good excerpt from one of the pdf's above, but does CT guy have the citation anywhere?
Hydrogen peroxide can be used for dechlorination, in other words to remove residual chlorine. Residual chlorine forms corrosive acids when it is oxidised by air or condensates on process systems.
When chlorine reacts with hydrogen peroxide, hydrogen peroxide falls apart into water and oxygen. Chlorine gas hydrolyses into hypochlorous acid (HOCl), which subsequently ionises into hypochlorite ions (OCl).
Cl2 + HOCl + H+ + Cl
HOCl + H+ + Cl
After tha, hydrogen peroxide reacts with hypochlorite:
OCl- + H2O2 (g) -> Cl- + H2O + O2
The reaction between hydrogen peroxide and hypochlorite takes place very quickly. Other organic and inorganic substances cannot react with hypochlorite.
Read more: http://www.lenntech.com/processes/d...nfectants-hydrogen-peroxide.htm#ixzz1GQVfarZO
Advantages
Contrary to other chemical substances, hydrogen peroxide does not produce residues or gasses. Safety depends on the applied concentration, because hydrogen peroxide is completely water soluble.
Disadvantages
Hydrogen peroxide is a powerful oxidizer. It reacts with a variety of substances. It is therefore diluted during transport, as a safety measure. However, for hydrogen peroxide disinfection, high concentrations are required.
Hydrogen peroxide slowly decomposes into water and oxygen. An elevation of temperature and the presence of pollutions enhance this process.
The concentration of hydrogen peroxide in a solution slowly decreases. This is caused by the following reaction:
2 H2O2 → 2 H2O + O2
This is a redox reaction. Hydrogen molecules partly function as reductors and partly as oxidizers.
Is hydrogen peroxide efficient?
The efficiency of hydrogen peroxide depends on several factors, such as pH, catalysers, temperature, peroxide concentration and reaction time.
Read more: http://www.lenntech.com/processes/d...nfectants-hydrogen-peroxide.htm#ixzz1GQWMG0Kk
perhaps one of them, that know their shit, could explain to us how h202 couldn't possibly remove or bind chlorine, yet the above shows a cited study that states otherwise? (source provided by you, Microbeman)
In any even, it was not a smartasses post, and now that you actually found out something you didn't know...does it now make more sense that I would post it, mad?Blackstrap does not neutralize chlorine. Where are we getting that from?
Perhaps the chap that stated one or two drops per gallon was thinking about H202 instead of molasses?
I'm not sure of the need for all the arguing....
In regards to removing chloramine, if it's even necessary, one would use sodium thiosulfate. A carbon filter could also be used, as could commercial water conditioners designed to remove it, but I believe they'd contain carbon...... I believe the levels are so small that it would have no ill effects upon plants regardless.
You can go to aquarium supply stores and get a bottle for about $2.00. What organic matter are you going to neutralize it with?
You can go to aquarium supply stores and get a bottle for about $2.00. What organic matter are you going to neutralize it with?
I wonder, what happens if you have organic matter, h2o2, and chlorine all in the same water?