What is the osmotic pressure of an intravenous solution prepared by dissolving 44.0 g of dextrose (sugar), C6H12O6, in enough water to make 1.00 L of solution? Dextrose is a nonelectrolyte and body temperature is 37.0 ∘C.

6.20atm

Explanation:

Volume = 1L

Mass of dextrose (C6H12O6) = 44g

First, let us calculate the molarity of dextrose sugar. This is illustrated below:

Molar Mass of dextrose (C6H12O6) = (12x6) + (12x1) + (16x6) = 72 + 12 + 96 = 180g/mol

Number of mole of dextrose = Mass / Molar Mass = 44/180 = 0.244mol

Molarity of dextrose = mole / Volume

Molarity of dextrose = 0.244/1

Molarity = 0.244mol/L

Using the osmotic pressure formula, we can simply solve as illustrated below:

Π = iMRT

i = 1 (since dextrose is non electrolyte)

M = 0.244mol/L

R = 0.082atm. L/K / mol

T = 37°C = 37 + 273 = 310K

Π = ?

Π = iMRT

Π = 1 x 0.244 x 0.082 x 310

Π = 6.20atm