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7 March, 22:33

An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 ml of solution. the solution has an osmotic pressure of 1.2 atm at 25 °c. what is the molar mass (g/mole) of the compound?

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  1. 7 March, 22:39
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    M=n (pie) / RT

    n=osmotic pressure (1.2 atm)

    M=molar of the solution

    R=gas constant (0.0821)

    T = temperature in kelvin 25+273

    M=[1.2atm / (0.0821L atm/k mol x 298k) ]=0.049mol L

    M = moles of the solute / litres of solution (250/1000)

    0.049 = y/0.25

    moles of solute is therefore = 0.01225mol

    molar mass=33.29 g/0.01225mol=2.7 x10^3g/mol
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