1.  For the system NH4Cl(s)   =  NH3(g)  +  HCl(g), if the concentration

     of NH3 is doubled, the equilibrium constant will, at constant

     temperature,


     A.  double.

     B.  increase, but by less than a factor of two.

     C.  remain the same.

     D.  be halved.


 2.  Which of the following is the correct equilibrium constant Kc

     expression for the following reaction?


P4(s)  +  10 Cl2(g)   =  4 PCl5(g)


     A.  Kc = [PCl5]4 / [P4][Cl2]10

     B.  Kc = [Cl2]10 / [PCl5]4

     C.  Kc = [PCl5]4 / [Cl2]10

     D.  Kc = [P4][Cl2]10 / [PCl5]4


 3.  At 1200 K, Kc = 36 for the reaction


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


     What is Kc for the following reaction at 1200 K?


HI(g)  =  1/2 H2(g)  + 1/2 I2(g)


     A.  6

     B.  0.056

     C.  18

     D.  0.17


 4.  For the reaction,


2 NO(g)  +  O2(g)   =  2 NO2(g)


     the relation between Kp and Kc is


     A.  Kp  =  Kc(RT)-1

     B.  Kp  =  Kc(RT)1

     C.  Kp  =  Kc

     D.  Kc  =  Kp(RT)-1


 5.  Which of the following will not raise the equilibrium partial

     pressure of NH3 in the following reaction?


N2(g)  +  3 H2(g)   =  2 NH3(g)      exothermic


     A.  adding more H2(g)

     B.  raising the temperature

     C.  decreasing the volume of the container

     D.  adding more N2(g)


 6.  Consider the following equilibrium at 25oC:


H2(g)  +  I2(g)   =  2 HI(g)           delta Ho = +51.8 kJ


     The quantity of HI(g) in the equilibrium mixture can be increased by


     A.  increasing the pressure.

     B.  adding a catalyst.

     C.  both increasing the temperature and adding more H2(g).

     D.  both decreasing the temperature and adding more I2(g).


 7.  At a given temperature, an equilibrium mixture consisting of 1.0 mol

     of H2S, 4.0 mol of H2, and 0.80 mol of S2 is contained in a 4.0 L

     vessel.  What is the equilibrium constant, Kc, for the following

     reaction?

2 H2S(g)   =  2 H2(g)  +  S2(g)


     A.  12.8

     B.  0.80

     C.  1.6

     D.  3.2


 8.  One mole of HI is placed in a 5.00 L container at 458oC.  If Kc =

     2.06 x 10-2 at this temperature, calculate the equilibrium

     concentration of I2 for the reaction below.


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


     A.  4.03 x 10-2 M

     B.  2.23 x 10-2 M

     C.  2.06 x 10-2 M

     D.  9.33 x 10-2 M


 9.  Sufficient PCl5 was introduced into a 2.00 L evacuated flask at

     250oC so that the initial PCl5 pressure was 0.244 atm.  Once

     equilibrium for the following reaction was reached, the total

     pressure inside the flask was observed to be 0.472 atm.  What

     is Kp for the reaction at 250oC?


PCl5(g)   =  PCl3(g)  +  Cl2(g)


     A.  0.308

     B.  3.25

     C.  0.517

     D.  1.03


10.  What is the molar solubility at 25oC of Fe(OH)3 in pure water?

     (Ksp for Fe(OH)3 is 1.1 x 10-39)


     A.  1.0 x 10-18

     B.  6.5 x 10-13

     C.  4.5 x 10-10

     D.  1.0 x 10-9


11.  The molar solubility of PbI2 is 1.25 x 10-3 M at 25oC.  What

     is the Ksp for PbI2 at this temperature?


     A.  7.81 x 10-9

     B.  1.56 x 10-8

     C.  1.50 x 10-2

     D.  1.95 x 10-9


12.  What is the molar solubility at 25oC of PbBr2 (Ksp = 4.6 x 10-6)

     in 0.200 M NaBr?


     A.  1.0 x 10-2 M

     B.  1.2 x 10-4 M

     C.  2.3 x 10-5 M

     D.  4.6 x 10-6 M


13.  For the following reaction which of the statements are true?


H2S  +  HPO42-   =  HS-  +  H2PO4-


     1.  HPO42- and HS- act as Bronsted-Lowry bases. 

     2.  HPO42- and H2PO4- act as Bronsted-Lowry acids. 

     3.  H2PO4- and H2S are conjugate acid-base pairs. 

     4.  H2S and H2PO4- are Bronsted-Lowry acids.


     A.  1 and 4

     B.  1 and 2

     C.  2 and 3

     D.  3 and 4


14.  Which of the following is not a conjugate acid-base pair?


     A.  NH4+ ;  NH3

     B.  H2O ;  OH-

     C.  H2SO4 ;  SO42-

     D.  H2PO4- ;  HPO42-


15.  The strongest acid that can exist in HF(l) is


     A.  H3O+

     B.  HF

     C.  H2F+

     D.  F-


16.  What is the pH of a 1.8 x 10-3 M solution of NaOH(aq) at 25oC?


     A.  2.74

     B.  5.60

     C.  8.40

     D.  11.26


17.  What is the molar concentration of OH- at 25oC in an aqueous

     solution that has a pH of 8.50?


     A.  3.2 x 10-9 M

     B.  8.5 x 10-5 M

     C.  3.2 x 10-2 M

     D.  3.2 x 10-6 M


18.  When 0.050 mol of a weak acid, HA, was dissolved in enough

     water to make 1.50 L of solution, the pH of the solution was

     found to be 2.10 at 25oC.  What is Ka for this weak acid?


     A.  2.5 x 10-3

     B.  1.9 x 10-3

     C.  2.4 x 10-1

     D.  1.5 x 10-3


19.  What is the molar concentration of H3O+ in a 1.0 x 10-3 M solution

     of hypochlorous acid, HOCl, at 25oC?  Ka = 3.0 x 10-8.


     A.  1.8 x 10-5

     B.  5.9 x 10-3

     C.  7.1 x 10-7

     D.  5.5 x 10-6


20.  What is the pH of a solution at 25oC that is 0.010 M in HCl and

     0.025 M in HNO3?


     A.  1.46

     B.  1.60

     C.  1.82

     D.  3.60


21.  Which of the following salts result in basic solutions when

     dissolved in water?


CH3COONa,   KCN,   LiNO3,   NH4Br


     A.  CH3COONa and KCN

     B.  LiNO3 and NH4Br

     C.  KCN and LiNO3

     D.  CH3COONa and NH4Br


22.  What is the pH of a 0.50 M solution of NaCN at 25oC?  Ka for HCN

     is 4.0 x 10-10.


     A.  2.45

     B.  11.55

     C.  4.90

     D.  9.10


23.  In which of the following pairs are the stronger acids listed

     first?


1. H2S, H2Se     2. HNO3, HNO2    3. HCl, HF    4. HBrO3, HBrO4


     A.  1 and 2

     B.  2 and 3

     C.  3 and 4

     D.  1 and 4


24.  Which of the following represents the correct order of increasing

     acidity for the indicated species in aqueous solution?


     A.  H2O  <  NH3  <  HF  <  HBr

     B.  HF  <  NH3  <  HBr  <  H2O

     C.  NH3  <  H2O  <  HBr  <  HF

     D.  NH3  <  H2O  <  HF  <  HBr


25.  Which of the following would one expect to be capable of acting

     as Lewis bases?


1. Mg2+      2. AlCl3      3. OH-      4. CO


     A.  1 and 2

     B.  2 and 3

     C.  3 and 4

     D.  1 and 4