1. What is the osmotic pressure of a solution made by dissolving 85.0 g of gluco

Question

1. What is the osmotic pressure of a solution made by dissolving 85.0 g of glucose, C6H12O6, in enough water to form 150.0 mL of solution at 42.0 C ?

2. What is the vapor pressure (in mm Hg) of a solution of 17.5 g of glucose (C6H12O6) in 71.5 g of methanol (CH3OH) at 27C? The vapor pressure of pure methanol at 27C is 140mm Hg.

3. The van't Hoff factor for KCl is i = 1.85. What is the boiling point of a 0.90 m solution of KCl in water? For water, Kb = 0.51(C kg)/mol.

4. A 2.00 M solution of CaCl2 in water has a density of 1.17 g/mL. What is the mole fraction of CaCl2?

Explanation / Answer

1. What is the osmotic pressure of a solution made by dissolving 85.0 g of glucose, C6H12O6, in enough water to form 150.0 mL of solution at 42.0 C ?

P = M*RT

M = mol/L =mass/MWL = 85/(180*0.150) = 3.14814

T = 42+273 = 315

P = (3.14814*0.082*315) = 81.316456 atm

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