Decades ago, camphorsulfonic acid found more than a curious spot on the lab shelf. Chemical industries eyed it for its strength as an acid and its solid, crystalline nature. The material told a story of a shift in organic synthesis, especially as researchers in the late 20th century chased sharper tools for enantioselective processes and better protection schemes. Over time, chemists started to lean on this sulfonic acid because it handled tough jobs with consistency. Instead of dealing with old-fashioned acids that played havoc with sensitive molecules, folks could turn to camphorsulfonic acid and see improved outcomes in pharmaceuticals, pigments, and a host of flavor compounds. Labs saw demand swell, pushing companies to refine how they made and handled it, and spurring decades of technical work to make purer, more predictable batches. The compound helped mark a change, making certain organic transformations more accessible and safer to achieve.
Camphorsulfonic Acid Dl 10 grabs attention first as a solid acid, packed into off-white crystals, sometimes powdery, sometimes a little chunkier. Its melting point lands comfortably above room temperature, so manufacturers can ship and stock it with low risk of accidental liquefaction. In the world of synthetic acids, it draws utility not from sheer brute force, but because it combines strength with selectivity, and it's known for handling moisture without turning to sludge. Companies sell it under different names, and it shows up in a raft of process aids, synthesis routes, and as a standout acid catalyst where more hazardous alternatives would risk damaging gear—or operators.
Pick up a sample, and you'll see crystals with slight hygroscopic leanings—they’ll pull in water over time from the air, which gives a clue to storing them somewhere dry. With a molecular weight that doesn’t shock the scales, camphorsulfonic acid dissolves easily in water and polar solvents. The structure tells a lot about its reliability: a bicyclic camphor backbone offers rigidity, while a strong sulfonic group brings acidity akin to mineral acids. The acid strength and unique physical profile suit it for fine chemistry, as well as handling in busy lab environments where controlling exothermic reactions and impurities becomes a daily challenge.
Retail and industrial labels print out details that go beyond just a product code and batch number. Detailed sheets note purity percentage, melting point, solubility, and any regulatory notations tied to international transport. Some suppliers fold in HPLC and GC-MS trace impurity data as buyers want certainty, especially for pharmaceutical intermediates. The specifications track consistency, as variances will knock off reaction yields or color the final compound with rogue byproducts. To this day, the tightest specs come from those targeting active pharmaceutical ingredient manufacture, because no one wants unqualified batches making their way into health products.
In practice, camphorsulfonic acid comes from reacting camphor with sulfonating agents, typically fuming sulfuric acid, under careful control. The chemist guides the process through temperature and acid concentration, then crystalizes and purifies the material by repeated washing and solvent manipulation. Over the years, labs found that gentler methods increase purity and cut down on the stench and fumes that strong acids and oxidizers produce. Environmental experts joined the conversation in the 21st century, nudging newcomers toward greener sulfonation chemistries. Even today, most manufacturers keep a close eye on byproducts and the careful neutralization of any waste streams.
Synthetic chemists value camphorsulfonic acid for specific transformations as much as for any broad-spectrum acidity. It donates protons with gusto, so it speeds up acetalizations, hydrolyses, and esterifications where precision matters. The stereochemistry of the camphor group helps coax asymmetric reactions for certain specialty compounds, making it a favorite chiral acid catalyst in research labs. Turns out, this means that the acid doesn’t just hit and run—its structure influences not only the rate but also the 3D shape of product molecules. Sometimes, specialist groups will modify it further to produce sulfonate salts, tweaking the backbone for studies in organocatalysis or for custom ion-exchange properties.
Walk down the specialty aisle of a chemical supplier and you’ll see camphorsulfonic acid listed under several names. Chemists from different regions or generations will swap between “DL-10-camphorsulfonic acid,” “2-camphorsulfonic acid,” or the official IUPAC handle. For some, “CSA” does the trick, and in European catalogues, it can even show up as “camphoric acid sulfonate.” These labels appear not just for branding, but because each variant implies slight differences in the mixture’s stereochemistry or purification route, and in regulated environments, detail on the label helps avoid costly missteps.
Handling this acid doesn’t bring the terror of hydrofluoric acid or the smoke of phosphoric acid. Still, folks working with it wear gloves, goggles, and stay aware of its dustiness. Storage protocols call for sealed containers away from strong bases or oxidizers, since even a solid acid like this can kick-start reactions if spilled. Industrial users keep an eye on air filtrations, preventing dust buildup. Suppliers look toward the GHS and European REACH guidelines for labeling, and every shipment moves with an updated safety data sheet in tow. Spills, when they happen, don’t bring panic—water and a bit of common sense finish the cleanup. The reassuring part comes from decades where careful monitoring turned up few long-term health worries, giving technicians more confidence to use it routinely.
Put this acid to work and the reach spans from classic lab benches to massive reactors. It reacts in the synthesis of beta-lactam antibiotics—helping shape the structures that end up saving lives in operating rooms. Outside the pharmaceutical world, it finds itself lining up in dyestuff synthesis, offering color stability and consistency batch after batch. In electronic chemicals manufacturing, it brings sharp definition to certain etching processes. For anyone who values precision in stereochemistry or patterning, camphorsulfonic acid gives them a certain edge. Even the perfume industry leans on it, coaxing out notes and esters that would falter without a strong acid touch.
Academic groups gravitate toward camphorsulfonic acid as a test case for catalyst design and enantioselective transformations. It lands as a reference point in hundreds of studies, providing a bridge from chiral natural product chemistry to medicinal synthesis labs. Patents roll out yearly with tweaks—sometimes a new solvent system, sometimes as part of a process to build better API intermediates. Recent curiosity has focused on how to recycle spent acid and close the loop for industrial green chemistry. Research into polymer-bound acid versions kicked off, allowing easier separation and reuse. As innovation in pharmaceuticals ratchets up, so does the attention researchers give this old, reliable acid.
Toxicologists spent years watching for systemic effects, chronic exposure symptoms, and possible cumulative damage from routine contact. Most findings suggest low acute and chronic risks—so long as workers avoid eating, drinking, or breathing dust clouds at work. Ingestion brings possible gastric upset, as anyone who’s worked around powerful acids would expect. Eye and skin exposure need treatment, but reports of long-term organ damage remain rare. That said, regulators keep toxicology data up to date, especially as industries use higher tonnages each year. Animal studies gave some reassurance early on, with rapid clearance in controlled dosing. Each update in the literature solidifies a picture of a substance to respect, but one that doesn't demand extraordinary caution for typical lab procedures.
The coming years look busy for camphorsulfonic acid, but in more specialized arenas than in decades past. Drug discovery projects hunger for chiral catalysts, and CSA keeps showing up as the acid of choice for fine-tuning new molecular frameworks. As green chemistry standards rise, manufacturers and research teams look harder for ways to recover and recycle acid, make use of water-based systems, and reduce dependence on hazardous reagents during preparation. Companies that figure out how to recover and reprocess the acid for closed-loop systems will find themselves ahead in regulatory and cost battles. On the university front, new hybrid catalysts inspired by camphorsulfonic acid are pushing into organometallic and peptide chemistry, showing that a classic compound still has lessons left to teach.
Camphorsulfonic Acid Dl 10 might not be a name that pops up in everyday conversation. Despite its obscure profile, it plays a solid role in the world of chemistry and industry. Anyone working in pharmaceutical labs or engaged with advanced material research probably knows this compound well. I’ve seen firsthand, through collaborations with chemical engineers and researchers, just how crucial such chemicals become when developing drugs or fine-tuning specialty products.
One of the major points about Camphorsulfonic Acid Dl 10: drug manufacturing. It’s not a medicine by itself, but serves as an intermediate, helping chemists build complex molecules. The compound often assists in forming salts of basic pharmaceutical ingredients, which can improve how drugs dissolve and get absorbed in the body. I spoke with a pharmacist who explained that poor solubility is a real headache for drug developers. Camphorsulfonic Acid can make formulations more reliable and effective, giving patients a better shot at successful treatment. The market reflects this go-between role. Pharma manufacturers lean on it for synthesizing antibiotics, heart medications, and antivirals. According to reports from pharmaceutical industry analysts, using compounds like Camphorsulfonic Acid leads to greater consistency during production, minimizing waste and costs. That’s vital for companies running at tight margins.
This compound also shows up in other labs—especially organic chemistry research. Scientists use it as a catalyst and acidifier in reactions that demand strong, stable acids. Its unique properties often cause reactions to proceed faster, or produce cleaner results with less fuss. One common example is during the synthesis of specialty plastics or advanced polymers. During my time consulting with a materials science team, I saw how careful selection of acids like Camphorsulfonic Acid can define the end-product's performance.
Chemicals that play such an important role deserve respect. Like many potent acids, Camphorsulfonic Acid Dl 10 needs proper handling. Safety data shows that direct exposure causes irritation and, in some cases, long-term health effects. Workers need gloves, goggles, and well-ventilated spaces. In my own lab days, protocols for acids like this came before any experiment started. The chemical industry takes things seriously, abiding by safety rules from regulatory bodies like OSHA and the EPA. Compliance means having proper documentation, storage, and disposal systems in place. Companies that cut corners face fines—and, more importantly, put workers and communities at risk.
The future brings tighter scrutiny as new regulations emerge. There’s ongoing demand for greener alternatives that reduce environmental impact. Researchers are looking at designing similar compounds from renewable sources, or engineering processes that rely less on aggressive chemicals. Substitution doesn’t always come easy but pushing for less hazardous methods pays off. Sharing best safety practices and updating training can prevent workplace injuries. Industry dialogue with regulatory agencies helps everyone stay up to date on risks and solutions.
Camphorsulfonic Acid Dl 10 rarely lands in the spotlight, yet it shapes everything from pills and medical devices to specialty materials. By digging into its uses and safety practices, we see just how much invisible chemistry supports daily life, and how responsible handling safeguards those involved.
Anyone working in chemistry or pharmaceuticals bumps into a wide range of reagents, some straightforward, some a little trickier. Camphorsulfonic Acid DL 10 sits in that “tricky but important” category. Its chemical formula is C10H16O4S, and the recognized CAS number is 5872-08-2. This combination—a sulfonic acid derived from camphor—packs a punch because it fuses the unique properties of both organic and acidic chemistry in one solid powder.
Camphorsulfonic acid doesn’t turn up in everyday conversation, but anyone tinkering in a synthetic lab knows its real-world usefulness. This acid gets called up for its strength and its ability to dissolve in both water and many organic solvents. Small molecules that do heavy lifting—like this one—often separate success and wasted effort. Peptide synthesis, chiral resolutions, and catalyst preparations all benefit from this specialized acid’s structure. There is an entire legion of researchers who have avoided long, complicated columns simply by reaching for this camphor-based acid.
From the pharmaceutical sector to materials science, Camphorsulfonic Acid DL 10 helps build complexity and purity in new compounds. Its chiral nature means it plays a role not just as a reactant but sometimes as a building block, helping scientists steer reactions in just the right direction. I remember laboring through trying to isolate clean intermediates until a senior chemist handed me a sample of this acid. Suddenly, reactions that had been sluggish zipped along. Sometimes, the right tool is the difference between wrapping up a synthesis by dinner or working through the night.
The risks with chemicals like camphorsulfonic acid aren’t theoretical. This compound requires respect—eye protection, gloves, good ventilation are non-negotiable. Anyone ignoring these basics remembers fast, as the acid’s strength isn’t only an asset in a flask. Workers need clear training, and facilities need robust protocols for spills, storage, and emergency response. I’ve seen lax attention lead to accidents, each one preventable with better habits and clear procedures.
Despite its value, there’s always room to do better. Companies sourcing camphorsulfonic acid should ask for transparency on purity reports and supply chain documentation. Counterfeit or misidentified chemicals waste time and, worse, risk big health and safety issues. Purchasing managers—whether in academia or industry—push suppliers for certificates of analysis and lot records. When researchers can trust what’s in the jar, progress speeds up and hazards drop.
Environmental concerns follow closely behind. Smart labs plan for responsible waste collection and push for greener alternatives where possible. Camphorsulfonic acid can’t always be replaced, especially where its unique chiral properties shine, but using only what’s needed and disposing of it properly shows care for more than just the results at the workbench.
Understanding and respecting chemicals like Camphorsulfonic Acid DL 10 makes a tangible difference to success and safety. With the correct chemical formula (C10H16O4S) and CAS number (5872-08-2), users can search properly, order what’s needed, and maintain safe, efficient labs that drive discovery rather than risk or waste.
Camphorsulfonic Acid Dl 10 gets used plenty in synthesis labs and sometimes even in pharmaceutical research. The white, crystalline powder might look harmless, but anyone who's spent time in a chemical prep room knows looks don't tell the whole story. This acid is strong, and contact with skin or eyes will burn. Inhaling the dust can irritate airways, and long-term exposure carries the risk of damaging mucous membranes. A little slip while weighing or mixing goes from minor nuisance to chemical burn in seconds.
I once handled a batch of this acid during a bench project and learned quickly how sharply it stings a small cut or unprotected wrist. This compound pulls in moisture fast, so it clings to skin and spreads even after contact. The safety data says eye exposure risks corneal injuries, and extended skin contact causes redness, pain, and even severe burns. I’ve seen lab mates develop rashes after skipping gloves—there’s nothing overblown about those hazard signs. Some reports note this acid can release toxic fumes if heated or accidentally mixed with the wrong reagents, turning a routine experiment into a frantic cleanup.
Solid routines matter most. Always work with gloves that resist acids—nitrile and Neoprene do well—and change them if any powder lands on the cuff. Goggles with side shields help prevent splashes and dust from reaching the eyes. A lab coat with snug sleeves stops splatter from getting under protective gear. I keep a fume hood open, even for small quantities, since good ventilation and local exhaust protect against dust and vapor that can otherwise travel into breathing zones.
Spills happen fast, especially while weighing fine powders. Practice keeps those events minor. For cleanup, grab a spill mat and a scoop or spatula, never your hands. Damp disposable towels pick up leftover traces and avoid stirring up more dust. Keep neutralizing solutions ready—baking soda for small spills or a commercial acid neutralizer. All contaminated paper or gloves go straight into a sealed chemical waste bag to avoid accidental contact down the line.
Safety data from reputable chemical suppliers warn that camphorsulfonic acid exposure risks serious eye and skin injuries and long-term respiratory harm. The Occupational Safety and Health Administration states that acids of this strength call for chemical splash goggles, impervious gloves, and clear labeling at every storage or use point. The CDC notes that acids with a high capacity to damage tissues require speedy first-aid: immediate flushing with water for fifteen minutes after splash exposure, and medical evaluation for anything beyond minor irritation.
Training makes a big difference. Short, clear safety instructions before every new batch or process—especially for students and new techs—can prevent injury. Replacing open bench work with closed systems or powder-dispensing enclosures reduces exposure for everyone. Posting laminated safety instructions, with quick access to eyewash stations and showers nearby, helps embed good habits and readiness.
Storing camphorsulfonic acid away from bases and oxidizers, in well-labeled containers with tight-fitting lids, stops accidental mix-ups that could start hazardous reactions. For those in charge of workplace safety, routine spot-checks and encouragement to report near-misses support a culture that values safety over speed.
No shortcut beats plain familiarity with the risks and honest respect for lab hazards. Good safety habits, protective gear, and clear emergency procedures make handling camphorsulfonic acid about as safe as possible, keeping avoidable injuries out of the picture.
Camphorsulfonic Acid Dl 10 carries quite a reputation in labs and manufacturing plants. Purity does not just mean a cleaner ingredient; it often decides the difference between smooth reactions and headaches down the line. Researchers and chemists usually expect this substance to hit purity levels around 98% or more. Vendors tend to push for this number because traces of unreacted raw materials, water, or unidentified by-products can throw off results or damage equipment.
I remember watching an industrial chemist in a pharma plant rant for nearly five minutes after a batch went wrong due to lower-purity material. That small percentage gap can cause expensive delays. Consider: even if the chemical’s shelf life looks long on paper, unseen impurities break down reactions or corrode expensive glassware. Manufacturers who guarantee high purity often rely on advanced recrystallization, distillation, and repeated filtration. Acid with true 98% purity gives peace of mind for both researchers and plant operators since purity is not just a marketing claim, but a measure of consistent results and reduced troubleshooting in real-world production.
Some folks believe stuffing every chemical into a generic locked cabinet gets the job done. Experience says otherwise. Camphorsulfonic Acid absorbs water from the air. Over a few weeks, a container with a loose or ill-fitting cap can suck up moisture and clump, changing both concentration and reactivity. In one lab, I saw technicians pour out powder that had fused into a strange, solid block after two months in an open room — a classic mistake when someone skipped reading the safety data sheet.
Best practice calls for airtight, non-reactive containers. Polyethylene bottles or heavy glass with Teflon-lined caps stop both leaks and accidental air exposure. I learned from a chemical supplier that keeping the acid in a cool, dry room — think 15-25°C — pretty much guarantees lasting stability. Avoid stacking pulped cardboard boxes or storing anything acidic near metals or oxidizers. Small details like labeling containers with open dates and adding silica gel when shipping during humid months prevent expensive loss. Anyone handling chemicals in bulk knows that spoilage from exposure adds up over time. Lab audits reveal that half-open or poorly labeled chemicals wind up wasted more often than people admit, creating safety headaches and driving up costs.
Over the years, I’ve noticed that groups who take extra care with purity testing and airtight storage see fewer accidents and more reliable product output. Camphorsulfonic Acid Dl 10 rarely causes trouble in a controlled environment, but slip-ups come from small, preventable lapses. Safety data sheets highlight that moisture reacts with the acid, sometimes releasing fumes or creating a slipping hazard. Training teams to recognize the telltale signs — stickiness around the cap, discolored powder, strange smells — keeps people and product safe. Some facilities go as far as using digital sensors monitoring humidity inside chemical storage rooms. Simple habits like cleaning spills quickly, sealing containers right after use, and double-checking labels make a bigger impact than any fancy equipment.
High purity and careful storage turn what could be a risky, unstable supply into a reliable tool. For producers and laboratories, sticking with suppliers who pride themselves on transparency and proper handling pays off, not only for smooth science but for the people behind the glassware. Newcomers might overlook these practices, but those with experience know these details drive results and keep everyone safe on the job.
Handling camphorsulfonic acid, especially the DL 10 version, brings back memories of troubleshooting in a university lab. The material comes as a white crystalline powder with a strong, almost medicinal smell. People usually turn to it for asymmetric synthesis or as a resolving agent; its acids groups give it unique solubility characteristics.
My own benchwork taught that camphorsulfonic acid dissolves smoothly in water and alcohols like methanol and ethanol. Water at room temperature works great for most needs, as the acid is quite soluble. If someone uses a polar organic solvent, methanol gets the job done even in a cold lab. I’ve tried acetone and isopropanol; both will do, but expect slower dissolution as the temperature drops.
Protect yourself. Gloves and eye protection reduce risks. The powder stings if it gets on the skin or eyes.
Set up clean glassware. For a typical 1 M solution, weigh out the desired amount with a dry, accurate balance. Say you want 100 mL of 1 M solution — measure 23.2 grams and transfer it to a beaker or flask.
Start with about 70 mL of your chosen solvent. Add the acid gently, stirring with a glass rod or a magnetic stirrer. In my experience, camphorsulfonic acid dissolves faster in water. Sometimes you’ll notice a brief exothermic reaction—a little warmth in the flask. That’s normal and usually nothing to worry about if quantities stay small.
Keep mixing until everything disappears. Top up the flask to the 100 mL mark once everything dissolves. Check the solution for cloudiness or undissolved solids. If something lingers, heating the mixture in a water bath at 30–40°C encourages solubility without damaging the acid.
Every chemist hits a roadblock. On rare occasions, camphorsulfonic acid refuses to dissolve completely, especially at higher concentrations or in less polar solvents. Acidic groups attract water, so switching to a more polar solvent or gentle heating typically solves the problem. Filtration through a medium-porosity filter removes stubborn particles. My go-to move: warm, patient stirring over fifteen minutes — usually does the trick.
Reliable solution preparation sets the stage for precision in downstream chemistry. If you only half-dissolve your acid, you risk throwing off your entire reaction. It’s not just theoretical: faulty solutions delay work, waste costly reagents, and force grateful reliance on the lab manager for another order.
Camphorsulfonic acid solutions can degrade if left exposed. Always store finished solutions in tightly sealed, labeled glass bottles. I learned this the hard way—left an open flask for a weekend, came back to crystal crust and a weird residue. Store everything away from sunlight and moisture; humidity turns the powder lumpy and sticky over time.
Much of chemistry boils down to small details. Preparing a solution of camphorsulfonic acid DL 10 isn’t tricky, but attention matters in handling, measuring, and storing. Understanding how each solvent works, making sure everything dissolves, and protecting your solutions against time and the elements—all these steps support quality work that delivers consistent results.
| Names | |
| Preferred IUPAC name | 1,7,7-Trimethylbicyclo[2.2.1]heptan-2-one-10-sulfonic acid |
| Other names |
10-camphorsulfonic acid DL-10-Camphorsulfonic acid DL-10-CSA Camphor-10-sulfonic acid 10-(Sulfooxy)camphor |
| Pronunciation | /ˌkæm.fɔːr.sʌlˈfɒn.ɪk ˈæs.ɪd diː ɛl ten/ |
| Identifiers | |
| CAS Number | 5872-08-2 |
| Beilstein Reference | 1720247 |
| ChEBI | CHEBI:61253 |
| ChEMBL | CHEMBL19036 |
| ChemSpider | 2507971 |
| DrugBank | DB11263 |
| ECHA InfoCard | ECHA InfoCard: 100.009.798 |
| EC Number | 2623-23-6 |
| Gmelin Reference | 85902 |
| KEGG | C01712 |
| MeSH | D007595 |
| PubChem CID | 656597 |
| RTECS number | GF9625000 |
| UNII | RY1C009U5O |
| UN number | UN3261 |
| CompTox Dashboard (EPA) | DTXSID5034711 |
| Properties | |
| Chemical formula | C10H16O4S |
| Molar mass | 232.29 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.34 g/cm3 |
| Solubility in water | soluble in water |
| log P | -2.3 |
| Acidity (pKa) | -1.2 |
| Basicity (pKb) | -11.68 |
| Refractive index (nD) | 1.515 |
| Viscosity | 425.0 mPa.s at 20°C |
| Dipole moment | 6.5 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 356 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1181.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1756 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | QJ01CA91 |
| Hazards | |
| Main hazards | Causes severe skin burns and eye damage. |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05 |
| Signal word | Warning |
| Hazard statements | H314: Causes severe skin burns and eye damage. |
| Precautionary statements | Precautionary statements: P280, P305+P351+P338, P310 |
| NFPA 704 (fire diamond) | 3-1-2-W |
| Flash point | Flash point: 107 °C |
| Autoignition temperature | 185 °C |
| Lethal dose or concentration | Lethal dose or concentration: "LD50 Oral Rat 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): LD50 Oral Rat 2000 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.7 mg/m3 |
| Related compounds | |
| Related compounds |
Camphorsulfonic Acid Camphor-10-sulfonic acid CSA DL-10-Camphorsulfonic acid (±)-10-Camphorsulfonic acid |
