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Long before textbooks standardized the distinction between organic and inorganic chemistry, curious minds mixed acids and alcohols to see what would happen. That’s how the early threads of ester discovery began, with folk like Berzelius tossing out the word “ester” in the 19th century to capture an entire family of acid-alcohol reaction products. Inorganic acid esters carne onto the scene a bit later but earned a reputation just as fast. Take phosphates or sulfates—every chemist’s shelf shows bottles with unassuming labels, but inside those bottles, the echoes of ancient laboratories meet modern industry. Today’s manufacturers and researchers still dip back into those old findings. They don’t just repeat experiments—they expand the uses in everything from vaccines to fire retardants. When historians pull at the roots of chemical manufacturing, inorganic acid esters always spring up as evidence of how practical chemistry spun out from pure curiosity.
Looking at inorganic acid esters, diversity stands out far more than monotony. Phosphate esters, sulfate esters, nitrate esters, and borate esters each crop up across industries. In agriculture, phosphate esters ride inside fertilizers and pesticides; in healthcare, they slip into DNA treatments and nerve agents (in both good and bad ways); in daily life, cleaning agents often rely on these compounds for their efficiency. Back in my student days, running reactions to produce simple dimethyl sulfate opened my eyes to how one “class” of chemicals forms the backbone of myriad products. Unlike biology’s tendency to stick to carbon, these esters build their bridges with metal and nonmetal backbones, flipping common reactivity rules on their heads. And wherever one finds manufacturing or modern medicine, one will find a shelf groaning under the weight of neatly labeled bottles containing high-purity inorganic acid esters.
There’s a world of difference between handling a glass bottle of diethyl sulfate and pouring a vial of trimethyl phosphate. One drifts up as an invisible vapor that makes your nose tingle; the other lurks as a liquid with high flashpoint, waiting to dazzle or disappoint. Some of the simplest esters smell faintly sweet, masking danger beneath a pleasant odor. Chemistry students joke about the “olfactory warning,” but anyone who’s worked with these compounds knows better than to sniff-test esters. Many inorganic acid esters dissolve readily in water or alcohols; some, especially the bigger phosphate esters, stand nearly insoluble in anything but wildly polar solvents. It’s not rare to see a new researcher misjudge the volatility or reactivity of an ester, only to learn that even minuscule amounts can have outsized effects in both labs and the environment.
No two labs tackle technical specs in exactly the same way, but a few constants pop up for these chemicals. The purity must always meet the demands of the project; even trace chlorine, sulfur, or water can torpedo an experiment. The bottle label matters—real lessons arrive when you accidentally swap an alkyl phosphate for a sulfate and trigger a slow, sticky mess. Regulatory authorities keep close watch on labeling, leaning on the Globally Harmonized System (GHS) and OSHA’s Hazard Communication Standard. That means every shipment must bear fine print about risks and emergency action, so a stray bit player like dimethyl sulfate never lands in an unprepared hand. No matter how seasoned one gets, a moment’s casualness in reading chemical labels can lead to ruined reactions and safety drills.
During my early forays into esterification, mixing alcohol with acids seemed simple—just add sulfuric acid, heat, and you get your ester. Then reality arrived: inorganic acid esters demand more finesse. Phosphorylation calls for dry solvents and precise control over pH; sulfation often rides on the back of chlorosulfonic acid, and it’s easy to blister a finger or corrode a flask. Large-scale processes turn even trickier, demanding reactors with acid-resistant linings, constant fume management, and near-perfect reagent feeds. The old acid-catalyzed pathway sometimes falls out in favor of modern, greener protocols, replacing strong acids with enzymes or solid-state catalysts in a nod toward sustainability. Still, capacity and speed often trump eco-friendliness in industrial settings, keeping innovation marching forward for safer, cleaner prep methods.
What cloaks inorganic acid esters with importance isn’t just their base formula, but the wild range of reactions they catalyze or undergo themselves. In the hands of a skilled chemist, a simple phosphate ester transforms into flame retardants, lubricants, or even antiviral drugs. Many esters hydrolyze fast under heat or base, shifting to original acids and alcohols, making them responsive ingredients in cleaning products or as breaking agents in controlled-release systems. Change a side group, swap an alkoxy for an aryloxy, and the physical behavior tilts. Researchers keep running headlong into new ways to shift reactivity: some tinker with electron-rich esters to boost conductivity, others add bulky groups to block hydrolysis. In the lab, a whiteboard fills quickly with possible reaction pathways—each tweak in the chemistry bringing new possibilities or hazards to the surface.
Chemistry throws up a blizzard of names per compound. Walking through chemical catalogs, a single phosphate ester sometimes masquerades under half a dozen labels—dibutyl phosphate, DBP, phosphoric acid dibutyl ester, and so on. The confusion isn’t just academic; misnaming can mislead during experiment planning, create logjams in supply chains, and, worse, lead to unsafe mishandling. On the consumer side, product names lean toward catchiness or simplicity, nowhere near the rigor demanded by regulatory bodies or researchers. I’ve learned never to rely solely on a trade name—defaulting to IUPAC standards keeps both safety and results intact. Knowledge gaps widen quickly when synonyms spin out of control, yet the baseline need remains: call a compound by a single, indisputable name so that safety, import/export, and compliance don’t get tangled up.
Any discussion of inorganic acid esters circles back to one core reality: some compounds pack a punch well beyond their weight. Dimethyl sulfate, for example, can slip invisibly through a lab, posing serious risks before anyone can react. Others, like triphenyl phosphate, see routine use in plastics and electronics, but spill management and air filtration never become optional. I’ve been in workshops that replayed disaster stories, drilling into staff the need for gloves, goggles, and fume hoods, no matter how routine the procedure. Regulations mandate engineering controls, specialized storage, and meticulous labeling; some labs even run regular leak checks just for their ester stocks. Years in chemistry teach that shortcuts, especially with these reactive molecules, turn minor errors into full-blown incidents. Only steady attention—not just to what’s written in the manuals, but to the day-to-day routines—keeps accidents off the news and workers out of emergency rooms.
Open a medicine cabinet, fuel a jet, or test a circuit board—step inside most industries and inorganic acid esters show their hand. Pharmaceutical labs synthesize prodrugs from phosphate esters, unlocking controlled release of active agents inside the body. Fire retardants often owe their power to sturdy—or sometimes sluggishly reactive—ester bonds. In electronics, phosphate and borate esters wind up as plasticizers or dielectric fluids for transformers. Back in college, the night before an exam, I crammed tables listing every industrial application for these molecules, amazed that something with an arcane formula could land in everything from toothpaste to anti-static sprays. In modern agriculture, they slip into pesticide design, sometimes speeding up soil nutrient cycles, sometimes raising the eyebrows of environmental watchdogs. Each field claims its own unique angle, reworking the chemistry just enough to solve specific problems without ignoring the risks.
Innovation never slows in this field. Researchers watch antistatic agents, fire retardants, and pharmaceuticals all pull new tricks from the same underlying compounds. Industry demand for flame-resistant building materials has funded entire wings of labs dedicated to tweaking phosphate esters for lower toxicity and higher performance. Green chemistry pushes for reusable catalysts and benign solvents, demanding less hazardous waste and tighter toxin controls. Teams experiment with microencapsulation techniques, marrying inorganic acid esters with biodegradable shells to minimize leaching into water systems. What looked like a solved chemical toolkit twenty years ago now bursts with possible avenues—from custom syntheses targeting single-use medical devices to advanced MRI contrast agents.
Stories of mishap and mystery—illness linked to mysterious vapor, lab accidents that forced major chemical recalls—propelled much of the current research into the toxicity of inorganic acid esters. Regulatory agencies now fund studies not just in lab animals, but up and down ecosystems, tracing ester breakdowns through soils, rivers, and even into livestock. Chronic exposure to organophosphate esters raised alarms over nerve damage, leading regulatory bans and tighter workplace standards. In my own training, toxicology courses emphasized the importance of proper waste disposal and exposure assessment. Modern science leans hard on accurate toxicological profiles, feeding directly into occupational health standards and consumer product design. There’s real momentum for alternatives, as launch after launch of “greener” esters attempts to sidestep the pitfalls of their more hazardous ancestors.
The tide keeps pulling research toward not just better performance but also safer, more sustainable production and use. Environmental pressures drive companies to engineer esters that break down quickly after use, leaving no troublesome residue in water or soil. The drive for circular chemistry—reusing old molecules as building blocks instead of discarding them—brings endless room for creative problem-solving. Universities and industry partners look at the dual frontiers of bio-based feedstocks and high-precision catalysis, looking for ways to keep up supplies without leaning too heavily on fossil sources. The sharpest minds don’t just tolerate regulation—they lean into it, viewing environmental and worker safety standards as routes for innovation rather than obstacles. In my experience, the difference between leaders and laggards in this chemical family isn’t who makes the flashiest compounds, but who makes them responsibly for the long haul.
Walk into any well-stocked chemistry lab, and inorganic acid esters have a spot on the shelf. These compounds show up in reactions as reagents, helping chemists create new molecules or modify existing ones. Phosphoric acid esters, for example, pop up in organic synthesis to protect certain chemical groups or activate others. Sulfate esters work hard in the lab too, especially when someone wants to introduce or manipulate sulfate groups in a molecule. Their ability to transfer and modify chemical parts really speeds up research and opens doors in drug discovery and material science.
On the farm, life doesn’t get easier without chemistry’s contribution to pest control. Certain inorganic acid esters, like organophosphate esters, play a big role in agricultural chemicals. Farmers rely on these esters in pesticides to manage insects and fungi. These compounds are effective at what they do, making the difference between healthy crops and ruined harvests. As handy as they are, they aren’t without controversy. Organophosphate esters can present health risks to people and wildlife, so strict monitoring and new research into safer alternatives matter for everyone’s well-being.
Look at power grids, electronics, and even some vehicles, and you’ll spot the handiwork of inorganic acid esters in fire safety products. Triphenyl phosphate and similar esters help make plastics, coatings, and foams less flammable. If you’ve ever noticed the tough outer casing of electrical cables or insulation, there’s a good chance it contains these esters to keep fires from spreading. These chemicals aren’t just about meeting regulations—they protect lives and property. Concerns over toxicity and persistence in the environment make it important to develop new solutions, but esters have saved countless buildings from disaster.
Many shoppers don’t give much thought to what makes toothpaste foam, shampoo lather, or detergents break up greasy stains. Yet, inorganic acid esters such as sodium lauryl sulfate shape these products. They work as surfactants, lowering surface tension, so water can mix with oil and dirt. This role makes cleaning agents more powerful and personal care products more pleasant to use. Some people worry about skin irritation or long-term exposure, fueling research into gentler alternatives. But right now, these compounds set the standard for effective, affordable cleaning and hygiene.
Take a look at what goes on inside the body: phosphate esters naturally exist in DNA, ATP, and many metabolic pathways, making life possible. In industry and medicine, synthetic versions of inorganic acid esters help deliver drugs more effectively, stabilize formulations, and improve diagnostic tests. Some intravenous fluids feature phosphate or sulfate esters to maintain the body’s balance, especially in hospitals where precision saves lives. The careful design of these compounds means better results for patients and more reliable treatments on pharmacy shelves.
With all their uses, inorganic acid esters deserve careful handling, both for human health and the environment. Over years working in research, strict protocols and protective gear always top the list during chemical handling. Industry players now focus on greener chemistry, designing esters that break down more easily and pose less risk. Regulatory agencies keep a sharp eye on new materials, demanding data and transparency from manufacturers. People benefit most when innovation goes hand-in-hand with responsibility, so the world can keep using these versatile compounds without regret.
Ask around in any chemical lab or manufacturing site, and you’ll hear a mix of opinions on inorganic acid esters. Some folks recall that sharp, biting smell from their early days in the science building. Others remember the warning stickers slapped across every bottle. The big question keeps coming up: How risky are these compounds, really?
What surprises most people is just how many everyday processes lean on inorganic acid esters. Take sulfuric acid esters as an example—they show up in detergents, pharmaceuticals, even plastics. These esters play a supporting role in products that make life easier, yet open up a bottle in a poorly ventilated space and you’ll feel your nose burn. That’s a real warning sign.
Some inorganic acid esters release toxic fumes when they break down. For instance, phosphoric acid esters, widely used as flame retardants, carry significant health risks. According to occupational safety data, prolonged exposure to their vapors can hit the nervous system, irritate the eyes and skin, and even damage organs over time. The Environmental Protection Agency has flagged several types as hazardous air pollutants. So, it’s not just paranoia—these chemicals demand respect.
Many lab accidents underscore the hidden dangers. Years back in my own chemistry class, a student underestimated an acid ester’s toxicity and forgot proper gloves. That short contact left a burn that took weeks to heal. No need for extreme measures, but clear protocols around personal protective equipment aren’t just red tape—they keep those hidden burns and rashes from becoming routine.
The trouble with some inorganic acid esters is how easily they get into places they shouldn’t. Certain organophosphates, a subset of acid esters, have been linked to neurological symptoms in people exposed through groundwater. Research collected by the Agency for Toxic Substances and Disease Registry shows how persistent these molecules can be in air, soil, and water. Regulators worldwide work hard to set thresholds based on this data, but it’s not easy—especially with new compounds hitting shelves every year.
It’s tempting to look the other way, but ignoring risks only adds to the problem. The good news is that smart habits actually make a difference. Ventilation systems, regular training, and label literacy cut accidents by huge margins. Simple steps like storing acid esters far from oxidizers, using properly rated gloves, and logging every container help prevent most horror stories.
Developers are also stepping up through “green chemistry” choices. By switching to less toxic esters or biodegradable alternatives, manufacturers can reduce health hazards without cashing in profits. It doesn’t always mean turning every process upside down, but rather poking at old recipes and cutting out the nastiest stuff where possible.
Years in and out of labs have taught me that respect for chemicals isn’t about fear—it’s about knowing what you’re handling and making choices rooted in real data. Hazardous or toxic? Absolutely, some inorganic acid esters fall into that category. Dismissing them as safe across the board invites trouble. Solutions start with solid training, honest communication between workers and managers, and up-to-date labeling. By paying attention now, communities and industries avoid crisis down the road.
If you have any experience working in a chemistry lab or a manufacturing site, you quickly learn that safety calls for both rules and respect for what you’re dealing with. Inorganic acid esters, used in labs and industry for everything from reagents to pesticides, bring health and fire hazards that don’t cut corners for anyone. Taking them lightly can mean stories nobody wants to hear.
Every storage room isn’t built the same. Inorganic acid esters usually ask for cool, dry spaces with good ventilation. Damp corners and stuffy closets risk turning a bottle into a future headline if vapors build up or spills go unnoticed. Sometimes, I’ve seen people throw them on a shelf “out of the way.” Later, one discovers a sticky mess where a cracked cap led to slow corrosion and a clean-up job that could’ve been much worse.
Not every plastic container is up for the job. Certain esters chew through plastic or even glass over time. The best practice uses containers provided by the chemical supplier — replacing them risks unexpected reactions. Always label clearly, because mistakes with look-alike bottles never end well. We double-checked every bottle during audits; a simple label saves both time and potential hospital trips.
Mixing incompatible chemicals causes more accidents than people admit. Inorganic acid esters react with bases, reducing agents, or organic materials, sometimes giving off poisonous gases. Segregated storage keeps them away from these “enemies.” Color-coded cabinets and physical separation go a long way; plenty of incidents start with a misplaced bottle bumping into trouble.
Wearing gloves, goggles, and lab coats doesn’t make you invincible, but skipping them makes burns and inhalation more likely. Uncapping bottles slowly, away from face level, gives you a chance to notice odd smells — an early warning that’s easy to miss with distractions. Fume hoods aren’t just decorations. After a near-miss with a whiff of something sharp, I never opened these bottles outside a hood again.
The difference between a near-miss and a hospital visit often lies in how fast you know what to do after a spill. Emergency showers, neutralizing agents, and an easy-to-read spill plan on the wall are all critical. Routine training sessions keep everyone on the same page. Regulatory requirements often specify disposal, and ignoring these rules leads to fines or worse. Proper labeling, hazardous waste containers, and careful documentation are standard for good reason.
Reading a Material Safety Data Sheet once doesn’t make you an expert. Newcomers and old hands need hands-on drills, not just paper checklists. I’ve watched flustered colleagues remember the right steps from those drills when an accident happened. Retelling the “why” behind each step — not just following orders — always makes more of an impact than repeating what’s on a sign.
Experience keeps proving that shortcuts bring trouble. Proper storage, regular training, and careful handling protect people and keep costly mistakes at bay. Responsibility isn’t about paranoia; it’s about understanding that chemicals, like inorganic acid esters, bring both opportunities and risks that require respect and vigilance. Every accident avoided builds trust in the team and the process — the kind of trust people notice, even if they never mention it out loud.
Walk into any chemical manufacturing plant and you’ll probably run into tanks or drums of inorganic acid esters. Factories use them to make plasticizers, flame retardants, and all sorts of plastic goods. From vinyl flooring that stands up to spilled drinks, to wiring insulated with flexible coatings, these esters lie behind many everyday products. Take phosphate esters, for example. They add flexibility to plastics and turn up the heat resistance, which comes in handy for anything plugged into the wall—computer cables, appliance insulation, and even coating in cars.
Printers and paint makers rely on things like sulfonic acid esters. These keep ink from drying out inside a pen but make sure it dries when it hits the page. In paints and coatings, certain esters help create glossy finishes or make the paint stick better to metal, plastic, or wood. In fact, if your front door’s finish has stayed bright for years, chances are good that inorganic acid esters played a part. This chemistry keeps rust at bay and preserves colors under sunlight and rain.
Households and hospitals depend on surfactants, and many of those come from inorganic acid esters—especially the sulfate and phosphate types. These surfactants break down grease, push grime out of fabric, and lift oil off your hands during hand-washing. The science here is simple: mix an ester into soap and suddenly, dirt and oil have nowhere to hide. The FDA tracks their safety, and studies show that these compounds help keep modern life clean and manageable.
On fields and in food plants, farmers and processors use these esters as emulsifiers, pesticides, and stabilizers. In the past, phosphate esters helped fertilizers cling tightly to soil, which means more nutrients reach roots. In warehouses, food techs depend on ester-based additives to hold sauces together or stop margarine from separating. Safety remains a priority: oversight by food regulators ensures anything added to food stays within safe limits.
Modern industry needs strong, stable lubricants. Inorganic acid esters get mixed into synthetic oils that keep presses running and wind turbines spinning. In aviation and power plants, phosphate-based options slow wear on engines, keep bearings from grinding, and handle extreme pressure. Their resistance to fire can mean the difference between a minor hiccup and a disaster when machines get hot. Factory managers lean on these chemistries to cut downtime and boost safety.
Pharmaceutical labs count on esters for making certain active ingredients more soluble. During manufacturing, phosphate esters work as intermediates or help assemble complex compounds. Researchers look for these tools to fine-tune how medicine gets absorbed. Health authorities such as the WHO and the US FDA oversee the process, making sure these compounds meet high standards before anything hits the pharmacy shelf. When symptoms fade after taking a medication, chemistry like this is often behind the scenes.
Every one of these industries faces new challenges: tighter safety rules, growing demand for recycling, and pressure to use fewer resources. Switching to greener production of inorganic acid esters, recycling them from post-consumer goods, or finding less hazardous alternatives can help. Research keeps pushing the envelope— from making products that last longer, to coming up with ways to clean up wastewater after use. Real progress happens when scientists, regulators, and industry folks work together, making sure tomorrow’s breakthroughs serve both people and the planet.
Inorganic acid esters show up in labs, factories, even in medicine. These aren’t your typical table-top esters—they come from inorganic acids like sulfuric, phosphoric, or nitric acid, not the familiar organic carboxylic acids. People often use them in fertilizers, flame retardants, plasticizers, and even as intermediates in chemical syntheses. Their personalities, so to speak, depend a lot on which acid and alcohol combine to form them.
If you look at their appearance, most inorganic acid esters—think dimethyl sulfate or triethyl phosphate—pour as clear, colorless liquids, or sometimes stay as crystals. They don’t smell sweet like organic esters; some even pack a harsh, nose-tickling odor or sting the throat. Their boiling points can swing from moderately low to sky-high, depending on their structure. For instance, dimethyl sulfate boils around 188°C, while some phosphate esters don’t give up vapor until temperatures climb above 200°C.
Most of these esters don’t mingle with water, staying in separate layers when someone tries to mix them together. The few that do dissolve, like some phosphate esters, do so because they welcome hydrogen bonds or have polar groups that blend with water. Solubility in organic solvents is a habit—not a rule. Esters with short alcohol groups blend more easily, while those with bulkier chains shy away.
Density tells another story. Inorganic acid esters pack more weight than water. For example, diethyl sulfate’s density lands above 1.18 g/cm³. Storage and handling need careful planning because some of these liquids flow easily through gloved hands, while others stick around as low-melting solids.
Chemical behavior separates these esters from their organic cousins. Take their hydrolysis, for example—strong acid or base splits their bonds, and products differ depending on the acid. Sulfate esters break down in water, giving back alcohols and sulfuric acid. Phosphate esters resist a little more, but over time, or with a push from heat or acid, they give way.
People can’t overlook hazards. Many inorganic acid esters like dimethyl sulfate or diethyl sulfate come with real risks. These vapors can burn eyes and lungs or even raise the odds of long-term damage if someone doesn’t wear the right gear. Some are carcinogenic, or at least strongly suspected, which keeps them behind strict safety regulations. Even phosphate esters, often called safer, need care because a few breakdown products harm wildlife and linger in rivers and soil.
Factories rely on these esters for more than just reactions. Their heat resistance helps them serve as flame retardants in electronics, while their ability to soften plastics makes products flexible and tough. Safety isn’t just about chemical knowledge; it’s about practice. Proper ventilation, spill containment kits, and emergency showers aren’t window dressing—they’re essentials for anyone working around these chemicals.
Moving past the workplace, environmental health stands out. Phosphate esters find their way into waterways, and once there, can help algae overgrow and choke lakes. Cleaning up means smarter regulations, better waste treatment, and more careful tracking from factory to landfill. For many of us, that’s a sign that the chemical world influences everyday life, far beyond beakers and test tubes.
Safer substitutes start with smarter chemistry. Finding less toxic alcohols or tweaking reaction pathways can lower risks. Training workers to handle, store, and transport these esters makes a difference. Governments and companies working together have already cut down a lot of accidental releases, proving regulation works best when backed by research and on-the-ground experience.
Real progress demands looking at the full journey—how these esters get made, where they go, and how to reclaim or treat what’s left. By blending chemistry knowledge with public health and environmental responsibility, it’s possible to keep benefits high and side effects low.
| Names | |
| Preferred IUPAC name | oxyacid ester |
| Other names |
Acid esters Inorganic acid esters Esters of inorganic acids |
| Pronunciation | /ɪnˈɔːɡænɪk ˈæsɪd ˈɛstərz/ |
| Identifiers | |
| CAS Number | 68909-24-0 |
| Beilstein Reference | 66456 |
| ChEBI | CHEBI:37622 |
| ChEMBL | CHEMBL2096652 |
| ChemSpider | Inorganic Acid Esters ChemSpider ID: **23318** |
| DrugBank | DB01369 |
| ECHA InfoCard | Inorganic Acid Esters ECHA InfoCard: "03-2119444617-41-XXXX |
| EC Number | 2.7.7.1 |
| Gmelin Reference | Gmelin Reference: 7 |
| KEGG | C01164 |
| MeSH | D018355 |
| PubChem CID | 6857425 |
| RTECS number | TT2975000 |
| UNII | 21U3PR1UAK |
| UN number | 3265 |
| CompTox Dashboard (EPA) | CompTox Dashboard (EPA) of product 'Inorganic Acid Esters' is "DTXSID4020223 |
| Properties | |
| Chemical formula | R-OXOY |
| Molar mass | Variable |
| Appearance | Colorless liquid or crystalline solid |
| Odor | odorless |
| Density | 1.62 g/cm³ |
| Solubility in water | Soluble |
| log P | -2.0 |
| Acidity (pKa) | -3 ~ 3 |
| Basicity (pKb) | 3–10 |
| Magnetic susceptibility (χ) | Mostly diamagnetic |
| Refractive index (nD) | 1.540 |
| Viscosity | Low to high |
| Dipole moment | 1.97 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 117.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | various |
| Pharmacology | |
| ATC code | S01XA |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H314: Causes severe skin burns and eye damage. |
| Precautionary statements | P210, P221, P223, P231, P280, P301+P330+P331, P305+P351+P338, P370+P378, P501 |
| NFPA 704 (fire diamond) | 3-0-2-W |
| Explosive limits | Not explosive |
| Lethal dose or concentration | Lethal dose or concentration: "LD50 oral (rat): >2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): 1550 mg/kg (rat, oral) |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Inorganic Acid Esters: 0.1 ppm |
| REL (Recommended) | REL (Recommended Exposure Limit) of product 'Inorganic Acid Esters' is "5 mg/m3". |
| Related compounds | |
| Related compounds |
Organophosphates Sulfate esters Nitrate esters Phosphate esters Silicate esters Borate esters Carbonate esters |
