Copper Acetate Tetrahydrate: Beyond the Blue-Green Crystals
Historical Development
Back before the periodic table shaped chemistry classes and laboratories, skilled craftspeople used copper salts for pigments and fabric dyes in ancient civilizations. One of the earliest recorded copper compounds, verdigris, shares a family tree with copper acetate, and artists prized it for its distinctive blue-green hue in paintings and manuscripts. Alchemists and experimenters in the medieval world mixed copper with vinegar, sometimes placing this concoction on plates to speed up the harvest of pure, crystalline copper acetate. Over time, improved methods for purification and synthesis replaced kitchen chemistry with controlled reactions. By the late 19th and early 20th centuries, chemical producers introduced higher standards and purities, both for research and industrial manufacturing. These days, a bottle of copper acetate tetrahydrate may sit quietly on a lab shelf, but it carries centuries of pigment production, chemical tinkering, and practical advances in copper chemistry behind its vivid surface.
Product Overview
Copper acetate tetrahydrate forms as deep blue-green monoclinic crystals. What stands out in any chemical storeroom is its unique color, somewhere between emerald and turquoise. As a salt formed from copper(II) and acetic acid, this compound lands squarely in the realm of specialty chemicals. Folks working in research, fine arts restoration, and catalysis keep jars of it handy. Laboratories order it by the kilogram, while niche chemical suppliers sometimes market small amounts for glass making, pyrotechnic effects, or preservation of wood. Its presence goes beyond surface color—this compound interacts chemically in useful ways that make it far more than a pretty face in the bottle.
Physical & Chemical Properties
Copper acetate tetrahydrate brings more to the table than striking visuals. As a hydrate, it carries four water molecules per unit, contributing to its crystal stability and solubility profile. Each crystal melts and loses water at moderate temperatures, so storing it in dry conditions preserves its strength and consistency. Dissolved in water, the solution sports a strong blue color, showing off clear copper ions. Its formula reads Cu(CH3COO)2·4H2O. Handling it with bare hands encourages a vinegar tang, a small hazard of contact with acetate anion. In air, the crystals hang onto moisture fairly well, and direct sunlight encourages slow decomposition. Altogether, this salt’s properties demand solid handling practices among chemists and industrial operators.
Technical Specifications & Labeling
Producers assign product codes, lot numbers, and purity percentages to each container, aiming for transparency from laboratory grade to high-purity analytical reagent. Standard analysis targets greater than 98% total purity, and the water content aligns closely with the tetrahydrate formula. Certificates of analysis often list limits on chloride, sulfate, and iron as contaminant traces, helping buyers confirm quality for demanding experiments. Product labeling, under international standards like GHS, highlights hazards such as toxicity to aquatic life and possible risks to skin and eyes. Every bottle includes the chemical’s structure, safety pictograms, signal words, and supplier contact details, serving both legal requirements and the needs of research staff relying on accurate information.
Preparation Method
Commercial-scale synthesis follows established recipes that have roots in historical experimentation—just on a bigger, cleaner scale. Reacting copper(II) oxide or basic copper carbonate with acetic acid in solution yields the acetate salt within hours, and filtration pulls out unreacted solids. As the liquid cools, blue-green crystals form, growing to full size overnight or even over several days at room temperature. Drying under reduced heat or in desiccators maintains the correct water content, a crucial step for high stability and performance. Some labs recycle copper byproducts from other processes, turning industrial byproducts into pure acetate for research and manufacturing. Each method reinforces the value of simple ingredients handled with care and experience, reminding anyone involved that reliable chemical products often spring from clear, methodical routines.
Chemical Reactions & Modifications
Chemists prize copper acetate’s reactive nature, not just its soothing color. In reactions, it donates copper(II) ions for complex formation, redox reactions, and synthesis of organic compounds. Catalysis ranks among its most widespread uses—helping form carbon-carbon bonds, activate hydrogen peroxide, or modify oxidation states in specialized syntheses. Heating the compound liberates acetic acid and leaves behind black copper oxide, standing as a classic example for undergraduate labs. Substituting the acetate ions through double exchange reactions leads to a family of copper(II) salts, fueling curiosity and experimentation among both academic and industrial chemists. These reactions sow results in everything from fine chemicals and chemical sensors to the synthesis of specialty polymers and stabilized pigments.
Synonyms & Product Names
On shipping manifests and laboratory shelves, copper acetate tetrahydrate appears under different labels. Cupric acetate, blue verditer, and Paris green (an arsenical cousin) all stem from related chemistry, muddling things for those new to the world of copper salts. Catalogs might list CAS number 6046-93-1 or refer to “copper(II) acetate tetradydrate,” emphasizing its +2 copper state and four waters of hydration. Occasionally, old literature calls it “distilled verdigris,” a throwback to its painterly heritage. Knowing these synonyms helps buyers, researchers, and regulatory authorities keep communications clear, especially when regulatory compliance or hazard labeling demands exact naming.
Safety & Operational Standards
Safety remains a front-line concern. Like most copper(II) salts, copper acetate tetrahydrate irritates skin and eyes on contact—nitrile gloves and safety goggles serve as routine barriers. Inhalation of fine dust can trigger respiratory symptoms, so fume hoods and careful handling keep the risks low. Even low dose, copper ions build up in aquatic environments, so waste disposal rules push for strict containment and treatment before discharge. Material safety data sheets lay out these requirements, including what to do in case of a spill or accidental exposure—something every chemical user needs to review before getting started. Regular workers train on these protocols, and safety checklists, spill kits, and first aid gear stay within arm’s reach in every responsible lab and factory.
Application Area
Copper acetate finds real work in both the commercial world and in research. Catalysis stands out as a primary use, especially for organic synthesis relying on transition metals to trigger key reactions. Pigment makers have turned to copper acetates for stable greens and blues, especially in restoration and conservation work, where near-historical methods prove more authentic than synthetic alternatives. Some pyrotechnicians favor copper acetate for producing blue flames in fireworks displays, drawing on its strong emission lines in the visible spectrum. In agriculture, some formulations once served as fungicides or wood preservatives, but regulatory changes over the years scaled back these uses over environmental concerns. Analytical chemists tap it during redox analysis, and battery researchers examine copper-based salts for their conductivity and charge-transfer behaviors. With every application, the compound’s copper chemistry delivers value, shaping a broad and evolving marketplace.
Research & Development
Scientists and engineers keep pushing on copper acetate’s potential, branching out from classic pigment and catalyst work. Nanotechnology researchers explore its use as a copper nanotube and nanostructure precursor, driving advances in sensing and catalysis at the smallest scales. Photochemical studies highlight its activity in energy conversion and solar devices, where copper’s electron-hopping skills help build promising new materials. Coordination chemists dig into the molecular architecture, mapping out how acetate ligands tune metal properties for everything from biomimetic models to magnetic materials. The creativity shows—with every unexpected twist on classic chemistry, a new angle on copper acetate emerges, shaped by modern tools and multidisciplinary approaches.
Toxicity Research
Copper’s dual role as a biological trace element and environmental toxin frames an ongoing conversation in toxicity studies. Researchers look at low-dose accumulation in aquatic life, linking copper exposure with altered growth and reproductive patterns. In humans, short-term exposure through skin or dust tends to be mild, with irritation or mild gastrointestinal symptoms, but chronic overdose or ingestion brings severer risks, particularly for children and sensitive groups. Occupational safety experts track permissible exposure limits, updating recommendations as new data arrives. Waste management specialists monitor downstream contamination, tying regulatory guidance to the long-term health of waterways and soil. These efforts foster a safer relationship with a compound both useful and potentially hazardous, ensuring that benefits do not come at the expense of long-term public or environmental health.
Future Prospects
Looking ahead, copper acetate tetrahydrate stands ready for adaptation and evolution. Demands for greener, more sustainable chemical practices open doors for new, catalyst-driven synthesis that cut down on toxic byproducts and energy use. Electronics researchers already tinker with copper salts in printable circuits and energy storage, and green chemistry initiatives favor copper’s relative safety over heavier metal catalysts. In pigment and art restoration, the call for archival methods returns copper acetate to its roots, powered by modern analytical controls. Regulatory changes and environmental monitoring will keep guiding how much and where the compound finds work, with research likely to sharpen both safety protocols and performance specs. The intersection of tradition and innovation keeps copper acetate firmly on chemists’ radar, with as-yet untapped uses waiting for a spark of fresh insight.
Beyond the Lab Shelf: What Makes It Useful
Chemistry classrooms often display jars of blue-green crystals with complicated labels, one of which might read copper acetate tetrahydrate. Teachers might highlight the color change as it meets a flame, or hand it over during a titration lab for practice. In the real world, though, this compound reaches far past textbook demonstrations. I got my introduction to copper acetate tetrahydrate during a summer internship at a small metal finishing shop, where color was key and every formula packed a punch.
Colorful Contributions in Pigments and Dyes
Copper acetate tetrahydrate shows up in pigment production, offering a stable and distinct blue-green hue. Artists through the years have benefitted, as this compound delivers shades that last longer on canvas than many alternatives. Textile houses still turn to copper acetate to produce dyes, especially when consistency across batches matters. There’s a reason we still see its fingerprints in the palettes of genuine frescoes or historical paintings—nothing quite matches its vibrancy. In my own amateur painting experiments, the brightness and depth of copper acetate-based pigments stand out even against modern blends.
Boosting Chemical Reactions in Catalysis
This compound isn’t just about looks. Industries that lean on chemical reactions value copper acetate tetrahydrate for its catalytic abilities. I recall a project in university, where we produced polyesters using this salt as a catalyst, streamlining reactions and lowering waste. Real-world manufacturers follow the same logic, bringing this material into large-scale organic syntheses, including pharmaceutical and agricultural processes. Copper’s unique properties help speed up transformations that would slog along otherwise.
Protecting Wood from the Elements
The world doesn’t always remember how chemistry helps keep daily life ticking. Take wood preservation—copper acetate tetrahydrate plays a vital role here. Its antifungal and antibacterial nature shields wood from rot, mold, and insect damage. In small-town carpentry shops, simple treatments with this compound mean fence posts and siding last years longer, even in wet climates. Having replaced my own deck after a season of rot, I’ve seen firsthand the impact of underestimating these protective treatments.
Tackling Environmental and Medical Needs
Research centers dig deeper into less visible uses of copper acetate tetrahydrate. Scientists lean on it in biochemical testing, especially in identifying sugars and proteins. Environmental testing labs rely on its reactivity to detect pollutants in water and soil samples. Medical researchers work with it to explore new antibacterials, banking on copper’s toxicity to harmful microbes. Even though new discoveries replace old standbys, copper compounds linger where reliability trumps novelty.
Moving Forward: Handling With Respect
Every compound that offers benefits comes with responsibilities. Copper acetate’s toxicity creates risks that science classrooms and commercial plants both need to manage. Long-term exposure, especially for workers handling powders or solutions without protection, can cause health problems. Safer packaging, robust protective gear, and educational outreach in labs all help. Communities and companies focusing on copper-based solutions have learned to keep these safety nets strong—nobody takes shortcuts with a compound like this one.
For all its quirks, copper acetate tetrahydrate keeps delivering real-world results. It brings color, speeds chemical reactions, guards wood, and aids research. Users—from artists and chemists to carpenters and environmental scientists—rely on its steady performance, echoing a long history of practical chemistry at work.
Chemicals in Everyday Life
Anyone who’s dabbled in home chemistry projects or followed stories about water contaminants probably recognizes that chemicals shape much of what we deal with, for better or worse. Copper Acetate Tetrahydrate may not sound familiar at first, but that green-blue salt pops up in labs, classrooms, and even in the preservation of wood. The formula, Cu(CH3COO)2·4H2O, reveals more than what’s written on a label. Every part of this formula guides both its use and safety.
What Makes This Compound Matter?
Growing up, science class felt tough until experiments showed that certain compounds hold answers. Color changes, funky reactions, and the occasional safety lecture made dry formulas come alive. Copper Acetate Tetrahydrate stands out because its structure gets hands-on in both research and practical use. Plenty of museums use solutions of this salt to control fungus on artifacts. Gardeners rely on its antifungal power too, though regulations shift as we learn more about copper’s downsides for soil and water.
Chemistry teaching relies on hands-on examples. Watch this crystal dissolve and you spot copper ions in action—turning the solution that vivid blue tells beginners right away that chemistry’s more than black-and-white rules. Kids learn about water molecules “locked” around metal ions, and why those water molecules change how the salt behaves compared to anhydrous copper acetate.
Health, Environment, and Why Knowledge Counts
Personal safety ties in tightly with knowing a compound’s formula. Handling copper acetate at home, hoping to try old-school wood treatment, calls for solid precautions. Accidentally mixing it with the wrong household product could cause new, risky substances. Everyone deserves clear information to judge what’s safe. A clear formula empowers folks to look up toxicity risks, soil compatibility, and environmental impacts, right from the start.
Food chain effects taught me to double-check what goes into my garden. Runoff from excessive copper-salt applications can easily harm beneficial insects, worms, and even backyard pond life. These facts aren’t abstract panic—they've changed the way local gardening co-ops recommend plant treatments. The chemical formula in hand lets communities talk directly to chemists and regulators, making new rules that work on the ground.
Solutions and Safer Use
Access to trustworthy information tops the list for safer chemical handling. Teachers need clear guides showing how to spot hydrate compounds from their formulas. Homeowners should get easy lookups for environmental risks before taking advice off an old forum post. Community workshops on chemical literacy bring together neighbors and experts. That’s a meaningful way to catch outdated habits or risky shortcuts before trouble starts.
Labeling and educational campaigns worked with fertilizers, prompting smarter choices. Those who shop at hardware stores often find clear diagrams on packaging now; a similar approach could boost safe use of lab and industrial chemicals. Science doesn’t need to hide behind jargon. Each part of the formula, like Cu for copper or those four H2O molecules, carries a story people deserve to hear.
Why Proper Storage Matters
Chemistry has always held a practical side for me. Years in a school laboratory taught me that chemicals don’t wait for a mishap — trouble finds the unprepared. Copper acetate tetrahydrate looks harmless, those blue-green crystals almost inviting. Yet, mix a pinch of moisture, careless placement, and you’re looking at ruined samples, damaged labels, maybe even health risks. This powder can fire up a strong vinegar-like smell, and a lax approach brings skin or eye irritation. In my experience, storage isn’t just about preservation; it’s about respect for what you keep on the shelf.
The Trouble with Heat and Moisture
Summer ended most of our old lab’s chemical stock. Humidity snuck through window cracks, gnawing labels and turning many bottles into sticky messes. Copper acetate tetrahydrate hates damp air. These crystals soak up moisture, cake together, and lose value for experiments. Left in sunlight or near a radiator, the color shifts and odd odors appear. I saw students puzzle over spoiled material that didn’t react as it should, all for lack of a sealed bottle or cool cupboard. Reports from safety agencies remind us: warm, wet, or crowded spots degrade purity and, in rare cases, cause the chemical to break down and release acetic acid fumes. It all starts small — an unsealed cap or jar pushed too close to a heat vent.
What Works: The Hands-On Approach
I learned most by cleaning up after myself, not by reading a perfect protocol. At the bench, I’d grab an airtight glass jar, add a label with big writing, and date it without thinking twice. Chemicals don’t wait for emergencies. A glass jar seals out water better than plastic in my experience. Polyethylene or polypropylene containers often flex, warping over months, and don’t block water vapor as tightly. Keeping the container upright matters, too: spills tempt disaster.
Next, the storage spot. A metal chemical cabinet with good airflow works best, away from the steam of a nearby sink. No sunlight, no heater sitting underneath. Some folks opt for a temperature log, especially in university settings, to keep the shelf below 25 degrees Celsius. There’s a reason for all this. The right conditions extend the shelf life, limit product waste, and stop you from breathing in any acetic acid that sneaks out. GHS safety sheets outline risks, but nothing beats routine checks for leaks, changing labels at the start of each semester, and chucking out clumpy, discolored stock.
Personal Practices, Safer Spaces
Lessons stay with me. I make storage easy: keep chemicals in labeled, tightly sealed glass containers, in cool, dry spots above eye level. Accidents drop sharply through routine — a weekly glance, a check for cracked jars, and a rule to keep workspaces uncluttered. Labs that share records of near-misses and update their routines create safer environments for everyone. Educators and researchers do better with straightforward training, clear signage, and enough storage space to avoid overcrowding.
Facing Problems with Straightforward Solutions
Every laboratory faces lapses. Swapping out old shelving, adding dehumidifiers, and giving newer staff hands-on storage walkthroughs beats written warnings. A good sign points out which chemicals sit away from acids or reducing agents. Small improvements, like spill trays and extra gloves, turn annoying chores into habits that avoid incidents. Copper acetate tetrahydrate doesn’t ask much: keep it dry, cool, and out of reach for the curious or the careless, and you'll get long life and consistent results.
Why Safety Isn’t Just a Rule, It’s Daily Practice
Pulling Copper Acetate Tetrahydrate off the shelf brings back memories of crowded undergrad labs and the blue smudges that always seemed to stain fingers. Safety rules might look straightforward on a wall poster, but it’s the small habits that keep people out of trouble. This salt, with its bright blue-green color, signals danger even before any safety data sheet gets read. Any chemical demanding respect for contact, inhalation, or ingestion has left its mark in science classrooms and industry offices everywhere.
Gloves, Goggles, and Never Cutting Corners
Once, a rushed student skipped gloves and spent the afternoon washing persistent traces of blue off their hands. The lesson stuck: skin contact is never harmless. Nitrile gloves and sturdy goggles come out for every handling, whether a few grams get weighed or a solution gets mixed. Splashy stories—literally—make their way around chemistry circles: someone accidentally tips a beaker and ends up with a nasty skin rash or stinging eyes. For home tinkerers and seasoned researchers alike, personal protective equipment stands as the first line of defense.
Air Matters Just as Much as Surfaces
Copper acetate puts off light dust and can irritate lungs with surprising speed. Years of working in shared spaces drilled in the routine: fume hoods stay on, and containers get opened only inside them. That trade-off between convenience and safety almost always becomes a regretful anecdote. Airflow isn’t just for toxic gas experiments; even crystalline dust from common metal salts carries risks for breathing and long-term health. A good lab will have those air systems whirring and never skimp on safety checks.
Don’t Treat Spills Casually
Dropping a bottle on the bench or floor always turns into a group effort. Everyone nearby moves fast to limit contamination, block off the area, and reach for spill kits—never just a towel and a shrug. Copper salts stain and can poison surfaces, so the cleanup goes beyond aesthetics. Gloves, paper towels, strong ventilation, and orderly disposal in the hazardous waste stream keep those accidents from becoming bigger problems. Lab veterans know a little time spent cleaning with care beats the trouble a casual attitude creates.
Good Habits and Clear Procedures Equal Fewer Emergencies
Copper Acetate Tetrahydrate isn’t the world’s scariest compound. Still, real experience teaches that basic procedures work: keep amounts small, double-check labels, mark containers clearly, and never leave the bottle in reach of someone untrained. Eating or drinking in the workspace always stays off-limits, no matter how long the shift drags on. Documentation and regular training sessions give even old hands reason to pause and update their routines.
Being Proactive with Long-Term Health
This compound has triggered headaches and nausea in those unlucky enough to take safety shortcuts. Over time, repeated exposure can hurt the liver and kidneys, so blood tests and health check-ins move from a regulatory box to tick to something people do for themselves. Long-term safety boils down to a culture—a sense that anyone can speak up, correct a slip-up, or ask for backup handling an unfamiliar compound. Personal stories and small reminders keep the message alive better than any rulebook.
Solutions that Work
Regular training, easy access to safety data, and a well-stocked first-aid station form the backbone of any well-run lab or workshop. Introducing checklists for opening, handling, and disposing of copper salts gives everyone a practical reference point, not just lab newcomers. Inviting feedback and sharing close calls around the table keeps everyone sharp. If government rules seem strict or overbearing, those with firsthand experience quickly see that those rules reflect lessons learned in sweat, spilled chemicals, and the occasional trip to the nurse.
Real Risks in Chemistry Labs and Beyond
Copper acetate tetrahydrate shows up as these blue-green crystals on classroom tables and in some industrial formulas. A flashy color doesn’t make it safe, though. My high school chemistry teacher always said, “Treat anything on the shelf like it could harm you.” Turns out, his advice rings especially true here. Swallowing this compound doesn’t just give you an upset stomach—it can actually lead to copper poisoning. The body needs copper in trace amounts, but the jump from helpful to harmful happens much quicker than most folks expect. Excess copper messes with the liver and kidneys. Short-term symptoms can be harsh: vomiting, abdominal pain, diarrhea, and in tough cases, organ damage.
Breathing in copper acetate dust isn’t any better. Workplaces using the compound need good ventilation. Inhaling even small amounts has set off coughing, throat irritation, and headaches for people inside chemical plants. Skin contact comes with trouble too. Handling the crystals without gloves leads to rashes or even a shiny green stain on your hands. That’s the copper ions, reacting with your sweat—already a sign you’re getting exposed.
Hazards for Home, School, and Environment
The eyes of kids light up when those copper acetate crystals appear in science class projects. They look edible, even a little like candy. Here’s the hard truth: small kids can mistake them for treats and end up in the ER. Safety education falls short if teachers and parents don’t make the dangers clear. Mixing up chemical storage with regular cabinet space at home or school brings predictable, preventable accidents.
In the backyard or garden, copper acetate appears in some fungicide mixes. People run into trouble by mixing up hobby chemicals without reading the fine print on warning labels. Plants and soil absorb extra copper, and too much stunts roots and harms worms and insects. Runoff leaches into streams where fish and other life choke on the overload. In my neighborhood, the local pond had a fish die-off tied to hobbyists pouring the wrong leftover chemical solution down the drain. A minor spill on a Saturday can ripple through the food chain by Tuesday.
Facts, Oversight, and Better Safety
The United States Environmental Protection Agency sets a maximum contaminant level for copper in drinking water at 1.3 milligrams per liter for a reason. The U.S. Centers for Disease Control and Prevention backs up tight controls on copper acetate in workplaces as well. Accidents and health issues spike when these limits aren’t respected. People using copper acetate should never go without gloves, goggles, and good airflow.
Calling copper acetate tetrahydrate ‘mildly toxic’ misses the point. It's easy to underestimate a chemical that seems common or is part of a home chemistry kit. Protecting kids, pets, and the planet needs less complacency and more habit-building: label everything, clean up without shortcuts, get rid of leftovers responsibly, and keep any chemical crystal away from mouths and little hands.
Supplying clear warnings and requiring real training for teachers, small farmers, and home users will close a gap that regulations alone can't bridge. Companies that produce and package copper acetate can print hazard symbols and better storage instruction right on the box. Curiosity drives learning, but safety locks in the lesson for life.
| Names | |
| Preferred IUPAC name | copper(II) acetate tetrahydrate |
| Other names |
Cupric acetate tetrahydrate
Copper(II) acetate tetrahydrate Acetic acid, copper(2+) salt, tetrahydrate Cu(CH3COO)2·4H2O |
| Pronunciation | /ˈkɒp.ər əˈsiː.teɪt ˌtɛtrəˈhaɪ.dreɪt/ |
| Identifiers | |
| CAS Number | 6046-93-1 |
| Beilstein Reference | 358672 |
| ChEBI | CHEBI:35206 |
| ChEMBL | CHEMBL250483 |
| ChemSpider | 61362 |
| DrugBank | DB09456 |
| ECHA InfoCard | ECHA InfoCard: 100.013.797 |
| EC Number | 204-935-2 |
| Gmelin Reference | 16467 |
| KEGG | C00528 |
| MeSH | D003995 |
| PubChem CID | 3034426 |
| RTECS number | AH5950000 |
| UNII | U83H6O4A2Y |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | dtxsid7024460 |
| Properties | |
| Chemical formula | Cu(C2H3O2)2·4H2O |
| Molar mass | 249.68 g/mol |
| Appearance | Blue-green crystalline solid |
| Odor | Odorless |
| Density | 1.884 g/cm³ |
| Solubility in water | 72 g/L (20 °C) |
| log P | -2.6 |
| Acidity (pKa) | 4.75 |
| Basicity (pKb) | 7.96 |
| Magnetic susceptibility (χ) | −0.95×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.544 |
| Viscosity | Viscous |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 209.9 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | −1748.2 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -1164.8 kJ/mol |
| Pharmacology | |
| ATC code | A12CX |
| Hazards | |
| Main hazards | May cause respiratory irritation. Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. Toxic to aquatic life with long lasting effects. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | Hazard statements: H302, H315, H319, H332, H410 |
| Precautionary statements | Precautionary statements: P264, P270, P273, P301+P312, P330, P391, P501 |
| Lethal dose or concentration | LD50 oral rat 710 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 710 mg/kg |
| NIOSH | WN3500000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Copper Acetate Tetrahydrate: 1 mg/m³ (as Copper, dusts and mists) |
| REL (Recommended) | 35 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Copper(II) sulfate
Copper(II) nitrate Copper(II) chloride Copper(II) carbonate Copper(I) acetate Acetic acid |
