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Question

A decimolar solution of K4[Fe(CN)6] is 50% dissociated at 300 K. Calculate the Osmotic pressure of solution.

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Solution

Degree of dissociation, x=50%=0.5
Van't Hoff factor, i=number of moles after dissociationtotal number of moles initially=1+4x1
i=1+4(0.5)=1+2=3
Decimolar solution means the molarity of solution is M/10 or 0.1 M. That is, 0.1 mole of solute is dissolved in 1 L of solution. Since, 1 L=1/1000 m3, therefore it can be said, 0.1 mole of solute is dissolved in 1/1000 m3 volume of solution.
We have, πV=i nRT
π=nVRT
π=osmotic pressure
V=volume of solution
n=number of moles of solute
R=universal gas constant=8.314 Nm mol1K1
T=temperature=300K
i=Vant Hoff factor=3
π=3×0.10.001×8.314×300
π=7.48×105 Nm2=7.48×1051.013×105atm
π=7.38 atm

1140701_1173148_ans_7f62756dbb174217be07a2976c737634.jpg

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