Question

Which solution has the highest boiling point?

a) 0.50 m C₁₂H₂₂O₁₁
b) 0.50 m C₆H₁₂O₆
b) 0.50 m C₂H6O₂
d) All of these solutions will have the same boiling point

Answer 1

The boiling points of solutions vary based on the molal concentration and the van 't Hoff factor. The solution with 0.4 m Al2(SO4)3 has the highest boiling point among the given examples due to the greatest number of particles it produces upon dissociation.

Step-by-step explanation:

When comparing the boiling points of solutions, the elevation of the boiling point depends on the amount of solute and the type of particles it dissociates into. Each solution will have a different boiling point based on the solute's ability to cause boiling point elevation.

The boiling point of a solution increases with the molal concentration of solute species, according to the formula Δт = Ктт. In order of increasing boiling point for the examples given, we would examine the van 't Hoff factor, which is the number of particles into which a solute dissociates in solution. A higher van 't Hoff factor leads to greater boiling point elevation.

1. 0.10 m C6H12O6 (glucose, a non-electrolyte, does not dissociate)
2. 0.06 m NaCl (dissociates into 2 particles: Na+ and Cl-)
3. 0.4 m Au(NO3)3 (dissociates into 4 particles: Au3+ and 3 NO3-)
4. 0.4 m Al2(SO4)3 (dissociates into 5 particles: 2 Al3+ and 3 SO4 2-)

Therefore, given their respective molalities and the number of particles produced upon dissociation, the solution with 0.4 m Al2(SO4)3 will have the highest boiling point due to its high van 't Hoff factor.