chem 102 winter 12 make up exam a questions and answers
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CHEM 102 Winter 12 Make-Up
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CHEM 102 Winter 12 Make-Up Exam (A) Questions and Answers
b b 2 4 ac
x
Potentially useful 2a
information: pH
log
base
pKa acid
ΔG° = ΔH° - T ΔS°
ΔG = ΔG° + RT ln Q
ΔG° = - RT ln K
R = 8.314 J mol-1 K-1
1. Please choose the letter “a” as your answer for this question.
2. A buffer solution
a. contains more than the expected amount of solute for a particular temperature and is
therefore unstable.
b. contains the maximum amount of solute possible for a particular temperature.
c. changes color upon addition of strong base.
d. contains an equal number of hydronium and hydroxide ions.
e. resists changes in pH upon addition of acid or base.
3. A buffer solution is 0.500 M in acetic acid and 0.500 M in sodium acetate. The pH is 4.74. What is the
pH after the solution is diluted by a factor of 2?
a. 4.44
b. 4.49
c. 4.74
d. 4.99
e. 5.04
4. What is the pH of a 500 mL solution containing 0.28 mol HClO (Ka = 3.5 × 10-8) and 0.31 mol ClO ?
a. 7.50
b. 7.25
c. 7.65
d. 7.41
e. 7.20
5. Which acid, in combination with its conjugate base, would be the best choice to make a buffer of pH =
3.70?
a. dihydrogen phosphate (Ka = 2.9 107)
b. acetic acid (Ka = 1.8 105)
c. benzoic acid (Ka = 6.3 105)
d. formic acid (Ka = 1.8 104)
e. hydrofluoric acid (Ka = 6.8 104)
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, 6. In a buffer solution, if [A] < [HA], which of the following is true?
a. pH < pKa
b. pH = pKa
c. pH > pKa
d. pH < 7.00
e. pH > 7.00
7. Which statement about the titration of 0.10 M HNO3 (strong acid) with 0.10 M KOH (strong base) is not
correct?
a. The endpoint always comes before the equivalence point.
b. The pH at the equivalence point is 7.00.
c. The initial pH is 1.00.
d. At the equivalence point the pH increases sharply.
e. The net ionic equation is H3O+ + OH 2H2O.
8. What volume of 0.106 M NaOH is needed to neutralize a 50.0 mL sample of 0.095 M HNO3?
a. 55.8 mL
b. 50.0 mL
c. 44.8 mL
d. 10.1 mL
e. 5.19 mL
9. Which acid-base titration would yield a titration curve of the general form shown?
a. H2CO3 titrated with NaOH
b. NaOH titrated with H3PO4
c. Na3PO4 titrated with HCl
d. H2SO4 titrated with NaOH
e. H3PO4 titrated with NaOH
10. Which equation could be used to calculate the molar solubility (S) of Fe(OH)2?
a. Ksp = 2 S2
b. Ksp = S2
c. Ksp = 4 S3
d. Ksp = S3
e. Ksp = 2 S3
11. The solubility of manganese(II) hydroxide (Mn(OH) 2) is 2.2 × 10-5 M. What is the Ksp of Mn(OH)2?
a. 1.1 × 10-14
b. 4.3 × 10-14
c. 2.1 × 10-14
d. 4.8 × 10-10
e. 2.2 × 10-5
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