Calculate Ph of 0.001 M Naoh

Introduction

The pH of a solution is a measure of its acidity or alkalinity, defined as the negative logarithm (base 10) of the hydrogen ion concentration ([H⁺]). For strong bases like NaOH, the pH can be calculated directly from the concentration of the base.

When NaOH dissolves in water, it completely dissociates according to the equation:

This means that every mole of NaOH that dissolves produces one mole of hydroxide ions (OH⁻). The concentration of hydroxide ions is equal to the concentration of NaOH in the solution.

How to Calculate pH

The pH of a strong base solution can be calculated using the following formula:

Where:

• [OH⁻] is the concentration of hydroxide ions in moles per liter (M)
• log₁₀ is the base-10 logarithm

For a 0.001 M NaOH solution:

1. Determine the concentration of hydroxide ions: [OH⁻] = 0.001 M
2. Calculate the logarithm of the hydroxide ion concentration: log₁₀(0.001) = -3
3. Add 14 to the logarithm: pH = 14 + (-3) = 11

Example Calculation

Let's calculate the pH of a 0.001 M NaOH solution step by step:

1. Given: [NaOH] = 0.001 M
2. Since NaOH is a strong base, [OH⁻] = [NaOH] = 0.001 M
3. Calculate log₁₀(0.001) = -3
4. Apply the pH formula: pH = 14 + (-3) = 11

The pH of a 0.001 M NaOH solution is 11.

Interpreting Results

A pH of 11 indicates a strongly alkaline solution. This means:

• The solution contains a high concentration of hydroxide ions (OH⁻)
• It will react strongly with acids
• It may cause skin and eye irritation
• It can corrode metals

When working with NaOH solutions, always handle them with care and wear appropriate protective equipment.