Preparation of 0.1 N AgNO3 in 100 mL
Introduction
Silver nitrate (AgNO3) is a commonly used chemical in various laboratory applications, including analytical chemistry, biochemistry, and molecular biology. In this article, we will outline the preparation of 0.1 N (normal) AgNO3 solution in 100 mL.
Materials Needed
- Silver nitrate (AgNO3) crystals
- Distilled water
- A 100 mL volumetric flask
- A balance or scale
- A pipette or measuring cylinder
Preparation
Step 1: Calculate the Amount of AgNO3 Required
To prepare 0.1 N AgNO3 solution, we need to calculate the amount of AgNO3 required. The molecular weight of AgNO3 is 169.87 g/mol. Since we want to prepare 0.1 N solution, we need to calculate the amount of AgNO3 required for 100 mL of solution.
Molarity (M) = Number of moles of solute per liter of solution
For 0.1 N AgNO3 solution, we need to calculate the number of moles of AgNO3 required for 100 mL (0.1 L) of solution.
Number of moles = Molarity x Volume (L)
Number of moles = 0.1 x 0.1 = 0.01 moles
Weight of AgNO3 required = Number of moles x Molecular weight
Weight of AgNO3 required = 0.01 moles x 169.87 g/mol = 1.6987 g
Step 2: Weigh AgNO3
Using a balance or scale, weigh out approximately 1.6987 g of AgNO3 crystals.
Step 3: Transfer AgNO3 to Volumetric Flask
Transfer the weighed AgNO3 crystals to a 100 mL volumetric flask.
Step 4: Add Distilled Water
Add distilled water to the volumetric flask until the volume reaches 100 mL. Mix the solution well to dissolve the AgNO3 crystals completely.
Step 5: Verify the Solution
Verify that the solution is clear and free of any undissolved particles. If necessary, filter the solution through a filter paper or a 0.2 μm membrane filter to remove any impurities.
Conclusion
The preparation of 0.1 N AgNO3 solution in 100 mL is now complete. This solution can be used in various laboratory applications, including analytical chemistry, biochemistry, and molecular biology. Always handle AgNO3 with caution, as it can cause skin and eye irritation.
