0.1 M Sodium Hydroxide Preparation and Standardization
Introduction
Sodium hydroxide (NaOH) is a strong base commonly used in various chemical reactions, including titrations and neutralization reactions. In analytical chemistry, it is essential to have a standardized solution of sodium hydroxide to ensure accurate results. This article outlines the preparation and standardization of a 0.1 M sodium hydroxide solution.
Preparation of 0.1 M Sodium Hydroxide Solution
To prepare a 0.1 M sodium hydroxide solution, you will need the following materials:
- Sodium hydroxide pellets (NaOH)
- Distilled water
- A weighing balance
- A beaker or volumetric flask
Procedure
- Weighing: Weigh 4.0 grams of sodium hydroxide pellets using a weighing balance.
- Dissolution: Carefully add the weighed sodium hydroxide pellets to a beaker or volumetric flask containing approximately 500 mL of distilled water. Wear protective gloves and goggles.
- Dissolve: Stir the mixture until the sodium hydroxide pellets are completely dissolved.
- Dilution: Dilute the solution to a final volume of 1 liter using distilled water.
- Mixing: Mix the solution thoroughly to ensure homogeneity.
Standardization of 0.1 M Sodium Hydroxide Solution
To standardize the prepared 0.1 M sodium hydroxide solution, you will need a primary standard acid, such as potassium hydrogen phthalate (KHP).
Materials
- Potassium hydrogen phthalate (KHP)
- Distilled water
- A burette
- A conical flask
- Phenolphthalein indicator
Procedure
- Weighing: Weigh approximately 0.5 grams of potassium hydrogen phthalate using a weighing balance.
- Dissolution: Dissolve the weighed potassium hydrogen phthalate in approximately 50 mL of distilled water in a conical flask.
- Titration: Add a few drops of phenolphthalein indicator to the potassium hydrogen phthalate solution.
- Titration: Titrate the potassium hydrogen phthalate solution with the prepared 0.1 M sodium hydroxide solution using a burette until the color changes from colorless to pink.
- Calculation: Calculate the exact molarity of the sodium hydroxide solution using the following formula:
Molarity (M) = (Weight of KHP (g) / Molar mass of KHP (g/mol)) / Volume of NaOH solution (L)
Result
The prepared 0.1 M sodium hydroxide solution is now standardized and ready for use in various chemical reactions and titrations.
Conclusion
In this article, we have outlined the preparation and standardization of a 0.1 M sodium hydroxide solution. The prepared solution is essential in analytical chemistry for various applications, including titrations and neutralization reactions. By following this procedure, you can ensure accurate results in your chemical experiments.
