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Chemtrails - Lab Report On Air Grab Thru HEPA Filter[/FONT]
'This is the final Lab Report RE: air material analysis. This was a 28 day collection via HEPA filter, 8 hours per day collection. Please note the extremely high Aluminum reading 12,800,000 ppb.'
http://www.rense.com/general82/chemm.htm
Thanks stretch i value your support over this fact about chemtrails, others like scratch, juan, FUBAR ,Dexter Sinister,just like jumping in my threads and punting there asinine comments in cos they think they look smart,truth is they are too blind, dumb, or stupid to think about the facts cant they understand the implications of constant spraying would cause in what 10-15 years, who knows what medical conditions will arise.
Barium (pronounced
/ˈbɛəriəm/) is a
chemical element. It has the symbol
Ba, and
atomic number 56. Barium is a soft silvery
metallic alkaline earth metal. It is never found in nature in its pure form due to its
reactivity with
air. Its oxide is historically known as
baryta but it reacts with water and carbon dioxide and is not found as a mineral. The most common naturally occurring minerals are the very insoluble barium sulfate, BaSO4 (
barite), and barium
carbonate, BaCO3 (
witherite).
Benitoite is a rare gem containing barium.
Notable characteristics
Barium is a
metallic element that is chemically similar to
calcium but more reactive. This metal
oxidizes very easily when exposed to air and is highly
reactive with
water or
alcohol, producing
hydrogen gas. Burning in
air or
oxygen produces not just
barium oxide (BaO) but also the
peroxide. Simple compounds of this heavy element are notable for their high
specific gravity. This is true of the most common barium-bearing mineral, its
sulfate barite BaSO4, also called 'heavy spar' due to the high density (4.5 g/cm³).
Applications
Barium has some medical and many industrial uses:
- Barium compounds, and especially barite (BaSO4), are extremely important to the petroleum industry. Barite is used in drilling mud, a weighting agent in drilling new oil wells.
- Barium sulfate is used as a radiocontrast agent for X-ray imaging of the digestive system ("barium meals" and "barium enemas").
- Barium carbonate is a useful rat poison and can also be used in making bricks. Unlike the sulfate, the carbonate dissolves in stomach acid, allowing it to be poisonous.
- An alloy with nickel is used in spark plug wire.
- Barium oxide is used in a coating for the electrodes of fluorescent lamps, which facilitates the release of electrons.
- The metal is a "getter" in vacuum tubes, to remove the last traces of oxygen.
- Barium carbonate is used in glassmaking. Being a heavy element, barium increases the refractive index and luster of the glass.
- Barite is used extensively in rubber production.
- Barium nitrate and chlorate give green colors in fireworks.
- Impure barium sulfide phosphoresces after exposure to the light.
- Lithopone, a pigment that contains barium sulfate and zinc sulfide, is a permanent white that has good covering power, and does not darken in when exposed to sulfides.
- Barium peroxide can be used as a catalyst to start an aluminothermic reaction when welding rail tracks together. It can also be used in green tracer ammunition.
- Barium titanate was proposed in 2007[2] to be used in next generation battery technology for electric cars.
- Barium Fluoride is used in infrared applications.
- Barium is a key element in YBCO superconductors.
History
Barium (
Greek barys, meaning "heavy") was first identified in 1774 by
Carl Scheele and extracted in 1808 by Sir
Humphry Davy in
England. The oxide was at first called barote, by
Guyton de Morveau, which was changed by
Antoine Lavoisier to baryta, from which "barium" was derived to describe the metal.
Occurrence
Because barium quickly becomes oxidized in air, it is difficult to obtain this metal in its pure form. It is primarily found in and extracted from the
mineral barite which is crystallized barium sulfate. Because barite is so insoluble, it cannot be used directly for the preparation of other barium compounds. Instead, the ore is heated with carbon to reduce it to
barium sulfide[1]
BaSO4 +
2C →
BaS +
2CO2 The barium sulfide is then hydrolyzed or reacted with acids to form other barium compounds such as the
chloride,
nitrate, and
carbonate.
Barium is commercially produced through the
electrolysis of molten
barium chloride (BaCl2)
Isolation (* follow):
(
cathode) Ba2+* + 2
e- → Ba(
anode) Cl-* → ½Cl2 (
g) + e-
Compounds
The most important compounds are barium peroxide, barium chloride,
sulfate,
carbonate,
nitrate, and
chlorate.
Isotopes
Main article: isotopes of barium
Naturally occurring barium is a mix of seven stable
isotopes. There are twenty-two isotopes known, but most of these are highly
radioactive and have
half-lives in the several millisecond to several minute range. The only notable exceptions are 133Ba which has a half-life of 10.51 years, and 137mBa (2.55 minutes).
Precautions
All water or acid
soluble barium compounds are extremely
poisonous. At low doses, barium acts as a muscle stimulant, while higher doses affect the
nervous system, causing cardiac irregularities, tremors,
weakness,
anxiety,
dyspnea and
paralysis. This may be due to its ability to block
potassium ion channels which are critical to the proper function of the nervous system.
Barium sulfate can be taken
orally because it is highly insoluble in water, and is eliminated completely from the digestive tract. Unlike other
heavy metals, barium does not
bioaccumulate.
[2] However, inhaled dust containing barium compounds can accumulate in the lungs, causing a
benign condition called
baritosis.
Oxidation occurs very easily and, to remain pure, barium should be kept under a petroleum-based fluid (such as
kerosene) or other suitable
oxygen-free liquids that exclude air.
Barium acetate could lead to death in high doses.
Marie Robards poisoned her father with the substance in Texas in 1993. She was tried and convicted in 1996
