1. Acid Rain

2. Acid Rain Overview Unusually Acidic Precipitation Extremely harmful to various ecosystems Another term for wet acid deposition The term was first coined in 1972 In the 70’s scientists began to realize the implications and repercussions it has on the environment In 1990 the Clean Air Act put a limit on the amount of SO 2 production of power plants, but while this has limited Acid rain it has not ended it or any of its lasting effects

3. Causes Acid rain is almost uniformly caused by human-made emissions – NO, NO 2, CO 2, SO 2, SO 3 These are produced by electricity generation, factories, and motor vehicles Particularly harmful are the vast emissions of electrical power plants that utilize coal or other fossil-fuels

4. Causes In the past short smokestacks led to the destruction of local ecosystems The newer, taller smokestacks failed to solve the problem, however, and simply dispersed emissions across a wider area

5. Causes There are natural causes for acid rain as well, such as volcanic eruptions, forest fires, and lightning However these cause only a minute amount of acid rain in the greater scheme of things For example, the eruption of Mount Saint Helens released only about what one factory produces in a year

6. Chemical Process Previously mentioned sources emit harmful pollutants – The most common and most potent are NO x and SO 2 The gases are dispersed via the wind to other locations At this point they dissolve into precipitation to form sulfuric acid, ammonium nitrate and nitric acid

7. Chemical Process Example: – Sulfur from burning oil and coal  SO 2 – SO 2 is converted into SO 3 – SO 3 reacts with water to create sulfuric acid – SO 3 (g)+H 2 O(l)  H 2 SO 4 (aq)

9. Acidity of Acid Rain Pure water has neutral pH of 7. Normal rainwater is slightly acidic, at around 5.6, due to the dissolution of CO 2 from the surrounding atmosphere Acid rain typically has pH values between 3 and 4, but has been recorded to be as low as 2.7 in some cases, only a little above the acidity of battery acid, and in the range of that of vinegar

10. Effects 1. Pollution of Soil: – Higher acidity can kill microbes in soil by denaturing their enzymes – Important nutrients, such as Magnesium and Calcium, are leached away, changing the chemistry of the soil and affecting sensitive species – Releases aluminum into the soil

11. Effects 2. Plant Life – Effected soil affects plants’ ability to withstand cold temperatures and insects, fight off disease, and reproduce – The aluminum in the soil makes it difficult for plants to take up water – The acid can also soak into their leaves and kill them killing the plant in the process

12. Effects 3. Erosion: – Acidity erodes stone, especially those with high amounts of calcium carbonate. – The acid reacts with the calcium carbonate to create gypsum (CaSO 4 ·2H 2 O), which then flakes off: CaCO 3 (s) + H 2 SO 4 (aq) ⇌ CaSO 4 (aq) + CO 2 (g) + H 2 O (l) – This can destroy buildings and statues – Acid also increases the corrosion rate of metals such as iron steel copper and bronze

13. Effects 4. Human Health: – The acid in the rainwater is too diluted to have direct adverse effects, but the particulates responsible for acid rain do have an adverse effect – Increased amounts of fine particulate matter in the air contribute to heart and lung problems including asthma and bronchitis – The acidic water can corrode water pipelines. The high lead levels in water and sulfate pollution are harmful to human health

14. Effects 5: Pollution of Rivers and Lakes: – Fish can’t survive at the low pH of an acidic environment – Whole populations of fish wind up dead, entire lakes and rivers in Europe with no normal aquatic life left – Acid rain makes waters acidic and causes them to absorb the aluminum, which makes its way from soil into lakes and streams – At pHs lower than 5 most fish eggs will not hatch and lower pHs can kill adult fish