The empirical formula of a nonelectrolyte is $C{H_2}O$. A solution containing 3 g of the compound exerts the same osmotic pressure as that of $0.05\;M$ glucose solution. The molecular formula of the compound is

Which of the following aqueous solutions, each containing 10g of solute in 250 ml of water, will have the highest osmotic pressure? (A) Glucose ($C_6H_{12}O_6$) (B) Urea ($CH_4N_2O$) (C) Sucrose ($C_{12}H_{22}O_{11}$) (D) Fructose ($C_6H_{12}O_6$)

A solution of sucrose (Molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure $(R = 0.082\;{\rm{ }}L{\rm{ }}atm\;{{\rm{K}}^{ - 1}}\;{\rm{mo}}{{\rm{l}}^{ - 1}})$ at 273 K?

At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?

(Mol. wt NaCl =58.5, ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4} = 98.0\;{\rm{g}}{\rm{.mo}}{{\rm{l}}^{ - 1}})$

The phenomenon in which cells are shrinked down if placed in hypertonic solution is called :

Which of the given solutions has highest osmotic pressure?

Two isotonic solutions, A and B, are separated by a semipermeable membrane. Solution A contains a non-electrolyte solute, while solution B contains an electrolyte solute that dissociates into two ions. Which statement accurately describes the initial net movement of solvent?

${\rm{0}}{\rm{.004}}\;{\rm{M}}\;{\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is isotonic with 0.01 M glucose.Degree of dissociation of ${\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is

The following solutions were prepared by dissolving 10 g of glucose $({C_6}{H_{12}}{O_6})$ in 250 ml of water $({P_1}),$ 10 g of

Urea $(C{H_4}{N_2}O)$ in 250 ml of $({P_2})$ and 10 g of sucrose $\left( {{C_{12}}{H_{12}}{O_{11}}} \right)$ in 250 ml of water $({P_3}).$ The right option for the decreasing order of osmotic pressure of these solutions is:

Which of the following shows maximum depression in freezing point?

Water will boil at 101.5$^\circ C$ at which of the following pressure?