Colligative Properties and Chemical Kinetics Review

Flashcards covering key concepts from the lecture notes on colligative properties, including vapor pressure, freezing point depression, boiling point elevation, osmosis, and basic chemical kinetics.

Colligative Properties

Properties whose value depends only on the number of solute particles, not on their identity. Their value depends on the concentration of the solution.

Vapor Pressure Lowering

The phenomenon where the vapor pressure of a solvent above a solution is lower than the vapor pressure of the pure solvent due to solute particles replacing some solvent molecules at the surface.

Raoult's Law

A law that describes the vapor pressure of a solvent above a solution, often expressed as Psolution = Xsolvent * Ppuresolvent.

Freezing Point Depression ("ΔTf")

A colligative property where the freezing point of a solution is lower than that of the pure solvent, calculated as ΔTf = Kf * m.

Boiling Point Elevation ("ΔTb")

A colligative property where the boiling point of a solution is higher than that of the pure solvent, calculated as ΔTb = Kb * m.

Osmosis

The flow of solvent from a solution of low concentration into a solution of high concentration across a semi-permeable membrane.

Semi-permeable membrane

A membrane that allows solvent molecules to flow through it but not solute particles.

Osmotic Pressure ("π")

The pressure required to stop the flow of solvent across a semi-permeable membrane, given by the formula πV = nRT or π = MRT.

Van't Hoff Factor ("i")

A factor that accounts for the number of particles an electrolyte dissociates into in a solution, used in colligative property calculations (e.g., ΔTf = i * Kf * m).

Ion Pairing

The association of oppositely charged ions in an electrolyte solution, which can cause the measured Van't Hoff factor to be less than the expected value.

Rate Law

An expression that relates the rate of a chemical reaction to the concentrations of its reactants, typically in the form Rate = k[A]^n[B]^m.

Order of Reaction

The exponent to which a reactant's concentration is raised in the rate law. The 'overall order' is the sum of the individual orders for all reactants.