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Scribes in the Middle Ages chased after the secrets of powerful acids. Among them, hydrochloric acid took on legendary status as alchemists tried to dissolve gold and hunt for the philosopher's stone. Modern chemistry emerged, and names like Johann Rudolf Glauber and Joseph Priestley brought a clearer, evidence-based approach. Their discoveries led directly to what people know as hydrochloric acid. No longer just the stuff of dreams or laboratories filled with mystical smoke, it became a practical tool for a literal world—industry, medicine, and research found real uses, not elusive miracles. Those stories often get left out of classroom texts, but they remind us that curiosity-driven work laid the foundations for the essentials of today's manufacturing and scientific progress.
Open a bottle labeled "Hydrochloric Acid" and you'll find a water-clear liquid, often with a sharp, choking odor. Anyone who's ever caught a whiff knows how quickly caution kicks in. It's a solution of hydrogen chloride gas in water, usually ranging from about 10% to 38% for industrial grades. Most of the time, labs and factories don't fuss around with high purity unless some precision process calls for it. So much of what makes this acid valuable is that it's easy to handle, pack, and transport in containers made from glass, certain plastics, or coated steel. Watch a loading dock at a chemical supply warehouse, and you’ll see workers taking real care: gloves on, eye protection in place, with storage areas vented and marked.
Some liquids bring both convenience and danger, and hydrochloric acid fits that bill neatly. It’s colorless, doesn't burn, but reacts wildly with metals, bases, and certain organic chemicals. Pour it on limestone or even regular concrete and bubbling starts as it eats through the surface, releasing carbon dioxide. Its boiling point drops below that of water, and since vapors rise easily, labs with poor ventilation soon fill up with a harsh, stinging mist. Basic chemistry texts list the pH around 1 in concentrated form—about as corrosive as things get outside of highly specialized acids. Touching it brings quick regret, as it burns skin and eyes on contact. Spill some, and you catch the unmistakable tang in your nose and throat. Still, that same reactivity gives it unmatched utility for things like dissolving rust, processing steel, and producing other chemicals.
Walk into any chemical warehouse and you'll find hydrochloric acid in drums, bulk tanks, and small bottles—each with prominent hazard symbols and concentration information. Safety teams, regulatory agencies, and quality control specialists have shaped the standards over decades, requiring honest labeling and clear technical specs. You won’t catch sloppy language or missing hazard markings, because authorities like OSHA and various environmental agencies hit companies hard for failures. If you’re in the business, you learn to check for gross weight, net weight, purity, and even manufacturing method on every single label before putting the drum on the line. The most successful outfits—big or small—train every worker to scan those symbols, double-check delivery manifests, and treat every shipment as if something could go off with the wrong move.
Two main production processes—direct synthesis and industrial byproduct recovery—get most of the world’s hydrochloric acid to market. The direct route burns hydrogen and chlorine to form hydrogen chloride gas, which then dissolves in pure water. Electrolysis plants, set up to split salt water into chlorine and sodium hydroxide, churn out plenty of byproduct HCl as well. The reaction might sound simple, but controlling water quality, venting off excess gas, and minimizing rust corrosion in the pipes takes real practical experience. The best engineers partner with seasoned operators, keeping processes smooth and safe. Even small slip-ups—wetting the wrong spot, letting joints rust, or missing a leak—can bring trouble to a halt for days.
Hydrochloric acid is a chemistry workhorse. It doesn’t just dissolve metals and rocks. Mix it with sodium hydroxide, and you make table salt; treat it with calcium carbonate, and you strip scale from boilers or treat swimming pool water. Industrial chemists rely on it to clean metal surfaces before electroplating or painting; nobody wants the paint peeling in a year because of leftover oxides. If you attach specialized molecules, you get organochlorine compounds used in plastics, pesticides, and solvents. Even pharmaceutical labs use small, careful applications to tweak molecular structures, purify drugs, or control the pH in delicate reactions. For young lab techs, learning the fine line between just enough and too much hydrochloric acid forms part of the basic apprenticeship in hands-on science.
On official paperwork, it's hydrochloric acid or HCl solution. On the shop floor, people just call it "muriatic acid," especially in trades like pool care and masonry. Old scientific texts mention "spirit of salt," which hints at its roots as a reaction product from salt and sulfuric acid. These different names show just how deeply woven it is into work and daily life, not just the stuff of formal study. It’s a reminder that chemicals and their roles don’t always wear the same labels in labs, construction yards, and shipping manifests.
You won’t see hydrochloric acid kept around without good reason and strict controls. Not in any half-responsible setting, anyway. Trained technicians check storage tanks daily and keep neutralizing agents—like soda ash and lime—close at hand. Anyone who's worked through a slick-floored spill knows the pressure to get things neutralized and cleaned fast, before someone takes a burn or local air quality tanks. Long gone are the days of casual handling with only a vague sense of the risks. Safety glasses, acid-resistant gloves, and specialized face shields are standard gear for a reason. Environmental agencies keep tabs on usage and disposal, knowing that a careless dump can spell disaster for soil and water. Even among careful users, hydrochloric acid occasionally brings on close calls—just browse community message boards in the chemical trades for stories and hard-won lessons.
Steelmakers lean hard on hydrochloric acid; acid pickling runs coat after coat off pipes and sheets, stripping out rust before the metal heads to automotive or construction plants. Folks in water treatment dose it into filtration systems to keep pH levels safe and gear clean. Homeowners use weaker blends for cleaning brick, scrubbing stucco, clearing patio efflorescence, or punching up acidity in swimming pools. It's a part of oil and gas extraction, helping drillers fracture rock layers for easier crude extraction. Laboratories use it every single day for classic analytical tests—nobody running titrations or digging into basic pH work skips over HCl. In pharma and food processing, it finds quiet roles in fine-tuning pH or managing ingredient purity. Each of these uses builds up, brick by brick, creating a quiet but vital backbone for modern industry.
Researchers dig into hydrochloric acid’s interactions across every level of chemistry. Some focus on creating corrosion-resistant coatings or smarter containment materials that last longer and save costs. Others look for greener production techniques, aiming to capture and reuse hydrogen chloride gas with better efficiency. As companies work to shrink carbon footprints, interest in byproduct recycling picks up speed. Niche pharma companies invest in novel synthetic routes that use HCl to build new drug molecules or find safer, less hazardous tweaks. The research pipeline hits everything from environmental monitoring—catching invisible leaks—to producing cutting-edge composite materials. Whatever the focus, ongoing trial and error show that even an old standby like hydrochloric acid remains a living part of scientific discovery, not a relic of the past.
Start handling hydrochloric acid carelessly, and the results come fast—burns, blurred vision, sometimes coughing fits that don’t end until you reach fresh air. Medical studies have tracked acute and chronic exposure, laying out the damage to skin, eyes, lungs, and internal systems. Animal research and workplace health surveys confirm what veterans know: even small splashes, left unwashed, can scar skin or damage eyes permanently. Long-term exposure—often from vapor, not visible spills—raises the odds of respiratory conditions and worsens asthma. Whenever people talk about chemical safety, hydrochloric acid sits near the top of the list for both caution and respect. The lesson gets handed down from mentor to apprentice: never trust that a “minor” acid won’t harm you, and always wash injuries immediately. For anyone working with it for years, toxicological research and practical experience line up so closely that ignoring guidelines just doesn’t make sense.
Hydrochloric acid hasn’t changed much since scientists first tamed it, but how people use it, store it, and think about its lifecycle has shifted. Environmental regulations get stiffer every year, driving chemical plants and end users to rethink disposal and leakage controls. Companies invest in closed-loop systems that recover nearly pure hydrogen chloride, lowering costs while trimming waste. As more research shifts toward renewable feedstocks—like green hydrogen and chlorine sourced from electrolysis powered by sustainable electricity—hydrochloric acid could even stop being a fossil-fueled byproduct and become a net-zero contributor. Engineers and scientists are continually searching for substitute processes that cut down on corrosive waste, use less acid, or bring more recycling into the workflow. If the last century turned hydrochloric acid from a mysterious laboratory staple into a basic industrial tool, the coming years look poised to make it safer for workers, kinder to the environment, and even more central in fields as varied as electronics and sustainable materials.
Factories rely on hydrochloric acid for cleaning metal surfaces. Walk through a steel plant, and you’ll spot huge tanks filled with a strong HCl solution. Workers dunk steel inside to strip away rust and unwanted oxides before shaping or coating the metal. Without this acid bath, car frames and appliances wouldn’t last as long or look as polished. The process helps the protective coating bond tightly, reducing waste and reworking.
At the grocery store, you sometimes find food labels listing “acidulant” or “processing aid.” That’s often hydrochloric acid behind the scenes. Food companies use it to adjust pH in products like corn syrup, sauces, and canned goods. HCl breaks down starch into sugars during syrup production, making sweeteners for sodas and snacks. Afterward, neutralizing agents make sure the acidity is safe, and the final product is free of strong acid. Since it’s tightly regulated, you won’t taste HCl in the food, but the process would stall without it.
Municipalities add hydrochloric acid to control the pH in water before it flows from taps. Too much mineral buildup clogs pipes and makes water taste metallic. By lowering pH, HCl helps keep the water clear, limits bacteria, and protects the system. Swimming pool owners know the drill. Pool supply stores stock HCl to keep water safe and sparkling, dissolving scale on pool walls while balancing the chemical mix. Getting the dose right stops pool irritation and keeps swimmers healthy.
Factories use hydrochloric acid to make dozens of products found around the house. It reacts with limestone to release calcium chloride, a de-icing agent for roads in winter. Chemical plants use it to produce PVC, a staple in pipes and window frames. The acid helps synthesize household cleaners and dyes, working as a basic building block for many common supplies. Without this acid, production would grind to a halt, and everyday materials would cost much more.
Scientists reach for hydrochloric acid for analytical tests, sample preparation, and research. In high school chemistry classes, it's often the first strong acid students handle. It can adjust the acidity in solutions, dissolve minerals, or help identify unknown substances. My own experience as a student included carefully measuring and adding HCl to watch a rock sample fizz, helping me see how acids react in real life. The acid’s reliability and consistency make it a lab staple.
The world of medicine also draws heavily from hydrochloric acid. Drug makers use it to set the right pH for tablets and liquid medications. Over-the-counter digestive aids often contain HCl to mimic or supplement the acid in our stomachs. Proper acidity ensures that medications dissolve at the intended rate and reach the right part of the body. In the background, chemical engineers test and adjust the properties to guarantee quality and safety in every batch.
Though useful, HCl poses risks if misused. Its fumes and concentrated form can burn skin and eyes. Strict rules cover how workers store, transport, and use it. Protective gear, ventilated spaces, and emergency wash stations aren’t optional extras. On a personal level, stories abound of burns avoided by wearing goggles or learning about safe disposal in school science labs. Improved training, clear labels, and advances in packaging prevent most accidents. Keeping up with regulations and making sure people know the risks will keep industrial and household users safe, without losing the benefits hydrochloric acid brings.
Anyone who has spent time in a lab or worked with chemicals knows hydrochloric acid can burn through just about anything. I've seen its damage firsthand—skin that didn't get washed right away turned red, and hardware left unprotected pitted and corroded in mere hours. So taking precautions around it isn’t optional—it’s a matter of keeping your skin, eyes, and lungs out of harm’s way.
The basic gear for handling hydrochloric acid always includes decent goggles, gloves that actually resist acid (nitrile or neoprene, not those cheap latex ones), and a sturdy lab coat. Skip these, and it’s like riding a motorcycle without a helmet. Splash-proof face shields help in case something spills or reacts more violently than expected.
Lab technicians and students sometimes learn the hard way that cotton or polyester clothes don’t hold up against splashes. Rubber aprons add an extra barrier. Choose shoes that clean up easily and cover your feet fully—no open-toe shoes, ever. Accidents happen quickly, so nobody should be left improvising in emergency situations.
Hydrochloric acid fumes can hit hard. In my experience, a strong whiff stings the nose and throat and leaves you coughing for hours. Avoid that by working only in spots with good fume extraction. A proper fume hood pulls vapors away from your face. Cracking a window—or worse, ignoring it—never measures up to this standard. Respirators rated for acid vapors come in handy if you’re pouring a lot.
Hydrochloric acid attacks metal and reacts with lots of substances, so never store it in any old container. Go for chemical-resistant plastic, keep it sealed tight, and never store it next to flammable or reactive chemicals like ammonia or bleach. One mistake, and suddenly you’re dealing with dangerous chlorine gas. In shared spaces, clear labels and separate shelves bring order to chaos.
It’s not uncommon to knock over a bottle or have a cracked container leak silently onto the floor. It pays to know exactly where the nearest eyewash station and safety shower are, and to train everyone in reaching them with eyes closed—panic scrambles thinking. For small spills, neutralizing with baking soda then mopping up with disposable rags saves a lot of grief, but larger spills usually require officially approved spill kits and someone calling for backup.
Years in the lab have shown me that basic training and reminders prevent most mishaps. New hires can’t just get handed a set of rules—they need demonstrations, examples, and walk-throughs. Supervisors who stay involved, checking that procedures are followed, tend to prevent shortcuts and complacency. Regular drills remind everyone that emergencies won’t wait for perfect timing.
Creating a space where people speak up if they spot unsafe behavior really makes a difference. Peer pressure cuts both ways—if the norm is to wear gloves and eye protection, everyone does. If it’s cool to grab acid bare-handed, accidents become routine. Management should reward safe practices, not just productivity.
Automating some chemical handling with pumps and closed systems removes direct contact and cuts down risk. Hydration stations and signage reminding about PPE work remarkably well. Good communication between team members about process changes or supply shortages stops surprises before they start.
Hydrochloric acid has its place in science and industry, but demands respect and careful planning. Every safety step matters—not just for the person handling it, but for everyone in the room.
Hydrochloric acid packs a punch. Just a splash gives a nasty burn, and the fumes irritate your lungs. Plenty of stories show how a simple slip-up—sometimes a loosely sealed cap or a cracked container—leads to big problems. In more than twenty years around labs, manufacturing plants, and school storerooms, I've seen stains on concrete, corroded shelves, and even ruined electronics from fumes drifting out of poorly sealed drums. Mistakes with this acid rarely go unnoticed; you’ll hear the hiss, smell the sharp fumes, or watch metal rust before your eyes.
Dyed bottles or makeshift jugs do nothing but invite disaster. Manufacturers use high-density polyethylene (HDPE) jugs for good reason. Glass works too, but only borosilicate glass—cheap glass breaks apart as soon as it meets concentrated acid. Avoid any metal—even stainless steel can't handle long-term exposure. Over the years, plastic wins on durability and safety. Make sure caps fit tightly, but let out a hiss from time to time for venting (just a little, in a fume hood). Otherwise, pressure builds and turns that jug into a squirt gun.
Store hydrochloric acid away from water sources and especially away from bases. Acid fumes chase humidity, and every drop of water in the air ends up pulling acid vapor with it. Put acid on the bottom shelf, inside a chemical storage cabinet made for corrosives. Cabinets painted with acid-resistant coating or lined with plastic go a long way. It keeps leaks contained, protects the concrete, and makes cleanup possible after a spill.
Many folks shrug off the advice to keep acids and bases apart. During a school inspection, I found hydrochloric acid stacked next to bleach and ammonia. One spill there, and you’re mixing a gas cloud straight out of a chemistry nightmare. Every chemical safety course says “segregate acids from bases and oxidizers.” It’s simple advice, and ignoring it has left people with burns or worse. Use labels you can read from across the room, and add pictograms so everyone—from students to experienced workers—knows what’s inside each container.
Acid fumes linger. They eat through metal shelving, wiring, or even lab instruments. Good ventilation makes a big difference. Spend money on a vented cabinet rated for corrosive materials. A fume hood gives even better protection, especially in tight spaces or high-volume areas. Retrofit old cabinets with exhaust fans if you can't swap them out immediately.
The best acid storage setup means nothing if workers or students don’t know the drill. Review the Safety Data Sheet every six months. Post emergency numbers and spill kits nearby. Regular safety meetings help everyone remember not to set acid next to break-room snacks or to check for leaks after every use. PPE—like gloves, goggles, and aprons—should be close at hand, not stashed away. In every incident I’ve seen, the difference between a minor scare and a trip to the hospital lay in how fast and clearly people responded.
Tracking new chemistry innovations matters, but no technology replaces sturdy plastic, sharp eyes, and smart storage. As more people learn to respect hydrochloric acid, stories about preventable spills will get rarer. Let's keep those lessons sharp and simple so nobody repeats old mistakes.
Some products stand out in chemistry for their sheer power—hydrochloric acid belongs to that group. I’ve handled it in labs, seen its effect in industry, and learned how its concentration shapes what it can do. Most people outside a laboratory might picture all acids the same, but small changes in concentration unlock entirely different worlds of application and risk.
Walk into any chemical supply house and you’ll see hydrochloric acid labeled as “muriatic acid,” often around 31% to 37% concentration by weight. That bracket reflects how companies manufacture and ship it in bulk—and for good reason. Above about 38%, the acid fumes heavily and becomes difficult to manage outside specialized setups. Laboratories go for the upper limit, typically labeled “concentrated,” at about 37% HCl, which equals roughly 12 molar.
I remember the first time I opened a fresh bottle of concentrated hydrochloric acid, a sharp gust hammered my nose. That experience brought the safety rules home for me real quick. The fumes can damage lungs in moments. The strong stench means it’s impossible to ignore its power.
Concentration shapes function. Pool cleaners, bricklayers, and scale-removers use muriatic acid at concentrations around 20% to 32%. For households, the product might drop even lower for safe surface cleaning—diluted to about 10%. In the lab, full-strength hydrochloric acid makes fast work of dissolving metals and prepping samples, but no one pours it without goggles, gloves, and plenty of ventilation.
The variation isn’t just for safety. Higher acid strengths accelerate chemical reactions. For industrial metal cleaning before galvanization, workers want fast, complete removal of oxides, so they turn up the concentration. But in food processing, pickling, or water treatment, only weaker solutions are suitable.
I’ve seen serious injuries from acid handled without respect or understanding. News headlines feature accidents from diluted or mislabeled products. Data from the U.S. National Poison Data System points to hundreds of hydrochloric acid exposures every year, mostly in the home. Many cases involve workers using acids at concentrations higher than they realized because of poor labeling or improper storage.
Businesses need to check product labels and safety sheets carefully. Every gallon should specify the acid percentage. If it’s not clear, that’s a red flag for safety and compliance.
Anyone working with hydrochloric acid should demand clear, accurate labeling—percent by weight or molarity, not vague terms like “full-strength.” Suppliers can help with better packaging, tamper-evident seals, and accessible technical sheets. Training goes beyond a single safety talk. Practice with small batches first, keep neutralizers like baking soda nearby, and make sure to store acids well away from incompatible chemicals like bleach or ammonia.
For schools and hobbyists, smaller, pre-diluted packages help reduce risks. In industry, automated dispensers and fume hoods offer more control. As someone who’s seen the aftermath of mistakes, I’d put education and vigilance ahead of any hardware—because the real danger comes from shortcuts, not the acid itself.
Hydrochloric acid delivers powerful results, but only when the concentration matches the job and users understand exactly what’s in the bottle. Knowledge, accurate product data, and personal respect for the chemical form a safety net every time the cap twists open.
Hydrochloric acid isn’t a mystery to people working in labs, workshops, or even those tackling home improvement jobs. Folks might know it as muriatic acid. Pool upkeep, brick cleaning, and some hobby chemistry projects all bring this chemical to the table. Its strength as an acid makes it downright hazardous. The sting in your nose or burns on your skin aren’t just stories in warning labels—they’re warnings you’ll feel if you ignore basic precautions.
Instructions often say “neutralize and dispose of safely” as if those words are interchangeable with plain water and optimism. Pouring hydrochloric acid straight down a sink or into a drain is reckless. You’re risking plumbing, putting workers and wildlife in danger, and possibly breaking the law. In my own workshop, I quickly learned that taking shortcuts leads to ruined pipes and expensive plumber visits.
Knowing you have to bring that acid solution up to a neutral pH—close to 7—really matters. Mixing hydrochloric acid with the wrong thing, or just dumping it, can create chlorine gas. Not only does this make you cough, it can actually kill you in high doses. Reading a few too many industrial accident reports drives this home. Sometimes, disaster comes down to ignorance or impatience instead of some unusual technical error.
It’s not magic. People often use baking soda (sodium bicarbonate) or garden lime (calcium carbonate) to “kill” hydrochloric acid. In my garage, I always add the acid to a bucket of cold water, never the other way around. This keeps any splashes under control. Slowly sprinkling baking soda into that mixture, with a long wooden spoon or stick for stirring, brings a predictable fizz but saves you from burns or acid clouds in your face.
Waiting for those bubbles to stop is tedious but important. If I’m ever unsure, I pull out some cheap litmus paper from a hardware store. Only after the paper stops showing red or orange—just blue or green—do I feel okay about moving the liquid to the next step. In bigger projects, I’ve watched responsible contractors opt for large neutralizing tanks and regular wastewater testing. Large volumes, like those from pool companies, often get checked by local authorities before release. This isn’t just about following the rules—it’s about not poisoning the community with a bad decision.
Home users and DIY fans can take spent, neutralized solutions to a hazardous waste facility or follow city guidelines for disposal. Local rules matter. In the lab or factory, employees track the acid in waste logs and call the haz-mat crew for anything above small batches. Hospitals and schools avoid ever pouring straight acid down a drain. I keep a copy of my region’s chemical disposal program close, after the city once fined my neighbor for improper acid disposal. Most local governments run drop-off sites that take these solutions every few months. The paperwork’s a headache, but it’s a cure for sleepless nights worrying about contaminated water or soil.
Ignoring hydrochloric acid’s power puts people and pets in real danger. Facts from the CDC, OSHA, and EPA back this up with real-life examples of injury, groundwater damage, and costly cleanups. Communities that share tips—how to use a splash shield, where to get litmus strips, which facility accepts neutralized acid—end up with fewer accidents. Safety becomes part of the culture. That’s what really keeps everyone safe: not a new gadget, but folks willing to share what actually works and why mistakes have lasting consequences.
| Names | |
| Preferred IUPAC name | Hydrochloric acid |
| Other names |
Muriatic Acid Spirits of Salt Hydrogen Chloride Solution |
| Pronunciation | /ˌhaɪ.drəˌklɔː.rɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 7647-01-0 |
| Beilstein Reference | 1904225 |
| ChEBI | CHEBI:17883 |
| ChEMBL | CHEMBL1233558 |
| ChemSpider | 2157 |
| DrugBank | DB09161 |
| ECHA InfoCard | 03-2119484869-23-0000 |
| EC Number | 231-595-7 |
| Gmelin Reference | 1446 |
| KEGG | C00077 |
| MeSH | D006871 |
| PubChem CID | 313 |
| RTECS number | MW4025000 |
| UNII | RWA8R6J2KR |
| UN number | UN1789 |
| Properties | |
| Chemical formula | HCl |
| Molar mass | 36.46 g/mol |
| Appearance | Colourless, fuming liquid |
| Odor | Pungent |
| Density | 1.18 g/cm³ |
| Solubility in water | miscible |
| log P | -1.25 |
| Vapor pressure | 40.6 kPa (@ 20 °C) |
| Acidity (pKa) | -6.3 |
| Basicity (pKb) | -7 |
| Magnetic susceptibility (χ) | -38.6 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.332 |
| Viscosity | 1.9 cP (for 37% solution at 25°C) |
| Dipole moment | 1.08 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 186.90 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | −92.30 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -92.30 kJ/mol |
| Pharmacology | |
| ATC code | A09AB57 |
| Hazards | |
| Main hazards | Corrosive, causes severe skin burns and eye damage, harmful if inhaled, may cause respiratory irritation, reacts violently with bases and some metals. |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05, GHS07 |
| Signal word | Danger |
| Hazard statements | H290, H314, H335 |
| Precautionary statements | P234, P260, P264, P271, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501 |
| Explosive limits | Not explosive as a gas. |
| Lethal dose or concentration | LD₅₀ oral rat: 900 mg/kg |
| LD50 (median dose) | LD50 (oral, rat): 900 mg/kg |
| NIOSH | 0031 |
| PEL (Permissible) | PEL = 5 ppm (Ceiling) |
| REL (Recommended) | REL: 5 ppm (7 mg/m³) |
| IDLH (Immediate danger) | 50 ppm |
| Related compounds | |
| Related compounds |
Hydrobromic acid (HBr) Hydroiodic acid (HI) Hydrofluoric acid (HF) Chlorine (Cl2) Sodium chloride (NaCl) Sulfuric acid (H2SO4) Aqua regia |
