What is the osmotic pressure of a solution made by dissolving 85.0 g of glucose, C6H12O6, in enough water to form 525.0 mL of solution at 25.0 ∘C ?

Answer 1

Osmotic pressure (π) = MRT

M = molarity = moles/liter = 85.0 g x 1 mol/180g/0.525 L = 0.899 M

R = gas constant = 0.0821 Latm/Kmol

T = temperature in K = 25.0 + 273 = 298K

π = (0.899 M)(0.0821 Latm/Kmol)(298K) = 21.99 atm = 22.0 atm (to 3 significant figures)