In this video I carry out the prep of potassium hexacyanomanganate(III) as described in Inorganic Laboratory Preparations pages 86-88.

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I react chunks of iron covered with sodium potassium cyanide (a byproduct of the sodium potassium cyanide synthesis) with ~6M HCl to produce very fine particles of Prussian Blue. The acid reacts with the cyanide ion to produce HCN in solution. The acid also dissolves the iron producing ferrous chloride. Oxygen in solution reacts with some of that producing ferric chloride. Once Fe(II), Fe(III), and CN- are all present Prussian Blue forms and precipitates out in fine particles. This is allowed to settle, the liquid is decanted, and the solid is rinsed with water. This process is repeated several times until all of the ferric chloride solution has been removed.

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Demonstration of the color changes an aqueous solution of K4[W(CN)8] undergoes when it's placed in direct sunlight. In reality this sequence of color changes took almost exactly an hour (the final change from maroonish-purple to bright purple is slow). This would make an excellent classroom demonstration of photo-chemistry and photo-decomposition of a chemical compound.

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In this video I prepare potassium octacyanotungstate from sodium tungstate dihydrate, potassium borohydride, and sodium potassium cyanide. HCN gas is generated as a byproduct of the reaction. This prep comes from "The Preparation of Potassium Octacyanotungstate(IV) Dihydrate" by JG Leipoldt, LDC Brock, and PJ Cillers. The DOI is 10.1002/zaac.19744070311

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Calcium carbide dropped into water generates highly flammable acetylene gas.

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In this video I try and fail to prepare samarium(II) iodide but I do succeed in producing samarium(III) iodide.

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In this video I make potassium hexacyanochromate(III) K3[Cr(CN)6] from potassium chromate.

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In this video I make potassium selenocyanate from potassium ferrocyanide and gray selenium powder.

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In this video I make silver chlorite from sodium chlorite and silver nitrate. I then demonstrate how unstable this compound is and how it will explode on percussion when mixed with sulfur. Silver chlorite reacts explosively with a number of other substances and all in all is a pretty dangerous (but also really fun) compound.

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Please consider supporting this channel! Thank you! :-) In this real time video I demo a mix of chems so powerful that it completely dissolved a 16.53 gram tungsten rod in about 4 minutes. This mix of chems is a molten 1:1 mix of potassium nitrate and potassium hydroxide and it's so strong that virtually no metal can withstand it.

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Niobium metal reacts with molten KOH to produce potassium niobate and hydrogen gas. The melt is so hot that the hydrogen bubbles exploded on contact with air.

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Niobium metal burning in an atmosphere of bromine vapor and argon in real time.

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In this video I prepare niobium pentabromide from coarse granulated niobium metal and bromine. The niobium reacts with the bromine vapor (not the liquid) and niobium pentabromide distills off. To obtain a bottled pure product this prep should be done with a horizontal apparatus using a large diameter quartz glass tube. Not having one of those I had to settle for making the compound and then allowing it to decompose after taking it out of the apparatus to produce niobic acid (hydrated niobium pentoxide).

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In this video I prepare the interhalogen compound iodine monobromide from equimolar amounts of elemental bromine (10 grams) and elemental iodine (15.88 grams). IBr is an interesting compound since the iodine bears a partial positive charge and the bromine a partial negative carge. IBr is used to cleave carbon-metal bonds to produce organic iodides and metal bromides. It is also used to convert alkenes into vicinal bromoiodides, effect the electrophilic cyclization of homoallylic carbonates, and alpha-bromination of steroidal aldehydes and ketones. IBr has also been used for brominating phenol and aryl ether derivatives. (Information taken from the Encyclopedia of Reagents for Organic Sythesis).

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In this video I demonstrate how to do thin layer chromatography by carrying out the process on harmala alkaloid extracts from three different plants: peganum harmala (syrian rue), passiflora incarnata (passion flower), and banisteriopsis caapi (the ayahuasca vine). I also discuss the various harmala alkaloids in detail as well as the use of thin layer chromatography to monitor the progress of organic syntheses.

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In this video I prepare sodium orthotellurate Na6TeO6 from telluric acid Te(OH)6 using molten sodium hydroxide. Just a heads up the text in the video is a little screwy for some reason. They are still readable so I decided to go with it rather than spend hours trying to fix it. I will make sure the text is fixed in the next video.

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In this video I demonstrate an analytical technique often used in organic chemistry to confirm the identity and/or purity of a solid compound with a reasonably sharp melting point.

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This synthesis is the first step in the conversion of vanillin to 3,4,5-trimethoxybenzaldehyde, the immediate precursor to mescaline. The prep of 5-bromovanillin from vanillin and bromine in methanol is an easy prep to carry out and would be a good organic synthesis for a beginner amateur chemist.

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In this video I carry out the prep of beta-nitrostyrene from benzaldehyde and nitromethane as described in Vogels Textbook of Practical Organic Chemistry, 5th Edition, page 1035. This type of reaction is called a Henry Reaction and it has great synthetic utility as a carbon-carbon bond forming reaction. This kind of reaction featured heavily in the various synthetic procedures given in PIHKAL although I should stress that beta-nitrostyrene itself is neither listed nor controlled and can't be used to make any controlled substance that I am aware of (not easily anyways).

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In this video I prepare α-tellurium trioxide TeO3 from orthotelluric acid Te(OH)6 or as it is more commonly written H6TeO6. α-TeO3 is more reactive than β-TeO3 and forms tellurates on reaction with strong alkali. Hot tellurium trioxide is also a powerful oxidizing agent.

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Please consider supporting this channel! Thank you! :-) In this video I carry out a superior prep of pure selenic acid from elemental selenium using a technique that I read about on atomistry's page about selenic acid (linked below). Crushed gray selenium is dissolved in HNO3 and the resulting mixture of HNO3 and H2SeO3 is oxidized using one of several reagents. I chose elemental bromine but chlorine can be used if steps are taken to prevent the HCl formed from reducing selenic acid back to selenous acid (HBr does not have this problem which is why I went with Br2 instead). Other choices are potassium bromate, potassium permanganate, or you could just dissolve selenium in chloric acid. Once oxidized the mixture is made slightly alkaline with ammonia water and then the selenate ion is precipitated out by addition of aqueous barium chloride. The barium selenate is filtered off (it filters very easily unlike barium sulfate), rinsed well, and then mixed with slightly less than the stoichiometric amount of 1.65M H2SO4 (any dilute strength is OK). The mix is heated, the barium sulfate filtered off (UGH!) and then the solution evaporated down at a temp of less than 120C to give pure aqueous selenic acid.

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In this video I prepare selenium dioxide from pellets of elemental selenium. The final product is sublimated in order to purify it. Selenium dioxide is a precursor to many other selenium compounds and it is also a reagent in organic synthesis (Riley oxidations).

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A short video showing selenium dissolving in hot, concentrated nitric acid to produce a mixture of selenous acid and selenic acid. The brown gas is nitrogen dioxide.

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In this video I first convert chunks of elemental tellurium into what is probably tellurium dioxide. This is then used to prepare (NH4)2TeCl6 from ammonium chloride and HCl.

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Rhodanide Video "Chemistry short: Tellurium Decaoxotrisulfate"
https://www.youtube.com/watch?v=sd-i0WOPEz8

In this video I prepare (ACN)2Pd(NO2)2 from (ACN)2PdCl2 using silver nitrite that I prepared from silver nitrate and sodium nitrite. Bis(acetonitrile)dinitropalladium(II) is used in organic chemistry for the oxidation and nitration of alkenes (Encyclopedia of Reagents for Organic Synthesis).

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