On questions #1 to #20, all you need do is circle
the letter of the correct answer. There is only one correct answer
per question on #1 to #20. On problems #21 to #24, you must show
all your work. A correct answer on #21 to #24 with no work shown
will receive no credit.
1. An aqueous solution of KHSO3 is:
2. An aqueous solution of C2H5NH3F
is:
3. Arrange 0.10 M aqueous solutions of the following
substances in order of increasing pH.
| KH2PO4 | K3PO4 | K2HPO4 | H3PO4 |
a. K3PO4 < H3PO4
< K2HPO4 < KH2PO4
b. H3PO4 < K3PO4
< KH2PO4 < K2HPO4
c. H3PO4 < K3PO4
< K2HPO4 < KH2PO4
d. H3PO4 < KH2PO4
< K2HPO4 < K3PO4
e. KH2PO4 < K2HPO4
< H3PO4 < K3PO4
4. An aqueous solution of Cu(NO3)2
is:
5. Which of the following would indicate a basic
solution ?
6. At the equivalence point in the titration of CH3NH2
with HNO3, which of the following statements is true ?
7. Phenolphthalein is an appropriate indicator for
the titration in problem # 6.
8. 30.0 ml of 0.100 M HNO3 is added to
70.0 ml of 0.100 M KOH. Calculate the pH of
the resulting solution.
9. 40.0 ml of 0.100 M HNO2 is added to
60.0 ml of 0.100 M KOH. Calculate the pH of
the resulting solution.
10. The resulting solution in problem # 9 is a buffer
solution.
11. Each of the following pairs of solutions is mixed. Only one of them does not result in formation of a buffer solution. Identify that pair.
b. 500 ml of 0.500 M NH4Cl with 500 ml of 0.250 M KOH
c. 500 ml of 0.500 M NH4Cl with 500 ml of 0.250 M NH3
d. 500 ml of 0.500 M NH3 with 500 ml of 0.250 M HBr
e. 500 ml of 0.500 M NH3 with 500 ml
of 0.500 M HBr
12. What is the conjugate base of AsH3
?
13. In which of the following titrations would phenolphthalein
not be a suitable indicator ?
14. Which of the following weak acid/conjugate base
pairs would be suitable for making a buffer with a pH of 7.58 ?
15. Consider the reaction associated with the dissociation
of water:
As the temperature is decreased, which of the following
statements is true ?
b. Both the pH and the pOH of water decrease.
c. The pH increases and the pOH decreases.
d. The pH decreases and the pOH increases.
16. Which of the following substances is a Lewis
Base ?
17. In which of the following solvents would BaCO3(s)
be most soluble ?
18. Which of the following solids would be most soluble
in 0.10 M HCl ?
19. Calculate the pH of a saturated solution of Ca(OH)2(s).
21. How many milliliters of 0.250 M NH4Cl
would have to be added to 450 mls of
0.350 M KOH in order to produce a buffer solution
with a pH of 9.10 ?
22. Calculate the pH at the equivalence point in
the titration of 33.50 ml of 0.3400 M KF with 0.4150 M HBr.
23. A buffer solution is made by adding 250 mls of
0.500 M NaOH to 350 mls of 0.660 M HAc. 50.0 mls of 0.500 M HCl is then added
to this buffer solution. Compute the final pH of the resulting solution.
24. 240 mls of 0.100 M AgNO3 is added to 260 mls of 0.0500 M Na3PO4 producing a precipitate of Ag3PO4(s). Calculate the concentrations of Ag+ and PO43- remaining in solution.