The osmotic pressure of the blood is $7.65\;atm$ at $37 ^ oC$. Calculate the mass of glucose $(C_6H_{12}O_6)$ dissolved per liter of intravenous solution to have the same osmotic pressure as blood!
$\Pi=[glucose]RT$ $[glucose]=\frac{\Pi}{RT}=\frac{7.65}{0.082\;310.15}=0.30\frac{mol}{L}$ $n_{glucose}=[glucose]\cdot 1=0.301\;mol$ $m_{glucose}=n_{glucose}\cdot M_{glucose}=0.301 \cdot 180=54.1\;g$
