Some more answers *EDIT

Veronica said in reply to this post
//www.curezone.org/forums/fm.asp?i=1332972#i


>>>Man, you are just intent on pushing your bad info aren't you!? Miracle-Mineral-Supplement DOES NOTTTT turn into chloride at any point once you add the citric acid OR once ingested.

You say "ClO2(chlorine dioxide) becomes ClO2-(chlorite) which then becomes Cl-(chloride)" YOU ARE UTTERLY WRONG WRONG WRONG WRONG WRONG.

Please, where did you got this information? Please show me the equation for how you got THIS LOL!!



The information is available on several sites such as those of companies using chlorine dioxide as a biocide and also in Jim Humbles book.

Here is a quote from JH's book (part 2 chapter 14)

'When a chlorine dioxide ion contacts a harmful pathogen it instantly accepts
five electrons from the pathogen, or it might be more descriptive to
say that it instantly tears off five electrons. An extremely fast
chemical reaction is in essence an explosion, and this is exactly what
happens on a microscopic level. The damage to the pathogen is a
result of losing electrons to the chlorine ion and the release of energy.
The pathogen, basically, is oxidized by chlorine ions and as a part of
the action the chlorine becomes a harmless chloride (table salt). Two
atoms of oxygen are released as ions from the chlorine dioxide ion
but the oxygen has little effect other than to attach to hydrogen ions
making water or attach to a carbon ion to make carbon dioxide.
It is the process of the chlorine dioxide ion oxidizing pathogens or
other harmful chemicals that is beneficial to the body. Although the
two oxygen ions of the chlorine dioxide ion are released, their charge
level does not result in oxidation. The same process continues
throughout the body where chlorine dioxide ions contact pathogens.'


Heres a site that explains chlorine dioxide fairly clearly and maybe similar to where Jim Humble got some of his information from

http://www.lenntech.com/water-disinfection/disinfectants-chlorine-dioxide.htm


From the site

The following comparisons show what happens when chlorine dioxide reacts. First, chlorine dioxide takes up an electron and reduces to chlorite:
ClO2 + e- > ClO2-

The chlorite ion is oxidized[should say reduced]and becomes a chloride ion:
ClO2- + 4H+ + 4e- > Cl- + 2H2O

These comparisons suggest that chlorine dioxide is reduced to chloride, and that during this reaction it accepts 5 electrons. The chlorine atom remains, until stable chloride is formed. This explains why no chlorinated substances are formed.

Also on wiki which you may like

http://en.wikipedia.org/wiki/Chlorite


You can see there a table which shows the oxidation states of chlorine
chlorite is +3 and chloride is -1, chlorine dioxide is the same oxidation state as chlorate, +5. This means chlorite accepts 4 to become chloride and chlorine dioxide accepts 1 to become chlorite. In total chlorine dioxide accepts 5 to become chloride.

Here is the wiki page on oxidation states
http://en.wikipedia.org/wiki/Oxidation_state


Down the bottom are the oxidation states of oxygen you will see that oxygen has 8 oxidation states

-2 in most oxides. e.g. ZnO, CO2, H2O
-1 in all peroxides.
-1/2 as in superoxides. e.g. KO2
-1/3 as in ozonides. e.g. RbO3
0 as in O2
+1/2 as in dioxygenyl. e.g. O2+[AsF6]-
+1 in O2F2
+2 in OF2

in chlorine dioxide it is in a -2 state as it is in chlorite
when it leaves the chlorite it forms an oxide with
an ion such as hydrogen and carbon
it cannot oxidize in this state, only as O2 is it used in cell respiration

Hope that clears things up

*EDIT

I just noticed that on the lenntech site they made a mistake which I have corrected above.
Here is an EPA(US environmental protection agency) document giving similar information

'Chlorine dioxide (ClO2) is a neutral compound of chlorine in the +IV oxidation state. It disinfects by oxidation; however, it does not chlorinate. It is a relatively small, volatile, and highly energetic molecule, and a free radical even while in dilute aqueous solutions. At high concentrations, it reacts violently with reducing agents. However, it is stable in dilute solution in a closed container in the absence of light (AWWA, 1990). Chlorine dioxide functions as a highly selective oxidant due to its unique, one-electron transfer mechanism where it is reduced to chlorite (ClO2-) (Hoehn et al., 1996).
The pKa for the chlorite ion, chlorous acid equilibrium, is extremely low at pH 1.8. This is remarkably different from the hypochlorous acid/hypochlorite base ion pair equilibrium found near neutrality, and indicates the chlorite ion will exist as the dominant species in drinking water. The oxidation reduction of some key reactions are (CRC, 1990):

ClO2(aq) + e- = ClO2-

E° = 0.954V

Other important half reactions are:

ClO2- + 2H2O +4e- = Cl- + 4OH-

E° = 0.76V

*note in this case chloride and hydroxide ions are formed. water is of course hydrogen hydroxide


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