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20 January, 12:35

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.

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  1. 20 January, 16:03
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    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
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