0.1 N H2SO4 Preparation Formula
Introduction
Sulfuric acid (H2SO4) is a strong acid widely used in various industries, including chemical synthesis, pharmaceuticals, and biochemistry. In laboratory settings, a 0.1 N (normal) solution of H2SO4 is commonly used as a reference solution or as a reactant in various analytical and synthesis procedures. In this article, we will provide the preparation formula and guidelines for preparing a 0.1 N H2SO4 solution.
Preparation Formula
To prepare 0.1 N H2SO4, you will need:
Materials:
- Sulfuric acid (H2SO4): concentrated solution (95-98%)
- Distilled water
Preparation Formula:
- Calculate the volume of concentrated H2SO4 required:
- Molecular weight of H2SO4: 98.08 g/mol
- Normality (N) of the desired solution: 0.1 N
- Volume of the desired solution: 1 L (1000 mL)
- Calculate the number of moles of H2SO4 required: 0.1 N x 1000 mL = 10 mmol
- Calculate the volume of concentrated H2SO4 required: 10 mmol / (95% x 18 mol/L) ≈ 6.04 mL
- Add the calculated volume of concentrated H2SO4 to a 1-L volumetric flask.
- Add distilled water to the flask to a total volume of 1000 mL.
- Mix the solution well to ensure complete dissolution of the acid.
- Label and store the solution in a clean, dark glass bottle.
Precautions and Safety Considerations
- Always handle concentrated sulfuric acid with caution, as it is highly corrosive and can cause severe burns.
- Wear protective gear, including gloves, goggles, and a lab coat.
- Perform the preparation in a well-ventilated area, away from heat sources and open flames.
- Follow proper disposal procedures for the prepared solution.
Conclusion
By following the preparation formula and guidelines outlined in this article, you can prepare a 0.1 N H2SO4 solution with accuracy and safety. Remember to handle the concentrated acid with care and follow proper laboratory protocols to ensure a safe and successful preparation.
