The osmotic pressure at $17 \ ^oC$ of an aqueous solution containing $1.75 \ g$ of sucrose per $150 \ mL$ solution is .......... $atm$.

Calculate the temperature of $0.05 \ M$ sucrose solution in Kelvin if the osmotic pressure of the solution is $1.5 \ atm$. $[R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}]$

For a very dilute solution of an electrolyte,which of the following relations is correct? (Assume other parameters are constant)

What is the relationship between the osmotic pressures of $6.00 \ g \ L^{-1}$ $CH_3COOH$ $(\pi_1)$ and $7.45 \ g \ L^{-1}$ $KCl$ $(\pi_2)$ solutions?

Which one of the following solutions of compounds shows the highest osmotic pressure? ($AB, AB_2$ and $A_2 B_3$ are ionic compounds)

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: