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09-08-2005, 03:34 AM | #11 |
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I can see calcium deposits after 3hrs of electrolysis. However I'm stopping the process temp due to the fact that chlorine might be released (in my bedroom!) while I'm sleeping.
I will be starting another pc by using solar power |
10-08-2005, 01:41 AM | #12 |
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Seems like there is too much current used. Serious precipitation occurs.
Its greenish because oxidation by the anode. |
10-08-2005, 01:45 AM | #13 |
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Despite of all the precipitation, there is still calcium deposit after 12hrs.
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10-08-2005, 01:47 AM | #14 |
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This is the solar cell which will be replacing the transformer. It will be providing 10VDC for the electrolysis.
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10-08-2005, 08:59 PM | #15 |
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After getting a mixture of greenish precipitate with brown scum. I have decided to split the anode and cathode into 2 separate containers.
This is the anode container with the green precipitate and the cathode container with brown precipitate. |
10-08-2005, 09:38 PM | #16 |
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While I'm not good with chemistry, I will try to explain whats happening here. Please do correct me if there are any errors.
The positive terminal (anode) is oxidising and will breakdown salt (sodium chloride, NaCl). Oxidation of chloride ions to chlorine 2Cl- ---> 2Cl2 + 2e- Chlorine + water -> hypochlorous acid + hydrochloric acid Cl2 + H2O ---> HOCl + HCl Both are liquid form of chlorine suitable for disinfection. The green precipitate could be any metal chlorides, maybe iron chloride (greenish) The negative terminal (cathode) is reducing. Reduction of sodium ions Na+ + e- ---> Na Reaction of sodium to sodium hydroxide (caustic) Na+ + H2O ---> 1/2H2 + NaOH So what if both acids(HCl & HOCl)produced at the anode react with the NaOH produced at the cathode? HCl + NaOH ---> NaCl + H2O and, HOCl + NaOH ---> NaOCl + H2O The final product of electrolysis is:
NaCl + H2O ---> NaOCl + H2 NaOCl = Sodium hypochloride aka bleach! The same stuff used for bleaching clothes. IMHO, electrolysis is not suitable for hobbyist tanks. The by products of saltwater electrolysis are far too dangerous to be used in our small tanks. |
10-08-2005, 09:38 PM | #17 |
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hhhmmm..
this is interesting... i assume that the steel electrode used is not inert and if so it reacts... so the green precipitate at the anode is from the oxidation of iron to iron 2+ ...precipitate being Fe(OH)2 and the brown precipitate is iron 3+ as it is being further oxidised by air to form Fe(OH)3 however i have no idea what the brown precipitate at the cathode is... this is really interesting |
10-08-2005, 09:52 PM | #18 | |
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thanks for testing the method out...it really is too dangerous for carrying out in our tanks |
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10-08-2005, 10:29 PM | #19 | |
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Quote:
I may bring this experiment offshore and see what happens |
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