Carbon tetrachloride would have the highest boiling point for a 0.10 m nonelectrolyte solution.

This question involves colligative properties, specifically boiling point elevation (ΔTb\Delta T_bΔTb​), given by ΔTb=Kb×m×i\Delta T_b=K_b\times m\times iΔTb​=Kb​×m×i. For a nonelectrolyte, i=1i=1i=1, and m=0.10m=0.10m=0.10, so ΔTb\Delta T_bΔTb​ depends directly on the solvent's ebullioscopic constant KbK_bKb​. The solvent with the highest KbK_bKb​ yields the greatest elevation, thus the highest final boiling point (pure boiling point + ΔTb\Delta T_bΔTb​).

Solvent Options and KbK_bKb​ Values

These are the standard options from identical problems:

Solvent| KbK_bKb​ (°C/m)| ΔTb\Delta T_bΔTb​ for 0.10 m
---|---|---
Carbon tetrachloride| 5.03| 0.503°C
Benzene| 2.53| 0.253°C
Diethyl ether| 2.02| 0.202°C
Water| 0.512| 0.0512°C
Acetic acid| 3.07| 0.307°C

Carbon tetrachloride tops the list because its KbK_bKb​ is unmatched here, elevating boiling by 0.503°C—nearly 10x water's effect.

Why This Matters

Higher KbK_bKb​ reflects stronger solute-solvent interactions in that medium, amplifying the elevation. Pure solvent boiling points vary (e.g., water 100°C, benzene ~80°C), but the question targets the solution's final TbT_bTb​, so max ΔTb\Delta T_bΔTb​ wins regardless.

TL;DR: Carbon tetrachloride—its Kb=5.03°C/mK_b=5.03°C/mKb​=5.03°C/m gives the biggest ΔTb=0.503°C\Delta T_b=0.503°CΔTb​=0.503°C.

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