• aqueous solutions – solutions in which water is the dissolving medium

• solution – homogeneous mixture of two or more substances
• solvent – component that is present in greatest quantity
• solutes – substances dissolved in the solvent

• concentration – the amount of solute dissolved in a given quantity of solvent or solution
• molarity – number of moles of solute in a liter of solution

• dilution - obtaining a lower concentration of a solution by adding water
• moles solute before dilution = moles solute after dilution

• electrolyte – substance whose aqueous solution contains ions
• nonelectrolyte – substance that does not form ions in solution

• dissociate – when ions separate from a solid being dissolved

• the molecular structure is maintained

• strong electrolytes – ionic compounds that exists entirely of ions in solution
• weak electryolytes – molecular compounds that produce a small amound of ions
• chemical equilibrium – equilibrium of forming ions and recrystalizing ions

• substances that ionize to form hydrogen ions
• proton donors

• substances that ionize to form hydroxide ions

• strong acid, strong base – strong electrolyte
• weak acid, weak base – weak electrolyte

• neutralization reaction – when an acid and base are mixed
• produces water and a salt

• molecular formula – and equation written to show the complete chemical formulas of reactants and products
• spectator ions – ions that do not play a role in a reaction
• net ionic equation – equation where the spectator ions are removed
• only soluble strong electrolytes are written in ionic form

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• for methathesis to occur:
• 1) the formation of an insoluble product
• 2) the formation of either a weak electrolyte or a nonelectrolyte
• 3) the formation of a gas that escapes from solution

• precipitate – insoluble solid formed by a reaction in solution
• solubility – amount of substance that can be dissolved in a given quantity

• all common ionic compounds of the alkali metal ions and of the ammonium ion are soluble in water

• hydrogen and hydroxide react to form water
• insoluble metal oxides react with acids

• carbonates and bicarbonates

• oxidation – loss of electrons
• reduction – gain of electrons

• whenever one substance is oxidized, some other substance must be reduced
• metals react with acids to form salts and hydrogen gas

• activity series – list of metals arranged in order of decreasing ease of oxidation
• active metals – alkali metals and alkaline earth metals
• any metla on the list can be oxidized by ions of elements below it

• statndard solution – solution of known concentration
• titration – a known solution that undergoes a specific chemical reaction of known stoichiometry with the solution of unknown concentration
• equivalence point – stoichiometrically equivalent quantities of reactants are brought together
• indicator – used to show the endpoint of the titration