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Science Chemistry Chemistry: An Atoms-Focused Approach

Why the van’t Hoff factors of electrolytes are greater than those of nonelectrolytes. Solution: The van’t Hoff factors of electrolytes are greater than those of nonelectrolytes because electrolytes dissociate into ions and nonelectrolytes do not. Explanation: The van’t Hoff, i , is the ratio of the experimentally determined value of a colligative property to the expected value if the solute did not dissociate into ions in a solution. Colligative properties and van’t Hoff factors are linked to the number of dissolved particles in the solution. Since one mole of electrolyte such as N a C l dissociates into two moles of particles, (cation and anion), the van’t Hoff factor is expected to be 2.0 for an aqueous solution of N a C l . Similarly, van’t Hoff factor for the solution of C a N O 3 2 is 3.0 , because one mol of calcium ions and two moles of nitrate ions are produced per mole of the solute. However, for a non-electrolyte, like ethylene glycol, one mole of solute will produce only one mole of dissolved particles, since the solute does not dissociate into its ions. Thus, the van’t Hoff factor of a nonelectrolyte will be 1.0 . Therefore, the van’t Hoff factor for electrolytes will be greater than those of nonelectrolytes. Final Statement: The van’t Hoff factor of electrolytes depends on the number of particles produced upon dissociation in solution.

Why the van’t Hoff factors of electrolytes are greater than those of nonelectrolytes. Solution: The van’t Hoff factors of electrolytes are greater than those of nonelectrolytes because electrolytes dissociate into ions and nonelectrolytes do not. Explanation: The van’t Hoff, i , is the ratio of the experimentally determined value of a colligative property to the expected value if the solute did not dissociate into ions in a solution. Colligative properties and van’t Hoff factors are linked to the number of dissolved particles in the solution. Since one mole of electrolyte such as N a C l dissociates into two moles of particles, (cation and anion), the van’t Hoff factor is expected to be 2.0 for an aqueous solution of N a C l . Similarly, van’t Hoff factor for the solution of C a N O 3 2 is 3.0 , because one mol of calcium ions and two moles of nitrate ions are produced per mole of the solute. However, for a non-electrolyte, like ethylene glycol, one mole of solute will produce only one mole of dissolved particles, since the solute does not dissociate into its ions. Thus, the van’t Hoff factor of a nonelectrolyte will be 1.0 . Therefore, the van’t Hoff factor for electrolytes will be greater than those of nonelectrolytes. Final Statement: The van’t Hoff factor of electrolytes depends on the number of particles produced upon dissociation in solution.

Solution Summary: The author explains why the van't Hoff factors of electrolytes are greater than those of nonelectrolytes.

Chemistry: An Atoms-Focused Approach

Chemistry: An Atoms-Focused Approach

14th Edition

ISBN: 9780393912340

Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster

Publisher: W. W. Norton & Company

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Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to a…

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Chemistry: An Atoms-Focused Approach

Ch. 11 - Prob. 11.1VP Ch. 11 - Prob. 11.2VP Ch. 11 - Prob. 11.3VP Ch. 11 - Prob. 11.4VP Ch. 11 - Prob. 11.6VP Ch. 11 - Prob. 11.7VP Ch. 11 - Prob. 11.8VP Ch. 11 - Prob. 11.9VP Ch. 11 - Prob. 11.10VP Ch. 11 - Prob. 11.11QA

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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY