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Stories of copper sulfate go back to the days of alchemy and fledgling chemistry. In the past, people used the blue crystals—hydrated copper sulfate—as blue vitriol, a tool for making pigments and fighting fungal blights in vineyards. Centuries saw the transformation of crude extraction methods into precise chemical manufacturing. As advances rolled in, scientists learned to strip away the water, yielding the white, powdery anhydrous form known as copper(II) sulfate anhydrous. It was never a passing obsession; this compound powered early battery research, kept crops healthy, and enabled chemists to push analytic frontiers. Even today, researchers dig through 18th- and 19th-century experiments, searching for techniques that inform modern processes.
Few laboratory staples pull as much weight as anhydrous copper sulfate. This fine, white powder acts both as a drying agent and an analytical tool. Students set eyes on the blue-to-white color change in school, learning the basics of hydration and chemical detection. Factories use it in raw material processing. Agriculture, medicine, and chemistry call on its properties often. Many see it as just another chemical bottle, but anyone with hands-on experience will tell you that those unlabeled powders hold the key to simple, robust tests and countless synthetic reactions.
Anhydrous copper sulfate takes the form of a white or greyish powder. Moisture in the air quickly triggers its signature blue color, signaling the transition to the pentahydrate. The molecular structure, CuSO4, carries a formula weight close to 159.6 g/mol. Not all chemicals react so strongly to water, turning color right before your eyes. That quality makes it perfect for checking moisture, whether in solvents, powders, or air in the lab. At high enough temperatures—beyond 600°C—copper sulfate breaks down further. Moisture, light, and acid all drive changes in this material, so long-term storage needs careful attention.
Every industry values consistency, and copper sulfate shows how a label turns into real-world results. Laboratories source copper sulfate by purity level—analytical grade for critical reactions, industrial grade for large-scale use. Labels do more than show a name; they list CAS numbers (7778-98-7 for anhydrous), impurities, manufacturing date, and storage warnings. Proper containers block humidity, since a cracked lid means ruined powder and failed experiments. On the job, I've seen batches lose their potency within days if stored near steam lines or open-air shelves. The right packaging preserves shelf life and ensures labs can trust what comes from the bottle every time.
Most major producers rely on the direct heating of copper sulfate pentahydrate. They work with rotary kilns, controlled oven heating, or vacuum systems. The key—drive off the five water molecules, but don’t let the sulfate or copper ions break down. Smaller batches for research often go into crucibles, where careful heat application produces a steady color change, signaling the transition to anhydrous form. Impurities or over-heating degrade the yield. Many students get their first lesson in careful heating with copper sulfate, learning that patience and attention beat shortcuts in the lab. Standardization of prep methods remains a focus in industry, since various impurities or incomplete dehydration still plague manufacturers.
Anhydrous copper sulfate quickly reacts with water, picking up five water molecules and turning a brilliant blue. Drop it into solutions with ammonia, and it yields deep blue complexes—a classic test for the presence of copper ions. Acidic or basic solutions lead to precipitates and transformations. In synthetic chemistry, this compound absorbs trace amounts of water from solvents, priming other reactions for success. Understanding these reactions saves a lot of troubleshooting, especially for those of us who’ve wasted hours over poor yields before realizing the drying step failed. Chemists continue to uncover new modifications, using copper sulfate in organic reactions, catalysis, and material science.
Professional circles know anhydrous copper sulfate by several names: Copper(II) sulfate, Cupric sulfate, and copper sulphate anhydrous. The hydrated version often gets called blue vitriol or blue stone. Terminology shifts by region, supplier, and application. Order forms from different countries show variations—something that catches seasoned procurement teams who might receive the wrong product if not careful. Knowing the full slate of synonyms keeps confusion at bay, especially as supply chains stretch across multiple continents.
Safe handling sets experienced technicians apart from newcomers. Anhydrous copper sulfate may look benign, but exposure can irritate eyes and skin, and dust inhalation causes health problems. Safety data sheets demand gloves, goggles, and proper ventilation. Storage needs low humidity, sealed containers, and clear labeling, preventing accidental hydration and mistaken use. Spills cleaned up with care, since fine powder becomes airborne quickly. Accidental mixing with reducing agents or organics may trigger unwanted reactions. Facilities lay out clear protocols for handling, disposal, and training, as regulatory agencies tighten standards with each incident reported.
Copper sulfate's reach spans water purification, electroplating, textile dyeing, animal nutrition, and soil treatment. Laboratories depend on it to detect moisture and trace water content in organic liquids, a step that determines if synthetic reactions succeed or languish. Water treatment plants use copper sulfate to limit algae growth, taking advantage of its toxic effects on certain organisms at controlled doses. In veterinary medicine, it's sometimes added to animal feed as a supplement for copper-deficient livestock. The diversity of applications means supply chains stay robust and researchers constantly look for new areas to employ this trusted compound.
Modern research targets both efficiency and sustainability. Companies experiment with lower-energy dehydration processes, greener production flows, and recycling spent copper sulfate from industrial wastewater. Each time a new analytical method arises, researchers test copper sulfate to see where it fits best. Chemists continue exploring its uses in catalysis, energy storage, and imaging, digging deep to find reactions that benefit from the compound’s unique properties. Programs around the globe share their findings, accelerating breakthroughs that influence industry standards. My own work has shown that rarely does a week pass without someone in the lab reaching for this chemical during moisture analysis or for teaching basic qualitative analysis—proof of its ongoing relevance.
Toxicologists gaze at copper sulfate with caution. Studies reveal harm to aquatic life at concentrations that barely disturb human users. Chronic exposure in mammals links to gastrointestinal, renal, and hepatic effects. Occupational health experts warn against repeated inhalation and skin contact, and who hasn’t heard stories of accidental poisonings during improper storage? Large-scale spills in farms and waterways forced regulators to tighten controls and push for remediation strategies. Recent work investigates copper bioaccumulation, focusing on long-term environmental impact. Researchers explore chelators or alternative treatments for copper sulfate poisoning, aiming to mitigate accidents in agricultural and industrial settings.
Research trends point to new growth areas. Energy storage and advanced batteries harness copper salts for higher capacity and stability. Water treatment grows increasingly dependent on selective biocides, and copper compounds come under review for low-resistant, targeted applications. Catalysis continues to yield surprises, with anhydrous copper sulfate supporting reactions in organic synthesis with fewer side effects and byproducts. Academic research combines old-school chemical intuition with new technologies, optimizing production and minimizing waste. Environmental concerns push green synthesis pathways and advanced recycling. Chemical education leans on copper sulfate as a critical teaching material for the next generation of scientists, making sure the legacy remains alive and evolving.
I still remember my old chemistry classroom—cabinets that smelled of chalk and vinegar, high shelves stacked with bottles covered in dust. One jar, marked “CuSO4 (anhydrous),” held a blue-white powder that never got much attention. Odd, considering how often it turns up in real life. Most people spot blue copper sulfate crystals in garden centers, but the dry, waterless version works hard in labs, on farms, and even in electronics. Its uses might seem obscure, but dig just a little and the list gets long.
Anhydrous copper sulfate stands out as a moisture-hunter in science classes and real-world labs. Sprinkle it on a damp surface and watch the color snap blue; it’s like magic, but it just shows the powder grabbing water molecules. Chemists rely on this trick to check if solvents have dried out properly. Even new graduates keep a dish of it handy, just to spot leaks or mistakes in their reactions. The color change means the chemical does its job instantly, no waiting.
Farmers use anhydrous copper sulfate to help animals grow healthy. Copper keeps cell functions running well in cattle, sheep, and pigs. Some soils miss out on enough copper, which means adding a pinch to animal feed gets recommended by vets or agricultural consultants. If the powder goes directly into animal diets, it gets measured out in tiny amounts—too much can cause real harm. Responsible suppliers test it for purity to make sure heavy metals stay low.
Electronics can’t run on guesswork, and this is where anhydrous copper sulfate comes up again. Manufacturers add it as an electrolyte in batteries and plating baths. The absence of water in the powder keeps the chemistry stable—so every connection stays reliable and free of short circuits. More broadly, copper sulfate works in mining too. It helps separate copper ores using flotation, a process where small tweaks in chemistry mean the difference between profit and waste. I once visited a copper plant as a journalist—the technician showed how a jar of anhydrous copper sulfate shaped giant machines downstream. Each small batch mattered.
Anhydrous copper sulfate helps control fungus and algae in swimming pools, grapevines, and even public ponds. Sprayed on crops, it beats back mildew and root rot. Copper-based fungicides proved effective well before modern chemicals crowded store shelves—and they’re still around because they work. In glassmaking, copper sulfate adds rich blues and greens to bottles and windows. Cleanup crews also use it to remove traces of hazardous materials in industrial spills. In each case, safety depends on following strict guidelines, since copper can build up in soil and water if handled carelessly.
Every use of anhydrous copper sulfate calls for knowledge and care. Whether it goes into animal feed, laboratories, batteries, or fields, supervision and testing keep its benefits ahead of its risks. I’ve seen how one spill or a wrong scoop can create headaches for people and nature. Regular training, better labelling, and smart policies help keep accidents rare. For those of us who seldom think about that faded blue powder, it’s probably a sign that lots of folks are using it safely every day.
Anhydrous copper sulfate doesn’t play games with moisture. It clings to water from the air, shifting color and losing its key chemical property. It doesn’t just absorb a little; left out in a humid lab or storeroom, it pulls in enough water to become mushy and pale blue. Think of it like leaving sugar out in the rain. You need the solid, gray-white granular form for most chemical reactions and industrial processes, as it doesn’t work the same way once hydrated. Most of us learned this the hard way in high school labs, coming back after a weekend to find what looked like blue slush instead of the stuff we needed for our experiment. If you’ve worked in a place with no dedicated dry cabinet, you remember watching your store manager grumble about ruined stock.
Everyone who deals with chemicals understands the rule: keep it dry, keep it shut, keep it labeled. Copper sulfate really drives home why. Always store it in an airtight container. Screw caps beat snap-on lids. Sealing with a rubber gasket or even parafilm helps. Forget cardboard boxes and paper bags—they let in more air than you think. Some folks try double-containment: a plastic bottle sealed tight, kept inside a weatherproof plastic box with some fresh silica gel packs. Silica gel does a great job acting as a backup, hoovering up any stray moisture before copper sulfate does.
Placement matters, too. Shelving near sinks or open windows brings in damp air. A top shelf in a cool, dry storeroom works much better. Metal shelving beats wood, since wood can “breathe” moisture in and let it out slowly. In larger labs or industry, a dry cabinet—dehumidified, temperature-controlled—is gold. Small setups or home labs might use a repurposed old fridge, unplugged, with desiccant inside. Remember to check those silica gel packs every month or two, swapping or recharging them if the color indicator says they’re saturated.
I still recall the faded masking tape labels on glass jars from a volunteer project in an old school storeroom. Nobody could read what was inside unless they opened it. One wrong scoop and you have a mess: copper sulfate contaminating another reagent or the other way around, moisture sneaking in during confusion. Label every container with clear names, dates opened, and hazards. Anhydrous copper sulfate isn’t highly toxic, but you don’t want copper dust blowing onto skin or eyes, so gloves and goggles are standard in my kit.
Most containers in professional settings include hazard and handling symbols. Always check those before opening. A forgotten jar at the back of a shelf might have crystallized shut or broken, so inspect for cracks and leaks, especially in old glass bottles. Everyone benefits from a short refresher now and then, reminding staff and students about these protocols. More than one person has made the rookie mistake of handling copper sulfate with wet gloves, creating small blue stains that take ages to scrub off.
Proper storage isn’t about fancy equipment—just consistent, careful habits. Inventory copper sulfate regularly. Rotate stock, use older material first, and toss anything clumpy or discolored. Keep lids wiped free from residue, since spillover can absorb moisture and “bridge” the seal, ruining the balance inside. Some smaller labs install a humidity meter near their storage to track seasonal changes. If numbers start creeping up, it means time to swap out desiccants or reseal jars.
Storing anhydrous copper sulfate with care means better experiments, fewer ruined supplies, and less cleanup. Most spills and ruined batches trace back to a forgotten open jar, a bad seal, or skipped label. With a little planning, you save money and avoid headaches. Your time stays focused on results, not mishaps.
Anybody who’s handled chemicals in a lab or an industrial site will recognize the bright blue crystals of copper sulfate. The anhydrous form skips the color and comes as a grey-white powder, which gives it a more innocuous appearance. That appearance can be misleading. This is a compound encountered in chemistry classrooms, water treatment plants, and even in agriculture as a fungicide or pesticide. Every bottle carries a warning label for good reason.
Copper sulfate’s toxicity doesn’t hit you with a rotten-egg stench or a dramatic cloud of smoke. It’s sneaky, mostly dangerous by ingestion, inhalation, or through cuts on your skin. Swallowing even relatively small amounts often triggers serious poisoning. The stomach burns, vomiting begins, and diarrhea can follow. In more severe cases, copper sulfate will damage the liver and kidneys, or cause blood problems. The U.S. National Library of Medicine details hospital cases: some folks suffered permanent organ damage. I’ve seen minor accidents leave coworkers with months of stomach issues.
The danger isn’t limited to swallowing. If copper sulfate powder lands on a cut or abrasion, it stings and inflames, and sometimes blisters appear. The eyes feel especially vulnerable—copper sulfate causes immediate pain and damage upon contact. Dust in the air becomes a risk all on its own. Without a mask or proper ventilation, it irritates the nose and throat. Workers sometimes brushed off basic dust protection, only to end up coughing for days. Chronic exposure may tip the scales toward longer-term respiratory troubles.
A spill isn’t just unsightly. Copper sulfate contaminates floors or surfaces and sticks to shoes and tools. Sweeping or improper wiping just tosses the dust airborne, putting it straight into lungs or onto skin. At agricultural sites, runoff sometimes carries it into streams, where it kills off aquatic life in shocking numbers. State fishery boards have published advisories on copper sulfate’s effects: local trout, frogs, and aquatic insects die off long before you see a visible blue tinge to the water.
One of the best things I learned in labs and plant sites comes from experienced foremen: don’t bend rules for simple jobs. Gloves, safety glasses, and a decent dust mask sound like overkill until you watch an ambulance cart someone off for a chemical burn or a lung concern. Handwashing seems obvious, but plenty of cases stem from someone rubbing their eyes or eating a snack without scrubbing their hands first—especially after handling the “safer-looking” anhydrous powder.
Engineering controls like fume hoods, good air circulation, or slurry systems keep dust down. On farms or in municipal treatment plants, bottle labels and safety data sheets help folks recognize the signs of copper poisoning fast. Disposal gets trickier: never wash it down a drain or toss it into regular trash. Local environmental agencies usually run “household hazardous waste” drop-off events. If you work around copper sulfate, or keep it at home for any reason, treating it with respect makes the difference between a handy tool and a serious health hazard.
Blue crystals in a science classroom can grab a student’s attention quicker than most textbooks ever could. Copper sulfate, often recognized by its vivid blue color, plays a key role in many classroom experiments and industrial processes. But not all copper sulfate comes in the same form. Some of it is bright blue and filled with water; some sits crisp, white, and bone-dry. The difference between anhydrous and hydrated copper sulfate isn’t just in the color—there’s a deeper chemical lesson that resonates in real life, too.
Hydrated copper sulfate, usually labeled CuSO4.5H2O, contains water locked into its crystal structure. This isn’t just dampness stuck to the surface. Five water molecules bond right in with the copper sulfate, making it the familiar blue powder or chunk popular among teachers and students. Anhydrous copper sulfate, CuSO4, lacks those water molecules. It forms a stark white powder, nearly unrecognizable compared to its hydrated counterpart.
The real-world difference starts at a glance. Blue versus white reveals if water’s present or not. Chemists often use anhydrous copper sulfate to check for moisture in a solution. Add a pinch of white powder; blue color means water has just latched onto the crystals, making the reaction clear and visual. Lab techs rely on these changes to check for leaks or keep chemicals dry, which can matter for safety and product quality.
Copper sulfate doesn’t only find friends in chemical labs. Farmers mix hydrated copper sulfate into fungicides and algaecides. They spray vineyards and lakes, trusting the reliability of those blue crystals to keep crops and water supplies safe. The hydrated form dissolves more easily, making it ready for spreading or mixing. Its water content does slightly dilute the actual copper sulfate concentration, but the convenience of the blue crystals outweighs this for routine use.
Anhydrous copper sulfate takes a spot in electrical and refrigeration sectors. Its water-absorbing talent is useful when drying solvents or keeping delicate equipment moisture-free. The white powder’s lack of water lets it soak up every stray drop from the air or a solution. If a process fails because of humidity—say changing the physical properties of an industrial product—the humble white powder steps in to save the day.
Safety and storage demand attention here. Hydrated copper sulfate’s extra water means it stores well in regular containers at moderate humidity. The bright blue color warns handlers, as copper sulfate can be toxic if eaten or handled carelessly. Pets and young children see blue powder and might think it’s candy, so it should always stay locked away.
Anhydrous copper sulfate, with its absorbent tendencies, often comes in sealed containers or single-use packets. Exposure to air turns it blue in minutes, so it can’t hang around loosely in a workshop. Workers count on seeing that color change as proof of moisture—but it also means the product needs careful handling and replacement after use.
To avoid waste and contamination, companies make sure to seal up both forms of copper sulfate after each use. Clear instructions and regular training keep users aware of the possible risks. Tech upgrades, like moisture sensors, help reduce reliance on chemical indicators where mistakes could be costly. Copper sulfate does a job that digital tools can now often support, but its visible, reliable reaction keeps it valuable.
Walking through any chemistry class, it’s tough to miss the usual trick: add a bit of water to a white powder, see it flip to blue. That small show is the easiest way to spot anhydrous copper sulfate. This stuff, in its dry state, holds a plain white color, almost chalk-like. The story behind it isn’t just for students, though. In many labs and workplaces, knowing this difference makes real safety and accuracy a lot more likely.
Labs use copper sulfate all the time, for tasks from checking for water in solvents, to teaching students what a chemical reaction looks like. The moment moisture sneaks in, anhydrous copper sulfate turns blue, thanks to water molecules latching onto its structure—hydrated form steps in. The white anhydrous powder doesn’t just give a color trick; it tells you if the kit or solvent you’re handling has moisture leaking in.
Think about the hassle in chemical research if a small batch of anhydrous copper sulfate got swapped with blue crystals. Results swing wide, projects stretch longer, and sometimes small errors lead to bigger worries later down the road. Even outside a lab, farmers using it for fungus control need to know what form they’re working with. One slip-up, and they’re not getting what they paid for—or risks increase in the field.
People use simple ways to check anhydrous copper sulfate. Scoop a spatula tip and sprinkle it on a dry surface, dab on a droplet of clean water, and watch. Blue means it’s the real deal. Heat also tells a story: if you see steam or water vapor and a color shift to white, you just drove away the moisture. In school, watching those steps inspires a lot more than lectures ever could.
At home, chemistry fans sometimes keep a small tub of it (sealed up, of course) to check if household solvents like acetone or ethanol are really water-free. Toss a pinch in—white stays white if all’s dry. It’s good practice and cuts down on mistakes or ruined batches, whether you’re testing for fun or troubleshooting a stubborn project.
Anhydrous copper sulfate won’t wait long in the open air before dragging in moisture. Air-tight containers or desiccators are the real solution. Some add a packet of silica gel, just for good measure. Proper labeling stops mix-ups: once it soaks up water and goes blue, it doesn’t work for moisture detection anymore.
Using a simple compound like anhydrous copper sulfate seems basic, but doing it with care and repeating tests keeps things safe and accurate. Many problems show up in labs and farms when small checks get skipped or ignored. Staying alert for the white powder—not just for a science trick, but for reliable work—can make or break a job.
| Names | |
| Preferred IUPAC name | Copper(II) sulfate |
| Other names |
Copper(II) sulfate anhydrous Cupric sulfate anhydrous CuSO4 Bluestone anhydrous Blue vitriol anhydrous |
| Pronunciation | /ænˈhaɪ.drəs ˈkʌp.ər ˈsʌl.feɪt/ |
| Preferred IUPAC name | Copper(II) sulfate |
| Other names |
Blue Vitriol Bluestone Sulphuric acid copper(II) salt Cupric sulfate anhydrous |
| Pronunciation | /ænˈhaɪ.drəs ˈkʌp.ər ˈsʌl.feɪt/ |
| Identifiers | |
| CAS Number | 7758-98-7 |
| Beilstein Reference | 1821150 |
| ChEBI | CHEBI:76208 |
| ChEMBL | CHEMBL1201466 |
| ChemSpider | 65660 |
| DrugBank | DB09153 |
| ECHA InfoCard | 03d8e3e3-4e42-4a9c-829a-4420441bedd7 |
| EC Number | 231-847-6 |
| Gmelin Reference | 1265 |
| KEGG | C06916 |
| MeSH | D003689 |
| PubChem CID | 24462 |
| RTECS number | GL8900000 |
| UNII | 7M7D50YH80 |
| UN number | UN3077 |
| CAS Number | 7758-98-7 |
| Beilstein Reference | 3588010 |
| ChEBI | CHEBI:23413 |
| ChEMBL | CHEMBL607195 |
| ChemSpider | 202613 |
| DrugBank | DB09153 |
| ECHA InfoCard | 03c678bc-5b31-47b5-8e12-0d4267b3d12b |
| EC Number | 231-847-6 |
| Gmelin Reference | 1424 |
| KEGG | C01847 |
| MeSH | D003637 |
| PubChem CID | 24462 |
| RTECS number | GL8900000 |
| UNII | KD3H49U404 |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | Q180215 |
| Properties | |
| Chemical formula | CuSO4 |
| Molar mass | 159.609 g/mol |
| Appearance | White or grayish-white powder |
| Odor | Odorless |
| Density | 3.6 g/cm³ |
| Solubility in water | 24.4 g/100 mL (20 °C) |
| log P | -1.4 |
| Vapor pressure | Negligible |
| Acidity (pKa) | Approximately 2.0 (for H₂SO₄, the acid formed upon hydration) |
| Magnetic susceptibility (χ) | +53.1·10⁻⁶ cm³/mol |
| Dipole moment | 0 D |
| Chemical formula | CuSO4 |
| Molar mass | 159.609 g/mol |
| Appearance | White powder |
| Odor | Odorless |
| Density | 3.6 g/cm³ |
| Solubility in water | 23.1 g/100 mL (20 °C) |
| log P | -7.62 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 6.0 |
| Magnetic susceptibility (χ) | +53.6 × 10⁻⁶ cm³/mol |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 109.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -769.9 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1561 kJ/mol |
| Std molar entropy (S⦵298) | 109.5 J/(mol·K) |
| Std enthalpy of formation (ΔfH⦵298) | -771 kJ mol⁻¹ |
| Pharmacology | |
| ATC code | V09AA10 |
| ATC code | V09AA05 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes serious eye irritation, may cause respiratory irritation, toxic to aquatic life with long lasting effects |
| GHS labelling | GHS02, GHS07, GHS09 |
| Pictograms | GHS06,GHS09 |
| Signal word | Danger |
| Hazard statements | H302, H315, H319, H410 |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Explosive limits | Non-explosive |
| Lethal dose or concentration | LD50 oral rat 300 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 300 mg/kg |
| NIOSH | WF9400000 |
| PEL (Permissible) | PEL: 1 mg/m³ |
| REL (Recommended) | 10 mg/m3 |
| IDLH (Immediate danger) | 300 mg/m³ |
| Main hazards | Harmful if swallowed, causes severe skin burns and eye damage, may cause respiratory irritation, toxic to aquatic life with long lasting effects |
| GHS labelling | GHS02, GHS07, GHS09 |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. H315: Causes skin irritation. H319: Causes serious eye irritation. H410: Very toxic to aquatic life with long lasting effects. |
| Precautionary statements | P264, P270, P273, P280, P301+P312, P330, P305+P351+P338, P308+P313, P501 |
| NFPA 704 (fire diamond) | **NFPA 704 (fire diamond) for Anhydrous Copper Sulfate:** "2-2-0 |
| Explosive limits | Non-explosive |
| Lethal dose or concentration | LD50 (oral, rat): 300 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 300 mg/kg |
| NIOSH | WN3325000 |
| PEL (Permissible) | PEL: 1 mg/m³ |
| REL (Recommended) | 10 mg/m³ |
| IDLH (Immediate danger) | Cu: 100 mg/m3 |
| Related compounds | |
| Related compounds |
Copper(II) sulfate pentahydrate Copper(II) chloride Copper(II) nitrate Copper(II) carbonate Copper(II) oxide |
| Related compounds |
Copper(II) sulfate pentahydrate Copper(II) oxide Copper(II) chloride Copper(II) nitrate Copper(I) sulfate |
