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Tetrabutylammonium hydrogen sulfate, sometimes remembered by those who studied classic phase-transfer catalysis, traces its roots back to the growth of organic synthesis in the mid-twentieth century. Before chemists landed on the clever idea of using quaternary ammonium salts for facilitating tricky reactions in two-phase mixtures, many transformations stalled at the boundary between oil and water. The rise of phase-transfer catalysts in the 1960s meant that simple salts gained unprecedented value beyond just being side-products or bystanders in tired laboratory drawers. Over the years, more researchers discovered that the specific hydrogen sulfate variant offered solubility and activity not seen in its chloride or bromide cousins, meaning chemists finally managed to drive sulfuric acid reactivity into nonpolar solvents. People today owe that to a handful of creative researchers armed with little more than glassware, patience, and a truckload of curiosity.
Tetrabutylammonium hydrogen sulfate (TBAHS) looks unremarkable to the naked eye—a white, sometimes sticky, powder that absorbs water from the air faster than you can write its name. In lab catalogs, it usually sits under specialty reagents, popping up wherever scientists need to coax two unwilling reactants together. I’ve worked with TBAHS mainly as a phase-transfer agent, but the reach of this humble salt stretches further. Labs order it for controlling pH in non-aqueous mixtures or as an electrolyte in complex, advanced batteries. While a bottle might linger on a shelf for months, once a synthesis calls for it, no other replacement seems to muster the same blend of availability and performance, especially when compared to clumsier, more corrosive alternatives.
With its chemical formula C16H37N.HSO4, TBAHS often presents itself as a colorless, crystalline powder, though older samples sometimes pick up a yellowish hue from decomposed contaminants. It weighs in at just under 340 grams per mole and melts somewhere above 190°C, though charring can occur before you get a confident melting point. It dissolves very easily in polar organics, like acetonitrile and dimethylformamide, but also stays barely soluble in pure water. That rare balance forms the core secret to its effectiveness—move ions from water to organic phases with far less resistance than raw sulfuric acid or sodium sulfate. I recall more than one project where we abandoned less-soluble alternatives and saw new yields from forgotten reactions. As a salt of a strong acid, its solutions are quite acidic, and it releases odors typical for ammonium and sulfate compounds if mishandled.
Bottles of TBAHS arrive with clear technical sheets. Purity hovers above 98%, and smart suppliers make sure to mention the typical water content, as excess moisture can ruin sensitive applications. Containers will always list precise batch numbers, manufacturing dates, and require storage away from light and moisture. Labelling must match strict chemical regulation standards, such as GHS, flagging the salt’s potential irritancy and mandating gloves or goggles. In my own experience, mishandling leads to sticky residues that seem endless to clean. Safety advice never feels wasted on anyone who’s had to scrub a benchtop for an hour because someone left a spatula with TBAHS out in humid weather. Certificates of analysis should match all incoming batches, especially for pharmaceutical or electronics work. Tracking down a batch discrepancy can ruin a week’s progress, so well-labeled bottles earn their keep.
Production of tetrabutylammonium hydrogen sulfate involves neutralizing tetrabutylammonium hydroxide with sulfuric acid. The procedure demands a slow, steady combination in an ice bath, as too-rapid mixing can lead to localized heating and side reactions, including oiling-out or unwanted byproducts. Following the blend, evaporation under reduced pressure removes excess solvent, yielding a syrupy residue that’s best crystallized with acetone or another nonpolar organic. Filtering and drying form a chunky white mass that only turns truly free-flowing after hours in a desiccator. Every step, from titration to final drying, depends on careful attention; slip up, and water or unreacted acid lurks in the product, ready to sabotage later syntheses. I remember one case in graduate school: The product looked pure, but hidden water degraded the next round of reactions—teaching a costly lesson about patience in preparation.
TBAHS stands out as a nonreactive, “holding” ion: Its main function involves ferrying reactive anions like hydroxide, acetate, or peroxydisulfate from the water layer into an organic solvent. In nucleophilic substitution reactions, TBAHS enables classical Williamson ether synthesis in two-phase conditions, saves time in the preparation of crown ether complexes, and helps build up sulfonylureas or other heterocycles that flounder in single-phase media. Sometimes, researchers have altered the butyl chains, swapping them for ethyl or hexyl variants, improving solubility or phase preference for very specific reactions or engineering needs. Decorative trifles to some, but a world of a difference when the subtle interaction between salt and substrate means the contrast between a failed synthesis and a life-saving drug.
Tetrabutylammonium hydrogen sulfate has collected several nicknames over the years. Chemists often shorten it to TBAHS, but labels may also mention N,N,N-tributylbutan-1-aminium hydrogen sulfate, or even “quartammonium hydrogen sulfate” for quick cataloging. Commercial suppliers slap on their own identifiers, but the essentials always reflect the quaternary ammonium core and acidic sulfate counterion. For anyone scouting a global marketplace—watch for synonyms such as tetra-n-butylammonium bisulfate or 1-butyl-3-butylamino-propylammonium sulfate. Ease of global sourcing and regulatory tracking benefits from these multiple names, though confusion can arise for the novice.
TBAHS, like most phase-transfer salts, should never be underestimated. Direct contact brings moderate skin and eye irritation—chemical burns pop up in the medical literature. Spill some dust or solution, and the area develops a slippery film that’s hazardous in a crowded lab. I’ve seen more than one new student wipe a forehead with a glove, only to wind up with redness or soreness for a day. Safety Data Sheets list the relevant risks—the substance demands solid gloves, proper eye protection, and a fume hood whenever glittering powder turns to dust. Should ingestion happen, call poison control straight away—quaternary ammonium salts bring their own set of risks to the gastrointestinal tract. Standards in professional laboratories stress strict inventory control, with logs and lockups for bulk stores. Regular waste audits catch inadvertent releases to the environment, cutting down on potential contamination.
Phase-transfer catalysis continues to form the backbone of TBAHS usage: hydrolysis, oxidation, and halogenation reactions leap in efficiency with just a dash of this salt. In pharmaceutical development, TBAHS helps researchers build key intermediates when simpler acids or bases won’t cut it. Organic chemists prize it for constructing energetic or delicate molecules—zwitterions, esters, or sulfonamides that stubbornly resist synthesis below its influence. Recently, researchers in electrochemistry have added TBAHS to their playbook for improving conductivity in non-aqueous batteries, supporting the buildup of solid-electrolyte interfaces or boosting ion mobility inside advanced power cells. Plenty of undergraduate labs still depend on TBAHS for demonstrations of two-phase reactivity and catalyst recycling. The list of applications keeps growing, as new industries now seek ionic liquids or green reaction media and find themselves circling back to this old staple.
From bench to industry, research has pivoted toward making best use of TBAHS in sustainable reaction designs. Groups everywhere keep hunting for alternatives to hazardous solvents, and established phase-transfer systems with TBAHS fit that bill. Academic reports over the last five years have highlighted innovative ways to recycle the catalyst; one favorite method relies on magnetic nanoparticles as supports, allowing easy recovery after each cycle. Polymer chemists, too, now tinker with TBAHS-modified monomers, seeking unique copolymers with tailored ion-exchange or conductivity properties. Even in the field of green chemistry, there’s renewed interest: processes using TBAHS often remove the need for excess acid or base, translating to fewer waste streams and less downstream treatment. Young chemists today may take the salt for granted, but as a teaching tool for green methodology, TBAHS continually earns respect.
Animal studies and in-vitro cytotoxicity trials point out that TBAHS can disrupt cell membranes, with acute exposure causing measurable local tissue irritation or more serious effects at higher doses. Chronic exposure lurks as a bigger unknown; little is published on long-term impacts for environmental or occupational contact. I once watched a safety seminar where a case of accidental skin exposure led to days of irritation and lost work hours. Environmental data remain spotty, though the stability of quaternary ammonium compounds in soil and water signals that accidental release should not be taken lightly. Treatment of waste streams must run through proper chemical neutralization or incineration, avoiding sloppy disposal down the drain. Institutes conducting new studies sometimes publish fresh LD50 values, but risk management in the lab environment stays conservative, emphasizing prevention and preparedness rather than reaction.
Looking ahead, TBAHS seems poised to keep finding new niches. As energy storage technology bends toward ionic liquids and solid-state batteries, salts like TBAHS help researchers tweak interfaces and boost efficiency in systems that will power everything from electric cars to grid storage. Innovative pharmaceutical research values its compatibility with green solvents, opening shortcuts to difficult building blocks. Advances in sustainable chemistry push phase-transfer catalysts to the center of efficiency—not just to improve reaction speed, but to limit waste and hazard at the source. Ongoing molecular engineering could see TBAHS-based hybrids in everything from smart materials to novel filtration media. In the hands of persistent innovators, this workhorse salt looks ready for decades more use and discovery, chiming in as both a workhorse of the modern lab and a testbed for the next wave of chemical ingenuity.
Tetrabutylammonium hydrogen sulfate may not roll off the tongue, but it serves a real purpose in labs around the world. Walk into any research chemistry space and you find a collection of bottles with complex names, each pulled from the shelf for a specific task. From my time working alongside organic chemists, it became clear that some chemicals stick around for the breakthroughs. This one has a reputation for solving tricky reaction problems, especially those that involve two substances that just refuse to mix and work together.
One big reason scientists use tetrabutylammonium hydrogen sulfate involves its power as a phase-transfer catalyst. In simple terms, this chemical acts a bit like a referee between water-loving and oil-loving substances. Usually, in classic organic reactions, you watch two different liquids—oil and water—ignore each other completely. Mixing reactants that only like one type of environment turns into a headache. Adding this catalyst turns up surprising results. Suddenly, those stubborn substances start reacting together, thanks to the extra push from tetrabutylammonium hydrogen sulfate.
For example, reactions such as nucleophilic substitutions and alkylations, both common in drug synthesis and industrial chemistry, get a big boost from this catalyst. I’ve seen real-world results where a reaction that led to disappointing yields suddenly works with tetrabutylammonium hydrogen sulfate in the mix. Without it, some medicines would take longer, cost more, or just produce too much waste.
My years working with process engineers taught me the importance of minimizing waste and using greener reactions. Companies want products that are safer, more sustainable, and cheaper to make. Tetrabutylammonium hydrogen sulfate often helps in this area. It cuts down on the need for extra solvents and energy. By making stubborn reactions happen at lower temperatures or using less toxic materials, the process leaves behind a lighter footprint on the environment.
This compound pops up in other corners of modern research and industry. Electrochemistry experiments sometimes rely on it for stable and efficient performance. In analyzing ions or running separations, lab techs reach for this salt since it helps to carry electrical charges across phases. Some analytical methods, like ion chromatography, benefit from it as a supporting electrolyte, delivering faster and more reliable readings.
Of course, every solution carries baggage. Regular handling of quaternary ammonium salts brings safety concerns. Over the years, I’ve seen plenty of chemists double-checking their protective gear and waste disposal plans. Proper storage and cleanup remain important. Ignoring these steps can lead to costly mistakes or health risks.
Research and education make the biggest difference in chemical safety and effectiveness. Universities and industry leaders spend real time training new scientists to weigh the risks of every material, even those that deliver huge benefits like tetrabutylammonium hydrogen sulfate. The science community keeps looking for even friendlier options, yet right now, this catalyst holds its place as a reliable partner in pushing chemistry forward—whether for better medicines, cleaner manufacturing, or sharper lab results.
Every time I talk about reagents or specialty chemicals, the conversation often turns to formulas. Their underlying structure gives away so much about how a substance behaves, reacts, and even poses risks. Tetrabutylammonium hydrogen sulfate, carrying the chemical formula C16H37N·HSO4, stands as no exception. One glance unpacks a bulky organic cation paired with a powerful inorganic acid anion.
I’ve had my hands on this compound in the lab, where it acts as a phase-transfer catalyst or an organic synthesis partner. It's made up of a tetrabutylammonium cation, which is C16H37N, and a hydrogen sulfate anion, HSO4-. Those butyl groups attached to the ammonium core nudge it towards being soluble in organic solvents while holding onto ionic properties from the sulfate end.
Some chemists favor these ammonium salts for their knack at ferrying ions between water and organic phases. Those translating complicated synthesis steps into workable bench protocols will find that, without a handy formula like C16H37N·HSO4, confusion seeps in quickly. It’s easy to slip up if someone swaps the ammonium out or confuses hydrogen sulfate with plain sulfate.
Anyone working in an industrial or academic lab can tell stories about how a correct formula saves hours or even days. Once, I forgot just how sensitive these ammonium salts are to moisture, thinking they’d handle exposure with a shrug. The compound started pulling in water, changing weight and even shifting in reactivity. With its formula, you can calculate how much to use with accuracy, prevent costly mistakes, and stay on the right side of safety.
Take environmental work. Sometimes tetrabutylammonium hydrogen sulfate gets used to prep samples for analysis by growing the solubility range. A wrong guess at composition could lead to an underestimation of potential environmental hazards or inefficient processing, sending labs back to square one.
In pharmaceutical research, process chemists lean on such chemicals for smooth transitions between steps. One slip with the formula, and reactions stall or create side products you do not want. Each element in C16H37N·HSO4 signals how the compound will interact and which safety measures are required since the hydrogen sulfate part can be especially aggressive under some conditions.
Experience has shown me that clear formulas prevent confusion. Handling a compound like tetrabutylammonium hydrogen sulfate, knowing exactly what you’re dealing with, leads to smarter use. To support best practices, always check the label, reference trusted databases like PubChem, and confirm the structure before use. This keeps research, industrial processes, and teaching running efficiently and safely.
More industries are leaning on specialty chemicals like this for greener, faster, or more selective processes. As new challenges pop up in chemical manufacturing, pharmaceuticals, and environmental science, the tools and formulas we reach for matter now more than ever.
Tetrabutylammonium hydrogen sulfate doesn’t sit in a lot of household pantries. This chemical finds its main calling in laboratories, helping researchers push boundaries in organic synthesis, phase-transfer catalysis, and sometimes in analytical labs separating different compounds. Lab workers, students, and even some industry folks may handle it, so safe storage stops being a footnote and becomes a priority.
Over the years, I’ve seen chemicals like this ignored on back shelves, lids half-closed, paper labels curling off with humidity. Most accidents in labs don’t come from grand explosions — just slow neglect. For Tetrabutylammonium hydrogen sulfate, direct contact with eyes or skin prompts stinging irritation. Spilled or mishandled, the compound calls for several uncomfortable minutes at the emergency eyewash. Inhaled dust from this compound can make anyone cough and regret skipping the dust mask. The hidden risks always show up when you least want them.
Let’s talk about the nuts and bolts. Tetrabutylammonium hydrogen sulfate stores best in a dry, cool place away from direct sunlight. Humidity ruins many chemical salts by helping them absorb water from the air — “hygroscopic” is the word chemists love, but call it a moisture-magnet in plain English. Once it clumps or dissolves, measurements start to miss the mark, experiments take a hit, and expensive supplies get wasted.
Leave it out on an open bench and before long there’s a gluey mess. So, a tightly sealed bottle makes all the difference. Glass containers with threaded plastic caps keep the air out better than cheap jars. Always slap a clear label with bold writing, noting contents, date, and hazard warnings. No one wants to discover unknown white powder months later and play chemical roulette.
Even simple compounds need thoughtful separation from acids, bases, or strong oxidizers. Don’t store Tetrabutylammonium hydrogen sulfate with strong acids or bleach. If a leak or spill pops up nearby, bad chemical reactions can produce gases or heat. Locking the compound in its original container, inside a chemical storage cabinet lined with spill trays, puts a solid barrier between a routine day and an emergency.
Keep the storage zone ventilated, not a stuffy broom closet. Good airflow whisks away any dust or fumes before they turn into a health risk. I’ve watched colleagues cough their way through poor storage setups — headaches and distractions never help a day’s work.
Gloves and goggles stand as the frontline gear during storage or handling. No one ever enjoys a chemical splash on bare skin. A nearby spill kit with absorbent pads, gloves, and waste bags gives a quick fix for small accidents. Disposal shouldn’t go down the sink; proper waste streams protect both the building’s plumbing and the greater environment.
A well-stocked lab doesn’t just keep chemicals — it protects the people using them. I’ve spent years working with researchers from all walks of life, and the safest labs always run on clear protocols and smart habits. Tetrabutylammonium hydrogen sulfate isn’t infamous, but any shortcut on storage only guarantees more headaches in the future. Good habits in labeling, sealing, separating, and using proper gear leave room for discoveries, not disasters.
Most people never hear about tetrabutylammonium hydrogen sulfate outside of a lab. Chemists see it as a useful reagent, especially for reactions in organic synthesis. The casual observer probably imagines it sitting harmlessly in a glass bottle, tucked away on a shelf. The reality looks different for anyone handling this chemical regularly.
Research and experience both point out several clear risks. Tetrabutylammonium hydrogen sulfate carries hazard labels for a reason. It irritates skin and eyes if handled without proper protection. Breathing in its dust can make your throat and nose burn. Accidentally swallowing it calls for an urgent trip to the emergency room. These dangers aren't rare situations — they happen whenever someone skips their gloves, goggles, or fume hood.
MSDS (Material Safety Data Sheets) compiled from years of workplace incidents and laboratory studies classify this compound as harmful. The European Chemicals Agency lists it as a Category 2 skin irritant and warns of eye damage. The National Institutes of Health has flagged it for causing discomfort, pain, even burns if not managed with respect. Those aren't just bureaucratic warnings; they draw from real incidents where people got burned or suffered allergic reactions.
Handling these risks isn't hard if a lab keeps solid practices. Gloves stop skin contact, goggles protect eyes from stray splashes or flying powder, and simple ventilation keeps any fumes out of people's lungs. Labs that treat every chemical with suspicion have fewer accidents. That comes from building a safety culture, not just putting up posters or making a rulebook.
An overlooked spill or careless cleanup holds consequences beyond a quick rash. Chronic exposure—meaning the same small exposures over weeks or months—can slowly sensitize someone, bringing allergic reactions out of nowhere. Chemicals like tetrabutylammonium hydrogen sulfate don’t need much time to work under the skin. A chemistry professor once pointed out the toll on hands after just a few careless months: cracked skin, persistent sensitivity, and more sick days than anyone wants.
The compound gains more attention as labs search for less toxic alternatives. Some suppliers have started labeling their products more aggressively, giving extra warnings in their catalogs. Others recommend substitutes for similar reactions. But the world of chemistry still sees a lot of tetrabutylammonium hydrogen sulfate in use, especially where nothing else does the job quite as well.
Education works better than top-down rules alone. New chemists learn faster and safer if senior staff share real-world stories: the time a hasty reaction forced an emergency room visit, or how thick gloves prevented a close call. Some companies go further, introducing digital checklists and mandatory safety training before anyone touches a container. That upfront investment pays back in fewer injuries and reduced insurance claims.
On a policy level, updating safety data sheets whenever new research surfaces helps everyone. Regulators and industry groups reviewing workplace standards drive better handling practices in schools, factories, and research centers. Leftover chemicals don't belong in regular garbage bins—hazardous waste protocols prevent groundwater contamination and keep waste handlers safe.
Tetrabutylammonium hydrogen sulfate doesn’t belong on the “most dangerous” list, but it never becomes harmless. Respecting its risks means fewer surprises, longer careers, and a safer environment in and out of the lab.
Most folks in a laboratory come across tetrabutylammonium hydrogen sulfate as a white, sometimes off-white, solid. The crystals can appear powdery or granular, not much different from the salt on a table. Pick it up, it feels dry, not sticky. Touch leaves no strong residue. This isn’t some mystery goop; it behaves much like plenty of common lab salts.
Grabbing a scoop, you notice the compound’s density runs toward the heavier side, but not brick heavy. The powder doesn’t float if you blow; it tends to drop like sand. Pouring into a container doesn’t kick up clouds, unless you go at it with excessive force. This helps with cleanup, since powders that puff everywhere make for headaches. Manufacturers ship it in sealed jars for a reason—humidity creeps in fast. The chemical loves water, pulling in moisture from the air before you know it. Leave the cap off in a damp room, and soon the material starts to look clumpy, even slightly sticky. Anyone working in an organic synthesis lab will tell you: store tetrabutylammonium hydrogen sulfate with care, desiccator or tight jar.
In solvents, this salt shows its true colors. Drop some in water or alcohol, and it melts right in, making a clear solution. In less polar solvents—say, simple hydrocarbons—it barely budges. This doesn’t just help chemists choose the right solvent; the ease of dissolving in polar liquids underlies much of its use as a phase-transfer catalyst. If the solution looks cloudy, something went wrong with either the quality or the solvent choice. The melting point falls in the 195–201°C range, which might seem high, but in a lab, that means you need more than just a hot plate if you want to see this solid liquefy on its own.
As for odor, tetrabutylammonium hydrogen sulfate keeps pretty quiet. Open a fresh container, and most noses catch only the faintest whiff, if anything at all. This lack of strong smell means accidental releases sometimes go unnoticed, so vigilance with storage remains crucial. It doesn’t corrode through gloves, but it does irritate skin and eyes. Gloves and goggles aren’t just for show—you’ll notice a tingle fast if you spill it. Inhalation isn’t a big risk, since dust doesn’t jump off the jar, but it pays to avoid stirring up fine particles.
People working with tetrabutylammonium hydrogen sulfate often point to its stable, user-friendly solid form. It stores well if humidity stays out and dissolves fast in the right liquid. Scale-up from a gram to kilos works smoothly since the bulk doesn’t change character. These qualities matter most in labs pressed for time and precision. Still, there’s an art to keeping it dry and a lesson about not underestimating simple handling challenges. An unsealed jar means ruined material, wasted reactions, and extra costs.
The most practical solution starts with airtight containers and well-labelled desiccant packs. Education in rookie labs about moisture-sensitive solids cuts waste. Automated dispensing tools help at scale, keeping hands out of jars and making sure humidity doesn’t get its chance. Even the best material turns useless if handled the wrong way. Technical details mean little if day-to-day storage isn’t up to the task. Good habits—tightly capped jars, clean scoops, a dry workbench—make or break the routine use of tetrabutylammonium hydrogen sulfate in research and production.
| Names | |
| Preferred IUPAC name | tetrabutylazanium hydrogen sulfate |
| Other names |
TBAHS Tetrabutylammonium bisulfate N,N,N-tributylbutan-1-aminium hydrogen sulfate |
| Pronunciation | /ˌtɛtrəˌbjuːtɪl.əˈmoʊniəm ˈhaɪdrɪdʒən ˈsʌlfeɪt/ |
| Identifiers | |
| CAS Number | [32503-27-8] |
| 3D model (JSmol) | `3D model (JSmol)` string for **Tetrabutylammonium Hydrogen Sulfate**: ``` CCCC[N+](CCCC)(CCCC)CCCC.OS([O-])(=O)=O ``` |
| Beilstein Reference | 1721422 |
| ChEBI | CHEBI:38761 |
| ChEMBL | CHEMBL1907851 |
| ChemSpider | 20777 |
| DrugBank | DB11106 |
| ECHA InfoCard | 100.208.693 |
| EC Number | 262-089-7 |
| Gmelin Reference | 82867 |
| KEGG | C14156 |
| MeSH | D000072645 |
| PubChem CID | 69100 |
| RTECS number | WN9825000 |
| UNII | 8P736Z53H3 |
| UN number | Not regulated |
| CompTox Dashboard (EPA) | DTXSID7020140 |
| Properties | |
| Chemical formula | C16H37NO4S |
| Molar mass | 339.54 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.13 g/cm3 |
| Solubility in water | soluble |
| log P | 0.4 |
| Acidity (pKa) | -1.99 |
| Basicity (pKb) | 8.6 |
| Magnetic susceptibility (χ) | -61.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.422 |
| Viscosity | 60 cP (25 °C) |
| Dipole moment | 6.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 310.7 J·mol⁻¹·K⁻¹ |
| Pharmacology | |
| ATC code | No ATC code |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H315, H319, H335 |
| Precautionary statements | Precautionary statements: "P264, P280, P302+P352, P305+P351+P338, P332+P313, P337+P313, P362+P364 |
| NFPA 704 (fire diamond) | 1-1-0 |
| Flash point | > 113 °C |
| Lethal dose or concentration | LD50 Oral Rat 2150 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 730 mg/kg |
| NIOSH | WN2975000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | No REL established |
| Related compounds | |
| Related compounds |
Tetrabutylammonium sulfate Tetrabutylammonium bisulfate Tetrabutylammonium hydrogen phosphate Tetraethylammonium hydrogen sulfate Tetrabutylammonium chloride |
