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?

Equimolal solutions will have the same boiling point, provided they do not show :

At $100^{\circ}C$, a solution of $5g$ of a non-volatile solute in $100g$ of benzene has a vapour pressure of $745 mmHg$. If $K_b$ for benzene is $2.53$, calculate the boiling point elevation of this solution.

The slope of a graph plotting osmotic pressure ($\Pi$) against concentration ($\mathrm{mol\ L^{-1}}$) is found to be $41.46 \mathrm{L\ bar\ mol^{-1}}$. Using the ideal gas constant $\mathrm{R}=0.083 \mathrm{L\ bar\ mol^{-1} K^{-1}}$, determine the temperature at which the osmotic pressure measurements were conducted.

The depression in f. p. of 0.01 ${\rm{m}}$ aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio :

$X$ is dissolved in water. Maximum boiling point is observed when $X$ is ….($0.1\;M$ each)

The vapour pressure will be lowest of

The mass of glucose that should be dissolved in 50 g of water in order to produce the same lowering of vapour pressure as is produced by dissolving 1 g of urea in the same quantity of water is

Two solutions of glucose have osmotic pressure 1.0 and 3.5 atm. If 1 L of first solution is mixed with V L of second solution, the osmotic pressure of the resultant solution becomes 2.5 atm. Volume of second solution is

The freezing point of the 0.05 molal solution of non-electrolyte in water is

Osmotic pressure of blood is 7.65 atm at 310 K. An aqueous solution of glucose that will be isotonic with blood is ……….wt./vol.