Acid Rain - Meaning, Definition, Causes, Effects, Examples, FAQs

Acid Rain - Meaning, Definition, Causes, Effects, Examples, FAQs

Team Careers360Updated on 02 Jul 2025, 04:24 PM IST

Acid rain is a precipitation that is more acidic than normal water, including rain, snow, fog, and dew that contain high levels of acidic components. As carbon dioxide gas combines with it to generate weak carbonic acid, regular rain is mildly acidic, with a pH of around 5.6. For example:

This Story also Contains

  1. What Causes Acid Rain
  2. Environmental Effects of Acid Rain
  3. Examples of Acid rain
Acid Rain - Meaning, Definition, Causes, Effects, Examples, FAQs
Acid Rain

CO2 + H2O → H2CO3

There are two types of acidic deposition: wet and dry. Dry deposition of harmful particles and gases adheres to the ground through dust and smoke in the absence of precipitation.

As natural and unpolluted rainwater has a pH between 5.6 and 6.5 (acidic) due to the reaction of water with CO2, it is classified as acid rain when its pH is less than 5.6. The acidity of rainwater is caused by the natural presence of three compounds and acid rain (CO2, NOx, and SO2) in the troposphere, which are emitted through coal combustion in power plants and gasoline combustion in automobiles. Acid rain pH can range from 5.6 to 3.5, and in certain situations, it can even fall below 2.

File:- Acid rain damaged gargoyle -.jpg

What Causes Acid Rain

Mineral acids such as carbonic acid, nitric acid, and Sulphuric Acid are the principal causes of acid rain.

Acid rain causes

  1. Carbonic acid is formed when carbon dioxide gas molecules react with water molecules (H2CO3). Carbonic acid's capability (H2CO3). The H2CO3 (carbonic acid) molecule possesses the potential to supply H+; because of this, the molecule is classified as an acid. As a result, it is in charge of reducing the pH of a solution.

CO2 + H2O → H2CO3

H2CO3 → H+ + HCO3-

  1. The molecule of nitric oxide (NO), which is generated during lightning storms by the reaction of nitrogen and oxygen, two prevalent atmospheric gases, contributes to the natural decrease of pH (acidity) of precipitation. Nitric oxide (NO) is oxidized to nitrogen dioxide (NO2) in the air, which then reacts with water to form nitric acid (HNO3). In a reaction similar to the dissociation of carbonic acid indicated in the equation below, this acid dissociates in water to produce hydrogen ions (H+) and nitrate ions (NO3-), reducing the pH of the solution once more.

NO + ½ O2 (g) → NO2 (g)

N2 (g) + O2 (g) → 2NO (when lightning strikes in the atmosphere, a reaction occurs.)

3NO2 (g) + H2O → 2HNO3 (aq) + NO (g)

Nitric acid is responsible for around one-fourth of the pH drop in rain (HNO3).

The presence of sulphuric acid (H2SO4) in rainwater accounts for the reduction of pH in most water bodies. Despite the fact that sulphuric acid is produced naturally. Sulphuric acid is produced nearly completely by human activity, particularly the combustion of sulphur-containing fossil fuels in power plants. It is produced naturally in trace amounts through biological decomposition and volcanic activity.

Sulphur in these fossil fuels reacts with water to generate sulphuric acid when they are burned.

SO2 (g) + O2 → SO3 (g) + H2O → H2SO4

Sulphuric acid is an extremely powerful acid. As a result, it is regarded as a strong electrolyte that easily dissociates in water to produce H+ and HSO4- ions. The hydronium ion (H+) and sulfate ion may dissociate further from the HSO4- ion (SO42-) As a result of the presence of H2SO4, the concentration of H+ ions in the rainwater rises substantially, and the pH decreases to a dangerous level.

H2SO4 → HSO4- + H+

HSO4- → SO42-+ H+

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Environmental Effects of Acid Rain

Acid rain increases the number of inorganic and biological reactions that have negative environmental consequences, resulting in a global environmental disaster.

  1. Many huge lakes have become so acidic (low pH lakes) that fish can no longer survive in them.

  2. The breakdown of many naturally occurring soil minerals produces metal ions. These metal ions are then swept away in the runoff, resulting in a variety of consequences:

a) The mobility of harmful ions such as Al3+ in the water supply increases due to the acidic situation.

b) The loss of essential minerals, such as Ca2+, from the soil in the process of neutralizing sulphuric acid, which generates a Ca2+ deficit, kills trees and damages crops.

  1. It affects both animals and the Human respiratory system.

  2. Acid rain has an impact on the aquatic ecosystem when it falls and runs into rivers and ponds. It creates water pollution by changing the chemical composition of the water to a state that is damaging to the aquatic ecosystem's ability to exist.

  1. Corrosion of water pipes is also a result of acid rain. As a result, heavy metals such as iron, lead, and copper are leached into drinking water.

  2. It causes damage to stone and metal structures and monuments.

NCERT Chemistry Notes :

Examples of Acid rain

Acid rain has a significant impact on the Taj Mahal, one of the world's seven wonders. Many companies in the city of Agra produce sulfur and nitrogen oxides into the atmosphere. People continue to utilize low-quality coal and firewood as a source of household energy, exacerbating the problem. Acid rain reacts with marble (Calcium Carbonate) in the following way:

CaCO3 + H2SO4 → CaSO4 + H2O + CO2

The corrosion of this lovely monument is caused by the production of calcium sulfate.

2. The Statue of Liberty, which is made of copper, has also been affected by the cumulative impact of acid rain and oxidation for over 30 years and is thus turning green.

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Frequently Asked Questions (FAQs)

Q: How does acid rain impact agricultural productivity?
A:
Acid rain can reduce agricultural productivity by leaching nutrients from soils, damaging crops directly, and increasing soil acidity. This can lead to reduced yields and may require increased use of lime and fertilizers to maintain soil fertility.
Q: How has our understanding of acid rain and its effects evolved since it was first recognized as an environmental issue?
A:
Since acid rain was first recognized as a problem in the 1960s, our understanding has greatly expanded. We now know it's a complex issue involving atmospheric chemistry, ecosystem dynamics, and human activities. Research has revealed its wide-ranging impacts on terrestrial and aquatic ecosystems, as well as human health and infrastructure. This evolving understanding has led to more effective policies and mitigation strategies, although challenges remain in addressing this global environmental issue.
Q: What are some natural and artificial methods for mitigating acid rain effects in ecosystems?
A:
Natural mitigation includes the buffering capacity of certain soils and water bodies. Artificial methods include liming of lakes and soils to increase pH, reforestation with acid-tolerant species, and the use of alternative, low-sulfur fuels. Long-term solutions focus on reducing emissions of sulfur dioxide and nitrogen oxides at their sources.
Q: How does acid rain affect the cycling of mercury in the environment?
A:
Acid rain can increase the mobility and bioavailability of mercury in ecosystems. It can enhance the conversion of mercury to its more toxic form, methylmercury, in aquatic environments. This can lead to increased mercury accumulation in the food chain, posing risks to wildlife and human health.
Q: What is "episodic acidification" and why is it important in freshwater ecosystems?
A:
Episodic acidification refers to short-term spikes in acidity, often during spring snowmelt or heavy rains. These events can be particularly harmful to aquatic life, causing stress or mortality even in ecosystems that seem to tolerate chronic low-level acidity. Understanding these episodes is crucial for protecting sensitive aquatic species.
Q: How do acid rain effects vary with altitude?
A:
Acid rain effects often increase with altitude due to several factors: higher precipitation rates, thinner soils with less buffering capacity, and more frequent cloud and fog cover (which can contain higher concentrations of acids). This makes high-altitude ecosystems particularly vulnerable to acid deposition.
Q: What is the role of ammonia in acid rain chemistry?
A:
Ammonia, often from agricultural sources, can play a complex role in acid rain chemistry. While it can neutralize acids in the atmosphere, it can also contribute to nitrogen deposition and, when oxidized in soil, can actually increase soil acidity.
Q: How does acid rain impact the cultural heritage and historical monuments?
A:
Acid rain can cause significant damage to cultural heritage sites and historical monuments, particularly those made of limestone, marble, or other carbonate-rich materials. It can erode surfaces, dissolve carvings, and weaken structures, leading to the loss of irreplaceable cultural artifacts.
Q: What role do volcanic eruptions play in natural acid rain formation?
A:
Volcanic eruptions can produce natural acid rain by releasing sulfur dioxide and other gases into the atmosphere. While these events can cause significant local or regional acidification, they are typically short-lived compared to the chronic acid rain caused by human activities.
Q: How does acid rain affect the nitrogen cycle?
A:
Acid rain, particularly from nitrogen oxides, can alter the nitrogen cycle by increasing nitrogen deposition in ecosystems. This can lead to nitrogen saturation in some areas, changing plant community composition and potentially contributing to eutrophication in water bodies.