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Standard XII

Chemistry

Raoult's Law

A 0.01 m aq...

Question

A $0.01 m$ aqueous solution of $K_{3} [F e (C N)_{6}]$ freezes at $- {0.062}^{\circ} C$ . What is the apparent percentage of dissociation? $[K_{f}$ for water $= 1.8]$
[Note : Write the value to the nearest integer]

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Solution

$Δ T_{f} = i K_{f} m$

$Δ T_{f} = 0^{o} C - (- 0.062^{o} C) = 0.062^{o} C$

$m = 0.01 m$

$K_{f} = 1.86$

$Δ T_{f} = i K_{f} m$

$0.062^{o} C = i \times 1.86 \times 0.01 m$

The vant Hoff factor $i = 3.33$

The degree of dissociation $α = \frac{i - 1}{n^{'} - 1}$

$α = \frac{3.33 - 1}{4 - 1}$

$α = \frac{2.33}{3} = 0.776 = 77.6 %$

The value to the nearest integer is 78.

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Similar questions

A 0.01m aqueous solution of $K_{3} [F e (C N)_{6}]$ was found to freeze at $- {0.062}^{\circ} C$ . If Kf for water is ${1.86}^{\circ} C$ /molal then the apparent percentage of dissociation is:

Q. 0.01 m aqueous solution of

K_{3} [F e {(C N)}_{6}]

freezes at

- 0.0 62^{\circ} C

, what is the apparent percentage of dissociation ?

(k_{f} (H_{2} O) = 1.86 K k g {m o I}^{- 1})

Q. A

0.15

molal solution of

K_{4} [F e (C N)_{6}]

in water freezes at

- {0.65}^{\circ} C

. What is the apparent percentage of dissociation of this compound in this solution?

[K_{f}

for water

= {1.86}^{\circ} C m o l^{- 1}]

Q. Van't Hoff factor of centimolal solution of

K_{3} [F e {(C N)}_{6}]

3.333.

Calculate the percent dissociation of

K_{3} [F e {(C N)}_{6}]

(Round off to the nearest integer).

Q. A solution containing 0.85g of

Z n C l_{2}

in 125.0 g of water freezes at

- {0.23}^{0} C

. The apparent degree of dissociation of the salt is:
(

k_{f}

for water

=1.86 K kg mol^{-1}

, atomic mass ;

Z n = 65.3

and

C l = 35.5

)

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A 0.01m aqueous solution of K3[Fe(CN)6] freezes at −0.062∘C. What is the apparent percentage of dissociation? [Kf for water=1.8] [Note : Write the value to the nearest integer]

ΔTf=iKfm ΔTf=0 oC−(−0.062 oC)=0.062 oC m=0.01 mKf=1.86ΔTf=iKfm 0.062 oC=i×1.86×0.01 mThe vant Hoff factor i=3.33 The degree of dissociation α=i−1n′−1α=3.33−14−1α=2.333=0.776=77.6%The value to the nearest integer is 78.

A $0.01 m$ aqueous solution of $K_{3} [F e (C N)_{6}]$ freezes at $- {0.062}^{\circ} C$ . What is the apparent percentage of dissociation? $[K_{f}$ for water $= 1.8]$
[Note : Write the value to the nearest integer]