CHEM 11H Lecture Notes - Lecture 4: Spectator Ion, Solubility Table, Strong Electrolyte
31 Oct 2017
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Document Summary
Water, the most common solvent in nature. Water is the solvent in aqueous solutions. Aqueous chemistry - chemistry taking place in water, very common and very important (eg. our bodies, ocean, treatment plants, etc. ) Polarity gives water its ability to dissolve many compounds. Not all ionic compounds dissolve in water (eg. calcium carbonate) Covalent compounds do not dissociate in water. Nonpolar molecules do not dissolve in water ( like dissolves like ) Substance dissolves in water but no ions. Dissociated ions from soluble salts, strong acids/bases. Insoluble substances when 2 soluble solutions are mixed. Solid formed is called precipitate (ppt for short) Complete ionic equation: showing all species as present in solution. Don"t break up insoluble salts (precipitate), weak, or nonelectrolytes. Net ionic equation: showing only species that changed. Arrhenius definition: produces h+ (or protons) in solution. Ex: hcl (aq) h+ (aq) + cl- (aq) In reality, h+ exists as h2o+ (hydronium ion) but used interchangeably.
