© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Barium chloride dihydrate has been a part of the chemical landscape since researchers in the 18th and 19th centuries started exploring mineral compounds for their unique properties. It came out of the mines and straight into early industrial chemistry labs, where people noticed its strong reaction with sulfate ions. Old textbooks and field notes highlight barium chloride as a chemical test agent long before it became a staple in modern manufacturing. Early chemists also struggled with the safety hazards, since barium salts drew caution signs almost as soon as they arrived on the scene. The compound’s story shows the progression from basic research to large-scale production, echoing broader shifts in the chemical industry—more demand, more quality control, and eventually, stricter regulations.
Barium chloride dihydrate, BaCl2·2H2O, appears as white, odorless crystals. In solid form, these crystals dissolve smoothly in water, leaving behind no residue. You find it packed in airtight containers because it soaks up moisture from the air. This property, in my own experience working with chemical stocks, means you can almost always spot a neglected bottle by the way the crystals fuse together. The product stands out for its steady concentration and lack of impurities, an important trait for both lab analysis and batch processes in chemical plants.
Each gram of barium chloride dihydrate weighs heavily on the scale with a molar mass of 244.26 g/mol—hydration water counts in this calculation, which can trip up newcomers who expect the anhydrous version’s lighter number. The melting point lands near 113°C, and heating pushes off the water, changing both its physical appearance and chemical behavior. As a strong ionic salt, it dissociates almost completely in water, providing a reliable source of barium ions. This explains why it's a staple in tests for sulfate—if a white precipitate appears, sulfate is present. The water of hydration directly influences the handling and reaction rates, a detail I learned first-hand in failed attempts at syntheses that called for the dry version. Barium chloride in its hydrated form is much less prone to caking but needs careful sealing to prevent loss of water content.
Bags and bottles of barium chloride dihydrate must always carry an explicit warning label, not just for regulatory needs but for everyday lab safety. Documentation lists not just molecular formula and batch number, but also shelf life, recommended storage temperature (around 20°C, low humidity), and any detectable impurities, like iron or trace metals, down to parts per million. The need for traceability has ramped up with international standards—everything from REACH in Europe to OSHA in the US questions purity claims. Even small variations matter: too much impurity can spoil analytical outcomes or lower the quality of end products. Packing, usually in HDPE drums or glass bottles, has evolved alongside these labeling standards, aiming to minimize contamination and avoid accidental mixing with incompatible substances (especially acids or organic matter).
You get barium chloride dihydrate from treating barium carbonate or barium sulfide with hydrochloric acid. Start with a slurry, stir until the raw material dissolves, filter to pull out any solid residue, then cool the solution to crystallize the product. This process, I’ve found, calls for patience. Skipping filtration or rushing the cooling step leads to mixed batches or uneven hydration—a sure way to end up with off-grade material. Large chemical plants automate much of this, with constant monitoring of temperature, pH, and purity. Though this method seems simple, subtle differences in process control change the final quality. Water loss, for example, shifts the compound toward the anhydrous salt, which handles very differently in application.
At its core, barium chloride dihydrate functions as a robust barium ion source. Mix it with sodium sulfate or sulfuric acid, watch as barium sulfate pops out as an insoluble white solid—this basic test remains a mainstay in water analysis. In industry, barium chloride is used to clean brine solutions by pulling out unwanted sulfates before they clog up downstream systems. Chemists have explored tweaks, such as substituting chloride with other halides or adding agents to control crystal size, aiming to tailor the product for specific uses. Some researchers test its role in organic synthesis reactions, exploring its ability to alter reaction rates or change product yields.
Scan through chemical catalogs or shipping manifests, and you’ll run across a mix of names: barium chloride dihydrate, dichlorobarium hydrate, and sometimes just “BaCl2·2H2O.” Older literature may call it baryta muriatica, stemming from 19th-century naming conventions. Anyone ordering or tracking this compound must keep an eye on these aliases to avoid mix-ups with the anhydrous version or similar barium salts. Even on the job, I’ve seen shipments delayed or rejected over confusion about synonyms—small difference, big outcome for lab schedules.
No one gets casual around barium compounds. Even though the dihydrate may look harmless, ingestion or inhalation leads to severe health risks—muscle weakness, irregular heartbeat, sometimes worse. Personal experience with emergency response plans drives home the need for clear labeling, gloves, goggles, and rapid access to washing stations. Work areas get monitored with continuous air testing if powder is handled in bulk. Standards from groups like OSHA, NIOSH, and the European Chemicals Agency shape these practices, requiring everyone working with barium salts to stay updated on permissible exposure limits and emergency procedures. Disposal isn’t a casual matter, either—waste streams containing barium get sent for specialized treatment to avoid poisoning local waterways or soil.
Industries turn to barium chloride dihydrate for water treatment, heat-treating baths, and the production of pigments and other barium compounds. Its strong sulfate scavenging power helps keep boilers and industrial filtration systems clear. In research, it remains a go-to for analytical chemistry, both in classic gravimetric sulfate detection and modern spectrometry calibrations. Those working on specialty glass, ceramics, and even fireworks count on its unique properties. Every kilogram of product in these fields traces its way through careful handling and strict formulation requirements. In my own work, mistakes in measurement or quality led to significant setbacks in analytical processes or required costly repetition of procedures.
Academic and industrial labs keep digging for new angles on barium chloride dihydrate. Some researchers lock eyes on new roles in material science, such as crystal growth experiments or non-traditional catalysts. Others weigh regulatory trends and try to devise barium-free alternatives that retain similar performance where toxicity proves challenging. Environmental and occupational health research remains a strong focus, with studies analyzing exposure routes, improved scrubber designs, and safer production cycles. Technical journals highlight persistent questions about trace metal contamination and its effects on advanced sensor technologies. The ongoing balancing act calls for new methods and better transparency, challenges anyone in the field quickly comes to appreciate.
Toxicity research doesn’t leave much room for doubt—soluble barium salts disrupt potassium channels in the human body, leading to rapid onset symptoms in exposure cases. Controlled animal studies, dating back to the mid-20th century and continuing now, give detailed thresholds for acute and chronic toxicity. Public health efforts continue to translate these studies into actionable workplace standards and community guidance, especially where water sources risk barium contamination. There is a demanding focus on accurate risk communication, particularly after exposure incidents in industrial settings or areas with contaminated well water. Anyone working in regulatory or emergency planning remembers case studies where lax standards triggered investigations and rushed remediation.
Barium chloride dihydrate finds itself at an interesting crossroads. Regulatory scrutiny is climbing, especially as global supply chains tighten controls on hazardous materials. Scientists keep probing for smarter ways to use it and, in some cases, phase it out where alternatives stack up better on safety or sustainability grounds. The call for greener manufacturing and cleaner water treatment methods might shift demand toward less toxic options down the road, but for now, barium chloride dihydrate holds onto a vital role. Continued advances in handling technology, predictive monitoring systems, and lab testing standards all point to a future where the compound remains essential, but used with sharper awareness and higher accountability.
If you have ever walked past a water treatment facility or toured a chemical lab, odds are good that barium chloride dihydrate has passed through those spaces. This chemical, with its two water molecules clinging to every unit of barium chloride, steps in where precision and reliability matter. Take water treatment as one clear example. Many cities depend on it to pull out sulfate ions from the water, stopping the buildup of stubborn scales in plumbing and heavy machinery. Sulfate build-up can force massive repair jobs in municipal water systems, not to mention home appliances. That’s enough to nudge anyone into paying attention to how things get filtered.
Chemistry labs still turn to barium chloride dihydrate for classic tests to spot sulfate ions. You mix it into a solution, and a white precipitate signals the presence of sulfates. I’ve watched high schoolers' eyes light up during this experiment; that little cloud in the bottom of a test tube carries more chemistry lessons than a textbook. Beyond teaching, laboratory staff use it for more technical jobs, from calibrating analytical instruments to prepping chemicals for further synthesis. Mixing chemicals always carries risks, so training teens to use it safely really sticks with me.
Barium chloride dihydrate steps onto factory floors every day. Glass manufacturers look for it to make glass bright and help impurities settle out during melting. Tile makers draw on it for glossy glazes that don’t warp in the kiln. In grease production, it finds a spot in formulating lubricating oils and greases for machinery, especially where heat and load get intense. These aren’t always flashy uses, but take away the right lubricant and those factory lines grind to a halt fast. In the realm of dyes and pigments, textile workers use it for lasting colors that don’t fade in the wash or sun.
Barium compounds demand respect, and barium chloride dihydrate sits near the top in terms of toxicity. Breathing in its dust or swallowing even tiny amounts can cause severe health issues—affecting muscles, nerves, and the heart. There’s a reason it stays under lock and key in most settings. Workers suit up with gloves, goggles, and ventilation to keep harm at bay. Waste disposal follows strict protocols, keeping contaminated water from seeping into rivers and soil. Families living near industrial sites should ask questions about dumping practices—most problems with heavy metal pollution sneak in quietly over years, not weeks.
Lately, some industries turn to safer chemicals that don’t carry as much risk of poisoning or environmental trouble. For sulfate removal, techniques like ion exchange or using other salts sometimes work without tipping the risk scale. Schools and hobby labs often swap out barium chloride for less hazardous teaching aids unless the specific reaction calls for it. Staying informed about chemical safety gives everyone—from science teachers to city engineers—a head start on preventing accidents.
Barium chloride dihydrate won’t vanish from chemical shelves overnight, but its use calls for care. Knowing where it turns up—in water treatment, glass, dyes, or classrooms—keeps people cautious and gives communities a voice in how chemicals shape their surroundings. Every facility using it needs clear rules, careful storage, and responsible cleanup—lessons every industry should take to heart.
Barium chloride dihydrate isn’t just a tongue-twister for chemistry students. It’s a salt used in labs, industrial processes, and even in fireworks. People might wonder if it’s as dangerous as some chemicals, or just another specialized material most folks never encounter. Either way, understanding its hazards means more than reading the label.
Barium doesn’t get into the human body naturally. When barium chloride dihydrate enters the system—usually through swallowing, breathing in the dust, or skin contact—it quickly gets absorbed. Once it’s in, health issues can pile up in a hurry. Swallowing even small amounts can lead to serious trouble: muscle weakness, breathing problems, stomach pain, and sometimes irregular heartbeats. High enough doses, or repeated exposure, can even be fatal.
A lot of folks working around these chemicals remember tales from old chemistry classes. Stories where someone spilled a powder and ended the day in the ER. These aren’t just exaggerations. The CDC recognizes water-soluble barium compounds like this one as hazardous, and the EPA set strict limits for barium in drinking water—usually below 2 milligrams per liter. Scientists link higher concentrations to blood pressure spikes and long-term kidney damage.
Factories and plants that use barium chloride can accidentally send it into the ground or water supply. Cleanup crews don’t take this lightly. Fish and aquatic life are very sensitive to elevated barium levels, which can disrupt delicate food webs. Runoff without proper controls might not seem dramatic, but over years it builds up and impacts the streams, rivers, and groundwater where people and animals drink.
Most people won’t deal with barium chloride dihydrate outside of work or school. In labs and industry, strict protocols make all the difference. In my own experience in chemical storage, one missed step—like skipping gloves or forgetting to double-check container seals—meant risking a spill. I learned quickly from one close call: never treat these substances lightly.
Proper safety gear stands as the first line of defense. Workers shield themselves with gloves, goggles, and well-ventilated workspaces. Training keeps teams alert to hazards both obvious and hidden. Emergency eyewash stations and showers, plus strong labeling practices, help avoid slip-ups. Even cleaning up gets special attention: contaminated waste doesn’t go in the regular trash or down the drain.
Looking beyond just barium chloride, companies experiment with substitutes, especially if public or environmental safety is at risk. Some processes now use less hazardous chemicals or adapt workflows to avoid using barium-based salts at all. Sharing best practices and open reporting of incidents supports a culture focused on safety over speed or convenience.
Since barium chloride dihydrate can cause both human and environmental harm, finding newer, less toxic compounds and prioritizing tight handling standards have become important for anyone working with these materials.
Barium chloride dihydrate shows up in labs and industry settings quite a bit. Its crystalline white form makes it look harmless, but anyone who’s spent time around chemicals knows appearances don’t count for much. This compound brings along a real risk if moisture or loose handling get involved. The safety data sheets spell out clear health warnings. Inhaling dust or getting it on your skin won’t do you any favors. In my years of lab work, a lapse in basic chemical storage has caused far more headaches than even the most chaotic syntheses.
This compound pulls in water from the air, thanks to its hygroscopic nature. That means bags tucked in drippy storerooms or jars left unsealed slowly clump up and lose their crisp, crystalline shape. I remember finding old bottles in a supply closet—soaked and caked together. That mistake cost plenty of material and more work. Airtight containers make a big difference. Glass bottles with screw caps or plastic jars with tight lids keep out moisture. Adding a desiccant pack helps, especially in places where humidity stays high year-round.
Every time I’ve seen people skip proper labeling, confusion—and sometimes real danger—followed. Mark the container clearly, showing the full chemical name and hazard symbols. Extra labels for poison or water-reactive properties can save trouble in the long run. Store barium chloride dihydrate apart from acids or anything with sulfates, since a nasty reaction or unwanted barium sulfate sludge can pop up. Storing on a dedicated shelf keeps leaks contained and clear of food or drinking areas. Dealing with chemical splashes or spills once taught me to never relax about separation.
Workers and students sometimes underestimate how risky these salts get if handled with bare hands or spilled carelessly. Gloves and protective gear aren’t just a box to check. I’ve seen skin rashes and lab messes from skipping these steps. Good ventilation in the storage area helps stop dust from floating around—a real plus for older facilities with less-than-ideal air flow. Regular checks help spot leaks or damaged containers. I always keep a small supply of spill kits and instructions nearby, written clearly enough for anyone to follow. This approach makes emergency response smoother if the worst ever happens.
Disposing of unsalvageable barium chloride calls for separate containers. I’ve dealt with too many mixed-waste barrels full of uncertainty—a headache during inspections. Sticking to the rules means working with trained professionals for hazardous waste removal. Keep all paperwork ready. Audits come around without warning, and nothing frustrates inspectors more than a missing label or mystery jar. Experience has taught me that consistent checks and sticking to proven protocols build both trust and safety.
Learning from small mistakes matters. Dry, well-ventilated spaces and simple habits—like checking seals and labels before leaving the storeroom—pay off. Training new folks on storage basics saves everyone time and hassle. Building a routine around chemical safety turns vague policies into real protection for people and property.
Barium chloride dihydrate often pops up in chemistry labs, college classrooms, and industries dealing with testing or synthesis. The formula points to a clear structure: BaCl2·2H2O. It contains one barium ion, two chloride ions, and two water molecules. That water isn’t just clinging on for the ride—its presence changes the substance’s weight, handling, and the way it dissolves.
From years helping students prep for practical exams, I’ve seen confusion spring up when hydrates get mixed with their anhydrous twins. You can’t just ignore those water molecules; doing so risks throwing off measurements or botching reactions. For new chemists, misreading a formula often means wasted reagents or the hassle of recalculating in the middle of a busy lab session.
To get accurate results in chemical reactions, knowing the molar mass counts. Every gram used affects yields, purity, and safety. For BaCl2·2H2O, calculating molar mass means you stack up the atomic masses:
Add these up for a total molar mass of 244.27 g/mol. Double-checking these numbers isn’t just about being detail-oriented. Over the years, I’ve watched lab partners fumble a titration because the wrong molar mass slid into a notebook.
Mistaking barium chloride for its anhydrous variant can spell trouble. The hydrate’s water lightens your needed dose. This slip pushes you off-target for everything from titrations to precipitation tests. Take water analysis as an example. In the classical sulfate test, any error in formula means your observed result breaks from reality. It doesn’t just slow you down—it hobbles trust in your data.
In industry, where every batch impacts product quality or regulatory compliance, formula mix-ups stack up to lost money. Companies risked recalls before simply from prepping batches with wrong mass data. Being casual about these numbers has real-world consequences far beyond a bad lab grade.
Plenty of mix-ups come from fast-paced work or ignored details. Printed labels fade, old lab manuals get readers guessing, and digital databases offer more results than answers. To avoid wrong calculations, I always double check and push students to do the same. Modern lab scales and inventory systems let teams scan and cross-reference formulas, but vigilance can’t slack.
Regular reviews of supply labels, training sessions on hydrate recognition, and spot quizzes in academic settings have a big impact. Early lessons stick. Familiarity with formulas like BaCl2·2H2O pays off every time you work with a new hydrate, or when mistakes would cost safety. Checking the numbers, as routine as it seems, turns into habit. For me, and for those coming up in science, painstaking care with formula and mass never grows old.
Barium chloride dihydrate doesn’t usually scream danger at first glance. White, powdery, and often handled in schools or labs, plenty of folks have underestimated its hazards. My early time working with lab chemicals taught me the value of reading those safety sheets, and barium chloride reminds me why. Once inside the body, barium ions can disrupt heart rhythms and muscle function. Skin and eye contact cause irritation, but eating or breathing in the dust poses a bigger threat. These aren’t just warnings meant for the shelf—they’re based on real events in chemistry classrooms and small factories.
Personal protection makes the most difference. Lab coats, nitrile gloves, and snug-fitting safety goggles give a basic shield, keeping the powder off bare skin and out of your eyes. Masks with a P2 or N95 rating will stop dust from getting in your lungs during weighing or mixing. If you ever doubted why labs stress “no eating, no drinking,” think about this: trace amounts of toxic powders on your hands can sneak into meals or water without you noticing. I learned early on to treat every powder with respect, not just the ones sporting scary warning stickers.
Spills can happen, and in cramped labs or storerooms, powders find their way into corners fast. Dry sweeping kicks dust into the air, raising exposure risks. Instead, wet paper towels or HEPA-filtered vacuums should handle any messes. Double bags and clear labeling signal to anyone nearby that this isn’t just table salt. Old stains from spilled chemicals aren’t just unsightly—they’re a hidden hazard.
Handwashing feels tiresome after a long session, but it’s almost a ritual among experienced lab workers for good reason. Removing gloves isn’t enough, since fine dust clings to wrists or under nails. Prompt washing also keeps family members safe when you leave work behind.
Ventilation cuts down the risk. Mixing and pouring inside a fume hood takes away most of the dust before it floats into the breathing zone. A small investment in proper air flow means less worry about invisible dangers. In places without a fume hood, opening windows or using extraction fans helps, but nothing beats the containment a hood provides.
Barium chloride belongs in tightly sealed containers far from food and general supplies. Lockboxes and chemical safes, even simple ones, prevent curious hands—especially children—from touching things they shouldn’t. For waste, never send barium compounds down the sink. They contaminate water and are toxic to fish and birds. Methodical labeling, collecting waste in secure containers, and using registered disposal services keep local ecosystems safer. Remembering a colorless powder can poison a stream miles away makes those extra steps feel worth every minute.
I’ve worked in spaces where old habits and shortcuts almost led to accidents. Teams with up-to-date training move more confidently, spot mistakes faster, and handle emergencies with less panic. Regular refreshers and honest discussions about near-misses create a culture where asking questions is normal. People protect themselves and each other better.
| Names | |
| Preferred IUPAC name | Barium dichloride dihydrate |
| Other names |
Barium chloride hydrate Barium chloride-2-water Barium dichloride dihydrate |
| Pronunciation | /ˈbeə.ri.əm ˈklɔː.raɪd daɪˈhaɪˌdreɪt/ |
| Identifiers | |
| CAS Number | 10326-27-9 |
| Beilstein Reference | 1368732 |
| ChEBI | CHEBI:61385 |
| ChEMBL | CHEMBL1201221 |
| ChemSpider | 85911 |
| DrugBank | DB11204 |
| ECHA InfoCard | 03b7d5d2-b15d-43dd-9d91-ed7f2a7ae5e5 |
| EC Number | 233-788-1 |
| Gmelin Reference | 85032 |
| KEGG | C14185 |
| MeSH | D002060 |
| PubChem CID | 25312 |
| RTECS number | CQ9626000 |
| UNII | 55I8T049F6 |
| UN number | UN1564 |
| CompTox Dashboard (EPA) | DTXSID4044373 |
| Properties | |
| Chemical formula | BaCl2·2H2O |
| Molar mass | 244.26 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 3.856 g/cm³ |
| Solubility in water | soluble |
| log P | -1.8 |
| Vapor pressure | <0.1 hPa (20 °C) |
| Magnetic susceptibility (χ) | -63.6e-6 cm³/mol |
| Refractive index (nD) | 1.635 |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 190.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -855.2 kJ/mol |
| Pharmacology | |
| ATC code | V09BA02 |
| Hazards | |
| Main hazards | Toxic if swallowed, causes serious eye irritation, harmful if inhaled |
| GHS labelling | GHS07; GHS09; Warning; H302; H319; H410 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. |
| Precautionary statements | P264, P270, P273, P280, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-0-2-W |
| Explosive limits | Not explosive |
| Lethal dose or concentration | Oral rat LD50: 168 mg/kg |
| LD50 (median dose) | > 118 mg/kg (Rat, oral) |
| NIOSH | CY1400000 |
| PEL (Permissible) | PEL (Permissible): TWA 0.5 mg/m³ (as Ba) |
| REL (Recommended) | 0.5 mg/m³ |
| IDLH (Immediate danger) | 50 mg/m³ |
| Related compounds | |
| Related compounds |
Barium chloride Barium sulfate Barium hydroxide Barium nitrate Barium carbonate Calcium chloride |
