Chemistry: Principles and Reactions
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ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Transcribed Image Text:I Review | Constants | Periodic Table
Colligative properties are those that depend on the
number of solute particles. Because electrolytes
dissociate into ions, the concentration of particles in the
solution is greater than the formula-unit concentration of
the solution. For example, if 1 mol of Na2SO4 totally
dissociates, 3 mol of ions are produced (2 mol of Na+
ions and 1 mol of SO4 ions). Thus, a colligative
property such as osmotic pressure will be three times
greater for a 1 mol L1 Na2SO4 solution than for a
1 mol L nonelectrolyte solution.
Part A
Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that
freezes at – 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C kg mol1.
Express your answer to three significant figures and include the appropriate units.
• View Available Hint(s)
However, complete dissociation of electrolytes does not
always occur. The extent of dissociation is expressed by
the van't Hoff factor, i:
HẢ
moles of particles in solution
i
moles of solute dissolved
Value
Units
The equations for colligative properties can be written to
include i. For example,
AT: = im x Kf
Submit
AT
— im х Къ
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