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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, 95.21g (mol .wt) will be present in `(100 xx 95.21)/(5 xx 1000)=1.904L`
Now, `pi V= ST` (Since n=1)
or `pi= (ST)/(V) rArr pi = (0.082 xx 273)/(1.904)=11.76` atm
van.t Hoff factor, `i= ("Actual number of particles in solution")/("Number of particles taken")`
Degree of dissocition, `alpha = (i-1)/(n-1)` (Here, n=3)
`alpha= ((16)/(11.76)-1)/(3-1)=0.1802 or 18.02%`
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