A sample of a volatile liquid was found to have a vapour density of 30. If 0.2 moles of the liquid occupies 4.9 L at 1 atm and 273 K, what is the abnormal molar mass of the liquid?

A sample of a volatile liquid was found to have a vapour density of 30. If 0.2 moles of the liquid occupies 4.9 L at 1 atm and 273 K, what is the abnormal molar mass of the liquid?

The van't Hoff factor for 0.1 M $Ba(NO_3)_2$ solution at 25 °C is 2.74. The degree of dissociation is:

Which of the following colligative property is used to determine molar masses of proteins ?

A dilute aqueous solution of a certain electrolyte shows a freezing point depression three times greater than that of a non-electrolyte solution of the same molality. Assuming complete dissociation, how many ions are formed when one formula unit of the electrolyte dissolves?

The van’t Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is

A certain substance ‘A’ tetramerises in water to the extent of 80%. A solution of 2.5 g of A in 100 g of water lowers the freezing point by $0.3^\circ C$. The molar mass of A is

If a solute undergoes dissociation in a solvent, its observed molar mass will be:

The vapour density of undecomposed ${{\rm{N}}_2}{{\rm{O}}_4}$ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to ${\rm{N}}{{\rm{O}}_2}.$ The per cent dissociation of ${{\rm{N}}_2}{{\rm{O}}_4}$ at the final temperature is :

Which of the following electrolytes will have the highest van't Hoff factor (i) in a dilute aqueous solution, assuming complete dissociation?

(a) NaCl

(b) $CaCl_2$

(c) $Na_3PO_4$

(d) $MgSO_4$

A solute when distributed between two immiscible phases remains associated in phase II and dissociated in phase I. If αis the degree of dissociation and n is the number of molecules associated then :