RU_KLO - 18-12-2023 at 06:47
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]
Metacelsus - 18-12-2023 at 07:50
Why can't you confirm the molarity of the reagents and mix an equimolar amount? This would be much easier.
Anthracene - 18-12-2023 at 18:26
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 - 18-12-2023 at 22:06
Just estimate the amount of reagents roughly, then add an excess of sulfuric acid. You’ll get mostly the bisulfate.