The Van’t Hoff factor offers insight on the effect of solutes on the colligative properties of solutions. It is denoted by the symbol ‘i’. The Van’t Hoff factor can be defined as the ratio of the concentration of particles formed when a substance is dissolved to the concentration of the substance by mass.
The extent to which a substance associates or dissociates in a solution is described by the Van’t Hoff factor. For example, when a non-electrolytic substance is dissolved in water, the value of i is generally 1. However, when an ionic compound forms a solution in water, the value of i is equal to the total number of ions present in one formula unit of the substance.
For example, the Van’t Hoff factor of CaCl2 is ideally 3, since it dissociates into one Ca2+ ion and two Cl– ions. However, some of these ions associate with each other in the solution, leading to a decrease in the total number of particles in the solution.
This factor is named after the Dutch physical chemist Jacobus Henricus Van’t Hoff, who won the first Nobel Prize in chemistry. It is important to note that the measured value of the Van’t Hoff factor for electrolytic solutions is generally lower than the predicted value (due to the pairing of ions). The greater the charge on the ions, the greater the deviation.
Effects of Association/Dissociation
Association is the joining of two or more particles to form one entity.
An example of the association of two particles is the dimerization of carboxylic acids when dissolved in benzene.
Dissociation refers to the splitting of a molecule into multiple ionic entities.
For example, sodium chloride (NaCl) dissociates into Na+ and Cl– ions when dissolved in water.
Meghna Thapar 4 years ago
The Van’t Hoff factor offers insight on the effect of solutes on the colligative properties of solutions. It is denoted by the symbol ‘i’. The Van’t Hoff factor can be defined as the ratio of the concentration of particles formed when a substance is dissolved to the concentration of the substance by mass.
The extent to which a substance associates or dissociates in a solution is described by the Van’t Hoff factor. For example, when a non-electrolytic substance is dissolved in water, the value of i is generally 1. However, when an ionic compound forms a solution in water, the value of i is equal to the total number of ions present in one formula unit of the substance.
For example, the Van’t Hoff factor of CaCl2 is ideally 3, since it dissociates into one Ca2+ ion and two Cl– ions. However, some of these ions associate with each other in the solution, leading to a decrease in the total number of particles in the solution.
This factor is named after the Dutch physical chemist Jacobus Henricus Van’t Hoff, who won the first Nobel Prize in chemistry. It is important to note that the measured value of the Van’t Hoff factor for electrolytic solutions is generally lower than the predicted value (due to the pairing of ions). The greater the charge on the ions, the greater the deviation.
Effects of Association/Dissociation
Association is the joining of two or more particles to form one entity.
An example of the association of two particles is the dimerization of carboxylic acids when dissolved in benzene.
Dissociation refers to the splitting of a molecule into multiple ionic entities.
For example, sodium chloride (NaCl) dissociates into Na+ and Cl– ions when dissolved in water.
0Thank You