Chemistry Solutions: Properties, Concentration, and Laws

Types of Solutions

• Solutions are homogeneous mixtures composed of a solute (the substance being dissolved) and a solvent (the dissolving medium).
• Solutions can be categorized based on the state of solute and solvent as solid-solid, solid-liquid, liquid-liquid, and gas-liquid solutions.

Concentration of Solutions

• Concentration measures the amount of solute present in a given amount of solvent or solution.
• Common units of concentration include molarity (M), molality (m), mole fraction (∗X∗), and mass percent (∗w/w∗, ∗w/v∗, or ∗v/v∗).

Colligative Properties

• Colligative properties are properties of solutions that depend only on the number of solute particles and not on their nature.
• These properties include vapor pressure lowering, elevation of boiling point, depression of freezing point, and osmotic pressure.

Raoult's Law

• Raoult's Law states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent in the solution.
• It is applicable to ideal solutions, where the interactions between solute-solute, solvent-solvent, and solute-solvent molecules are similar.

Non-Ideal Solutions

• In non-ideal solutions, deviations from Raoult's Law occur due to interactions between solute and solvent molecules.
• These deviations can lead to positive or negative deviations from ideal behavior.

Colligative Property Calculations

• Various formulas are used to calculate changes in colligative properties such as vapor pressure, boiling point, freezing point, and osmotic pressure based on the number of solute particles present.

Henry's Law

• Henry's Law relates the solubility of a gas in a liquid to the pressure of the gas above the solution.
• It states that the concentration of a dissolved gas is directly proportional to the partial pressure of that gas above the solution.