Interpretation: To explain why diethyl ether is more soluble than di-hexyl ether in water.
Concept Introduction: The solubility of the compound depends upon the extent of the hydrogen bonding. The greater the extent of hydrogen bonding, the greater will be the solubility. It also depends upon the size of the alkyl group. The size of the alkyl group is inversely proportional to the solubility.
Answer to Problem 58A
The size of the alkyl group is higher in di-hexyl ether as compared to that of di-ethyl ether therefore, the boiling point of the di-ethyl ether is higher as compared to that of di-hexyl ether.
Explanation of Solution
The solubility will depend upon the hydrogen bonding. If the extent of hydrogen bonding is more then the solubility will also be high. With the increase in the alkyl chain, the extent of hydrogen bonding decrease, and the solubility will also decrease. The di-ethyl ether has a smaller hydrocarbon chain as compared to that of di-hexyl ether. Hence, diethyl ether, due to its shorter hydrocarbon chain is easily soluble in water as compared to di-hexyl ether which has a higher hydrocarbon chain than di-ethyl ether.
Since the hydrocarbon chain is shorter in di-ethyl ether there is a greater extent of hydrogen bonding. The greater the extent of hydrogen bonding higher is its solubility. Hydrogen bonding and solubility are proportional to each other. Therefore, a shorter hydrocarbon chain favors solubility.
Chapter 23 Solutions
Chemistry 2012 Student Edition (hard Cover) Grade 11
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