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19 September, 22:11

An aqueous dextrose solution having a density of 1.04 g/cm3 freezes at - 1.15°C. Find the osmotic pressure of this solution at 25°C. Kf of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

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  1. 19 September, 22:18
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    K=14.1 atm

    Explanation:

    1.15 = m x 1.86

    m = 0.618 = > 0.618 moles in 1 Kg of water

    mass dextrose = 0.618 mol x 180.16 g/mol=111.3 g

    mass solution = 1000 g + 111.3 = 1111 g

    Volume solution = 1111 / 1.04 g/cm^3 = 1069 cm^3 = 1.069 dm^3

    molarity = 0.618 / 1.069=0.578

    osmotic pressure = M x R x T = 0.578 x 0.08206 x 298

    K=14.1 atm
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