© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
People have worked with nickel compounds since the eighteenth century. Nitrato de Niquel II Hexahidratado appeared as industries moved away from basic nickel salts toward compounds that could dissolve cleanly and offer controllable reactions. Back in the early days, Swedish chemist Axel Cronstedt identified nickel as a distinct element, carving the way for further studies and a deeper understanding. Later, as electrochemistry advanced and demand for metal finishing grew, industries leaned heavily on nickel nitrate for its solubility and efficiency in plating baths and catalysts. This compound became a staple in technical laboratories, feeding scientific curiosity and industrial progress by bridging the gap between elemental nickel extraction and real-world applications in coating, ceramics, and electronics. There’s no denying that its availability and the reliable nature of its preparation made it a trusted reagent, especially in Europe’s chemical production boom throughout the nineteenth and twentieth centuries.
Nitrato de Niquel II Hexahidratado’s formula—Ni(NO3)2 · 6H2O—produces deep emerald-green crystals. In storage rooms and workshops, these crystals catch the eye but serve an important purpose beyond aesthetics. They dissolve well in water, making them ideal for anyone needing a kick of nickel ions in solution. From basic chemistry sets to research lines developing advanced nanomaterials, this salt steps up where others fall short. Whether folks are pursuing catalyst preparation, ceramics coloring, or battery research, this nickel nitrate often lands on their shelves. The ease of measurement and consistent release of nickel ions put it ahead of competing nickel salts for many applications.
This compound, in its pure state, forms translucent to dark green crystals. Its melting point sits around 56.7°C, and those working in the lab feel the solid rapidly start to lose water above room temperature, often leaving puddles if not sealed well. It shows remarkable solubility in water and many alcohols, making solution preparation almost foolproof. The compound’s density reaches near 2.05 g/cm3. Nitrato de Niquel II Hexahidratado remains oxidizing by nature, due to the nitrate groups, and releases nitrous fumes on heating or contact with certain reducing agents. This behavior not only requires proper ventilation during handling but also highlights the risk of unwanted chemical reactions around organic material.
Industrial and laboratory supplies of Nitrato de Niquel II Hexahidratado often list technical grades by minimum nickel content—frequently above 20% by weight. Purity standards require absence of impurities like copper, cobalt, or lead below specified ppm thresholds. On labeling, suppliers print not only the full chemical name but also the molecular formula and CAS number (13478-00-7). Labels must show hazard statements describing oxidizing power and toxicity, alongside globally standardized pictograms. For storage, manufacturers advise tightly sealed containers with clearly written manufacturing and expiry dates because this salt draws moisture. Legal regulations, especially in the EU and the US, enforce strict labeling rules due to its classification as a hazardous substance.
Industrial-scale production of Nitrato de Niquel II Hexahidratado typically involves dissolving nickel metal, oxide, or carbonate in nitric acid. Chemists initially dissolve pure nickel chips or powder in concentrated nitric acid, sometimes with gentle heat to start the vigorous effervescence. The solution cools down, and once saturated, green hexahydrate crystals appear upon controlled evaporation. For higher quality, some manufacturers recrystallize the salt to cut down on mixed-metal impurities, using distilled water and carefully controlled temperatures. On the bench, small amounts often pop up from similar methods—students and professionals alike learn quickly to keep the area well aired to avoid headaches from evolving nitrogen oxides.
This salt acts not only as a nickel source but as a reactive partner in many synthesis projects. Its oxidation makes it valuable in creating nickel oxides through controlled heating, important in solid state chemistry and electronic ceramics. Researchers sometimes treat it with strong bases, producing nickel hydroxide, a precursor in battery technology and catalyst manufacture. In organic chemistry, it plays a role as a Lewis acid, activating certain carbonyl compounds for further transformations. The hydrated form can convert to anhydrous salt by dehydration, but this demands careful temperature monitoring to prevent decomposition. Reactivity with reducing agents serves a dual function: both nickel metal recovery and laboratory demonstrations of redox reactions. In the world of coordination chemistry, this nickel salt opens doors to a range of nickel-ligand complexes—students and professionals often use it to illustrate vivid ligand-field color changes.
In the commercial realm, suppliers trade Nitrato de Niquel II Hexahidratado under several names, including Nickel(II) Nitrate Hexahydrate and Nickelous Nitrate Hexahydrate. Some catalogs refer to it as Nickelnitrat-6-Wasser in German-speaking markets or Nitrato de Níquel hexahidratado in Spain and Latin America. Trade names like NiNitrate 6H2O surface in specialty chemical distributors’ lists. Import/export documents cite it as UN2725 (oxidizing solid), highlighting transportation requirements.
Everybody who handles Nitrato de Niquel II Hexahidratado recognizes its risks. The compound can cause dermatitis or allergic reactions for those who become sensitized from repeated exposure. Its oxidizing properties demand that operators keep it away from combustibles and store it in dry, sealed environments. Proper personal protective equipment—gloves, goggles, and well-fitted masks—offer basic defense against dust and skin contact. Workplaces should rely on eye wash stations and good ventilation. Laws under the REACH regulation in Europe and OSHA in the United States set exposure limits and enforce training requirements. Containers require secure closure, and processes involving heating or decomposition must deploy gas capture or fume extraction. Spills or accidental releases must be managed with dry, inert materials and not directly into drains or soil to protect water sources.
Nitrato de Niquel II Hexahidratado supports a wide swath of industries and research projects. Electroplating shops use this salt for creating tough, corrosion-resistant nickel coatings on metal goods—from automotive parts to consumer electronics. Manufacturers of ceramics and pigments turn to this salt to impart green and blue hues or introduce functional properties in glazes and glass. Battery researchers depend on its high solubility for producing nickel hydroxide and oxide electrodes, which form the backbone of many rechargeable cells. Laboratory chemists draw on this compound for a wide spectrum of nickel coordination and catalysis research. Textile dye manufacturers, especially in the past, have turned to it as a mordant, although environmental regulations today clamp down on this usage. Water treatment researchers sometimes study its use as a feedstock for nickel-based catalysts that break down organic pollutants.
Advances in materials chemistry rely heavily on reliable sources of nickel ions, and Nitrato de Niquel II Hexahidratado fits the bill. In battery technology R&D, teams use it to grow uniform nickel oxyhydroxides and spinels for next-generation battery electrodes, as seen in advanced lithium-nickel systems. Catalyst researchers push boundaries by using this salt to build supported catalysts or unique nanoparticle morphologies, aiming to increase efficiency and cut costs for hydrogenation and environmental clean-up. Students in university labs often choose it as a teaching aid in inorganic synthesis, linking theoretical knowledge with hands-on practice. Some biotech research delves into its role in bio-inspired catalysts and metalloproteins, trying to tap nickel’s unique redox behaviors for enzymatic models. As nanotechnology carves new ground, nickel nitrate serves as a feeder material for growing nanostructured films and wires, pulling the research community toward more efficient, compact devices.
Public health experts pay close attention to compounds like Nitrato de Niquel II Hexahidratado. Chronic exposure to nickel compounds, including this one, increases risks for skin sensitization, respiratory issues, and even carcinogenicity in some cases. Animal studies and workplace health monitoring point to inhaled dust and direct skin contact as primary contributors to health effects. Epidemiological work shows that people with a history of nickel allergy develop rashes or dermatitis after extended low-level exposures. Modern toxicity research revolves around improving detection thresholds, creating better protective barriers, and finding less hazardous alternatives where possible. Environmental studies show that nickel ions, if leached into water sources, can harm aquatic life, pressing regulators to impose limits on discharge and waste disposal. Cutting-edge projects evaluate biological markers of exposure and develop protocols for rapid response in case of spills or overexposure incidents.
Looking forward, Nitrato de Niquel II Hexahidratado faces both pressure and promise. Battery advancements and the renewable energy movement drive up demand for nickel-based materials, putting this compound on the front lines of sustainable technology development. At the same time, ongoing toxicity concerns—and tightening regulations in Europe, North America, and East Asia—push researchers to explore safer alternatives or closed-loop recycling. Companies investing in green manufacturing aim to find ways to reclaim nickel from spent salts, cutting down on mining and improving responsible sourcing. New synthesis techniques, like flow chemistry or greener solvents, may reshape manufacturing, reducing both waste and human risk. On the academic side, Nitrato de Niquel II Hexahidratado keeps its appeal as a backbone reagent in chemical education and novel catalyst research. As the world’s appetite for high-performance materials and cleaner processes grows, nickel nitrate hexahydrate’s versatility and efficiency help keep it relevant—provided all parties keep safety, health, and environmental well-being squarely in view.
Nitrato de Niquel II hexahidratado often comes up in chemistry classrooms, but its impact spreads well beyond academia. Inside the small, pale green crystals lies a tool used in countless processes, each aiming to solve important problems in the real world.
Nickel plating touches just about every device in modern life. Electronics manufacturers rely on this compound for the nickel solution in electroplating baths. Batteries, wiring connectors, and small appliance parts get a thin, reliable nickel coating to boost resistance against corrosion and wear. As someone who has tinkered with home electronics, I can say firsthand: subpar plating shows up fast, with connectors turning dull or rusty, breaking circuits. Nitrato de Niquel II hexahidratado assembles a smooth layer of nickel, preserving performance in humid summers or damp basements alike.
Hardware shops stock nickel-plated tools that hold up through years of rugged use, and that surface starts with solutions containing this nickel salt. With the tech industry sharpening its focus on long-lasting, repairable products, the humble salt finds more work than ever before.
Large-scale chemical plants turn to nickel compounds as catalysts, driving reactions that would otherwise crawl along. The hydrated nitrate form offers a convenient way to add nickel into these recipes. In refining petroleum, making synthetic fuels, or building specialty plastics, catalysts sit at the core of processes that power transport and manufacturing. Factories value reproducibility and reliability, two things this compound can deliver. In R&D labs, switching metal salts in a test reaction can make the difference between a breakthrough and a dead end.
Years of lab work taught me that the right chemical—picked for its simplicity and purity—can calm headaches before they start. Many synthesis routes call for a nickel source that dissolves easily and doesn’t bring along unwanted contaminants. Nitrato de Niquel II hexahidratado fits the bill. Its high solubility in water shortens prep time. Researchers developing new battery chemistries or cobalt-free superalloys often use this salt for early-stage experiments, enabling quick adjustments to get the best mix for strength and stability.
Wastewater coming from plating shops or refineries collects more than just oils and grime. It grabs unwanted metal ions, including nickel. Treating this water safely requires knowing the exact form and solubility of those ions. Operators handling Nitrato de Niquel II hexahidratado keep close records and use strict storage rules to avoid accidental nickel leaks. Recycling nickel from wastewater or spent solutions reduces demand for new mining, a practical step toward sustainability. My own brushes with small-scale plating taught me how even trace nickel can stress rural wells and fish ponds, so stricter controls matter.
Nickel compounds, including this one, raise flags for skin sensitivity and respiratory risks. Workers in plating plants, labs, and waste treatment must wear gloves and goggles, even for routine tasks. Regulations keep exposure in check. Safe handling improves not just productivity but the wellbeing of people behind the scenes. Science can push industry forward, but safety must never trail behind.
Practical education stands as a real solution: routine safety training, transparent documentation, and open communication between chemists and regulators. Investing in recycling tech closes resource loops and shrinks environmental footprints. The future of industry leans on materials like Nitrato de Niquel II hexahidratado, but it also depends on responsible stewardship—where progress and care go hand-in-hand.
Niquel II nitrate hexahydrate, or nickel(II) nitrate hexahydrate, lands in labs and classrooms under many different names. Its shimmering green crystals look almost inviting, but the chemical can cause more harm than its appearance suggests. The dangers aren’t just written down in textbooks; I’ve seen peers struggle with skin rashes after a couple of careless touches. The real trouble starts when someone underestimates how easily chemical safety slips can happen, turning a routine experiment into a hospital run.
This compound makes quick work of bare skin. Just brushing against it might leave you with a persistent itch or red, irritated patches. One day, fresh gloves in the chemical storeroom saved me from learning this the hard way. The nickel ions love to burrow in, causing allergic reactions—some folks find out about their nickel allergy in the worst way possible, over a lab sink, with their hands swelling up. Wash with soap as soon as anything spills, and never trust a torn glove to shield you. I keep a checklist by my chemical cart—good gloves, goggles, and a lab coat every single time. Skipping gear to save time doesn’t pay off.
The dust from nickel(II) nitrate isn’t just annoying—it poses a real threat to lung health. In high school chemistry, a friend inhaled it during a cleanup gone wrong. Difficulty breathing landed him in the nurse’s office. Science backs up the risks: the International Agency for Research on Cancer lists nickel compounds as carcinogenic. Respirators or a fume hood stop fine powders from floating up where you least expect them. Working with the stuff for years, I learned to avoid shortcuts. It’s easy to believe you’re safe until a spill lifts a cloud, and coughing reminds you why precautions matter.
Nickel(II) nitrate hexahydrate brings more to the table than just contact or inhalation hazards. It oxidizes easily, feeding fires if mixed with the wrong materials. Sealing containers tightly and keeping them away from combustibles prevents big problems. I once saw a tiny spill turn into a minor scare when a scrap of paper nearby caught a little too much heat. These moments turn lessons from a chemistry manual into real-life urgency. Disposal also means thinking about the bigger picture—pouring leftovers down the drain dumps toxins into water systems, hurting both people and wildlife. Facilities that follow hazardous waste rules protect the rest of us just by doing their job right.
My approach comes down to habits: never handle this stuff without a plan, clean up right away, and never skip the safety gear. Peer-reviewed sources like the CDC and PubChem back up these recommendations, not just tradition or hearsay. Plenty of accidents come from trusted routines or a sense that nothing bad has happened before—so why worry?
Training and retraining matter. I’ve run demos for students and watched as experienced techs answer questions on the spot. Mistakes still happen, which makes regular safety drills and open conversations about errors important. The best labs aren’t just clean; they’re places where nobody’s afraid to double-check a friend’s gear or remind each other why goggles aren’t a fashion statement.
Simple respect for what nickel(II) nitrate hexahydrate can do keeps everyone safer—both seasoned chemists and new students. Take it from someone who’s cleaned up more than a few spills: treating these risks seriously changes outcomes for the better.
Science classrooms always had a smell, and it wasn’t just the frog tanks or the vinegar from volcano projects. Chemical storage often caused its own flavor of trouble, especially with the greenish-blue crystals of Nitrato de Niquel II hexahidratado. Even now, looking at this compound in an industrial or lab setting, certain lessons come to mind. This isn’t table salt—care shapes every step you take.
Water-laden air loves nickel nitrate. Left out, these crystals suck moisture straight from the room. Humidity always tries to sabotage chemical storerooms. Stack a bag of this on a wooden shelf during a summer thunderstorm, you’ll see clumps form by the next morning. That spells risk, not just for the material’s purity but also the way it deals with other chemicals. Closed containers come first—heavy plastic or glass with tight lids. There’s nothing fancier or more effective. Throw in a desiccant packet if the weather refuses to cooperate.
Nickel nitrate breaks down if it gets too warm. High temperatures can spark dangerous gases. Anyone who’s smelled the metallic tang of decomposing nitrate compounds knows the warning. Put bags or jars away from hot pipes or sunlight streaks. Storage behind a locked, ventilated door works well. The room should run cool—comfortable to work in, but not cold enough for condensation on the walls.
Never keep strong oxidizers near fuel or solvents. Nitrato de Niquel II hexahidratado teams up with organic dust or spill residues to create fast fires. Mix-ups happen: a container drops, powder scatters, someone nearby is handling acetone or oil rags. Segregated cabinets shield against the domino effect. Cabinets labeled “Oxidizers” serve their purpose. In many labs, these sit apart or inside a flammable-resistant room.
Say it in every training session: nickel compounds are toxic. Chronic exposure runs the risk of skin rashes or lung irritation. Gloves matter—so do lab coats. Pointing out dusty fingerprints on doorknobs helps young techs build habits. Handwashing turns into a safety drill, not a suggestion.
Spills come from carelessness, cracked glass, or a jostling elbow. Nickel nitrate dissolves fast and stains deeply. Keep absorbent materials, nitrile gloves, and sodium carbonate on the spill cart. Staff should learn to seal off the area and clean up right away to avoid tracking dust everywhere. Parts of the safety plan rely on routine: bins at every worktable, clear instructions by the door.
A faded sticker means trouble. Labels need chemical names, date of receipt, and hazard warnings. Old glass jars with mystery crystals end up costing time and safety. Staff appreciate color-coded systems, even bold Sharpie notes, especially in a room with twenty similar bottles.
Experience teaches caution faster than paperwork. Outdated storage creates headaches, unnecessary risks, and sometimes serious harm. Nitrato de Niquel II hexahidratado demands the same respect as acids or strong bases. People deserve clear rules and working equipment to back them up. Every busy lab finds this out sooner or later.
Nature doesn’t leave much to chance, and chemistry rarely surprises those who handle its principles regularly. Nitrato de Niquel II hexahidratado—known in English as Nickel(II) nitrate hexahydrate—comes with the chemical formula Ni(NO3)2 · 6H2O. Chemists use this formula to understand both the substance’s behavior and its potential risks. There’s nothing mysterious or rare in its structure: one nickel ion sits paired with two nitrate ions, and water molecules—six of them—bind up the crystal form. This formula puts it firmly in the category of hydrous salts, those colorful and often striking relics of electrolytic and precipitation processes.
Knowledge of formulas shapes lab safety and experiment design. In my time working with metal salts, memorizing these numbers felt less about passing an exam and more about avoiding costly—and sometimes dangerous—missteps. Nickel isn’t especially forgiving with mistakes; people who overlook its hydration state risk forming unexpected solutions or breathing unwanted dust.
Nickel nitrate hexahydrate doesn’t hide in a lineup of chemicals. Pull it from a container and the first thing anyone notices: its vivid emerald-green crystals. Solid at room temperature, it forms a crystalline structure reminiscent of shattered glass, yet more regular—you can practically count facets under the right light. To the uninitiated, it appears almost decorative, resembling gemstones or colored rock sugar. In practice, workers treat it with caution, gloved and goggled, mindful that beauty in a chemical cabinet does not mean harmlessness.
Humidity plays tricks on this compound. Toss it into damp air and you’ll notice clumping, a telltale sign of hygroscopic salts pulling water from their surrounds. Storage in airtight containers isn’t just a habit; it protects both the chemical and the people managing it.
Getting the formula right is more than a theoretical detail. Nickel nitrate hexahydrate often finds its way into electroplating, textile dyeing, and certain synthesis processes. The formula tells users exactly what to expect from it. Too little water in the crystal structure, and reactions change unexpectedly; too much, and concentrations fall, sometimes ruining an entire batch. Visual recognition helps too. I’ve avoided errors by double-checking that unmistakable green before measuring powders in an open lab.
Professional settings demand more than intuition. Clear labeling, regular training, and up-to-date safety sheets cut down on accidents. Teaching new staff to recognize not just the name, but the look and feel, proves just as important as explaining molecular diagrams.
Nickel(II) nitrate’s reputation comes with good reason. The substance is toxic, especially with repeated or prolonged exposure. Anyone handling it benefits from routine monitoring, frequent glove changes, and a no-nonsense approach to spills. Facilities investing in fume hoods and personal protective equipment display responsibility, not just compliance.
Opportunities for improvement always exist. Automation reduces direct handling, and real-time inventory systems help prevent expired or degraded chemicals from staying in storage. Schools and small labs benefit from outreach programs and online training. Sticking to well-supported practices keeps people safe and products reliable.
Nitrato de Niquel II hexahidratado goes by the formula Ni(NO3)2·6H2O. It looks like a greenish crystal and finds frequent use in labs and industry, especially for nickel plating, catalysis, and ceramic coloring. Tiny amounts can even end up in research for batteries or pigments. Walking into a room where this compound gets used, you instantly notice the label warnings. There’s good reason for that.
This nickel salt carries recognized health hazards. Direct contact with skin or eyes brings itching, redness, and sometimes blistering. Experience with accidental exposure on my own hand led to stinging that lasted into the next day, serving as a reminder to never skip gloves. Inhalation is another real problem, often ignored by those rushing through a small job without proper ventilation. Inhaling the dust or solution mist can cause coughing, shortness of breath, and throat pain. Chronic exposure to nickel compounds links with worse health threats, including increased cancer risk (International Agency for Research on Cancer lists nickel compounds as carcinogenic). The Centers for Disease Control and Prevention notes that those working in industrial settings with nickel see higher rates of nasal and lung cancer than those without such exposure.
Nickel nitrate, being water-soluble, also raises risks if ingested. Even tiny quantities can cause nausea, abdominal pain, or vomiting. Ingestion rarely happens outside the workplace, but accidents do occur, especially if food or drink catches contamination from poor lab hygiene. For people with nickel allergies, which aren't rare, the mere touch of nickel compounds triggers dermatitis.
A spill does not just disappear. Waterways exposed to nickel nitrate suffer not only ecosystem damage—fish and microorganisms show toxicity symptoms even at low concentrations. Environmentally, once soluble nickel salts make their way into the water system, reversal takes effort and money. Personal experience working with water remediation teams taught me that chemical spills take a village to clean, and long-term impact can stick around long after the green color fades.
Repeated safety drills in labs and workshops hammer home a few simple steps that protect health. Gloves form the first defense, followed by splash goggles and long-sleeved coats. Fume hoods or good room ventilation cut down airborne risks. These steps look like overkill—right up until someone ignores them and pays the price. Labeling matters, too. Mixing up compounds, even for a moment, invites trouble, and a missing warning sticker often spells danger. Hand washing after work, keeping food away from the lab, and regular air quality checks all rank up there with best moves for health.
Facilities switching to less hazardous alternatives where possible makes a difference. Where replacement does not work, education goes a long way. Consistent training keeps people alert. Reporting minor incidents—burns, spills, or dust clouds—should never meet silence, given how cumulative exposure works. On the regulatory side, following OSHA and international guidance draws a clear line for both employers and employees.
Nitrato de Niquel II hexahidratado stands on the list of useful but hazardous chemicals. Its risks, both short and long term, call for respect and proper management. Through hard-earned habits and a commitment to safe workplaces, people can keep the benefits without suffering needless health costs.
| Names | |
| Preferred IUPAC name | nickel(II) nitrate hexahydrate |
| Other names |
Nickel(II) nitrate hexahydrate Nickel dinitrate hexahydrate Nickelous nitrate hexahydrate Ni(NO3)2·6H2O |
| Pronunciation | /niˈtɾato ðe ˈnikel seɣis eksi.i.ðaˈɾato/ |
| Identifiers | |
| CAS Number | 13478-00-7 |
| Beilstein Reference | 412483 |
| ChEBI | CHEBI:78078 |
| ChEMBL | CHEMBL24403 |
| ChemSpider | 54654 |
| DrugBank | DB13372 |
| ECHA InfoCard | 100.033.447 |
| EC Number | 023-043-00-X |
| Gmelin Reference | 85492 |
| KEGG | C18797 |
| MeSH | D009696 |
| PubChem CID | 22587 |
| RTECS number | QR6300000 |
| UNII | 24YO95J2MR |
| UN number | UN2725 |
| Properties | |
| Chemical formula | Ni(NO3)2·6H2O |
| Molar mass | 290.79 g/mol |
| Appearance | Green crystalline solid |
| Odor | Odorless |
| Density | 2.05 g/cm³ |
| Solubility in water | Very soluble |
| log P | -1.0 |
| Acidity (pKa) | 9.86 |
| Basicity (pKb) | -6.6 |
| Magnetic susceptibility (χ) | +962.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.53 |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 286.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -174.8 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -478.7 kJ/mol |
| Pharmacology | |
| ATC code | V07AV |
| Hazards | |
| Main hazards | Oxidizing, Harmful if swallowed, Causes serious eye damage, May cause an allergic skin reaction, May cause cancer, May cause damage to organs through prolonged or repeated exposure, Very toxic to aquatic life with long lasting effects |
| GHS labelling | GHS07, GHS09, GHS03 |
| Pictograms | GHS05,GHS07,GHS09 |
| Signal word | Danger |
| Hazard statements | H272, H302, H350, H360D, H373, H400, H410 |
| Precautionary statements | P210, P220, P264, P273, P280, P302+P352, P305+P351+P338, P310, P370+P378, P501 |
| NFPA 704 (fire diamond) | 2-3-0-OX |
| Flash point | No flash point |
| Lethal dose or concentration | LD50 oral rat 175 mg/kg |
| LD50 (median dose) | LD50 oral rat 175 mg/kg |
| NIOSH | KW2975000 |
| PEL (Permissible) | 1 mg/m3 |
| REL (Recommended) | 2 mg/m³ |
| IDLH (Immediate danger) | Nickel(II) nitrate hexahydrate IDLH: "25 mg Ni/m³ |
| Related compounds | |
| Related compounds |
Acetato de níquel(II) Carbonato de níquel(II) Cloruro de níquel(II) Sulfato de níquel(II) Óxido de níquel(II) |
