The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. The pH of the solution is

The correct answer is 1.88

Concept:-

• Degree of Ionization: It is the fraction or percentage of a substance that has been ionized when introduced into a solution. In the context of acids, this refers to how much of the original acid has ionized in the solution.
• α = [H⁺]/[HA_initial]
• pH: pH is a measure of the hydrogen ion concentration in a solution. It provides insights into the acidity or alkalinity of a solution. The pH is calculated using the formula:

pH = -log[H+]

where [H+] is the concentration of hydrogen ions in the solution.

• Acid Ionization: When acids ionize in solution, they donate a proton (H+) to the solution, ultimately increasing the [H+] and lowering the pH. The concentration of H+ ions can be calculated by multiplying the original concentration of the acid by its degree of ionization.

Explanation:-

You are given that the degree of ionization (α) of a 0.1 M bromoacetic acid solution is 0.132.

This means that 0.132 moles of the bromoacetic acid have ionized for every 1 mole of the initial acid.

Now, we can calculate the pH using the formula for weak acid dissociation:

So, we have:

[H+] = α x [HA_initial] = 0.132 x 0.1 M = 0.0132 M

Now, calculate pH:

pH = -log₁₀(0.0132) ≈ 1.88

So, the pH of the solution is approximately 1.88.

The correct answer is 2) 1.88.