Preparation Calculation of 0.1 N NaOH Solution
Introduction
Sodium hydroxide (NaOH) is a strong base commonly used in various laboratory applications, including analytical chemistry, biochemistry, and pharmaceutical industries. In many experiments, a specific concentration of NaOH solution is required, and 0.1 N NaOH is one of the most frequently used concentrations. In this article, we will discuss the preparation calculation of 0.1 N NaOH solution.
What is Normality (N)?
Normality (N) is a measure of the concentration of a solution, defined as the number of equivalents of the solute per liter of solution. One equivalent is the amount of substance that reacts with one mole of hydrogen ion (H+) or hydroxide ion (OH-). For strong bases like NaOH, one equivalent is equal to one mole.
Preparation of 0.1 N NaOH Solution
To prepare 0.1 N NaOH solution, we need to calculate the amount of NaOH required to make 1 liter of solution. The molar mass of NaOH is 40 g/mol, and we want to prepare 1 liter (1000 mL) of solution.
Calculation:
- Calculate the number of moles of NaOH required:
1 mole NaOH = 40 g NaOH
Number of moles = Normality x Volume (L) = 0.1 N x 1 L = 0.1 mole
- Calculate the mass of NaOH required:
Mass of NaOH = Number of moles x Molar mass = 0.1 mole x 40 g/mol = 4 g
Preparation Procedure:
- Weigh 4 g of NaOH pellets in a clean and dry container.
- Gradually add distilled water to the container while stirring until the NaOH pellets are completely dissolved.
- Transfer the solution to a 1-liter volumetric flask.
- Add distilled water to the flask until the volume reaches 1 liter.
- Mix the solution well and store it in a clean and labeled container.
Conclusion
By following the calculation and procedure outlined above, you can prepare 0.1 N NaOH solution accurately and easily. Remember to handle NaOH with caution, as it is a strong base that can cause skin and eye irritation. Always wear protective gloves and eyewear when handling NaOH and its solutions.
