bismuthate
National Hazard
Posts: 803
Registered: 28-9-2013
Location: the island of stability
Member Is Offline
Mood: self reacting
|
|
The reaction question thread.
I thought it would be nice to have a thread where people can ask how does ******** react with ********. So I'll start off.
NaNH2+PH3==>NaPH2+NH3?
2Na+2PH3==>2NaPH2+H2?
3NaNO3+AsCl3==>As(NO3)3+3NaCl?
[Edited on 7-12-2013 by bismuthate]
[Edited on 7-12-2013 by bismuthate]
|
|
|
Random
International Hazard
Posts: 1120
Registered: 7-5-2010
Location: In ur closet
Member Is Offline
Mood: Energetic
|
|
Many reactions are possible but another question is under what conditions.
For example hydrogen and ammonia looks simple on paper until you see actual pressure and heat required.
|
|
|
bismuthate
National Hazard
Posts: 803
Registered: 28-9-2013
Location: the island of stability
Member Is Offline
Mood: self reacting
|
|
Yeah it would be nice if people added in under what conditions they react, but this is just a question of how a reaction proceeds.
|
|
|
Zyklon-A
International Hazard
Posts: 1547
Registered: 26-11-2013
Member Is Offline
Mood: Fluorine radical
|
|
I was wondering if barium nitrate could react with potassium perchlorate to make barium perchlorate and potassium nitrate.
Solubility of perchlorate is 66.48 g/100 mL (25 °C), While potassium perchlorate is only 1.5 g/100 mL (25 °C).
I think it wont work actually, just looking at the solubility data.
Can anyone provide a professional opinion on the subject?
|
|
|
mnick12
Hazard to Others
Posts: 404
Registered: 30-12-2009
Location: In the lab w/ Dr. Evil
Member Is Offline
Mood: devious
|
|
Quote: Originally posted by Zyklonb  | I was wondering if barium nitrate could react with potassium perchlorate to make barium perchlorate and potassium nitrate.
Solubility of perchlorate is 66.48 g/100 mL (25 °C), While potassium perchlorate is only 1.5 g/100 mL (25 °C).
I think it wont work actually, just looking at the solubility data.
Can anyone provide a professional opinion on the subject? |
Indeed the poor solubility of potassium perchlorate indicates that the equilibrium highly favors KClO4 over Ba(ClO4)2. Potassium perchlorate is kind
of a dead end for making other perchlorates. Sodium perchlorate or would be a better option, however if the intended use is pyrotechnic applications
removing all the sodium ions could be very difficult. I would start with ammonium perchlorate, although it is more expensive.
|
|
|
Zyklon-A
International Hazard
Posts: 1547
Registered: 26-11-2013
Member Is Offline
Mood: Fluorine radical
|
|
Ammonium perchlorate is generally made from perchloric acid.
| Quote: |
.......however if the intended use is pyrotechnic applications...... |
No, I'll be using it to make perchloric acid, according to this reaction: Ba(ClO4)2 (aq) + H2SO4-->
BaSO4 (s) + HClO4 (aq).
I guess I can find another method to make barium chlorate.
|
|
|
DraconicAcid
International Hazard
Posts: 4333
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
| Quote: | I thought it would be nice to have a thread where people can ask how does ******** react with ********. So I'll start off.
NaNH2+PH3==>NaPH2+NH3? |
It should. Phosphine will be a stronger acid than ammonia. Nasty stuff to work with, though.
| Quote: | | 2Na+2PH3==>2NaPH2+H2? |
It should. I know that triphenylphosphine will react with sodium to give NaPPh2 and NaPh (which was protonated under the reaction conditions, but I
don't recall what they were).
| Quote: | | 3NaNO3+AsCl3==>As(NO3)3+3NaCl? |
I doubt it. The arsenic-chlorine bond has significant covalent character, and I wouldn't expect the nitrate to bond as strongly.
[Edited on 6-3-2014 by DraconicAcid]
[Edited on 6-3-2014 by DraconicAcid]
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.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
