1.
……………………………. RBMahajan

2.
1. Dry deposition
- Acidic gases and particles
2. Wet deposition
- Acidic rain, fog and snow

3.
What is Acid rain?
- Acid rain is rain,
snow or fog that
is polluted by acid
in the atmosphere
and damages the
environment.
ACID RAIN DROP

4.
• Sources of primary pollutants
• Deposition of secondary pollutants

5.
 Produced by natural phenomena and
anthropogenic activities [like combustion
of fossil fuels , oxidation of organic
material in soils , volcanic eruptions,
biomass burning]
 It is soluble in water
 It can be oxidised within airborne water
droplets producing sulphuric acid

6.
Produced by Combustion Of Fuels
Residential, cars , commercial
Industrial furnaces, electrical-utility
boilers, Engines, other equipment
 It is soluble in water
 It can be oxidised within airborne water
droplets producing nitric acid

7.
Acid Rain
(Acid Precipitation)
Any precipitation carrying dissolved acids from natural or man made causes.
Examples;
a. CO2 dissolves in H2O---------> Creates carbonic acid (H2CO3)
b. Sulfur dioxide (from internal combustion) mixes with H2O ---------> Sulfuric Acid (H2SO4)
c. Nitrogen oxides (from internal combustion) mixes with H2O ---------> Nitric Acid (HNO3)
*Acid precipitation may have a pH as low as 3. Very Acidic!
*Acids in the air may be carried thousands of miles from their source, polluting soil & water in pristine areas!

8.
 marble and limestone are calcium carbonate
(2CaCO3 + 2SO2 + O2 --> 2CaSO4 + 2CO2);
 sulfur dioxide in dry deposition increases
metal corrosion
(Fe + SO2 + O2 --> FeSO4);
 protective oxide layer removed from metals
(Al2O3 + 3H2SO4 -->Al2(SO4)3 + 3H2O

9.
• Depends on
– Transport downwind
– Buffering in soils
(alkalinity)
• On thin, non-buffering soils
• On buffers
– carbonate rocks, limestone
often used for buildings,
• Limestone and
concrete structures

10.
 Leaching (washes) out essential nutrients
from soil like;Mg(2+), Ca(2+), K(+) ions
 Damages roots by releasing Al(3+) ions
from rocks;
 SO2 blocks stomata and prevents
photosynthesis;
 Leaves are damaged by acidity.

11.
• Forests

12.
aluminum oxide trapped in rocks can
be released and Al(3+) interferes with
gills' ability to take in O2;
(Al(OH)3 + 3H(+) --> Al(3+) + 3H2O)
nitric acid can cause eutrophication
(plant deaths, anaerobic decomp, etc)
destruction of food chain pH 4 is dead
lake

13.
• Lakes, rivers - Deduced diversity and
abundance of aquatic ecosystems

14.
 Effects of acid deposition on human life-
 acid gases irritate respiratory tract; increased
risk of asthma, bronchitis, emphysema;
 poisonous metal ions released from pipes are
tied to some diseases (Alzheimer's)

15.
 reduce industrial emission levels,
 alternative energy sources,
 reduced demands for fossil fuels,
 reduce acid rain damage in lakes by adding
lime/calcium hydroxide to neutralize acids
(CaO + H2SO4 --> CaSO4 +H2O)

16.
Problem- In this experiment, you will,
1. Generate three gaseous oxides, CO2, SO2, and NO2.
2. Simulate the formation of acid rain by bubbling
each of the three gases into water and producing
three acidic solutions.
3. Measure the pH of the three resulting acidic
solutions to compare their relative strengths
 You can use data logger.
 You will be assessed for DCP and CE

17.
Acid Formation Equation Explanation
Sulfurous Acid
Sulfuric Acid
Sulfuric Acid #2
Nitrous Acid
Nitric Acid
Acid Deposition work sheet
1.What is acid deposition?
2.How is carbonic acid a natural contributor to acid rain? Provide equations to support your
response:
3.There are four common routes for Wet Acid Deposition, complete the table:

18.
Environmental Effect on Detailed information regarding effect
Appropriate Equations
Explanation of Process
Limit the Production
Neutralize the effects
1.What are the five environmental effects of acid rain? Explain each below:
:
1.There are two generic methods to counter acid deposition, describe each method below: