Pick the answer that most likely represents the substances’ relative solubilities in water.
A. CH₃CH₂CH₂CH₃ < CH₃CH₂CH₂OH < HOCH₂CH₂OH
B. CH₃CH₂CH₂OH < CH₃CH₂CH₂CH₃ < HOCH₂CH₂OH
C. CH₃CH₂CH₂CH₃ < HOCH₂CH₂OH < CH₃CH₂CH₂OH
D. HOCH₂CH₂OH < CH₃CH₂CH₂OH < CH₃CH₂CH₂CH₃
E. HOCH₂CH₂OH < CH₃CH₂CH₂OH < CH₃CH₂CH₂CH₃
Answer (3)
the naswer should be A
The correct answer for substances relative solubilities in water is option (A) CH₃CH₂CH₂CH₃ < CH₃CH₂CH₂OH < HOCH₂CH₂OH.
To determine the relative solubilities of these compounds in water, we need to consider hydrogen bonding and polarity:
CH₃CH₂CH₂CH₃ (Butane): This is a nonpolar molecule without any hydrogen bonding capability, making it the least soluble in water.
CH₃CH₂CH₂OH (Propanol): This has an -OH group allowing for hydrogen bonding, making it more soluble than butane.
HOCH₂CH₂OH (Ethylene glycol): This has two -OH groups, which significantly increases its ability to hydrogen bond, making it the most soluble in water among the three.
The compounds rank in solubility in water as Butane < Propanol < Ethylene Glycol due to the increasing ability to participate in hydrogen bonding.
The relative solubility of the mentioned substances in water is determined by their ability to form hydrogen bonds. The correct ranking from least to most soluble is Butane < Propanol < Ethylene Glycol, which corresponds to option A. This reflects how the presence of hydroxyl groups enhances solubility due to hydrogen bonding capabilities.
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