Colligative Properties of Solutions

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Questions and Answers

What effect do solutes have on the vapor pressure of a solvent?

  • They increase vapor pressure.
  • They completely eliminate vapor pressure.
  • They inhibit solvents from escaping as gas, decreasing vapor pressure. (correct)
  • They do not affect vapor pressure.

What is the primary cause of boiling point elevation when solutes are added to a solvent?

  • Solutes decrease the density of the solvent.
  • Solutes make it more difficult for the solvent to escape as gas, requiring more energy. (correct)
  • The presence of solutes reduces the temperature at which a solvent boils.
  • The solutes increase the heat capacity of the solvent.

In the formula for boiling point elevation, $ ext{Δ}T_b = iK_b m$, what does the variable 'i' represent?

  • The number of dissolved molecules in the solution.
  • The initial temperature of the solvent.
  • The molal concentration of the solute.
  • The number of dissociated particles from the solute. (correct)

Which of the following compounds would have an 'i' value of 2 when dissolved in solution?

<p>Both A and C (A)</p> Signup and view all the answers

What does the constant $K_b$ represent in the formula for boiling point elevation?

<p>The boiling point elevation constant unique to each solvent. (D)</p> Signup and view all the answers

What do colligative properties of solutions depend on?

<p>The number of solute particles (B)</p> Signup and view all the answers

Which colligative property results in a decrease in the vapor pressure of a solution?

<p>Lower Vapor Pressure (A)</p> Signup and view all the answers

What effect does the presence of solute particles have on the boiling point of a solution?

<p>It raises the boiling point (A)</p> Signup and view all the answers

What happens to the freezing point of a solution when solute particles are added?

<p>It decreases (C)</p> Signup and view all the answers

In which type of solution is the effect of solutes on colligative properties most significant?

<p>Highly concentrated solutions (B)</p> Signup and view all the answers

What effect does the addition of a solute have on the vapor pressure of a solvent?

<p>It lowers the vapor pressure. (A)</p> Signup and view all the answers

What formula represents the relationship between molality and boiling point elevation?

<p>$ riangle T_{BP} = i imes K_{bp} imes m$ (A)</p> Signup and view all the answers

What happens to the freezing point of a solvent when a solute is added?

<p>It decreases. (D)</p> Signup and view all the answers

In the context of ionic compounds, what does the van't Hoff factor ($i$) represent?

<p>The number of ions produced when the compound dissolves. (A)</p> Signup and view all the answers

Which colligative property is affected by the number of solute particles present in a solution?

<p>Osmotic pressure of the solution. (D)</p> Signup and view all the answers

Flashcards

Colligative Properties

Properties of solutions that depend on the number of solute particles, not their type.

Lower Vapor Pressure

The vapor pressure of a solution is lower than the pure solvent due to solute particles interfering with solvent molecule escape.

Boiling Point Elevation

Boiling point of a solution is higher than the pure solvent due to reduced solvent vapor pressure.

Freezing Point Depression

Freezing point of a solution is lower than the pure solvent due to solute particles disrupting the solvent structure.

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Concentration and Colligative Properties

The effect of solute particles on colligative properties is greater in more concentrated solutions.

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Change in Boiling Point (ΔTb)

The change in boiling point of a solution compared to the pure solvent.

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Van't Hoff Factor (i)

The number of particles a solute dissociates into when dissolved in a solvent.

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Boiling Point Constant (Kb)

A constant specific to a solvent that relates the molality of a solution to its boiling point elevation.

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Vapor Pressure Depression

The reduction in a solvent's vapor pressure caused by the addition of solute particles.

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Osmotic Pressure

The pressure that must be applied to a solution to prevent the inward flow of pure solvent across a semipermeable membrane.

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