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Chemistry evolves on the back of small discoveries, and the story of 1-butanesulfonic acid sodium salt proves that point. Before synthetic surfactants became mainstream, chemists looked for ways to separate complex mixtures and to stabilize solutions. In the early days of ion-exchange chromatography, a need emerged for effective ion-pairing agents that could work with both polar and nonpolar compounds. Researchers experimented with octanesulfonate and similar salts. The butane-variant found its seat when scientists focused on shorter chain sulfonates for improved control in analytical techniques. Decades ago, gains in process control and fractional distillation let companies manufacture sulfonic acids on a meaningful scale. At university labs and pilot plants, the move from bench chemistry to bulk batches steadily brought the compound from textbooks to warehouses. By the 1980s, sodium 1-butanesulfonate often showed up in the toolkit of HPLC (high-performance liquid chromatography) operators, especially in pharmaceutical and environmental labs.
1-Butanesulfonic acid sodium salt, sometimes called sodium butanesulfonate, works as an agent for controlling solubility and improving separation in liquid mixtures. Chemists reach for it when they aim for precision in cations’ retention times during chromatographic runs. The white, crystalline solid carries a reputation for easy handling and near-complete solubility in water, which allows it to blend into most standard laboratory buffers. The surfactant properties add utility; some industrial developers value its mildness compared to longer alkanesulfonate cousins. Despite a narrow window of popular use, researchers still turn up new applications every year.
With a molecular formula of C4H9SO3Na, this compound stands as a prime example of how substitutions on small organic molecules can produce big shifts in function. The powder dissolves in water almost instantly, giving a clear and colorless solution. No heavy odor comes off the material, and its melting point generally lands well above room temperature, often around 260°C. The sodium ion stabilizes the sulfonate, rendering it shelf-stable under most storage conditions found in laboratories or manufacturing spaces. Unlike some sulfonate salts that clump with humidity, sodium 1-butanesulfonate keeps a free-flowing nature. The presence of a four-carbon alkyl chain between the head-group and backbone influences both solubility and reactivity, offering a unique balance between hydrophilic and hydrophobic character.
Industry catalogs often sell this salt at purities above 99%, guaranteeing minimal interference from moisture or organic contaminants. Lot traceability shows up as a standard feature, letting users track batch data and match it to specific analytical requirements. Labeling runs beyond basic safety data and reaches into details about assay methods, average particle size, and trace-metal content—especially for pharmaceutical or food testing. Packaging comes in multi-layered jars or sealed foil pouches, with explicit instructions for dry, cool storage. Hazmat rules typically don't apply at common usage volumes, so shipping runs smooth to most destinations. Electronic-grade variants, with caps on individual ionic impurities, target the needs of microelectronics and specialty glass industries.
Producers rely on the reaction between 1-butanesulfonic acid and sodium hydroxide, a straightforward acid-base neutralization. The butanesulfonic acid itself often arises from direct sulfonation of butane using sulfur trioxide or fuming sulfuric acid, followed by strict purification steps. Once sodium hydroxide joins the mix, the resultant salt undergoes repeated crystallization and washing to pare down trace contaminants. Large producers set up closed systems to limit air and moisture uptake throughout the cycle. The technical challenge—keeping alkyl chain length uniform, suppressing side-products like propane derivatives—demands diligence in temperature, pressure, and reactant ratios. Refineries scale up the process by using continuous reactors and inline spectroscopic monitoring, making sure each batch meets analytical-grade standards.
The chemistry of 1-butanesulfonic acid sodium salt lends it to a handful of modifications; the sulfonate group enables further transformations, such as esterifications or nucleophilic substitutions, under the right conditions. In synthesis labs, chemists might swap the sodium cation for other alkali metals, creating variants with subtle property shifts. The hydrophobic tail allows coupling reactions with longer hydrocarbons or aromatic rings, letting developers fine-tune surfactant behaviors. When used as an ion-pairing reagent, its performance changes with pH and ionic strength—so method development must pay close attention to buffer composition. Chemical stability under high heat, mild acids, and light bases means the compound resists most common decomposition routes, a trait valued in analytical setups running round-the-clock.
Staying current with trade and regulatory names helps avoid mix-ups. Sodium 1-butanesulfonate, sodium butanesulfonate, and sodium n-butanesulfonate all refer to this compound, and chemical suppliers sometimes list it as Sodiumn-butane sulfonate. In catalogs, one may also spot n-butanesulfonic acid sodium salt or 1-n-butanesulfonic acid sodium salt—variations that emphasize the straight-chain (normal) structure. For lab procurement, those slight differences in naming tip technicians off to the correct product, especially for buyers who juggle isomers or closely related alkylsulfonates.
Handling practices borrow from best-in-class chemical safety: dust masks and gloves shield staff from accidentally inhaling or contacting fine powders. Although toxicity remains modest compared to many inorganics, standard operating procedures call for eye protection and spill containment. Safety data sheets point out that the compound can cause mild skin or eye irritation but lacks severe acute or chronic health risks. Industrial users often implement closed transfer systems or local exhaust ventilation when weighing or dissolving large quantities. Training on proper chemical waste practices prevents improper drain disposal and keeps local water systems safe, especially in regions with strict discharge rules. From my time in university labs, I saw that proactive housekeeping, double-checking container labels, and keeping emergency eyewash nearby kept the atmosphere orderly and safe, even in fast-paced settings.
The strongest demand for 1-butanesulfonic acid sodium salt sits in analytical chemistry, particularly in HPLC methods that call for ion-pairing agents. Clinical labs depend on it for separating amino acids, peptides, and selected pharmaceuticals where conventional buffer systems fall short. Environmental scientists deploy the compound to track pollutants that resist traditional separation, using its surfactant properties to capture and isolate trace analytes in water and soil. Beyond the lab, niche uses include electroplating baths, textile dye stabilization, and as a performance additive in specialty detergents. In high-purity glass manufacturing, electronic engineers use it to minimize static buildup during particle suspensions. Food chemistry and flavor analysis also find value in its strong electrolyte nature, helping to measure minute differences in taste-active compounds with higher reproducibility. Years ago, while monitoring groundwater cleanup efforts, I saw 1-butanesulfonic acid sodium salt play a key role in tracking organics leaching from old landfill sites.
Active research continues on optimizing the use of this salt in pharmaceutical quality control and trace contaminant detection. Scientists aim to sharpen limits of detection for hormones, antibiotics, and persistent organic pollutants in challenging matrices like blood, wastewater, and processed foods. Analytical method developers modify buffer systems and gradients around sodium butanesulfonate to pull apart compounds with only minor chemical differences. Some R&D teams experiment with mixed surfactant systems, combining the compound with cationic or nonionic species for a custom-tailored effect. In industrial settings, sustainability evaluations look at sourcing, waste byproducts, and energy efficiency in the upstream process. Regulatory and academic collaboration explores greener routes, aiming for bio-based feedstocks or solvent minimization, as research funders set stricter benchmarks for environmental impact.
Toxicologists focus on acute and chronic effects, zeroing in on exposure scenarios in both lab and environmental settings. Testing shows low oral toxicity in animal models, with high LD50 values and no clear evidence of carcinogenicity, reproductive, or developmental harm at occupational doses. Still, the compound acts as a mild irritant for eyes, mucous membranes, and occasionally skin, so worker safety training enforces diligent hygiene and PPE. Ecotoxicity data, while incomplete, hint at low bioaccumulation potential and rapid breakdown in water, lessening long-term risk to aquatic life. Labs with animal handlers or ongoing bioassays have added this salt to their chemical inventory management plans so accidental cross-contamination doesn’t compromise regulated studies.
The path ahead for 1-butanesulfonic acid sodium salt depends on adaptability in emerging industries. Biopharmaceutical companies increasingly demand traceable, ultrapure reagents for high-sensitivity assays, and quality managers expect robust supply chains for key chromatography chemicals. With the ongoing rise of personalized medicine and complex biomolecule manufacturing, demand for reliable ion-pairing agents looks set to climb. Hints from the environmental sector suggest a push for even cleaner water standards, driving analytical labs to rely on trusted standards like sodium butanesulfonate for next-generation testing protocols. Green chemistry priorities nudge producers to investigate biogenic feedstocks and energy-efficient synthesis, aiming to keep the compound competitive as a low-impact specialty chemical. From direct experience supporting instrument method validation, I have seen how improved supply consistency—in purity, labeling, and safety—strengthens customer trust and ensures these basic salts keep powering scientific discovery well into the future.
I’ve spent time organizing benches and getting splashes of all sorts of sodium salts on my lab coat, but 1-Butanesulfonic Acid Sodium Salt always drew attention from folks looking for more than just a boring buffer. The most common scene: bottles of this stuff stacked in the analytical chemistry section, dotted with dusty textbooks and half-eaten lunches. Here’s why: chromatographers depend on this compound to tweak separation in High-Performance Liquid Chromatography, or HPLC. It looks like a simple white powder, but it changes the way molecules behave. I remember times when baseline noise disappeared just by swapping in this salt for something more basic. That’s no accident.
During analysis, ions interact with the separation media in a column. Some molecules cling too hard, others rush through. This curse and blessing creates good science—if you can control it. By dumping in 1-Butanesulfonic Acid Sodium Salt, scientists can “shield” or “mask” certain charges, fine-tuning just which molecule sneaks out next. It comes in handy for amino acids, peptides, and drugs. I’m talking about medicines for the heart, the mind, and infections that still stump doctors. Journals keep reporting improvements in separation, peak clarity, and speed just from this additive.
Most folks won’t bump into 1-Butanesulfonic Acid Sodium Salt at the grocery store. Doctors, though, benefit from its behind-the-scenes work. Hospital labs use it in mobile phases to find blood markers that confirm heart attacks or monitor treatments. Drug companies stick with it during purity checks. If you hear about a new medicine with fewer side effects or a more reliable dose, chances are this compound or one like it played a supporting role. Traces end up in quality assurance sheets and FDA filings because no one wants a false positive—or to miss a sign of real trouble.
Food labs also use this salt. It can help spot preservatives and contaminants. Water utilities and environmental watchdogs run similar chemical tests, aiming to differentiate between harmless and dangerous molecules. Public safety, not just academic curiosity, drives the interest. After Flint and other crises, rigorous chemical separation methods pull up silent threats long before they cause harm. Even in small towns, you’ll find ion-pairing agents like this discussed at town meetings when results come back from outside labs.
Here’s the honest side: not every scientist likes tossing 1-Butanesulfonic Acid Sodium Salt into their solvents. It can gum up expensive equipment if folks don’t clean things right. Disposal, storage, and even sourcing sometimes run into regulation—a reality in budgets and compliance. The salt brings value, but only if handled with respect for both lab safety and the bottom line.
Lab techs and managers keep pushing manufacturers to offer greener and more cost-effective analogs. At the same time, more training can help reduce mistakes that lead to equipment damage. Investing in standardized operating procedures, paying attention to solvent compatibility, and regular machine maintenance can all stretch every dollar further and keep technology accessible for smaller clinics or labs facing economic pressure.
From a scientist’s point of view, the story of 1-Butanesulfonic Acid Sodium Salt goes beyond one chemical. It’s another example of problem-solving, stubborn curiosity, and the never-ending quest for clearer answers. Real science, driven by people who want results that matter in the real world.
Anyone who’s spent time working in a lab or reading a label on a bottle of reagents has seen complicated chemical names. Some roll right off the tongue, some take a few tries. “1-Butanesulfonic acid sodium salt” falls in the second camp. Its chemical formula, C4H9SO3Na, is what tells us how atoms stack up. But the stuff isn’t just a jumble of letters; it’s a good example of why chemistry meets real-world problems in a clear way.
1-Butanesulfonic acid sodium salt isn’t a household word, but anyone doing chromatography or working with ion-pair reagents will recognize its value. It acts as an ion-pairing agent—helping scientists separate tricky compounds more cleanly. Just like the right tool makes a job easier in a workshop, this salt can transform a fuzzy analysis into a tidy data set. More accuracy in separation translates to less guesswork in things like pharmaceutical testing. Precision isn't just something chemists care about for the sake of it; sloppy data in medicine can hurt people.
The formula C4H9SO3Na tells a simple story. The butane chain (C4H9-) is basic carbon and hydrogen, the backbone of plenty of organic compounds. Change just a bit on the end—swap in a sulfonic acid group (-SO3H)—and the molecule picks up a negative charge. Shop for the sodium salt version and you’ll see that sodium (Na) tags along, balancing things out. This little change pushes the compound from something potentially irritating to a useful helper in the lab.
Walking through a lab or a warehouse, I’ve seen scientists give chemicals like this one due respect. The sulfonic acid group makes the compound a bit more water-friendly than other organic compounds. That’s a big part of why it helps in chromatography—mixing with water and organic solvents to shuttle ions along so they separate smoothly. I’ve watched time spent troubleshooting separation problems drop after switching to a good ion-pair agent like this. Still, handling needs care. Splash it on skin or spill it on a bench and you’re in cleanup mode. Chemical safety data sheets remind us that even useful compounds demand vigilance; gloves and goggles aren’t just for show.
The debate over chemicals in science and the environment isn’t going away. Sodium butanesulfonate might not make headlines, but it sits in a long line of substances helping people get reliable, repeatable results. Researchers rely on consistency. Without it, pharmaceutical analysis could go haywire, leading to bad batches or unsafe medicines. Education around safety, transparent sourcing, and regular quality checks go a long way toward building trust. From reading bottles on supply shelves to interpreting data, I’ve learned that knowing a formula is one part of making science smoother and safer for everyone involved.
Many chemists, including students and those working in labs, come across sodium 1-butanesulfonate when looking for a useful additive. This compound often finds its way into chromatography, ion pairing, and analytical research. The question pops up often: will it actually dissolve in water, or will it sit at the bottom of your beaker?
Working in a lab, it’s easy to tell if something will play nicely with water or not. Sodium 1-butanesulfonate, thanks to its sulfonate group, shows a knack for water solubility. The sodium ion and sulfonic acid group attract water molecules, which leads to strong hydration. Drop a scoop of this white crystalline powder in ordinary room-temperature water and stir, and you get a clear solution, not a cloudy suspension. It’s not just a claim—literature lists solubility upwards of 100 grams per liter at room temperature.
Many researchers, myself included, rely on this trait. Prepping a mobile phase for ion-pair chromatography just works better when everything goes into solution. Imagine scraping together several hours to finish a buffer only for the salt to refuse to dissolve. It doesn’t happen with this one. A bottle of the sodium salt sitting on my shelf never failed me, even as brands changed and sources varied. This is backed up by reputable references from chemical catalogs (such as Sigma-Aldrich, Alfa Aesar, and others) listing strong solubility in water.
In the analytical world, reliability matters. HPLC (High-Performance Liquid Chromatography) analysts run samples on tight deadlines. Delays lead to missed windows for stability samples and failed production timelines. The predictable behavior of sodium 1-butanesulfonate can mean the difference between a clean chromatogram and wasted solvents. Its hydrated ions help attach to analytes for better separation. If the salt refused to dissolve, it would push labs towards more expensive or toxic alternatives, increasing both costs and risks for solvents and waste.
The pharmaceutical industry, constantly searching for reliable reagents with minimum surprises, often chooses this additive. Having a salt that doesn’t precipitate, lump, or demand special solvents ends up saving hours in the lab. Safety increases since it doesn’t force chemists to reach for organic solvents like acetonitrile more than necessary. That also matters for those working in teaching labs, where students depend on consistent, safe, and predictable results.
Not every water supply or lab environment is equal. Impurities, residual solvents, or cold workspaces may slow things down. Warm water, a little stirring, and patience bring even stubborn batches into solution. If there’s still struggle, the problem almost always links back to contamination or old, poorly stored reagent, not the nature of the salt.
This consistency gives laboratories confidence. With global supply chains sometimes lurching and unfamiliar brands showing up on purchase orders, having a salt that keeps on dissolving makes daily bench work less of a guessing game. Reliable solubility also helps environmental labs, where avoiding persistent organic pollutants and solvent waste reduction is a growing need.
Accessible data and regular supplier checks will help labs everywhere avoid solubility headaches. Communication between producers and scientists closes the loop, rooting out quality issues before they hit the bench. Investing in reliable, water-soluble salts like sodium 1-butanesulfonate keeps science rolling along, with less waste and more trustworthy results.
Chemistry labs live and breathe numbers. In my own research, seeing that purity percentage on a reagent bottle meant more than just a label—sometimes, it decided if my whole week would yield useful data. Purity for 1-Butanesulfonic Acid Sodium Salt typically gets set around 99%, at least for analytical needs like HPLC or ion chromatography. For those outside the lab world, that means nearly every molecule in the jar is what you expect it to be. High purity keeps the chemistry clean and prevents side reactions that waste time and resources.
Having worked alongside colleagues who analyze everything from pharmaceuticals to food, I’ve seen how even small impurities in chemicals ripple through entire projects. One percent contamination can clog an instrument, distort a trace-level result, or spoil a synthetic reaction. The industry sets tough standards for this exact reason. Producers often guarantee a minimum of 99% by titration or NMR, and reputable suppliers issue certificates of analysis outlining exactly what sits in each batch: water content, trace metals, and identification methods.
Nobody wants mystery chemicals in the mix. In drug analysis, let’s say you’re developing a new process for a generic medication. If the sulfonic acid salt you’re using brings along hidden extras, even at 0.1%, that can transform a clean chromatogram into an unreadable mess. I’ve watched analysts chase unexplained peaks for days, only to finally switch suppliers and see their chromatography fall in line. Pure raw materials shave hours off troubleshooting and support accurate compliance reporting—something everyone wants to avoid headaches with auditors.
Numbers alone don’t tell the whole story. Water content, for example, sneaks into hygroscopic salts like this one. If a salt captures too much water, it throws off weighing accuracy and dilutes chemical activity. Most labs demand less than 1% water content by Karl Fischer titration and double-check with loss-on-drying studies. Even trace metals like iron or copper matter: they can catalyze unwanted reactions or interfere with sensitive detectors. I once saw an entire HPLC run go sideways because a supplier’s otherwise high-purity sulfonic acid salt was loaded with iron contamination.
Beyond the stated 99% threshold, solid suppliers run a full identification panel for sodium, organic purity, and residual solvents. They publish the results. Specs might also call out limits for chloride, sulfate, or even heavy metals below 10 ppm. A couple of the best labs out there make sure to publish their method for each test—nobody wants to buy something blind.
Transparency in sourcing and traceability keeps everyone honest. Anyone working on regulated products should expect to see a full Certificate of Analysis and, if needed, in-house confirmation by running reference standards. My teams always kept a secondary supplier, just in case lot-to-lot consistency slipped.
Choosing suppliers who show full analytical data matters more than cutting costs for budget-grade reagents. Always check batch paperwork for current testing methods and trace results. Store salts in well-sealed containers with desiccant packs to fend off extra water. For the ultra-cautious, a quick lab check for water content and heavy metal contamination can squash problems before they start. Quality doesn’t end at the factory—the users shape it with every shipment they inspect and every bottle they reject.
Chemicals fill shelves across research labs and industrial spaces, but not all salts act the same. I’ve seen how the little things—unsealed containers, forgotten humidity—can turn promising reagents into messy problems. With 1-Butanesulfonic Acid Sodium Salt, getting the storage details right saves a lot of headaches, and dollars, too.
This compound loves picking up water from the air. Left out, the crystals clump and grow sticky. People sometimes treat it like just another powder, and that’s where trouble starts. Damp salt makes weighing inaccurate and messes with reaction outcomes. Laboratories lose time, researchers lose confidence, and data gets sketched with question marks as everyone chases problems the human eye can’t spot.
A good storage routine starts with smart containers. Glass or high-grade plastic jars with tight-fitting lids shut out both moisture and air. I always look for containers with silicone gaskets: even a small air gap can undo the whole effort. The best habit is clicking the lid tightly after each use—I've watched colleagues scoop out what they need, pop the lid back on, then store the jar upright to avoid spills. Simple, but it works every time.
Humidity finds its way into containers if you leave them near sinks or lab dishwashers. Dry places matter. Dry cabinets or dedicated chemical refrigerators keep the physical integrity intact, which leads to more reliable results. Around 25°C, out of sunlight, does the trick. Direct sun or hot radiators can speed up breakdown or discoloration, and we all know what sunlight does to sensitive chemicals.
I learned this lesson after a close call: mixing up sodium salts because the label faded. Use permanent ink to note the purchase date, lot number, and even the moisture content if known. A quick check before pouring prevents hours of wasted time down the line. If you share space, a laminated copy of storage instructions taped near the shelf doesn’t hurt—reminders make for a safer team.
Manufacturers choose packaging for a reason. Those screw-capped bottles and lined seals keep the salt clean and dry through shipping jolts and long storage. Whenever possible, keep bulk product in those containers, transferring only small amounts to secondary jars. My experience in shared academic labs taught me that decanting the whole stash leads to more contamination risks and lost material.
Old chemicals at the back of the shelf rarely inspire trust. I keep a monthly routine of checking my reagents, making sure none show lumps or unexpected color. At the first sign of caking, I discard the batch—the cost of a new bottle is nothing compared to losing a day’s work chasing mysterious results. Regular checks tie in with good documentation, so anyone reading my lab book knows exactly what went into each experiment.
No one wants an accident from tossing unused salt in the sink. Local waste protocols exist for a reason. Sulfonate salts might not seem toxic, but combining them with cleaning chemicals or acids sometimes gives off fumes or clogs drains. Better to package leftovers carefully and take them to the proper disposal point.
Chemistry rewards those who care about the details. Keeping 1-Butanesulfonic Acid Sodium Salt dry, cool, and tightly sealed might sound basic, but it protects both experiments and the people running them. I’ve learned that a few minutes spent on careful storage pays off with months of reliable, drama-free results.
| Names | |
| Preferred IUPAC name | sodium butane-1-sulfonate |
| Other names |
Sodium butane-1-sulfonate Sodium n-butanesulfonate 1-Butanesulfonic acid sodium salt Sodium 1-butanesulfonate |
| Pronunciation | /ˈwʌn.bjuːˈteɪn.sʌlˈfɒnɪk ˈæsɪd ˈsoʊdiəm sɔːlt/ |
| Identifiers | |
| CAS Number | “2386-54-1” |
| Beilstein Reference | 1041858 |
| ChEBI | CHEBI:63693 |
| ChEMBL | CHEMBL159871 |
| ChemSpider | 14189 |
| DrugBank | DB15988 |
| ECHA InfoCard | ECHA InfoCard: 100.016.995 |
| EC Number | 213-934-3 |
| Gmelin Reference | 60453 |
| KEGG | C01183 |
| MeSH | D017367 |
| PubChem CID | 23665784 |
| RTECS number | WO8585000 |
| UNII | U37E6MNO0G |
| UN number | UN2817 |
| CompTox Dashboard (EPA) | DTXSID7046611 |
| Properties | |
| Chemical formula | C4H9NaO3S |
| Molar mass | 176.18 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.36 g/cm³ |
| Solubility in water | soluble |
| log P | -2.5 |
| Vapor pressure | Negligible |
| Acidity (pKa) | -2.1 |
| Basicity (pKb) | -5.3 |
| Magnetic susceptibility (χ) | -44.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.427 |
| Dipole moment | 7.4517 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 346.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1096.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1620 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05, GHS07 |
| Signal word | Warning |
| Hazard statements | H315, H319 |
| Precautionary statements | P280-P305+P351+P338-P337+P313 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | 157.1°C |
| Lethal dose or concentration | LD50 Oral Rat 1960 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 >2000 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | REL (Recommended): 5 mg/m³ |
| IDLH (Immediate danger) | Not listed |
| Related compounds | |
| Related compounds |
Methanesulfonic acid Ethanesulfonic acid Propanesulfonic acid sodium salt Hexanesulfonic acid sodium salt Octanesulfonic acid sodium salt |
