Water is a small, polar molecule, capable of forming hydrogen bonds. Based on this, what types of substances would you 1. expect to be soluble in water? 2. If you expect that the intermolecular forces will be stronger in liquid A, compared to liquid B, how would you predict the vapour pressures of the two liquids to compare? What would you predict about their normal boiling points? 3. When you are determining if a solid is soluble in a particular solvent, why is it important to use a very small amount of the solid? What could happen if you used a large amount of solid?

Water is a small, polar molecule, capable of forming hydrogen bonds. Based on this, what types of substances would you 1. expect to be soluble in water? 2. If you expect that the intermolecular forces will be stronger in liquid A, compared to liquid B, how would you predict the vapour pressures of the two liquids to compare? What would you predict about their normal boiling points? 3. When you are determining if a solid is soluble in a particular solvent, why is it important to use a very small amount of the solid? What could happen if you used a large amount of solid?

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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