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Hexavalent
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This would work in theory, but would again be limited by the very low solubility of calcium hydroxide in water.
Again, what is wrong with buying it from stores (it is very cheap and often very pure) or online? It is much easier to buy it than to make it, unless
you are purely doing it to explore the science or as a 'proof of concept' experiment.
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Manifest
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Quote: Originally posted by Hexavalent  | This would work in theory, but would again be limited by the very low solubility of calcium hydroxide in water.
Again, what is wrong with buying it from stores (it is very cheap and often very pure) or online? It is much easier to buy it than to make it, unless
you are purely doing it to explore the science or as a 'proof of concept' experiment. |
Would you need to add water? You could do it dry...
I said for the record. I have already bought some from Boots(thank you!)
Also, there is something just fucking awesome about making things yourself and as you said exploring the science.
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Hexavalent
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I'll drink to that
Glad you found your NaOH in Boots.
I see, be you proposing heating stoichiometric quantities of calcium hydroxide and sodium carbonate in a vessel, and then dumping the contents into
water? That would make sense, and I rather think it would work. I've prepared ammonia gas previously by dry heating NH4Cl with with
Ca(OH)2...perhaps the same concept works here too? I might try that sometime if I have spare time in the lab, and I shall report back.
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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elementcollector1
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The above never occurred to me... it would certainly be an interesting method of preparation.
Now, how do we go about getting potassium carbonate, and thus make KOH?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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blogfast25
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| Quote: Originally posted by elementcollector1 | The above never occurred to me... it would certainly be an interesting method of preparation.
Now, how do we go about getting potassium carbonate, and thus make KOH? |
Potassium carbonate is historically known as 'potash' (from which also the name 'potassium' is derived). 'Potash' is literally the leachate obtained
from leaching wood ash with hot water (in pots). Filtering and evaporating the filtrate yields a poor quality K2CO3. Yield is small and varies.
Better K2CO3 is obtained from calcining OTC Cream Of Tartar. That grade is known as 'pearl potash' because it is superior to potash.
There are threads on all that here.
And yes:
Ca(OH)2(s) + K2CO3(aq) === > CaCO3(s) + 2 KOH(aq)
... works.
[Edited on 10-12-2012 by blogfast25]
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Random
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| Quote: Originally posted by Manifest | | Quote: Originally posted by Random | I make NaOH that can comfortably dissolve aluminium with baking soda and ca(OH)2 solid large excess, add water, mix and leave for some time, then I
filter everything and store it
I am not sure what concentration it is though. |
I don't understand what you mean.
You can dissolve aluminium and baking soda with the NaOH?
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No...I make my own NaOH solution by mixing a large excess of Ca(OH)2(s) with baking soda and add some water then filter.
I am not sure which concentration the solution is but it can dissolve aluminium easily.
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Manifest
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| Quote: Originally posted by Random | | Quote: Originally posted by Manifest | | Quote: Originally posted by Random | I make NaOH that can comfortably dissolve aluminium with baking soda and ca(OH)2 solid large excess, add water, mix and leave for some time, then I
filter everything and store it
I am not sure what concentration it is though. |
I don't understand what you mean.
You can dissolve aluminium and baking soda with the NaOH?
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No...I make my own NaOH solution by mixing a large excess of Ca(OH)2(s) with baking soda and add some water then filter.
I am not sure which concentration the solution is but it can dissolve aluminium easily. |
LOL.
I can't see how I didn't understand you when you posted it.
I'm stupid I guess.
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