# the osmotic pressure of solution of non volatile , non -electrolyte solute is 7.6 atm at 27 degree celcius , then boiling point of same solution is (kb and molarity same)

Dear Student,

For finding the boiling point of the solution, we will firstly calculate the concentration by using the formula:

$\mathrm{\pi }=\mathrm{mRT}$
m = molality (concentration)
R = 0.0821 L atm mol-1 K-1 (Gas constant)
T = 27o C = 300 K   (Temperature)
$\mathrm{\pi }$ = 7.6 atm  (Osmotic pressure)

Now, we will calculate the Elevation in freezing point by using the relation:

Kb = 0.512 °C/molal     (Since, no information is given about Kb, so I am assuming that we have water as a solvent & this is the boiling point constant of water)
m = 0.31 mol/kg

So,

Now, finally the boiling point will be,

Hope it Helps!!

Regards

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