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AlphaDecay
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I have some MnO2 from zinc-carbon batteries, but I won't use it since it is too impure, and I don't know what is the best way to dispose of it. Any
ideias? I searched for information on MnO2 MSDS about disposal and found nothing.
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Metacelsus
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I would just put it in the trash. Manganese dioxide is insoluble, so it won't migrate out of a landfill.
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bismuthate
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So, how could I get a cerium containing solution from CeO2 (without H2SO4).
Also why does Na2MoO4 not react with HCl to give MoO3?
[Edited on 26-12-2014 by bismuthate]
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Oscilllator
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Quote: Originally posted by bismuthate  | So, how could I get a cerium containing solution from CeO2 (without H2SO4).
Also why does Na2MoO4 not react with HCl to give MoO3?
[Edited on 26-12-2014 by bismuthate] |
I believe it does. In the past I have observed a white precipitate upon acidification of Na2MoO4
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Argentum
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Can I evaporate a solution of KOH with heating in a glass beaker? I know molten hydroxides can eat glass but just heating it up to evaporate water
will eat through my beaker?
Also, do anybody knows how to purify slaked lime, Ca(OH)2?
Thanks!
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DraconicAcid
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Hot concentrated KOH solution will etch glass.
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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bismuthate
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Add vinegar to the Ca(OH)2 and then add KOH to that and filter.
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Argentum
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Thanks Draconic and bismuthate for your help!
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bismuthate
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Why are solutions of Cr chloride and sulfate different colors when chloride and sulfate ions are colorless and they both have the hexaaquachromium
ion?
Or does CrCl3 form a chloroaquachromium ion? And if so how come it doesn't go purple upon dilution?
[Edited on 29-12-2014 by bismuthate]
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DraconicAcid
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Chromium(III) is very slow to exchange ligands. If you were to dissolve chromium in hydrochloric acid, you could conceivably get a
triaquotrichlorochromium(III) complex, a tetraaquodichlorochromium(III) complex (in cis and trans varieties, which will also be different colours),
pentaaquochlorochromium(III) ion, or hexaaquochromium(III). Diluting the solution will not quickly convert the chloro complexes into the
hexaaquochromium(III) ion- ligand exchange can take weeks, depending on the solution conditions.
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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Backyard Chemist
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Recently bought a bag of Calcium ammonium nitrate and was wondering how to separate the ammonium nitrate. Repeated filtration? A simple method please.
And btw i'm not planning on using it as an explosive, going to use it to make some potassium nitrate.
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DraconicAcid
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| Quote: Originally posted by Backyard Chemist | Recently bought a bag of Calcium ammonium nitrate and was wondering how to separate the ammonium nitrate. Repeated filtration? A simple method please.
And btw i'm not planning on using it as an explosive, going to use it to make some potassium nitrate.
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If you add potassium carbonate to that, the calcium should precipitate out as calcium carbonate. Filter that out, and heat the solution to drive off
carbon dioxide and ammonia, leaving potassium nitrate.
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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Backyard Chemist
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All right thanks!
I have a few questions if you don't mind:
1. If I was just to isolate the ammonium nitrate I could just heat the calcium ammonium nitrate solution and filter it right?
2. wouldn't a saturated solution of potassium chloride and ammonium nitrate produce potassium nitrate?
Thanks in advance
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gdflp
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1. Yes, though it wont be very efficient since there is approximately a 5:1 mol ratio of calcium to ammonium nitrates. A more efficient way would be
to add ammonium sulfate just until calcium sulfate stopped precipitating, then filter the solution. This will leave you with approximately 6
equivalents of ammonium nitrate in solution.
2. Yes it will due to solubility differences if chilled to low enough temperatures. This will result in some chloride and ammonium contamination
though, so recrystallizing it would be useful to increase the purity. In addition, potassium nitrate is still rather soluble at low temperatures, so
a lot of product will be lost in the solution. Adding potassium hydroxide, or potassium carbonate and heating, will result in a much better, purer
yield of potassium nitrate.
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Backyard Chemist
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How long would it have to cool for in order to let the AN crystals to appear? How much can you expect from this process?
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Zephyr
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All of you questions have been answered previously and it will save both you and me time if you first search for the answers yourself.
But while I'm here, I might as well help you out 
Firstly, when crystallizing something, the colder the solution gets the more of your product and impurities will crystallize out (Usually).
In the case of your ammonium nitrate, at 20 degrees Celsius every 10ml of solution will contain 15 grams of your product, meaning you will lose 15g of
ammonium nitrate for every 10 ml of solution you crystallize. This means that in order to maximize your yield, you will need to boil off most of the
water before crystallizing. And because of your (hopefully) low amounts of impurities, you final product should be reasonably pure.
Secondly, you need to find the best possible yield. Because the molecular weight of ammonium nitrate is 80 and the weight of calcium ammonium nitrate
is 584, the yield will be about 13 percent of total ammonium nitrate based on calcium ammonium nitrate. Minus whatever you don't crystallize. So I'd
you start with 1kg of CAN you can expect about 110 g total ammonium nitrate.
[Edited on 12-30-2014 by Pinkhippo11]
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Backyard Chemist
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Thanks mate!
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Jylliana
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Does Bismuth(aq) react with copper(s)?
Because my redox table says it should, but my eyes say it doesn't.
I'm confused.
I tried to make elemental bismuth out of bismuth subcarbonate.
EDIT: I think my Bismuth is readily dissolving in my HCl-solution where it's in.
!@#$ How am I gonna fix that.. Neutralizing wil just yield bismuth oxide again >.<
[Edited on 6-1-2015 by Jylliana]
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Pasrules
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| Quote: Originally posted by Jylliana | Does Bismuth(aq) react with copper(s)?
Because my redox table says it should, but my eyes say it doesn't.
I'm confused.
I tried to make elemental bismuth out of bismuth subcarbonate. |
This reactivity series I found would say no. However it also says platinum is more reactive than gold which I had to argue at my chemistry teacher
about because that's what school syllabuses teach. Most of these tables I find vary text book to text book and arn't all done in the same conditions.
Next questions which is more reactive gold or platinum...? Because I've seen platinum take a far longer amount of time in Aqua Regia.
Atropine, Bicarb, Calcium.
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gdflp
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Based on the reactivity series, platinum is less reactive than gold. Though I don't believe that the speed of dissolution in acids is a good measure
of it.
@Jylliana
Copper will plate onto bismuth metal, not the other way around. You will need a more reactive metal such as Fe, Zn, Mg, etc. This is a useful reference.
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CuReUS
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I have a few questions :
1.what is the best chemical test to confirm an aromatic aldehyde(benzaldehyde) from an aliphatic aldehyde other than burning it and seeing if the
flame is sooty ?
2.why cant the H of an aldehyde group(CHO) be pulled out,why only the alpha H is removed ?
3.why does ethanol on treatment with conc H2SO4 give an oily layer(ethyl hydrogen sulphate) at one time and a white precipitate
at another ?
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Jylliana
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I always believed that Gallium was a pretty non-toxic metal. Nothing special about it, except it's low melting point.
Why is it that it requires HAZMAT shipping from everywhere I've looked?
I know it forms an alloy with a lot of stuff, but just shipping it in a vial or bottle shouldn't be a problem? Or is there something about this metal
that I overlook?
[Edited on 13-1-2015 by Jylliana]
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Brain&Force
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No, it's not toxic, it'll just dissolve stuff too easily.
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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If you remove the alpha hydrogen, you get an anion that is stabilized by resonance. If you pull off the aldehyde carbon, you don't get any resonance.
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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Jylliana
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I found a very old dessicator in my lab. I wouldn't be surprised if it hasn't been touched for over 20 years.
I want to use it, but the two halves are VERY stuck together. I think the silicon grease has dried out or something.
I've tried pulling very hard, prying with a screwdriver, asking it politely, but nothing works. I am afraid the thing may shatter if I use more force
or heat.
Do you have any ideas?
I did manage to lift the stopper on top, so there is no vacuum.
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