Ethanesulfonic acid sodium salt monohydrate has old roots in the world of organic chemistry. Its journey started in the days when sulfonic acids carved their spot as crucial synthetic building blocks. Researchers first explored sulfonates for their water-solubility, finding that sodium salts of simple sulfonic acids worked well as buffers and ionic conductors. Generations grew up seeing these salts in titration labs and glass vials on chemical shelves. As technology advanced, producing high-purity reagents became less about trial and error and more about process optimization, giving rise to refined versions like the monohydrate of ethanesulfonic acid sodium salt.
Chemists value ethanesulfonic acid sodium salt monohydrate because of its stability and range of applications. Unlike many reagents that demand dry storage and careful handling, this one remains resilient. It dissolves smoothly in water, doesn’t produce offensive odors, and offers predictable results for those who depend on repeatable experiments. Even those who don’t count themselves as industry insiders likely benefit from products or drugs whose purification or synthesis steps harness ethanesulfonic acid derivatives.
Anyone who’s handled this compound notices its crystalline nature and characteristic white color. The monohydrate includes a single water molecule for each sodium ethanesulfonate unit, shaping its weight and behavior in different environments. It melts at a high temperature, doesn’t readily volatilize, and tolerates usual fluctuations in lab humidity. As a strong acid salt, it delivers reliable buffering in the acidic range. In solution, it sheds sodium ions and ethanesulfonate anions, making it useful for controlling ionic strength and acidity in chemical reactions or biological assays.
Producers keen on meeting research and industrial expectations stick to rigorous standards. Purity often meets or exceeds 99%, with residual moisture kept within narrow limits for the monohydrate form. Labels specify batch number, assay, water content, storage instructions, and any potential hazardous classifications. Proper labeling proves essential. Numerous labs have learned the hard way that even a small labeling oversight can wreck a successful analysis or cause hours of troubleshooting. Standardization and traceability support not just quality assurance, but the broader scientific trust in chemical supply chains.
The production of ethanesulfonic acid sodium salt monohydrate doesn’t break from the pattern of sulfonates in general. It usually starts with the sulfonation of ethane under controlled conditions to form ethanesulfonic acid. Neutralization with sodium hydroxide follows, converting the acid to its sodium salt. The controlled addition of water during recrystallization ensures the stability of the monohydrate, balancing purity and ease of handling. By tweaking the process, manufacturers can control crystal size and level of hydration, making this a fine-tuned operation rather than a set-it-and-forget-it reaction.
Chemists don’t confine ethanesulfonic acid sodium salt monohydrate to mislabelled bottles on a shelf. They push its boundaries in catalysis, ionic exchange, and as a starting point for further chemical modifications. The compound’s stability and ionic character give it a job in facilitating organic transformations or acting as a supporting electrolyte in electrochemical research. Certain synthetic pathways employ it as a reactant for the introduction of ethanesulfonate groups, broadening molecular diversity for drug candidates and specialty materials.
Across markets and scientific communities, you’ll hear this material called sodium ethanesulfonate monohydrate, or just sodium ethanesulfonate. A few lab catalogs list it as “sodium ethane sulfonate monohydrate” or use trade names in line with their own branding rules. These varied names point back to the same core structure and hydrate state—avoiding confusion takes diligence, as synonym juggling can trip up even seasoned chemists searching for the right product.
Every handling protocol, from material transfer to waste disposal, gets shaped by the nature of sulfonic acid salts. Though sodium ethanesulfonate monohydrate lacks the acute hazards of many industrial acids or bases, it still asks for gloves, eye protection, and proper ventilation. Spills on the bench top mean cleanup to prevent slippery surfaces or contaminated samples. Employees working with kilograms of the material need training tailored for chemical exposure, with safety showers and spill kits ready. Enviromental compliance standards continue to tighten, so disposal involves neutralization steps to protect waterways and ecosystems. On the job, even the so-called “mild” chemicals deserve respect and care.
Chemistry textbooks don’t hit home how often sodium ethanesulfonate finds its way into real processes. In my own work, I’ve seen it anchor buffer systems for pharmaceutical R&D, stand in for other sulfonate salts in calibration solutions, and even ease purification during HPLC runs. Its predictable dissociation and low UV absorption reduce headaches in high-sensitivity analytical applications. Production sites lean on it for synthesizing specialty surfactants. Even some biological systems stretch its uses, since it influences osmolarity and cell response in carefully designed experiments.
Academic and industrial researchers keep probing ethanesulfonic acid sodium salt monohydrate for fresh uses. New methods in green chemistry experiment with it as a benign sulfonating reagent instead of more hazardous alternatives. Some teams work to tweak the hydrate level or modify the counterion, chasing down improved solubility or enhanced catalytic properties. Technical advances in reactor design and continuous flow chemistry have also made it easier to produce and manipulate sulfonates, widening the scope for innovation. I’ve watched project leaders invest serious time in comparing its effects side-by-side with longer-chain sulfonate salts, sometimes finding advantages that only show up under carefully controlled modern methods.
Compared to many other sulfonic acid salts, the sodium monohydrate form has consistently shown low toxicity in mammalian systems during laboratory evaluations. Oral and dermal exposure tests generally yield high LD50 values, indicating that acute risks remain limited under routine lab use. But chemical safety means much more than avoiding immediate harm. Chronic exposure studies continue to track subtle effects on cellular function and organ systems. Environmental research stays focused as well—because even salts can disturb aquatic systems at high concentrations, researchers push for thorough understanding and clear guidance about responsible disposal in both academic and industrial settings.
People who track specialty chemicals know that ethanesulfonic acid sodium salt monohydrate still has unrealized potential. With industries shifting toward cleaner processes and searching for robust, low-impact reagents, this salt draws attention as a proven performer. Green chemistry principles encourage its use in upgrading catalysis, selective functionalization, and sustainable manufacturing. Analytical labs—struggling with increased regulatory demands and higher throughput expectations—benefit from reliable and stable salts that don’t compromise safety or accuracy. As new pharmaceutical molecules and next-generation polymers emerge, chemists keep looking for reagents that offer both flexibility and predictability, two qualities this humble compound continues to deliver. The next breakthroughs in energy storage, diagnostics, or even agriculture may surprise us with just how essential certain simple sulfonates become in the quest for cleaner, safer, and faster solutions.
Ethanesulfonic acid sodium salt monohydrate sounds complex, but its impact spills out well beyond chemistry textbooks. I remember sitting in my college lab, pipetting solutions, barely aware of all the “invisible” helpers behind research. This compound was one of them—hidden in plain sight, doing quiet, essential work.
Hospitals and clinics depend on accuracy. Lab technicians—many working late into the night—lean on stability in their work. This chemical is a favorite tool for pharmaceutical researchers and clinical labs. It acts as a buffering agent, keeping solutions at precise pH levels. That means medications remain safe and perform as intended, especially those drugs that break down easily or change their structure if the acidity swings even a little.
A striking example lies within intravenous drug development. Many modern medications, especially those delivered directly into the bloodstream, can lose effectiveness if their environment grows too acidic or too basic. During my internship at a pharmacy, pharmacists explained how the wrong buffer can cause drugs to clump or lose their punch. Ethanesulfonic acid sodium salt monohydrate offers reliable pH control—protecting patients from risk and companies from expensive recalls.
Diagnostic kits rely on accuracy down to the molecule. Think of a diabetic checking blood sugar or a lab analyzing viruses. Ethanesulfonic acid sodium salt monohydrate steps in as a stabilizer in those kits, so results do not swing with temperature shifts or shipping delays. Getting the right answer—fast—affects real lives. Lives sometimes hang in the balance. If you have ever waited nervously for medical results, you have felt that urgency.
Everyday products tap the resourcefulness of this chemical. In the world of electroplating and metal finishing, factories dip auto parts, jewelry, or circuit boards in special baths to build up protective coatings. Those baths need ingredients that won’t throw off the process. This compound keeps metal ions steady in solution, reducing costly errors. I have talked to folks on the shop floor who say the right chemistry means their products last longer and meet strict safety standards.
At the foundation, safe handling of these chemicals requires real knowledge. Workers and students need regular training so mistakes stay rare. Regulations evolve; keeping up prevents toxic accidents. Consumers can press makers of pharmaceuticals and industrial products for transparency about ingredients and safety steps. Trusting science means everyone—patients, workers, buyers—gets a fair shake.
Finding better buffers and safer chemicals also pushes companies to put research into sustainability. Greener options, less waste, fewer side effects on waterways—this keeps communities healthier and labs compliant with strict environmental rules.
From what I have seen, a single ingredient, tucked away in a bottle on a shelf, might shape everything from your next hospital visit to the shine on your car. Ethanesulfonic acid sodium salt monohydrate offers reliability, but it also reminds us: the small things in science often influence the big picture in life.
Ethanesulfonic acid sodium salt monohydrate isn’t something most people encounter on their daily walks, but its name pops up often enough in labs and industrial supply lists. Its chemical formula comes out as C2H5NaO3S·H2O. That puts together a two-carbon backbone, a sulfonate group, a sodium ion, and a single water molecule tagging along. The formula might seem like a jumble of letters and numbers, but for many working in chemistry, each part tells a clear story about reactivity and handling.
Now, speaking about the weight, scientists turn to molecular weight to measure out precise quantities. Combining all those atoms in the formula gives a molecular weight of 156.17 g/mol. That means a dry scoop from a fresh container matches calculations exactly, which cuts down on the kind of guesswork that can cause problems in research or production. I remember in the early days, more than a few projects stumbled just because somebody misread the hydrate’s weight.
In a working lab, the sodium salt of ethanesulfonic acid fills several roles. It serves as a buffer, providing a steady environment for chemical reactions. Some pharmaceutical syntheses call for buffering agents with a strong sulfonic acid group because weaker acids won’t always keep reaction conditions consistent. As a water-soluble salt, it dissolves smoothly, helping researchers avoid clumping or uneven reactions. That might not sound glamorous, but anyone who has ever mixed a lumpy solution learns to appreciate smooth solubility in a hurry.
Outside of the lab, this salt’s reliability keeps experiments and production lines moving. In my own work, standardized chemicals like this one cut down on troubleshooting. Unexpected results often come from poorly measured, contaminated, or ill-defined chemicals. Having a precise formula and molecular weight saves time and resources, especially in high-throughput settings where every minute counts.
With every chemical input comes the usual risks. Some salts, especially hydrates, absorb more water from the air, which can shift measured weights. Inaccurate weighing gives off-kilter results, wasting effort and money. Storing the sodium salt monohydrate in airtight containers, away from humidity, keeps it consistent. Just a small lapse—leaving the container open—turns a well-calibrated buffer into an unpredictable variable.
Another practical worry surfaces in supply chains. Certain regions face shortages or unexpected cost spikes, often traced back to bottlenecks with precursor chemicals or higher shipping costs. That kind of unpredictability pushes many labs and companies to keep a reliable backup supply. Finding reputable suppliers becomes as crucial as understanding the molecule’s reactivity. Online certificates of analysis and batch-specific purity reports add a layer of transparency, making it easier to trust that what’s in the jar matches the label.
People outside of chemistry rarely think about how much happens behind the scenes just to keep research reliable and reproducible. Accurate chemical formulas and solid molecular weights give researchers confidence to move ahead with their ideas. It’s not so much about memorizing numbers or letter codes, but understanding their importance in real-world applications. Handling ethanesulfonic acid sodium salt monohydrate with the right respect for its properties turns routine lab work into smart, effective science.
Working with chemicals day in and day out has taught me one simple truth: proper storage keeps everybody safe and makes life easier for anyone who handles these substances. Ethanesulfonic Acid Sodium Salt Monohyd finds its place in many labs, often playing a silent but critical role in pharmaceuticals and chemical synthesis. Forgetting about it until you need it can cost more than just time. Ignoring advice about storing this material might ruin your experiment or even put health at risk.
This chemical isn’t one for wild swings in temperature or humidity. Dampness gets in the way fast, which brings clumping, caking, and sometimes even contamination. In my own lab, a humidity-controlled storeroom saved more than a few chemicals from going to waste on days when old buildings played tricks with the weather. Cool storage helps slow down unwanted reactions. Most research teams target room temperature — around 15-25°C — for a reason. Too much heat sometimes breaks down chemicals or causes them to react. Good ventilation keeps fumes or dust from hanging around, especially if a spill happens.
A tight container seals out moisture and air, both of which bring problems. I like containers with strong snap-lids or screw tops. Bags rip too easily, and loose covers invite trouble. If you see anything crusty on the lid, clean or replace it right away. This substance doesn’t play well with strong acids or bases. I’ve watched cross-contamination spoil more stock than carelessness. Strong acids or bases in the same cupboard might set off side reactions or turn minor problems into real hazards. I always set aside one shelf for chemicals like this and use clear labels. Clear space between different chemical groups works better than a complex classification chart stuck to the wall.
Labels solve more problems up front than people think. I write the name, date received, and expiry date — old habits are best here. If something looks off—color, smell, unexpected texture—never guess. Chemicals rarely announce their decline with a big show. When possible, use up older stock before ordering more. It’s always tempting to grab a fresh bottle, but money and safety stay in line when everyone rotates according to dates.
Simple precautions protect everyone. For this material, gloves and goggles keep your skin and eyes out of harm’s way. Dust masks stop sneaky particles. In the group I worked with, we always kept spill kits and flushing stations in place, even if nobody remembered the last time they needed them. With enough chemicals on hand, basic first aid and emergency contacts on a card above the storage bench mean you never fumble when seconds count.
Every bottle eventually runs dry or goes out of date. Leaving unwanted stock lying around invites mix-ups and makes disposal hard. Most sites require collection for hazardous waste. It’s tempting to pour things down the drain or toss them out, but regulations exist for a reason. I always send expired material out with the proper paperwork. Nobody likes an audit gone wrong just because the rules seemed inconvenient once.
Good storage for Ethanesulfonic Acid Sodium Salt Monohyd looks pretty simple: dry and cool spot, tight container, clear labels, clean separation from strong acids or bases, and no shortcuts on safety gear or disposal. Like most good lab habits, it takes a little effort at first, but the peace of mind and smooth workflow always return more than you spend.
Most chemical names sound daunting and honestly, Ethanesulfonic Acid Sodium Salt Monohyd carries that same scientific vibe. Concerns about its safety pop up, especially when it’s mentioned in pharmaceutical labs or research settings. Folks want real answers—not industry jargon—about what health risks come into play if it’s handled daily, spilled, or inhaled.
Working with chemicals invites a level of unpredictability, but some basics bring clarity. This compound shows up in labs, especially as a buffer or reagent. Unlike the more infamous acids and salts that cause immediate harm, this one doesn’t pack a punch with outright toxicity. Still, putting on gloves and using goggles isn’t just for show. Skin or eye contact with almost any concentrated salt can irritate or burn, and inhaling dust from dry powders can start up coughing or throat irritation.
Researchers at reputable organizations like NIH and the European Chemicals Agency list Ethanesulfonic Acid Sodium Salt Monohyd as relatively low-hazard for acute exposure. There’s no evidence of it causing serious conditions like cancer, reproductive damage, or gene mutations in humans. The material safety data sheets back this up—occupational exposure limits haven’t been established, reflecting its low toxicity compared to stronger rival chemicals. Still, those working with it in powdered form see it as a respiratory irritant. Long-term or repeated exposure to the dust won’t pass without consequence: chronic irritation and respiratory discomfort remain probable if you’re careless.
My time in chemistry labs has taught me to respect every compound equally. Treating low-toxicity chemicals lightly often creates regret. Once, a spill went ignored during a busy afternoon in our biochemistry suite. Fingers felt itchy for hours—nothing severe, just a reminder that ‘low hazard’ never equals ‘no risk.’ That experience gave everyone in the room more respect for basic gloves, sleeves, and eye protection. Ventilation fans had more value after that as well.
The real safeguard is not in the compound itself but in routines. Using fume hoods, controlling dust, and preventing skin contact prevent most incidents. This is common practice for much of science and industry, but things go smoother when someone reinforces those habits during training. Regular safety audits help—an extra set of eyes spots what individuals often miss.
Disposal should follow local chemical waste rules. Wastewater streams can concentrate residues, and an attitude of casual disposal creates environmental headaches later. Regulatory agencies value an informed workforce, so up-to-date safety training counts. Companies that post clear guidelines and support open conversations about chemical incidents build safer labs and workspaces.
Clear guidance reduces uncertainty. People trust science more when lab workers, educators, and suppliers explain what a chemical can—and can’t— do. As for Ethanesulfonic Acid Sodium Salt Monohyd, it won’t ruin health with casual contact, but it won’t wait for a careless mistake before leaving a mark. Gloves, good habits, honest answers, and recognizing limits help keep both workers and communities safe from unnecessary harm.
Grabbing a bottle of Ethanesulfonic Acid Sodium Salt Monohydrate for the lab bench, the first question I ask always circles back to purity. In my experience, quality matters more than the label claims—because not every batch works out the same in sensitive reactions or analytical setups. Purity for this salt usually falls in the range of 98% or above when ordered from established chemical suppliers. Reputable brands publish assay values right on their certificates of analysis. Analytical and synthesis work both suffer without this sort of transparency.
Years ago, I tried to cut costs with a cheaper batch from an unfamiliar vendor. The product looked fine, but a simple titration gave unexpected results. Turns out, even trace contaminants like chloride or sulfate skew performance in precision tasks. Friends running high-performance liquid chromatography remind me that impurities often show up as ghost peaks, wasting time. A clean product—meaning minimal water, metal, and organic residue—saves everyone hassle, not just in synthesis but in analytical work.
Quality grades keep things straightforward when reading through catalogs. Analytical grade stands out, promising over 99% purity, almost no detectable heavy metals, and low water content. My students use this for strict assay standards and calibration curves—nobody wants their reference baseline thrown off by strange cations or organic detritus in the salt.
Reagent grade, often near 98% purity, finds its way into most lab routines. It works for buffer preparation, everyday chemical reactions, and bulk processes where a fraction of impurity has low impact. In academic work, this level often balances cost with reliability, making repeated experiments easier to reproduce.
Industrial-grade material, sometimes hovering just above 90% purity, stays off my personal shortlist for important analytical work. Bulk users in manufacturing might choose this to control price, factoring in extra purification steps downstream. Most suppliers publish certificate details online, so checking for things like iron, calcium, or sulfate helps make informed choices.
Lab heads and procurement teams always ask about the product’s moisture level, since the “monohydrate” tag includes a water molecule per formula unit. Moisture swings affect the actual mass weighed and the stoichiometry if not accounted for—tricky for those making buffers by the book. Some suppliers test and declare the loss on drying, which really helps keep results internally consistent. According to Sigma-Aldrich, their analytical grade salt usually features less than 0.5% loss on drying, so you can trust your calculations.
Unexpected metal contamination cropped up in one project I joined, causing wild variations in catalyst behavior. Reputable suppliers trace impurity profiles for sodium, potassium, calcium, and iron, even in batches flagged as reagent grade. It’s worth crosschecking the actual certificate, especially since some industrial processes react strongly to foreign cations even at low part-per-million levels. Extra diligence helps dodge mystery problems in sensitive projects.
Reliable purity protects lab results and downstream applications. The best producers publish validated quality control data, showing batch-to-batch consistency. Third-party audits and clear certificates of analysis make all the difference. Online reviews from research communities give extra information about supplier reputation and customer service. Established brands rarely hide their data—transparency here ties directly to the “trust” arm of E-E-A-T.
If cost constraints force a step down in grade, running validation tests on each batch helps reduce chance of error and ensures peace of mind. Nothing compares to catching impurities early, before they spike analytical error or slow production. Years of sharing protocols taught me this: spend on quality early, and the results will pay you back with fewer repeat runs, less troubleshooting, and cleaner data overall.
| Names | |
| Preferred IUPAC name | Sodium ethanesulfonate monohydrate |
| Other names |
Sodium ethanesulfonate monohydrate Sodium ethylsulfonate monohydrate |
| Pronunciation | /ˌɛθeɪn.sʌlˈfɒn.ɪk ˈæs.ɪd ˈsoʊdiəm sɔːlt məˈnɒhɪdreɪt/ |
| Identifiers | |
| CAS Number | 15687-15-7 |
| Beilstein Reference | 1723884 |
| ChEBI | CHEBI:38760 |
| ChEMBL | CHEMBL1231702 |
| ChemSpider | 20208873 |
| DrugBank | DB11272 |
| ECHA InfoCard | ECHA InfoCard: 100.020.220 |
| EC Number | 220-091-7 |
| Gmelin Reference | 188681 |
| KEGG | C01487 |
| MeSH | D017115 |
| PubChem CID | 23665790 |
| RTECS number | WN6500000 |
| UNII | 3K13K0459A |
| UN number | UN3263 |
| CompTox Dashboard (EPA) | DJ01M374LB |
| Properties | |
| Chemical formula | C2H5NaO4S·H2O |
| Molar mass | 164.16 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.41 g/cm3 |
| Solubility in water | Soluble in water |
| log P | -3.1 |
| Vapor pressure | 0.01 hPa (20°C) |
| Acidity (pKa) | -2.0 |
| Basicity (pKb) | 7.90 |
| Magnetic susceptibility (χ) | -58.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.424 |
| Dipole moment | 6.08 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 189.7 J/(mol·K) |
| Std enthalpy of formation (ΔfH⦵298) | -1178.3 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1066 kJ/mol |
| Pharmacology | |
| ATC code | A16AA06 |
| Hazards | |
| Main hazards | Causes serious eye irritation. |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05 |
| Signal word | Warning |
| Hazard statements | Hazard statements: "Causes serious eye damage. |
| Precautionary statements | P264, P280, P301+P312, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | 1-0-0 |
| Lethal dose or concentration | LD₅₀ Oral Rat: 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 2000 mg/kg |
| NIOSH | KM0875000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Ethanesulfonic Acid Sodium Salt Monohyd: "Not established |
| REL (Recommended) | 0.5 mg/m³ |
| Related compounds | |
| Related compounds |
Methanesulfonic acid sodium salt Ethanesulfonic acid Ethanolamine Sodium sulfate Methanesulfonic acid |
