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Bedlasky
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[*] posted on 5-5-2019 at 08:54


I had solution of hypomanganate in fridge stable for at least 20 minutes. I wasn't really examine stability of solution, I just dilute it and pour in to the drain. But now it's interested me, I will let you know when I test it.

Quote: Originally posted by maxstar  
Again, dark blue sediment appears.


In my experience - mixed solution of manganate and permanganate have dark blue colour (see starting chemical chameleon or try put excess of permanganate to alkaline solution of thiosulfate). But this is precipitate - this may be different.
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woelen
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[*] posted on 18-5-2019 at 12:55


I made K2Cr3O10 and ampouled this.


I made this chemical by dissolving K2Cr2O7 and some CrO3 in boiling hot highly concentrated HNO3 (70% or so, maybe even a little more). The nitric acid I made by distillation from H2SO4 and KNO3 and a little water to make really concentrated acid. In such concentrated acid an amazingly large amount of K2Cr2O7 can be dissolved and when that is done, then it also is possible to dissolve some CrO3 in it as well. In order to do so, the liquid must be boiling hot, otherwise you don't get all of it dissolved.

After that, I put the flask with the acid and dissolved chromium compounds in a hot water bath, which I slowly let cool down. The next day I had a big crop of beautiful red K2Cr3O10. I put this on a glass fritte and used some paper tissue on the other side of the fritte to absorb the acid and any CrO3 which still is dissolved in it. This was quite scary, the acid with CrO3 is a very harsh oxidizer and after ten seconds or so, the paper tissue with acid soaked in it starts to fume and hiss. So, I had a bucket with water nearby and dumped the paper tissue with absorbed acid in that immediately. I repeated this procedure until no more acid could be absorbed in paper tissue. At this point, the solid already was quite dry.
Next, I put the solid in a petri dish and put it in an oven at 100 C for 20 minutes or so. I finally put the petri dish in a plastic jar, in which I also put a small dish, full of NaOH. This absorbs acid vapor and after several days I had a perfectly dry product, which could be ampouled nicely.

Below follow pictures of the ampouled product on a white background and on a black background:


K2Cr3O10.jpg - 895kB


K2Cr3O10_on_black.jpg - 1.5MB


I also made pictures where the compound is kept near the container of my K2Cr2O7. These pictures nicely show the difference between K2Cr2O7 and K3Cr3O10.

K2Cr2O7_K2Cr3O10.jpg - 1.9MB

K2Cr2O7_K2Cr3O10_on_black.jpg - 1.9MB

Once the K3Cr3O10 is completely dry and free of acid, it is not hygroscopic anymore, and it can be kept around very well. I will use this sample in my element collection as an addon to the chromium sample (together with Cr2O3, CsCr-alum, K2CrO4, K2Cr2O7).


[Edited on 18-5-19 by woelen]




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[*] posted on 20-5-2019 at 06:34


Very nice! I'm also curious what it would look like next to CrO3. Is it an intermediate between the oxide's dark red and dichromate orange?
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woelen
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[*] posted on 20-5-2019 at 11:58


It indeed is an intermediate color. CrO3 is darker.
I can make a picture of K2Cr3O10 besides some CrO3. Expect that picture one of these days . . .




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Bedlasky
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[*] posted on 23-5-2019 at 10:55


Interesting compound with beautiful colour. Sadly I saw this compound only on pictures :(.
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[*] posted on 23-5-2019 at 23:42


Hi.

Here is photo of one of my crystals of ammonium-ferric sulfate. Crystal weight is 37,7g. On photos has beautiful pale violet colour but currently is transparent on edges (but middle is still pale violet) and surface is little bit rusty but it doesn't become rusty even more. I store it in paraffin oil to prevent water losses (on the air it lose water and becomes rusty).

IMG_20190513_210044.jpg - 2MB IMG_20190513_212630.jpg - 2.1MB
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[*] posted on 26-5-2019 at 12:27


orangePeels.jpg - 145kB
Figure 1: I started stockpiling orange peels in my freezer, telling myself that I'd steam distill them some day. By the time the freezer was full & I got around to the project, I had 2.63 kg hoarded.

organgeOil.jpg - 46kB
Figure 2: When I was done, I had 41.80 g of orange oil collected, for a dry mass percent of ~1.6% oil. I measured its density as 0.837 g/mL.

Also, my house smelled like Froot Loops the whole time :cool:





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[*] posted on 26-5-2019 at 15:56


@mayko
Nice! That's the largest batch of limonene extraction I've ever seen!




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[*] posted on 26-5-2019 at 22:44


That's interesting. How much solvent did you need for this extraction? And what solvent did you use? Did you recover the solvent by distilling it off and using it again? Could you provide some more details on how the extraction was done?

Another question I have is what you can do with this orange oil? Does it have some specific interesting chemical properties, which can be used in nice chemical experiments?




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[*] posted on 27-5-2019 at 05:34


Quote: Originally posted by woelen  
That's interesting. How much solvent did you need for this extraction? And what solvent did you use? Did you recover the solvent by distilling it off and using it again? Could you provide some more details on how the extraction was done?

Another question I have is what you can do with this orange oil? Does it have some specific interesting chemical properties, which can be used in nice chemical experiments?


I hope he used steam distillation, it's relatively fast, in one morning I processed about 1kg of peels in a few batches, using a solvent would require lots of it (just to cover the peels) and even more for washings, the beta carotene would also be extracted so a distillation is mandatory. Meh steam distillation is better:D
The oil should be mainly limonene, it's used as a solvent

Quote: Originally posted by mayko  
Got some orange peels steam-distilling, no broken glassware yet!

EDIT found this in everyday chemistry hahaha



[Edited on 27-5-2019 by Ubya]





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[*] posted on 30-5-2019 at 04:54


Yep, this was a steam distillation... actually several. I've never really gotten the hang of the technique so I decided to just do it over and over for practice. I hadn't thought as far ahead as a use for the orange oil! I might mix some with alcohol and spray it on paper to make scented stationery for my letter writing. :)

In the process I learned that orange oil is produced industrially from the waste from orange juice production by pressing rather than steam distillation.




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[*] posted on 3-6-2019 at 01:56


Here's some Uranyl Nitrate sample and Thionyl Bromide :)

SAM_5864.JPG - 1.9MBSAM_5867.JPG - 2MB
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[*] posted on 3-6-2019 at 02:11


shouldn't uranyl nitrate be UO2 (NO3)2?
is that an uranium (IV) (with oxygen!?) nitrite?
i think you messed up the formula a bit:D





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[*] posted on 3-6-2019 at 02:47


@Chemscience how much is that?:o



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[*] posted on 3-6-2019 at 03:13


That sample of uranyl nitrate is beautiful.

@Ubya: Uranyl ion has uranium in its +6 oxidation state. The ion is UO2(2+) and the nitrate salt is UO2(NO3)2.




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[*] posted on 3-6-2019 at 03:47


Quote: Originally posted by fusso  
@Chemscience how much is that?:o


Just enough to convince me to get my own !

Oh please do post a picture in UV light :)
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[*] posted on 3-6-2019 at 04:10


Fresh made Picric acid drying out befor being converted to Ammonium Picrate

https://en.wikipedia.org/wiki/Picric_acid

https://en.wikipedia.org/wiki/Dunnite



20190602_203621.jpg - 2MB

Some Iron 2 Sulphate for a 1,4, Dioxan synth I have planed along side some Copper Nitrate



[Edited on 3-6-2019 by XeonTheMGPony]

P8150594.JPG - 1.3MB
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[*] posted on 3-6-2019 at 09:18


Ups ... Sorry :) Yup i did messed up the formula jej e.. Sorry .. Nex post is on UV for Herr Haber and the correct formula =) .. btw nice Ferrous Sulphate.I'm very interested in your synthesis of Dioxane, so i'm expectant for the post :)
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[*] posted on 4-6-2019 at 17:39


Here's 20gr of Uranyl Nitrate in UV light :)

SAM_5883.JPG - 1.5MBSAM_5885.JPG - 1.5MB
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[*] posted on 5-6-2019 at 03:35


Quote: Originally posted by woelen  
That sample of uranyl nitrate is beautiful.

@Ubya: Uranyl ion has uranium in its +6 oxidation state. The ion is UO2(2+) and the nitrate salt is UO2(NO3)2.


yup i know, i was messing around trying to interpret the wrong formula:P

@chem science: beautiful sample, uranium is one of my favourite elements, if not the most





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[*] posted on 7-6-2019 at 11:51


6-Monodeoxy-6-monoazido-beta-cyclodextrin synthesized via refluxingMono-6-O-(p-toluenesulfonyl)-β-cyclodextrin and sodium azide in an aqueous solution..
Used as synthetic intermediate. The azide is reduced to make 6-Monodeoxy-6-monoamino-beta-cyclodextrin or used in click chemistry to attatch subsituted functional groups which can be used to bind/trace movement in vivo. One example is performing an amidation reaction between the amino-cyclodextrin and biotin( biotinylation). When tested on mice, the movement of the cyclodextrin within the cell can be traced by introduction and binding of streptavidin or avidin. Cyclodextrins can act as "cages" for molecules such as steroids and facilitate drug delivery. B-cyclodextrin itself is combined with DMSO and a specific therapeutic drug to permit effective drug delivery through cellular walls.

IMG_0108.JPEG - 1.1MB72.png - 6kB
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[*] posted on 13-6-2019 at 03:15


some tetraphenylcyclopentadienone made at uni

20190612_234333-1.jpg - 756kB





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[*] posted on 13-6-2019 at 04:46


Ubya,

Whoops! You need to change the name of your compound or the structure on the page.

AvB
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[*] posted on 14-6-2019 at 05:11




20190614_150530-1.jpg - 522kB

AvB you are totally right, my bad.



ps can't edit my last post (can't edit any of mesagges on this thread but this one, the button is not there, wtf?)

[Edited on 14-6-2019 by Ubya]





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[*] posted on 14-6-2019 at 05:13


Black organic compound?Weird.



Useful sites:
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Molecular mass and elemental composition calculator: https://www.webqc.org/mmcalc.php
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