Hexabromobenzene - 21-8-2025 at 18:11
In my topic on electrochemical production of sulfuric acid I cited an interesting paper. It says that at a current density of 10 A/100 cm2 chloride
ions not destroy lead
This led me to wonder whether it is possible to obtain chlorates and perchlorates on small lead anodes. Of course, using small anodes will reduce the
current efficiency and it will probably be necessary to add sulfate to the chloride to reduce the solubility of lead, but it can work
Perhaps the anode can be wrapped in synthetic fabric to prevent destruction. Even if the anode is destroyed, you can use electrolysis to get the
spongy lead back and melt the electrode again as described in my topic on recycling lead batteries.
What do you think about this?
The main mechanism of lead protection in sulfuric acid without impurities is the high anode potential
Topic
[Edited on 22-8-2025 by Hexabromobenzene]
Hexabromobenzene - 21-8-2025 at 18:24
I'm not sure if you can make chlorate this way, but maybe you can make perchlorate?
MrDoctor - 21-8-2025 at 21:05
i have interacted with someone who had success but with great difficulty. a small one is likely out of the question though since the formation of
bubbles creates massive insulated voids that concentrate the current everywhere else, exceeding that local areas maximum density. if you experiment
with this youll likely want to do so under strong stirring.
also, you can indeed go straight from chloride to perchlorate, figuratively, but theres no clean transition where you just have chlorate, youll have
to concede to an unfinished chlorate batch, or one with perchlorate present. i dont recall the reaction conditions but i think that you need to begin
with chlorite present, theres a way to do it.
As for the lead, technically it still must be lead dioxide, just not the heavy sponge kind. with the weaker, less effective alpha type, you need to
run it hard within the range that it is catalytically active, i dont know where that is, it might just be at the peak there.
mysteriusbhoice/neru chan, figured this one out, shared said findings, and it has since been replicated, so if you dig, im sure its somewhere to be
found. its pretty much just, a certain temp, current density, and if not lead dioxide sponge then, a well made passivation layer like by using as an
anode for some time in sulfuric acid.
anyway attached is an image they shared with me once, the discussion wasnt about perchlorates, they just brought this up about how anodes can be
catalytically active for certain reactions at specific current densities, and lead dioxides is really high.
-note- it may be the case that it only works with NaCl, and possibly also only with , i want to say, persulfate? some sort of pH buffer may also be
employed, thats all i remember though, take with a grain of salt.
[Edited on 22-8-2025 by MrDoctor]
Hexabromobenzene - 21-8-2025 at 21:29
In my experience, lead anodes can work for weeks without significant destruction in a sulfuric acid solution. They are passivated because at the
electrolysis potential, a protective layer of lead dioxide is always formed and lead dioxide conducts current well
But if you add an easily oxidizing substance (depolarizer), then the lead anode will corrode even under a layer of lead dioxide
But if the substance has a high oxidation potential, then this will work. Of course, it will not be as stable as lead dioxide itself. You also need to
add a sulfate additive to prevent the leakage of lead ions from the anode.
I think you can synthesize persulfates and perchlorates with a lead anode
But you will not be able to obtain chlorine or oxidize, for example, ethanol
You can also try to first do electrolysis in an alkaline solution to coat the lead with alpha dioxide.
[Edited on 22-8-2025 by Hexabromobenzene]