RU_KLO
Hazard to Others
Posts: 150
Registered: 12-10-2022
Location: Argentina
Member Is Offline
|
|
Potassium bisulfate ot Potassium sulfate?
I need Potassium bisulfate (for prosessing further to Potassium pyrosulfate)
from wiki:
KOH + H2SO4 → KHSO4 + H2O
now, why not:
2KOH + H2SO4 → K2SO4 + 2H2O
(wiki ask for equimolar, So the understanding is first equation)
These means that no K2SO4 is produced? or there will be contamination of sulfate in the bisulfate?
If I use ph as neutralization point (to get the bisulfate - for example because I cannot confirm molarity of reagents)
Which ph should be aimed? (from diferent sources, ones said KHSO4 = ph 1, others KHSO4 ph 3-4)
Thanks
[Edited on 18-12-2023 by RU_KLO]
Go SAFE, because stupidity and bad Luck exist.
|
|
|
Metacelsus
International Hazard
Posts: 2532
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Why can't you confirm the molarity of the reagents and mix an equimolar amount? This would be much easier.
|
|
|
Anthracene
Harmless
Posts: 1
Registered: 4-12-2023
Location: Stone Island
Member Is Offline
Mood: Curious
|
|
Have you looked into directly buying bisulfate as a Ph lowering chemical for pools?
It is most certainly cheaper and easier accessible than both KOH and sulfuric acid anywhere.
If you are set on the goal of obtaining polysulfate by thermal decomposition but struggling with molarity of reagents this seems like the way forward.
|
|
|
Sir_Gawain
Hazard to Others
Posts: 287
Registered: 12-10-2022
Location: Due South of Due West
Member Is Offline
Mood: Yes.
|
|
Just estimate the amount of reagents roughly, then add an excess of sulfuric acid. You’ll get mostly the bisulfate.
“Alchemy is trying to turn things yellow; chemistry is trying to avoid things turning yellow.” -Tom deP.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
