A Case for Testing Source: Chemtrail Crimes September 3 2000
A case for the environmental testing of barium and
barium compounds now exists. This case is developed from the following
sequences of events and reasoning:
1. Meteorological study. Each of these topics will now be discussed in greater
detail.
1. Meteorological Study:
A reasonable case can be made, based upon meteorological
considerations and observations, that an aerosol particle, especially
of a salt nature, is regularly being introduced into the atmosphere as
a direct result of the unidentified aircraft operations under
consideration. The premise for this case begins with the
meteorological studies of relative humidity at flight altitude begun
in August of 1999 in Santa Fe, NM and continuing through the middle of
the current year. These studies show the repeated and regular
appearance of
cirrus, cirro-stratus and cirro-cumulus cloud deck formations as a
direct result of aircraft operations under conditions of
extremely low relative humidity (avg. 30%). Historic
meteorological observations coupled with reliable sources
demonstrate that such cloud formations are not to be expected,
except under the most unusual of conditions, unless the relative
humidity (with respect to water, per convention and standard
measurement) is greater than 70%. This contradiction is of the
greatest significance, and the rapid, recent and extreme
variation in environmental conditions and activity must be both
explained and accounted for. Observations, on a continuous and
sustained basis since the beginning of 1999, show aircraft as
the source of the materials, having been clearly photographed,
observed, and documented leaving persistent and continuous trails
of an unidentified substance which transforms itself into the "cloud"
formations under the stated conditions of extreme low relative
humidity. The reliable sources referred to include Vincent Schaefer,
inventor of cloud seeding in 1946, the United States Naval
Postgraduate School in Monterey, CA, the contemporary textbook
"Meteorology", by Joseph M. Moran, and a
recent study by both NOAA and NASA. Please refer to the relative
humidity studies elsewhere on this site for further information on
this topic.
In seeking an explanation for this variation, it is
helpful to begin the consideration with the "unusual case" of cloud
formation at relative humidity levels as low as 70%. It is
stated by Schaefer and others that the most likely occurrence of
such cloud formations is best exemplified along the coastline,
where microscopic salt particles, or cloud nuclei, frequently
exist. Such water-seeking nuclei are referred to as hygroscopic.
Therefore, it is observed that the introduction of hygroscopic nuclei
can alter the process of cloud formation to some degree, although it
is seldom to never expected to be effective under relative humidity
levels less than 70%. Most cloud formation, of any type, is the result
of nuclei processes.
Next, it is beneficial to consider the models for cloud
formation, especially cirrus cloud formation, to identify the most
prominent variables that should be considered. Once such
model is presented by Paul J. Demott, at the Department of
Atmospheric Science at Colorado State University. This model
deals specifically with laboratory studies of cirrus cloud
processes. Although any laboratory model is by necessity a
simplification of nature, it remains useful. The primary
variables of the model are temperature, relative humidity, and
aerosol size. Special attention should be given to this last
variable mentioned.
Analysis of this model also results in an important
conclusion: The smaller the size of the nuclei in the atmosphere , the
greater the rate of cirrus cloud formation.
The objective at this stage of the analysis is to
identify what process can be responsible for altering the tenets of
conventional meteorology, and what will provide for repeated cloud
formations under conditions of extremely low relative humidity. The
suggestions given as a result of the above analysis are twofold:
First, it is expected and anticipated that the material in question
delivered from the aircraft is likely of a salt nature, and second,
that it is of an extremely small size.
It is also observed that precipitation seldom
accompanies the cirrus cloud formations that result from the aircraft
delivery, and yet it is a fact that the "clouds" do form. Therefore,
the expectation at this stage is that we are seeking a salt material,
presumed to be extremely small (.e.g., micron, or sub-micron level
quite possible), and that it possesses strong dessicating, or drying,
properties. This latter quality would explain the apparent
contradiction between the frequent appearance of "clouds" and the
associated drought that we find the country to be currently
undergoing. In short, the
introduction of massive amounts of hygroscopic aerosols is
suspected as being one of the major constituents of this program.
2. An anonymous source of information stated to be
reliable:
Information has been offered to the public by an
anonymous source in the earlier portion of the year 2000. This source
is simply stated to be reliable to the highest order, and it is stated
that the identity of the source must be protected. This source states
that the material being delivered by aircraft is composed of barium
salts, and that it is being used in
connection with advanced radar studies. No further information
on this aspect of the research is available at this time.
3. Chemistry analysis:
If we postulate that the source of information
referenced above is indeed reliable, it is worthwhile to investigate
the implications of combining the information that has been presented.
It is at least noteworthy to recognize that two independent sources
each make the case of a salt material being used.
The next stage of this analysis requires an
investigation into barium and barium compounds. I am not a chemist by
profession, but the following information has been acquired:
Barium occurs naturally in two primary forms, barium
carbonate (BaCo3) and barium sulfate (BaSO4). The material is mined
from the earth in these forms. Barium carbonate is commonly known as
witherite, and significant deposits occur in both the United States
and China. There are many other compounds of barium that can be
developed chemically, but this analysis will start with the simplest
case of that which can be mined in abundance and economically from the
earth. Of these two forms of naturally occurring barium, greater
attention has been devoted to barium carbonate for the following
reasons:
1. If barium carbonate is subjected to significant heat,
the combustion process results in the production of barium oxide and
carbon dioxide. It should be mentioned that in all attempts to
determine the actual source of emissions from the aircraft, even under
telephoto conditions, the engines have never been eliminated from
consideration and remain suspect. The fact that other delivery
mechanisms have been observed and recorded does nothing to interfere
with this claim.
2. Barium oxide is a whitish powder.
3. Barium oxide absorbs water, and is used as a
dessicant for that reason.
4. Barium oxide induces respiratory distress, especially
bronchitis.
5. Barium sulfate does not possess these same
properties, and is consequently of less interest at this time.
The first of 5 chemical reactions will therefore be
presented. As I do not make any claim to being a chemist, any errors
found quantitatively or in basic concept to these reactions will be
appreciated.
BaCO3 ->(heat)-> BaO + CO2
The interesting properties of barium oxide (BaO) have
been mentioned. They are especially interesting because they begin to
satisfy the circumstances of meteorological observations and science,
feasible methods of delivery, economics, and formation, consistent
chemical attributes, correlation with observed patterns of dehydration
in the atmosphere, conformal in appearance, and satisfies at least in
part the observed and reported health affects upon the population.
It is not adequate to stop the investigation at this
point. It is now necessary to devote more attention to the chemistry
of barium oxide, and to learn what is expected if it were released
into or formed within the atmosphere. I offer the following chemical
equations as original work, which will be helpful to confirm or refute
by anyone with further knowledge on this subject:
Barium oxide combines with water very aggressively. I
have the reaction as:
BaO + 9H2O -> Ba(OH)2 * 8H2O
The resulting compound from this reaction is termed
barium hydrate, or barium hydroxide, octahydate. Barium hydrate exists
as a whitish powder or crystal form.
This reaction explains why barium oxide is used
commercially as a dessicating, or drying agent. It would therefore be
expected to extract the moisture out of the air. If produced at a suff
iciently small size, this reaction goes a long way to explain the
observed alterations in cloud formation under
conditions of extremely low relative humidity. It would also be
consistent with the laboratory model for cirrus cloud formation
mentioned earlier, as well as with the anonymous declaration of
barium salts. Barium oxide is indeed considered to be a salt,
and it possesses a relatively high degree of solubility.
4. pH testing of rainwaters:
If we accept the previous set of events to be from a
reasonable scenario, it is worthwhile to further attempt to validate
the ideas. One such method that can be used to assist in the process
is the pH testing of rainwaters, i.e., the testing for acidity and
alkalinity. This method is suggested because of the presence of the
hydroxides in the reaction above, which indicates an expected
alkalinity that presumably would affect the rainwaters.
Rainwater samples have been collected on 5 different
occasions in the southern Santa Fe, NM area, and they have been tested
for pH. It should be mentioned that collectable rainwater in the
location mentioned has been an extremely rare event since before
October of 1999 to the present day. Extreme drought is now
characteristic of this location, and the city of Santa Fe itself is
under the next to highest level of water restrictions that can be
imposed under law. As such, collection and ph testing of rainwater by
interested readers is both welcomed and encouraged. This can be
accomplished relatively easily and inexpensively with pH test kits
available at aquarium or pet stores.
The results of this testing are as follows:
June 26 : 6.6 The average of these tests is 6.46, with a sample
standard deviation of 0.19. The pH scale ranges from 1 to 14, with 1
being extremely acidic and 14 being extremely alkaline.
Distilled water has a pH of 7.0.
The results show that the rainwater samples above are
slightly acidic. These results have caused me some surprise, as my
expectation was that the rainwater should test on the alkaline side of
the scale because of the presence of the hydroxides if the original
hypothesis involving barium carbonate is correct.
At this point, the question was approached in a more
open manner, and the question was rephrased in the following form:
What is the pH of rainwater EXPECTED to be?
The inquiry has resulted in some level of surprise. Two
sources have been located in the research on this question thus far,
one of them being a professor at the University of Hawaii. A question
was posed to the professor in almost exactly the same form that it
arose within my work, and this was: Why is the rainwater at a low pH,
such as 5.5 to 6.5, when the rivers and lakewaters are showing a pH at
or greater than 7.0, i.e, acidic rainwaters and alkaline groundwaters?
The answer was given that it is actually normal for rainwater to have
a pH of between 5.6 and 5.8. In other words, an acidic quality to
rainwater at this level is expected. This was stated to occur because
of the combination of rainwater with carbon dioxide in the atmosphere,
forming carbonic acid through a perfectly normal and natural process.
Both sources found stated the pH of rainwater is expected to be at
this level, i.e, 5.6-5.8. Acid rain was stated to be in the class when
the pH is less than 5.0. The conclusion from this investigation,
albeit a surprise to myself, is that rainwater is naturally somewhat
acidic.
Considering the results obtained from local rainwater
samples with a pH of 6.5, the new information above now casts a
different and more congruent interpretation. The rainwater tested
locally does show a result which is relatively more alkaline than the
expected values, if the two sources are
presumed to be correct. An explanation for the relatively more
alkaline nature is best explained with the presence of
hydroxides (OH) as supposed in the original hypothesis which led
to the test in the first place.
The results at this stage, therefore, continue to be
consistent, albeit in a surprising manner with respect to pH testing.
This is one reason that it will be helpful for other readers to
investigate the local pH testing of rainwaters across the country, and
to continue to verify the baseline acidic nature
which has been stated by the two sources.
5. Physical sample collected in association with
aircraft activity:
Another stage of testing of the barium carbonate -
barium oxide - barium hydrate hypothesis offered will involve the
collection of physical samples if and when they are available. Reports
of a whitish powder have occurred intermittently throughout the last
two years in association with the aircraft activity, and have been
reported on the message forum. With a single exception, samples of
material of this nature have not been received by myself.
One sample has been received in August of 2000 which
satisfies the criteria of being a whitish powder. It was collected in
Denver CO on the surface of an automobile after aircraft were observed
emitting continuous trails which subsequently developed into the
common cloud decks. The amount of material collected was incredibly
minute, and exists as a whitish powder or dust. The amount of material
available raised the question as to whether or not microscopic
examination was even possible.
6. Testing of chemical hypothesis:
A microscopic chemical test of the sample referred to
above has been conducted. This test was quite difficult to perform
because of the extremely limited amount of material available, and the
results remain in need of substantiation or refutation.
If indeed there is the unusual presence of a barium
compound in our atmosphere, particularly barium hydrate, it would be
valuable to have a chemical test to help define it's existence. The
following chemical reactions are offered (again, if errors are found,
please notify me):
Ba(OH)2*8H2O + 2 HCL -> BaCl2 + H2(gas) + 9H2O
Ba(OH)2*8H2O + H2SO4 -> BaSO4 + H2(gas) + 9H2O
My research indicates that barium hydrate, if combined
with hydrochloric acid, will form barium chloride, which in turn is
highly soluble in water. Barium hydrate, if combined with sulfuric
acid, will precipitate barium sulfate, a generally insoluble crystal.
These results are expressed with the two equations above.
Such a test has been conducted with the powdered sample
received. The results would be less ambiguous if more materials were
available for testing, but as it was, the amount available for each
test resided on the sharp end of a needle.
Three trials were performed. Observations in all cases
were out of necessity completed under the microscope due to the
extreme scarcity of the material being analyzed. In each trial, the
whitish powder immediately dissolved in the hydrochloric acid as
hypothesized. In each trial, the whitish powder subjected to sulfuric
acid did result in crystal formations. These crystals were
photographed under the microscope and will be presented on the web
page of this article. The amount of material available for testing was
a critical factor, and the need remains to continue this testing as
the occasion permits. The results of these tests appear to be
consistent with the original hypothesis that is presented, i.e. barium
salts or compounds may now have an unusual presence in our environment
as a result of aircraft aerosol operations.
Original White Powder Sample 480x
White powder subjected to sulfuric acid 480x Crystal
formations apparent
White powder subjected to sulfuric acid 480x
Crystal formations apparent
White powder subjected to hydrochloric acid 480x
Dissolves immediately, air bubbles remain.
7. Solubility and equilibrium considerations
There are additional relevant properties of barium
compounds, and the earth alkali elements, of which barium is a member.
The capacity of barium oxide and barium hydroxide to absorb water
appears to be rather striking. Consulting a table of solubility of
salts in water, barium oxide is listed most definitely as a soluble
salt. Furthermore, when ranked with 60 other salt forms by the
solubility constant, barium oxide ranks as number one and as the most
soluble within those listed. The solubility constant for barium oxide
is stated as .0614; this number outranks the other listings in the
table by a factor of hundreds to thousands to multiples of thousands.
In addition, an intriguing reference has been found that
describes the ability of certain salt forms to absorb water under
varying conditions of relative humidity. Although the
specific case of barium hydrate has not been identified as of
yet, there does appear to be the case of certain salts absorbing
moisture under relative humidity conditions as low as 30%. The
specific case referred to identifies a hydrate form of strontium
chloride at 0deg C. This salt form under these conditions will
absorb moisture under relative humidity conditions of 27%. In
addition, strontium is within the same elemental group as
barium, the earth alkali series. These findings further substantiate
the consideration of barium salts being used in a
dessicating aerosol form, supporting the observations of "cloud"
formation under conditions of extreme low humidity. Attempts
will be made in the future to specifically define the moisture
absorption capacities of barium salt forms with respect to relative
humidity, but the above example demonstrates the feasibility of
atmospheric modifications as have been observed.
[The following information is predictive in nature, and
is not intended for the casual reader. It attempts to predict the
equilibrium constant of the hydrate reaction involved:
If the salt form in question does indeed absorb moisture
at relative humidities of 30% or greater at temperatures of -50deg C.
(flight altitude), then the pressure of the water vapor within the
hydrate form should equal approximately .0143torr. This is based upon
the following:
Pressure of water vapor at -50deg C. is .0477torr (1mb =
.750062torr) Therefore:
P(H2O) / .0477torr = .30 If the hydrate form is indeed barium hydrate
[Ba(OH)2*8H2O]: Kp (equilibrium constant in atmospheres) =
(1.882E-5)^8 = 1.57E-38 atm. at -50deg C.
An important question to now answer is: What is the
equilibrium constant, in atmospheres, of the barium hydrate equation
that has been hypothesized within this discussion? If reasonable
agreement from the actual equilibrium barium hydate chemical reaction
with the above calculation is found, then an adequate explanation for
the observations recorded has been found. Any assistance from those
knowledgeable in the determination of this constant for the reaction
specified is appreciated.]
8. Environmental testing : water, soil, air:
A logical case has been developed within this article to
substantiate the need for environmental testing of barium or barium
compounds in our water, air and soil. This case does not exclude
considerations given to additional tests for different compounds or
materials in the future. This case does not eliminate the need to
evaluate other forms of physical material associated with aircraft
operations, such as the sub-micron fibers or gel samples received and
reported. This case does not exclude the need for further
identification of certain
biological components identified within the fibrous materials
mentioned previously.
This case does establish a reasonable requirement and
need to test for barium or barium compounds within our environment
based upon a logical set of events, reasoning, and tests. Barium is
subject to rather stringent environmental restrictions on the amount
permitted in the water supply, e.g.., 2ppm. This case is dependent
upon considerations arising from the science of meteorology,
information sources that are consistent with observation reports,
physics, pH testing and chemistry.
It is recommended that the readership pursue this
testing at a serious and professional level, and that the results be
disclosed to the public at the earliest convenience. Any errors or
revisions in this report will be made as circumstances require or
dictate.
Appreciation is extended to numerous participants on the
message forum that have both initiated and contributed signficantly to
this research topic.
Clifford E Carnicom
by Clifford E Carnicom
http://www.carnicom.com/case1.htm
2. An anonymous source of information stated to be reliable.
3. Chemistry analysis.
4. pH testing of rainwaters.
5. Physical sample collected in association with aircraft
activity.
6. Testing of chemical hypothesis.
7. Solubility and equilibrium considerations.
8. Environmental testing : water, air, soil.
June 27 : 6.6
Aug 17 : 6.2
Aug 18 : 6.3
Aug 19 : 6.6
P(H2O) = .0143 torr
P(H20) = 1.882E-5 atmospheres
Santa Fe NM
Authored at Vallecito Reservoir CO
September 3 2000
Edited September 5 2000