How to Dilute a 10% Solution to 0.05%: A Comprehensive Guide

Whether you are a chemistry student or a professional handling chemical solutions, occasionally you might encounter the need to dilute a concentrated solution to achieve a specific concentration. This guide will walk you through a step-by-step process to convert 16 ounces of a 10% solution to a 0.05% solution. We will use the dilution formula which is commonly known as the dilution equation.

Understanding the Dilution Equation

The basic principle behind diluting a solution is to maintain the amount of solute while changing the solution's volume. The dilution equation is:

C1V1 C2V2

Where:

C1 initial concentration (10% in this case) V1 initial volume (16 ounces) C2 final concentration (0.05%) V2 final volume (unknown)

This equation allows us to find the final volume of the solution after dilution, which is essential for calculating how much water we need to add.

Step-by-Step Process to Dilute the Solution

Convert Concentrations to Decimals: C1 10% → 0.10 C2 0.05% → 0.0005 Substitute Known Values into the Equation:

Given the equation:

0.10 × 16 0.0005 × V2

Solve for V2: First, calculate the left side: 1.6 0.0005 × V2 Then, divide both sides by 0.0005: V2 1.6 / 0.0005 3200 ounces Calculate How Much Water to Add:

To determine how much water to add:

Water to add V2 - V1 3200 ounces - 16 ounces 3184 ounces

Conclusion

By following the steps mentioned above, you will dilute 16 ounces of a 10% solution to a 0.05% solution by adding 3184 ounces of water. This process can be generalized to any concentration and volume conversion using the dilution formula.

Additional Considerations

Often, the dilution formula is expressed as:

M1V1 M2V2

This formula is mathematically equivalent but can be used with any concentration units (e.g., %, PPB, PPM) and any volume units (e.g., ml, liters, ounces, gallons) as long as the units are consistent on both sides of the equation. This flexibility makes the formula versatile for various applications in chemistry and related fields.

FAQs

What is the total volume of the diluted solution?

The total volume of the diluted solution is 3200 ounces, which is derived from the equation as explained above. This volume includes the initial 16 ounces of the original solution and the water added.

Can I use this formula for other concentration and volume ratios?

Yes, the dilution formula can be applied to any concentration and volume ratios as long as you use the same units throughout the calculation. The key is to ensure that the concentration and volume units are consistent.

How can I dilute a specific volume to a certain concentration?

To dilute a specific volume of a solution to achieve a desired concentration, you can rearrange the dilution formula to solve for the initial volume (V1) or the final volume (V2) as needed.

Final Thoughts

Dilution is a fundamental concept in chemistry and related fields. Understanding and correctly applying the dilution formula can save time and ensure accurate results in your experiments or chemical processes. Always double-check your calculations to avoid errors and ensure precision in your work.