Question

The osmotic pressure of blood is $8.21atm$ at ${37}^{o}C$. How much glucose would be used for an injection that is at the same osmotic pressure as blood?

• A. $22.17g{L}^{-1}$
• B. $58.14g{L}^{-1}$
• C. $61.26g{L}^{-1}$
• D. $75.43g{L}^{-1}$

Answer 1

The correct option is B $58.14g{L}^{-1}$

The osmotic pressure of a solution is the pressure difference needed to stop the flow of solvent across a semipermeable membrane.

$\pi =\frac{nRT}{V}=MRT$

Where $\pi =8.21atm$ is osmotic pressure

$R=0.0821Latm{K}^{-1}mo{l}^{-1}$ is gas constant

$T=37+273=310K$ is temperature

M is the molarity of solute. and n is no. of moles of solute present.

$M=\frac{\pi }{RT}$

$⟹\frac{m}{V}=\frac{8.21\times 180}{0.0821\times 310}=58.14g{L}^{-1}$

So, the correct option is $B$