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gluon47
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Ok, thanks for your help
reality is an illusion 
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CharlieA
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Quote: Originally posted by HeYBrO  | no i doubt it, the doubly bonded carbon ( called a cumulated diene or allenes) is sp2 so would be linear and hence there would be significant ring
strain and the bond to N and C being stretched would make it very unstable. any one else want to add?
I have to go with you on this one. With my framework Darling models I couldn't get the ring to close with a sledgehammer... and I didn't want to break
my models. |
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Ramium
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Would diacetone alcohol work as a catalyst for the production of potassium from potassium hydroxide and magnesium? Its a tertiary alcohol just like
other common catalysts such as tert-butanol.
Any ideas?
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Darkstar
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| Quote: Originally posted by Ramium | | Would diacetone alcohol work as a catalyst for the production of potassium from potassium hydroxide and magnesium? Its a tertiary alcohol just like
other common catalysts such as tert-butanol. |
There are two problems here. First, diacetone alcohol has a carbonyl group that would get reduced to a ketyl by both magnesium as well as potassium.
Second, the highly basic conditions would just deprotonate the carbon between the carbonyl and hydroxyl group, dehydrating the diacetone alcohol to
mesityl oxide, which now has a conjugated pi-system that is even more prone to reduction.
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Ramium
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Oh ok. Thats unfortunate. Thanks anyway
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CharlieA
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| Quote: Originally posted by CharlieA | | Quote: Originally posted by HeYBrO | no i doubt it, the doubly bonded carbon ( called a cumulated diene or allenes) is sp2 so would be linear and hence there would be significant ring
strain and the bond to N and C being stretched would make it very unstable. any one else want to add?
I have to go with you on this one. With my framework Darling models I couldn't get the ring to close with a sledgehammer... and I didn't want to break
my models. |
I tried to connect the allene moiety with models this morning. The best I could do was an 8-membered ring containing the allene oiety and 1
tetrahedral N and 4 tetrahedral carbons, and this structure also seemed to have a little strain. |
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Ramium
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One more question
Would chlorbutol (trichloro-2-methyl-2-propanol) work as a catalyst for potassium production from KOH and Mg?
Its a tertiary. Maybe the three chlorine atoms would be a problem?
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Romix
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Acetic acid
Can acetic acid be made from recrystallized copper acetate?
By displacing copper with lead, and adding HCl to it?
Last time I tried, it didn't crystallize out in cold. Because of low concentration?
Acetate of copper seems to be more stable then chloride.
[Edited on 5-4-2016 by Romix]
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Metacelsus
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Yes, the chlorine atoms would be a problem, as you noticed.
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Texium
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Threads Merged
5-4-2016 at 09:01 |
Jstuyfzand
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Gold anodes
Can gold be used as an anode in brine electrolysis or things like copper sulphate?
I can get gold plated things from electronics, its much more common than platinum.
I tried a small gold plated wire, it turned black!
Thoughts?
Thanks!
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Darkstar
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| Quote: Originally posted by Ramium | Would chlorbutol (trichloro-2-methyl-2-propanol) work as a catalyst for potassium production from KOH and Mg?
Its a tertiary. Maybe the three chlorine atoms would be a problem? |
Yes, they would be a problem, as already mentioned. Keep in mind that magnesium and potassium are both extremely powerful reducing agents. This means
you're going to need an alcohol that doesn't have any easily reducible functional groups or they will react with both your initial magnesium metal, as
well as any potassium metal that does form. The reaction conditions are also going to be highly basic as well, so your alcohol can't have a bunch of
acidic protons that will get removed by the hydroxide and alkoxide ions, or by reduction from the magnesium or potassium metal. (although, in this
case, there aren't any)
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Bean
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Fischer Esterification
I was wondering if sulfamic acid could be used as a catalyst for Fischer esterification or even making ethers such as diethyl ether. Does anyone have
experience using this. According to Wikipedia it can be used for esterification, but I am unsure if this applies to all reactions for example between
ethanol and ethanoic acid etc. It also has a pKa of 1.0, is this suitable. Also, apparently when it reacts with alcohols organosulfates are formed-
could this allow it to be used to produce ethers?
Thanks.
[Edited on 8-4-2016 by Bean]
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IceDahl
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Calcium Nitrate
I found something that I find quite strange. Calcium nitrate is rated "3" on the Instability/reactivity part of the Fire Diamond. While potassium
nitrate and sodium nitrate is 0 on the yellow.
The "3" on the yellow is desctibed as: "Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under
confinement before initiation, reacts explosively with water, or will detonate if severely shocked".
Is calcium nitrate really so unstable compared to sodium or potassim nitrate?
I have heated small amounts of calcium nitrate with a butane torch before but nothing happened.
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Mabus
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Is that Fire Diamond used for anhydrous Ca(NO3)2 or for the tetrahydrate form?
Because I can see reason for the anhydrous form, but not for the hydrate.
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UC235
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No, sulfamic acid undergoes solvolysis in alcohols to yield ammonium alkylsulfates which are only a slightly acidic salt. It's an interesting prep but
not too useful.
Even if it didn't undergo solvolysis, for Fischer esterification, you really need a strong acid to have a good reaction rate. The acid needs to
protonate the alcohol. Alkyloxoniums have a pKa of ~-1.7 so you ideally want an acid with a lower pKa than that to achieve significant quantities of
the intermediate.
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Bean
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Thanks for the reply.
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Texium
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Threads Merged
8-4-2016 at 12:16 |
Texium
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Threads Merged
8-4-2016 at 12:18 |
The Volatile Chemist
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I recently dissolved some 99% Sn solder in HCl. All that's left out of solution is the resin core (the rest was 1% Pb). Is it feasible to crystallize
out a chloride of tin, or should I just precipitate it out as a hydroxide or basic carbonate or something...?
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Bean
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Sodium hydrogen sulfate (bisuslfate) as Fischer esterification catalyst ?
Thanks in advance,
Bean.
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Deathunter88
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| Quote: Originally posted by The Volatile Chemist | | I recently dissolved some 99% Sn solder in HCl. All that's left out of solution is the resin core (the rest was 1% Pb). Is it feasible to crystallize
out a chloride of tin, or should I just precipitate it out as a hydroxide or basic carbonate or something...? |
Yes, it is very possible to crystallise out tin(II) chloride if you leave some excess tin in solution and wait for the evaporation. (no heating!)
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S.C. Wack
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Heating isn't necessarily an issue. Blanchard gives directions that depend on heating (among other things), as the dihydrate crystallizes out of the
saturated solution on cooling. Vaporization by air will provide acidic air, dealt with in whichever way.
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The Volatile Chemist
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| Quote: Originally posted by S.C. Wack | | Heating isn't necessarily an issue. Blanchard gives directions that depend on heating (among other things), as the dihydrate crystallizes out of the
saturated solution on cooling. Vaporization by air will provide acidic air, dealt with in whichever way. |
Hmm, makes sense I guess, but I've seen many other metal solutions hydrolyzed (I think that's canon usage), so I'll try it with a little product
first.
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yobbo II
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(18) If f (โ1) = โ7 and f (x) = g(โ6 ยท x), what point must satisfy y = g(x)?
Can someone do this?
TIA
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aga
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Twelvety, obviously.
OK. This has been happening a lot recently.
It's time the wizard responsible owns up to synthesising a Hormunculus, again.
Yes, the Globe Bottles and any dried Mouse Blood will be taken away if you do, but that is all.
If not, and we Will find you, your bodkin shall be severely shriven.
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yobbo II
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This dude says sixthedy.
http://openstudy.com/updates/53b95693e4b09f140ca68b23
Thanks googness shakespeareannn is my first language.
Yob (licenced to diff.)
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Dr.Q
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What is the solubility of formaldehyde in isopropanol and ethyl acetate
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