Determining the pH of a Nitric Acid Solution

Determining the pH of a Nitric Acid Solution

Understanding the pH of a solution is crucial for many applications, from water treatment to laboratory experiments. This article will guide you through calculating the pH of a 7602 mL solution containing 1.2 grams of nitric acid (HNO3).

Concepts and Terminology

The pH of a solution is a measure of the concentration of hydronium ions ([H3O ]) and is defined by the equation:

pH -log[H3O ]

Nitric acid (HNO3) is a strong acid, which means it dissociates completely in water to produce hydronium ions and nitrate ions:

HNO3 H2O → H3O NO3-

Therefore, for every mole of HNO3 that dissociates, one mole of H3O is produced.

Calculation Steps

Convert the mass of nitric acid to moles:

Given: 1.2 grams of Nitric acid

Molar mass of HNO3 63.01 g/mol

Calculating moles:

1.2 g HNO3 × (1 mole HNO3 / 63.01 g HNO3) 0.019 moles HNO3

Convert volume from milliliters to liters:

Given: 7602 mL of solution

7602 mL × (1 L / 1000 mL) 7.602 L

Calculate the molarity of nitric acid:

Molarity (M) is defined as:

M moles of solute / liters of solution

Molarity of HNO3 0.019 moles / 7.602 L 0.0025 M

Therefore, the concentration of H3O is also 0.0025 M.

Calculate the pH of the solution:

Using the pH equation:

pH -log[H3O ]

pH -log(0.0025) ≈ 2.6

Conclusion

By following these steps, we determined that the pH of a 7602 mL solution containing 1.2 grams of nitric acid is 2.6. This calculation is essential for both educational and practical applications, ensuring that the solution's acidity is accurately understood.

Related Keywords

pH nitric acid molarity