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Chemistry grows layer by layer, and 1,10-Phenanthroline tells a story with real depth. Born out of curiosity for nitrogen heterocycles in the late 1800s, this compound landed in the spotlight when scientists searched for molecules capable of binding metal ions. Werner’s groundbreaking coordination chemistry drew 1,10-Phenanthroline out of dusty bottles and into real-world experiments. Generations of researchers mapped this molecule’s potential, noting its knack for forming stable complexes with transition metals. By the middle of the twentieth century, analytical chemists began trusting this ligand as a mainstay in detecting and measuring metals in everything from ores to blood samples. Over time, the crystal-clear results it offered shaped entire textbooks, leading to widespread applications across laboratories and industries.
Most chemists recognize 1,10-Phenanthroline hydrate as a staple reagent, appearing as a slightly off-white or pale yellow powder. The hydrate form, which contains one water molecule per formula unit, improves ease of handling by stabilizing the compound during storage. Sold by reputable suppliers worldwide, this material stands out as more than just another chemical on the shelf. Its ability to grab onto metal ions creates a foundation for quantitative analyses and helps researchers unravel the mysteries within solutions that would remain otherwise obscure to the naked eye. The molecule’s legacy lives in its versatility and reliability—a direct result of nearly a century of hands-on use and relentless refinement.
Holding a small vial of 1,10-Phenanthroline hydrate, you notice the solid tends to cake under normal room conditions, a consequence of the embedded water. Its melting point floats in the mid-80s Celsius, but dehydration or prolonged heating changes that swiftly. Solubility in water is moderate, and it goes into solution more easily with certain organic solvents, making it accessible for various experiments. The compound’s planar aromatic structure loads the molecule with stability and a distinct odor, and the chelating nitrogen atoms form robust bonds with copper, iron, and other ions. Its chemical signature means it resists breakdown under standard bench conditions, allowing generations of scientists to trust it as a reliable ligand for both qualitative and quantitative work.
Lab vials labeled “1,10-Phenanthroline hydrate” often come with a purity rating above 99% for analytical grade, signaling that rigorous purification has minimized the presence of impurities or by-products. Enlightened labeling empowers users, spelling out warnings about moisture sensitivity or recommended storage in sealed containers, away from harsh light or heat. These specifications urge careful weighing and storage, as excess water content can throw off the delicate stoichiometry in sensitive reactions. Matching the lot number to batch-specific certificates of analysis brings peace of mind for every careful technician or researcher who needs repeatable outcomes in analytical chemistry or synthesis.
The fundamental approach for preparing 1,10-Phenanthroline involves starting from starting materials like o-phenylenediamine and glyoxal. Through controlled condensation and subsequent purification steps, this yields the core heterocycle. To ensure high-quality product, manufacturers add a carefully measured step—hydration—introducing a specific water content that boosts stability and simplifies transport. Plenty of chemistry students have tried homegrown versions of such syntheses in university labs, but quality and reproducibility require industrial controls. Crystallization, filtration, washing, and drying stand as pillars in refining the substance for research, each step tweaking the yield and purity with skill acquired from decades of trial and error.
It’s no overstatement to say 1,10-Phenanthroline changes the game in inorganic and analytical chemistry labs. The molecule, with its two nitrogen donors, bites onto metals like copper, iron, nickel, and zinc, wrapping around them and forming highly colored complexes. This property gives it a starring role in colorimetric assays. Redox reactions involving 1,10-Phenanthroline push the limits of detection in environmental and clinical samples—think of the orange-red copper complex churning through endless test tubes. On the modification side, researchers tinker with substitutions on the aromatic rings to tailor selectivity for different metal ions or adjust solubility, unlocking specialized uses in catalysis and sensing. Through derivatization, chemists expand its reach, crafting ligands customized for new challenges.
The world of chemistry overflows with synonyms, and 1,10-Phenanthroline is no exception. Ask an older chemist and you might hear “Phen” or “o-Phenanthroline” pass their lips, hinting at a long history with this versatile chelating agent. Scientific literature sometimes shortens it to “Phen” or plugs alternative spellings like “orthophenanthroline.” Catalogs for scientific supplies list variant names, but beneath it all, each name points back to the same rugged, nitrogen-laden molecule that shapes the work of countless researchers across fields ranging from analytical chemistry to catalysis and materials science.
Safety concerns in today’s chemical landscape carry real and weighty consequences. Direct contact with 1,10-Phenanthroline can irritate skin and eyes, and inhalation of dust calls for concern. Laboratories stock safety data sheets and advise working with gloves, goggles, and dust masks. Spills require a cautious approach—sweep up with minimal dust generation, dispose of contents by established protocols. Consistent training and clear signage reduce accidental exposures. Modern standards lean on principles like green chemistry and waste minimization, pushing for safe disposal and substitution with less hazardous ligands in non-essential uses without sacrificing research integrity. Companies and regulatory bodies focus on constant updates to operational guidelines so every handler understands the risks and acts accordingly.
For anyone who’s measured iron in water samples, 1,10-Phenanthroline means the promise of specificity and reliable results. Environmental chemists detect trace metals in rivers, giving communities a heads-up on contamination. Clinical laboratories measure metal content in blood, finding clues for diagnoses. Walk into an industrial QC department and you’ll find 1,10-Phenanthroline at the heart of copper or nickel assessments critical to electronics and metallurgy. The molecule’s role extends into academic research—aiding mechanistic studies in coordination chemistry and powering biomimetic catalysts. Its colorful complexes light up assay tubes and microplates, translating chemistry into simple visual cues that inform real-world decisions, from public health to mineral processing.
Research doesn’t rest, and neither does the need for finely tuned analytical tools. Current directions with 1,10-Phenanthroline hydrate push boundaries in sensor development—researchers embed the molecule in polymers, design test strips, and link it to nanomaterials, aiming for portable metal detection that fits in your pocket. Chemists hunt for new derivatives, experimenting with ring modifications to boost selectivity and decrease background noise in complex matrices. In catalysis, the compound partners with transition metals to drive efficient organic transformations, helping industry cut costs and emissions. Academic conferences buzz with talks on new analytical protocols, while interdisciplinary teams apply this familiar ligand to problems in materials science, electrochemistry, and beyond.
Questions about toxicity never fade in chemical research. Animal exposure studies and toxicity screens for 1,10-Phenanthroline hydrate reveal risks tied to high doses, particularly with oral or parenteral administration. Acute exposure produces neurotoxic symptoms and disrupts normal cellular function, though the material’s danger decreases under careful lab handling. Environmental impact studies point to the compound’s moderate persistence but limited bioaccumulation, guiding prudent disposal practices. Data collection continues as researchers balance the clear scientific benefits against potential ecological consequences. The drive for safer analytical reagents stands strong, pushing ongoing efforts to routinely reevaluate and minimize risks where feasible.
Looking forward, it’s hard to ignore 1,10-Phenanthroline’s resilience amid changes in analytical science. Digital detection, miniaturization, and push-button chemistry demand ligands that won’t let scientists down. Innovations in green chemistry beg for alternatives, yet few substances surpass the accuracy or versatility of classic phenanthroline complexes in metal determination. Growth in tandem assay formats, sensor integration, and cheap portable diagnostics rests partly on this molecule’s shoulders. Industry and academia keep a close eye on new derivatives that retain analytical muscle but lower toxicity and footprint. The next generation of chemists will likely carry 1,10-Phenanthroline’s spirit into unknown applications, guided by deep-rooted trust born from experience and countless reliable results.
I remember walking into a lab in college and seeing all these glass vials filled with names I could barely pronounce. On one shelf, a small bottle labeled “1,10-Phenanthroline Hydrate” kept popping up during experiments that involved metals. I quickly learned that this compound packs a serious punch when it comes to helping chemists measure, detect, and study metal ions. Simply put, it's a chemical that helps us see what often stays hidden.
The real magic of 1,10-Phenanthroline Hydrate shows up in analysis. Scientists use this compound as a ligand, which means it grabs onto certain metals, especially iron. In practice, it forms a striking red-orange complex with Fe(II), which catches the eye and gives a straightforward way to measure iron in water, food, and biological samples. If you’ve ever checked a water sample for iron and got a color change, there’s a good chance this chemical helped make it happen. At this point, I’ve used it more times than I can count for basic colorimetric tests—a classic method for anyone who works in environmental science or biochemistry labs.
Iron keeps the world running. This element pops up in everything from blood to building infrastructure. The ability to find and measure iron accurately can keep drinking water safe, help farmers know if soil holds enough nutrients, and give hospitals the information they need for treating patients. Contaminated water from old pipes, for example, often brings iron along for the ride, turning water rusty and sometimes unsafe. Without a cheap and reliable tool, you’re guessing what's actually in that water. 1,10-Phenanthroline Hydrate plays its part by making the unseen visible—a foundation for good science and public safety.
While its strongest handshake comes with iron, 1,10-Phenanthroline Hydrate doesn’t limit itself there. Nickel, copper, and several other metals also respond to its presence. Just last year, I ran a few tests tracking nickel in water runoff, using this compound to create a colored complex easy to spot under laboratory lights. Researchers reach for it when they want accurate readings without fussing with more expensive, complicated instruments.
University chemistry classes keep 1,10-Phenanthroline Hydrate on hand because it teaches some basic but crucial lessons. New students get immediate visual proof that chemical bonds matter, and they see that analytical chemistry relies as much on simple observation as on high-tech methods. At a time when science education often faces budget cuts, affordable, reliable reagents matter more than ever. A bottle of this stuff costs just a few dollars and delivers a whole curriculum’s worth of teaching moments.
Industry and research continue to search for even more sensitive, less toxic ways to analyze metals, but the classics keep a strong foothold. Making chemical detection safer and simpler remains a challenge worth tackling. Green chemistry approaches push for substitutes with fewer hazards, but few can match the simplicity and reliability I’ve seen from 1,10-Phenanthroline Hydrate.
I’ve watched colleagues try to invent around it, but this compound hangs on for good reason. Whether helping protect public health or teaching the next wave of scientists, its impact reaches far beyond the laboratory shelf.
1,10-Phenanthroline shows up a lot in chemistry labs. Anyone who spent hours in an undergraduate wet lab probably met it during titrations or learned about the striking colors it brings out when mixed with metals. The formula for the pure compound—1,10-phenanthroline itself—stands as C12H8N2. Once a single molecule of water nestles in, it becomes the hydrate we talk about in storerooms and in experimental procedures: C12H8N2·H2O. That single dot makes a difference, turning a basic raw ingredient into something precise and reliable for chemical reactions.
Knowing exact formulas avoids guesswork. Old-school chemists didn’t always have up-to-date stockroom lists, but precision keeps research reproducible. Anyone preparing a solution for titration needs the hydrate’s formula in order to get a true concentration. Most commercial bottles of phenanthroline list the hydrate instead of the anhydrous version. It saves headaches and confusion, especially for younger chemists eager to make things work the first time.
Curiosity about the numbers is more than just a habit. For 1,10-phenanthroline monohydrate, the calculation stacks up like this:
Tallying everything up, the molecular weight comes out close to 198.21 g/mol. Sometimes, you’ll see labels rounded to 198.2 g/mol, or up to 198.22 g/mol depending on whose periodic table you checked in college. Accuracy matters for molarity and dosing. Cutting corners on numbers for 1,10-phenanthroline hydrate ripples into experiments, giving unreliable readings in something as routine as an iron analysis.
Chemical details show up in real work. In my own college years, a small error in weighing out phenanthroline hydrate cascaded into hours of troubleshooting poor endpoints in colorimetric titrations. These compounds act as ligands, binding to metals and forming complexes that change color. Iron determination often uses phenanthroline hydrate for its clear orange-red complex, making it easy to see how much iron you’ve got, even in city water samples. Any misstep in formula or weight, and all the data from those water quality tests can lose their value.
Research, quality control, and teaching students all demand attention to the small print—especially with hydrates. Knowing the right formula and molecular weight for 1,10-phenanthroline hydrate prevents wasted resources and guides experimenters toward results they can trust. Reliable sources like Sigma-Aldrich, PubChem, and peer-reviewed chemistry handbooks agree on these details for a reason: reproducibility anchors science, even if it takes a little extra effort with the calculator up front. Taking time to check your math and verify your chemicals pays off with solid findings at the end of the day.
Anyone who spends time in a lab knows the headache that comes with ruined chemicals. All those plans, hours of prep, and then finding out a reagent’s turned useless. 1,10-Phenanthroline hydrate has this way of picking up moisture and reacting with air—little habits that demand respect both from beginners and seasoned researchers.
Water likes to sneak in wherever it can. Storing this compound in a damp place can turn a precise tool for complexometric titrations into a useless lump. A colleague once told me about a batch reduced to clumps over a soggy weekend in July—he swore by investing in decent desiccators after that. Dry conditions let you return to the bottle weeks later with full confidence.
Direct sunlight doesn’t just warm things up. Light can start unwanted chemical changes in many laboratory compounds, and phenanthroline is no exception. It’s tempting to stack bottles near a window for easy access, but chemical stability trumps convenience every time. Amber bottles make a difference, blocking UV and reducing the risk of degradation. Simple steps like this save both money and time—nobody wants a ruined titration halfway through.
Lab air isn’t as clean as we think, especially when people open the door every few minutes. Oxygen does more harm than most expect, especially over long weekends. Tightly sealed containers keep unwanted reactions in check. My habit: after every use, clean the bottle’s rim and close the cap tight. Even short lapses add up, and the difference between a reliable chemical and guesswork stems from these small actions.
Mix-ups in storage lead to unnecessary mistakes. An unlabeled jar can cause confusion and set back a day’s work. Clear, durable labels help everyone avoid misunderstandings. I’ve seen teams spend hours tracing an error back to swapped bottles. Keep the original packaging when possible—manufacturers’ instructions carry real value, including batch information and safety data. It’s a small effort for better traceability.
The regulatory landscape for chemicals tightens every few years. Following strict storage protocols protects not just research results, but also the health of anyone walking into the lab. Spills or accidental exposure bring more than lost chemicals—they can trigger inspections, fines, or worse. Flammable cabinets, secondary containment, and controlled access don’t just tick boxes. These practices prevent accidents and protect reputations.
A reliable home for 1,10-Phenanthroline hydrate starts with a low-humidity cabinet, preferably a desiccator, away from heat and light. Use tightly sealed amber glass bottles. Check labels and expiry dates during regular inventory. Train every lab member to recognize deteriorated material—if it looks clumped, discolored, or unusual, it usually means trouble. Dispose of questionable stock safely rather than risking unpredictable results.
Storing 1,10-Phenanthroline hydrate with care brings hidden rewards. Consistency in these habits shields valuable experiments from setbacks and prevents waste. Labs that enforce smart organization see fewer mistakes, lower costs, and safer environments. A chemical’s value lies not just in its purity but in the respect with which it’s handled every day.
Chemicals make modern life possible, but they can also raise tough questions about health and safety. University chemistry labs, industrial plants, and even classrooms see bottles labeled with names most folks have never pronounced out loud. Among these sits 1,10-Phenanthroline Hydrate—a name long enough to make anyone pause. To the average person, it looks pretty obscure, but for researchers, students, and workers in manufacturing, this compound comes up during analytical tests.
1,10-Phenanthroline Hydrate works best in the lab as a chelating agent—helping measure and separate metals. The fact that it reacts with certain ions makes it valuable for detecting iron or copper. That kind of chemistry matters in water quality testing and environmental monitoring. But every positive has a flip side, and safety never takes a vacation in the lab.
According to the European Chemicals Agency, this hydrate is marked with an exclamation mark pictogram: it irritates eyes, skin, and the respiratory system. Swallowing or inhaling it brings risks, including burning sensations in the mouth and throat. A single splash can leave you with a nasty red rash. Stories swirl in academic circles about students accidentally spilling reagents and suffering chemical burns or allergic reactions.
The toxicity of 1,10-Phenanthroline Hydrate doesn't only revolve around a quick spill or sniff. There’s evidence that animal exposure to large amounts can damage organs. Laboratory accidents rarely make headlines, yet mishandling chemicals sometimes ends with permanent injuries. Acute oral LD50 tests in rodents show enough toxicity that people should keep a close eye on safety data sheets. Add some reports of possible aquatic toxicity, and it’s clear: this isn’t a harmless white powder.
Back in graduate school, I ran across this chemical during trace metal analysis. After hours in a dusty, crowded lab, that strange, metallic-smelling powder always got treated with respect. Gloves and goggles became second nature—not just because professors said so, but because small mistakes brought big consequences. A classmate once handled an unlabeled vial only to find out the hard way she’d picked up 1,10-Phenanthroline Hydrate. Her inflamed skin told the story better than any data sheet. That experience taught me to approach every unfamiliar label with caution.
Safety doesn't come from warning labels alone; it grows from real habits. Reading the datasheet before use should never feel like a chore. Proper storage—away from incompatible substances, tightly sealed—matters just as much as wearing gloves. Laboratories that train people to respect every bottle—regardless of how common or exotic the name—cut down on accidents. Waste management must get equal attention, since careless disposal can leak toxins into water systems and harm wildlife.
Ultimately, no one expects every person to memorize every chemical hazard. Still, learning to ask questions, using protective gear, and knowing the risks behind each bottle offer better protection than luck. Science thrives where people look out for each other and take informed risks instead of reckless ones.
1,10-Phenanthroline hydrate gets plenty of use in labs, especially for detecting metal ions like iron using simple color tests. Before even thinking about measuring out chemicals, it helps to know this is an organic ligand. It comes as an off-white or yellow powder, and the hydrate version carries a little water within its structure—important, because that changes its true weight and affects the precision needed for reliable results.
Start by checking that you have a reliable balance. Accuracy matters here because small measurement errors throw off the solution strength. Make sure you’ve got distilled or deionized water on hand. Tap water introduces minerals and odd ions that ruin clean solutions. A clean glass beaker will serve well, and a glass rod or magnetic stirrer helps get the powder dissolved fully. Gloves and goggles keep you safe because the powder irritates skin and eyes.
Water in the hydrate can trip up those who are used to working with anhydrous powders. Always check the label for the exact hydrate version. Lab books spell out that 1,10-phenanthroline monohydrate, for example, weighs more than the pure "anhydrous" chemical. To make 100 mL of a 0.1% solution, you’ll be weighing out 0.1 grams for that 100 mL mark. It helps to zero the weighing vessel on the balance, then slowly tap in the powder, avoiding static or wind drafts by keeping movements calm and steady.
Pour about 80 mL of your clean water into the beaker first—don’t fill up to the line yet. Sprinkle your powder right onto the water, then stir gently with your rod. 1,10-Phenanthroline doesn’t always dissolve right away. Sometimes warming the beaker in a water bath speeds things along, but too much heat brings risks if you’re not watching. Once the solution turns clear, top it up with water to reach the 100 mL mark. Swirl it gently to avoid splashing excess powder on the side walls.
Light and air change the chemical over time, so pour your finished solution into a dark bottle. Some people use amber glass or wrap clear bottles with aluminum foil. Label the bottle with the concentration, date, and your initials. Refrigerating extends shelf life, but any cloudiness or odd smells warn that you should mix a fresh batch.
Some folks find the solution stubbornly cloudy. That points to undissolved bits or impurities in the water or powder. If this happens, try filtering through a paper filter, or source fresher reagent and purer water. Simple cleaning of all glassware pays dividends in avoiding contamination. I’ve seen entire experiments go off track from careless rinsing or residual soap.
Waste solution doesn’t belong in the sink. Collect unused solution in a marked waste container and contact your institution’s safety officer about proper disposal. With personal awareness and a sharp eye for detail, preparing 1,10-Phenanthroline hydrate solution becomes routine. Getting the basics right means accurate experiments and clean data—fundamentals that everyone learns in their first proper chemistry class.
| Names | |
| Preferred IUPAC name | Phenanthrene-1,10-diamine monohydrate |
| Other names |
1,10-Phenanthroline monohydrate o-Phenanthroline hydrate |
| Pronunciation | /waɪl.tɛn fɪˈnænθrəˌliːn ˈhaɪ.dreɪt/ |
| Identifiers | |
| CAS Number | 5144-89-8 |
| Beilstein Reference | 391420 |
| ChEBI | CHEBI:28598 |
| ChEMBL | CHEMBL4220765 |
| ChemSpider | 10321428 |
| DrugBank | DB13383 |
| ECHA InfoCard | 03b5f3b0-2f3a-40e5-9814-7c2f29272c9e |
| EC Number | 200-629-2 |
| Gmelin Reference | 181580 |
| KEGG | C06535 |
| MeSH | D010623 |
| PubChem CID | 68011 |
| RTECS number | SF7875000 |
| UNII | E251U4Y6PL |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C12H8N2·H2O |
| Molar mass | 198.22 g/mol |
| Appearance | White to yellow crystals or powder |
| Odor | Odorless |
| Density | 1.3 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -0.93 |
| Acidity (pKa) | 5.04 (conjugate acid) |
| Basicity (pKb) | -4.9 |
| Magnetic susceptibility (χ) | -53.0e-6 cm³/mol |
| Refractive index (nD) | 1.658 |
| Viscosity | Viscous liquid |
| Dipole moment | 2.61 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 198.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -54.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3497 kJ/mol |
| Hazards | |
| Main hazards | Causes skin irritation. Causes serious eye irritation. Harmful if swallowed. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302 + H312 + H332: Harmful if swallowed, in contact with skin or if inhaled. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 2-1-1 |
| Flash point | > 199.6°C |
| Lethal dose or concentration | LD₅₀ Oral Rat 1320 mg/kg |
| LD50 (median dose) | Oral rat LD50: 1320 mg/kg |
| NIOSH | SN4550000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 mg/m³ |
| Related compounds | |
| Related compounds |
1,10-Phenanthroline Bathophenanthroline Phenanthroline Neocuproine |
