Which solution has the highest vapor pressure? a. 20.0 g of glucose (C6H12O6) in 100.0

step 1 Question 70, which solution has the highest vapor pressure? So A, B, and C, all three solutions

Which solution has the highest vapor pressure? a. 20.0...

Which solution has the highest vapor pressure? $$\begin{array}{l}{\text { a. } 20.0 \text { g of glucose }\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right) \text { in } 100.0 \mathrm{mL} \text { of water }} \\ {\text { b. } 20.0 \mathrm{g} \text { of sucrose }\left(\mathrm{C}_{6} \mathrm{H}_{22} \mathrm{O}_{11}\right) \text { in } 100.0 \mathrm{mL} \text { of water }} \\ {\text { c. } 10.0 \mathrm{g} \text { of potassium acetate } \mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \text { in } 100.0 \mathrm{mL} \text { of water }}\end{array}$$

Which solution has the highest vapor pressure?
$$\begin{array}{l}{\text { a. } 20.0 \text { g of glucose }\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right) \text { in } 100.0 \mathrm{mL} \text { of water }} \\ {\text { b. } 20.0 \mathrm{g} \text { of sucrose }\left(\mathrm{C}_{6} \mathrm{H}_{22} \mathrm{O}_{11}\right) \text { in } 100.0 \mathrm{mL} \text { of water }} \\ {\text { c. } 10.0 \mathrm{g} \text { of potassium acetate } \mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \text { in } 100.0 \mathrm{mL} \text { of water }}\end{array}$$

Key Concepts

Mole Fraction

The mole fraction is a way of expressing the concentration of a component in a mixture, defined as the ratio of the number of moles of that component to the total number of moles of all components in the solution. In the context of vapor pressure lowering, a higher mole fraction of the solvent means a higher vapor pressure, while a lower mole fraction, due to the addition of solute particles, results in a lower vapor pressure.

Electrolyte versus Non-Electrolyte Behavior

Electrolytes dissociate into ions in solution, which increases the effective number of solute particles compared to non-electrolytes, which do not dissociate. This difference is crucial in colligative properties because a solution containing an electrolyte will experience a greater reduction in vapor pressure compared to a solution with an equivalent amount of a non-electrolyte, due to the higher particle concentration produced by ionization.

Raoult's Law

Raoult's Law states that the vapor pressure of a solvent in a solution is directly proportional to the mole fraction of the solvent. When a non-volatile solute is added, it decreases the mole fraction of the solvent, thereby lowering the vapor pressure. This law is key to predicting how the presence of solute particles, regardless of their nature, influences the vapor pressure of solutions.

Colligative Properties

Colligative properties are characteristics of solutions that depend only on the number of solute particles present, not on their identity. These properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The concept is crucial for understanding how the addition of a solute, which reduces the number of solvent molecules at the surface, alters the vapor pressure of the solvent in any solution.

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