The vapor pressure of water at 25 degrees Celsius is
23.76 mm of Hg; Kf for water is 1.86 (degree Celsius kg/mol). The
normal boiling point of chloroform is 61.0 degrees Celsius and Kb
is 3.63 (degree Celsius kg/mol) R=0.08206 (L atm/mol.k).
1. What is the vapor pressure of a solution on 10.0g of NaNO3 in
25.0g of water?
2. What is the freezing point of a 0.20 m
aqueous solution of sucrose at 1 atm pressure?
3. What is the osmotic pressure, pi, of a 0.100 M aqueous solution
of a CaCl2 at 25 degrees Celsius
1) We know from Raoult's law
P0-P/P0 = i x mole fraction of solute
P0 = 23.76 mm and i = 2 for NaNO3(two ions)
mole fraction of NaNO3 = (10/85) /[(10/85) + 25/18]
= 0.1176/1.50
Thus 23.76-P /23.76 = 2 x [0.1176/1.5]
P = 20.03mm
2) depression in freezing point is calculated
Delta Tf = i xKf x m
= 1x 1.86 x 0.2
= 0.372
Thus the freezing point of solution = 0C -0.372
= -0.372C
3) We can calculate osmotic pressure using
pi = i x CRT where C = molar concentration
R = gas constant
T= temperature in K
pi = 3 x 0.100mol/L x 0.08206 L.atm/K.mol x 298K
= 7.34atm
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