Problem 22 Explain the acidic nature of sul... [FREE SOLUTION]

Chapter 8: Problem 22

Explain the acidic nature of sulphur dioxide based on its reactivity with water.

Short Answer

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Short Answer: Sulfur dioxide is acidic because it reacts with water to form sulfurous acid (H2SO3), which is a weak acid that releases hydrogen ions (H+) in water, leading to an acidic solution. This reaction also contributes to the formation of acid rain, demonstrating the acidic nature of sulfur dioxide.

Step by step solution

Write down the chemical reaction between sulfur dioxide and water

We can start by writing down the chemical reaction between sulfur dioxide (SO2) and water (H2O). The reaction is the following: SO2 + H2O 鈫� H2SO3 This reaction forms sulfurous acid (H2SO3) as a product.

Analyze the properties of the product

Now that we know the product formed in the reaction, we will look at its properties. Sulfurous acid (H2SO3) is a weak acid, meaning it does not fully dissociate into ions in water. However, it still releases hydrogen ions (H+) when dissolved in water, leading to an acidic solution. The dissociation of H2SO3 can be represented by the following equilibrium reaction: H2SO3 <=> H+ + HSO3- The more hydrogen ions released by the H2SO3, the more acidic the solution will be. Since sulfur dioxide reacts with water to form H2SO3, which then releases H+ ions in water, it can be considered an acidic substance.

Understand the role of sulfur dioxide in acid rain formation

Sulfur dioxide is one of the major contributors to acid rain. When SO2 is released into the atmosphere by burning fossil fuels or as a result of volcanic activities, it reacts with the moisture in the atmosphere to form H2SO3. This sulfurous acid then falls to the ground in the form of acid rain, causing damage to the environment, structures, and living organisms. To conclude, sulfur dioxide has an acidic nature because it reacts with water to form a weak acid, H2SO3. This acid releases hydrogen ions, which lead to an acidic solution. The role of sulfur dioxide in acid rain formation further highlights its acidic characteristics.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sulfur Dioxide Reaction with Water

When sulfur dioxide (\( \text{SO}_2 \)) comes into contact with water (\( \text{H}_2\text{O} \)), it undergoes a chemical transformation. This reaction results in the formation of sulfurous acid (\( \text{H}_2\text{SO}_3 \)), a notable compound. This process can be represented by the following equation:\[\text{SO}_2 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_3\]This interaction is a key step in understanding why sulfur dioxide is considered acidic. The simple combination of sulfur dioxide with water highlights how certain gases can directly affect water chemistry and lead to the formation of acidic solutions.

Sulfurous Acid Formation

The formation of sulfurous acid (\( \text{H}_2\text{SO}_3 \)) begins with sulfur dioxide dissolving in water. This reaction is crucial as it converts a gaseous pollutant into a compound dissolved in liquid form. Sulfurous acid itself is a weak acid. This means it only partially separates into ions when mixed with water. This incomplete dissociation is an important characteristic that affects the acidity of the solution.

Sulfurous acid acts as a bridge between gas and acid rain formation.
It is not stable and tends to dissociate, adding hydrogen ions to the solution.

Even though sulfurous acid is not as strong as some other acids, its ability to release hydrogen ions contributes to the acidity of the solution it dissolves in.

Acid Rain Formation

Acid rain becomes a problem when sulfur dioxide is present in the atmosphere. When released, possibly from burning fossil fuels or volcanic activities, sulfur dioxide interacts with atmospheric moisture. This reaction yields sulfurous acid, which is carried to the ground in raindrops, creating what we know as acid rain. Acid rain can have several negative impacts:

Damage to natural ecosystems, as it lowers the pH of water bodies.
Harm to structures and buildings, particularly those made of limestone and marble.
Adverse effects on plant life and soil, making it less fertile.

This phenomenon underscores the importance of reducing sulfur dioxide emissions to mitigate environmental damage.

Weak Acid Dissociation

Sulfurous acid, being a weak acid, doesn't completely ionize in water. The dissociation can be represented by the equilibrium:\[\text{H}_2\text{SO}_3 \rightleftharpoons \text{H}^+ + \text{HSO}_3^-\]This equation shows that only a part of the sulfurous acid molecules break down to release hydrogen ions (\( \text{H}^+ \)) and bisulfite ions (\( \text{HSO}_3^- \)). The concept of weak acid dissociation is fundamental because:

It explains why sulfurous acid contributes to acidity but not as strongly as strong acids like hydrochloric acid.
In equilibrium, the concentration of undissociated acid remains significant, affecting the amount of free \( \text{H}^+ \) ions in the solution.

Understanding this equilibrium helps in grasping the nuanced behavior of sulfurous acid as it participates in environmental processes such as acid rain formation.

91影视

Explain the acidic nature of sulphur dioxide based on its reactivity with water.

Short Answer

Step by step solution

Write down the chemical reaction between sulfur dioxide and water

Analyze the properties of the product

Understand the role of sulfur dioxide in acid rain formation

Key Concepts

Sulfur Dioxide Reaction with Water

Sulfurous Acid Formation

Acid Rain Formation

Weak Acid Dissociation

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