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What Is the Boiling Point of a Solution That Contains 0.50 Mol of NaCl in 1.00 KG of Water?
Introduction:
Boiling point is defined as the temperature at which a liquid changes into its gaseous state. The boiling point of a pure substance, such as water, is a well-known constant. However, when a solute is dissolved in a solvent, it can affect the boiling point of the solution. In this article, we will explore the concept of boiling point elevation and calculate the boiling point of a solution containing 0.50 mol of NaCl in 1.00 kg of water.
Boiling Point Elevation:
Boiling point elevation occurs when a solute is added to a solvent, resulting in an increase in the boiling point of the solution compared to the pure solvent. This phenomenon can be explained by the presence of solute particles, which disrupt the intermolecular forces between the solvent molecules. As a result, more energy is required to break these intermolecular forces, leading to an increase in the boiling point.
The boiling point elevation can be calculated using the equation:
ΔTb = Kb * m
Where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant, and m is the molality of the solution.
Calculating the Boiling Point Elevation:
To calculate the boiling point of a solution containing 0.50 mol of NaCl in 1.00 kg of water, we need to determine the molality of the solution and the molal boiling point elevation constant.
Molality (m) is defined as the number of moles of solute per kilogram of solvent. In this case, we have 0.50 mol of NaCl dissolved in 1.00 kg of water. Thus, the molality can be calculated as follows:
m = moles of solute / mass of solvent in kg
m = 0.50 mol / 1.00 kg = 0.50 mol/kg
The molal boiling point elevation constant (Kb) is a characteristic property of a solvent and is typically provided in reference tables. For water, the Kb value is 0.512 °C/m.
Now, we can substitute the values into the boiling point elevation equation:
ΔTb = Kb * m
ΔTb = 0.512 °C/m * 0.50 mol/kg
ΔTb = 0.256 °C
Therefore, the boiling point of the solution containing 0.50 mol of NaCl in 1.00 kg of water will be elevated by 0.256 °C compared to the boiling point of pure water.
FAQs:
Q: How does the boiling point elevation occur?
A: Boiling point elevation occurs due to the presence of solute particles in the solution, which disrupt the intermolecular forces between solvent molecules, requiring more energy to reach the boiling point.
Q: Is boiling point elevation a universal phenomenon?
A: No, boiling point elevation is specific to each solvent and depends on the molal boiling point elevation constant characteristic of that solvent.
Q: Can the boiling point be elevated indefinitely by adding more solute?
A: No, there is a limit to the boiling point elevation. Eventually, the solute particles will reach a concentration where they become saturated and can no longer disrupt the intermolecular forces effectively.
Q: Can boiling point elevation be observed in all solutions?
A: Boiling point elevation can only be observed when a non-volatile solute, such as NaCl, is dissolved in a volatile solvent, such as water.
Q: How is boiling point elevation useful in everyday life?
A: Boiling point elevation has practical applications in cooking, where the addition of salt to water increases the boiling point, allowing food to cook at higher temperatures and reducing cooking time.
Conclusion:
The boiling point of a solution containing 0.50 mol of NaCl in 1.00 kg of water can be calculated using the boiling point elevation equation. The molality of the solution and the molal boiling point elevation constant are required to determine the boiling point elevation. Boiling point elevation occurs due to the presence of solute particles, which disrupt the intermolecular forces of the solvent. The calculated boiling point elevation provides valuable information about the behavior of solutions and has practical applications in various fields.
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