Aqueous Solutions

Lesson One Notes

• Chemicals can be classified as

  • Salts - Ionic (metal + nonmetal) (CuCl)

  • Molecules - Covalent (only nonmetals0

  • Acids - begins with H (HCl)

  • Bases - Ends with OH (NaOH

• Chemicals dissolving in water

  • Soluble - Dissolves in water, (aq)

  • Insoluble - Doesn’t dissolve in water (s)

    • Ionic compounds will dissolve in water if:

      • They contain an alkali metal (Group 1)

      • They contain ammonium (NH₄⁺)

      • They contain Nitrate (NO₃⁻)

    • Covalent substances do not dissolve in water

• Water Molecules

  • The forces in water pull cations and anions apart to dissolve some ionic compounds

  • Since covalent substances do not have ions, they cannot be ionized

• Electrolytes

  • Strong electrolytes - Dissolve in water and conduct electricity

  • Nonelectrolyte - doesn’t dissolve in water and doesn’t conduct electricity

Lesson Two Notes

• Strong acids

  • HCl, HBr, HClO4, H2SO4, HNO3

• Strong Bases

  • Group one hydroxide (NaOH) (Ca, Sr, Ba + Hydroxide)

• strong acids and bases completely ionize in water

  • Weak acids and bases bairly ionize

  • If it dissolves partially in water, it is a weak electrolyte bairly conducts electricity

• Naming acids

• Precipitation - Double displacement. Only happens if an insoluble product forms.

• Spectator ions are omitted from an equation to simplify it

  • The new equation is called the net ionic equation

Lesson Three Notes

• In strong acids and bases, there are spectator ions

• The H+ ion in a strong acid is NOT the spectator ions

• The OH- ion in a strong base is NOT the spectator ion

  • The other ion is the spectator ion

• Nonmetal oxides react with water to form acids

• Meta oxides react with water to form bases