A Student Requires 2.00 L Of 0.100 M NH 4 NO 3 0.100 \, \text{M} \, \text{NH}_4\text{NO}_3 0.100 M NH 4 ​ NO 3 ​ From A 1.75 M NH 4 NO 3 1.75 \, \text{M} \, \text{NH}_4\text{NO}_3 1.75 M NH 4 ​ NO 3 ​ Stock Solution. What Is The Correct Way To Prepare The Solution?Use The Formula $M_i V_i = M_f

Introduction

Preparing a diluted solution is a crucial task in various fields, including chemistry, biology, and medicine. It requires attention to detail and a thorough understanding of the underlying principles. In this article, we will guide you through the process of preparing a diluted solution using the formula $M_i V_i = M_f V_f$, where $M_i$ and $V_i$ are the initial molarity and volume of the stock solution, and $M_f$ and $V_f$ are the final molarity and volume of the diluted solution.

Understanding the Problem

A student requires 2.00 L of $0.100 \, \text{M} \, \text{NH}_4\text{NO}_3$ from a $1.75 \, \text{M} \, \text{NH}_4\text{NO}_3$ stock solution. The student needs to determine the correct way to prepare the solution using the given stock solution.

The Formula: $M_i V_i = M_f V_f$

The formula $M_i V_i = M_f V_f$ is a fundamental concept in chemistry that relates the initial and final molarities and volumes of a solution. To prepare a diluted solution, we need to use this formula to calculate the required volume of the stock solution.

Calculating the Required Volume of the Stock Solution

To calculate the required volume of the stock solution, we can rearrange the formula as follows:

$$V_i = \frac{M_f V_f}{M_i}$$

Substituting the given values, we get:

$$V_i = \frac{(0.100 \, \text{M})(2.00 \, \text{L})}{(1.75 \, \text{M})}$$

$$V_i = \frac{0.200 \, \text{M} \cdot \text{L}}{1.75 \, \text{M}}$$

$$V_i = 0.114 \, \text{L}$$

Preparing the Solution

To prepare the solution, the student needs to measure out 0.114 L of the $1.75 \, \text{M} \, \text{NH}_4\text{NO}_3$ stock solution and dilute it to a final volume of 2.00 L using a solvent, such as water.

Tips and Precautions

When preparing a diluted solution, it is essential to follow proper laboratory procedures to ensure accuracy and safety. Here are some tips and precautions to keep in mind:

• Use a clean and dry glassware: Make sure the glassware is free from any contaminants or residues that may affect the accuracy of the measurement.
• Measure the volume accurately: Use a pipette or a burette to measure the required volume of the stock solution.
• Use a solvent that is compatible with the solute: Choose a solvent that is compatible with the solute and will not react with it.
• Label the solution correctly: Label the solution with the correct concentration and volume to avoid any confusion.
• Store the solution properly: Store the solution in a well-ventilated area, away from direct sunlight and heat sources.

Conclusion

Preparing a diluted solution requires attention to detail and a thorough understanding of the underlying principles. By using the formula $M_i V_i = M_f V_f$ and following proper laboratory procedures, you can prepare a diluted solution with accuracy and safety. Remember to always follow proper laboratory procedures and take necessary precautions to ensure the quality and safety of the solution.

Frequently Asked Questions

Q: What is the formula for preparing a diluted solution?

A: The formula for preparing a diluted solution is $M_i V_i = M_f V_f$, where $M_i$ and $V_i$ are the initial molarity and volume of the stock solution, and $M_f$ and $V_f$ are the final molarity and volume of the diluted solution.

Q: How do I calculate the required volume of the stock solution?

A: To calculate the required volume of the stock solution, you can use the formula $V_i = \frac{M_f V_f}{M_i}$.

Q: What are the tips and precautions for preparing a diluted solution?

A: Some of the tips and precautions for preparing a diluted solution include using clean and dry glassware, measuring the volume accurately, using a solvent that is compatible with the solute, labeling the solution correctly, and storing the solution properly.

References

• [1] "Chemistry: An Atoms First Approach" by Steven S. Zumdahl
• [2] "General Chemistry: Principles and Modern Applications" by Linus Pauling
• [3] "The Chemistry of Solutions" by John W. Moore

Additional Resources

• [1] "Preparing Diluted Solutions" by the American Chemical Society
• [2] "Diluted Solutions" by the Royal Society of Chemistry
• [3] "Preparing Solutions" by the National Institute of Standards and Technology
  

Introduction

Preparing a diluted solution is a crucial task in various fields, including chemistry, biology, and medicine. It requires attention to detail and a thorough understanding of the underlying principles. In this article, we will answer some of the most frequently asked questions about preparing a diluted solution.

Q&A

Q: What is the formula for preparing a diluted solution?

A: The formula for preparing a diluted solution is $M_i V_i = M_f V_f$, where $M_i$ and $V_i$ are the initial molarity and volume of the stock solution, and $M_f$ and $V_f$ are the final molarity and volume of the diluted solution.

Q: How do I calculate the required volume of the stock solution?

A: To calculate the required volume of the stock solution, you can use the formula $V_i = \frac{M_f V_f}{M_i}$.

Q: What are the units of measurement for molarity and volume?

A: The units of measurement for molarity are moles per liter (M), and the units of measurement for volume are liters (L).

Q: How do I prepare a diluted solution from a concentrated stock solution?

A: To prepare a diluted solution from a concentrated stock solution, you need to measure out the required volume of the stock solution and dilute it to the final volume using a solvent, such as water.

Q: What are the tips and precautions for preparing a diluted solution?

A: Some of the tips and precautions for preparing a diluted solution include using clean and dry glassware, measuring the volume accurately, using a solvent that is compatible with the solute, labeling the solution correctly, and storing the solution properly.

Q: What are the common mistakes to avoid when preparing a diluted solution?

A: Some of the common mistakes to avoid when preparing a diluted solution include:

• Using contaminated or dirty glassware
• Measuring the volume inaccurately
• Using a solvent that is not compatible with the solute
• Not labeling the solution correctly
• Not storing the solution properly

Q: How do I store a diluted solution?

A: To store a diluted solution, you should:

• Store it in a well-ventilated area, away from direct sunlight and heat sources
• Use a clean and dry container
• Label the solution correctly
• Store it in a cool, dry place

Q: How do I dispose of a diluted solution?

A: To dispose of a diluted solution, you should:

• Follow the guidelines for disposing of chemicals in your institution or laboratory
• Wear protective gear, such as gloves and goggles
• Dispose of the solution in a designated container
• Rinse the container thoroughly with water

Conclusion

Preparing a diluted solution requires attention to detail and a thorough understanding of the underlying principles. By following the formula $M_i V_i = M_f V_f$ and taking necessary precautions, you can prepare a diluted solution with accuracy and safety. Remember to always follow proper laboratory procedures and take necessary precautions to ensure the quality and safety of the solution.

Frequently Asked Questions

Q: What is the formula for preparing a diluted solution?

A: The formula for preparing a diluted solution is $M_i V_i = M_f V_f$, where $M_i$ and $V_i$ are the initial molarity and volume of the stock solution, and $M_f$ and $V_f$ are the final molarity and volume of the diluted solution.

Q: How do I calculate the required volume of the stock solution?

A: To calculate the required volume of the stock solution, you can use the formula $V_i = \frac{M_f V_f}{M_i}$.

Q: What are the tips and precautions for preparing a diluted solution?

A: Some of the tips and precautions for preparing a diluted solution include using clean and dry glassware, measuring the volume accurately, using a solvent that is compatible with the solute, labeling the solution correctly, and storing the solution properly.

References

• [1] "Chemistry: An Atoms First Approach" by Steven S. Zumdahl
• [2] "General Chemistry: Principles and Modern Applications" by Linus Pauling
• [3] "The Chemistry of Solutions" by John W. Moore

Additional Resources

• [1] "Preparing Diluted Solutions" by the American Chemical Society
• [2] "Diluted Solutions" by the Royal Society of Chemistry
• [3] "Preparing Solutions" by the National Institute of Standards and Technology