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Author: Subject: The short questions thread (3)
CHRIS25
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[*] posted on 4-4-2013 at 02:06


How does one test for the presence of ammonium in Ferrous ammonium sulphate? Suspecting that upon crystalization I have only ferrous sulphate.

The latter I also made and it is the exact same colour as my supposed ferrous ammonium sulphate, although I have extremely large crystals from the Ferrous ammonium Sulphate, I know that as I was neutralizing the ammonia solution with H2SO4 i went past the neutralisation stage and so brought it back with the addition of more ammonium solution. The consequences of which meant that there was no longer an equimolar amount of pre-prepared ferrous sulphate mixing with the ammonium sulphate. Thankyou.




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DraconicAcid
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[*] posted on 4-4-2013 at 07:58


Quote: Originally posted by CHRIS25  
How does one test for the presence of ammonium in Ferrous ammonium sulphate? Suspecting that upon crystalization I have only ferrous sulphate.


Place a small amount of it into a small beaker. Dampen a piece of litmus paper and stick it to a watch glass and set it on the beaker. Add sodium hydroxide solution to your solid material. If ammonium is present, it will be converted to ammonia, which will turn the paper blue.




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confused
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[*] posted on 4-4-2013 at 10:08


how badly would a round bottom flask be stressed if it was heated directly on a hotplate without an oil bath to about 300°C+?
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Mailinmypocket
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[*] posted on 4-4-2013 at 10:41


Quote: Originally posted by confused  
how badly would a round bottom flask be stressed if it was heated directly on a hotplate without an oil bath to about 300°C+?


I often use air baths with foil skirts to heat flasks on a hot plate around that temperature, no problem. Don't let the RBF touch the hotplate-that might cause stress.
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Pyro
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[*] posted on 4-4-2013 at 10:42


depends on the quality of the flask, if the bottom is touching the hotplate, if you have wrapped Al foil around the top to catch the heat.
personally I think you will never get the flask up to 300*C without an oil bath




all above information is intellectual property of Pyro. :D
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BobD1001
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[*] posted on 4-4-2013 at 20:01


Could anyone say if the following bottle be okay for storage of Concentrated Nitric acid?

http://www.amazon.com/Wheaton-Capacity-Polypropylene-Polyeth...

Would there be concern of pressure buildup from concentrated nitric, and would an amber reagent bottle with a glass stopper better suit my needs?

Thank you
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confused
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[*] posted on 4-4-2013 at 20:30


should be ok for nitric acid...not sure about the pressure though, where are you storing it and what concentration is it in?
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BobD1001
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[*] posted on 4-4-2013 at 21:21


Quote: Originally posted by BobD1001  
Could anyone say if the following bottle be okay for storage of Concentrated Nitric acid?

http://www.amazon.com/Wheaton-Capacity-Polypropylene-Polyeth...

Would there be concern of pressure buildup from concentrated nitric, and would an amber reagent bottle with a glass stopper better suit my needs?

Thank you


To Add:

The concentrated nitric acid will be produced by vacuum distillation, so likely in the neighborhood of 90%+. It will be stored at ambient temperature as I do not have a lab freezer, this ambient temperature will be a relatively constant approximately 21 degrees C.

[Edited on 5-4-2013 by BobD1001]
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CHRIS25
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[*] posted on 5-4-2013 at 04:51


Quote: Originally posted by DraconicAcid  
Quote: Originally posted by CHRIS25  
How does one test for the presence of ammonium in Ferrous ammonium sulphate? Suspecting that upon crystalization I have only ferrous sulphate.


Place a small amount of it into a small beaker. Dampen a piece of litmus paper and stick it to a watch glass and set it on the beaker. Add sodium hydroxide solution to your solid material. If ammonium is present, it will be converted to ammonia, which will turn the paper blue.

Thankyou, or basically do as you suggest but could stick the litmus directly to the inside of the beaker near the top, will try anyway.




‘Calcination… is such a Separation of Bodies by Fire, as makes ‘em easily reducible into Powder; and for that reason ‘tis call’d by some Chymical Pulverization.’ (John Friend, Chymical Lectures London, 1712)

Right is right, even if everyone is against it, and wrong is wrong, even if everyone is for it. (William Penn 1644-1718)

The very nature of Random, Chance development precludes the existence of Order - strange that our organic and inorganic world is so well defined by precision and law. (me)
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Pyro
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[*] posted on 5-4-2013 at 05:32


you should get the type with the aluminium lining. the Al will passivate and won't let it through the cap.



all above information is intellectual property of Pyro. :D
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[*] posted on 7-4-2013 at 07:31


but doesn't the PTFE liner prevent nitric acid fumesfrom passing through the cap?
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[*] posted on 7-4-2013 at 07:35


im trying to obtain some mercury metal would a mercury tilt switch or mercury thermometer contain more mercury?
(i know it's a waste of perfectly great thermometers but those are the only 2 sources a can get mercury in my country :( )
im asuming that a thermometer with a higher temperature range would contain more mercury?
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hissingnoise
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[*] posted on 7-4-2013 at 08:10


You shouldn't assume that all tilt switches will contain elemental mercury . . .
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[*] posted on 8-4-2013 at 04:47


...wouldn't a mercury tilt swtich contain mercury?
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[*] posted on 8-4-2013 at 05:08


Question.

Good use for large amounts of Ca(OH)2?




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[*] posted on 8-4-2013 at 05:20


limewater to test for CO2?
synthesis of Sodium/Potassium hydroxide with reaction between sodium/potassium carbonate and calcium hydroxide?
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[*] posted on 8-4-2013 at 05:23


Potassium carbonate... OTC?

Edit: then I could decomp the resulting Calcium carbonate into CaO?

[Edited on 8-4-2013 by Finnnicus]




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[*] posted on 8-4-2013 at 05:25


i got mine at a store selling pottery supplies, usually used as a glaze
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[*] posted on 8-4-2013 at 05:29


possible, but that would require alot of heat above above 840 °C
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[*] posted on 8-4-2013 at 09:56


Quote: Originally posted by Finnnicus  
Question.

Good use for large amounts of Ca(OH)2?

Make benzene?




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[*] posted on 8-4-2013 at 15:07


Explain.



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[*] posted on 8-4-2013 at 15:35


A dry distillation of Ca(OH)2 and sodium benzoate yields benzene and friends. You can find more information in the member publications, I believe.
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[*] posted on 8-4-2013 at 17:10


Lovely thank you.



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[*] posted on 12-4-2013 at 19:06


So I am building a magnetometer, and I need a liquid or solid that has the most hydrogen atoms per volume, does anyone know what hydrocarbon or other substance would have the most hydrogen molecules per volume that is easily obtainable.

Thanks for your help
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[*] posted on 12-4-2013 at 19:24


Water? 2 mol H atoms / 18 g ; 1 g / cm^3 = 0.111 mol H atoms / cm^3
Paraffin wax? ~2 mol H atoms / 14 g ; ~0.8 g / cm^3 = 0.114 mol H atoms / cm^3




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