Question

why alcohols are more soluble in water compared to ether?​

Answer 1

• Alcohols have higher boiling point than ethers of same molecular mass because in alcohol there is the presence of intermolecular hydrogen bonding. Alcohols form H-bonds with water due to the presence of −OH group. ... As a result, alcohols are comparatively more soluble in water than ethers of comparable molecular

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Answer 2

Explanation:

ANSWER :-

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For two liquids to be miscible / soluble in each other, their intermolecular bonding must have similar strengths. Ammonia can dissolve in water because they both form strong hydrogen bonds.

Ethers are nonpolar and can only form London forces, a very weak type of intermolecular force. So ethers cannot dissolve in water because the two types on bonding do not do well together.

Alcohol also form hydrogen bonds. However, alcohols are made of a hydroxy group and an alkyl group. Alkyl groups are not as polar as hydroxy groups, so they can also display London forces. Therefore ether can bond with the alkyl groups of alcohols, allowing the two compounds to mix together

EXTRA INFORMATION:-

Alcohols contain an--OH group attached to a saturated carbon. The common names for alcohols are based on the name of the alkyl group.

CH3OH Methyl alcohol

CH3CH2OH Ethyl alcohol

CH3CHOHCH3 Isopropyl alcohol

The systematic nomenclature for alcohols adds the ending -ol to the name of the parent alkane and uses a number to identify the carbon that carries the --OH group. The systematic name for isopropyl alcohol, for example, is 2-propanol.

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