Question

There is a solution of 200 g of glucose $\left(C_6{H}_{12}{O}_6\right)$, containing 7.2 g of solute. The temperature of the solution is ${27}^{o}C$. Calculate the osmotic pressure of the solution.

Answer 1

Molar mass of $C_6{H}_{12}{O}_6=180g$

$\text{Moles of glucose}{C}_6{H}_{12}{O}_6=\frac{7.2}{180}=0.04moles$

Mass of solution $=200g$

Since, $1g=1ml$, therefore, Volume of solution $=200ml=0.2L$

We know, $\pi =MRT$

where, $\pi =$ osmotic pressure

$M=$ molarity of solution

$R=$ universal gas constant

$T=$ temperature $=27+273=300K$

$\pi =\frac{0.04}{0.2}\times 831\times 300$

$\pi =49,860kPa=4.986\times {10}^{4}kPa=498.6atm$