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 NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO, 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/m. 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 the van't Hoff factor, i: expressed by O B) ? moles of particles in solution moles of solute dissolved 7.80 kg The equations for colligative properties can be written to include i. For example. AT = K - m-i Submit Previous Answers AT K m-i
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 NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO, 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/m. 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 the van't Hoff factor, i: expressed by O B) ? moles of particles in solution moles of solute dissolved 7.80 kg The equations for colligative properties can be written to include i. For example. AT = K - m-i Submit Previous Answers AT K m-i
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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Transcribed Image Text: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 NazSO4 totally dissociates,
3 mol of ions are produced (2 mol of Nat ions and
1 mol of SO, ions). Thus, a colligative property such
as osmotic pressure will be three times greater for a 1 M
NazSO, solution than for a 1 M 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/m.
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
the van't Hoff factor, i:
dissociation is expressed by
HA
moles of particles in solution
moles of solute dissolved
7.80
kg
The equations for colligative properties can be written to
include i. For example,
Δ
K - m-i
Submit
Previous Answers
AT,
K m i
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