Doug's Lab - 2015-05-20
In this video, I make 68% nitric acid from sulfuric acid and potassium nitrate.
I think the bottom equation is missing a 2 before the first reactant (KNO3) to be balanced.
I might be wrong.
Thanks for the videos.
this is how mu kitchen looks when I cook schnitzel.
worddunlap Or čevapčič. Google it if you dont know.
@Žan PekošakHaha I know both. Croatia have some interesting foods indeed.
My kitchen looks like that when I make guláš (goulash).
he wasted the sulphate down the drain cause "it's cheap" lmao
If you mix it with cheap slaked lime to neutralisation makes a good tomato fertilizer.
Very nice (process and production)!
I'm jealous of your lab.
:-)
You are missing a 2 in front of the KNO3 on the bottom reaction on the whiteboard. Anyway, thanks for all the videos. I started studying chemistry about 6 years ago independently in my free time and these videos sure help make up for the lack of lab time that one misses out on going to Amazon Technical. I just bought my first (easily plugged Graham) condenser and if not for this video it would surely have been destroyed. Thank you very much!
The warning at 7:00 happened to me. Sulfuric acid exploded everywhere. Wish I'd watched this video before!
Doug love your videos have learned so much from you and them. like your sense of humor and your throughness.
Have you tried using a heavy oil as an anti foam agent in the reaction chamber, or would that oxidize in the N0x?
potassium sulfates are good for fertilizer purposes
Nice video, I love chemistry I want to have a lab like yours one day 😀.
i know this video is old,but i still watch it when i have a question or two about distilling nitric. thanks again!
GGGGGGGGreat.
I would use the forerun to start the next reaction. And also include the undistilled nitric acid in the next make
Cool, thanks for the video learned a lot looking forward to o-chem in college. btw random story everyone had a friend who spilt 6 molar hcl on his arm then proceeded to run his burning arm over a lit bunsen burner on accident! you think you're accident prone think again!
Hmmm, I was always taught that wearing gloves when handling HNO3 was a 'no-go'?
only with the fuming stuff.
Did you determine the molarity of any of your HNO3 solutions by titration?
Probably he determined it by density. Titrating that concentration of HNO3 involves repeated dilutions, which causes errors to build up, and it also does waste some valuable nitric acid. Density is much more accurate, if you have a volumetric flask, an analytical scale and you know the temperature. You can determine it with an error of less than 0,0125% if your volumetric flask and your scale are good (and you also do the procedure correctly)
Hi! tel me how is named your intro song
Can you make a video with the following method:
urea carbamide + sodium hydroxide = ammonia.
Ammonia + glowing copper / platina = NOx
Is it doable?
So here's a question: can you add hydrogen peroxide to the solution to be distilled to scavenge any nitrogen dioxide formed and convert it back into nitric acid before it escapes?
Please make a video on functional group tests
love this vid & use your recipeee, i have a big bag of 20. 0. 0. amonium sulfate ??? is there any nitrates in that kind of fertilizer ? dont know how to test for nitrates . thanx, bill.
I love your channel that I just discoverd! I'm a computer programmer but want to build a home lab and play with Science.
better go do that chemistry
What a set-up...I second E&F...(-TVC)
HI Doug, I went ahead and gave this reaction a try last night and everything went great! I used sodium nitrate instead of potassium nitrate and did everything on a 1M scale versus your 4M × 2 setup, but I was able to obtain around 85ml of non-azeotropic nitric acid. Once I buy a 24/40 thermometer adapter I'll go ahead and distill this again to bump the concentration up to 68%. I noticed the "foaming" you were talking about as the reaction mixture boiled away and I definitely appreciated the warning about not letting this get out of hand. My reaction went from a boiling liquid, to a boiling syrupy bubbling consistency, and then eventually the boiling and bubbles decreased to almost nothing. I figured this was the correct stop-point as I assumed that if I turned the heating mantle up any higher the reaction mix would start violently bumping rather than boiling. Any thoughts? My yield was around 85ml but I had estimated being able to get around 110ml of acid solution. I just played it safe since this was my first time doing this reaction and your warning about the hot sulfates making a mess and cracking glassware had me being cautious
Why didn't you make a fractional distillation for this?
Great video as usual! What camera do you use? It looks really nice. I use a Nikon D3300 for my videos.
@Gooferking Science Yeah, those Nikons are great cameras. Mine is not a DSLR, just a glorified superzoom. I use a Panasonic DMC-FZ200 and a Casio Exilim EX100. Depends on the application. I film in 1920x1080 at 60fps with the panasonic or 30fps with the Casio.
Subbed for this.
imo these are the best chemistry videos on youtube
Had two ideas for trying to avoid the chance of foamover creating a mess: running the initial reaction of sulphuric and kno3 with the boiling flask in an ice bath before moving to boiling off the first run of distillate. Or, just running the whole reaction on a smaller scale. Or I could just do as ordered and mix my reagents extra slowly.
In case anyone wants to know, I titrated the nitric acid that was more dilute and I got 58% nitric acid. Adjusting for innacuracies I'd say about 53-55%.
Man you have 2 heating mantles Sick.
let's cook yo
With your fume hood that is just going out side or are you pushing it through some kind of carbon filter? And great vids yes lab envy oh lots of lab envy......thanks again. My interest is the aqua rega
not a chemist just love this stuff but from watching cody,s lab i thought you could not dissolve copper in pure (68%) nitric as it coated the copper and prevented further reaction , did you add water to your jar ?
I guess you´re talking about fuming nitric acid here (about 100%), azeotropic nitric acid (68%) does pretty well in dissolving copper :)
zeue hcucu Exactly.
100% pure nitric acid is not possible... the rest is obviously, water.
Juan Lopes yes, it is possible. Reply if you want the description of the process.
Can you extract the water from already azeotropic acid? perhaps adding a hydroscopic nitrate salt?
YOU SHOULD TEACH
What will happen if you add molecular sieves to the 68% nitric acid? Will it make it more pure or will the sieves absorb nitric acid too?
The molecular sieves are destroyed by strong acids
Not a chemist :) i read something about ozone reacting with air n2 mostly ? forming nitrous oxide n20 then bubbling it thru water will form nitric acid (weak) author was skimming over this because his point was that insuring no n2 reaction prior to bubbles 100% ozone ( i guess mixed with o2) ozone is amazing at at oxidizing water or whatever but i digress. could nitrous oxide be made to bubble thru perhaps at some pressure in 68% nitric acid to form nitric acid withing that 32% water of the solution or is there better (maybe free ways) I consider ozone free ish
0:01 it seems a breaking bad scene
Giuseppe 33 Only if he started with the barrel with the bee on it
1-you can use vacuum hood instead of boiling Nitric acid to purify it.
2-you can get benefit for the nitrogen oxide in HNO3 by freezing the whole solution to force nitrogen oxide to combine with the diluted water and give HNO3 molecules.
3- you can use also H2O2 to dilute HNO3, this would increase the yield and form more HNO3 molecules.
4 HNO2 <-> 2 H2O + 2 N2O3
4 HNO3 <-> 2 H2O + 2 N2O5
2 N2O3 <-> 4 NO + O2
2 N2O5 <-> 4 NO2 + O2
4 NO + 2 O2 <-> 4 NO2
nitrous acid <-> water + nitrous anhydride
nitric acid <-> water + nitric anhydride
nitrous anhydride <-> nitric oxide + oxygen
nitric anhydride <-> nitrogen dioxide + oxygen
nitric oxide + oxygen <-> nitrogen dioxide
NO2 and NO are free radicals
NO2 = NOO
"Nitrosyl oxide"
HNO2 = NOOH
"Nitrosyl hydroxide"
HNO3 = NO2OH
"Nitryl hydroxide"
N2O5 = NO2NO3 = (NO2)2O
"Nitryl nitrate"
"Dinitryl oxide"
N2O4 = NONO3
"Nitrosyl nitrate"
N2O3 is deep blue
N2O5 is colorless
NO is colorless
NO2 is orange brown
N2O4 is colorless
high temp<-- 2 NO2 <-> N2O4 -->low temp
condense temp: 21C / 70F
freeze temp: -11C / 12F
(you yourself can freeze acid gas)
this means that lowering the temperature will draw the gas into the water.
HNO2 + H2O2 <-> HNO3 + H2O
NO + H2O2 <-> NO2 + H2O
H2O2 turns NO into NO2 and turns HNO2 into HNO3.
nitrous acid leads to nitrites
nitric acid leads to nitrates
enjoy
Hi Doug, I'm a huge fan. You have great methods, very safe and are very thorough. That is why I would like to see a video on Diethyl either and how you go about storing it and your methods of preventing peroxides. Look forward to your next video.....
Does the KNO3 need to be recrystallized first?
"slowly poors In stump remover" Hey that's not 100% potassium nitrate!
Do you still make videos?
do a tour of your lab!!!!
i need a help about making kno3 witout any nitrate salt PLEASE!!! can u make a video about making kno3 from nitric acid and potassium hydroxide i need your help (i have %65 concentrated nitric acid) thanks
Muhammed Can AYDOĞDU you can't really make it without a nitrate salt...
That is one beast of an apparatus.
It would be cool if you could condense some nitrogen dioxide too!
Can you think of anything that could substitute Nitric Acid?
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Mercury in a big bottle 4:41
these videos have gotten me into wanting to do chemistry, but i'm not sure if ill be able to ;-;
perfectly poached penguin if you're passionate and have money you can do it =p also some experience to be safe.
Hey demons, it's laboy
Ali Moeeny - 2015-05-22
Your videos are great, both they look good, and have great content. Just 30 seconds of intro is too much man. 10second max, 5 sec even better. Keep up the good work though.
Mr-Nice-Guy j - 2016-04-22
was going to say the same. 30 sec intro is way to long
scientia eterna omnes supera! - 2018-04-10
Ali Moeeny
I agree, but I kind of really like the intro
Michael Smith - 2019-03-27
It's to show you what he is doing, and why. It's not a good idea to do chemistry without at least knowing something about the reaction you are performing.