Calculate Ph of 0.01 Molar Solution of Sodium Hydroxide

Introduction

The pH scale measures how acidic or basic a solution is, with values ranging from 0 (very acidic) to 14 (very basic). A pH of 7 is neutral. Sodium hydroxide (NaOH) is a strong base that dissociates completely in water, making it ideal for pH calculations.

When NaOH dissolves in water, it forms hydroxide ions (OH⁻), which increase the concentration of these ions in the solution. The pH is then calculated using the concentration of hydroxide ions.

How to Calculate

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

1. Determine the molar concentration of hydroxide ions (OH⁻). For a 0.01 molar solution of NaOH, the concentration of OH⁻ is equal to the concentration of NaOH because NaOH completely dissociates in water.
2. Calculate the pOH using the formula: pOH = -log[OH⁻].
3. Convert pOH to pH using the relationship: pH = 14 - pOH.

Example Calculation

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

1. The concentration of OH⁻ is 0.01 mol/L.
2. Calculate pOH: pOH = -log(0.01) = 2.
3. Calculate pH: pH = 14 - 2 = 12.

The pH of a 0.01 molar solution of NaOH is 12, indicating it is strongly basic.

Interpretation

A pH of 12 for a 0.01 molar solution of NaOH means the solution is highly alkaline. This is expected because NaOH is a strong base that completely dissociates in water, releasing a large number of hydroxide ions.

In practical terms, this solution would feel slippery to the touch and would react strongly with acids. It's important to handle such solutions with care to avoid skin irritation or chemical burns.