Chemists began exploring sulfonic acids in the early 19th century, chasing new materials for emerging industries. Octanesulfonic acid entered the scene when researchers noticed shorter-chain sulfonic acids proved tough enough for many chemical processes, but lacked certain stability. By adding more carbons, scientists achieved strong detergency balanced with lower volatility. Labs in Germany and the US refined its synthesis during the 1940s, tracking growing interest in specialty surfactants and electrolytes. Decades of work shifted the use of sulfonic acids from bulk industrial formulations to targeted roles in analytic chemistry, and octanesulfonic acid quickly attracted attention from those pushing frontiers in chromatography.
Octanesulfonic acid, known for its straightforward C8 alkyl chain paired with a sulfonic acid group, serves as more than another chemical on the shelf. Chemists count on it for ion pair formation, buffer creation, and as a mobile phase modifier in high-performance liquid chromatography (HPLC). This compound finds its way into research work, pharmaceutical product development, and more advanced industrial processes like surfactant design. Whether it turns up bottled for analytical labs or used in electrochemical setups, scientists count on it for both reliability and specific ionic properties.
The solid form displays as a crystalline powder, white or off-white, sometimes taking in moisture from the air. Its melting point sits high enough to ease storage, but doesn’t challenge standard lab conditions. Odor is faint, but its solubility in water is strong, thanks to that sulfonic head. The carbon chain imparts a modest hydrophobicity; this keeps the compound stable yet responsive during chemical processes. Acid strength remains high, approaching pKa values near -1, which secures its place as a powerful acid among its peers. It resists degradation at room temperature, doesn't oxidize readily, and offers good shelf life with proper handling.
Sources sell standard grades at purity levels exceeding 98%. Labels display warnings to signal skin and eye irritation risks, alongside details on storage: cool, dry conditions with no sunlight. Bottles usually list CAS number 126-58-9, country of origin, and batch serial for quality tracking. Manufacturers supply certificates of analysis, verifying purity by titration and checking for water content. Some users demand trace metal levels below 5 parts per million for use in sensitive analysis. The technical sheets describe granular size range, water solubility, and sometimes offer advice for dissolving or mixing, so chemists don’t waste time during setup.
Industrial labs prepare octanesulfonic acid by sulfonating 1-octene, usually in the presence of sulfur trioxide or chlorosulfonic acid. The process is straightforward yet precise; reaction temperature sits under constant monitoring to keep side products at bay. Workers dilute the crude acid and filter the results for clarity. This batch then gets neutralized and often crystallized from a solution, where quality teams test it for remaining solvents or potential impurities. The method stands as a modern upgrade over earlier, less efficient sulfonation routes: yields improved, product purity grew, and environmental concerns dropped as waste handling improved.
Octanesulfonic acid reacts predictably thanks to that strong sulfonic acid group. It forms salts with alkali metals such as sodium or potassium, often without need for rigorous controls. The resulting salts serve as even more soluble agents, popular for mobile phases in HPLC. Researchers test its reactivity with amines, alcohols, and specialized organic reagents, hoping to tailor surfactant properties or make new industrial additives. Under the right conditions, the alkyl tail resists most chemical attack, giving the acid backbone resilience during modifications. This makes it a key intermediate for newer compounds, especially where controlled hydrophobicity matters.
Besides its common name, products list synonyms: n-octane-1-sulfonic acid, 1-octanesulfonic acid, and frequently, its salt names such as sodium octanesulfonate. Commercial brands sometimes abbreviate to OSA or designate the sodium variant SOS, each depending on the intended market. Databases and chemical catalogs always include the unique CAS number. Some trade names differ slightly, but the structure remains the same across suppliers, since industry standards demand consistent identity for use in regulated analysis and chemical synthesis.
Lab handling routines call for gloves, standard goggles, and care to avoid dust or splashes. SDS documents warn about irritation to the skin, eyes, and, with enough exposure, mucous membranes. Spills mean immediate cleanup with water and soap before anything dries out. Disposal guidelines push for neutralization and collection; nobody wants runoff in waste streams. For bulk storage, facilities vent containers to prevent build-up of acidic vapors. Technicians rely on air extraction when dissolving the powder at larger scale, keeping air clear during weighing and transfer. Any user training involves quick instruction on spill management and first aid for prolonged contact.
Analytical chemistry leans heavily on octanesulfonic acid, especially in HPLC for separating charged molecules, peptides, or even pharmaceuticals where subtle ionic changes alter retention times. Biochemical labs slip it into protein purification schemes or peptide mapping tasks, securing sharper results during quality control. Some manufacturers include it in electrochemical setups, balancing ionic content in fuel cells, pushing for efficiency gains in processes that harness small ionic differences. Water analysis teams apply it in tracking trace contaminants and in complex matrix separations where standard agents fall short. No matter the field, chemists reach for it when they need strong, consistent ion-pairing with a straightforward hydrophobic profile.
Teams keep testing modified alkyl sulfonic acids by adjusting chain length, branching, and swapping out counter ions, hoping to push applications further in analytical separation and green chemistry synthesis. Newer research covers biodegradable forms, exploring ways to minimize environmental impact after use. Scientists aim for tailor-made acid strengths and probe unique solvent compatibility. Ongoing work at the interface of analytical chemistry and material science tries to harness the surfactant action of these molecules in smarter drug delivery and new nanomaterial fabrication. Collaborations across pharmaceutical and environmental research regularly surface, where separating low-level analytes could mean quicker, more accurate diagnostics.
Data show octanesulfonic acid causes mild to moderate irritation with contact; concentrated doses harm cell membranes and trigger inflammation. Researchers test for mutagenicity, reproductive risk, and chronic toxicity, with current evidence suggesting low environmental carryover risk when properly handled. Oral and dermal LD50 studies in animals point to moderate toxicity only at high doses. Aquatic toxicity remains a future focus as waste standards grow tighter, and disposal in closed systems stands as a must for any operation using kilogram quantities. Staff training, material safety reports, and strict storage rules keep the workplace risk profile low, but safety teams still call for routine air monitoring and process checks.
Demand for high-purity separation agents and stable surfactant molecules means octanesulfonic acid isn’t going away any time soon. Analytical chemistry, with its rising standards in pharmaceutical quality control and environmental monitoring, drives continued upgrades in purity and sustainability. Chemists look at greener synthesis methods, aiming for higher yields, less waste, and renewable raw materials. The push for lower toxicity derivatives opens a door for new sulfonic acid variants. Researchers expect smarter molecule design and integration into next-generation chemical frameworks, touching electronics, clean energy, and advanced materials. As the world leans more on precision analysis and sustainable chemistry, octanesulfonic acid and its relatives look set to play a steady, dependable part in this evolution.
In the world of chemical reagents, some names rarely make headlines, but they play a crucial role behind the scenes. Octanesulfonic acid is one of these. If you walk into any lab running high-performance liquid chromatography (HPLC), odds are you’ll spot a bottle of it somewhere on the shelf. Most people outside research circles don’t realize how a single reagent like this can shape what scientists discover and how quickly they can find answers.
HPLC isn’t some academic luxury. Pharmaceutical companies trust it to check if medicines contain what they promise. Water authorities use it to spot trace contaminants. Researchers need their samples to separate cleanly so they can figure out what’s in them. Octanesulfonic acid acts as an ion-pairing agent. That means it sticks to specific molecules—often small, charged ones—and helps shuttle them out of complex mixtures. Suddenly, that mystery compound hiding in a water sample stands out, clear as day.
My time in a pharma lab taught me how crucial reliable separation can be. If your tools aren’t up to the job, the results look muddy, and your effort gets wasted. With the right concentration of octanesulfonic acid in the eluent, sometimes a hard-to-find molecule pops up clearly on the detector for the first time. That’s not just satisfying, it’s essential when a delay could hold up a life-saving drug release.
Any discussion about octanesulfonic acid requires attention to safety. Lung and eye irritation show up quickly if you get careless, and spills eat through gloves in seconds. A strong training culture goes a long way. I learned to treat sulfonic acids with respect, checking compatibility charts before mixing and using extra ventilation. Companies need to stay alert for possible supply chain issues because not just any substitute works safely.
Poor disposal practices raise chemical loads in water systems. Octanesulfonic acid can persist, especially if poured down a drain without treatment. Regulations keep tightening for good reason—persistent chemicals disrupt aquatic life. Responsible labs invest in neutralizing waste, using activated carbon filtration or advanced oxidation when possible. Incentives for greener chemistry keep labs searching for alternatives, but no easy substitute offers the same reliability yet.
The global science community keeps pushing for safer, cleaner chemicals. Some research teams experiment with plant-based surfactants or biodegradable analogs. Change takes time. The trick is high purity: small impurities often spoil results. Until new options catch up, strict protocols for handling and disposal make a difference. In my experience, even small tweaks in concentration or pH during method development can lower the amount of octanesulfonic acid needed, reducing both risks and costs.
People sometimes overlook the infrastructure supporting advances in diagnostics, drug discovery, and water quality. Octanesulfonic acid illustrates how the details matter as much as the headline stories. A reagent like this isn’t flashy, but it drives reliability, accuracy, and accountability in data generation. That matters not just for lab techs, but for anyone relying on science for safe medicines, clean water, and clear answers.
Octanesulfonic acid lands in a range of scientific and industrial applications. You’ll find it in analytical labs, and it ends up as a partner in ion-pairing for liquid chromatography. I’ve spent plenty of hours in a chemistry lab, and it’s clear—no one grabs the bottle of octanesulfonic acid without gloves and goggles. Its strong, sharp smell hits first and warns of its bite, but the real danger goes deeper.
Direct contact leaves serious burns. I’ve seen a careless moment end with red, blistered skin that takes weeks to heal. Contact with eyes has even harsher results: permanent damage can follow, and there’s pain and panic that rush to the surface.
Breathing in vapors isn’t just uncomfortable. Irritation in your throat and lungs comes on fast, and in a poorly ventilated room, the risk jumps. Prolonged breathing can trigger chronic issues—a fact that’s underlined by material safety data sheets and echoed by workplace protocols.
Swallowing even a small amount brings immediate illness. Nausea, abdominal pain, chemical burns inside the digestive tract—these symptoms need real medical attention. I remember a safety briefing where someone brought up how fast things can turn severe in a mistaken sip or splash.
Repeated exposure becomes a concern for lab workers. Skin and airway irritation don’t ease up because the body builds up tolerance—the effects stack up, slow but steady. It reflects the kind of slow burn that often slips past people who treat any acid as “just another chemical.”
Many people overlook what happens after the experiment ends. Octanesulfonic acid doesn’t blend harmlessly into waste water. It rolls downstream, affecting aquatic life. Sulfonic acids, by design, stick around instead of breaking down quickly. Studies out of Europe and North America have highlighted persistent downstream contamination and its impact on sensitive ecosystems. It’s not unique to this compound, yet every bottle poured down a drain counts.
Every responsible laboratory puts clear rules in place. Storage in corrosion-resistant containers, routine checks on ventilation, and easy access to emergency showers all help. Training matters as much as written warnings—learned this early on during internships where mistakes were shared as cautionary tales.
Choosing alternatives for certain processes helps reduce unnecessary exposure. Research into greener solvents and reagents offers hope, but a shift takes time and resources. In places where transition isn’t practical, focus rests on better engineering controls, thorough training, and a culture of respect for the risks.
Proper disposal stands as a non-negotiable responsibility. Neutralization is possible, but not something to attempt without knowledge—experts need to sign off to protect both workers and the environment. Regulations give important guidelines, but industry needs to keep pace and anticipate future risks.
Stories from the lab remind us: Familiar chemicals, handled daily, can leave a deep mark if underestimated. Octanesulfonic acid isn’t the most notorious substance out there, but its hazards should never fade into the background. Vigilance, ongoing training, safe alternatives, and environmental stewardship become more than checklists—they keep people and ecosystems safe for the long haul.
Octanesulfonic acid brings a mix of benefits and challenges for anyone dealing with laboratory chemicals. We’re talking about a strong acid, corrosive to skin and eyes, with enough punch to cause burns and respiratory problems if it escapes from a poorly capped container. Nobody likes to discover a bottle leaking fumes in the back of a storage cabinet. Public health agencies, such as OSHA and the CDC, urge extra caution with acids of this nature. Even homegrown labs have seen disasters from a loose lid or a misread label. In my academic days, a rushed cleanup almost ended with a ruined shelf and a ruined week.
Temperature control plays a bigger role than most realize. At room temperature, octanesulfonic acid won’t just evaporate away, but any heating or direct sunlight hastens decomposition, which creates dangerous byproducts, not to mention risk of pressure buildup inside containers. In my own experience, hot summer days inside a poorly ventilated supply closet spelled trouble. The safest bet—always keep it in a cool, shaded area away from direct sunlight and sources of heat. Industrial safety experts agree: lower temperatures mean less vapor and less risk of accidental exposure.
A lot of spills come down to bad containers. Polyethylene bottles or glass containers with acid-resistant lids offer the best option here. Metal lids or even regular plastic containers can corrode, crack, or react over time, which leads to leaks. More than once, I’ve seen labs cut corners with reused bottles only to regret it once fumes or a leak develop. Most reputable chemical suppliers ship their products in containers that can handle the job—changing this setup increases your risk unnecessarily. So, stick with what works: tight-sealing, acid-compatible bottles, with clear, permanent labels that don’t rub away after a week.
Acids never play well with bases, oxidizers, or organics. Get them together in the wrong workspace, and you can end up with dangerous reactions, fires, or toxic gases. I remember one incident where storing acids too close to a bleach solution ended with a quick evacuation. Shelve octanesulfonic acid away from incompatible chemicals—ideally, use a separate, acid-resistant cabinet. OSHA and chemical hygiene plans spell out these segregation rules for a good reason: a tiny error leads to a big mess.
Breathing in acid vapors isn’t just uncomfortable—it’s dangerous over time. Always pick a storage spot with good airflow, never stuff acid in a cramped or poorly ventilated corner. Industrial hygiene guidelines push for local exhaust ventilation in storage areas where volatile acids are kept. A good friend of mine who once ignored this advice spent a week with a sore chest after cleaning up a fume-heavy closet.
Any lab worth its salt keeps neutralizing agents—such as sodium bicarbonate—within arm’s reach. Quick action can contain small spills, but cleanup crews need gloves, goggles, and access to running water before approaching a mess. Never underestimate splash potential—more than once, handling a supposedly dry bottle has led to a stinging surprise. Proper protocols matter, from quick cleanups to reporting every incident, no matter how small.
Even the best storage plan fails without careful people. Whether it’s a university lab, a small business, or a multinational plant, regular safety training makes the difference. Walking through the right process for acid storage once a year beats any sign or label for preventing accidents. In my own experience, that single refresher catches details that manuals overlook, keeping both the staff and the supplies out of trouble.
Octanesulfonic acid demands respect—keep it cool, tightly sealed, separated from incompatible substances, and within a well-ventilated space. Safety isn’t about ticking boxes; it’s about attention to the day-to-day routines that keep dangerous chemicals from becoming today’s headline.
Chemistry sometimes feels distant, but for anyone working in a lab or managing quality in water treatment, tiny details pack a punch. Octanesulfonic acid doesn’t get paraded in headlines, yet workers rely on it in HPLC analysis to help pinpoint traces of contaminants and pharmaceuticals faster than tap water runs from a faucet. Its molecular formula, C8H18O3S, isn’t just a string of letters and numbers — it lays out the foundation for its structure and how it behaves in the real world.
Every atom in the formula tells a story. Take the eight carbons: they build the “backbone” of the molecule, just like octane in gasoline. The eighteen hydrogens hang off that chain, keeping it stable. The three oxygens and one sulfur make up the sulfonic acid portion, which isn’t just tagging along — this group matters in all the ways the compound dissolves, reacts with other chemicals, or moves through a chromatography column. The sulfonic acid group is what flips octane from an oily hydrocarbon chain to a water-loving, acid-acting helper.
Labs trust the structure for a good reason. In HPLC, scientists use octanesulfonic acid as an “ion-pairing” agent. That means it grabs onto certain molecules in a water sample, helping them show up in a test so analysts can see if a pollutant is hanging around at a dangerous level. Being clear about the formula prevents errors when chemists mix solutions, and it lets researchers around the world speak the same “language,” boosting accuracy in studies and regulatory work.
A single digit in a molecular formula can mean the difference between an effective cleaning agent and a dangerous irritant. The confirmed formula of octanesulfonic acid (C8H18O3S) keeps manufacturing and lab work reliable. Hospitality, hospitals, and municipal water labs lean on chemical supplies with the right formula, knowing a mismatch can end in equipment breakdowns or missed threats to health.
This acid’s production comes with responsibilities. Like all strong acids, skin and eye contact should get avoided, and plenty of ventilation cuts down any breathing risks. Chemical suppliers and buyers watch for validated formulas through safety data sheets (SDS), double-checking that what’s on the label matches the science. Mistakes can mean failed experiments, wasted money, or even neighborhood evacuations in the worst cases.
Strength in chemical safety grows from facts. Global standards like ISO and the United States Pharmacopeia link a chemical’s formula with its identity. Quality audits follow the same trail, starting from C8H18O3S and tracing it through the supply line.
Access to accurate and timely information remains crucial. Universities, companies, and regulators could support collective platforms where chemists and health experts share updates, alerting others to purity problems or new research on health impacts. Open-access chemical databases have become daily tools for both students and experts; they thrive on input from real-world users who spot unexpected results.
Trust in any chemical rests on knowing its exact structure. For octanesulfonic acid, a small label — C8H18O3S — opens the gate to deeper reliability everywhere from testing city water to keeping drug production in step with safety standards.
I’ve worked in research labs that juggle a mix of benign and hazardous chemicals every day. Octanesulfonic acid always landed on the “extra caution” shelf, far from the general-use acids and solvents. Its surfactant qualities make it valuable, sure, but they also mean contact hazards and environmental issues pile on fast. Folks who spend their days in chemistry or pharmaceuticals know the irritation it can cause to skin, eyes, and lungs. Direct exposure tends to bite back immediately. A single splash or whiff leaves no illusion about the need for real protective gear.
Leaving anything like octanesulfonic acid lying around as regular lab waste breaks both protocol and common sense. Regulations clamp down hard because water systems can only handle so much. The Environmental Protection Agency and Occupational Safety and Health Administration list this compound as hazardous. Local authorities stack on their own restrictions. Pouring it down the sink not only threatens aquatic life due to its corrosive and bioactive properties, but also lands institutions hefty fines or worse.
Labs that treat safety gear like a suggestion rather than a rule soon learn the fast way. Typical disposable gloves don’t last long against potent acids, and standard lab coats do little without face shields and proper ventilation. Splash goggles and chemical-resistant gloves prove necessary, not overkill. Some engineers switch to fume hoods for every procedure, cutting down on accidental inhalation or spillage.
In my labs, we had a cardinal rule: label all containers, even for short-term storage. Drifting away from this habit brings confusion and risk, especially when waste bins start to fill. Firms contract with licensed waste management companies for proper off-site disposal. Neutralizing octanesulfonic acid at the bench can turn into a chemical lottery. Unexpected reactions aren’t worth the gamble, as neutralization often releases heat or additional fumes. Commercial waste handlers use tested protocols that avoid those risks. Tracking disposal keeps incidents traceable, which auditors appreciate almost as much as the fire marshal.
No single policy covers every situation, and relying on posters or online reminders never matches genuine team culture. Training makes a difference, especially for new hires or students learning lab routines. I’ve seen peer checks catch mistakes that written protocols missed. Shared vigilance—knowing that you’re responsible for your own safety and your coworkers’—fills the gaps formal rules leave open. That spirit keeps close calls and accidents rare.
Ordering only what you’ll use limits excess waste. Keeping chemical stocks low means less to store, less to toss, and smaller accidents if containers fall off shelves. Using dedicated waste containers for acid waste and labeling each by main hazard speeds up emergency response. Partnerships with environmental specialists or hazardous waste companies ensure pickups happen on schedule, leaving less room for risky improvisation.
Looking at octanesulfonic acid through a practical lens, handling and disposal bring real responsibility. Experience in the lab reminds us: danger comes less from the chemical itself, more from lapses in attention or shortcuts in process. Smart habits, protective gear, and working relationships with professionals keep problems small and manageable.
| Names | |
| Preferred IUPAC name | 1-sulfooctane |
| Other names |
1-Octanesulfonic acid n-Octanesulfonic acid Perlatolic acid |
| Pronunciation | /ɒkˈteɪn.sʌlˌfɒn.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 5324-84-5 |
| Beilstein Reference | 1710228 |
| ChEBI | CHEBI:37936 |
| ChEMBL | CHEMBL334089 |
| ChemSpider | 162109 |
| DrugBank | DB03766 |
| ECHA InfoCard | 100.016.348 |
| EC Number | EC 211-573-2 |
| Gmelin Reference | 6066 |
| KEGG | C01795 |
| MeSH | D017370 |
| PubChem CID | 12038 |
| RTECS number | TC3150000 |
| UNII | U1F8H0A1T7 |
| UN number | UN2585 |
| Properties | |
| Chemical formula | C8H18O3S |
| Molar mass | 210.29 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Odorless |
| Density | 1.18 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -0.38 |
| Vapor pressure | 0.02 mmHg (20°C) |
| Acidity (pKa) | -2.8 |
| Basicity (pKb) | 12.6 |
| Magnetic susceptibility (χ) | -6.2e-6 cm³/mol |
| Refractive index (nD) | 1.4300 |
| Viscosity | 13 cP (25 °C) |
| Dipole moment | 0.931 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 234 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1012.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -4761.7 kJ/mol |
| Pharmacology | |
| ATC code | V03AB37 |
| Hazards | |
| Main hazards | Corrosive; causes severe skin burns and eye damage; harmful if swallowed; may cause respiratory irritation. |
| GHS labelling | GHS02, GHS05 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H314: Causes severe skin burns and eye damage. |
| Precautionary statements | P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P312, P321, P363, P405, P501 |
| NFPA 704 (fire diamond) | 3-0-2-Acid |
| Flash point | > 210 °C |
| Autoignition temperature | 250°C |
| Lethal dose or concentration | LD50 oral rat 670 mg/kg |
| LD50 (median dose) | LD50 (median dose) of Octanesulfonic Acid: 2000 mg/kg (rat, oral) |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1% |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Methanesulfonic acid Ethanesulfonic acid 1-Butanesulfonic acid Hexanesulfonic acid Decanesulfonic acid |
