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People searching for reliable, controllable ways to change or clean up industrial chemicals rarely turn to ancient history. Still, modern chemistry stands atop centuries of trial, error, and the willingness to sift through countless new compounds. Sodium Hydroxymethanesulfinate, which many know as Rongalite, showed up in the early 20th century to meet the textile industry’s hunger for a stable, solid reducing agent. Instead of working with unstable sulfur dioxide generators, chemists figured out a shelf-stable salt form that kept some of sulfur’s unique reactivity but let factories measure, ship, and dose it without elaborate precautions. The “dihydrate” form, which carries two water molecules bound into its crystal, gave further stability by reducing the risk of decomposition or dusting. Chemists in Europe and Asia helped drive its development, as water-soluble reducing agents became critical to processing vat dyes, manufacturing rubber goods, and cleaning up environmental messes left by heavy metals or dyes.
Talking about Sodium Hydroxymethanesulfinate Dihydrate by its full name rarely happens on the factory floor. Most folks in dyes, rubber processing, or laboratory settings just reach for “Rongalite” or even “Formamidine Sulfinate.” It looks like a white, crystalline powder, dissolves in water fast, and packs enough punch to reduce a raft of organic and inorganic compounds. Its design fits daily jobs inside textile dyeing, leather tanning, water treatment, and specialty chemical labs. What sets it apart? Sturdy chemical bonds keep it stable until dissolved, making storage in regular containers possible and letting users rely on predictable dosing without worry over wild reactions. Small mistakes don’t trigger runaway chemical hazards that compounds like sodium dithionite or hydrazine might cause. This trait gives workers more confidence during busy production shifts.
Rongalite dihydrate comes off as a white, odorless solid. It feels a bit cool and slippery in the hand—common with salt hydrates. Dissolve it in water and the solution turns slightly basic, thanks to the sodium content. Its chemical identity, HOCH2SO2Na·2H2O, means the molecule binds two water units per sodium hydroxymethanesulfinate group; this makes the powder bulkier and a bit heavier by weight than the anhydrous form, but far less prone to forming irritating dust. The hydrate crystal structure means it’s not fussy about ambient humidity, which keeps it from clumping or decomposing in storage. Heat does break down its bond with water and, if pushed way past 100°C, the chemical itself decomposes, releasing formaldehyde and sulfur dioxide among other things. Mix it with acids and you’ll liberate sulfur dioxide—hence its key industrial application as a clean, measured SO2 source.
Most industrial buyers look for a consistent assay (usually greater than 98%) for sodium hydroxymethanesulfinate dihydrate. The labeling on large sacks or bottles points out its dihydrate form and underscores storage recommendations—cool, dry, out of direct sunlight. While regulatory groups such as REACH or the U.S. EPA want chemical distributors to include hazard statements about respiratory irritation or aquatic risks, the solid form proves less risky than spraying solutions or gaseous alternatives. The labeling rarely focuses on glamour—just batch number, net weight, purity, and whether additives like stabilizing agents sneak into the mix.
Making Sodium Hydroxymethanesulfinate Dihydrate is a balancing act between cost, yield, and safety. The most established process routes formaldehyde and sodium dithionite or sodium bisulfite through an aqueous reaction, where careful temperature and pH control nudges the reaction toward the desired sulfonate. Skipping steps or ignoring temperature triggers nasty byproducts, including thiosulfates or even dangerous gases. To get to the dihydrate, chemical plants simply crystallize the product from water-rich solutions, setting up controlled cooling so that two water molecules clamp onto each functional group. Wash and dry the crystals gently to avoid hydrolysis or caking—the art is in keeping a chemical that holds water without picking up too much humidity from the air.
Chemists appreciate sodium hydroxymethanesulfinate for its versatility in reduction reactions. It shifts transition metal ions from higher to lower oxidation states, strips oxygen from a range of colored textile dyes, and even supports organic synthesis by neutralizing stubborn oxidants. Reactions with mineral acids drive out sulfur dioxide, which then strips unwanted color or residues from fabrics and paper. In advanced fields, researchers experiment with derivative compounds, trying to tweak its molecular structure to yield more stable, or more potent, reducing agents for electronics assembly or green chemistry initiatives. The core ability—to cleanly donate electrons and yield innocuous byproducts—keeps it valuable, no matter what modifications the next wave of chemists dream up.
Anyone browsing through chemical catalogs soon learns that this compound’s history travels across languages and industries. “Rongalite” still rolls off the tongue for anyone in the dye trade. “Formamidine Sulfinate” pops up in more technical papers, especially those focused on organic synthesis. “Sodium Formaldehyde Sulfoxylate” describes its build more directly. All these names point back to that same, stable, dihydrate structure. The proliferation of synonyms can create confusion if users order the wrong grade, so the tight-knit community around rubber, textile processors, and specialty labs just shrugs and double-checks the CAS number to play it safe.
Nobody likes unexpected chemical burns, allergic reactions, or cleanup nightmares at work. Sodium hydroxymethanesulfinate dihydrate flies under the hazard radar compared to its more volatile cousins, but taking shortcuts can still cause trouble. The plain dust may irritate the nose, eyes, or throat for workers without masks or proper extraction. Wet spills get slippery fast, and uncontrolled acid contact pumps out lung-tickling sulfur dioxide. Factory floors established clear routines: respirators for bulk handling, gloves for every shift, and extra caution in the mixing room. Those routines keep injury rare and keep insurance rates from ticking up. In my experience, training new workers in the straightforward but non-negotiable handling of Rongalite means fewer mistakes later, especially for those who come from labs where chemical standards vary more than you might expect.
Many of us first hear of sodium hydroxymethanesulfinate through its core job in textile dyeing, where it strips color to prep cottons or builds up vibrant shades through reduction. Its utility spreads further: clean-up chemistries in municipal water plants, bleaching processes for paper and pulp, or even as a mild reducing agent in pharmaceutical manufacturing. The stability and clean reaction profile open doors to roles in electronics, recycling, and specialty coatings. Environmental researchers lean on it during trials to mop up heavy metals or break down persistent organic pollutants in soils and waters. This practical utility sustains market demand and spurs new technical tweaks from research labs aiming to expand or green up the reach of industrial-scale reducing agents.
No single product holds its market position forever without regular reinvention. Researchers today keep tweaking the salt for enhanced activity at lower temperatures, higher pH tolerance, or better fit with biodegradable process streams. Papers from Europe and Asia often focus on minimizing byproducts or capturing more of the liberated SO2 for energy and material reuse. In my own outreach to labs and pilot plants, the talk drifts toward integrating sodium hydroxymethanesulfinate into multi-step processes, where every chemical input needs traceability and environmental accountability. The push for more circular chemical economies motivates the search for recovery, reuse, and responsible disposal methods. Some teams even explore how trace impurities in the salt—such as residual formaldehyde—might impact application areas ranging from medical diagnostics to specialty coatings.
No industrial reducing agent rolls off the trucks as completely hazard-free. Toxicologists gave sodium hydroxymethanesulfinate an honest shake over the decades. Standard safety studies point to mild irritation from dust and solution contact, with few systemic effects unless someone intentionally ingests large amounts—something that rarely aligns with routine operation. The liberation of SO2 during misuse or accidental spills creates more concern for asthmatics or those with sensitive airways, so protocols push for strict air monitoring in closed spaces. Unlike some other sulfur-based reducing agents, concerns over long-term carcinogenicity or bioaccumulation have not surfaced in peer-reviewed studies. Still, regulators in Europe and Asia maintain moderate restrictions on maximum residue levels in finished products, especially for any food-contact polymers or filtration resins. Operators benefit by staying current with these updates, since downstream customers ask pointed questions about chemical inputs to meet their own regulatory reporting.
Most chemical products follow a predictable arc—introduction, growth, maturity, decline as safer or greener options come up. Sodium hydroxymethanesulfinate dihydrate finds itself at an inflection point for that very reason. The rise of environmentally worried buyers and tougher global rules could push for plants to curb SO2 emissions, improve waste water management, and develop lower-impact alternatives. Yet, the low cost, predictable storage, and time-tested safety record keep Rongalite on spec lists for applications from synthetic leather to electronics. Future research seems poised to drive down any negative emissions, broaden suitability for green processing, and fine-tune physical properties to mesh with automated dosing or in-line analytical controls. My sense from industry meetings is that this salt will undergo incremental—not radical—redefinition. Factory managers, environmental scientists, and everyday chemical handlers all have a stake in keeping it safe, reliable, and fit for next-generation processes, just as their predecessors did nearly a century ago.
Sodium hydroxymethanesulfinate dihydrate, better known to many in industry circles as sodium formaldehyde sulfoxylate, serves a pretty specific purpose across several manufacturing processes. Those who work around textiles, paper mills, and photography have probably come across it—even if the name doesn’t roll off the tongue. The compound shows off its usefulness by breaking down certain chemicals and bringing color to fabrics and paper.
Textile plants rely on sodium hydroxymethanesulfinate dihydrate during fabric processing. It acts as a reducing agent, stripping away excess dye and making whites look brighter. Brands care a lot about repeatable shades, so this compound helps operators reset fabrics. Anyone who's ever done household laundry knows how hard it can be to remove unwanted stains or colors. Now scale that up to industrial loads and it gets much trickier. That’s where sodium hydroxymethanesulfinate dihydrate really shines, because it tackles both color correction and fixes mistakes in a batch by neutralizing reactive dyes. The chemical cleans up after spills that can otherwise mean wasted fabric and lost profit.
Paper manufacturing also sees benefits from the same reducing power. Wood pulp often arrives with colors and oxygen-based impurities. Adding sodium hydroxymethanesulfinate dihydrate clears out these shades, giving paper its uniform appearance. A paper plant I toured a while back showed me how much cleaner their batches looked after switching from traditional chlorine-based methods. The environmental footprint shrinks when companies use alternatives to heavy bleaches—plus, worker safety improves with fewer toxic byproducts.
In the world of photography, old-school film labs depended on sodium hydroxymethanesulfinate dihydrate to develop images. It works behind the scenes, fixing images as part of the solution baths. Even though digital has taken over, plenty of professional printers still keep this compound stocked for special printing effects. Chemicals like this make it possible to fine-tune each photograph, giving artists more control over the final look.
Handling chemicals like sodium hydroxymethanesulfinate dihydrate takes real care. Direct exposure can irritate skin, eyes, and the respiratory system. Plants train workers to use gloves, goggles, and good ventilation. Waste management also becomes a priority. Modern factories collect runoff and neutralize it before letting water leave the plant. This not only protects staff but keeps harmful substances out of local streams and ground supplies.
Many industries hunt for greener approaches, searching for replacements that cut down on chemical waste. Some labs experiment with enzyme treatments or oxygen-based compounds, hoping to match or surpass the efficiency of sodium hydroxymethanesulfinate dihydrate. It’s not easy to find eco-friendly options that deliver the same results at a comparable cost or speed, but research moves ahead. Companies that want a sustainable image—and real change—test new blends and processes every year.
Sodium hydroxymethanesulfinate dihydrate carries a long track record in textiles, paper, and photography. Without it, these products wouldn’t look the same. The push for safer handling and reduced environmental impact drives continual improvement. As more operators swap out hazardous chemicals for this one, or look toward new alternatives, everyone benefits from a cleaner, safer way to bring color to the world around us.
Sodium Hydroxymethanesulfinate Dihydrate isn’t a household chemical. It finds its way into industrial applications, especially in textile, paper, and sometimes even in photographic industries as a reducing agent. Having handled storage for various fine chemicals in a busy factory environment, I’ve seen projects derailed by sloppiness at this stage. So, what does good storage look like for a chemical of this kind?
This compound has a soft spot for water in the air. Even a slightly humid storeroom can become a problem before you know it. Clumping, cake-formation, or the risk of early decomposition come up fast if containers stay open for too long. Sealed, airtight packaging works best. In the plants I’ve worked at, double-bagging inside a drum and even silica gel packs inside the secondary bag kept problems at bay. Dedicated dehumidifiers and dry cabinets prove their worth over time.
Not every chemical demands refrigeration. Sodium Hydroxymethanesulfinate Dihydrate prefers a middle ground. Storage at room temperature – usually below 25°C – keeps it stable. Heat accelerates its breakdown and can give off sulfur dioxide or formaldehyde, both of which spell trouble for health and the working environment. High or swinging temperatures risk crystal structure changes, even if you don’t see it right away. Routine checks with temperature loggers tell you if a room’s drifting into the danger zone.
Bright light, especially sunlight, chips away at purity. A windowless storeroom offers consistency. If natural lighting remains impossible to avoid, opaque or amber containers limit UV harm. In one busy facility, a well-meaning cleaner left a lid off near a sunlit window—product gone bad. So covering stock with UV-safe sheeting adds one more cheap insurance policy.
Chemicals like this don’t mix well with acids, oxidizing agents, or nitrites. In my own experience, color-coded storage shelves simplify the process. Red tags for “keep away from acids,” blue for “safe with bases” help new staff who don’t know all the labels yet. Keeping a clear inventory, with physical barriers for incompatible chemicals, reduces the risk of unexpected reactions. Material Safety Data Sheets often stress this, but seeing poorly-organized storerooms shows how easily simple steps are skipped.
Only use containers rated for chemicals. Thick, high-density polyethylene and well-sealed HDPE drums or bottles keep product safe. Thin plastic gives way or leaks over time. Labels matter too – easy to read, waterproof, and stuck on tightly. Handwritten or faded labels open the door to cross-contamination or misidentification. Every time I’ve seen a messy label, there’s been a mistake waiting to happen. Regular checks and a sharpie in the storeroom drawer save serious headaches later.
Even with correct storage, some slow decomposition happens over time, which can mean whiffs of sulfur dioxide or formaldehyde. Ventilated storage limits this buildup. Simple air exchanges, a well-maintained HVAC, or spot extractors in cabinets keep air fresh and workers safe. I’ve always insisted on weekly checks for odors and residue, no matter how “stable” the product claims to be.
Even the best protocols mean nothing unless people follow them. Short training sessions for staff, frequent spot inspections, and honest feedback catch small mistakes before they become big problems. A detailed storage log—location, temperature, humidity, container type—saves product and keeps you on the right side of regulations.
Respect the quirks of Sodium Hydroxymethanesulfinate Dihydrate, and safe, stable storage becomes routine. Ignore the details, and small slip-ups quickly snowball into bigger, costlier problems.
People often feel uneasy when they see chemical names like sodium hydroxymethanesulfinate dihydrate on an ingredient list. The word itself sounds intimidating, almost like something from a lab thriller. This chemical works as a reducing agent, mainly in printing, dyeing, and even as a food additive. The question isn’t whether it has a long name—what most want to know is, does this compound actually pose a threat to health or the environment?
Companies use sodium hydroxymethanesulfinate dihydrate because it works well and keeps costs down. Everyone from industrial workers to lab technicians can tell you that safety matters most. Based on safety data from regulators in the U.S. and Europe, the main risks come through direct exposure. Skin contact leads to irritation. Dust from the powder form causes coughing or breathing trouble. Accidental splashes can hurt the eyes. Ingestion would likely upset the stomach, but it doesn’t line up with chemicals best known for dramatic, acute toxicity.
None of that means it’s harmless. Oxidizing chemicals that share some of its traits sometimes break down into gases like sulfur dioxide, especially in high heat or acid. Sulfur dioxide stings the lungs and triggers asthma even in low doses. Proper storage and handling make a huge difference, so industrial users rely on personal protective equipment and good ventilation.
No trustworthy research links sodium hydroxymethanesulfinate dihydrate to cancer or birth defects in real-world scenarios. Big data sets from workplace exposure studies back that up. That said, chronic exposure to dusty environments brought on by poor safety habits does increase risk for respiratory or eye problems.
It makes sense to worry about what happens if large amounts go down the drain. Fortunately, this compound breaks down under regular wastewater treatment. There’s little risk of it showing up in drinking water at dangerous levels. Fish and other aquatic life usually face more trouble with heavy metals and pesticides than this particular reducer. In my years guiding high school chemistry labs, I’ve learned to never dismiss the power of basic care in preventing spill-over incidents. Clean habits and strict oversight keep low-risk chemicals from becoming a larger problem.
Trying to erase risk is unrealistic, but reducing it is practical and expected. Using gloves and goggles, keeping powders contained, running fans, and keeping emergency eyewash stations nearby all help. Labeling every bucket and container matters, too. Forgetting such basics has tripped up even the most experienced workers.
Regulators set exposure limits for chemicals for good reason. Managers ought to remind their people about these standards regularly, not just during annual training. At home, most folks will never run into sodium hydroxymethanesulfinate dihydrate. If you do, maybe in a craft kit or DIY project imported from abroad, there’s no harm in checking safety sheets or reaching out to someone with experience.
Chemistry makes our lives easier, brighter, and sometimes more flavorful. Fear grows fastest where no information exists. So, inspecting the evidence shows sodium hydroxymethanesulfinate dihydrate deserves respect, not fear. Just because something sounds alarming does not mean it is lurking as a hidden danger, waiting to strike. Taking precautions, following guidelines, and teaching proper habits protect both workers and the environment.
Anyone who works in a lab or manages chemical supplies knows the headache of shelf life. Sodium Hydroxymethanesulfinate Dihydrate, often found in a pale, crystalline form, stays reasonably stable in the right conditions, but age and storage mistakes can mess with its performance. Take it from someone who has seen a colorless solution develop a weird yellow tinge just because it sat too long in a humid corner — every chemical has its breaking point.
This compound doesn’t just magically degrade overnight. Instead, you start to notice gradual shifts. Exposure to moisture, light, and air will kickstart unwanted chemical reactions. Sodium Hydroxymethanesulfinate Dihydrate in its dihydrate form already contains water molecules, so extra humidity tips the balance and invites clumping or conversion into less useful forms. A well-sealed and cool storage space buys you about 12 to 24 months. Beyond that, any quality guarantee evaporates and every risk of inaccurate lab results rises.
I’ve opened jars that were only a year old, stored tight, and everything was fine. Other times, a careless storage clerk stacked containers in direct sunlight, causing a chain reaction of spoilage among expensive chemicals. Fluctuating temperature especially torpedoes shelf life, so steady, cool storage really pays off.
Labs and factories keep a close eye on expiry dates because old or degraded material risks not just money, but safety. Picture a textile batch that comes out uneven because the reducing agent misfired. Or something more serious: if someone unexpectedly inhales decomposition fumes, that’s a hospital visit nobody wants. Old stock also produces byproducts that complicate waste disposal, increasing costs and regulatory headaches.
Busy operations like to squeeze every drop of value, so people look for ways to extend storage. Still, nothing replaces proper timing and handling. Marking purchase and opening dates matters more than most realize. Blind trust in manufacturer guarantees just invites trouble, especially since companies base labeled shelf life on best-case storage, not on the rough-and-tumble reality of a working lab or warehouse.
You can protect Sodium Hydroxymethanesulfinate Dihydrate by following a few low-tech steps: keep containers tightly closed, store them away from moisture and sunlight, and keep the room cool. Dessicant packs are cheap insurance. Regular inventory checks help spot any issues before they grow into expensive problems. If a batch shows any clumping or discoloration, it’s not worth gambling with — replacement saves time and reputation.
Reliable quality depends on respect for expiration. Drawing on honest experience, I can say that chemicals rarely forgive shortcuts. Make shelf life a priority, educate every hand that touches the inventory, and treat safe storage as a non-negotiable. Costs drop, product safety improves, and trust in lab results stays strong. Keeping an eye on the shelf life of Sodium Hydroxymethanesulfinate Dihydrate saves money and avoids unseen risks that nobody wants to clean up after.
Anyone who’s spent time in a lab knows this: handling chemicals without proper caution can mean trouble. Sodium Hydroxymethanesulfinate Dihydrate, known in many places as Rongalite, lands on the shelf somewhere between the common and the potentially hazardous. Touching, breathing in, or accidentally eating even a small amount of this substance can irritate skin, eyes, and breathing passages. Mistakes with this one sometimes leave people feeling the aftermath for days, and there’s enough research showing health problems linked with even short-term exposure.
Before even thinking about handling this chemical, grab your gloves. Nitrile or neoprene both work. Add a set of chemical splash goggles and, in places where dust hangs in the air, a lab coat and dust mask. This isn’t a time to trust open-toed shoes or short sleeves. One careless moment and you may head home with a rash or worse. Handle it in a well-ventilated space. Fume hoods aren’t just fancy furniture: they pull away dangerous vapors and dust, cutting down on what you breathe in. These steps seem basic, but skipping them for the sake of speed has landed plenty in the emergency room.
Sodium Hydroxymethanesulfinate Dihydrate reacts with acids and some strong oxidizers. If you store it near cleaning solutions, pool chemicals, or acids, there’s a chance for releases of toxic sulfur dioxide. I’ve seen cramped storerooms jammed with mismatched chemicals; that’s where small mistakes lead to big disasters. Always label containers clearly and keep them in cool, dry, and tightly closed storage, well away from acids and oxidizers. Even if a closet looks empty, double-check every time you reach for a container: the extra step saves a world of trouble.
Spills sometimes trigger panic, but they don’t have to. Anyone who drops or knocks over a container should start by keeping people out of the way. Spraying water or sweeping can stir up more dust or trigger unwanted reactions. Use a HEPA-filtered vacuum or dampen powders with a bit of water to keep dust low. Shovel the material into a sealed, labeled drum. Bag contaminated gloves and rags, too. Air out the area and double-check before saying the job’s finished. Never let a spill linger as an “I’ll-get-to-it-later” task.
Throwing this chemical in the regular trash or pouring it in the drain won’t cut it. Most cities treat sodium salts as hazardous waste for a reason. Local hazardous waste facilities accept sealed containers, and they use processes that neutralize and contain the danger. It’s illegal in many places and downright dangerous for the environment to ignore these disposal rules. A single dump down the wrong drain can damage wildlife and water supplies. That’s not a legacy anyone should leave behind.
Safe handling practices start way before the chemical hits the bench. Regular training, clear safety protocols, and shared responsibility between workers and supervisors create safer workplaces. Everyone should feel empowered to call out poor storage, sloppy habits, or broken safety gear. No amount of paperwork replaces a culture where people watch out for each other. Labs and factories run better—and accidents become rare—when safety isn’t just a box to check off, but an everyday habit.
| Names | |
| Preferred IUPAC name | sodium;hydroxymethanesulfinate;dihydrate |
| Other names |
Sodium Formaldehyde Sulfoxylate Dihydrate Sodium Rongalite Dihydrate Sodium Formoxylate Dihydrate Rongalit Dihydrate |
| Pronunciation | /ˌsoʊdiəm haɪˌdrɒksaɪˌmiːθeɪnsʌlˈfɪneɪt daɪˈhaɪdreɪt/ |
| Identifiers | |
| CAS Number | 871-58-9 |
| Beilstein Reference | 151873 |
| ChEBI | CHEBI:61357 |
| ChEMBL | CHEMBL72758 |
| ChemSpider | 160993 |
| DrugBank | DB11382 |
| ECHA InfoCard | 14e7d2e2-0f01-4b43-82a9-4d0a5480a219 |
| EC Number | 262-051-7 |
| Gmelin Reference | 74358 |
| KEGG | C01697 |
| MeSH | D015547 |
| PubChem CID | 23665704 |
| RTECS number | VV6390000 |
| UNII | 415O8P61UO |
| UN number | UN3346 |
| Properties | |
| Chemical formula | NaCHO2S·2H2O |
| Molar mass | 210.16 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.6 g/cm³ |
| Solubility in water | Very soluble in water |
| log P | -3.4 |
| Vapor pressure | <0.01 mmHg (20°C) |
| Acidity (pKa) | 7.2 |
| Basicity (pKb) | pKb: 6.8 |
| Magnetic susceptibility (χ) | -49.0e-6 cm³/mol |
| Refractive index (nD) | 1.420 |
| Dipole moment | 1.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 230.6 J·K⁻¹·mol⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -602.98 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1243 kJ/mol |
| Pharmacology | |
| ATC code | A01AB11 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | **"GHS05, GHS07, Danger, H302, H315, H318, P280, P305+P351+P338"** |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P264, P270, P273, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 2-0-0 |
| Lethal dose or concentration | LD50 oral rat 2620 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat 820 mg/kg |
| NIOSH | WX8C2-ED1S |
| PEL (Permissible) | PEL: 15 mg/m³ |
| REL (Recommended) | 30 mg/m³ |
| IDLH (Immediate danger) | No IDLH established. |
| Related compounds | |
| Related compounds |
Sodium formaldehyde sulfoxylate Sodium dithionite Sodium bisulfite Formaldehyde Sodium sulfite |
