0.1 N NaOH Solution Preparation
Introduction
Sodium hydroxide (NaOH) is a strong base commonly used in various laboratory applications, including titrations, pH adjustments, and cleaning purposes. A 0.1 N NaOH solution is a common concentration used in many laboratory procedures. In this article, we will guide you through the preparation of a 0.1 N NaOH solution.
Materials
- Sodium hydroxide (NaOH) pellets
- Distilled water
- Laboratory balance
- Volumetric flask (1000 mL)
Preparation
Step 1: Calculate the Amount of NaOH Required
To prepare a 0.1 N NaOH solution, you need to calculate the amount of NaOH required. The molecular weight of NaOH is 40.00 g/mol. A 0.1 N solution means that the solution contains 0.1 moles of NaOH per liter of solution.
Calculation:
Moles of NaOH required = Normality x Volume (in liters) = 0.1 mol/L x 1 L = 0.1 mol
Mass of NaOH required = Moles x Molecular weight = 0.1 mol x 40.00 g/mol = 4.00 g
Step 2: Weigh the NaOH Pellets
Using a laboratory balance, accurately weigh 4.00 g of sodium hydroxide pellets.
Step 3: Dissolve the NaOH Pellets
Place the weighed NaOH pellets in a 1000 mL volumetric flask. Gradually add distilled water to the flask while stirring until the NaOH pellets are completely dissolved.
Step 4: Dilute to the Mark
Once the NaOH pellets are dissolved, add distilled water to the flask until it reaches the 1000 mL mark.
Step 5: Mix Well
Mix the solution well to ensure that the NaOH is evenly distributed throughout the solution.
Preparation Complete
Your 0.1 N NaOH solution is now ready to use. Store the solution in a clean, labeled container and keep it away from direct sunlight and heat.
Safety Precautions
- Wear protective gloves, goggles, and a lab coat when handling NaOH.
- Handle NaOH with care, as it can cause skin and eye irritation.
- Dispose of any waste NaOH solution according to local regulations and guidelines.
By following these simple steps, you can prepare a 0.1 N NaOH solution for your laboratory needs.
