Blood cells will remain as such in

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

An aqueous solution has an osmotic pressure of $4.92 \text{ atm}$ at $300 \text{ K}$. Calculate the molarity of the solution. $(R = 0.082 \text{ L atm mol}^{-1} \text{ K}^{-1})$ (in $\text{ M}$)

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 are isotonic $(R = 0.082 \ atm \ K^{-1} mol^{-1})$?

Which of the following statements is correct for an aqueous solution of $6 \ g \ L^{-1}$ urea and $17.12 \ g \ L^{-1}$ sucrose? [Molar mass of urea $= 60 \ g \ mol^{-1}$,Molar mass of sucrose $= 342 \ g \ mol^{-1}$]