Chemistry likes to keep its history close. In the early 20th century, 1,3-Propanesultone turned up as researchers looked for new sulfonate compounds. Back then, folks didn’t have all the synthetic tools we do. Still, by passing 3-hydroxy-1-propanesulfonic acid through a cyclization process, the industry shaped a molecule with utility nobody saw coming. Its emergence sat at the intersection of growing plastics needs, advances in organic synthesis, and the search for better ways to make detergents, additives, and electrolytes. Laboratories shifted their approach from labor-intensive cages to more streamlined batch production once they figured out how flexible its reactivity proved in a flask.
At its core, 1,3-Propanesultone stands as a colorless, stable liquid or low-melting solid. Not many household names exist for it, but seasoned chemists recognize this intermediate by its bite in making sulfonate esters. Beyond the laboratory, you’ll find it as a vital backbone in electrolyte additives for advanced batteries, essential for smooth function in electrolytic capacitors, as well as building blocks for detergents, dyestuffs, and modifiers for polymers. The industry’s move to alternative energy and electronic materials keeps demand alive for this unsung molecule.
If you ever catch a whiff of it, you’re likely in a strictly monitored setting. 1,3-Propanesultone weighs in at a density of roughly 1.35 g/cm³ and boils well above 200 °C, meaning it doesn’t jump into the air without some serious encouragement. Its melting point floats in the low teens Celsius, so it can be handled as a liquid in most climates. Its chemical stability masks a core of potent reactivity; the three-membered sulfonate ring is itching to open when it meets nucleophiles. Water? It won’t stand a chance. This hydrolysis provides the business end for many of its applications.
Demand from electronics and specialty chemicals calls for high purity, with the technical grades running above 98% in most catalogs. Labels read “Corrosive” and “Toxic,” along with necessary UN numbers for transport. Owing to its cyclic sulfonate structure, the liquid’s handled in glass or corrosion-resistant steel, sealed tight, with clear hazard pictograms on each drum. Global regulatory frameworks, especially European REACH and US OSHA, frame how it gets shipped and stored, especially with worker safety at the forefront.
To make 1,3-Propanesultone, traditional routes keep things fairly direct. The old hands use cyclodehydration of 3-hydroxy-1-propanesulfonic acid under acidic conditions, with agents like phosphorus pentoxide or concentrated sulfuric acid stripping water to close up the sulfonate ring. It’s a thermal process, often run under an inert atmosphere to push yields and keep unwanted by-products low. The product needs careful purification by distillation under reduced pressure, offering up high-purity sulfone that slides into downstream applications without fuss.
The beauty of 1,3-Propanesultone lives in its ability to ring-open. Once exchanged with an alkoxide, amine, or even water, the structure yields the corresponding sulfonic acid derivative. This fundamental, reliable ring-opening underpins how it attaches sulfonate groups to a vast array of molecules. Those wanting more than just the sulfonic acid head for further modification, leveraging this base reaction to graft the sultone onto complex backbones—think biopolymers, polymers for fuel cells, or ionic liquids. In short, it’s the sort of molecule that lets a chemist build new scaffolds with sharp selectivity.
1,3-Propanesultone pops up under various tags: Propane-1,3-sultone shows up in journals, while sultone C3 or 1,2-oxathiolane 2,2-dioxide might appear on data sheets. These names reflect its structural quirks, with “sultone” shouting out its ring sulfonate nature. Catalogs stick to “1,3-Propanesultone” for clarity, recognizing chemists might also ask for “PS” or “1,3-PS” shorthand, especially in fast-paced research settings.
Use of 1,3-Propanesultone demands healthy respect. Dust and fumes carry serious health risks; this compound causes eye, skin, and respiratory irritation, with longer-term exposure linked to carcinogenicity in animal models. Strong procedures matter here: gloves, splash goggles, and local exhaust ventilation come standard during handling. Staff receive up-to-date training, spill kits sit ready, and monitored storage avoids high humidity and heat. National safety agencies, including NIOSH and the EU ECHA, demand controlled use, strict labeling, and medical monitoring in workplaces. The safety culture around this material flows from lived experience—small mistakes can lead to big consequences.
Walk through a modern battery lab or advanced polymer workshop, and 1,3-Propanesultone shows up as a quiet workhorse. As an electrolyte additive, it boosts battery cycle life and stability by forming robust solid-electrolyte interphases, especially in lithium-ion cells. In materials science, the compound’s sulfonation ability tunes polymer membranes for fuel cells, controls dye solubility for inkjet formulations, and modifies surfaces for improved wetting. It’s hard to look past water treatment—where charged functional groups built off this sultone help pull metals and organics from waste streams. Every field shapes its use differently.
Every research chemist looking for unique functionalization reaches for 1,3-Propanesultone sooner or later. The most exciting developments happen where this sultone meets green chemistry. Scientists hunt for ways to make its cyclization less energy-hungry, swap out harsh acids for milder catalysts, and recover more product with less waste. In the lab, new polymer surfactants and membrane technologies emerge using its sulfonation powers, especially where fuel cells, ion-exchange resins, and separation membranes in medicine are concerned. Data from global research journals highlight a jump in battery research—teams look to this sultone for safer, longer-lasting storage through advanced solid-electrolyte formulations.
Toxicologists have looked hard at 1,3-Propanesultone for years. Its ring structure, while great for sulfonation, brings health hazards that modern regulations take seriously. It acts as an alkylating agent, meaning accidental exposure runs the risk of permanent tissue or genetic changes. Studies on rodents showed positive carcinogenic trends, which led to strict workplace limits, routine air sampling, and tough personal protective equipment requirements. Medical surveillance programs sprung up in response. Researchers continue probing for exact mechanisms behind its toxicity, aiming for clearer action thresholds and better therapies if exposures occur.
Chemists and engineers keep one eye on the regulatory landscape and another on technical needs. The push for safer battery materials, ever-tighter emission controls, and next-generation medical devices leaves room for growth—if safety standards keep apace. For industry, the trick lies in marrying robust process containment and greener, lower-hazard synthesis routes. Research continues into sultone analogues with lower toxicity but similar reactivity, as well as recycling and re-purposing routes for spent materials. In my own experience, the real leap comes not from the molecule itself, but from careful, creative management combining old-school caution with new chemistry’s power.
Every so often, a chemical with a complicated name sparks curiosity. 1,3-Propanesultone fits this bill. In my years working alongside folks in batteries and tech, this compound keeps popping up in places most people never notice. Although it draws little attention outside of labs, its influence trickles down to products many people rely on daily, especially in energy storage.
For the average person, lithium-ion batteries just need to work—powering phones, laptops, bikes, and even cars. What surprises a lot of people is how sensitive these batteries remain to chemical fine-tuning. 1,3-Propanesultone plays a supporting role. Engineers use it as an electrolyte additive. The tricky bit with lithium batteries is keeping them safe and long-lasting. A tiny amount of 1,3-Propanesultone helps build a solid electrolyte interphase (SEI) layer during early charging cycles. This layer gives batteries a tougher skin: less risk of degradation, fewer chances of dangerous side reactions.
No chemical story is simple, especially when it comes to safety. 1,3-Propanesultone isn’t something you’d find in household cleaners; researchers flag it as a potential carcinogen. From a risk management perspective, strong controls must exist at factories and labs. Workers rely on gloves, masks, sealed containers—no short-cuts. I remember a plant visit years back, watching a team triple-check every seal before loading 1,3-Propanesultone into a mixing tank. These steps keep it where it belongs.
Regulations come into play, too. European authorities and OSHA in the United States both keep close tabs. Even with chemistry that offers benefits, health risks push industry to handle the compound with extra respect. Out in the world, batteries using tiny amounts of 1,3-Propanesultone won’t leak it during regular use, offering reassurance to end users.
Innovation always arrives right alongside concern. As battery demand climbs, research also picks up on alternative compounds. The idea: keep the best parts—long life, high capacity—but ditch the hazards. Universities and industry have pumped millions into finding the next generation of additives. Plenty of folks in battery science talk up organic molecules and polymers aimed at giving batteries an edge, with less toxicity. Some research already nudges companies toward new molecules with similar or better performance and fewer headaches.
Every technology choice builds on compromise. 1,3-Propanesultone gives batteries a practical boost, helping smooth over known sticking points, without spilling into headlines. The real challenge lands in using what works while respecting risk. Training, solid regulation, and a stubborn push for safer chemistry keep things moving. Smart industry leaders don’t just stick with what’s comfortable; they scan for new answers. That approach applies whether in a chemistry lab or a boardroom. As battery-powered technology rolls forward, this kind of pragmatism and transparency makes all the difference.
Many folks might never hear about 1,3-propanesultone unless they’re working in chemistry labs or industrial plants. It’s a colorless liquid, used to make electrolytes for batteries, sulfonate surfactants, and even as an intermediate in chemical syntheses. On paper, it looks like just another chemical name that slips into the background of factory floors and technical textbooks. But the reputation of 1,3-propanesultone raises some real questions about safety and responsibility, especially for workers and communities living close to where it’s handled.
I come at this topic as someone who’s spent time in manufacturing—safety briefings and tightly laced boots are routine. Stories spread quickly about accidents, sudden rashes, persistent coughs, and the quiet dread that sinks in when a material’s label carries a skull and crossbones. The fear with 1,3-propanesultone isn’t just hype. Multiple studies and regulatory agencies have flagged this compound for cancer risk, especially through skin contact or inhalation. The European Chemicals Agency officially classifies it as “carcinogenic, mutagenic, and toxic for reproduction.” The U.S. National Toxicology Program and International Agency for Research on Cancer have both found enough evidence to consider it a probable human carcinogen.
Direct exposure may lead to burns, eye injuries, and lung damage. In a poorly ventilated lab or a plant with lax controls, 1,3-propanesultone doesn’t give many second chances. I’ve seen safety teams lock up even small bottles of this stuff, posting loads of warning signs. People working with batteries rarely handle raw propanesultone directly, but in battery manufacturing or MSDS sheets, the concern never disappears. It isn’t the type of chemical you want spilled on your hands or wafting through your workroom.
Risk isn’t some abstract concept when talking about chemicals with a proven record of harm. The American Conference of Governmental Industrial Hygienists suggests an occupational exposure limit so low—a worker would hardly smell it before it becomes dangerous. In animal studies, cancers develop after regular, small exposures. Danger from chronic use isn’t always visible, but it’s documented. For anyone reading labels in the workplace, that’s a big deal.
Companies really can’t dodge the need for strict controls here. That starts with better safety data. Too many workplaces rely on generic safety protocols. I value clear training, easy access to PPE gear, and emergency plans that actually make sense in the real space. Engineering controls like local exhaust ventilation and closed processes can turn the tide. Regular air monitoring helps spot risks before they become disasters. At home, this means demanding those same standards from companies making things we use—batteries, electronics, cleaning products.
Switching to less risky substitutes stands out as a long-term move. Some newer battery technologies now use alternatives that don’t pose the same cancer risk. Pushing for this shift means putting worker health and community safety ahead of short-term profits. Regulators and advocacy groups need to keep up pressure, too—reviews, bans, and transparent reporting close the gap between lab evidence and safety on the ground.
Dangerous or not, a chemical’s story lives in the details: how we use it, control it, and insist on respect for the people who get close to it. 1,3-Propanesultone makes the case that technical knowledge isn’t enough if nobody acts on it. Responsibility means recognizing facts, working together, and never settling for safety on paper alone.
For people interested in chemistry or working in laboratories, knowing the formula for every compound they handle isn’t optional—it’s a safety and performance imperative. 1,3-Propanesultone carries the chemical formula C3H6O3S. This rings a bell for those who associate sulfur’s presence in molecules with distinct reactivity and certain risks during handling. Sulfur and sultones both belong to categories stirring up stronger reactions than many common lab materials.
1,3-Propanesultone offers more than a mouthful of a name. It’s used for making sulfonate groups, crucial for surfactants, ionic liquids, and some electrolytes. Picture someone working with lithium batteries, searching for that extra bit of stability or conductivity—there’s a real chance 1,3-propanesultone shows up in their toolbox. I’ve seen researchers pick this compound precisely for its ring structure, which opens up for chemical modification, dialing in properties that basic options can’t touch.
It’s impossible to discuss 1,3-propanesultone and gloss over safety. The same structure that makes it a chemical workhorse also puts it on watch lists worldwide. It’s classified as a potential carcinogen, and a single lap in a glove-free environment can become a story you don’t want to tell. The vapor isn’t just unpleasant; it’s dangerous. Labs that value health and compliance have rigid protocols for its storage and use. Safety goggles, gloves, fume hoods—these aren’t optional accessories, they’re essential gear any time a bottle gets cracked open.
There’s a push for greener alternatives to sultone compounds, and for good reason. Wastewater and accidental release don’t just vanish. They threaten fish, animals, and the neighborhoods those waterways cross. In my own experience, regulatory teams never let the blinders go up once a safer route pops up, and green chemistry scouts for these alternatives across the industry. Effort goes into discovering replacements that keep the performance but lose the risk, ideally involving renewable feedstocks or more benign byproducts. Technical hurdles remain, but each year brings the finish line closer.
Regulation doesn’t always keep pace, so information-sharing sometimes fills the gaps. Universities, industry groups, and government agencies release detailed guidance, from recognized handling tips to disposal methods that keep sultones away from public waterways. I remember reading about a case where improper handling led to a major review of national workplace safety standards, which pushed for ongoing education instead of occasional reminders.
1,3-Propanesultone, defined at its root by the formula C3H6O3S, sits at the crossroads of innovation and caution. Anyone who works with it should balance its power with respect for its hazards—which starts with knowing the details, practicing vigilance, and keeping an eye on the future of greener solutions.
On the surface, 1,3-Propanesultone looks like a simple chemical—colorless, clear, a little like a bottle of water. Dig a bit deeper and it shows its true nature. Many in the science and battery fields know this substance for its use as an electrolyte additive in lithium batteries and as a reagent in lab chemistry. It can quietly hide a pretty aggressive side: it irritates skin, damages airways if inhaled, and worse, acts as a probable human carcinogen.
Let’s be upfront. Proper storage isn’t just a box to check off a safety list. It’s about health, protecting colleagues, protecting the space, keeping the business above water, and meeting real ethical standards.
Tucking away hazardous liquids takes more than a sturdy shelf. For 1,3-Propanesultone, the main enemies are moisture, light, and loose lids. Moisture opens the door to hydrolysis, which breaks the compound down into more corrosive products, some of which can make a hazardous mess. Light can do its share of damage, causing decomposition.
The best move is a tightly closed amber bottle, marked and sealed. Glass usually beats out plastic for long-term storage. My experience in a university lab taught me the value of labels. Years ago, we used masking tape and a marker, but something always wore off or smudged. Permanent labels, typed, big letters, full hazard symbols—these have saved more than one team from confusion, accidents, and a rush to the MSDS binder.
Every chemical needs a home, and for 1,3-Propanesultone that’s a dedicated, ventilated chemical cabinet, kept cool and dry. Forget that quick “stash under the desk.” Spacing stored bottles apart separates incompatible substances, should a leak ever happen. In places with climate swings or shoddy HVAC, the temptation to leave bottles in uncontrolled storage closets grows, but skipping that control risks narrowing that crucial safety margin.
Labs often manage a strange dance between convenience and protocol, especially during busy months and equipment upgrades. I’ve noticed, the easier the lock and the more visible the labeling, the more these hazardous chemicals stay put. Cabinets with built-in spill containment keep small leaks from evolving into bigger disasters. If your shop or lab can manage, install a basic temperature monitor with warning signs for humidity. Simple tools keep quiet risks from turning into expensive emergencies.
People make the real difference. Rotating chemical stocks, checking containers for crusty lids, and keeping the chemical hygiene officer in the loop—all these create a working routine. In my old lab, sharing a physical logbook for every bottle turned into a catch-up spot for everyone. Issues, near misses, and product lifecycles ended up in those notes, acting like a back-up memory.
Disposal is just as much a part of storage as delivery: old, contaminated, or unknown bottles never hang around. Trained staff handle and dispose of the leftovers, following local laws and environment protocols. This protects not just us, but the neighbors and the trash collectors, who probably never signed up for hazardous chemical roulette.
Every storage decision winds up affecting air quality, water pipes, and even the people who mop the floors at night. Responsible storage says everyone’s safety counts, not just that of the person wearing a lab coat. In the end, it’s about showing respect for each other, the wider community, and the next folks who’ll use that space.
Simple, clear habits with 1,3-Propanesultone shield lives and livelihoods—and that counts for a lot.If you ever run into 1,3-Propanesultone in a lab or industrial setting, you won’t forget the warnings attached to it. Plenty of chemicals have caution labels, but this one carries a reputation for real harm. It sits on a shortlist of chemicals flagged by major health agencies for being a probable carcinogen. Skin burns, lung injury, and cancer all turn up in the research. Real-world chemistry comes with real consequences, and too many people take shortcuts until something goes wrong.
Working with 1,3-Propanesultone turns gloves and goggles from recommended gear to non-negotiable shields. I used to think nitrile gloves were always enough, but for this stuff, double-gloving with heavy-duty nitrile or even neoprene creates a sturdier barrier. Face shields over safety goggles mean you’re protected from accidental splashes; just last year, a major university put out a lab notice because someone lost a patch of skin to a drop on an unprotected cheek.
This chemical doesn’t need to be boiling to get airborne. Lower levels can harm the lungs and throat. Running work in a certified fume hood gives far better protection than trusting a room’s ventilation. I’ve seen rushed chemists try to skip the hood and crack open a window, but that won’t cut it—practically every safety review and fact sheet from NIOSH or the European Chemicals Agency calls for a real fume hood. Respirators can help as a backup for spills, but don’t replace a dedicated ventilation setup when handling the compound as a liquid or powder.
If I’ve learned anything from working in shared spaces, it’s that chemical labels rub off, lids get mixed up, and bad habits spread fast. Every container should have a fresh, readable label with the chemical name and hazard symbols. Sealing unused chemicals right away and never using open containers reduces accidental touches and evaporation risk. Used pipettes, gloves, and wipes need to hit a sealed hazardous waste bin, not the everyday trash. Sticking to this routine doesn’t just help the next shift— it’s also the way to avoid hidden exposures that end up causing symptoms or injuries much later.
I saw an accident during my first year in a college lab: a jar tipped onto the floor, splashing who-knows-what. Our professor’s speed with the spill kit made the difference between a close call and a disaster. Fast access to neutralizing agents like sodium bicarbonate and plenty of absorbent pads means any spill can get contained and neutralized before it spreads. Emergency eyewash showers and sinks where workers can instantly reach them matter more with substances like this—every second counts in minimizing exposure.
I’ve worked in spaces where the culture made safety stick and in others where people just hoped for the best. Regular hands-on training, real drills, and open-door communication lines about safety mistakes actually keep people alert. Peer reminders, surprise audits, and supervisors who practice what they preach make a bigger difference than new equipment ever could. For a chemical as notorious as 1,3-Propanesultone, cutting corners is never worth the long-term consequences. Taking these precautions every single time reduces risks and sets a standard for everyone who comes after.
| Names | |
| Preferred IUPAC name | 1,2-Oxathiolane 2,2-dioxide |
| Other names |
1,2-Oxathiane 2,2-dioxide β-Propanesultone Propanesultone PS |
| Pronunciation | /ˈproʊ.peɪn.sʌlˌtoʊn/ |
| Identifiers | |
| CAS Number | 1120-71-4 |
| 3D model (JSmol) | `/usr/share/jmol/jsmol/jsmol.php?model=CCS(=O)(=O)O&inline` |
| Beilstein Reference | 1730527 |
| ChEBI | CHEBI:8717 |
| ChEMBL | CHEMBL131884 |
| ChemSpider | 82105 |
| DrugBank | DB01830 |
| ECHA InfoCard | 100.004.528 |
| EC Number | EC 214-317-9 |
| Gmelin Reference | 82263 |
| KEGG | C01778 |
| MeSH | D011364 |
| PubChem CID | 7926 |
| RTECS number | TP4550000 |
| UNII | U3F85U449E |
| UN number | UN3279 |
| CompTox Dashboard (EPA) | urn:lsid:epa.gov:compToxDashboard:DTXSID9020663 |
| Properties | |
| Chemical formula | C3H6O3S |
| Molar mass | 122.15 g/mol |
| Appearance | Colorless liquid or crystalline solid |
| Odor | Odorless |
| Density | 1.348 g/mL at 25 °C (lit.) |
| Solubility in water | 6.7 g/100 mL (25 °C) |
| log P | -1.37 |
| Vapor pressure | 0.05 mmHg (25 °C) |
| Acidity (pKa) | 1.48 |
| Basicity (pKb) | 1.96 |
| Magnetic susceptibility (χ) | -31.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.448 |
| Viscosity | 9.1 mPa·s (20 °C) |
| Dipole moment | 4.54 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 194.8 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -589.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1794.3 kJ mol⁻¹ |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06, GHS08 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H302, H311, H331, H351, H314 |
| Precautionary statements | P210, P260, P264, P280, P301+P310, P305+P351+P338, P308+P311, P330, P501 |
| NFPA 704 (fire diamond) | 1-2-0-♢ |
| Flash point | 138 °C |
| Autoignition temperature | 460 °C (860 °F; 733 K) |
| Explosive limits | Explosive limits: 1.5–7.7% (in air) |
| Lethal dose or concentration | LD50 oral rat 300 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat 300 mg/kg |
| NIOSH | ST2392000 |
| PEL (Permissible) | PEL: 2 ppm |
| REL (Recommended) | 0.2 mg/m³ |
| IDLH (Immediate danger) | 250 mg/m3 |
| Related compounds | |
| Related compounds |
1,4-Butanesultone Methanesulfonic acid Ethanesulfonic acid |
