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<DIV><FONT face=Arial>Dear Ron</FONT></DIV>
<BLOCKQUOTE
style="BORDER-LEFT: #000000 2px solid; PADDING-LEFT: 5px; PADDING-RIGHT: 0px; MARGIN-LEFT: 5px; MARGIN-RIGHT: 0px">
<DIV style="FONT: 10pt arial">----- Original Message ----- </DIV>
<DIV
style="FONT: 10pt arial; BACKGROUND: #e4e4e4; font-color: black"><B>From:</B>
<A title=rwhongser@web.de href="mailto:rwhongser@web.de">Ronald
Hongsermeier</A> </DIV>
<DIV style="FONT: 10pt arial"><B>To:</B> <A
title=stoves@lists.bioenergylists.org
href="mailto:stoves@lists.bioenergylists.org">Discussion of biomass cooking
stoves</A> </DIV>
<DIV style="FONT: 10pt arial"><B>Sent:</B> Thursday, August 08, 2013 10:22
AM</DIV>
<DIV style="FONT: 10pt arial"><B>Subject:</B> Re: [Stoves] more on ocean
acidification</DIV>
<DIV><BR></DIV>
<DIV>Dear Kevin,<BR><BR>isn't a billion 10^9 ? and billion billion therefore
10^18?</DIV>
<DIV> </DIV>
<DIV><FONT face=Arial># You are correct. I was out by a factor of a million. I
hate it when I make errors that big. :-( However, the good news there is
1,000,000 times as much water to absorb the Anthropogenic CO2, and it
could take 1,000,000 times as long for the average Ocean pH to be
changed, at the current rates of emission.</FONT><BR><BR>the factors include
water's ability to chemically shunt organic and inorganic contained and bottom
materials within the pH system, which means we'd have to be able to at least
model the composition of an average ocean bottom re. minerals, overall ocean
avg. temp, surface to bottom migration, etc.<BR></DIV>
<DIV><FONT face=Arial># The issues are indeed complex.</FONT></DIV><FONT
face=Arial></FONT>
<DIV><BR>I am an ecologically sympathetic person, but see more danger
presently from legal, semi-legal and illegal fishing practice to the overall
health of the oceans.</DIV>
<DIV> </DIV>
<DIV><FONT face=Arial># In addition to these issues, there is also the issue
of "micro plastics" dispersed through the water column. </FONT><BR><BR>I am
also sympathetic with the concerns of Cecil Cook re. poisons, but think it
somewhat confusing to put CO2 in the same class as CCl4. Depending on the
amount of time between the cleaning process and the dipped sleeve there could
well have been quite a significant amount of Carbon Tet in the water,
especially in view of the proportions of scale-- I well remember being able to
tell when I walked through the door of our house if my mother had brought
things home from the cleaners and the odor was remarkable for some time after
removing the plastic or paper wrappers of the day. And no, we don't know
everything, which should make us more cautious not only in our actions, but
also in concretizing our fears.</DIV>
<DIV> </DIV>
<DIV><FONT face=Arial># Agreed! The World Environment has a lot of real and
imagined problems, and we need science, Truth, and Fact to determine which are
the most serious problems, and which should be acted upon first.
</FONT></DIV><FONT face=Arial></FONT></BLOCKQUOTE>
<BLOCKQUOTE
style="BORDER-LEFT: #000000 2px solid; PADDING-LEFT: 5px; PADDING-RIGHT: 0px; MARGIN-LEFT: 5px; MARGIN-RIGHT: 0px">
<DIV><FONT face=Arial>Best wishes,</FONT></DIV>
<DIV><FONT face=Arial></FONT> </DIV>
<DIV><FONT face=Arial>Kevin</FONT></DIV>
<DIV><BR><BR>regards,<BR>Ron von Bayernmittelwochenwochenende<BR><BR></DIV>
<DIV class=moz-cite-prefix>On 08.08.2013 13:41, Kevin wrote:<BR></DIV>
<BLOCKQUOTE cite=mid:ED190DCE2EF24891AC010075E38B6600@usera594fda0bf
type="cite">
<META name=GENERATOR content="MSHTML 8.00.6001.23507">
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<DIV><FONT face=Arial>Dear Paul</FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>Crispin indicates that the mass of the ocean is about
1.33 billion billion tons, i.e., 1.33 x 10^12 tons. That is a lot of
water.</FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>The oceans are now alkaline. Some CO2 additions will
lower the pH of the ocean, but the oceans will still be
alkaline.</FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>How much CO2 would be required to actually make the
oceans acidic? </FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>At current rates of anthropogenic CO2 production, how
long would it take for the Oceans to actually become acidic?</FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>Thanks!</FONT></DIV>
<DIV> </DIV>
<DIV><FONT face=Arial>Kevin</FONT></DIV>
<BLOCKQUOTE
style="BORDER-LEFT: #000000 2px solid; PADDING-LEFT: 5px; PADDING-RIGHT: 0px; MARGIN-LEFT: 5px; MARGIN-RIGHT: 0px">
<DIV style="FONT: 10pt arial">----- Original Message ----- </DIV>
<DIV
style="FONT: 10pt arial; BACKGROUND: #e4e4e4; font-color: black"><B>From:</B>
<A title=paul.olivier@esrla.com href="mailto:paul.olivier@esrla.com"
moz-do-not-send="true">Paul Olivier</A> </DIV>
<DIV style="FONT: 10pt arial"><B>To:</B> <A
title=stoves@lists.bioenergylists.org
href="mailto:stoves@lists.bioenergylists.org"
moz-do-not-send="true">Discussion of biomass cooking stoves</A> </DIV>
<DIV style="FONT: 10pt arial"><B>Sent:</B> Thursday, August 08, 2013 7:08
AM</DIV>
<DIV style="FONT: 10pt arial"><B>Subject:</B> Re: [Stoves] more on ocean
acidification</DIV>
<DIV><BR></DIV>
<DIV dir=ltr>
<DIV>
<DIV>
<DIV>Crispin,<BR><BR></DIV>The term that the scientific community uses is
"ocean acidification," and this is a very real environmental problem that
most people in the scientific community do not deny.<BR><BR></DIV>Many
thanks.<BR></DIV>Paul Olivier<BR></DIV>
<DIV class=gmail_extra><BR><BR>
<DIV class=gmail_quote>On Thu, Aug 8, 2013 at 12:27 PM, Crispin
Pemberton-Pigott <SPAN dir=ltr><<A
href="mailto:crispinpigott@gmail.com" target=_blank
moz-do-not-send="true">crispinpigott@gmail.com</A>></SPAN> wrote:<BR>
<BLOCKQUOTE
style="BORDER-LEFT: #ccc 1px solid; MARGIN: 0px 0px 0px 0.8ex; PADDING-LEFT: 1ex"
class=gmail_quote>
<DIV lang=EN-CA link="blue" vlink="purple">
<DIV>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Dear
Friends</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">I
have been catching up on less important correspondence after being in
Asia for a while. There is one thing that still needs to be put down
like a broken-legged horse and that of course is the idea that
CO<SUB>2</SUB> ‘acidifies’ the ocean.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Because
this is a high school chemistry level topic and I know some of us took
other things – or as the drummer in my brothers class said, “I don’t
remember Chemistry, I was stoned that year.”</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">So
for those of you who were also stoned that year or can’t remember back
that far, here is a simple review of pH with special reference to the
oceans, CO<SUB>2</SUB> and the false, badly mis-named idea that
CO<SUB>2</SUB> ‘increases the acidity of the oceans’.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">The
term pH refers to one of three distinct chemical conditions which bear
no relationship to each other. One is called acidity, another is called
alkalinity and third is ‘neutral’. Acidity and alkalinity are so
different that if equal in ‘strength’ they cancel each other completely
leaving a neutral condition. Different pH numbers refer to different
conditions.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Acid
solutions (it has to be a solution with water in it) have a chemistry
that has Hydrogen atoms stripped of their single electron. They are thus
positively changed and seeking an electron. This they will happily strip
out of anything passing by if they can find it, tearing the molecules to
bits in the process which is why acids ‘eat’ things.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Alkaline
solutions (again, involving water) have molecules that have an extra
electron available (but not Hydrogen) and are thus negatively charged.
They will give away an electron happily, often wrecking the object that
receives it which is why they eat things too but by a completely
different process.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Both
acidic and alkaline solutions can corrode things like metals and rocks.
One takes electrons and one gives them. Quote opposite. The two
conditions are so incompatible they cannot be present at the same time
in a mixed solution. It is one, the other or ‘neutral’ if neither
condition is present.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">If
you have an alkaline solution like the ocean (pH 7.8 - 8.4 depending on
where you are, the time of day and a host of other things) and you want
to neutralise it so that all its spare electrons are taken up by various
things, you would have to add something acidic. Adding CO<SUB>2</SUB> by
bubbling it through the seawater will convert some of the CO<SUB>2</SUB>
(about 1%) to carbonic acid which has a deficiency of electrons and that
acid will merge with whichever passing opportunity presents itself. The
corresponding alkaline molecule will be neutralised as its spare
electron will be passed to the carbonic acid molecule (which has an
H<SUP>-</SUP> in it) and afterwards neither will have any charge. Both
will be neutralised if the charges are balanced.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Because
this happens very quickly, you cannot actually find any carbonic acid in
the ocean. Nor any other acid. The oceans are not acidic at all.
Any ocean has quite a store of available electrons. Anything acidic you
dump into the sea is quickly neutralised and the pH drops slightly
because it is closer to a neutral condition. The oceanic capacity to
hand over electrons to any passing electron gap is very, very large.
There are several processes that would begin to offer electrons but do
not because the ocean is too alkaline to allow them to get started. The
ability to do this is called the ‘buffering’ capacity. You may remember
‘Bufferin’ the pill that neutralises stomach acid. The pill is alkaline
and has a large buffering capacity so it can hand a lot of electrons
over to the acid in the stomach, thus neutralising it. If you took a
whole bottle of Bufferin pills, your stomach would not become less and
less and less acidic. It would be neutralised and then become alkaline
and remains so until the spare electrons were taken up in a neutralising
process. People are, in general, alkaline and should eat alkaline foods
to remain healthy. Excess acid is a problem.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">By
the same measure, reducing the availability of spare electrons in the
ocean water does not <I>at all</I> make the water acidic because it
still has many more available electrons. It is less alkaline, but it is
not acidic at all – zero in the ‘acidic scale’ (there isn’t one).
</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">In
order to make a convenient metric for describing these two conditions
(which can cancel each other out very predictably) the pH scale is used.
Above 7.0 the solution has available electrons and is termed alkaline.
Below 7.0 is has a deficiency of electrons and is called ‘acidic’. The
reason for the use of two different terms is they are chemically
dissimilar and cannot coexist.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Acidity
of a solution is often represented by the Hydrogen equivalent
[H<SUP>+</SUP>]<SUB>T</SUB> which is the total number of Hydrogen
electrons that would be needed to neutralise it.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Alkalinity
is often expressed in terms of its equivalence to Calcium Carbonate
CACO<SUB>3</SUB> in mg/Litre.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
Can CO<SUB>2</SUB> ‘acidify’ water? </SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
Yes, if the water is neutral to begin with, or already acidic, like rain
water. Because rain water is acidic, when it falls into the ocean it
neutralises the drops of seawater where it touches, before becoming
diluted again by the surrounding ocean. Rainwater does not impart to the
ocean any microscopic ability to withdraw electrons. It is quickly
neutralised by some seawater. When it is finished a few seconds later,
the acid has been destroyed.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
If one bubbled CO<SUB>2 </SUB>through sea water, would it eventually
become acidic?</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
Yes. If you were to first neutralise all the available electrons by
mopping them up, after that it would start to become acidic. It would
not considered be acidic at all until the whole body of the sample had
first been neutralised. These two conditions cannot co-exist.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
What about ‘acid rain’. </SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
All rain is acidic. It is acidic because fresh water absorbs CO2 rapidly
from the atmosphere, converting about 1% into carbonic acid. This falls
into the oceans and reacts with the available alkaline molecules. It is
easy to acidify rain. It is very difficult to neutralise the oceans
because of the rocks upon which they sit which have a huge, massive
buffering capacity. There are numerous life cycles of creatures that
withdraw CO<SUB>2</SUB>, CO3<SUP>-2</SUP> and HCO<SUB>3</SUB>- when it
is available. Obviously CACO<SUB>3</SUB> is high on the list for uptake
by creatures that make shells.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
Which has a larger impact on ocean alkalinity: atmospheric
CO<SUB>2</SUB> or rain containing CO<SUB>2</SUB>?</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
Not clear. Rain has a big effect because oceans actually have difficulty
picking up enough CO<SUB>2</SUB> to drive the level much above 600 ppm
because of the limited surface area compared with the volume and the
huge buffering capacity. Rain is much higher - about 1120 ppm
CO<SUB>2</SUB>. Global rainfall totals about half a million cubic
kilometers per year and contains about 600 billion tons of
CO<SUB>2</SUB> which is about 20 times <A
href="http://www.global-greenhouse-warming.com/anthropogenic-climate-change.html"
target=_blank moz-do-not-send="true">human</A> output. </SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
What is the mass of the oceans?</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
1.332 billion billion tons.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
Do reputable scientific organisations refer to ‘acidifying’ the oceans
even though that is not, chemically, what it happening?</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
Yes. NASA <A
href="http://www.earthobservatory.nasa.gov/Features/OceanCarbon/"
target=_blank moz-do-not-send="true">does</A>. “As we burn fossil fuels
and atmospheric carbon dioxide levels go up, the ocean absorbs more
carbon dioxide to stay in balance. But this absorption has a price:
these reactions lower the water’s pH, <SPAN
style="BACKGROUND: yellow">meaning it’s more acidic</SPAN>.”</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Q.
But it is less alkaline, not more acidic. Why do they write that when it
is untrue, in fact it is unscientific?</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">A.
I don’t think anyone knows. Perhaps they too missed Chemistry in
high school.</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">+++++++</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt">Regards<BR>Crispin</SPAN></P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; COLOR: #1f497d; FONT-SIZE: 11pt"></SPAN> </P>
<P class=MsoNormal><B><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; FONT-SIZE: 11pt"
lang=EN-US>Sent:</SPAN></B><SPAN
style="FONT-FAMILY: 'Calibri','sans-serif'; FONT-SIZE: 11pt" lang=EN-US>
Friday, July 26, 2013 3:25 PM<BR><B>Subject:</B> [Stoves] more on ocean
acidification</SPAN></P>
<DIV class=im>
<P class=MsoNormal> </P>
<DIV>
<P class=MsoNormal><A
href="http://www.scientificamerican.com/article.cfm?id=noaa-scientists-embark-voyage-asses-ocean-acidification"
target=_blank
moz-do-not-send="true">http://www.scientificamerican.com/article.cfm?id=noaa-scientists-embark-voyage-asses-ocean-acidification</A><BR
clear=all><BR>-- <BR>Paul A. Olivier PhD<BR>26/5 Phu Dong Thien
Vuong<BR>Dalat<BR>Vietnam<BR><BR><BR></P></DIV></DIV></DIV></DIV><BR>_______________________________________________<BR>Stoves
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clear=all><BR>-- <BR>Paul A. Olivier PhD<BR>26/5 Phu Dong Thien
Vuong<BR>Dalat<BR>Vietnam<BR><BR>Louisiana telephone: 1-337-447-4124
(rings Vietnam)<BR>Mobile: 090-694-1573 (in Vietnam)<BR>Skype address:
Xpolivier<BR><A href="http://www.esrla.com/" target=_blank
moz-do-not-send="true">http://www.esrla.com/</A> </DIV>
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