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Etaoin Shrdlu
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Apparently. http://www.arkat-usa.org/get-file/34424/
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Töilet Plünger
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I'll answer my own question: lithium nitrate. Though I'm not sure if it'll burn nicely; I haven't tried it yet.
[edit] it does!
[Edited on 2014-5-6 by Töilet Plünger]
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elementcollector1
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Solubility Data: (NH4)2SO4 in HNO3 / H2SO4?
Exactly what it says - is ammonium sulfate soluble to any appreciable degree in either of these acids, at low temperatures (assume 0 to 20 degrees C)?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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Oscilllator
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I imagine they would be soluble to a limited degree. Nitrating baths can be made of NH4NO3 and H2SO4, and the NH4NO3 dissolves into the sulfuric acid
to an appreciable extent to create nitric acid. This is a very similar situation.
I don't know the precisely how soluble they would be, but I imagine you should be able to get a 5-10% soln fairly easily
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Hegi
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Soxhlet extractor question
I´m buying soxlet extractor with volume of 150 ml and I was looking for extraction thimbles.. They are not cheap at all and what I found is package
of 25 pieces with size 34mm in external diameter and lenght 100mm for 35 pounds with shipping.. my question is if it would fit in and work ? Does
anyone know? Or shall I rather look for 22x80 thimbles? 
Our webpage has been shut down forever cause nobody was willing to contribute. Shame on you all!!!
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Etaoin Shrdlu
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Give the supplier your dimensions and ask them.
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Zyklon-A
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Quote: Originally posted by elementcollector1  | Solubility Data: (NH4)2SO4 in HNO3 / H2SO4?
Exactly what it says - is ammonium sulfate soluble to any appreciable degree in either of these acids, at low temperatures (assume 0 to 20 degrees C)?
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http://www.uea.ac.uk/~e770/aim/model2/descr2.htm
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solo
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.......when halogenating an aldehyde with the alpha carbon without any free hydrogens, if there is al alkene adjacent to the alpha carbon will the
halogenation favor the aldehyde or the alkene or both.....solo
Note- March 5th edition page 914 sectsion 14-3, talks about the halogenation of aldehydes with the alpha carbon abscent of any hydrogens
[Edited on 9-5-2014 by solo]
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Metacelsus
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If there are no alpha hydrogens, halogenation will not occur (what atom would the halogen replace?). I think the halogen would just add across the
double bond.
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solo
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.......the hydrogen on the aldehyde...as stated on the reference provided......will get halogenated, but my question is will the alkene be halogenate
as well or just the aldehyde site.....solo
[Edited on 9-5-2014 by solo]
It's better to die on your feet, than live on your knees....Emiliano Zapata.
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Metacelsus
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So the reaction forms an acyl halide? Very interesting . . .
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solo
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.....well, if it halogenates an aldehyde with no alpha hydrogen it would be great...if only the alkene attached to the alpha carbon is not
halogenated with this particular type of aldehyde.....one can do many things with that .....hence the reason for my inquiry....solo
[Edited on 10-5-2014 by solo]
It's better to die on your feet, than live on your knees....Emiliano Zapata.
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Metacelsus
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edition of what?
Also, what would prevent the alkene from being halogenated?
Can you be more specific about conditions, substrate, etc.?
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Brain&Force
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I mixed potassium nitrate in methanol. It doesn't appear to dissolve, but the methanol turns blue. I've also had this happen with a sample of methanol
sitting in a low-oxygen environment with just a match in it (there weren't any nitrates in the methanol). What causes this?
At the end of the day, simulating atoms doesn't beat working with the real things...
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Zephyr
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I have recently made what I believe to be copper nitrite, by the addition of copper sulfate to a small excess sodium nitrite. The solution is dark
green, similar to concentrated copper chloride. I wish to isolate the copper nitrite, but am unsure about how to go about it. Does anyone have any
information on copper nitrite? Or any ideas on how to separate it?
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Etaoin Shrdlu
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You just have a mixture of copper, sodium, sulfate, and nitrite ions now.
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Zephyr
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Yes I know. However this doesn't answer any of my questions. I have looked in the Merck index and in the CRC, and neither contain anything on copper
nitrite.
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Etaoin Shrdlu
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Sorry, let me try again. You haven't "made" copper nitrite because none of the compounds changed states, you have made a mixture of copper, sodium,
sulfate, and nitrite ions.
I'm almost 100% certain you can't isolate copper nitrite without it decomposing. Maybe with highly specialized equipment and conditions. Sodium
sulfate looks marginally less soluble than copper sulfate or sodium nitrite at cool temperatures, perhaps it is possible to crystallize that
out...
[Edited on 5-14-2014 by Etaoin Shrdlu]
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bismuthate
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So earlier today a mixed solutions of povidone iodine that was neutralized with excess sodium thiosulfate. This instantly precipitated an orangish
yellow precipitate. What happened here?
EDIT: it starts out yellow and turns orange quickly.
[Edited on 15-5-2014 by bismuthate]
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Metacelsus
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The reaction should produce tetrathionate. Could this possibly be decomposing to sulfur?
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bismuthate
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The yellow is much brighter that sulfur.My theory is that the tetrathionate decomposes to the sulfide.
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Brain&Force
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More flame questions:
First of all, is it possible to color the flame of a fireplace or some other wood fire (in other words, a vapor-diffusion flame)? I've tried just
dumping copper sulfate on wood fires, but with very little change.
Second, when it is said that the bluest part of a flame is the hottest, isn't that technically inaccurate? Isn't the bluest part the best-mixed part
of the flame, where there is enough oxygen to burn completely? And isn't the color caused by the emission spectrum of the burning substance?
At the end of the day, simulating atoms doesn't beat working with the real things...
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DraconicAcid
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| Quote: Originally posted by Brain&Force | More flame questions:
First of all, is it possible to color the flame of a fireplace or some other wood fire (in other words, a vapor-diffusion flame)? I've tried just
dumping copper sulfate on wood fires, but with very little change. |
Copper perchlorate works wonderfully well for this.
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.
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alexleyenda
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| Quote: Originally posted by Brain&Force |
Second, when it is said that the bluest part of a flame is the hottest, isn't that technically inaccurate? Isn't the bluest part the best-mixed part
of the flame, where there is enough oxygen to burn completely? And isn't the color caused by the emission spectrum of the burning substance?
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How wonderful, I am studying that right now in physics. Every particle that moves (has heat) emits electromagnetic radiations (visible light,
infrared, etc.). Particles around our temperature (20°C) emits infrared light. When it gets hotter, the energy emited is stronger, the frequency gets
higher and the wavelenght lower : we start to get to the visible spectrum, things are red (like heating ovens). When it gets a bit hotter, it
continues to go up the spectrum, it gets yellow. Once it gets hotter than that, it is around the middle of the visible spectrum, it emits a good
quantity of light of all the wavelengths of the spectrum : all colors together = white. When the energy is higher, the light emited is at the top of
the visible spectrum (blue) and UV. That's why UV protection is used by those who bind metal together ( I don't know the word for it in english).
Finaly, when it is hotter than that, it is 100% UV or even stronger. The equation to know the principal wavelength emited is "0,0029/T " where T is
the temperature in Kelvins. For exemple, the wire in a light bulb is around 3000K, its principal wavelenght is 967 nanometers, which is infrared. It
also emits light near that number. 700 being red, that's why light bulbs with wires are red/yellow. It also means that most of its power is lost in
infrared that we cannot see, that's why these bulbs efficiency is so bad. The spectrums look like this : (http://faculty.virginia.edu/consciousness/images/black%20bod...)
That being said, light is also created not only by heat, but also when an electron absorbs energy, get to an higher level of energy, then release the
energy absorbed as a photon (light) to get back to normal. Depending of the electronic configuration of the atoms, it can only acces to precise levels
of energy, so it will always let go only precise amounts of energy corresponding to these levels. That is why compounds let go different colours. The
addition of the wavelengts they can release makes their color.. (That is how fluo light bulb work, the electrons of a gas that emit wavelengths in the
visible spectrum are excited by an electrical current, then release their energy as light. That is why these bulbs are a lot more efficient than the
others which release a lot of invisible particules of light). These spectrums looks like this : http://utahscience.oremjr.alpine.k12.ut.us/sciber06/9th/stan...
[Edited on 19-5-2014 by alexleyenda]
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alexleyenda
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I thought about it, I didn't really answer cleary. To answer more directly to your question, the bluest part really is the hottest, except if you put
a compound in it with an emission spectrum that releases blue.
Yes, it is usually the best mixed part where it burns completely, because the more it burns, the more energy is released, the hotter it gets, the
frequency gets higher and the wavelenght (in that case) gets more blue.
The color may be caused by the emission spectrum of the burning substance, but most of the time, it is not. Most molecules and atoms require extreme
excitation to give off visible light, a flame is not enough to triger that, except in the case of some compounds such as copper, lithium and all.
[Edited on 19-5-2014 by alexleyenda]
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