CHEM 101 1nd Edition Lecture 11Outline of Last Lecture I. Chemical ReactionsII. Chemical EquationsIII. Balancing EquationsIV. Calculations Based on Chemical EquationsV. Chemical EquilibriumVI. Aqueous SolutionsOutline of Current Lecture I. Aqueous SolutionsII. Solutions: Soluble Ionic CompoundsIII. Solubility and IonizationIV. Precipitation Reaction: Molecular EquationsCurrent LectureI. Aqueous Solutionsa. Aqueous Solution: a liquid solution in which the solvent is waterb. Many reactions take place in aqueous solutionc. It is therefore important to know what happens to substances when laced in water.II. Solutions: Soluble Ionic Compoundsa. Electrolytesi. Electrolyte: a substance that when dissolved in water conducts electrify1. How do they conduct electricity?a. They ionize in aqueous solutionb. Ions carry the electricity2. Some electrolytes dissociate completely or nearly completely3. Weak electrolytes dissociate slightly4. How do we represent this in an equation?a. Single arrow indicates complete or nearly compile ionizationb. Double indicates incomplete ionizationii. Non-electrolytes: a substance that does not conduct electricity when dissolved in waterThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.1. Sugar, CH4, and other compounds that remain as molecules in wateriii. Weak Electrolyte: stand in a kind of middle groundIII. Solubility and Ionizationa. Now that we have introduced the concepts of solubility and ionization, the next step with be to predict if two compounds in water will react and what the products will be.i. Precipitate: Insoluble compoundb. Solubility Rulesi. Do not memorize, use!ii. Silver Compounds1. Nitrates are generally soluble as are chlorides.iii. Sulfides1. Sulfides are generally not solubleiv. Hydroxides1. Generally not soluble except when the caton is a Group IA metal.IV. Precipitation Reactions: Molecular Equationsa. The ions in reactant compounds exchange, or transpose, ions. i. AgNO3 (aq) + KCl (aq) --> AgCl + KNO31. Is it soluble?a. KNO3 is soluble, because al parts are solubleb. AgCl is not soluble, because of silverii. Pb(NO3)2 (aq) + (NH4)2S (aq) --> PbS + 2 NH4NO31. Is it soluble?a. NH4NO3 is soluble, because all parts are soluble.b. PbS will be solid iii. The equations written above are molecular (or formula unit) equations.1. NOTE: KNO3 an NH3NO3 do not form unless water is
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