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This CHEM 102 sample final is from sewveral years ago and since then the Content of CHEM 101 & CHEM 102 has been modified. Sme things on this final may now be in CHEM 101, while subjects may now be covered in CHEM 102 that are not covered by this final.


Question 1

For the following cell half-reactions, give the standard potential of the cell and the species produced at the anode.

AgCl(s) + e- ----> Ag(s) + Cl-

Ni2+ + 2 e- ----> Ni(s)

a) 0.01V, AgCl

b) 0.01V, Ni2+

c) 0.45V, AgCl

d) 0.45V, Ni2+*

Question 2

A solution is initially 0.10 M in MnCl2, NaOH is added until the solution is .010 M in OH-. The final concentration of the Mn2+ is:

a) 4.5 x 10-10 M*

b) 2.1 x 10-7 M

c) 4.5 x 10-8 M

d) 2.2 x 10-12 M

Question 3

A solution is 0.10 M in HCl and 0.010 M in H2S. Calculate the HS- concentration.

a) 1.0 x 10-14 M

b) 1.0 x 10-9 M

c) 1.0 x 10-8 M*

d) 1.0 x 10-7 M

Question 4

The concentration of Ag(I) ions in a saturated solution of Ag2C2O4 is 2.2 H 10-4M. What is the solubility product constant of Ag2C2O4.

a) 1.0 x 10-9

b) 5.0 x 10-12*

c) 1.1 x 10-11

d) 1.3 x 10-12


Question 5

Covalent substances which form molecular solutions are:

a) ionic

b) electrolytes

c) nonelectrolytes*

d) immiscible

Question 6

Calculate the pH of a 0.010 M solution of HC2H3O2.

a) 10.63

b) 2.00

c) 12.00

d) 3.37*

Question 7

When NH3 is dissolved in water the resut is a(n):

a) base*

b) salt

c) hydride

d) acid

Question 8

What is the oxidation state of the transition metal in [Cr(OH2)6](NO3)3 ?

a) 1

b) 2

c) 3*

d) 0

Question 9

What is the pOH of a 0.0060 M KOH solution?

a) 5.12

b) 2.22*

c) 11.78

d) 8.88


Question 10

Calculate the pH of a 0.010 M solution of aqueous NH3.

a) 3.37

b) 12.0

c) 2.00

d) 10.63*

Question 11

Balance the following redox reaction and select the correct coefficent for water.

H+ + S2O32- + CrO42+ ----> SO42- + Cr3+ + H2O

a) 17*

b) 12

c) 4

d) None of these

Question 12

What is produced at the cathode when aqueous CuBr2 is electrolyzed?

a) Cu*

b) Br

c) O2

d) H2

Question 13

Which of the following redox reactions will occur as written?

a) Fe3+ + Zno ----> Fe2+ + Zn2+

b) Sno + Fe2+ ----> Sn2+ + Feo

c) Sno + Sn4+ ----> 2 Sn2+

d) both a and c*

Question 14

What weight of MnO4- is required to oxidize 5.32 grams of Fe2+ to produce Fe3+

and Mn2+?

a) 2.65 g

b) 2.26 g*

c) 3.01 g

d) 5.05 g


Question 15

What type of isomerism is demonstrated by the pair of isomers below?

a) linkage

b) optical*

c) ionization

d) none of the above

Question 16

What is the molarity of the solution that results when 25.0 g of HCl is dissolved in enough water to make 200 mL of solution?

a) 1.72 M

b) 6.86 M

c) 3.24 M

d) 3.43 M*

Question 17

Select the correct formula for potassium hexachloroplatinate(II)

a) K4[PtCl6]*

b) K2[PtCl6]

c) K4[PtCl4]Cl2

d) K[PtCl6]

Question 18

A 25.0 mL solution of 0.050 N Na2S2O3 was used in the titration of 15 mL of an iodine solution to iodide and S4O62-. Calculate the normality of the iodine solution.

a) 0.083 N*

b) 0.010 N

c) 0.041 N

d) 0.170 N

Question 19

A buffer solution was prepared by dissolving 0.020 mole of propionic acid (HC3H5O2) and 0.015 mole of sodium propionate in enough water to make 1.00 liter of solution. Calculate the pH of the buffer.

a) 4.50

b) 4.80

c) 4.38*

d) 6.20

Question 20

At equimolar concentrations of Fe(II) and Fe(III), what must the [Ag+] be so that the voltage of the galvanic cell made from Ag+|Ag and Fe3+|;Fe2+ electrodes equals zero?

Fe2+(aq)|Fe3+(aq)|sat'd KCl|Ag+(aq)|Ag(s)

a) 0.03M

b) 0.31M*

c) 1.37M

d) 3.22M

Question 21

Calculate the normality of a KOH solution which required 14.2 mL to neutralize 10.0 mL of 1.50 N H2SO2.

a) 1.06 N*

b) 3.00 N

c) 1.50 N

d) 2.13 N

Question 22

What is the pH of a 0.50 M H2CO3 solution?

a) 2.63

b) 3.33*

c) 4.63

d) 10.25

Question 23

100 mL of 0.100 M NaOH is mixed with 50.0 mL of 0.200 M HC2H3O2. Calculate the final pH.

a) 8.88

b) 5.21

c) 5.12

d) 8.79*

Question 24

Calculate the mole fraction of chloroform (CHCl3) in a solution that is 25 % chloroform, 35 % benzene (C6H6) and 40 % acetone (C3H6O) by weight.

a) 0.80

b) 0.64

c) 0.32

d) 0.16*

Question 25

A solution is 0.10 M in H2CO3 and 0.10 M in HCl. The carbonate concentration is:

a) 1.6 x 10-8 M

b) 0.10 M

c) 2.4 x 10-16 M*

d) 5.6 x 10-11 M

Question 26

At 475oC, the equilibrium constant for the reaction:

H2(g) + I2(g) <------> 2 HI(g)

is 48.8. What is the concentration of HI in equilibrium with 0.4 g of H2 and 12.7 g of I2?

a) 0.488

b) 247.9

c) 0.699*

d) 15.7

Question 27

How many grams of a 10.0 % by weight KOH solution will contain 12.9 g of KOH?

a) 1.29 g

b) 1290 g

c) 12.0 g

d) 129 g*

Question 28

If 33.3 g of C2H6O2 is added to 76.7 g of water, what is the boiling point of the solution?

a) -1.30 oC

b) 103.6 oC*

c) 3.57 oC

d) -13.0 oC

Question 29

What type of isomerism is illustrated by the pair of compounds below?

a) linkage isomerism

b) stereoisomerism

c) optical isomerism

d) coordination sphere isomerism*

Question 30

In the reaction between the highly soluble salts NaCl and AgNO3 which ions are not spectator ions?

a) Na+ and NO3-

b) Ag+ and Cl-*

c) Ag+ and NO3-

d) Na+ and Cl-

Question 31

The strength of an electrolyte is determined by the:

a) concentration of its ions in solution*

b) oxidation state of an ion

c) number of ionic bonds

d) number of covalent bonds

Question 32

How many grams of sodium could be produced from molten NaCl in 1.00 hour by a current of 100 amperes?

a) 11.8 g

b) 19.5 g

c) 33.6 g

d) 85.8 g*

Question 33

How many grams of washing soda (Na2CO3) are needed to exactly neutralize 25.0 mL of vinegar. Vinegar is approximately 0.875 M HC2H3O2.

a) 2.32 g

b) 3.24 g

c) 1.16 g*

d) 69.6 g

Question 34

Select the correct name for Ni(NH3)2Br2

a) bisaminenickel(II) bromide

b) diamminedibromonickel(II)*

c) triamminenickel(II) dibromide

d) diamminenickel(II) dibromide

Question 35

If 5.0 mL of 0.60 M HCl is added to 20 mL of solution which is 0.12 M in both NH3 and NH4Cl, what is the final pH?

a) 7.00

b) 4.63

c) 9.15*

d) 9.38