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Question

100 mg of a protein is dissolved in just enough water to make 10.0 mL of solution. If this solution has an osmotic pressure of 13.3 mm Hg at $${ 25 }^{ 0 }C$$, what is the molar mass of the protein? 
[R=0.0821 L atm $${ mol }^{ -1 }$$ $$K^{ -1 }$$ and 760 mm Hg=1 atm]


Solution

Mass of protein $$(w_2) =0.1$$$$ g$$
$$R=0.082$$ $$L atm/(k mol)$$
$$T = 298 K$$
$$\pi=13.33$$ mm of Hg $$= \cfrac{13.33}{760}=0.0175\ atm$$

volume of solution $$=0.01L$$
Using,
$$M_2 = \cfrac{W_2RT} { πV}$$
We get
$$M_2 = \cfrac{0.1\times0.082\times298} { 0.0175\times0.01}
$$$$= 13963.42\ g/mol$$

Chemistry

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