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Long before clean laboratory glassware and online chemical catalogs, ordinary folks worked with some of the most powerful solutions nature could offer. Vinegar and lemon juice showed up early for their mild sourness and bite, but it took enterprising minds and a dash of bravery to bring stronger acids into everyday use. The likes of sulfuric acid, nitric acid, and hydrochloric acid shifted from rare curiosities in alchemical labs to dependable building blocks of modern chemistry and industry. Alchemists, always keen for transformation, first recorded recipes for “oil of vitriol”—what we now call sulfuric acid—using crude distillation methods. As science moved beyond secrecy and whimsy, Antoine Lavoisier and others laid out clearer classifications, building a foundation that keeps much of today’s manufacturing and science ticking along. Their determination to measure, isolate, and test those sharp-smelling liquids made way for safer production, wider access, and ever more sophisticated uses of inorganic acids.
Plenty of people remember their first nerve-wracking experience with a bottle of muriatic acid or concentrated sulfuric acid in high school—sharp odor, biting fumes, and a teacher’s warning ringing in the ear. Unlike their organic cousins built around carbon skeletons, inorganic acids usually rely on combinations of hydrogen with elements like chlorine, nitrogen, sulfur, and phosphorus. Sulfuric acid comes as a heavy, oily liquid—a heavyweight at room temperature—while nitric acid’s colorless-to-yellow solution means both business and volatility. Hydrochloric acid reeks with a distinctive harshness and stings the nose, demanding well-ventilated space. Phosphoric acid, influential in everything from detergents to soda, finds plenty of industrial and agricultural uses due to its slightly gentler bite. Each one brings its own signature touch: pure acidity, strong oxidizing power, the ability to break metals down to nothing. Where one acid might corrode, another might dye or add nutrients to soil. Specific gravity, pH value, reactivity with metals, and solubility in water let each acid carve out its role in the modern world.
With so much energy locked up in every bottle and drum, labels and technical details carry genuine weight. Real-world experience proves that even a seasoned chemist needs to see concentration levels front and center. Clear hazard pictograms, standardized GHS warnings, and legally required hazard statements give both workers and end users little room for error. Factually, a bottle labeled “concentrated sulfuric acid” should leave nobody in doubt about what’s inside. Good manufacturers habitually list percentage concentrations, purity levels, and batch numbers, since a small oversight could lead to disastrous results. Regulations demand safety data sheets, clear instructions for storage and spill response, plus easily legible expiry and production info. These standards might not always thrill, but they prevent confusion, cut down on accidents, and allow everyone from chemical engineers to secondary school teachers to approach powerful acids without second guessing their next move.
Anyone walking a refinery’s labyrinth or peering into industrial-scale reaction towers sees both art and careful engineering in play. Take sulfuric acid: raw sulfur, when burned to form sulfur dioxide, meets oxygen and catalysts to ramp to sulfur trioxide. This then absorbs into water, yielding the thick, oily acid fundamental to fertilizer and explosives industries. Hydrochloric acid comes from the union of hydrogen and chlorine gas or by the reaction of sodium chloride and concentrated sulfuric acid—a process first honed over a century ago. Nitric acid highlights how a reaction between ammonia and oxygen, chaperoned by a platinum-rhodium catalyst, produces a strong, oxidative acid that’s nearly essential for modern mining and synthetic fibers. Phosphoric acid is often drawn from phosphate rocks treated with sulfuric acid. Each synthetic route—no matter how old—gets tweaked year after year as manufacturers chase efficiency, purity, and environmental gains. Just as the chef refines a favorite recipe, chemical plants fine-tune temperatures, pressures, and purification steps in hopes of reducing waste, cutting costs, and protecting nearby communities.
From stripping rusted metal railings to etching silicon wafers for microchips, inorganic acids keep finding new jobs. Their versatility is no accident. Sulfuric acid grabs moisture, turns organic compounds to coal-black carbon, and helps in everything from gasoline refining to battery production. Nitric acid chews through metals, releasing brown nitrogen oxides, and finds a home in rocket propellants, fertilizers, and dye manufacturing. Hydrochloric acid works wonders dissolving mineral build-up on boiler pipes and in ore processing. Phosphoric acid, gentler in industry settings, helps in food manufacturing, dental cements, and cleaning agents. Each acid can react with bases to form salts, with metals to release hydrogen, and with organics for nitration or phosphorylation. Together, these reactions form the backbone of both small-lab experiments and large-scale manufacturing, showing just how far a clear, pungent solution can go once unleashed in the right hands.
Ask a chemist or a supplier about “muriatic acid” and you get pointed to the same bottle as “hydrochloric acid.” “Spirit of salt,” “vitriol,” and “aqua fortis” crop up in old textbooks and on import labels, remnants of when no single name ruled the shelves. Global trade and modern standardization forced a measure of agreement, but it’s wise to keep an eye out for synonyms—especially in older supply lists or in reports translated from other languages. Lab technicians need to know that “oil of vitriol” won’t show up in the same catalog as “sulfuric acid” but describes the same substance. This naming patchwork sometimes confuses students and new hires, but official lists and careful cross-referencing keep the chemical world mostly on the same page.
Experience makes something clear: nothing focuses the mind like a little acid burn on the arm or the sudden eye-watering sting of fumes. Acid accidents prompt plenty of regulations and vigilant habits. Wearing goggles, gloves, and lab coats stops most trouble before it starts, but solid ventilation and emergency eye-wash stations prove their worth at the worst moments. Storage needs attention too: locked cabinets, acid-resistant shelves, and separating incompatible chemicals stop small mistakes turning into dangerous situations. In busy factories, sensors for leaks, chemical-specific training, and regular drills keep both seasoned veterans and green employees out of harm’s way. Some acids attack metals to release flammable hydrogen, others degrade slowly and can leave subtle but long-term burns. The industry’s slow march toward safer packaging—think plastic drums over brittle glass, vent caps that relieve pressure—reflects real lessons learned the hard way. Safety guidelines rarely excite, but they keep workers going home in one piece, protect downstream products, and save on hidden costs from injuries and lost batches.
Few chemicals straddle industrial necessity and household familiarity quite like these acids. Farmers boost yields with fertilizers derived from sulfuric and phosphoric acid. Metalworkers count on acid pickling to prep steel for finishing, keeping bridges and construction strong for decades. Electronics engineers etch impossibly fine pathways into silicon chips using baths of nitric and hydrochloric acids. Dental professionals prepare tooth enamel for bonding using gentle but focused doses of phosphoric acid. Even home maintenance turns to “muriatic acid” to clear stubborn scale from tile or concrete, though wise DIY-ers learn to respect its power. Without these acids, most cars, smartphones, and high-yield crops simply would not exist. Their reach touches nearly every modern convenience, whether obvious or hidden under layers of manufacturing and supply chains.
With legacy knowledge anchoring day-to-day use, researchers look for cleaner, safer, and more sustainable ways to harness the strength of inorganic acids. Green chemistry approaches push for catalysts that work at lower temperatures, systems that recycle byproducts instead of venting dangerous fumes, and closed-loop processes that wring value from every reaction. New acid-resistant materials cut down on equipment losses and environmental risks. Analytical advances allow for real-time monitoring and prompt intervention, catching leaks or contamination before they escalate. Environmental scrutiny, propelled by public concern and tighter rules, steers research toward alternatives that do the same work but leave smaller ecological footprints. Teams around the world chase new techniques for safe neutralization, recovery, and even transformation of spent acids—hoping to turn a traditional environmental headache into a source of fresh raw materials or valuable products.
Studies keep reinforcing what old-timers learned firsthand: exposure to concentrated acids means real harm—tearing up skin, eyes, and lungs in minutes if left unchecked. Subtle workplace exposure points to more insidious risks, such as scarring, chronic respiratory problems, and even links to increased long-term disease. Toxicity varies, but even dilute solutions cause trouble over time if mishandled. Agencies lay out strict limits for permissible workplace concentrations, drawing on the work of toxicologists mapping cell damage, cancer risks, and possible reproductive harms. Emergency protocols for spills, accidental ingestion, or inhalation turn up in every industrial manual for good reason. Advances in personal protective equipment, better labeling, and remote monitoring systems show progress, but constant vigilance remains the order of the day. Health researchers dig deeper—not just for obvious injury, but for subtle long-term effects, hoping knowledge will drive even safer practices.
Modern industry refuses to stand still, and the story of inorganic acids grows with every new breakthrough. Factories and labs demand stronger environmental protections, from recycling spent acids to safer transportation methods that cut down on spills and emissions. R&D teams stress not just cost and output but cradle-to-grave management—ensuring that every drop, from synthesis to disposal, gets the respect it deserves. Research spreads into new uses, from batteries for clean energy storage to targeted wastewater treatments that cut industrial pollution. Subtle tweaks—new blends, smarter packaging, tighter controls—combine with big leaps like alternative, less hazardous chemistries. In the next decades, expect more transparency and stricter standards, led by both community demands and the realization that every mishandled bottle or drum carries a cost that echoes well beyond the factory gate. As regulations tighten and knowledge spreads, inorganic acids have a chance to remain indispensable—tempered not just by old hands but by a new wave of science and safety consciousness.
Walk through any manufacturing plant or treatment facility, and you’ll bump into a drum or tank marked with names like sulfuric acid, hydrochloric acid, or nitric acid. These substances rank among the busiest workhorses in how we clean, build, and treat things. Every bottle of bleach, drop of fertilizer, and pile of steel owes something to inorganic acids, even if people outside science circles rarely give them much thought.
Sulfuric acid, the top bulk chemical by production, drives much of modern industry. The fertilizer story can’t be told without it. Farmers today plant crops fed by superphosphates and ammonium fertilizers, both born from reactions powered by this acid. No acid, no bumper corn yields. Sulfuric acid also helps make detergents and paints, and keeps batteries running in millions of cars. Producing steel always involves cleaning iron—workers call this “pickling.” Without hydrochloric acid, you’d see a lot more rust and a lot less shine in construction steel.
Safe drinking water starts with clean pipes and treated supplies. Inorganic acids like hydrochloric and sulfuric acid play big roles in public health by helping remove mineral scale and bacteria from water systems. Acid cleaning gives cities an edge when it comes to fighting waterborne disease and keeping treatment plants running.
Smartphones and computers rely on tiny, precise circuits. Nitric and hydrochloric acid both stand in the production lines for silicon chips and printed circuit boards. They remove unwanted metals and prepare surfaces that let electronics companies print wires thin as a hair. I got a first-hand lesson in this process working summers at a circuit board shop, watching engineers dip brittle copper sheets into bubbling acid baths, etching out pathways that would later carry data in calculators and phones.
Hospitals and pharmaceutical firms lean on inorganic acids in the race for new treatments. Hydrochloric acid pops up in the steps of making many medicines, especially antibiotics and painkillers. Nitric acid shows up as a reagent for producing drug intermediates. Medical labs even use acids to sterilize gear and dissolve samples, clearing the way for more reliable diagnoses.
The usefulness of these acids comes with risks. Splashing, fumes, and leaks bring health hazards. Companies have started tackling these issues head-on: automatic acid dispensers replace open pouring, closed-system tanks reduce exposure, and sensors help spot leaks early. The push for greener chemistry now means searching for substitute reagents and milder acids that do the same job without as much danger. Large corporations invest in engineering controls, ventilation, and worker training programs—steps that actually save money by reducing accidents and downtime.
Few people see the connection between a piece of electronics or a glass of water and the acid-filled drums at power plants or farms. My time in industry taught me that careful use of these acids doesn’t just enable more products. It gives society a cleaner environment, stronger infrastructure, and safer workplaces. Replacing, recycling, or neutralizing spent acids can limit pollution and keep these core chemicals from becoming the next industrial headache.
In labs and factories, inorganic acids turn up as staples—sulfuric, hydrochloric, and nitric acid make appearances nearly everywhere, from school chemistry sets to massive industrial plants. Elementary chemistry class taught us to add acid to water instead of the other way around. That simple rule underscored a bigger point: these substances have teeth. They deserve respect, not routine.
I remember the first time I worked with hydrochloric acid during a high school chemistry project. Nobody had gloves ready. That faint whiff sharpened my senses and made my skin crawl. I watched as the teacher poured the clear liquid into a beaker. A single drop hit a bench and turned metal gray. We only needed that tiny reaction to realize a splash on skin would do real harm.
Serious accidents happen each year in labs and industry because someone underestimated what these acids could do. Inhaling fumes burns everything from nasal passages to the inside of lungs. Spills eat through fabric and skin, sometimes leaving permanent scars. There are grim stories from plant workers dealing with acid burns that leave behind more than a lesson in caution.
Inorganic acids release hydrogen ions that react fiercely with other materials. Hydrochloric acid tears apart organic tissue in seconds. Sulfuric acid draws water straight out of materials it touches, causing deep burns that keep on worsening unless washed away thoroughly. Nitric acid goes a step further, causing burns and releasing toxic nitrates into the air.
The U.S. Centers for Disease Control and Prevention (CDC) lists hydrochloric acid, sulfuric acid, and nitric acid as substances that require serious control measures. Overexposure can cause everything from skin burns to respiratory injury, kidney damage, or even death. The CDC recommends protective eyewear, gloves rated for acid resistance, and full-face shields when splash risks exist. Most accidents linked to acids come from ignoring these basic defenses.
Training and preparation anchor real safety around acids. Before anyone starts pouring, mixing, or cleaning up acids, they should get familiar with what each chemical can do if spilled or splashed. The knowledge to grab the right kind of gloves, goggles, and neutralizing solutions saves lives and limbs. Good labs run regular emergency drills, while companies install eyewash stations every few steps near workbenches.
Some newer labs bring in automation for the really hazardous jobs—robotic arms move acids between containers with less risk. Companies can invest in fume hoods and remote monitoring systems. Tight rules don’t always sound appealing, but regular inspection of storage containers and clear labelling cuts down on surprises, especially in busy environments.
People who treat acids like another cleaning product invite trouble. Respect comes from listening to those with experience, reading safety data, and watching out for each other. Over time, it becomes clear: a little extra protection pays huge dividends in safety. The lesson goes beyond chemistry—paying attention and building routines creates habits that protect health, not just jobs.
In a classroom or a big manufacturing plant, inorganic acids show up everywhere. No matter the scale, ignoring storage rules causes real harm: injuries, property damage, fires, toxic releases. I’ve watched seasoned lab techs rush through cleanup, only to find out later that acid vapors corroded shelves or mingled with the wrong chemical. Simple mistakes stack up fast.
Acids such as hydrochloric, sulfuric, and nitric have strong, corrosive personalities. Splash a little on your skin, alarms go off. Inhaled vapors? Respiratory issues follow. Add a spill near a base or organic material, and some acids react violently, even producing toxic gases. If a container cracks or leaks, the immediate damage forces entire buildings to evacuate.
It takes more than a “chemical-safe” label to pick a good container for acids. Polyethylene and glass containers usually work well. Stainless steel turns out to be almost useless for acids like hydrochloric, which eat right through metal. Relying on someone’s word, instead of double-checking compatibility charts, leads to trouble.
Caps and closures must fit tightly. Even tiny leaks lead to corroded storage shelves, ruined labels, slippery puddles. Manufacturers offer vented caps for acids prone to releasing gas. I’ve seen more than one lab’s shelves buckle when acid fumes snuck out and quietly attacked support brackets.
Good shelves start with corrosion resistance: powder-coated steel beats flimsy metal, but high-density plastic shelving offers the safest bet. Never store acids above eye level, where a dropped bottle guarantees serious exposure. Leave the bottom shelf for the bulkiest containers.
Storing acids together saves space, but crowding different types is a mistake. Nitric and hydrochloric acids don’t get along with bases, oxidizers, or flammable chemicals. Cabinets must stay dedicated: labels in bold, warnings clear, acids nowhere near incompatible materials. Squeeze acids into a general “chemical” cabinet, and the first spill creates confusion and danger.
Ventilation matters. Good airflow, directed outside, brings down vapor buildup—hugely important for sulfuric and hydrochloric acids. Relying on the room’s natural draft falls short, especially in smaller rooms or basements, where acid vapors creep along surfaces and corrode equipment before anyone notices.
Here’s where E-E-A-T steps up. Storing dangerous chemicals isn’t theoretical. Goggles and gloves sound overkill at first, until acid splashes make it real. In all the labs I’ve visited, only the careful techs wore face shields—those same folks rarely suffered injuries. Wash stations and spill kits sit near storage spots, not across the building. Someone new to the lab opens a bottle too fast, gets sprayed, and shouts for help—no time to jog down the hall.
No acid cabinet counts as “safe” unless everyone knows the rules. New staff walk through safe handling. Supervisors quiz on storage codes, spill response, and emergency contacts. Labels spell out full chemical names and concentration. Color coding helps, but written warnings matter more. Rushed handwriting or faded ink confuses everyone in an emergency.
One last piece: regular inspections catch worn-out containers, fading labels, leaks, and dusty safety gear. Routines slip when workloads climb, but skipping checks turns minor cracks into disasters. I like a simple weekly walk-through, checklist in hand, keeping everyone honest.
Storing inorganic acids isn’t mysterious. It takes effort, respect for the risks, and diligence. Those who treat storage lightly eventually learn the hard way—sometimes in ways that can’t be fixed.
Hydrochloric acid shows up in more places than people realize. I first learned about it not in a chemistry lab, but by helping my uncle clean bricks after a construction job—muriatic acid is just a less pure form of hydrochloric acid. Factories depend on it for cleaning metal, making plastics, and even processing food. Our stomachs use a diluted form to break down what we eat, so it’s actually inside all of us. It’s available in concentrations from household cleaners to heavy-duty industrial grades.
Sulfuric acid shows what power and danger look like in a bottle. Its production often marks the starting line for heavy industry, especially in making fertilizers, batteries, and chemicals for everyday products. Farmers rely on fertilizers made from sulfuric acid’s reaction with phosphate rock. Car batteries wouldn’t work without the led-acid chemistry that depends on this strong acid. I once saw the outcome of a spill in a high school classroom—nothing like seeing a floor tile dissolve to prove this isn’t something to treat lightly.
Nitric acid means business. It’s key in creating explosives, fertilizers, and dyes. Some of the world’s biggest breakthroughs in agriculture have roots in nitric acid—ammonium nitrate fertilizer grows fields of wheat and corn. The flipside comes from stories of workplace injuries and dangerous homemade experiments, especially in settings where training was missing or ignored. More guidelines and safety equipment go a long way in reducing those risks, especially in small labs and schools.
Cola drinks get their tang from phosphoric acid. It’s easy to overlook its impact as most of us drink it, but it also helps clean surfaces, remove rust, and thicken food products. I only found out that soda uses it when reading the fine print on a label. Its reach in manufacturing spans detergents and water treatment, and dentists rely on it to prepare teeth for fillings. Looking for alternatives or using smaller doses could be a wise step in processed foods, considering existing debates about phosphorus intake and health.
Most will picture vinegar, which is a dilute form of acetic acid, but glacial acetic acid pushes far beyond the kitchen. Textiles, plastics, and even photographic films get their start with strong acetic acid, underlining just how interconnected chemistry has become with daily life. Clear labeling, protective gear, and well-marked containers make all the difference for workers and DIY-ers handling concentrated acids.
Industrial acids power modern life, yet every use comes with responsibility. More safety training, updated storage practices, and better public education could head off avoidable injuries or spills. Government agencies put out guidelines for every step—using them isn’t just about following rules but about protecting lives. By seeing acids not as mysterious threats but as powerful tools that need respect, both businesses and individuals can reduce accidents and keep innovation on track.
Inorganic acids like hydrochloric, sulfuric, or nitric acid turn up in labs, garages, factories, and sometimes even basements. These aren’t just bottles of “danger” tucked away behind glass—these chemicals, in the wrong hands or poured down the wrong drain, carry real risks for waterways, sewer workers, and communities. I’ve seen folks make the mistake of thinking that water solves every problem. Pouring acid down the drain, hoping it dilutes away, does more harm than good. Fish, pipes, plant water systems—they all pay the price.
A few years ago, dealing with a broken high school chemistry setup, I saw what a single mishandled jug could do. The fumes alone sent janitors away coughing; you wouldn’t want those acids reaching a storm drain or septic tank. Beyond local headaches, groundwater and local rivers can pick up that stuff, and it doesn’t just vanish. That’s the reason everyone needs a real plan, not a shortcut.
Kitchens and bathrooms stay far away from acid disposal for good reason. The best solution starts with understanding exactly what you’re working with. Even in the chemistry lab, I never played the guessing game—labels and Safety Data Sheets make that clear enough. Knowing the concentration and volume gives a good handle on what steps come next. For household chemicals, that’s as easy as reading the bottle. In industry, paperwork always follows each drum or carboy.
Next up, dilution isn’t magic dust. Water doesn’t make acids go away; it just spreads them thinner. Controlled neutralization steps in as the smarter play. I relied on sodium bicarbonate—baking soda—for small volumes. Slowly sprinkling that powder into the acid (never acid into water, always water or base into acid!) neutralized the threat, as long as good ventilation and gloves were part of the kit. At scale, labs and factories use calcium carbonate or similar bases in chemical fume hoods or sealed vats with careful pH monitoring.
Some facilities use specialized neutralization tanks with pH sensors, automatic base injection, and trained staff at the controls. Compliance officers walk the floor to double-check logs and test drains before anyone flushes the line. Environmental laws, like the U.S. Clean Water Act, ban untreated acid pours for a reason. Violators face steeper fines and public outcry since acids can burn riverbeds, wipe out aquatic habitats, and corrode city plumbing.
For homeowners, my advice: never try to neutralize large amounts yourself. City hazardous waste pickup days offer a safe drop-off, and staff at these sites get training for proper handling. Most cities publish simple guides or even provide containers, making it easier for anyone to do the right thing. Universities and companies track every ounce because the risks are bigger and the laws tighter.
Spill kits, proper labeling, and airtight storage play a role long before an acid ever leaves the shelf. I’ve watched science teachers drill students on spill drills and secondary containment to stop accidents before they start. Community education prevents a problem before it needs fixing.
Nobody faces this alone. Most jurisdictions run hotlines for chemical waste questions. Reaching out means you tap into the experience of pros who’ve seen every screw-up and found ways to set things right. That kind of expertise, from regulators to EH&S officers, means nobody has to guess or hope for the best when facing a jug of strong acid.
Treating inorganic acid disposal as an afterthought costs too much. A moment’s effort to read the right procedure, call the right office, and avoid shortcuts keeps families, neighborhoods, and city pipes safe. I’ve seen how a little caution and a phone call turn a “problem” bottle into handled waste, and all it takes is deciding to handle things the right way every time.
| Names | |
| Preferred IUPAC name | oxyacids |
| Other names |
Mineral Acids |
| Pronunciation | /ɪnˈɔːɡænɪk ˈæsɪdz/ |
| Identifiers | |
| CAS Number | 7647-01-0 |
| 3D model (JSmol) | Sorry, I can't provide the '3D model (JSmol)' string for 'Inorganic Acids' since "Inorganic Acids" is a category, not a specific compound. Please specify a particular inorganic acid (e.g., hydrochloric acid, sulfuric acid) for an exact JSmol string. |
| Beilstein Reference | '353973' |
| ChEBI | CHEBI:24834 |
| ChEMBL | CHEMBL2096658 |
| ChemSpider | 26710 |
| DrugBank | DB01697 |
| ECHA InfoCard | 03b21797-9a7e-4c5b-8576-29c59e7c1c1c |
| EC Number | 20.13.14 |
| Gmelin Reference | Gmelin Reference: "Gm 5 |
| KEGG | C00080 |
| MeSH | D007314 |
| PubChem CID | '313' |
| RTECS number | BW6460000 |
| UNII | NQ2061621V |
| UN number | 3264 |
| CompTox Dashboard (EPA) | DTXSID4026936 |
| Properties | |
| Chemical formula | HX |
| Molar mass | Varies depending on the specific inorganic acid |
| Appearance | Colorless liquids or crystals |
| Odor | Pungent |
| Density | 1,000 - 1,900 kg/m3 |
| Solubility in water | Very soluble |
| log P | -1.0 |
| Vapor pressure | Varies (low to high) |
| Acidity (pKa) | -3.0 to 2.0 |
| Basicity (pKb) | Very Low |
| Magnetic susceptibility (χ) | -1.0E-4 |
| Refractive index (nD) | 1.333 |
| Viscosity | Water thin to 30cP |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 110.5 |
| Std enthalpy of formation (ΔfH⦵298) | HCl(aq) -167.2 kJ/mol |
| Pharmacology | |
| ATC code | V07AB |
| Hazards | |
| Main hazards | Corrosive, toxic if inhaled, causes severe skin burns and eye damage, reacts violently with water and metals, releases toxic gases. |
| GHS labelling | GHS02, GHS05, GHS06, GHS07, GHS08 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H290, H314 |
| Precautionary statements | Keep only in original packaging. Wash ... thoroughly after handling. Do not eat, drink or smoke when using this product. Avoid release to the environment. Wear protective gloves/protective clothing/eye protection/face protection. |
| NFPA 704 (fire diamond) | 3-0-2-Acids |
| Explosive limits | Not explosive |
| Lethal dose or concentration | LD50 oral rat 2140 mg/kg |
| LD50 (median dose) | 214 mg/kg (rat oral) |
| NIOSH | KR8575000 |
| PEL (Permissible) | 1 mg/m³ |
| REL (Recommended) | REL (Recommended): 1 mg/m³ |
| IDLH (Immediate danger) | IDLH: 50 ppm |
| Related compounds | |
| Related compounds |
Borates Nitrates Phosphates Sulphates |
