A chemistry teacher prepares a dilution series for a titration lab. She starts with a 2.4 M HCl solution and needs a final concentration of 0.015 M in a 500 mL volumetric flask. What is the volume (in mL) of the original solution required?

Tue, 05 May 2026 05:31:28 +0000

**A chemistry teacher prepares a dilution series for a titration lab. She starts with a 2.4 M HCl solution and needs a final concentration of 0.015 M in a 500 mL volumetric flask. What is the volume (in mL) of the original solution required?** In modern chemistry classrooms across the United States, preparing precise dilution solutions is a fundamental skill that supports hands-on learning in titration labs. With a growing interest in STEM education and lab-based experimentation, instructors rely on accurate dilution calculations to guide students safely and effectively. This particular scenario—starting with a strong 2.4 M hydrochloric acid solution and diluting it to 0.015 M in a 500 mL volumetric flask—highlights a core challenge in laboratory technique. Understanding the math behind these dilutions not only reinforces key chemistry principles but also prepares students for real-world applications in research, environmental testing, and industrial quality control. A chemistry teacher prepares a dilution series for a titration lab. She starts with a 2.4 M HCl solution and needs a final concentration of 0.015 M in a 500 mL volumetric flask. What is the volume (in mL) of the original solution required? This calculation is essential for establishing consistent, safe experimental conditions. Titration works best when solutions are accurately prepared, ensuring reliable readings and repeatable results—cornerstones of effective science education. The dilution process relies on the principle that concentration and volume are inversely proportional when diluting a solution:
**C₁V₁ = C₂V₂**
Where:
- C₁ = initial concentration (2.4 M)
- V₁ = unknown initial volume (in mL)
- C₂ = final concentration (0.015 M)
- V₂ = final volume (500 mL)