Damnit!!! I was just reading up on this very compound the other day on atomistry. Now I have to come up with another one to make. Why do you have to raise the bar so damn high for with extremely awesome preps like this? You're killing me here! 😜😂
@@PoorMansChemist Relaaax.... a little OsO4 never hurt anyone... well maybe it did. Maybe it even killed someone... multiple people... just do osmium chemistry dammit!!
@@friskydingo5370 The osmyl bromide salts do exist, but they're much more difficult to make (which is okay, because failure in either direction results in either osmyl oxybromide salts or osmium hexabromide, both of which would be cool).
I knowticed that the Os precipitate formed when the mixture was exposed to air. When you put the cap back on it drove the reaction to re desolve. This might be due to the Cl gass forming and being trapped. The reaction you saw in the beginning might require some air. It just an observation. However, it might help you figure out what was exactly going on. 👍
In the first attempt, you can see the OsO4 wetting the glass just before it gets reduced. It was interesting to see it crash and re desolve. The 2nd attempt, the addition of magnesium, might have precipitated some metallic os. I'd try different reagents until you find the best one. It should crash out fast and not re desolve. It's looks like an iodine clock reaction 😂. Just curious did you ever have the os Xrf. I just found out most of my sintered os is only 91 percent pure. That might account for the aprox 10%loss I found it totaly amazing that it came with a coa it had me fooled for years untill I had it xrf. 2 samples from 2 diffrent sources showed up at 91 and 90 percent. This might explain a lot. The major impurities were ruthenium and tungsten. Both were from reputable companies. I'd have everything checked just to be sure. As far as the re desolve you probaly just need to adjust the amount of reagents you use. Thanks for the video😊 Stay awesome 👌
That was the osmic acid. It's supposed to crash out and redissolve. That's what I wanted originally, but perhaps the use of concentrated HCl was too much and the solution needed to be less acidic. Osmic acid is one of the most important building blocks of osmium chemistry. So if you see it crash out temporarily, that's a good sign.
@The_OsmiumChannel Yah, that is what you mentioned yesterday looks like you were right. Extremely interesting stuff. I knew the chemestry would work for ruthenium I never thought about it with osmium. The sodium hypochlorte rought never occurred to me. Grate job and I'm sure you'll improve your results. Looks like exactly what you said. To much HCL
@@The_OsmiumChannel I have a friend who runs the Neptunium channel. He had a GC-MS maby you can ask him to have a look at your result. He has some grate videos as well check him out and tell him I referred you. 😊
@@The_OsmiumChannel 😁😉 yup. I've always gone the easy route of O2 and heat in sealed glassware and then distilling off the OsO4 then reduceing it. It is much easier to handle in watter. Your aproch is defantaly unique. The most comon ways are some you have mentioned before that require a furnace and molten alkaline. Your aproch is unique and deserves further experimentation. I look forward to our next video.
Very interesting and I liked the addition of mg at the end. Do you need sintered or compressed powdered osmium to be able to disolve it in hot hypochlorite/hydroxide bleach or can a normal bead be disolved this wayalbeit much slower?
@@SodiumInteresting Every time I've tested Os beads in hot bleach, they don't lose enough mass to register a difference on my scale. It's also possible I didn't heat them long enough or hot enough. Sintered osmium surprised me. I'm sure at points in the video you saw the bleach wasn't always boiling, and yet the bullion was still dissolving noticeably quick, but that was only after enough of the smooth exterior dissolved. For a bead I'd recommend 12% industrial strength bleach, and add a good amount of NaOH to it as a safety precaution.
Great Video. What is ratio of Sodium hydroxide and Sodium hypochlorite in accordance with its weight? The sodium hydroxide is dissolved in the Sodium hypochlorite 10% solution, that's right?
Damnit!!! I was just reading up on this very compound the other day on atomistry. Now I have to come up with another one to make. Why do you have to raise the bar so damn high for with extremely awesome preps like this? You're killing me here! 😜😂
@@PoorMansChemist 😁😂😂 I guess you'll have to go the bromine route.😁
@@PoorMansChemist your clorab video was amazing 👏
@@PoorMansChemist Relaaax.... a little OsO4 never hurt anyone... well maybe it did. Maybe it even killed someone... multiple people... just do osmium chemistry dammit!!
@@The_OsmiumChannel I see a shirt in the future. It says " chemestry is dangerous (dangerous crossed out) is FUN 😁
@@friskydingo5370 The osmyl bromide salts do exist, but they're much more difficult to make (which is okay, because failure in either direction results in either osmyl oxybromide salts or osmium hexabromide, both of which would be cool).
Those sparkles at the end made for a magnificent surprise this was very unique chemistry.
I knowticed that the Os precipitate formed when the mixture was exposed to air. When you put the cap back on it drove the reaction to re desolve. This might be due to the Cl gass forming and being trapped. The reaction you saw in the beginning might require some air. It just an observation. However, it might help you figure out what was exactly going on. 👍
In the first attempt, you can see the OsO4 wetting the glass just before it gets reduced. It was interesting to see it crash and re desolve. The 2nd attempt, the addition of magnesium, might have precipitated some metallic os. I'd try different reagents until you find the best one. It should crash out fast and not re desolve. It's looks like an iodine clock reaction 😂.
Just curious did you ever have the os Xrf. I just found out most of my sintered os is only 91 percent pure. That might account for the aprox 10%loss I found it totaly amazing that it came with a coa it had me fooled for years untill I had it xrf. 2 samples from 2 diffrent sources showed up at 91 and 90 percent. This might explain a lot. The major impurities were ruthenium and tungsten. Both were from reputable companies. I'd have everything checked just to be sure. As far as the re desolve you probaly just need to adjust the amount of reagents you use. Thanks for the video😊
Stay awesome 👌
That was the osmic acid. It's supposed to crash out and redissolve. That's what I wanted originally, but perhaps the use of concentrated HCl was too much and the solution needed to be less acidic.
Osmic acid is one of the most important building blocks of osmium chemistry. So if you see it crash out temporarily, that's a good sign.
@The_OsmiumChannel Yah, that is what you mentioned yesterday looks like you were right. Extremely interesting stuff. I knew the chemestry would work for ruthenium I never thought about it with osmium. The sodium hypochlorte rought never occurred to me. Grate job and I'm sure you'll improve your results. Looks like exactly what you said. To much HCL
@@The_OsmiumChannel I have a friend who runs the Neptunium channel. He had a GC-MS maby you can ask him to have a look at your result. He has some grate videos as well check him out and tell him I referred you. 😊
@@friskydingo5370 Yeah ruthenium probably would have formed the RuCl3. Osmium compounds are like "you know, I'd rather just go +8"
@@The_OsmiumChannel 😁😉 yup.
I've always gone the easy route of O2 and heat in sealed glassware and then distilling off the OsO4 then reduceing it. It is much easier to handle in watter. Your aproch is defantaly unique. The most comon ways are some you have mentioned before that require a furnace and molten alkaline. Your aproch is unique and deserves further experimentation. I look forward to our next video.
Very interesting and I liked the addition of mg at the end.
Do you need sintered or compressed powdered osmium to be able to disolve it in hot hypochlorite/hydroxide bleach or can a normal bead be disolved this wayalbeit much slower?
@@SodiumInteresting Every time I've tested Os beads in hot bleach, they don't lose enough mass to register a difference on my scale. It's also possible I didn't heat them long enough or hot enough.
Sintered osmium surprised me. I'm sure at points in the video you saw the bleach wasn't always boiling, and yet the bullion was still dissolving noticeably quick, but that was only after enough of the smooth exterior dissolved.
For a bead I'd recommend 12% industrial strength bleach, and add a good amount of NaOH to it as a safety precaution.
Great Video. What is ratio of Sodium hydroxide and Sodium hypochlorite in accordance with its weight? The sodium hydroxide is dissolved in the Sodium hypochlorite 10% solution, that's right?
And how many temperature for this reaction?