1 / 13

Acid Deposition

Acid Deposition. pH Scale. 7 is neutral As numbers decrease, acidity increases As numbers increase, alkalinity increases. pH Scale. Q - How much more acidic is a pH of 3 than a pH of 7? A – 10,000 times pH is a logarithmic scale. Rain.

lewismartinez
Télécharger la présentation

Acid Deposition

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Acid Deposition

  2. pH Scale • 7 is neutral • As numbers decrease, acidity increases • As numbers increase, alkalinity increases

  3. pH Scale • Q - How much more acidic is a pH of 3 than a pH of 7? • A – 10,000 times • pH is a logarithmic scale

  4. Rain • From a natural and unpolluted atmosphere has a pH of close to 6.0 • Results form reaction of water vapor and CO2 in the atmosphere forming a weak carbonic acid (H2CO3): • CO2(g) + H2O(l) H2CO3(aq) • Since carbonic acid is a weak acid it partially dissociates: • CO2(g) + H2O(l) H+(aq) + HCO3-(aq)

  5. Acid Rain • Has a pH below 5.6 • Reaction of water vapor with sulfur dioxide (SOx) and nitrogen oxides (NOx)

  6. Acid Rain form Sulfur compounds (SOx) • Sulfur dioxide reacts with water to form sulfurous acid (H2SO3): • SO2(g) + H2O(l) H2SO3(aq) • Sulfur dioxide (SO2) can be oxidized gradually to sulfur trioxide (SO3): • 2SO2(g) + O2(g) 2SO3(g) • Sulfur trioxide (SO3) reacts with water to form sulfuric acid (H2SO4): • SO3(g) + H2O(l) H2SO4(aq)

  7. Acid Rain from Nitrogen compounds (NOx) • Oxides of nitrogen, particularly nitrogen dioxide (NO2) react with water to form nitrous acid (HNO2) and nitric acid (HNO3): • 2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq)

  8. Effects of Acid Rain • Damages buildings and marble statues by reacting with calcium carbonate to from soluble calcium hydrogen carbonate (calcium bicarbonate, Ca(HCO3)2): • CaCO3 + acid rain Ca(HCO3)2

  9. Effects of Acid Rain

  10. Effects of Acid Rain • Leaches aluminum and calcium form the soil into the ground water, lakes and rivers; poisoning fish and plant roots • Aluminum reacts negatively with the gills of the fish • irritating them • causing a build up of mucous • resulting in suffocation

  11. Effects of Acid Rain • Disrupts the process of photosynthesis • Damages plant life • Slows the production of chlorophyll • Sulfuric acid kills plants • “Crown dieback” • Leaves at the top (crown) of trees die • Leaving a sparse thin crown that progressively increases and moves its way down the tree

  12. Crown Dieback

  13. Assignment • 3.5.1 and 3.5.2 – Chemistry of acid Precipitation and Possible Effects

More Related