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Strontium chloride hexahydrate didn’t spring out of nowhere. Its roots reach back to the discovery of strontium itself, traced to a Scottish lead mine at the end of the 18th century. Strontianite, the mineral source, gave its name to strontium, fueling curiosity among early chemists. Growing up near mining regions, I witnessed firsthand the lasting mark mineral discoveries leave, not just in textbooks but in whole towns shaped by extraction and experimentation. That sense of place shows up in every flask of strontium chloride hexahydrate, which found use quickly after strontium’s introduction for refining sugar and giving fireworks their red flare. Even back then, the salt was more than a mineral oddity—it became intertwined with industry and daily life.
On the lab bench, this compound takes the form of white crystalline chunks, cool and satisfying to the touch. Its formula, SrCl2·6H2O, spells out its two main ingredients paired with six molecules of water. That hydration isn’t just a chemical formality; it affects just about every feature, from melting point to solubility. Water-laden salts like this one dissolve quickly in cold liquids and sometimes clump together in the air if storage gets sloppy. These practical details shape handling habits in both school and industrial labs. The hexahydrate releases its water with only gentle heat, which matters when drying or using it as a precursor in synthesis.
The purity of strontium chloride hexahydrate often reaches up toward analytical and reagent grades, a far cry from the less regulated salts used in de-icing roads. Labels list water content and hint at trace impurities, especially barium, since it shares a chemical kinship with strontium. Regulatory requirements set limits on such contaminants due to barium’s health risks, a sign that chemistry goes hand-in-hand with responsible handling. Shelf life, storage temperature, and batch traceability—these demands crowd the label because accuracy and safety protect workers down the line.
Manufacturers aren’t just dumping strontium metal into acid. In practice, most production starts with strontianite or celestine minerals, which get processed to strontium carbonate. Dissolving this intermediate in hydrochloric acid gives strontium chloride. Recrystallization after evaporation pulls out the salt, which then captures water from the air to become the familiar hexahydrate. Working during my undergraduate years, I learned these steps call for patience, careful temperature control, and a reliable eye for when a solution has reached true saturation. Rushing the process or cutting corners leads to subpar yields or, worse, unexpected reactions.
Strontium chloride hexahydrate doesn’t just sit pretty on a shelf. Its chemical reactivity opens up an array of transformations. Drop it into a solution of sodium sulfate, and strontium sulfate falls out as a solid—an old-school way to test for sulfate ions that still appears on school exams. On heating, it gives off its water of crystallization, transforming into the anhydrous form. In solution, it acts as a straightforward supplier of strontium ions, which matters for chemists crafting strontium salts of more exotic anions. Old textbooks cite its role in qualitative inorganic analysis because its reactions are colorful and satisfying, providing a sense of direct engagement with materials.
Ask five chemists about this substance, you'll hear strontium dichloride hexahydrate, SrCl2·6H2O, or just “strontium chloride hex.” This patchwork of names can spark confusion, but the underlying compound stays the same. Recognizing the multiple names echoes global habits in science—one person’s carbide is another’s acetylide. I’ve seen confusion over synonyms spark mix-ups in stores and technical writing. Researchers, procurement officers, and students all benefit from clear communication, which keeps drawers and flasks correctly stocked.
Working with strontium chloride hexahydrate demands respect. Direct contact might irritate the skin or eyes, and airborne dust isn’t pleasant to breathe. The old maxim applies: treat everything as potentially hazardous until proven otherwise. Standard rules—gloves, goggles, and decent ventilation—aren’t just formalities. Data sheets flag potential toxicity, especially because some strontium compounds can mimic calcium in the body, pushing into places they don’t belong. Waste handling and disposal need attention in line with local regulations, which vary from country to country. During my time in research, these details shaped good habits and meant lab safety drills mattered, not because of legal demands but because nobody wants an avoidable incident.
This material crops up in surprising places. The most visible role lands in pyrotechnics, giving fireworks their deep red glow—a practical lesson in elemental flame colors that feels magical at every summer festival. In the lab, strontium chloride provides a simple source of strontium ions, vital for studies on calcium mimics in biology and experimental treatments in osteoporosis research. Older generations saw its use in refining beet sugar, a fact echoed in agricultural records and patents from the early 1900s. Fish keepers notice it, too, adding stony minerals to saltwater tanks to mimic natural ocean chemistry. Use in radiotherapy circles around the radioactive isotope strontium-89, where the chloride salt acts as the vehicle for targeted cancer treatments. Each application reflects shifting priorities over time, from pure chemical interest to targeted medical needs.
Research involving strontium chloride hexahydrate continues to branch out. Scientists probe how strontium affects skeletal development, especially as the element stands in for calcium within living tissues. Teams use this compound to simulate marine conditions, supporting the growth of delicate corals in aquarium studies. In analytical chemistry, strontium chloride finds a place as a matrix modifier, making atomic absorption measurements more reliable by flattening out the impact of tricky interferences. I’ve watched colleagues test new battery chemistries and even probe superconductor properties, with strontium sitting center stage in the materials list. Studies like these keep pushing the boundaries and show how materials with humble industrial histories can drive innovation far from their original uses.
Most research sees strontium chloride hexahydrate as low- to moderate-risk. Ingestion could stress kidneys and interfere with normal bone turnover if doses get too high, a concern supported by animal studies and medical case reports. Unlike its barium relatives, which send up serious toxicology flags, strontium’s profile is less harsh, yet occupational exposure needs oversight just the same. Regular monitoring and attention to cumulative exposure matter, especially in manufacturing, handling, or scientific work. Concern for aquatic life pops up in wastewater studies, pressing manufacturers to limit environmental release. From my own safety training, transparency about risks always beats overconfident downplaying.
Interest in strontium chloride hexahydrate keeps growing, especially as materials science and healthcare chase new advances. In medical technology, its potential grows as researchers seek less invasive pathways to osteoporosis treatment—early data suggests strontium’s effect on bone health may someday translate into improved therapies for an aging population. Environmental technologies may see greater reliance on strontium salts for water treatment or pollution monitoring, given their distinct chemical signatures. Electronics and innovative materials don’t seem to let go of strontium either; new work explores its utility in producing specialty glasses, ceramics, and energy storage devices. Drawing from years watching trends, I see these shifts as a reminder that old compounds keep reinventing themselves in fresh contexts, driven by relentless curiosity and problem-solving demands.
I spend a lot of time around chemicals both in the lab and talking shop with folks in manufacturing. Strontium chloride hexahydrate might not roll off the tongue, but it pops up in some places where most people wouldn’t expect. This salt, which looks like colorless crystals, draws water from the air easily. Working with it tends to leave your hands dry if gloves aren’t in the mix. Still, it’s not your typical everyday pantry staple—unless you’re making fireworks or running diagnostics in a hospital lab.
Every time my family heads to a fireworks show, I remember how much chemistry ties into that big red glow in the sky. The deep crimson flashes people cheer over often come from strontium compounds, and strontium chloride hexahydrate is one of the best for the job. It blends well into pyrotechnic mixtures, giving off a rich red color no other substance quite matches. The stability of this compound makes it safe to handle (with regular lab safety) and reliable for fireworks technicians working long hours before big events.
Hospitals use strontium chloride hexahydrate in some diagnostic imaging and laboratory reagents. When blood gets tested for trace metals or doctors look for details in bone scans, strontium might show up behind the scenes. Its reactivity helps deliver clear results, making life easier for technicians reading out scores of samples each shift. This isn’t as flashy as fireworks, but reliable laboratory chemicals help give doctors a fighting chance at catching health issues early. In my experience, the reliability of these compounds can mean fewer false positives—less stress for patients waiting on results.
Friends who run home saltwater aquariums rely on strontium chloride to supplement water. Corals and some marine invertebrates need it for healthy growth. Aquarium owners mix measured amounts of this chemical into their tanks, and quality can make or break a prized coral setup. Strontium supports the growth of hard corals’ skeletons, almost alongside calcium. Too little, and the tank’s inhabitants show dull color and slow growth; too much, and things go wrong just as quickly. Regular testing at home safeguards these delicate environments. Credible brands disclose strontium content on their supplements, which helps people who just want to keep their reef tanks thriving without risking their livestock.
Lab supply catalogs list strontium chloride hexahydrate for things like protein detection and chemical synthesis. From what I’ve seen, its role in these workflows centers on reliable reactivity. Industrially, some processes use it to make magnets, refine zinc, or even as a part of toothpaste for sensitive teeth. Toothpaste companies use the substance because strontium ions can block the tubules in dentin, lowering tooth sensitivity for a lot of people. That’s not a claim—they publish studies showing clinical results, and dentists often recommend these brands to patients with chronic tooth pain after whitening.
In all these areas—fireworks, medicine, aquariums, and toothpaste—end users look for purity, safety, and reliable sourcing. Customers often feel nervous about unfamiliar chemical names, so it pays to check sourcing information and certifications. Full transparency builds trust, and I’ve found that companies willing to talk about quality control earn long-term customers. As regulations shift, suppliers who keep up do better in the long term, whether supplying hospitals or hobbyists shopping for reef additives.
Strontium chloride hexahydrate shows up in labs and classrooms, yet people outside chemistry circles don’t talk about it much. The chemical formula is SrCl2·6H2O. The substance calls for a close look because, whether in teaching experiments or working with medical manufacturing, the makeup of a compound shapes its role in the world.
SrCl2·6H2O appears direct, but those six water molecules—pointed right at in the “hexahydrate” part—do more than take up space. In my own work handling this compound, I’ve dealt with weighing it for preparing solutions. Forgetting about those waters of hydration means you end up with a solution too strong and that defeats the accuracy so many scientific processes count on.
It isn’t just a matter for students filling out a worksheet. In a real chemical reaction, every bit counts. Not accounting for those waters can throw an experiment off, leading to frustration and wasted resources. Direct experience reinforces that difference—ScCl2 (anhydrous) and SrCl2·6H2O don’t weigh the same for the same number of strontium and chloride ions in solution, and practical chemistry relies on those correct weights.
Compounds like this help with more than chemistry class. In medical imaging, strontium salts sometimes shine as markers. In pyrotechnics, strontium chloride lends color to fireworks—think of that bright red glow at the county fair. Makers of such products pay attention to those six water molecules: too much water changes the behavior of the chemicals in storage and use. Too little, and the formula isn’t right for those precise effects.
Once, in a small fireworks demo, a friend tried to make a batch using what he thought was plain strontium chloride, but he overlooked the hydration level. The mix didn’t burn as expected, missing the red intensity he aimed for. That’s experience pointing straight back to the formula, and to the need for real knowledge over shortcuts.
Working hands-on with SrCl2·6H2O, mistakes can creep in if you ignore those waters. Fact-checking with reliable sources stands out as a step too often skipped, both in industry and teaching. The PubChem entry provides specifics. It matches up with trusted lab reference material, adding support to real-world handling advice.
Chemicals demand respect. Beyond learning the formula, handling strontium chloride hexahydrate safely means storing it away from moisture and writing clear labels. All too often, I’ve seen ambiguous jars on shelves—one mistake and someone uses the wrong chemical, risking safety or ruining a batch. Setting standards for accurate labeling and regular review could prevent those close calls.
Accurate formulas offer a foundation for good science. Telling students and coworkers to double-check chemicals—especially hydrated compounds—saves trouble down the road. Bringing digital scales, safety sheets, and reputable chemical catalogs into daily routines adds simple checks without straining budgets.
In every setting—schools, factories, home labs—reading and using the correct chemical formula makes all the difference, shaping results and supporting health and safety. That’s more than memorizing a string of letters and numbers; it’s about recognizing their real-world weight.
Strontium chloride hexahydrate looks harmless enough—just a white, crystalline solid—but chemicals like this get fussy about their surroundings. Years working in labs taught me a lot about the ways simple habits can keep you safe and save money. For folks using this compound, storage isn’t just about following rules; it matters for health, safety, and getting the most out of every bottle.
Growing up in the Midwest, I saw humidity fine-tune everything from bread to paint—chemicals behave the same way. Strontium chloride hexahydrate draws in air and moisture, and if left open, that harmless jar can turn to sludge. It also breaks down faster with too much heat, and that can throw off results fast, whether it’s in a classroom experiment or a big manufacturing process.
Locked cabinets in a dry, cool area—think 15 to 25°C (59 to 77°F)—keep the integrity of the solid longer. In my old college lab, we always kept jars capped tightly right after use. Glass containers with airtight lids work best. If you leave the jar open on a humid day, you waste product, and everything smells faintly chemical, no matter how careful you think you are.
People forget how easily powders and crystals pick up other substances. One day I watched a colleague use a scoop for one salt, then absentmindedly dip it into the strontium chloride jar. End result? Weeks later, the strontium sample changed color and started clumping. Clean, dry scoops and good labeling make a big difference.
Never put strontium chloride hexahydrate near acids or other reactive chemicals. The reaction risk jumps, especially if there’s even the smallest spill in a crowded cabinet. Chemicals like this should always get their own spot, up high and away from heavy traffic.
At one lab, a leak above a chemical shelf wrecked more than a dozen bottles. We switched to secondary containment trays under everything. If something spilled or broke, trays kept it from running wild. No one needs an avoidable cleanup or exposure.
Sometimes, suppliers send strontium chloride in plain white jars. Handwriting fades. Permanent, chemical-proof labels fix that problem. Every time I open a storage cabinet and see a shelf lined with clearly marked containers, I feel more confident. It’s a small step that keeps others safe, especially new team members or students.
Don’t forget what happens at the end of a bottle. Make sure the original packaging or an approved replacement can handle what’s left—nothing flimsy. A well-sealed bag in a tough container stops leaks and keeps anyone handling trash or recycling safe.
Even a small splash from a broken jar can irritate skin or eyes. Make sure everyone knows to flush exposed skin with running water and get help if anything feels wrong. Over the years, I’ve seen how a little training saves a lot of headaches.
Storing strontium chloride hexahydrate well is about respect for the product and for people. Care now beats complications later. Humidity, heat, sloppy labeling, and crowded shelves all lead to trouble. Treating chemicals right helps keep every project safer and more reliable, from research labs to high school classrooms.
Strontium chloride hexahydrate shows up in fields like chemistry labs, pyrotechnics, and even some aquarium care routines. It often lands on the bench as colorless or white crystals. Tons of university students running titrations or flame tests have brushed it off as another harmless powder. The reality always turns out a bit more complicated.
The crystals look harmless. Accidental contact rarely causes burns or severe wounds, but direct skin or eye exposure leads to irritation. Redness, itching, or a stinging sensation often follows. These reactions remind us that even chemicals grouped in the “mild” category still deserve respect. Wearing gloves or goggles isn’t just OSHA red tape—it spares a lot of hassle. Plenty of people, including myself, have felt the sting of a chemical splash because they dropped the safety glasses for half a second.
Dust from strontium chloride hexahydrate has a way of spreading in a poorly ventilated room. Breathing it in can stir up coughing, sore throat, or a scratchy nose. I’ve seen techs wiped out for a whole workday after careless handling during weigh-outs. Safety data sheets rank the oral toxicity as low compared to more dangerous lab chemicals, but that doesn’t turn it into candy. Some research points to possible nausea or mild digestive trouble after swallowing a chunk, and even low-hazard chemicals get riskier with larger doses.
A lot of folks trust that since strontium naturally exists in soil and water, the hydrated salt should blend in unnoticed. Not always. Tossing excess amounts down the drain works against regulations in many locations. If enough gets into the environment over time, fish and aquatic life face a chemical cocktail they never evolved to handle. Aquarists sometimes use small, measured amounts to supplement tanks, but reckless dumping comes with its own set of problems.
Old health studies point out that most strontium compounds don’t act like heavy metals, but there have been scares. Early research on radioactive strontium compounds caused nervous chatter, leading folks to paint all strontium salts with the same brush. That’s not accurate. The radioactive versions pose much greater health problems than plain strontium chloride hexahydrate. Still, the panic led labs and schools to tighten up chemical labeling and disposal habits.
Safe storage and handling don’t need to be complicated. I keep mine sealed in a dry spot away from food or heat. Bags of proper nitrile gloves and splash-resistant goggles aren’t optional gear. If there’s a chemical spill, cleaning up right away with plain water works better than waiting for the janitor. Local authorities lay out clear rules for chemical trash, so no shortcuts.
Teaching newcomers to respect even the “less toxic” labels matters. I bring the same care to strontium chloride hexahydrate as to anything else in the storeroom. People in this business know you only make a mistake once—after that, you upgrade your precautions fast.
Looking up the safety sheet before working with any lab chemical pays off every time. Relying only on a label or someone’s offhand comment never cuts it. People stay safe by keeping fundamentals front and center: eye protection, good ventilation, and keeping the material off your hands and out of your mouth.
Working together, labs, teachers, and regulators build a routine where respect for chemicals, even the ones with milder reputations, spreads from one generation of students and workers to the next. The goal: informed, careful use instead of taking unnecessary risks.
The purity of any chemical salt really stacks the deck for outcomes in research and production. Strontium chloride hexahydrate isn’t just another white powder. In my time working with reagents, seeing the difference between 98% and 99.5% pure batches translated to everything from clear crystal growth to wild variability in results. You want consistency, whether managing a lab or troubleshooting scale-up in a plant. Impurities introduce unwanted variables—often invisible—that drift into experiments or contaminate finished products.
Grade labels on strontium chloride hexahydrate tell a story. Reagent grade goes through more rigorous testing for contaminants and heavy metals. Manufacturers put it through tight filtration and analysis, sometimes with certificates showing sodium, magnesium, or barium present only in the low parts per million. ACS grade usually matches or exceeds minimum requirements set by the American Chemical Society, guaranteeing predictable behavior for analytical chemistry.
Technical grade stands a notch lower, aimed mostly for large-scale industrial use. Here, a small percentage of other compounds will ride along, and most technicians don’t lose sleep over a bit of color drift or batch-to-batch aesthetic changes. For glass manufacturing, water treatment, or pyrotechnics, paying for ultra-high purity doesn’t always justify the extra cost.
I once ran a simple titration expecting a textbook end point, only to find muddled results—the culprit was a “technical” product that snuck in unexpected iron contamination. That’s enough to throw your entire analysis, cost you a few days, and stir up doubt in results.
Most reputable suppliers put their purity front and center. Typical high-purity strontium chloride hexahydrate lands at 99% to 99.5% minimum purity by assay. Analytical data sheets spell out upper limits for iron (Fe), barium (Ba), calcium (Ca), and sulfate or nitrate ions—some dropping below 0.005%. You should always ask for a CoA (certificate of analysis) with each batch.
Laboratories tied to diagnostics, spectroscopy, or similar high-resolution work stick to the purer grades. Even for those not running NMR or advanced techniques, grabbing batches below 98% starts to invite oddball results, batch drift, or failed standards.
Sourcing from suppliers who document trace metals and batch history pays off over time. I learned the value of supplier transparency—the one time we skipped, an unreported spike in lead content put a whole round of testing in question. Looking past basic purity, I always press for trace heavy metals and solvent residue information.
Companies following ISO or related quality standards bring a level of discipline that helps avoid surprises. That translates to skip-proof reliability, especially across long research projects or regulatory submissions.
Not every supplier runs with the same discipline. Take time to check for ISO or GMP certification. Top-tier suppliers give details for water content and limits on magnesium, sodium, or potassium. In my experience, a supplier who responds quickly to requests for spectrographic data and batch certifications earns more business in the long run.
Purity may look like a simple number, but it’s the difference between repeatable success and avoidable headaches. The right grade gives confidence, not just to meet a protocol, but to drive new discoveries or keep large-scale production on track.
| Names | |
| Preferred IUPAC name | strontium dichloride hexahydrate |
| Other names |
Strontium dichloride hexahydrate Strontium(II) chloride hexahydrate Strontium chloride, 6-hydrate |
| Pronunciation | /ˈstrɒn.ʃi.əm klaɪˈrʌɪd ˌhɛk.səˈhaɪ.dreɪt/ |
| Identifiers | |
| CAS Number | 10025-70-4 |
| Beilstein Reference | 3589798 |
| ChEBI | CHEBI:75961 |
| ChEMBL | CHEMBL1201682 |
| ChemSpider | 21541917 |
| DrugBank | DB09149 |
| ECHA InfoCard | 100.029.214 |
| EC Number | 233-971-6 |
| Gmelin Reference | 81665 |
| KEGG | C14436 |
| MeSH | D013320 |
| PubChem CID | 24868154 |
| RTECS number | WK8570000 |
| UNII | ZL6J3QG9C3 |
| UN number | UN1760 |
| CompTox Dashboard (EPA) | DTXSID3055613 |
| Properties | |
| Chemical formula | SrCl2·6H2O |
| Molar mass | 266.62 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 1.9 g/cm³ |
| Solubility in water | Very soluble |
| log P | -4.0 |
| Acidity (pKa) | 7.0 (H₂O) |
| Magnetic susceptibility (χ) | +1020.0e-6 cm³/mol |
| Refractive index (nD) | 1.465 |
| Viscosity | Viscosity: 1.3 cP (20 °C) |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 322.6 J/(mol·K) |
| Std enthalpy of formation (ΔfH⦵298) | -1332.6 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | Strontium Chloride Hexahydrate does not have a widely reported standard enthalpy of combustion (ΔcH⦵298) value because it is an inorganic salt and does not combust in the conventional sense. |
| Pharmacology | |
| ATC code | V09GX02 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. |
| Precautionary statements | P264, P270, P280, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-0-1 |
| Lethal dose or concentration | LD₅₀ Oral - Rat - 1,750 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 = 2,257 mg/kg |
| NIOSH | # 10025-70-4 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Strontium chloride Strontium nitrate Strontium carbonate Strontium sulfate Strontium hydroxide |
