Does chlorine dioxide interact with flouride in drinking water?

Not Bill! I am neither an expert nor biochemical, only researched the best sources on the Internet. My major interest is to help.

I agree Iodine supplementation protects thyroid from harmful fluoride.
Fluoride was used in past to suppress thyroid.
Fluoride is Halogen just like iodine the problem is that fluoride is "stronger". Therefore when fluoride enters the body it's atom
replaces iodine's atom and impairs thyroid function.One start to have under active thyroid ( Hypothyroidism2)even when blood test doesn't show it .To test If your thyroid is under active check your body temperature in the morning after you wake up for three days,keep thermometer close to your bed so don't have to get up (important).If you are below 97F 36.1C degrees you
have Hypothyroidism.I did the test my self and my temp was 35C !It can be corrected with careful iodine supplementation .
Lugols Solution is what I used which is Potassium iodide .LUGOL'S SOLUTION should be in every medicine cabinet.

some of the symptoms:

excessive sweating (at night too)
Fatigue
Sluggishness
Increased sensitivity to cold
Constipation
Pale, dry skin
A puffy face
Hoarse voice
An elevated blood cholesterol level
Unexplained weight gain
Muscle aches, tenderness and stiffness
Pain, stiffness or swelling in your joints
Muscle weakness
Heavier than normal menstrual periods
Brittle fingernails and hair
Depression
More info:
Dr Mark Starr,Dr Jerry Tennant--Guests on Coast to Coast I learned a lot from Them!
www.stopthethyroidmadness.com/
tennantinstitute.com/TIIM_MAC/Welcome.html
doctorapsley.com/

Does chlorine dioxide oxidize fluoride?

I was just thinking of a guess in terms of electronegativity. Since F has small radius and high electronegativity and Cl and O share with probably about the same electron affinity (as well as electronegativity, I haven't even looked it up), that there is no way Cl and O would lose electrons to an ion of F. I think my guess is supported by your correct use of oxidation potentials. But really I wonder if I should be using electronegativity and affinity.

Chlorine dioxide will not oxidize fluoride. The oxidizing and reducing powers of chemicals are given by their oxidation or reduction potentials. The oxidation of fluoride to fluorine requires an oxidizing agent with potential greater than +2.87 volts. Chlorine dioxide, however, only exhibits an oxidizing potential of +0.95 volts.

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Just speaking off the top of my head - so forgive the simplicity - but if I recall correctly fluoride is used in pharmaceuticals so often because it is "sticky". Devastating and sticky. Great combo.
You can deliver a drug into the system and fluoride will basically glue it in place. It doesn't sound as though there is any way chlorine dioxide can get rid of fluoride - might even form a new compound with it according to what alfernandes just posted. That puts us back at square one - having to physically separate fluoride from water.

Until there is found to be a way to get rid of fluoride IN the water without that process of physical separation, it looks like it must be dealt with in other ways. Monmorillonite, tamarind, and boron can remove it from the body, and then the challenge becomes not allowing it back in.
I know there's a lot of discussion about distilled vs. RO water - I'm leaning toward adding minerals to distilled. I've even pondered simply dropping plain old mineral supplements right into the water, shaking it up, capping off the container, leaving it to dissolve, and calling it a day.

MWeather Excuse me most is not that we are commenting. We're talking about the interaction of Chlorine Dioxide with Fluoride (fluorine).This chemical process interferes with Chlorine Dioxide generating Chloryl Fluoride (CLO2F) understands.

To Bill about the interaction between Chroline dioxide with fluoride


Chlorine Dioxide may readily be converted into Chloryl Fluoride (ClO2F), by elementary fluorine or other fluorinating agents.

Chloryl Fluoride (CLO2F)

Chloryl Fluoride was first obtained in 1942 by Schmitz and Schumacher, by fluorinating Chlorine Dioxide with elementary fluorine. This method is, however, troublesome because of the extraordinary violence of the reaction and, as a result, no further investigation on CLO2F on appeared for 10 years. In recent years the formation of the CLO2F has been studied by several workers. Three routes are available, namely fluorination of KCLO3, CLO2, CL2O6 with elementary fluorine or other fluorinating agents.

Preparation and formation of CLO2F

a. Fluorination of KCLO3. The action of elementary fluorine on KCLO3 represents a method for the formation of the Chloryl Fluoride rather than one for its preparation since it is formed only in small amounts and the main product is perchloryl fluoride. These reactions are carried out between - 40° and + 30°C. Formation of CLO2F is thought to arise from the combination of fluorine witn CLO2 produced by decomposition of the CLO3- anion, and is thus directly related to the formation from CLO2 and fluorine. The course of the reaction when fluorine acts on potassium chlorate is discussed more fully when perchloryl fluoride is considered. Fluorination of KCLO3 may also be effected with other agents and the yields of CLO2F are than better. Thus interaction with CLF3 or BrF3 leads almost exclusively to CLO2F because of the higher reaction temperature needed.

12KCLO3 + 20 BrF3 → 12KBrF4 + 4Br2 + 6O2 + 12CLO2F.

Fluorsulfonic acid may also be used. It may be thought of as HF-SO3, the HF being the actual fluorinating agent, while SO3 serves to combine with water liberated in the reaction. This method gives a 30% yield of CLO2F based on the KCLO3 used, in addition to Chlorine, Chlorine dioxide and oxigen.

b. Fluorination of CLO2. Chlorine dioxide combines directly with fluorine to form CLO2F. As already mentioned chloryl fluoride was first obtained in this way. When the reactants are brought together at room temperature only spontaneous decomposition of CLO2 into chlorine and oxigen is observed. Formation of CLO2F takes place only if the reactants are brought together at suitable partial pressures which are exactly maintained, or if, after condensing them together, they are warmed slowly from - 78°C to + 20°C. Reaction is homogeneous and bimolecular; at low CLO2 concentrations and low pressures the rate controlling step is

CLO2 + F2 → CLO2F + F.

This is followed by the wall reaction 2F - F2. This reaction was developed later by Schumacher into a preparative method. Large quantities of CLO2F may be prepared by leading fluorine into liquid CLO2 at -50°C.
Chloryl fluoride may also be prepared on a larger scale when fluorine is passed into solutions of CLO2 in indifferent solvents; this eliminates the necessity for working with large quantities of condensed CLO2. While in the case of carbon tetrachloride the relatively high crystallization temperature of the solvents limits the working temperature to a minimum of -20°C, at which only low concentrations are possible, it is feasible with CFCL3 at -78°C to reach 3 millimole of CLO2F per ml of solution. Such solutions are execellent for use in studying further reactions of chloryl fluoride. By cooling such solutions to -110°C, CLO2F may be separated and obtained pure after distillation.
The simplest method for preparing chloryl fluoride is certainly to use AgF2 as fluorinating agent. When a slow stream of CLO2 is passed at room temperature through a tube filled with argentic fluoride, quantitative reaction occurs and quite colorless chloryl fluoride may be condensed out in a
trap cooled to -78°C.

AgF2 + CLO2 → AgF + CLO2F.

Consumption of argentic fluoride may readily be followed by observing the movement of boundary between AgF2 (brown) and AgF (yellow), and in this way excess of CLO2 can be avoided. Cobalt trifluoride acts in the same way as AgF2. Chloryl fluoride is also produced when gaseous Chlorine dioxide is passed through liquid BrF3 at +30°C.

6CLO2 + 2BrF3 → 6CLO2F + Br2.

To back up what Bill is getting at...

Citizens groups frequently target fluoride, which is added to the water supply of most municipalities to help cut down on tooth decay in children, as a possible carcinogen. The Journal of Epidemiology, in 2001, linked fluoride as the genetic cause of cancer. A 1990 National Toxicology Program study determined fluoride could be the cause of cancers affecting the mouth, pharynx, colon and rectum. Another study, with results published in the Journal of Environmental Pathology, Toxicology and Oncology in 2001, linked osteosarcoma, a rare bone cancer, with fluoride.

www.freedrinkingwater.com/water-education/medical-water-cancer.htm

alfernandes wrote: To Bill about the interaction between Chroline dioxide with fluoride


Chlorine Dioxide may readily be converted into Chloryl Fluoride (ClO2F), by elementary fluorine or other fluorinating agents.

Chloryl Fluoride (CLO2F)

Chloryl Fluoride was first obtained in 1942 by Schmitz and Schumacher, by fluorinating Chlorine Dioxide with elementary fluorine. This method is, however, troublesome because of the extraordinary violence of the reaction and, as a result, no further investigation on CLO2F on appeared for 10 years. In recent years the formation of the CLO2F has been studied by several workers. Three routes are available, namely fluorination of KCLO3, CLO2, CL2O6 with elementary fluorine or other fluorinating agents.

Preparation and formation of CLO2F

a. Fluorination of KCLO3. The action of elementary fluorine on KCLO3 represents a method for the formation of the Chloryl Fluoride rather than one for its preparation since it is formed only in small amounts and the main product is perchloryl fluoride. These reactions are carried out between - 40° and + 30°C. Formation of CLO2F is thought to arise from the combination of fluorine witn CLO2 produced by decomposition of the CLO3- anion, and is thus directly related to the formation from CLO2 and fluorine. The course of the reaction when fluorine acts on potassium chlorate is discussed more fully when perchloryl fluoride is considered. Fluorination of KCLO3 may also be effected with other agents and the yields of CLO2F are than better. Thus interaction with CLF3 or BrF3 leads almost exclusively to CLO2F because of the higher reaction temperature needed.

12KCLO3 + 20 BrF3 → 12KBrF4 + 4Br2 + 6O2 + 12CLO2F.

Fluorsulfonic acid may also be used. It may be thought of as HF-SO3, the HF being the actual fluorinating agent, while SO3 serves to combine with water liberated in the reaction. This method gives a 30% yield of CLO2F based on the KCLO3 used, in addition to Chlorine, Chlorine dioxide and oxigen.

b. Fluorination of CLO2. Chlorine dioxide combines directly with fluorine to form CLO2F. As already mentioned chloryl fluoride was first obtained in this way. When the reactants are brought together at room temperature only spontaneous decomposition of CLO2 into chlorine and oxigen is observed. Formation of CLO2F takes place only if the reactants are brought together at suitable partial pressures which are exactly maintained, or if, after condensing them together, they are warmed slowly from - 78°C to + 20°C. Reaction is homogeneous and bimolecular; at low CLO2 concentrations and low pressures the rate controlling step is

CLO2 + F2 → CLO2F + F.

This is followed by the wall reaction 2F - F2. This reaction was developed later by Schumacher into a preparative method. Large quantities of CLO2F may be prepared by leading fluorine into liquid CLO2 at -50°C.
Chloryl fluoride may also be prepared on a larger scale when fluorine is passed into solutions of CLO2 in indifferent solvents; this eliminates the necessity for working with large quantities of condensed CLO2. While in the case of carbon tetrachloride the relatively high crystallization temperature of the solvents limits the working temperature to a minimum of -20°C, at which only low concentrations are possible, it is feasible with CFCL3 at -78°C to reach 3 millimole of CLO2F per ml of solution. Such solutions are execellent for use in studying further reactions of chloryl fluoride. By cooling such solutions to -110°C, CLO2F may be separated and obtained pure after distillation.
The simplest method for preparing chloryl fluoride is certainly to use AgF2 as fluorinating agent. When a slow stream of CLO2 is passed at room temperature through a tube filled with argentic fluoride, quantitative reaction occurs and quite colorless chloryl fluoride may be condensed out in a
trap cooled to -78°C.

AgF2 + CLO2 → AgF + CLO2F.

Consumption of argentic fluoride may readily be followed by observing the movement of boundary between AgF2 (brown) and AgF (yellow), and in this way excess of CLO2 can be avoided. Cobalt trifluoride acts in the same way as AgF2. Chloryl fluoride is also produced when gaseous Chlorine dioxide is passed through liquid BrF3 at +30°C.

6CLO2 + 2BrF3 → 6CLO2F + Br2.

I see now that there is a reaction but excuse my ignorance -- Is this a dangerous reaction to humans?
Should there be a serious warning applied to the use of chlorine dioxide that it is NOT to be mixed in any way with water that has flouride.

This is basically the purpose of my original question and that is Do we need a serious warning applied to our protocols not to mix these two chemicals together?

Your concern is noted Bill.

Here is a report with the first pages of a study done for Fort Collins, Colorado water treatment works. It shows they directly mix CLO2 and Fluorosilicic acid to gain the treatment advantages for their purpose (whatever that may be) and if this was dangerous to human health as a poisonous outcome, I am sure this practice would not be allowed.

Link: www.healthdistrict.org/fluoridereport/title.tableofcontents.intro.pdf

I am trying to see if i can find an inorganic chemical reaction indication between ClO2 and H2SiF6 to see the effects and indications. Not a chemist, but this is not a mystery also.

Personally I am glad and grateful I can avoid the fluoridation in my own drinking water....