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Cupric Phosphate: A Closer Look at Its Story, Science, and Place in the World
Historical Development
Cupric phosphate entered the scene not by accident, but because people saw potential in copper’s chemistry beyond wires and metal plating. It first hit chemistry texts in the late nineteenth century when researchers started exploring copper’s reactions with various phosphates. Before long, labs and manufacturers realized compounds like cupric phosphate held benefits for agriculture, pigments, and even medicine. Production stayed small for decades since the main value was in copper metal or simple salts. As analytical methods improved, especially in the 1950s and 60s, industries became more serious about complex copper phosphates, leading to broader use in fertilizers and specialty ceramics. Few people outside laboratories paid any attention back then. Still, as applications grew across scientific fields, so did its profile, especially when research on micronutrient deficiencies highlighted copper’s role in plants and animals.
Product Overview
Cupric phosphate stands as an inorganic compound featuring copper in its +2 oxidation state bound to phosphate ions. Most commonly, it shows up as a blue-green powder or crystalline solid, sometimes going unnoticed among a shelf of other transition metal salts. Its solubility in water remains low, making it suitable for slow-release applications rather than quick-dissolving treatments. Some manufacturers prefer to deliver it as a hydrated form to aid in handling, but the anhydrous version gets used for more specialized chemistry. Its color—ranging from a greenish-blue in crystalline form—stems from copper’s d-d electronic transitions, which is why similar hues appear in copper minerals. Consistency in particle size and composition determines how well it performs in industrial settings. In the market, the compound travels under several trade names, though savvy buyers keep an eye on chemical purity, hydration state, and packing standards more than on the label design.
Physical & Chemical Properties
The scientific community knows cupric phosphate by its formula Cu3(PO4)2. As a solid, it carries a density around 4 g/cm³, enough to settle quickly in a beaker. Heat doesn’t phase it much until the temperature crosses above 400°C, when decomposition kicks in, and copper oxides or phosphates take over. It barely dissolves in water—solubility lingers well below a milligram per liter—so it tends to persist in soils unless strong acids enter the mix. Moisture in the air doesn’t break it down, but intense acids, especially nitric or sulfuric types, will chew through its lattice and free up the copper. Under a microscope, characteristic orthorhombic crystals show up, but real-world batches tend to look like fine powder, sometimes clumpy if stored long. In the presence of strong reducing or complexing agents, copper ions leave their phosphate partners behind, showing why this compound sits below copper sulfate on the chemical activity chart.
Technical Specifications & Labeling
Suppliers ship cupric phosphate with tight specifications. Purity counts—a grade hitting above 98% keeps chemical engineers calm. Key technical data includes maximum allowable levels for lead, arsenic, and cadmium, to keep it fit for feed additives or fertilizer use. Moisture content comes next, especially if storage or shipping crosses humid climates. Safety data sheets stick close to regulatory rules, offering info on particle size distribution, pH suspension values, bulk density, and possible contaminants. Labels stay clear—batch numbers, net weight, proper hazard statements, and manufacturing origin, as required by global chemical laws. Customers in Europe or North America expect compliance with REACH and TSCA, and for agriculture or animal feed, extra documentation proves that trace elements won’t push a sample over safe exposure thresholds.
Preparation Method
Typical industrial synthesis of cupric phosphate relies on reacting soluble copper salts—like copper sulfate or copper chloride—with sodium or ammonium phosphate. Two clear solutions go together, forming an immediate blue-green precipitate once mixed. Operators filter out the solid, rinse impurities, and dry either at room temperature or in a low-temperature oven to avoid decomposition. Lab purists sometimes reach for purer reactants, go slow to control crystal size, or dial in pH with buffers, which can mean more time and higher costs. Some older patents describe fusion-based processes where copper oxides react directly with phosphoric acid, mostly for bulk products. For analytical or high-purity needs, repeated washing and crystallization step up the quality, while mass-production just needs to nail the precipitation and separation steps for scale and safety.
Chemical Reactions & Modifications
Cupric phosphate proves itself stubbornly stable under most storage and usage conditions. Strong acids break it down quickly, releasing blue copper ions into solution and forming soluble phosphate salts. In contrast, alkaline conditions barely budge it, but in the presence of complexing agents like EDTA, copper gets chelated and shifts out of the solid phase. Sodium borohydride or other potent reducers will pull copper down to the elemental state, but most industrial users focus on ion-exchange reactions or partial substitution to create mixed-metal phosphates. Thermal treatment above 400°C leads to conversion to copper pyrophosphate and release of water, which suits ceramic and glass applications. For coloring or catalysis, researchers sometimes dope the phosphate lattice with small amounts of other transition metals, shifting chemical behavior and optical properties.
Synonyms & Product Names
A handful of names show up time and again, depending on context. Chemists prefer “copper(II) phosphate” or “cupric phosphate,” which follow the systematic IUPAC style. Agricultural suppliers sometimes add “tribasic copper phosphate” since it can help distinguish from monobasic or dibasic salts. In industrial catalogs, “copper orthophosphate” drops in occasionally, especially when talking about specific crystal forms. Across languages and regions, product codes or catalog numbers mean more than the marketing name, especially when sourcing from multiple countries. Synonyms help buyers avoid confusion, but nothing matters more than the correct chemical formula for ordering and regulatory compliance.
Safety & Operational Standards
Servicing agriculture, industry, and science means keeping safety up-front. Cupric phosphate lands in the moderate hazard zone—it won’t ignite easily, nor does it explode under rough handling. Inhaling fine dust can bring on irritation in the lungs or cause coughing, especially without good ventilation. Chronic overexposure by swallowing can slowly build up copper in the body, potentially causing liver and kidney problems. Workers use gloves, dust masks, and eye protection as a matter of course, keeping material away from food or drink. Storage recommendations suggest tightly sealed containers, out of sunlight, away from strong acids or reducing agents. Regulatory agencies require proper waste disposal in line with local standards—usually as non-hazardous unless mixed with more dangerous chemicals. Safety data sheets guide emergency response if spills or accidental contact happen, and every workplace handling it must keep those files updated.
Application Area
Farming sees most of the bulk demand, with cupric phosphate filling in the copper deficit in soils lacking enough trace metals. Blending it into fertilizers means crops pick up the element at a steady pace, without the quick spike that other copper sources sometimes cause. In the animal nutrition world, feed premixes sometimes get a sprinkle of cupric phosphate to keep livestock healthy, particularly where pasture doesn’t provide enough micronutrients. Pigment manufacturers lean on its blue-green shade for ceramics, glazes, and sometimes glass—though it tends to compete with copper carbonate or oxide, depending on color needs. Specialty metal finishing and electroplating jobs draw on its phosphate group for surface treatments, improving corrosion resistance or prepping metals for more complex coatings. Researchers tap into its stability and slow-release properties for controlled chemical release studies or as a template for making more complicated phosphates.
Research & Development
Recent years brought a steady march of new studies, especially as researchers look for better-controlled micronutrient release in soils and hydroponics. Analytical chemists use high-purity cupric phosphate for calibration and reagent applications. Some work points to medical uses—in wound dressings or antimicrobial surfaces—though copper leaching rates must stay within safe lines. Nanotechnology investigates copper phosphate nanoparticles for catalysis or as starting points for more advanced composites, where the phosphate matrix helps prevent particle growth. Material scientists explore this compound as a way to engineer new ceramic components that withstand heat and chemical attack, while environmental experts see promise in targeted remediation of soils or water through selective precipitation of heavy metals. Academic researchers follow these leads, with patents and papers showing up on a regular basis, each trying to fine-tune what this old mineral salt can accomplish in the modern lab and factory.
Toxicity Research
No one calls cupric phosphate benign, but its toxicology earns it the label “handle with care, not with alarm.” Acute toxicity, measured as LD50 in animal models, falls in the hundreds of milligrams per kilogram, lower for copper-sensitive species but higher than many lead or arsenic compounds. Chronic exposure builds up copper in tissues, so regular medical monitoring comes standard for workers with frequent contact. Environmental fate studies show that it tends to stick tightly to soil particles, rarely leaching unless extreme acidification occurs, lowering risk to water tables under normal use. Still, misuse poses serious risk—high application rates can harm both crops and beneficial soil bacteria. Ongoing animal feed research monitors absorption rates, bioavailability, and copper levels in milk, meat, or eggs, since trace element overload shows up strongest in sensitive livestock. Regulatory limits rest comfortably below any dose that might cause trouble, but safety in practice depends on careful sticking to recommended use patterns and workplace hygiene rules.
Future Prospects
Rising demand for sustainable agriculture and green chemistry drives discussions about cupric phosphate’s future. As copper deficiency in soils grows in certain regions, especially where intensive cropping or erosion depletes minerals, targeted use of slow-release copper salts looks better than ever. Research into microencapsulation may soon yield smarter fertilizers, where the copper phosphate core stays protected until roots draw near. In the world of advanced ceramics, improved control over particle size and purity could give the electronics industry new tools for making heat-resistant components. The hunt for low-cost antimicrobial coatings pushes attention toward phosphate compounds, given their balance of stability and bioactivity. At the intersection of environmental remediation and nanotechnology, one can imagine designers using this material to filter or immobilize toxic metals in contaminated sites. Regulatory shifts will likely keep tightening quality and safety standards, yet the basic utility of copper phosphate—feeding soils, designing pigments, and crafting new materials—keeps it relevant across old and new industries.
Seeing Cupric Phosphate Beyond Its Formula
It’s easy to hear the words “cupric phosphate” and picture some mystery blue powder sitting on a laboratory shelf, far removed from the everyday world. In reality, this compound serves several practical purposes, weaving itself through agriculture, health care, and research. I remember being surprised just how widely a substance like this could reach when I saw it pop up on a fertilizer label in a rural supply store, miles away from any chemistry lab.
Feeding Plants What They Need
No farmer wants crops turning yellow from lack of nutrition. Soil can lose its natural reserves of copper over time, especially after years of harvesting row crops. This is where cupric phosphate steps in. It delivers copper, which corn, wheat, and other plants need for healthy growth. Without it, you see stunted plants and reduced yields. I’ve seen growers check their fields after a bad harvest, scratching their heads, only to discover the soil’s micronutrients have run dangerously low. Adding cupric phosphate as part of a balanced fertilizer blend brings copper back into the soil, supporting enzyme activity and the synthesis of chlorophyll—the pigment that keeps plants green and growing.
Nutrition and Health Applications
Cupric phosphate doesn’t just help crops. Pharmaceutical companies use it to create mineral supplements. Copper matters for people, too—our bodies rely on it for forming red blood cells and keeping nerves healthy. Supplements containing copper get prescribed to folks with diagnosed deficiencies, and cupric phosphate often acts as the source. Still, copper can’t be treated lightly. Too much can become toxic, so supplements always follow clear dosing guidelines. It shows why accurate formulation in laboratories matters, both for the safety of patients and public confidence in medicine. Researchers continue to look for better delivery methods and more natural ways to rebalance deficiencies without risk.
Research in Chemical Labs
Walk into a chemistry lab at any research university, and you’ll probably find cupric phosphate among the reagents. Its predictable behavior makes it helpful for testing reactions involving copper ions. Scientists use it to grow crystals for structural studies that help us understand everything from simple salts to complex proteins. I remember a classmate spending weeks coaxing the perfect blue-green crystal out of solution to map the shape of a new compound. Discoveries in these areas eventually spill out to manufacturing new materials, electronic devices, and medicines. Lab work can be slow, but without building blocks like cupric phosphate, progress would grind to a halt.
The Reality of Safe Handling
There’s no escaping the risks of chemical contact in industrial and agricultural settings. Handling cupric phosphate requires attention to storage, dust control, and disposal, much like any mineral supplement or fertilizer. Improper disposal can load soils and waterways with unwanted copper, impacting fish and wildlife. The answer isn’t to ban such materials: it’s to treat them with respect, training staff and using proven safety protocols. Regulatory oversight and regular audits help keep both workers and the surrounding environment protected, pairing human benefit with responsible use. The more companies share their practices and monitoring data, the more public trust they earn.
Why Cupric Phosphate Matters in Chemistry and Life
Science class never taught me shortcuts. Chemistry, for one, liked to test patience and attention to detail. Copper compounds, especially the one called cupric phosphate, come up more often than people guess. Its chemical formula, Cu3(PO4)2, comes from knowing that “cupric” means copper in the +2 oxidation state. Combine three copper ions (Cu2+) with two phosphate ions (PO43-) and the charges balance out.
Behind the Formula: Real Uses and Why They Matter
On paper, Cu3(PO4)2 just looks like a cluster of letters and numbers. In industry and research, this stuff matters. Farms sometimes use copper-based compounds, though mostly in small amounts, to fend off mold and fungus. If soil leans toward deficiency, plants benefit from micronutrients like copper and phosphorus. A fertilizer containing cupric phosphate tackles both problems at once.
I remember visiting a vineyard where mildew threatened entire rows of grapes. The field manager pulled out a bag of a blue-green powder and explained that copper-based mixtures saved many seasons. He mentioned keeping an eye on the dose; too much copper can harm not only plants but also the people and wildlife downstream. This matters most in agriculture-heavy regions, especially near fragile water supplies.
Environmental Concerns and Human Exposure
Phosphates and copper, while essential in small portions, stack up if mismanaged. Some rivers show traces of both, especially near old mining zones or farm runoff points. While washing off the land, these minerals gather in water—sometimes leading to unexpected algae blooms or shifts in aquatic life. Scientists connect excess phosphate and copper together in discussions about responsible waste treatment and sustainable farming.
The Environmental Protection Agency tracks these substances for good reason. According to EPA publications, small traces pose little danger, but higher levels have been linked to problems for aquatic life. In people, high doses of copper cause stomachaches, or worse, if ingested chronically. That's why industries watch discharge and treatment so closely.
Solutions: Science, Policy, and Better Practices
Solving these issues means connecting scientists, farmers, and policymakers. On the ground, switching from broad copper spraying to smarter, targeted application has already dropped chemical loads in sensitive areas. Water treatment facilities now filter better for both metals and phosphorus. Some universities run community projects, teaching home gardeners and small-scale farmers about using copper compounds only as needed, and always reading the label.
Lab research on sustainable substitutes shows promise. By exploring biological controls for fungi, more farms might step away from routine copper compounds. Phosphate recovery from wastewater also grows each year, promising reductions in river overloading. Solutions begin with understanding what Cu3(PO4)2 brings to the table and treating it with the respect—not suspicion—it deserves.
Looking Through the Basics
Cupric phosphate, with its blue-green appearance, turns up in fertilizers, animal feed, and the paint industry. Many folks never hear about it outside of textbooks and safety datasheets. Even so, as cities expand and industries crank out more products, new chemicals keep ending up around workplaces, communities, and sometimes food. Ordinary people, not just chemists, deserve to know what’s drifting into their air, soil, and water.
Understanding the Risks
Safety starts with understanding what cupric phosphate really brings to the table. The compound holds copper in its +2 oxidation state, making the copper ion its most important feature. Copper is essential for health—as a trace mineral, it supports enzymes and keeps nerves working. But like salt or iron, too much copper causes real harm.
If you ever worked near copper-rich chemicals, you know about the tight protocols for storage and cleanup. Breathing in copper dust can irritate the lungs. Swallowing high doses leads to nausea, vomiting, and even liver or kidney damage. There’s no getting around it: cupric phosphate means copper exposure, and with enough contact, toxicity shows up in the organs that handle waste and filtration.
Hazard Profiles and Real-Life Incidents
Toxicologists have studied copper to death—decades of work in labs and farm fields. The US EPA sets clear limits: for copper in drinking water, it’s 1.3 milligrams per liter. Anything above that, and pipes start to leach, or heavy use of copper-based pesticides gets questioned. Occupational limits, such as OSHA’s guidelines, push for keeping things below 1 milligram per cubic meter of air. People ignore those rules at their own peril: documented cases exist where industrial spills or mishandled fertilizers led to poisoned livestock and burned crops.
Stories from farm workers sometimes reveal more than any scientific paper: headaches and metallic taste after a spill, skin rashes from splashes, more fatigue than normal. Chronic exposure never has just a simple outcome—sometimes copper accumulates in the liver, slowly raising the risk of long-term illness. News from some Asian countries even links dumping of copper compounds to river pollution, destroying fish stocks and ruining local water supplies.
Common Sense Steps and Solutions
No magic fix solves the risks from cupric phosphate. Proper training for workers means fewer health problems. Gloves, masks, and good ventilation go a long way—neglecting these often leads to trouble. Spill kits and emergency eyewash stations need to stay in working order, not stuck in the corner. Small businesses sometimes cut corners; regular inspections and government oversight keep everyone honest.
On the environmental side, storing and disposing of wastes away from water sources makes a difference. Containment measures stop run-off and protect farms and wild areas. Farmers who stick with good practices—measuring and timing applications, safeguarding storage tanks—see fewer losses and sick animals.
Ordinary people can check water quality reports and ask questions about field applications nearby. Local advocacy has forced companies to change their ways more than once. Each step stacks up; no one wins by ignoring potential hazards, and communities do better when everyone looks out for each other.
Understanding the Real Risks
Cupric phosphate doesn’t show up in headlines or get much attention in daily conversation, but walk into any lab, supply closet, or warehouse dealing with chemicals, and it’s there. It’s a blue-green powder that helps in agriculture, electroplating, and a few other special corners of industry. This compound isn’t the most dangerous item sitting on a shelf, but taking its storage lightly opens the door to problems no one wants to deal with.
Moisture, Air, and Safety: What Counts Most
Experience working with various salts has shown me that moisture changes everything. Cupric phosphate, left out in the open, tends to clump or even degrade because it readily absorbs water from air. Humidity in the room leads to sticky messes and trouble with weighing or transferring. If you keep this powder in a sealed, air-tight plastic or glass container, you dodge all these headaches. No need for fancy or custom solutions; good, clean containers with lids that actually seal do the trick.
Don’t ignore temperature either. Shelves in air-conditioned storage stay cooler, with less fluctuation in humidity. I once watched a batch spoil slowly in a sunlit storage room, just because the jar sat near a hot window. Cool and dry spaces help preserve not just the chemical itself but all the work built around it.
Labeling and Organization: Not Just Red Tape
Sloppy labeling always spells trouble. Sharpie scrawled on masking tape wears off, lids get swapped, and powder ends up in the wrong spot. Clear, printed labels with the chemical name, date received, and hazard notes keep everyone safe. I’ve seen confusion in community labs where similar-looking jars got mixed up, leading to near-misses with disposal procedures. Keeping cupric phosphate labeled and separate from incompatible materials fits right into basic lab hygiene. Anyone could walk in, do a quick check, and tell what’s what.
Fire, Leaks, and What Happens When Things Go Wrong
While cupric phosphate doesn’t burn, some materials stored nearby might. If fire sweeps through a store room, chemicals react in ways that surprise even veterans. Always keep this powder far from combustibles—rags, paper, and volatile solvents. One mishap years ago taught me never to keep flammable stuff near anything that could add fuel to a fire or release noxious fumes if heated. A small, well-marked secondary tray or bin under the jars catches spills and keeps reactive powders apart. Those simple steps go far to contain a leak you don’t see coming.
The Law Isn’t Just Bureaucracy
Rules from OSHA and local organizations often seem like overkill, but most were written in response to accidents. Regular audits of storage fit right into responsible handling. It’s tempting to cut corners—skip an inventory check or leave a lid loose on a busy day—but those small slip-ups stack up fast. In my own experience, accidents rarely stem from one huge mistake; trouble usually sneaks in through everyday neglect.
Share Knowledge, Build Safer Habits
Don’t stash chemistry knowledge behind closed doors. At one workplace, short safety trainings on real storage errors kept the whole team alert and ready to stop problems before they start. Treating storage as everyone’s job, not just the manager’s, turns a shelf of powders into something managed, safe, and trouble-free. Cupric phosphate may be forgettable, but good practices around it make any workplace run safer and smoother. Keep it dry, cool, labeled, and away from fire, and never underestimate the value of a clear system everyone can trust.
Appearance Tells a Story
Cupric phosphate grabs your eye with its striking blue-green color. Spend a little time in a chemistry lab, and you start to appreciate just how much a mineral’s shade can signal its makeup. This compound, with the formula Cu3(PO4)2, stands out from bland salts and powders you run into daily. Its fine crystalline texture and powdery form look distinct in a bottle or under the microscope.
Solubility and Why It Matters
Cupric phosphate barely dissolves in water. Pour it into a glass, and it’ll just settle at the bottom. This physical property shapes its usefulness out in the world. Consider fertilizers—farmers value copper, but the challenge lies in delivering it to soil without rapid runoff or loss. Since cupric phosphate doesn’t wash away easily, it sticks around in the soil, sending copper slowly into crops. That’s a bonus for both the grower and the environment. It also resists dissolving in alcohol, limiting its reach to water-based reactions. With strong acids, it breaks down, so in lab settings, phosphoric acid can free up copper ions from this compound during experiments or industrial processes.
Melting and Thermal Holding Power
Raise the heat and cupric phosphate keeps its form up to around 1,000°C. It doesn’t melt under the heat of the average kiln or flame. In practice, this kind of stability proves useful in ceramics and glassmaking. The compound hangs in through firing, surviving temperatures that make other additives break down or flee as gases. This thermal endurance translates to better durability in ceramics—something you’d notice if you work with glazes or specialty glass.
Density Has a Role Too
Scoop up a gram of cupric phosphate and it takes up less space than you’d expect just by glancing at its powder. Its density stands at about 4 g/cm³. Handling it in the lab, you catch this difference. A beaker with a cupric phosphate sample simply feels heavier than one filled with, say, talc or calcium phosphate. For anyone designing a process or packaging for fertilizer blends, paint pigments, or mineral supplements, knowing the heft per volume makes a difference in storage and shipping costs.
Shape and Particle Behavior
Chemical companies often grind cupric phosphate to a fine powder. It clumps if humidity runs high, but for the most part, it flows much like other crystalline salts. Pour it from a jar and it forms tiny pyramids, resisting easy spreading. The shape and size of its crystals can affect how evenly it mixes when added to other powders—an issue for both lab technicians and folks in industrial mixing plants.
Practical Impact and Safer Handling
Cupric phosphate doesn’t give off dust as much as lighter, fluffier powders. Still, it shouldn’t be inhaled or left on hands for long. The color makes spills obvious, so mistakes are easy to spot and clean. With copper compounds, personal experience tells me it’s wise to keep gloves handy and label containers clearly. Skin staining and respiratory irritation aren’t rare if you skip protection. Storage comes down to keeping it dry and sealed, as moisture will change the way it flows and mixes.
Solutions and Applications
Lab and industry workers who understand these physical features get better results. In fertilizer factories, blending cupric phosphate with other ingredients works best if the plant keeps humidity controlled and watches for caking. For pigment makers, understanding its thermal and color stability opens doors to specialty glazes and paints designed for durability and visual impact. Improving packaging—using sealed, dense containers—helps keep shipments safe and minimizes loss. These changes, brought about by watching the way cupric phosphate acts, lead to smarter work and safer outcomes for everyone from chemists to farmers.
| Names | |
| Preferred IUPAC name | copper(II) phosphate |
| Other names |
Copper(II) phosphate
Cupric orthophosphate Copper phosphate |
| Pronunciation | /ˈkjuːprɪk ˈfɒs.feɪt/ |
| Identifiers | |
| CAS Number | 7758-98-7 |
| 3D model (JSmol) | Cu3(PO4)2 |
| Beilstein Reference | 190682 |
| ChEBI | CHEBI:33354 |
| ChEMBL | CHEMBL1201581 |
| ChemSpider | 22205 |
| DrugBank | DB14275 |
| ECHA InfoCard | 03c8f7d2-d5f6-4698-89f7-4b91c5c797b5 |
| EC Number | 231-846-0 |
| Gmelin Reference | 77488 |
| KEGG | C00939 |
| MeSH | D003555 |
| PubChem CID | 24857 |
| RTECS number | GL8575000 |
| UNII | 2P98F3VW3E |
| UN number | 3078 |
| Properties | |
| Chemical formula | Cu3(PO4)2 |
| Molar mass | 380.58 g/mol |
| Appearance | Blue, crystalline powder |
| Odor | Odorless |
| Density | 2.80 g/cm3 |
| Solubility in water | Insoluble |
| log P | -37.86 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 1.8 (pKa₁), 7.2 (pKa₂) |
| Basicity (pKb) | ~5.6 |
| Magnetic susceptibility (χ) | +1160.0e-6 cm³/mol |
| Refractive index (nD) | 1.629 |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 109.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1282 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1607 kJ/mol |
| Pharmacology | |
| ATC code | A12CB02 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and serious eye irritation, may cause respiratory irritation, very toxic to aquatic life with long lasting effects |
| GHS labelling | **GHS07, GHS09** |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H410: Very toxic to aquatic life with long lasting effects. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | Health: 2, Flammability: 0, Instability: 0, Special: - |
| Lethal dose or concentration | LD50 (oral, rat): >5,000 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 207 mg/kg |
| NIOSH | VW0525000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Cupric Phosphate: "1 mg/m3 (as Cu, OSHA) |
| REL (Recommended) | 200 mg Cu/L |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Copper(II) sulfate
Copper(II) chloride Copper(II) carbonate Copper(I) phosphate Iron(III) phosphate |
