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:

A solute exhibits an observed molar mass twice its normal molar mass in a particular solvent. What is the van't Hoff factor (i) for this solute in that solvent?

Acetic acid on dissolution in benzene will show :

The van’t Hoff factor $i$ for a compound which undergoes dissociation in one solvent and association in other solvent is respectively

The van’t Hoff factor $i$ for a compound which undergoes dissociation in one solvent and association in other solvent is respectively

The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of van’t Hoff factor, ‘i’ is :

The experimental molar mass of a solute is found to be lower than its theoretical value. This indicates:

If the observed osmotic pressure of a 0.1 M solution of $K_2SO_4$ is 3 times the expected value for a non-electrolyte at the same temperature, what is the van't Hoff factor (i)?

Which of the following is incorrect?

0.2 molal aqueous solution of a monobasic acid is 60% ionised. If Kb for water is $0.52\,K\,kg\,mo{l^{ - 1}}$ then the boiling point of the solution will be

A substance is completely trimerised on dissolution in a solvent. The van’t Hoff factor (i) for such change is :