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Statement A: Solubility of alcohols in water goes on increasing with increasing molecular weight.
Statement B: Boiling point of alcohols goes on increasing with increasing molecular weight.
  • a)
    Statement A is true; Statement B is false.
  • b)
    Statement B is true; Statement A is false.
  • c)
    Both the statements A and B are true
  • d)
    Neither statement A nor statement B is true.
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
Statement A:Solubility of alcohols in water goes on increasing with in...
Solubility of alcohols in water decreases with increasing molecular weight. The first three alcohols (methanol, ethanol and propanol) are completely miscible. Each alcohol consists of a carbon chain (always non-polar) and a OH group (which is polar). The solubility of alcohols starts to decrease with butanol. Alcohols are considered immiscible after heptanol
Boiling point of alcohols increases with increasing molecular weight. The boiling point of alcohols increases as the length of the hydrocarbon chain increases.
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Most Upvoted Answer
Statement A:Solubility of alcohols in water goes on increasing with in...
Statement A: Solubility of alcohols in water goes on increasing with increasing molecular weight.
Statement B: Boiling point of alcohols goes on increasing with increasing molecular weight.

Explanation:

Statement A: The solubility of alcohols in water is influenced by the presence of the hydroxyl (-OH) group. Alcohols with smaller molecular weights, such as methanol (CH3OH) and ethanol (C2H5OH), are highly soluble in water because they can form hydrogen bonds with water molecules. These hydrogen bonds allow the alcohol molecules to mix and dissolve in water.

However, as the molecular weight of alcohols increases, their solubility in water decreases. This is because the hydrocarbon chain in higher molecular weight alcohols becomes larger and more nonpolar, reducing their ability to form hydrogen bonds with water. Instead, they tend to form stronger intermolecular forces with themselves, resulting in lower solubility in water.

Therefore, Statement A is false.

Statement B: The boiling point of alcohols is primarily determined by the strength of their intermolecular forces. As the molecular weight of alcohols increases, the size and surface area of the molecules also increase. This allows for stronger dispersion forces (London forces) between the alcohol molecules.

Dispersion forces are attractive forces between molecules caused by temporary fluctuations in electron distribution. Larger molecules have more electrons, leading to stronger dispersion forces. These stronger intermolecular forces require more energy to overcome, resulting in higher boiling points.

Therefore, Statement B is true.

Conclusion:
Based on the explanation above, we can conclude that Statement A is false and Statement B is true. Thus, the correct answer is option 'B': Statement B is true; Statement A is false.
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Statement A:Solubility of alcohols in water goes on increasing with increasing molecular weight.Statement B:Boiling point of alcohols goes on increasing with increasing molecular weight.a)Statement A is true;Statement B is false.b)Statement B is true;Statement A is false.c)Both the statements A and B are trued)Neither statement A nor statement B is true.Correct answer is option 'B'. Can you explain this answer?
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