Aqueous Chemistry and Solutions

Concentration: Amount of solute divided by amount of solvent or solution.
Molarity (M): Defined as moles of solute per liter of solution.
- Symbol: Capital M.
- Acts as a conversion factor (moles/liter or liter/moles).

Process: Dissolve a calculated mass of solute in sufficient water to achieve the desired total solution volume (V).

Process of reducing a solution's concentration by adding more solvent (typically water).
Formula: C1V1 = C2V2 (where C is concentration and V is volume).
Moles of solute are conserved during dilution.
Important: This formula is exclusively for dilution problems, not stoichiometry.

Covalent Compounds (e.g., sugar, alcohol): Disperse in water but do not ionize.
Ionic Compounds: Water 'separates' ionic compounds into individual ions.
Acids:
- Strong Acids: Completely ionize in water (all hydrogen atoms are lost as ions).
- Weak Acids: Partially ionize in water (only some hydrogen atoms are lost as ions).
Polyatomic Ions: Remain intact as a single unit when dissolved; they do not further dissociate (e.g., SO4^{2-}, NO3^{-}).

Substances that form ions in solution and conduct electricity.
Pure water: A poor conductor of electricity.
Pure ionic compound (solid): A poor conductor of electricity.
Aqueous ionic compound solution (e.g., salt water): A good conductor of electricity.

Not all ionic compounds are soluble in water; solubility rules predict this.
Equation Types:
- Molecular Equation: A balanced chemical equation showing complete formulas and phase scripts ((s), (l), (g), (aq)).
- Total Ionic Equation: Shows all soluble ionic compounds as their dissociated ions.
- Net Ionic Equation: Represents only the species directly involved in the chemical change, excluding spectator ions.
Spectator Ions: Ions present in the solution that do not participate in the chemical reaction.

Precipitation Reactions: Occur when two aqueous solutions are mixed, leading to the formation of an insoluble solid (precipitate).
Acid-base reactions are also covered.