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Calculate H+ and Ph of 0.010 M Hno3

Reviewed by Calculator Editorial Team

This calculator determines the hydrogen ion concentration (H+) and pH of a 0.010 M nitric acid (HNO3) solution. Nitric acid is a strong acid that completely dissociates in water, making it ideal for demonstrating acid-base chemistry principles.

Introduction

When nitric acid (HNO3) dissolves in water, it dissociates completely according to the equation:

Dissociation Equation

HNO3(aq) → H+(aq) + NO3-(aq)

For a 0.010 M HNO3 solution, the concentration of H+ ions is equal to the concentration of HNO3 because the acid is 100% ionized. The pH is then calculated using the pH formula for strong acids.

Calculation Method

The calculation follows these steps:

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

Key Formulas

[H+] = M (for strong acids)

pH = -log[H+]

For our specific case of 0.010 M HNO3:

  1. [H+] = 0.010 M
  2. pH = -log(0.010) = 2.00

Worked Example

Let's calculate the H+ concentration and pH for a 0.010 M HNO3 solution:

  1. Given: Molarity of HNO3 = 0.010 M
  2. Since HNO3 is a strong acid, [H+] = 0.010 M
  3. Calculate pH: pH = -log(0.010) = 2.00

Result Interpretation

A pH of 2.00 indicates a strongly acidic solution, which is characteristic of dilute nitric acid. This solution would turn blue litmus paper red and react vigorously with bases.

FAQ

Why does HNO3 have the same concentration as H+?

HNO3 is a strong acid that completely dissociates in water, so the concentration of H+ ions equals the concentration of HNO3.

What is the pH range for strong acids?

Strong acids typically have pH values between 0 and 1, with more dilute solutions approaching pH 0.

How does temperature affect the pH of HNO3 solutions?

Temperature has a negligible effect on the pH of strong acid solutions because the dissociation is complete and the equilibrium constant is very large.