The von’t Hoff factor for LiCl at 0.118 m solution at 10 0 C and the osmotic pressure in torr is to be determined. Concept Information: The van't Hoff factor is defined as the ratio between the actual concentration of particles formed when the substance is dissolved and the concentration of the constituent as interpreted from its mass. For most of the non-electrolytes that are dissolved in water, the van't Hoff factor is, generally, 1 . The freezing points of solutions are all lesser as compared to the pure solvent and are directly related to the molality of the solute. Δ T f = T f (solvent) − T f (solution) = i × K f × m Here, Δ T f is the freezing point depression, T f (solution) is the freezing point of the solution, T f (solvent) is the freezing point of the solvent, K f is the freezing point depression constant, and m is the molality. Osmotic pressure can be expressed by following equation: Π = i M R T Here, Π is the osmotic pressure, i is the von’t Hoff factor, M is the molality, R is the gas constant and T is the temperature.
The von’t Hoff factor for LiCl at 0.118 m solution at 10 0 C and the osmotic pressure in torr is to be determined. Concept Information: The van't Hoff factor is defined as the ratio between the actual concentration of particles formed when the substance is dissolved and the concentration of the constituent as interpreted from its mass. For most of the non-electrolytes that are dissolved in water, the van't Hoff factor is, generally, 1 . The freezing points of solutions are all lesser as compared to the pure solvent and are directly related to the molality of the solute. Δ T f = T f (solvent) − T f (solution) = i × K f × m Here, Δ T f is the freezing point depression, T f (solution) is the freezing point of the solution, T f (solvent) is the freezing point of the solvent, K f is the freezing point depression constant, and m is the molality. Osmotic pressure can be expressed by following equation: Π = i M R T Here, Π is the osmotic pressure, i is the von’t Hoff factor, M is the molality, R is the gas constant and T is the temperature.
Solution Summary: The author explains the van't Hoff factor for LiCl and the osmotic pressure in torr. The freezing points of solutions are all lesser as compared to the pure solvent.
The von’t Hoff factor for LiCl at 0.118 m solution at 10 0C and the osmotic pressure in torr is to be determined.
Concept Information:
The van't Hoff factor is defined as the ratio between the actual concentration of particles formed when the substance is dissolved and the concentration of the constituent as interpreted from its mass.
For most of the non-electrolytes that are dissolved in water, the van't Hoff factor is, generally, 1
.
The freezing points of solutions are all lesser as compared to the pure solvent and are directly related to the molality of the solute.
ΔTf=Tf(solvent)−Tf(solution)=i×Kf×m
Here, ΔTf is the freezing point depression, Tf(solution) is the freezing point of the solution, Tf(solvent) is the freezing point of the solvent, Kf is the freezing point depression constant, and m
is the molality.
Osmotic pressure can be expressed by following equation:
Π=iMRT
Here, Π is the osmotic pressure, i is the von’t Hoff factor, M is the molality, R is the gas constant and T is the temperature.