Which Solution Has The Highest Boiling Point?1) 1.0 M K N O 3 1.0 \, M \, KNO_3 1.0 M K N O 3 ​ 2) 2.0 M K N O 3 2.0 \, M \, KNO_3 2.0 M K N O 3 ​ 3) 1.0 M C A ( N O 3 ) 2 1.0 \, M \, Ca(NO_3)_2 1.0 M C A ( N O 3 ​ ) 2 ​ 4) 2.0 M C A ( N O 3 ) 2 2.0 \, M \, Ca(NO_3)_2 2.0 M C A ( N O 3 ​ ) 2 ​

Introduction

In chemistry, the boiling point of a solution is a critical property that depends on various factors, including the concentration of the solute, the type of solute, and the properties of the solvent. In this article, we will explore which solution has the highest boiling point among four given options: $1.0 \, M \, KNO_3$, $2.0 \, M \, KNO_3$, $1.0 \, M \, Ca(NO_3)_2$, and $2.0 \, M \, Ca(NO_3)_2$. We will analyze the boiling points of these solutions using the principles of colligative properties and the properties of the solutes.

Colligative Properties

Colligative properties are properties of a solution that depend on the concentration of the solute particles, regardless of their identity. The boiling point elevation is a colligative property that is directly proportional to the concentration of the solute particles. The boiling point elevation is calculated using the formula:

ΔTb = Kb * m

where ΔTb is the boiling point elevation, Kb is the boiling point elevation constant, and m is the molality of the solution.

Boiling Point Elevation of KNO3 Solutions

The boiling point elevation of a KNO3 solution depends on the concentration of the KNO3 particles. Since KNO3 is a strong electrolyte, it completely dissociates into K+ and NO3- ions in water. Therefore, a 1.0 M KNO3 solution contains 2.0 M K+ and NO3- ions.

The boiling point elevation of a 1.0 M KNO3 solution is:

ΔTb = Kb * m = 0.51 K/m * 2.0 M = 1.02 K

The boiling point elevation of a 2.0 M KNO3 solution is:

ΔTb = Kb * m = 0.51 K/m * 4.0 M = 2.04 K

Boiling Point Elevation of Ca(NO3)2 Solutions

The boiling point elevation of a Ca(NO3)2 solution also depends on the concentration of the Ca(NO3)2 particles. Since Ca(NO3)2 is a strong electrolyte, it completely dissociates into Ca2+ and 2NO3- ions in water. Therefore, a 1.0 M Ca(NO3)2 solution contains 1.0 M Ca2+ and 2.0 M NO3- ions.

The boiling point elevation of a 1.0 M Ca(NO3)2 solution is:

ΔTb = Kb * m = 0.51 K/m * 3.0 M = 1.53 K

The boiling point elevation of a 2.0 M Ca(NO3)2 solution is:

ΔTb = Kb * m = 0.51 K/m * 6.0 M = 3.06 K

Comparison of Boiling Point Elevations

The boiling point elevations of the four solutions are:

• 1.0 M KNO3: 1.02 K
• 2.0 M KNO3: 2.04 K
• 1.0 M Ca(NO3)2: 1.53 K
• 2.0 M Ca(NO3)2: 3.06 K

The solution with the highest boiling point elevation is the 2.0 M Ca(NO3)2 solution, which has a boiling point elevation of 3.06 K.

Conclusion

In conclusion, the solution with the highest boiling point is the 2.0 M Ca(NO3)2 solution. This is because Ca(NO3)2 is a strong electrolyte that completely dissociates into Ca2+ and 2NO3- ions in water, resulting in a higher concentration of solute particles and a higher boiling point elevation. The boiling point elevation of a solution is a critical property that depends on the concentration of the solute particles and the properties of the solvent. Understanding the boiling point elevation of a solution is essential in various applications, including chemical engineering, pharmaceuticals, and food processing.

References

• Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
• Chang, R. (2010). Physical chemistry for the biosciences. University Science Books.
• Levine, I. N. (2014). Physical chemistry. McGraw-Hill Education.

Table of Contents

1. Introduction
2. Colligative Properties
3. Boiling Point Elevation of KNO3 Solutions
4. Boiling Point Elevation of Ca(NO3)2 Solutions
5. Comparison of Boiling Point Elevations
6. Conclusion
7. References
8. Table of Contents
   Q&A: Boiling Point Elevation of Solutions =============================================

Introduction

In our previous article, we explored the boiling point elevation of solutions and determined that the 2.0 M Ca(NO3)2 solution has the highest boiling point elevation. In this article, we will answer some frequently asked questions about boiling point elevation and provide additional information to help you better understand this concept.

Q: What is boiling point elevation?

A: Boiling point elevation is the increase in the boiling point of a solvent caused by the presence of a solute. It is a colligative property that depends on the concentration of the solute particles.

Q: Why does boiling point elevation occur?

A: Boiling point elevation occurs because the presence of a solute in a solvent disrupts the formation of hydrogen bonds between the solvent molecules. This disruption requires more energy to break the bonds, resulting in a higher boiling point.

Q: What factors affect boiling point elevation?

A: The boiling point elevation of a solution is affected by the following factors:

• Concentration of the solute: The higher the concentration of the solute, the greater the boiling point elevation.
• Type of solute: The type of solute can affect the boiling point elevation. Some solutes, such as salts, can dissociate into multiple ions, increasing the boiling point elevation.
• Properties of the solvent: The properties of the solvent, such as its molecular weight and polarity, can affect the boiling point elevation.

Q: How is boiling point elevation calculated?

A: Boiling point elevation is calculated using the formula:

ΔTb = Kb * m

where ΔTb is the boiling point elevation, Kb is the boiling point elevation constant, and m is the molality of the solution.

Q: What is the boiling point elevation constant (Kb)?

A: The boiling point elevation constant (Kb) is a constant that depends on the solvent. It is typically expressed in units of K/m (kelvin per mole).

Q: Can boiling point elevation be used to determine the concentration of a solute?

A: Yes, boiling point elevation can be used to determine the concentration of a solute. By measuring the boiling point elevation of a solution, you can calculate the concentration of the solute using the formula:

m = ΔTb / Kb

Q: What are some practical applications of boiling point elevation?

A: Boiling point elevation has several practical applications, including:

• Chemical engineering: Boiling point elevation is used to design and optimize chemical processes, such as distillation and crystallization.
• Pharmaceutical industry: Boiling point elevation is used to determine the concentration of active ingredients in pharmaceutical formulations.
• Food processing: Boiling point elevation is used to determine the concentration of solutes in food products, such as sugar and salt.

Conclusion

In conclusion, boiling point elevation is an important concept in chemistry that has several practical applications. By understanding the factors that affect boiling point elevation and how to calculate it, you can apply this concept to a wide range of fields, from chemical engineering to food processing.

References

• Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
• Chang, R. (2010). Physical chemistry for the biosciences. University Science Books.
• Levine, I. N. (2014). Physical chemistry. McGraw-Hill Education.

Table of Contents

1. Introduction
2. Q: What is boiling point elevation?
3. Q: Why does boiling point elevation occur?
4. Q: What factors affect boiling point elevation?
5. Q: How is boiling point elevation calculated?
6. Q: What is the boiling point elevation constant (Kb)?
7. Q: Can boiling point elevation be used to determine the concentration of a solute?
8. Q: What are some practical applications of boiling point elevation?
9. Conclusion
10. References
11. Table of Contents