Calculate the osmotic pressure of a solution containing $0.025 \ mol$ of glucose in $100 \ mL$ of water at $300 \ K$. $\left[R = 0.082 \ atm \ dm^3 \ mol^{-1} \ K^{-1}\right]$ (in $atm$)

Which of the following pairs of solutions is expected to be isotonic at the same temperature?

In an osmosis process,the volume of the solution:

$A$ solution of a nonvolatile solute is obtained by dissolving $0.8 \ g$ in $0.3 \ dm^3$ of water. The solution has an osmotic pressure of $0.2 \ atm$ at $300 \ K$. Calculate the molar mass of the solute. $[R = 0.082 \ atm \ dm^3 \ K^{-1} \ mol^{-1}]$

When $10 \ g$ of glucose (osmotic pressure $P_1$),$10 \ g$ of urea (osmotic pressure $P_2$),and $10 \ g$ of sucrose (osmotic pressure $P_3$) are dissolved in $250 \ mL$ of water,the correct relationship between the osmotic pressures of these solutions is:

Which of the following aqueous solutions should have the highest osmotic pressure?