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Chapter 12: Problem 68

What is the van't Hoff factor? What information does it provide?

Short Answer

Expert verified
The van't Hoff factor ('i') provides insight into the number of particles a substance can produce in a solution, telling us about its potential to alter a solution's colligative properties like boiling point, freezing point, and osmotic pressure. Essentially, it serves as an indicator of a substance's behavior in a solution.

Step by step solution

01

Definition

The van't Hoff factor, or 'i', is a dimensionless factor used in physical chemistry to account for the effect of solute particles in a solution on its properties. It allows us to estimate the nature and magnitude of colligative properties like boiling point elevation, freezing point depression, and osmotic pressure.
02

Calculation

In theory, the van’t Hoff factor equals the number of particles (ions or molecules) a substance can produce in solution. For example, for non-electrolytes like sucrose that do not dissociate in solution, 'i' equals 1. For electrolytes that do dissociate in solution, like NaCl, 'i' is typically greater than 1. However, in practice, 'i' can be less than the theoretical value due to interactions between solute particles in highly concentrated solutions that briefly bring them together as though they are a single particle.
03

Information 'i' provides

The van't Hoff factor is crucial in predicting the extent of a solute's effect on the colligative property of a solution, helping scientists and chemists understand the solution's behavior. Through 'i', you can estimate whether a substance will dissociate in solution and the extent of its dissociation - whether it's a non-electrolyte, weak electrolyte, or strong electrolyte. Moreover, knowing 'i' can aid in calculating the colligative properties of more complex solutions.

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Most popular questions from this chapter

The osmotic pressure of \(0.010 \mathrm{M}\) solutions of \(\mathrm{CaCl}_{2}\) and urea at \(25^{\circ} \mathrm{C}\) are 0.605 atm and 0.245 atm, respectively. Calculate the van't Hoff factor for the \(\mathrm{CaCl}_{2}\) solution.

Explain why ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}\right)\) is not soluble in cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\)

What are colligative properties? What is the meaning of the word "colligative" in this context?

Use Henry's law and the ideal gas equation to prove the statement that the volume of a gas that dissolves in a given amount of solvent is independent of the pressure of the gas. (Hint: Henry's law can be modified as \(n=k P,\) where \(n\) is the number of moles of the gas dissolved in the solvent.)

Explain each of the following statements: (a) The boiling point of seawater is higher than that of pure water. (b) Carbon dioxide escapes from the solution when the cap is removed from a carbonated softdrink bottle. (c) Molal and molar concentrations of dilute aqueous solutions are approximately equal. (d) In discussing the colligative properties of a solution (other than osmotic pressure), it is preferable to express the concentration in units of molality rather than in molarity. (e) Methanol (b.p. \(65^{\circ} \mathrm{C}\) ) is useful as an antifreeze, but it should be removed from the car radiator during the summer season.
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