Suppose you have a pure solvent that has a boiling point of 78 degreeC. How woul

Question

Suppose you have a pure solvent that has a boiling point of 78 degreeC. How would this boiling point change if a non-volatile solute was dissolved in the solvent, and what is responsible forthis change? The boiling point of the solution would be 78 degreeC. When a solution is boiled, only the solvent vaporizes, so the boiling would still take place at 78 degreeC. The boiling point would be above 78 degreeC. The presence of the non-volatile solute lowers the equilibrium vapor pressure, so a higher temperature is needed for the equilibrium vapor pressure to become equal to the atmospheric pressure. The boiling point would be below 78 degreeC. The presence of the non-volatile solute increases the equilibrium vapor pressure, so the temperature does not need to be as high for the equilibrium vapor pressure to become equal to the atmospheric pressure. The boiling point would be above 78 degreeC. because in the boiling process, both the solute and the non-volatile solute must vaporize. A higher temperature is required to vaporize the non-volaiile solvent.

Explanation / Answer

b) Boiling point incerease

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.