S-Camphorsulfonic acid roots back to the intersection of organic chemistry and natural products in the late 1800s. As synthetic chemistry gained a foothold, the search for soluble sulfonic acids found camphor—a familiar terpene from the camphor laurel tree—ripe for exploration. Early researchers spotted that reacting camphor with sulfuric acid under controlled heat unlocked something special—a sulfonated acid, sturdy and adaptable. Both European and Asian chemical circles picked up the method, turning out the first reliable batches long before the modern supply chains of specialty chemicals existed. Within a handful of generations, pharmaceutical and catalysis sectors stamped their approval, using this acid as a chiral auxiliary and resolving agent for transforming racemic bases. Old journals highlight its reliable performance as others came and went, cementing its reputation in both laboratories and industrial plants.
S-Camphorsulfonic acid has always drawn interest for its blend of natural origin and industrial adaptability. Pure samples appear as white crystalline powder or larger clear crystals, holding up well in storage and transport with minimal fuss. Anyone who handles it remembers the characteristic camphoraceous smell, pungent but not unpleasant. Highly soluble in water and most polar organics, it dissolves quickly—a trait that opens the door for countless uses. As a strong organic acid, with a pKa pushing down to about -1.2 in water, it stands shoulder-to-shoulder with other well-known sulfonic acids. Its chiral (R) or (S) forms, depending on the source, mean chemists can nudge molecules in the direction they want during asymmetric syntheses or resolutions.
At the bench, this compound feels solid and dependable. Its melting point hovers near 190°C, a temperature that shrugs off most accidental exposures to mild heat. Above that, decomposition sets in, producing sulfur-based fumes—hence the need for good ventilation. S-Camphorsulfonic acid doesn’t give up its protons easily in nonpolar media, but it’s a beast in water. Density sits between 1.3 to 1.4 g/cm³, giving a familiar heft in the palm. Chemists appreciate its stability in sealed containers and resistance to slow decomposition in daylight, avoiding the headaches that sensitive reagents often deliver.
Manufacturers print labels showing content above 99%, confirming solid-phase purity by HPLC or melting-point checks. Water content lands under 1%. Custom lots can list heavy metal traces, but a typical high-spec batch from a reputable supplier reads as lead-free and negligible in other contaminants. Shipping labels often warn about skin and eye hazard—no surprise for a strong organic acid. Storage instructions push for dry, cool places, with a tight cap, steering clear of open flames and oxidizers. Lab-grade drums often bear a UN3261 code for safety oversight, alerting users and transporters to its corrosive potential.
Industry and academia usually lean on a direct sulfonation process. It starts with natural camphor—either from the laurel tree extraction or terpene isolation. This camphor meets concentrated sulfuric acid, sometimes in the presence of acetic anhydride to tweak conversion. Heating the mix carefully, chemists catch the exothermic curve and keep it steady so the camphor rings don’t shred apart. After holding the reaction, the crude acid crystals out once cooled, and repeated washes in cold acetone kick out oily residues and unreacted camphor. Laborious but reliable, this method still sets the standard, and greener tweaks try to lower sulfuric acid waste or swap in milder sulfonating agents—though most commercial plants stick to the classic playbook.
S-Camphorsulfonic acid often earns its keep as a chiral acid or resolving agent, steering other molecules by forming salts and breaking up racemic mixtures. In organic synthesis, it nudges imines or lactones toward favored stereochemistry when partnered with amines or alcohols. It’s also a strong acid catalyst, racing through acid-catalyzed hydrolyses and esterifications, or bringing order to chaos in rearrangement and addition reactions. Chemists have used its sulfonic acid group as a handle, attaching it onto metal surfaces or into polymer networks, expanding its reach into material science. Downstream, oxidation converts the sulfonic group to sulfuric acid derivatives, or reduction opens up bridges to amine-functionalized materials. Its robust architecture stands up to repeated exposure, making it popular in both one-shot and cyclic reaction systems.
Literature stashes plenty of alternate titles for this acid: S-(+)-Camphorsulfonic acid, CSA, 10-Camphorsulfonic acid, and (1S)-(+)-10-Camphorsulfonic acid—all part of the same catalog. Japanese patents may call it “Kanpurosurufon san,” German chemists prefer “S-Camphorsulfonsäure,” but buyers recognize them all by the same structure and function. For anyone checking chemical databases, cross-searching these variants rounds up the right MSDS, regulatory, and toxicological details.
Anyone working with strong organic acids keeps one eye on the MSDS and the other on the clean-up kit. S-Camphorsulfonic acid falls squarely into the corrosive category, causing burns if splashed on the skin or eyes and irritating airways in dust form. Serious mishaps are rare with modern gear, yet the substance deserves respect. Gloves, goggles, and dust-free hoods prevent most problems. Toxicology studies peg its acute oral and dermal toxicity as low compared to mineral acids, but chronic exposure, especially through inhaled dust, spells trouble over time. Waste handling sticks to local rules—neutralizing spent batches with alkali before sewer disposal whenever regulations permit.
Most chemists hear about S-Camphorsulfonic acid through its work in pharmaceuticals. It makes racemic drugs easier to separate into single enantiomers, pushing purity in medicines. Certain antibiotics, cardiovascular, or CNS drugs appeared on the market years earlier because this reagent sorted out their mirror-image confusion. On the industrial side, its acid power leads to quick, clean reactions in dyes and flavors, shrinking reaction times. Electronic material engineers recently picked it up as a dopant for polyaniline, tailoring the conductivity of polymers for sensors and flexible circuits. Paints, adhesives, and custom polymers in the food-contact sector sometimes lean on its stable, non-volatile acid for crosslinking or chain modification. Innovators in battery technology and thin-film coatings pore over its properties to push product performance without heavy-metals baggage.
Lab notebooks and digital publishers have posted a steady stream of patents and breakthroughs tied to S-Camphorsulfonic acid. Teams refining asymmetric catalysis reach for this acid and its derivatives, creating new routes to chiral amines and amino alcohols. Polymer science labs experiment with it as a built-in acid group, controlling self-assembly in nanostructures. Green chemistry working groups investigate ways to make the sulfonation process friendlier—tackling the waste and energy hit, eyeing alternatives to heavy mineral acids. These research lines all flow toward making the process smarter, the footprint smaller, and the applications fresher.
Toxicologists cast a skeptical eye on anything that blends strong acidity with a biological backbone. Acute exposure data show that S-Camphorsulfonic acid causes irritation at moderate to high doses but doesn’t trigger the broad spectrum of systemic toxicity seen with some modern solvents or acids. Inhalation—a common lab hazard—brings coughing or sore throat, but the compound clears from the system promptly if not misused. Animal studies tracking mutagenicity, teratogenicity, or long-term carcinogenic potential have yet to turn up major red flags, supporting its track record as a low-concern auxiliary when handled right. Still, regulators press for fresh datasets and transparent safety communications as the compound’s production volume edges upward.
S-Camphorsulfonic acid lines up as a persistent favorite for old and new sectors. Pharmaceutical innovation, especially in asymmetric synthesis and solid-form design, keeps pushing its use in resolving agents and salt screening. Polymer development faces a relentless demand for new acids that perform across temperature ranges and meet food- or medical-grade criteria; S-Camphorsulfonic acid shows steady growth prospects because it already checks most boxes. Sustainable chemistry circles look for tweaks in production—less sulfur waste, more renewable camphor sources, less energy drain. Efficient recycling of spent acid and cradle-to-grave data collection could set new operational standards and reassure future buyers. It’s tough to find a catalyst or resolving agent so well documented, with the operational resilience earned from decades of real lab and factory use—backed by ongoing improvements as researchers tie new discoveries to trusted methods.
I remember the buzz in the lab back in grad school whenever someone managed to get their hands on S-camphorsulfonic acid. It’s more than just a tongue-twister for chemists. This stuff lives on chemistry shelves because it brings serious value as an acid catalyst. Look at the way many pharmaceuticals come together—with delicate steps, each needing strong but reliable acids to push the molecules where you want them. S-camphorsulfonic acid steps in to drive those reactions, and it doesn’t just break bad; it helps form bonds in a controlled way, a kind of traffic cop for tricky chemistry.
If you’ve taken a prescription tablet, there’s a good chance some acid catalyst played a hand in making it. S-camphorsulfonic acid helps shape active ingredients in crucial heart drugs, antibiotics, and antivirals. Pharmaceutical companies lean on this acid to create salts of active molecules. Salts often give a drug the right strength, shelf life, or absorption rate in the human body. In some antiretroviral drugs, this acid helps create a salt form that is easier for the body to use, making a difference between an effective treatment and one that passes right through.
Leading universities and industrial chemists reach for S-camphorsulfonic acid in stereoselective synthesis. From my bench experience, working on reactions that need high selectivity isn’t just about luck or brute force. This acid helps control which “hand” a molecule forms. If you want only the “right hand” version of a drug—because that’s what works in the body—S-camphorsulfonic acid can push the reaction in that direction. This saves months of wasted effort and piles of unusable product. Companies like Merck cite this acid in journal articles on new synthetic routes for blockbuster drugs, highlighting how it shapes high-value ingredients in ways you can’t reliably do with weaker or less specific acids.
It’s not all about pharmaceuticals. Dyes, pigments, and certain plastics that show up in everyday objects get their boost from precisely controlled reactions, often using acids like S-camphorsulfonic. Textile and paint manufacturers look for sharp, clean color. By bringing the right acid into the mix, chemists get color stability, depth, and lasting quality. Artists and craftspeople may not realize a crucial acid stands behind the scenes, but I’ve seen plenty of chemical supply lists for art restoration that include it for preparing fine surface treatments and varnishes.
Powerful reagents need careful handling. Chemists know that S-camphorsulfonic acid is potent. It demands respect and attention to safety practices. Laboratories and factories need strong protocols for storage and disposal, and anyone who’s worked with it can share stories of skin burns or worse when precautions slip. Regulatory bodies like OSHA and the EPA watch how companies treat such chemicals, and safety data sheets hammer home the risks. The field keeps evolving, and there’s a growing demand for “greener” catalysts, with lower risks and less environmental impact. New research explores alternatives, but the properties of S-camphorsulfonic acid set a high bar for performance.
I’ve seen research efforts pouring into catalysts that do what S-camphorsulfonic acid does, without the same hazards or waste. In the race for safer, cleaner manufacturing, universities and startups experiment with bio-based or recyclable acids. Funding drives this search, with agencies supporting green chemistry grants. Progress is slow but steady. Industry can speed the shift by supporting early-stage work, sharing real-world data, and adopting cleaner alternatives where they match up. Until then, the power and subtlety of S-camphorsulfonic acid keep it in play for jobs too tough for the easy stuff.
S-Camphorsulfonic acid, known in chemistry circles for its strong, sharply acidic punch, carries the formula C10H16O4S. This formula says plenty in a language every chemist recognizes: the backbone, ten carbons, comes from natural camphor. Toss in a sulfonic acid group, and the camphor molecule turns into a key additive with serious practical value. The full IUPAC name, (1S)-1,7,7-Trimethylbicyclo[2.2.1]heptane-2-sulfonic acid, doesn’t roll off the tongue, but the stuff shows up in labs around the globe because it makes certain reactions snap to attention.
Formulas always look impressive, but context gives them life. I’ve seen S-Camphorsulfonic acid find its groove in the pharmaceutical industry. It’s a trusted acid catalyst for synthesizing chiral drugs. I remember an organic class lab where we tried making a simple sugar derivative. The reaction limped along—until we added a pinch of camphorsulfonic acid. The yield soared, the process sharpened up, and we saw why it gets mentioned in serious synthetic chemistry.
Its structure brings more than strength. That sulfonic group tacks onto camphor, cranking up that solubility in water and making it far more manageable compared to other acids. You end up with a strong acid that’s safer to handle than sulfuric acid, and better suited for delicate reaction settings. This matters in a world where lab safety and workflow bottlenecks slow down research time and again.
Knowing the chemical formula isn’t just trivia. In a manufacturing environment, precision counts—wrong measurements risk millions. Having C10H16O4S signals to a trained eye what kind of weights, concentrations, and interactions to expect. Teams rely on this number for paperwork, safety, and mixing processes. The hazard sheets hanging on the wall mention it. So does the customs paperwork when this acid ships across borders for a new round of drug synthesis in another country.
Working with S-Camphorsulfonic acid brings up some of the classic lab headaches. It’s hygroscopic, meaning it pulls in moisture from the air and turns clumpy if left exposed. I once spent a frustrating hour scraping ruined granules out of a weighing dish. Keeping chemicals dry might sound obvious, but it’s one of those rules everybody breaks once, and never again. The formula hints at this, as those sulfonic groups attract water like magnets.
Storage and handling policies need updating in busy research environments. Training for new lab staff should include not only the procedures but also “why” a chemical like S-Camphorsulfonic acid demands respect. The tight carbon framework and strong acid group present moderate health risks, so full PPE matters. Clear signage, sealed containers, and regular audits help prevent waste and keep teams safe—lessons I learned firsthand during inventory checks after a leaky bottle cost us half a month’s supply.
Teams relying on S-Camphorsulfonic acid do better by investing in tight management systems: digital inventory tracking, humidity controls in storage spaces, and regular reviews of handling rules. Suppliers who offer batch certificates and clear expiration dates stand out. Universities and research labs that share stories about best practices and common mistakes set a tone where everyone feels comfortable being cautious and asking questions rather than guessing about “routine” chemicals.
The formula C10H16O4S serves as a reminder that behind every bottle sits a blend of ingenuity, risk, and small decisions that shape big results in labs and factories everywhere.
S-Camphorsulfonic acid appears on plenty of chemical suppliers’ lists. Chemists use it as a catalyst, especially in organic synthesis and the making of some pharmaceutical ingredients. It comes as a white, crystalline powder and dissolves easily in water and many organic solvents. I’ve worked with it in a couple of university and lab settings, mostly for specialty reactions that need solid acid without the mess of strong mineral acids like sulfuric.
Plenty of folks wonder if S-Camphorsulfonic acid is dangerous. Straight to the point: it’s considered an irritant. If it gets on your skin or eyes, expect reddening, burning, or stinging sensations—about what you’d expect from coming into contact with other strong organic acids. Swallowing it can burn the throat and stomach. Breathing in its dust, and I’ve made that mistake, leaves you coughing and uncomfortable. But the effects are acute, not long-term or carcinogenic, according to available research.
The European Chemicals Agency classifies it as harmful if swallowed and as causing serious eye irritation. No evidence links it to long-term toxicity, cancer, or reproductive harm at the typical levels used in laboratories. Safety Data Sheets from major suppliers echo these findings: avoid direct contact, don’t breathe the powder, and use gloves and goggles—standard lab safety advice. On days I prepped S-Camphorsulfonic acid in undergrad labs, a dust mask made a noticeable difference for comfort and caution—one sneeze could spread it everywhere, making those PPE protocols matter.
Getting rid of S-Camphorsulfonic acid means following procedures for acid waste, not just tossing it down the sink. The substance breaks down easily in water, but dumping it untreated into drains could harm aquatic creatures by shifting water pH. Cleanup involves neutralizing spills with sodium bicarbonate or a similar base, then diluting and disposing of it as the guidance says. Most university labs treat acid residues carefully, and for a good reason—accidents with concentrated acids leave permanent reminders on benches, floors, and people’s hands.
Risks from S-Camphorsulfonic acid shrink when treated with respect. Wearing gloves, safety glasses, and sometimes a dust mask eliminates most exposure hazards. A fume hood or well-ventilated space limits dust inhalation. Training new chemists, especially undergraduates, on the right way to handle these acids lowers the risk of accidental burns or inhalation. I remember a friend forgetting gloves once; the rash told its own story about why a minute of precaution saves hours of discomfort.
Lab supervisors and managers should keep clear signage and up-to-date training for everyone handling acid catalysts. Eye-wash stations and spill kits need to stay stocked and within reach. If smaller-scale users ever hesitate, they should reach for less potent acids or alternative catalysts, depending on the reaction—they sometimes offer what you need without the risks. No need to be alarmist, but taking S-Camphorsulfonic acid seriously keeps work running smoothly and everyone safer.
S-Camphorsulfonic acid isn’t something people tend to toss around carelessly. Every chemist who handles it knows the white, crystalline powder can quickly go south if it’s not stored right. This compound reacts to moisture faster than lunch disappears from the office fridge, and that just creates problems for both purity and lab safety. In my own work setting, an open bottle meant crumbled, yellowed clumps within a week. Best case, it loses punch. Worst case, it eats through paper, produces nasty fumes, or becomes outright hazardous.
Dryness comes before anything else. Even lab veterans forget how easily S-Camphorsulfonic acid seeks out ambient moisture, pulling water from the air until the powder cakes into lumps. Those clumps are more than ugly—moisture can set off hydrolysis, making the acid lose strength. I once saw an entire 500g batch ruined because storage happened in an ordinary storeroom with a leaky air conditioner. Results: warped containers, sticky mess, disposal headaches. Storing it in a tightly capped plastic or glass bottle goes a long way. For extra dry conditions, most folks slide in a silica gel packet near the acid—simple and effective.
Temperature shifts cause trouble too. In summer months, a shelf beside a sunny window may heat up enough to speed up decomposition, which breaks down the compound and can release fumes. Nobody wants to tackle unexpected spills or wonder why assays start drifting. A stable spot at room temperature, far from direct sunlight or heat sources, solves this. Refrigeration isn’t just overkill; it can backfire if condensation forms every time the bottle gets pulled out. Cool, consistent room temperature makes much more sense.
Acids eat metal, and S-Camphorsulfonic acid isn’t any gentler. I once saw a rusty lid wreak havoc, filling the bottle with orange powder and compromising the whole batch. Polyethylene, polypropylene, or quality glass containers stay stable without corroding. Those who use original packaging usually fare best. Whenever repackaging happens, clear labeling with the date and safety warnings matters. GHS labels and up-to-date lot numbers prevent confusion, stop lab accidents, and keep everybody on the same page.
So much of storing hazardous chemicals isn’t about compliance checklists, but just respecting the stuff. Schools and small labs sometimes overlook simple precautions—stashing everything together for convenience. S-Camphorsulfonic acid should go with other acids, isolated from bases, oxidizers, and substances with strong odors. Even a lidded secondary container or storage bin helps confine leaks. Gloves and goggles become routine when measuring or decanting, since the fine powder can irritate skin and eyes fast. I’ve seen sharp young chemists learn that lesson after just one careless swipe—nobody does it again.
No chemical storage talk finishes without mentioning disposal. Old or degraded S-Camphorsulfonic acid doesn’t get tossed in the trash or washed down a drain. Lab protocols dictate hazardous waste collection, following environmental safety standards set by local regulations. Keeping a small spill kit near acid stores has saved more than one mess in my experience. Absorbents, gloves, neutralizers—a little prep spares a lot of regret.
From careful sealing to mindful temperature control, the best storage habits protect both the acid’s reliability and everyone who handles it. A few extra steps make all the difference—both for quality science and safe working conditions.
Anybody who’s worked a day in a chemistry lab probably remembers the first time they got a whiff of S-Camphorsulfonic Acid—or tossed a handful on the balance, feeling its powdery grit crunch under the spatula. This is a compound that doesn’t blend into the background. S-Camphorsulfonic Acid, or CSA, grabs attention for a few reasons. The solid comes out of the jar as bright white crystals. Hold it under the light, and you'll catch a bit of sparkle, like sugar on a windowsill. The crystals may seem innocent, but they give off a strong, biting smell. Most would prefer the jar stay closed.
This isn’t some amorphous, dull mass. CSA tends to form these chunky, irregular grains, giving it a distinctly tactile presence on the bench. Chemists running reactions or prepping samples learn pretty quickly that exposure to air can cause these crystals to soak up moisture from the room. After a few hours, the contents in an open vial turn a little clumpy. This hygroscopic behavior actually matters when you’re weighing it—too much time exposed, and your amounts start to drift from what the balance reports.
Unlike many acids that eat holes through most surfaces, S-Camphorsulfonic Acid shines as a solid acid that won’t vaporize and leave a room filled with choking fumes. The melting point lands around 190°C, which places it up with chemicals that don’t just disappear with a warm day. In practical use, if you’re stuck in an un-airconditioned lab come summer, you can count on those white crystals sticking around, not running off or turning to slime unless water's gotten in.
Solubility makes or breaks a compound in most synthetic settings. CSA hits high marks here, dissolving easily in water, methanol, and a handful of other common solvents. Toss it into cool water, and even with minimal stirring, you’ll see it disappear in short order. This quick solubility lets synthetic chemists turn to CSA as a mild acid in delicate reactions—something that won’t sit around undissolved, slowing reactions or interfering with their reproducibility. I’ve watched bench partners switch away from less cooperative acids after struggling with clumps at the bottom of their flasks.
CSA is famous for being less aggressive than some of its cousins. You don’t see it leaving burns or etched marks across a workspace after a small spill. Still, those highly soluble crystals need respect. Splash some water or sweat and CSA together on your palms, and you’ll feel the sting as it makes quick work of breaking down into strong acid. So gloves are the routine, and working near a sink is wise. Safety data point out its corrosive touch—I'm reminded of times cleaning up after clumsy spills and feeling the tingle as I wiped down a stained bench.
Purity stands out as a practical issue here. These chunky, white CSA crystals don’t hide much, so contamination jumps out during routine use. If moisture creeps in, you’ll see caking, sometimes leading to extra filtration or crystallization steps. Thoughtful storage, sealed jars, and desiccants go a long way to keeping things clean and reliable for the next user. From my own experience, a tightly-sealed jar means you get the same quick, clean solubility batch after batch—which, for many researchers, spells less headache, less wasted material, and fewer unpredictable surprises in their daily routine.
| Names | |
| Preferred IUPAC name | (1S,4R)-1,7,7-trimethylbicyclo[2.2.1]heptan-2-ylsulfonic acid |
| Other names |
Camphorsulfonic acid CSA 10-Camphorsulfonic acid S-(+)-Camphorsulfonic acid S-CSA |
| Pronunciation | /ˈɛs ˈkæm.fər.sʌlˈfɒn.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 5872-08-2 |
| 3D model (JSmol) | `3D model (JSmol)` string for **S-Camphorsulfonic Acid**: ``` C1CC2(C(C1(C)S(=O)(=O)O)CCC2)C ``` *(This is the SMILES string for S-Camphorsulfonic Acid, suitable for input into JSmol or similar 3D molecular viewers.)* |
| Beilstein Reference | 390874 |
| ChEBI | CHEBI:50561 |
| ChEMBL | CHEMBL77977 |
| ChemSpider | 14888 |
| DrugBank | DB11272 |
| ECHA InfoCard | 100.007.209 |
| EC Number | EC 214-946-9 |
| Gmelin Reference | 89155 |
| KEGG | C06367 |
| MeSH | D017628 |
| PubChem CID | 68198 |
| RTECS number | GG3150000 |
| UNII | J9Z523B41B |
| UN number | UN2580 |
| CompTox Dashboard (EPA) | DTXSID7030930 |
| Properties | |
| Chemical formula | C10H16O4S |
| Molar mass | 232.29 g/mol |
| Appearance | White crystalline powder |
| Odor | odorless |
| Density | 1.252 g/cm³ |
| Solubility in water | Very soluble |
| log P | -2.1 |
| Acidity (pKa) | -1.2 |
| Basicity (pKb) | 1.2 |
| Magnetic susceptibility (χ) | -5.46·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.554 |
| Viscosity | Viscous liquid |
| Dipole moment | 5.7636 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 206 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -1650 kJ/mol |
| Hazards | |
| Main hazards | Causes severe skin burns and eye damage. Harmful if swallowed. |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H314, H302 |
| Precautionary statements | Precautionary statements: ``` P261, P280, P301+P312, P305+P351+P338, P337+P313 ``` |
| NFPA 704 (fire diamond) | 3-0-2-Acido |
| Flash point | > 180 °C |
| Autoignition temperature | 400 °C |
| Lethal dose or concentration | LD50 oral rat 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 2000 mg/kg |
| NIOSH | BV8225000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | “1 mg/m³” |
| Related compounds | |
| Related compounds |
Camphoric acid Camphor Camphorsulfonylimine |
