Make Potassium Nitrate from Instant Cold Packs and Potassium Hydroxide
Warning: This reaction will produce large quantities of toxic ammonia gas. Perform the reaction outside or in a fume hood. Potassium hydroxide is highly corrosive; wear gloves when working with it.
Also note that this video is for those interested in the chemistry, it's not cheaper/better/easier than buying it.
Some instant cold packs contain ammonium nitrate as their active ingredient and when mixed with potassium hydroxide will produce potassium nitrate and ammonia gas.
Get an instant cold pack that clearly says it contains ammonium nitrate, cut it open, and pour the contents into a container. If its unused there will be a water pouch that you can discard. The rest of the pack is ammonium nitrate. Usually its coated in an anti-caking agent so it'll be off-color.
Some lab notes for the month of august 2020
I was exploring more nitric acid and wanted to see if calcium nitrate and sodium bisulfate would be viable. The rationale is that the reaction of calcium nitrate and sulfuric acid is well-known but almost never done directly since it produces insoluble calcium sulphate that solidifies into a rock in the flask. It has to be drilled out and risks break the flask. The traditional way to use calcium nitrate is the "wet process" where we first mix it with water and then add sulfuric acid. The calcium sulfate precipitates out and the dilute nitric acid is filtered and purified by distillation. This is slow and laborious so i was wondering if sodium bisulfate could be advantageous in producing a residue that didn't need to be drilled. This would save time and less risk of breaking glassware.
So i mixed 49g of calcium ammonium nitrate decahydrate with 150g of sodium bisulfate monohydrate and heated it directly in the "dry process" of making nitric acid. Nitric acid was distilled over and the yield was 85%. But more importantly the solid residue of sodium sulfate, sodium bisulfate and calcium sulfate was soluble. Upon addition of water it dissolved into a slurry that could easily be poured out. So i think the process is superior to using sulfuric acid as there is overall less labor involved.
For thoroughness i also tried the wet process by first dissolving the calcium nitrate in 50mL of water and adding sodium bisulfate. After distillation the yield was 95% but with 50mL of extra water diluting it. Personally i prefer higher concentration acid and don't mind the lower yields of the dry process.
Anyway. I was going to do additional nitric acid experiments but my hotplate failed.
Turns out the temperature sensor failed open and the safety limit of the hotplate refused to turn it on. It was a simple matter of finding the broken sensor and replacing it. The interesting note is that the hotplate uses a PT1000 RTD and it seemed the original was spot welded in. I didn't have spot welding capability so i used copper foil to crimp the connection.
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https://www.youtube.com/watch?v=Xa2OMNaHn_Y
We demonstrate the magnetic properties of dysprosium nitrate.
Dysprosium nitrate is paramagnetic and is thus attracted to a magnetic field. The salt itself is clear with a beige/yellow tinge and is thus quite unusual among common magnetic materials that are usually opaque or metallic. By itself dysprosium isn't very useful but can adjust the magnetic properties of other materials and is therefore very useful to make the components of motors, actuators and hard drives.
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https://www.youtube.com/watch?v=4YSmr1psa_0
Paramagnetic fluid or “parafluid” is a fluid that is attracted to a magnet. It’s weaker than the more famous ferrofluid but is transparent and somewhat easier to make. To make it, a paramagnetic salt like manganese (II) nitrate is dissolved in water until saturated. The solution is paramagnetic and will be attracted to a magnet. But because it’s so weak the attraction is limited. To assist, a density matched suspension of the parafluid in an immiscible carrier fluid is needed. In this video, dichloromethane was used and the correct density for the solution of manganese nitrate and water was found by trial and error.
Chloroform is an even better carrier fluid and in fact is dense enough that it must be diluted with dichloromethane instead of the manganese nitrate solution. I recommend using using chloroform and dichloromethane if you have it. I didn't use it at the time of the video because I didn't have it on hand.
Other paramagnetic salts include manganese (II) chloride, manganese (II) sulfate, gadolinium nitrate, dysprosium nitrate, etc.
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https://www.youtube.com/watch?v=MUKFaxy-z7s
We gather up our observations and data so far and construct a mechanism. In doing so we notice a few gaps and use them to find even better catalysts for the sodium production reaction.
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Through Patreon (preferred): https://www.patreon.com/NurdRage
Through Bitcoin: 1NurdRAge7PNR4ULrbrpcYvc9RC4LDp9pS
Glassware generously provided by http://www.alchemylabsupply.com/
Use the discount code "nurdrage" for a 5% discount.
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In this video we make triboluminescent or smash-glow crystals.
Triboluminescence is the phenomena where light is generated when something is rubbed or fractured. The exact mechanism by which triboluminescence works is still under investigation, but the best theories so far propose that the breaking of the structure causes charge separation that release energy upon recombination. This energy is picked up by nearby atoms, in this case europium, and released as light according to their ionization or fluorescence spectra.
Many substances exhibit triboluminescence including sugar and tape. But Europium Tetrakis (Dibenzoylmethide)Triethylammonium is one of the strongest available and its glow can easily be captured by a camera.
It's made by mixing 100mL of Ethanol, 2.93g of dibenzoylmethane, 1.4g of europium nitrate pentahydrate and 1.9mL of triethylamine. The mixture is heated until everything dissolves and then allowed to cool slowly to obtain crystals that are filtered off and washed with ethanol. After thorough drying they are ready for use.
A frequently asked question is if this stuff is hot when it is used. The answer is no, the crystals do not undergo a chemical transformation and thus they do not release or consume heat, but remain at constant temperature. There may be some small heating due to friction when they are broken, but that is not from the crystals or a special property of triboluminescence.
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https://www.youtube.com/watch?v=xQhLSoB-uBE
In this video we make "Wildfire" from Game of Thrones.
I've collaborated with my friend PixelLitch and sent him the bottle of wildfire which he used in his video here:
https://www.youtube.com/watch?v=UkwaE0J5QFM
The wildfire in this video is actually an azeotropic mixture of trimethyl borate and methanol. Trimethyl borate burns with an intense green flame that looks very much like wildfire from "Game of Thrones".
To make it we mix 200g of Borax, 650mL of methanol and 100g of sulfuric acid (98%). We then set up a fractional distillation column and distill of the fraction at 54 degrees Celsius which is azeotropic trimethyl borate.
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https://www.youtube.com/watch?v=iyHOBQl-yQI
In this video we purify sulfuric acid by distillation using a heating mantle we built in a previous video.
The reason why we need a special heating mantle is because most don't get hot enough to boil sulfuric acid.
Click here for our original video on how to make a high temperature heating mantle:
http://www.youtube.com/watch?v=N5meDWAqYes
The heating mantle in the video is connected to a variac autotransformer off-camera. But a light dimmer switch can provide the same power control for a fraction of the cost. Alternatively, a PID controller may be used.
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https://www.youtube.com/watch?v=tgUH0HXrOKE