Home
Class 12
CHEMISTRY
Determination of the molar mass of aceti...

Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by:

A

association

B

dissociation

C

complex formation

D

partial ionization

Text Solution

Verified by Experts

The correct Answer is:
A

Due to hydrogen bonding acetic acid dimerise in benzene
Promotional Banner

Similar Questions

Explore conceptually related problems

1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its freezing point by 0.40K. The freezing point depression constant of benzene is "5.12K.kg mol"^(-1) . Find the molecular mass of the solute.

The freezing point of 0.02 mol fraction solution of acetic acid (A) in benzene (B) is 277.4K . Acetic acid exists partly as a dimer 2A = A_(2) . Calculate equilibrium constant for the dimerisation. Freezing point of benzene is 278.4K and its heat of fusion DeltaH_(f) is 10.042 kJ mol^(-1) .

Acetic acid tends to form dimer due to formation of intermolcular hydrogen bonding. 2CH_(2)COOHhArr(CH_(3)COOH)_(2) The equilibrium constant for this reaction is 1.5xx10^(2)M^(-1) in benzene solution and 3.6xx10^(-2) in water. In benzene, monomer does not dissociate but it water, monomer dissociation simultaneously with acid dissociation constant 2.0xx10^(-5) M. Dimer does not dissociate in benzene as well as water. The molar ratio of dimer to monmer for 0.1M acetic acid in water (neglecting the dissciation of acetic acid in water ) is equal to :

When 1.20g of sulphur is melted with 15.00g of naphthalene, the solution freezes at 77.2^(@)C . What is the moalr mass of this from of sulphur. Data for Napthalene Melting point, m.p 80^(@)C Freezing point depression constant, k_(f) = 6.80^(@)Cm^(-1)

For a dilute solution containing a nonvolatile solute, the molar mass of solute evaluated from the elevation of boiling point is given by the experssion: