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Growing up around a family-run hardware store, chemicals always sparked my curiosity long before I ever peered at a scientific journal. Tetrapropylammonium chloride, tucked into the very broad basket of quaternary ammonium salts, quietly entered chemical literature in the earlier half of the 20th century. Labs reaching past simple organic syntheses sought out new ways to tailor molecules for industry and research. During the postwar boom, with catalysis and solvent systems stretching old boundaries, this compound's preparation and utilization gained some momentum. It never grabbed headlines, but chemists searching for effective phase transfer catalysts saw value—and as green chemistry goals push for lower toxicity and greater efficiency, its legacy grows. Over time, researchers evolved its manufacture and applications, such as modifying the ways we work with inorganic framework syntheses or as intermediates in pharmaceutical pipelines.
Ask anyone involved with laboratory or industrial chemistry about quaternary ammonium salts, and they’ll likely describe Tetrapropylammonium chloride as sturdy, reliable, and just a bit under the radar. This chemical stands out for its role as an organic cation source—a mouthful, sure, but indispensable for tasks involving zeolite formation, facilitating the assembly of complex crystalline lattices. Its utility stretches into catalysis, surfactants, and specialty material syntheses. It rarely steals the show, but any process engineer or academic toiling in material science or organic synthesis recognizes its contribution as essential, not filler.
Confronted with a bag or bottle of Tetrapropylammonium chloride, I see a white or off-white solid, crystalline and hygroscopic, with a notable ability to pull moisture from air. This property, often a hassle when working in humid climates, pushes those handling it toward careful storage. Solubility in water tips toward the high end, though its interaction with organic solvents makes it flexible in lab protocols. Chemically, it's stable below high temperatures and resists breaking down unless introduced to strong bases, oxidizers, or elevated heat. Its molecular formula—C12H28ClN—offers four propyl groups orbiting a central nitrogen, and this specific structure influences its role in crafting designer molecules or guiding inorganic structures to form orderly frameworks. Its melting range often lands above 200 °C, and the presence of the chloride counterion serves double duty both in balancing charge and driving certain reactivity under the right circumstances.
On any lab shelf, labeling accuracy means less risk and more peace of mind. Tetrapropylammonium chloride carries standard warnings due to mild irritant potential. Chemical labels should indicate purity grade and presence of moisture, as these impact results in sensitive syntheses. From bottles supplied to major research institutions, purity often exceeds 98%, and manufacturers sometimes flag any residual starting materials or by-products. Test results reported by trusted labs keep surprises off the workbench. Accurate batch IDs support recalls and troubleshooting, reducing downtime for those scaling up to pilot runs or industrial processes. It’s surprising how often minor labeling missteps knock entire production lines off schedule—standardized presentation of technical specs makes sizeable differences in workflow continuity.
Colleagues in synthetic chemistry circles sometimes swap tales of poor yields and side reactions, often solved by tweaking or rethinking reaction routes. The typical method for Tetrapropylammonium chloride involves an alkylation of ammonia using propyl halides—usually propyl chloride—with an eye on controlling exothermicity and side products. Using solvents like acetonitrile or ethanol, the process benefits from measured heat and careful addition of reagents. Post-reaction workup involves removing unreacted starting materials, followed by crystallization or recrystallization to chase off colored impurities. Washing with non-polar solvents helps strip away grease and odorous leftovers. It might sound straightforward, but kinetic quirks and side reactions can crop up—small factors such as even humidity and the choice of purification route threaten overall yield or purity.
Handle Tetrapropylammonium chloride with a sense of respect for its modest but versatile chemistry. While not explosive, it reacts under strong base or at high temperatures, allowing for cation exchange reactions and serving as a source for further functionalization. For instance, reacting with silver salts can replace the chloride with other anions, enabling its use as a cation template or intermediate. In more advanced material science projects, scientists employ this molecule to modulate crystal growth or stabilize reactive intermediates. Some organometallic syntheses depend on it as a phase transfer catalyst, shuttling reactants between aqueous and organic layers, which traditional salts cannot accomplish without similar cationic structures. In these settings, tweaking the counter ion or alkyl chain length tunes selectivity or performance—always a striking example of how a small, seemingly unremarkable molecule influences reactions far bigger than itself.
Chemical industries and researchers know Tetrapropylammonium chloride by a handful of names, leading to label confusion if ordering teams skip the fine print. The most common alternatives include N,N,N-Tripropylpropan-1-aminium chloride and TPACl. Catalogs from established suppliers often list it under these names or CAS number 136-91-2. Clear nomenclature prevents accidental misordering of structurally similar, yet functionally distinct, compounds.
Personal safety takes precedence in any interaction with Tetrapropylammonium chloride. Though it carries a moderate risk profile—mostly irritant to skin, eyes, and lungs—you cannot ignore good lab hygiene. Storage in well-sealed, moisture-free conditions preserves integrity and prevents unnecessary exposure. It irritates on contact, so gloves and eye protection go beyond formal requirement and reflect plain good sense. Its dust poses problems if inhaled, making local ventilation or work within a fume hood essential. In spill scenarios, dry sweeping and ventilation offer practical control, and disposal must follow local regulations, especially because release into open water could threaten aquatic habitats—it’s not overtly biocidal at trace levels, but recurrent exposure never bodes well for sensitive environments. Too often, labs grow complacent with moderately hazardous chemicals, only to regret avoidable accidents. On the operational side, training matters more than documentation or written protocols. Handling and emergency procedures should move from paper to workplace culture, engrained in daily routine. I’ve seen slips ignored for the sake of speed; a culture of safety saves time and money over cutting corners.
Tetrapropylammonium chloride’s niché runs deep. Zeolite synthesis, for one, would not reach contemporary complexity or performance without the organic cation’s intervention—it steps in as a template during hydrothermal synthesis, guiding aluminosilicate frameworks to precise pore geometries. Move over to organic laboratories and you’ll spot it ferrying ions across phase barriers, helping with stubborn bond formations. Its action in phase transfer catalysis, acting not only as a facilitator but as a fine-tuning element, impacts yields and selectivity in pharmaceuticals, agrochemicals, and specialty polymers. Tried-and-true performance in industrial applications gives plant managers and chemists confidence during scale-up. My own university days saw batches of specialty materials assembled in part thanks to its stabilization of otherwise-finicky intermediates. The beauty lies in its simplicity: it brings opportunities to complicated chemistry, opening up reaction possibilities and material properties not accessible by simpler salts.
Researchers rarely grant headlines to basic salts. Still, Tetrapropylammonium chloride generates steady, meaningful progress in several fields. Material scientists depend on it for templating tasks during preparation of advanced zeolites and mesoporous materials. Catalysis researchers routinely investigate how swapping cation sizes or shapes translates into faster reactions or greener routes. Environmental chemists probe its effect on pollutant breakdown and removal, keenly aware that every improvement in catalysis or selectivity brings big downstream savings. There’s also a steady drumbeat in pharmaceutical research—screening for better intermediates, safer solutions, and more reliable yields. University chemistry departments, working with ever-shrinking budgets and surging expectations, often rely on chemicals like this one because it’s affordable, accessible, and widely documented. R&D never carries the drama of drug launches, but in these quieter, foundational compounds, whole new classes of technology, medicine, and industry often start with humble steps forward.
Every compound entering wide use, especially those with environmental exposure risk, brings regulatory scrutiny and valid concern. Research around Tetrapropylammonium chloride generally finds low to moderate toxicity, with acute exposure causing skin and eye irritation, and chronic exposure—rare in laboratory conditions—bringing about more significant respiratory issues. Its oral toxicity stands higher than table salt but much lower than well-known hazardous substances. Regulators and academic groups watch its aquatic impact, spotting sensitivity among fish and invertebrates at higher concentrations. Wastewater treatment plants rarely spot trouble, but wide distribution or spillages could build up in sediment or bioaccumulate under the right conditions. These findings push operators to avoid routine release, reinforcing the need for responsible handling and disposal protocols. I’ve seen projects derailed for underestimating chronic environmental exposure of otherwise “safe” salts—careful monitoring and ongoing, independent study form essential parts of its continued use.
Times keep shifting toward sustainability and more demanding chemical performance. Tetrapropylammonium chloride, once wielded as a quiet supporting player, now finds itself invited into a broader range of applications—driven by new material science initiatives, advanced catalysis goals, and environmental remediation needs. Researchers actively look for less toxic, more effective alternatives to older phase transfer systems, and refinement of synthesis methods aims to further cut down on waste and by-products. Novel uses in electrochemistry and nanomaterial construction suggest even broader horizons. As global carbon reduction efforts push chemical manufacturers into adopting greener processing routes, compounds offering predictable, tunable cationic behavior—without high human or ecological burden—come into sharper focus. I see Tetrapropylammonium chloride standing out more by the year, not for being extraordinary, but for consistently doing its job without posing unnecessary risk—precisely the kind of dependable chemical our changing world needs.
People who spend their days in chemical research or specialty manufacturing run into some complicated-sounding ingredients. Tetrapropylammonium chloride stands out with its long name and specialized uses. I remember my early months in a university research lab, stumbling onto a bottle with this wordy label. It looked intimidating, but once I dug into its use, it all made sense. This salt plays a bigger role in modern science and technology than its dusty jar suggests.
In synthetic chemistry, scientists rely on compounds like tetrapropylammonium chloride to drive reactions that wouldn’t work as smoothly otherwise. For instance, it acts as a phase-transfer catalyst. Instead of leaving reactants stubbornly stuck apart, it helps them meet and react by shuttling ions between water and organic mixtures. Anyone who's done undergraduate lab work can tell you: that kind of help means fewer headaches and fewer failed experiments.
The importance stretches beyond the classroom. Professionals in drug development and new material research also tap into this compound’s power. Producing advanced drugs often means moving ingredients between oily and watery mixtures. Relying on a catalyst like tetrapropylammonium chloride moves things along, saving both time and costly resources. Pharmaceutical production already faces enough delays—cutting a single step might mean safer treatments hitting shelves sooner.
Beyond laboratories, this ingredient lines up for several key industrial roles. In the manufacture of zeolites, tetrapropylammonium chloride acts as a template. Zeolites are porous minerals, like tiny molecular sieves. Oil refining plants use them to turn crude oil into gasoline and other fuels. The template molecule shapes pores in the crystal as the zeolite forms, then gets removed, leaving behind a perfectly crafted structure. A lack of the right template can mean a less efficient refinery, higher energy costs, and more environmental strain.
Another spot where this compound steps up: the electronics industry. Creating specialty coatings, etchants, and certain types of conductive plastics often calls for tetrapropylammonium chloride. Think of all the screens, circuits, and chips built every day. Improving electronics means constantly refining materials, and each improvement, no matter how small, connects to real-life benefits—faster devices, longer battery life, less e-waste.
With great usefulness comes responsibility. Tetrapropylammonium chloride, like many synthetic chemicals, warrants careful storage and handling. Some industrial processes produce waste that could harm the environment if left unchecked. Companies ignore safe practices at their own peril. Lab workers—myself included—have learned the hard way that good gloves and fume hoods aren’t optional. Regular staff training and well-maintained equipment go hand in hand with using chemicals like this safely.
Environmental awareness is rising too. Researchers look for biodegradable options and less hazardous methods wherever possible. Industry leaders who put money toward greener alternatives not only follow regulations—they leave a better future for everyone. Open information about risks, proper disposal, and safer replacements makes a big difference.
Tetrapropylammonium chloride may not show up in household news, but it plays a part in shaping the products we count on. From fuels to medicines to electronics, this compound helps drive progress. Responsible use and ongoing research will keep that progress pointing in the right direction.
Tetrapropylammonium chloride crops up in the chemical world as a quaternary ammonium compound. This substance turns up in lab settings, in certain industrial processes, and sometimes as a phase-transfer catalyst during organic synthesis. Honestly, most folks will never see it outside a chemistry class or a specialty workplace. For the handful who do cross paths with it—usually scientists, lab techs, or folks working around chemical plants—knowing what it does to your body makes a big difference.
Safety sheets flag tetrapropylammonium chloride as an irritant. If you get it on your skin or in your eyes, you notice pretty quick—redness, itching, and maybe burning. Someone breathing in its dust can expect a sore throat, maybe some coughing or feeling short of breath. Ingesting it risks stomach pain and other digestive problems. While these symptoms sound manageable with prompt rinsing or cleaning up, the stories always point one way—take exposure seriously, even if the dose is small.
I’ve spent enough time in university labs to know just how fast something can go from “contained” to “where’s the eyewash station?” Most chemical accidents don’t come from wild spills, but from simple slips: cracking a container seal too hard, picking up the wrong pipette, or just one jolt while carrying a flask. For tetrapropylammonium chloride, it means a real incentive for gloves, goggles, and strict labeling.
Nobody likes playing guessing games with their health. Right now, research on chronic effects from this compound looks thin. There isn’t a stack of cancer studies or proof of impacts on human DNA. At the same time, quaternary ammonium compounds sometimes leave residues and can build up. Some of their relatives have gotten attention for causing skin allergies over time. That’s never good news for anyone handling chemicals daily.
If you’re tasked with handling any quaternary ammonium salt, understand your risk doesn’t just vanish after a day at work. Even indirect contact can leave a mark. There’s wisdom in what veteran lab instructors always say: Don’t take work home on your hands or your clothes.
Everyone benefits when safety trumps speed. Any lab or processing plant using tetrapropylammonium chloride needs safeguards front and center. Think fume hoods that pull away harmful vapors, gloves that stand up to corrosive agents, storage rooms locked and labeled, safety showers near at hand. Safety officers who answer questions quickly help prevent confusion, not just after-the-fact paperwork.
Education carries real weight here. It’s not about scaring staff into submission; it’s about respect for the material. Clear training, regular drills, honest discussion after mistakes—all of these defend workers better than any thick binder gathering dust.
Staying safe doesn’t have to shut down productivity or innovation. Sometimes, the European Chemicals Agency (ECHA) or US authorities update their hazard ratings as new studies come out. Staying updated matters. Risk assessment evolves, especially for substances that don’t see a lot of publicity. Sometimes, a less hazardous substitute turns out to work just as well, with far fewer risks. Switching over can save future headaches.
Responsibility sits squarely with organizations and leaders to make science safer day in and day out. Individuals also play a part—by asking tough questions, checking labels, and taking small precautions before small risks become big problems.
Tetrapropylammonium chloride carries the chemical formula C12H28NCl. The name spells out the structure clearly: four propyl groups attached to a nitrogen atom, with a single chloride anion balancing the charge. The formula breaks down into twelve carbons, twenty-eight hydrogens, one nitrogen, and one chlorine. Each propyl group brings three carbons and seven hydrogens. Bumping these counts up four times calls for some careful arithmetic, and that’s how the total numbers land. For anyone curious about the backbone, the structure shows off all those propyl groups symmetrically tied to the nitrogen.
Curiosity about this salt often starts in university chemistry labs. Many folks–myself included–have handled it while fussing over phase-transfer reactions or learning about quaternary ammonium compounds. It doesn’t show up on drug store shelves, yet chemists and chemical engineers often keep it nearby. Industries and academic labs value these sorts of salts for their specialty role in both organic synthesis and crystallography.
Looking inside most chemical processes, we find that not all reactants or catalysts get to run the show. Some do the background lifting—facilitating transfer, making certain reactions viable, or stabilizing intermediate products. Tetrapropylammonium chloride turns heads for just that reason. As a quaternary ammonium salt, it acts as a phase-transfer catalyst, bridging the stubborn gap between water and organic solvents. This type of synergy speeds up reactions that might otherwise stall. Companies dealing with fine chemicals, polymers, or specialty materials appreciate how it helps manage solubility headaches and improves yields in synthesis.
With every synthetic or industrial chemical, it’s wise to ask about safety and environmental footprint. Tetrapropylammonium chloride, like its other quaternary cousins, can pose real hazards if handled carelessly. Skin and eye irritation pop up as risks, and spills in the wrong environment may strain wastewater systems. Few people fuss over these hazards at home, but I’ve witnessed accidents in research labs that forced quick thinking and thorough cleanup. It reminds me of how important solid habits around chemical labeling, storage, and disposal remain.
On the environmental front, quaternary ammonium salts can linger in aquatic environments and disrupt microbial ecosystems. Regulatory bodies such as the Environmental Protection Agency monitor and sometimes limit discharge levels for similar chemicals. Good stewardship means tracking inventories, limiting waste, and choosing greener solvents or processes where possible. Lab managers face no shortage of challenges, but the push toward best practices around handling makes a lasting difference.
Experience teaches that improved education and transparency go far. New users in training learn quickly when shown real consequences, not just abstract warnings. Sharing stories about accidents and recovery, offering firsthand accounts of why protocols must stick, and making safety equipment easy to reach strengthens those habits.
Chemical suppliers can take the lead by offering detailed safety data, supporting green chemistry initiatives, and adopting eco-friendly packaging. Researchers who look for alternatives—such as phase-transfer catalysts with better environmental profiles—drive innovation. Small adjustments in choice or process, over many hands and thousands of uses, gradually reduce risk and cost.
Knowing the chemical formula for tetrapropylammonium chloride does more than solve a quiz. It opens up a wider conversation about the chemistry shaping our daily world, the need for responsible stewardship, and the hidden connections between the laboratory and the environment we share.
Tetrapropylammonium chloride pops up in research labs, chemical manufacturing, and some specialty synthesis work. I remember working in an academic lab, where everything involving specialty chemicals had a story behind it—the staple was always: know where things are, keep them in the right spot, and respect what they might do if things go wrong.
From my time in university, mishandling chemicals didn’t just mean wasted resources or delayed experiments. It sometimes landed colleagues in the emergency room. That experience underscored the plain fact: proper storage protects people, protects data, and helps keep costs down by limiting waste. Tetrapropylammonium chloride comes with its risks, so controlling how you store it helps avoid those lessons the hard way.
1. Keep It DryTetrapropylammonium chloride picks up water from the air. I once saw what too much humidity did to a batch of this salt—clumpy mess, ruined. Store it in a tightly sealed container. A desiccator cabinet works well for small quantities. I recommend silica gel packets in the storage area if the budget allows, especially if humidity starts creeping up.
2. Store in a Cool SpotHeat speeds up chemical reactions. Even if this ammonium salt doesn’t spontaneously combust, excess warmth degrades its quality over time. On sweltering summer days, our lab fridge proved its worth—lower temperature kept things stable and extended shelf life. Some facilities opt for dedicated climate control. A simple shelf in a dark corner, shielded from direct sunlight and heating vents, can help if there’s no specialized equipment available.
3. Avoid Light ExposureClear plastic jars sitting in a sunny window sometimes look pretty, but that’s no way to treat sensitive chemicals. Exposure to light encourages breakdown, so opaque jars or at the very least, keeping them out of sight lines is a best bet.
4. Keep Away from Incompatible ChemicalsMixing storage is like mixing up spices—you never want to find out the hard way that two ingredients turn nasty together. Tetrapropylammonium chloride doesn’t play nice with strong oxidizers and strong acids. Our facility color-coded shelf labels so everyone in the room could spot what went where at a glance. Cross-contamination becomes much less likely with some basic organization.
Good storage goes beyond matching chemicals to containers. In my experience, mistakes almost always happen from tiredness or rushing. Clear labels on every jar help, especially if you use both the chemical and the common name. Regular safety training—drills, quick refreshers, or even just a weekly chat—keeps the right procedures top of mind.
One spill is too many. Every time I disposed of open containers or used up a batch, I made sure to use only specifically marked waste containers. A worksite with clearly posted cleanup procedures and spill kits nearby leaves less room for accidents. It’s about keeping people safe and avoiding contamination down the line.
Safe storage isn’t a box-ticking exercise. It’s about respect—respect for the science, the environment, and everyone working with these chemicals. Implementing careful habits saved my old lab both money and frustration. Lower risk means fewer problems and smoother days on the job.
Tetrapropylammonium chloride shows up in the world of surfactants, which slip into shampoos, detergents, and even some cleaning agents you find under the kitchen sink. Surfactant makers lean on this compound because it helps coax oil and water into mixing together. So, every time those two usually stubborn liquids blend into a creamy or foamy texture, there’s likely a quaternary ammonium compound behind the scene. Lab technicians I’ve known appreciate how predictable this chemical behaves during synthesis, so production lines run smoother and produce fewer unwanted byproducts.
I once sat in on a materials science seminar where the production of specialized silica earned a spotlight. Tetrapropylammonium chloride stood out as a structure-directing agent in these stories. This chemical doesn’t just show up for the ride—it shapes the microscopic pores in the silica, helping researchers grow zeolites and other highly ordered structures. These zeolites, in turn, unlock new efficiencies in petroleum refining and wastewater purification. Engineers working with catalysts take special notice since yields and performance can jump up with just the right fine-tuning in synthesis, and this compound gives them that edge.
Scrolling through technical forums late at night, you’ll come across plenty of folks talking shop about electroplating baths. Tetrapropylammonium chloride often pops up here as an additive. Plating managers count on it for controlling how metal ions lay down onto surfaces. Anyone who’s tried to plate a circuit board at home knows how finicky this process can get—too rough, and the metal flakes, too smooth, and it’s brittle. This compound stabilizes the whole act, providing a steadier finish that holds up to scrutiny.
Drug companies searching for new compounds often seek out reliable intermediates to keep reactions heading in the right direction. Tetrapropylammonium chloride does a lot of quiet heavy lifting in this department. It’s part of the choreography that nudges synthesis steps along, letting chemists prepare active pharmaceutical ingredients more cleanly and predictably. A colleague in pharmaceutical manufacturing pointed out that skipping the right ammonium salts often means more headaches, higher costs, and wasted time troubleshooting byproducts no one asked for in the first place.
I remember my early years in a chemistry lab, running organic reactions and scrambling to find reagents that could push reactions over the finish line. This was one that sat on our shelf more often than not. It works as a phase transfer catalyst—a real bridge-builder between oil-like reagents and water-based solutions. Chemists have found ways to scale up their processes, cut back on harsh conditions, and trim down costs just by putting it to use.
This chemical isn’t without its baggage. Waste streams containing tetrapropylammonium chloride ask for careful handling—unchecked, they can harm aquatic life. Wastewater treatment plants have started keeping closer tabs and introducing filtration and breakdown steps just for these types of chemicals. Manufacturers focusing on closed-loop systems, and tighter tracking, lower both environmental footprints and regulatory headaches. Pushing for more biodegradable alternatives takes time, but research groups are starting to make headway.
Tetrapropylammonium chloride holds its own in several industries. Chemists and engineers value tools that turn raw materials into something useful, reliable, and cost-effective. Staying mindful of where it goes after the workday ends matters just as much as its performance inside the factory or lab.
| Names | |
| Preferred IUPAC name | tetrapropylazanium chloride |
| Other names |
Tetrapropylammonium chloride TPACl N,N,N-Tri-n-propylpropan-1-aminium chloride |
| Pronunciation | /ˌtɛtrəˌproʊpiːlˈæməniəm ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 136-91-2 |
| 3D model (JSmol) | ``` data:Tetrapropylammonium chloride 3D; N(+)(C(C)CC)(C(C)CC)(C(C)CC)(C(C)CC).[Cl-] ``` |
| Beilstein Reference | 1718113 |
| ChEBI | CHEBI:87154 |
| ChEMBL | CHEMBL1533126 |
| ChemSpider | 10217 |
| DrugBank | DB11126 |
| ECHA InfoCard | 13b6c540-5f96-4d8c-a4b3-14a1361931b7 |
| EC Number | 208-923-9 |
| Gmelin Reference | 8224 |
| KEGG | C14419 |
| MeSH | D017822 |
| PubChem CID | 66121 |
| RTECS number | TR3150000 |
| UNII | 68F4418E4Y |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C12H28ClN |
| Molar mass | 243.87 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 0.89 g/cm3 |
| Solubility in water | Very soluble |
| log P | -0.8 |
| Vapor pressure | < 0.01 mmHg (20 °C) |
| Acidity (pKa) | -3.0 |
| Basicity (pKb) | 1.82 |
| Magnetic susceptibility (χ) | -62.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.422 |
| Viscosity | Viscosity: 1.3 cP (20 °C) |
| Dipole moment | 6.51 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 286.2 J·mol⁻¹·K⁻¹ |
| Hazards | |
| Main hazards | Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS07 |
| Signal word | Danger |
| Hazard statements | H315, H319, H335 |
| Precautionary statements | Wash thoroughly after handling. Do not eat, drink or smoke when using this product. |
| NFPA 704 (fire diamond) | 1-0-0 |
| Lethal dose or concentration | LD50 Oral Rat 350 mg/kg |
| LD50 (median dose) | 1700 mg/kg (rat, oral) |
| PEL (Permissible) | Not established |
| REL (Recommended) | 10 mg/m3 |
| Related compounds | |
| Related compounds |
Tetraethylammonium chloride Tetrabutylammonium chloride Tetramethylammonium chloride Tetrahexylammonium chloride Tetraoctylammonium chloride |
