that smoother dissolve saves a lot of hassle and helps keep results predictable.
Another angle—medicine. Pharmacies use calcium chloride in IV solutions for patients who need calcium in a hurry. Mistake the hydrate level and the dose can be dangerously off. Accuracy here isn’t just smart chemistry; it’s a matter of health and safety.
Walk into any hardware store and you’ll spot “calcium chloride” bags for ice melt. Many only list “calcium chloride” without mentioning if it’s hydrated or not. I’ve seen people trying to use leftover ice melt in pools or aquariums, not realizing the formula might be off. That “·2H₂O” isn’t just a confusing label—it determines how much real calcium you’re putting in.
Clear labeling helps regular people make smarter choices, and more science classes should teach what those water molecules actually do. If you’re working with recipes or chemical mixes, tracking the full formula avoids all sorts of surprises. One simple solution: always check the packaging for the full chemical formula before buying or using any calcium chloride product.
Knowing the formula CaCl₂·2H₂O keeps your chemistry sharp and saves a lot of headaches. It keeps ice at bay in winter, smooths out the science in the lab, and can even tip the balance between a smooth cheese or a chunky mess. In the end, the sum of these little details decides whether something works—or really works well.
Calcium chloride dihydrate seems simple at first glance, just another salt with a long name. But let me tell you, storing this compound asks for some real-world attention. One spring, a leaking bag in my garage taught me more about moisture and chemicals than any textbook. This compound craves water. Leave the bag open, and it grabs hold of any moisture in the air. In a busy lab or warehouse, slack storage means cakes of sticky powder faster than you think.
Calcium chloride dihydrate acts like a sponge. As it soaks up water, it forms clumps, sometimes dissolving into a puddle. That changes its texture, ruins its flow, and can knock out its quality for future uses. More than that, if it pools on a shelf, you risk corrosion and possible safety mishaps. Back in college, I lost a pound of material to one humid day—nobody suggested tossing it into an open bin, yet that's what someone did. The result? Mess and wasted money.
Simple steps protect both product and people. Airtight, sealed containers make the biggest difference. Thick plastic buckets with gasketed lids handle the job well. For extra assurance, double-bagging before stashing inside a tub helps. Even glass jars work if the lid seals tight. After every use, snapping that lid closed keeps the powder from clumping. My workshop stash stays bone-dry for months that way, no matter the season.
Heat and humidity speed up clumping and spoilage. Storing the compound in a cool, dry spot—the kind where cardboard boxes don’t go limp—slows down those problems. Not every facility has climate control, but picking a spot clear of the furnace or hot water pipes helps. In bigger operations, a dehumidifier keeps the storage room under control, especially during rainier stretches. I’ve seen summer storms raise the warehouse humidity in hours. Keeping bins away from doors and windows makes a huge difference.
Clear labels cut down on accidents. Too often, chemicals end up in lookalike jars—someone guesses, someone guesses wrong, and mistakes happen. A well-marked shelf, some warning symbols, and a reminders on the bin prevent costly confusion. The real world moves fast. Proper labeling slows everyone down just enough to notice.
Even with the best habits, spills do happen. Dry sweepers can kick the powder into the air, so damp cloths mop up safely without spreading dust. Gloves matter. This compound can get irritating, so keeping a box handy saves trouble. In one shop, we set aside a spill kit next to the main storage. Quick, contained cleanup helped us avoid bigger problems on busy days.
Storing calcium chloride dihydrate well saves time and money. It keeps the material effective, prevents waste, and simplifies safety. Nobody wants to pay for ruined product or mess with sticky piles of powder. Small steps, like choosing dry containers and well-marked shelves, protect both the budget and the people doing the work. Good habits outlast warnings on the bag—they become how the job gets done right every single time.
Anyone living in a snowy area recognizes the white pellets scattered on sidewalks and roads every winter. Calcium chloride dihydrate rarely takes a day off in cold regions. Its strength comes from its ability to draw moisture from the air, which makes it quick to melt ice and snow even when temperatures drop far below freezing. Unlike rock salt, it keeps working at much lower temperatures, which means roads stay safer for drivers and pedestrians. In the summer, city crews turn to the same stuff for gravel roads. Spread on dusty rural routes, it holds down loose dirt by attracting water, so clouds of dust bothering neighbors and clogging air filters become far less common.
Construction never stops just because the weather turns chilly. Calcium chloride dihydrate often finds its way into fresh concrete mixes, speeding up how fast the material sets and gains strength. This matters on job sites where roadways, bridges, or sidewalks face tight deadlines, or when crews work during the colder months. Quick setting reduces downtime and lowers the chances of cracks caused by freeze-thaw cycles, helping projects finish on time and stick around longer. The American Concrete Institute points out the value of this additive, though good crews stay careful to avoid rusting any reinforced steel inside the concrete by checking how much to use.
Almost every kitchen relies on well-preserved ingredients. Cheese, tofu, and vegetables like cucumbers and tomatoes spend some time with calcium chloride dihydrate in their processing. In cheese making, it helps milk to curdle properly, making cheesemakers’ days a bit easier and more reliable. Vegetable canners drop it into brine to keep pickles crispy and tomatoes firm, so nobody bites into something mushy after months on the shelf. Brewmasters use it too, fine-tuning water content for better tasting beer and clearer brews.
Hard water frustrates homeowners. Calcium chloride dihydrate steps in at water treatment plants, where staff use it to adjust the mineral balance and remove impurities. It also plays a role in keeping swimming pools balanced, making sure calcium stays at a useful level to prevent leaky, pitted plaster. On the industrial side, oil and gas operations pump it down wells to keep drilling fluids stable. Plumbers and handymen may turn to it in special cases to clear deep drain clogs by breaking up tough, greasy blockages.
Hospital labs and drug factories depend on carefully controlled conditions. Calcium chloride dihydrate keeps some medicines stable and helps control reactions in labs. For some medical uses, doctors rely on it to treat patients with dangerously low calcium levels. Its history in healthcare stretches back decades and speaks to careful oversight and proof of its safety.
Using calcium chloride dihydrate makes daily life smoother, but it always brings responsibility. Responsible handling and proper storage prevent unwanted spills and skin irritation. Rules already exist, but more training and clearer labeling at stores and job sites can help everyone, from road crews to hobby brewers, stay safe. It’s smart to track how run-off from winter roads might affect local streams and lakes. Communities who rely on it every day can shape future guidelines by sharing their experiences and watching new studies on environmental impact.
| Names | |
| Preferred IUPAC name | Calcium chloride dihydrate |
| Other names |
Calcium chloride, dihydrate Calcium dichloride dihydrate Calcium chloride-2-water CaCl₂·2H₂O |
| Pronunciation | /ˈkæl.si.əm ˈklɔː.raɪd daɪˈhaɪdreɪt/ |
| Identifiers | |
| CAS Number | 10035-04-8 |
| Beilstein Reference | 1368731 |
| ChEBI | CHEBI:86156 |
| ChEMBL | CHEMBL1201201 |
| ChemSpider | 57312864 |
| DrugBank | DB09462 |
| ECHA InfoCard | 05b16199-ec71-403c-b19a-6da8c217d221 |
| EC Number | E509 |
| Gmelin Reference | 778 |
| KEGG | C00238 |
| MeSH | D002121 |
| PubChem CID | 6636659 |
| RTECS number | EV9800000 |
| UNII | XN1XP22C7D |
| UN number | UN1748 |
| Properties | |
| Chemical formula | CaCl2·2H2O |
| Molar mass | 147.02 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 0.85 g/cm³ |
| Solubility in water | Well soluble |
| log P | -2.0 |
| Vapor pressure | <0.1 kPa (20 °C) |
| Basicity (pKb) | 8.31 |
| Magnetic susceptibility (χ) | −37.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.439 |
| Dipole moment | 2.95 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 151.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1127.1 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -234.7 kJ/mol |
| Pharmacology | |
| ATC code | A12AA04 |
| Hazards | |
| Main hazards | Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS05 |
| Pictograms | GHS05, GHS07 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P280, P301+P312, P305+P351+P338, P330, P337+P313, P501 |
| NFPA 704 (fire diamond) | 1-0-1 |
| Explosive limits | Non-explosive |
| Lethal dose or concentration | LD₅₀ Oral - Rat - 1,000 mg/kg |
| LD50 (median dose) | 2,300 mg/kg (rat, oral) |
| NIOSH | WT4840000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 5 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Bromochlorodifluoromethane Calcium chloride Calcium chloride anhydrous Calcium chloride hexahydrate Calcium chloride, solution Chlorine Hydrochloric acid Hypochlorous acid Potassium chloride Sodium chloride |
