Lecture Outline – MAP-UA 203 - Energy and Environment
April 3, 2012
HW due April 10, 11:
Ch. 6: 6, 7, 9, 10, 12, 14-16 (calculate the pH in parts d-g of #14),
18, 20, 33, 36
Today's lecture will begin our discussion of acid rain.
While the problem
of acid rain does not make for screaming headlines today, it does adversely affect plant
and animal life, and causes corrosion of metals and erosion of monuments.
cases where acidic fogs have persisted in urban areas, there have been serious
consequences to human health.
The chapter begins by defining acids and bases
chemically. The pH scale for quantifying acidity is then introduced.
Sources of acid rain
(production of oxides of sulfur and nitrogen by combustion of fuels) are discussed as well
as the deleterious effects of acid rain, and what can be done to control the problem.
Acid rain is rain having a pH < 5.3. (As we will see later on, carbon dioxide, which is
normally present in the atmosphere, dissolves in rain, giving it an acidic pH even in the
absence of other pollutants.)
Acid rain leads to:
corrosion of metal
damage to stone and marble
damage to vegetation
We are going to look at the following topics:
What is an acid?
pH and molarity
sources of acid rain
effects of acid rain
politics of acid rain
Acids are substances that release H
(hydrogen ions or protons) into solution.
hydrogen atom that has lost its single electron.
Because a hydrogen ion is just a hydrogen nucleus, which is
, the charge on
the hydrogen ion is
It is thus very reactive, looking for electrons
In water solution, hydrogen ions attach themselves to water molecules
(using one of the unused electron pairs on the oxygen).
The result is the H
But most chemists still call it H