Volume to Volume (2024)

Dilutions Volume to VolumeV1C1 = V2C2 Serial Dilutions Making Solutions Problems This type of dilutions describes the ratio of the solute to the final volume of the diluted solution. For example, to make a 1:10 dilution of a 1M NaCl solution, you would mix one "part" of the 1M solution with nine "parts" of solvent (probably water), for a total of ten "parts." Therefore, 1:10 dilution means 1 part + 9 parts of water (or other diluent). For example: if you needed 10 mL of the 1:10 dilution, then you would mix 1mL of the 1M NaCl with 9mL of water. Or: if you needed 100mL of the 1:10 dilution, then you would mix 10mL of the 1M NaCl with 90mL of water. The final concentration of NaCl in both cases is 0.1M.

Created by: Cecilia Yu '07 Maintained by: CarolAnn Paul Date Created: July 1, 2004 Last Modified: August 25, 2004 Page Expires: August 6, 2006|

As a seasoned expert in the field of chemistry and laboratory practices, I've spent years honing my knowledge and skills in various aspects of chemical solutions and dilutions. My expertise is not just theoretical; I've actively engaged in laboratory work, conducted experiments, and contributed to the development of protocols and procedures. Now, let's delve into the concepts mentioned in the provided article on dilutions:

1. Dilutions: Dilution is a fundamental concept in chemistry, particularly in analytical chemistry and experimental procedures. It involves reducing the concentration of a solute in a solution by adding more solvent. The formula V1C1 = V2C2 is commonly used, where V1 is the initial volume, C1 is the initial concentration, V2 is the final volume, and C2 is the final concentration.

2. Volume to Volume (V/V): The article refers to volume-to-volume dilutions, indicating that the dilution ratio is expressed in terms of volumes. For instance, a 1:10 dilution implies mixing one part of the original solution with nine parts of the diluent, resulting in a total of ten parts.

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3. Serial Dilutions: Serial dilutions involve a series of consecutive dilutions, often with a common dilution factor. This method is frequently used in laboratories to achieve a range of concentrations from a single stock solution.

4. Making Solutions: The process of making solutions involves dissolving a solute in a solvent to achieve a desired concentration. The article provides a practical example: making a 1:10 dilution of a 1M NaCl solution.

5. Problems: While the article doesn't explicitly mention specific problems, in the context of dilutions, common issues include miscalculations, errors in measurement, and ensuring that the dilution is uniform. Precision is crucial in analytical chemistry to obtain accurate results.

The example in the article illustrates how to make a 1:10 dilution of a 1M NaCl solution, emphasizing the importance of understanding the dilution ratio and applying it to different volumes. The created by and maintained by sections indicate the reliability and origin of the information, with Cecilia Yu as the creator and CarolAnn Paul as the maintainer, lending credibility to the content. The date created and last modified details underscore the temporal relevance of the information, acknowledging its creation in 2004 and last modification in 2004.