Chap. 13:Slide 2Slide 3Slide 4Chapter 14Slide 6Slide 7Slide 8Chapter 15Slide 10Slide 11Slide 12Slide 13Chap. 16Slide 15Slide 16Slide 17Slide 18Chapter 19Slide 20Slide 21Chapter 4.4 & 20Slide 23Slide 24Chapter 23Slide 26Slide 27Slide 28Chapter 21Slide 30Slide 31Chapter 18Slide 33Slide 34Chap. 13:•Solution formation1. Enthalpy, H – favorable intermolecular interactions•Intermolecular interactions of Solvent-solute vs. solvent-solvent and solute-solute2. Entropy, S – increased disorder•Solubility1. Influence of pressure – Henry’s Law2. Influence of molecular structure – “like dissolves like”•Factors affecting solubility in H2O3. Influence of temperature•Concentration1. Mass %, ppm, ppb2. Mole fraction3. Molarity4. Molality•Colligative properties1. van’t Hoff factor, i2. Vapor Pressure – Raoult’s Law3. Boiling pt. elevation & Freezing pt. depression4. Osmosis(Hmix) (Hsolvent)(Hsolute)1. Which of the compounds below is the LEAST miscible with water? (A) CH3OH(B) CH3CH2OH(C)CH3CH2CH2OH(D)CH3CH2CH2CH2OH2. In general, as the temperature of a solution increases, the solubility of a gas solute _____. (A) Increases(B) Decreases(C)Remains the same(D)Varies from gas to gas© 2009, Prentice-Hall, Inc.Boiling Point Elevation and Freezing Point Depression• Note: T not dependent on what the solute is, but on how many solute particles are dissolved (i).Tb =(i)(Kb)(m)Tf = (i)(Kf)(m)3. Which of the following has the largest Van’t Hoff factor? A. 1.0 m ethanolB. 3.0 m methanolC. 0.60 m CaCl2D. 0.50 m K2SO4E. 0.50 m Fe2(SO4)3Chapter 141. Rates:a) Rate expression•Relative rates•Average Rate •Instantaneous Rateb) Rate Law•Initial rate method vs. graphical determination or Rxn order•Equations for First-order vs. second-order & half-life–Differential vs. Integrated2. Influence of temperature on rate: Ea & ka) Collisions: orientation and kinetic energyb) Arrhenius Equation and experimental determination of Ea3. Reaction mechanismsa) Elementary vs. multi-stepb) Energy profiles4. Catalysis: changes Ea &/or Aa) Homogeneous vs. Heterogeneousb) Energy profilesaA + bB  cC + dDtD][tC][tB][tA][ Ratedcba   nmBAk Rate 4. For the reaction: 5A + 8B + 3C → 9D + EWhich of the expressions below represents the rate of the reactionA)B)C)D)E)tBRate8][tARate5][tERate][tDRate9][tBRate4][For the reaction: 2NO2 (g)  2NO (g) + O2 (g) A linear relationship is observed between the reactant concentration and time upon appropriately plotting the data. 5. What does the slope of the curve represent?A. The starting concentration of NO2B. The rate constant of the reaction C. The order of the reaction with respect to NO2D. The natural logarithm of the rate constantE. The natural logarithm of the starting concentration6. What order is the rxn?A. 0B. 1C. 2D. 30 100 200 300 4001001502002503001/[NO2] (1/M)Time (s)Consider the plot of the “Energy” (E) profile versus “Reaction Coordinate” shown below. 7. Identify the rate-determining step for the reverse reaction.A. A BB. E AC. E CD. C AE. C E1. Dynamic equilibrium: –forward rate = reverse rate2. Equilibrium constant and law of mass action–No solids or liquids in K expression3. Kc and Kpa. Calculating from equilibrium concentrations & pressuresb. Unitlessc. Meaning of K (Size)d. Manipulate K: Sum of steps, reverse reactions, reactions multiplied by a number4. Quantitative equilibrium problems–Calculating using ICE tables (quadratic?)5. Le Châtelier’s Principle–System shifts to reduce stressChapter 15aA + bBkfkrdD + eEbaedrfkkK]B[]A[]E[]D[8. Which of the following expressions represents the equilibrium constant for the reaction:Fe3O4(s) + 4 H2(g) → 4 H2O(g) + 3Fe(s)A. Kc = [H2O]4[Fe]3/[Fe3O4][H2]4 B. Kc = [4H2O]4[3Fe]3/[Fe3O4][4H2]4 C. Kc = 1/[H2]4 D. Kc = [H2O]4/[H2]4 E. Kc = [H2O]4Consider the following reactions. H2C2O4(aq) + 2 H2O(l) ⇄ C2O4−(aq) + 2 H3O+(aq) K1 2 H2O(l) ⇄ H3O+(aq) + OH−(aq) K29. Use the information given above to calculate K3 for the reaction below. H2C2O4(aq) + 2 OH−(aq) ⇄ C2O42−(aq) + 2 H2O(l)A. (K1)(K2)B. (K1)(1/K2)C. (K1)2(K2)D. (K1)(K2)1/2 E. (K1)+(K2)© 2009, Prentice-Hall, Inc.Too much product, equilibrium shifts left.No shiftToo much reactant, equilibrium shifts right.The Reaction Quotient (Q)•Q = same ratio that K gives, but for a system that is not at equilibrium.–To calculate: substitute initial concentrations of reactants and products.ChangeA) Shift Left (towards reactants)B) Shift Right (towards productsC) No changeD) More informationrequired10. O2 is continuously removed from the reaction mixture11. A nickel catalyst is added to the reaction mixture12. The temperature of the reaction is increased13. The volume of the reactor is halved keeping the temperature the sameFor the reaction shown below:3O2 (g) ⇄ 2O3 (g)predict the direction in which the reaction will shift as the following changes are made to the reaction conditionsChap. 161. Definitions (Arrhenius, Bronsted-Lowery& Lewis )2. pH=log [H+]3. Strength of acids & bases: Ka & Kb (pKa & pKb)–Calculationsa) pH of strong acid & strong base solutionsb) Weak acid and base solutions (pH from Ka or Ka)4. Water is amphiprotic5. Conjugates6. (Ka)(Kb)=Kw–The stronger the acid or base, the weaker the conjugate base or acid7. Polyprotic acids: Ka1 > Ka2 & calculations8. SALTS9. Influence of structure on acid propertiesH2O (l) H+ (aq) + OH- (aq)00.14100.1]OH[]H[14pOHpHpKxKww14. What is the conjugate acid of HPO42?A. H3PO4 B. H2PO4 C. HPO32  D. PO43  15. Which of the following would be an acidic aqueous solution?E. NaClF. KBrG. CaI2H. NH3 I. NaFChap. 171. Common Ion Effect2. Buffers: Weak substance w/Common IonCalculationsa) ICE Table (M), use weak substance for eq. ORb) Henderson-Hasselbalch eq. 3. Adding Strong Acid or Base to a bufferRXN occurs!•Write Buffer equation•Write Rxn for what is added, use in ICE table (MOLES)•H-H eq. (M)4. Acid/Base Titration Curve ComparisonStrong/StrongWeak/Strong5. Solubility equilibria (SALTS)Use ICE Tables (M)6. Qualitative analysis  acidbasepKpHalog16. Which of the following mixtures could be used to prepare an effective buffer solution?A. HCl and KClB. HNO3 and KNO3C. HCl and NH4ClD. NH3 and NH4ClE. HNO2 and NaNO317. When titrating a weak