(A) In water,$CH_3COOH$ acts as a weak electrolyte and undergoes partial dissociation into $CH_3COO^-$ and $H^+$ ions,resulting in a lower observed mo

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Acetic acid undergoes dissociation in water and association in benzene.

(A) In water,$CH_3COOH$ acts as a weak electrolyte and undergoes partial dissociation into $CH_3COO^-$ and $H^+$ ions,resulting in a lower observed molecular mass $(60)$.In benzene (a non-polar solvent),$CH_3COOH$ molecules form intermolecular hydrogen bonds,leading to the formation of dimers. This association results in an observed molecular mass of $120$ (double the normal mass).

Class 12 Chemistry Solutions Abnormal molecular mass

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The molecular mass of acetic acid $(CH_3COOH)$ dissolved in water is $60$,whereas when dissolved in benzene,it is $120$. This difference in behavior is because:

A
Acetic acid undergoes dissociation in water and association in benzene.
B
Acetic acid undergoes association in water and dissociation in benzene.
C
Acetic acid remains unaffected in both solvents.
D
Acetic acid undergoes dissociation in both solvents.

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Abnormal molecular mass

If $0.1 \ M$ solution of $NaCl$ is isotonic with $1.1 \ w \%$ urea solution, the degree of ionisation of $NaCl$ is $($Molar masses of urea and $NaCl$ are $60 \ g \ mol^{-1}$ and $58.5 \ g \ mol^{-1}$, respectively.$)$

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In a solution of sulfur in carbon disulfide,$80 \%$ of the sulfur exists as $S_8$ and the remaining exists as $S_2$. The van't Hoff factor '$i$' will be:

Medium

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In a solvent,$50\,\%$ of an acid $HA$ dimerizes and the rest dissociates. The van't Hoff factor of the acid is $.....\times 10^{-2}$. (Round off to the nearest integer)

DifficultJEE MAIN 2021

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If the degree of dissociation of an aqueous solution of a weak monobasic acid is determined to be $0.3$,then the observed freezing point depression will be $.....\%$ higher than the expected/theoretical freezing point depression. (Nearest integer)

MediumJEE MAIN 2023

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When acetic acid is dissolved in benzene,its molecular mass:

Medium

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The molecular mass of acetic acid $(CH_3COOH)$ dissolved in water is $60$,whereas when dissolved in benzene,it is $120$. This difference in behavior is because:

Similar Questions

If $0.1 \ M$ solution of $NaCl$ is isotonic with $1.1 \ w \%$ urea solution, the degree of ionisation of $NaCl$ is $($Molar masses of urea and $NaCl$ are $60 \ g \ mol^{-1}$ and $58.5 \ g \ mol^{-1}$, respectively.$)$

In a solution of sulfur in carbon disulfide,$80 \%$ of the sulfur exists as $S_8$ and the remaining exists as $S_2$. The van't Hoff factor '$i$' will be:

In a solvent,$50\,\%$ of an acid $HA$ dimerizes and the rest dissociates. The van't Hoff factor of the acid is $.....\times 10^{-2}$. (Round off to the nearest integer)

If the degree of dissociation of an aqueous solution of a weak monobasic acid is determined to be $0.3$,then the observed freezing point depression will be $.....\%$ higher than the expected/theoretical freezing point depression. (Nearest integer)

When acetic acid is dissolved in benzene,its molecular mass:

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