When 10.0 mg of sucrose is dissolved in enough water to make 100.0 mL of solution at 25.00 °C, an osmotic pressure of 5.43 mmHg is measured. What is the molar mass of sucrose? Show your work, and provide your answer in g/mol.
P= 5.43 mm Hg
= (5.43/760) atm
= 0.0071 atm
T= 25.0 oC
= (25.0+273) K
= 298 K
use:
P = C*R*T
7.145*10^-3 = C*0.08206*298.0
C =2.922*10^-4 M
volume , V = 1*10^2 mL
= 0.1 L
use:
number of mol,
n = Molarity * Volume
= 2.922*10^-4*0.1
= 2.922*10^-5 mol
mass(solute)= 10.0 mg
= 0.01 g
use:
number of mol = mass / molar mass
2.922*10^-5 mol = (0.01 g)/molar mass
molar mass = 3.423*10^2 g/mol
Answer: 3.42*10^2 g/mol
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