Знание
Cobalt Acetate Anhydrous: Insightful Commentary on Its Role and Development
Historical Development
Cobalt acetate anhydrous popped up on the radar when chemists explored cobalt’s value in pigments and catalysts during the industrial revolution. In the early 1800s, cobalt really gained popularity among glassmakers for its intense blue tint, but curiosity didn’t stop at color—it spread to the substance’s other compounds. Researchers found, as they worked with cobalt in analytical chemistry, that its acetate form handled reactions pretty efficiently. Factories scaled up production as the synthetic dyes and chemical manufacturing boomed, especially in the 20th century. Cobalt compounds, once reserved for art and glass, grew into an integral part of organic synthesis and electronics, where cobalt acetate anhydrous cemented its reputation. Each step in modern chemistry—from transition metal catalysis to battery technology—owes something to persistent work with cobalt salts, driven by both necessity and experimentation.
Product Overview
Cobalt acetate anhydrous, a neat crystalline powder, regularly delivers cobalt ions where moisture throws a wrench in typical lab work. As someone who has managed chemical inventories, I find dry cobalt acetate to be less fussy than its hydrated relatives. Handling it in a lab or industrial setting means less worry about clumps or variable concentrations. This product consistently appeals to anyone working on fine chemicals synthesis or running pilot plants that cannot afford surprises in feedstock quality.
Physical & Chemical Properties
Cobalt acetate anhydrous brings a pinkish tone and granular texture, often recognized before the bottle even gets labeled. Its melting point hovers just above 200°C, which matters for thermal decomposition processes. Solubility in water keeps it versatile; it dissolves readily, letting its cobalt cations do their job in various chemical settings. Unlike some transition metal salts, this compound doesn’t break down unless pushed hard with heat or strong reducing agents. Air doesn’t touch its stability much, but humid storage conditions risk hydration, so tight sealing helps retain the anhydrous state. When introduced to acids or bases, cobalt acetate dissolves or precipitates predictably, meaning no nasty or dangerous surprises for seasoned handlers.
Technical Specifications & Labeling
Reliable supply hinges on clear labeling and a thorough specification sheet. Purity levels typically exceed 98%, and as someone careful about cross-contamination, I check for trace metal impurities, especially iron or nickel. Particle size and bulk density might seem dull, but these affect dosing and blending, particularly in automated reactors. Every batch gets a CAS number—71-48-7 stands out here—along with manufacturer data such as batch code, shelf life, and hazardous materials symbols. Good practice includes storage instructions plain as day, mentioning desiccators or airtight containers, and an emergency contact line for suspected exposure. I’ve seen that well-labeled packaging heads off half the headaches, as it saves trouble both in inventory and in case of a spill.
Preparation Method
Factories synthesize cobalt acetate anhydrous by reacting cobalt(II) oxide or basic cobalt carbonate with glacial acetic acid, running the process hot to drive out water. The method produces aqueous cobalt acetate, which is dried under vacuum or in an inert current, stripping every hint of moisture. Efficient distillation setups and chemical engineers watch temperatures closely, aiming for a smooth transition from wet to dry salt. Smaller labs may follow similar steps but usually in glassware, using rotary evaporators and carefully measured stoichiometry. It’s a lesson in patience: rush drying and impurities linger; slow and steady yields pure, anhydrous crystals. Years working in scale-up taught me this consistency often beats speed in specialty chemicals.
Chemical Reactions & Modifications
Cobalt acetate anhydrous acts as a springboard for dozens of transformations. In catalytic processes, this salt lends its cobalt(II) ions to acetoxylation and oxidation reactions. In organic synthesis, it helps build complex molecules, forming stable but reactive intermediates. Reacting with phosphines or nitrogen ligands, it forms coordination complexes that can unlock advanced catalytic cycles. Reducing agents knock cobalt down to its metal form or shift it to other oxidation states, handy for both material science and plating. Sometimes, acetates react with halides to churn out new salts or hybrid materials, showing off cobalt’s adaptability across science and engineering fields.
Synonyms & Product Names
Chemists and suppliers swap out several names: cobalt(II) acetate anhydrous, cobaltous acetate, and cobalt(II) ethanoate pop up in catalogs. Across languages, the structure stays the same, reflecting acetic acid’s bonding with cobalt. Commercial sources, especially in Asia and Europe, brand it with internal codes or trade names, but everyone circles back to standard nomenclature for safety and customs forms. I’ve avoided errors more than once by double-checking these synonyms while ordering or transferring inventory. If two names sound similar but one specifies ‘anhydrous’, you sidestep mistakes with careful review.
Safety & Operational Standards
Handling cobalt acetate anhydrous in any lab means treating it with real concern for health. Dust inhalation irritates the lungs, and cobalt ions carry known toxicity—so gloves and goggles land on my hands and face before the lid comes off. Proper local exhaust in fume hoods and spill trays protects against airborne particles. Companies lean hard on GHS labeling, displaying health hazard icons, and outlining PPE requirements. Regular staff training, from waste disposal right up to first aid drills, makes sure everyone knows what to do in an accident. As regulations tighten, especially for potential carcinogens like cobalt compounds, good labs prioritize workplace monitoring, periodic medical checks for workers, and robust incident reporting. Personal experience tells me that shortcuts or carelessness, even on busy days, just magnify risks that linger long after one shift ends.
Application Area
Cobalt acetate anhydrous takes on a hefty role in chemical industries and research labs. Catalysis stands out—acetic acid production and oxidative coupling reactions both lean on this substance. In PET resin manufacturing, it functions as a catalyst for polymerization, helping build plastics for bottles and textiles. It upgrades paint dryers and inks, and improves the finish in metal plating. My time working with radiolabeling and advanced batteries opened my eyes to how cobalt salts enable better imaging agents and power storage. Academic labs chase new compounds using cobalt acetate as a precursor, whether in coordination chemistry or new magnetic materials. Its reach stretches between bulk manufacturing and boutique synthesis, linking old-school chemistry to cutting-edge tech.
Research & Development
Most innovation with cobalt acetate anhydrous happens where green chemistry and advanced electronics intersect. Research teams tinker with lower-waste oxidation routes and support materials to capture and recycle spent catalyst. Nanotechnology benefits from controlled cobalt deposition, and researchers push to miniaturize electronic components using these salts. Pharmaceutical developers investigate cobalt complexes for anti-cancer and antimicrobial drugs, tinkering with the acetate’s core structure to improve biological activity. Lab groups across continents share results in peer-reviewed journals, seeking safer and more efficient uses of cobalt compounds. Years reviewing funding proposals showed me the healthiest R&D pipelines pull talent from surface science, catalysis, and biomedical fields—no one discipline pulls ahead unless they stay curious about cobalt acetate’s next trick.
Toxicity Research
Cobalt acetate anhydrous ranks as hazardous if inhaled, ingested, or brought repeatedly into contact with skin. Study after study confirms cobalt ions can cause DNA damage, trigger allergic reactions, or disrupt heart function when exposure goes unchecked. Regulatory bodies—including OSHA, REACH, and NIOSH—dictate strict permissible exposure limits and demand thorough risk assessments. Animal models point to both acute and chronic toxicity, urging safer handling protocol not just in the plant but all the way through waste disposal. This attention, built from clear clinical and chemical evidence, pushes companies and researchers to substitute safer alternatives or build in robust engineering controls. I’ve seen firsthand that early planning, accurate exposure monitoring, and careful adherence to regulations blunt most hazards, but complacency always threatens progress.
Future Prospects
If trends stay on track, cobalt acetate anhydrous looks poised for a more specialized future. Advances in batteries and electric vehicles, where cobalt compounds improve energy density, might shift demand from bulk chemical synthesis toward advanced energy research. At the same time, improvements in hydrogen production and green catalytic cycles keep chemists working out new reactions where cobalt acetate plays a starring role. Environmental pressures push industries to recycle more cobalt and minimize disposal risks, calling for better recovery processes and alternatives that reuse or replace this compound. Having spent time in both research and compliance meetings, I sense that as demand for greener tech rises, so will transparent sourcing and lifecycle tracking of cobalt acetate. Scientists and regulators both seem to pull in the same direction, shaping its future around safety, sustainability, and smarter application—driven by decades of learned experience and a keen eye on where chemistry can help solve society’s biggest puzzles.
The Importance of Cobalt Acetate Anhydrous
Cobalt acetate anhydrous might not grab headlines like tech gadgets or clean energy breakthroughs, but many pieces of everyday life depend on what happens with this powdery chemical. Over the years working in industrial manufacturing, I’ve watched cobalt acetate anhydrous make its mark, far away from public attention, but not far from our daily experience.
Catalyst Powerhouse for Plastic and Paint
Polyester fibers, bottles, and films start with a chemical reaction called polymerization. Cobalt acetate anhydrous steps in as a key catalyst in this process. Thanks to its chemical properties, it speeds up reactions that link molecules to form the tough, flexible plastics holding our drinks or carrying our groceries. The next time I spot a clear plastic bottle, it’s hard not to think of the teamwork between chemists and industrial workers using a bag of this cobalt salt to make it happen.
Paints and inks shine brighter and cure faster with the help of cobalt acetate anhydrous. It acts as a drying agent, pulling oxygen from the air, which helps finishes harden fully. In art and construction, a wall’s glossy coat or a magazine’s vibrant colors often owe something to chemists who measure out this compound in just the right amounts.
Batteries and the Push Toward Sustainability
Electric cars and smartphones rely on lithium-ion batteries, and cobalt forms an essential ingredient in the cathodes. Cobalt acetate anhydrous helps prepare the precursors for the metallic cobalt needed in these batteries. With demand for longer battery life and safer charging, companies chase purer, more reliable cobalt compounds, and refined cobalt salts make all the difference.
Not all cobalt mining meets ethical standards. My background in chemical supply chains reminds me of the need for transparency from mine to factory. Manufacturers now track their cobalt sources, seeking ethical suppliers and investing in recycling. By improving traceability, the industry shrinks the risks of child labor or environmental harm.
Petrochemicals to Pharmaceuticals
Refineries often turn to cobalt acetate anhydrous to remove sulfur from petroleum products. Sulfur scrubbing helps cut down on harmful emissions from fuels, so a clean fuel standard starts with smart chemistry. In the pharmaceutical world, cobalt acetate gets used in synthesizing vitamins and other medical ingredients. Purity here isn’t just a buzzword—it can influence patient health.
What Needs to Change?
Handling chemicals like cobalt acetate anhydrous carries risks. Safety gear and strong ventilation stay high on my list after seeing colleagues with chemical burns or respiratory trouble. Training programs and clearer labeling can go a long way. Chemical spills rarely get public attention, but workers remember them.
As new battery technologies and stricter rules change the landscape, the call for alternatives won’t go away. Scientists work on manganese or iron-based chemistries, hoping to reduce dependence on cobalt. Until then, industry leaders must keep pushing for better supply chain rules and invest in recycling, because every reused gram of cobalt cuts down the need for new mining.
Final Thought
Cobalt acetate anhydrous links up with some big problems and promising solutions—from cleaner air to longer-lasting electronics. Each step forward, whether in greener chemistry or better worker protection, comes down to the way people handle a substance few have even heard of, but almost everyone relies on.
Chemical Identity and Significance
The chemical formula for Cobalt Acetate Anhydrous is Co(C2H3O2)2. This means each molecule contains one cobalt atom and two acetate groups. The 'anhydrous' part means no water molecules join this specific compound, which changes how it behaves in reactions. This isn’t just textbook knowledge — those details shape how it gets put to work in labs and factories.
Personal Experience in Practical Use
I’ve handled cobalt acetate in the lab. Anhydrous forms always demand close attention because water brings its own problems if you’re aiming for reliable results. Projects involving organic synthesis or creating catalysts often use cobalt compounds. If you grab a hydrated version by mistake, the extra water throws off the mass calculations, leading to odd results. Cobalt acetate anhydrous delivers more precision. Scientists and students alike learn pretty quick that chemical formulas aren’t trivia — they anchor a lot of what works or doesn’t in the lab.
Why Purity and Formula Make a Difference
Purity means outcomes you can predict and trust. A batch that swaps in hydrated cobalt acetate by accident introduces water, opening up unwanted reactions. Take catalyst production: industries that make paint driers or PET plastics will see efficiency nosedive if they cut corners with the wrong cobalt salt. Even small impurities or hydration mess up color, texture, and even safety. Knowledge about exact formulas flows into better decisions from the lab bench to full-scale production lines.
Industrial and Academic Impacts
Cobalt acetate anhydrous doesn’t just stay in the lab. Businesses count on it, especially those making adhesives, dyes, and ceramics. Academic labs turn to it when building tools to map new reactions. I’ve seen researchers waste precious weeks because they didn’t double-check whether they grabbed cobalt acetate anhydrous or a hydrated cousin. Mistakes at this step create project setbacks and add unexpected expenses. Knowing formulas and using them precisely saves more than just pride — it prevents real-world losses.
Safety is Never Optional
Working with cobalt compounds, including cobalt acetate anhydrous, brings health risks. Cobalt dust can irritate the lungs and long-term exposure links to more serious issues. Lab safety procedures aren’t just red tape; they’ve kept many, including myself, out of the doctor’s office. Gloves, fume hoods, and proper storage keep workplaces safe and compliant. Companies that treat this lightly run into legal and ethical trouble fast.
Pushing for More Awareness and Training
One solution is more practical training focused on chemical identity, not just rote memorization of names. Chemistry textbooks and safety manuals should spell out the differences between anhydrous and hydrated salts — with real-world examples that stick. Companies and schools need regular refresher courses for all staff who handle these materials. Making the right tools and safety gear available, and making access easy, stops accidents before they start.
Looking Forward
The chemical formula, Co(C2H3O2)2, isn’t just a line on a label. It defines the identity and purpose of cobalt acetate anhydrous. Knowing and respecting the difference improves lab safety, saves time, and strengthens product quality across industries. Clear training and a sharp focus on chemical identity open the door to fewer mistakes, safer workplaces, and more reliable results.
Why Storage Conditions Matter
Cobalt acetate anhydrous works as a strong catalyst in industries like pigments, ceramics, and batteries. It gets the job done, but storage mistakes bring more risk than many realize. I've handled specialty chemicals for years and learned early that improper storage does more than shorten shelf life—it puts health and workspaces in jeopardy. This particular salt won’t forgive humidity or casual housekeeping. If moisture creeps in, you end up with a mess that can clump, degrade, or sometimes even react.
The Key Risks in Storage
Anyone who's opened a poorly stored drum of cobalt acetate finds clumps or a caked layer. Dry, tightly sealed environments prevent this problem. The anhydrous form grabs water straight from the air, so forget about open bags or loosely capped jars. Store it with a tight-fitting lid and always return what you take out—never leave it open for “just a minute.”
Shelf neighbors matter. Never park cobalt acetate near food, strong acids, oxidizers, or reducing agents, even for a day. One overlooked jar can turn a safe storeroom into a hazard if something leaks or spills. Incompatible chemicals in close quarters sometimes react, creating gas, heat, or corrosive goo. It’s a lesson learned quickly in any chemistry lab or factory floor.
Temperature and Light
This substance keeps best at room temperature, away from heaters, sunlight, or anywhere temperatures swing between extremes. Heat speeds up decomposition. UV rays, too, chip away at its structure over time. I’ve seen companies opt for storage closets inside their main building rather than an outdoor shed for this reason; these spaces let you control temperature and reduce the risk of sun exposure. Cold storage isn’t needed, but wild fluctuations bring nothing but trouble.
Moisture Control is Non-Negotiable
Desiccators, silica gel packs, or purpose-built dry cabinets work wonders. In high-humidity regions or during rainy seasons, a standard storeroom often isn’t enough. I’ve seen humidity climb during summer months, defeating even well-sealed jars unless extra measures get used. Monitoring tools that log temperature and humidity help spot trends before problems start. Physical checks—running a gloved hand over the container, shaking for clumps—add another layer of assurance.
Safety for Workers and the Environment
No one wants to breathe in cobalt dust. Designated storerooms that limit traffic, keep substances locked and labeled, reduce this risk. Safety datasheets, gloves, and proper signage go far and cost little. In the event of a spill, immediate clean-up with specialized equipment keeps the material and everyone safe.
Cobalt acetate isn’t a chemical to take lightly. Suppliers follow strict packaging, and once it arrives, storage practices determine how safe and effective it stays. I encourage updating storage policies yearly, double-checking shelving, and running practice drills for spills or exposure incidents. Each time a team refreshes its training, costly mistakes become less likely.
Simple Steps, Big Impact
Choose airtight containers. Keep storage cool, dry, and dark. Block off incompatible chemicals. Invest in humidity control tools if needed. Training and vigilance matter far more than fancy equipment. Over the years, I’ve seen these habits save product, protect people, and keep processes smooth. Small, everyday decisions shape safety and reliability far more than any single purchase or manual.
Understanding the Risks
Cobalt acetate anhydrous comes up in labs, battery production, pigments, and as a chemical intermediate. Nobody talks about cobalt compounds at family dinners, but the safety conversation matters. Cobalt acetate anhydrous raises legitimate concern due to toxic effects, supported by real case studies and workplace observations.
Living with Heavy Metals
A few years back, I toured a specialty chemical plant and watched workers handle cobalt materials with care. Gloves, masks, ventilation — not for show, but because cobalt compounds can cause skin or eye irritation, or lung problems when inhaled. Inhalation, actually, is the main route for workplace exposure. The dust floats, settles on surfaces and clothing, making it easy for anybody nearby to run into health problems. Cobalt compounds, including cobalt acetate, connect with asthma-like symptoms, chronic bronchitis, and even heart issues with repeated exposure.
Toxicity Isn’t Just a Lab Statistic
Cobalt as a metal supports some essential processes in the body — vitamin B12 for example depends on it. Still, inhaling or ingesting cobalt salts goes beyond any helpful dose. The European Chemicals Agency classifies cobalt acetate anhydrous as a carcinogen, citing evidence for increased cancer risk, especially with long-term exposure. Animal studies echo these findings, flagging risks for the liver, kidneys, and thyroid.
The International Agency for Research on Cancer places cobalt compounds in a group signaling possible cancer risk to humans. Workers and researchers who touch or inhale dust see this risk become personal.
What Safety Looks Like in Practice
Good ventilation stands as a frontline defense. During my visit, the safest labs had local exhaust hoods running constantly. Respirators weren’t negotiable for job tasks with any open powder. The standard safety goggles and nitrile gloves do not just collect dust — they block contact, and supervisors make sure nobody skips protocol.
Storage matters. Cobalt acetate anhydrous demands sealed containers and secure chemical cabinets marked with clear hazard signs. Spills require careful cleanup, with designated gear and trained staff. These simple practices cut down the risk for anyone on-site.
The Bigger Picture: Solutions for Safer Handling
Routine air monitoring and biological sampling offer more than paperwork. Regular checks allow teams to catch toxic exposure before symptoms emerge. Substitution might sound easy on paper, but finding alternatives for cobalt-based catalysts or dyes takes time and money. In some places, companies slowly switch to less toxic ingredients or shift processes so workers stay separated from open powders.
Education makes the most difference. Incoming workers at chemical facilities soak up hours of training, not just to pass audits but to stay safe for the long haul. In my experience, open discussions about health effects and warning signs bring the dangers out of the manual and into the real world. Every case of accidental exposure is one too many.
Facing the Future
More research brings clarity, but the body of evidence already signals that cobalt acetate anhydrous needs careful handling. Strict exposure limits and ongoing training support the best outcomes. For those in science, industry, or regulatory agencies, putting safety before productivity isn’t just smart — it saves lives.
Understanding What Purity Means Here
Stepping into a lab or glancing at a spec sheet, purity almost jumps off the page. It’s not a buzzword. Purity for something like cobalt acetate anhydrous controls how well your process runs, how safe it is, how pure your final product turns out, and how much trust you can put in the numbers printed on a container.
A look at any reputable chemical supplier shows most cobalt acetate anhydrous hovers at a minimum purity of 98%. That number matters because the trace metals, water content, and other not-so-friendly extras can change chemistry down the line.
Sulphate, chloride, iron, and copper level limits often squeeze under 0.01%, sometimes even less for pharmaceutical or battery-grade materials. Water—the silent saboteur—gets held below 0.5% for true “anhydrous” quality. These aren’t just pretty numbers for a catalog. Engineering teams, battery manufacturers, dye formulators, and researchers all rely on these details.
What Drives Purity Demands?
I learned early that chemical purity isn’t academic. At a factory mixing up catalytic solutions, trace nickel in cobalt acetate threw off results. Coupling that lesson with what I’ve seen in labs, a few tenths of a percent can spoil an entire batch or give wrong readings. In energy storage, those “other” metals spark unwanted reactions or bring down battery performance.
The wrong impurity stings extra hard in pharma work or catalyst prep. Sometimes, a batch starts off looking clear and perfect, only for low-level sodium or zinc to wreck the process halfway through. Pure cobalt acetate anhydrous doesn’t just boost consistency. It opens the door for tight process control and fewer surprises.
Testing Backed by Facts
As someone trained to spot shortcuts, I don’t just take purity numbers at face value. Top suppliers hand over certs of analysis that detail each lot. Independent verification—running samples through ICP-OES for metals, thermogravimetrics for water content, plus a close eye on insoluble residues—pulls the curtain back. The most trustworthy labs follow standards like ACS, ISO, or similar benchmarks, reporting findings to the third decimal place.
Sometimes a producer goes beyond. For battery-grade or analytical work, purity stretches up toward 99.5% or even higher, with total heavy metals below one part per million. It takes better inputs, tighter controls, and more transparent documentation.
Fixing Gaps in Purity and Knowledge
Most problems with chemical purity start with cut corners or weak supply chain oversight. Asking for trace impurity analysis is non-negotiable, holding suppliers to clear, published limits. End-users who test incoming batches lower their risk of bad surprises. Simple steps, like storing tightly sealed containers or opening only what’s needed, guard against moisture sneaking in.
Education, honest communication, and pushing suppliers to stick to published standards give everyone more confidence. If standards lag behind real-world application needs, industry groups and buyers can push for stricter specs and broader testing.
Relying on trusted research, pushing for consistent quality, and learning from lab mistakes move the whole field forward. A few decimal points in purity aren’t just math—they’re the difference between a project’s success and another round of troubleshooting.
| Names | |
| Preferred IUPAC name | Dicoobalt diacetate |
| Other names |
Acetic acid cobalt(II) salt anhydrous
Cobalt(II) acetate anhydrous Cobalt diacetate Cobaltous acetate anhydrous Anhydrous cobalt acetate |
| Pronunciation | /ˈkoʊ.bælt ˈæs.ɪ.teɪt ænˈhaɪ.drəs/ |
| Identifiers | |
| CAS Number | 6147-53-1 |
| Beilstein Reference | 1698736 |
| ChEBI | CHEBI:91248 |
| ChEMBL | CHEMBL1201794 |
| ChemSpider | 11423 |
| DrugBank | DB14537 |
| ECHA InfoCard | 100.011.798 |
| EC Number | 209-170-2 |
| Gmelin Reference | Gmelin Reference: 57407 |
| KEGG | C05572 |
| MeSH | D003055 |
| PubChem CID | 10159 |
| RTECS number | AG7325000 |
| UNII | UA6K4A6NLW |
| UN number | UN3283 |
| CompTox Dashboard (EPA) | DTXSID2034697 |
| Properties | |
| Chemical formula | C4H6CoO4 |
| Molar mass | 176.00 g/mol |
| Appearance | Pink to Red Crystalline Powder |
| Odor | Odorless |
| Density | 1.7 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -1.0 |
| Vapor pressure | 0.0677 mmHg (25°C) |
| Acidity (pKa) | 10.4 |
| Basicity (pKb) | 11.2 |
| Magnetic susceptibility (χ) | +3600×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.544 |
| Dipole moment | 4.74 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 155.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -751.9 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1808 kJ/mol |
| Pharmacology | |
| ATC code | V03AB56 |
| Hazards | |
| GHS labelling | GHS labelling: "Danger; H302, H317, H319, H334, H341, H350, H360, H372, H410; P201, P202, P273, P280, P302+P352, P305+P351+P338, P308+P313, P501; GHS07, GHS08, GHS09 |
| Pictograms | GHS07,GHS09 |
| Signal word | Danger |
| Hazard statements | H302+H332: Harmful if swallowed or if inhaled. H317: May cause an allergic skin reaction. H319: Causes serious eye irritation. H350: May cause cancer. H410: Very toxic to aquatic life with long lasting effects. |
| Precautionary statements | P261, P264, P270, P272, P273, P280, P302+P352, P304+P340, P308+P313, P314, P333+P313, P362+P364, P391, P405, P501 |
| Flash point | > 360 °C |
| Autoignition temperature | 485 °C |
| Lethal dose or concentration | LD50 oral rat 614 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 636 mg/kg |
| NIOSH | Not Listed |
| PEL (Permissible) | 0.1 mg/m3 |
| REL (Recommended) | ENVREL |
| IDLH (Immediate danger) | 250 mg/m3 |
| Related compounds | |
| Related compounds |
Cobalt(II) acetate tetrahydrate
Cobalt(II) chloride Cobalt(II) nitrate Cobalt(II) sulfate Nickel acetate Iron(II) acetate |
