Chapter 13 and Chapter 14

Hydration

A specific type of solvation where the solvent is water, involving interactions between solute and solvent molecules.

Enthalpy Change (ΔHsoln)

The overall enthalpy change for solution formation, including the separation of solute molecules (ΔH1), separation of solvent molecules (ΔH2), and formation of solute-solvent interactions (ΔH3).

Spontaneous Processes

Processes that occur naturally and favor a decrease in energy (exothermic) and an increase in disorder (entropy).

Dynamic Equilibrium in Saturated Solutions

A state where dissolution and crystallization processes occur at equal rates in a saturated solution.

Solubility

The amount of solute required to saturate a solution.

Like Dissolves Like

A principle stating that polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.

Henry's Law

A principle stating that the solubility of a gas in a liquid increases with increasing pressure, expressed as Cg = kPg.

Molarity (M)

A measure of concentration defined as the moles of solute divided by the liters of solution.

Colligative Properties

Properties that depend on the number of solute particles in a solution, not on their identity.

Tyndall Effect

The scattering of light by colloid particles, demonstrating their presence in a mixture.

Reaction Rate

The speed at which a chemical reaction occurs, typically expressed in molarity per second (M/s).

Activation Energy (Ea)

The minimum energy required for a reaction to occur, crucial for determining reaction rates.

Arrhenius Equation

An equation that shows the relationship between the rate constant (k) and temperature, k = Ae^(-Ea/RT).

Catalyst

A substance that increases the rate of a reaction without being consumed in the process.

Enzyme

Biological catalysts that facilitate biochemical reactions in living organisms.

Lock-and-Key Model

A model describing how a substrate precisely fits into the active site of an enzyme.