© 2026 Sinochem Nanjing Corporation,
All Right Reserved
The story of titanium trichloride solution begins deep in the age of industrial chemistry, after titanium’s discovery in the late 18th century. Researchers found themselves drawn to titanium’s unique attributes—resistance to corrosion and remarkable strength—but isolating titanium compounds took decades of work. My own university years introduced me to the persistent efforts of chemists like Matthew Hunter, who unlocked new ways to prepare pure titanium and its compounds, including the purple-hued titanium trichloride. With industrial-scale processes rolling out through the twentieth century, chemical companies started producing quantities large enough to drive research into polymerization and electronics—fields that now rely on titanium trichloride’s specific properties. This evolution says a lot about how scientific curiosity can push new materials from the lab into daily use, often in ways their discoverers didn’t imagine.
Mention “titanium trichloride solution” in chemical circles and most think of a dense, dark violet liquid, often stabilized in hydrochloric acid. Unlike many metal salts that show up as dull powders, this compound’s strong color hints at its reactivity and power as a reducing agent. The solution owes its striking appearance to titanium’s transition state, swinging between oxidation numbers as it participates in electron transfer and redox chemistry. With a boiling point that sits high and a penchant for rapid hydrolysis when exposed to air, working with it often means battling fumes or quick degradation—something anyone in inorganic chem knows well. My first run-in with this solution ended with a ruined shirt and a newfound respect for well-ventilated fume hoods. The hydrochloric acid environment helps keep the trichloride stable, but if you spill it, the sharp, acrid smell in the air leaves little doubt about its volatile nature.
Shopping for titanium trichloride doesn’t feel like picking up a regular solvent. Bottles often feature warnings in large text and color codes signaling corrosivity and toxicity. Labels specify concentration, generally expressed as percent weight in a given stabilizing medium, usually hydrochloric acid. This isn’t a product you pour blindly into a beaker. Each shipment arrives with a certificate clarifying trace metals, water content, and actual TiCl3 concentration. Years in the field with poorly labeled bottles have taught me to never trust handwritten tags or ambiguous abbreviations—inconsistent specification or tampered labels signal danger. Proper storage matters, too: the material eats through regular caps if left unchecked, so resin- or glass-lined containers dominate storage rooms. These aren’t just regulatory hoops; anyone who has watched a poorly sealed bottle fume in a stockroom will remember the importance of robust packaging for life.
Sitting in a classroom for hours training as a chemist, those old flowcharts stick in memory: starting from titanium tetrachloride and passing hydrogen, zinc, or even aluminum through it at controlled temperatures. With the right reducing agent, the tetrachloride sheds a chlorine atom, and titanium trichloride crystallizes out. Dispersing those crystals in hydrochloric acid, the base for most commercial solutions, produces that unmistakable violet color. The choice of reducing agent and reaction control makes the difference between a useful solution and a mess of unwanted byproducts. Companies invest heavily in purification here because low-grade material, full of mixed oxidation states or excess acid, will yield inconsistent results in applications like polymerization. The art lies in walking the line between speed and purity—too quick, and yields drop; too slow, and expenses rack up. As someone who’s prepared this in smaller scales, you quickly learn the dangers that can come from minor lapses in timing or temperature, especially as fumes and exotherms can get out of hand.
Titanium trichloride’s appetite for electrons earned it a place in many chemical toolkits, especially in reducing nitro groups or shifting carbon skeletons in drug synthesis. The solution reacts strongly not just with water but with air—exposing it to atmospheric humidity triggers hydrolysis, with a cloud of hydrochloric acid vapor that signals to even the least experienced bench chemist that time is short and reactions must be set up in a glovebox or at the very least a solid fume hood. It serves as an initiator in olefin polymerizations, key during the early days of plastics manufacturing. Adding modifications like ligand exchange or partial reduction opens doorways in organometallic research: such reactions have led to breakthroughs in controlled polymer growth, catalyst design, and even battery technology. Grasping these reactions starts by understanding hands-on mishaps. I recall a group project going sideways after we missed the speed of reaction between trichloride and an alcohol, underlining how finely balanced and reactive this solution truly stands.
Over time, the industry settled on a handful of common synonyms—titanous chloride for TiCl3, or even “titanium(III) chloride solution” in some catalogs. Local conventions stick, too; some hands refer to it simply as “purple titanium” or “titanium trifluoride,” confusing it with a different compound. Trade names pop up, attached to slight tweaks in composition aimed at niche applications, usually listed for specialty polymer manufacturing or catalyst components. Each name change often reflects a shift in formulation or integration with other chemicals, a sign of market adaptation. In the field, especially in older labs, you still find hand-me-down monikers that skip technicalities, which sometimes leads to misunderstanding if you’re not careful. Grasping these varying names comes from time spent both at the bench and with older colleagues who remember industry shifts—there is no substitute for experience reading between the lines.
Few chemical solutions earn the respect, or wariness, of titanium trichloride. Its combination of hydrochloric acid and high reactivity guarantees that any lapse in handling can lead to burns, breathing trouble, or worse. Good labs run regular safety drills not just for show; accidents happen fast. I still remember a senior technician calmly neutralizing a minor spill while the rest of us panicked over the immediate release of choking fumes—experience trumps formal training in the heat of the moment. Eye protection, full-coverage gloves, and chemical-resistant aprons aren’t optional, given the solution’s propensity to spray if mishandled. Ventilation isn’t a courtesy but a necessity, as even small leaks can create a health risk. Newcomers learn quickly that titanium trichloride strips away any overconfidence, rewarding those who stick to strict protocol and punishing the complacent. Extensive data from regulatory agencies backs up these on-the-ground lessons: beyond the immediate burn risk, inhalation exposure can lead to chronic respiratory issues, so care and discipline define work with this material. Firms that demonstrate best practices share stories of detailed checklists, buddy systems during transfers, and locked storage cabinets, all steps that might feel excessive until you witness a near miss.
The reach of titanium trichloride extends well out of the chemistry department. Polymer manufacturers rely on it to kickstart Ziegler-Natta catalysts, shaping polypropylene and polyethylene production. Those plastics end up everywhere, from milk jugs to medical devices, powered by catalytic cycles that begin with this unassuming purple solution. Organic chemists use it to selectively reduce compounds, a trick that made it a staple on the bench for years, especially before gentler reducing agents came along. Electronics firms tap into its ability to modify surface conductivities on ceramics and metals, part of a wider effort to enhance battery characteristics or strengthen circuit materials. In cosmetics and pigments, traces of titanium derivatives owe their origin to complexation agents derived from trichloride. It’s the behind-the-scenes role that fascinates me most: invisible to the consumer, this solution shapes countless compounding processes, colors, and polymers without fanfare or public awareness. The fact that a single compound underpins such a diverse array of industries shows how foundational a well-characterized reagent can become, driving innovation quietly but powerfully.
Academic and industrial interest in titanium trichloride keeps rising, especially as sustainability pressures push firms to cut waste and cost during polymer synthesis. Teams worldwide continue tinkering with catalyst supports, aiming to extend the utility of titanium trichloride with fewer byproducts and milder conditions. My own encounters with students trying to minimize hazardous waste highlight a truth: every tweak to the process, from solvent choice to reaction temperature, can slash environmental impact or boost efficiency. Nanotechnology circles investigate titanium trichloride for use in metal-organic frameworks and hybrid materials, seeking properties that go well beyond traditional polymerization. Patent databases overflow with attempts to functionalize titanium compounds, whether for catalysis, photovoltaic cells, or smart coatings that interact with their environment for medical or aerospace purposes. The relentless march of research rarely stops, and while fads come and go, the centrality of core reagents like titanium trichloride keeps them under the spotlight as scientists push boundaries and chase the next breakthrough.
Much as industry strives to harness the benefits of titanium trichloride, toxicity cannot be swept aside. Decades of toxicity assays point to acute risks: inhalation leads to heavy respiratory impact, and skin contact can eat away tissue. Regulatory reviews from authorities such as the U.S. Occupational Safety and Health Administration draw upon these findings to set exposure thresholds and guide personal protection measures. Industrial hygiene professionals never tire of reminding staff to watch for symptoms of overexposure—persistent cough, eye watering, or chronic bronchitis in long-term cases. Animal studies reinforce the need for vigilance, casting light on both local effects (burns, irritation) and potential systemic impacts if absorbed over prolonged periods. The message is clear: while titanium trichloride drives progress in crucial industries, unguarded use courts disaster. Ongoing research now digs into persistence in the environment and secondary effects, especially as waste streams from polymer plants land in municipal treatment systems. From what I’ve seen in laboratory audits, facilities that succeed in mitigating toxicity do not skimp on training or cut corners on containment. Sharing data and outcomes between academia and industry has driven safer practices worldwide, a trend that needs encouraging if we’re to keep titanium trichloride both productive and out of accident statistics.
Watching trends in specialty chemicals, future prospects for titanium trichloride seem tied to two factors: clean technology and high-performance materials. The push to build more efficient catalysts will keep the research pipeline flowing as engineers compete for better polymers, lower energy use, and thinner electronics. A strong market for recyclable or biodegradable plastics could put pressure on producers to engineer new trichloride-based systems with greener credentials—less hazardous stabilizers, more benign reaction conditions, tighter emission controls. Battery research also pulls titanium compounds into the spotlight, with trichloride derivatives showing promise for next-generation energy storage. With investment flooding into sustainable chemistry, collaborative innovation between public and private sectors looks set to accelerate, bridging gaps between theoretical research and practical application. There’s every reason to believe this complex, challenging, reactive purple solution will stay relevant, fueling breakthroughs that don’t just make day-to-day life more convenient, but safer and less polluting. For all its risks and quirks, titanium trichloride embodies the twin truths of modern chemistry: progress demands respect for both potential and hazard, and knowledge—shared openly and applied wisely—remains the tool that channels power toward human benefit rather than harm.
Titanium trichloride solution might not sound familiar to most outside of specialized labs, but it quietly shapes much of what we encounter daily. It’s a critical catalyst in producing polypropylene and other polyolefins—plastics that surround us in packaging, automotive parts, appliances, and even the fibers in our clothing. Talking with friends who work in chemical plants, the process always comes up with genuine appreciation; they know how much precision and care goes into managing these powerful reagents.
Factories rely on titanium trichloride solution to help link simple molecules together and form long polymer chains. Without this compound, we’d go back to heavier, less flexible alternatives to things like food wrappers or lightweight car interiors. These plastics created using titanium trichloride last longer and handle tougher tasks, reducing frequent replacements and material waste.
The use of titanium trichloride extends beyond plastics. Refineries lean on it to purify gasoline and other fuels. A cleaner burn, thanks to improved removal of unwanted compounds, means fewer emissions on our commute. According to industry reports, improved catalysts in petroleum processing trim down sulfur that would otherwise pollute the air.
Chemists also value titanium trichloride in creating unique alloys and specialty metals. These metals go into airplanes, medical implants, and advanced electronics. Being able to tweak the structure of metals lets engineers create lighter, more durable products with less raw material, helping both the environment and the bottom line.
Labs put titanium trichloride to work in research projects ranging from new solar cells to pharmaceuticals. A friend of mine, who works at a university lab, describes experiments where titanium trichloride helped make new compounds with unique properties. The solution often acts as a starting point for building blocks that wind up in everything from new medicines to environmental sensors.
Handling titanium trichloride isn’t without challenges. It reacts sharply with water, releasing hydrogen chloride gas—a serious health risk and a reason for tight controls. Chemical producers and users follow strict safety rules and training when moving or mixing this solution. Multiple inspection agencies regularly check for leaks or unwanted releases, and researchers consistently publish studies about hazards and incident prevention.
Titanium trichloride’s reach stretches across numerous industries. Still, the heavy reliance on this solution should push everyone to focus on safety, efficiency, and environmental responsibility. Some companies explore newer catalysts that avoid the harshness or toxicity of current chemicals. Others tweak the structure of their plastics to make recycling easier or lessen the need for tough chemicals in the first place.
Including workers in safety planning, investing in cleaner technologies, and sharing data about risks and best practices help the entire industry lift its standards. Experience working with hazardous materials teaches a valuable lesson: real progress takes steady attention to both results and well-being. As new uses for titanium trichloride solution emerge, industry and regulators owe it to everyone to do the job right.
Grabbing a bottle labeled "Titanium Trichloride Solution" from a chemical supply shelf, most folks see a deep purple liquid and might not think twice about what’s actually in it. To a chemist or an industrial processor, though, the numbers on the spec sheet do all the talking. Titanium trichloride doesn’t just show up pure and ready for use—it’s a shifting mixture, heavily dependent on how it’s made and stored.
A typical commercial solution walks in at a concentration ranging from about 20% to 30% titanium trichloride (TiCl3) by weight. These numbers come straight from manufacturer datasheets and peer-reviewed sources. This solution isn’t just TiCl3 swimming solo in the bottle. It includes hydrochloric acid and sometimes a touch of free chlorine, all relics of the production process. The dense purple color comes from TiCl3 ions dissolved in the acid, but the strength of the acid impacts stability and shelf life.
Using this stuff in a research lab, I’ve seen how batch-to-batch swings in concentration pose problems. Minor miscalculations, or letting a bottle absorb moisture from the air, and the numbers on the label don’t match what’s in the flask. Quality control methods—titration, specific gravity, sometimes absorption spectroscopy—give that real-world check. For industrial reactors and pilot plant startups, engineers want clear, reliable specs. Nobody likes to scrap a batch just because the solution drifted off-target by a percentage point or two.
Digging into purity, this is where things get finicky. Titanium trichloride doesn’t just carry the base metal and three chlorines—it picks up extras. These “impurities” might come straight from the ore or sneak in with the reagents. Iron, vanadium, and trace sodium find their way in, sometimes at parts-per-million levels you’d only spot with top-shelf analysis.
From a chemical safety standpoint, even a whisper of the wrong element can spark unwanted side reactions. If you’re making polymers or dipping into organic synthesis, iron can act like sand in your gears, shutting down catalysts just as the reaction gets going. Suppliers usually guarantee a “purity” above 99% for technical grades, but high-purity demands can go beyond this; trace metal analysis with ICP-OES or atomic absorption spectrometry gives the researcher confidence about what’s actually in bottle. These tools aren’t only for perfectionists—they cut down on waste by letting you match your inputs to your process.
Poor quality control and confusion over what “concentration” or “purity” actually means don’t just frustrate scientists. They cause real headaches in scale-up, with batches that stall or products that fail to meet rigorous specs. In an industry built on process reliability and repeatability, a simple mislabel or underdog impurity can cost a company millions in lost time and materials.
For those sourcing titanium trichloride, the most practical solution always lands on checking certificates of analysis, running your own verifications, and working with suppliers who open up about their manufacturing steps. Skipping shortcuts and running baseline checks saves much more than it costs. Attention to detail in both lab and industry doesn’t just protect your bottom line—it builds trust in the science and the product moving forward.
Titanium trichloride solution stands out as a tough customer in the chemical cabinet. It reacts quickly with air and water, which can catch some people off guard during storage and transport. You can't just set it on a shelf in any old spot and forget about it. This isn’t just being cautious; it’s looking after the safety of everyone nearby and making sure expensive supplies don’t go to waste.
Tank choice makes a big difference. Glass bottles, while great for some chemicals, can’t handle the rough and tumble of titanium trichloride. Steel or iron starts to corrode once this solution gets loose. Polyethylene usually doesn’t last. Experience points you straight to stainless steel (lined) or high-quality glass-lined tanks. These options didn’t get picked out of thin air—a ton of corrosion tests and real-world spills tell the story. Tight, sealed lids matter. No one wants the gas that forms if this stuff hits moisture escaping and causing headaches—or worse.
Rooms used for storage should stay dry, cool, and well-ventilated. Humidity brings big problems by inviting chemical reactions that release hydrogen chloride gas, which lingers and burns throats and eyes. Heat can speed things up in all the wrong ways. Shelves made for chemical containers, away from high-traffic areas and far from incompatible substances like strong bases or oxidizers, keep things safer.
Accidents tend to follow the same patterns—improper storage and sloppy housekeeping top almost every report I’ve seen. Regular housekeeping checks, with someone actually opening cabinets and looking for leaks or residue (instead of just ticking boxes), improve everyone’s odds.
Grab appropriate gloves—nitrile or specialty laminate types, not the regular stuff from the food prep drawer. Chemical splash goggles, not just safety glasses, block stray drops from finding your eyes. Wipe up small spills with plenty of neutralizing agent—like sodium bicarbonate—before mopping. If you ignore a puddle, it’ll eat through surfaces or even start a fire. Always use fume hoods or chemical workspaces; breathing in the fumes is asking for trouble.
Moving this solution between rooms or facilities isn’t a job to assign to an untrained hand. Drum cradles and leak-proof carts work well, but people should respect that even new drums develop cracks. One slip and you’re chasing emergency cleanup. My own past work in a plant drilled “double-check every clamp, even the ones you trust” into my muscle memory for good reason.
One headache pops up again and again—folks thinking leftover material or wash water can just go down the drain. This is the fastest way to break plumbing, pollute ground water, or start unplanned reactions. Most local rules demand collection in well-labeled drums and collection by certified waste professionals, followed by neutralization at an approved site. One call to your environmental coordinator saves a truckload of legal trouble.
Training doesn’t end once someone watches a video. Refresher drills, periodic checks, and updating the storage area as new hazards emerge show a commitment to responsibility. It builds trust—and it protects both your supply and your people.
Titanium trichloride solution looks pretty harmless at first glance. The clear or blueish-purple liquid doesn't exactly scream danger sitting in a beaker. But anyone who has worked around chemical stockrooms knows better. Underneath the smooth surface, this stuff packs a punch—both to people and to lab equipment.
Corrosive chemicals have a way of making their presence known—think of the stinging smell of hydrochloric acid or the slippery risk of sodium hydroxide spills. Titanium trichloride isn’t any less threatening. It eats through skin, metal, and even some plastics, especially once it grabs a sip of moisture from the air and produces hydrochloric acid gas. I’ve watched brand new lab benches pockmarked from careless splashes, and I’ve heard the horror stories from colleagues nursing chemical burns or ruined clothing.
When that solution spills and touches water, even the humidity floating in the room, it reacts quickly. It sends up white vapors—hydrogen chloride—that irritate eyes and lungs almost immediately. Those are not just warning signs; they're a clear message: respect what you’re handling.
This compound owes its nasty streak to its thirst for water. Once it touches any source of moisture, it hydrolyzes and generates hydrochloric acid right there on the spot. That's why glassware fogs up, and why skin and metal suffer so much damage. Hydrochloric acid is famous for a reason—few materials can withstand its attack for long.
The fact sheet doesn’t hide the truth. OSHA classifies titanium trichloride as both hazardous and corrosive. The Environmental Protection Agency and the Globally Harmonized System lay out requirements for strict labeling and safe handling procedures. Respirators, heavy gloves, and eye shields aren’t just suggestions; they’re basic equipment.
Ignoring protocols with this stuff costs more than a scold from the safety officer. I've seen titanium trichloride burn through clothing, etch stainless steel containers, and contaminate expensive analytical gear. The residual fumes linger, making plain breathing tricky if he fume extraction isn’t doing its job. Even tiny spills can trigger hours of downtime or even evacuation in a busy space.
Labs sometimes treat hazardous materials as routine, especially after handling acids and bases for years. But titanium trichloride serves up sharp reminders about complacency. One careless move, one rushed cleanup, and injury or expensive damage can follow in minutes.
Experienced hands learn to keep this solution far from water and open air, moving quickly and methodically in the fume hood. Double-gloving and buying the right face shields saves more than money on medical bills; it spares untold headaches when a small oversight spirals.
Engineering controls help, too. Good ventilation, well-sealed containers, and strict storage rules turn a dangerous job into a manageable one. Training should focus on both what the chemical can do and how it acts—real stories about what happens during an accident sink in far better than dense manuals or slick posters.
Building a real culture of care—one where workers look out for each other and don’t cut corners—matters more than any single piece of equipment. I’ve watched new lab techs transformed by a proper walk-through and shared experience from veterans. Taking titanium trichloride seriously means understanding the hurt it can cause and staying vigilant with every step.
The lifespan of Titanium Trichloride Solution doesn’t show up as a handy “best by” date on the bottle. In the chemical world, shelf life depends on a handful of things, but the main culprits are air and water. Titanium Trichloride reacts fast with moisture—even the kind that sneaks in from a loosely tightened lid. If it meets oxygen, the solution sets off on a path towards becoming titanium dioxide and hydrochloric acid. Some label this compound as unforgiving, and I can’t disagree; leave it uncapped for too long, and you’ll see it lose its signature purple color, signaling changes under the surface that matter.
Lab techs and quality teams tend to write the received date right on the container, along with storage guidelines. Outfits that rely on this chemical—especially in metallurgical or catalyst prep—usually set their own rule: use it within one year. There’s not a magic number imposed by vendors, though many say six to twelve months if the seal stays tight. Temperature swings hurt longevity. Put the bottle in a cool, dry spot, and its contents last longer. Throw it in a hot, humid storeroom, and you’ll speed up its transformation. More than one researcher has found out too late that heat invites nasty by-products and corrosion inside the cap.
It’s tempting to count days, but real quality comes down to ongoing checks. Open up a bottle you haven’t touched for a while; look for cloudiness, red-brown deposits, or a faded hue. These all signal a solution past its prime, and using it risks failed results or ruined equipment. A smart practice involves pulling a small sample and testing concentration and activity every few months. Some manufacturers publish quality data showing drops in purity over time, especially with repeated use. This is why seasoned chemists push for “first-in, first-out” rotation—a simple trick that avoids sad surprises and wasted money.
Ignoring expiration signs brings headaches that run deeper than waste. Titanium Trichloride fumes sting the nose and lungs, and leaks can chew through shelving or protective gloves. Outdated product may let down anyone depending on its reducing power, but the real risk lies in handling errors or sudden reactions. The Material Safety Data Sheet calls for tight storage and regular inspection, and those warnings come with reason. Health authorities, like OSHA, back up strict timelines and handling procedures, making sure people in the room stay safe.
Long-term, the best defense sits with solid habits. Date every container. Keep a log of each use and storage condition. Store only as much as the next job needs. Over-ordering might seem efficient, but chemicals degrade, and wasted oversupply adds stress for everyone. Investing in training pays off more than cutting corners, and companies focused on safety see fewer accidents and less downtime. Respecting expiration isn’t about following a rule—it’s about working smarter and keeping everyone protected.
| Names | |
| Preferred IUPAC name | Titanium(3+) trichloride |
| Other names |
Titanium chloride Titanium(III) chloride solution Trichlorotitanium solution Titanous chloride, solution |
| Pronunciation | /taɪˈteɪniəm traɪˈklɔːraɪd səˈluːʃən/ |
| Identifiers | |
| CAS Number | 7705-07-9 |
| Beilstein Reference | 3586695 |
| ChEBI | CHEBI:30430 |
| ChEMBL | CHEMBL1200273 |
| ChemSpider | 22221 |
| DrugBank | DB14546 |
| ECHA InfoCard | 03d2d497-027e-43a8-8aa5-f800f8a47e32 |
| EC Number | 231-441-9 |
| Gmelin Reference | 28546 |
| KEGG | C06811 |
| MeSH | D013972 |
| PubChem CID | 24634 |
| RTECS number | WS4255000 |
| UNII | 93C257R186 |
| UN number | UN3264 |
| Properties | |
| Chemical formula | TiCl3 |
| Molar mass | 154.23 g/mol |
| Appearance | Purple liquid |
| Odor | Pungent |
| Density | 1.13 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -1.429 |
| Vapor pressure | Negligible |
| Acidity (pKa) | Strong acid |
| Basicity (pKb) | 1.81 |
| Magnetic susceptibility (χ) | Paramagnetic |
| Refractive index (nD) | 1.5 |
| Viscosity | 3 – 5 cP |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 207.8 J·mol⁻¹·K⁻¹ |
| Pharmacology | |
| ATC code | '' |
| Hazards | |
| Main hazards | Corrosive, releases toxic hydrogen chloride gas on contact with water, causes severe skin burns and eye damage, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS02,GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | Hazard statements: H314, H290, H331, H410 |
| Precautionary statements | P264, P280, P301+P312, P302+P352, P305+P351+P338, P304+P340, P330, P337+P313, P332+P313, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 3-0-2-W |
| Autoignition temperature | 140 °C (284 °F) |
| Lethal dose or concentration | LD50 Oral Rat: 3160 mg/kg |
| LD50 (median dose) | > 3,160 mg/kg (rat, oral) |
| NIOSH | GY1225000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit): 1 mg/m³ |
| REL (Recommended) | Recommended Exposure Limit (REL): 2 mg/m³ |
| IDLH (Immediate danger) | IDLH: 10 ppm |
| Related compounds | |
| Related compounds |
Titanium tetrachloride Titanium dioxide Titanium(III) oxide |
