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Le Chatelier's Principle for Del N Equals to 0

We have two s...

Question

We have two solutions, one is 1 L of 0.1 M $N a C l$ and the other is 2 L of 0.2 M $C a C l_{2}$ . Using only these two solutions, a solution of $2.5 L$ volume can be prepared which has $[C l^{-}] = 0.34 M$ . Calculate the osmotic pressure of the solution prepared.
Given: $t = 300 K, (R = 0.082 L a t m m o l^{- 1} K^{- 1})$

10.8

atm

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12.8

atm

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5.6

atm

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None of these

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Solution

The correct option is B $12.8$ atm
The expression for the osmotic pressure is $π = C R T$

Here, C is the concentration. Its expression is

$C = [C l^{-}] + [N a^{+}] + [C a^{2 +}] = (0.34 + \frac{0.1 \times 0.5}{2.5} + \frac{0.2 \times 2}{2.5}) = 0.34 + 0.02 + 0.16 = 0.52$
Note :

We have to use 500ml of NaCl soln and 2 L of CaCl $_{2}$ solution.

Substitute values in the expression for the osmotic pressure.
$π = 0.52 \times 0.082 \times 300 a t m = 12.792 a t m$

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We have two solutions, one is 1 L of 0.1 M NaCl and the other is 2 L of 0.2 M CaCl2. Using only these two solutions, a solution of 2.5 L volume can be prepared which has [Cl−]=0.34M. Calculate the osmotic pressure of the solution prepared.Given: t=300K,(R=0.082 L atm mol−1K−1)