HDTenEightyP/NetNews huggingface dataset:
From: howard@netcom.com (Howard Berkey)
Subject: Re: Soft Drink Ingredient
Organization: Netcom Online Communications Services (408-241-9760 login: guest)
Date: Fri, 18 Dec 1992 18:18:33 GMT

In article <A21067@F.maus.de> Sevo_Stille@f.maus.de (Sevo Stille) writes:
>ornitz@kodak.kodak.com wrote in SCI.CHEM,A65354@HB
>
>While quinine in soft drinks may have been a useful trick to smuggle a malaria
>prophylactic into the gin tonics of drunk colonial officers, it is hardly a
>suitable flavour for todays soft drinks - stuff like tonic water and bitter
>lemonades probably escaped from the drugstores into the bars during prohibition
>and its "medical" applications of cocktails.

It's still used in some tonic water, though.


>
>True quinine tonic water (Schweppes Kenia still used to sell pretty strong
>stuff some years ago...) has a strange blueish hue, which might be mimicked
>with glycerol ester of wood rosin, to give quinine replacement tonics the
>colour of the real stuff.


Quinine is cool for drinks in a nightclub setting because it
fluouresces with a pale blue color when exposed to UV light.  Fairly
brightly, too.  Black lights in clubs can make it fluouresce.

-Howard



-- 
::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::
Howard Berkey                       			   howard@netcom.com
			  WARNING: Intel Inside
... .. ...   ... .. ...   ... .. ...    ... .. ...   ... .. ...   ... .. ...
Newsgroups: sci.chem
From: gcook@horus.cem.msu.EDU (Greg Cook|xxxxxx)
Subject: Re: Stable Orbitals: 1/2 full
Organization: Michigan State University
Date: Wed, 16 Dec 92 13:33:37 GMT

From article <1992Dec13.040948.7448@cronkite.ocis.temple.edu>, by sklar@picasso.ocis.temple.edu (Dave Sklar):
> 
> stable?  It seems intuitive, but intuition is pretty worthless inside an
> atom.                            ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
 ^^^^^

I'm not so sure about that.  :-)

-----------------------------------------------------------------------
Gregory R. Cook                           gcook@horus.cem.msu.edu
Department of Chemistry                   cookgreg@student.msu.edu
Michigan State University                 cook@msucem.BITNET
Newsgroups: sci.chem
From: rmcory@uwovax.uwo.ca
Subject: Re: Acid-base equilibrium (triprotic)
Organization: University of Western Ont, London
Date: Wed, 16 Dec 1992 04:47:14 GMT
Summary: Buffer problem for head scratchers...
Keywords: acid/base triprotic

In article <c60a-gx.724438370@danube.Berkeley.EDU>, c60a-gx@danube.Berkeley.EDU (Jeffrey Twu) writes:
> Alright, I've been pondering over this question for the last few days,
> and have deduced it impossible to solve (with respect to the constraints,
> not the difficulty).  I would like your comments on it.
> 
> You are given four stock solutions, each one molar (1 mol/L) in their
> concentrations:  H3PO4, NaH2PO4, Na2HPO4, Na3PO4 (charges omitted).  From
> only these four solutions (no H2O lying around), you will make a buffer

Sorry, I'm afraid you have to have some H2O! Someone is pulling your leg.

> solution with the following restraints:
> 
> 1) pH = 6.8 (reasonably buffered around there)
> 2) total volume of new solution = 1 liter
> 3) Free phosphate concentration = [PO4] = 0.10 M

What is undoubtedly required here is ***TOTAL*** "phosphate" conc = 0.10 M, 
which in this case would be [H2PO4] + [HPO4] since at pH 6.8 the concs of
H3PO4 and PO4 would be negligible.

Otherwise, the problem is impossible, since [PO4] cannot be 0.10 M at pH 6.8.

> 
> How much of each solution will you use?
> 
> You are given the following data:
> _Acid_	       _pKa_	_Ka_
> H3PO4		2.148	7.11 * 10^-3
> H2PO4		7.199	6.32 * 10^-8
> HPO4	       12.15	7.1  * 10^-13
> 
> Now, if this problem is actually impossible as written, would it be
> solvable if you removed one or more of the constraints?  (This question
> isn't part of the actual problem.)
> 
> (BTW, nothing weird like vaporizing solutions to a new concentration of
> anything; this is one of the exam questions from a <quantitative>
> chemistry final.)
> 
> Jeff
> +-Just remember:------------------------------------------------------------+
> |	Take it easy.							    |
> |		...and don't forget that human touch.	   	            |
> +<c60a-gx@danube.berkeley.edu>_________________________________<Jeffrey Twu>+


-- 
--------------------------------------------------------------
Prof. Robert M. Cory, Chemistry Dept, U. Western Ontario, London N6A 5B7 CANADA
Office (519)679-2111x6339; Home (519)472-8866; FAX (519)661-3022; cory@uwo.ca
From: pete@physchem.ox.ac.uk (Pete Biggs)
Newsgroups: sci.chem
Subject: Re: Glow Sticks
Keywords: Glow
Date: 16 Dec 92 09:55:14 GMT
Organization: Physical Chemistry Laboratory, South Parks Road, Oxford OX1 3QZ
Originator: pete@joule.pcl


In article <15DEC199201342361@zeus.tamu.edu>, wdb3926@zeus.tamu.edu (BRUTON, WILLIAM DANIEL) writes:
> Glow Sticks...
> 
> You know those liquid filled cylinders that you can buy at camping stores?
> When you break a small capsule in the center of the plasitc stick
> by bending the cylinder the capsule breaks and two liquids mix and
> give off a bright green glow....bright enough to read by...
> 
> Any idea what the two liquids are?
> 
> Dan

The bulk liquid is a derivative of fluorocene (sp?) modified to enhance the
brightness/efficiency and to shift the wavelength a bit.  The glass ampule
contains hydrogen peroxide (or some other such oxidising agent).

Pete

-- 
=============================================================================
Pete Biggs                          Janet: pete@uk.ac.ox.physchem
                                    Internet: pete@physchem.ox.ac.uk
=============================================================================
Newsgroups: sci.chem
From: xslkkk@oryx.com (kenneth k konvicka)
Subject: EtSH Stability in Propane                                              EtSH Stability in Propane??? 
Organization: Oryx Energy, Dallas, Texas.
X-Newsreader: Tin 1.1 PL5
Date: Fri, 18 Dec 1992 19:13:07 GMT

Anybody know how long this odorant is stable in liquid propane?
Years or longer?  I understand its dosage as an odorant is only
a few ppm.
From: alanchem@csd4.csd.uwm.edu (Alan Scott Olson)
Newsgroups: sci.chem
Subject: Re: Soft Drink Ingredient
Date: 15 Dec 1992 17:54:06 GMT
Organization: Computing Services Division, University of Wisconsin - Milwaukee
Distribution: usa
NNTP-Posting-Host: 129.89.7.4

In article <1992Dec15.153655.15312@rosevax.rosemount.com> scotbri@flower.rosemount.com (Scott Brigham) writes:
>I was reading the label on my bottle of Schweppes Bitter Lemon
>and noticed the last ingredient is "glycerol ester of wood rosin".
>What is this and why am I drinking it?
>=========================
> scotbri@rosemount.com  
> Scott Brigham  (AA0HU)
> St. Paul, MN  USA
>=========================

And as a followup...why do manufacturers put shellac in pills?

-- 
 ______________/ Alan S. Olson  Swanson Environmental, Inc. \_________________
/     e-mail to alanchem@csd4.csd.uwm.edu  OR  alan@alchemy.chem.uwm.edu      \
|          Want some good music?  Check out Milwaukee's own BoDeans           |
+-----------------------------------------------------------------------------+
Newsgroups: sci.chem
From: "patrick evans" <patrick.evans@canrem.com>
Subject: modelling
Reply-To: "patrick evans" <patrick.evans@canrem.com>
Organization: Canada Remote Systems
Distribution: sci
Date: 17 Dec 92 19:09:39 EST


  Before I go any further, I would like to thank those who mailed me in
response to previous questions regarding the silicon polymer and
explosives.  The opportunity to reply was missed partly due to an
over-active mail deletion-by-date system!  Nevertheles....

  I am currently in need of any basic step-by-step methods or algorythms
for determining the 3 dimensional shape and orientation of simple
organic compounds.  Essentially, I plan to model these molecules with a
program, but have more programming experience than chemistry.  Also, any
information relating to the structure and or lattice structures of
elemental inorganic comounds would also be appreciated.  As of right
now, I have the "basic" lattice structure for several (ie. rhombic,
hexagonal,etc.).

  As part of the final goal, I would like to take any formula (with a
relative complexity, of course) and use a processes to lay down the
structure via a normal 3d coordinate system which is then sent to the
modeller to be rendered.  Is it *possible* to figure these out, or
is a data base of pre-defined structues (I would like to avoid this)
required?  If so, would you post it for me (any form is fine, verbal
steps can be translated and written out)?

  Also, any suggestions relating to Stereochemistry and CAD modelling
would be greatly appreciated. Thanks ahead of time!


<>  "The meek will inherit the Earth.           Fatline from the     <>
><  The rest of us will go to the stars."            Gods            ><
><                                                                   ><
><  From the Dual-Processor Computer Of: Patrick.Evans@Canrem.COM    ><
--
Canada Remote Systems  - Toronto, Ontario
World's Largest PCBOARD System - 416-629-7000/629-7044
From: nick@gepard.msk.su (Ovcharenko Nickolay Yurievich)
Newsgroups: sci.chem
Subject: BEE VEDOM: Where to use? Information needed.
Date: 18 Dec 92 13:07:48 GMT
Reply-To: nick@gepard.msk.su
Organization: GEPARD, Ltd

Dear gentlemen!
Here in Russia we are going to produce bee vedom. Would you help us in finding
medical or pharmacological centers interested in long-time cooperation. If
scientists or other specialists will contact with us, it will be great.
     Sincerely  Nickolay Ovcharenko
     nick@gepard.msk.su
     fax (095)-135-70-30
Newsgroups: sci.chem
From: cec@imager (Charles Cunningham)
Newsgroups: sci.chem
Subject: vanadium dioxide
Summary: How to make single crystal VO2?
Keywords: vanadium oxide, single crystal
Date: 15 Dec 92 23:07:21 GMT
Organization: Laboratory for Experimental Astrophysics

Does anybody know how to make a single-crystal piece of vanadium dioxide?

Also, is anybody familiar with some way to get an atomically flat surface
on VO2?

Thanks,
Charles Cunningham
cec@llnl.gov

-- 
 ___________________________________________________________________________
|                              |                                            |
| Charles E. Cunningham        | "Deeep Huuurting!  DEEEP HUUR-TING!!!"     |
| Physicist                    |                                            |
Newsgroups: sci.chem
From: rsb@.mcc.com (Richard S. Brice)
Subject: types of chemical bonds
Originator: rsb@ptolemy.mcc.com
Organization: MCC, Austin, Texas
Distribution: usa
Date: Thu, 17 Dec 1992 15:19:35 GMT



Can someone explain to a chemistry novice what the real physical 
differences are between covalent and ionic bonds?  Can one tell by
looking at some properties of atoms (molecules?) whether they will
combine with one or the other type of bonds?  The high school
chemistry book my kids are using really muddles through these
issues in a very unclear way.

Thanks

R. Brice
MCC Corp

Newsgroups: sci.chem
From: polowin@chem.queensu.ca (Joel Polowin)
Subject: Re: types of chemical bonds
Organization: Dept. of Chemistry, Queen's University
Distribution: usa
Date: Thu, 17 Dec 1992 21:39:39 GMT

In article <1992Dec17.202252.23289@sifon.cc.mcgill.ca> bspencer@cs.mcgill.ca (Brian SPENCER) writes:

>Also, a pure ionic bond is electrostatic in nature. That is, there are
>attractive and repulsive attraction between positively and negatively
>charged ions. In general, an ionic molecule sets itself up so as to
>maximize the attractive forces and minimize the repulsive ones.

I get twitchy over the phrase "ionic molecule".  Except (perhaps) in the	
gas phase, there really isn't such a thing; in solution the ions are generally
dissociated, and in a crystal there's an ionic lattice with no defined 
molecular units.

Joel Polowin
polowin@silicon.chem.queensu.ca, polowin@chem.queensu.ca,
polowinj@qucdn.queensu.ca
Newsgroups: sci.chem
From: singley@helix.nih.gov (Erick Singley)
Subject: Re: What is in those 'bubbling' lamps?
Keywords: lamps
Organization: (National Institutes of Health, Bethesda, MD)
Date: Wed, 16 Dec 1992 15:00:18 GMT

>LavaLamps are still available, in several colors and sizes. Someone
>on the net posted an address a few years ago, which I've lost; a phone
>call to The Exploratorium Store (San Francisco, CA 415 561-0393 mail order)
>will get you your choice.

The store "Spencer Gifts" can be found in many malls in the Maryland area:
Ivrsn Mall (Hillcrest) - 423-2668
Montgomery Mall - 365-8820
Wheaton Plaza - 933-1353
Forest Village - 736-6888
Columbia Mall used to (donno anymore..) and the Security Mall now has one.
Donno if the above numbers are (410) or (301) due to our state's area code split
:)  They should have several different colors and whatnot, too. Umm, hmm now I
see that the first poster about his is .au (australia?) This might not help
much then...  :)
Erick
--
singley@clinpharm.niaaa.nih.gov
Newsgroups: sci.chem
From: billn@hpcvaac.cv.hp.com (bill nelson)
Subject: Re: White gold
Organization: Hewlett-Packard Company, Corvallis, Oregon USA
Date: Sun, 13 Dec 1992 09:45:13 GMT

kenneth@davy.uio.no (Kenneth Ruud) writes:
: In article <1992Dec9.072759.22917@ucsu.Colorado.EDU> lorenzo@spot.Colorado.EDU (Eric J. Lorenzo) writes:
: >
: >   What exactly is white gold?  Is it a naturally found metal?  It definately
: >   costs more in jewelry form.
: >
: White gold is not found naturally as a metal, because it is an alloy made of
: gold, nickel and palladium. Im'm afraid I don't know the exact composition in
: percent, but perhaps somone out there can help?

White gold usually contains either 25% platinum or 12% palladium.

Bill
From: treesh@bach.helios.nd.edu (carey treesh)
Newsgroups: sci.chem
Subject: Re: Glow Sticks
Keywords: Glow
Date: 16 Dec 92 18:27:58 GMT
Organization: OUC, University of Notre Dame

There has got to be a bit more too it then just mixing H202 with a florsenent
dye.  From what I know about it, the H202 is mixed with some sort of 
thing called and "ester oxolate".  The dye is also mixed with some kinda ester
I think.  

I have some good info on how they make these, I will post it tonighe.  

ctfm
Newsgroups: sci.chem,sci.engr.chem
From: totty@flute.cs.uiuc.edu (Brian Totty)
Subject: ??? Borden Chemical on Net ???
Organization: Picasso Group, DCS, University of Illinois, Urbana-Champaign
Date: Fri, 18 Dec 1992 21:58:26 GMT

Does anyone know if Borden Chemical Co. is on the net?  If someone has a net
address for some Borden site, I would greatly appreciate it!

   /                       Brian Totty             o o
  /__  __  o     Department of Computer Science     o  
 /  / /   /          1304 W. Springfield Ave       \_/  "We have corn in
/__/ /   /               Urbana, IL 61801                Massachusetts too!"
Gradual Student         totty@cs.uiuc.edu
From: mkaiserman@hpb.hwc.ca
Newsgroups: sci.chem
Subject: Re: Tobacco, How Does It Cause Cancer ???
Date: 13 Dec 92 14:03:04 EST
Organization: Health and Welfare, Canada

In article <1992Dec9.195502.131314@ns1.cc.lehigh.edu>, jrb6@ns1.cc.lehigh.edu (JAMES RONALD BERARDI) writes:
> 
> 
>     I always thought it was the (-)-Nicotine that caused cancer.
> Benzo[a]pyrene is a product of its combustion, which is the
> corinogen.  It is converted in the liver to an epoxy diol that
> can induce mutations leading to the uncontrolled growth of certain
> cells.  The epoxi diol produced by oxidation in the liver
> is called  7,8-Dihydroxy-9,10-epoxy-7,8,9,10-tetrahydrobenzo[a]pyrene
> I picked this up in one of my chem books.
> 
> 
> 
> 
> Jim
> 
         > "Give a man a fish and you feed him for a day.
> Teach the man how to fish and you feed him for the rest of his life."     -?
> 
> 
> -- 
> 
>     |     |   \    ____________________
>     |     |    \  /||||||||||||||||||||\
>     |     |     \/|||/  ||||||||||  \|||\||||||||||||||||||||||||/
>     |     |     /||___ |||||||||||| ___||\||||||||||||||||||||||/
>     |     |    /||||||\ \||||||||/ /||||||\||||||||||||||||||||/
>     |     |   /||||||||\/        \/||||||||\||||||||||||||||||/

Benzo[a]pyrene is only one of at least 50 carcinogens found in tobacco
smoke.  It would be pointless to suggest that any one is the prime cause of
lung cancer in humans.  It seems that each one, individually or in
combination with others, can cause lung cancer.  Inj reality, it is the
entire tobacco smoke mixture that is toxic .

It might interest you to know that tobacco contains lead, pesticide
residues and nitrosamines.  These products are regulated in other consumer
goods but seem to be ignored when found in tobacco.






Newsgroups: sci.chem
From: c60a-gx@danube.Berkeley.EDU (Jeffrey Twu)
Subject: Acid-base equilibrium (triprotic)
Summary: Quantitative chemistry problem
Keywords: acid base equilibrium triprotic
Organization: University of California, at Berkeley
Date: Tue, 15 Dec 1992 16:52:50 GMT

Alright, I've been pondering over this question for the last few days,
and have deduced it impossible to solve (with respect to the constraints,
not the difficulty).  I would like your comments on it.

You are given four stock solutions, each one molar (1 mol/L) in their
concentrations:  H3PO4, NaH2PO4, Na2HPO4, Na3PO4 (charges omitted).  From
only these four solutions (no H2O lying around), you will make a buffer
solution with the following restraints:

1) pH = 6.8 (reasonably buffered around there)
2) total volume of new solution = 1 liter
3) Free phosphate concentration = [PO4] = 0.10 M

How much of each solution will you use?

You are given the following data:
_Acid_	       _pKa_	_Ka_
H3PO4		2.148	7.11 * 10^-3
H2PO4		7.199	6.32 * 10^-8
HPO4	       12.15	7.1  * 10^-13

Now, if this problem is actually impossible as written, would it be
solvable if you removed one or more of the constraints?  (This question
isn't part of the actual problem.)

(BTW, nothing weird like vaporizing solutions to a new concentration of
anything; this is one of the exam questions from a <quantitative>
chemistry final.)

Jeff
+-Just remember:------------------------------------------------------------+
|	Take it easy.							    |
|		...and don't forget that human touch.	   	            |
+<c60a-gx@danube.berkeley.edu>_________________________________<Jeffrey Twu>+
Newsgroups: sci.chem
From: dnash@uxa.cso.uiuc.edu (Dave Nash)
Subject: Re: TIME HAS INERTIA - NewScientist Article
Organization: University of Illinois at Urbana
Date: Mon, 14 Dec 1992 07:32:59 GMT

In article <1992Dec14.023025.20353@dmp.csiro.au> lachlan@dmp.csiro.au (Lachlan Cranswick) writes:
>
>This is more proof that sci.chem is ceasing to be a happening
>place.  Where are our crackpots and resident loonies?           


They're already here -- we just seem to get a less ...ahh, virulent strain.
You see, sci.physics is full of people with freaky ideas about time, whereas
sci.chem has people with freaky ideas about speed.

-- 
David Nash                  | Gradual Student, Chemistry
                            | University of Illinois (Urbana)
(dnash@uxa.cso.uiuc.edu)    | This .sig is made of 100% recycled electrons.
(nash@aries.scs.uiuc.edu)   | No binary trees were killed to make it.
From: pavlovic@ehsc.orst.edu (James Pavlovich)
Newsgroups: sci.chem
Subject: Re: Soft Drink Ingredient
Date: 16 Dec 92 00:13:16 GMT
Article-I.D.: ehsc.pavlovic.16.724464796
Distribution: usa
Organization: Environmental Health Sciences Center, Oregon State University
NNTP-Posting-Host: massspec1-0079-e.als.orst.edu

In article <5079@equinox.unr.edu> whitbeck@equinox.unr.edu (Michael Whitbeck) writes:
>From: whitbeck@equinox.unr.edu (Michael Whitbeck)
>Subject: Re: Soft Drink Ingredient
>Date: 15 Dec 92 22:51:26 GMT
>In article <1992Dec15.153655.15312@rosevax.rosemount.com> scotbri@flower.rosemount.com (Scott Brigham) writes:
>>I was reading the label on my bottle of Schweppes Bitter Lemon
>>and noticed the last ingredient is "glycerol ester of wood rosin".
>>What is this and why am I drinking it?
>>=========================
>> scotbri@rosemount.com  
>> Scott Brigham  (AA0HU)
>> St. Paul, MN  USA
>>=========================
>
>wood rosin is obtained from the extraction of pine
>stumps with naptha followed by distillation. The
>raw material is graded by color and consists of a
>mixture of high mol. wt. acids, abietic acid may
>dominate [the mixture may often be referref to as
>abietic acid]. The glycerol ester is of course the
>product from reacting the acids with glycerol.
>
>Why are you drinking it? -- I don't know; does it
>taste good?
>
>
>My *guess* is that it either contributes to the
>texture or the bitter taste of the beverage.
>
>Mike W.

I suspect it has to do with the texture of the drink or what they refer to 
in food sciences as "mouth feel". In a similar vien, I have heard (but 
cannot verify) that they used to put things like chloroform in soft drinks 
to get a slight throat numbing effect that people for some reason liked in 
their sodas.  

JGP
Newsgroups: sci.chem
From: ggawboy@magnus.acs.ohio-state.edu (Galen F Gawboy)
Subject: Re: intro. quant. chem.
Keywords: Intro text.
Organization: The Ohio State University
Date: Sat, 12 Dec 1992 00:14:13 GMT

In article <ng4.724058457@husc10> ng4@husc10.harvard.edu (Ho Leung Ng) writes:
>
>   Hello.  I am an undergraduate struggling in my intro. course in quantum
>chemistry.  I would appreciate it if people could refer me to some helpful
>books which are relatively easy to understand.  Our texts are Levine's
>Quantum Chem., 4th ed., and Karplus and Porter's Atoms and Molecules.  Both
>books are pretty good, but difficult to follow at times (at least for me).
>Thank you.
>
>Ho Leung Ng

    If you have had Multi-Variable calculus, I would recomend:

    "Quantum Chemistry", by Eyring, Walter, and Kimball. If you are
taking inro quantum chemistry, and are having difficulties understanding the
material of your texts, it is my suspicion that your difficulties arise
from the lack of detail in your current texts. The Eyring book is 
the best introduction to the derivation of atomic term symbols I have seen.
It is a tad more mathematically rigorous than Levine or Karplus and Porter. It
can be found in the library and there also exists a Dover paperback addition
which can be found in the COOP, or any other good bookstore. Sometimes a 
"simpler" explanation is not a clearer explanation.

    Hope this helps.

-Regards

Galen F. Gawboy
Chemical Physics
The Ohio State University