7.7 - Acid Rain

Nitric Acid (HNO3)

A secondary pollutant formed when NO2 reacts with water vapor in the atmosphere. Dissociates from HNO3 to H+ and NO3 - ions.

Env. effects of acid rain

Death of species with narrow pH tolerance rangesIncreased solubility of toxic metals like aluminum and mercury in soils and watersLeeching of positively charged soil nutrients like Calcium, Magnesium, Potassium.Decreased biodiversity and food web interruption

Nitrate ion

NO3- formed by dissociation of nitric acid (HNO3)

Sulfate ion

SO4 2- formed by dissociation of sulfuric acid (H2SO4)

Hydrogen ion

H+, released by the dissociation of sulfuric and nitric acid. The more acidic something is, the greater the concentration of H+ ions

Sulfuric acid (H2SO4).

A secondary pollutant formed from the reaction of SO2 with oxygen and water in the atmosphere. Dissociates from H2SO4 to H+ and SO4 2- ions

Mitigating Acid Rain

Reducing NOx and SO2 emissions is the number one way to reduce acid rain.
Crushed limestone, marble dust, eggshells (anything with calcium carbonate) can be added to soil or waters in order to neutralize pH

Limestone

a sedimentary rock consisting mainly of calcium carbonate.

Calcium carbonate (CaCO3)

A basic compound that is often used to neutralize acidic soils, waters, or other substances. Neturalizes the pH by absorbing excess H+ ions.