People living along trade routes centuries ago watched as what looked like white crystals built up on the inside of their chimneys after burning animal dung and salty plants. Ammonium chloride, known in old texts as sal ammoniac, made its way through ancient markets as both a mysterious substance and a practical commodity. Alchemists in Egypt and China ground those crystals by hand, trying to capture new medicines or metal treatments. As chemistry found its feet in the 18th and 19th centuries, laboratories gave ammonium chloride new roles. Commercial factories in the 20th century spun up production so much that most laundry, fertilizer, and food processing facilities relied on buckets of these white granules stacked in their storerooms. Modern research, everything from batteries to biology, still borrows from the same ancient knowledge.
Ammonium chloride looks simple: tiny, transparent or white cubes, odorless, each grain easy to measure. This salt comes from the straightforward interaction of ammonia and hydrochloric acid—one of the first pure chemicals I learned to make in school. Its chemical formula, NH4Cl, points to a mix of a mild base and a strong acid, which helps explain its slightly sour taste and ready solubility. Large-scale use covers everything from galvanizing metals and regenerating batteries, to cough syrups and fire extinguishers. Grocery and pharmacy shelves show off its less industrial side; licorice candies owe their tang to ammonium chloride, and pharmacy cough remedies count on its ability to loosen thick mucus. The stuff doesn’t draw the same curiosity as exotic lab reagents, but the world leans on it just the same.
The first time I handled ammonium chloride, I noticed its fine, gritty texture—almost silky, unlike table salt’s sharp edges. It dissolves in water without fuss, releasing a cooling sensation because it draws in energy as it breaks up. In the lab, this property makes it handy for quick cold packs. Ammonium chloride starts to break apart when heated, splitting into ammonia and hydrogen chloride gases at around 338°C. The crystals sublimate with enough heat, a trait that makes it easy to separate from other solids in a mixture. Though stable and non-flammable by itself, ammonium chloride won’t sit quietly near strong bases or oxidizers. Its mildly acidic solution can corrode soft metals but won’t trouble stainless steel or ceramics. Anyone handling this powder long enough develops a knack for storing it away from dampness, as moisture invites clumping and slow degradation.
A supplier takes ammonium chloride straight from the production line to packaging, marking bags or bottles with batch numbers, purity (usually above 99% for food and pharmaceutical grades), and intended use. Those three letters—NH4Cl—stand alongside hazard warnings: “Store in a dry place,” “Keep away from incompatible substances,” “Avoid inhalation of dust.” In my own years buying chemicals for the lab, I learned to scan for those specs. Regulations demand clear statements on country of origin, manufacturing date, and any additives used for food processing. Food-grade product must skip every contaminant test, from heavy metals to arsenic traces. Users in the battery or galvanizing world read for particle size and moisture content, not candy makers’ concern about taste and safety. Honest labeling builds trust, making the supply chain work without second-guessing every white powder delivered.
Traditional manufacturers pass a steady stream of ammonia gas through concentrated hydrochloric acid. The reaction bubbles and steams, throwing out ammonium chloride in a cloud. Factories often collect this in large settling tanks, letting the salt settle before filtration, washing, and drying. Some routes reclaim ammonium chloride as a byproduct from the Solvay process (better known for soda ash), where it spins out while processing sodium chloride and limestone. Growing up in a rural area, I watched small workshops create batches for local shops using just glassware and stove heat, cooling the vapor to get pure crystals. The biggest production lines automate all of this, adding steps to purify, dry, and sometimes grind the salt for different customers’ needs. Despite the volume, the process relies on a reaction my own high school chemistry set could handle—no elaborate equipment required.
If you pour ammonium chloride into a basic solution, like sodium hydroxide, ammonia rises out, sharp and smelly. Metal finishers spread it on hot iron, where it reacts to remove oxide scales, prepping the surface for tin or zinc. In organic synthesis, ammonium chloride helps drive some substitutions, offering up its ammonia group for small molecule building blocks or acting as a weak acid when needed. It features in buffer solutions for biochemistry experiments, especially where precise pH means the difference between working DNA and wasted effort. Though the salt itself stays simple, researchers play with modifications—adding trace minerals, blending with other salts for targeted agricultural uses, altering particle size for more controlled release, or adding coatings to fit medical or food applications. Most of these tweaks emerge where a standard product fails, like adding anti-caking agents to keep food mixes fresh or binding it into slow-release fertilizer pellets.
Over the years, I’ve stumbled across a mess of names for ammonium chloride. Old books call it sal ammoniac. Some chemical supply catalogs list it as amchlor, especially in industrial settings. Food processors prefer the simple “ammonium chloride,” though in northern Europe, it sometimes appears in licorice ingredient labels as salmiak. Certain pharmaceutical guides use the Latin “Ammonii Chloridum,” especially where compounding is involved. Steel and metallurgy manuals often just say “flux” or “cleaning salt,” leaving newcomers to guess the actual composition. Even in agriculture, the same crystals might be sold as “nitrogen supplement” or “soil amendment.” Knowing these alternative names comes in handy, particularly for anyone tracking regulations or managing imports, as different authorities use their own terminology based on where the chemical ends up.
Working with ammonium chloride rarely involves high drama, but basic caution wraps every stage. The dust can irritate the lungs, nose, or eyes, so anyone running large batches or mixing dry product wears masks and goggles—the same rule my old lab supervisor drilled into all newcomers. Chemical storage standards say to keep it in tightly closed containers, away from heat, strong acids, and bases. In food factories, strict cleaning cycles ensure no cross-contamination. The U.S. Occupational Safety and Health Administration (OSHA) sets exposure limits, pegging ammonium chloride fumes at no more than 10 mg/m3 for an 8-hour shift. European agencies echo those guidelines. Anyone loading or unloading bulk shipments gets proper gloves, and spill kits include plenty of water and cleanup gear to avoid kicking dust into the air. Training workers on safe transfer practices—mistakes can lead to respiratory problems or, less often, skin rashes—reduces every day risks. Emergency data sheets detail first aid and fire-fighting measures, consoling for anyone with a nagging sense of “what if.”
Factories from Asia to North America run through tons of ammonium chloride each year, feeding it into dry cell battery production where it carries charge between electrodes, a quiet but crucial role. Cleaning and fluxing lines at tin or zinc plating shops keep barrels in the corner, using them to draw oxide layers off metal before applying a new finish. Textile makers rely on the chemical for dyeing and printing, where it helps fix color onto fibers. Pharmacies use pharmaceutical-grade product in expectorants—those “chesty cough” syrups many families swear by. Food manufacturers in Nordic countries sprinkle it into licorice, producing a signature taste both shocking and addictive. On farms in some regions, ammonium chloride enriches soil or adjusts pH. Laboratories use it in buffers, analysis kits, or protein separation experiments. Even fire extinguisher companies pick ammonium chloride for its cooling and smothering qualities in dry chemical powders. Each application calls for a slight shift in purity or processing, but the same powder moves smoothly from industrial to culinary and clinical settings.
Scientists have not left ammonium chloride in the past. Analytical chemists push its limits in separating proteins or modifying polymer reactions, using its buffering qualities to keep sensitive processes humming. Battery engineers remain keen on improving charge capacity and shelf life, often looking at innovative mixes involving ammonium chloride in electrolyte solutions. Food technologists study ways to mask its intense taste, so that licorice treats appeal to wider markets without losing the familiar sting. Agricultural researchers spend seasons testing ammonium chloride against other nitrogen sources, hoping for better yields in tough soils with less runoff and environmental stress. Pharmaceutical labs develop delivery systems that blend ammonium chloride with slow-release coatings, focusing on targeted cough medications and improved absorption. Most development rides on real-world needs for improved process efficiency and product safety. Reports showing gains in crop productivity or breakthroughs in medical formulations highlight how basic chemicals can still spark new ideas given enough curiosity and investment.
No chemical escapes the microscope these days, least of all something with food and pharmaceutical exposure. Toxicologists review studies measuring how much ammonium chloride animals or people can handle before problems show up. Swallowing moderate amounts produces mild irritation, often limited to upset stomach in adults. High doses, whether deliberate or accidental, can depress blood pH, leading to metabolic acidosis—a risk spelled out on every package intended for clinical or veterinary use. Skin exposure rarely causes trouble unless in direct, wet contact for hours. Long-term animal tests show little cancer risk, but European regulators require regular revalidation. Food authorities in both the U.S. and E.U. set strict limits: the FDA considers ammonium chloride “generally recognized as safe” for food use up to specified levels. Teachers still use live demonstrations to explain chemical toxicity versus hazard: ammonium chloride, with its low volatility, does not behave like cyanide or lead, but its handling still deserves respect. This balance between utility and caution marks most progress in chemical safety.
Looking ahead, ammonium chloride shows potential well beyond its long-held niches. As battery technology advances and the world leans into renewable energy storage, researchers scour familiar chemicals for improved performance—ammonium chloride, that stalwart of old dry cells, gets tested for new roles in supercapacitors or eco-friendly salt batteries. In agriculture, global conversations about soil damage and water contamination push companies to refine fertilizers using nitrogen compounds less likely to leach. Ammonium chloride offers controlled release when blended carefully, cutting down greenhouse gas emissions and promoting soil health. Biotechnology companies apply its buffering strength to enzyme production and therapeutic proteins, solving modern technical problems with a trusted classic. Most of the real growth rests in fine-tuning: smarter coatings, less dust, targeted blends for crops, and formulations that unlock new markets from North America’s farmlands to Asia’s electronics powerhouses. Every trend, every new set of regulations, drives incremental changes in how this chemical connects old knowledge with future needs.
Talk to anyone who’s spent time in a laboratory, and chances are they’ve handled ammonium chloride at some point. It's a chemical with plenty of everyday uses that reach way beyond the walls of a lab. As someone who grew up around both a hardware store and a family full of teachers, I’ve seen ammonium chloride take shape in all kinds of settings—sometimes sitting in plain sight, other times tucked away, quietly making things happen.
If you’ve ever scrubbed away stubborn rust from old tools, you might have noticed that it pops up in metalwork. Metalworkers count on it to clean the surfaces of metals, especially before soldering. It removes oxidation so the solder grabs hold. No fancy equipment needed, just some elbow grease and this powder.
In the medicine cabinet, doctors and pharmacists use it for a very different purpose. Ammonium chloride shows up in cough medicine. It can break up mucus, helping to clear congested airways. Hospital pharmacies sometimes rely on it during emergencies to help adjust body chemistry, especially for folks whose kidneys need a nudge to balance acids and bases. The science here is straightforward—bring pH in line, help the body keep running as it should.
Not everything connected to ammonium chloride involves heavy industry or hospital corridors. It even has a home in the kitchen, though not in the way most people imagine. Bakers never sprinkle it on bread, but it’s hiding in licorice. In places like the Netherlands and Finland, salty licorice candy owes its strong, unmistakable flavor to ammonium chloride. Kids in those countries grow up eating it, and it’s as much a part of their childhoods as peanut butter sandwiches are for many Americans.
Farmers use it too—mainly as a supplement in animal feed. Dairy cows sometimes benefit from its ability to support urinary health. It helps create the right conditions in a cow’s body to reduce the risk of certain conditions linked to high pH in urine.
The fact that ammonium chloride is so versatile speaks to its utility, but it also means people need to handle it carefully. Its use in food always comes in small amounts, and health agencies keep a close eye on those levels. In workplaces, anyone using it for cleaning or soldering makes sure to wear gloves or a mask if there’s dust floating around. Regulatory agencies like the FDA and EFSA set strict guidelines for both food and industrial use.
While I’ve never seen anyone get sick from a salty licorice binge, I have seen what happens if someone handles too much without proper care—mostly irritated skin or a bad cough. Knowledge, a clear set of rules, and a respect for safety gear keep these risks in check.
As more people move toward greener chemistry and safer workplaces, manufacturers turn to better training programs and improved ventilation systems. Some companies substitute less hazardous chemicals when possible, but for certain jobs, ammonium chloride remains the go-to. The key will be using good science to keep both people and the planet safe, while not losing the practical benefits this chemical still offers across so many corners of life.
Most people bump into ammonium chloride without realizing it. It pops up in cough syrups, licorice candies, fertilizers, and even batteries. This white salt brings a salty-sour tang to snacks, and it plays a big part in keeping crops healthy. In warehouses, it's stacked in sacks. In labs it sits on shelves, waiting for the next experiment.
Skin doesn’t burn instantly from a dab of ammonium chloride, but repeated exposure dries out your hands and may cause irritation. Eyes react faster—dust or tiny crystals sting and leave eyes red. Breathing in its dust tickles your nose and can set off sneezing fits, coughs, and that scratchy-throat feeling. Bigger doses may make your chest feel tight or cause wheezing, especially if you have asthma or allergies.
Accidents spike where safeguards slip. A moment’s inattention sends powder into the air, onto faces, or under nails. After several years working around chemicals, I’ve seen folks shrug off masks and gloves, only to end up with cracked knuckles and watery eyes. A friend once splashed a solution and spent hours rinsing his burning irises. Most recovered after basic first aid and good soap, but ignoring the basics brings nothing but regret.
Kids poking around cleaning products or factory workers moving sacks see the most danger. The more you scoop, pour, or mix, the greater your chance of breathing in dust or rubbing it into your skin. If you have open cuts, ammonium chloride bites a little more. Asthma suffers need to pay extra attention since dust brings along breathing flare-ups.
Medical research and workplace safety standards set limits for exposure. Ammonium chloride doesn’t stack up like lead or mercury on the danger scale, but safety sheets call for respect. The Occupational Safety and Health Administration (OSHA) recommends limiting exposure to minimize irritation. Ingesting large amounts by accident can bring nausea, vomiting, or belly pains. Most household uses include only trace amounts, meaning candies and syrups steer clear of big risks. The European Food Safety Authority confirms it doesn’t harm in small, regulated doses.
Gloves, dust masks, and goggles become essential in busy environments. Cleaning up spills right away keeps floors dry and prevents skin or eye contact. Most mistakes happen on rushed days or when someone forgets their gear. I learned after a single bout of redness that it’s worth a few extra seconds to gear up before scooping or pouring.
Washing hands well stops problems before they start. After finishing a job—whether in the lab, the warehouse, or the garden—simple soap and water wash away any leftovers. Keeping ammonium chloride away from food preparation counters and out of children’s reach adds another layer of protection. Labels and storage matter as much as the gloves themselves.
Paying attention dissolves most of the risks. Safety data sheets give the rundown, but real safety comes from routine. Protect exposed skin, keep eyes out of the line of fire, wear a mask in dusty zones, and keep containers closed when not in use. Every task gets easier—and safer—when you slow down, follow directions, and take a moment to tidy up. In the long run, smart habits beat shortcuts every time.
Anyone who has handled ammonium chloride can tell you—this chemical looks pretty unassuming. It shows up as a white, crystalline solid, similar to table salt at first glance. If you run your fingers over it, you’ll notice its fine grains don’t clump much in dry air. If you crush it, the powder gets even finer, giving it a soft, almost silky feel. Sometimes, the crystals might take on a slightly gray shade, but most batches end up pure white, making it easy to spot any impurities.
Pop ammonium chloride into water, and it dissolves quickly. Add a spoonful to a glass and you’ll see those white crystals vanish without much stirring. This ready solubility sets it apart from other salts used in labs and factories. The dissolve-and-disappear act not only helps in chemistry class, but also makes ammonium chloride a reliable material in the food industry and in batteries. There’s a cooling sensation when dissolved, which points to its endothermic process—energy snatched from the surroundings, not given off. If you’ve ever mixed it into a sports drink powder or notice cough drops with a cool finish, this cooling effect is often behind it.
If you heat ammonium chloride, it skips the liquid phase entirely and jumps straight from solid to gas. This trait, called sublimation, used to impress me in the school science fair: a beaker of the stuff, a flame, and suddenly there’s a white smoke filling the air. In reality, that’s not smoke—it’s a cloud of tiny solid particles forming again as the gas cools. This property proves valuable in the lab. Scientists use ammonium chloride to demonstrate phase changes or purify mixtures by simple heating.
Hold it to your nose, and you won’t pick up much of a smell. The taste is sharply salty and cooling, showing up in specific foods and medicines. People in Scandinavia might recognize it from salty licorice candies. As someone who grew up experimenting with kitchen science, I learned quickly not to taste things from the chemistry set, but ammonium chloride stands as an exception, with its presence in food-safe products and remedies for sore throats.
Run a metal spoon over it, and you’ll find ammonium chloride soft enough to scrape. The crystals break apart without much effort. Its density stays moderate—about 1.53 grams per cubic centimeter—so it sinks gently in water. This kind of property means storage remains straightforward, and you don’t need fancy equipment for handling.
Keep ammonium chloride sealed away from moisture, and it’ll last almost indefinitely. Humid air turns it sticky as it pulls water from the atmosphere; soon enough, those dry crystals start clumping. Plenty of old-school apothecaries and warehouse managers have stories about forgotten jars turning into bricks after sitting through rainy seasons.
Breathing in large amounts of ammonium chloride dust will irritate lungs and eyes. Some careful handling goes a long way here—ventilation and face masks keep workers safe in factories and classrooms. Like most salts, it poses little risk in small, controlled uses, but larger spills need clean-up and disposal by people who know what they are doing. Training kids and beginners in basic safety pays off quickly with hands-on materials like this one.
Ammonium chloride finds its way into labs, food processing, metalwork, and even in medications. Whether you’re overseeing a school chemistry lab or working in a factory, treating chemicals with respect isn’t just a box to tick on a safety checklist. Many folks learn the hard way that a minute spent now can spare days of cleanup and hassle later. Storing ammonium chloride isn’t just an afterthought—a smart approach keeps people safe, products reliable, and workspaces running smoothly.
I remember the first time a bag of ammonium chloride sat too long in a humid storeroom. The crystals clumped, making them pretty much unusable for lab work. Moisture transforms ammonium chloride from a tidy, easy-to-weigh powder into a sticky mess. The solution looks simple enough: leave the container shut and store it in a spot that stays dry. In practice, this means using airtight jars, buckets with secure lids, or original sealed packaging. Shelves work well—just steer clear of the floor, where a spill, leaky pipe, or damp patch brings in extra trouble.
Heat brings out the worst in many chemicals, and ammonium chloride fits that bill. High temperatures speed up decomposition and might even trigger a chemical reaction if the container gets too hot or comes into contact with metal filings. A spot away from heaters, furnaces, or direct sunlight becomes the smarter choice. Think of the same rules you’d use for storing flour or sugar—cool and away from extremes. Simple habits pay off, especially over the long haul.
Ammonium chloride isn’t especially dangerous on its own, yet the real risks show up after an accidental mix with strong bases or concentrated acids. Hydrogen gas and other irritants form when someone lumps ammonium chloride in with cleaning supplies, bleach, or open bottles of ammonia. Segregate chemicals by what sets them off, not just by their alphabet on a shelf. Labeling each shelf and sticking to clear, separate storage reduces confusion—even my stubborn colleagues see the difference in fast-moving production lines.
Though ammonium chloride doesn’t fume unless heated, a poorly ventilated storeroom turns a spill into a breathing issue fast. Even one bag ripped open in a closed closet leaves a lingering tang in the air. I’ve walked into storerooms that made my eyes water before I even found the culprit. If a storeroom window isn’t an option, a basic mechanical exhaust fan prevents buildup. Good air, good work, fewer headaches.
Handwritten tape on jars fades; stickers peel off. Permanent labels—ideally with date received, expiration, and hazard information—keep everyone on the same page. During audits or inspections, one glance at a label can spare a half-hour of shuffling bags or guessing at contents. Couple that with a storeroom log, and repeat mistakes fade away. For anyone juggling many chemicals, this habit pays off more than any fancy storage cabinet money can buy.
Smart storage doesn’t require high-tech solutions. Just a few tweaks—a dry space, firm lids, clear labels, cool temperatures, and a bit of separation—sum up the difference between a manageable supply and a risky mess. I’ve seen it in schools, shops, commercial food plants, and home workshops. Sound storage builds trust, avoids waste, and—most important—keeps people safe without extra fuss.
Ammonium chloride shows up in places we’d never guess—cough medicine, fertilizers, even old-school fire extinguishers. It sounds like something that belongs in a chemistry class, but for many folks working in food, agriculture, or manufacturing, it’s part of daily life. I’ve worked next to labs and warehouses stocked with this stuff, and the concern isn’t just theory. Getting a handle on what’s at stake matters for anyone around it, whether at work or at home.
Breathing in ammonium chloride dust or fumes stings. You notice it fast: coughing, a scratchy throat, burning in your nose. Spilled granules, even the dust scattered in the air, can set off a coughing fit by irritating the airways. Folks with asthma have it worse; exposure might tighten the chest and trigger attacks. The Occupational Safety and Health Administration (OSHA) set exposure limits for a reason. Overloaded lungs work harder, and it’s not calming your nerves staring at a hazy cloud on the warehouse floor.
Touch matters, too. I’ve gotten ammonium chloride powder on my skin by accident. Sweat blends with those crystals and itches start up, sometimes followed by redness or small rashes. Rub your eyes during clean-up, and that burning sensation lashes out. In my experience, soap and water give relief, but you stay alert for lingering redness or swelling.
Ammonium chloride isn’t just industrial; it even goes into some candies and cough suppressants. Eating a tiny bit is usually safe because the body flushes it out quickly. Raise that dose, though, and things go south. Stomach aches, nausea, and vomiting don’t sound rare for folks who’ve ingested too much. As a diuretic, ammonium chloride can upset body chemistry, lowering blood pH and causing metabolic acidosis. In hospitals, doctors keep a close eye on patients given medical doses for that reason.
Accidental swallowing from workplace spills pushes the risk much higher. Cases have sent folks to the ER with confusion and breathing trouble. Acute symptoms hit hard if pre-existing health problems are in the mix. I’ve seen company training emphasize never ignoring powder on lunchroom tables or drink areas during shifts.
High-level exposure isn’t just a bad day, it can threaten life. OSHA’s permissible exposure limit—10 mg per cubic meter over an eight-hour shift—reflects studies showing lung damage when that barrier’s crossed. As with any chemical, repeated or long-term exposure multiplies risks. A Swedish study found workers exposed to ammonium chloride dust for years had more frequent respiratory issues.
Firefighters used to use ammonium chloride-based extinguishers. Clearing up after fires, inhaling leftover fumes or residue, caused lasting effects in some cases—long-term lung changes and chronic cough have all been reported.
Staying safe starts with respect for handling guidelines. Gloves, masks, and well-ventilated workspaces become non-negotiable, not optional extras. Industrial safety data sheets spell out spill clean-up steps, but nothing replaces real training. Good workplaces run regular drills and pay attention when anyone complains of cough or irritation. Air quality monitors have proven worth it, spotting rising dust before symptoms spread.
Workers should get regular health checks. Immediate medical advice turns a scary exposure into a handled incident. Above all, spreading real information—never treating ammonium chloride like a harmless powder—shifts risk down. Listening to stories from exposed colleagues adds urgency. Changes don’t take big budgets, just steady attention and valuing health over short-term convenience.
| Names | |
| Preferred IUPAC name | azanium chloride |
| Other names |
Sal ammoniac Ammonium muriate Salmiac |
| Pronunciation | /əˈmoʊniəm ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 12125-02-9 |
| Beilstein Reference | 3587156 |
| ChEBI | CHEBI:31206 |
| ChEMBL | CHEMBL1357 |
| ChemSpider | 554 |
| DrugBank | DB01378 |
| ECHA InfoCard | 03e4b8e1-e9ec-4f1f-9a18-7a500c7d4d84 |
| EC Number | 215-749-8 |
| Gmelin Reference | 82238 |
| KEGG | C01537 |
| MeSH | D000647 |
| PubChem CID | 25517 |
| RTECS number | BP4550000 |
| UNII | F87A39M527 |
| UN number | UN3077 |
| Properties | |
| Chemical formula | NH4Cl |
| Molar mass | 53.49 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.527 g/cm³ |
| Solubility in water | 36 g/100 mL (25 °C) |
| log P | -3.27 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 9.24 |
| Basicity (pKb) | 8.10 |
| Magnetic susceptibility (χ) | -33.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.642 |
| Dipole moment | 1.47 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 94.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -314.43 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | −314 kJ/mol |
| Pharmacology | |
| ATC code | R05CB01 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes eye and skin irritation, may cause respiratory irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS07, GHS09 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 2-0-0 |
| Autoignition temperature | 630 °C (1166 °F) |
| Lethal dose or concentration | LD50 oral rat 1650 mg/kg |
| LD50 (median dose) | LD50 (median dose) of Ammonium Chloride: 1650 mg/kg (oral, rat) |
| NIOSH | SN4725000 |
| PEL (Permissible) | 10 mg/m3 |
| REL (Recommended) | 4 mg/kg bw |
| IDLH (Immediate danger) | 250 mg/m3 |
| Related compounds | |
| Related compounds |
Ammonium nitrate Ammonium sulfate Sodium chloride Potassium chloride Ammonium carbonate |
