Please enable JavaScript.
Coggle requires JavaScript to display documents.
Acid Deposition (Stronger than Carbonic Acid H2CO3 (Can get to pH 2)…
Acid Deposition
Stronger than Carbonic Acid H2CO3 (Can get to pH 2)
Nitric Acid
Nitrous Acid
Sulphurous Acid
Sulphuric Acid
Effects
Environmental Impact
Low pH
Fish cannot survive
Fish eggs cannot hatch
Leech essential plant nutrients from soil
Aluminum present in soil at high pH values in the form of insoluble aluminum hydroxide (Al(OH)3)
Release aluminum ions → damage roots of plants → prevent uptake of water
Aluminum Ions (Al3+) leached
Harmful effects on fish's gills
Prevent oxygen uptake and leading to death by asphyxiation due to excess secretion of mucus
Loss of species 🔪 Food Chain
Domination of acid-tolerant species. Ex. Sphagnum moss
Buildings
Limestone + Marble: Forms of Calcium Carbonate (CaCO3)
CaCO3 (s) + H2SO4 (aq) → CaSO4 (aq) + H2O (l) + CO2 (g)
Iron, steel, aluminum
Rate of rusting (electrolytic process) increases
Greater concentration of ions in acid-rain
Humans
Affect Mucous membranes and lungs
Irritation
Exacerbated symptoms of Asthma
Other Respiratory Conditions
Reducing Acid Deposition
Pre-combustion methods
Remove sulfur
Hydrodesulphurisation (Remove sulphur from refined petroleum products)
High Pressure + High Temperature + Catalyst
Product → Hydrogen sulfide (H2S)
Post-combustion methods
Remove sulfur
React with base
Flue gas desulphurisation
Aqueous suspension of calcium carbonate and calcium oxide
Product → Calcium sulfite (sulfate(IV) → Calcium sulfate
Reactions
CaCO3 (s) + SO2 (g) → CaSO3 (s) + CO2 (g)
CaO (s) + SO2 (g) → CaSO3 (s)
2CaSO3 (s) + O2 (g) → 2CaSO4 (s)
Neutralize soil and lakes pH
Limestone (CaCO3)
H2SO4 (aq) + Ca(OH)2 → CaSO4 (aq) + 2H2O (l)
Calcium Hydroxide (Ca(OH)2)
H2SO4 (aq) + CaCO3 (s) → CaSO4 (aq) + H2O (l) + CO2 (g)
Wet Deposition
Examples
Acid Rain
pH < 5.0
Water + Nitrogen Oxides (NOx)/Sulfuric Dioxide (SO2)
Snow
Fog
Rain Water
pH = 5.6
CO2 and Water -> CO2 (g) + H2O (l) ⇌ H2CO3 (aq)
Dry Deposition
Acidic particles and gases fall to the ground via dust and smoke (absence of precipitation)
Can be washed into streams, lakes, and rivers
Nitrogen monoxide (NO)
Formation (High Temperatures)
Lightning Storms - Nitrogen + Oxygen
Internal Combustion Engines
N2 (g) + O2 (g) → 2NO• (g)
2NO• (g) + O2 (g) → 2NO2• (g)
2NO2• (g) + H2O (l) → HNO3 (aq) + HNO2 (aq)
Diesel (higher temperature) greater pollution than petrol
Reduces emissions with a catalytic converter
Sulfur Dioxide (SO2)
Photochemical Oxidation
Water Droplets (Dissolved SO2) + Catalyst (Soot + Fine metallic particles)
2SO2 (g) + O2 (g) → 2SO3 (g)
SO3 (g) + H2O (l) → H2SO4 (aq)
(Natural) Volcanic Eruptions
Coal + Oil that contain sulfur - Power Stations
Combustion and Oxidation: S (s) + O2 (g) → SO2 (g)