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Sodium acetate has roots in both science and everyday life. Ancient Egyptians knew of vinegar and salt, which when mixed, can lead to the formation of sodium acetate. In the 18th century, chemists began isolating and experimenting with salts created from acetic acid. By the 19th century, sodium acetate anhydrous saw common use in textile dyeing and the production of various synthetic chemicals. Early chemists valued its versatility and straightforward synthesis. Today, the shift from artisanal to industrial production highlights just how much it has graduated from a small-scale laboratory curiosity to a key component for manufacturing, food processing, and research.
You’ll find sodium acetate anhydrous as a white, granular powder. Unlike its trihydrate cousin, it contains no water molecules in its crystal structure. This gives it a longer shelf life and makes it better suited for applications requiring precise moisture control. Industries choose the anhydrous form to avoid unwanted water in sensitive processes. Sodium acetate plays a behind-the-scenes role in everything from concrete longevity to tempering heating pads, shaping outcomes in subtle ways people rarely recognize outside of specialties like food science or laboratory chemistry.
With a melting point near 324°C and a molecular weight of about 82 g/mol, sodium acetate anhydrous stands up to high temperatures and resists clumping under dry conditions. Its high solubility in water lets it dissolve quickly, releasing sodium ions and acetate ions. Unlike many simple salts, sodium acetate remains stable even after cycling through heating and cooling, which allows predictable performance in heat packs and chemical syntheses. Its moderate alkalinity (pH around 9 in solution) gives it special value as a buffering agent, keeping acidity or alkalinity in check in foods, pharmaceuticals, and research buffers.
Packages list sodium acetate anhydrous with labels identifying content, grade (reagent, technical, or food), purity (often over 99%), and storage requirements, like dry sealed containers. High-quality suppliers mark certification, intended use, and any trace impurity levels, satisfying regulatory authorities and users demanding traceability. Labels also note standard hazard identification: while generally considered safe, dust inhalation, rubbing into eyes, or improper disposal can cause trouble, so proper marking keeps handlers informed and protected.
Simple chemistry produces sodium acetate anhydrous: neutralize acetic acid (usually vinegar or its concentrated form) with sodium carbonate or sodium hydroxide. A brisk, fizzing reaction forms sodium acetate and either water or carbon dioxide as byproducts. Removing the remaining water leaves the anhydrous form, typically by evaporation and subsequent heating to drive off the last traces of moisture. Commercial operations fine-tune this method with controlled temperatures, vacuum ovens, and quality checks to ensure batch-to-batch consistency.
Most chemical reactions involving sodium acetate anhydrous center around its ability to donate acetate ions. These can trigger the formation of other organic or inorganic compounds. In the laboratory, mixing sodium acetate with certain acids produces free acetic acid. It also buffers pH ranges essential for biochemical experiments and food preservation. In organic synthesis, sodium acetate can react with alkyl halides to build diverse esters and related chemicals. Sometimes, modifying the sodium acetate molecule enables researchers to design new materials, like biodegradable plastics or advanced catalysts.
Sodium acetate anhydrous appears on inventory lists and research papers under names such as “ethanoic acid sodium salt,” “acetic acid sodium salt,” or “sodium ethanoate.” CAS numbers and purity grades add another layer for tracking specific lots, particularly in industries with heavy regulatory oversight or high stakes for purity and traceability.
Workers exposed to sodium acetate anhydrous rely on proper training and good handling practices to avoid unnecessary contact or inhalation. Regulatory agencies like OSHA or the European Chemicals Agency set guidelines on exposure, storing the powder in sealed, labeled containers away from moisture sources and corrosive chemicals. Cleanup calls for sweeping with care, since it becomes slippery when wet. Disposal guidelines require dilution and neutralization before discharge into sewers or landfills to keep community water and soil safe.
Sodium acetate anhydrous works quietly but reliably across diverse realms. In food processing, it serves as a preservative and seasoning agent, especially in potato chips, ready-meals, and certain sauces. Buffering agents in lab research, diagnostic kits, and pharmaceuticals depend on its predictable behavior in solution. Construction crews add it to concrete to speed curing or enhance resistance to extreme cold, while textile factories use it to fix dyes on fibers. Chemical manufacturers deploy sodium acetate in the synthesis of dyes, pigments, and perfumes. Even heating pads and “hot ice” packs draw on the salt’s ability to store and release heat at just the right moment.
Scientists continue to probe the boundaries of sodium acetate anhydrous. Advances in nanotechnology and biodegradable packaging owe something to this humble salt. Current projects study its capacity to host or carry other compounds, including targeted drug delivery agents or lightweight materials for aerospace. Analytical chemists rely on its buffering capacity to improve precision and reliability in testing, moving beyond classical pH control into new fields like microfluidics and automation. From my own work in research labs, I’ve seen how a well-prepared sodium acetate buffer can make all the difference in experimental reproducibility—for better DNA extraction or enzyme assays.
Toxicity studies present sodium acetate anhydrous as a low-risk substance in most settings. The US FDA and EU food safety authorities list it as “generally recognized as safe” at typical concentrations. Researchers have explored effects of high exposure, noting mild gastrointestinal disturbances at overconsumption levels, but long-term effects appear negligible compared to synthetic additives or heavy metals. Environmental assessments suggest sodium acetate breaks down in water into simple, natural compounds, keeping it clear of red-flag status. Anyone handling the powder should still avoid direct ingestion or contact, particularly for children and pets, as a precaution.
As more industries chase sustainable manufacturing and safer chemicals, sodium acetate anhydrous seems set for broader adoption. Food and pharmaceutical companies look for ingredients with clean safety records and reliable supply chains. Engineers developing “smart” concrete or heat-regulating building materials see sodium acetate as a cost-effective tool. Emerging clean-energy research explores its use in phase-change materials for environmental control, while advances in green chemistry inspire new ways to recycle or repurpose acetate byproducts. If current trends hold, sodium acetate anhydrous will play an even larger part in helping industries balance performance with environmental and consumer safety demands.
Sodium acetate anhydrous shows up in places people might not expect. Scientists rely on it in labs for making buffer solutions. These mixtures keep pH levels steady, which means reactions go as planned. Without this kind of tool, a simple blood test or DNA extraction can take much longer or yield unclear results. Hospitals use sodium acetate for dialysis and certain intravenous medications. It helps replace lost electrolytes and manages blood acidity for patients with kidney issues.
Every winter, folks slip those pocket-sized heat packs into their gloves. At the heart of many is sodium acetate anhydrous. Add water, and this white powder becomes a “hot ice” solution. With a click of a metal disc, the mixture solidifies, releasing gentle heat. This isn’t just a fun trick for children; it’s also a dependable comfort during cold games or outdoor work. The process doesn’t require batteries or wires, which limits mess and risk for users.
Cooks and food producers often use sodium acetate to give snacks like salt and vinegar chips a sharp, unique flavor. Its tangy taste comes from its role as a pickling agent and seasoning. This chemical also stops spoilage in some processed foods. Studies from the U.S. Food and Drug Administration have cleared sodium acetate as safe, showing careful oversight before it lands on plates. With preservatives like these, less food ends up wasted, and people find it easier to keep pantries stocked.
Factories turn to sodium acetate during textile dyeing. It keeps color bright by stabilizing pH, so fabrics resist fading. Concrete workers count on this compound to prevent water from harming freshly poured surfaces during cold weather. By disrupting salt buildup, sodium acetate extends the lifespan of sidewalks and parking lots. Many cities look for alternatives to rock salt because it damages plants and corrodes cars, so sodium acetate offers a less aggressive option.
One concern comes from overuse, especially in urban areas that spread acetate-based deicers each winter. Researchers have noticed that too much sodium can still run off into waterways and affect fish. More environmental studies will guide how much is too much. Manufacturers need to track sourcing: quality varies based on how the raw material was purified. Purity matters for doctors and patients, who count on consistent results from even small doses in medical treatments.
Better training could help workers in food and construction use only what’s necessary, trimming waste. Cities often get the best results by blending sodium acetate with other salts or using cutting-edge sensors that tell crews exactly how much to apply. Education around recycling and proper disposal can shrink negative impacts on rivers and wildlife. Companies that commit to higher purity standards stand to gain trust from customers, doctors, and municipalities.
Life runs more smoothly with chemistry that fits into ordinary routines. Sodium acetate anhydrous isn’t just for chemists in lab coats. From kitchens to hospitals and snowy sidewalks, its reach extends quietly into daily tasks. The next time a winter glove feels warmer, or food lasts longer without spoilage, thank a simple yet versatile compound doing its job behind the scenes.
Sodium acetate anhydrous comes with the chemical formula CH3COONa. People see this compound in chemistry labs, industrial processes, and even household products. Whether someone’s involved in textile dyeing or looking for a safe de-icing agent, sodium acetate often finds a place on the list.
The formula CH3COONa tells a clear story. It shows that a molecule contains two carbons, three hydrogens, two oxygens, and a single sodium atom. Anyone working with it can break down the molecular composition to better understand reactions and potential byproducts. I’ve found that once you get comfortable with breaking down these formulas, predicting reactions or safety requirements gets simpler. For students learning about acids and bases, identifying the acetate ion (CH3COO-) and sodium cation (Na+) is an easy intro to ionic compounds.
Molar mass brings practical information to the lab bench. For sodium acetate anhydrous, you add up the atomic masses:
Total that up, and you get about 82.03 g/mol. Chemists rely on this number every single day. Preparing a buffer? The molar mass tells you how many grams you’ll pour into your flask for the right concentration. That’s often what separates a smooth experiment from an afternoon spent troubleshooting.
In school, the idea of “mole” calculations felt abstract. Training in a teaching lab, I realized how much it matters to have the right amounts—under-dosing means weak reactions, over-dosing creates waste. In my experience, weighing precise amounts of sodium acetate beats guessing with a scoop. Take heating pads: those reusable ones people snap to warm their hands. Each holds a solution of sodium acetate. The right mass determines how well the pad heats up and resets.
Industrial players in textile dyeing lean on sodium acetate’s buffering properties. The molar mass helps control how much to add for consistent dye shades. In food preservation, especially as a seasoning, people need to know how much will dissolve or preserve without overpowering the taste. Getting this wrong can change an entire batch’s texture or shelf life.
Miscalculations can cause real harm. For some, sodium acetate seems harmless, but precision matters. Consider chemical safety sheets—they reference the formula and molar mass because health codes depend on it. Handling large quantities means exposure risks rise. Mistakes in mass mean spills or improper storage become more likely.
In any situation where accuracy matters—be it lab, classroom, or factory—clear knowledge saves time, money, and often health. Solutions grow from better education and clear labeling. I encourage mixing practical training with strong scientific basics and keeping those chemical references close by.
Sodium acetate anhydrous keeps its chemical properties only when shielded from water. The name alone points to a key issue: anhydrous means it lacks water. Tossing it in a damp spot or letting it hang around open containers changes it fast. The powder pulls water from the air easily. Clumpy, water-soaked sodium acetate doesn’t mix the same way and throws off any reaction, lab test, or product using it. A dry, tightly-sealed container works best, and strong plastic or glass with solid lids take care of most storage worries. If you open the jar often, humidity absorbs in with every breath of air, so working in a low-humidity lab or bringing out only what you need at a time saves the rest from going bad.
High heat never helps. Sodium acetate might handle room temperatures, but storing it next to heaters or in sunlight can make it cake, yellow, or degrade. Sitting next to cold or frosty spots won’t hurt the powder, but big swings from cold to warm drag in water from the air. Room temperature, around 20 to 25°C (68 to 77°F) suits its long-term storage. Smaller containers cut down on condensation risk if a room gets warm during the day and cool at night. If your storage room drifts outside that range, moving your supply to an inside cupboard can help.
Packed shelves and chemical cabinets often hold more than sodium acetate alone. Open bags of acids, bases, and organics crowd together. This brings up another risk: dust, fumes, or spilled liquids sneak into open containers or poorly sealed jars. Any unknown substance alters both the safety and the performance of the chemical. In my years working next to sloppy neighbors in shared labs, I've watched sodium acetate go cloudy and lumpy after sitting near open bleach containers. Assigning separate shelves or cubbies helps, as does training everyone to close lids tight and wipe up spills right away. Don’t use a scoop or spatula you’ve dipped in something else — always grab a fresh tool if you might mix up traces of another chemical.
Years in warehouse storage have taught me the value of keeping chemical stock in order. A clear label with the name, opening date, and batch number matches both safety rules and plain logic. Even common chemicals can surprise you — I once had to toss out a whole batch after a new technician refilled a sodium acetate jar with a slightly different grade. Mixing them, even if both are sodium acetate, can upset formulations down the line. Take a pen to every new jar and set reminders to review your oldest stock every six months. If the dry powder shows caking, moisture, or odd colors, toss it out. Don’t risk failed experiments or compromised safety.
Many problems shrink with simple habits. Keep containers tightly closed, stash them in cool, dry spots, and avoid the temptation to store them near reactive or pungent chemicals. Check expiration, and stop the spread of moisture and dust. Investing in airtight jars pays off fast. Explaining the reasons behind careful handling and sharing real stories of lost supplies or botched experiments has convinced more people than any printed safety sheet. If you work with sodium acetate anhydrous, treat each jar with a bit of respect, and you’ll keep your supply reliable for months or even years.
Most people bump into sodium acetate anhydrous during school science experiments, or maybe in reusable hand warmers. In labs and some food processes, it stands out because it does its job quietly and effectively. But just because it’s not screaming for attention doesn’t mean you should skip safety. I’ve watched colleagues take substances for granted and pay the price—dry skin, eye irritation, and sometimes a nasty cough. Those aren’t things anyone wants just for the sake of getting a task done.
This salt won’t turn you into a comic book villain or cause explosions, yet dry, powdery chemicals find their way into creases on your hands, and if you rub your eyes, things get miserable fast. Even dust floating around can irritate lungs. The science says sodium acetate isn’t toxic. Yet, a powder can cause problems when you breathe it in, eat it by mistake, or let it collect on your skin all day. Stories from those who work in chemical prep rooms back it up. Short cuts with basic safety make for ruined afternoons.
Don’t act like gloves and goggles are just set dressing. Gloves seal off your skin from direct contact. Eye protection helps stop you from spending the next hour flushing your eyes at a sink. Work over a tray or at a ventilated bench—spills happen, and it saves clean-up and exposure. Even though sodium acetate seems a low threat, dust still leads to sneezing fits and itchy skin. Close the jar when finished. Don’t let powders float around, waiting to find their way up your nose.
People ignore their noses and throats while pouring. Inhaling dust won’t leave you poisoned, but enough can feel like breathing in a cloud of flour—itchy, unpleasant, and distracting. Respirators or a dust mask give an extra layer. Skip eating or drinking in the room, or you risk an accidental taste test—trust me, the tang isn’t worth it. Hand washing after the fact helps finish the job, stopping chemical traces from joining you at lunch.
Sodium acetate shows up in more places than science class. The food world uses it because it helps control flavors and prevents spoilage. The general feeling in the industry is that, used right, it doesn’t bring major risks when mixed into food. Even so, bulk handling looks different from kitchen usage. Commercial operations use gloves and keep the powder out of the air—proven methods to stop exposure.
Experience helps cement good habits. I’ve learned from mistakes—seeing how minor exposure feels and watching repeat offenders end up with irritated skin. Sites with solid training see fewer issues: people recognize that even a safe chemical becomes problematic in careless hands. Training goes beyond reading a label; it’s about understanding what happens if you skip that basic step.
Handling sodium acetate anhydrous isn’t a high-wire act, but carelessness brings more grief than the extra minute it takes to dig out gloves. The science, history, and my own missteps all point the same way. Put up common-sense barriers, pay attention to what your body tells you, and maintain respect for the small things. That’s the simplest and most effective path to safety in any setting.
Sodium acetate anhydrous sits in countless labs, factories, and classrooms. Chemists reach for it to adjust pH or create heat packs, while others use it in leather processing and textile dyeing. But in every storeroom, someone’s always asking: is this stuff still good, or is it time to toss the whole drum?
Pure sodium acetate anhydrous—C2H3NaO2—shows impressive stability in its sealed, dry form. I’ve opened old chemical storage bins, sometimes with jars over six years old, and the sodium acetate powder has looked unchanged—white, clumpy but dry, no odd smells or colors. According to chemical databases, its recommended shelf life often runs between 3 and 5 years if kept sealed and away from moisture. That’s pretty long by lab chemical standards.
In practice, shelf life hinges on storage. Air-tight containers make a real difference. Sodium acetate anhydrous pulls water right out of the air, turning clumpy or even wet if the lid or packaging lets in humidity. That hydrated form doesn’t destroy the chemical but means you lose the “anhydrous” quality. If you’re running a reaction where water ruins the results, that’s a problem. In my own lab days, any bottle with caked or damp powder meant checking its suitability before using it in a sensitive procedure.
Leaving bottles open—especially in a humid environment—shortens shelf life rapidly. I remember finding an old bottle in a college storeroom, half full and open for who knows how long. The powder had clumped into a hard mass. Analysis still showed sodium acetate, but not the water-free stuff the label claimed. Use in a process that needs dryness, and you’re suddenly troubleshooting failed reactions.
Temperature makes a difference too. While sodium acetate holds up at room temperature, storing it by the window, or in a warehouse without climate control, leads to swings in temperature and humidity. Over a couple of summers, that can transform even tightly sealed bottles.
Chemistry suppliers, including Sigma-Aldrich and Fisher, usually grade sodium acetate anhydrous as stable for up to five years if sealed and kept in dry conditions. That aligns with industry safety sheets and data from reputable manufacturers. The United States Pharmacopeia lists similar storage guidance. These aren’t just best guesses—data backs up those numbers, both in quality control testing and in published stability studies.
Label dates clearly and close containers right away. Store the chemical in a cool, dry place, off the floor and away from direct sunlight. Desiccators or cabinets with moisture-absorbing packets help, especially in humid climates. In shared labs or warehouses, training everyone to respect storage protocols makes a bigger difference than locking cabinets. In my experience, taking five seconds to seal a jar tightly saves hundreds of dollars in replacements and keeps those “why didn’t this experiment work” moments to a minimum.
If humidity sneaks in, drying sodium acetate in a low-temperature oven (below 120°C) often restores it for most uses—just remember that this won’t work for every high-sensitivity process, and you should always confirm purity before critical applications.
Don’t assume just because a bottle’s old it’s useless. With sodium acetate anhydrous, visible clumping, wetness, or label damage signal more risk than the manufacture date alone. Trust experience and knowledge from chemical suppliers, and keep records on your stock. The payoff comes in longer-lasting chemicals, less waste, and smoother lab or production runs.
| Names | |
| Preferred IUPAC name | Sodium acetate |
| Other names |
Sodium ethanoate Anhydrous sodium acetate Ethanoic acid, sodium salt, anhydrous |
| Pronunciation | /ˌsəʊdiəm əˈsiːteɪt ænˈhaɪdruəs/ |
| Preferred IUPAC name | Sodium ethanoate |
| Other names |
Acetic acid sodium salt Sodium ethanoate Anhydrous sodium acetate |
| Pronunciation | /ˈsəʊ.di.əm əˈsiː.teɪt ænˈhaɪ.drəs/ |
| Identifiers | |
| CAS Number | 127-09-3 |
| Beilstein Reference | 3568733 |
| ChEBI | CHEBI:52217 |
| ChEMBL | CHEMBL1359 |
| ChemSpider | 5059 |
| DrugBank | DB09210 |
| ECHA InfoCard | 100.007.380 |
| EC Number | 204-823-8 |
| Gmelin Reference | 60829 |
| KEGG | C00258 |
| MeSH | D017673 |
| PubChem CID | 3220 |
| RTECS number | AJ4300010 |
| UNII | OTCDR5SKN4 |
| UN number | “1841” |
| CAS Number | 127-09-3 |
| Beilstein Reference | 3568736 |
| ChEBI | CHEBI:32139 |
| ChEMBL | CHEMBL1357 |
| ChemSpider | 5045 |
| DrugBank | DB09161 |
| ECHA InfoCard | 100.007.278 |
| EC Number | 204-823-8 |
| Gmelin Reference | 52512 |
| KEGG | C01756 |
| MeSH | D017783 |
| PubChem CID | 3354292 |
| RTECS number | AJ4300010 |
| UNII | NSV4444K330 |
| UN number | 1841 |
| CompTox Dashboard (EPA) | UFA84T0T3T |
| Properties | |
| Chemical formula | C2H3NaO2 |
| Molar mass | 82.03 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.528 g/cm³ |
| Solubility in water | Very soluble |
| log P | -4.3 |
| Vapor pressure | <0.1 hPa at 20 °C |
| Acidity (pKa) | 4.76 |
| Basicity (pKb) | 9.15 |
| Magnetic susceptibility (χ) | -37.6×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.484 |
| Viscosity | 100 cP (5% in water at 20°C) |
| Dipole moment | 1.74 D |
| Chemical formula | NaC2H3O2 |
| Molar mass | 82.03 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.528 g/cm³ |
| Solubility in water | Freely soluble in water |
| log P | -4.3 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 4.76 |
| Basicity (pKb) | 9.26 |
| Magnetic susceptibility (χ) | -38.0e-6 cm³/mol |
| Refractive index (nD) | 1.464 |
| Viscosity | 50 – 70 cP |
| Dipole moment | 1.74 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 86.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -708.4 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -947.7 kJ/mol |
| Std molar entropy (S⦵298) | 86.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -711.0 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -947.7 kJ/mol |
| Pharmacology | |
| ATC code | B05XA04 |
| ATC code | B05XA04 |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | NFPA 704: 1-0-0 |
| Flash point | > 250°C (closed cup) |
| Autoignition temperature | > 607 °C (1125 °F; 880 K) |
| Lethal dose or concentration | LD50 (Oral, Rat) 3530 mg/kg |
| LD50 (median dose) | 3,532 mg/kg (Rat, oral) |
| NIOSH | SN1225000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Sodium Acetate Anhydrous: Not established. |
| REL (Recommended) | 0.3 g (as sodium acetate) |
| IDLH (Immediate danger) | No IDLH established. |
| Main hazards | May cause eye, skin, and respiratory tract irritation. |
| GHS labelling | GHS07, GHS hazard statements: H319 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | Health: 1, Flammability: 1, Instability: 0, Special: - |
| Autoignition temperature | > 607°C (1125°F) |
| Lethal dose or concentration | LD50 (oral, rat): 3530 mg/kg |
| LD50 (median dose) | 3,530 mg/kg (Rat, oral) |
| NIOSH | SN1225000 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | Lower – 0.5 g, Upper – 0.75 g |
| Related compounds | |
| Related compounds |
Sodium acetate trihydrate Potassium acetate Calcium acetate Magnesium acetate Ammonium acetate Sodium formate Sodium propionate |
| Related compounds |
Sodium acetate trihydrate Acetic acid Sodium carbonate Sodium chloride Potassium acetate |
West Ujimqin Banner, Xilingol League, Inner Mongolia, China
