Set the following solutions in increasing order of vapour pressure:
$3 m$ $N a_{2} S O_{4}$ ,
$1 m$ $U r e a$
$0.4 m$ $A l C l_{3}$
$0.2 m$ $N a C l$

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Solution

The correct way increasing order is:

$3 m$ $N a_{2} S O_{4}$ < $1 m$ $U r e a$ < $0.4 m$ $A l C l_{3}$ < $0.2 m$ $N a C l$

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Similar questions

Assume 100% ionisation in the following equimolal aqueous solution :

(a) 1m CaCl₂(b) 1m sucrose (c) 1m AlCl₃(d) 1m KCl

Arrange them in the increasing order of osmotic pressure:

0.1 N

.1 N N a C l, 0.1 N

N a_{2} S O_{4}

0.1 N N a_{2} P O_{4}

27^{o} C

N a C l > N a_{2} S O_{4} > N a_{3} P O_{4} > u r e a

π = \frac{Δ T_{b}}{K_{b}} \times S T

The osmotic pressure of equimolar solutions of urea, BaCl2 and AlCl3 will be in the order-

N a C l

u r e a

M g {C l}_{2}

A l C l_{3}

N a C l, M g C l_{2}, A l C l_{3}

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