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A 5% solution of anhydrous MgCl2 at 0^@ ...

A 5% solution of anhydrous `MgCl_2` at `0^@` developed 16 atm osmotic pressure. What is the degree of dissociation of `MgCl_2?`

Text Solution

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Mass of `MgCl_2` is present in 100ml of solution =5g
Therefore, 95.21 g(mol. wt.) will be present in `(100 xx 95.21)/(5 xx 1000)=1.904L`
Now, `piV=ST" (Since n=1)"`
or `pi=(ST)/(V) rArr pi=(0.082 xx 273)/(1.904)=11.76atm`
van't Hoff factor `i=("Actual number of particles in solution")/("Number of particles taken")`
Degree of dissociation `alpha=(i-1)/(n-1)`
`alpha=((16)/(11.76)-1)/(3-1)=0.1802 or 18.02%`
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