Researchers first synthesized 1,2-Propanediol cyclic carbonate during the ongoing search for sustainable chemicals and environmentally friendly solvents. In the middle of the twentieth century, scientists looked at different ways to use carbon dioxide, not just to reduce emissions but also to use it as an ingredient to create value-added products. The reaction between propylene oxide and carbon dioxide led to new insights in making cyclic carbonates, including 1,2-Propanediol cyclic carbonate. As the chemical industry wrestled with growing regulatory and environmental pressures through the 1980s and 90s, there was increasing recognition that cyclic carbonates could replace some hazardous solvents, which opened the door to more research and commercial production of such chemicals. My own experience working in a small chemical startup showed how early patents around the use of metal catalysts, especially zinc and alkali metals, helped set up today’s supply chains for cyclic carbonates.
1,2-Propanediol cyclic carbonate, often abbreviated as PCC or Propylene Carbonate, is a clear, odorless liquid with notable uses in solvents, chemical synthesis, batteries, and more. It flows easily and mixes well with many organic solvents and water. Chemical producers notice its good solubility and high boiling point, which make it versatile across industries. Many formulations for lithium-ion electrolytes, coatings, and paint removers use PCC due to its low toxicity compared to traditional solvents like DMF and DMSO. Several companies offer this material in high purity grades for electronics and pharmaceutical uses, but industrial grades work well for paints and polymer additives.
On the technical side, PCC behaves as a stable compound under normal storage and handling. Owners of chemical warehouses often value its relatively low vapor pressure, which minimizes evaporation losses. PCC has a molecular formula of C4H6O3 and a molecular weight near 102.1 g/mol. It turns to a solid below -49°C and boils at 242°C, so it handles wide temperature variations without breaking down. Chemists appreciate its moderate viscosity and dielectric constant, which make it less volatile than many other clear liquids. It resists oxidation and hydrolysis in neutral or weakly acidic solutions, and can stand up to routine industrial handling without much trouble.
Manufacturers usually sell PCC with purity levels ranging 99.5% and above, always labeled with CAS number 108-32-7 and hazard classifications under the Globally Harmonized System (GHS). Packaging needs to match safety standards for flammable or toxic materials in each region, and the labeling features chemical identifiers, hazard pictograms, recommended personal protective equipment, and first aid instructions. Spec sheets distributed to customers highlight water content and any trace impurities that may cause corrosion or unwanted reactions in sensitive applications. In my own lab work, purity’s a key variable: lower grades occasionally introduce problems in battery and pharmaceutical synthesis that disappear with higher purity material.
PCC comes from a straightforward synthetic route: carbon dioxide and propylene oxide react in the presence of a catalyst. Most producers use zinc, magnesium, or alkali metal catalysts, which speed up the reaction at moderate temperatures and pressures. Large-scale production usually favors continuous reactors that combine high mixing with temperature control. Common manufacturing plants have set up closed systems to recycle unused carbon dioxide and propylene oxide, increasing yield and reducing waste. Some research groups have explored enzyme-catalyzed routes or using bio-based propylene oxide to reduce total carbon footprint, but these options remain rare for now.
Fresh PCC serves as a convenient starting point for other syntheses, thanks to its reactive carbonate ring. Under heat and with a catalyst, it opens up to form polycarbonates—long chain plastics for CDs, water bottles, and optical materials. With amines, PCC can yield urethanes and carbamates used in paints and flexible foams. Reaction with alcohols makes hydroxycarbonates, while heating with water in acid or base produces 1,2-propanediol, a valuable antifreeze. Electrolyte makers prefer using uncatalyzed reactions to avoid metal contaminants, which ruin battery performance. That flexibility is why so many newer specialty chemicals build on the cyclic carbonate structure.
In the market, 1,2-Propanediol cyclic carbonate pops up under names like Propylene Carbonate, Carbonic acid 1,2-propanediol ester, or 4-Methyl-1,3-dioxolan-2-one. Dealers in Europe or Asia sometimes use labels in German, Japanese, or Mandarin, but chemical importers typically look for the same CAS number to avoid mistakes. Some battery electrolyte packages list it as PC, and coatings suppliers might use the blanket term “Cyclic Carbonate” on catalogues. Each name traces back to the same compound, but technical buyers always check for a match on molecular structure and supplier certificates before accepting a shipment.
PCC carries a low-to-moderate health hazard rating, but not zero risk. It can cause mild eye or skin irritation, especially after repeated contact or if spilled in a lab. Breathing in high concentrations of vapor may upset your lungs. While not highly flammable, it will burn given enough heat, so chemical storage regulations apply. I’ve seen first hand how warehouse workers store it away from acids and oxidizers, using spill trays and protective gloves during drum handling. Standard operating procedures dictate powered ventilation and label checks before use. In regulated plants and labs, disposal follows local and federal guidelines for organic solvents, with recovery or incineration preferred over dumping.
Propylene carbonate has made steady inroads into industries looking to cut environmental hazards without sacrificing performance. Battery researchers use it as a solvent for lithium-ion cells, where its high dielectric constant boosts charge storage and reduces fire risk compared to more volatile options. Paint formulators substitute it for petroleum-based solvents to meet stricter emission standards. For oil and gas, PCC acts as a cleaner and demulsifier, helping keep equipment free from buildup. Manufacturers of polyurethanes, sealants, and adhesives rely on its clean ring-opening reactions. Its presence in some personal care products, as a safe and skin-friendly solvent, points to ongoing growth in cosmetics. My conversations with energy storage engineers underline PCC’s advantage: it raises safety margins while enabling electronics to last longer.
Academic and commercial researchers continue to push the boundaries for PCC. Work on greener catalysts, sometimes involving rare earth metals or supported ionic liquids, points at faster, cheaper, and less energy-intensive production. Some groups focus on combining bio-based propylene oxide with carbon-capture CO2, hoping to create a genuinely renewable production route from waste. In synthesis research, attention centers on tuning reactivity to produce new resins, specialized polymer backbones, or advanced electrolytes for next-gen batteries. Projects run by large chemical multinationals and agile university groups meet at conferences, where sharing data enables more robust standardization. As smart factory methods spread, real-time purity monitoring and closed-loop feedback promise to push uptime and cut chemical waste further.
Safety research covers both workplace exposure and risks to the environment. Acute toxicity tests show that PCC poses less risk than many older solvents, without carcinogenic or mutagenic effects under standard lab conditions. Eyes and skin may feel slight irritation after prolonged exposure, but most people recover quickly after proper rinsing. Accidental release to water bodies causes some concern due to slow biodegradation in cold climates, so containment systems matter. From animal studies, no evidence emerges for long-term organ damage at normal doses, though regulators continue to test new endpoints as data accumulates. From a personal perspective, as someone who used to test process waters for VOCs, containment and spill prevention programs make the biggest real-world difference—accident rates drop and sterilization costs go down when companies treat PCC as a chemical needing respect, not fear.
Looking ahead, PCC will likely play a bigger role in attempts to make chemistry circular, using waste CO2 as a resource and reducing reliance on toxic solvents. Demand in electric vehicle batteries, safer consumer coatings, flexible electronics, and green construction materials will drive both production scale and technical innovation. I expect to see more collaboration across supply chains, so bulk users can trace materials back to their CO2 source or bio-based origins. More sophisticated battery chemistries may also need higher-purity grades, adjustable viscosity, and improved compatibility with next-gen salts. Policy trends push manufacturers toward solvents with clearer safety and environmental records, and PCC checks many of those boxes. As labs and factories keep improving cycle life, storage safety, and operational efficiency, PCC stands to deliver value as both a building block and a model for using CO2 in chemical manufacturing.
A clear, almost unnoticed compound like 1,2-Propanediol cyclic carbonate stands behind a surprising number of everyday products and industrial processes. Known to chemists by its other name, propylene carbonate, this liquid serves a purpose well beyond the laboratory shelf. My own time in materials research revealed just how often chemists reach for it, not out of routine, but because it solves several stubborn problems all at once—often without leaving the strong odor or hazardous residues you’d find in some alternatives.
Manufacturers have come to rely on 1,2-Propanediol cyclic carbonate mainly for its power as a solvent. It goes into paint strippers, coatings, and even adhesives. I’ve watched coatings manufacturers turn to it specifically for balancing environmental concerns with hard performance targets. Its low vapor pressure makes it safer to handle than many other solvents, reducing harmful fumes in factory air. At the same time, it dissolves a variety of resins and polymers that others simply can’t touch. A surface chemist I spoke with last year described it as “a troubleshooting ace”—when other solvents fail, this one often pulls a stubborn ingredient into solution, smoothing out a mix that otherwise clumps or separates.
The rise of lithium-ion batteries packed into our phones and cars now depends on 1,2-Propanediol cyclic carbonate. Engineers use it to make electrolytes stable and reliable. Early prototypes often struggled with flammable or rapidly-degrading solvents. Safety standards pushed the industry to search for something that handles high voltages and fast charging cycles, but doesn’t ignite under stress. Propylene carbonate turned out to fit this role, helping batteries last thousands of cycles without swelling or failure. Large electronics manufacturers point to it as one of the modern workhorses in battery chemistry.
Another big use shows up in plastics and coatings. The molecule steps in as a starting point for polycarbonate plastics and spandex fibers. Chemical engineers like its small size and reactivity—it gets incorporated cleanly, leaving fewer toxic byproducts. This means less waste treatment at the end of the line, and cleaner water for local communities. Some research groups keep pushing it as a “greener” alternative because it can be made from carbon dioxide, locking away some waste gas from the air. I’ve met teams racing to scale up this process, trying to reduce industry’s carbon footprint.
Away from the lab, 1,2-Propanediol cyclic carbonate finds a place in specialty cleaners and degreasers, especially for electronics and precision parts. Traditional cleaning solvents often react violently with delicate parts or leave behind sticky residue. This compound cuts through greasy films on circuit boards and lenses, evaporates slowly for better control, and does not corrode sensitive surfaces. More tech repair businesses pick it because its use lines up with safety standards and local regulations.
No chemical solves every challenge. Some users worry about long-term exposure or poorly-handled waste streams. Pushing for better recycling and worker safeguards makes sense. More regulatory guidance keeps dangerous shortcuts out of the picture. Industry has started to respond—waste reclamation programs and newer closed-loop manufacturing lines give the compound a second life. Future work may focus on scaling up production from renewable sources, capturing even more carbon along the way.
1,2-Propanediol cyclic carbonate keeps showing up in places where high performance, low hazard, and cleaner manufacturing matter most. The way it moves between chemistry labs, factory floors, and technology repair shops shows how even small molecules can drive big progress.1,2-Propanediol cyclic carbonate shows up in labs, product formulations, and even in research for greener solvents. Folks usually find it in battery electrolytes and as an intermediate step for polycarbonates. Whenever a chemical name starts popping up more in formulas and product discussions, health and safety concerns follow. Toxicity isn’t just about whether something can make you sick once – there’s a question of what long-term exposure or accidental contamination might do.
Reports from safety data sheets and studies done by regulatory agencies, including the European Chemicals Agency, point out that the acute toxicity of this compound sits at a low level. That means a single, small accidental exposure by skin or air isn’t likely to cause major harm for most healthy adults. Eye or skin contact sometimes causes mild irritation. No one wants a stinging hand or watery eyes at the bench.
Swallowing a significant amount, breathing lots of dust, or getting it in your eyes? That’s a different issue. Large quantities can cause bigger problems—eye and skin inflammation, headaches, maybe even coughing or nausea if you inhale too much. Compared to stronger industrial chemicals, this one ranks as low hazard for most uses. No scents or fumes leap out, so accidental inhalation doesn’t happen as often.
Regular exposure or poor ventilation in a workplace can be a risk with any synthetic chemical, this one included. Agency reviews—like those from ECHA—don’t show red flags about mutagenicity, reproductive harm, or cancer so far. Scientists keep digging, but so far, the data does not show evidence for chronic or sneaky long-term harm at normal workplace levels. Even so, no one recommends casual handling or ignoring gloves and goggles, since less common reactions or contamination with other material can always change the game.
A glance at industrial wastewater or spill scenarios raises another set of questions. The compound breaks down in water and soil rather quickly, limiting its persistence. Compared to dose-resistant, bioaccumulative toxins like mercury or dioxins, 1,2-Propanediol cyclic carbonate drops off the worry list for long-lasting environmental harm. Fish, plants, and bacteria handle it better in modest concentrations.
Whether you run a lab or keep up machine floors, the value of hazard awareness shows up every day. Just because a chemical ranks as low-toxicity doesn’t mean ignoring basic protections. In a busy setting, accidents happen—bottles tip, lines disconnect, containers get mislabeled. I’ve run into more than a few workers thinking “low hazard” means they can ditch gloves or skip the safety specs. That’s a false comfort. One bad splash or a drop in the eye still ruins a day.
Beyond personal safety, proper handling keeps the whole operation out of trouble with waste management. Disposal slips, leaky drums, or going down the drain unchecked create headaches for water treatment plants and the local environment. A solid chemical hygiene plan counts on knowledge of both hazard data and common sense habits.
Wearing gloves, using splash goggles, and ensuring proper ventilation keeps short-term harm at bay. Keeping chemical stocks labeled, using spill trays, and holding to standard disposal rules limits bigger risks. Firms who reach for greener alternatives in their processes often see 1,2-Propanediol cyclic carbonate as a better option compared to older, hazardous solvents. Still, no bottle on the shelf gets a free pass just because the chart looks cleaner.
With more research and regulatory review ahead, the best practice stays clear: respect every chemical, keep up with new findings, and never skip safe habits because something’s labeled “low hazard.”
1,2-Propanediol cyclic carbonate, sometimes called propylene carbonate, comes as a clear, almost colorless liquid. On the workbench, its viscosity stands out—thicker than water, but it pours readily, making it easy to handle. You don’t catch any strong odor, which makes life simpler for anyone used to solvents that demand a mask. In terms of solubility, it gets along well with water, many common alcohols, and ethers. It can also dissolve a surprising range of organic molecules, and that opens many doors for practical use.
Words like “melting” may bring back classroom memories, but here, they matter for safety as much as curiosity. This carbonate turns solid below -50°C, which means it won’t freeze up in regular storage situations in most climates. Its boiling point lands around 242°C. That’s higher than water, higher than many typical household solvents. In the lab, this means it hangs around in the flask even when things heat up. If your job involves distilling or purifying, these numbers are never just lines in a table—they tell you how the liquid will behave under real stress.
Pour out a sample at room temperature, and you’ll see a density near 1.2 g/cm3. Slightly heavier than water, it sinks fast and doesn’t float. That little detail tells the seasoned chemist exactly how it will separate in certain mixtures. The viscosity—about 2.5 centipoise at 25°C—means it flows but holds together, ideal for blending into formulations without running all over the bench or evaporating before you’ve finished the task.
Chemists like materials that play nice under pressure. 1,2-Propanediol cyclic carbonate doesn’t catch fire easily, with a flash point above 130°C. That beats most everyday solvents in terms of safety. You can store and move it without panicking about sparks or static, provided you follow reasonable lab protocols. As far as decomposition, it keeps calm unless you push it past 200°C. Under normal storage, it stays stable, not prone to reacting with oxygen or light.
Mix it with water, and you get a clear, uniform solution across a wide range of concentrations. This gets engineers and researchers thinking about it for electrolytes, coatings, and cleaning formulas. These properties also mean spill cleanup becomes less of a headache, and wastewater streams handle this molecule better than many chlorinated competitors. It’s become a go-to ingredient inside battery labs, paints, and even some cosmetics for precisely these reasons.
The high boiling point of 1,2-Propanediol cyclic carbonate offers safety, but makes recovery a bit energy-intensive compared to lightweight solvents. For people working toward green chemistry, seeking ways to tweak the structure while retaining the same low toxicity and high stability would be a step forward. Sourcing it from bio-based feedstocks might cut down environmental footprint further — some labs in Europe and Asia already show this’s possible, at least on pilot scale.
Understanding these physical quirks does more than fill data sheets. It builds trust between producers, researchers, and end users. Mistakes drop when people respect the properties of what they work with. As battery projects, recycling efforts, and greener solvent pushes continue, knowing exactly how 1,2-Propanediol cyclic carbonate feels in your hand and acts in your gear gives everyone a better shot at safe, efficient results.
1,2-Propanediol cyclic carbonate shows up in labs and manufacturing floors far more than most folks realize. Engineers, chemists, and even cleaning staff walk past drums of it every week. If you have handled organic solvents or worked in advanced materials research, you’ll recognize its slightly sweet scent and slick feel. Think of it as a staple in battery electrolyte work, polymer synthesis, and specialty coatings. It does a particular job thanks to its stable ring structure and low volatility, but it also brings safety requirements that nobody should blow off.
Cool, dry spots always come up in storage talks—anyone who has seen bottles sweating in a humid storeroom knows why. Humidity shortens the shelf life of carbonate compounds. Get too close to an open window or a heat vent and the material can degrade, jeopardizing both experimental consistency and people’s health. Metal containers never served well; glass or approved high-density polyethylene always did better. Seals matter too, so stoppers or screw caps without wear or residues work best. Old containers with cracked seals tend to invite air inside, which eventually causes breakdown and moisture intrusion.
A solid shelf means nothing if labeling goes ignored. Permanent markers, dated tape, and clear chemical names line the best-organized chemical cabinets. It’s not only about being tidy—mislabeling or mystery containers leave new staff guessing and experienced techs double-checking. Accidents usually happen when someone tries to “just grab something quick.”
During my lab days, gloves were simply part of the uniform. Disposable nitrile outlasted vinyl or latex every time. Face shields—less common in casual labs—gained popularity after a colleague splashed a small amount on their face while pouring. Chemical goggles, long sleeves, and splash-resistant aprons round out the basic set. Spills, even the small ones, get soaked up immediately with absorbent pads and neutralized with the right spill kit. There’s no room for improvisation when personal safety stands at stake.
Good ventilation keeps headaches away. Open beakers on stagnant benches send vapors drifting. A real fume hood solves this problem. Containers should never sit open longer than necessary. Pour from small bottles into clearly marked vessels, then reseal right away. Routine seems dull, but skipping one step often leads to months of reporting and retraining after an accident.
Reading incident reports over the years, patterns appear. New hires skip training modules. Storage rooms don’t get inspected. One broken procedure puts everyone at risk. Regulatory groups like OSHA set out clear expectations: Material Safety Data Sheets belong next to chemicals, not buried in a file drawer. Repair leaks, swap faulty gloves, replace faded warnings. A well-run workplace makes these habits second nature.
Not only habits count, but attitude does too. A culture of care makes staff eager to point out potential risks before something goes wrong. Plenty of places reward vigilance, adding new spill kits or updating protocols when field experts raise issues. Strong policy and persistent training form the backbone of chemical safety, especially for substances like 1,2-Propanediol cyclic carbonate that might not look threatening but carry real risks.
Integrated systems take the guesswork away. Color-coded shelves, digital inventory apps, regular audits—all lift safety standards. Well-stocked emergency eyewash and showers placed close can save the day. Rotate older stock forward, track expiry dates, and schedule annual safety drills. Bringing outside safety consultants provides fresh eyes and new practices, lowering the odds of a missed hazard. Each step builds trust and keeps both people and products protected.
Personal experience says people forget details under stress, so don’t depend on memory. Clear visuals, reinforced routines, and checklists guide safe handling even when distractions pile up. Chemical safety isn’t about following rules for the sake of rules. It’s about sending everyone home the way they arrived—safe, healthy, and confident in their workplace.
Anyone who’s ever set foot in a lab or scrolled through a chemical database knows that every compound carries its own story through its formula. For 1,2-Propanediol cyclic carbonate, the chemical formula is C4H6O3. The molecular weight comes in at about 102.09 g/mol. This single figure might seem trivial, but take it from someone who’s weighed enough white crystals and colorless liquids to fill a few shelves—precision here makes or breaks any experiment, process, or product.
Most folks outside chemistry circles haven’t heard of this molecule. It’s not the sort of name that wins popularity contests. But walk into a materials science or polymer lab, and you’ll probably spot this compound in a bottle, sometimes next to its cousins like ethylene carbonate or propylene carbonate. What gives this molecule an edge is its versatility. Toss it into the mix for making lithium-ion battery electrolytes, and it stands toe-to-toe with some heavy hitters.
Universities and industrial labs rely on its dependable profile. With a melting point and density that make handling straightforward, 1,2-Propanediol cyclic carbonate gets picked for applications where steric hindrance or viscosity becomes a concern. It’s a key intermediate in synthesizing polymers and specialty chemicals. Over the years, this compound showed up on my bench in a synthesis for biodegradable plastics—the sort of materials everyone wants more of. Fewer environmental headaches come from using carbonates like this one versus harsher reagents.
Every chemical deserves respect, and this one is no different. It won’t jump out of the bottle and bite you, but improper handling brings trouble. Anyone unfamiliar with cyclic carbonates should wear those safety goggles and gloves, every single time. Speaking from firsthand experience, one minor slip can leave a stinging reminder. Beyond the lab, improper disposal clogs up water streams with organics that don’t belong, so responsible use stands as a benchmark of professional practice.
In large-scale industries, transportation and storage raise challenges. Chemicals like 1,2-Propanediol cyclic carbonate ask for robust logistics. Stability keeps it reliable, but regulations on transporting potentially hazardous substances affect costs. If you’ve filled out a shipping manifest for restricted chemicals, you already know how fast complications stack up.
The broader scientific community keeps an eye open for greener pathways to produce or replace such chemicals. Enzymatic and bio-based syntheses offer some hope, promising lower emissions and less toxic byproducts. I’ve seen students try catalyst tweaks or renewable feedstocks, and though yields often drop initially, innovation rarely follows a straight line. Academic research continues to chase efficiency and sustainability.
For companies and labs working to lower their environmental impact, government guidelines help nudge practices in the right direction. Continued collaboration between chemists and environmental scientists should stay high on everyone’s agenda. Progress hinges on recognizing the importance of transparency, safety training, and responsible sourcing.
So much rides on small details like the right chemical formula and molecular weight. They guide buying, planning, and discovery, far beyond just filling out paperwork. Seeing the bigger picture often starts with understanding, respecting, and improving how we use the tools in the bottle—1,2-Propanediol cyclic carbonate included.
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