joejoe
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KHSO4
can anyone tell me where i can get KHSO4.
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hissingnoise
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I don't usually answer a question with another, but how many places have you tried so far?
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woelen
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You can make it from H2SO4 and K2CO3 (or KOH). Simply mix amounts at correct stoichiometry,
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Jor
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But you will lose a good amount of strong acid, wich is valuable, in the form of CO2. I always find it a waste. Also when I want to generate CO2 from
NaHCO3, I use vinegar, and no hydrochloric acid. Maybe it's a mental thing, i just don;t like the idea of wasting something like HCl on plain CO2.
If I would want to make it, I would take make some profit out of the situation, and I would add conc. H2SO4 to a conc. KBr solution slowly, and after
addition, let it cool. the crystals are relatively pure KHSO4, and you didn't waste your acid: you converted KBr in HBr (a valuable reagent), instead
of turning carbonate in CO2.
Or ofcourse add KCl to conc. H2SO4, and bubble the gas (HCl) in water. You are left with KHSO4 and some hydrochloric acid.
However, for really pure KHSO4, react K2CO3 with H2SO4.
[Edited on 14-1-2009 by Jor]
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kclo4
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Better to add H2SO4 to Na2SO4 to make it. Since you would be using half the acid.
You can buy it at most stores as sani-flush, or pH down for swimming pools. Read the ingredients in those.
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not_important
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can anyone tell me where i can get KHSO4.
Better to add H2SO4 to Na2SO4 to make it. Since you would be using half the acid.
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Hmmm ... a little nuclear chemistry there. But the idea is correct, if it is the potassium salt desired K2SO4 can be (or once could be) found as a
fertiliser.
Another way is to fuse equimolar quantities of K2SO4 and (NH4)SO4, or two moles of (NH4)SO4 with one mole of K2CO3, or equmolar amounts of (NH4)2SO4
and KHCO3. The second hydrogen of H2SO4 is a fairly weak acid, and ammonium salts tend to decompose when heated; heating a mixture drives off the
ammonia and in this case leaving KHSO4.
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Ebao-lu
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yes, just add H2SO4(any concentration) to K2SO4 in equimolar amounts and heat to remove water
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Formatik
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Also make sure to not heat too strongly. KHSO4 when heated in the molten state (Mp. 213.8° in an open vessel) only slowly releases its water and a
part of it converts to K2S2O7. This conversion occurs more readily in a vacuum, heating at 230 to 350°C at pressure of 30-40 mmHg, H2O loss is 70%,
and the mixture contains 68% K2S2O7. Above 400°, decomp. occurs forming H2SO4, SO2 and O2.
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BlindedAchievement
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http://www.citychemical.com/productdetails.asp?Pid=P7634
It is here where you will find your chemical.
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