Solution formation 1 Enthalpy H favorable intermolecular interactions 2 Entropy S increased disorder Hmix 3 Factors affecting solubility in H2O Influence of temperature Concentration 1 2 3 4 Hsolvent Influence of pressure Henry s Law Influence of molecular structure like dissolves like Intermolecular interactions of Solvent solute vs solvent solvent and solute solute Solubility 1 2 Mass ppm ppb Mole fraction Molarity Molality Colligative properties 1 2 3 4 Chap 13 van t Hoff factor i Vapor Pressure Raoult s Law Boiling pt elevation Freezing pt depression Osmosis Hsolute 1 Which of the compounds below is the LEAST miscible with water A CH3OH B CH3CH2OH C CH3CH2CH2OH D CH3CH2CH2CH2OH 2 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 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 2009 Prentice Hall Inc 3 Which of the following has the largest Van t Hoff factor A 1 0 m ethanol B 3 0 m methanol C 0 60 m CaCl2 D 0 50 m K2SO4 E 0 50 m Fe2 SO4 3 Chapter 14 1 Rates a Rate expression Relative rates Average Rate Instantaneous Rate b Rate Law aA bB cC dD Rate A B C D a t b t c t d t Rate k A B n Initial rate method vs graphical determination or Rxn order Equations for First order vs second order half life Differential vs Integrated 2 Influence of temperature on rate Ea k a Collisions orientation and kinetic energy b Arrhenius Equation and experimental determination of Ea 3 Reaction mechanisms a Elementary vs multi step b Energy profiles 4 Catalysis changes Ea or A a Homogeneous vs Heterogeneous b Energy profiles m 4 For the reaction 5A 8B 3C 9D E Which of the expressions below represents the rate of the reaction B A Rate 8 t B C A Rate 5 t Rate E t D 9 t D Rate E Rate B 4 t 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 B C D E The starting concentration of NO2 The rate constant of the reaction The order of the reaction with respect to NO2 The natural logarithm of the rate constant 300 The natural logarithm of the starting concentration 6 What order is the rxn A B C D 0 1 2 3 1 NO2 1 M 250 200 150 100 0 100 200 Time s 300 400 Consider the plot of the Energy E profile versus Reaction Coordinate shown below 7 Identify the rate determining step for the reverse reaction A B C D E A B E A E C C A C E Chapter 15 1 Dynamic equilibrium forward rate reverse rate aA bB kf kr dD eE k f D d E e K a b kr A B 2 Equilibrium constant and law of mass action No solids or liquids in K expression 3 Kc and Kp a Calculating from equilibrium concentrations pressures b Unitless c Meaning of K Size d Manipulate K Sum of steps reverse reactions reactions multiplied by a number 4 Quantitative equilibrium problems Calculating using ICE tables quadratic 5 Le Ch telier s Principle System shifts to reduce stress 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 4 Consider the following reactions H2C2O4 aq 2 H2O l C2O4 aq 2 H3O aq K1 2 H2O l H3O aq OH aq K2 9 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 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 No shift Too much reactant equilibrium shifts right Too much product equilibrium shifts left 2009 Prentice Hall Inc For 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 conditions Change 10 O2 is continuously removed from the reaction mixture 11 A nickel catalyst is added to the reaction mixture 12 The temperature of the reaction is increased 13 The volume of the reactor is halved keeping the temperature the same A B C D Shift Left towards reactants Shift Right towards products No change More information required Chap 16 1 Definitions Arrhenius Bronsted Lowery Lewis 2 pH log H 3 Strength of acids bases Ka Kb pKa pKb Calculations a b pH of strong acid strong base solutions Weak acid and base solutions pH from Ka or Ka 4 Water is amphiprotic pK w pH pOH 14 00 5 Conjugates 6 Ka Kb Kw H2O l K w H OH 1 0 x10 14 H aq OH aq The stronger the acid or base the weaker the conjugate base or acid 7 Polyprotic acids Ka1 Ka2 calculations 8 SALTS 9 Influence of structure on acid properties 14 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 F G H I NaCl KBr CaI2 NH3 NaF Chap 17 1 Common Ion Effect 2 Buffers Weak substance w Common Ion Calculations a b ICE Table M use weak substance for eq OR 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 Strong 5 Solubility equilibria SALTS pH pK a log Use ICE Tables M 6 Qualitative analysis base acid 16 Which of the following mixtures could be used to prepare an effective buffer solution A B HCl and KCl HNO3 and KNO3 C HCl and NH4Cl D NH3 and NH4Cl E HNO2 and NaNO3 17 When titrating a weak base with a strong acid a good indicator to use would be A B C D methyl red color change at pH 5 bromothymol blue change at pH 7 phenolphthalein change at pH 9 None of the above 18 What happens when NaOH is added to a buffer composed of CH3COOH and CH3COO A B C D There is no reaction because C2H3O2 and HC2H3O2 form a buffer The NaOH reacts with C2H3O2 converting some of it into HC2H3O2 The NaOH reacts with HC2H3O2 converting some of it into …