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What is the molar mass of the sugar? 262.0 mL sample of sugar?

A 262.mL sample of a sugar solution containing 1.22 g of the sugar has an osmotic pressure of 30.3 mm Hg at 35 degrees C.

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  • Dr W
    Lv 7
    5 年前

    "morse" equation

    .. P = i M R T

    where

    .. P = osmotic pressure = 30.3mmHg

    .. i = van't hoff factor = # of particles 1 particle of solute dissociates into = 1 in this case

    .. M = molality = moles solute / Liter solution

    .. R = gas constant = 0.08206 Latm/molK

    .. T = temp in K = 308.15K

    a few quick examples of i for further problems

    .. 1 NaCl --> 1 Na(+) + 1 Cl(-).. 1 particle --> 2 particles... i=2

    .. 1 MgCl2 --> 1 Mg(+2) + 2 Cl(-).. 1 particle ---> 3 particles.. i=3

    .. 1 glucose --> 1 glucose.. glucose doesn't dissociate.. 1 --> 1 particle... i=1

    ***********

    this problem

    .. (1) use that equation and solve for M

    .. (2) use volume solution (262mL) and M to determine moles solute

    .. (3) molar mass = mass / mole

    *******

    *******

    more hints

    .. M = P / (i x R x T) = 30.3mmHg x (1atm/760mmHg) / (1 x 0.08206Latm/molK x 308.15K)

    .. M = ___ mol solute / liter solution

    then

    .. 262.0mL x (1L / 1000mL) x (___ mol / Liter) = ___ mol solute

    then

    .. molar mass = 1.22g / ___ mol solute = ___ g/mol

    you get to finish

    ********

    btw.. the number i get about 3000g/mol is very high. But there are some polysaccharides in that range.

    https://en.wikipedia.org/wiki/Polysaccharide

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