Find the Concentration of Hydrogen Peroxide by Titration with Potassium Permanganate

In this video we find the concentration of hydrogen peroxide by titration using domestically available chemicals and equipment.
Hydrogen peroxide is titrated using potassium permanganate solution that was standardized with sodium oxalate. The titration is performed in a solution of sodium bisulfate to provide the acidic protons needed to run the reaction. Sodium oxalate is titrated with the potassium permanganate at 70 Celsius until a lingering pink or brown color is observed. The amount titrated is used to determine the actual concentration of the potassium permanganate.
Once the concentration is known, hydrogen peroxide is titrated with potassium permanganate until a lingering pink color is observed. Using the known concentration of permanganate the concentration of the hydrogen peroxide can be determined.
Related videos:
Making Sodium Oxalate: • Make Sodium Oxalate - ...
Donate to NurdRage!
Through Patreon (preferred): / nurdrage
Through KZbin Memberships: / @nurdrage
Glassware generously provided by www.alchemylabsupply.com/
Use the discount code "nurdrage" for a 5% discount.
Twitter: / nurdrage
Reddit: / nurdrage
Instagram: / nurdrageyoutube

[@NurdRage]

Now you know why i made sodium oxalate.

[@SHIEET817]

Years ago

[@NurdRage]

@@SHIEET817 no i posted it last week.

[@borttorbbq2556]

​@@NurdRage it's nice to see you back.

[@borttorbbq2556]

​@CHICAGO TEEN you might be thinking of Nile red.

[@highlander723]

analytical chemistry is the equivalent of flipping burgers you say..... I feel insulted.

[@Alloran]

I used to teach this error propagation to students in my IB physics and this is a fantastic example of how the error grows at each step and with each calculation. I think I'm gonna use this video as homework this semester. I want them to tell me why my measuring devices dictates my method and why using the minimum possible number of measurements or calculations to reach my end point is preferential to a possibly more accurate method that requires more steps or calculations with the measurements.

[@mitchellr6819]

I’m in a general physics series right now, my professor really pushes propogation of error and significant figures. I’m so excited to see it here!

[@pierreproudhon9008]

@@mitchellr6819I finished general physics a earlier this year and all the professors I've had didn't seem to care that much about it. Did some error propagating calcs in the accompanying labs but that's pretty much it.

[@ravencrovax]

"Trust nothing and verify as much as you can." Sounds like how I live my life.

[@GodlikeIridium]

And you're right doing so.

[@BillAnt]

Especially the wifey/girlfriend. ;D

[@ianmcewan8851]

[As an applied mathematician with a specialty in measurement and error analysis] no evisceration necessary!! Nicely done in a half hour vid.Really no quibbles at this level.

[@methyleneblue_]

i've been watching your videos for more than a decade iirc now 😭 thank you for doing what you do!

[@Saumiiiii]

same here hahaha

[@SharpMagnets]

I remember being 10 and being OBSESSED with these nurdrage videos. Now I’m 22 and I re-found you. I’ve never been happier.

[@Swannilization]

YES! I had to do this in a lab practical back in the day. Thanks for showing the workhorse stuff!

[@nathanhays1746]

I did this same process including making the standard to titrate permanganate. I was surprised that my 30yo jug of h2o2 was actually _more_ concentrated. Hadn't realized that h2o evaporates faster than the peroxide degrades.

[@NurdRage]

Wow that's pretty cool. I wonder if mine started at 5.0% and drifted upward from evaporation. Maybe I'll test it again next year to see.

[@nathanhays1746]

@@NurdRage In the h2o2 powered hobby rocket community a common way to get high test peroxide is to put a fan on an open container and leave it overnight before the launch. Loses peroxide of course, but starter 35% concentration is pretty cheap. Distilling is dangerous because you must heat it past 100C to drive off the water. Vacuum distillation is problematic out on the range and transporting high test peroxide is no bueno. Luckily, leaving the inhibitors in doesn't interfere with the permanganate-infused platinum gauze catalyst that the h2o2 passes through as it is pumped into the chamber. "Motivational" chemistry! Absolutely love your work!

[@kohizeri_daisuki]

Thank you for the video! Now I know why I am dead set on pursuing chemistry when I start college in a few months. My head aches a bit with the intricacy of the processes and techniques, but the utter beauty and satisfaction I get when I can say for sure that this substance has this concentration and it is all thanks to my work takes all that ache away. Thank you for inspiring me along with other science youtubers to pursue this field ❤

[@thomasrogers8239]

We used peroxide solutions in mold mitigation back in the day, you might look into IAQ 2000 or it's daughter product IAQ 6000 for a more concentrated peroxide starting solution. I'm remembering it being labeled as being either 15 percent or 30 percent peroxide and we absolutely diluted it before spraying stuff down because it had a nasty habit of burning our skin if we accidently got spray on us.

[@stamasd8500]

Baquacil oxidant you can get at pool supply stores is nominally 27% H2O2. It's fairly inexpensive, $15-20 per gallon.

[@MCPicoli]

I can get it at 50% concentration as a pool cleaning agent here. Very cheap too. YMMV, I am in Brazil.

[@booboyBL]

Many years ago, I was a lab tech. for a major manufacturing chemical company. I worked in various lab departments, including 3 years in analytical services carrying out titrations and various other analysis techniques, (chromatography, photometry, spectroscopy and others). I sort of miss those days

[@idontknowyet2875]

Man, I wish this video was out 2 months ago You explain the general process really well

[@binaryblade2]

Oh shit, new nurdrage video just dropped.

[@ejkozan]

Wonderful video! And all this discussion of errors! I just love it!

[@koukouzee2923]

I own a vial of 102% pure sodium hydroxide The purity source was the retailers "trust me bro "

[@bradleyhowes848]

So awesome to see! I’m a glass artist and I batch my own colors that are very sensitive to the redox of the base glass as well as the furnace atmosphere. I definitely think some of these principles and techniques can help get a more relatable color!

[@KrashFries]

you can actually add traces of manganese (MnO2 is cheap and convenient) to the glass and have it oxidize to a light pink or indigo!

[@bradleyhowes848]

@@KrashFries indeed, however this depends on the redox of the glass, pushing the Mn ion to the +2 or +3, colored or colorless, and also dependent on the fluxes in the glass, sodium will tend towards brown and potassium towards purple. Further, trace amounts as a decolorizer can solarize from clear to colored over a period of years. The techniques the NurdRage uses though will help to reduce error in more complicated glasses involving the controlled growth of silver nano particles in the glass.

[@clintongryke6887]

Really good; thorough and clear. Takes me back to A-level (U.K.).....

[@Carlos_GS]

Very interesting, thanks for sharing this process in such detail :D

[@austinrosh6491]

So happy to see you posting again keep up the good work your the reason for my chemistry career

[@trevmac2248]

Excellent detail & presentation! Thank-you for sharing!

[@Mpdarkguy]

Hi I just wanted to tell you that I grew up with your videos and recently I've been tasked to narrate a specific and technical presentation. I took a lot of inspiration from your style and I've received great feedback so far! I am not in a chemistry related industry by any means, but I can somewhat easily follow what you're doing with just high school level knowledge, and I think that says a lot about the way you present your videos. Thanks a lot for giving me a boost in more than one way!

[@Thecompanioncrate]

Return of the Mack. In all seriousness I appreciate these more recent videos I needed to review this stuff.

[@sulaimanabdullah952]

Great video, clear, concise, informative. Thank you

[@Bludgeoned2DEATH2]

Interesting! I work as a chemist in a manufacturing lab in one of the products we make is an H2O2 containing hair spray for the summer and to analyze it we use this potassium permanganate titration and you’re right we use sulfuric acid to acidfy the solution prior to titration!

[@theSILKROAD210]

Thank you for your great work! Right now I am doing my Bachelor thesis in medicinal / synthetic chemistry, and I am watching your great videos since my apprenticeships as a Chem. Laboratory assistant. imagine I had access to this kind of educational content back then, that would have been great. future generations will be so lucky to have access to this kind content. please continue this great work, it is a big contribution towards free and accessible Science education.

[@stamasd8500]

Very useful, thank you. Keep'em coming!

[@Gauss247]

This is absolutely fascinating. The level of detail and understanding you have are mind blowing! Also very didactic delivery. I love all your videos. Thanks for all of them! I hope you can keep them coming.

[@GQuack]

Glad you're back, Lithium. Loved your content since the old days(2013).

[@nickbonsavage2586]

Great to see you're still active. Thought you retired from youtube there for a bit. This is great stuff. Thank you. About ten years ago i started getting into chemistry as a hobby, this last year I began at a university and im going for a chemistry degree. I'm 34 and figure as long as I finish before I'm 40 I'm ok haha. Anyway, your videos were what I watched all throughout the years that helped build my interest and it's just great that you're still at it. You played a large part in building my fascination and interest of chemistry. I'm sure I'm not the only one that you helped inspire.

[@erikziak1249]

Not even half a minute in and I am literally "LOL" ing. This is the content I subscribed for. 🙂

[@mitchellr6819]

I gotta be honest, I got sooo excited when you brought up propogation of error.

[@imikla]

This is super exciting! Thank you!

[@javersongoulartfilho9439]

Now this is an amazing lecture. You got me impressed and subscribed! Regards from Brazil!

[@KF-16-65]

Thanks for the video! Great refresher on some of the stuff I learned in an analytical chemistry class not too long ago.

[@edgeeffect]

I have huge "nostalgia" for Pot. Permang. - partially because your "making Pot. Permang. from batteries" video was the beginning of my KZbin science adventure. You've done wonders to improve my amateur-grade titration too - it's time to put my burette away and "go gravometric" from now on. All in all, another excellent video.

[@frollard]

Thank you as always for sharing!

[@Mst2halo]

Hey we have the same digital scale! I watched you all the time when I was in my early teens. I always had a natural interest in chemistry, but you amplified that sir. Glad to see you are still involved in chemistry and uploading videos. I have a lot of catching up to do!

[@davidjones6661]

"Not even I have one".... "and I've got a ****ing rotovap!"

[@thestimpy2101]

Me and my kids have missed your content.

[@Josue31627]

"Trust as little as possible and verify as much as possible" is good life advice too. Great video as usual. I was reminded of Periodic Video's "Accidental Reaction" video near the beginning. I actually found titration fun back when I took college chemistry. But often I made too many errors in my error calculations... oopsie.

[@JoshuaNicoll]

I was only thinking to myself I needed to titrate my H2O2 I had concentrated a bit, your methods and justifications are always a delight to watch.

[@bedlaskybedla6361]

Very nice video NurdRage! You well explained basics of volumetric analysis. I like that measuring of titrant with scales, it present alternative approach for someone who doesn't have a burette. If you want, I can share some experience with bromatometry, this method isn't often mentioned and it can be very useful (especially for organic chemists). I tried determination of phenols, anilines, O-alkyl phenols, hydrazines, unsaturated carboxylic acids, ascorbic acid, Sn2+ and Sb3+ salts. I also did few not well known, but interesting titrations, like Mn2+ using KMnO4, NO3- using FeSO4 or amines using HClO4. I also plan UV catalysed oxalate determination using Na3VO4.

[@randomergy683]

Yesssss! Perfect timing for this video! I've had some concentrated peroxide for awhile that I'm not sure what the concentration is and was wondering how I could go about determining the concentration.

[@handpaper6871]

If you know that it contains only peroxide and water, just measuring its density will get you within ~1%.

[@stevensexton5801]

"I just want you to be aware that it exists", as an engineer I love that statement.

[@aSCrouton]

Going to run through this myself, such a good crash course. Would love to see videos of testing for different functional groups, basically a way to test and identify different pure substances

[@vitamin9165]

Nice vid. I think this is super important stuff for the amateur chemist to know when you don't have good sources for things and the precision kinda elevates things from just fucking around in a basement to a real science in my opinion.

[@kid_missive]

Thanks for the video! I do a lot of these exact titrations at my job so it was neat to see someone with your reputation discuss them. We have, in the past, used NaOH to titrate oxalic acid, then keep that around to check KMnO4 solutions. I have lately been checking NaOH against dry KHP, but it never occurred to me to use oxalate as a single primary standard for both acid/base reagents and oxidation/reduction reagents... Oxalate also has some useful chelating properties I seem to remember. That would be super if it could be standard for complexometry too.

[@NurdRage]

Oxalic acid needs to be checked because it absorbs water, and it decomposes if you try to dry it. But sodium oxalate is great because it's stable enough to be dried. Might be worth looking into buying a certified standard version of it. At the very least it saves you two steps from KHP and NaOH.

[@GodlikeIridium]

It always depends on the exact use case. A primary reference substance for titration has to be easy to purify, stable and easy to dry (again and again). Besides that, similar to the analyte you'll be titrating after the determination of the exact molarity or a factor. So for acid-base titrations we use KHP if intended for the titration of anorganic salts. For acid-base titrations of halogen salts of organic amines we use benzoic acid (a beautiful example to teach recrystallization btw). Because of the different pH at equality. For redox reactions oxalic acid. For complexometric titrations calcium carbonate. TRIS or trizma base gets readily used too and I've even seen a very niche procedure using sulfamic acid, this one doesn't really make sense though.

[@kid_missive]

@@NurdRage I am going to be implementing this as soon as I have time. Thanks for your insight!

[@AcoAegis]

That's really cool, I never knew how that all worked (or why molality existed). Thank you for sharing

[@LubeIn]

Great video

[@AL6S00740]

wooohooo

[@2486jdc]

this is, and has for a long time been, my absolute favorite youtube channel. i would love to have even half the understanding of this shit. i got into chemistry for the wrong reasons but your videos definitely helped transform it into a healthy interest. you sir, deserve a statue.

[@NurdRage]

thanks man. Whenever i'm feeling down, or wonder if i'm doing okay, i read comments like yours and i'm motivated again to keep going.

[@2486jdc]

no problem man. stay genius!

[@picosoft2033]

oh yesss! after a long time one of my popular and inspiring chemists uploaded a new video! 😇😇😇

[@Marbslab]

Very useful.

[@CHIROTHECA]

He is back! FInally!

[@apricotcharms4126]

Holy shit bucket the granddaddy of KZbin chemistry is still posting. I used to watch you all the time as a kid back in 09

[@piranha031091]

If you're doing gravimetric titration, you may want to use polyethylene or PTFE beakers instead of glass ones. They're much lighter, which minimizes the relative error from your scale. Also avoids overloading the scale in some cases.

[@rafaelgcpp]

Sir, you made me freeze to my soul, remembering my days at university physics lab, measuring stuff to learn how to deal with precision... This is the seed of nightmares!

[@charlesurrea1451]

Yep! Sounds like work.

[@erikziak1249]

OK, even though I LOLed at least two times in the first minute of this video, the last 5 minutes were very serious and valuable to anyone doing this.

[@TechsavvyScientist]

Technically molality refers to moles of solute divided by kg of solvent (not solution) the error is not big though since it’s a dilute solution.

[@GodlikeIridium]

Do you have a source for that? I'm pretty sure molarity is defined as moles of solutes by volume of solution, SI in mol/m3 but usually in mol/L. And not all titrants and other solutions are as much diluted. For example a 1 M solution of silver nitrate is 170 g of AgNO3 in 1000 mL of solution, or in the definition you mentioned 830 g of water. That's a huge difference. Edit: And a definition in mass by mass would make it almost impossible to handle and use for titration and the dividor being solvent instead solution would make it unnecessarily complicated. I do like the way he titrated in the video though. Never seen that :D

[@tbird81]

Molality vs molarity?

[@Neofizz]

After watching for years, I really like your viewpoint and ingenuity. I'm curious if the PPM of a colloidal silver solution can be discovered by titration.

[@jwrm22]

After watching dozens of these videos, I still don't know much about chemistry. These steps are very similar to other sciences, where I'm most adept in Electronics Engineering. Nothing beats measuring the actual parameters of a component, instead of just following the datasheet.

[@vicgarcia1043]

The lab I work in uses something called the Monte Carlo simulation in order to estimate measurement uncertainty. For those who are unfamiliar, the best way I can explain this is that after taking multiple measurements of something, a computer program mathematically simulates a number of possible iterations of this measurement (say a hundred, or a thousand iterations), and we derive our measurement uncertainty estimation from there. I'd like to know what your thoughts are on this. Great video as always! :)

[@thebackyardspaceprogram]

He's back!

[@gigglysamentz2021]

I'd love to check B12 content in vitamin supplements!

[@davemarchitto6485]

Quantitative analysis suuuuuuuuuks.

[@JanJeronimus]

When you where drying the primary perhaps also weigh during the dry process to check if it dryed completely. (Perhaps you did this, however i did not see it in the videos.) This is easy to do and also adds some reliability.

[@Nagria2112]

nice! thats my work :D im an ANALytical chemist in pharma and we titrate alot.

[@KMyGProductions]

This video gave me flashbacks of my junior Quantitative Analysis course in college and now I’m glad I didn’t get a job as an analytical chemist

[@BrendaEM]

Nudge, nudge. We need an epoxy-like system that can be recycled. Bonus for it being not an endocrine disrupter. So, we need two chemicals that when mixed together harden, and resists water--yet can be readily dissolved with a 3rd chemical, which is not normally around. Hmm. I wonder if you could make an Arduino device that has an phototransistor and an LED separated by a short distance. The opacity of your solution during titration could be read numerically--instead of eyeing it. An old insulin pump or parstaltic pump could be used to dropwise additon--until the titration point is reached. Interesting videos, as always. Thank you.

[@dimaminiailo3723]

Interesting moment: both Na2C2O4 and H2O2 consume 2 e per mol, thus you could totally drop KMnO4 itself and go on the ratio of the reducing agents. Speaking about the next topic, I'd want to see the determination of brass' composition via iodometry. You can use your oxalate as the primary standard although it could be a really long way to the answer which you'd probably not like

[@peejay1981]

As an Electrical Engineer who knows nothing about chemistry this video feels just like home compared to your normal stuff! Measure and quantify everything multiple times, then crunch some numbers and figure out the errors.

[@johnmyers379]

Your the only person that I can't wait until u get mad I know it's coming it makes my day lol

[@djdrack4681]

I've worked in an industrial food MFG that made whey protein powder. (My job was micro testing both pre-products, finished products, and environmental [air, water lines, drains, floors and puddles on the floor, etc]) During the process, they boil off the excess water, (don't quite me) but I believe react it with H2O2, acetone, honestly I forget. But we also have lines EVERYWHERE in the plant (basically big a## hoses) to wash equipment, the concrete floor etc to try and keep the bacteria levels low. One line was plain tap water, the other was some cleaner I think was something akin to star-sans, a semi-foaming quick rinse cleaner) ANYWAYS: one of the tests we did was testing the water coming into the plant and at some of the water tanks we had (which would be used to flush some systems). It was basically titration work just like this to detect H2O2 levels, because there could be cross-contamination at times with this from one of the systems (somehow, because the plant was old as hell, and many things quite 'questionable'). Since they dind't want ppl to use sulphuric acide, we were in fact using sodium Oxalate and potassium permanganate as well. So, when I say it was very similar to this, it was VERY. I think we also used hcl if I remember correctly, but as its been years since I worked there I forget why.

[@NurdRage]

Interesting! I think you can use HCl if you're not too concerned with accuracy since HCl chews up some permanganate before it reacts. Maybe your lab determined the error was acceptable for your application.

[@djdrack4681]

@@NurdRage Lets just say the QA side had a lot of 'wide' margins for acceptable results. More than some of us may say were 'OK' lol

[@fishyerik]

Great video! Not the quick and easy way to get a ballpark figure of the H2O2 concentration I was hoping for, but great video. My mind started to figuring out ways to automate the more tedious parts just while watching the video. And I suspect the video was just a small fraction of all the time it took to do for very experienced person, as the most of the most tedious parts were sped up or cut out, and the video also had great narration. I was thinking, couldn't a peristaltic pump and a camera and some software be used to automate the titration? In this particular example a light source, photoresistor and an arduino should enough to control the pump.

[@NurdRage]

actually, if you want a fully automated titration and you are allowed to use electronics, then looking the topic of "coulometric titration". You basically stick electrodes into the solution and measure the peroxide content by electrolyzing it. a great deal more complicated, but once you set it up, you just add in a precisely known quantity and press a button to get the results.

[@fishyerik]

@@NurdRage Thank you! I later realized I can just add a catalyst and measure the amount of oxygen gas.

[@jacob127409]

My previous job was an analytical chemist and let me tell you I still dealt with customers but it was mostly emails and while I was yelled at a lot less I had to explain to people what numbers meant and why I need them or why they need them. Most of them were in supply chain positions so difficult to explain to them between GC TCD and GC PDID which was not fun.

[@jolioding_2253]

In our quant analysis lab we had to qunatitatively analyse some aluminium salt using Chinolin-8-Ol which did not really work for more than 3 people in the lab because our filters just would not dry properly and get to a constant weight even after 6 drying/exiccation cycles so maybe if you have to capabilities I'd like to see you try it.

[@Jkauppa]

proper copper electroplating setup on top of any conductive substrate

[@ivanmartindelcampo]

Can you talk about matrix effects and how analytical chemist go about that! Maybe you can quantify how much water, fat, and salt there is in common food while describing matrix effects

[@markywarky1234]

Could you do a relatively uninteresting but academically relevant titration? Oxidising Fe2+ to Fe3+ using acidified permanganate comes up a lot at A level / IB level, and it would create a useful academic resource. Many thanks and thanks for a great video.

[@dimaminiailo3723]

the titration of iron requires fluorides, I'm not sure it would be interesting in the branch of amateur chemistry

[@rodneyvinen1594]

Very nice video. An extension would be to test the concentrating of peracetic acid. KMnO4 reacts with H2O2 but not with peracetic acid. Idometric titration gives the amount of H2O2 and peracetic acid. Finally some mathematics gives the concentration of peracetic acid. Peracetic acid is used in the food industry and is available to the amateur.

[@jeremiahbullfrog9288]

This is fantastic, you answered all my questions throughout the discussion. I was surprised at the low concentration: seems it would be much cheaper to use a double dose of drug store 3% H2O2 instead of this "oxygen bleach" product.

[@cheeseburger118]

Analytical was my least favourite chem class in uni but this was cool! I remember titrating VO(2+) to VO2(+) in inorganic which is also self indicating (dark blue to orange-ish if I remember correctly). It was fun trying to refer to them though since we called both of them "vee oh two plus" lol

[@bangbangliu2146]

I think a video on iodometry would be interesting too.

[@stazeII]

My favorite class in all of chemistry undergrad was organic analysis (3rd term of o-Chem lab). Group of unknowns had to be identified over course of term. Was so much fun, and stressful (grade was based on how many we got through, and if we were right). Going from that to biochem and then pchem was not nearly as fun. Lol.

[@erikhartwig6366]

Yes! Great Video. Very interesting. Regarding analytical chem, If you have 2 different products, but suspect they are the same, how does one analyze/test them to see if they are in fact, the same product? Im curious because i use a specific cleaner for when i make beer at home. However, there is a similar cleaning product sold for doing laundry (that my wife uses) that is less expensive but seems to work in much the same way. the only difference is the marketing and labeling. I am suspicious that they are the same.

[@NurdRage]

for a quick and rough determination, you would use something called "Thin layer chromatography", it wouldn't tell you if they are the same, but would indicate if they were substantially different. If you wanted to be more sophisticated you'd use something like HPLC-Mass spectrometry to really figure out if they are the same.

[@gamefreak2016]

Hey, I’ve watched your videos for ages and I often watch NileRed and it got me curious of your thoughts about him? Is he a bit reckless as a chemist or do you like what he does? (I understand if you’d rather not answer btw haha)

[@spudd86]

Error gets really fun when you have to take into account the inherent error in the floating point number system that computers actually calculate in.

[@weldmaster80]

He lives!

[@DaNiKzz]

26:00 "Mass of Karen ego" lmaoo true

[@scottmclaughlin1410]

Analytical chemistry, mmm good stuff

[@gigglysamentz2021]

How do you get the density of all the solutions?

[@AmdMatar94]

thanks a lot for this work .. can you explain me please why we took the molar ratio 5/2 for H2O2 from MnO4 not the (3/2 for KMnO4) , i used oxalic acid instead, in case of KMnO4 is 0.1N so would be molality is 0.0158 mol/kg ?

[@RaistlinMaj]

Finally someone shared an approximation of the mass of Karen Ego's

[@NvTwist]

Perfect video to point anyone to when they say “woah why is lab grade cost a lot more?”

[@Whatisuswold]

everything you've made is great but I still would love for you to make a video on how to prepare perchloric acid by electrolysis of table salt using my beloved platinum plated titanium electrode and then combining it with hydrochloric acid. after all finally work with ammonium,potassium,sodium,strorium,calcium,barium and copper hydroxide to create colorful cannons and rockets on your house and head.

[@jamessshep6106]

Is there a way to make oxalic acid from obtaining calcium oxalate from leafy plants ? Would sulfuric acid be the route used to convert from calcium oxalate to oxalic acid?

[@9daywonda]

Informative as ever Mr. Rage. Are the rumours true that you are really Charlie Sheen post Hollywood?

[@BruceNJeffAreMyFlies]

Wait, I'm not the only one who actually says anal ytical? My experience was genuinely starting to look like I was the only chemist on the planet with a sense of humour!

[@claireradke7029]

'amateur chemists like us' I'm in the wrong fucking building