The following is a limited selection of questions from previous exams provided to help you become
familiar with the format/type of questions that are generally presented on the ch101 exams.
This is NOT representative of the full list of exam4 concepts or of the proportion of questions from the
covered concepts. Please refer to the study guide/ WebAssign /tophat examples for a more
comprehensive description of exam 4 material.
An answer key will be posted to the class website.
1. What mass of K2SO4 (grams) is required to make 45 mL of a 0.15 M K+ solution?
a) 0.26 grams
b) 0.13 grams
c) 0.59 grams
d) 1.2 grams
2. Select the substance that is a strong electrolyte
a) KNO3
b) HNO2
c) AgI
d) CH3OH
3. Consider the value of the solubility constant, Ksp= 1.8 x 10-10, for the following reaction
AgCl(s) « Ag+(aq) + Cl1-(aq) and select the best statement:
a) Equilibrium concentrations of Ag+ and Cl1- are very high
b) AgCl is highly soluble
c) DGo for the forward reaction is negative
d) None of the above statements is correct
4. A solution is known to contain one of the following anions: ClO41-, I1-, SO42- or NO31-. If a
precipitate was observed with the addition of Pb2+ but no precipitate forms with Ag1+,
what is the identity of the anion?
a) ClO41b) I1c) SO42d) NO315. Choose all the following materials that can be added to 1.0 liter of water to make a
solution that is 0.30 M in SO42-.
I. 0.30 mol CaSO4
IV. 0.30 mol (NH4)2SO4
a) I, V
d) I, III, V, VI
II. 0.10 mol Al2(SO4)3
V. 0.30 mol MgSO4
b) I, II, IV, V
e) IV, V
III. 0.60 mol Li2SO4
VI. 0.60 mol Ti(SO4)2
c) II, IV, V
6. Which of the following reactions does NOT yield a precipitate?
I. Sodium chromate + Nickel(II) iodide
II. Copper(II) sulfate + Barium acetate
III. Ammonium perchlorate + potassium iodide
IV. Silver nitrate and sodium bromide
a) II only
d) I and II
b) III only
c) III and IV
e) I, II, and III
7. What is the conjugate base of H2O?
a) OH1b) H3O1+
c) O28. Consider the following acid-base reaction and select the stronger base, F1- or BrO1-?
HF + BrO- ® F- + HBrO
K = 360000
1a) F
b) BrO19. Write the net equation for the acid-base reaction that takes place when solutions of
magnesium hydroxide and nitric acid are mixed. Use a single arrow for reactions in
which K ≥ 103
a) Mg2+ + NO31- ® Mg(NO3)2
b) H3O+ + NO31- ® HNO3
c) H3O+ + OH1- ® 2H2O
d) H3O+ + OH1- « 2H2O
e) HNO3 + OH1- ® H2O + NO31f) HNO3 + OH1- « H2O + NO3110. Determine the value of the equilibrium constant for the acid base reaction that takes
place when solutions of sodium hydrogen phosphate and ammonium chloride are
mixed.
a) 0.0090
b) 1.1 x 102
c) 0.00086
d) 1.2 x 103
11. Write the Net Reaction or None for the following: Lead solid is added to an acidified
solution of KMnO4
a) MnO4- + 5K + 8H+ ® Mn2+ + 5K1+ + 4H2O
b) 2MnO4- + 5Pb + 16H+ ®2Mn2+ + 5Pb2+ + 8H2O
c) MnO4- + Pb + 8H+ ®Mn2+ + Pb2+ + 4H2O
d) 2K1+ + Pb ®2K + Pb2+
e) None
12. Indicate whether the following standard cell reactions would take place in a galvanic or
an electrolytic cell. Zn2+(aq) + 2 I1-(aq) → Zn(s) + I2(s)
a) Galvanic
b) electrolytic
13. Determine whether a reaction takes place when the following are mixed?
An iron nail is placed in zinc sulfate solution
a) Yes
b) No
c) Cannot tell
14. Refer to the standard reduction potential table and identify the redox couple at the
cathode and the oxidizing agent (OX) in the electron transfer that takes place when Ag1+,
Ag, Ni2+, and Ni are mixed.
a) Ni2+/Ni at cathode and OX is Ni
b) Ni2+/Ni at cathode and OX is Ni2+
c) Ag1+/Ag at cathode and OX is Ag1+
d) Ag1+/Ag at cathode and OX is Ag
15. Select the correct statement about an extensive redox reaction
a) DGo > 0 and Eo > 0
b) DGo < 0 and Eo > 0
c) DGo > 0 and Eo < 0
d) DGo < 0 and Eo < 0