知識について
Cupric Chloride Anhydrous: A Down-to-Earth Commentary
Historical Development
Cupric chloride, or copper(II) chloride, goes way back to the roots of inorganic chemistry. Alchemists in early times ran experiments with copper compounds, but it wasn’t until the rise of analytical science in the 18th and 19th centuries that the true nature of cupric chloride became clear. Hobbyists and professionals alike tinkered with greenish-blue crystals, curious about this salt’s potential. The shift from curiosity to utility happened through the Industrial Revolution, as copper’s role in electrical and chemical production became apparent. Chemists refined extraction and purification processes over decades, making the compound more reliable for science and industry. Labs and manufacturers steadily improved methods for isolating the anhydrous form — tight control of moisture and temperature producing the familiar yellow-brown powder. This evolution speaks to a broader story: the ability to turn chemical knowledge into technology, and then improve upon it, rests on generations stubborn enough to keep asking questions.
Product Overview
Walk into any lab supply store, you’ll find cupric chloride among the shelf staples. Sold under names like copper(II) chloride anhydrous or simply CuCl2, the substance tends to come as a fine, light brown or yellow powder in tightly sealed containers. Its chemical properties — ability to dissolve in water, react with other metals, form complex ions — make it essential in practical applications. From my own work, I can say that even modest quantities end up stretched across projects: etching printed circuit boards, kicking off syntheses for pigments, playing a role in even unique artistic experiments where metallic finishes or revealing chemical patterns matter. The price tag reflects both its utility and general abundance; it isn’t hard to get, though the anhydrous kind often calls for careful storage in cool, dry environments. I’ve watched students and experienced chemists alike choose this substance for predictable, repeatable reactions, which shows its reputation for reliability isn’t just marketing fluff.
Physical & Chemical Properties
Anyone who has handled this compound can tell you that cupric chloride anhydrous is a moisture magnet. Left out in open air, it hungrily siphons water from its surroundings, shifting from a dusty powder to a clumpy, green mass. Drop it in water, you get a vivid blue solution as it hydrates. With a molecular formula of CuCl2, it weighs in at about 134.45 grams per mole. It holds together at room temperature but starts to decompose above 620°C, where copper(I) chloride and chlorine gas can form if the heat keeps climbing. Acids dissolve it with ease, while bases and strong reducing agents convert it to other copper compounds. Its capacity to switch gears — both color and composition — under different conditions is what gives chemists precision, whether they are fine-tuning reaction rates or controlling metal content in industrial processes. For someone used to juggling several hazardous substances, cupric chloride’s stability actually comes as a relief. You can depend on it for consistent physical behavior as long as you don’t leave it out for humid air to find.
Technical Specifications & Labeling
On the label, you’ll spot clear details: purity is usually listed above 99% for analytical grade, backed by batch numbers and hazard icons. Manufacturers are required to include UN codes and standard markings under frameworks like GHS (Globally Harmonized System), which warn users about possible toxicity, environmental hazards, and reactive qualities. The density, melting point, and molecular weight appear so users can line up their measurements exactly. For food or pharmaceutical uses — not common, but not unheard of — even stricter testing and certification comes into play. Precision here isn’t a luxury; I’ve seen whole research projects grind to a halt because of mislabeled or inconsistent batches. Trustworthy labeling, backed by transparent sourcing and third-party verification, builds the confidence researchers and industry players need to keep pushing for better results.
Preparation Method
Most cupric chloride anhydrous starts life with copper metal or copper(II) oxide meeting concentrated hydrochloric acid. The initial blue-green hydrate forms and then, using careful heating under vacuum or with a drying agent, the anhydrous form emerges. The process can get tricky, since a slip in temperature or a stray drop of moisture means the product rehydrates and loses its punch. I’ve observed technicians hover over hot plates, balancing the risk of decomposition against the peril of a product ruined by stray water vapor. Industrial operations scale this process up with controlled reactors and drying towers, but the principles remain the same: chemistry that looks straightforward but hides plenty of subtle challenges. Doing it right means you get a consistent, storable, and dependable anhydrous powder, ready for action wherever copper chemistry is needed.
Chemical Reactions & Modifications
Cupric chloride isn’t content to sit idle—it plays a part in everything from etching metal surfaces to catalyzing reactions that build up organic molecules. Drop it into a beaker with metallic iron, and a redox reaction shifts it to copper metal while iron dissolves as iron(II) chloride. I’ve run this reaction to strip protective coatings, watching the distinctive red copper deposit out. In organic chemistry, cupric chloride serves as a mild oxidant, guiding delicate transformations without wrecking sensitive bonds. It can couple with ammonia to form deep blue complexes, or react with sodium sulfide to yield copper sulfide, a black pigment historically prized in pottery. This adaptability, spanning mineral metathesis, electron transfer, and coordination chemistry, keeps it in play across hundreds of protocols. Its behavior remains controllable, letting researchers push boundaries without losing sight of safety or practicality.
Synonyms & Product Names
In catalogs and safety sheets, you’ll find cupric chloride anhydrous under names like copper dichloride, copper(II) chloride, Cuprichlorid, or even just CuCl2. Europe and Asia sometimes go for older names — Butter of Copper, or Kupferchlorid — while American suppliers stick to the formula. Some industries use product codes like “copper chloride dry technical grade” to signal slight variations in purity or particle size. Over time, these synonyms built up a confusing history, but in practice most chemists recognize the characteristic appearance and handle it with the same basic caution. This cluster of names points to deep roots in academic tradition, but also shows how global chemistry never really let go of its old habits.
Safety & Operational Standards
You hear plenty of stories from people who didn’t pay attention to the safety sheet. Cupric chloride, like a lot of copper compounds, poses real hazards to skin and the respiratory system. Dust or fumes irritate mucous membranes, and ingestion or serious exposure means a trip to the doctor. Smart practice means working in a well-ventilated fume hood, wearing gloves and goggles, and storing the chemical away from acids, alkalis, and reducing agents that could trigger unwanted reactions. Waste solutions require special handling; copper ions do real damage in aquatic environments, so dumping leftovers is out of the question. Regulations have only gotten stricter, with shipments requiring clear labels and containers tough enough to survive drops or leaks. In my own workspaces, clear protocols and buddy checks mean everyone from student to supervisor stays sharp and healthy. Even small spills or unintended exposure can throw off a whole day and jeopardize years of lab reliability.
Application Area
Out in the field, cupric chloride crops up in dozens of applications. PCB makers use it to strip copper from circuit board blanks, taking advantage of its ability to etch cleanly and evenly. Textile workers apply it as a mordant, fixing dyes into fabrics so the colors last wash after wash. Wood preservation sometimes leans on its antifungal and insecticidal powers, though environmental concerns have started to shift this use. Catalysis in organic synthesis, production of pigments, and even photography — anywhere copper’s variable oxidation state brings value — all benefit from cupric chloride’s unique properties. My own experiences span etching metals for art pieces to setting up demonstrations for classrooms; versatility almost doesn’t cover it. Each use brings new wrinkles, but the underlying chemistry connects them all, showing how a single compound threads into so many technologies.
Research & Development
Researchers are always on the hunt for ways to refine old tools, and cupric chloride sits inside that cycle. Recent work has gone into improving etching efficiency to reduce toxic waste, creating recovery processes that pull copper ions out of industrial runoff. In catalysis, the goal is to use less, recover more, and create higher-value products — whether that’s pharmaceutical intermediates or specialty polymers. Surveys of scientific journals show an uptick in environmental and “green chemistry” approaches, with engineers trying to close the loop on copper’s life cycle. Even in high school and undergraduate labs, students investigate cleaner synthesis and safer uses, building the next generation of safer, more efficient workflows. Talking to colleagues at conferences, I hear constant stories about iterative gains: better sensors, stronger pigments, smarter recycling. It’s a grind, but every improvement gives a little more breathing room, both economically and environmentally.
Toxicity Research
Copper compounds draw a lot of attention from toxicologists, and cupric chloride stands near the front of the line. Study after study confirms that shakily handled copper salts run up the risk for both acute and chronic health problems. Lab animals exposed to high doses develop liver and kidney problems; environmental biologists flag the danger to fish and invertebrates. Regulatory authorities in North America and Europe maintain strict exposure limits: workplace air, wastewater, and product residues all require testing and recordkeeping. Experience in the lab tells me a little care goes a long way — labeling, training, and regular risk assessment keep the bad outcomes rare. Yet as research pushes new uses, the scientific community must keep pace with understanding long-term effects, bioaccumulation, and detailed mechanisms of toxicity at cellular levels. Progress needs responsible stewardship, clear communication, and a willingness to improve standards as the facts come in.
Future Prospects
Looking ahead, cupric chloride sits in a complicated spot. There’s no sign that demand for printed electronics, specialty coatings, or advanced catalysis will slow. At the same time, society expects cleaner manufacturing, tougher regulations, and near-perfect recycling. I see promise in new recovery techniques, from electrochemical separation to green solvents that allow the copper to stay useful without the waste. Collaborations between academic labs and industry players may push safer, more efficient catalysts that use copper chloride in lower doses or confined systems. It’s not all blue-sky optimism — ongoing global trends in electronics, infrastructure, and sustainability suggest that this old salt can keep adapting without giving up its practical strengths. The push for more responsible, knowledge-backed use gives hope not only for innovation, but also for keeping people and planet in mind.
What It Really Does in the World
Cupric chloride anhydrous stands out for one reason—it gets jobs done where other chemicals fall short. On my first day interning in a small metal finishing plant, I saw workers reach for this bright green powder to prep metal surfaces for plating. With just a scoop added to their chemical baths, tarnished copper sheets soon gleamed. The reaction acted fast, stripping away oxides that would wreck the final product. For factories like this, it helps keep production lines moving and waste low, and there’s always a place on the shelf for another 25-kilo bag.
Making Printed Circuit Boards
Tech shops making printed circuit boards (PCBs) rely on cupric chloride. During etching, it dissolves unwanted copper from boards without damaging what needs to stay. Every time I’ve seen the process, a clear etch means less troubleshooting and faster assembly. Cupric chloride reacts predictably, so engineers aren’t left guessing. Fewer errors means less material scrapped and more reliable electronics in everything from laptops to washing machines.
A Key Ingredient in Dyes and Pigments
This chemical keeps showing up in places you might not expect. Textile factories use it to deepen blues and add vivid greens in their dyes. Because it reacts with other ingredients to create strong, lasting colors, the garments don’t fade after two washes—giving brands a reputation for quality. I remember inspecting rolls of dyed cotton where the color consistency sold the shipment. For paint and ink makers, it brings deep shades that artists and printers lean on every day.
Lab Reagent and Science Tool
In school labs, cupric chloride helps students understand chemical reactions. Teachers use it for experiments that show how metals can change states or swap partners with other chemicals. I joined a high school class where students tested reactions by dipping bits of aluminum into cupric chloride solution. They watched a cloud of bubbles and reddish metal form. This hands-on experiment sparked their curiosity more than any textbook ever could. Universities pick this compound for research on crystal growth or catalysis too, keeping science moving forward.
Treating Wood and Controlling Pests
Woodworkers use cupric chloride as a preservative. I met a craftsman sealing fence posts with it to slow rot and keep termites away. Instead of losing boards to decay after one wet season, the wood lasted for years. Agricultural suppliers blend it with other agents, helping safeguard crops from fungal diseases. This chemical forms a barrier so plants can keep growing and yields don’t dip just from a rainy spell.
Challenges and Solutions
Using cupric chloride has its risks. It can irritate skin, eyes, and airways, so protective gear becomes standard on factory floors and in labs. Facilities that recycle spent etching solutions recover copper and process the leftovers responsibly. Regulations keep disposal safe and monitor workplace exposure. Companies switching to automated dispensing cut down on human contact. Training workers and updating safety sheets are two steps I’ve seen that stop problems before they happen. For anyone using cupric chloride, staying responsible not only keeps people safe but builds trust with customers and local communities.
Understanding Cupric Chloride Anhydrous
Cupric chloride anhydrous shows up in different industries, from laboratory benches to manufacturing floors. Its chemical formula, CuCl2, might look simple, but behind those letters, there’s more than just a set of elements stuck together. With copper holding the +2 oxidation state and paired with two chloride ions, the structure lets it participate in key reactions, help with analysis, and even spur on chemical production where accuracy isn’t just recommended, it’s critical.
My Encounters With CuCl2
During undergraduate days, handling cupric chloride didn’t seem like a big deal. We used it to prepare pigments and practice chemistry techniques. One spill later, though, the real world importance of chemicals—and of knowing precisely what each one represented—became clear. Safety data made a lot more sense afterward. Mislabeling even a single element can lead to more than wasted time; lab safety, data accuracy, and even outcomes for industry scale processes ride on knowing you’re working with CuCl2, rather than something else entirely.
CuCl2 In Everyday Life
Beyond the classroom, this blue-green compound ends up in wood preservation, textiles, and dyes. Workers rely on its reactivity. Chemists look for predictable reactions. Anyone ordering, shipping, or storing chemicals depends on that formula meaning the same thing every time. Mistakes here add up, whether it’s through health risks to handlers or ruined product batches. I’ve heard more than one story about shipments flagged for having the wrong certificate, all because someone got sloppy with the formula or didn’t understand its significance. Reliability here isn’t academic—it’s real dollars and real safety.
Potential Pitfalls and Fixes
Using a compound like cupric chloride isn’t all smooth sailing. Even today, poor training leads to mix-ups. New hires in a plant once confused cupric chloride with cuprous chloride (CuCl). Only after redoing an entire batch did they realize the error—costing the company thousands and creating unnecessary waste. Precision in names and formulas isn’t bureaucracy, it’s the foundation for working safely and profitably.
Legal compliance also depends on correct identification. Regulatory authorities hold companies responsible for their inventory lists, safety sheets, and labeling. Inaccurate chemical identification gets flagged fast, stripping away trust with partners or customers. Emergency workers arriving at a scene count on clear labels to manage chemical spills or exposures safely.
Making Things Safer and More Reliable
Here’s where good habits save real trouble. Training workers to respect chemical formulas matters. Straightforward labeling, regular audits, and easy-to-read datasheets take the guesswork out of handling even the simplest compounds. Digital inventory tools that scan and verify formulas, or simple cheat sheets for lab staff, dramatically lower mistake rates. I encourage folks not just to memorize, but to understand what each formula represents in terms of risk and reactivity.
Trust is fragile in the world of chemicals. The right label, forged by habit and science, helps keep workplaces safe and production on track. The formula CuCl2 stands out as a reminder: small details, respected and repeated, make all the difference.
Cupric Chloride Anhydrous: A Closer Look at the Risks
Cupric chloride anhydrous does more than just sit on a laboratory shelf. It loves moisture, which means it reacts and changes if left out in the air. I’ve worked in labs where a failure to keep this compound tightly sealed led to ruined samples and safety headaches for the team. It absorbs water, clumps, and can become hazardous. This isn’t a risk to brush aside, especially considering inhalation or skin contact brings real dangers. Copper salts may trigger respiratory issues, skin irritation, and even severe reactions if handled carelessly. For these reasons, proper storage does more than protect product quality—it protects people, too.
Straightforward Storage Solutions
Start with containers that don’t mess around. Glass jars with high-quality plastic lids or tightly sealed HDPE bottles usually do the trick. Skip metal, as it reacts, and avoid cardboard or weak plastics that can degrade over time. Sitting in more than a few labs, I’ve watched careless choices lead to powder leaking out and reacting with the air. It’s simpler and cheaper to get the right container from the start.
Desiccators become essential in most climates. Even rooms that feel dry by human standards have enough ambient humidity for the powder to pull in water and form lumps. If you don’t store this chemical with drying agents such as silica gel or activated alumina, expect trouble. Switching to desiccators solved countless issues for our lab team, cutting down on waste and complaints from colleagues.
Shielding From Light and Heat
Sunlight speeds up degradation. Store cupric chloride anhydrous in a cool, dark spot—think cupboards, not open shelves. Chemicals on exposed shelving tend to fade in color and sometimes jumpstart chemical breakdowns. Temperatures should stay stable and moderate, nowhere near oven-like or freezing zones. A storage room that keeps a consistent range delays spoilage and prevents unwanted reactions. From what I’ve seen, high temperatures can even cause containers to warp or crack—a total mess.
Label Everything and Address Emergencies
Every container should show what’s inside and provide a warning about the risks. Following clear labeling keeps mistakes to a minimum and gets the right response if spills happen. Spill kits in the same storage area matter just as much. With powdery copper salts, spills can spread fast, and cleaning late only makes things harder. Having gloves, safety goggles, and a good dustpan nearby pays off. I’ve watched colleagues fumble for supplies during spills, losing time and composure. Preparedness makes every workplace safer.
Clear Policies and Training Support Safe Storage
Regulatory agencies like OSHA and EPA publish guidelines for chemical handling, and sticking to their advice just makes sense. In my experience, ongoing staff education changes how seriously everyone takes these guidelines. Refresher courses and posted safety reminders go a long way to avoid the slip-ups that lead to exposure or contamination. At smaller companies, periodic audits or simple checklists made a real difference. Even the seasoned chemists sometimes let their guard down.
Better Storage Means Fewer Risks—and Less Waste
Efficient storage keeps both the workers and the product safe. Small investments in airtight containers, desiccants, and good training return big dividends in safety and productivity. From my years in labs and storage rooms, I’ve found that shortcuts almost always end up costing more in ruined chemical stock, wasted time, and health scares. Cupric chloride anhydrous isn’t forgiving when ignored, but solid storage habits keep the headaches to a minimum.
Real Risks in Everyday Chemistry
Cupric chloride anhydrous isn’t the kind of compound most people encounter beyond a laboratory, but that doesn't mean its health risks only matter to chemists. This blue-green solid features in industrial processes, research labs, and sometimes in high school science classrooms. Growing up with a scientist parent, I saw firsthand how routine chemicals can cause harm without caution.
What Happens on Contact or Inhalation?
Direct exposure deserves respect. If someone breathes in the dust, irritation happens fast. Nose and throat feel scratchy. Headaches pop up. Extended or repeated exposure leads to tightness in the chest, coughing, and more serious respiratory issues. If the compound touches skin or eyes, you get stinging and redness. Copper compounds, including cupric chloride, slip through skin and find their way into the bloodstream. I once saw a colleague need a trip to urgent care—his rash from careless contact lasted days.
Swallowing Isn’t Just a Bad Idea—It’s Dangerous
Accidental ingestion doesn’t just leave a bad taste. Stomach lining meets copper ions and violent nausea follows. Vomiting and abdominal pain come next followed by diarrhea. Swallow enough and it can injure the liver and kidneys. I’ve read about copper poisoning cases from industrial sites, with victims needing intensive care for severe toxicity—even long after the exposure stopped.
Understand Toxicity: Not Just “Dangerous Chemicals”
It's easy to ignore risk until you suffer. The Centers for Disease Control and Prevention (CDC) classifies cupric chloride as toxic. Long-term exposure, through work or otherwise, may trigger chronic effects: anemia, kidney damage, and liver problems. There’s evidence copper salts may cause allergic reactions. I remember a safety seminar where a nurse described ongoing copper exposure pushing patients into lasting anemia—not because of dramatic accidents, but because nobody paid attention to daily habits.
Safety Practices Matter—Every Time
Health agencies like OSHA and NIOSH give clear directions. Wear gloves and goggles. Work in a fume hood. Practice good hand hygiene. Never eat or drink in the lab. I’ve watched shortcuts backfire even among professionals who’d handled chemicals for years. Institutions can reduce harm by posting clear hazard labels and never letting protective gear lapse. Regular training goes a long way. Too often, familiarity with chemicals breeds carelessness, so it helps when leaders set the right tone.
Next Steps and Better Habits
Substitution makes the most difference where possible. Picking less hazardous chemicals, finding closed-system handling, and automating dispensing processes reduce chances of harm. If forced to use cupric chloride anhydrous, workers must make safety part of their routine. Supervisors bear the responsibility to keep information easy to access and instructions easy to follow. Both the World Health Organization and the CDC post clear safety sheets—easy for anyone to download and study before grabbing a reagent bottle.
From Personal Responsibility to Collective Safety
Ignoring health risks doesn’t make them disappear. Each person in a workplace, classroom, or lab impacts the health of those around them. Building the habit of double-checking labels, using the right protection, and never assuming a “small” exposure is harmless makes all the difference. Looking back at real incidents and health reports drives the message home: safety isn’t just about compliance—it’s about people getting home healthy every day.
Defining Purity in Cupric Chloride Anhydrous
Cupric chloride anhydrous, known to a lot of us in labs as CuCl2, plays a genuine role for chemists, teachers, and plenty of industry professionals. If you’ve stood hunched over a beaker and watched the deep green crystals dissolve, you start to care about what exactly you’re working with. Purity is no small technicality—it sets the tone for every reaction, every result, every bit of research. In straightforward supply, most manufacturers offer Cupric Chloride Anhydrous at purity levels hovering around 98% to 99%. This percentage means direct chemical content, not counting the crumbs of water, iron, and maybe a dusting of other metals mixed in during production or packaging.
The Reasons Purity Actually Matters
A lot of processes depend on a consistent, trusted product. When I ran a DIY copper plating demo for students, anything but high-purity cupric chloride gave weird, unpredictable spots on coins. On the bigger industrial scale, electronics manufacturers chasing quality copper etching come to a hard conclusion: contaminants in the batch drag down yields, send scrap rates up, and create downtime. It’s frustrating knowing a tiny impurity in the crystal can throw off a week’s work.
For researchers, especially in pharmaceuticals or catalysis, high purity can mean the difference between a paper you can trust and one that needs a retraction. Lab results start losing credibility fast if the baseline has unwanted metals or moisture. Contaminants like sodium, magnesium, and even traces of organic material play spoiler. Testing for these takes time, but skipping this step causes damage to both reputation and safety.
Where Purity Can Slip
Every step in the supply chain introduces risk—sourcing, storage, and even transport. I’ve seen bags with seals broken or flakes clumped into bricks because of humidity. Technical grade (around 97–98%) can sometimes slip to 95% when mishandled. The shelf at the back of a humid storeroom is not kind to anhydrous salts. You start to see hydrolysis, and suddenly the “anhydrous” part is questionable.
Checking and Certifying What You Get
Reputable suppliers offer a certificate of analysis. These certificates spell out not just copper content, but also give a proper rundown of contaminant levels—often with figures for iron, lead, and arsenic. Some labs don’t even accept shipments without this printed assurance. High-end grades—sometimes labeled as “ACS Reagent” or “Analytical Reagent”—push the bar to 99% and above, but prepare your wallet for the privilege.
The key is confirmation. Simple colorimetric tests pick up excess iron, but for rigorous work, atomic absorption or ICP-OES shows what is really in the mix. Batch testing keeps suppliers honest, and many industries make it routine. I learned early not to trust “green” alone; sometimes those crystals hide surprises.
Improving Standards and Handling
The fix starts with better storage—airtight, in dry rooms, with moisture indicators. Even small operations benefit from split-lot testing. Industry-wide, a push for more transparent data sharing between users and suppliers could help every link in the chain. Auditing suppliers, rotating stock, modernizing packaging, these sound basic, but ignoring them costs money and time.
Cupric chloride’s purity isn’t just a number on a bag. For finding flaws, keeping experiments meaningful, or producing reliable circuit boards, purity sets the stakes. Keeping a sharp eye on what goes into the jar up front saves plenty of headaches later.
| Names | |
| Preferred IUPAC name | Copper(II) chloride |
| Other names |
Cupric dichloride
Copper(II) chloride Copper chloride Copper bichloride Dicopper chloride Copper(II) chloride anhydrous |
| Pronunciation | /ˈkjuː.prɪk ˈklɔː.raɪd ˌænˈhaɪ.drəs/ |
| Identifiers | |
| CAS Number | 7447-39-4 |
| Beilstein Reference | 358691 |
| ChEBI | CHEBI:64350 |
| ChEMBL | CHEMBL1201606 |
| ChemSpider | 10486598 |
| DrugBank | DB09153 |
| ECHA InfoCard | 100.895. |
| EC Number | 231-210-2 |
| Gmelin Reference | 1204 |
| KEGG | C00942 |
| MeSH | D003456 |
| PubChem CID | 24856 |
| RTECS number | GL8900000 |
| UNII | 03G83B4T6L |
| UN number | UN2802 |
| Properties | |
| Chemical formula | CuCl2 |
| Molar mass | 134.45 g/mol |
| Appearance | Brown powder |
| Odor | Odorless |
| Density | 3.386 g/cm³ |
| Solubility in water | Readily soluble in water |
| log P | -0.2 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 6.5 |
| Basicity (pKb) | 8.0 |
| Magnetic susceptibility (χ) | +1440.0e-6 cm³/mol |
| Refractive index (nD) | 1.709 |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 118.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -220.1 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -206.4 kJ/mol |
| Pharmacology | |
| ATC code | A16AX01 |
| Hazards | |
| Main hazards | Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. Toxic to aquatic life with long lasting effects. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H302, H315, H319, H332, H410 |
| Precautionary statements | P264, P270, P273, P280, P301+P312, P302+P352, P304+P340, P305+P351+P338, P308+P313, P330, P332+P313, P337+P313, P362+P364, P391, P501 |
| NFPA 704 (fire diamond) | 2-0-2-Aqu |
| Lethal dose or concentration | LD50 oral rat 584 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 584 mg/kg |
| PEL (Permissible) | PEL (Permissible): 1 mg/m3 (as Cu) |
| REL (Recommended) | 1 mg/m3 (as Cu) |
| IDLH (Immediate danger) | 100 mg/m3 |
| Related compounds | |
| Related compounds |
Copper(I) chloride
Copper(II) sulfate Copper(II) nitrate Copper(II) acetate Copper(II) oxide |
