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Nickel salts have always mattered to both industry and science. My first real look at Nickel(II) acetate tetrahydrate, that crisp blue-green powder, came back in my undergraduate days when we tried to use it in organic synthesis labs. Nickel made its debut in the late 18th century, after an era when pure metals meant coinage and little else. By the 19th century, chemists developed ways to react acetic acid with nickel carbonate, finding the tetrahydrate form unexpectedly handy because of its easy handling and storage. Today, the compound’s consistent performance offers an anchor when other reagents shift and drift. Despite technological leaps in materials, this salt still earns its keep in many corners of both academia and manufacturing.
Nickel(II) acetate tetrahydrate brings more depth to a chemist's toolkit than its unremarkable name might suggest. It typically appears as light green, almost aquamarine crystals that dissolve easily in water, making it especially attractive in plating baths and for catalysts. A close look reveals it as a transition metal salt that swaps ligands and bridges gaps between organic and inorganic processes. The tetrahydrate version—four water molecules firmly attached—offers reliable solubility and better shelf-life, which matters during extended storage or careful batch processing. Its role in the production of specialty ceramics, catalysts, and dyes places it at the intersection of chemical curiosity and industrial workhorse.
Nickel(II) acetate tetrahydrate makes its presence clear with a soft blue-green color, a gentle yet unmistakable sign of hydrated nickel ions. In solid form, it holds onto its water tightly, only letting go above 120°C—a trait students quickly learn after a failed attempt at “dry” samples. In solution, its dissociation is complete, with one nickel ion teaming up with two acetate anions. The molecule signals its identity with a melting point near 250°C and clear solubility in water and alcohols—both useful in many reaction schemes and industrial baths. The compound’s mild odor, reminiscent of vinegar, hints at its acetic backbone, indicating the presence of the carboxylate group. This acetate bridge links to nickel’s d-electrons, which offer catalytic potential or serve as a precursor for more complex organonickel compounds. At the bench, its chemical stability and ease of weighing mean less time troubleshooting and more time experimenting.
Chemistry relies on clear labels and known standards. Nickel(II) acetate tetrahydrate generally features a formula of Ni(CH3COO)2·4H2O and a molar mass just over 248 grams per mole. Purity benchmarks head north of 98 percent for most laboratory uses; high-end electronics work even demands 99.5 percent or more. Real-world batches often carry trace impurities like chloride or sulfate, but reliable vendors document those limits, letting researchers calibrate results and factories keep plating baths consistent. Safety labels warn of contact hazards, pointing to the potential for skin and respiratory sensitivity—a concern in both science classrooms and large-scale plants. These precautions aren’t just bureaucratic: the links between chronic nickel exposure and allergic or respiratory effects have shown up too often to ignore. Tight labeling and handling standards grew out of hard experience—nobody looks forward to a recall or accident report, and those sampling “just a little for testing” without gloves tend to learn lessons the tough way.
Manufacturing nickel(II) acetate tetrahydrate isn’t rocket science, but sloppy work seldom leads to good product. Most producers start by reacting nickel carbonate or nickel hydroxide with glacial acetic acid under precise heat and agitation. Once the reaction runs its course, careful crystallization produces fine green-blue crystals, each loaded with exactly four water molecules. The key challenge comes down to impurities—rushing the process traps unwanted ions or dried out solids, undermining purity later on. Some plants tweak the solvent system, adjusting temperature or stirring until the crystals reach ideal size and shape for either laboratory bottles or industrial bins. Filtering at precisely the right moment, followed by air drying at modest temperatures, ensures the compound doesn’t lose hydrate water or absorb environmental carbonates. Over the years, improvements in control systems and batch reactors have cut waste, improved yields, and made the compound available at scale for industries ranging from electronics to catalysts.
Every lab or process needs a reliable nickel source, and nickel(II) acetate tetrahydrate plays the part well. Dissolved in water or alcohol, it readies itself for redox reactions as a source of the Ni2+ ion. Once in solution, it jumps into ligand exchange with amines, phosphines, or other organic molecules, driving forward complex syntheses. I've watched its gentle reactivity shave minutes off reaction times for coupling reactions, and it has served as a shortcut for producing nickel oxides and hydroxides when heated or treated with strong bases. For catalysis, this salt often acts as the beginning, not the end—like when forming nickel nanoparticles for hydrogenation or electrocatalysis. Acetate ions linger, sometimes stabilizing particles, sometimes stepping aside as more stubborn ligands elbow in. A seasoned chemist sees its flexibility as a bonus, knowing a diverse set of transformations and surface modifications all trace back to this reliable green salt.
Chemistry’s old language has a way of giving the same thing many faces. Nickel(II) acetate tetrahydrate shows up on shelves under several aliases. Those in a rush call it just nickel acetate. Dig a little deeper and you’ll spot names like nickel diacetate tetrahydrate, nickelous acetate tetrahydrate, or its IUPAC form: nickel(2+) acetate tetrahydrate. Manufacturers’ catalogs rarely stick with just one label, often listing CAS numbers (6018-89-9) to settle potential confusion. This web of synonyms trips up newcomers but veterans keep a close watch—no one likes discovering a reagent was the wrong hydrate or the wrong basicity halfway through a complex project.
For all its usefulness, nickel(II) acetate tetrahydrate carries real risks. Skin and eye exposure can cause rashes or worse. Breathing dust—especially in places with poor ventilation—leads to long-term trouble, with the documented link between nickel exposures and cancers or respiratory issues too great to ignore. Hardware manufacturers and research labs install exhaust hoods, eye-wash stations, and strict glove policies for good reason. Storage in tightly sealed, non-reactive containers keeps humidity from fiddling with hydrate content and staves off accidental contamination. Disposal demands attention too: direct discharge into the environment isn’t just bad form, it triggers fines and ethical headaches. In practice, containers get clearly marked, procedures get drilled, and, at the smart workplaces, routine health checks are part of the safety culture. More regulations are sure to follow, but the best defense is always a workforce that treats chemicals with the gravity they deserve.
Ask a chemical engineer, and the word “plating” will come up quickly. Nickel(II) acetate tetrahydrate lands in the core of many nickel electroplating baths, coating everything from microchips to jewelry thanks to its clean, even deposit. Ceramics get a boost in color and performance when the acetate salt delivers nickel in a controllable, soluble form. Lab researchers, meanwhile, lean on it for synthesizing specialty nickel catalysts and precursors for organometallic compounds, often choosing this source for ease of weighing and consistency across batches. In environmental research, its role shifts towards simulating nickel pollution or testing remedial strategies. Electronics and textile dyes both pull nickel acetate solutions into their processes to alter conductivity or tint—proof that old salts find new life in emerging industries. Much like copper and iron salts, nickel’s acetate keeps gaining ground not just thanks to its chemical properties, but its reliability in plant and lab alike.
Academic and commercial labs keep pushing the limits of what nickel(II) acetate tetrahydrate can do. The compound has earned its spot as a starting material for green catalysis—especially where mild, aqueous conditions beat heavy metals or toxic organics. I’ve watched research groups investigate new complexes, using this salt to seed nano-catalysts for hydrogen evolution or to stabilize unusual oxidation states for selective synthesis. Several studies have targeted the “one-pot” conversion of simple acetates into functionalized organic frameworks—nickel’s redox behavior and acetate’s lability add just the right touch of flexibility. Recent work in electrocatalytic water splitting points to nickel(II) acetate as a solid precursor for nanostructured films or porous electrodes. By tracing performance from basic salt all the way to applied device, scientists highlight just how much potential one simple compound can offer, sparking both new patents and plenty of papers.
Nickel exposure’s darker side stops this compound from becoming just another shelf staple. Toxicologists have flagged repeated contact with nickel salts—including the tetrahydrate acetate—as a significant health risk for workers and, sometimes, users of finished products. Chronic exposure links to skin allergies, asthma, and even cancer. Several animal models pinpoint the trouble at low concentrations, especially in airborne dust or dissolved aerosol forms. Case studies of industrial workers back up those findings, whether from surface plating baths or dusts in powder handling. Regulatory agencies keep updating exposure limits, pushing for lower and lower permissible levels. While the obvious solution involves robust personal protective gear and localized ventilation, real change comes with systemic monitoring—noting who works with the compound, for how long, and under what environmental conditions. Too many fields ignored nickel's risks for too long, but modern labs and smart managers have shifted their focus towards minimizing exposure at every step. Further research into chronic effects keeps inching guidelines tighter, forcing industries to confront the gap between past practices and present expectations.
The story of nickel(II) acetate tetrahydrate isn’t finished yet. Clean energy demands, sustainable catalysis, and electronic miniaturization all point to a growing appetite for nickel compounds that blend solubility with reliable reactivity. Emerging research into catalytic water splitting, bio-active materials, and low-temperature surface modification suggest this old salt still has plenty to offer. The big challenge will be balancing those technical advances with worker and environmental safety, especially as regulatory scrutiny sharpens. Transitioning towards closed-loop systems, improved waste handling, and ever-safer production will remain at the center of any industrial plan involving nickel. As science aims for greener, cleaner ways to make things, and as engineers try to squeeze more from less, compounds like nickel(II) acetate tetrahydrate will stay in the mix—sometimes as the starting point, sometimes as the solution itself.
Nickel(II) acetate tetrahydrate comes with the chemical formula Ni(CH3COO)2·4H2O. This formula tells more than just the raw elements in the compound. For anyone working in a lab, handling industrial chemistry, or even teaching high school science, recognizing this structure brings clarity. The nickel ion in the +2 oxidation state pairs with two acetate groups, and four water molecules attach themselves to make the tetrahydrate version.
Those four water molecules aren’t just hanging around for bragging rights. They change everything—shelf stability, reaction rates, solubility, and the results you see in the beaker. I remember my first trial using the anhydrous form and wondering why my crystal yield was off. It was the water changing the weight per mole. I messed up the math, and nothing lined up with the textbook. That lesson stuck with me and returns in every hands-on lesson I give to new lab techs.
Nickel(II) acetate tetrahydrate gets a lot of attention in electroplating, ceramics, and as a catalyst. Getting the formula exactly right matters for industries relying on consistency and predictability. Electroplating, for example, needs nickel ions that dissolve easily and predictably. Four water molecules make that happen, affecting both solubility and ion mobility. Skip the hydrate, and you’ll get uneven coating, wasted nickel, and products that junk out early. Those mistakes turn expensive quickly if you’re coating turbine blades or circuit boards.
Anyone handling this compound should focus on purity and proper sourcing. Science moves forward because people care about precision—adopting tools and protocols that make repeatable results. My trust in chemical suppliers comes only after checking their certificates of analysis and doing quick spot-tests. There’s no room for guesswork when handling something as crucial as a catalyst precursor or plating bath ingredient.
Nickel compounds have their safety issues, and this hydrate brings no exception. Always use gloves, lab coats, and protective goggles. Inhaling nickel dust or letting it touch skin leads to allergies and in some cases can spark more serious reactions. Safety Data Sheets (SDS) lay out the rules, and they matter as much as the formula itself, especially around students and new workers. Practices like double-checking storage—keeping containers dry, clearly labeled, and locked up—kind of become a ritual. These steps keep everyone healthy and let the project move forward.
Better education could clear up a lot of confusion around formulas like Ni(CH3COO)2·4H2O. If schools and training programs spend more time working through live examples and less time just memorizing facts, people spot these details faster. Even professionals can overlook hydrate distinctions in a rush, and that’s where mistakes and costly recalls creep in. More real-world problem-solving and transparent supplier chains could lower risks and boost both safety and value in end products.
Ask a chemist about Nickel(II) Acetate Tetrahydrate, and you might get a look that suggests you’re about to dive deep into lab talk. Yet, its impact stretches far beyond a shelf in a storeroom. Chemically, this compound pulls in water and forms a pale-green, easily dissolvable salt. While this might sound technical, what really matters is where this salt lands once it leaves the bottle.
Anyone who has handled tools, coins, or even a shiny doorknob has likely brushed fingers against a surface touched by nickel plating. Plating with nickel helps block corrosion, boost durability, and add reflective shine. Companies reach for nickel acetate solutions during the electroless plating process—a method that coats metals without the need for electric current. This chemical supplies the nickel ions, and it’s this reaction that lets an even coating settle onto a surface.
Artisans shaping and coloring glass lean on minerals to bring out beautiful hues. In glass factories, adding certain amounts of nickel acetate creates soft blue or green tints or controls unwanted yellow tones. It’s a balancing act—too much throws off the color, too little leaves glass looking dull. This sort of chemistry doesn’t make headlines, but it does shape the look of countless bottles, windows, and works of art.
Researchers view nickel(II) acetate as a reliable starting point for growing crystals or preparing other nickel compounds. You’ll spot glass bottles labeled with its name in many labs, especially those focused on materials science or catalysis. During earlier years working around chemistry benches, preparing catalyst samples meant reaching for this compound again and again—test tubes bubbling as new complexes formed.
Catalysts push chemical reactions along, helping industries make everything from plastics to fuels with less waste and less energy. Nickel compounds hold a strong spot in this area, and nickel(II) acetate often plays a role in preparing these catalysts. The acetate version dissolves without much fuss, letting scientists blend it into reactions with other metals or supports.
While solar panels and batteries can seem like futuristic tech, their heart relies on solid knowledge of materials science. Some nickel-based electrodes wouldn’t come together without a chemical like nickel(II) acetate. Manufacturers dissolve it and coat surfaces, creating the right conditions for energy storage and capture. Reports show that researchers exploring new battery designs keep turning back to nickel compounds for their stability and performance.
Good chemistry respects risks. Nickel(II) acetate, like many nickel salts, can irritate skin or eyes and poses bigger dangers with long exposure. Responsible handling includes gloves and well-ventilated spaces—I remember strict safety reminders in classrooms and workspaces. Regulatory agencies across the world keep a close eye on nickel compounds, setting exposure limits to protect workers and the environment.
Demand for refined materials keeps rising, especially as electronics and renewable energy expand. This means understanding the smart, safe handling of chemicals like nickel(II) acetate matters more each year. Creating efficient recycling processes and searching for greener alternatives will likely shape its story in labs and factories worldwide.
I’ve spent years working in labs and around manufacturing spaces. You find all kinds of chemicals. Nickel(II) acetate tetrahydrate doesn’t look very dangerous—pale-green crystals, almost neat looking. Still, stories do the rounds of unexpected hospital visits and chronic symptoms from folks who skipped the safety gloves just once. It’s not something to mess with, even if it seems routine in plating shops and research labs.
Research holds a mirror to what workers have known for ages: nickel compounds carry real risks. Inhalation and skin exposure bring most trouble. According to the International Agency for Research on Cancer (IARC), nickel compounds fall into the “carcinogenic to humans” category. That’s not just handshake agreements in dusty workshops. Long studies connect some nickel salts—like those in nickel(II) acetate—to higher cancer rates in lungs and sinuses, especially for people who process nickel for years. Even falling short of cancer, chronic symptoms creep up, like persistent skin rashes or breathing issues if somebody ignores safety advice long enough.
Acute poisoning can hit hard, too. Swallow some of this salt by accident and you risk stomach pain, nausea, and vomiting. There’s even a record of kidney and liver damage with heavy, repeated exposure. You might think a quick rinse will fix a splash on the skin but nickel allergy means something else. This salt triggers itchy blisters and rough red patches, not always easy to shrug off. Once someone picks up a nickel allergy, it tends to stick around for life.
I hear gripes about government safety rules, but reading a nickel(II) acetate label closely gives you a window into the real solution. OSHA, NIOSH, and their cousins in other countries set limits for airborne nickel dust for a reason. A little slip, a missed mask, or torn gloves can bring years of regret. No need for elaborate lessons—a good ventilation fan and nitrile gloves save you more trouble than skipping a few safety steps for speed.
Too often, someone skips the safety glasses thinking “it won’t happen to me.” The next day, their eyes are burning. Simple, direct safety measures stop the worst. It means gloves rated for chemicals, not just dishwashing rubber, lab coats, goggles built for splashes, and knowing where the nearest eyewash station hides. Even a low-budget setup can work if everyone keeps gear clean and shares responsibility. If you see someone cutting corners, speak up. That small moment might keep them out of clinic later.
There’s a slim chance nickel(II) acetate pops up on your kitchen shelf, but craft kits and metallurgy sets bought online sometimes sneak it in. The warning remains the same—secure storage, tough containers, nothing left within easy reach of kids. Disposing of spent nickel solutions in the drain means asking for trouble. Heavy metals linger in water and soil. Some communities face real nickel pollution in rivers and farmland from sloppy dumping. It always costs less to treat these chemicals as hazardous from the start, rather than clean up later.
Safety takes more than equipment. Training helps people recognize danger, spot leaks, and react fast without panicking. Regular reminders and open talk about experiences—close calls, weird rashes, unexplained coughs—push people to take safety seriously. Encouraging folks to flag outdated safety sheets or replace worn-out gloves protects everyone. If an employer won’t pay for gear, push back. Every person has the right to a safe workspace, and most companies don’t change unless someone demands it.
In the end, nickel(II) acetate tetrahydrate may look harmless, but evidence and personal stories point to a need for real respect. Safety gear, training, and strict storage turn the hazard into just another tool—not a health gamble.
Nickel(II) acetate tetrahydrate often arrives in chemistry labs as a pale green crystal, a hint at its role in plating, catalysts, and research. Not everyone works with it every day, but for anyone handling this compound, safety rides as priority number one. Nickel compounds show up on lists of substances with potential health risks, with some scientific studies tying long-term exposure to skin issues and, in worse cases, a risk of cancer.
The chemical formula tells part of the story: it holds four water molecules. That means it reacts to humidity more than dry powders. If left on a bench, it will soak up water from the air, clump, or spoil, leaving it much less reliable for use in precise experiments.
Solid, leakproof containers offer a first line of defense. I learned early to reach for plastic or glass jars with screw-tight lids. A clean, dry jar keeps air exchange low and seals out humidity. For folks new to chemistry, the urge to re-use jam jars or coffee tins might be strong, but these containers rarely block enough moisture or corrosion over time. I’ve seen metal lids corrode fast, especially near any salty or moist samples.
Labeling goes hand-in-hand with good containers. A clear chemical name, date received, any hazard symbols—this takes seconds and saves headaches later. Ignoring clear labeling can land a chemist in trouble if someone else picks up the jar without knowing the risks.
Low shelves, away from heat vents or windows, help avoid swings in temperature or sunlight. Direct sun can break chemical bonds or, in some cases, accelerate slow reactions. Humidity is an enemy—chemicals with water in their structure lose quality quickly if stored beside sinks, humidifiers, or inside old fridges with leaky seals.
Good labs install dedicated chemical storage cabinets. Painted or coated metal doors protect against corrosion, and some cabinets vent to direct any fume buildup safely outside. I’ve always believed in restricting access as well. Any chemical on a public shelf mixes risk with curiosity—labeling and locked storage limits this problem before it starts.
Anyone who’s worked through a sodium acetate spill knows clean-up routines matter. For nickel(II) acetate tetrahydrate, dry gloves, eye protection, and, if quantities climb above a gram or two, a dust mask offer solid defense. Spills call for damp paper towels, never dry sweeping, to keep dust from rising.
Disposing unused or broken-down material properly often gets skipped if storage is sloppy. Universities and companies train teams on waste handling for a reason. In any real-world setting, falling behind on chemical checks leads to containers growing crusty and labels fading, which turns a research space into a minefield for newcomers. Regular inventory checks and a common chart for all to see have kept my teams on track.
Nickel (II) acetate tetrahydrate works quietly behind the scenes in research and industry. Storing it well means more than just tidy shelves—it means protecting yourself, others, and the work itself from preventable harm. Building a habit of proper chemical stewardship has paid back with fewer accidents, higher reliability, and a lab culture of looking out for each other, every day.
Nickel(II) acetate tetrahydrate, with the formula Ni(CH3COO)2·4H2O, looks complicated at first glance. But its use in everyday chemistry labs, university classrooms, and industrial applications gives it practical value far beyond a textbook. Understanding its molecular weight means more than memorizing a number—it gives you the confidence to prepare solutions, calculate yields, and check purity quickly.
Let’s get hands-on. The molecular weight combines the atomic contributions from nickel, carbon, hydrogen, and oxygen. Arriving at the correct number isn’t just a routine calculation; accuracy here sets up good science for everything that follows. For many students and technicians, the formula acts as a roadmap:
Pile those together and you get a total molecular weight of about 248.86 g/mol. For anyone weighing out this compound, especially in a teaching lab, this number bridges the gap between theory and hands-on work. The hydration matters—a dry version adds error if you don’t account for water molecules. If you set up a lab experiment using nickel(II) acetate tetrahydrate and ignore these waters, results shift, and reports lose credibility. It’s a detail that experienced chemists catch right away, building habits that translate to fewer mistakes in the real world.
In plating or catalyst production, molecular weight controls how much nickel you’re actually delivering. Too little and coatings come out thin and patchy. Too much creates waste—and nobody likes throwing away expensive material. College labs typically use this compound to introduce students to gravimetric analysis. If students use the wrong weight, their calculations throw off, and it can erode confidence in results. This isn’t just a classroom problem. Factory processes depend on similar math to make sure chemical baths remain stable. Everyone—from seasoned engineers to new hires—relies on accurate numbers to keep things running.
Quality control teams use the molecular weight to double-check formulations. With regulations on heavy metals tightening every year, it’s not just an academic exercise. Nickel compounds require careful handling because of their toxicity and impact on health. Getting the dose wrong could trigger compliance issues and even lead to fines or unsafe products. Keeping an eye on the right formula, and rechecking that molecular weight, stops a simple math slip from spiraling into major setbacks.
In my own lab experience, neglecting the hydration part has tripped up more than a few undergrads. Rushing through prep, they grab a bottle, scoop out the powder, and discover later that they’ve got inconsistent results. I’ve seen entire lab sessions spent backtracking just to fix the miscalculation. Bringing awareness to these details during training helps establish strong habits. Small habits like taking a pause to verify the molecular weight—even for compounds you think you know—cut down mistakes, save time, and teach responsibility.
Industry benefits too. Scrupulous record-keeping and clear labeling alert coworkers to watch for the correct tetrahydrate form. Incorporating a simple double-check into supply chains easily avoids headaches later. Attention to these details builds trust in the lab and in finished products on the shelf, ensuring each step meets internal and regulatory standards.
| Names | |
| Preferred IUPAC name | tetraaquabis(acetato-κO)nickel(II) |
| Other names |
Nickel diacetate tetrahydrate Acetic acid, nickel(2+) salt, tetrahydrate Nickel(2+) acetate tetrahydrate Nickel acetate tetrahydrate |
| Pronunciation | /ˈnɪk.əl ˈtuː ˌæs.ɪ.teɪt ˌtɛt.rəˈhaɪ.dreɪt/ |
| Identifiers | |
| CAS Number | 6018-89-9 |
| Beilstein Reference | 14607 |
| ChEBI | CHEBI:62968 |
| ChEMBL | CHEMBL1230900 |
| ChemSpider | 158430 |
| DrugBank | DB14541 |
| ECHA InfoCard | 100.029.214 |
| EC Number | 208-601-1 |
| Gmelin Reference | 87817 |
| KEGG | C16268 |
| MeSH | D009537 |
| PubChem CID | 151799 |
| RTECS number | QR6400000 |
| UNII | X2O60URQJF |
| UN number | UN3077 |
| Properties | |
| Chemical formula | Ni(CH3COO)2·4H2O |
| Molar mass | 248.86 g/mol |
| Appearance | Blue-green crystals |
| Odor | Odorless |
| Density | 1.744 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -2.6 |
| Acidity (pKa) | 7.5 |
| Basicity (pKb) | 12.31 |
| Magnetic susceptibility (χ) | +2680e-6 |
| Refractive index (nD) | 1.422 |
| Viscosity | Viscous solid |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 286.7 J⋅mol⁻¹⋅K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1337.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1208 kJ/mol |
| Pharmacology | |
| ATC code | V03AB45 |
| Hazards | |
| Main hazards | May cause allergic skin reaction, causes serious eye irritation, may cause cancer, may cause damage to organs through prolonged or repeated exposure, toxic to aquatic life with long lasting effects |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS07 |
| Signal word | Danger |
| Hazard statements | H302, H317, H334, H350i, H360D, H373, H410 |
| Precautionary statements | P261, P273, P280, P302+P352, P304+P340, P305+P351+P338, P308+P313, P501 |
| NFPA 704 (fire diamond) | Health: 2, Flammability: 0, Instability: 0, Special: - |
| Explosive limits | Not explosive |
| Lethal dose or concentration | LD50 Oral - rat - 350 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 350 mg/kg |
| NIOSH | AT9300000 |
| PEL (Permissible) | 1 mg/m3 |
| REL (Recommended) | 0.015 mg Ni/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Nickel(II) acetate Nickel(II) chloride Nickel(II) sulfate hexahydrate Nickel(II) nitrate hexahydrate Nickel(II) carbonate basic Nickel(II) oxide Cobalt(II) acetate tetrahydrate Copper(II) acetate monohydrate |
