The van’t Hoff factor (i) indicates the number of particles a solute provides when dissolved in a given solvent, usually water, to affect colligative properties such as boiling point elevation and freezing point depression. In non-aqueous solvents, such as ethanol, a slight amount of water as a solute will act as a solute, but because it is a polar covalent molecule dissolving in another polar covalent molecule, its van’t Hoff factor will be 1 (only one particle with no dissociation). Water cannot be considered a solute in itself (water as the solvent), and even if it were, its van’t Hoff factor would only be (55.6 + 2E-7)/55.6≈1, which is the concentration of particles (H2O + H+ + OH–) divided by the concentration of H2O at 25°C. Covalent non-acidic molecules such as glucose have i = 1 since they do not dissociate. Strong acids with 100% dissociation have i ≈ 2 (ion-coupling can reduce the actual factor). Weak acids have i that depends on their Ka but is generally barely above 1. Ionic compounds dissociate into ions and have i ≈ the number of ions (again, reduced due to ion coupling).
The van’t Hoff factor (i) indicates the number of particles a solute provides when dissolved in a given solvent, usually water, to affect colligative properties such as boiling point elevation and freezing point depression. In non-aqueous solvents, such as ethanol, a slight amount of water as a solute will act as a solute, but because it is a polar covalent molecule dissolving in another polar covalent molecule, its van’t Hoff factor will be 1 (only one particle with no dissociation). Water cannot be considered a solute in itself (water as the solvent), and even if it were, its van’t Hoff factor would only be (55.6 + 2E-7)/55.6≈1, which is the concentration of particles (H2O + H+ + OH–) divided by the concentration of H2O at 25°C. Covalent non-acidic molecules such as glucose have i = 1 since they do not dissociate. Strong acids with 100% dissociation have i ≈ 2 (ion-coupling can reduce the actual factor). Weak acids have i that depends on their Ka but is generally barely above 1. Ionic compounds dissociate into ions and have i ≈ the number of ions (again, reduced due to ion coupling).
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The van’t Hoff factor (i) indicates the number of particles a solute provides when dissolved in a given solvent, usually water, to affect colligative properties such as boiling point elevation and freezing point depression. In non-aqueous solvents, such as ethanol, a slight amount of water as a solute will act as a solute, but because it is a polar covalent molecule dissolving in another polar covalent molecule, its van’t Hoff factor will be 1 (only one particle with no dissociation). Water cannot be considered a solute in itself (water as the solvent), and even if it were, its van’t Hoff factor would only be (55.6 + 2E-7)/55.6≈1, which is the concentration of particles (H2O + H+ + OH–) divided by the concentration of H2O at 25°C. Covalent non-acidic molecules such as glucose have i = 1 since they do not dissociate. Strong acids with 100% dissociation have i ≈ 2 (ion-coupling can reduce the actual factor). Weak acids have i that depends on their Ka but is generally barely above 1. Ionic compounds dissociate into ions and have i ≈ the number of ions (again, reduced due to ion coupling).
The van’t Hoff factor (i) indicates the number of particles a solute provides when dissolved in a given solvent, usually water, to affect colligative properties such as boiling point elevation and freezing point depression. In non-aqueous solvents, such as ethanol, a slight amount of water as a solute will act as a solute, but because it is a polar covalent molecule dissolving in another polar covalent molecule, its van’t Hoff factor will be 1 (only one particle with no dissociation). Water cannot be considered a solute in itself (water as the solvent), and even if it were, its van’t Hoff factor would only be (55.6 + 2E-7)/55.6≈1, which is the concentration of particles (H2O + H+ + OH–) divided by the concentration of H2O at 25°C. Covalent non-acidic molecules such as glucose have i = 1 since they do not dissociate. Strong acids with 100% dissociation have i ≈ 2 (ion-coupling can reduce the actual factor). Weak acids have i that depends on their Ka but is generally barely above 1. Ionic compounds dissociate into ions and have i ≈ the number of ions (again, reduced due to ion coupling).
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