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A century ago, scientists thought about water a lot, wondering how simple changes at the atomic level could spark breakthroughs. Swapping out the regular hydrogen atom for deuterium—that slightly heavier cousin—led researchers to a whole new landscape. In the early 1930s, the discovery of deuterium by Harold Urey and colleagues set things in motion. Fast forward, sodium deuteroxide, which looks like an unassuming white powder, found itself under the spotlight. Chemists started preparing it soon after, using heavy water to tease apart subtle differences in chemical behavior. The real push came during and after World War II, where heavy water’s role in nuclear research made sodium deuteroxide an essential building block for both basic laboratory science and strategic development. From then, it became a staple for isotope chemistry, enabling both academic research and industrial use.
Sodium deuteroxide comes across as straightforward—basically, it’s the deuterated version of sodium hydroxide. On paper, the structure looks identical: sodium ions danced with deuterium-laden oxide ions. But the real difference shows up in how it acts in the lab, especially in sensitive work where each atom’s weight counts. Most scientists run into this compound when trying to swap out normal hydrogen with deuterium in molecules, which radio-labels or tracks reactions for both pharmaceutical research and theoretical chemistry. In small bottles, it usually travels as pellets or concentrated solutions, always stored away from air and moisture, ready to jumpstart reactions that a regular base just can’t do as precisely.
At first glance, sodium deuteroxide looks and behaves quite like sodium hydroxide—it absorbs water quickly, dissolves in heavy water, and sits as a powerful base. Many seem surprised to find that just a small bump in atomic mass can tip the scales for reaction rates and pathways. That extra neutron in deuterium makes for slight but measurable kinetic isotope effects. These oddities ripple through organic and inorganic chemistry. The melting point, solubility, and reactivity stick close to its lighter cousin, but the deuterium slows down certain reaction steps, making the compound valuable for studying reaction mechanisms. In handling, it feels caustic and highly hygroscopic, so proper containment in well-sealed containers remains a standard lab practice. The solution takes on a slightly slippery feel, but trained hands know just how quickly it attacks glassware and skin if not respected.
Every bottle needs to state its purity and the source of deuterium—nobody wants to pay premium for ordinary sodium hydroxide masquerading as the real deal. Labels mention the concentration, the heavy water source, and sometimes even the ratio of sodium to deuterium. For higher-end uses, labs demand a deuterium enrichment that tops 99 percent, and manufacturers have to justify every decimal point since impurities can ruin sensitive experiments. Most research-grade products call out key warnings and Chemical Abstracts Service numbers, helping busy scientists confirm what’s inside at a glance. Information on batch analysis and the storage conditions often comes tucked into the paperwork, especially for big research contracts.
Making sodium deuteroxide in the lab takes care and patience. The common route starts with heavy water, D2O, which isn’t cheap, so everything revolves around minimizing waste. In one approach, sodium metal reacts directly with heavy water, creating the deuterated base and releasing deuterium gas. This method feels straightforward, but it’s not for the faint of heart—sodium metal means business, and everything needs to be set up in an inert atmosphere, away from the tiniest hint of moisture or oxygen. Commercial preparations may run more elaborate, column-based purification after synthesis to squeeze out as many impurities as possible. Assembling the setup often takes longer than the reaction itself, but anyone who’s handled sodium on the bench knows cutting corners means ruined product or ruined glassware.
Sodium deuteroxide operates as a heavy-handed base, primed to pull off exchange reactions that regular sodium hydroxide can’t quite match. It comes into play when swapping hydrogens for deuteriums in organic molecules—a vital process for tracking molecular movements in chromatography, nuclear magnetic resonance studies, and even in drug metabolism research. In organic synthesis, it facilitates challenging deprotonations, helping chemists study isomerization reactions, tautomeric shifts, and ester saponification where tracing a deuterium atom through each transformation reveals how molecules really behave. Many a PhD thesis hinges on the differences measured using sodium deuteroxide, showing that a single extra neutron can open new doors in mechanistic exploration. Besides, chemists adjust its concentration and purity to fit the sensitivity of their work, knowing full well that stray protons creeping in from the air can cloud precious results.
Some call it sodium deuterate, others stick with sodium deuteroxide. UChem, D-NaOH, and other short-hands show up in technical literature, especially for those who like to keep notebooks tidy. Even catalogues from chemical suppliers swap among these terms, prompting researchers to double-check before clicking “order.” The differences feel subtle, but missing the mark means wasted time or unexpected results, a risk every experienced chemist tries to avoid with a glance at the labeling or safety data.
Sodium deuteroxide doesn’t pull punches when it comes to safety. It tears into organic tissue just like regular sodium hydroxide, causing burns on skin and eyes in seconds. Protective gear—gloves, goggles, lab coats—becomes non-negotiable. Most labs require working under fume hoods with tight-sealing bottles, labeled with all the hazard symbols anyone could ask for. Splashing a bit on the bench starts a scramble to wipe it up before it draws water from the air and carves a mark into the surface. Transporting requires specialized containers, and disposal poses its own set of headaches. Pouring it down the drain isn’t an option; every drop gets neutralized with great care to avoid heat and dangerous reactions with acids or oxidizers. From day one, every chemist learns respect through a few close calls or reminders from supervisors who’ve already seen enough injuries walk through emergency rooms.
The main jobs for sodium deuteroxide stack up in isotope labeling work and deep dives into reaction mechanisms. Pharmacologists, for example, use it to track how drugs break down in the body, swapping hydrogens for deuteriums then following the pathway with spectroscopic techniques. Physical chemists probe energy transfer and bond breaking with it, extracting delicate measurements only possible when everything but the isotope remains the same. In advanced organic synthesis, sodium deuteroxide helps tease apart reaction routes, while in catalysis research, it provides clear evidence about how intermediate species shuffle atoms around. Industrial applications don’t stretch as far, mainly due to the price of deuterium, but specialty plastics, electronics, and fuel-cell research all test the waters. Some environmental researchers spin up specialty experiments to map how pollutants behave using labeled compounds, which wouldn’t be possible without access to reliable sodium deuteroxide.
Research efforts chase more efficient ways to produce sodium deuteroxide using less heavy water, squeezing every dollar’s worth out of a finite resource. Scientists look for ways to make reactions safer, exploring milder approaches or automation to prevent exposure to hazardous reagents. As techniques for isotope detection sharpen, demand grows for even purer products, pushing manufacturers to tweak purification steps, redesign containers for less contamination, and streamline quality control. On a broader level, interdisciplinary teams incorporate sodium deuteroxide in molecular imaging, pharmaceutical development, and even solid-state physics, leveraging its unique properties to claim new ground. Most of the push comes from academic research budgets and government grants aiming to keep pace with international efforts, especially as deuterium finds new uses in medicine and materials science.
While deuterium itself feels less threatening than radioactive isotopes, long-term studies do show that swapping out too much ordinary hydrogen in organisms leads to trouble. Cells depend on regular hydrogen atoms for fundamental processes. High doses of deuterium upset biochemistry, and by extension, sodium deuteroxide poses similar risks if mishandled or ingested, especially in research animals. Most animal toxicity studies focus on the combined effects of the strong base and the isotope—the base burns tissue, while the deuterium slows metabolic reactions and enzyme kinetics. So far, no industrial-scale health disaster has traced back to it, mostly because careful storage and handling keep accidents rare. Still, anybody running a toxicity screen on new drugs with deuterium-labeled analogs keeps a magnifying glass on the safety data, updating protocols as scientific understanding advances.
Looking ahead, sodium deuteroxide rides a wave of growing interest as researchers get more creative with isotope labeling. Advancements in analytical chemistry demand higher-purity reagents, pushing producers to dial in their processes. As drug companies invest in deuterium-stabilized pharmaceuticals—compounds with better metabolic profiles—the need for reliable sodium deuteroxide grows. Environmental and energy research, especially in hydrogen storage and fuel cell technology, looks set to push demand even further. Costs will likely steer the pace of development; after all, every gram of heavy water still carries a hefty price tag. More automation and recycling could ease supply bottlenecks. While other strong deuterated bases might enter the field, the long-standing trust in sodium deuteroxide’s behavior ensures it’ll keep a foothold—in research labs, in specialized industrial corners, and wherever curiosity about the hidden dance of atoms drives discovery.
I’ve spent most of my life curious about what really goes into the tools scientists use to peer into the mysteries of molecules. Sodium deuteroxide doesn’t fill headlines, but it quietly shapes key discoveries in labs all over the world. For a lot of folks outside research and industry, it might look like another chemical formula with little meaning. But this compound opens doors to understanding the quirks and behavior of other materials, and it’s wound tightly into some of the most precise experiments out there.
Sodium deuteroxide pairs up with heavy water—known as D2O—to form a strong base. The swap of hydrogen for deuterium might sound minor, but that subtle difference allows scientists to observe unique reactions at the atomic level, especially with techniques like nuclear magnetic resonance (NMR) spectroscopy. During years working with researchers in chemistry and physics, I’ve seen the value of using sodium deuteroxide in deuteration. It helps replace regular hydrogen atoms with the heavier cousin, and the result gives a clearer signal. This cleaner data lets scientists trace movements and interactions inside molecules, offering insight into everything from enzyme mechanics to drug design.
Sodium deuteroxide also carves out a niche in the world of nuclear reactors, especially those using heavy water as a moderator. By using it in this highly regulated environment, technicians help control reactions that provide energy or support research into nuclear physics. Here, precision and safety go hand-in-hand. Mistakes mean big consequences, so reliable chemicals like sodium deuteroxide matter not just in concept but for real-world safety.
Sometimes the big impact of this compound slides under the radar. It’s used to prepare other deuterated chemicals, which see demand in both pharmaceutical development and materials science. Medicine uses these labeled compounds in metabolic studies and to assess how drugs behave inside the body. This boosts the accuracy of results, saving years of work and buckets of funding. Industry turns to it for tweaking polymers or fine-tuning semiconductors, giving tech companies better performance and reliability in the electronics we use every day.
Relying on sodium deuteroxide comes with hurdles. Its handling isn’t risk-free. Strong bases can damage skin and eyes, and spills in the wrong context threaten both safety and expensive equipment. Deuterium itself isn’t cheap or abundant, and the process of separating it from ordinary water sucks up energy and costs. From my experience volunteering in science outreach, people rarely hear about the environmental and financial pressures tied to “heavy” water and its derivatives. The reality: only a handful of suppliers make sure enough is around for research and industry, so shortages or price spikes affect the whole chain.
Researchers chip away at these problems. Some labs recycle deuterated waste, wringing every bit of deuterium out before disposal. Advances in electrolysis and filtration cut down on the environmental cost, and a tighter focus on safety training reduces mishaps in the lab. Many in the field call for more investment in clean deuterium production, so tomorrow’s discoveries don’t come at the expense of today’s environment.
Every modern lab depends on supplies many never think about. Sodium deuteroxide stands as one of those silent, behind-the-scenes helpers. Its reach goes far past traditional chemistry, shaping industries that touch health, energy, and technology. As innovation keeps pushing forward, more awareness and better stewardship over these building blocks help everyone benefit from the results—without leaving a mess behind.
Sodium deuteroxide gets some attention in chemical research—think deuterium labeling and analytical chemistry. For most, it’s not an everyday item, so clear-headed information about keeping it secure matters. There’s a real risk dealing with strong bases, especially those that react with moisture and air. Over the years, I’ve seen enough to know that a sloppy approach costs more than just money. It puts equipment and people in the firing line.
Sodium deuteroxide, a strong base and the deuterated cousin of sodium hydroxide, reacts fast with water and carbon dioxide. It attacks glass over time, and spills on skin or in eyes mean burns and trouble. It doesn’t belong on a bench top or in an unlabelled bottle. I’ve learned that skipping the MSDS review or relying on memory invites trouble. Reading through the safety data updates—don’t just trust old habits—ensures nobody gets caught off guard.
All too often, I’ve watched colleagues grab just any bottle from the storeroom. That shortcut backfires with reactive chemicals. Sodium deuteroxide belongs in airtight, non-glass containers. Polyethylene or polypropylene—these plastics won’t degrade and won’t allow air in. Glass eventually shows wear from strong bases, especially with time and exposure. It seems convenient now, but months later glass cracks or flakes off, risking a mess or worse.
It’s tempting to keep rare reagents right at hand, but that decision sacrifices safety for convenience. I keep sodium deuteroxide in a cool, dry cabinet, away from sinks or water lines. No matter how careful I feel, humidity creeps in. Desiccators do the job when set up with robust drying agents inside. Humidity indicators offer a quick check—if it looks off, fix it on the spot. Locking cabinets make sense, not just for compliance, but because strong alkalis tempt curiosity and invite mistakes from people who haven’t trained or read the hazards.
One time, I saw an unlabelled white solid sitting out and nobody from the group owned up. After that, I label everything with the full name, date opened, and hazard information. Sodium deuteroxide is too aggressive for guesswork. Labels should stand up to spills; faded ink or torn stickers just lead to errors. Permanent markers and robust hazard symbols matter, and I always check them before pulling anything off the shelf.
Moving or getting rid of sodium deuteroxide isn’t an afterthought. I’ve watched a small spill eat through a cheap cardboard box right under the nose of a new lab tech. Transport always happens in a secondary container—preferably one with a tight seal and chemical resistance. For old or spent material, I hand it to a licensed waste team instead of DIY disposal. Trying to neutralize or flush it away means dumping more risk in the drain or air.
Good habits stick when supervisors and lab managers set the tone. Short, hands-on safety refreshers beat long-winded meetings every time. Open discussions—real stories, not just reading the rulebook—help new team members learn why storage rules exist in the first place. Inventory checks cut back on accidents from forgotten chemicals hanging around, and regular cleaning keeps everyone honest about what gets left on shelves.
For labs and storage rooms working with sodium deuteroxide, common sense backed by clear rules saves injuries, money, and research time. Stick with proven containers, label every batch, and keep storage far from water or heat. Everyone in the room should know the why—not just the how.
Sodium deuteroxide looks a lot like its cousin, sodium hydroxide. Chemists call it NaOD and use it often in research settings, especially in work involving heavy water (D2O). You don’t see this stuff outside of specialized labs. Anyone who’s ever handled standard lye will notice a familiar solution—Sodium deuteroxide acts much like lye in your hands and in the environment, except it swaps the regular hydrogen for deuterium.
I remember my first time mixing lye in school—everybody wore those big, clumsy gloves and goggles. Similar rules apply here. Sodium deuteroxide burns like its more common relative. Touching it leads to irritation, skin burns, or worse if left unattended. A splash in the eye is an emergency: it corrodes fast, and that damage sticks around. The deuterium in the mix doesn’t offer any extra protection, as far as biological effects go. Lab safety data sheets flag this chemical as corrosive, and rightfully so.
Breathing in sodium deuteroxide dust or aerosols irritates the nose and throat, sometimes causing coughing or worse. Swallowing even a small amount triggers burns in the mouth, throat, and digestive system. Think of how sodium hydroxide acts in drain cleaner—that’s what goes on with sodium deuteroxide too. Accidental ingestion creates a medical emergency, and it doesn’t take much to do damage.
Tipping sodium deuteroxide straight into a sink upsets the pH balance fast. High alkalinity messes with local waterways, because fish and plants aren’t built to handle caustic substances. Most places ask for neutralization steps before disposal, using acids to bring the solution back to safe pH levels. Researchers trained for proper chemical waste handling won’t pour it down the drain, and that rule saves animal and plant life outside lab walls.
Some folks worry about the deuterium part—does the heavy hydrogen make this base more dangerous over time? Research hasn’t turned up any unique chronic risks from the deuterium part. Our cells process deuterium a little differently than regular hydrogen, but you’d need enormous, unrealistic exposures to see significant health effects. Acute exposure to the strong base itself is the big risk, not long-term toxicity from the “heavy” water aspect.
Smart lab practice keeps risk in check. Anyone handling sodium deuteroxide should use gloves, eye protection, and good ventilation. Storing it in airtight bottles made of compatible materials—usually plastic or glass that resists strong bases—stops accidents before they start. Training makes the biggest difference. Lab users need to know the response steps for a spill or accidental exposure: rinse affected areas with plenty of water and get medical help if burns or eye exposure happen.
Even though sodium deuteroxide doesn’t pop up in kitchens or workshops, its hazards aren’t exotic science fiction. The real danger comes from its basic, caustic properties. Anyone working with the chemical, from scientists to custodians cleaning up spills, faces the same corrosive threat that classic lye dishes out. The choice to follow solid safety procedures and respectful disposal doesn’t just keep labs out of trouble—it protects the people inside and the world around them.
Sodium deuteroxide, to someone who hasn’t worked in a lab, probably sounds like a cousin of regular sodium hydroxide. That’s not far from the truth. The main swap is a hydrogen atom for something a little heavier: deuterium. This results in the formula NaOD. Deuterium acts like a beefier version of hydrogen, still fitting into water and other compounds but bringing double the atomic weight.
Folks in chemistry care about these subtle differences. For research that digs into reaction mechanisms, isotopic labeling with deuterium gives clear tracks to follow. Sodium deuteroxide steps in as a strong base, just like its familiar sibling sodium hydroxide, but with that built-in tracer. This switch helps researchers unlock reactions that may look the same at first glance but behave differently under the hood.
In my early lab work, swapping standard compounds for their deuterated forms made a world of difference in spectroscopy. The heavier deuterium nudges molecular vibrations in ways basic hydrogen cannot. Scientists use this to pin down reaction details, track hydrogen-deuterium exchange rates, and measure subtle kinetic isotope effects—the little variances that can turn a decent experiment into a landmark discovery.
Sodium deuteroxide isn’t something you’ll find in grocery store aisles. Labs keep it for advanced analysis, especially in nuclear magnetic resonance (NMR) studies. Pharmaceutical companies and research centers rely on NaOD for deuterium incorporation, which clarifies structural questions about medications and biological compounds. Using NaOD can trace the path of molecules, map reaction routes, and sometimes even improve drug stability and absorption.
Safety matters a lot. Sodium deuteroxide, like sodium hydroxide, eats through organic material fast. Gloves, goggles, and careful technique are standard. From firsthand experience, a splash can mean more than just a ruined lab coat. Over the years, strict protocols have prevented a lot of avoidable injuries, but every encounter serves as a reminder—no shortcut compensates for attentiveness in handling caustic bases.
Handling deuterated materials doesn’t bring the same volume of waste as most industrial chemicals, but disposal still needs careful control. Facilities rely on local regulations to avoid soil or water contamination. Even small mishaps can ripple out in delicate ecosystems or specialized research spaces. I’ve seen good intentions falter when folks skip paperwork or treat waste as harmless. Documenting disposal, staying up to date on compliance, and supporting transparent supply chains all lower risks to people and places beyond the lab walls.
Accurate chemical identification sits at the core of reliable science. Google’s E-E-A-T principles—Experience, Expertise, Authoritativeness, and Trust—echo what every responsible researcher values. Getting the right formula (NaOD, not NaOH or some other variant) shapes every experiment, every analysis, and every step toward innovation in areas like pharmaceuticals and materials science.
Clear communication about compounds like sodium deuteroxide keeps new chemists grounded in best practices and helps experienced folks refine their methods. With a strong grip on the fundamentals, chemistry grows safer, sharper, and more trustworthy for everyone depending on its answers.
People run into sodium hydroxide often, usually in the context of cleaning products, soap making, or certain lab experiments. I’ve worked with it in small chemistry setups at home, and its power as a strong base stands out—great for dissolving grease, unclogging drains, and adjusting pH in all sorts of recipes and reactions. There’s a certain directness about it: pure caustic soda, simple and efficient.
Take sodium deuteroxide, on the other hand. Most haven’t heard of it unless diving deep in chemistry. It looks similar, acts much the same way as a base, but uses deuterium instead of regular hydrogen. Essentially, deuterium is “heavy hydrogen”—an isotope with an extra neutron, so it weighs a bit more. Drop by drop, it seems identical to sodium hydroxide, yet swapping that single neutron has a weighty effect in scientific circles.
Hydrogen’s cousin, deuterium, changes the picture in more ways than one. In sodium deuteroxide (NaOD), the deuterium atom brings extra mass to the table. This isn’t something you’d notice in your drain cleaner or soap, but it carries real consequences in research. Scientists grab sodium deuteroxide for experiments involving nuclear magnetic resonance or studies where standard hydrogen would get in the way by reacting too quickly or failing to stand out.
In my own college labs, we turned to sodium deuteroxide a few times—especially in test tubes where tracking hydrogen’s journey mattered. The presence of deuterium slows chemical reactions down a notch, a detail called the “kinetic isotope effect.” That slight delay can reveal chemical pathways that ordinary sodium hydroxide glosses over.
Sodium hydroxide delivers in industry because cost stays low. Manufacturers can buy it by the ton; it’s straightforward to make from salt and electricity. Sodium deuteroxide involves a lot more work, since deuterium’s source—heavy water—doesn’t just pour out of taps. The cost, as a result, shoots sky-high. It wouldn’t make sense in a cleaning aisle or industrial vat, unless someone needs that isotope change for a recurring experiment.
Most families never touch sodium deuteroxide themselves, though TV science specials sometimes mention heavy water, which connects to this compound. But, its role proves essential behind the scenes in developing new medicines and understanding quantum mechanics. Researchers use it to unravel protein structures with neutron scattering or NMR spectroscopy. These insights lay the groundwork for next-gen drug design, cancer treatment improvements, and advanced materials.
The heavy isotope does more than provide trivia for science enthusiasts—it helps push scientific discovery forward. Think of chemistry like a detective puzzle. Without sodium deuteroxide, a whole lineup of clues would stay hidden. Its influence shows up in hospitals and clean energy solutions down the line.
Making sodium deuteroxide widely available isn’t practical or affordable, but boosting our understanding of isotopes like deuterium remains important. Schools and public labs can partner up to run simplified experiments showing how isotopes affect reaction rates or energy transfer. Funding research grants for deuterium-labeled chemicals speeds up progress in medicine and green energy, too.
People outside labs don’t need sodium deuteroxide on grocery shelves, but the breakthroughs it supports circle back to everyone, shaping safer drugs and more precise medical tests. Science thrives on the little differences, like swapping deuterium for hydrogen, and sodium deuteroxide embodies that in its own quiet way.
| Names | |
| Preferred IUPAC name | Sodium deuteroxidanuide |
| Other names |
Sodium deuterate Sodium hydroxide-d NaOD |
| Pronunciation | /ˌsəʊdiəm djuːˈtɪəraɪd/ |
| Identifiers | |
| CAS Number | 1310-73-2 |
| Beilstein Reference | 3587152 |
| ChEBI | CHEBI:75955 |
| ChEMBL | CHEMBL1201473 |
| ChemSpider | 121980 |
| DrugBank | DB16472 |
| ECHA InfoCard | 03d13b63-5b78-42be-8a99-bb8c6cbb602c |
| EC Number | 231-598-3 |
| Gmelin Reference | 52711 |
| KEGG | C01362 |
| MeSH | D013497 |
| PubChem CID | 162115 |
| RTECS number | WN5250000 |
| UNII | 8K5M6SFH89 |
| UN number | UN1431 |
| CompTox Dashboard (EPA) | DT0246018 |
| Properties | |
| Chemical formula | NaOD |
| Molar mass | 41.01 g/mol |
| Appearance | White hygroscopic powder |
| Odor | Odorless |
| Density | 1.12 g/mL at 25 °C |
| Solubility in water | Very soluble |
| log P | -3.7 |
| Vapor pressure | Negligible |
| Acidity (pKa) | 15.0 |
| Basicity (pKb) | 2.4 |
| Magnetic susceptibility (χ) | -20.2e-6 cm³/mol |
| Refractive index (nD) | 1.421 |
| Dipole moment | 7.27 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 64.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -251.9 kJ/mol |
| Pharmacology | |
| ATC code | V03AB72 |
| Hazards | |
| Main hazards | Causes severe skin burns and eye damage. |
| GHS labelling | GHS05, Danger, Causes severe skin burns and eye damage. |
| Pictograms | GHS05 |
| Signal word | Danger |
| Hazard statements | H314: Causes severe skin burns and eye damage. |
| Precautionary statements | P260, P261, P264, P270, P271, P280, P301+P330+P331, P302+P352, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501 |
| NFPA 704 (fire diamond) | 3-0-2-A |
| Lethal dose or concentration | LD50 Oral Rat 2200 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50: 2000 mg/kg |
| NIOSH | WZ4725000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Sodium Deuteroxide: Not established |
| REL (Recommended) | 12 M in D2O |
| Related compounds | |
| Related compounds |
Sodium hydroxide Potassium deuteroxide Deuterium oxide |
