jokoron
Harmless
Posts: 2
Registered: 26-11-2016
Member Is Offline
Mood: No Mood
|
|
What concentration of HCl can I expect?
I am planning on making HCL with sodium bisulfate and table salt. I will bubble the product gasses through water. Assuming that I will bubble an
excess of gas, what concentration of HCl can I expect? How will the temperature of water effect the concentration? Also what will happen if I bubble
the gas through H2O2 instead of water?
[Edited on 27-11-2016 by jokoron]
|
|
|
greenlight
National Hazard
Posts: 737
Registered: 3-11-2014
Member Is Offline
Mood: Energetic
|
|
Highest concentration you could obtain would be 37-38% at standard atmospheric pressure then the water would not absorb any more.
For the second answer, small amount of chlorine gas?
Be good, otherwise be good at it 
|
|
|
AJKOER
Radically Dubious
Posts: 3026
Registered: 7-5-2011
Member Is Offline
Mood: No Mood
|
|
In very dilute conditions, mixing HCl, created from the action of chlorine and water along with hypochlorous acid, with a small amount of H2O2
reportedly results in HOCl. To quote from Watts Dictionary of Chemistry, page 16:
"—6. Addition of H2O2 Aq (containing 2-45 p.c. H2O2) to a large excess of Cl Aq produces HClOAq, according to Fairley (B. A. 1874, 57); if much H202
is added, the HClOAq is decomposed forming HClAq, H20, and evolving O."
Link: https://books.google.com/books?pg=PA16&dq=Watt+preparati...
There is also another confirming reference: "Chemistry, inorganic and organic: with experiments" By Charles Loudon Bloxam, page 182:
"Hypochlorous acid is formed when a weak solution of hydrogen peroxide is added to a large excess of chlorine water; Cl2 + H2O2 = 2HCl0. With an
excess of the peroxide, HClO + H2O2 = HCl + H20 + 02."
[Edit] I can see paths to justify the above comment based on the act of dilution itself, which could raise the pH of the hydrogen peroxide solution,
making the H2O2 more prone to decomposition (including radical decomposition pathways), or the presence of solar light, or even transition metal
impurities. The latter could introduce, for example, Fenton and Fenton-type reactions producing hydroxyl radicals that can directly react with
chloride, resulting in products, including chlorine radicals, thereby removing HCl. See, for example, Table 5 at https://www.google.com/url?sa=t&source=web&rct=j&...
In more concentrated settings, from reporting on this forum, to quote observations by Woelen:
"More surprisingly, I also noticed that I obtained an oscillating reaction with 30% HCl and 30% H2O2. Simply mix the two liquids in a test tube at a
HCl : H2O2 = 2 : 1 volume ratio and observe the oscillating pattern in the evolution of gas. The mix alternatingly produces chlorine gas (low bubbling
activity) and oxygen gas (strong bubbling activity)."
Link: http://www.sciencemadness.org/talk/viewthread.php?tid=7622#p...
[Edited on 28-11-2016 by AJKOER]
|
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
