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So it's not getting rid of chlorine, it's just getting rid of free chlorine? Is the hydrochloric acid better to have in the water than free chlorine? Or is it e

So it's not getting rid of chlorine, it's just getting rid of free chlorine? Is the hydrochloric acid better to have in the water than free chlorine? Or is it easier to filter out?

pixl97 4y ago
What I don't know is how many PPM of free chlorine to what PH level of water you end up with, and I'm sure there's a number of factors there. But, from what I'm reading there are a number of acid resistant microbes that can survive in a low ph environment, so you have to bleach/chlorinate the systems at a regular level. https://www.avidityscience.com/media/wysiwyg/4230-MI4179_-_Drinking_Water_Acification.pdf https://www.avidityscience.com/media/wysiwyg/4230-MI4179_-_D...
gus_massa 4y ago
It does not break the Chloride atoms. Chloride can form many molecules: One "family" is NaCl (table salt) , HCl (hydrochloric acid = muriatic acid), Cl-. They can kill bacterias when they are concentrated, but they are nor so powerful when diluted enough. Another "family" is Cl2 (chloride gas), NaClO (bleach[1]), HClO , ClO-. All of them are "free chloride" because they are essentially equivalent. If you ignore the Cl2 and compare the other 3 with the ones in the other family, the difference is that they have and additional oxygen. This oxygen can go out and "burn" a part of a bacteria, and enough "burns" will kill the bacteria. I'm not sure of the details, because I know chemistry but not too much, but from https://solar2000.co.za/wp-content/uploads/2019/11/Solar2000-article-Chlorine-consumption-by-UV.pdf https://solar2000.co.za/wp-content/uploads/2019/11/Solar2000... the idea is that there is always a small amount of innocuous contamination in water, and UV can make the bleach react with it. The reaction is something-H + HOCl (bleach) -> something-Cl+ HOH (water) The "contamination" exchanges one of it's hydrogens with a chlorine in the bleach, and the bleach is transformed into water. So the chorine atoms don't disappear, but now they are in a molecules that will not cuse "burns" to the bacterias. [1] It's more complicated, but let's call this bleach to simplify.

So it's not getting rid of chlorine, it's just getting rid of free chlorine? Is the hydrochloric acid better to have in the water than free chlorine? Or is it easier to filter out?

pixl97 4y ago

What I don't know is how many PPM of free chlorine to what PH level of water you end up with, and I'm sure there's a number of factors there. But, from what I'm reading there are a number of acid resistant microbes that can survive in a low ph environment, so you have to bleach/chlorinate the systems at a regular level. https://www.avidityscience.com/media/wysiwyg/4230-MI4179_-_Drinking_Water_Acification.pdf https://www.avidityscience.com/media/wysiwyg/4230-MI4179_-_D...

gus_massa 4y ago

It does not break the Chloride atoms. Chloride can form many molecules: One "family" is NaCl (table salt) , HCl (hydrochloric acid = muriatic acid), Cl-. They can kill bacterias when they are concentrated, but they are nor so powerful when diluted enough. Another "family" is Cl2 (chloride gas), NaClO (bleach[1]), HClO , ClO-. All of them are "free chloride" because they are essentially equivalent. If you ignore the Cl2 and compare the other 3 with the ones in the other family, the difference is that they have and additional oxygen. This oxygen can go out and "burn" a part of a bacteria, and enough "burns" will kill the bacteria. I'm not sure of the details, because I know chemistry but not too much, but from https://solar2000.co.za/wp-content/uploads/2019/11/Solar2000-article-Chlorine-consumption-by-UV.pdf https://solar2000.co.za/wp-content/uploads/2019/11/Solar2000... the idea is that there is always a small amount of innocuous contamination in water, and UV can make the bleach react with it. The reaction is something-H + HOCl (bleach) -> something-Cl+ HOH (water) The "contamination" exchanges one of it's hydrogens with a chlorine in the bleach, and the bleach is transformed into water. So the chorine atoms don't disappear, but now they are in a molecules that will not cuse "burns" to the bacterias. [1] It's more complicated, but let's call this bleach to simplify.