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Lecture 8


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David Brock

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CHEM 1A03 LECTURE 8 OCT 17 – WATERAND AQUEOUS SOLUTION Properties of Water • Unusually high boiling point of liquid water at STP • Density of ice is less than that of liquid water. • High specific heat capacity – absorbs thermal heat for storage/distribution/release • Water dissolves a variety of solutes as a solvent. Strong salvation properties for most polar molecules/ions. o Solubization of polar/ionic solutes: Hydration o Energetically favorable H2O solute interactions. • Ion Hydration, Sodium Pumps + Ion Transport, Protein Folding, Activity and Drug Binding, Solubility, Toxicity and Bioaccumulation Auto-Ionization of Water • Water is amphoteric and conductive – acts as an acid and a base with itself to produce hydronium and hydroxide. • pH = -log[H 3] = 7.0. Non Electrolyte Strong Electrolyte Weak Electrolyte Neutral Molecule Fully Charged Ions Partially Ionized Molecule Electrolytes Major Types of Aqeuous Chemical Reactions: K is a measure of extent of rxn and transformation 1. Solubility or Precipitation Reactions: (ion transfer) Lab 2 Cu(NO3)2(aq) + 2 NaOH(aq)  2. Reduction-Oxidation (Redox) Reactions: transfer) Lab 2 Zn (s) + Cu2+ (aq)  Zn2+ (aq) + Cu (s) 3. Acid-Base Reactions: (proton transfer)
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