Chlorine Dioxide precipitates iron from the blood

[Guest guest]

The conclusion I draw from this site: http://www.chlorine-dioxide.com/index.asp?option=chem

is that long term use will strip iron from the blood which is the

oxygen carrying mechanism.

This in turn will lead to the tiredness one member here testifies to.

Now, from CureZone: http://www.curezone.com/forums/fm.asp?i=1045349#i

**** EXACT QUOTE ****

Chemistry of Iron Oxidation

Chlorine dioxide and the chlorite byproduct rapidly oxidize Fe (II) to

Fe (III), which precipitates in sedimentation or is removed by

filtration. After the initial reaction by the chlorine dioxide gas per

Equation 1, the chlorite by product (above pH 6.5) continues to convert

the soluble Fe (II) to Fe (III) by the following reaction based on

Equation 2 (2):

4 Fe (II) + ClO2 + 10H2O ⇌ 4 Fe (OH)3(s) + Cl- + 8H+ [Eq. 3]

In typical applications of chlorine dioxide to water streams containing

iron, manganese, and other oxidizables, about 50-70% of the chlorine

dioxide is initially converted to chlorite while simultaneously

oxidizing some iron and manganese (Eq. 1). The chlorite formed is

capable of continuing to oxidize iron according to Equation 3 where 1

mg of soluble ferrous iron will be converted to 1 mg of ferric iron by

0.3 mg/L of chlorite.

The reactivity of chlorite and the ferrous ion is well known, as it is

common practice to use ferrous chloride or ferrous sulfate to reduce or

eliminate chlorite in drinking water treated with chlorine dioxide.

Dosage rates of 1.0 mg ferrous were demonstrated to remove 0.3 mg

chlorite at full-plant scale in El Paso Texas (7). If manganese is

available in the source water, then additional chlorine dioxide may be

needed to oxidize it from the soluble Mn+2 form to the precipitated

Mn+4 form.

Chemistry of Manganese Oxidation

As in iron oxidation, chlorine dioxide and chlorite react rapidly with

soluble manganese by oxidizing it to manganese dioxide based on the

following equation.

5Mn+2 + 2ClO2 (gas) + 6H2O ⇌ 5MnO2 + 12H+ + 2Cl- [Eq. 4]

Equation 4 indicates about 0.5 mg of chlorine dioxide is required to

oxidize 1 mg of soluble manganese to the precipitated form of manganese

dioxide, based on the complete reaction of chlorine dioxide and

chlorite to chloride. For example, a chlorine dioxide dose of 1.4 mg/L

with 1.0 mg/L chlorite residual may oxidize up to 2 mg/L of soluble

manganese to the precipitated manganese dioxide state. In the United

States, about 40% of raw water supplies exceed 0.3 mg/L iron and 0.05

mg/L manganese. Often, source waters contain both iron and manganese.

In these waters, the sum of each parameter should be determined for the

total amount of chlorine dioxide and chlorite byproduct required for

complete oxidation (1-7).

http://www.mixeddisinfectants.com/Product%20Bulletin%20-%20Fe%20Mn%20Reduction.pdf

I really don't know exactly what this means in terms of dosing and how

much mineral is lost in, for example, one drop of MMS, or for that

matter, if it is even applicable to the human body. However, it must be

determined for the further understanding of how to properly supplement

our body with iron and manganese while using MMS.

In addition, I am concerned about the iron's transformation, as it

sounds like it is converted into something unusable, which may lead to

problems of its own...

I don't want to upset anyone here but these are important

considerations if you want to supplement with MMS, also this is why I

still feel that it may be better to use MMS as a short-term detox

protocol, at least until more is known.

Hopefully, someone with knowledge on matters of chemistry can better

explain this information and make sense of it all, but until then

caution should be used.

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At this point, I conclude short term usage at heavier dosage 10 - 15

drops perhaps in two successive days is ok, then perhaps wait a week or

two and repeat, but don't use on a continuous basis.

I am neither doctor nor chemist -- Levi Philos