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Standard XII

Chemistry

Orthoboric Acid

A solution co...

Question

A solution containing 0.1 mole of urea in 1 L ofglacial acetic acid, when cooled the first crystalwhich appears at the freezing point contain themolecules of

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Q. The freezing point of a solution containing

0.2 g

of acetic acid in

20 g

of benzene is lowered by

0. 45^{o} C

Calculate the degree of association of acetic acid in benzene (

K_{f}

for benzene is

5.12 K

{m o l}^{- 1}

Q. Depression of freezing point of 0.01 molal aqueous Acetic Acid solution is 0.0204 degree Celsius. 1 molal urea solution freezes at -1.86 degree Celsius. Assuming molality equal to molarity, pH of Acetic Acid solution.

Q. The freezing point of a solution containing

0.2

g of acetic acid in

20.0

g benzene is lowered by

{0.45}^{o} C

. The degree of association of acetic acid in benzene is:

[Assume acetic acid dimerizes in benzene and

K_{f}

for benzene

= 5.12

K kg mol

^{- 1}

]

Q. The freezing point of a solution containing

0.3 g m s

of acetic acid in

30 g m s

of benzene is lowered by

0.45 K

. Calculate the Van't Hoff factor.
(at. wt. of

C = 12, H = 1, O = 16, K_{f}

for benzene

= 5.12 k k g m o l e^{- 1})

Q. The freezing point of a solution containing

0.2 g

of acetic acid in

20 g

of benzene is lowered by

{0.45}^{\circ} C .

. Calculate the degree of association

(β)

for acetic acid.
Given :

(K_{f})_{Benzene} = 5.12 K k g m o l^{- 1}

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