It's funny how half of the people commenting are kids studying the subject and the other half is adults trying to work out how to make alcohol at home 😂😂
Actually I think it's 1/3rd each of those two groups and 1/3rd kids trying to learn how to make alcohol at home so they can bear studying the subject. ;-)
0:09 Extraction, Chromatography, and Distillation 0:37 Lower Boiling Point boils out as vapor, Higher Boiling Point remains in the glass. 1:13 The Setup - A Roundbottom Flask - A Heat Source - A Thermometer - A Condenser - A Receiving Flask to collect the distillate 2:35 Distillation tips 3:50 Useful for Separating chemical Compounds 4:34 Fractional Distillation 4:47 Azeotrope (ex. Ethanol and Water)
👏🏼👏🏼👏🏼👏🏼very good !!! Using simple distillation, I’ve managed to graph the difference in boiling points between ethanol and water. This video explains why the alcohol distillate was quite diluted.
Hello professor! Thank you for the video! I have a question if the disfance between the condenser and the vapor, the side arm, is longer, is it recommended to add a layer of isolation to the side arm so the temperature of the vapor does not fall down until it reaches the condenser?
I worked, or was around, the Scotch whisky industry for a number of years.....you just explained my job :) The stills at Srpingbank and Laphroaig never looked like this ;)
Thank you! I have my second Organic a lab tomorrow on this . The first one was extraction and drying and my conical vial ended up exploding due to human error . Methylene chloride everywhere !Wish I would have researched beforehand.
wow. every video I watch their like: So you want to put this here then explode this then drink this? This was so easy to understand, this made so much sense. Thanks
Can i get a clarification? The cold water.. is that just something you need to just have to make it work or is the process itself worked into the condensing process?
the 0+34 setup matches some work i'm doing distilling off the ca 1000 ml 190 ethanol from a hemp soak to recover and re-use it ( 190 is $20. / liter here in colorado ) . the 1+39 setup looks interesting. and i wonder if it would work too to hasten the whole process. ( the liter of starting 'green' alcohol w/ -oid's extracts takes 2 - 2.5 hr to distill down to the last 75 ml of the -oid's extracts to be saved ). the actual outflow is about 4.5 ml per minute of nice-looking 78*C clear ethanol. (5300' elev) that 1+39 column is a 'vigreaux' is it not ? i like its bent side arm at the top side. plus wanting to know when the use of a vigreaux is called for. could someone tell me the name of the 'bent adapter' at lower end of the condenser , that connects to the receiving flask ? to find one on ebay a correct name is most handy. since 190 has 5% water in it your mention of azeotropes got me wondering if that is a factor with what i'm up to in extracting the -oid's from hemp w/ an ethanol solvent one thing i got seeing your vid' today is that the 'condenser' works 2 roles. vertically it can be used to reflux a 190/hemp mixture and angled downward it condenses the 190 vapors back to liquid form. i'd been mixed up about it all. one surprise doing this all is the lack of vapors getting into the room and being smelled. the condenser is doing its job for that to be so
Hi Prof. Dave - love your stuff. However, haven't you over simplified the stuff about the boiling points of the two components and setting the heat between them so that one boils off and not the other? Because the BP of the mixed solution will have a BP between the two component BPs, proportional to the amount of each component, following Raoult's Law. Setting the heat below this BP will only result in evaporation vapours, and you cannot raise the solution temp above the mixture BP. Also, what you describe suggests that as long as the mixture is boiling but at a temperature below the BP of the higher-boiling component, only the substance with the lower boiling point will boil off, but isn't it true that both substances will boil off when the mixture is boiling, this time in proportion to the respective entropy of vaporisation of each component?
this note is to thank you for your message. thought provoking. new thinking called for. it had me open my 3'd ed Wm'son 'org exp_s' to ch. 5 on 'dist_n' and get refreshed w/ Raoult's law. and , sure enough, distillation is as messy as liq-liq solvent extractions with their Kx distribution coeff's . and how repeat runs are necessary for more purity. as then the unwanted amount in one phase is the less via the Kx factor one thing learned is his recomendation of using Chore Boy copper sponge pads as a packing material in the column for all the extra rust-free surface area it gives you. and , yes, it does appear prof. dave is on the spot w/ having to choose how deep to go on presenting this subject. keeping it limited in complexity is wise & likely comes from being used to having an audience of freshman . thumbs up for prof' Dave , whatever the reason
would you mind to explain, why chromatography just separates based on polarity? I have performed quite a few chromatographies on my own at work, and I am quite certain, that a SEC is not splitting up components based on polarity, just based on molecule size (Size Exclusion Chromatography) Or a chromatography with Heparin Sepharose Gel seperates molecules based on their affinity to heparin. I know, that especially C16 to C20 gels are used for splitting up components based on their polarity, but that's just a fraction of what is possible with chromatography. And there are a ton more types of chromatography, for example IEX (Ion exchange chromatography), which allows proteins to be seperated by their charge, etc.
@@cousinofgod7951 Dude he said that he works a lot of hours in making these videos in his ask professor dave episode.. and u r saying it is not difficult??
@@ProfessorDaveExplains Oh sorry, i might use words incorrectly, what i mean by my question is why do we measure the temperature of the vapor, but not the temperature of the liquid, using the thermometer. btw, thank you for the lesson
@@banhatnguyen1282 The thermometer actually cannot go into the liquid since it would be too close to the flame so it would provide for an inaccurate reading of the boiling point. It may be higher than it actually is.
Can somebody help me: I tryed destilating odors from wood shavings and it worked out quiet well with soft woods, or woods with resin, but I had no success with hard woods so far (like cherry, peer...). Somebody recently told me that the oilie destilatable components of most hard woods react below 100° C, so they loose the scente when boiled in water... I once tried alcohol as a medium to destilate, but the result just smelled like alcohol. Has anybody tips for this (PS I don´t have the tools to lower the preasure whilst destilating)
I understood more in this 6 min video than the two hour lab, after watching this I knew I messed up my entire experiment, now how to write a paper about it :( why can't professors explain better...going to try and watch these pre lab.
You normally use distillation to separate known liquids of known boiling points. If you have a contaminated starting material or a mystery liquid - you probably wouldn't use distillation until you had refined the starting material through other means. Or you would just end up with two unknown products that you would separate further. Or you would use fractional distillation.
@@jacquiwatson2249 But in the mixture of two known liquids while carrying out distillation, wouldnt there still be the high boiling point liquid out of the mixture of two evaporating as evaporation occurs at all temperatures
@@MoizAsimagar I think the answer to your question is no, evaporation doesn't occur at all temperatures - for example - water evaporates at 100degC. It doesn't evaporate at 20degC. Distillation separates two liquids with two different boiling points. The one with a lower boiling point will collect in the condenser and the other will remain in the flask. You keep the temperature fixed on the flask to make one boil, but not hot enough to boil the other. To you it will appear that the mixture is boiling but in actual fact, only one liquid is hot enough to turn into vapour. The other stays in the flask (as long as you don't turn the heat up).
@@MoizAsimagar Dont trust him, water still boils even in ice phase. Refer: chemistry.stackexchange.com/questions/7449/why-does-water-evaporate-at-room-temperature
Tolong bantu aku 🙏 Aku bingung dalam metode destilasi, Tepat nya saat pengambilan zat murni Aku sengaja pakai sempel obat yg ada 5 kandungan di dalam nya, setelah selesai aku Ekstrak,, maka aku saring dan mendapatkan Residu & Filtrat nya, Tapi aku bingung bagaimana cara memisahkan kemurnian dalam zat zat tersebut dengan menggunakan metode Destilasi, padahal aku sudah catat titik didih dari ke 5 zat tersebut, ini titik didih nya: Zat A > Titik didih: 400 °C Zat B > Titik didih : 260°C Zat C > Titik Didih : 379 °C Zat D > Titik didih : 520 °C Zat E > Titik didih : 232 °C Sebagai contoh jika aku mau mendapatkan kemurnian zat B, bagaimana cara melakukannya ?? 🤔🤔🤔 Siapa tau ada yang bisa kasih tahu, 🙏
