What Is Acid Deposition Definition Formation Reactions and Effects
Acid rain is given as a popular expression for the more scientific term - acid deposition that refers to the several ways where acidity can move from the atmosphere to the surface of Earth. Acid deposition includes acidic rain and other forms of acidic wet deposition - such as sleet, hail, snow, and fog (or cloud water). Also, acid deposition includes the dry deposition of gases, acidic particles, which may affect landscapes during dry periods. Hence, acid deposition is capable of affecting landscapes and living things, which reside within them even when precipitation is not taking place.
About Acidity
Acidity is the measure of hydrogen ions (H+) concentration in a solution. The pH scale measures whether a solution is either acidic or basic. The substances are considered acidic below a pH value of 7, and every unit of pH below 7 has 10 times more H+, or 10 times more acidic, than the unit above it. For example, rainwater with a pH of 4.0 has a concentration of 100 micro equivalents of H+ per litre, whereas rainwater with a pH value of 5.0 contains a concentration of 10 micro equivalents of H+ per one litre.
Nitrogen Cycle
[Image will be uploaded soon]
Normal rainwater is defined as weakly acidic due to the absorption of carbon dioxide (CO2) from the atmosphere, which is a process that produces carbonic acid and forms organic acids that are generated from biological activity. Additionally, volcanic activity may form nitric acid (HNO3), hydrochloric acid (HCl), and sulfuric acid (H2SO4) based on the emissions associated with particular volcanoes.
The generation of nitrogen oxides from atmospheric molecular nitrogen (N2) conversion by lightning and the organic nitrogen conversion by wildfires are two other natural causes of acidification. The geographic range of any given natural source of acidification, on the other hand, is very limited, and in most instances, it only lowers the pH value of precipitation to around 5.2.
Sulfur Cycle
Sedimentary rocks that emit hydrogen sulphide gas, as well as human sources such as fossil-fuel combustion and smelters, all of which release sulphur dioxide into the atmosphere, are mentioned below as major sulfur-producing sources.
[Image will be uploaded soon]
Anthropogenic activities, specifically the burning of fossil fuels (oil, coal, natural gas) and the smelting of metal ores, are the primary causes of acid deposition. In the US, electric utilities produce around 70% of SO2 and around 20% of NOx emissions. Fossil fuels, which are burned by vehicles, account for around 60% of NOx emissions in the US. Sulfuric and nitric acids are generated in the atmosphere and react with water, when SO2 and NOx, respectively.
The acid rain chemical reaction is given below.
The simplest reactions of acid rain chemical formula or the formation of acid rain chemical equation are given as:
SO2 + H2O → H2SO4 ↔ H+ + HSO4 ↔ 2H+ + SO42
NO2 + H2O → HNO3 ↔ H+ + NO3
By the equation of acid rain given above,
[Image will be uploaded soon]
Wet deposition products are created by these specific reactions in the aqueous phase (for example, in cloud water). They can produce dry, acidic deposition in the gaseous phase. Also, acid formation can take place on particles in the atmosphere.
Where the fossil fuel consumption is large and the emission controls are not in place to reduce NOx and SO2 emissions, the acid deposition will take place in areas downwind of the emission sources, often ranging from hundreds to thousands of km away. In that type of area the pH of precipitation may average 4.0 to 4.5 annually, and the pH of individual rain events may sometimes drop below 3.0.
Ecological Effects of Acid Deposition
Effects on Lakes and Rivers
In the late 1960s and early 1970s, when the regional effects of acid deposition were first noted in parts of western Europe and eastern North America, in the chemistry, the changes of both the lakes and rivers, often in a few remote areas, were linked to declines in the health of aquatic species such as crayfish, the resident fish, including the clam populations.
Excess amounts of acid deposition in the sensitive areas caused tens of thousands of streams and lakes in both Europe and North America to become very more acidic than they had been in the previous decades. Acid-sensitive areas are the ones, which are predisposed to acidification due to either the soil regions having a low buffering capacity or a low acid-neutralizing capacity (ANC).
Effects on Forested and Mountainous Regions
Forests in southern Scandinavia, central Europe, and eastern North America displayed troubling signs of forest dieback and tree mortality in the 1970s and 1980s. In a survey conducted in 1993, 27 European countries have revealed that air pollution damage or mortality in 23% of the 100,000 trees surveyed.
Also, it is likely that the dieback was the result of several factors, including the acid deposition (for example, soil acidification and buffering capacity loss), exposure to the ground-level ozone, possible excess fertilization from the nitrogen compound deposition (such as ammonium, nitrates, ammonia compounds), and general stress, which is caused by a combination of these factors.
Once a tree is in a weakened condition, it is very likely to succumb to other environmental stressors such as insect infestation, drought, and pathogen infections. Often, the forest dieback areas were found to be associated with regions having low buffering capacity where damage to the aquatic ecosystems because of acid deposition was also taking place.
The below figure shows the spruce trees, which are damaged by acid rain in Karkonosze National Park, Poland.
[Image will be uploaded soon]
FAQs on Acid Deposition in Chemistry Complete Guide
1. What is acid deposition in chemistry?
Acid deposition is the process by which acidic components formed from atmospheric pollutants are deposited on the Earth’s surface as rain, snow, fog, or dry particles. It mainly results from sulfur dioxide (SO2) and nitrogen oxides (NOx) released during fossil fuel combustion reacting with water and oxygen in the atmosphere. These reactions produce strong acids such as H2SO4 (sulfuric acid) and HNO3 (nitric acid), which lower the pH of precipitation and soils.
2. What causes acid deposition?
Acid deposition is caused by the atmospheric oxidation of sulfur dioxide and nitrogen oxides into sulfuric and nitric acids. The main causes include:
- Burning of coal and oil in power plants → releases SO2
- Vehicle exhausts → release NO and NO2
- Industrial processes and smelting of metal ores
- Natural sources like volcanic eruptions
These gases react with oxygen and water vapor to form acidic compounds that are later deposited as wet or dry deposition.
3. What is the chemical reaction for the formation of sulfuric acid in acid deposition?
Sulfuric acid in acid deposition forms when sulfur dioxide is oxidized and reacts with water in the atmosphere. A simplified set of reactions is:
- 2SO2(g) + O2(g) → 2SO3(g)
- SO3(g) + H2O(l) → H2SO4(aq)
The product, H2SO4, dissociates in water to release H+ ions, lowering the pH of rainwater.
4. What is the reaction for the formation of nitric acid in acid deposition?
Nitric acid in acid deposition forms from the oxidation of nitrogen dioxide in the atmosphere. A simplified reaction is:
- 4NO2(g) + O2(g) + 2H2O(l) → 4HNO3(aq)
The resulting HNO3 increases the concentration of hydrogen ions (H+) in rainwater, contributing to acid rain and acid deposition.
5. What is the difference between wet deposition and dry deposition?
Wet deposition involves acidic substances dissolved in precipitation, while dry deposition involves acidic gases and particles settling without precipitation.
- Wet deposition: Acidic rain, snow, sleet, or fog containing H2SO4 and HNO3
- Dry deposition: Acidic particles and gases (like SO2, NO2) deposit directly on surfaces and later react with moisture
Both types contribute to soil acidification, water acidification, and material corrosion.
6. What is the normal pH of rainwater and how does acid deposition change it?
Normal rainwater has a pH of about 5.6, but acid deposition can lower it to 4.0 or even 3.0.
- Pure rainwater is slightly acidic due to dissolved CO2 forming carbonic acid: CO2(g) + H2O(l) → H2CO3(aq)
- Acid rain contains stronger acids like H2SO4 and HNO3
Because pH is logarithmic, a drop from 5.6 to 4.6 means the rain is 10 times more acidic.
7. How does acid deposition affect soil chemistry?
Acid deposition affects soil chemistry by increasing H+ concentration and leaching essential nutrients.
- Hydrogen ions replace nutrient cations like Ca2+, Mg2+, and K+
- Essential nutrients are washed away from the soil profile
- Toxic metal ions like Al3+ become more soluble
This chemical imbalance reduces soil fertility and harms plant growth.
8. How does acid deposition affect lakes and aquatic life?
Acid deposition lowers the pH of lakes and rivers, making the water harmful to aquatic organisms.
- Fish and amphibians are sensitive to pH below 6
- Increased Al3+ concentration damages fish gills
- Reproductive cycles of aquatic species are disrupted
A lower pH shifts the chemical equilibrium in water, increasing toxicity and reducing biodiversity.
9. How does acid deposition damage buildings and monuments?
Acid deposition reacts with calcium carbonate in marble and limestone, causing chemical weathering.
- Marble and limestone contain CaCO3
- Reaction with sulfuric acid: CaCO3(s) + H2SO4(aq) → CaSO4(s) + CO2(g) + H2O(l)
This reaction forms gypsum (CaSO4), which flakes off, leading to erosion of buildings and monuments.
10. How can acid deposition be reduced?
Acid deposition can be reduced by lowering emissions of sulfur dioxide and nitrogen oxides.
- Using scrubbers in power plants to remove SO2
- Installing catalytic converters in vehicles to reduce NOx
- Switching to low-sulfur fuels and renewable energy sources
- Applying limestone (CaCO3) to neutralize acidic lakes (liming)
These measures decrease acid-forming pollutants and help restore environmental chemical balance.
