In article . com,
says...
I give up. My Masters degree in Physics is of no value here. My
Bachelors degree in Math is of no value here. My 20 years with the
university (retired) means nothing. Someone with an opinion (however
false) instead of facts of physical science, seems to be more able to
swing the belief of the uninformed.

I will try to explain it again.

The vacuum will hold the column of water in the tube.

Dont believe it?
Test this statement, take a simple soda straw stick in in a glass of
water put your finger over the end and lift it out. The 8" column of
water stays in the straw because of the vacuum in the top of the
straw. Now remove your finger and the water drops out. So, it
doesn't TAKE a 32' column of water, but that is the tallest column of
water that will be suspended, a simple law of physics.

Thats why a lift pump like the old rocker handle pitcher pumps have to
be replaced with either submerged or Jet pumps in deeper wells. A
lesser column WILL work however. At the top is a vacuum. If its 32
feet, thats the greatest vacuum you can create. There is salt water
on one side and fresh water on the other. The salt water will boil
earlier because of the salt content.

Now test that statement.
Put a pot on the stove and then before it comes to a boil add salt.
Voila, it begins to boil.


BZZZZT!!! FALSE!!!


Salt water DOES NOT boil at a lower temperature than fresh water. It
boils at a higher temperature. When you add salt to heated water,
it appears to boil because the water is superheated near the bottom of
the pan and the salt crystals provide "nuclei" that start the boiling
process. You can easily verify this by starting with two pans
of water, one salty and one fresh and heating them to their respective
boiling points and measuring the temperature. More explicit
instructions, aimed at middle school students are at:

http://aquarius.nasa.gov/pdfs/prop_fresh_sea.pdf


snip


Mark Borgerson






SNIP

Boiling Point Elevation
The boiling point of a solution is higher than that of the pure
solvent. Accordingly, the use of a solution, rather than a pure
liquid, in antifreeze serves to keep the mixture from boiling in a hot
automobile engine. As with freezing point depression, the effect
depends on the number of solute particles present in a given amount of
solvent, but not the identity of those particles. If 10 grams (0.35
ounces) of sodium chloride are dissolved in 100 grams (3.5 ounces) of
water, the boiling point of the solution is 101.7°C (215.1°F; which is
1.7°C (3.1°F) higher than the boiling point of pure water). The
formula used to calculate the change in boiling point ( Tb) relative
to the pure solvent is similar to that used for freezing point
depression:

Tb = i Kb m,

where Kb is the boiling point elevation constant for the solvent
(0.52°C·kg/mol for water), and m and i have the same meanings as in
the freezing point depression formula. Note that Tb represents an
increase in the boiling point, whereas Tf represents a decrease in
the freezing point. As with the freezing point depression formula,
this one is most accurate at low solute concentrations.

From:
http://www.chemistryexplained.com/Ce...roperties.html

On Mon, 08 Oct 2007 05:33:39 -0700, Keith
wrote:

Boiling Point Elevation
The boiling point of a solution is higher than that of the pure
solvent. Accordingly, the use of a solution, rather than a pure
liquid, in antifreeze serves to keep the mixture from boiling in a hot
automobile engine.....
From:
http://www.chemistryexplained.com/Ce...roperties.html


Actually, no. Ethylene glycol in its pure liquid state boils near
200 degC
http://www.dow.com/ethyleneglycol/about/properties.htm

It is usually cut to 50% dilution for use as an antifreeze.

Brian Whatcott Altus OK

Brian Whatcott wrote:
On Mon, 08 Oct 2007 05:33:39 -0700, Keith
wrote:

Boiling Point Elevation
The boiling point of a solution is higher than that of the pure
solvent. Accordingly, the use of a solution, rather than a pure
liquid, in antifreeze serves to keep the mixture from boiling in a hot
automobile engine.....
From:
http://www.chemistryexplained.com/Ce...roperties.html


Actually, no. Ethylene glycol in its pure liquid state boils near
200 degC
http://www.dow.com/ethyleneglycol/about/properties.htm

It is usually cut to 50% dilution for use as an antifreeze.

Brian Whatcott Altus OK

Since he used the term "solvent", the assumption, at least on my end, is
that he's talking about a solvent/solute system, not a solution of
miscible liquids.

Keith Hughes

In article , betwys1
@sbcglobal.net says...
On Mon, 08 Oct 2007 05:33:39 -0700, Keith
wrote:

Boiling Point Elevation
The boiling point of a solution is higher than that of the pure
solvent. Accordingly, the use of a solution, rather than a pure
liquid, in antifreeze serves to keep the mixture from boiling in a hot
automobile engine.....
From:
http://www.chemistryexplained.com/Ce...roperties.html


Actually, no. Ethylene glycol in its pure liquid state boils near
200 degC
http://www.dow.com/ethyleneglycol/about/properties.htm

It is usually cut to 50% dilution for use as an antifreeze.

True---when mixing liquids, the boiling point is somewhere between
the boiling points of the two.

Radiators and cooling systems are pressurized so that the system
can have an elevated boiling point.


Mark Borgerson