Match the following aqueous solutions with the appropriate letter from the column on the right. A. Highest boiling point 1. 0.16 m CrBr2 2. 0.18 m (NH4)2s B. Second highest boiling point 3. 0.17 m MnClz C. Third highest boiling point 4. 0.46 m Sucrose(nonelectrolyte) D. Lowest boiling point

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Boiling Point Elevation
The boiling point of a solution INCREASES with the number of dissolved solute particles.

This is summarized by the expression: Tb = m i Kb

Where:
Tb is the increase in the boiling point = Tb(solution) - Tb(pure solvent)
m is the molality of the solution = (# moles solute / kg solvent)
i is the "van't Hoff" factor = (# moles of solute particles / mole of solute)
  For nonelectrolytes: i = 1
  For strong electrolytes: i = number of (cations + anions)
  For weak electrolytes: 1 < i < number of (cations + anions)


Kb is the boiling point elevation constant. It depends only on the SOLVENT.

Example:
Na2SO4 is a soluble salt. It breaks into two Na+ cations and one SO42- anion in solution.
i = 2 + 1 = 3

CH3COOH is a weak acid. It breaks into a few CH3COO - anions and a few H+ cations.
1 < i < 2.
 
Match the following aqueous solutions with the appropriate letter from the column on the right.
A. Highest boiling point
1. 0.16 m CrBr2
2. 0.18 m (NH4)2s
B. Second highest boiling point
3. 0.17 m MnClz
C. Third highest boiling point
4. 0.46 m Sucrose(nonelectrolyte)
D. Lowest boiling point
Transcribed Image Text:Match the following aqueous solutions with the appropriate letter from the column on the right. A. Highest boiling point 1. 0.16 m CrBr2 2. 0.18 m (NH4)2s B. Second highest boiling point 3. 0.17 m MnClz C. Third highest boiling point 4. 0.46 m Sucrose(nonelectrolyte) D. Lowest boiling point
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