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Van't Hoff Factor

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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 $KCl, NaCl$ etc. in $H_{2} O$ .
(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:

A

(N H_{2})_{2} C O

solution > NaCl solution >

N a_{2} S O_{4}

solution >

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

solution

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B

NaCl solution >

N a_{2} S O_{4}

solution >

(N H_{2})_{2} C O

solution >

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

solution

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C

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

solution >

N a_{2} S O_{4}

solution > NaCl solution >

(N H_{2})_{2} C O

solution

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D

N a_{2} S O_{4}

solution >

(N H_{2})_{2} C O

solution >

NaCl

solution >

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

solution

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Solution

The correct option is B NaCl solution > $N a_{2} S O_{4}$ solution > $(N H_{2})_{2} C O$ solution > $K_{4} [F e (C N)_{6}]$ solution
$N a C l$ solution
$n_{N a C l}$ = $\frac{1}{58.5}$ in 100 ml
in 1000 ml = $\frac{1 \times 10}{58.5}$ = 0.17
$π = C \times R \times T \times n$
$π = 0.17 \times R \times T \times 2$
= 0.34RT

$N a_{2} S O_{4}$ solution
$n_{N a_{2} S O_{4}}$ = $\frac{1}{142.04}$ in 100 ml
in 1000 ml = $\frac{1 \times 10}{142.04}$ = 0.007
$π = C \times R \times T \times n$
$π = 0.007 \times R \times T \times 3$
= 0.021RT

$(N H_{2})_{2} C O$ solution
$n_{(N H_{2})_{2} C O}$ = $\frac{1}{60}$ in 100 ml
in 1000 ml = $\frac{1 \times 10}{60}$ = 0.016
$π = C \times R \times T \times n$
$π = 0.016 \times R \times T \times 1$
= 0.016RT

$K_{4} [F e (C N)_{6}]$ solution
$n_{K_{4} [[F e (C N)_{6}]}$ = $\frac{1}{368.35}$ in 100 ml
in 1000 ml = $\frac{1 \times 10}{368.35}$ = 0.0027
$π = C \times R \times T \times n$
$π = 0.0027 \times R \times T \times 5$
= 0.0027RT

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Similar questions

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

KCl, NaCl

H_{2} O

.
(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}

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

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

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

KCl, NaCl

H_{2} O

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

If the degree of dissociation of an electrolyte

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is 25% in a solvent, then:

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

KCl, NaCl

H_{2} O

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

One mole of

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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

KCl, NaCl

H_{2} O

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

If the degree of dissociation of an electrolyte

A_{2} B_{3}

is 25% in a solvent, then:

Q. The ratio of the value of any colligative property for

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

solution to that of

{F e}_{4} {[F e {(C N)}_{6}]}_{3}

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