Barium- The Poison No One Talks About

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					Barium: The Poison No One Talks About Barium is just as dangerous as
arsenic, mercury and lead. It shows up regularly in public water supplies
and yet there is almost no awareness of it.

Exposure to small amounts of barium, dissolved in water, may cause a person to
experience these problems:
1. Breathing difficulties
2. Increased blood pressure
3. Heart rhythm changes
4. Stomach irritation
5. Muscle weakness
6. Alterations in nerve reflexes
7. Damage to your brain, liver, kidney and heart

When Barium is continually sprayed in the atmosphere it falls to earth and will get in water
supplies. (-- Duh! )

Barium Tests are Positive -- Clifford Carnicom

                  Barium: The Poison No One Talks About
By Richard Mesquita, AquaMD
AquaMD is the water testing division of the American Water Council, a nationally respected
provider of water education and testing services.
Have you ever heard of the metal barium? If you haven't, you're not alone. Barium just
hasn't gotten the media coverage that lead, arsenic and mercury have received in recent
years. Nevertheless, barium is just as dangerous to your health as those other metals and
shows up regularly in public water supplies.
Where Does Barium Come From?
Barium was first identified in 1774 by Carl Scheele and first extracted by Sir Humphrey
Davy of England in 1808. Since then, different forms of barium have been widely used in
the manufacture of countless products:

       Paint                   Linoleum
       Tile                    Cosmetics
       Glass                   Pharmaceuticals
       Rubber                  Spark plugs
       Textiles                Vacuum tubes
       Electronics             Fireworks
       Paper                   Fluorescent lamps
       Soap                    Rat poison


Because barium is used often in so many manufacturing operations, a lot of waste is
produced that needs to be removed from the environment. How much? In 2002, the
Environmental Protection Agency reported more than 222 million pounds of barium and
barium compounds were legally released into the air, wells, lakes, rivers and landfills.
Ten states account for about half of all legal barium released in this country:
   1. Texas (17.1 million pounds)

   2. North Dakota (15.7 million pounds)

   3. Illinois (11 million pounds)

   4. Alabama (10.2 million pounds)

   5. Michigan (10.1 million pounds)

   6. Colorado (10.1 million pounds)

   7. Minnesota (8.8 million pounds)

   8. Ohio (8.2 million pounds)

   9. Montana (7.9 million pounds)

   10.Indiana (7.8 million pounds)

And 26 additional states released anywhere from 1 -- 7 million pounds of barium apiece
into the environment. Of course, none of these statistics take into consideration the illegal,
unreported dumping of barium metals into the environment.
How Barium Poisons Our Water Supply
In light of the millions pounds of barium released into the environment each year, it was
only a matter of time until this toxic metal made it into our public water supply. Even
worse, some forms of barium dissolve very easily in water, meaning, once it enters the
water supply, it can spread quickly over great distances.
In fact, this has already occurred. Public water supplies contaminated with barium are
everywhere. The magnitude of the problem grows worse with each passing day.
Looking at lab tests conducted on public water supplies that crossed my desk over a week's
time, I found the vast majority showed some level of barium contamination. Some of the
lab tests I reviewed were conducted on water from six states: Virginia, New York,
California, Texas, Massachusetts and Oregon.
Again, these were only lab results that crossed my desk in one week. But that also
illustrates how widespread the problem really is.
How Barium Affects Your Health
Exposure to small amounts of barium, dissolved in water, may cause a person to
experience these problems:
   1. Breathing difficulties

   2. Increased blood pressure

   3. Heart rhythm changes

   4. Stomach irritation
   5. Muscle weakness

   6. Alterations in nerve reflexes

   7. Damage to your brain, liver, kidney and heart

To date, barium has not been shown to cause cancer and has not been linked to infertility
or birth defects. Not yet, anyway...
I urge you to find out if barium and other harmful contaminants are in your water supply.
If they are, for the sake of you and your family's health, you may want to consider a water
purification system that treats those specific problems. Please be aware, however, no
single system treats every problem.
Then, see your health practitioner about removing the contaminants that may have
accumulated in your body.
Dr. Mercola's Comment:
Please don't fool yourself into thinking that you can tell your water is safe by the way it
looks, tastes, or smells.
Some contaminants in water are so harmful that they are measured in "parts per million"
or "parts per billion." In other words, just a drop of these poisons added to gallons and
gallons of water can be very harmful.
Just installing a filter to purify your drinking water may not be enough. You could still be
exposed to contaminated water when you:
   1. Shower or bathe

   2. Wash your hands

   3. Wash laundry

   4. Rinse fruits and vegetables

   5. Wash dishes, glasses, and other utensils


                    BARIUM TESTS ARE POSITIVE
                                       Clifford E Carnicom
                                      Santa Fe, New Mexico
                                           May 24 2004

A series of qualitative chemical tests and deductions now confirm without doubt the
presence of significant amounts of barium within atmospheric samples. Citizens may now
begin the process of collecting the sample materials for formal submission to public
environmental agencies and private labs for identification. The testing process can be done
at modest expense and the results from laboratory analysis can now be qualitatively and
independently verified without great difficulty. Any testing service employed will need to
be able to demonstrate no vested interest in the outcome of the results, accuracy of method,
and the willingness to have the testing process independently monitored.

The material under analysis has been collected by a plate ionizing filter; it may also be
collected with conventional fiber filtration over a longer period of time. HEPA filter
collection and subsequent electrolysis of the filter material placed in distilled water has also
proven successful. Extended time periods may be required to collect a sufficient volume of
material for electrolytic processing and external testing preferences. Readers are referred
to previous articles1,2 for two methods of collection. The use of electrolysis is significant in
producing a final compound for testing purposes. The solid materials (powder/ crystals)
collected by the plate ionizing filter, assuming they satisify the test procedures described on
this page, will be sufficient for laboratory analysis. Qualitative chemical tests and flame
tests positively establish the significant presence of barium compounds within the
atmospheric sample.

Citizens with sufficient environmental concern are encouraged to begin this process of
sample collection and identification, along with the documentation of the responses of both
public and private environmental services.

Additional Notes:

The process of collection and analysis is summarized as follows:

1. Solid materials are collected with the use of a plate ionizing filter or fiber based filters as
described previously.1,2

2. The material can be subjected to low power microscopic viewing to verify similiarity of
material form before proceeding. The powder/crystal material under collection has a tan,
beige or gray cast to it. The presence of fibrous materials within the sample is not the focus
of this report, and further analysis of those materials may occur at a later time.

3. The solid powder/crystal material that is the subject of this report will be found to
dissolve easily within distilled water. Extremely small samples have been used for all tests
as the material requires time and effort to collect in sufficient quantity. For testing
purposes, samples of a fraction of a gram have been dissolved within a few milliliters of
distilled water.

4. Solutions of higher concentrations, e.g., 1 part solid to 3 parts water will be found to be
strongly alkaline. This indicates the presence of a base and hydroxide ions. A pH value of 9
was recorded in the test that is the subject of this report.

5. A weak solution (fraction of a gram to 40ml water) will be found to permit significant
electrolysis reactions. A variety of electrodes have been used to verify the chemical results,
including aluminum, iron, copper, silver and graphite electrodes. The work at this point
establishes the presence of a soluble metallic hydroxide form in solution.

6. Chromatography experiments and comparative analysis allows us to conclude that the
atomic mass of the metallic cation under examination is greater than that of copper, or
greater than 63.5 atomic mass units.3 Cations under reasonable consideration4 therefore

Ag+, Au+2, Ba+2, Bi+3, Cd+2, Ce+4, Cs+, Ga+3, Hg+2, Pb+2, Rb+, Sb+3, Sn+2, Sr+2

7. The results of electrolysis with graphite electrodes permits us to conclude that a reactive
metal is a component5 of the metallic hydroxide under examination.

8. The electrochemical series and the half-reaction electrode potentials are therefore
consulted6,7 to establish a list of reasonable candidates for the cation of the metallic salt
which disassociates in solution to permit electrolysis. The list of candidate cations, with the
condition of hydroxide formation included, is now reduced to:

Ba+2, Sr+2, Rb+ and Cs+ with oxidation potentials of 2.91, 2.90, 2.98 and 3.03 volts

It is noticed that this group is now closely confined within the periodic table, and that
chemical properties of these elements are in many ways shared. It is also instructive to note
the remarkable similiarity in the work functions of these elements, which is an expression
of the ionization capabililty of the element.

9. Each of these cations must form a soluble hydroxide. Solubility tables8 indicate that these
conditions are satisified by each of the hydroxide forms: Ba(OH)2, Sr(OH)2, RbOH and

10. Practical levels of worldwide production of the elements are helpful to consider9.
Barium and strontium both are produced at high tonnage levels worldwide, rubidium and
cesium are inconsequential in production. Barium production is stated at 6 million tons per
year, strontium at 137,000 tons, cesium at 20 tons and rubidium in such low levels as to not
be available. Common hydroxide forms are also to be considered in this analysis. This
reduces the candidate cation list to strontium and barium, whereupon additional
conditions of qualitative testing are to be imposed.

11. The material in solution must produce a cation and a hydroxide ion in solution.
Precipitate tests are conducted with carbonate, oxalate and sulfate compounds for the
existence of barium or strontium ions, using a combination of the unknown with sodium
carbonate, sodium oxalate and copper sulfate10. The material in question forms a
precipitate under all three conditions. The consideration of barium hydroxide and
strontium hydroxide continues to be valid under under these results.
12. The precipitate formed with the use of copper sulfate is hypothesized to be barium
sulfate. The precipitate formed under electrolysis is also hypothesized to be a barium
sulphate compound. Solubility tests are necessary to test this hypothesis. The precipitate
and the compound formed from electrolysis pass the solubility tests when subjected to
water, hydrochloric acid, sulfuric acid and ethanol. The identification of barium sulphate
remains valid. The sulfate precipitate fails the solubility test for strontium sulfate, as
strontium sulfate is soluble in hydrochloric acid. The sulphate compound that has been
formed by both displacement and electrolysis is highly insoluble, and is insoluble in
hydrochloric acid.

13. The solubility test for barium carbonate should also be verified. The carbonate
precipitate is soluble in hydrochloric acid and passes this test. The identification of barium
compounds in the analysis remains valid. No solubility tests for barium oxalate are

14. The next test which is to be conducted is the flame test. Barium burns yellow-green
under the flame test12,13. A sample of the electrolysis compound, identified as barium
sulphate, is subjected to a flame test using a nichrome wire. The compound is observed to
burn with a yellow-green color. The identification of barium compounds within the
analysis is valid under all conditions and circumstances examined.

15. The final test is a viewing of the spectrum of the flame test with a calibrated
spectroscope and an optical spectroscope. Dominant green and yellow emission spectral
lines are measured at approximately 515 (wider line, boundary line) and 587 nanometers
(narrow and distinct), they are confirmed with the optical spectroscope, and they
correspond to the green and yellow wavelengths specified for the flame test. A secondary
wide line in the green portion of the spectrum borders at approximately 560nm. For
comparison purposes, the spectrum of barium chloride and barium hydroxide test salts in
solution appears and measures identically within the green portion of the spectrum. The
identification of barium compounds within the analysis remains valid under all conditions
and examined and tests conducted.

The most reasonable hypothesis at this point is that the original compound is a barium
oxide form. This compound readily combines with water to form barium hydroxide. The
ionizing plate filter and the fiber filter both appear to be successful at accumulating the
solid form of this metallic salt. Solubility, pH, precipitation, chromatography, electrode,
electrolysis, flame, spectroscopy and spectroscopy comparison tests all support the
conclusion within this report that significant levels of barium compounds have been
verified to exist and are now to be examined in the atmospheric sampling process. This
report corroborates, at an elevated level, the previous research that is available on this site.

This page is subject to revision.

1. Clifford E Carnicom, Electrolysis and Barium, (,
May 27, 2002
2. Carnicom, Sub-Micron Particulates Isolated, (,
Apr 26, 2004
3. Frank Eshelman, Ph.D., MicroChem Manual (Frank Eschelman,, 2003), 1-4, 76.
4. Gordon J. Coleman, The Addison-Wesley Science Handbook (Addison-Wesley, 1997), 130.
5. Andrew Hunt, A-Z Chemistry, (McGraw-Hill, 2003), 125.
6. David R. Lide, CRC Handbook of Chemistry and Physics, (CRC Press, 2001), 8-21 to 8-31.
7. Fred C. Hess, Chemistry Made Simple, (Doubleday, 1984), 89, 91.
8. Lide, 4-37 to 4-96.
9. John Emsley, The Elements, (Clarendon Press, 1998), 30-31, 46-47, 176-177, 196-197.
10. University of Nebraska-Lincoln, The Identification of Ions,
11. Lide, 4-44.
12. Hunt, 152-153.
13. Infoplease Encyclopedia, Flame Test,

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