Calculate Ph of 0.05m Hio3

Introduction

The pH of a solution is a measure of its acidity or alkalinity. For the weak acid HIO3 (iodic acid), we can calculate its pH using the concept of acid dissociation constant (Ka). This guide will walk you through the process of calculating the pH of a 0.05M HIO3 solution.

How to Calculate

To calculate the pH of a 0.05M HIO3 solution, follow these steps:

1. Determine the dissociation constant (Ka) of HIO3. For this calculation, we'll use Ka = 1.3 × 10⁻2.
2. Set up the equilibrium expression for the dissociation of HIO3.
3. Solve for the concentration of H⁺ ions using the quadratic formula.
4. Calculate the pH from the concentration of H⁺ ions.

Formula

The key formula for calculating the pH of a weak acid is:

Where:

• pH is the measure of acidity
• [H⁺] is the concentration of hydrogen ions
• Ka is the acid dissociation constant (1.3 × 10⁻2 for HIO3)
• [HIO3] is the concentration of iodic acid (0.05M in this case)

Example Calculation

Let's calculate the pH of a 0.05M HIO3 solution using the formula:

So, the pH of a 0.05M HIO3 solution is approximately 2.09.

Interpreting Results

A pH of 2.09 indicates that the solution is acidic. This is expected since HIO3 is a weak acid. The result shows that the solution is not strongly acidic, which aligns with the weak acid nature of HIO3.