Chemistry has a knack for pushing us into places where the rules of nature get tested, and the story of 2-(Perfluorohexyl)ethanesulfonic acid runs right along that course. Fluorinated surfactants kicked off in earnest in the middle of the twentieth century, with perfluoroalkyl substances (PFAS) quickly grabbing the attention of manufacturers and scientists alike. The urge for materials that could shrug off heat, extinguish fires, and resist chemical attacks led to vigorous research, where the longer perfluoro chains got rolled out across countless applications, many poorly understood outside the lab. Warnings about certain PFAS started echoing in the late 1990s, but in the early days, the word was optimism. Production of compounds like 2-(Perfluorohexyl)ethanesulfonic acid grew out of a push for performance over easy environmental breakdown, shaping a legacy that outlives most careers—both literally and figuratively.
2-(Perfluorohexyl)ethanesulfonic acid stands out in the class of perfluoroalkyl sulfonic acids, recognized for its six fully fluorinated carbon atoms linked to an ethanesulfonic acid group. This structure bestows a strong resistance to degradation, both thermally and chemically, positioning it as a workhorse for demanding industrial environments. The substance can be found as a clear to off-white solid or viscous liquid, and the unique combination of the perfluorohexyl moiety with the sulfonic acid group makes it especially useful in specialty surfactants, wetting agents, and protective coatings where conventional organics fall short.
Chemically, 2-(Perfluorohexyl)ethanesulfonic acid exhibits a striking stability unmatched by most organic acids. With a molecular formula of C8H5F13O3S and a molecular weight hovering around 452–455 g/mol, the presence of multiple C–F bonds suppresses most reactivity, ensuring outstanding chemical resistance. It carries a low volatility and an unusually high water solubility compared to other perfluoroalkyl acids, thanks to its sulfonic acid group, which also raises the acidity well above many non-fluorinated analogues. The surface-active properties stem from its amphiphilic design: a hydrophobic perfluoroalkyl tail paired with a hydrophilic sulfonic acid head, granting it remarkable wetting and spreading performance on both polar and non-polar surfaces.
Producers typically provide 2-(Perfluorohexyl)ethanesulfonic acid at a minimum assay of 98%, noting the presence of potential byproducts such as shorter-chain PFAS or related sulfonic derivatives. Materials arrive labeled with clear hazard warnings, including irritant and environmental risk symbols, in compliance with the Globally Harmonized System. Lab containers bear the proper shipping name, UN identification numbers, batch details, and recommended storage conditions. Often the label also specifies perfluorohexyl chain length, signal word “Danger,” and explicit notes on handling protocols to prevent contamination or exposure.
Synthesis of 2-(Perfluorohexyl)ethanesulfonic acid generally follows a two-step journey: first, a perfluorohexyl precursor undergoes olefin functionalization or halogen exchange to create a reactive intermediate, often a perfluoroalkyl iodide. Introduction of an ethylene fragment via nucleophilic substitution transforms the backbone, after which sulfonation—frequently with sulfur trioxide or chlorosulfonic acid—grafts the sulfonic acid group onto the molecule. The process, while straightforward on paper, calls for scrupulous attention to moisture exclusion, inert atmosphere processing, and careful quenching to prevent both yield loss and downstream environmental impact.
Most reactions involving 2-(Perfluorohexyl)ethanesulfonic acid exploit the sulfonic acid functionality. Salt formation forms the foundation for product diversification; neutralizing with bases yields sodium or ammonium salts suitable for various commercial needs. The perfluorohexyl chain itself resists chemical modification—an advantage in uses demanding durability, trouble for anyone contemplating synthetic redesign. In laboratory research, the sulfonic acid group also enables coupling to polymer backbones, introducing superhydrophobicity or charge transport traits to the host materials. Despite all the chemistry expertise collected so far, the options for degrading or transforming the perfluorinated tail remain limited, fueling calls for innovation in PFAS remediation.
Science and trade go hand in hand with a pile of names for the same stuff. You’ll encounter this molecule under the names perfluorohexylethanesulfonic acid, PFHxES, and sometimes as hexafluoropropylene oxide dimer acid sulfonate, depending on heritage or brand lineage. Catalogs may show related sodium or potassium salts, but the acid form stays at the core. These names matter far beyond paperwork; slight linguistic mix-ups often trip up international sourcing and regulatory compliance.
Experience teaches caution with PFAS compounds. 2-(Perfluorohexyl)ethanesulfonic acid requires strict handling, starting with good ventilation, full personal protective equipment, and exclusion of food and drink from all workspaces. Splash contact brings risk of eye and skin irritation; inhalation risks are serious in aerosol-generating processes. Waste management shapes protocol. PFAS materials resist typical degradation—incineration in controlled settings often stands as the last resort. Best practice includes air-tight storage in corrosion-resistant containers, spill-prevention plans, and regular staff training on emerging PFAS research. Facilities are required to monitor effluent and emissions, keeping close records to meet increasing regulatory intensity worldwide.
Unlike simpler surfactants, 2-(Perfluorohexyl)ethanesulfonic acid finds its niche where reliability, surface energy modification, and high-performance demands stress ordinary molecules beyond their limits. It joins specialty coatings for electronics, where it guards board assemblies against moisture creep, and it slips into formulations for high-durability firefighting foams. The oil and gas sector turns to it for pipeline treatments, drilling mud modifiers, and corrosion inhibitors that function in the face of severe chemical or thermal insult. Its presence in laboratory reference materials plays a key role in environmental analytics, setting detection standards for other PFAS.
The push for safer and more effective PFAS alternatives means constant evaluation. Researchers study structure-performance relationships, hunting for the sweet spot between chemical resilience and environmental persistence. Analytical teams race to perfect detection for parts-per-trillion levels, often using the acid as a traceable reference molecule. Work carries on in developing functionalized versions, grafted to advanced membranes for water treatment, and in blending strategies that limit migration from consumer products without losing fire suppression or anti-corrosion properties. Progress still meets friction from both cost and regulatory scrutiny, sustaining a climate of careful optimism and measured innovation.
Reports on 2-(Perfluorohexyl)ethanesulfonic acid echo the wider story of PFAS, raising heavy flags about bioaccumulation, persistence, and systemic toxicity. Animal studies show kidney and liver effects at moderate doses, reproductive issues at higher concentrations, and immune system modulation that isn’t easy to predict or quantify in the wild. The acid’s water solubility increases its mobility through soil and groundwater, opening up exposure routes far from original points of use. Epidemiological surveillance efforts—though hampered by sparse long-term data—find measurable levels in various human populations. Regulatory attention continues to grow, with ever-stricter guidance from groups like the US EPA and European Chemicals Agency, demonstrating a common-sense movement to protect public health.
The future for 2-(Perfluorohexyl)ethanesulfonic acid looks anything but stable, with regulators homing in on PFAS as a global priority. Calls for phase-out of the riskiest structures force industry to chase costlier or less effective stand-ins. Meanwhile, breakthroughs in degradation chemistry and environmental monitoring promise some relief. Forward-looking industries invest in substitution efforts, green chemistry platforms, and closed-loop processes to keep both product value and societal trust intact. In universities and contract labs, energetic teams test everything from plasma-based treatments to specialized bioremediation, driven by the hope that the next generation of fluorinated chemistry finds a balance between usefulness and responsibility. For now, the acid represents both the power and the pitfalls of modern chemical innovation in full measure.
2-(Perfluorohexyl)ethanesulfonic acid belongs to the PFAS family—per- and polyfluoroalkyl substances—which have been around since the 1940s. This particular compound lands in the spotlight thanks to its ability to repel oil, grease, and water. Manufacturers have found it useful in multiple sectors, especially in specialty coatings, firefighting foams, and cleaning agents for industrial settings. If you've ever worked in an industry that deals with harsh chemicals or environments where keeping things stain-free matters, it’s likely that this substance (or a close relative) has done some of the heavy lifting.
The chemical structure of 2-(Perfluorohexyl)ethanesulfonic acid sets it apart for high-stress jobs. Its carbon-fluorine bonds are some of the strongest in organic chemistry. That strength gives it persistence—nothing in the environment easily breaks it down. Companies use it in metal plating to keep surfaces corrosion-free. The textile business leans on it for stain resistance in everything from carpeting to technical workwear. Electronics production brings another need, since semiconductors and circuit boards often call for cleaner, more predictable environments. In my conversations with engineers, they point to PFAS-based products—sometimes including this acid—as the only option that gets the job done every time.
Here’s where the trouble starts. While the chemical’s resilience helps in manufacturing, it poses a headache the moment it escapes the controlled world of factories. PFAS chemicals have been labeled “forever chemicals.” They move in soil and water and stack up in animal and human tissues. The Centers for Disease Control and Prevention and environmental groups have found them in drinking water and in the blood of people across the globe. Studies from Harvard and leading institutions link these compounds—including 2-(Perfluorohexyl)ethanesulfonic acid—to health problems like immune dysfunction, thyroid disease, and certain cancers.
Some regulators have already set tougher limits for PFAS contamination and are forcing industries to rethink their chemical portfolios. The Environmental Protection Agency rolled out tighter drinking water standards, putting pressure on companies to phase out these substances. International efforts, like those by the Stockholm Convention, pull some of the most hazardous PFAS off the market. Still, my friends in industry say they feel pressure since safer alternatives don’t always exist—or don’t match up in performance yet.
Modern labs are racing to develop fluorine-free coatings and cleaners. Engineers try swapping out old approaches for biodegradable surfactants. Some towns invest in better water filtration, using activated carbon or reverse osmosis. Cleanup technologies advance fast, but costs add up quickly for small communities. I’ve seen local governments struggle with this, torn between the need to protect residents and budgets that don’t stretch far.
2-(Perfluorohexyl)ethanesulfonic acid delivers impressive results for industry, but the flip side keeps growing harder to ignore. Pressure for transparency around chemical use ramps up each year, and the public now asks more questions about long-term safety. Progress here means more than new formulas—it calls for trust, accountability, and better choices at every level of production and regulation.
2-(Perfluorohexyl)ethanesulfonic acid belongs to that large family of chemicals called PFAS—per- and polyfluoroalkyl substances. PFAS don't break down in the environment for ages, so every year more of these compounds pile up in our water, soil, and even the food we eat. They get used to make things waterproof, greaseproof, or stain-resistant. If you’ve ever used a non-stick frying pan or worn a waterproof jacket, you’ve had a brush with this class of chemicals.
Scientists and regulators started being wary of PFAS years ago for good reason. Studies link various PFAS, including ones similar to 2-(Perfluorohexyl)ethanesulfonic acid, with health problems in people. Exposure can lead to higher cholesterol, changes in liver enzymes, and higher risks for certain cancers, based on work from organizations like the EPA and CDC. Research at the community level has connected contaminated drinking water to immune issues, hormone disruption, and even birth complications. In some places, fish caught in streams tested positive for PFAS far above safe levels, so regular folks fishing for dinner ended up with more than just protein on their plates.
Kids face higher risks. Their smaller bodies and still-developing systems can’t deal with toxics the same way adults do. Even small amounts in drinking water have drawn concern. Studies in animals show that long-chain PFAS, which include compounds like 2-(Perfluorohexyl)ethanesulfonic acid, collect in blood, liver, and other tissues. In my own city, worries about PFAS in school water fountains led to expensive filter replacements and new rules about testing citywide. Communities shouldn’t have to worry about basic necessities like water; this isn’t an abstract discussion when parents see headlines about local school water making kids sick.
Once PFAS hits groundwater, it moves slowly but sticks around a long time. Unlike other pollutants, PFAS don’t break down by sunlight, bacteria, or time. As a result, low-level contamination in one area can travel and spread wider each year. PFAS bioaccumulate—meaning animals and people who eat plants or fish from polluted water keep absorbing more of these chemicals over time. Predators at the top of the food chain, including humans, get the highest exposure. I’ve read about small towns where farmers discovered their well water wasn’t safe even for livestock. Cleaning up these chemicals is no small task; it takes specialized filters and a lot of money.
One way to reduce risk is requiring companies to phase out long-chain PFAS and look for safer alternatives. Some large companies have already made the switch under consumer and regulatory pressure. Public databases are tracking PFAS sources, and new water testing rules are cropping up across the country. Putting limits in place before problems spiral out of control protects people and ecosystems better than waiting for disaster.
Regular updates on water quality and direct communication help build trust. People want to know what’s in their tap water or their favorite fishing spot, and they deserve real answers, not just technical jargon or delays. Legal action against polluters has helped fund cleanups, but more proactive steps make a difference for future generations. Supporting research into non-toxic alternatives, and holding firms accountable for clean water, keeps public health in focus.
Long-chain perfluoroalkyl sulfonic acids grab attention for both their chemistry and health impact. In my time reading up on industrial chemicals and regulation, it’s become clear that knowing not just a molecule’s name but also its structure lets us understand why these substances behave the way they do. 2-(Perfluorohexyl)ethanesulfonic acid bears a mouthful of a name—maybe it sounds removed from daily life, but its makeup really drives a story seen in modern water safety debates.
Talk about 2-(Perfluorohexyl)ethanesulfonic acid starts with that perfluorohexyl tail. Six carbons, all fluorinated, connect to an ethane chain, finishing at a sulfonic acid head. The carbon-fluorine bond causes much of the trouble and benefit. This bond holds tight against heat, stress, or decay. So, the molecule sticks around—both in products and in our environment.
Looking at the chemical formula: C8H5F13O3S. Here, eight carbon atoms create the skeleton; five hydrogens remain (necessarily fewer because so many spots already carry fluorine). Thirteen fluorine atoms shield the hexyl segment. Three oxygen atoms, together with sulfur, shape the sulfonic acid end. This arrangement stops breakdown in the environment, which has inspired a ton of global research into persistent “forever chemicals.”
Years ago, people saw value in chemicals like this because water and oil just slid right off them. Carpets, firefighting foams, cleaners—these goods all turned to perfluorinated chains for protection. Over time, more evidence piled up about water contamination and human exposure. This was no small concern. Research connected perfluoroalkyl substances to immune effects, some cancers, and problems in fetal development.
In the lab and in living systems, this molecule’s shape and bonds lead to trouble. The structure blocks the body’s usual routes for breaking down and removing synthetic compounds. Water supplies from the U.S. to Europe now show trace levels that won’t budge unless special filters come into play. People can find clear examples in the news: towns fighting to get these molecules out of drinking water, scientists pushing for better detection methods, and policymakers setting new safety limits.
The chemical backbone here both solves and creates problems. Strong, stable, easy to use in tough environments—industries built on these features. But now that we see the flip side, solutions demand something more. Non-fluorinated alternatives can do the same job in some applications; research groups across the map race to fill in the blanks for others.
Technology plays a role, too. Labs have come up with special adsorbents and advanced oxidation processes to snag these persistent compounds from water. At the same time, strict regulations spur industry away from compounds with such relentless chemical stability. I’ve heard experts say innovation comes fastest when the public demands better through policy and market choices. Genuine progress means balancing function with health and environmental protection—the key lesson behind every molecule that once looked too good to question.
2-(Perfluorohexyl)ethanesulfonic acid slips into the spotlight because it’s a perfluoroalkyl substance. That means it lingers for ages in water, soil, and even inside living things. Last summer, I toured a lab where a chemist told me these compounds punch above their weight: tough and persistent, and not the kind of thing you want to spread around. Many countries already clamp down on how people use and dispose of these chemicals due to growing health concerns and environmental risks.
Storing 2-(Perfluorohexyl)ethanesulfonic acid starts with the basics. Glass, stainless steel, or polyethylene containers give the best shield. I’ve watched people edge toward cheap plastics, but those can crack or dissolve if exposed long enough. Containers need tight seals. Don’t just toss this stuff on an open shelf — always set it in a well-marked, dedicated cabinet, away from sunlight and heat.
Everything starts with labeling. The last time our supply closet mixed up a jar, it came close to a disaster. Labels need large, clear lettering and include hazard symbols so nobody gets caught off guard. Separate this acid from flammable solvents, strong bases, or anything reactive. No shortcuts. I saw a minor spill once in a university lab, and the headache from fumes pushed that rule home for good.
Handling the acid gets risky without real barriers between you and potential splashes. Full nitrile gloves, safety goggles with side shields, and a lab coat cover the basics. Face shields work best for larger transfers. No one ever expects a container to tumble, but I’ve seen sleeves save skin from a quick splash. Always open and use near a chemical fume hood. I remind trainees: respect that vent, don’t ignore a whiff or weird odor.
My own experience says comfort works against safety. It’s tempting to rush or stretch the rules under pressure. Bit by bit, you risk traces of acid on door handles, computer keyboards, or even your phone. So hand washing should never get skipped. Wash before and after, even if you wore gloves. One chemist in my old lab set phone reminders because old habits die hard.
If a leak hits the counter or floor, drop everything else and pull out the spill kit. Most labs have neutralizing agents, absorbent pads, and safe disposal bags ready. Avoid paper towels or rags. Nobody likes reporting an accident, but hiding it never works — tiny bits left behind can keep causing trouble for months. Alert everyone, evacuate if the spill’s large, and follow the training as rehearsed. In the worst case, emergency showers and eyewash stations should always stay unblocked and ready.
There’s no way around the fact that 2-(Perfluorohexyl)ethanesulfonic acid demands specialist waste handling. Local hazardous waste teams usually step in, and unmarked waste containers won’t cut it. Never pour this stuff down the drain. Fact: in a New Jersey community, trace PFAS built up for years in the water supply and only got noticed after new guidelines caught up with better testing methods.
All in all, knowledge and respect guard both yourself and your neighbors from the stubborn reach of these chemicals. People, the environment, and even the lab fridge will thank you for thinking ahead and following real safety measures each time this acid appears on the shelf.
Sometimes the most influential tools in industry don’t show up on the packaging or in daily headlines, but play a big role nonetheless. With a name that's a mouthful, 2-(Perfluorohexyl)ethanesulfonic acid has quietly worked its way into some of the most crucial sectors, taking advantage of its unique chemical makeup that adds resilience wherever it lands. Growing up in a family of electricians, I saw firsthand how performance chemicals took wiring and circuit protection to a new level. Many substances came and went, but the ones that truly stuck around offered something rare—stability and reliability under stress.
I once helped replace old, finicky circuit boards in a local school's computer lab. The old materials couldn’t handle heat or moisture over time—they broke down, requiring constant replacement. Today, some manufacturers turn to chemicals like 2-(Perfluorohexyl)ethanesulfonic acid to add durability to semiconductors, resistors, and battery components. The acid provides a stable surface that shrugs off water and oil, extending the life of electronics. That reliability isn’t just a perk; it means less e-waste and lower replacement costs. According to a 2023 IEEE report, electronic industries value perfluorinated compounds for their role in keeping sensitive components safe from breakdown—a small addition, but one that heads off headaches for users and tech teams alike.
Firefighters count on foams to handle stubborn fuel-based fires. 2-(Perfluorohexyl)ethanesulfonic acid gets blended into some foams thanks to its ability to repel oil and water, making it a key ingredient in “AFFF” foams. I’ve spoken with rural fire departments that keep these foams on hand for the rare but devastating tanker fires. Quick, even spread on hard-to-reach surfaces can make the difference between control and catastrophe. But perfluorinated chemicals, including this acid, raise red flags for environmental impact. In 2022, a study from the Environmental Working Group flagged their persistence in groundwater near military training sites. That brings up tough questions—do we chase better alternatives or double down on cleanup technology? Some emerging solutions, like fluorine-free foams, may eventually push older formulations aside, but for now, many teams feel stuck between effectiveness and long-term safety.
Industries keep looking to cut down on material waste and improve product lifespans. I watched a small automotive repair shop work magic on corrosion-prone parts using coatings enhanced by fluorinated acids. Instead of quickly eroding, brake or fuel system components resisted salt and road grime far longer. That's not just a win for mechanics—it’s a money-saver for car owners, too. Research from the Society of Protective Coatings in 2021 confirmed that these materials help slow rust in everything from wind turbines to ships, cutting maintenance costs and accidents from equipment failure. Yet keeping these chemicals where they belong—off city soils and rivers—remains a challenge tossed between manufacturers and regulators.
Innovators often chase products that offer peak performance with less environmental baggage. Some chemical engineers work on substituting perfluorinated acids with biodegradable replacements, especially for consumer-facing uses. Plant-based surfactants and cleaner chemistry can’t always match fluorine’s effectiveness yet, but every step forward helps. In the meantime, setting up collection and disposal programs, tightening manufacturing standards, and investing in cleanup tech shows real promise. Progress means finding balance—making things last longer and work better, while keeping our health and water in mind.
| Names | |
| Preferred IUPAC name | 2,2,3,3,4,4,5,5,6,6,7,7,8,8,8-pentadecafluorooctane-1-sulfonic acid |
| Other names |
PFHxES 2-(Perfluorohexyl)ethanesulfonic acid Perfluorohexanesulfonylethanoic acid |
| Pronunciation | /tuː pɜːrˌfluːroʊˈhɛksɪl ˌɛθeɪnsʌlˈfɒnɪk ˈæsɪd/ |
| Identifiers | |
| CAS Number | 27619-97-2 |
| 3D model (JSmol) | `3DJChemMol("CC(C(C(C(C(F)(F)S(=O)(=O)O)(F)F)(F)F)(F)F)(F)F")` |
| Beilstein Reference | 2033883 |
| ChEBI | CHEBI:141423 |
| ChEMBL | CHEMBL2176938 |
| ChemSpider | 21541996 |
| DrugBank | DB11357 |
| ECHA InfoCard | ECHA InfoCard: 100.221.057 |
| EC Number | 80612-21-9 |
| Gmelin Reference | 84168 |
| KEGG | C20362 |
| MeSH | D079625 |
| PubChem CID | 101687764 |
| RTECS number | GW4584000 |
| UNII | OJ9G4KC8G6 |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | 'DTXSID301118794' |
| Properties | |
| Chemical formula | C8HF17O3S |
| Molar mass | 464.17 g/mol |
| Appearance | White powder |
| Odor | Odorless |
| Density | 1.7 g/mL at 25 °C |
| Solubility in water | Insoluble in water |
| log P | 2.91 |
| Vapor pressure | 1.94E-02 mm Hg at 25 °C |
| Acidity (pKa) | 1.31 |
| Basicity (pKb) | 1.35 |
| Magnetic susceptibility (χ) | -1.06e-6 cm³/mol |
| Refractive index (nD) | 1.302 |
| Viscosity | 650 cP |
| Dipole moment | 3.5736 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 256.2 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -2240.6 kJ/mol |
| Hazards | |
| Main hazards | Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H332, H314 |
| Precautionary statements | P260, P261, P264, P273, P280, P301+P330+P331, P304+P340, P305+P351+P338, P312, P337+P313, P363, P391, P403+P233, P405, P501 |
| LD50 (median dose) | LD50 (median dose): >2000 mg/kg (rat, oral) |
| NIOSH | TT8222000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 2-(Perfluorohexyl)ethanesulfonic acid is not specifically established by OSHA. |
| REL (Recommended) | 0.1 mg/m³ |
| IDLH (Immediate danger) | NIOSH does not have an established IDLH value for 2-(Perfluorohexyl)ethanesulfonic acid. |
| Related compounds | |
| Related compounds |
Perfluorooctanesulfonic acid Perfluorobutanesulfonic acid Perfluorohexanoic acid Perfluorooctanoic acid 2-(Perfluorooctyl)ethanesulfonic acid |
