1.  Select the correct form of the equilibrium constant Kc for

     the following reaction.


2 ZnS(s)  +  3 O2(g)   =  2 ZnO(s)  +  2 SO2(g)


     A.  [ZnS][O2]3/2 / [ZnO][SO2]

     B.  [Zn]2[SO2]2 / [ZnS]2[O2]3

     C.  (2[ZnO] +  2[SO2]) / (2[ZnS] + 3[O2])

     D.  [SO2]2 / [O2]3


 2.  If Kp = 2.5 at 3000 K for the reaction


CO2(g)   =  CO(g)  + 1/2 O2(g)


     what is Kp at 3000 K for the reaction


2 CO(g)  +  O2(g)   =  2 CO2(g)


     A.  0.5

     B.  6.25

     C.  0.63

     D.  0.16


 3.  What is the relationship between Kc and Kp for the

     following reaction?


CO(g)  +  H2O(g)   =  CO2(g)  +  H2(g)


     A.  Kc = Kp

     B.  Kp = Kc(RT)-2

     C.  Kc = Kp(RT)-2

     D.  Kc = Kp(RT-1)


 4.  If the exothermic reaction


2 SO2(g)  +  O2(g)   =  2 SO3(g)


     is at equilibrium, which of the following will not raise the

     equilibrium partial pressure of SO3(g)?


     A.  Adding more O2(g).

     B.  Decreasing the volume of the container.

     C.  Adding more SO2(g).

     D.  Raising the temperature.


 5.  delta H is negative for the reaction


2 NOCl(g)   =  2 NO(g)  +  Cl2(g).


     Which one of the following sets of two reaction conditions is

     favorable for the production of NO? (Assume equilibrium is

     reached rapidly).


     A.  low T, add NOCl

     B.  high Ptot, add Cl2

     C.  high T, low Ptot

     D.  high T, add NOCl


 6.  Consider the reaction


SO2(g)  +  Cl2(g)   =  SO2Cl2(g)


     Initially [SO2] = 0.0200 M and [Cl2] = 0.0500 M.  If [SO2] =

     0.0080 M at equilibrium, what is Kc?


     A.  39

     B.  8.0

     C.  188

     D.  Kc cannot be determined from the information given.


 7.  Exactly 2.00 mol each of carbon monoxide and water are sealed in a

     4.00 L flask at 1100 K.  Kc for this reaction is 0.550.


CO(g)  +  H2O(g)   =  CO2(g)  +  H2(g)


     Calculate the concentrations of all species at equilibrium.


     A.  [CO2] = [H2] = 0.160 M;  [CO] = [H2O] = 0.340 M

     B.  [CO2] = [H2] = [CO] = [H2O] = 0.500 M

     C.  [CO2] = [H2] = 0.213 M;  [CO] = [H2O] = 0.287 M

     D.  [CO2] = [H2] = [CO] = [H2O] = 0.742 M


 8.  Kc = 0.35 for the following reaction at some temperature T1.


H2(g)  +  I2(g)   =  2 HI(g).


     If one mole of H2 and one mole of I2 are placed in a 1.0 L container,

     the equilibrium concentration of HI is


     A.  0.23 M

     B.  0.46 M

     C.  0.63 M

     D.  0.77 M


 9.  For the following reaction, Kp = 10.0 at some temperature T2.


H2(g)  +  I2(g)   =  2 HI(g)


     If the initial concentrations are PH2 =  0.010 atm, PI2 =  0.0025 atm,

     and PHI =  0.020 atm, which of the following statements is true?


     A.  The system is at equilibrium.

     B.  At equilibrium PHI > 0.020 atm.

     C.  At equilibrium PH2 > 0.010 atm.

     D.  At equilibrium PH2 = PI2.


10.  Which one of the following salts is least soluble in water on a

     molar basis?


               CaF2      Ksp = 3.9 x 10-11

               PbCl2     Ksp = 1.6 x 10-5

               AgCl      Ksp = 1.8 x 10-10

               AgIO3     Ksp = 3.1 x 10-8


     A.  CaF2

     B.  PbCl2

     C.  AgCl

     D.  AgIO3


11.  Copper(I) bromide, CuBr, has a measured solubility of 2.0 x 10-4

     mol/L at 25oC.  Calculate its Ksp value.


     A.  4.0 x 10-8

     B.  8.0 x 10-12

     C.  3.2 x 10-11

     D.  8.0 x 10-8


12.  What is the molar solubility of Cu(OH)2 in 0.010 M NaOH?

     Ksp[Cu(OH)2] = 1.6 x 10-19


     A.  1.6 x 10-15 M

     B.  4.0 x 10-16 M

     C.  3.4 x 10-7 M

     D.  1.6 x 10-8 M


13.  Ksp for PbCl2 is 1.6 x 10-5.  In a mixture of 5.0 mL of 0.10 M

     Pb(NO3)2 and 5.0 mL of 0.020 M NaCl, which of the following is

     correct for the solubility equilibrium of PbCl2?


     A.  Q = 5.0 x 10-4

     B.  Q = 5.0 x 10-6

     C.  Q = 5.0 x 10-8

     D.  Q = 5.0 x 10-12


14.  Select the three strongest acids from the following list:


HNO3,   H2CO3,   H2SO4,   HSO4-,   HNO2,   HF,   HI,   HCN


     A.  HNO3,  H2SO4,  HSO4-

     B.  H2CO3,  HNO2, HF

     C.  HF,  HI,  HCN

     D.  HNO3,  H2SO4,  HI


15.  For the reaction


H2O  +  HPO42-   =   OH-  +  H2PO4-


     which one of the following is correct?


             Acids                Conjugate Acid-Base Pairs

     A.  H2O;   H2PO4-              H2O/HPO42- ;   H2PO4-/OH-

     B.  H2O;   HPO42-              H2O/OH- ;   HPO42-/ H2PO4-

     C.  H2O;   H2PO4-              H2O/OH- ;    H2PO4-/HPO42-

     D.  HPO42-;  H2PO4-            HPO42-/OH-;   H2PO4-/H2O


16.  A solution is found to have a pH of 10.45.  What is [H3O+]?


     A.  3.5 x 10-11 M

     B.  2.8 x 10-4 M

     C.  1.0 M

     D.  3.55 M


17.  What is the pH at 25oC of a 4.0 x 10-4 M solution of Ca(OH)2?


     A.  3.4

     B.  10.6

     C.  3.1

     D.  10.9


18.  Which one of the following statements is incorrect?


     A.  Kw is temperature dependent.

     B.  Water is amphoteric.

     C.  In pure water, the concentrations of H3O+ and OH- are equal.

     D.  At 25oC, pKw equals 7.00.


19.  What is the pH of a solution that is 0.100 M in HCl and 0.050 M

     in HNO3?


     A.  2.3

     B.  1.3

     C.  1.0

     D.  0.8


20.  Benzoic acid is a weak monoprotic acid with Ka = 6.3 x 10-5.

     Calculate the pH of a 0.050 M solution of this acid.


     A.  1.30

     B.  2.75

     C.  6.14

     D.  5.50


21.  What is the percent dissociation in a 0.0500 M solution of ammonia?

     (Kb for NH3 is 1.8 x 10-5).


     A.  0.036

     B.  1.9

     C.  8.5

     D.  0.42


22.  Ka for HF is 3.5 x 10-4.  Calculate Kb for the fluoride ion.


     A.  3.5 x 10-4

     B.  1.0 x 10-7

     C.  2.9 x 10-11

     D.  1.0 x 10-14


23.  Which one of the following salts forms an acidic solution when

     dissolved in H2O?


     A.  NaNO3

     B.  NH4Cl(s)     (Kb for NH3 is 1.8 x 10-5)

     C.  KCN          (Ka for HCN is 7.2 x 10-10)

     D.  NaHCOO       (Ka for HCOOH is 1.8 x 10-4)


24.  Within a group in the periodic table, the acidity of the binary

     hydrides increases from top to bottom, for example


H2O  <  H2S  <  H2Se  <  H2Te


     This trend can be explained by


     A.  the leveling effect.

     B.  changes in oxidation state.

     C.  the H-X bond strengths.

     D.  hydrolysis.


25.  In the reaction


Cd2+(aq)  +  4 I-(aq)   =  CdI42-(aq)


     Cd2+ can be classified as a(n)


     A.  Arrhenius acid.

     B.  Lewis acid.

     C.  Bronsted-Lowry acid.

     D.  base in all three theories.