Properties of Solutions

These flashcards cover key concepts from the lecture on the properties of solutions, including definitions, examples, and critical principles you need to know for the exam.

What is the process called when solute concentration increases and solute particles reattach to the solid?

Crystallization.

What is a saturated solution?

A solution at dynamic equilibrium where no more solute can dissolve.

What does 'like dissolves like' imply about solubility?

Polar solutes dissolve best in polar solvents, and nonpolar solutes in nonpolar solvents.

What are the three types of intermolecular forces (IMFs) involved in solution formation?

Solute-solute, solvent-solvent, and solvent-solute interactions.

What happens to the vapor pressure of a solvent when a nonvolatile solute is added?

The vapor pressure of the solvent decreases.

What is Henry's Law?

It states that the solubility of a gas (C) is proportional to its partial pressure (P) over the solution.

What are colligative properties?

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

What is the van’t Hoff factor for NaCl?

2, because it dissociates into Na⁺ and Cl⁻ ions.

How does temperature affect the solubility of gases?

Gases become less soluble as temperature increases.

What is the definition of molarity (M)?

Moles of solute per liter of solution.

What are the effects of solute particles on the freezing point of a solution?

Solute particles lower the freezing point compared to the pure solvent.

What type of solution contains more solute than the solubility limit under specific conditions?

Supersaturated solution.

Why do ionic solutes not dissolve in nonpolar solvents?

Due to weak interactions between the ionic solute and nonpolar solvent.

What is Raoult’s Law?

States that the vapor pressure of a solvent in a solution is equal to the mole fraction of the solvent multiplied by the vapor pressure of the pure solvent.

In what type of solution do solute particles settle over time?

Suspension.

What type of forces are involved in the stabilization of hydrophobic colloids?

Adsorbed ions or emulsifying agents.

What is the formula for calculating the boiling point elevation?

ΔTb = iKb m.

What is a dynamic equilibrium in a solution?

When the rate of dissolution equals the rate of crystallization.

What are the qualitative terms used to describe solution concentration?

Dilute and concentrated.

What is molality (m)?

Moles of solute per kilogram of solvent.

What effect does adding a nonvolatile solute have on the boiling point of a solution?

Raises the boiling point compared to the pure solvent.

What defines a colloid?

A mixture where particles are 1-1000 nm in size and do not settle.

What is the relationship between solubility and temperature for most solids?

Solubility increases as temperature increases.

What is an example of a hydrophilic colloid?

Proteins such as enzymes or antibodies.

What type of solution has particle size greater than 1000 nm?

Suspension.

What happens to a supersaturated solution when disturbed?

It tends to crystallize.

Which type of solute is more soluble in water: polar or nonpolar?

Polar solute.

What is the effect of pressure on the solubility of a gas?

Increases solubility of the gas.

What is the significance of the term 'adsorption' in chemistry?

Particles stick to a surface.

What is the significance of the term 'absorption' in chemistry?

Particles go inside another phase.

What type of suspension is milk classified as?

Emulsion.

How can one predict which solute will dissolve better in a solvent?

Using the principle of 'like dissolves like'.

What is the role of emulsifying agents in a colloid?

They help stabilize mixtures of oil and water.

What describes a nonvolatile solute?

A substance that does not evaporate.

What is the impact of longer nonpolar chains on solubility in water?

Reduces water solubility.

What are molecular compounds that do not dissociate into ions called?

Nonelectrolytes.

What occurs when a solution reaches its saturation point?

Dynamic equilibrium is established; solvation and crystallization occur at equal rates.

What is an example of a volatile substance?

A substance with measurable vapor pressure.

How do ionic solutions behave in terms of colligative properties?

They dissociate into multiple particles, affecting the calculations.

Why are vitamins like vitamin C considered water-soluble?

They contain multiple hydroxyl (OH) groups.

Which has a higher impact on boiling point elevation, ionic or molecular solutes?

Ionic solutes, due to higher van’t Hoff factors.

What phenomenon allows you to see a beam of light passing through a colloid?

Tyndall effect.