Understanding the Dissociation of HClO2

Oct 13, 2025 by windailys.com 33 views

Introduction

In chemistry, understanding the behavior of weak acids is crucial for predicting the concentration of hydrogen ions (H3O+) in a solution. A weak acid is one that does not completely dissociate in water, resulting in a relatively low concentration of hydrogen ions. In this article, we will explore how to calculate the concentration of H3O+ at equilibrium in a solution containing a weak acid, specifically HClO2 (chlorous acid).

Understanding the Dissociation of HClO2

HClO2 is a weak acid that partially dissociates in water according to the following equation:

HClO2 (aq) + H2O (l) ⇌ H3O+ (aq) + ClO2- (aq)

The dissociation constant (Ka) for HClO2 is 1.1 × 10-2. This value indicates the extent to which the acid dissociates in water.

Calculating the Concentration of H3O+

To calculate the concentration of H3O+ at equilibrium, we can use the following equation:

Ka = [H3O+][ClO2-] / [HClO2]

We are given the initial concentration of HClO2 as 2.85 × 10-2 M. Since HClO2 is a weak acid, we can assume that the concentration of HClO2 remains relatively constant throughout the dissociation process.

Let's denote the concentration of H3O+ as x M. Since the dissociation of HClO2 produces one H3O+ ion for every one ClO2- ion, the concentration of ClO2- will also be x M.

Substituting these values into the Ka equation, we get:

1.1 × 10-2 = (x)(x) / (2.85 × 10-2)

Simplifying the equation, we get:

1.1 × 10-2 = x^2 / (2.85 × 10-2)

Multiplying both sides by (2.85 × 10-2), we get:

3.15 × 10-3 = x^2

Taking the square root of both sides, we get:

x = √(3.15 × 10-3)

x ≈ 1.77 × 10-2

Therefore, the concentration of H3O+ at equilibrium is approximately 1.77 × 10-2 M.

Conclusion

In this article, we calculated the concentration of H3O+ at equilibrium in a solution containing a weak acid, HClO2. We used the dissociation constant (Ka) to determine the concentration of H3O+ and found that it is approximately 1.77 × 10-2 M. This value indicates the relatively low concentration of hydrogen ions in a solution containing a weak acid.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
Chang, R. (2010). Chemistry. McGraw-Hill.

Additional Resources

Khan Academy: Acid-Base Chemistry
Chemistry LibreTexts: Acid-Base Equilibrium

Frequently Asked Questions

Q: What is the dissociation constant (Ka) for HClO2? A: The dissociation constant (Ka) for HClO2 is 1.1 × 10-2.
Q: How do I calculate the concentration of H3O+ at equilibrium? A: To calculate the concentration of H3O+ at equilibrium, use the Ka equation: Ka = [H3O+][ClO2-] / [HClO2].
Q: What is the concentration of H3O+ at equilibrium in a solution containing 2.85 × 10-2 M HClO2? A: The concentration of H3O+ at equilibrium is approximately 1.77 × 10-2 M.
Frequently Asked Questions: Calculating the Concentration of Hydrogen Ions in a Weak Acid Solution =============================================================================================

Q: What is the dissociation constant (Ka) for HClO2?

A: The dissociation constant (Ka) for HClO2 is 1.1 × 10-2. This value indicates the extent to which the acid dissociates in water.

Q: How do I calculate the concentration of H3O+ at equilibrium?

A: To calculate the concentration of H3O+ at equilibrium, use the Ka equation:

Ka = [H3O+][ClO2-] / [HClO2]

This equation can be rearranged to solve for [H3O+]:

[H3O+] = √(Ka * [HClO2])

Q: What is the concentration of H3O+ at equilibrium in a solution containing 2.85 × 10-2 M HClO2?

A: The concentration of H3O+ at equilibrium is approximately 1.77 × 10-2 M.

Q: What is the significance of the concentration of H3O+ in a weak acid solution?

A: The concentration of H3O+ in a weak acid solution is a measure of the acidity of the solution. A higher concentration of H3O+ indicates a more acidic solution.

Q: How does the concentration of H3O+ change with the concentration of HClO2?

A: The concentration of H3O+ is directly proportional to the concentration of HClO2. As the concentration of HClO2 increases, the concentration of H3O+ also increases.

Q: What is the relationship between the Ka and the concentration of H3O+?

A: The Ka is a measure of the extent to which the acid dissociates in water. A higher Ka value indicates a greater extent of dissociation, which results in a higher concentration of H3O+.

Q: Can I use the Ka equation to calculate the concentration of H3O+ for any weak acid?

A: Yes, the Ka equation can be used to calculate the concentration of H3O+ for any weak acid, as long as the Ka value and the initial concentration of the acid are known.

Q: What are some common sources of error when calculating the concentration of H3O+?

A: Some common sources of error when calculating the concentration of H3O+ include:

Incorrectly measuring the initial concentration of the acid
Not accounting for the dissociation of the acid
Not using the correct Ka value for the acid

Q: How can I improve my understanding of acid-base chemistry?

A: To improve your understanding of acid-base chemistry, try the following:

Practice solving problems involving acid-base chemistry
Read and review relevant texts and resources
Watch video lectures and online tutorials
Participate in online forums and discussions

Conclusion

Calculating the concentration of hydrogen ions in a weak acid solution is an important concept in acid-base chemistry. By understanding the dissociation constant (Ka) and the relationship between the Ka and the concentration of H3O+, you can calculate the concentration of H3O+ in a weak acid solution. Remember to practice solving problems and to review relevant texts and resources to improve your understanding of acid-base chemistry.