CHM 101 Lecture Notes - Lecture 4: Aqueous Solution, Strong Electrolyte, Chemical Equation
Document Summary
Solution: homogenous fixture of 2 or more substances. Aqueous solution: a solution where solvent is water. Dissolve: solvent molecules surround and support solute molecules or ions. Strong electrolytes: conduct electricity when dissolved in water. Fully dissociates/ionizes: breaks up into cations and anions. Weak electrolyte: weak conductor when dissolved in water. Ch3cooh (aq) ch3coo- (aq) + h+ (aq) Nonelectrolyte: don"t conduct electricity when dissolved in water. Precipitation: ions in solution combine to form an insoluble solid salt. Molecular equation: written as though all species exist as molecules. Ionic equation: shows dissolved species as free ions. Net ionic equation: shows only the species that actually take part in the reaction. Spectator ions: ions that do not react in solution and remain as ions. Solubility rules (memorize!!: nitrates (no3-) are soluble, compounds containing alkai metal or nh4+ are soluble, most chlorides, bromides, and iodide are soluble. Ag+, hg2 2+, and pb2: most hydroxides are not soluble.
