DalisAndy
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Potassium peroxymonosulfate
What would the balanced decomposition in water of potassium peroxymonosulfate? Is there a mathematical why to tell? As a side question. I would like
to know the decomposition because I have a bottle of it my father was going to use for the pool but it reacts badly with his skin
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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kecskesajt
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KHSO5 + H2O -> KHSO4 + H2O2
Don't get in contact with his skin, but when it happens,flush it with warm water.
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PKMN
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What you have is simply a mix of:
- potassium sulfate
- sulfuric acid (not concentrated)
- hydrogen peroxide
So investigate these three chemicals to know.
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DalisAndy
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Sweet easy (relatively) sulfuric acid
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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DalisAndy
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Sweet easy (relatively) sulfuric acid
Elements Collected: 19/81 (Excluding all radioactive, using placecard for those)
Any tips or good sources are welcome.
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gdflp
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Quote: Originally posted by PKMN  | What you have is simply a mix of:
- potassium sulfate
- sulfuric acid (not concentrated)
- hydrogen peroxide
So investigate these three chemicals to know. |
That is incorrect. Since sulfuric acid is a significantly stronger acid than bisulfate in aqueous conditions, the equilibrium
H2SO4 + K2SO4 <--> 2 KHSO4 lies far to the right side. Very little free sulfuric acid
will be present.
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PKMN
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| Quote: Originally posted by gdflp | | Quote: Originally posted by PKMN | What you have is simply a mix of:
- potassium sulfate
- sulfuric acid (not concentrated)
- hydrogen peroxide
So investigate these three chemicals to know. |
That is incorrect. Since sulfuric acid is a significantly stronger acid than bisulfate in aqueous conditions, the equilibrium
H2SO4 + K2SO4 <--> 2 KHSO4 lies far to the right side. Very little free sulfuric acid
will be present. |
Practically same as sulfuric acid. Even NurdRage knowsthat.
[Edited on 23-8-2015 by PKMN]
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gdflp
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| Quote: Originally posted by PKMN | | Quote: Originally posted by gdflp |
That is incorrect. Since sulfuric acid is a significantly stronger acid than bisulfate in aqueous conditions, the equilibrium
H2SO4 + K2SO4 <--> 2 KHSO4 lies far to the right side. Very little free sulfuric acid
will be present. |
Practically same as sulfuric acid. Even NurdRage knowsthat.
[Edited on 23-8-2015 by PKMN] |
They are not practically the same compound. Sulfuric acid is a liquid and a strong acid while bisulfates are solids and weak acids. While they may
be interchangeable in some instances, they are most certainly not always interchangeable and there are many instances when sodium or potassium
bisulfate is useless in place of sulfuric acid.
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PKMN
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| Quote: Originally posted by gdflp | | Quote: Originally posted by PKMN | | Quote: Originally posted by gdflp |
That is incorrect. Since sulfuric acid is a significantly stronger acid than bisulfate in aqueous conditions, the equilibrium
H2SO4 + K2SO4 <--> 2 KHSO4 lies far to the right side. Very little free sulfuric acid
will be present. |
Practically same as sulfuric acid. Even NurdRage knowsthat.
[Edited on 23-8-2015 by PKMN] |
They are not practically the same compound. Sulfuric acid is a liquid and a strong acid while bisulfates are solids and weak acids. While they may
be interchangeable in some instances, they are most certainly not always interchangeable and there are many instances when sodium or potassium
bisulfate is useless in place of sulfuric acid. |
Only where dilute sulfuric acid is useless (e.g. making explosives, and dehydrations), bisulfate is useless. I think I said "dilute" already... And
bisulfate is almost liquid. It's always used dissolved or molten, like here. And of course it's not strong because it's diluted with other chemicals (sodium sulfate, water when dissolved).
And nobody can prove existance of persulfate anion.
For me it's analogous as hydrate, which is same as water.
Also bicarbonate = carbonate + carbonic acid.
Actually, it's a physical mixture.
Also, everybody can call me PhD here, if pokemon is hard to remember.
[Edited on 24-8-2015 by PKMN]
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gdflp
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| Quote: Originally posted by PKMN |
Only where dilute sulfuric acid is useless (e.g. making explosives, and dehydrations), bisulfate is useless. I think I said "dilute" already... And
bisulfate is almost liquid. It's always used dissolved or molten, like here. And of course it's not strong because it's diluted with other chemicals (sodium sulfate, water when dissolved).
And nobody can prove existance of persulfate anion.
For me it's analogous as hydrate, which is same as water.
Also bicarbonate = carbonate + carbonic acid.
Actually, it's a physical mixture.
Also, everybody can call me PhD here, if pokemon is hard to remember.
[Edited on 24-8-2015 by PKMN] |
There are many instances when dilute sulfuric acid can be used, but sodium bisulfate cannot. Some very simple examples are the synthesis of ionic
sulfates, qualitative and quantitative analysis, and concentrating dilute sulfuric acid to produce 90%+ sulfuric acid. Strong has nothing to do with
the concentration of compounds in water. YouTube videos are not reliable references.
What the hell are you talking about with persulfates? Bicarbonates are not the same as carbonates and carbonic acid, the equilibrium lies nearly
entirely towards bicarbonates at STP. Carbonic acid is unstable and will decompose to water and carbon dioxide, though this is of course an
equilibrium as well. Thus, if what you said had any merit, sodium bicarbonate would spontaneously lose carbon dioxide upon storage. It doesn't.
Let's see, what reincarnation is this?
We have :
-PhD.Chemist-
Ph.D.Chemist
PhD.Chemist
PhDChemist
P.h.DChemist
P.h.D.Chemist
PhD__Chemist
AsocialSurvival
vulture-admin-is-a-gay
EddyCu
Water2Gold
PKMN
You're getting quite the reputation, aren't you.(If you are who I think you are)
[Edited on 8-25-2015 by gdflp]
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