Calculate A The Ph of 0.10 M Hno3 Aq Solution

Introduction

The pH of a solution is a measure of its acidity or alkalinity. It's calculated using the concentration of hydrogen ions (H⁺) in the solution. For strong acids like HNO3, the pH can be directly calculated from the concentration of the acid.

Nitric acid (HNO3) is a strong acid that completely dissociates in water according to the equation:

This complete dissociation means that the concentration of H⁺ ions is equal to the concentration of HNO3 in the solution.

How to Calculate pH

The pH of a solution is calculated using the following formula:

For a strong acid like HNO3, the concentration of H⁺ ions is equal to the concentration of the acid. Therefore, for a 0.10 M HNO3 solution:

Using a calculator or logarithm tables, you can compute the pH value.

Example Calculation

Let's calculate the pH of a 0.10 M HNO3 solution step by step:

1. Identify the concentration of H⁺ ions: [H⁺] = 0.10 M
2. Take the negative logarithm (base 10) of the H⁺ concentration: pH = -log₁₀(0.10)
3. Calculate the logarithm: log₁₀(0.10) ≈ -1.0000
4. Take the negative of this value: pH ≈ 1.0000

Therefore, the pH of a 0.10 M HNO3 solution is approximately 1.00.

Interpreting the Results

A pH of 1.00 indicates a very acidic solution. This is consistent with the properties of strong acids like HNO3. The pH scale ranges from 0 to 14, with values below 7 indicating acidity, 7 being neutral, and values above 7 indicating alkalinity.

Understanding the pH of a solution is crucial in various scientific and industrial applications, including:

• Chemical manufacturing
• Environmental monitoring
• Food and beverage production
• Water treatment