Chem 1061 1st Edition Lecture 7Outline of Last Lecture I. Percentage YieldsII. Solution Stoichiometrya. Diluting a Solutionb. Solubilityc. Ionic Compound in a solutiond. Moles of Ions in a Solutione. Covalent Compounds in WaterIII. Writing Equations for Aqueous Ionic CompoundsOutline of CurrentIV. Total Ionic EquationV. Net Ionic EquationVI. Acid-Base Reactionsa. Acidb. Basec. Weak Acids/Basesd. Reactions of Acid + CarbonateCurrent LectureI. Molecular EquationPb(NO3)2(aq)+2KI(aq)PbI2(s)+2K(NO3)2(aq)II. Total (complete) Ionic Equation: Break up only aqueous ions!Pb^2+(aq)+2NOs^-(aq)+2K^+(aq)+2I^-(aq)PbI2(s)+2K^+(aq)+2NO3^-(aq)These 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.III. Net Ionic Equation : cancel out unchanged (spectator) ionsPb^2+(aq)+2I^-(aq)PbI2(s)IV. When all ions cancel out there is no net ionic equation. V. Acid Base ReactionsReaction of acid and base (neutralization)a. Acid: Produces H+ ions when dissolved in H2O (donates H+)b. Base: Produces OH^- ions when dissolved in water (accepts H+)c. Strong Acid/Base: one that dissociates completely into ionsd. Weak Acid/Base: dissociates very little into ions.Table 4.2 shows strong vs. weak acids and bases.e. Acid + Base Salt + Waterf. Reactions of acid and Carbonatei. Products include the formation of gasii. HCl(aq)+K2CO3(aq)KCl(aq)+(H2CO3)unstable
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