| Pages:
1
..
86
87
88
89
90
..
104 |
mayko
International Hazard
Posts: 1218
Registered: 17-1-2013
Location: Carrboro, NC
Member Is Offline
Mood: anomalous (Euclid class)
|
|
When I harvest lithium foil from batteries, I try to store it under mineral oil, but between its low density and entrained bubbles, it floats to the
top. I could probably add paperclips and a weight or something to keep it submerged, but I wondered if anyone else had protips?
al-khemie is not a terrorist organization
"Chemicals, chemicals... I need chemicals!" - George Hayduke
"Wubbalubba dub-dub!" - Rick Sanchez
|
|
|
TheMrbunGee
Hazard to Others
Posts: 364
Registered: 13-7-2016
Location: EU
Member Is Offline
Mood: Phosphorising
|
|
Quote: Originally posted by mayko  | | When I harvest lithium foil from batteries, I try to store it under mineral oil, but between its low density and entrained bubbles, it floats to the
top. I could probably add paperclips and a weight or something to keep it submerged, but I wondered if anyone else had protips?
|
I think it would float even without bubbles. Try less dense inert liquid or put something heavy (also inert) on top.
You could also store it in inert gel, or even solid. (maybe paraffin wax) not sure about compatibility, so research.
|
|
|
ninhydric1
Hazard to Others
Posts: 345
Registered: 21-4-2017
Location: Western US
Member Is Offline
Mood: Bleached
|
|
I know MrHomeScientist ampouled some lithium metal in an inert atmosphere, which eliminates the density issue entirely.
The philosophy of one century is the common sense of the next.
|
|
|
C6(NO2)5CH2CH(CH3)N(NO2)2
Harmless
Posts: 43
Registered: 4-4-2018
Member Is Offline
Mood: No Mood
|
|
what will precipitate first? Calcium hydroxide or ammonia gas?
I have been wondering if you can produce ammonia and a calcium salt from hydrated lime and an ammonium salt. According to this post: http://www.sciencemadness.org/talk/viewthread.php?tid=7464&a... You can add calcium hydroxide to ammonium chloride to produce ammonia
2NH4Cl+Ca(OH)2-->CaCl2+2NH3+ 2H20. I'd assume that this reaction would go in this direction due to all the different ions being in solution, and
the unstable combination (NH4OH) decomposing and "precipitating" ammonia gas. But in this post: https://www.sciencemadness.org/whisper/viewthread.php?tid=83... it says that you can make ammonium nitrate out of calcium nitrate by adding
ammonia solution: 2NH4OH+Ca(NO3)2-->2NH4NO3+Ca(OH)2. I suppose that makes sense that the calcium hydroxide would precipitate too, since it is
poorly soluble in water (unlike ammonium nitrate) But it also means that adding the calcium hydroxide to an ammonium salt would probably fail to
produce any reaction.
So I guess my question is this: Which compound comes out of solution first? and (sorry if this is spoonfeeding) if you hypothetically added calcium
hydroxide to a saturated solution of Calcium nitrate-ammonium nitrate double salts, would I get calcium nitrate and ammonia vapor, or would nothing
happen? or would it be a partial reaction, and the calcium hydroxide would stop dissolving prior to all the ammonium nitrate being converted?
[Edited on 14-1-2019 by C6(NO2)5CH2CH(CH3)N(NO2)2]
Put that in your pipe and smoke it!
|
|
|
j_sum1
Administrator
Posts: 6335
Registered: 4-10-2014
Location: At home
Member Is Offline
Mood: Most of the ducks are in a row
|
|
purple zinc chloride
I discovered today that I don't have any zinc chloride. Never mind I thought. I have some zinc from a D cell and plenty of hardware-store HCl of
reasonable purity.
After reacting, the resultant solution was a purple/lilac colour. Berating myself, I concluded that stray manganese dioxide from the battery was the
most likely culprit. So I repeated with some reagent grade zinc powder.
Same result. It must be some impurity in the HCl. But what? I know that Fe is common but I have tested the acid for Fe in the past with a negative
result. Is Mn or Co likely?
[Edited on 15-1-2019 by j_sum1]
|
|
|
clearly_not_atara
International Hazard
Posts: 2800
Registered: 3-11-2013
Member Is Offline
Mood: Big
|
|
^Also, solutions of iron chloride are brown.
The HCl itself isn't colored, but with zinc it is? If it were a simple metal chloride the addition of zinc should not change the color. Mn or Co will
be present as the divalent salt which should not undergo any sort of redox in this condition.
However, maybe the HCl is a little greenish? That would indicate chromium, as CrCl3 gives a green solution and CrCl2 a blue one. Additionally various
aqua-chloro chromium complexes are slow to interconvert and have many different colors.
|
|
|
clearly_not_atara
International Hazard
Posts: 2800
Registered: 3-11-2013
Member Is Offline
Mood: Big
|
|
I noticed that the reaction:
N2 + 5/2 O2 + 2 KOH >> 2 KNO3 + H2O
has ΔH = [2 * -494] + [-285] - [2 * -426] = -421 kJ/mol
Is it possible to induce this reaction somehow?
|
|
|
walruslover69
Hazard to Others
Posts: 235
Registered: 21-12-2017
Member Is Offline
Mood: No Mood
|
|
I can't imagine you would be able to on a small scale. You would probably need a really specialized catalyst. That nitrogen triple bond has a huge
activation energy.
I am really surprised how favorable the reaction is though.
[Edited on 29-1-2019 by walruslover69]
|
|
|
SHADYCHASE54
Hazard to Others
Posts: 150
Registered: 16-12-2010
Location: CaNaDay!
Member Is Offline
Mood: No Mood
|
|
I am wondering if anyone can suggest a way to remove a palladium chloride stain from a glass frit. I have tried conc. HCl acid which has reduced the
discoloration by approx. 80% however 80% is still not complete. Any suggestions would be appreciated as the funnel was brand new. Thanks .
|
|
|
UC235
National Hazard
Posts: 565
Registered: 28-12-2014
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by SHADYCHASE54 | | I am wondering if anyone can suggest a way to remove a palladium chloride stain from a glass frit. I have tried conc. HCl acid which has reduced the
discoloration by approx. 80% however 80% is still not complete. Any suggestions would be appreciated as the funnel was brand new. Thanks .
|
Hot aqua regia.
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
3,4,5-Trimethoxyben?
Hey chemoforumers,
Purchased some 3,4,5-trimethoxybenzaldehyde from a (seemingly) reliable source, however, I have my doubts. Material appears as white flakes/granules.
very hard and brittle, and doesn't seem to have any real smell.
I would have expected the compound to have very different physical properties, as similiar subst benzaldehydes (vanillin, 5-bromovanillin,
syringaldehyde) have very strong smells and form fine , non-brittle crystals. This might seem obsesive, but want to be sure I have the right stuff .
Anyone familliar with the substance? Does this sound like 3,4,5-trimethoxy ben, or definitely something else?
insoluble in society
|
|
|
fusso
International Hazard
Posts: 1922
Registered: 23-6-2017
Location: 4 ∥ universes ahead of you
Member Is Offline
|
|
Some time ago, I heated some sugar to make elemental carbon. The resulting mass is very brittle and won't make black marks on paper, unlike graphite.
Is it amorphous C?
|
|
|
clearly_not_atara
International Hazard
Posts: 2800
Registered: 3-11-2013
Member Is Offline
Mood: Big
|
|
It's called "sugar charcoal".
https://en.wikipedia.org/wiki/Sugar_charcoal
|
|
|
mayko
International Hazard
Posts: 1218
Registered: 17-1-2013
Location: Carrboro, NC
Member Is Offline
Mood: anomalous (Euclid class)
|
|
I've been reading about molybdenum chemistry, and it seems surprisingly complicated. One pathway I'm interested in trying out would include an
oxidation of molybdenum (V) oxytrichloride to molybdenum (VI) trioxide:
MoOCl3 ----????----> MoO3
it's not obvious to me how to do this. I can't find a lot of detail on the oxytrichloride; the book I'm reading says that it decays in cold water, but
doesn't give any further information. Any ideas?
al-khemie is not a terrorist organization
"Chemicals, chemicals... I need chemicals!" - George Hayduke
"Wubbalubba dub-dub!" - Rick Sanchez
|
|
|
SHADYCHASE54
Hazard to Others
Posts: 150
Registered: 16-12-2010
Location: CaNaDay!
Member Is Offline
Mood: No Mood
|
|
I am wondering if someone might have a user manual for Parr pressure vessels pre-magnetic stir drive? I recently aquired a 600ml stirred reactor
gland type stirrer however I am finding it quite impossible to source any of the 1980-90 Parr manuals or user guides. Any help would be appreciated.
|
|
|
SHADYCHASE54
Hazard to Others
Posts: 150
Registered: 16-12-2010
Location: CaNaDay!
Member Is Offline
Mood: No Mood
|
|
Another quick question, would anyone have a suggestion regarding a reasonably accurate vacuum gauge with error limit not exceeding (+)(-) 25-40torr. I
mean to connect it to a vacuum tank to determine (manual) on off cycles so as to maintain max. vacuum, as it isn't convenient in this circumstance to
connect a glass Hg Manometer. I am looking for one that is analog pressure gauge style. The reason i am bothering to ask, what may on the surface
appear a dim question, is that my previous purchase turned out to be useless junk. When i tested the vac. gauge and measured for accuracy it was off
between 110-118torr. and these values fluctuated considerably. So if anyone has bought an analog vac. gauge that is resonably accurate as well as
resonably priced could you please provide a link or a brand/model number I would appreciate it.
As alway thanks for any suggestions.
|
|
|
mayko
International Hazard
Posts: 1218
Registered: 17-1-2013
Location: Carrboro, NC
Member Is Offline
Mood: anomalous (Euclid class)
|
|
I've been turning some of my copper collection into copper sulfate, using sulfuric acid + peroxide. I decided to try a less hands-on approach by using
an aquarium pump to aerate sulfuric acid, copper, and water in a jug. It's taking longer than I'd expect, but there is also something happening that I
just can't wrap my head around. The air bubbling tube has collected several inches of crystal growth *inside the tube*, that is to say, the growth has
taken place against the flow of the air, and indeed has plugged the tube at least once. How could this happen? I could believe that a little spray
might sometimes make it a little bit up the tube, but surely it would be quickly cleared from the air flow?
al-khemie is not a terrorist organization
"Chemicals, chemicals... I need chemicals!" - George Hayduke
"Wubbalubba dub-dub!" - Rick Sanchez
|
|
|
karlos³
International Hazard
Posts: 1520
Registered: 10-1-2011
Location: yes!
Member Is Offline
Mood: oxazolidinic 8)
|
|
Would the reaction of a bromoketone and theobromine actually take place at 1-, on the amide between both carbonyls?
I believe it would due to their directing effect, but I am not sure.
And since I need to isolate the theobromine from cocoa, I will very likely only have a rather tiny amount of it to experiment.
|
|
|
RedDwarf
Hazard to Others
Posts: 167
Registered: 16-2-2019
Location: UK (North West)
Member Is Offline
Mood: Variable
|
|
Mayko
I'm guessing that what is happening is that you get capillary flow of the liquid up the tube. Aquarium air pumps are quite gentle so I'm imagining
laminar flow with very low flow rates at the walls to counter the capillary action. The air dries the liquid so that you get a smaller diameter tube
which increases the capillary action even more. This is as I said a guess 
|
|
|
DraconicAcid
International Hazard
Posts: 4356
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
Is there am acidic derivative of theobromine called chocolic acid (which would have the conjugate base chocolate)? Why the hell not?
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
|
|
|
bipolar
Harmless
Posts: 24
Registered: 24-3-2019
Member Is Offline
|
|
Does acetonitrile react with sodium metal? If so, what are the products of this reaction?
I'm hoping this might be the way to make some sodium cyanide. 
[Edited on 21-4-2019 by bipolar]
|
|
|
fusso
International Hazard
Posts: 1922
Registered: 23-6-2017
Location: 4 ∥ universes ahead of you
Member Is Offline
|
|
For amide/protein hydrolysis, which one is faster, basic or acidic? (assume base/acid has same initial concentration in both rxns)
|
|
|
fusso
International Hazard
Posts: 1922
Registered: 23-6-2017
Location: 4 ∥ universes ahead of you
Member Is Offline
|
|
Can piranha solution oxidize gold, Pt and other PGMs?
|
|
|
TheMrbunGee
Hazard to Others
Posts: 364
Registered: 13-7-2016
Location: EU
Member Is Offline
Mood: Phosphorising
|
|
No, piranha solution is sometimes used for cleaning of gold or Pt plated stuff.
|
|
|
TheMrbunGee
Hazard to Others
Posts: 364
Registered: 13-7-2016
Location: EU
Member Is Offline
Mood: Phosphorising
|
|
| Quote: Originally posted by bipolar | Does acetonitrile react with sodium metal? If so, what are the products of this reaction?
I'm hoping this might be the way to make some sodium cyanide.
[Edited on 21-4-2019 by bipolar] |
Seems like reducing acetonitrile yields acetic acid and ammonia, at least in ethanol.
Acetonitrile metabolizes in to cyanide, so all you need is volunteer as an one time reactor and a way to extract cyanide from dead body and you are
good to go.
|
|
|
| Pages:
1
..
86
87
88
89
90
..
104 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
