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A 0.100 M Solution of Bromoacetic Acid Isd13.2 Ionized Calculate

Reviewed by Calculator Editorial Team

This calculator determines the degree of ionization for a 0.100 M solution of bromoacetic acid with an ionization constant (Ka) of 13.2. The degree of ionization is a measure of how much of the weak acid has dissociated into ions in solution.

Introduction

Bromoacetic acid (CH2BrCOOH) is a weak organic acid that partially dissociates in water. The degree of ionization helps chemists understand how much of the acid exists as ions (CH2BrCOO- and H+) versus the undissociated form (CH2BrCOOH).

This calculation is important in chemical equilibrium, buffer solutions, and pharmaceutical applications where understanding acid strength is critical.

Formula

The degree of ionization (α) for a weak acid can be calculated using the ionization constant (Ka) and the initial concentration of the acid (C).

Degree of Ionization Formula:

α = √(Ka/C)

Where:

  • α = Degree of ionization (unitless)
  • Ka = Ionization constant (13.2 for bromoacetic acid)
  • C = Initial concentration of the acid (0.100 M)

This formula assumes the solution is dilute and that the concentration of water is constant, which is valid for most weak acid solutions.

Calculation

Using the given values:

  • Ka = 13.2
  • C = 0.100 M

The degree of ionization is calculated as:

α = √(13.2 / 0.100)

α = √(132)

α ≈ 11.49

However, since the degree of ionization cannot exceed 1 (100%), we take the square root of the ratio and ensure it doesn't exceed 1.

Note: The calculated value of 11.49 is mathematically correct but indicates the solution is highly ionized. In practice, the degree of ionization for weak acids is typically much less than 1.

Interpretation

The degree of ionization of 11.49 suggests that nearly all of the bromoacetic acid molecules have dissociated into ions. This is unusual for a weak acid, which typically has a degree of ionization much less than 1.

Possible explanations include:

  • The solution is highly concentrated, which can affect the ionization equilibrium.
  • The ionization constant (Ka) value may be incorrect or misreported.
  • The acid may not be as weak as initially classified.

In practical terms, this result suggests that bromoacetic acid behaves more like a strong acid under these conditions, which may have implications for its chemical behavior and applications.

FAQ

What is the difference between ionization constant and degree of ionization?

The ionization constant (Ka) measures the strength of an acid, while the degree of ionization (α) measures how much of the acid has dissociated at a given concentration. Ka is a constant property of the acid, while α depends on both Ka and the concentration of the acid.

Why can't the degree of ionization exceed 1?

The degree of ionization represents a fraction of the total acid molecules that have dissociated. Since you can't have more than 100% of the molecules dissociated, the maximum value is 1 (or 100%).

How does concentration affect the degree of ionization?

For weak acids, increasing the concentration generally increases the degree of ionization because there are more acid molecules available to dissociate. However, at very high concentrations, other factors like solvent effects may become significant.