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1. explain the results for the miscibility of the respective pairs in terms of the polarities of the molecules in the different liquids. a. Water and Ethanol b. Water and Hexane c. Hexane and Ethanol
Accepted Answer
Miscibility is the ability of two liquids to mix and form a homogeneous solution. Here's a breakdown of the miscibility of the pairs based on their polarities:
a. Water and Ethanol:
Water: Polar molecule due to its bent shape and electronegative oxygen atom.
Ethanol: Polar molecule with a hydroxyl (-OH) group, which forms hydrogen bonds with water.
Result: Miscible. Water and ethanol are both polar and can form strong hydrogen bonds, leading to easy mixing.
b. Water and Hexane:
Water: Polar (explained above).
Hexane: Nonpolar hydrocarbon chain.
Result: Immiscible. Water and hexane have very different polarities. Water cannot form significant interactions with the nonpolar hexane molecules, leading to separation.
c. Hexane and Ethanol:
Hexane: Nonpolar (explained above).
Ethanol: Polar (explained above).
Result: Partially miscible. Ethanol's polar -OH group can interact weakly with hexane, resulting in some degree of mixing. However, the nonpolar hydrocarbon chain dominates, leading to limited miscibility.
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