Calculate Ph of 0.01 Solution of Sodium Hydroxide

Introduction

The pH of a solution is a measure of its acidity or basicity. For a solution of sodium hydroxide (NaOH), which is a strong base, the pH can be calculated using the concentration of hydroxide ions (OH⁻) in the solution.

Sodium hydroxide is a common strong base used in various chemical processes. When it dissolves in water, it completely dissociates into sodium ions (Na⁺) and hydroxide ions (OH⁻). The concentration of hydroxide ions determines the pH of the solution.

How to Calculate pH

The pH of a solution can be calculated using the following steps:

1. Determine the concentration of hydroxide ions (OH⁻) in the solution.
2. Use the pOH formula: pOH = -log[OH⁻]
3. Calculate the pH using the relationship between pH and pOH: pH = 14 - pOH

For a 0.01 molar solution of sodium hydroxide, the concentration of hydroxide ions is 0.01 mol/L.

Example Calculation

Let's calculate the pH of a 0.01 molar solution of sodium hydroxide:

1. Given: [OH⁻] = 0.01 mol/L
2. Calculate pOH: pOH = -log(0.01) = 2
3. Calculate pH: pH = 14 - pOH = 14 - 2 = 12

The pH of a 0.01 molar solution of sodium hydroxide is 12.

Interpreting Results

A pH of 12 indicates a strongly basic solution. This means the solution has a high concentration of hydroxide ions (OH⁻) and will react strongly with acids. The solution will feel slippery to the touch and will turn red litmus paper blue.

In practical terms, a pH of 12 is characteristic of solutions used in cleaning, as a strong base, sodium hydroxide is effective at breaking down grease and organic materials.