Chemistry: A Molecular Approach (3rd Edition)

Published by Prentice Hall
ISBN 10: 0321809246
ISBN 13: 978-0-32180-924-7

Chapter 12 - Sections 12.1-12.8 - Exercises - Problems by Topic - Page 589: 32

Answer

CH2Cl2 is more soluble in water.

Work Step by Step

Since both molecules are non-polar, London dispersion forces now depend on the molar mass of the molecule. The higher the molar mass, the London dispersion forces are greater. Since CH2Cl2 has a higher molar mass, it will have stronger IMF's causing it to be more soluble in water.
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