Preparation of 0.1N H2SO4 Solution
Introduction
Sulfuric acid (H2SO4) is a strong acid widely used in various laboratory applications, including titration, chemical synthesis, and analytical chemistry. To prepare a 0.1N H2SO4 solution, it is essential to understand the concept of normality and the calculations involved.
What is Normality (N)?
Normality (N) is a measure of the number of equivalents of a solute per liter of solution. In the case of sulfuric acid (H2SO4), one equivalent is equal to one mole of H+ ions, which is half of a mole of H2SO4. Therefore, the normality of H2SO4 is half of its molarity.
Calculations for 0.1N H2SO4 Solution
To prepare 0.1N H2SO4 solution, we need to calculate the amount of H2SO4 required to produce 1 liter of solution.
Molarity of H2SO4 = 98.08 g/mol Normality of H2SO4 = ½ × Molarity = 0.5 × 98.08 g/mol = 49.04 g/mol
To prepare 0.1N H2SO4 solution, we need:
49.04 g/mol × 0.1 N = 4.904 g of H2SO4
Preparation of 0.1N H2SO4 Solution
Materials:
- Sulfuric acid (H2SO4)
- Distilled water
- Volumetric flask (1 L)
- Balance
- Pipette
Procedure:
- Weighing: Accurately weigh 4.904 g of H2SO4 using a balance.
- Dissolving: Slowly add the weighed H2SO4 to a volumetric flask while swirling the flask.
- Dilution: Add distilled water to the flask, slowly, while swirling, until the mark is reached (1 L).
- Mixing: Mix the solution thoroughly to ensure complete dissolution of H2SO4.
- Storage: Store the prepared 0.1N H2SO4 solution in a tightly closed container, labeled with the concentration and date of preparation.
Precautions
- Handle sulfuric acid with care, as it is highly corrosive and can cause skin and eye irritation.
- Wear protective gloves, goggles, and lab coats when handling H2SO4.
- In case of accidental spill, wash the affected area with plenty of water and seek medical attention if necessary.
By following these calculations and procedures, you can prepare a 0.1N H2SO4 solution accurately and safely.
