Calculate Molarity of 0.001m Nacl Solution Diluted From 1m Solumtio

Introduction

Dilution is a common laboratory technique used to prepare solutions of lower concentration. When you dilute a solution, you add more solvent to the existing solution, which decreases the concentration of the solute. The key to successful dilution is understanding the relationship between the initial and final concentrations and volumes.

In this guide, we'll focus on diluting a 1M NaCl solution to achieve a 0.001M solution. We'll walk through the dilution formula, provide a worked example, and answer common questions about the process.

Dilution Formula

The molarity of a solution after dilution can be calculated using the following formula:

This formula is based on the principle of mass conservation, which states that the amount of solute remains the same before and after dilution. The product of molarity and volume for the initial solution must equal the product of molarity and volume for the final solution.

Worked Example

Let's walk through an example to illustrate how to calculate the molarity of a 0.001M NaCl solution diluted from a 1M solution.

Example Problem

You have 100 mL of a 1M NaCl solution. You want to dilute this solution to a final volume of 1000 mL with water. What will be the molarity of the final solution?

Solution

1. Convert the initial and final volumes to liters:
   • Initial volume (V₁) = 100 mL = 0.1 L
   • Final volume (V₂) = 1000 mL = 1.0 L
2. Use the dilution formula to solve for the final molarity (M₂):

   M₁V₁ = M₂V₂

   (1 M)(0.1 L) = M₂(1.0 L)

   0.1 M·L = M₂·L

   M₂ = 0.1 M

3. The final molarity of the solution is 0.1 M.

This example shows that diluting a 1M NaCl solution to a final volume of 10 times the initial volume results in a 0.1M solution. If you want to achieve a 0.001M solution, you would need to dilute the initial solution to a much larger final volume.