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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 mol¯.

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 mol¯.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 64QAP
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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
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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