Explain why the van't Hoff factor for K2SO4 is less than its predicted value. The hydrated K⁺ and SO42- ions attract one another and effectively increase the number of free particles in the solution. The hydrated K⁺ and SO42- ions attract one another and effectively reduce the number of free particles in the solution. The number of moles of formula units is greater than the number of free particles in the solution. The hydrated K⁺ and SO42- ions repel one another and effectively reduce the number of free particles in the solution.
Explain why the van't Hoff factor for K2SO4 is less than its predicted value. The hydrated K⁺ and SO42- ions attract one another and effectively increase the number of free particles in the solution. The hydrated K⁺ and SO42- ions attract one another and effectively reduce the number of free particles in the solution. The number of moles of formula units is greater than the number of free particles in the solution. The hydrated K⁺ and SO42- ions repel one another and effectively reduce the number of free particles in the solution.
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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Question
Explain why the van't Hoff factor for K2SO4 is less than its predicted value.
The hydrated K⁺ and SO42- ions attract one another and effectively increase the number of free particles in the solution. |
The hydrated K⁺ and SO42- ions attract one another and effectively reduce the number of free particles in the solution. |
The number of moles of formula units is greater than the number of free particles in the solution. |
The hydrated K⁺ and SO42- ions repel one another and effectively reduce the number of free particles in the solution. |
Expert Solution
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Step 1
As ionic solutions contain fewer particles than predicted by the number of ions per unit ,so the vant hof factor for ionic compounds are lower than expected value and also ionic compounds don't dissociate completely in aqueous solution. Some ions also exist as ion pairs or the ions associated with each other with out disturbing the water molecules.
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