Preparation of 0.1M H2SO4 Solution for 1000mL
Introduction
Sulfuric acid (H2SO4) is a strong acid widely used in various laboratory applications, including titrations, acidic reactions, and as an electrolyte. In this article, we will guide you through the preparation of a 0.1M H2SO4 solution for 1000mL.
Materials Required
- Sulfuric acid (H2SO4) - 98% (concentrated)
- Distilled water
- Volumetric flask (1000mL)
- Pipette or measuring cylinder
Preparation of 0.1M H2SO4 Solution
To prepare a 0.1M H2SO4 solution, you will need to dilute the concentrated sulfuric acid with distilled water. Follow the steps below:
Step 1: Calculate the Volume of H2SO4 Required
Molarity (M) is defined as the number of moles of solute per liter of solution. To prepare a 0.1M H2SO4 solution, you need to calculate the volume of H2SO4 required.
Molarity of H2SO4 = 0.1 M Molecular weight of H2SO4 = 98.08 g/mol
Volume of H2SO4 required = (Molarity x Molecular weight) / Concentration of H2SO4 = (0.1 M x 98.08 g/mol) / 18M (concentrated H2SO4) = 5.45 mL
Step 2: Measure the Volume of H2SO4
Using a pipette or measuring cylinder, measure out 5.45 mL of concentrated H2SO4.
Step 3: Add Distilled Water
Add distilled water to the volumetric flask until the volume reaches 1000mL.
Step 4: Mix Well
Mix the solution well to ensure the acid is fully dissolved.
Precautions
- Always handle sulfuric acid with care, as it is a strong acid and can cause severe burns and damage to skin and eyes.
- Wear protective gloves, goggles, and lab coats when handling H2SO4.
- Ensure the work area is well-ventilated, and avoid inhaling the vapor.
Verification
To verify the concentration of the prepared H2SO4 solution, you can perform a titration reaction with a strong base, such as sodium hydroxide (NaOH).
By following these steps, you can successfully prepare a 0.1M H2SO4 solution for 1000mL. Remember to handle the acid with care and take necessary precautions to avoid accidents.
