Question

# A decimolar solution of potassium ferrocyanide is 50% dissociated at 300K. Calculate the osmotic pressure of the solution. (R=8.314JK−1mol−1)

A
3.74×105Nm2
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B
7.482×105Nm2
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C
14.96×105Nm2
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D
14.96×106Nm2
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Solution

## The correct option is C 7.482×105Nm−2K4[Fe(CN)6]⇌4K++[Fe(CN)6]4−Since the solution is 50% dissociated, the Vant Hoff's factor is as follows:i=[1+(n′−1)α]=[1+(5−1)0.5]=1+2=3The osmotic pressure, Π=iCRTHere, i is Vant Hoff's factor, α is the degree of dissociation, C is the molar concentration (0.1), R is the ideal gas constant (0.08206 L atm / mol. K), T is the absolute temperature, 300 KΠ=3×0.1×0.08206×300=7.385 atm=7.482×105 Nm−2∵1 atm=101325 Nm−2

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