Sciencemadness Discussion Board - Hydroclhloric acid (and HCl gas) production from salt (NaCl) electrolysis (small scale Chloralkali process)

Hydroclhloric acid (and HCl gas) production from salt (NaCl) electrolysis (small scale Chloralkali process)

experimenter_ - 9-4-2016 at 11:57

In brief, a concentrated sea salt solution is electrolysed, the gases (H2/Cl2) are reacted together under UV light and the resulting hydrogen chloride is dissolved in water.
Previous failed attempts and background ideas can be found in this thread [ https://www.sciencemadness.org/whisper/viewthread.php?tid=21... ]. I think that many of the problems have been solved and this method shows potential to produce practical amounts of hydroclhloric acid; at least my device. In the current stage of development the key elements of the design are the following:

- Two graphite electrodes (acquired from zinc batteries)
- A salt water container with two seperate compartments connected electrically with a "salt bridge" made out of filter paper
- A UV black light lamp in parallel with a glass tube where the gases combine

Check the attached schematics for the detailed info. There is also a picture of the device (not very pretty on the outside but she has hidden graces :-) )

My frist measurement on the efficiency of the device was the following:
A 0.2A input electrode current for 2h produced the equivalent of ~ 0.8ml 10% HCl solution (or 0.08gr HCl or ~ 0.0022 mol HCl). The theoretical amount according to Faraday law should be 0.015mol. Thus the efficiency is 6.8%.

Of course I'm not convinced that this number is the best efficiency I can get out of the device. For example I detect Cl2 in the output which means that a bigger UV tube is needed. Or my electronics to light the UV tube do not produce much current (I don't have ballast but a small HV transformer). Also I see the reaction tube to be full of droplets. Those are made of concentrated HCl that captures air moisture and never reaches the output water. If the glass tube is opened a white mist (HCl) evolves out of it (it gets hot also). Finally, in the electrolysis chamber, the Cl2 gas has a chance to touch the surface of the NaOH solution even if it is not bubbled through it (design flaw). Maybe it gets absorbed there? Anyway, there is a lot of room to apply fixes for better efficiency but even if it stays below 10% that is ok.

About the output capacity, in this crude form at 0.2A input current, the device would give 10ml of azeotropic HCl in 2 days. But the salt bridge can carry up to 2A and the electrodes can easily acquire more surface. So a target output capacity of 100ml per 2 days is not out of reach. The main limiting factor is the UV lamp, right now it is of a such small intensity that it can barely handle the gases produced by the 0.2 A electrolysis current.

In conclusion:
Pros
- Production of HCl out of salt and electricity only
- Production of hydrogen chloride gas. Instead of diluting it in water, other uses might be employed too.
- Production of NaOH out of electrolysis of salt
- Production of Cl2 or H2 separately is possible

Cons
- HCl acid produced is contaminated with dissolved Cl2 (major problem; working on its solution)
- Inherent dangers of explosion. For example, the glass tube where Cl2/H2 gases mix, if not exposed continualy to UV light, can build up a lot of Cl2/H2 gas that might explode and shatter it (unfortunately plastic tube blocks UV light). Also there is a lot of air space in the electrolysis container where Cl2/H2 gases could mix. Those are design flaws hopefully to be corrected in later versions. Some "watchdog" electronics could help with this problem too.
- Cl2 gas is poisonous if escapes in the air (well it is not so much since the smell threshold is far below the dangerous concentrations but still one cannot leave the device running unattended inside closed space)
- NaOH produced is contaminated with a lot of NaCl (but it is not a big problem for many applications)

Some questions:
- For how long will the device be able to work until some kind of failure happens? For example, will the carbon electrodes corrode too soon. Will the catholyte mix with the anolyte after some days (and the Cl2 will touch the NaOH)
- What is the maximum concentration of NaOH that can be achieved before the solution in the cathode must be changed with fresh NaCl? Why not reaching up to 100% ?
- Will a longer UV tube be able to eliminate all of the Cl2 before it touches the water? Should more H2 be added?

[Edited on 10-4-2016 by experimenter_]

macckone - 10-4-2016 at 11:46

Good writeup

elementcollector1 - 10-4-2016 at 14:15

Question: What is the purpose of the cell of NaCl to the leftmost side of the apparatus? It has no electrode, and I don't think it'll serve as a reservoir for NaCl, considering how slow it would come over the filter paper. (Edit: Is this a concentric-ring design? That would explain it.)

To answer some of your questions...

1) Hard to say. Usually, the limiting factor is either the electrodes corroding to pieces or the filter paper that is exposed to air drying out (at least, it was for me). A quick note: You don't need carbon electrodes on both sides. Use an iron or steel cathode; it'll have less internal resistance and thus transmit more current (for faster yield).

2) Again, hard to say. Theoretical maximum would be a saturated solution of NaOH in water. There shouldn't be much preventing this, because of all the ionic (and therefore conductive) species in solution.

3) If I recall, electrolysis that splits the water will produce 2 mol of H2 for every mol O2, and electrolysis that splits the salt will produce 1/2 mol of Cl2 at the same rate. At a ratio of 2 mol H2 to 0.5 mol Cl2... no, you shouldn't need to add more hydrogen. More UV light will most likely add to the yield, but I'm not sure.

Electrolysis, despite being one of my favorite things to do, is not my strong suit in terms of analysis. So if anything above is wrong... well, I guess you'll just have to take things with a grain of NaCl.

[Edited on 4-10-2016 by elementcollector1]

macckone - 10-4-2016 at 18:31

Limiting factors are filter paper degradation by sodium hydroxide, flow of sodium hydroxide back across the cell and electrode degradation.

WGTR - 10-4-2016 at 18:54

I think that graphite will be fine for an anode, so long as the amount of chloride ion is kept high, and the anolyte pH is kept fairly neutral or lower. Also, keep the cell running cool. These things help ensure that you're producing mainly chlorine instead of oxygen. Once you start getting oxygen at the anode, the oxygen goes ommm nom nom on the graphite, and it starts disintegrating.

experimenter_ - 11-4-2016 at 05:29

Thanks for the interest guys.

Quote: Originally posted by elementcollector1

(Edit: Is this a concentric-ring design? That would explain it.)

Yes, there is one more smaller pvc pipe inside the container glued to the bottom. The cables reach the electrodes through the bottom of the cylindric pvc box, not visible in the picture.

Quote: Originally posted by elementcollector1

3) If I recall, electrolysis that splits the water will produce 2 mol of H2 for every mol O2, and electrolysis that splits the salt will produce 1/2 mol of Cl2 at the same rate. At a ratio of 2 mol H2 to 0.5 mol Cl2... no, you shouldn't need to add more hydrogen. More UV light will most likely add to the yield, but I'm not sure.

I think that H2 and Cl2 are produced in equal moles. Na+ and Cl- require only one electron to reduce/oxidize so...
Wiki ( https://en.wikipedia.org/wiki/Chloralkali_process ) says: 2NaCl + 2H2O → Cl2 + H2 + 2NaOH

Quote: Originally posted by elementcollector1

... well, I guess you'll just have to take things with a grain of NaCl.

I miss scientific humour!

I've been looking around the forum and found some other relevant threads:
https://www.sciencemadness.org/whisper/viewthread.php?tid=22...
https://www.sciencemadness.org/whisper/viewthread.php?tid=25...
https://www.sciencemadness.org/whisper/viewthread.php?tid=17...

Also a link outside the forum:
http://woelen.homescience.net/science/chem/exps/miniature_ch...
(woelen is the owner of this forum?)

It seems that an unglazed flower pot can be used instead of the filter paper bridges and a titanium MMO anode (what is that MMO?) instead of the carbon electrodes. So, in case the paper bridge is eaten up or the electrodes corrode there are some possible future solutions.

My priority consideration now is to find a practical way to eliminate Cl2 from the output. Even when the H2/Cl2 flow through the UV tube is very slow the gas don't seem to react completely. I'm afraid that too much excess H2 will be needed or impractically long UV tube in order to eliminate Cl2. Leaving it in the sun few days will not do the trick.

Some guy suggested to bubble SO2 in the output water. Supposeddly reaction with Cl2 will give H2SO4 + HCl and then we distill the clean HCl out of H2SO4. But I doubt that SO2 + Cl2 (+ H2O) gives H2SO4 only.

Someone else suggested it is easier to make H2SO4 from the SO2 and then distill HCl out of NaCl. Hm, maybe ..

[Edited on 11-4-2016 by experimenter_]

New observations

experimenter_ - 11-4-2016 at 07:21

A new run for 9hours at 0.2A was completed. It produced the equivalent of ~2.7ml 10% HCl. The efficiency this time was about 11%. :cool:

An inspection on the insides showed that the electrodes show no sign of corrosion (probably due to the very small current; only 0.2A) and the anolyte is still acidic. The catholyte is very basic (NaOH) but it has almost dissolved the filter paper that was hanging on this side of the cell.

hissingnoise - 11-4-2016 at 07:25

Quote:

Someone else suggested it is easier to make H2SO4 from the SO2 and then distill HCl out of NaCl. Hm, maybe.

Jeez, am I missing something here . . . ?

Just to be clear, you can simply toss some salt into a flask, add enough conc. H₂SO₄ to cover it (reaction is immediate and vigorous) and dissolve the evolved HCl gas in water using an inverted funnel, et voilà!

When the initial reaction slackens, heating the sol. will drive it to completion!

And using distilled water gives pure acid as only HCl comes over . . .

aga - 11-4-2016 at 10:30

Quote: Originally posted by experimenter_

A new run for 9hours at 0.2A was completed. It produced the equivalent of ~2.7ml 10% HCl. The efficiency this time was about 11%. :cool:

Very nice experiment, and glad to see that you're improving the process.

Keep going !

Edit:

I read quite a while back an experiment that used a thin terracotta plant pot for the 'membrane' or 'salt bridge'.
Cannot remember where.

[Edited on 11-4-2016 by aga]

hissingnoise - 11-4-2016 at 12:02

Quote: Originally posted by aga

Quote: Originally posted by experimenter_

A new run for 9hours at 0.2A was completed. It produced the equivalent of ~2.7ml 10% HCl. The efficiency this time was about 11%. :cool:

Very nice experiment, and glad to see that you're improving the process.

Yeah, the big problem with HCl from salt/acid is that it can take as much as a full second to produce twice that amount of HCl.

experimenter_ - 11-4-2016 at 14:59

To hissingnoise:

Quote:

Someone else suggested it is easier to make H2SO4 from the SO2 and then distill HCl out of NaCl. Hm, maybe.

Jeez, am I missing something here . . . ?

You are right, but since the forum is called sciencemadness I hope it can host the method of this thread too. It is not the best or the most efficient but I find it a more elegant way to produce HCl. Something like an art project.

When completed, some other differences compared to the salt/acid method will be:

- If you live by the sea, there is no need to buy anything from anyone
- Besides HCl, it could give H2, Cl2 and NaOH out of nothing
- It is smaller than a distillation setup and more portable (no need for heating mantle, condenser etc..)
The drawback is that it requires patience but consider it like having a salt eating pet that keeps some company.

Don't judge it too soon, the current can rise up to 2A within the same device..

To aga:

Quote:

Thanks aga, I'll keep you updated! I think this is the thread you are talking about (or sth similar):
https://www.sciencemadness.org/whisper/viewthread.php?tid=27...

hissingnoise - 12-4-2016 at 05:18

Quote:

It is smaller than a distillation setup and more portable (no need for heating mantle, condenser etc..

WTF! This is about simply generating and dissolving a soluble gas in water!

Two friggin' containers connected by a short plastic tube . . .

I don't know where you got the idea that distillation was involved!

MrHomeScientist - 12-4-2016 at 06:19

I've done the "flower pot cell" before as an experiment to produce NaOH. It worked, albeit very slowly. The real problem I found is how to permanently seal the hole in the bottom of the flower pot. Tape falls off and caulk quickly degrades in the basic environment!

WGTR - 12-4-2016 at 10:21

Quote: Originally posted by experimenter_

One idea is to have a third (small) compartment in between the cathode and anode compartments. This is where fresh NaCl solution is added. The addition rate should be fast enough to keep the anolyte and catholyte from infiltrating the addition compartment, but not so fast that electrolysis can't keep the solutions from becoming diluted excessively. The overflow from both compartments can be collected as products.

The separators could be made from bundles of capillary tubing, or something that will allow laminar flow from the addition compartment, while limiting turbulence that could promote back-mixing between adjacent compartments, if that makes sense.

It might even be possible to use cotton wool as a separator in a larger glass tube, so long as the fresh NaCl flows through it at a rate that keeps the concentrated products away from it.

experimenter_ - 12-4-2016 at 12:25

Quote: Originally posted by WGTR

Thanks for the input; I think the idea is a bit advanced for the time being. Adding salt solution and removing products while electrolysis is running seems too much for me to apply.
But I'll keep your advice on capillary tubing. I could use them as a salt bridge after giving them U shape in case i can't find any other material that can withstand the lye solution. I would like to avoid the "flower pot" method.

Quote: Originally posted by MrHomeScientist

I've done the "flower pot cell" before as an experiment to produce NaOH. It worked, albeit very slowly. The real problem I found is how to permanently seal the hole in the bottom of the flower pot. Tape falls off and caulk quickly degrades in the basic environment!

I use "Bison montage kit" ( https://www.bison.nl/static/uploads/bison/folders/montagekit... ). It can withstand Cl2 and NaOH. I'm sure it can adhere onto the flower pot too. If you can find this glue, it worths to give it a try.

experimenter_ - 13-4-2016 at 06:35

Quote: Originally posted by hissingnoise

Quote:

It is smaller than a distillation setup and more portable (no need for heating mantle, condenser etc..

I wasn't aware that this method you describe could be employed practically; I was thinking that one should distill hydrochloric acid out of a dilute solution of H2SO4 and sea salt so that there is some water to come over together with the HCl gas in order to capture it (similar way to making nitric acid).
So, if a way to regain sulfuric acid from the sodium bisulfate could be found, this method could be compared with the direct NaCl electrolysis described in the thread. For example, if electrolysis of sodium bisulfate (towards sulfuric acid and NaOH) in a membrane cell could be applied, this would mean that salt can be converted to HCl by the use electricity only. The toxic Cl2 gas, danger of explosion and Cl2 contamination in the product would be avoided completely in that way but I'm afraid it has some of its own drawbacks too. If recycling the H2SO4 is possible I would consider it.

experimenter_ - 13-4-2016 at 08:56

Another way to remove dissolved Cl2 in the output HCl solution could be to react it with H2O2. In theory, this reaction happens:

HClO + H2O2 --> HCl + H2O + O2

I don't know yet what might happen in practice.

Bezaleel - 14-4-2016 at 09:40

Experimenter_, nice to read this thread on your efforts.

I'd like to point out that the efficiency in your first experiment was actually 14.9%, as 0.0022/0.015 = 0.149.

hissingnoise's method is much easier, but requires an acid to start with. Also, you would need to use a long tube from the funnel to your collecting flask, in order to catch any aerosols.

In you electrolysis setup, you might consider the following:

* Use UV LEDs (check ebay or suppliers whether the required wavelength is available). If you would use a mirroring tube in which you bore holes to fit your LEDs, you'd have a considerable improvement in efficiency with respect to UV. Your reaction tube runs inside the mirroring UV tube.

* Suspend the UV reaction tube vertically, so that condensation droplets will run into your flask.

* Use the membrane of a lead-acid battery. You'll need the old, wet type of battery. I used the membranes from these batteries with great success electrolysing NaOH solution with SS (stainless steel) electrodes (304 alloy works fine in that setup, 316 is not needed). They helped me keeping H2 and O2 separated.

experimenter_ - 14-4-2016 at 21:55

The points you made are right on spot Bezaleel. Your last point about the readily available membranes opens up many new possibilities. Obviously you have some good hands on experience on electrolysis, thanks.

elementcollector1 - 15-4-2016 at 05:30

Quote: Originally posted by Bezaleel

* Use the membrane of a lead-acid battery. You'll need the old, wet type of battery. I used the membranes from these batteries with great success electrolysing NaOH solution with SS (stainless steel) electrodes (304 alloy works fine in that setup, 316 is not needed). They helped me keeping H2 and O2 separated.

You mean like these batteries?

macckone - 15-4-2016 at 12:27

Those are gel type. Not all wet types have separators. Most likely are deep cycle wet cells.

Bezaleel - 17-4-2016 at 06:59

Quote: Originally posted by elementcollector1

Quote: Originally posted by Bezaleel

You mean like these batteries?

No, I think these are the newer type of dry cells. As far as I know, wet batteries always have compartments (cells) that can be refilled with water. They have screw caps on top of them for each cell. In my case the screw caps needed to be opened with a philips screw driver, see the picture.

Edit:

Quote: Originally posted by macckone

Those are gel type. Not all wet types have separators. Most likely are deep cycle wet cells.

Thanks, Macckone. I didn't know this, so I have been lucky opening one that did have the separators.

[Edited on 17-4-2016 by Bezaleel]

macckone - 17-4-2016 at 07:48

Yes that is a deep cycle from the picture.

One note on the three compartment system is that three compartment cells are used to
Recycle sodium sulfate into sodium hydroxide and sulfuric acid. Commercially they use
Membrane cells that are ion specific but there is no reason a diaphram cell could not do
The same thing to produce hydroxide and bisulfate. This could lead to otc sulfuric acid.
Epsom salt and baking soda yield sodium sulfate. Both are readily available in all but the
Worst war zones.

XeonTheMGPony - 29-4-2016 at 07:20

With out reading the whole thread I used a simpler combustion process, I built this system at 15 when I was far less interested int he science then I am now days.

I used a mercury cell: A tank with a partial divider, bottom filled with mercury till sealed. The tank was built to allow max surface area with minimal depth so it only took a few grams of mercury to accomplish the seal. Bottom of tank had a 316L SS nut and bolt and a second nut to attach the wire.

the brine tank, Same bolt configuration, but the positive electrode was finely coiled SS welding wire that was 1.5 inches from the bottom of the tank.

Tank was made of aquarium glass (When I was fifteen I had a weird obsession with making 2/300g terrariums so had ample glass working gear)

Top plate was machined to allow fluid in and the other side gasses out then it was epoxied on.

these tubes where led to water flash back arresters I had made out of film containers.

These then led to a large glass jar where the ends met at a spark plug, the third hole was the exhaust that led to ice water. The spark plug was driven by a high voltage supply and it was started first.

1 - Starting sequence: HV supply to the spark plug
2 - Check gas valve leading reactor to ensure they where off
3 - Start cell, and allow to build some pressure.
4 - Crack the chlorine line open and purge line
5 - Slowly open H2 line and then throttle up the chlorine till both where fully open and a self supporting flame was present

6 - Shut down the HV line to the spark plug.

That's all I really remember other then it worked well, I think now days I'd use a chromatography column with a couple 30guage hypodermic needles and BBQ sparker to kick off the reaction

Take the column and at the reservoir side put in a rubber stopper and push the needles in so the tips just meet.

run the discharge side to the ice water

precharge the column with Cl2 then once flooded start admitting the H2 and ignight to form the HCL. Should make a much more compact and efficient generator.

XeonTheMGPony - 29-4-2016 at 07:24

Quote: Originally posted by hissingnoise

Quote:

Someone else suggested it is easier to make H2SO4 from the SO2 and then distill HCl out of NaCl. Hm, maybe.

Why waste Sulfuric when you can do it super cheap with electricity and a cell? Only real consumables become water and salt!

experimenter_ - 29-4-2016 at 10:21

Quote: Originally posted by XeonTheMGPony

I built this system at 15 when I was far less interested int he science then I am now days.

Mercury and chlorine gas at the age of 15 ... :cool:

hehe

Quote: Originally posted by XeonTheMGPony

the brine tank, Same bolt configuration, but the positive electrode was finely coiled SS welding wire that was 1.5 inches from the bottom of the tank.

As I understand it, you used SS welding wire as the anode where chlorine is generated. Did you find it to be resistant to chlorine? Maybe I could replace the carbon electrode.

Thanks for sharing with us your findings.

XeonTheMGPony - 29-4-2016 at 12:59

it held up well enough when I was running it, cant remember much more then that been so long.

and as for the stuff I was playing with at that age that was the safest! Advantages of growing up in remote heavy industry

kt5000 - 4-5-2016 at 12:34

Quote: Originally posted by MrHomeScientist

I tried the same thing last fall. My wife found a bisque clay shot glass at a craft store with no hole in the bottom, the type you'd paint and bake in a kiln. It seemed to work well but the NaOH production was really, really slow.

Jstuyfzand - 11-5-2016 at 13:46

I was wondering you could just bubble the chlorine into the water, making HCl and HClO, and simultaneously expose the water to UV, I read somewhere that the HclO then turns into Hcl and o2 or just leaves the solution as chlorine gas.(?)

My attempt at chlor-alkali process:v0.1

Zandins - 23-6-2016 at 04:10

Greetings sciencemadness community,

For a while now, I have contemplated and tested various chloralkali setups, and seem to have found one that somewhat works.
The electrolytic cell is an empty ice-cream box with a total volume of 1.2 L. The cell is partitioned by an asbestos fiber diaphragm, held in place by epoxy resin glue. I originaly tried filter paper, which proved vulnerable to the strongly alkaline conditions. Asbestos,however, works well.
The cathode component is 4 times larger that the anode compartment, to accomodate more NaOH. For the cathode, a stainless steel strip with a surface area of 20 cm2 was used. The anode is a carbon rod taken from a battery. The anode corrodes in the acidid condictions, forming a paste of carbon particles on the surfac3 of the anode compartment.
Power is provided by 3 parallel PSUs on the 12V rail. After running the electrolysis for 6 hours at around 6A, circa 1L of 1.1M NaOH solution has been produced. This corresponds to 81.1% efficiency.
Once I get my gas-collection system running, I will start producing HCl by collecting the gases and exposing them to UVC.
Current problems with the setup:
1)Erosion of the graphite electrode. Here to stay until I get my PbO2 done;
2)Copper cable providing current to the anode is attacked by the Cl2 gas, producing CuCl2.
Would love to hear any thoughts, suvgestions, etc!

Zandins

[Edited on 2-7-2016 by Bert]

Please re-size your pictures to just large enough to show the details relevant to your post!!! You blew the margins, are you a mass nerderer or something...

http://www.sciencemadness.org/talk/viewthread.php?tid=66853#...

[Edited on 2-7-2016 by Bert]

[Edited on 2-7-2016 by Bert]

Jstuyfzand - 5-7-2016 at 13:43

Quote: Originally posted by Zandins

Greetings sciencemadness community,

For a while now, I have contemplated and tested various chloralkali setups, and seem to have found one that somewhat works.
The electrolytic cell is an empty ice-cream box with a total volume of 1.2 L. The cell is partitioned by an asbestos fiber diaphragm, held in place by epoxy resin glue. I originaly tried filter paper, which proved vulnerable to the strongly alkaline conditions. Asbestos,however, works well.
The cathode component is 4 times larger that the anode compartment, to accomodate more NaOH. For the cathode, a stainless steel strip with a surface area of 20 cm2 was used. The anode is a carbon rod taken from a battery. The anode corrodes in the acidid condictions, forming a paste of carbon particles on the surfac3 of the anode compartment.
Power is provided by 3 parallel PSUs on the 12V rail. After running the electrolysis for 6 hours at around 6A, circa 1L of 1.1M NaOH solution has been produced. This corresponds to 81.1% efficiency.
Once I get my gas-collection system running, I will start producing HCl by collecting the gases and exposing them to UVC.
Current problems with the setup:
1)Erosion of the graphite electrode. Here to stay until I get my PbO2 done;
2)Copper cable providing current to the anode is attacked by the Cl2 gas, producing CuCl2.
Would love to hear any thoughts, suvgestions, etc!

Zandins

[Edited on 2-7-2016 by Bert]

Please re-size your pictures to just large enough to show the details relevant to your post!!! You blew the margins, are you a mass nerderer or something...

http://www.sciencemadness.org/talk/viewthread.php?tid=66853#...

[Edited on 2-7-2016 by Bert]

[Edited on 2-7-2016 by Bert]

12V seems a bit high, have you tried 5V?
Corrosion should be less.

May I ask what route to PbO2 you are taking?

Zandins - 6-7-2016 at 03:07

Quote: Originally posted by Jstuyfzand

12V seems a bit high, have you tried 5V?
Corrosion should be less.

May I ask what route to PbO2 you are taking?

12V probably is overkill, although they were necessary to push any sizable current through the cell due to the small surface area of the carbon rod.
As for the PbO2, I plan to cast a lead plate and electroplate it with PbO2 in H2SO4 solution in-situ. There are varying accounts on the feasibility of this method, so I intend to try it out before moving to more sophisticated approaches.
The general problem seems to be the flaking of the PbO2 layer in strongly corrosive conditions. However, if the coating would be grown thick enough to prevent any of the substrate from being exposed, I conjecture it could hold, at least in a chlor-alkali cell(opposed to chlorate of perchlorate). Meanwhile I am also looking into platinized titanium - if any were to be found at a reasonable price, all the aforementioned problems would be eliminated.

Jstuyfzand - 6-7-2016 at 03:48

I saw something about graphite rods and anodes being corroded faster in basic environments, I guess chloralkali would be less harsh on the electrodes since the anode bath stays neutral when you are using a separated cell.

hissingnoise - 6-7-2016 at 07:23

Quote:

I saw something about graphite rods and anodes being corroded faster in basic environments

A graphite cathode in a chlorate cell is quite unaffected by the high pH which arises in a working cell!

Acidity at the anode is damaging, obviously...

Fleaker - 6-7-2016 at 07:30

Have you tried just plain ol' titanium for the anode of a chlorate cell?

Reason I ask is I have several hundred square foot worth of 16 gauge titanium CP2 sheet that I can easily shear up.

Jstuyfzand - 6-7-2016 at 07:37

Quote: Originally posted by Fleaker

Have you tried just plain ol' titanium for the anode of a chlorate cell?

Reason I ask is I have several hundred square foot worth of 16 gauge titanium CP2 sheet that I can easily shear up.

Titanium will passivate and no current will flow, wont work.

By the way, how are you all using these asbestos plates as diaphrams when that stuff is carcinogenic and prohibited?

Passivation

Zandins - 6-7-2016 at 07:38

As far as I am aware, titanium passivates in anodic conditions as it is oxidised to TiO2,which is nonconductive. Therefore, it can only be used as a cathode.