1.  For the equilibrium


2 NO(g)  +  Br2(g)   =  2 NOBr(g),


     the equilibrium constant expression is given by


     A.  Kc =[NOBr ]/[NO][Br2]

     B.  Kc =[NO]2[Br2]/[NOBr]2

     C.  Kc =[NOBr]2/[NO]2[Br2]

     D.  Kc =[NOBr]2/([NO]2 + [Br2])


 2.  For a specific reaction, which one of the following statements

     about the equilibrium constant is true?


     A.  It always remains the same.

     B.  It increases if the concentration of one of the products is

         increased.

     C.  It changes with changes in temperature.

     D.  It can be changed by a change in the volume of the container at

         constant temperature.


 3.  For which of the following reactions is Kp =Kc?


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

     B.  3 O2(g)   =  2 O3(g)

     C.  H2O(g)  +  C(s)   =  CO(g)  +  H2(g)

     D.  H2O(l)   =  H2O(g)


 4.  For the equilibrium N2O4(g)   =  2 NO2(g) at 90 C, Kc = 0.27.

     What is Kp at this temperature?


     A.  0.27

     B.  32

     C.  2.0

     D.  8.0


 5.  In which of the following equilibria is the yield of products

     increased by decreasing the volume of the reaction mixture?


     A.  CaCO3(s)   =  CaO(s)  +  CO2(g)

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

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

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


 6.  The equilibrium constant for 


NO(g)  +  Cl2(g)   =  NOCl2(g)


     is 0.0409.  The equilibrium constant for the reaction


NOCl2(g)   =  NO(g)  +  Cl2(g) is


     A.  0.00167

     B.  0.0409

     C.  1.02

     D.  24.4


 7.  If the equilibrium constant for the reaction,


2 H2(g)  +  CO(g)   =  CH3OH(g)


     is 0.20 at a particular temperature, what will happen in a mixture

     in which the partial pressures of all gases are initially 0.100 atm?


     A.  More CH3OH will be produced.

     B.  CO will be consumed.

     C.  More H2 will be produced.

     D.  No change will occur.


 8.  0.5 mol of NH4Cl(s) is placed in a 1.00 L flask and heated to a

     high temperature; an equilibrium is established:


NH4Cl(s)   =  NH3(g)  +  HCl(g)


     If there are 0.020 mol of HCl(g) present at equilibrium, what is Kc?


     A.  2.0 x 10-2

     B.  4.0 x 10-4

     C.  8.0 x 10-4

     D.  It cannot be determined from the information given.


 9.  Calculate the equilibrium concentration of H2 in a 1.0 L container

     initially containing 0.118 mol of HBr at 1400 K.  Kc = 1.5 x 10-5 at

     1400 K for the reaction


2 HBr(g)   =  H2(g)  +  Br2(g)


     A.  1.8 x 10-6 M

     B.  0.118 M

     C.  1.5 x 10-5 M

     D.  4.5 x 10-4 M


10.  The molar solubility of BaF2 (Ksp = 1.0 x 10-6) can be decreased by


     A.  adding NaF(s) to the solution.

     B.  adding more BaF2 to the solution.

     C.  adding more water.

     D.  doubling the volume of the container.


11.  The molar solubility of PbBr2 is 0.010 M.  What is the value of Ksp

     for PbBr2?


     A.  4.0 x 10-6

     B.  1.0 x 10-6

     C.  2.0 x 10-4

     D.  3.0 x 10-4


12.  What is the solubility of PbCl2(s) in 0.100 M NaCl(aq)?  The

     Ksp for PbCl2 is 1.7 x 10-5.


     A.  4.1 x 10-3

     B.  1.6 x 10-2

     C.  1.7 x 10-3

     D.  4.3 x 10-4


13.  In the equation


HF(aq)  +  OH-(aq)   =  H2O(l)  +  F-(aq)


     the Bronsted-Lowry acid(s) are


     A.  HF and F-.

     B.  HF and H2O.

     C.  HF only.

     D.  OH- only.


14.  Which of the following acids is strongest?


     A.  ascorbic acid, pKa = 4.10

     B.  benzoic acid, Ka = 6.46 x 10-5

     C.  butyric acid, pKa = 4.81

     D.  formic acid, Ka = 1.77 x 10-5


15.  If the pH of a solution is raised by 2.00 pH units, the [H3O+]

     concentration concentration is


     A.  lowered by a factor of 20.0.

     C.  lowered by a factor of 100.

     B.  raised by a factor of 10.0.

     D.  raised by a factor of 50.0.


16.  The concentration of H3O+ in an aqueous solution is 2 x 10-4 M.

     What is the OH- concentration?


     A.  5 x 10-11 M

     B.  2 x 10-11 M

     C.  3 x 10-10 M

     D.  2 x 10-4 M


17.  Which of the following lists only amphoteric species?  Assume all

     species are dissolved in water.


     A.  F-,  HF-

     B.  NH4+,  H2O

     C.  H2SO4,  HSO4-

     D.  H2O,  HSO4-


18.  Calculate the pH of a 0.15 M solution of HCN.  Ka of HCN = 

     4.0 x 10-10.


     A.  0.82

     B.  3.65

     C.  9.37

     D.  5.11


19.  What is the pH of a 0.015 M Ba(OH)2 solution?


     A.  1.82

     B.  1.52

     C.  12.48

     D.  12.18


20.  If the pH of a 0.1 M aqueous solution of HOBr is 4.8, what is Ka

     for this acid?


     A.  2.5 x 10 9

     B.  1.6 x 10 4

     C.  2.5 x 10 10

     D.  1.6 x 10 9


21.  What is the percent ionization of NH3 in a 0.200 M NH3(aq)

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


     A.  4.7

     B.  1.9 x 10-3

     C.  2.1

     D.  0.95


22.  One molar solutions of the following three salts,


		KI,  NaF, and NH4NO3


     will result in solutions that are, respectively,


     A.  basic, basic, and neutral.

     C.  acidic, neutral, and acidic.

     B.  neutral, basic, and acidic.

     D.  neutral, acidic, and basic.


23.  Calculate Kb for the conjugate base of acetic acid (Ka = 1.8 x 10-5).


     A.  5.6 x 10-10

     B.  1.8 x 10-19

     C.  1.8 x 10-5

     D.  3.2 x 10-10


24.  What is the pH of a 0.50 M sodium nitrite solution?  Ka(HNO2) =

     4.6 x 10-4 M.


     A.  5.48

     B.  8.52

     C.  1.82

     D.  12.17


25.  Which of the following pairs of acids has the weaker acid

     listed first?


     A.  HCl,  HF

     B.  H2SO3,  H2SO4

     C.  HClO4,  HClO

     D.  H3O+,  H2O