© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Acido heptafluorobutirico, known more widely by its English moniker heptafluorobutyric acid (HFBA), didn’t emerge out of thin air. Chemists in the twentieth century chased more exotic organofluorine compounds, each new synthesis fueled by the post-war chemical revolution. The field spun up quickly, partly thanks to landmark discoveries in fluorocarbon chemistry, with folks eager to see how fluorination could rewrite the rules for stability and reactivity. Somebody noticed early on that swapping hydrogen atoms for fluorine changed everything—from the boiling point to biological behavior. HFBA didn’t become a household name, but it showed up reliably wherever analytical chemists needed a high-quality ion-pairing agent or sample modifier. Not everyone in the lab needed it, but those chasing greater sensitivity in mass spectrometry or chromatography soon considered it a quiet workhorse. As commercial interest in environmental, pharmaceutical, and bioanalytical applications grew, so too did the precision with which suppliers could meet purity demands, hinting at a chemical that punches above its weight in niche but crucial roles.
Dig into a bottle of HFBA, and you’re dealing with a colorless, oily liquid with a nose-wrinkling, acidic odor. What sets it apart from regular butyric acid is the full house of fluorine atoms—seven, blanketing the carbon backbone. That blanket makes it resistant to both oxidation and classic breakdown routes, a trait fluorinated molecules share. HFBA’s structure—CF3CF2CF2COOH—lands it firmly in the category of perfluorinated carboxylic acids. Unlike infamous long-chain perfluorinated chemicals such as PFOA, HFBA usually comes in at four carbons, falling into a slightly different risk and performance zone. Its pungent edge, persistent properties, and hydrophobic nature combine in an oddly useful way for chemists searching for robust performance under tough analytical circumstances.
People working with HFBA know its boiling point hovers around 122°C, and its density edges over typical organic acids. The electronegativity of all that fluorine does more than just jack up the molecular weight—it tunes both the acid’s dissociation constant and its solvent compatibility. The molecule is surprisingly stable, showing little interest in giving up protons except in very strong bases. It shrugs off many oxidants and won’t catch fire easily, which may seem like a relief until you remember that its volatility and vapor are nothing to treat casually. The acid’s ability to alter surface energy and confer resistance to water marks its territory in advanced material research, while its keen acidity finds use in peptide chemistry and mass spectrometry.
Inside research labs, the grade of HFBA matters—trace impurities stand out quickly. Analytical standards outline purity above 99 percent. Product labels usually carry CAS numbers (375-22-4 for this acid), flashpoint values, and detailed storage instructions since prolonged exposure to air or light can drive down performance or stir up decomposition products. Labels also mark hazard statements—the acid stakes its claim as acutely corrosive and often gets shuttled into fume hoods or glove boxes when work extends beyond quick transfers. There’s a premium on sealed storage, as the volatility and strong odor can overwhelm open-bench space. Tracking inventory, date opened, and shelf life lines up with good laboratory practice, not because of legal red tape, but because lost potency or cross-contamination sabotages analytical data in subtle, frustrating ways.
Prepare HFBA by throwing together heptafluorobutyrate salts and hitting the right acidification conditions—think mineral acids under controlled cooldown while avoiding moisture spikes that could ruin yields. Industrial-scale synthesis means keeping fluorination runs contained, dealing with hazardous intermediates, and building in procedures for waste treatment. No home garage setup replicates these conditions safely. Lab-level tweaking focuses on final purity: distillation steps, solvent washes, and vacuum drying flag the difference between research and technical grades. Experienced chemists look at every step, minimizing side reactions that spit out unwanted fluorocarbons or accidental byproducts—nobody wants a bottle of mystery.
The world of organofluorines likes to play its cards close to the chest, so not just any reagent can nudge HFBA into action. Alkali metals, strong bases, or certain nucleophiles find traction, but most standard reduction or substitution tools bounce off with little result. The carboxylic acid group offers a limited handle—activation forms can allow coupling, esterification, or salt formation. Each modification tries to walk the tightrope between enhancing utility and not sacrificing the unique fluorinated stability. Researchers also test whether blending in other perfluorinated tags amplifies performance for environmental analytical methods, protein sequencing runs, or niche industrial catalysts. These routes don’t always pay off, but lucky tweaks sometimes birth a more effective tool for the analytical chemist’s arsenal.
You’ll see HFBA appear under several guises: heptafluorobutyric acid, perfluorobutyric acid, or, in a database search, 2,2,3,3,4,4,4-heptafluorobutanoic acid. Each name hints at its structure or function, helping buyers, researchers, and regulators find clarity in a crowded field of related chemicals. Sometimes commercial brands riff on these names for their catalogues, but no matter the branding, the core product’s function and hazard profile remain fixed.
Nobody learns to respect HFBA the easy way. The sharp smell cues most users to avoid open containers, but that’s just the start. Local exhaust ventilation, gloves, goggles, and acid-resistant lab coats headline most safety protocols. Solvent-resistant materials usually get the green light, though long-term exposure chews up weaker plastics and some elastomers. If you spill it, neutralizing with sodium bicarbonate works in small lab settings—industrial-scale accidents entail a messier, more expensive fix. Safety data sheets warn about vapor inhalation, skin burns, and chronic exposure risks. Disposing of HFBA takes more than just a neutralization step; collecting spent acid and sending it out for specialist waste management fits the norm wherever the compound gets routine use. Most folks don’t take shortcuts here since lab accidents can shut down programs, waste budgets, and demand health monitoring.
HFBA doesn’t grab the spotlight in mainstream manufacturing but instead earns its keep in sharp-focused research and commercial labs. You can spot it as a mobile phase additive in liquid chromatography techniques, where it enhances separation power or suppression of unwanted background signals. Mass spectrometry applications in pharmaceutical and environmental labs pull it off the shelf for similar reasons: it strengthens signal clarity for certain analytes, especially peptides or small organic molecules. Occasionally, materials scientists dabble with HFBA when modifying surfaces to resist water or certain oils, but most high-volume modifications pivot to longer perfluorinated acids. The acid’s strong acidity, chemical resistance, and volatility keep it relevant where process robustness and ultra-low contamination matter more than price per liter.
New synthetic routes, alternative fluorination strategies, and greener production approaches keep research on HFBA and its chemical cousins alive. Some groups look into tailoring HFBA’s properties further to coax different behavior in protein sequencing platforms or to fine-tune retention times in chromatographic runs. Others poke at biodegradability, hoping to unearth analogs less likely to accumulate in soil and water. Collaboration between academic labs, industry, and regulators is essential to draw lines around safe use and disposal. Funding doesn’t flow as freely as with high-profile pharmaceuticals, but steady progress in analytical chemistry and material science keeps HFBA’s future relevant. Technology advances quickly, but as detection limits shrink and new bioactive compounds demand analysis, small tweaks to HFBA’s chemistry or purity could open new frontiers.
Perfluorinated chemicals spark more scrutiny every year, and HFBA is no exception. Early animal studies flagged organofluorines as tricky—resistant to biological breakdown and prone to lingering in ecosystems. Exposure to high concentrations leads to irritation, tissue damage, and sometimes, longer-term health effects that aren’t fully understood. Safety assessments by regulatory agencies aim to keep environmental levels under control, particularly in wastewater and solvent emissions. Labs handling HFBA need to balance sharp chemical performance with protocols minimizing chance of environmental leakage. Researchers tracking bioaccumulation sometimes sound alarms, but the four-carbon chain of HFBA puts it in a somewhat different risk band than longer cousins linked to persistent organic pollutant lists. Debate continues around thresholds and safe exposure limits, and the call for deeper, longer-term toxicology data grows louder. Responsible handling and targeted research are ways forward—hopes hinge on smart containment, better waste treatment, and improved procedural transparency.
HFBA’s future rides on both technology trends and the regulatory climate. Analytical labs aren't slowing down—every year brings more sensitive instruments, more complex sample matrices, and stiffer accuracy demands. HFBA stays relevant as long as it sharpens data and survives cleanly in harsh chemical landscapes. Synthetic chemists tease out new analogs and look for greener fluorination footprints. Regulatory attention on perfluorinated chemicals casts a shadow—compliance could squeeze some applications, making way for less persistent alternatives or recycling protocols. Where market pressure and safety line up with cleaner, sharper lab results, HFBA found its niche. No magic bullet exists. Careful stewardship, ongoing toxicity research, and open data sharing between makers, regulators, and end users offer the best shot at harnessing the power of acido heptafluorobutirico without writing off environmental responsibilities.
Acido heptafluorobutirico doesn’t show up in dinner table conversations, but anyone who’s handled tough chemical syntheses recognizes the value it brings to the lab bench. It’s one of those small molecules with a big personality—built from a butyric acid core but swapped out for a powerful, seven-fluorine punch. Fluorinated acids like this one hold a special place in research and manufacturing, mainly because they behave a lot differently from the acids people meet in everyday life.
Labs working with advanced analytics use acido heptafluorobutirico as an ion-pairing agent in high-performance liquid chromatography (HPLC). I’ve spent enough time around analytical chemists to appreciate how much these folks sweat the details. With tiny traces making or breaking a result, a compound that shapes how molecules move through a column proves its worth. Heptafluorobutyric acid tweaks the interactions between the stationary phase and target molecules, so separation improves, giving sharper, more reliable peaks. A well-resolved chromatogram might be the only solid proof a drug compound even exists. Researchers rely on that kind of confidence.
Back in grad school, people in the next lab ran peptide maps for breakfast. They kept bottles of heptafluorobutyric acid at their elbows. Peptide chemists use it for both synthesis and purification. It acts as a counterion in mass spectrometry and supports clean, consistent signals for peptide and protein analysis. When accuracy means the difference between a correct protein sequence and a false lead, every step needs to count. Manipulating such a delicate process calls for strong yet predictable acids, and this fluorinated acid ranks among the handful that deliver.
Formulators and quality teams tap heptafluorobutyric acid to tweak how active ingredients dissolve. They don’t just pick any solvent off the shelf—bioavailability in new drugs sometimes hangs on tiny chemical tweaks. This acid can adjust the solubility of certain stubborn components. Facing FDA scrutiny, a small edge like that can make or break a development program. There’s a real pressure to innovate. Drug companies always hunt for tools that offer a consistent, controllable tweak to a process. This is one of those tools.
Powerful chemicals bring a catch. Heptafluorobutyric acid isn’t something to splash around. Strong acids, especially with fluorine atoms, mean safety rules tighten up. Gloves and goggles don’t even cover the full safety story—ventilation and spill controls become daily habits. Environmental teams raise another flag: fluorinated chemicals hang around in soil and water. Cleaning up later comes at a cost, both financially and for the reputation of an organization. I’ve seen research teams spend good money testing new waste neutralization methods, so nobody’s left with a problem that persists for generations. That’s an investment every lab has to consider up front.
Green chemistry programs now look for alternatives or recycling methods. Teams balancing efficiency with environmental health see the sense in minimizing use or searching for less persistent substitutes. More labs share protocols on using the smallest effective amounts or reclaiming valuable reagents before disposal. Keeping our tools sharp—and our ecosystems safe—matters in research that aims for progress without regret.
Acido heptafluorobutirico is not something you find in every garage or local lab. People usually run into it in specialized chemistry labs or certain manufacturing plants. Its strong acidity and reactive fluorinated structure require respect. Getting even a splash on your skin or breathing the fumes can cause real harm—think chemical burns, not just an itch or mild irritation.
Every lab hand who has worked with corrosive acids knows that gloves and goggles are the baseline. For acido heptafluorobutirico, nitrile gloves work better than latex, which breaks down too quickly. A splash-resistant face shield or goggles should go over the eyes. Add a lab coat, ideally with a chemical-resistant apron if there’s any chance of spills. Shoes should be closed-toe and sturdy. Fumes hang in the air, so a good lab always leans on the side of caution by running reactions in a dedicated fume hood with the sash kept low.
Strong acids like this one push out fumes that irritate lungs and eyes right away. An open window or a small fan does nothing to protect against invisible gases. Turning every experiment into a routine—checking that the fume hood pulls properly, keeping containers capped, and never working outside the hood—saves people from accidents that cause lifelong health problems.
In my earliest days in the lab, a spill kit looked like just another box on the wall. The first time a coworker knocked over a beaker, I realized that neutralizing powders, absorbent pads, and a ready shower station matter a lot more than the paperwork. With heptafluorobutyric acid, you want calcium carbonate or bicarbonate handy to neutralize. Water alone just splashes the acid. If it gets on skin, rinsing with running water for at least 15 minutes gives the best shot at minimizing damage. Every second counts.
Never park bottles of this acid next to anything that reacts with acids, like bleach or ammonia cleaners. Strong acids attack many plastics and metals, so bottles must be made of compatible materials—polyethylene or Teflon work best. Always store acids below eye level, on sturdy shelves with spill lips or trays underneath. Label everything, even temporary containers or syringes, so everyone knows what they’re reaching for. A quick glance can stop mistakes before they start.
No chemical is “safe” just because someone follows a checklist. A lot of trouble comes from shortcuts or trying to save time. In my experience, labs that take their training seriously see fewer accidents and smaller messes when things go wrong. Regular reminders about emergency showers, eye washes, and spill response keep the basics sharp. Sharing stories about near-misses helps, too; nothing sticks in the mind like seeing how easily tiny mistakes become big problems.
Pouring extra acid down the drain is asking for plumbing trouble and environmental fines. Special containers, marked for hazardous waste, help labs track how much they’re discarding and keep everything out of the regular trash. Scheduled pickups and clear labeling make life smoother for everyone and keep the community safe outside the lab walls.
Learning about chemicals often reminds me of my undergraduate days in the lab, fiddling with vials and pipettes, fingers always smelling faintly of something scientific. Ácido heptafluorobutírico sticks out partly because its name tells you a lot about its structure. It’s a mouthful, but each piece has meaning. “Ácido” signals it’s a carboxylic acid. “Heptafluoro” means seven fluorine atoms. “Butírico” hints at a four-carbon chain, like butyric acid but with a major twist due to all that fluorination.
Take ordinary butyric acid. Its formula runs C4H8O2. Those hydrogens get swapped out for fluorine atoms to make room for the electronegativity that fluorine drags into the mix. In heptafluorobutyric acid, you end up with C4HF7O2—or you can write it as C3F7COOH. That COOH at the end, familiar from biology class, marks the functional group that gives acids their personality.
Fluorine always changes the rules. Its presence in any organic compound often ramps up stability and alters reactivity. Ácido heptafluorobutírico turns up in chromatography labs, where separating molecules that look almost identical takes a little chemical muscle. The strong electron-withdrawing effects of those fluorines give this acid its edge. This gives scientists access to purer results, which ultimately can mean better medicines, cleaner water samples, and more accurate forensic data.
I’ve run into heptafluorobutyric acid in the context of high-performance liquid chromatography, or HPLC. In sample prep, even a small impurity can ruin a run. Using an additive like this acid with its unique properties helps coax better separation. Simply put, many research projects move forward because someone chose the right chemical.
It’s easy to look at acids—and especially those laden with fluorine—and feel a little hesitant. Rightly so. Exposure to fluorinated acids carries risks. They are corrosive, potentially toxic, and can produce harmful gases if mishandled. Material safety data sheets spell this out clearly. Safe labs use fume hoods, gloves, and goggles. In my own labs, one whiff of the distinct scent and everyone straightened up and checked the PPE. Chemical safety training shouldn't gather dust.
Environmental impact is another point to weigh in. Perfluorinated compounds linger in nature far longer than traditional organics. Unlike your garden-variety vinegar, these don’t break down easily. The scientific community continues looking for greener alternatives or ways to neutralize waste, but progress travels slowly when safety, convenience, and cost all compete.
One option is to swap in acids with fewer fluorines or different chemical groups if the chromatography loss can be tolerated. Research into enzyme-based treatment for waste products shows promise in degrading stubborn fluorinated compounds. Training remains crucial. Many accidents come from skipped steps, not unfamiliar chemicals. Well-labeled storage, regular inspections, and plain old respect for the bottle help maintain a safer relationship with any reactive compound.
The formula C3F7COOH represents more than just a collection of atoms. Each use brings up choices in safety, environmental impact, and scientific advancement. Careful handling and mindful disposal help researchers keep moving forward—without taking shortcuts that catch up years later.
ACIDO HEPTAFLUOROBUTIRICO shows up in the chemical world as an industrial workhorse, popping up in labs, manufacturing plants, and research facilities. Its uses cover specialty syntheses and unique applications in materials science and analytical chemistry. Yet, every time I see a bottle of this acid, I know it demands respect and careful handling. The hazards from mishandling go beyond property damage. They touch every person in and around storage spaces. Eyes, skin, air—the consequences get real fast. I’ve watched experienced colleagues pause before opening containers of strong acids, not out of fear, but because the stakes are so high.
This acid is highly corrosive. It can eat through organic tissue and certain plastics, and if vapors escape or a leak starts, everyone nearby gets exposed. Many acids play rough, but fluorinated varieties, like heptafluorobutyric acid, add another layer of danger: They release toxic vapors that can seriously harm the lungs or eyes. I met a researcher who underestimated just a small spill—he ended up in the hospital for respiratory support. That memory sticks with me. Security in storage is not only a line in a manual—it is personal safety, every day.
The right storage solution starts with material compatibility. ACIDO HEPTAFLUOROBUTIRICO demands containers made of PTFE or other resistant fluoropolymers. Ordinary plastics, metal cans, and glass sometimes fall short because the acid can chew through seals, hinges, or even container walls over time. I always double-check chemical compatibility before restocking our cabinets, because cutting corners is risky. My advice: No shortcuts, not even for temporary storage. If the container or label looks off or degraded, transfer the acid using proper protocol.
Temperature control makes a difference. Labs with poor ventilation or temperature swings see a spike in small leaks and vapor buildup. Store acid in cool, dry spaces—under 25°C. High heat speeds up vaporization, releases more fumes, and risks pressurizing tightly sealed bottles. That’s a recipe for a burst cap or a blown-out container. So, I make a habit to check thermostats and air conditioning units in chemical storage rooms, before the busy season kicks in.
Good airflow is crucial. I once worked in a space where local exhaust fans would fail unpredictably. Acid fumes would sneak into the hallways, setting off detectors. Designated acid cabinets with built-in ventilation keep vapors contained. Never treat general-purpose cabinets as a substitute—chemical-specific cabinets are worth every dollar.
Clear labeling can turn near-misses into safe outcomes. Avoid abbreviations that might confuse new team members. Write out or print “ACIDO HEPTAFLUOROBUTIRICO” and stick the hazard pictograms right on the front. In fast-moving labs, labels get smudged or fall off. Check weekly, not just once per quarter. I keep a stash of extra hazard labels for anything that starts to peel.
Plan for spills before they happen. Absorbent materials for fluorinated acids, neutralization agents, gloves, goggles, and a face shield should sit within arm’s reach, not buried in a locked storeroom. In my experience, most labs keep a spill kit, but few people review how to use it until something goes wrong. Run drills and talk through steps with your team at least once a year. Knowing who calls emergency responders and who manages the clean-up minimizes panic and injuries.
ACIDO HEPTAFLUOROBUTIRICO won’t cause trouble if you treat it with the caution it deserves. That means an acid-safe container, cool and ventilated storage, clear labeling, and a tested spill response plan. I’ve seen places where each of these safeguards worked together to stop an incident before it started. Respect the risks and build a system where safety practices are second nature. The peace of mind—and health of your team—make it more than worth the effort.
People come across plenty of strange chemicals at work, but acido heptafluorobutirico (also known as heptafluorobutyric acid) stands out for its unique mix of hazards. Its use shows up in everything from pharmaceuticals to chemical analysis labs. It’s strong, with a bite that’s easy to underestimate when hidden behind those lab goggles and gloves.
Few folks realize how quickly this acid goes after the skin. Splashing a tiny amount can bring sharp burns, redness, and blistering—think of handling something like industrial-strength bleach without protection. If I ever work in a lab, I trust the story of a coworker who brushed against just a drop: He felt burning that didn’t stop once he rinsed it off. It penetrates skin deeper than most cleaners at home. Health and safety data sheets point out the risk of lasting scars, or worse, if this acid gets into wounds.
The throat and lungs don’t get off easy either. Even vapors from acido heptafluorobutirico cause coughing, sore throats, and in some people, chest tightness. Weakening of the airway lining, similar to what you’d expect from strong acids, creeps up faster if the air’s warm or if there’s poor ventilation. Everybody hates the eye sting from chopping onions; try this acid in the air and it’s not just stinging—there’s potential for real eye damage. Reports from people in cleaning jobs or research labs tell about blurred vision or long-term irritation if they worked without goggles or had a spill.
Long-term use brings bigger worries. I read about some technicians who handled this chemical for years. Even without dramatic, one-time accidents, repeated low exposure led to chronic dry skin, eczema, asthma, and persistent coughing. Chemicals like this one can send subtle signals—dry hands, fatigue, missed workdays—before anyone realizes things have gone wrong. It sticks with you if personal protective gear isn’t worn every time. Respect slips; tiny mistakes add up fast.
Acido heptafluorobutirico counts as a perfluorinated compound. These molecules hang around in the water, soil, and living things longer than nearly anything else from the chemical factory. They don’t just vanish after rinsing away. Studies call out their links to hormone disruption and certain cancers in places with contaminated water. I remember reading about towns where these compounds got into groundwater—the clean-up takes years, if it’s possible at all. As the public learns more about PFAS (the class of chemicals this acid belongs to), trust in local water supplies takes a big hit and nerves run high.
Real talk: safety comes down to habits. Replace casual handling with strict glove and goggles use. Invest in up-to-date ventilation systems. Insist on proper training for new workers—share stories and mistakes, not just textbook warnings. Push your workplace to test local air and water for signs of chemical build-up. Switch out equipment as soon as it degrades, since worn seals or cracks don’t stay contained. Fight for proper disposal; don’t let shortcuts slip past routine just because the chemical’s name sounds complicated.
If you notice coworkers skipping steps or rolling their eyes at “extra paperwork,” speak up. Bringing it up can save pain, lost wages, and, frankly, lives—nothing speaks more clearly than someone who’s faced the risk directly.
| Names | |
| Preferred IUPAC name | 2,2,3,3,4,4,4-heptafluorobutanoic acid |
| Other names |
Heptafluorobutyric acid HFBA Perfluorobutyric acid 1,1,1,2,2,3,3-Heptafluorobutanoic acid |
| Pronunciation | /ˈa.si.ðo ep.ta.flwor.oβuˈti.ɾi.ko/ |
| Identifiers | |
| CAS Number | 375-22-4 |
| Beilstein Reference | 1721863 |
| ChEBI | CHEBI:52805 |
| ChEMBL | CHEBI:40420 |
| ChemSpider | 4846 |
| DrugBank | DB01927 |
| ECHA InfoCard | 21c8ba2c-b3bc-4bab-8beb-086e6e4cdb67 |
| EC Number | 206-203-2 |
| Gmelin Reference | 78655 |
| KEGG | C14377 |
| MeSH | D006520 |
| PubChem CID | 9863 |
| RTECS number | EL9100000 |
| UNII | F3GEC88T31 |
| UN number | UN2420 |
| Properties | |
| Chemical formula | C4HF7O2 |
| Molar mass | 214.04 g/mol |
| Appearance | Colorless liquid |
| Odor | Pungent |
| Density | 1.7 g/cm³ |
| Solubility in water | Soluble |
| log P | 2.1 |
| Vapor pressure | 12.7 hPa (20 °C) |
| Acidity (pKa) | 1.40 |
| Basicity (pKb) | 1.41 |
| Magnetic susceptibility (χ) | -9.3 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.252 |
| Viscosity | 0.89 cP |
| Dipole moment | 2.29 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 362.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1346.1 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1562 kJ/mol |
| Hazards | |
| Main hazards | Corrosive, causes severe skin burns and eye damage, harmful if inhaled, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H302, H314 |
| Precautionary statements | P260, P264, P270, P271, P301+P330+P331, P304+P340, P305+P351+P338, P310, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 3-0-0 |
| Lethal dose or concentration | LD50 oral rat 200 mg/kg |
| LD50 (median dose) | LD50 (median dose): 200 mg/kg (oral-rat) |
| NIOSH | RN7713 |
| REL (Recommended) | 0.5 ppm |
| Related compounds | |
| Related compounds |
Nonafluoropentanoic acid Perfluorooctanoic acid Perfluorobutanoic acid Perfluoropropionic acid Perfluorodecanoic acid |
