Thursday Sep. 8, 2016

Some Cajun music before class today from the Lost Bayou Ramblers "Blue Moon Special" (6:27) from a concert in Sweden, "Moi J'Connais Pas" (4:34) from a performance in France.

I'd give you the full period if today's quiz counted for credit.  But it's just for practice so we spent about 30 minutes tying up a loose end and looking ahead to material that we will be covering next week.

If you weren't in class today you can download a copy of the Practice Quiz and try answering the questions at home.  Then you can have a look at the answers and grade your work.

The downward force of air pressure


I am concerning that you might be thinking that a sea level pressure value of 14.7 psi might not sound like much.  But when you start to multiply 14.7 by all the square inches on your body it turns into a lot of pounds of force. 

The yellow box on the person's chest in the picture is a brick size, 4" x 8" = 32 square inch, area.  If you multiply 14.7 psi by 32 sq. in. you get 470 pounds!  It would take a stack of 90 to 100 bricks to produce that much weight.  Imagine lying on the beach with 90 bricks stacked up on your chest.  That's what the atmosphere is doing.

Why isn't the person in the picture above crushed by the weight of the atmosphere above.  The answer is that the person's body pushes back with the same amount of force.  Air does the same thing.  This is the topic we will explore next week.

The upward (and sideways) force of air pressure


Air pressure is a force that pushes downward, upward, and sideways.  If you fill a balloon with air and then push downward on it, you can feel the air in the balloon pushing back (pushing upward).  You'd see the air in the balloon pushing sideways as well. 



We would be able to see this by placing a brick on top of a balloon.  The balloon gets squished (pushed out sideways) but not flattened.  It eventually pushes upward with enough force to support the brick.  The squished balloon is what air at the bottom of the atmosphere looks like.  And it is supporting more than just one brick, it is supporting a pile 90 to 100 bricks tall (just like the yellow box on the chest of the guy at the beach).
Acid rain
Sulfur dioxide is one of the pollutants that can react with water in clouds to form acid rain (some of the oxides of nitrogen can also react with water to form nitric acid).  The formation and effects of acid rain are discussed on p. 12 in the photocopied Class Notes.


Acid rain is often a problem in regions that are 100s even 1000s of miles from the source of the sulfur dioxide.  Acid rain in Canada could come from sources in the US, acid rain in Scandinavia came from industrialized areas in other parts of Europe. 

Note at the bottom of the figure above that natural "pristine" rain has a pH less than 7 and is slightly acidic.  This is because the rain contains dissolved carbon dioxide gas.  The acid rain demonstration described below and done in class should make this point clearer.



Some of the problems associated with acid rain are listed above.

Acid Rain Demonstration

Some common acids are listed below.  In solution the acid molecules dissociate (split) into pieces.  The presence of H+ ions is what makes these materials acids.



And actually it isn't enough to just have H+ ions for something to be an acid.  There are H+ ions in pure distilled water and it's not an acid.  To be an acid the H+ ion concentration must be greater than is found in distilled water.  The H+ ion concentration in distilled water is 10-7 moles of H+ ions per liter of water.  A mole is just a number, a very large number (6 x 1023).  It's the same idea as dozen.  A dozen means you've got 12 of something.   10-7 moles of H+ ions per liter is 10-7 times 6 x 1023  =  6 x 1016 H+ ions per liter of water.  

The pH scale
We often use the pH scale to measure acid concentration.  An H+ ion concentration of 10-7 moles/liter corresponds to pH 7 (the pH value is computed by taking the -log10 of the H+ ion concentration).   Other than remembering the pH value of distilled water is pH7, these are all details you don't need to worry about.
 
It is also possible to have fewer H+ ions in a solution than would be found in distilled water.  A solution like this is basic.



Pouring some acid into water would increase the H+ ion concentration (from 10-7moles/liter to 10-3moles/liter, perhaps as shown in the example above).  Adding a base to water will decrease the H+ ion concentration (from 10-7moles/liter to 10-10moles/liter, perhaps).

Now we can proceed with the demonstration.  We will start with three 1000 mL beakers each filled with distilled water.  Some vinegar (contains acetic acid) was added to the left beaker. Some ammonia (a base) was added to the right beaker.

Acid/Base indicator solution
Then we added some bromothymol blue, a color indicator solution, to all three beakers.  Bromothymol blue has the amazing property of changing color depending on whether it is mixed with an acid (golden yellow) or a base (deep blue).



So far we have just reviewed the pH scale and introduced acid/base indicator solutions.

When sulfur dioxide is released into the air it reacts with the water in clouds to produce acid rain.  I really can't use SO2 in class because it's poisonous.  I'll use carbon dioxide, CO2, instead.


We added some Tucson tap water to a large 2000 mL beaker.  This represents a cloud.   We added some bromothymol blue to the tap water and it turned blue.  So we know that Tucson tap water is basic. 

A few small pieces of dry ice are put into a flask.  We close the flask with a stopper.  The end of a piece of tubing connected to the flask is immersed in the tap water.

Dry ice sublimes.  It turns directly from solid to ice (ordinary ice melts and turns from solid to liquid).  The gaseous CO2 is invisible but you can tell it is there because of the bubbles in the tap water.  Some of the CO2 dissolves as it bubbles through the water and slowly turns the water acidic.  You can tell that this is occurring because the bromothymol blue indicator turns from deep blue to green and eventually to yellow.


I call this a "sort of" acid rain demonstration.  That's because we haven't really produced acid rain.  Air contains carbon dioxide and the CO2 makes natural rain slightly acidic (pH5.6 or so).  To make true acid rain we would need a different gas, something other than carbon dioxide, something that would lower the pH below 5.6.

While we didn't actually produce acid rain, there is concern that increasing atmospheric concentrations of carbon dioxide will dissolve and acidify the world's oceans.  This is discussed in the following article from The Christian Science Monitor.  You can download a copy of the article here.



The main concern over increasing atmospheric carbon dioxide concentrations is global warming from enhancement of the greenhouse effect.  We will discuss this topic at some point during the semester.

Carbonated beverages contain dissolved carbon dioxide and are acidic.  Soft drinks also contain phosphoric acid which makes them even more acidic than the dissolved carbon dioxide would do.  With time the acidity of soft drinks can damage tooth enamel.