Calculate A The Ph of 0.10 M Hno3 Aq Solution

Introduction

The pH of a solution is a measure of its acidity or basicity. It's calculated using the concentration of hydronium ions (H3O+) in the solution. For strong acids like HNO3, the pH can be determined directly from the acid's concentration.

HNO3 is a strong acid, meaning it completely dissociates in water according to the equation:

This complete dissociation means the concentration of H+ ions equals the concentration of HNO3.

How to Calculate pH for HNO3

To calculate the pH of a HNO3 solution:

1. Determine the molarity (M) of the HNO3 solution
2. Calculate the concentration of H+ ions (same as HNO3 concentration for strong acids)
3. Use the pH formula: pH = -log[H+]

The formula used is:

Where [H+] is the concentration of hydrogen ions in moles per liter (M).

Example Calculation

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

1. Given: [HNO3] = 0.10 M
2. Since HNO3 is a strong acid, [H+] = [HNO3] = 0.10 M
3. Calculate pH: pH = -log(0.10)
4. pH = -(-1) = 1.00

The pH of a 0.10 M HNO3 solution is 1.00, indicating a very acidic solution.

Interpreting the Results

The pH scale ranges from 0 to 14, where:

• pH < 7: Acidic solution
• pH = 7: Neutral solution
• pH > 7: Basic solution

A pH of 1.00 indicates a highly acidic solution, which is expected for strong acids like HNO3.

In practical terms, a pH of 1.00 means:

• The solution is highly corrosive
• It can react strongly with bases
• It would turn blue litmus paper red