Boiling Point ElevationThe boiling point of a solution INCREASES with the number of dissolved solute particles. This is summarized by the expression: Tb = m i KbWhere:Tbis the increase in the boiling point= Tb(solution) - Tb(pure solvent)mis the molality of the solution= (# moles solute / kg solvent)iis 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.| 1. 0.16 m Zn(NO3)2| 2. 0.15 m CuCl2A. Highest boiling pointB. Second highest boiling point3. 0.18 m Bal2C. Third highest boiling point4. 0.52 m Sucrose(nonelectrolyte)D. Lowest boiling point

1. 0.16 m Zn(NO3)2 Van't Hoff factor i = 3 Elevation in boiling point constant for water Kb =…

Answered: Match the following aqueous solutions…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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: T_b = m i K_b

Where:

T_b	is the increase in the boiling point	= T_b(solution) - T_b(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)

K_b 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 SO₄^2- 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.
| 1. 0.16 m Zn(NO3)2
| 2. 0.15 m CuCl2
A. Highest boiling point
B. Second highest boiling point
3. 0.18 m Bal2
C. Third highest boiling point
4. 0.52 m Sucrose(nonelectrolyte)
D. Lowest boiling point

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