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The story behind dysprosium nitrate hydrate connects deeply with the evolving narrative of rare earth elements. Dysprosium first appeared on the scientific radar in the late 19th century. French chemist Paul Émile Lecoq de Boisbaudran pulled dysprosium from holmium oxide through painstaking separations. Early uses stayed limited due to the complexities of isolation, but in the 20th century, researchers found that rare earth elements, including dysprosium, could handle thermal and magnetic extremes. These discoveries opened doors for chemical compounds like dysprosium nitrate hydrate, which emerged as essential players in modern technology. The ability to control the synthesis and purity of this hydrate built a launchpad for advanced research in magnetism, optics, and catalysis. Watching the journey of dysprosium through decades of trial and error, I see how progress grows from persistence—breakthroughs rely on the tenacity of scientists who refuse to settle for partial solutions.
Dysprosium nitrate hydrate arises as a crystalline salt, bringing a straightforward structure to some of the more complicated problems in material science and engineering. The compound falls under the broader umbrella of rare earth nitrates and distinguishes itself through its solubility and reactivity. Industry and academia alike turn to dysprosium nitrate hydrate for its performance in doping, catalysts, specialty glass, and magnet fabrication. These uses spring from the synergy between dysprosium ions and the nitrate counterion, a relationship that shapes its chemical reactivity and material transformation potential. Quality hinges on achieving high purity and consistent hydration—differences here shift how the compound behaves under experimentation or in manufacturing processes. After working with chemical reagents on various research projects, I recognize how these behind-the-scenes decisions ripple through both basic research and finished products alike. Small improvements in preparation and handling eventually trickle out to electronics, healthcare, and beyond.
This compound shows itself as a colorless or slightly yellow crystal, easily dissolving in water and alcohols. Its hygroscopic nature encourages it to draw in moisture from the air, so handling under controlled conditions avoids frustrating clumping or loss of integrity. On the chemical side, the powerful oxidizing character of the nitrate group partners with dysprosium’s trivalent state to drive a wide array of reactions, from precipitation to complexation with organics and inorganics. Melting points can vary with the number of water molecules attached, and thermal decomposition pushes off nitrogen oxides, an observation that always reminds me of chemical safety’s non-negotiable status in the lab. The precise physical state—crystalline, granular, or amorphous—depends on preparation, influencing everything from how the compound dissolves to its shelf life. The solid state properties often tie directly into the technical hurdles faced by researchers or industrial chemists.
Decades of tightening regulatory expectations and growing customization have shaped how dysprosium nitrate hydrate finds its way into research labs and factories. Labels often call out not just chemical formula and hydration, but also purity, batch number, and the presence of trace metals. Specifications can drill down to the parts-per-million level, with companies and universities refusing anything less for high-stakes applications. From my experience, strict documentation brings peace of mind, knowing that every bottle matches what the project demands—otherwise, false data or failed syntheses follow. Technical information flags hazards too, often sporting symbols to alert handlers to oxidizer status and moisture sensitivity, and effective systems cross-reference regulatory lists to keep labs compliant.
Production of dysprosium nitrate hydrate starts with dysprosium oxide, processed with nitric acid under tightly controlled temperatures and dilution ratios. The solution is often carefully evaporated down, with chemists coaxing the water of hydration into the final solid through temperature and humidity adjustments. Over-crystallization or incomplete reaction means the product’s performance drops, so protocols build in checks at every stage—verifying pH, verifying clarity, filtering out insoluble debris. Recrystallization may follow, stripping away unwanted ions and contaminants that could sabotage sensitive work downstream. The number of hydrates commonly encountered—six, seven, sometimes five—depends on drying and crystallization’s intricate dance, and scientific teams keep close records so the compound’s water content matches its intended application. In my own work, the way a slightly altered humidity profile changes a batch underlined how much reliability comes through obsessive control and record-keeping. Engineers and chemists chase repeatable, documented routes because everything from research to manufacturing depends on consistency.
Dysprosium nitrate hydrate serves as a reliable source of Dy3+ ions—a launching point for preparing complex oxides, fluorides, phosphates, and other compounds. In school demonstrations, adding solutions of this nitrate to sodium carbonate brings a quick precipitation of dysprosium carbonate, which then paves the way for ceramic or optical material synthesis. In redox chemistry, the nitrate moiety steps up as an oxidizer, sometimes speeding along organic transformations or acting as a route to other rare earth salts. Coordination chemistry explores ligands tethering to the central ion, a key method for designing new catalysts or luminescent compounds. Over the years, I’ve found these reactions more than textbook curiosities; successful modification often decides whether new materials can leave the confines of lab notebooks for real-world products. Failures here sometimes uncover insights about stability or reactivity that ultimately guide safe and effective process scaling.
The label on a bottle might read “Dysprosium(III) nitrate hydrate,” “Dysprosium trinitrate hydrate,” or simply the CAS registry number. Trustworthy suppliers stick to IUPAC rules, but some stockrooms still use legacy names picked up from previous generations of chemists. International shipment or collaboration means sometimes deciphering technical jargon—clear naming avoids costly mistakes where a subtle change in hydration or purity alters whole experiments or production runs. My own frustration with mislabeled bags in shared labs underscored how one missing word or number can turn a routine protocol into a messy troubleshooting quest.
Dysprosium nitrate hydrate brings genuine safety considerations into focus. Strong oxidizing properties make storage away from combustibles a must, and personnel working with the compound guard against inhaling dust or letting the material come into prolonged skin contact. Standard PPE—gloves, laboratory coats, and safety glasses—remains the norm, but so does a careful look at reaction partners; accidental mixing with reducing agents brings a risk of heat and gas release. Airflow and containment matter; simple vigilance and a sound chemical hygiene protocol kept me and my colleagues out of trouble more than once. Labeling covers GHS hazard warnings, and up-to-date SDS copies remain within arm’s reach. Operational standards extend to waste disposal, since nitrate contamination in waterways or municipal systems seeds environmental headaches. Commitment to training and real-time hazard communication maintains both human and environmental safety as new uses and larger quantities enter circulation.
In the last decade, dysprosium nitrate hydrate carved out a spot in the pipeline of cutting-edge technologies. Its primary role connects to advanced magnets, especially in permanent magnet motors destined for wind turbines, electric vehicles, and consumer electronics. Magnetic strength and thermal stability of these devices stem directly from dysprosium’s unique electron structure, and nitrate forms simplify introduction of dysprosium into intermediate compounds and alloys. In optical materials, the compound facilitates production of specialty glasses with high refractive indices, supporting laser development and multi-spectral imaging. Some medical imaging fields rely on dysprosium-based agents for better tissue contrast, and the catalysis world continues to push the element into unexplored reaction cycles. Responsibility comes with broadening applications; the rise of dysprosium-based compounds makes questions about ethical sourcing and supply chain stability unavoidable. From personal experience teaching advanced inorganic labs, excitement over new applications rarely eclipses questions about long-term supply or environmental impact.
Pushing boundaries remains at the heart of research using dysprosium nitrate hydrate. Teams worldwide look for new crystalline phases and composite materials that harness the strong spin-orbit coupling and magnetic anisotropy which dysprosium affords. Nanoscale magnetism, high-capacity data storage, and quantum computing prototypes often turn back to this compound for starting materials. Partnerships between universities and manufacturers drive the hunt for more responsible preparation methods and recycling processes, given the heightened scrutiny on rare earth extraction. Next-generation optical amplifiers, waveguides, and bioimaging agents draw directly from synthesis protocols designed around dysprosium nitrate precursors. In discussions I’ve had with colleagues, the tension between pushing research frontiers and managing limited supply highlights the need for creative chemistry and cross-disciplinary awareness. Each improvement in yield, purity, or environmental footprint broadens the spectrum of what these compounds make possible for science and technology.
Toxicity remains an area needing constant attention as dysprosium nitrate hydrate moves into new spheres. Current data suggest moderate toxicity by ingestion or inhalation, with rare earth elements known to accumulate in bone and liver tissue after chronic exposure. Long-term environmental effects, particularly to aquatic life, prompt responsible disposal practices and ongoing biomonitoring. Laboratory studies have found low acute toxicity in standard testing models, but uncertainties around nanoparticle forms and chronic low-dose exposure push regulators and researchers to keep probing. My own experience reviewing toxicity data emphasizes gaps rather than answers—what is known often comes from high-dose or industrial incident contexts, and insidious effects related to low-level, persistent exposure get less attention. The chemical’s nitrate component can also cause methemoglobinemia through exposure, reinforcing the need for real chemical risk assessment and transparent labeling.
Outlook for dysprosium nitrate hydrate intertwines with the broader fate of rare earths. Demand from next-generation magnets, electric vehicles, and energy systems points to steady if not explosive growth. At the same time, the geopolitics of rare earth mining presses for better recycling and smarter resource management—shortages or price spikes challenge even the most resilient supply chains. Innovation in green chemistry seeks ways to regenerate or reuse dysprosium from spent devices, sidestepping some mining-related impacts. New research on single-atom magnets, luminescent medical probes, and high-entropy alloys could spark breakthroughs reliant on steady access to dysprosium-based compounds. Walking the line between promise and peril means developing transparent, robust regulatory oversight and committing funding for toxicity research. Whether in academic labs or manufacturing floors, careful stewardship of dysprosium compounds, including the nitrate hydrate, will decide how deeply these chemicals shape the next wave of technological advances.
Growing up, plenty of people never even heard the word “dysprosium.” Most folks still don’t think about it unless they’re deep in the science or tech industry. Dysprosium nitrate hydrate stands in the spotlight because it brings some unique attributes to the field of high-performance magnets and advanced materials. Getting a grip on what role it plays and why it matters helps explain a bigger story about rare earths, innovation, and the future of modern technology.
Walk into any shop that repairs electric vehicles or wind turbines, and there’s a good chance the technicians depend on magnets that use dysprosium compounds. Dysprosium nitrate hydrate works well as a precursor, feeding into the process that enhances neodymium-iron-boron magnets. These magnets offer reliability under heat and intense use—necessary for electric cars and wind farming.
The fact these magnets resist demagnetization under high temperatures makes them a backbone component for motor manufacturers. High-performance magnets support everything from laptop hard drives to advanced mining equipment. This makes dysprosium nitrate hydrate an essential building block in modern electronics and clean technology.
Move beyond magnets and dysprosium compounds show up in other corners of industry. Ceramics producers rely on specialty dopants to tune colors and physical properties in their materials. Dysprosium nitrate hydrate does that job, letting them achieve certain yellows and lightfast finishes.
The lighting industry, in its search for better energy efficiency and color accuracy, uses dysprosium salts. Halide lamps—favored in stadiums or on film sets—draw on dysprosium technology for whiter, brighter light. For me, seeing a sports event under clean, crisp floodlights is something most people don’t even know depends on rare earth chemicals.
Laser manufacturers turn to dysprosium compounds too. Coating optics or doping materials in solid-state lasers, dysprosium influences wavelength and stability. This technology finds roles in medical treatment, research, and manufacturing.
Getting a stable supply of dysprosium sources ranks as a tough challenge. The stuff doesn’t show up everywhere, and mining or processing can take a heavy environmental toll. China produces most of the world’s dysprosium, putting global manufacturers at the whim of trade policy and export controls.
As a science writer who’s followed rare earth supply chains, it’s clear a shift needs fresh ideas. Researchers are investing in ways to recycle used magnets—pulling out dysprosium and other rare earths for re-use. Smarter design keeps magnets efficient, using less dysprosium by targeting only the areas that need top heat resistance. Some teams experiment with fully synthetic materials, hoping to sidestep the rare earth problem altogether.
Recycling, better engineering, and more responsible mining all have a seat at the table. Moving forward, new sources and smart resource management will make sure that the next big step in technology doesn’t hit a roadblock over material shortages.
Dysprosium nitrate hydrate pops up in places most people never think to look. The chemical formula for dysprosium nitrate hydrate is Dy(NO3)3·xH2O, with “x” standing for the number of water molecules attached per formula unit. Most suppliers and labs encounter it as the pentahydrate, Dy(NO3)3·5H2O. That single formula reveals a lot about this compound and puts it right at the center of research involving lasers, nuclear reactors, and even the production of magnets in wind turbines and electric vehicles.
Every subscript and letter means something for scientists and manufacturers. People sometimes overlook exactly how much effort goes into breaking down complicated names into formulas. That number of hydrated water molecules shapes how the material feels, reacts, stores, and dissolves. As someone who has worked with rare earths in a university lab and who’s dealt with batches that arrived bone-dry versus crystalline and damp, the number of waters changes everything about how the powder pours, how it reacts, and how you should store it.
Having the right chemical formula in front of you stops expensive mistakes. Mix up anhydrous with pentahydrate, and your calculations go out the window. That means errors in laboratory results, wasted resources, and sometimes contaminated or ruined experiments—a real headache when some rare earths cost several thousand dollars per kilogram. Some professors keep outdated copies of formula sheets on hand for quick reference. I learned early on never to trust a single label and to double-check certificates of analysis.
Dysprosium might not be a household term, but it shapes technologies the world uses every day. Dysprosium nitrate hydrate feeds into processes that strengthen magnets. These magnets end up running inside phones, headphones, and cars. In the reactor world, dysprosium absorbs neutrons, keeping reactors running at a safe speed. The pentahydrate form dissolves well in water, which makes it easy to use in preparing solutions or thin films for electronics and optics projects.
Precision counts here. Patents depend on exact formulas for intellectual property protection. Environmental health relies on accurate labeling—mishandling nitrate salts creates risks for explosions in storage or mixing.
The formula isn’t just a code. It’s information that guides safe handling, storage, and transport protocols. In my own experience, short storage in humid conditions can shift the hydrate ratio, which then misleads anyone coming to use it later. Sourcing dysprosium nitrate hydrate from reputable suppliers matters more today than ever, with more counterfeit and impure batches reaching the market. Analysis tools like X-ray diffraction and thermogravimetric analysis help confirm that what’s in the drum matches what’s on the sheet.
There’s a lot riding on getting formulas right. Researchers, teachers, students, and engineers need to focus on chemical literacy—knowing formula conventions, hydration states, and what that means for daily work. Keeping up with the basics helps people innovate responsibly, saves time and money, and keeps everyone safer around materials that don’t get much attention but quietly power the world’s biggest leaps.
Walking into any research lab, shelves filled with chemicals reveal one unchanging truth: sloppy storage causes trouble. Chemicals like Dysprosium Nitrate Hydrate aren’t on every bench, but on the shelf or in the supply cabinet they demand respect. Scientists use this compound for magnetics, phosphors, and more, but the real experiment starts long before any beaker gets filled. One spill or botched setup turns a routine morning into a full-blown headache.
Dysprosium Nitrate Hydrate draws water from the air. That may sound harmless, but it can quickly wreck the chemical's usefulness and create waste. Open-air storage leads to lumps, stuck jars, or—worst of all—compromised results. Even seasoned lab techs can get tripped up if they don’t return the jar promptly or miss a shred of lint in the cap. I’ve seen entire batches lost just because someone left things out during inventory.
Tight-sealing containers aren’t a recommendation, they’re a must. Glass works best, although plastic sometimes gets the job done for short periods. An air-tight jar with a strong lid keeps moisture and contaminants away, meaning the compound stays reliable. Shelf life stretches out instead of shrinking down to a couple of weeks. After spending solid money on rare earth salts, no lab wants to fork out more because of “temporary” lids or a lazy repackaging job.
Every chemical store in a lab needs a dry and cool spot. Don’t think of the back corner or a cluttered fridge where people toss half-finished lunches. Dedicated cabinets—away from direct sunlight, humidity, and temperature swings—make sense. I know the hassle of sharing space, but isn’t it better to trade a few steps for batches that actually perform? Fluctuating temperatures condense water inside containers, which spells disaster for hygroscopic salts like this one.
Proper labeling is a lifesaver, not fussy protocol. Bags of mystery powder or jars missing clear data waste time and threaten safety. Dates, supplier information, and hazard warnings belong right on the label. In a busy lab, fresh hands or new hires often grab the closest jar. No one should have to guess what’s inside. Regular inventory checks flag problems before they hit project timelines.
Handling Dysprosium Nitrate Hydrate takes chemical-resistant gloves and goggles. Dust masks come out when transferring powders. Even with nothing spilled, a stray crystal can find its way onto your sleeve or hand. A dedicated spill kit stashed under the bench keeps accidents from growing into emergencies. Training up every new lab member saves more than just material—it prevents accidents that send people to the ER.
Disposal shouldn’t get treated as an afterthought. Unused Dysprosium Nitrate Hydrate and any spills should go through a hazardous waste stream, following local and institutional rules. Tossing it in the bin or tipping it down the drain is a shortcut that will cause massive headaches, both legal and environmental. Well-marked waste containers in a dedicated disposal area help keep things responsible.
Creating a culture of care with rare earth compounds benefits everyone—no exceptions. Careful storage, real respect for hazards, and better organization mean discoveries happen without delays, injuries, or legal headaches. Labs that manage Dysprosium Nitrate Hydrate well set a higher standard for safe, responsible research, no matter who's on shift.
Dysprosium Nitrate Hydrate isn’t something you see on a pharmacy shelf. Labs and factories use it for everything from magnets to research work. Whenever I come across rare earth chemicals in my career, I pay close attention to safety data sheets and firsthand stories from colleagues. The facts are clear: this compound poses hazards if people get careless with handling, storage, or disposal.
One thing I’ve learned in real-world lab settings: splash goggles make a difference. Accidents don’t schedule an appointment, and I’ve seen what happens when someone skips them. Safety goggles protect your eyes, and gloves—nitrile or neoprene—keep hands safe from direct contact. Long sleeves and closed-toed shoes add a layer of defense. Trust your nose less. Dysprosium compounds don’t always announce themselves with a strong odor, so you can’t count on your senses.
People often forget about ventilation until a strange smell fills the air. Even though Dysprosium Nitrate Hydrate isn’t as volatile as some chemicals, that dust floats around when weighing powder or cleaning up spills. Open windows, work in a fume hood if possible, and never treat this as an afterthought. Universities highlight this risk for good reason, and OSHA guidelines push for fume hoods for nitrates. Risks go up fast once you skip basics.
Spills scare people more than bottles on a shelf. Here’s the thing I tell newcomers: small spills get cleaned up with gloves, damp cloths, and a steady hand. Don’t kick up dust and don’t mix with other chemicals—certain combinations can heat up or release toxic fumes. Eyes flushed right away with water, skin washed with soap and water. Accidental ingestion or inhalation means a trip to the doctor, not a wait-and-see attitude. You can always replace chemicals, but you can’t replace your health.
This compound likes dryness and a stable temperature. Humidity breaks down packaging and can change how the chemical behaves. Store it in a closed, labeled container—away from acids, combustibles, and organic materials. I store similar compounds in cabinets far from heat sources, away from regular foot traffic, and on lower shelves to lower the chance of broken glass. Safe storage isn’t rocket science, but it takes discipline.
Hazardous waste deserves respect. Dumping Dysprosium Nitrate Hydrate down the sink or tossing in regular trash spreads contamination quickly. Environmental Protection Agency (EPA) rules spell out steps, and most labs have a log for disposal. Treat every small leftover as hazardous—collect it in a labeled waste container and deliver to the right collection point. Community safety hangs on these habits.
Training sessions matter. The sharpest chemists I know still check in with a colleague during tricky procedures. Sharing mistakes helps everyone learn—not just the person making them. Posters, reminders, and daily walk-arounds reduce risk. If you see something unsafe, speak up and act quickly.
Some places take pride in safety routines; others cut corners. Regular refreshers, shared lessons learned, and always having spill kits on hand go a long way. Mistakes cost more than money—they cost trust and health. Each day handling Dysprosium Nitrate Hydrate brings a new chance to respect that lesson and create a safer workspace for everyone.
I always enjoy seeing chemistry questions pop up in daily conversations. Dysprosium nitrate hydrate falls into the category of rare earth metal salts—a mouthful, but these materials are no strangers to the science bench. The first instinct for any chemist faced with a nitrate salt usually involves grabbing a beaker of water, giving it a good stir, and watching what happens. Nitrates, in general, tend to dissolve easily. Dysprosium nitrate hydrate is no exception; water breaks it right down.
The science here backs up what chemists have relied on for years: dysprosium nitrate hydrate dissolves well in water, forming a clear solution. Solubility like this isn’t just some academic note. It shapes how this chemical gets used every day. The nitrate group attached to dysprosium holds hands with water molecules, letting them surround the salt and pull those ions apart. This process isn’t just a neat lab trick; it fuels industries that need rare earth solutions for everything from magnets to lighting to research.
I’ve seen university labs use dysprosium nitrate hydrate as a starting point for preparing pure dysprosium compounds. The story always starts the same: dissolve the hydrate in water to get an easy-to-handle solution. Working with a dissolved salt, researchers can tweak pH or add other chemicals, watching new materials form right in front of them. Imagine working on lasers or new screen displays—the journey often begins with a bit of water and a small pile of dysprosium nitrate hydrate.
Solubility isn’t just about convenience; it carries environmental responsibility. Whenever you dissolve dysprosium nitrate hydrate, you create ions floating in the water. Improper disposal of these solutions could cause trouble for water supplies—rare earth metals aren’t something anybody wants running wild in rivers or streams. Some countries already keep strict rules about handling and waste, but labs everywhere need to respect those safety lines. Strong procedures, good labeling, and clear planning make a real difference. I’ve seen spills avoided because someone stopped to double-check the waste container before pouring out a solution.
Chemical solubility shapes much more than laboratory convenience—it also impacts cost. Extracting dysprosium from ores costs a lot of time and money, and converting it into a water-soluble nitrate cuts down on wasted resources. Still, the demand for rare earth elements pushes us all to ask tough questions. Can recycling catch up with usage? Some research groups already work on pulling dysprosium and other rare earths out of electronic waste. Simple chemistry—like dissolving in water—opens the door, but safe collection and careful processing set the real limits.
It’s easy to get lost in chemical textbooks, but facts from hands-on work make complex science approachable. Solubility data get published in peer-reviewed papers—check sources like the CRC Handbook of Chemistry and Physics or journal articles from established societies. Trust stems from repeated experiments, clear reporting, and willingness to answer tough questions. Dysprosium nitrate hydrate dissolves in water because science delivers consistent results, not just because someone repeats it online. If anyone’s curious, look into MSDS sheets or supplier technical data for confirmation.
| Names | |
| Preferred IUPAC name | dysprosium(3+) trinitrate hydrate |
| Other names |
Dysprosium(III) nitrate hydrate Dysprosium trinitrate hydrate Dysprosium nitrate, hydrate Nitric acid, dysprosium(3+) salt, hydrate |
| Pronunciation | /daɪsˈproʊziəm ˈnaɪtreɪt haɪˈdreɪt/ |
| Identifiers | |
| CAS Number | 10031-49-9 |
| Beilstein Reference | 3575949 |
| ChEBI | CHEBI:51813 |
| ChEMBL | CHEMBL4296376 |
| ChemSpider | 11350623 |
| DrugBank | DB14638 |
| ECHA InfoCard | ECHA InfoCard: 03d9f884-54e3-4ff9-8476-d2363046816b |
| EC Number | 236-403-1 |
| Gmelin Reference | 77939 |
| KEGG | C18698 |
| MeSH | D008456 |
| PubChem CID | 159454 |
| RTECS number | VO8225000 |
| UNII | P371X68GGL |
| UN number | UN3288 |
| Properties | |
| Chemical formula | Dy(NO3)3·xH2O |
| Molar mass | 373.06 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 2.68 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -4.3 |
| Basicity (pKb) | 8 at 25 °C |
| Magnetic susceptibility (χ) | +11600e-6 cm³/mol |
| Refractive index (nD) | 1.57 |
| Dipole moment | 1.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 427.8 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1977 kJ/mol |
| Pharmacology | |
| ATC code | V09XX04 |
| Hazards | |
| Main hazards | Oxidizing, harmful if swallowed, causes serious eye irritation |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS03, GHS07, GHS09 |
| Signal word | Danger |
| Hazard statements | H272, H315, H319, H335 |
| Precautionary statements | P264, P280, P301+P312, P304+P340, P305+P351+P338, P312, P330, P337+P313, P501 |
| NFPA 704 (fire diamond) | 1-0-0-ox |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 > 5000 mg/kg |
| NIOSH | Not established |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | 10-30°C |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Dysprosium(III) oxide Dysprosium(III) chloride Dysprosium(III) acetate Dysprosium(III) sulfate Dysprosium(III) fluoride |
