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Hexabromobenzene
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Electrolysis was performed using a new diaphragm with a layer of ion-exchange resin. The anode was iron. The amount of salt was 700 grams. 465 ml of a
solution weighing 600 grams was obtained, and some of the liquid remained in the crystallized salt(up to 50 ml). The sodium hydroxide yield was
approximately one-third-34% without remaining in salt. There was noticeably less iron oxide sediment in the anode chamber. In this case, approximately
1420 ml of iron chloride solution with a density of 1.23 was obtained.
If calculate based on ferric chloride, the yield is 57%. Of course, the ferric chloride solution contains salt, but there isn't much of it, and in any
case, the yield is too high.
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Hexabromobenzene
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I've reconsidered the theory. The data above is correct, and apparently the degree of sodium chloride decomposition by electrolysis cannot exceed 40%.
For potassium salts, the limit is somewhere just over 50%.
A layer of ion-exchange resin only slightly (a couple of percent) increases the current efficiency, but significantly inhibits the mixing of the
cathode and anode liquids. This isn't as critical when producing iron salts because iron hydroxide is immediately formed and blocks mixing. But it's
very important for producing sulfuric acid, for example.
If you have a huge pool of salt water, like the sea, you can always produce alkali or chlorides in very high yields.
An interesting fact is that even if the salt solution is only in one chamber, degree of sodium chloride decomposition is still one third.
[Edited on 12-1-2026 by Hexabromobenzene]
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Hexabromobenzene
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500 grams of calcium chloride dihydrate were dissolved in water to a volume of 3 liters. Electrolysis was carried out with an aluminum anode.
Approximately 6-8 Faradays of current were passed through the solution. 1135 grams of solution with a density of 1.2 were obtained in the anode
compartment. In the cathode compartment, a very large amount of a scale-like mass was obtained, which settled on the cathode. I cannot remove the
anode chamber without carefully breaking up the precipitate. The initial solution density was 1.1.
If we assume that only aluminum chloride is present in the anode chamber, then the yield is about 75%.
When might a similar synthesis be needed? For obtaining iron salts of carboxylic acids for pyrolysis and obtaining ketones.
Сurrent drops noticeably towards the end of the electrolysis at a voltage of 5 volts from 2.5-3 amperes to 0.7 amperes at the end. To complete the
electrolysis, the voltage needs to be increased.
[Edited on 24-1-2026 by Hexabromobenzene]
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Hexabromobenzene
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The alkali yield from potassium chloride will be revised. It is probably the same as from sulfate, about 50%. Additional experiments will be carried
out
The photo shows an aluminum anode and a stainless steel shower hose cathode. Convenient flexible cathode, but has high resistance. Several contacts
are attached to it, which are immersed in liquid during operation.
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Varungh
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I believe you can make ink from iron clorides. Those sell at a good price. You can try that.
Also any idea in how to obtain AlCl3 in neere anhydrous state? AlCl3(anhydrous) is useful to say the least.
Also AlCl3 hydrates release HCl on heating. Try that.
Use a borosilicate jar, thick. Maybe from those kitchen goods stores
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Hexabromobenzene
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I don't think you can obtain anhydrous aluminum chloride this way.
If you want it anhydrous, first obtain zinc chloride, calcine it, and mix it with aluminum powder.
Initially, I needed alkali, and the metal chlorides were a nice bonus. Then the method was improved. Reducing the anode area and adding a cation
exchange resin layer significantly increased the chloride yield.
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Hexabromobenzene
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Apparently, zinc chloride forms a stable anionic complex that sequesters zinc ions. This is good news, as it increases the current efficiency. I
achieved 35% salt conversion with only 70% of the theoretical charge. With a cation-exchange membrane, the efficiency would have been close to 100%.
Perhaps aluminum has similar properties.
Also, during electrolysis, a dense deposit builds up on the walls of the anode chamber, but thanks to the addition of a layer of ion-exchange resin
between the layers of fabric in the diaphragm, there is virtually no zinc hydroxide deposit that falls to the bottom. Zinc hydroxides are now formed
solely by electric current, not by alkali diffusion. Only small amounts of finely dispersed copper from the alloy contaminate the final solution.
Next, I will attempt to make a membrane from ground ion-exchange resin and polyethylene.
[Edited on 12-2-2026 by Hexabromobenzene]
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