chenbeier

https://images.app.goo.gl/RtqgCgdzHrNWMcpp9 https://images.app.goo.gl/48aDjbimwyGXnR3o8 Corrosion

That is your experience, I have another one. Old Lithiumcells get a white residue coming out the battery.

Of course yes, like every battery it will corrode and can harm electronically devices.

I wouldnt treat with any chemical, because corrosion will take place into the wire. This can cause overheating and probably also fire , depending on the current. The best is to cut and strip the wire again, if length is long enough. Or use cable lugs crimped or soldered.

I mean you can cutting or grinding the metal means scraping. The other one scrapping would be to dump the pump, but then I dont need cleaning of it.

Should be no problem to scrap the pumps. The green residue is also copper chloride. Cleaning with ammonia solutions possible.

Solder tips made by copper coated with iron, to prevent the dissolving. Pure copper , gold or silver get alloy with tin in will be dissolved.

Because we do not know the matrix of your water, easier it would be to take 1 l in a beaker , put a pH probe in and add slowly the acid during stirring. The consumed amount times 10,000,000 l gives the amount you have to add. There will be no free chlorine.

Stopp the Troll

Sorry you taking around the "hot porridge". No scientific datas. Tell us what are you doing.

I think it's only trolling, no scientific backgrounds.

Reaction 1 : 6CH4+2H2O+10O2 --> 6CO2+4H2+10H2O Reaction 2: C6H12O6+H2O+5O2 --> 6CO2+2H2+5H2O You have water as reactant and product makes no sense. You burn carbon and also partly hydrogen but also reduce hydrogen. This would be simple to Reaction 1 : CH4+ O2 --> CO2+2H2 Reaction 2: C6H12O6+3O2 --> 6CO2+6H2 Only oxidising the carbon but reducing hydrogen. But which plant use one of these processing.

I agree with that

Which people? Which nature’s efficient hydrogen production mechanisms you talking about. Never heard that nature produces hydrogen a reduced gas. Opposit oxygen by photosynthesis is well known.

I would try sulfur.

CrO3, H2CrO4, H2Cr2O7, etc. All are chromic acid.

Correct, it's difficult to keep it dry after open the container.

Chromium-VI-trioxide CrO3 is called in publics mouth as chromic acid. If it get wet then it reacts to a sludge n CrO3 + H2O => H2(CrO3)(n-1)CrO4 With n= 2 for example it will be H2Cr2O7 Dichromic acid.

For what reason you want to dry it. It's a very poisson and cancerogene stuff. Normally it will be dissolved in water or sulfuric acid as etching compound. Drying with Phosphorous pentoxide is possible.

You missing it's a weak acid. The dissociation of carbonic acid is not half H2CO3 half HCO3-. This is only valid if you have a buffer of carbonic acid and (sodium) hydrogencarbonate half half. Then pH is pKa according Hendersson Hasselbalch. pH = 0.5* (pka-logc) for weak acid.

But I don't think it's possible to get CO2 => C + O2 by electrolysis. Also with metal catalysts.

Only what exchemist already wrote The CO2 is converted to other compounds, which are conductive.

I think he want to electrolyze the liquid carbondioxide itself. But this is not working because it is not conductive.

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Because there are some more compounds in the battery like ammonium chloride, the practical voltage is 1,5 V https://www.azom.com/article.aspx?ArticleID=22363 The voltages can be found in electrical potential tables.