| Pages:
1
2 |
Romix
Hazard to Others (Literally)
Posts: 483
Registered: 19-6-2015
Member Is Offline
Mood: No Mood
|
|
What you guys think, could this reaction be fake?
Not seen it anywhere else other than this video, although seen it's formula on other chemical forums.
You can hear guys in the video choking on Ammonia!!!
If it's fake might save me going through all the hustle on page 1, hahaha!!!
https://www.youtube.com/watch?v=CVzoQhhqfPI
[Edited on 18-9-2024 by Romix]
|
|
|
clearly_not_atara
International Hazard
Posts: 2786
Registered: 3-11-2013
Member Is Offline
Mood: Big
|
|
What on Earth does that video have to do with making HCl?
You seem to be under the impression that a solution of chlorine in water is the same as the pure compound HOCl. This is not the case. An equilibrium
exists, similar to the situation with carbon dioxide.
Cl2 + H2O << >> HCl + HOCl
CO2 + H2O << >> H2CO3
Only a small percentage of the chlorine exists as HOCl. Preparing pure HOCl or even an aqueous solution is very difficult.
EDIT: You may be able to make HCl from Cl2 by membrane electrolysis. PbO2 anode, chlorine in the cathode chamber, probably Ti cathode. Not sure what
membrane would handle this.
It also appears that hydrogen peroxide might reduce aqueous chlorine. But IIRC it also oxidizes HCl to some extent. The resulting acid will not be
free of chlorine without further work.
[Edited on 18-9-2024 by clearly_not_atara]
|
|
|
Romix
Hazard to Others (Literally)
Posts: 483
Registered: 19-6-2015
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by clearly_not_atara  | What on Earth does that video have to do with making HCl?
You seem to be under the impression that a solution of chlorine in water is the same as the pure compound HOCl. This is not the case. An equilibrium
exists, similar to the situation with carbon dioxide.
Cl2 + H2O << >> HCl + HOCl
CO2 + H2O << >> H2CO3
Only a small percentage of the chlorine exists as HOCl. Preparing pure HOCl or even an aqueous solution is very difficult. |
Not believing it, why there is no equilibrium with HCl alone, but would be here.
Ok maybe there is with HOCl, I did notice release of Cl2 after reacting it deep in water, could just be escaping from blowing big current of Cl2 into
it and not having enough time to react with H2O or could be equilibrium, don't have enough experience with HOCl to tell!
|
|
|
Romix
Hazard to Others (Literally)
Posts: 483
Registered: 19-6-2015
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by Romix | | Quote: Originally posted by clearly_not_atara | What on Earth does that video have to do with making HCl?
You seem to be under the impression that a solution of chlorine in water is the same as the pure compound HOCl. This is not the case. An equilibrium
exists, similar to the situation with carbon dioxide.
Cl2 + H2O << >> HCl + HOCl
CO2 + H2O << >> H2CO3
Only a small percentage of the chlorine exists as HOCl. Preparing pure HOCl or even an aqueous solution is very difficult. |
Not believing it, why there is no equilibrium with HCl alone, but would be here.
Ok maybe there is with HOCl, I did notice release of Cl2 after reacting it deep in water, could just be escaping from blowing big current of Cl2 into
it and not having enough time to react with H2O or could be equilibrium, don't have enough experience with HOCl to tell!
|
There is equilibrium in close to concentrated HCl, even so HCl fumes, fumes are white, not yellow, like Cl2 should be!!!
|
|
|
RU_KLO
Hazard to Others
Posts: 207
Registered: 12-10-2022
Location: Argentina
Member Is Offline
|
|
Early in the study of elementary chemistry one learns that chlorine reacts with water in the sense of the expression
Cl2 + H2O <<>> HCl + HOCl
and that the hypochlorous acid decomposes thus,
HClO -> HCl + O
Owing to the instability of hypochlorous acid in the presence of hydrochloric acid, the first reaction progresses to a very limited extent and the
production of the end-products, oxygen and hydrochloric acid, is greatly accelerated by light. This accounts for the fact that aqueous solutions of
chlorine eventually become aqueous solutions of hydrochloric acid upon standing in the laboratory, and should thecefore be protected from the light.
THE PRODUCTION OF HYDROCHLORIC ACID FROM CHLORINE AND WATER
By H. D. Gibbs
(paper on this post:
https://www.sciencemadness.org/whisper/viewthread.php?tid=16...)
The reaction between HCl and HOCl, which is the reversal of Cl2 hydrolysis,
is a textbook reaction that has long been used for water disinfection and waste-water treatment.
"Catalysis of the reaction HCl+HOCl -> H2O+Cl2 on an ice surface"
https://doi.org/10.1016/S0009-2614(99)00683-1
So from this I understand that: or the HOCl is decomposed or transformed to Chlorine.
So no HOCl & HCl living together in peace.
Go SAFE, because stupidity and bad Luck exist.
|
|
|
Romix
Hazard to Others (Literally)
Posts: 483
Registered: 19-6-2015
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by RU_KLO | Early in the study of elementary chemistry one learns that chlorine reacts with water in the sense of the expression
Cl2 + H2O <<>> HCl + HOCl
and that the hypochlorous acid decomposes thus,
HClO -> HCl + O
Owing to the instability of hypochlorous acid in the presence of hydrochloric acid, the first reaction progresses to a very limited extent and the
production of the end-products, oxygen and hydrochloric acid, is greatly accelerated by light. This accounts for the fact that aqueous solutions of
chlorine eventually become aqueous solutions of hydrochloric acid upon standing in the laboratory, and should thecefore be protected from the light.
THE PRODUCTION OF HYDROCHLORIC ACID FROM CHLORINE AND WATER
By H. D. Gibbs
(paper on this post:
https://www.sciencemadness.org/whisper/viewthread.php?tid=16...)
The reaction between HCl and HOCl, which is the reversal of Cl2 hydrolysis,
is a textbook reaction that has long been used for water disinfection and waste-water treatment.
"Catalysis of the reaction HCl+HOCl -> H2O+Cl2 on an ice surface"
https://doi.org/10.1016/S0009-2614(99)00683-1
So from this I understand that: or the HOCl is decomposed or transformed to Chlorine.
So no HOCl & HCl living together in peace.
|
Thanks!
|
|
|
HoxonLabs
Harmless
Posts: 4
Registered: 17-9-2024
Location: Cambridge
Member Is Offline
Mood: Rude
|
|
You could heat the solution, expose it to UV light, or reduce it with sodium thiosulphate, for example.
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
