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Standard XII

Chemistry

Osmotic Pressure

If a is the...

Question

If $a$ is the degree of dissociation of $K_{4} [F e (C N_{6})]$ than an abnormal mass of complex in the solution will be:

M_{n o r m a l} (1 + 2 a)^{- 1}

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M_{n o r m a l} (1 + 3 a)^{- 1}

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M_{n o r m a l} (1 + a)^{- 1}

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M_{n o r m a l} (1 + 4 a)^{- 1}

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Solution

The correct option is C $M_{n o r m a l} (1 + 4 a)^{- 1}$
Solution:- (D) $M_{normal} {(1 + 4 a)}^{- 1}$
Dissociation of $K_{4} [F e {(C N)}_{6}]$ -
$Initially After dissociation K_{4} [F e {(C N)}_{6}] 1 1 - a ⟶ 4 K^{+} 0 4 a + {[F e {(C N)}_{6}]}^{-} 0 a$
Van't hoff factor $=$ Total moles after dissociation $= (1 - a) + 4 a + a = 1 + 4 a$
As we know that,
$i = \frac{Normal molar mass}{Abnormal molar mass}$
$\Rightarrow Abnormal molar mass = \frac{Normal molar mass}{i}$
$\Rightarrow$ Abnormal molar mass $= \frac{M_{normal}}{1 + 4 a}$
$\Rightarrow$ Abnormal molar mass $= M_{normal} {(1 + 4 a)}^{- 1}$
Hence the abnormal molar mass of $K_{4} [F e {(C N)}_{6}]$ is $M_{normal} {(1 + 4 a)}^{- 1}$ .

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If $M_{n o r m a l}$ is the normal molecular mass and $α$ is the degree of ionization of $K_{3} [F e (C N)_{6}]$ , then the abnormal molecular mass of the complex in the solution will be:

Q. The experimental values of colligative properties of many solutes in solution resembles calculated values of colligative properties.
However in some cases, the experimental values of colligative properties differ widely than those obtained by calculations. Such experimental values of colligative properties are known as abnormal values of colligative properties. The causes for abnormal values of colligative properties are:
(i) Dissociation of solute: It increases the colligative properties.
e.g.: Dissociation of

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etc. in

H_{2} O

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(ii) Association of solute: It decreases the colligative properties.
e.g.: Dimerisation of acetic acid in benzene.

Four different

100 ml

solutions are prepared by mixing 1 gram each of

N a C l, (N H_{2})_{2} C O, N a_{2} S O_{4}

and

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

at a temperature T. Correct order of osmotic pressure is:

Q. The boiling point of 0.1molal

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

solution will be :

(G i v e n K_{b} f o r w a t e r = 0.52 K k g {m o l}^{- 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. A

0.1 M

solution of

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

50 %

dissociated at

27^{\circ} C

. What will be its observed osmotic pressure?

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If a is the degree of dissociation of K4[Fe(CN6)] than an abnormal mass of complex in the solution will be:

If $a$ is the degree of dissociation of $K_{4} [F e (C N_{6})]$ than an abnormal mass of complex in the solution will be: