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Back in the late nineteenth century, chemists were often driven by curiosity over what happened when you fiddled with combinations of carbon, hydrogen, and other elements lying around in their collection of glass flasks. Phenylboronic acid first showed up in chemical literature after German chemist Wilhelm Schall described boronic acids using phenyl groups in the 1860s. Before the age of DNA sequencing and high-speed analytics, these compounds attracted attention for their sticky connection to sugars. Over decades, researchers pieced together its structure and forged new routes to make it more accessible in the lab. The rise of organoboron chemistry through the twentieth century, especially after the Suzuki coupling discovery in the 1970s, transformed phenylboronic acid from an academic curiosity to a staple building block for modern chemistry.
If you spend any amount of time in chemical manufacturing or synthetic laboratories, phenylboronic acid stands out for its versatility. It forms part of a family of boronic acids where a phenyl group attaches to a boron atom. This compound’s balanced reactivity lets chemists link carbon atoms together, fusing complex molecules for pharmaceuticals, electronic materials, and polymers. It has become a must-have for anyone working in cross-coupling reactions or sugar sensing applications. Whether packed in glass bottles or larger containers, it usually takes the form of a powder or crystalline solid that's easy to store compared to more reactive chemical cousins.
Phenylboronic acid typically looks like white or off-white crystals, sometimes clumping up if moisture gets in. It melts between 216°C and 220°C. Boronic acids show off their ability to interact with diols; specifically, phenylboronic acid binds with sugars through reversible covalent bonds. This chemical doesn’t dissolve much in water, which helps in separation processes, though it mixes freely in something like ethanol or dimethyl sulfoxide. Its boron-oxygen bonds give it some acidity, but its benzene ring can alter electronic effects in reactions. That balance between water resistance and reactivity forms a foundation for its everyday use in synthesis.
Every bottle of phenylboronic acid from a reputable supplier carries information like purity, lot number, and manufacturing date. Specifications call for high purity—usually at least 97%—with quantitative assays backing that up. Impurities, especially those affecting boron content or ring integrity, come under close monitoring. Labels must also cover the chemical’s molecular weight, which sits at about 121.93 g/mol, and CAS number—98-80-6—so buyers know what they’re dealing with. Storage guidelines call for tight lids and cool, dry shelves, staying away from acids, bases, or oxidizers that could ignite unwanted chemistry.
Phenylboronic acid does not make itself. Chemists usually build it by reacting phenylmagnesium bromide (from benzene) with trimethyl borate, followed by acidification. This old-school Grignard approach remains popular for its efficiency and broad compatibility. Other routes use direct borylation, where benzene meets boron reagents under catalytic conditions—these methods sidestep metal halides and cut down on waste. In the last few years, more sustainable processes swap out harsh solvents to lower the environmental toll. The exact tweaks sometimes depend on whether the end use sits in the lab or a plant churning out tons per month.
Ask a synthetic chemist about Suzuki-Miyaura coupling, and their eyes light up. Phenylboronic acid plays the starring role by providing the phenyl group to hook onto another aromatic ring in the presence of a palladium catalyst. This single reaction fuels the construction of biaryl structures essential for drug molecules, OLED displays, and crop protection chemicals. Beyond cross-coupling, phenylboronic acid’s affinity for diols means you find it acting as a sensor for glucose or—on a larger scale—modifying polymers to respond to sugar content. Newer research leverages its structure to produce boronate esters, linkers in molecular recognition, or even frameworks for selective drug delivery.
If you dig through catalogs, you’ll see phenylboronic acid called benzene boronic acid, phenylboronate, or even Benzeneboronic acid. The molecular structure—C6H5B(OH)2—leaves little confusion, though some suppliers brand it under in-house trademarks targeting pharmaceutical or materials labs. Chemists turn to it as a foundation for more complex boronic derivatives or use it straight for rapid prototyping in research settings.
Like many organic boronic acids, phenylboronic acid asks for safe handling but does not present the extreme hazards of volatile solvents or strong acids. Avoid breathing in dust or letting it contact your skin. Safety data sheets emphasize gloves, goggles, good ventilation, and dust control. Though not highly flammable or toxic, it needs storage away from moisture and incompatible chemicals. Disposal follows established hazardous waste guidelines, so workers never have to cut corners or risk local water supplies. Training and routine risk assessments build better lab habits for everyone using it by the kilo or milligram.
This compound forms a backbone for countless transformations. Drug makers use it to stitch intricate molecular frameworks in antihypertensives, anticancer agents, and anti-infectives. Diagnostics companies rely on boronic acids to craft glucose sensors, which translate sugar binding into electrical signals for blood monitoring strips. Material scientists feed it into cross-coupling reactions to produce organic electronics, light-emitting diodes, and advanced polymers that blend flexibility, conductivity, and selective recognition. Academic labs champion its value as a teaching tool, reinforcing lessons on reactivity and selectivity for new chemists.
Ongoing R&D circles around more sustainable synthesis and safer derivatives with targeted reactivity or biological compatibility. Analytical chemists dig deeper into its reactivity with cell-surface sugars for cancer detection and drug delivery. Some groups develop solid-supported phenylboronic acid to simplify purification or automate flow chemistry. Innovations in catalysis let researchers couple unactivated arenes or fine-tune electronic properties using para- or meta-substituted versions. These advances filter downstream, showing up in medicine and technology not long after the first reports in scientific journals.
Decades of work detail phenylboronic acid’s profile in cell cultures, animals, and aquatic environments. Acute exposure causes mild irritation—redness, sneezing, slight coughing—less severe than many laboratory chemicals. It doesn’t pile up in tissues or show high bioaccumulation. Regulatory agencies review animal studies before approving it for industrial or diagnostic processes. There’s ongoing watchfulness over breakdown products, as boron-containing residues sometimes pose aquatic risks. Routine audits of manufacturing sites keep emissions and exposures well under available threshold values.
New applications for phenylboronic acid keep emerging. Chemists now investigate boronic acid-based drugs able to recognize and block enzymes with pinpoint accuracy, offering treatments for cancer and metabolic disease. Sensor technologists harness its sugar-binding properties to develop wearable glucose monitors, moving beyond fingerpricks toward noninvasive, real-time tracking. Material developers see value in embedding phenylboronic structures into polymers for environmental sensors or “smart” adhesives that can be turned on and off by simple sugar solutions. Creative growth in methods for greener synthesis reduces both cost and waste, supporting large-scale production where regulatory scrutiny only grows tighter. As industries look for high-value molecules combining safety, selectivity, and flexibility, researchers and manufacturers will find themselves working with phenylboronic acid even more in the years ahead.
Phenylboronic acid might not pop up at the dinner table, but it turns more wheels behind the scenes than you might think. I’ve seen its name over and over again flipping through organic chemistry papers and working alongside research buddies at the lab bench. Chemists lean on it for a simple reason: it acts as a solid foundation in experiments that join molecules together, especially through Suzuki coupling. This reaction builds everything from medicines to materials for electronics.
The reason Suzuki coupling matters is because making new carbon bonds remains the bread and butter of drug discovery. Sometimes the easiest-looking chemical isn’t so easy to make. Phenylboronic acid, with its boron at the core, lets chemists swap atoms around and stick things together that otherwise stay stubbornly apart. Harvard and top pharma labs keep their shelves stocked for synthesizing cancer drugs or designing new antibiotics. Looking back through scientific literature, most blockbuster small-molecule drugs touch on chemistry that starts with or passes through reagents like this one.
There’s another side I find fascinating: phenylboronic acid can sense sugars, such as glucose or fructose. In diagnostics, this comes in handy for monitoring blood sugar. Some blood glucose sensors, which help people manage diabetes, use this chemical’s sweet tooth for sugars. It binds sugars and changes its electronic state—a property smart engineers built right into sensors. Whether you’re a patient with diabetes or the nurse running a clinic, accuracy and real-time results can change the rhythm of daily life.
What surprises many is how much this chemical touches our lives through industry. Polymer scientists use it to tweak water-loving materials called hydrogels. In wound dressings or tissue engineering, these gels bind with sugars and stick to wet tissues better. Medical device designers want phenylboronic acid for those sticky benefits. My friend in biotech once showed me hydrogel contact lenses made possible because of this chemistry—they remained soft and comfortable over long hours because of the way these molecules interact with the eye’s natural mucins.
Everything that helps advance technology or medicine deserves a look at safety. Phenylboronic acid isn’t a household toxin, but people handling it in bulk take precautions. The chemical can irritate skin and eyes. In my own experiments, gloves and goggles stood between me and irritation. Environmental checks ensure it doesn’t roll out into rivers or soil. Factory waste management plans need to include ways to treat or recycle leftover chemicals. Public trust grows when industry leaders talk plainly about these steps and back them up with audits. Proactive planning and transparency matter as much as performance in the marketplace.
There’s clear demand for versions that work even better or offer new reactions. Synthetic chemists keep adjusting its structure, trying to make future drugs safer or diagnostic strips faster. As someone who likes to tinker, I see big value in collaborating across borders—sharing blueprints and data speeds up the next big breakthroughs. With deeper partnerships between scientists and regulators, we can solve both safety and innovation puzzles together, and bring better solutions to the people who need them most.
Phenylboronic acid shows up in all sorts of research settings and chemical manufacturing. At its core, it’s a compound that consists of a benzene ring attached to a boronic acid group. The chemical formula for phenylboronic acid is C6H5B(OH)2. What does that break down to? You’ve got a benzene ring (C6H5—think six carbons arranged in a hexagon, with five hydrogens added on), and it’s linked to a boron atom with two hydroxyl (OH) groups attached. That simple arrangement gives the compound some unique properties that researchers and industry folks can’t ignore.
Grasping the significance of this formula helps in understanding why phenylboronic acid keeps showing up in scientific journals and industry applications. Boronic acids like this one bind with molecules containing diols, which are pairs of alcohol groups. In practical terms, this means they get used in fields as varied as diabetes research, chemical sensors, and pharmaceutical design. Even outside the lab, boron-containing compounds find their way into products such as contact lenses and antibacterial treatments. Pinning down the exact formula is not some fussy detail. It determines how the compound reacts, how it forms bonds, and how stable it’ll be under different conditions.
My own background in organic synthesis involved plenty of days mixing up batches of this exact compound. In those practical experiments, C6H5B(OH)2 acted as a go-between when linking different chemical building blocks. It’s become a staple in Suzuki coupling, enabling the creation of larger, more complicated molecules—including those in many cancer drugs. Bringing up its formula isn’t just for purity’s sake; minor tweaks in the molecular lineup change how the compound behaves. If the ratio shifts, or if some impurity sneaks in, the results get messy and unpredictable. It hammered home the idea that chemistry doesn’t just happen on paper; each molecule’s structure steers its behavior in the real world.
People sometimes treat chemical formulas like trivia answers. Precision matters. Anyone who’s worked with phenylboronic acid knows what happens if researchers start out with the wrong details: wasted time, wasted funds, and sometimes even safety risks. As open research and data-sharing become more important, accurate formulas help scientists avoid repeating old mistakes. More than that, it lets professionals across disciplines—medicine, environmental science, manufacturing—build off each other’s findings. In my circles, the difference between a successful experiment and an expensive mess often came down to just one misplaced atom or missing functional group in a formula.
For scientists and students wrestling with chemical formulas, a couple of things make all the difference. Staying vigilant with reference materials and databases like PubChem or ChemSpider sidesteps mix-ups. Double-checking with a mentor or colleague saves lots of headaches before hitting the lab bench. Open-access chemistry resources play a huge role too, giving global access to verified data about compounds like phenylboronic acid.
Phenylboronic acid’s formula, C6H5B(OH)2, sounds dry on its own but tells a story packed with human energy and trial-and-error learning. This small piece of information opens doors to breakthroughs in research, development, and practical problem-solving. Respecting these details builds a solid foundation for discovery and collaboration down the line.
A bottle of phenylboronic acid can seem harmless sitting in the corner of a lab shelf, but scratching beneath that surface tells another story. This white crystalline powder shows up in a pile of research projects—from Suzuki couplings in organic synthesis to sensing glucose for diabetes management. Plenty of folks underestimate the risks by treating its storage like sugar in the pantry. My own years working close to dusty stockrooms and high-pressure bench spaces have made me pretty picky about chemical storage, especially for compounds as useful—and picky—as phenylboronic acid.
If you leave the bottle uncapped or slack on precautions, you can almost guarantee clumping and slow degradation. Phenylboronic acid pulls in water from the air, leading to hydrolysis and decreased quality over time. Open a jar that’s been sitting out and you might catch a faint whiff of new compounds growing inside. Early in my career, a rushed batch ended up mild because water had creeped into the container, knocking down the compound’s punch. A few careless days left us tossing out an expensive bottle.
A desiccator isn’t just for professors who like the look of ancient glassware. These containers, loaded with silica gel or other drying agents, give phenylboronic acid a safe bunker away from humidity. Not everyone can afford a big, climate-controlled storeroom, but even a basic sealed jar with a desiccant packet can work wonders. I’ve seen budget-conscious labs keep things in snap-locked plastic boxes, just pairing the acid with plentiful silica gel to avoid sticky regrets.
Direct sunlight warms bottles unexpectedly, and with that heat comes a faster path toward breakdown. I once caught a colleague dropping off their chemical stock near a window. Even brief exposure caused caking, and tiny crystals started clumping together. Keep these containers tucked in a cool, shaded spot—think away from radiators, windows, and busy work areas—so rise-and-fall temperatures don’t wear away your supplies or lead to accidents.
Sharing benches creates storage mix-ups all the time. There have been mornings where someone mistook phenylboronic acid for a similar-looking reagent, leading to ruined reactions and doubled waste disposal. A bold, unmistakable label keeps everyone sure about what’s inside. I use waterproof markers and tape, jotting down the date the bottle was opened, to sidestep those “was this from last month or last year?” conversations. These small habits help everyone keep track, especially with staff turnover or shared research spaces.
Work with clean gloves. I’ve seen cross-contamination turn reliable reagents unreliable. Wear gloves, keep tools dedicated, and close containers tight after every use. Discard any powder that looks funky or shows contamination. I always keep racks of spatulas washed and dry—routine, maybe, but it keeps you out of trouble.
Lost product from poor storage ends up passing through hazardous waste channels—an expensive lesson and a burden on everyone involved. Dealing with unnecessary chemical waste costs more than just new bottles. Careful routines help keep budgets in check and the lab a safer place for everyone. Making smart storage a priority pays off over time, both in reliable experiments and fewer headaches down the line.
In research, phenylboronic acid shows up in all kinds of labs. Chemists use it during the Suzuki coupling reaction, one of those cornerstone methods for building bigger molecules. Pharmaceutical companies lean on this compound when piecing together new drug candidates. Some biochemists rely on it because it can “grab” sugars, letting them sense changes in glucose for blood sugar tests. There’s industrial use too — analytical tests or niche coatings. So its range is wider than most people realize.
Take a minute to think about safety in the lab. People often wonder, just how risky is phenylboronic acid to handle? You don’t see it splashed across everyday products, but anyone who has spent time with organic compounds learns to ask. Phenylboronic acid doesn’t pack the punch of highly toxic chemicals like cyanide or organophosphates. But it’s not leftover dessert, either. The Safety Data Sheets point to irritation: eyes, skin, and even lungs if there’s enough dust in the air. Spend a day weighing out powders, and even a mild irritant starts to matter for comfort and long-term health.
In animal studies, scientists noticed mild to moderate toxicity if you go well above what anyone would use in a typical experiment. A rat doesn’t react the same way as a human, but repeated high doses sometimes cause weight loss or affect the kidneys. That’s not unique in chemistry; lots of things become a problem at high enough amounts. Right now, there’s no evidence pointing to phenylboronic acid as a cancer-causing agent or a major disruptor of the body’s systems at the exposures you’d see in normal chemical work.
Still, the irritant point matters. I accidentally brushed a bit on my skin once while prepping for an undergraduate synthesis. Redness, itching, then a lingering sting for a few hours. That experience made gloves and sleeves a top priority from then on. Any chemical that can irritate skin can make for trouble if you skip the basics: gloves, glasses, and good ventilation.
Workplace habits decide risk as much as the chemical itself. Someone who takes shortcuts with powdered solids (not closing containers, skipping the balance hood) can crank up exposure in a hurry. Running an experiment with a full lab coat and a working exhaust hood cuts that danger way down. Institutional reviews—the kind EH&S departments run—flag phenylboronic acid as needing proper PPE and clean handling, but don’t keep it locked up with highly controlled toxins.
Waste disposal is another topic. Pouring leftover solutions or solids down the drain never seems wise. Most facilities keep their organic chemical waste separated, then use certified vendors for collection and destruction. This helps stop accidental environmental release, since boronic acids might stick around and build up over time if poured out regularly.
I’ve seen some labs that re-label reagent bottles with clearer, larger hazard warnings instead of sticking with the original small print. That helps remind even experienced users of the risks. Some university and company safety programs now include hands-on demos showing what actual exposure feels like, which brings home the importance of gloves and goggles more than any written protocol. Sharing stories—real slip-ups, not just theoretical examples—turns policy into habit. Simple upgrades, like safer bottle caps or quick reference posters near weighing stations, minimize the chances for eye-level mistakes.
For anyone outside the lab, phenylboronic acid rarely appears directly. Trained workers, good safety culture, and proper waste handling offer the best tools to keep its risks in check. That’s how science balances discovery with responsibility.
Anyone working in a synthetic chemistry lab knows pure chemicals don’t just make reactions easier—they stop all sorts of headaches down the line. Most folks reach for phenylboronic acid to couple up molecules using Suzuki-Miyaura reactions. Purity turns into a real issue, especially if the yield suddenly drops or if impurities sneak into sensitive downstream reactions. Developers in pharmaceuticals can’t have mystery spots popping up on HPLC, and folks working with electronics-grade materials know even a trace of contamination can ruin a lot of value.
Most package labels for phenylboronic acid in the US and Europe will list purity as a percentage. Laboratories and manufacturers tend to supply the compound at levels of 95% to 99%. Some bottles even advertise “99%+” to appeal to researchers chasing better reproducibility and fewer unknowns, especially when tight analytical specs matter.
The numbers can hide some complexity. You’ve got the weight of water and inorganic salts to think about, plus organic impurities—usually residual solvents or byproducts from the production process. These might look tiny on a weights analysis, but researchers know they cause real trouble. Purity claims get measured with methods like HPLC, NMR, or melting point determination. More reputable vendors give a certificate showing actual test data for each lot, not just a vague promise.
A good friend, running a medicinal chemistry campaign, had a round of experiments collapse because the phenylboronic acid he ordered came with traces of halogenated aromatics. Instead of the desired molecule, his NMR showed a byproduct he spent days trying to isolate, wasting bench time and patience. Impure acid can also drag water with it, which gets especially troublesome in anhydrous procedures.
Pharmaceutical chemists, myself included, need tight impurity profiles for regulatory submissions. It once took our lab a week to confirm a single contamination source—cheap phenylboronic acid that failed to deliver a clean endpoint. The frustration didn’t just slow us down; it called lab standards into question.
Trustworthy suppliers usually offer a few grades: 95%, labeled technical or industrial, and 98% or higher, marked “reagent” or “analytical.” For education or proof-of-concept work, people might get away with technical grade. Working on drug launches or materials for electronics? The 99%+ lot gets chosen every time. Look for manufacturers that regularly publish their certificates of analysis and back up claims with a batch number you can track.
Lab-scale chemists sometimes clean up the acid with recrystallization if ultra-pure material is absolutely necessary, but this adds its own challenges and takes time from actual research. My old PI would always ask for the batch's certificate before ordering in bulk, and we once switched vendors mid-project just to keep our QC manager happy.
Certifications from ISO or GMP-qualified suppliers matter. Only buy from sources known for transparency, since they openly share impurity profiles and don’t hide behind unverified claims. High-purity standards do push up the cost, but the time saved in troubleshooting far outweighs the price difference.
Modern chemistry relies on compounds that meet posted specs, but not all suppliers treat quality the same way. Any research or production team benefits from sticking to sources that keep analytical results front and center. Tighter sourcing guidelines build trust, speed up troubleshooting, and support better science wherever phenylboronic acid gets used.
| Names | |
| Preferred IUPAC name | Benzeneboronic acid |
| Other names |
Benzeneboronic acid Benzeneboronic acid, 97% Phenylboronate Benzene, boronic acid Phenylboron酸 PhB(OH)2 |
| Pronunciation | /fɪˌnaɪl.bɔːˈrɒn.ɪk ˈæs.ɪd/ |
| Identifiers | |
| CAS Number | 98-80-6 |
| Beilstein Reference | 1362476 |
| ChEBI | CHEBI:31607 |
| ChEMBL | CHEMBL1433 |
| ChemSpider | 54626 |
| DrugBank | DB04162 |
| ECHA InfoCard | 03e4f4b8-4b2c-454b-a6fa-dedaf44149c6 |
| EC Number | 201-830-0 |
| Gmelin Reference | 68225 |
| KEGG | C06568 |
| MeSH | D010615 |
| PubChem CID | 4769 |
| RTECS number | DB7250000 |
| UNII | 6GXD77Y9NS |
| UN number | UN2811 |
| Properties | |
| Chemical formula | C6H7BO2 |
| Molar mass | 121.93 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.18 g/cm3 |
| Solubility in water | Soluble |
| log P | 1.2 |
| Vapor pressure | <0.01 mmHg (25 °C) |
| Acidity (pKa) | 8.8 |
| Basicity (pKb) | 8.77 |
| Magnetic susceptibility (χ) | -70.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.554 |
| Dipole moment | 1.69 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 106.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -357.8 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3220 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. |
| GHS labelling | GHS07, Warning, H315, H319, H335 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. H315: Causes skin irritation. H319: Causes serious eye irritation. |
| Precautionary statements | P264, P270, P301+P312, P330, P501 |
| Flash point | 93 °C |
| Lethal dose or concentration | LD50 (oral, rat): 4060 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 2000 mg/kg |
| NIOSH | SF7790000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Phenylboronic Acid: "Not established |
| REL (Recommended) | 0.5-1.5 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Benzene Phenol Sodium phenoxide Phenylboronate ester Boron trifluoride Triphenylborane |
