What Is The Freezing Point (in $^{\circ} C$) Of A 0.321 M Aqueous Solution Of NaCl?- Enter Your Rounded Answer With 3 Decimal Places.- $K_{f}$ For Water = $1.86^{\circ} C / M$

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What is the Freezing Point of a 0.321 M Aqueous Solution of NaCl?

Understanding the Problem

The problem requires us to find the freezing point of a 0.321 M aqueous solution of NaCl. To solve this, we need to use the concept of freezing-point depression, which is a colligative property that depends on the concentration of the solute particles in the solution.

Colligative Properties and Freezing-Point Depression

Colligative properties are properties of solutions that depend on the concentration of the solute particles, regardless of their identity. Freezing-point depression is one such property, which is the decrease in the freezing point of a solvent due to the presence of a solute. The freezing-point depression is directly proportional to the molality of the solution and the freezing-point depression constant (Kf) of the solvent.

Calculating the Freezing Point

To calculate the freezing point of the solution, we can use the formula:

ΔTf = Kf × m

where ΔTf is the freezing-point depression, Kf is the freezing-point depression constant, and m is the molality of the solution.

Given that the molality of the solution is 0.321 m and the freezing-point depression constant for water is 1.86°C/m, we can plug in the values to get:

ΔTf = 1.86°C/m × 0.321 m ΔTf = 0.597°C

Rounding the Answer

Since the problem asks for the answer with three decimal places, we need to round the freezing-point depression to three decimal places. Therefore, the freezing-point depression is approximately 0.597°C.

Finding the Freezing Point of the Solution

To find the freezing point of the solution, we need to subtract the freezing-point depression from the freezing point of the pure solvent. The freezing point of pure water is 0°C, so we can subtract the freezing-point depression from this value to get:

Tf = 0°C - 0.597°C Tf = -0.597°C

Conclusion

In conclusion, the freezing point of a 0.321 M aqueous solution of NaCl is approximately -0.597°C. This is a result of the freezing-point depression caused by the presence of NaCl particles in the solution.

Understanding the Significance of Freezing-Point Depression

Freezing-point depression is an important concept in chemistry that has significant implications in various fields, including medicine, industry, and environmental science. For example, freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the production of pharmaceuticals and other chemicals.

Applications of Freezing-Point Depression

Freezing-point depression has several applications in various fields, including:

  • Pharmaceuticals: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the production of pharmaceuticals.
  • Industry: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the production of chemicals and other products.
  • Environmental Science: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the study of environmental pollutants.

Conclusion

In conclusion, the freezing point of a 0.321 M aqueous solution of NaCl is approximately -0.597°C. This is a result of the freezing-point depression caused by the presence of NaCl particles in the solution. Freezing-point depression is an important concept in chemistry that has significant implications in various fields, including medicine, industry, and environmental science.
Q&A: Freezing Point of a 0.321 M Aqueous Solution of NaCl

Frequently Asked Questions

We have received several questions from readers regarding the freezing point of a 0.321 M aqueous solution of NaCl. Below are some of the most frequently asked questions and their answers.

Q: What is the freezing point of a 0.321 M aqueous solution of NaCl?

A: The freezing point of a 0.321 M aqueous solution of NaCl is approximately -0.597°C.

Q: What is the freezing-point depression constant (Kf) for water?

A: The freezing-point depression constant (Kf) for water is 1.86°C/m.

Q: How is the freezing point of a solution calculated?

A: The freezing point of a solution is calculated by subtracting the freezing-point depression from the freezing point of the pure solvent. The freezing-point depression is calculated using the formula: ΔTf = Kf × m, where ΔTf is the freezing-point depression, Kf is the freezing-point depression constant, and m is the molality of the solution.

Q: What is the significance of freezing-point depression?

A: Freezing-point depression is an important concept in chemistry that has significant implications in various fields, including medicine, industry, and environmental science. It is used to determine the concentration of solutes in solutions, which is crucial in the production of pharmaceuticals and other chemicals.

Q: What are some applications of freezing-point depression?

A: Some applications of freezing-point depression include:

  • Pharmaceuticals: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the production of pharmaceuticals.
  • Industry: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the production of chemicals and other products.
  • Environmental Science: Freezing-point depression is used to determine the concentration of solutes in solutions, which is crucial in the study of environmental pollutants.

Q: Can you provide more information on the concept of freezing-point depression?

A: Yes, we can provide more information on the concept of freezing-point depression. Freezing-point depression is a colligative property that depends on the concentration of the solute particles in the solution. It is the decrease in the freezing point of a solvent due to the presence of a solute. The freezing-point depression is directly proportional to the molality of the solution and the freezing-point depression constant (Kf) of the solvent.

Q: How is the molality of a solution calculated?

A: The molality of a solution is calculated by dividing the number of moles of the solute by the mass of the solvent in kilograms. The formula for calculating molality is: m = n / m, where m is the molality, n is the number of moles of the solute, and m is the mass of the solvent in kilograms.

Q: Can you provide more information on the freezing-point depression constant (Kf)?

A: Yes, we can provide more information on the freezing-point depression constant (Kf). The freezing-point depression constant (Kf) is a constant that depends on the solvent and is used to calculate the freezing-point depression of a solution. The value of Kf for water is 1.86°C/m.

Conclusion

In conclusion, we hope that this Q&A article has provided you with a better understanding of the freezing point of a 0.321 M aqueous solution of NaCl and the concept of freezing-point depression. If you have any further questions, please do not hesitate to contact us.