Summary of Aqueous Reactions and Properties

General Properties of Aqueous Solutions

• Solution = homogeneous mixture of solute & solvent.

• Solute: smaller amount, Solvent: larger amount.

Electrolytes

• Electrolyte: substance that conducts electricity in water.

• Weak Electrolyte: not completely dissociated (e.g., CH3COOH).

• Strong Electrolyte: completely dissociated (e.g., NaCl).

Precipitation Reactions

• Precipitate: insoluble solid formed from reaction.

• Net ionic equations focus on the ions that participate in a reaction.

Solubility

• Solubility: maximum solute amount that dissolves in a solvent at specific temperature.

• Solubility Rules: e.g., Alkali metals and nitrates are generally soluble.

Acid-Base Reactions

• Arrhenius Acid: produces H+ in water. Arrhenius Base: produces OH- in water.

• Brønsted Acid: proton donor. Brønsted Base: proton acceptor.

• Neutralization Reaction: acid + base → salt + water.

Oxidation-Reduction Reactions

• Electron transfer reactions.

• Oxidation: loss of electrons; Reduction: gain of electrons.

• Oxidation numbers help in identifying oxidation state changes.

Solution Stoichiometry

• Molarity (M) = moles of solute / liters of solution.

• Dilution: MiVi = MfVf, where M = molarity and V = volume.

Titrations

• Used to determine unknown concentrations.

• Equivalence point: completion of reaction, monitored using indicators.