Exactly 100 grams of a saturated solution of sucrose in water was determined to contain 67.98 grams of sucrose, C12H22O11. Calculate the osmotic pressure of this solution at 25 C, if the density of the solution is 1.34 grams/ml.
Molar mass of C12H22O11,
MM = 12*MM(C) + 22*MM(H) + 11*MM(O)
= 12*12.01 + 22*1.008 + 11*16.0
= 342.296 g/mol
mass(C12H22O11)= 67.98 g
number of mol of C12H22O11,
n = mass of C12H22O11/molar mass of C12H22O11
=(67.98 g)/(342.296 g/mol)
= 0.1986 mol
use:
density = mass / volume to find volume of solution
volume of solution , V = mass/ density
= 100 g / 1.34 g/mL
= 74.6 mL
= 7.46*10^-2 L
Molarity,
C = number of mol / volume in L
= 0.1986/7.46*10^-2
= 2.662 M
T= 25 oC
= (25+273) K
= 298 K
use:
P = C*R*T
P = 2.662*0.0821*298
P = 65.1 atm
Answer: 65.1 atm
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