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People have relied on zinc compounds for thousands of years. Zinc chloride found its way into the world through alchemy and early chemistry labs, though its real moment came with industrialization. In the 19th century, factories demanded new metal treatments and chemical mediators. Zinc chloride caught attention for its ability to cleanse metals, preserve wood, and spark reactions. Chemists learned through soot-stained experiments and handwritten journals, passing techniques from generation to generation until its production reached commercial scale. As technology spread, the compound began appearing everywhere from textiles to the electrode paste in the first dry cells. Zinc chloride didn’t get locked in the past. Its routine roles grew as each decade rolled into the next, keeping the chemical industry ticking and reaching new trades.
Zinc chloride stands out with its white crystalline texture and sharp, biting taste (not recommended for the curious). Unlike its cousins, it feels greasy and clumps easily, taking up moisture from the air. The stuff dissolves quickly in water and alcohol, forming dense, transparent solutions. Chemists and manufacturers rely on bulk powder and granular forms, while researchers often work with laboratory-grade solutions. Labels often mention purity levels, target applications, and whether any stabilizers have been blended in. Whatever the form, most sellers promise a corrosive edge—just the thing industries look for in a salt that pushes boundaries.
This compound delivers a molecular weight near 136.3 g/mol, and its melting point hovers close to 290°C. It boils beyond 730°C, but way before that, you’ll see heavy fuming as it breaks down in air. You can melt it in a well-controlled lab furnace, but most plants never push the heat that far. Zinc chloride dissolves in water at rates exceeding 400g per 100ml (room temperature), making syrupy solutions that leach through wood, paper, or cloth. In high humidity, even sealed containers cake up thanks to its hygroscopic punch. The anhydrous powder releases hydrogen chloride when it meets water, so don’t breathe in that wake. Chemists lean on its high acidity and reactivity to shift molecules around or strip away stubborn compounds.
Industrial packages usually carry specifications for purity—often above 98% for technical grade, upticks for analytical grade, and sometimes stricter controls on heavy metals or mercury. Labels must show batch numbers, net weight, hazard symbols, and recommended storage protocols. Regulatory guidelines, such as the United Nations’ GHS and Europe’s REACH, have shaped labeling practices. Material Safety Data Sheets ride along with every shipment, warning about corrosive risks, storage away from moisture, and the danger of skin or eye contact. In my experience, confusion rarely comes from the chemical itself—mistakes come from ignoring the paperwork or from workers skipping gloves and goggles.
Making zinc chloride starts with raw metallic zinc and hydrochloric acid. Emptied under a fume hood, this union fizzes up hydrogen and leaves the salt behind. Factories recycle, condense, and dry out the resultant mixtures, filtering out unwanted metals or sulfur. Smaller labs sometimes take the simple route—just dunk zinc turnings in acid and evaporate the liquid away. Some high-purity versions grow from zinc oxide and ammonium chloride, skipping the risks of bubbling hydrogen. Purified products often need repeated crystallization and washing to remove any gritty residue or colored impurities. This long-standing process hasn’t shifted much since the late 1800s, though today’s mills use better automation, larger tanks, and stricter effluent controls.
Zinc chloride brings versatility to any lab bench. It acts as a Lewis acid, ready to grab lone electron pairs and rearrange molecules. Mix it with organic halides and see catalysts roar to life; toss it into cellulose pulp, and it swells the fibers for chemical treatment. Drop it into rubber compounding, and crosslinking gets a jolt. In water, zinc chloride hydrolyzes to form hydrates, releasing heat and leaving a trail of acidic solution. Add strong bases, and zinc hydroxide falls out as a fluffy white precipitate—handy for further refinement. Engineers sometimes tweak the chemical by pairing it with ammonium or sodium salts, slipping it into new roles or stabilizing for specific tasks. The fierce reactivity means tight protocols during transport and handling.
Zinc chloride hides behind many names, both scientific and commercial. Chemists shorten it to ZnCl2 in equations. You might spot “zinc dichloride” or simply “butter of zinc” in older literature. Trade suppliers sometimes blend it into “acid zinc flux” or “tinning solution,” especially for metalwork. Other downstream products might list anhydrous zinc chloride or its dihydrate, depending on the water content. Some specialty brands wrap the key ingredient in flame-retardant blends, textile finishes, or wood preservatives under specific brand names, never mentioning zinc chloride until you read the fine print. Knowing all the synonyms and product identities helps avoid mix-ups—especially in busy procurement offices.
No point sugarcoating it: zinc chloride delivers serious hazards if handled wrong. Skin contact causes chemical burns. Breathing dust or fumes can scar airways and ruin a day’s work—or worse. Safety teams set up ventilation hoods, order the right gloves (nitrile or neoprene, never cheap latex), and maintain eyewash stations close to the work zone. Workers train relentlessly, reading every Material Safety Data Sheet before opening new bags. Storage must mean dry zones far from food, acids, or incompatible chemicals. Spills need containment with proper neutralizers and prompt clean-up routines, since water triggers a caustic burst. Shipping cartons show hazard diamonds, restricted weights, and emergency contact numbers. These aren’t paperwork drills. Just one slip in a warehouse or lab can ruin years of clean safety records and, more importantly, cost someone their health.
Over the years, zinc chloride has worn many hats across industries. Galvanizers dab it on metals before coating to clean rust and scale. Woodworkers soak fenceposts to keep termites and fungi in check, though environmental rules have restricted some uses. In textile mills, ZnCl2 swells fibers ahead of mercerization or dyes, unlocking vibrant colors and improved textures. Energizer and Duracell once depended on zinc chloride for dry cell batteries—modern lithium types have taken over, but legacy flashlights still use the old zinc-carbon recipe. Water treatment teams add it to control fouling on heat exchangers and industrial pipes, though concerns about pollution force careful dosing and treatment.
Laboratories trust zinc chloride’s catalytic punch to streamline organic reactions, especially those that build carbon rings or swap chlorine atoms. In the world of rubber, it crosslinks polymers for flexible, durable sheets. Artists and crafters sometimes use zinc chloride in etching and engraving metals, opening patterns for jewelry or printmaking. Fireproofing specialists tout zinc chloride as part of old-school formulas for treated fabrics or lumber. Each use brings benefits, but the push for greener methods always hovers overhead—no company wants a dangerous legacy tied to obsolete chemistry.
Modern research chases new possibilities for zinc chloride. Scientists look at ways to recycle post-industrial solutions, recover valuable metals, or neutralize spent chemicals with less waste. Polymer chemists find fresh uses for zinc chloride in making biodegradable plastics and smart coatings. Some teams probe its value as a precursor for thin-film zinc oxide layers, used in solar cell manufacturing. Environmental researchers assess whether careful use in water treatment can extend the life of industrial equipment without leaching too much into ecosystems. Academic papers break new ground every year, often using computational modeling to predict reactivity and optimize yields.
This progress builds on experience from decades of trial and error. During my years in chemical supply, I watched customers request new grades of ZnCl2—from high-purity for microelectronics to robust, stable formulas that resist breakdown in high-moisture settings. No surprise, research directions follow the money: safer, greener, and more efficient versions win market share. Lab managers also look for quick, reliable diagnostic tests to check ZnCl2 strength and contamination levels, since process hiccups can shut down production lines.
Despite its usefulness, zinc chloride raises old worries about toxicity. On contact or inhalation, it damages tissues—exposure limits must get tight monitoring, especially in plants without automated handling. Medical journals track cases of acute poisoning, often accidental or due to poor ventilation. Long-term chronic exposure, even at low levels, can lead to respiratory illnesses, headaches, and metal fume fever, particularly risky for welders and industrial workers.
Wildlife studies add to the concern, as high discharge levels from untreated sites disrupt aquatic ecosystems, knock out beneficial microbes, and compromise water supplies. Toxicologists and environmental agencies use these findings to set strict discharge permits, workplace exposure limits, and remediation guidelines. My own aisle-walking in factories taught me that safety training, up-to-date PPE supplies, and air monitoring split safe shops from horror stories. Regulatory scrutiny keeps climbing, and ongoing research explores antidotes, chelators, and alternative compounds that could deliver similar performance with less risk.
Zinc chloride will keep moving forward, though its road isn’t simple. Modern industry wants chemicals that punch hard, pose fewer health risks, and break down cleanly once their work’s done. Innovation means exploring hybrid products—blends with organic salts, new catalysts, or safer delivery methods—that keep the core benefits while lowering hazards. Some battery makers revisit zinc chemistry, trying to squeeze more volts and cycles from time-tested cells. In construction, there’s hope for zinc chloride as a fireproofing or anti-corrosive agent with a smaller environmental footprint.
Environmental policy shifts could lead to phaseouts in areas where safer alternatives emerge. As a result, the chemical manufacturing world invests in process overhaul, raw materials tracing, and recycling programs that recover both zinc and chlorine from spent solutions. Academic groups highlight greener syntheses, such as processes that skip highly toxic reagents or recycle side-streams internally. New research on nanomaterials, coatings, and rapid diagnostics brings a bright edge to an old compound. From my seat, those on the frontlines—plant operators, researchers, safety pros—will shape the next chapter through persistent curiosity, relentless safety focus, and a willingness to adapt as challenges and science keep growing.
I’ve noticed certain chemicals pop up in places you wouldn’t expect. Zinc chloride is one of those. It’s a white, water-soluble salt that shows up quietly in factories, water treatment plants, and even the dentistry world. Most folks have no idea how it shapes products and processes behind the scenes, but anyone working around metalwork, electronics, or adhesives understands its reach.
I remember touring a hardware plant not long ago. Steel wire and sheet metal moved through liquid zinc chloride baths. The stuff strips away corrosion and oxide buildup, setting the stage for galvanized coatings to stick. Without this step, rust wins every time. Wire, nuts, and bolts fresh from zinc chloride treatment last years longer outdoors. When you look at a chain-link fence or a farm gate, think about how a simple chemical makes it stand up to rain and mud.
Zinc chloride forms a key part in old-school dry cell batteries—the kind you find in flashlights and remote controls. It’s the electrolyte enabling current to flow smoothly from one end to the other. The world’s not finished with AA and AAA batteries yet. In places with spotty electricity, they keep lights and radios running. In small electronics repair, I’ve pulled apart cheap batteries and found zinc chloride paste mixed inside.
Tap water quality isn’t something to take for granted. Factories rely on zinc chloride solutions to purify wastewater before it leaves the site. The compound binds to sludge and particles, pulling them together so they can be removed. Less sediment and fewer heavy metals end up in rivers. I’ve met engineers who inspect city water plants, and zinc chloride sits right on their chemical shelf alongside chlorine and alum. Cleaner water flows out to homes thanks in part to the work zinc chloride puts in behind the curtain.
Clothing manufacturers reach for zinc chloride during the dyeing process. It helps fibers soak up color evenly. As a result, that blue workshirt on your back keeps its color after months of wear. Paper mills have another use—the chemical strengthens sheets and boosts resistance to mold. Packaging stays firmer, meaning fruit, electronics, and medicine get a safer ride to customers. I’ve handled paper with and without these treatments. Treated stuff just feels tougher.
Zinc chloride’s glue-making talents surprised me first time I checked an old tube of multipurpose adhesive. It reacts with protein and cellulose, which tightens up bonds in plywood and pressed board. Soldering cabinets and electronics rely on good flux, and zinc chloride does the heavy lifting to keep metal surfaces clean so solder can stick. In carpentry and small electronics repair, proper joints hinge on this. There’s even a role in wood preservation—treated timbers push back hard against rot and termites in damp climates.
No commentary on zinc chloride should skip safety. Exposure to its solutions can irritate skin and eyes. In industry, gloves, eye shields, and well-ventilated spaces protect workers. On a broader scale, chemical recycling and better handling routines can shrink its environmental impact. Promoting education on safe use, along with development of less hazardous alternatives where possible, will keep both workers and the environment healthier in decades to come.
Zinc chloride pops up in more places than most realize. Factories depend on it for making batteries, galvanizing steel, and cleaning metal surfaces. It also shows up in some wood preservatives, textile processing, and even a few medical applications. At first glance, it appears to be just another useful chemical. But the question comes up often: Is it toxic? Does it pose a hazard to people or the environment?
Working in labs and around industrial settings, I watched experienced staff treat zinc chloride with respect. They wore gloves, goggles, and made sure there was enough ventilation. Most safety data sheets mention it causes burns and irritation if it gets on skin or splashes in eyes. Breathing in dust or fumes can also be risky. That didn’t feel like something to brush off.
Zinc chloride, when dry, acts as a strong irritant. If the dust gets into your nose or lungs, it causes coughing, shortness of breath, and a burning feeling. Inhaling larger amounts can sometimes bring on serious lung problems, even fluid buildup in the lungs—doctors call it pulmonary edema. Swallowing even a small dose leads to stomach pain, nausea, vomiting, and mouth or throat burns. The CDC flags zinc chloride as a corrosive material and urges caution in all settings.
Touching this compound isn’t a casual affair, either. On the skin, it causes redness and blisters. In the eyes, it brings pain and even damage to vision. Reports from poison centers point out that kids sometimes get into zinc chloride batteries; those cases often land someone in the ER.
Companies often drain water used in processes containing zinc chloride. Too much zinc disrupts aquatic life, harming fish and smaller critters long before it changes the taste or look of water for humans. Waste handling guidelines urge proper treatment before anything leaves a factory. Most regulations expect companies to keep levels well below thresholds set by local and international agencies.
Looking at scientific reports, the toxic dose varies based on exposure. Skin contact with solutions greater than 10% brings a high risk for burns, according to the European Chemicals Agency. Inhalation at levels around 1 mg/m³ requires action, as recommended by occupational health standards. Most workplaces handling this compound monitor air and surfaces daily. It isn’t the kind of chemical to keep in an open container or toss down the drain.
Training and equipment save lives with zinc chloride. Simple steps like wearing long sleeves and safety goggles make a difference. Using fume hoods means fewer fumes end up in someone’s lungs. Products at home—like batteries or wood preservatives—should stay out of reach of kids. Anyone handling larger amounts should always read the label, check for updated safety advice, and call in professionals for spills.
Companies using zinc chloride often look for less hazardous options or work on better containment methods. Regulatory oversight sometimes drives improvements, but worker experience shapes routines on the ground. Newer research into alternative chemicals continues, but so far, demand for zinc chloride keeps it a staple in industry. People working around it can demand clear labels, safety training, and routine monitoring.
Treating zinc chloride with respect comes down to awareness and practical steps. The risks aren’t just paperwork—they land in real emergency rooms and make a difference in health statistics. Using it safely protects not just workers, but whole communities downstream of factories. My own experience, and those of others I’ve worked with, points to one universal fact: educated caution offers the best protection.
Zinc chloride shows up in plenty of workplaces, from metal finishing to water treatment plants. It cleans, it reacts, it gets work done. Still, behind all that chemical usefulness sits a risk: this stuff can burn your skin, tear up your lungs, and bite through clothes. I’ve handled it in a lab, and a simple splash on a glove can leave a world of trouble. Getting smart about storage comes down to protecting people, the building, and your own peace of mind.
Strong, tight seals make the difference. I’ve seen careless choices—old bottles with loose lids, leaky sacks gathering powder on the floor. Zinc chloride draws moisture out of the air fast, then turns into an acid that eats through metal and leaves burn marks. Solid containers crafted out of glass, heavy-duty plastic, or lined metal will keep it stable. Check the seal before every use. A split cap or even a grime-clogged thread puts everybody at risk of fumes or sticky messes. Never pour leftover zinc chloride into some unlabeled jar; clear labeling and original packaging prove their worth whenever accidents happen or newcomers take over your shift.
Keep it cool, dry, and away from the common aisle. A shelf near a window or under a heater pretty much invites clumping and pressure. I’ve seen expensive product turn solid overnight because the storage room ran humid and hot. Store zinc chloride on a shelf below shoulder height to cut down on drops and spills. Everything nearby should shrug off a spill—ceramic tile, thick paint, not old wood or carpet. Always keep it away from direct sources of water: leaks, mops, and buckets invite dangerous reactions.
Zinc chloride does not play well with water, strong bases like ammonia or caustic soda, or combustible organic stuff. Mixing these creates heat, hazardous fumes, or even a fire. Place it on a shelf away from acids and cleaners—this saves time arguing over whose fault it was when bottles corrode and labels vanish.
Good storage only pays off if everyone knows the rules. Anyone pulling zinc chloride off a shelf ought to have access to gloves, goggles, and coats. Working with it should happen under an exhaust hood or with plenty of ventilation, not some cramped corner where nobody sees what’s happening. Post clear safety instructions right above the storage area. Regular training keeps the right habits sharp.
Nobody should dump leftover zinc chloride down a drain or tuck it into the regular garbage. Hazardous waste rules don’t just exist for show—local disposal services track, collect, and neutralize this stuff. Every shop needs a drum labeled just for zinc chloride waste. Accidental mixing in the trash leads to emergency cleanup, not just a slap on the wrist.
Even the best systems slip without regular care. Once a month, I look over the shelf, containers, and labels. New labels help when chemicals sit for months untouched. Catch small leaks and stains early, and you won’t ever stumble on a puddle that eats through the floor.
Working with chemicals like zinc chloride takes more than following a rulebook. Every safe decision adds to a chain that protects everyone in the building. Treating storage like common sense, not a chore you dodge after a long day, means everyone leaves work in one piece. Facts say it damages tissue and creates dangerous waste, but disciplined habits and clear storage turn risk into just another part of the job.
Zinc chloride has a simple chemical formula: ZnCl2. This means every unit contains one zinc atom and two chlorine atoms. Scientists have agreed on this formula for more than a century, so there’s little room for debate. The reason this compound matters goes far beyond basic chemistry. Whether you spot it on a label for a battery, find it on a lab shelf, or read about it in a high school textbook, ZnCl2 shows up everywhere zinc’s chemistry crosses paths with the practical world.
Zinc chloride usually shows up as a white, crystalline powder. Sometimes it looks a bit off-white, especially if it’s absorbed moisture from the air. This compound has a reputation for being hygroscopic; it pulls in water from its surroundings and can get sticky if exposed for long. That trait has thrown me for a loop in the lab more than once, turning what I expected to be a nice, free-flowing powder into a clumpy mess. Fresh from a sealed container, though, it catches the light and looks almost pure.
Out in the real world, quick recognition of what zinc chloride looks like becomes crucial on a busy production floor or during quality checks. If you get caught up with some off-color or clumpy material, you can’t just shrug it off and hope for the best. Factories use ZnCl2 in textile processing, adhesives, and batteries. Mistaking a degraded batch for the real deal could mean short circuits, leaky batteries, or poor fabric finishing. It’s not just the folks in white coats who care about a precise formula and a clean product shape—any mistake ripples through to the people handling everyday products.
Zinc chloride’s ability to soak up water presents a challenge, too. Some shipments lose their sharp, crystalline look by the time they reach the factory. Workers have to keep it in airtight containers or toss in special drying agents. You’ll also see teams checking for crustiness or unexpected colors—early signs that a batch got exposed. I’ve seen quality control staff nearly break out in a sweat just worrying about tracking every gram and keeping humidity at bay.
Industry can address problems linked to storage and product purity through better packaging and handling protocols. Storing zinc chloride in thick, sealed drums and avoiding clear plastic bags seems obvious, but you would be surprised how often shortcuts pop up just to save a buck. Sensors that track humidity near storage areas help as an extra line of defense. Training workers to identify unacceptable changes in texture or color pays off. It’s easy to scoff at these checks until one bad batch grinds a process to a halt.
A focus on laboratory-grade purity and proper moisture controls can also reduce contamination and keep unpredictable outcomes to a minimum. Whenever the right practices drop off, costs rack up—extra time, lost product, safety headaches, even disappointed clients. The chemical formula and physical appearance of zinc chloride aren’t just trivia for nerds. They shape the quality and performance of products and influence every hand that touches this material from mine to market shelf.
Zinc chloride isn’t a product you just toss in a box and forget. It can be corrosive, especially in certain forms. So, companies rely on sturdy, lined drums—usually made from steel with a tight-sealing lid—for the bulk of their shipments. For folks moving enormous volumes, there’s the option of intermediate bulk containers (IBCs). These are those familiar, heavy-plastic cubes framed in metal you’ve seen on trucks or factory lots. For smaller quantities, plastic pails do the trick. Wrapping up a chemical like zinc chloride in proper packaging isn't just smart—it’s the law. Regulatory folks keep close tabs on these shipments since leaks or spills can harm handlers, truck drivers, and the environment.
Take it from someone who’s helped unload shipments at a small manufacturing shop: sloppy packing can ruin your week. One time, the supplier didn’t seal their drum tightly and, by the time it reached us, we had a sticky, white mess on the floor. Beyond the hassle, spills like these cost money and put people at risk. Zinc chloride can burn skin and eyes, so workers expect solid packaging. Besides the physical container, clear hazard labels jump out as a must. Every drum or pail needs chemical warning stickers that stand up to bad weather and rough handling. This isn’t overkill; it's what keeps people paying attention and handling the product with care.
Shipping regulations for zinc chloride don’t leave much to chance. The rules under the Department of Transportation in the U.S., or ADR if you’re in Europe, can pile up quickly. Truckers look over the paperwork before letting a pallet of zinc chloride anywhere near their vehicle. They check for things like UN markings and transport hazard class codes, making sure everything lines up in the paperwork. If just one code or sticker is missing, things grind to a halt. For air or sea freight, dealing with international rules can spin heads—and eat up profits if documentation isn’t straight.
Moving tons of zinc chloride to a customer on the other side of the world isn’t just about putting it on a ship and calling it done. Heat or humidity can creep through weak containers, and pretty soon, the material clumps together or corrodes its way through the drum. I've seen exporters double-wrap drums in tough plastic stretch film and strap them onto pallets, all to keep shipments tight and safe. Folks moving smaller amounts sometimes go the extra mile, tossing silica gel packs in the pail to battle moisture, or scheduling quick deliveries so the stuff doesn’t get a chance to react with air.
Plenty of companies are fueling innovation here. Eco-friendly liners and clever sealing tech cut down on waste while holding up under stress. Digital barcodes on every container help trace shipments, revealing weak points in distribution before accidents happen. Teams now train more rigorously, running drills for leaks or exposures—sometimes even bringing in local fire departments for hands-on practice. It’s not just about ticking off boxes for compliance; it’s about sending people home safe at night and keeping the supply chain running smooth.
| Names | |
| Preferred IUPAC name | dichlorozinc |
| Other names |
Butter of Zinc Zinc(II) chloride Zinc dichloride |
| Pronunciation | /ˈzɪŋk ˈklɔː.raɪd/ |
| Identifiers | |
| CAS Number | 7646-85-7 |
| Beilstein Reference | 3587446 |
| ChEBI | CHEBI:49976 |
| ChEMBL | CHEMBL1233555 |
| ChemSpider | 6089 |
| DrugBank | DB14544 |
| ECHA InfoCard | 100.964.292 |
| EC Number | 231-592-0 |
| Gmelin Reference | Gmelin Reference: 8048 |
| KEGG | C14126 |
| MeSH | D015699 |
| PubChem CID | 3007855 |
| RTECS number | ZH1400000 |
| UNII | NW9CXQ99V3 |
| UN number | UN1840 |
| Properties | |
| Chemical formula | ZnCl2 |
| Molar mass | 136.30 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 2.91 g/cm³ |
| Solubility in water | 432 g/100 mL (25 °C) |
| log P | -0.2 |
| Vapor pressure | < 0.1 mm Hg (25°C) |
| Acidity (pKa) | 4.0 |
| Basicity (pKb) | 4.0 |
| Magnetic susceptibility (χ) | -3.9×10⁻⁶ |
| Refractive index (nD) | 1.673 |
| Viscosity | Viscous liquid |
| Dipole moment | 2.12 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 109.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -415.1 kJ/mol |
| Pharmacology | |
| ATC code | A12CB02 |
| Hazards | |
| Main hazards | Corrosive, causes burns to skin and eyes, harmful if swallowed or inhaled, causes respiratory tract irritation. |
| GHS labelling | GHS02, GHS05, GHS07, GHS09 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H302, H314, H410 |
| Precautionary statements | P260, P264, P270, P273, P280, P301+P312, P304+P340, P305+P351+P338, P330, P312, P362+P364, P391, P405, P501 |
| NFPA 704 (fire diamond) | 1-0-1-Acide |
| Lethal dose or concentration | LD50 oral rat 350 mg/kg |
| LD50 (median dose) | LD50 (median dose): 350 mg/kg (oral, rat) |
| NIOSH | ZNQ |
| PEL (Permissible) | PEL: 1 mg/m³ |
| REL (Recommended) | 500 mg/L |
| IDLH (Immediate danger) | 50 mg/m3 |
| Related compounds | |
| Related compounds |
Zinc bromide Zinc fluoride Zinc iodide Mercury(II) chloride Cadmium chloride |
