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Sodium hexanitrocobaltate(III) stretches back to the late 19th and early 20th centuries, landing in the public literature as part of a wave of coordination chemistry discoveries trailing Alfred Werner’s early findings about metal-ligand bonding. Researchers then looked to these strange, vivid compounds mostly for their vibrant colors and curious reactions with common ions. In college, I remember a dusty old jar tucked away on a shelf, its label worn, a quiet relic from when such compounds made big impressions in test-tube demonstrations. The true story is not about a single eureka moment, but a long simmer: over decades, this orange-yellow salt kept popping up as chemists chipped away at the rules that govern transition metal complexes. Its precise role evolved as our understanding of ligands, geometry, and oxidation states matured. Sodium hexanitrocobaltate(III) told us about how nitro groups can stabilize unusual valence states, and how delicate balancing acts control the reactivity of even the most “inert” cobalt centers.
Sodium hexanitrocobaltate(III) is less common than its cousins in the laboratory supply world. The salt usually appears as orange or yellowish crystals, eye-catching only to those of us who enjoy chemistry’s bolder shades. It never claimed popularity the way sodium ferrocyanide did, partly because of the tight leash required by its toxicity. This cobalt-based complex tends to turn up where careful precipitation reactions rule. Analytical chemists put it to use for spotting potassium ions in a sample—a far cry from swept-up industrial usage, but a niche that persists because it’s tough to beat for selectivity and contrast. The name doesn’t roll off the tongue, but it picks up quirky synonyms over the years: sodium hexanitritocobaltate(III), sodium cobaltinitrite, and even “Cobalt Yellow” in early pigment catalogs.
A pinch of sodium hexanitrocobaltate(III) in your palm looks unassuming, its orange tint hinting at the six stubborn nitro groups attached to the cobalt core. It dissolves well in water, but not in many organic solvents—a clear sign the sodium ions and polar nitrito ligands work overtime to keep everything together. Heat starts to break the compound down at around 70 to 80°C, which means storage requires a cool, dry place. Anyone who’s ever uncorked a bottle in a humid lab can attest to its tendency to clump, a reminder that hydration can sneak up on even the best-prepared. Chemically, it maintains a +3 oxidation state on cobalt, stabilized by the electron-hungry nitro groups. These donor atoms, arranged octahedrally, keep the complex tightly wound, resisting redox changes unless strong reducing agents come into play. Its sensitivity to light and temperatures makes for some anxious moments during longer experiments, as the color gradually fades with careless handling.
Regulation around labeling and transport of sodium hexanitrocobaltate(III) tightens each time new toxicological data comes out. Authorities now require explicit cobalt warnings on any commercial product. As cobalt compounds find scrutiny based on their environmental persistence and ability to trigger allergic reactions, labs face more pressure for accurate labeling and risk communication. Not only must the concentration of sodium and cobalt feature prominently, but disposal and storage directions also must be clear and specific. I have watched more than one university scramble to update their hazard communication plans, as once-quaint “use with care” margins grew into compliance checklists and digital inventory tracking. Too many accidents in the past came from assumptions, especially with complex cobalt salts. Proper labels and clear instructions now serve as insurance, not optional extras.
Synthesizing sodium hexanitrocobaltate(III) starts off with cobalt(II) nitrate or cobalt(II) salts dissolved in water. Nitric acid acts as both oxidizer and nitro group donor, and the process calls for controlled temperature and slow addition of sodium nitrite. The solution heats gently to encourage the formation of the desired cage-like structure. But patience is key: rushing the process muddies purity and yields. Filtration and careful washing with ice-cold water follow, because the product needs to be kept from decomposition or hydrolysis. Early chemists lacked the fine balances and grad students who once learned to prepare these compounds by hand sometimes spent days perfecting these details. Even modern automated syntheses struggle to scale cleanly, and you won’t find sodium hexanitrocobaltate(III) churned out by the ton. This is boutique synthesis as much as it is routine lab work.
Sodium hexanitrocobaltate(III) stands out thanks to its strong selective precipitation ability, especially with potassium ions. Drop by drop, it pulls potassium out of a mixed solution, creating a bright yellow insoluble salt—an old trick that still proves useful for confirming the presence of potassium in soils and medical samples. This selectivity doesn’t always carry over to other alkali metals, making the compound unique in its niche. Attempts to modify or chelate the structure with other ligands take finesse: push too hard with acids or bases, and the nitro groups start to come off, reducing the complex or tearing the structure apart. Researchers sometimes tweak the counterion, swapping sodium for lithium or ammonium to see what changes, but the heart of the chemistry comes back to the cobalt(III)-nitro bond. The structure tolerates a limited amount of substitution, but its stability hangs by a thread, rewarding careful eking out of variants with surprising shifts in color and solubility.
Dig through old texts, and you’ll find sodium hexanitrocobaltate(III) under an array of names—each one rooting it deeper in the history of coordination chemistry. “Sodium cobaltinitrite” appears in color theory books as a pigment additive. Analytical manuals favor “Cobalt Yellow,” which, tucked alongside Prussian Blue and Paris Green, once pointed to the earliest efforts at chemical staining and pigment manufacturing. Modern safety databases settle on sodium hexanitrocobaltate(III) for precision, while technical papers toggling between “hexanitrocobaltate(III)” and “sodium cobaltinitrite” create headaches for anyone searching the literature. Language here reflects both tradition and evolving scientific rigor, a reminder that chemicals live in both academic and industrial worlds. Each name marks a stage in our understanding, not just a label on a bottle.
Stories from old laboratory training sessions resonate when it comes to handling anything cobalt-based. We now know sodium hexanitrocobaltate(III) brings significant health risks: accidental ingestion or skin absorption can lead to systemic cobalt toxicity, with symptoms ranging from rashes to more severe organ damage. Inhalation of any dust draws immediate concern because nitro group byproducts and cobalt ions both exerting harmful effects. I recall training where instructors spent more time talking about glove use and fume hoods than about the chemistry itself—a clear shift from the old cavalier attitude. Disposal runs strictly under hazardous waste rules. Cobalt and nitrite ions accumulate in groundwater and disrupt ecosystems, requiring labs to deploy heavy-duty containment, meticulous tracking, and certified disposal companies. Teaching assistants and senior chemists reinforce protocols for working in small batches, minimizing exposure, and treating contaminated surfaces as high-risk zones. These changes reflect hard-learned lessons from past carelessness.
Analytical chemistry clings to sodium hexanitrocobaltate(III) for the reasons that once made it a staple in classic labs—the pinpoint selectivity for potassium. Soil analysis, forensic testing, and quality control in fertilizers all turn to the compound for quick, reliable colorimetric identification, especially when more expensive or delicate techniques aren’t practical. Medical technicians benefit from this shortcut when spot-checking potassium levels, saving money and time. The pigment industry once dabbled with the compound for its striking yellow color, though safety and light sensitivity now keep it out of mainstream coloring products. Experimental electrochemistry dabbles with redox-active cobalt centers, though the instability and toxicity of the salt limit widespread use. These application areas rarely generate headlines, but the compound’s footprint remains, quietly supporting legacy testing despite new technologies trying to push it out.
Researchers now focus on two main areas: improving the safety and environmental impact of sodium hexanitrocobaltate(III), and tweaking its performance for analytical work. Studies highlight how modifying the ligand environment might offer better selectivity or stabilize the cobalt center without trading off toxicity. Green chemistry approaches seek new routes to bring down energy use and solvent waste, while computational models try to predict new analogs that might shed some of the older compound’s dangers. I have seen how these projects pull in teams from different fields—synthetic chemistry, environmental science, even economics—all aiming to turn a boutique reagent into something less hazardous and more sustainable. While big breakthroughs remain rare, the steady accumulation of knowledge keeps options open for transforming this once-niche reagent into a safer, future-proofed tool.
Toxicity studies of sodium hexanitrocobaltate(III) don’t make for easy reading. Cobalt’s reputation for causing allergic reactions and chronic exposure issues drives many of the restrictions now in place. Acute poisoning leads to nausea, vomiting, and longer-term organ toxicity. The nitro ligands increase solubility, but release harmful byproducts if the complex falls apart in the environment or within living systems. Animal studies point to cumulative effects, especially when water sources pick up runoffs laced with cobalt compounds from industrial and academic waste. Regulators track not just human toxicity, but the compound’s environmental legacy—how it can linger or transform into other forms that disrupt aquatic life. These findings put significant constraints on routine use and call out for alternatives that retain the selectivity but shed the cobalt anchor. As safety data accumulates, calls for stricter limits and more transparent hazard labeling grow.
Sodium hexanitrocobaltate(III) stands at a crossroads, a relic from the founding days of coordination chemistry that still finds work in specialized analytical labs. On one side, legacy applications and unique selectivity keep it viable for potassium detection, especially in environments where other reagents fail. On the other side, ongoing toxicity concerns and regulatory shifts mean each new study inches the compound further from widespread use. Solutions could emerge from new ligand designs or by reengineering the cobalt center—approaches that integrate lessons from both green chemistry and toxicology. Funding continues for safer, more sustainable alternatives, but real breakthroughs will need collaboration across synthetic, analytical, and environmental specialties. The compound’s story offers a snapshot of how chemical innovation, practical needs, and health impacts intertwine. Those of us who spent endless hours in the lab with these vivid yellow crystals see both nostalgia and a challenge: how to preserve legacy knowledge while facing up to a future that demands safer, smarter choices.
People working in chemistry, analytical labs, or water treatment plants probably recognize the bright yellow crystals of sodium hexanitrocobaltate(III). The name sounds complex, but this compound has a specific job—one that relates closely to keeping things clean and safe. Most folks never see sodium hexanitrocobaltate(III) on a shelf at home, yet its fingerprint can be found in some key processes.
Most professionals run into sodium hexanitrocobaltate(III) during tests for potassium. Potassium keeps both plants and people healthy, so tracking its presence in soil, food, or biological samples really matters. Here’s the science: add sodium hexanitrocobaltate(III) to a solution suspected of containing potassium, and a bright yellow precipitate forms. This reaction signals potassium’s presence. Plant nurseries rely on it, medical labs rely on it, and agriculture scientists check soil health with it.
For example, a soil test in a small farm can make the difference between a strong or weak harvest. If potassium drops too low, yields slump. By using chemicals like sodium hexanitrocobaltate(III), farmers know exactly when and how to enrich their fields. That might sound technical, but the decisions start right here, with a rigorous potassium test. For folks working in labs, reliable potassium detection means catching health problems early—from muscle weakness to heart issues, potassium imbalance impacts people every day.
Walk into a water treatment plant and you’ll see stacks of pipes, meters, and tanks. Industrial water often contains harmful metals, and some of them, like potassium or cesium, need to be monitored closely. Sodium hexanitrocobaltate(III) allows engineers to detect potassium ions quickly without elaborate equipment. That means safer water for neighborhoods and factories.
Engineers have struggled with trace contamination in recycled water. With sodium hexanitrocobaltate(III), simple chemical tests catch rising potassium levels fast. It helps save time and money since more expensive technology isn’t needed at every stage. This compound plays a direct role in keeping big cities’ water safe and usable.
There’s a flip side here: cobalt and nitrates bring some worries for health and the environment. Long-term exposure to cobalt can pose risks. Nitrates can add to water pollution. So, labs using sodium hexanitrocobaltate(III) handle it carefully and dispose of leftover material by following strict rules. Responsible use stands at the center of all modern chemistry. If local agencies lack training or funds to handle such chemicals, mistakes happen, affecting workers or ecosystems.
Safer alternatives stand as a long-term goal for many chemical labs. Researchers keep searching for non-toxic reagents that match sodium hexanitrocobaltate(III) in reliability, but so far, nothing has knocked it off the shelf. Training lab staff on best practices and improving chemical waste management helps reduce risks right now.
Talking to environmental health officers about these risks opens up better support to smaller labs, especially those in developing regions. They need clear guidance and access to safe disposal systems. This compound plays a behind-the-scenes role in many systems that keep people healthy, crops growing, and water safe, so treating it with respect and care pays off for everyone.
Sodium hexanitrocobaltate(III) always drew attention in my chemistry classes because of its vivid yellow color and the complex arrangement of its atoms. The chemical formula—Na3[Co(NO2)6]—brings together sodium, cobalt, and nitrite groups into a single molecule, presenting a good example of coordination chemistry in action.
Beyond the string of letters and numbers, this formula represents a story about molecular architecture and the creativity of chemists. The three sodium ions balance out the charge on a bulky, negatively charged cobalt complex. The central cobalt atom holds onto six nitrite ions, creating an intricate octahedral structure. This isn’t just a trivia detail—it changes how the compound behaves in the real world. The arrangement of those nitrite groups makes the compound stable under typical lab conditions but sensitive in larger-scale processes or in contact with strong acids.
Mentioning sodium hexanitrocobaltate(III) usually raises eyebrows unless you’ve spent time in a chemistry lab. In practice, it’s far from obscure. The precision of its formula means chemists count on predictable reactions. For example, this compound plays an important role in testing for potassium ions. A drop of it in a solution can quickly reveal potassium’s presence by forming a characteristic precipitate. In my college years, this test made an impression—watching a clear liquid cloud up thanks to one neat chemical trick.
Complex compounds like this also offer lessons in safety. Sodium nitrite, one of the building blocks, poses health hazards if handled carelessly. Cobalt compounds add their own risks, from skin irritation to environmental concerns. Everyone in the lab, myself included, got a quick lesson in cautious technique and safe disposal. This heightened respect for chemicals follows me long after the class ends. Responsible practices never lose their relevance.
Outside the classroom, the systematic study of sodium hexanitrocobaltate(III) dates back over a century. Chemists have mapped its crystal structure countless times, confirming exactly how those atoms connect. According to the International Union of Pure and Applied Chemistry (IUPAC), the standardized formula ensures chemists in every part of the world can replicate results and compare data accurately. Recent journal articles still refer to this precise notation, showing the impact of agreed-upon language in science.
Working with such compounds requires more than knowledge of formulas. Institutions could put stronger emphasis on training students and early-career lab techs in safety and environmental stewardship. Substituting less hazardous materials, whenever possible, protects people and keeps labs sustainable. In some cases, digital simulations are beginning to stand in for physical experiments with risky substances. Using technology to avoid unnecessary exposure promises a safer future for both researchers and the environment.
Every bottle on a chemical shelf tells a story—Na3[Co(NO2)6] tells one about curiosity, risk, and the power of precise notation. For anyone handling it, care and respect matter as much as knowledge of the formula itself.
Anyone who’s handled specialty chemicals in a lab runs into tongue-twisting names. Sodium hexanitrocobaltate(III) fits right in, sounding exotic but raising real questions about its safety. I've spent years in university research labs and understand the tension between curiosity and caution. You can’t judge a chemical just by the way it sounds, but you can dig into what researchers and safety data sheets say—and it turns out, this one deserves respect.
Cobalt plays a key role in sodium hexanitrocobaltate(III), and cobalt compounds have a history in toxicology studies. Inhaling small particles of cobalt salts can cause respiratory problems. Being around cobalt compounds for long periods has even triggered allergic reactions like rashes and asthma attacks. The European Chemicals Agency lists cobalt as a substance of high concern because of its suspected cancer risks. Contact with cobalt-containing dust or solutions puts workers and students at risk if proper gear is skipped. Skin contact, inhalation, and accidental swallowing each open different doors to trouble.
This compound contains not just cobalt but a load of nitro groups. Chemists know these groups add danger. Under the right conditions, nitro compounds have triggered explosions and acute toxicity. In sodium hexanitrocobaltate(III), the nitro groups can react if the chemical is mixed with strong acids or reducing agents. The released gases don’t win any awards for safety, either: nitrogen oxides irritate the lungs, and at high levels, they can even kill.
Labs aren’t the only places that worry about sodium hexanitrocobaltate(III). Simple spills in waste streams could release cobalt into groundwater. This toxic metal doesn’t disappear—it builds up, harming aquatic plants, fish, and eventually the people or animals that depend on these sources. Once, I saw a wastewater report showing how trace cobalt measured up in river samples near an industrial facility. The report made it obvious: the more these substances get used, the bigger the cleanup tab in the long run. Real-world data confirms what theory hints at—these contaminants don’t just fade away.
During graduate school, I watched peers get complacent about lab protocols. No gloves? No goggles? It never ends well. Sodium hexanitrocobaltate(III) requires nitrile gloves, a lab coat, and safety goggles every time. Fume hoods stand between your lungs and an accidental chemical cloud. Safety data sheets from suppliers like Sigma-Aldrich recommend running any procedure with this chemical behind a protective barrier. Pressed for time? The minute you skip these steps, you create room for disaster.
In my experience, training matters just as much as labeling jars with the correct chemical name. Before opening a single bottle, people should know emergency procedures, disposal rules, and the possible health effects. Labs and factories can swap out sodium hexanitrocobaltate(III) for less harmful alternatives, cutting down on hazardous waste. Real progress comes from upstream design. Green chemistry pushes scientists to ask whether they need risky compounds at all. Some newer research projects already sidestep hazardous transition metal salts, using catalysts or reagents with a lower health burden on workers and the environment.
Chemicals like sodium hexanitrocobaltate(III) pack risks that go far past the basic recipe. With proper precautions, good training, and a push for safer substitutes, researchers and industry workers can keep curiosity alive without betting their health or the planet.
Sodium hexanitrocobaltate(III) isn’t something you want to leave out on a shelf with the cleaning products. This compound contains cobalt and is packed with nitro groups, making it a strong oxidizer. Sitting near combustible materials or under sunlight, it can provoke a reaction you don’t want. In my own work handling oxidizers, I’ve seen how a lack of respect for storage rules can end in lost research, damaged equipment, and in the worst case, injuries. For chemists and lab techs, basic procedures keep both people and property safe.
Don’t count on a costly safety cabinet to do the heavy lifting. The real keys: temperature, humidity, and isolation. This chemical prefers a cool space—room temperature, away from any heat source. Humidity control plays a big role. Dampness can degrade the compound, making it unpredictable. Silica gel packs or an automatic dehumidifier bring big peace of mind in changeable climates. Forgetting this step shortens chemical shelf-life and clogs up experiments with unreliable materials.
I’ve always relied on glass containers with airtight seals for this kind of substance. Screw tops work, but glass stoppers do better over the long haul because they don’t flex. Avoid plastic unless it has a strong chemical compatibility rating, since nitro compounds sometimes stain or even weaken certain plastics. A clear label on every jar matters, too. Use the date, compound name, and a bold warning sign about the contents. Lab guests or new techs need to know at a glance they shouldn’t open it without a supervisor.
Too many accidents happen by mixing the wrong chemicals in shared storage spaces. Always keep sodium hexanitrocobaltate(III) away from organics, acids, and all sorts of reducers. I keep a special shelf for oxidizers, locked if possible. It doesn’t have to be complicated—just a sturdy metal cabinet with a clear label for authorized use. In busy labs, tracking who opens that door has saved more headaches than I can count. Even a clipboard log helps when regulators come knocking or when something goes missing.
This chemical can’t hit the regular trash pile. In my experience, following up with local hazardous waste teams keeps everyone out of trouble. I keep neutralizing agents and spill kits nearby, right next to the cabinet. In the event of a leak or break, even after hours, quick response keeps small hiccups from spiraling. A posted spill response sheet—and regular drills—prepare new hires and keep old hands sharp. Focusing on chemical safety isn’t just red tape. It’s the reason everyone gets to go home at night, and it helps labs avoid fines and lost time from mistakes that are easy to prevent with a bit of preparation.
In my years working with tricky materials, the best approach sticks to basics: keep chemicals cool, dry, separated, secure, and properly labeled. Cutting corners on any step means chasing trouble down the line. Buying the right containers, organizing the space, and making safety checks routine pays off in fewer close calls and higher confidence every day you come in to work.
Sodium Hexanitrocobaltate(III) doesn’t turn up in daily conversation unless you work in a lab, handle analytical reagents, or dive into complex chemical syntheses. I’ve seen more than a few colleagues get a bit too relaxed just because a jar looks like every other salt on the shelf. That’s a mistake. Its deep yellow crystals pack more risk than their appearance suggests, and getting those safety basics wrong can mean real trouble for your health, your team, or your lab’s reputation.
From my own time working with this compound, personal protective equipment is non-negotiable. Gloves, splash-proof goggles, and a well-fitted lab coat form the front line. Skip any piece, and that’s where accidents punch through. Sodium Hexanitrocobaltate(III) can irritate eyes, skin, and—if inhaled—your lungs. The cobalt part brings its own baggage: repeated or high exposure may affect your respiratory system or trigger allergies.
Hygiene rules get overlooked, especially on busy days. It’s easy to forget that this isn’t the sort of substance to have lingering on your hands at lunch. Eating or drinking near your workspace gives you a shortcut for contamination. Dedicated washing stations matter here; a careless bite or sip can tell a tale your body won’t thank you for.
I used to cut corners in a shared lab when rushing, thinking a small weighing job wouldn’t matter. A stuffy room and dry powder make an easy path for inhaling tiny crystals. Sodium Hexanitrocobaltate(III) doesn't have much business being out in an open, unventilated area. Fume hoods clear the air—literally. They keep the dust away from your nose and lungs, keeping exposure down and stress low.
No one likes to admit to a spill, but the truth is, they happen. The best recovery doesn’t start with panic—it starts with readiness. I learned to have an emergency protocol taped near workbenches. Spilled powder demands careful collection with damp materials and proper disposal—no sweeping, no blowing, no half-measures. Leaving traces behind might expose others long after you’ve left.
Disposal means knowing your local rules. Tossing compounds containing heavy metals like cobalt in regular trash breaks the law and puts people in harm’s way. Trained specialists or a hazardous waste service should take care of that waste. Even small volumes matter. It’s about doing your part for the next person, or for anyone downstream in a waste facility.
It’s easy to stash eyewash bottles and emergency showers in a corner and hope for the best. I’ve seen those moments when someone actually needs them. A slow response, a blocked path, or empty bottles all add up quickly into regret and real harm. Regular checks—meaning someone actually uses and refills them—take as much time as a coffee break but save eyesight or skin.
Labs only run as safely as the culture inside them. Those quick reminders, the silent help from a colleague who points out a missed glove or unsecured container, make all the difference. A routine walk-through or refresher training can be more helpful than another line in a safety manual. I’ve seen mistakes, and I’ve seen those moments where someone’s voice saved the day.
The facts stay the same: Respect for Sodium Hexanitrocobaltate(III) starts with real habits, not just checklists.| Names | |
| Preferred IUPAC name | sodium;hexanitratocobalt(3−) |
| Other names |
Hexanitrocobaltate(III) sodium salt Sodium cobaltinitrite Sodium hexanitritocobaltate(III) Sodium cobalt yellow |
| Pronunciation | /ˌsəʊdiəm ˌhɛksəˌnaɪtrəʊkəʊˈbɒl.teɪt/ |
| Identifiers | |
| CAS Number | 13600-98-1 |
| Beilstein Reference | 1858735 |
| ChEBI | CHEBI:78029 |
| ChEMBL | CHEMBL1201649 |
| ChemSpider | 20210204 |
| DrugBank | DB11241 |
| ECHA InfoCard | 03bc1407-61a6-40fe-8c63-bdf7c4a18a4e |
| EC Number | 232-142-2 |
| Gmelin Reference | 107083 |
| KEGG | C06814 |
| MeSH | D017164 |
| PubChem CID | 16211957 |
| RTECS number | GF9590000 |
| UNII | 8A7R9F3MGL |
| UN number | UN3319 |
| Properties | |
| Chemical formula | Na₃[Co(NO₂)₆] |
| Molar mass | 437.94 g/mol |
| Appearance | Dark brown crystals |
| Odor | Odorless |
| Density | 2.35 g/cm3 |
| Solubility in water | Slightly soluble |
| log P | -4.37 |
| Vapor pressure | Negligible |
| Basicity (pKb) | 16.2 |
| Magnetic susceptibility (χ) | -0.73 x 10⁻⁶ |
| Refractive index (nD) | 1.590 |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 435.8 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -537.8 kJ/mol |
| Hazards | |
| Main hazards | Oxidizer, harmful if swallowed, causes skin and eye irritation, may cause allergic skin reaction, toxic to aquatic life |
| GHS labelling | GHS05, GHS06, GHS09 |
| Pictograms | GHS07,GHS09 |
| Signal word | Danger |
| Hazard statements | H272, H301, H311, H331, H334, H373, H410 |
| Precautionary statements | Precautionary statements: P260, P273, P280, P301+P312, P302+P352, P305+P351+P338, P308+P313 |
| NFPA 704 (fire diamond) | 2-0-2-OX |
| Lethal dose or concentration | Lethal dose or concentration: LD50 (oral, rat) > 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): >2000 mg/kg (oral, rat) |
| NIOSH | Not listed |
| PEL (Permissible) | PEL: 0.1 mg/m³ |
| REL (Recommended) | 0.1 mg Co/m³ |
| IDLH (Immediate danger) | IDLH: Not listed |
| Related compounds | |
| Related compounds |
Cobalt(III) fluoride Potassium hexanitritocobaltate(III) Cobalt(III) oxide |
