Long-chain alkyl halides turned heads in the early 20th century because chemists were looking for ways to make new surfactants and intermediates. Lauryl chloride got much of the spotlight, but 1-Chlorooctane filled a gap for those interested in shorter chain, hydrophobic molecules. Chemists first explored the halogenation of octane during the growth of organic synthesis, just as industry started to crank out bulk organics for soaps and plastics after World War II. Today, 1-Chlorooctane lines shelves of specialty chemical warehouses, a reminder of how small discoveries open up new tools. Current manufacturers in Europe and Asia base their production designs on methods worked out fifty years ago, showing that some reactions never go out of style.
1-Chlorooctane falls under alkyl chlorides, featuring a straight eight-carbon chain with a chlorine atom hanging off the end. You’ll spot it as a colorless, oily liquid, mild as far as organics go, though it will sting if inhaled too sharply. Labs often keep a bottle around for organic synthesis, particularly for introducing eight-carbon tails in surfactants, or using it as a feedstock for further alkylation steps. Some see it as a little-studied intermediate, but it’s a real workhorse for anyone who needs controlled reactivity and a specific hydrophobic profile. Despite not being glamorous on its own, it fits into broader schemes—pharma, agrochemicals, even specialty polymers. As chain lengths go, C8 isn’t too bulky nor too volatile, giving it a sweet spot among linear alkyl halides.
With a boiling point hitting around 179°C and a melting point down at −65°C, 1-Chlorooctane is clearly practical in a wide range of temperatures. Its density clocks in at roughly 0.87 g/cm³, lighter than water but heavier than many volatile organics. Not surprisingly, it refuses to mix with water and dissolves easily in nonpolar solvents like hexane or ether. Don’t mistake its mild smell for safety—chlorinated organics have a way of creeping through gloves and evaporating if left uncapped. Its refractive index lands around 1.426, so it shows up clear and unassuming in a glass flask. Chemically, the C-Cl bond stands firm, meaning you need a strong nucleophile or some decent heat to displace it. Sunlight or UV exposure may eventually crack it through photolysis, but in the bottle, it holds up well.
Bottles appear labeled by both IUPAC and trade names. Most commercial grades promise purity above 98%, sometimes even 99%+. Spec sheets break out impurity profiles—mass spectrometry and GC traces reveal any leftover octane or unreacted chlorinating agents. Typical labels warn against flames and urge storage in a cool, dry spot, since the vapor can form explosives if left unchecked near ignition sources. Documentation leans on GHS (Globally Harmonized System) symbols, including skull and crossbones, exclamation marks, or health hazard icons depending on concentration. Some countries insist on secondary barcodes or RFID tagging for tracking. Users inspect container seals, batch numbers, and expiry dates carefully since trace hydrolysis or polymerization, if unchecked, could change product specs quickly.
Traditional lab preparation sticks with the classic nucleophilic substitution on 1-octanol. Phosphorus trichloride, SOCl₂, or thionyl chloride converts the alcohol right to the alkyl chloride, sometimes with a dash of acid catalyst to move things along. Large-scale batches prefer continuous flow setups, reducing oxidative byproducts and controlling heat better. Each method produces side streams—hydrochloric acid, phosphorus oxychloride, or sulfur dioxide among them—which need scrubbing before venting and careful disposal to comply with modern emission standards. Occasional attempts exist at direct chlorination of n-octane, but selectivity stays low, and a cocktail of mono- and poly-chlorinated products is tough to purify. Most manufacturers refine the process over decades, tweaking ratios, improving distillations, and swapping out older glassware for lined reactors that handle the corrosive nature of chlorination chemistry.
In my own bench experience, 1-Chlorooctane shines most as a starting point for substitution. React it with sodium azide, and you get 1-azidooctane—a useful precursor for click chemistry. Drop in a strong alkali and you’ll kick off an elimination, chasing down traces of octene isomers in the pot. Grignard reactions rarely go well due to the low reactivity of the primary chloride, but switch to iodide via Finkelstein and things pick up. It forms ethers or thioethers when treated with alkoxides or thiolates, and can bridge to more complex structures in the hands of a creative synthetic chemist. Some polymer groups modify it into functionalized surfactant tails, or use it as a linker to attach hydrophobes to otherwise water-loving molecules. Each transformation highlights how that single chlorine atom opens the door for heavier manipulations when you want to swap out chain lengths or introduce complicated end groups.
Ordering 1-Chlorooctane can be tricky unless you know its aliases—n-octyl chloride jumps out as the most popular, but ChemSpider, PubChem, and chemical vendors sometimes list it as octyl monochloride or monochlorooctane. CAS Number 111-85-3 helps avoid confusions with similar chain lengths or secondary isomers, as does its EC Number 203-917-6 or UN shipping designation. Multinational suppliers give translations in half a dozen languages, which keeps global commerce humming but can confuse new chemists unless they double-check product codes. R&D labs pin its structure to C8H17Cl for clear communication.
Anyone used to working with organochlorines knows you don’t get careless. 1-Chlorooctane irritates skin, eyes, and the respiratory tract, so gloves and goggles remain non-negotiable. Fume hoods offer the best way to handle volumes beyond a few milligrams, especially if you’re heating or pouring. Spill management involves absorbent pads and caustic scrubbing agents, since the liquid will spread easily and resist water-based mops. Disposal guidelines follow hazardous organohalide procedures: incineration at licensed facilities for spent reagents or contaminated glassware, not casual sink disposal. Regular air monitoring in production plants checks for chronic exposure risks, while local regulators call for annual hazard training. Most companies keep SDS (Safety Data Sheets) online and in the lab binder, with emergency contacts posted in plain sight.
1-Chlorooctane finds itself at the cross-section of surfactant chemistry, agrochemical intermediates, and phase-transfer catalysis. Manufacturers graft its eight-carbon chain onto larger molecules to improve oil solubility or modify wetting properties of finished goods. You’ll see it in the backbone of some detergents, specialty antistatic agents, or as part of fungicide formulas. Researchers once exploited it for studying hydrophobicity in complex systems, and its alkylation power gets harnessed in custom pharmaceutical syntheses—especially when groups seek to dial in exactly how much grease or water-hatred a molecule needs. Production volumes don’t reach those of smaller alkyl chlorides (like ethyl or propyl), but niche demand keeps facilities running to serve high-value sectors.
R&D efforts have shifted towards greener synthesis and milder reaction conditions. Many chemists look for catalysts that reduce unwanted byproducts or energy inputs, hoping to push yields without broadening the impurity profile. Several groups pursue bio-based alcohols as starting materials, feeding into larger movements toward sustainable, less petroleum-dependent chains. Analytical teams lean heavily on GC-MS, NMR, and IR to track purity across production, battling trace chloroform or octene byproducts in every batch. On the academic front, research into mechanisms of alkyl halide reactions sometimes puts 1-Chlorooctane in the lineup alongside shorter linear analogs, using it to compare how reactivity and solubility trends evolve with chain length. The drive to extract more value from side streams or byproducts also guides process engineers.
Unlike aromatic chlorides, which get a bad reputation, straight-chain 1-Chlorooctane shows modest acute toxicity. Acute exposure may irritate the lungs and mucous membranes, though chronic data remains limited. Animal studies report relatively high LD50 figures, but its long-term ecological fate deserves careful tracking. It doesn’t persist like PCBs, but improper disposal runs the risk of building up in water or sediment. Regulatory agency reviews focus on occupational exposure limits rather than consumer safety, since 1-Chlorooctane rarely appears in foods or pharmaceuticals. I’ve watched safety officers lean heavily on VOC monitoring and periodic health screening, a reminder that careful risk management helps prevent surprises down the line. Researchers study its behavior under advanced oxidation, biodegradation, and photolysis to see how quickly and safely it breaks down outside the lab.
I see steady demand for 1-Chlorooctane in specialized chemical synthesis. As green chemistry picks up steam, companies want alternatives for hazardous reagents and waste-intensive processes. If catalysts emerge that let manufacturers swap out chlorine for less problematic groups—or use electrochemical halogenation with renewable energy—production could both scale and shrink its footprint. Analytical chemists might refine detection techniques, making trace-level monitoring in soils or waters routine. Market analysts note small growth in custom surfactants, especially as industries chase more environmentally friendly formulations that need just the right hydrophobic tail. Industrial partners will keep tweaking synthetic routes, hoping to drive down costs and up efficiency, but users at every level keep circling back to the same handful of chlorinated intermediates, reflecting just how persistent established building blocks remain in organic chemistry.
Every time I walk into a lab, there’s a sense of respect that goes along with chemical names and formulas. It’s not just a bunch of letters and numbers. The chemical formula of 1-Chlorooctane, written as C8H17Cl, packs a story about how atoms knit together to create something unique. Eight carbon atoms, seventeen hydrogens, and a single chlorine atom—all these come together to give 1-Chlorooctane its identity. Just as you might recognize a friend across a crowded room, chemists spot structure from formula just as fast.
For folks working in chemistry, the formula isn’t just neat trivia. It’s a set of instructions, a guide for what’s going on in that flask or beaker. 1-Chlorooctane, with its simple skeleton of a straight eight-carbon chain and that chlorine atom sitting on one end, gives away a lot about its behavior. Put this in the hands of a synthetic organic chemist, and the pathway for building new compounds unfolds quickly. The carbon chain acts as a steady backbone, and the chlorine doesn’t just sit there for decoration—it brings reactivity, opening the door to new reactions like nucleophilic substitution, where other atoms and groups can swap places with that chlorine.
Anytime you’re dealing with halogenated hydrocarbons like 1-Chlorooctane, you can’t ignore what the formula tells you about safety. That single chlorine atom can make a huge difference, making the compound less friendly to the environment compared to a regular hydrocarbon. It doesn’t dissolve in water, and it can hang around in soil or water far longer than anyone would like. I’ve watched workers double-check their safety data sheets before opening a bottle, knowing that what seems simple on paper can be hazardous in real life. Labels and chemical formulas become shields in the hands of careful users.
Most people will never handle a beaker of 1-Chlorooctane themselves, but its presence ripples out into parts of life you might not expect. It’s a stepping stone in the world of chemical manufacturing, helping to build more complex molecules—sometimes destined for pharmaceuticals, or for materials that line wires and cables. I’ve seen formulas like C8H17Cl scribbled down alongside to-do lists and project flowcharts in process plants and academic labs alike.
Chlorinated compounds raise tough questions about balancing innovation and environmental responsibility. I’ve talked with researchers eager to phase out certain chlorinated solvents, searching for alternatives that cut risks without losing effectiveness. Industry regulations and green chemistry both have parts to play, pushing for new synthesis methods that keep those chlorine atoms in check and less likely to end up in a landfill or river.
Trust in science comes from verifiable facts and careful transparency. The chemical formula of 1-Chlorooctane, C8H17Cl, is one piece of data that unlocks deeper understanding. By focusing on the details—structure, safety, and real-world uses—you connect the dots between the work behind the scenes and the world beyond the lab door. Building up that knowledge base, rooted in experience and responsible use, brings everyone closer to a safer, smarter way of working with chemicals.
1-Chlorooctane stands out among chlorinated alkanes for its straight, eight-carbon backbone and single chlorine atom. I come across this name most often in organic synthesis discussions and solvent formulation work. Its chemical structure gives it certain qualities that keep it in steady demand across several sectors. Not flashy, not as toxic as many other chlorinated solvents, and not wildly expensive, it quietly earns a place on many lab shelves and in a few large-scale chemical plants.
In organic chemistry labs, 1-Chlorooctane acts almost like a starter block. Chemists use it as an intermediate—basically, a step along the way to creating more complicated molecules. If you want to add an eight-carbon chain to a new compound, this molecule does the job. Through reactions such as nucleophilic substitution, it forms octyl derivatives, which turn up in surfactant production, pharmaceuticals, and agrochemicals. I remember watching a production chemist demonstrate how small tweaks with these haloalkanes yield big changes in target drug compounds, sometimes making or breaking their ability to dissolve in fat or water.
Manufacturers often seek non-polar, specialty solvents for extracting certain substances from mixtures. 1-Chlorooctane, thanks to its chain length and modest polarity from the chlorine, fills this role in specialized situations. It helps to pull organic molecules from aqueous solutions, especially in pilot research or analytical settings. I once saw this chemical in use in a research lab focusing on separating vitamin E derivatives. The staff praised its selectivity over shorter-chain chlorinated solvents, noting fewer byproducts and an easier clean-up.
GC (gas chromatography) and MS (mass spectrometry) labs make use of chlorinated hydrocarbons as reference points or calibrants. 1-Chlorooctane’s unique signature—thanks to the combination of a single halogen and its medium-length carbon chain—means technicians reach for it as a standard. In research facilities, getting accurate measurements from instruments makes or breaks a study. Using well-characterized chemicals like this one keeps results trustworthy when quantifying unknown mixtures.
Chain-length matters in chemicals built for surface activity and spreading power. 1-Chlorooctane lays the foundation for making octyl-based surfactants. These surfactants end up everywhere, from detergents to emulsifiers in food production to additives in paints and coatings. One clear advantage comes from the tight quality controls in its synthesis, which drive consistent results in building downstream specialty molecules.
Toxicity and persistence deserve some attention. Unlike many short-chain chlorinated solvents, 1-Chlorooctane does not vaporize as readily. That brings some handling advantages in the lab and on the shop floor. Long-term, environmental persistence still causes concern, so regulatory oversight tracks its use. Its chemical cousins caused widespread groundwater issues, prompting restrictions and improved handling plans. Modern protocols insist on closed systems and vapor capture, especially during large-scale synthesis and applications.
It can be tempting to chase after exotic chemicals for every synthesis challenge, but standard tools like 1-Chlorooctane prove their worth through reliability. Companies and laboratories that adopt strict handling policies and focus on achievable recyclability help limit environmental risk while benefiting from this molecule’s versatility. For me, the lesson from working alongside experienced chemists and safety officers is clear: stick with proven chemicals for demanding jobs, but never cut corners on containment or waste treatment.
1-Chlorooctane shows up in labs, sometimes in specialty manufacturing. Most folks have never heard of it. It carries a chemical structure where a chlorine atom connects to an eight-carbon chain. You won’t find this stuff in household cleaners or food packaging, but that doesn't mean its use lacks real-world impact.
Direct exposure can irritate your skin or eyes. Anyone who’s worked with similar chlorinated compounds knows they can pack quite a punch. A few years back, during a summer spent assisting in a university lab, I learned fast to respect even a clear liquid with no strong smell—rashes and headaches don’t wait for those who ignore safety data sheets.
Toxicity data on 1-chlorooctane isn't as deep as the pile for better-known substances, but related chemicals have shown effects in animal studies. Acute exposure in high concentrations can trigger coughing and dizziness. Chlorinated solvents, as a group, don’t play nice with the liver or central nervous system when inhaled or accidentally ingested in large quantities.
Longer-term risks have a way of sneaking up on us. Chronic exposure—think of poorly ventilated workspaces or storage leaks—could mean more serious trouble. We’ve all seen stories about workers at chemical plants facing cancers or neural damage later in life. Epidemiologists have linked some chlorinated hydrocarbons to cancer in animal studies. Regulators pay attention, listing many of these chemicals as possible human carcinogens.
Disposal dumps another layer of concern into the picture. Dumping 1-chlorooctane or letting it seep into drains introduces contamination risks. Chlorinated molecules don’t break down easily in soil or water. Runoff could move into drinking water supplies, creating long-term headaches for city planners and families alike.
Wearing gloves, goggles, and respiratory protection applies here. Moving workspaces outdoors or using chemical fume hoods really cuts down the odds of inhaling something you'll regret. It’s tempting, early in a career, to skip a step for speed, but accidents stick in your memory. Practical training and reinforced safety routines pay off for everyone, from students to seasoned techs.
Material Safety Data Sheets give a clear rundown on health risks—handling this chemical calls for the sort of respect you'd show any hazardous compound. Nobody expects to spill or splash, but anyone working in chemistry for long enough learns even small mistakes can create trouble.
Regulatory bodies like OSHA and the EPA regularly review substances like 1-chlorooctane. Tracking exposure limits keeps the danger in check, so any company using or disposing of it faces legal oversight. With public pressure rising over chemical safety, some companies look for alternatives, whether that means different solvents or switching up entire processes.
You don’t always need the harshest chemicals for the job. People working to develop less dangerous substitutes help protect the environment and their co-workers. Every safer alternative adds up—a lesson science and industry keep learning the hard way.
1-Chlorooctane, with its clean, eight-carbon chain and single chlorine atom, looks simple on paper. In the lab and out in the world, this molecule shows off a handful of key features. Colorless and clear, it pours out as a liquid, not much different from other medium-length alkanes. Its molecular weight hits 148.7 g/mol, so it doesn’t drift away quickly like lighter solvents. Instead, it sticks around. The boiling point sits close to 208°C. That makes it a solid choice for processes that use higher temperatures but don’t want to worry about evaporation loss every few minutes.
With a melting point of -54°C, 1-chlorooctane handles cold storage pretty well. I’ve seen technicians forget a bottle in the fridge overnight without unexpected crystallization. They come back, and the liquid looks just as before. That sort of resilience matters in research spaces where the climate might not be perfectly controlled.
Density marks a big difference between chlorinated compounds and their non-chlorinated cousins. 1-Chlorooctane clocks in at about 0.87 g/cm³ at room temperature, a bit heavier than plain octane. Suppose someone pours a drop into water: it doesn’t mix in, but floats briefly before forming a separate, oily layer. Water’s polar nature means it won’t pull chlorooctane molecules apart. In many organic chemistry labs, this property saves time during solvent separation and extraction steps.
Pulling up the safety sheets, I learned early on that you shouldn’t expect 1-chlorooctane to dissolve in water at all; it slips right past any drain trap if you spill it, carried by its hydrophobic backbone. But it teams up with many organic solvents. Ether, chloroform, or hydrocarbons like benzene or toluene—they all welcome chlorooctane without fuss.
Vapor pressure sits at about 0.357 mmHg at 25°C, so the liquid doesn’t give off much in the way of fumes unless heated well above room temperature. Good ventilation still matters, since many chlorinated organics bring a mild, somewhat sweet scent. Even at low concentrations, the odor lingers in glassware or spills, and it signals the need for decent airflow.
From my own time in the lab, 1-chlorooctane tends to act as a stable building block. Its single reactive spot—the chlorine—can trade places with other groups, leading to bigger and more complex compounds. Synthetic chemists appreciate how the chain length delivers the balance between reactivity and manageability.
Disposal of chlorinated organics always gets a second look. The density and volatility make 1-chlorooctane manageable from a containment perspective. Still, it’s smart to remember that chlorine atoms on organics often linger in the environment and may bring health risks if inhaled, ingested, or touched often. Safety data points out eye and skin irritation on contact. I’ve found gloves, goggles, and fume hoods cover the basics in real-world practice.
Some industries now swap out certain chlorinated chemicals for greener substitutions, especially for large-scale cleaning or production purposes. That’s not to say 1-chlorooctane lacks value—just that as research marches on, chemists keep an eye out for materials that deliver the same properties with less risk at the bench and in the waste stream. For now, knowledge and simple good practice guide its everyday use in chemistry labs everywhere.
Working with chemicals like 1-Chlorooctane hasn’t always felt like rocket science, at least not at first glance. You pop the drum open, take what you need, and move on to the next thing. Over time, this routine brings its share of lessons. Not every clear liquid is just waiting to join the chemistry party—some quietly demand respect. 1-Chlorooctane, with its faintly sweet odor and oily texture, falls in that exact group.
Ask anyone who’s spent time in a lab or industrial plant: shortcuts around proper handling eventually catch up. 1-Chlorooctane won’t explode at a sneeze, but vapors creep out easier than many anticipate. Breathing even low concentrations can lead to throat irritation. Splash enough of it on bare skin, and dryness or even a mild rash can show up uninvited. You get sloppy, and the stuff finds its way onto benches, gear, and sometimes, on bad days, people. Reading the safety data sheet once isn’t enough—real understanding comes from routine, not rules alone.
Years ago, I watched a colleague tuck a bottle of 1-Chlorooctane on the top shelf. On inspection day, it turned into a headache—quite literally. The cap wasn’t tight, vapors leaked, and it left more than a sour memory. So, airtight, chemical-resistant containers became the go-to. Not because a memo said so, but because smelling your way through a workday loses its charm fast.
Warmed storage is tempting, especially in winter, but heat brings problems. Temperatures above room level push those vapors out faster, and flammability becomes a real concern. Keeping things cool and shaded slows all the trouble down. Forgetting this turns small mistakes into emergencies. And separating 1-Chlorooctane from acids and oxidizers becomes less about shelf organization, more about avoiding fires and toxic smoke. That’s something none of us want in our workplace.
Gloves, goggles, and lab coats aren’t badges—they’re shields. At first, they feel bulky, maybe unnecessary for a colorless liquid. Over time, getting a little careless leaves you with itching hands or a weird taste in your mouth from unfiltered vapors. Nitrile gloves stand up best to chlorinated solvents, cutting corners with latex leads to splits and leaks.
Eye protection isn’t just for big spills. Fine splashes from pouring or pipetting catch even the cautious. Getting it in your eye is a hospital trip nobody wants. Using a fume hood stops those vapors from floating straight to your lungs. In a pinch, good ventilation—open doors and fans—helps but doesn’t replace local extraction. It’s a matter of respecting experience, not just compliance.
Reports show repeated low-level exposures throughout a career can add up, sometimes leading to chronic respiratory or skin issues. Occupational safety data keeps this fact front and center. Regulations recommend precise labeling, spill containment plans, and clearly defined ‘no food or drink’ areas. That isn’t bureaucracy for bureaucracy’s sake—it's the combined wisdom of thousands who made mistakes, shared stories, and adjusted their routines.
The push for hazard education starts at the top, but real change sticks around through peer reminders and habits built over time. Proper training and visible reminders help cement practices, but culture—team members who speak up, challenge shortcuts, and swap stories—drives safety further than lectures.
Respecting chemicals like 1-Chlorooctane turns from inconvenience into second nature as you see firsthand how small choices affect the whole operation. Storing and handling don’t need heroics, just honest attention and consistency, day after day.
| Names | |
| Preferred IUPAC name | 1-chlorooctane |
| Other names |
Octyl chloride
n-Octyl chloride Octane, 1-chloro- 1-Chlorooctyl Caprylyl chloride |
| Pronunciation | /ˈklɔːr.oʊ.ɒk.teɪn/ |
| Identifiers | |
| CAS Number | 111-85-3 |
| Beilstein Reference | 3581647 |
| ChEBI | CHEBI:34325 |
| ChEMBL | CHEMBL16153 |
| ChemSpider | 8624 |
| DrugBank | DB13925 |
| ECHA InfoCard | ECHA InfoCard: 100.003.929 |
| EC Number | 203-900-7 |
| Gmelin Reference | 7786 |
| KEGG | C14130 |
| MeSH | D002640 |
| PubChem CID | 12464 |
| RTECS number | RG0175000 |
| UNII | E1QY3J8W1J |
| UN number | UN3265 |
| Properties | |
| Chemical formula | C8H17Cl |
| Molar mass | 162.72 g/mol |
| Appearance | Colorless liquid |
| Odor | pleasant |
| Density | 0.827 g/mL at 25 °C (lit.) |
| Solubility in water | Insoluble |
| log P | 5.47 |
| Vapor pressure | 0.646 mmHg (at 25 °C) |
| Acidity (pKa) | pKa ≈ 50 |
| Basicity (pKb) | pKb = -3.3 |
| Magnetic susceptibility (χ) | -7.72e-6 cm³/mol |
| Refractive index (nD) | 1.4196 |
| Viscosity | 2.944 mPa·s (25 °C) |
| Dipole moment | 2.03 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 322.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -146.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -5377.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H304, H315, H319, H335, H411 |
| Precautionary statements | P210, P261, P280, P301+P312, P305+P351+P338, P370+P378, P403+P235, P501 |
| NFPA 704 (fire diamond) | Health: 1, Flammability: 2, Instability: 0, Special: |
| Flash point | 72 °C |
| Autoignition temperature | 180 °C |
| Explosive limits | Explosive limits: 0.9–7% |
| Lethal dose or concentration | LD50 (oral, rat): 3,160 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 3,135 mg/kg |
| NIOSH | CN8575000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 1-Chlorooctane: Not established |
| REL (Recommended) | 1 – 10 mg/L |
| Related compounds | |
| Related compounds |
1-Bromooctane
1-Iodooctane 1-Fluorooctane Octanol Octanoic acid |
