1. Neutralization Reactions & Environment
Chemical Reactions
Neutralization Reactions & Environment

2. Neutralization Reactions
Acid + Base  Salt + Water (Svante)
Salt – an ionic compound that is produced by the reaction of an acid and a base.
If the salt in insoluble a suspension of small, solid particles will be formed during the reaction and this is called a precipitate.
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)

3. Neutralization and Environmental Challenges
Acid Precipitation
Sulfuric Acid – H2SO4(aq)
S(s) + O2(g)  SO2(g)
2SO2(g) + O2(g)  2SO3(g)
SO3(g) + H2O(l)  H2SO4(aq)
Nitric Acid
Ammonia is reacted with air in the presence of a catalyst (platinum) to produce nitrogen dioxide.
Nitrogen dioxide is then reacted with water to form nitric acid: NO2(g) + H2O(l)  HNO3(aq)

4. Neutralization and Environmental Challenges
Acid Precipitation
Different oxides of sulfur (SO2 and SO3) and nitrogen (NO and NO2) are referred to as SOx and NOx. When they are burned in air they react with water to form sulfurous acid (H2SO3), sulfuric acid, nitrous acid (HNO2) and nitric acid.

5. Neutralization and Environmental Challenges
Normal rain is usually slightly acidic (5.5 – 6.2) due to carbon dioxide in the atmosphere: CO2(g) + H2O(l)  H2CO3(aq).
Adding the other acids to the atmosphere increases the acidity of the precipitation and it is normally now between 4 and 5 on the pH scale.
Acid precipitation is soluble in water (it joins water easily) and this poses a threat to lakes and ponds.
As the pH of a lake approaches 6, insects and other aquatic animals begin to die. As the pH approaches 5, plants and micro-organisms begin to die. Below 5 and all life in a lake or pond is gone and the water appears crystal clear.        

6. Neutralization and Environmental Challenges
Heavy Metals - Acid precipitation dissolves metals (aluminum, mercury and copper), which may leach into ground water that feeds rivers and lakes. In high concentrations these metals are harmful, even to us.
Ways to combat Acid Precipitation
Calcium carbonate (limestone) reacts with acids in a neutralization reaction. There are three factors that determine how limestone should be added to a lake:
1. Volume of water in the lake
2. Chemical composition and reactivity of its rocks and soil
3. Turnover time

7. Neutralization and Environmental Challenges
Turnover time refers to the time needed for all the water in the lake to be replaced by natural resources. If turnover time is short liming needs to be done more frequently.
It is important to understand that liming is not a solution. It like treating the symptoms instead of the problem itself. Liming cannot alter streams that are acidic or ice that has a low pH. Limestone also may kill plants and insects that are sensitive to calcium.

8. Neutralization and Environmental Challenges
Using Chemistry to Control Harmful Emissions
Scrubbers – anti-pollution device for removing polluting gases such as sulfur dioxide from industrial smokestack emissions. They can remove up to 95% of SO2 from smokestack emissions.
All sources of coal contain sulfur as a contaminant. When coal burns the sulfur is converted to sulfur dioxide. Calcium carbonate is added with the coal and air as it enters the furnace.

9. Neutralization and Environmental Challenges
The coal burns and CO2 and SO2 are produced. The heat breaks the CaCO3 into CO2 and CaO. In the furnace some of the SO2 reacts with CaO to form CaSO3 (calcium sulfite). Some SO2 remains unreacted and leave the furnace as exhaust.
This enters the scrubber where CaO in water is sprayed on the exhaust gases. Most of the remaining SO2 reacts with the dissolved CaO to again form CaSO3. A wet slurry of CaSO3 is formed and discarded.