Isotonic solutions have

Calculate the osmotic pressure exerted by a solution containing $0.822 \ g$ of solute in $300 \ mL$ of water at $300 \ K$. (Molar mass of solute $= 340 \ g \ mol^{-1}, R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1}$) (in $atm$)

In osmosis:

An artificial cell is made by encapsulating $0.2 \ M$ glucose solution within a semipermeable membrane. The osmotic pressure developed when the artificial cell is placed within a $0.05 \ M$ solution of $NaCl$ at $300 \ K$ is . . . . . . . . . .$\times 10^{-1} \ bar$. (Nearest Integer)
[Given : $R=0.083 \ L \ bar \ mol^{-1} \ K^{-1}$ ]
Assume complete dissociation of $NaCl$.

$A$ solution containing $10 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) per liter is isotonic with a $5 \% \ w/v$ solution of a non-volatile solute. The molar mass of the non-volatile solute is ......... $g \ mol^{-1}$.

The osmotic pressure in atmospheres of a $10\%$ solution of cane sugar at $69\,^oC$ is: