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Simulated Exam II (SF16Gc2E2F)
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1. What is HCOOH?
A.
B.
C.
D.
E.
Strong
Weak
Weak Acid
Strong Acid
None of the above
2. Take 2.49 x 10-2 moles of Ba(OH)2 in 4.53 x 102 mL. Calculate pH.
A.
B.
C.
D.
E.
7.42
11.47
13.04
7.05
None of the above
3. Select the strongest acid:
A.
B.
C.
D.
HN3 (pKa = 4.71)
HClO2 (pKa = 2.01)
HBrO2 (pKa = 4.69)
CCl3COOH ((pKa = 0.51)
4. True or False: the conjugate base of HSO4- is SO42-
5. Calculate the pOH of 0.3019 M HI solution
A.
B.
C.
D.
E.
13.5
0.52
1.34
7.05
None of the above
6. Find the pH from the given data below:
(0.6 M, C2H5NH2 Kb = 5.61 x 10-4)
A.
B.
C.
D.
E.
12.3
3.21
4.33
5.79
None of the above
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7. Find the pH from the given data below:


0.1 M NaC6H5COO
C6H5COOH Ka = 6.51 x 10-5
A.
B.
C.
D.
E.
3.43
8.59
5.98
9.43
None of the above
8. Find the pH from the given solution below:



0.536 M C6H5COOH
0.371 M C6H5COONa
C6H5COOH Ka = 6.51 x 10-5
A.
B.
C.
D.
E.
4.32
9.73
7.49
4.03
None of the above
9. Find the change of pH when a 10 mL, 0.5 M HClO solution (pH = 3.92) with the info below:



1.02 g NaClO added
Ka HClO = 3.0 x 10-8
Assume constant volume
A.
B.
C.
D.
E.
4.04
4.75
5.32
6.47
None of the above
10. Select the correct statement when a small amount of NaOH is added to a 0.1 M HF ideal buffer solution.
A.
B.
C.
D.
HF % ionization ↑
HF % ionization ↓
HF % ionization is constant
None of the above
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11. What is the pH if a solution is made with 100 mL of 2.5 x 10-2 M HCl and 1.00 x 102 mL of 1.0 x 10-1 M NaF (Ka HF =
7.24 x 10-4)
A.
B.
C.
D.
E.
4.32
4.73
3.47
3.62
None of the above
12. Select the correct statement regarding pH if a solution is made with 101 mL of 5.0 x 10-1 M HCl and 1.01 x 102 mL of
0.5 M HONH2 (Kb = 1.1 x 10-8)
A.
B.
C.
D.
Greater than 7
Equal to 7
Less than 7
None of the above
13. What is the pH for the solution below:
 0.3 M NaHCOO solution
 Ka HCOOH = 1.8 x 10-4
A.
B.
C.
D.
E.
8.93
9.79
8.61
6.39
None of the above
14. What is the pOH for the solution below:
 0.12 M (CH3)2NH2Cl
 Kb (CH3)2NH = 5.9 x 10-4
A.
B.
C.
D.
E.
5.85
8.55
8.15
11.31
None of the above
15. AgBr at 298K has a solubility of 8.8 x 10-7 mol/L. What’s the Ksp?
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16. Silver choloride (Ksp = 1.6 x 10-10). Select the correct answer for a solution made of:
 1.0 x 10-4 M CaCl2
 1.0 x 10-6 M AgNO3
A.
B.
C.
D.
E.
Q < Ksp, precipitate will form
Q > Ksp, precipitate will form
Q < Ksp, precipitate will NOT form
Q > Ksp, precipitate will NOT form
None of the above
17. What is the Ksp of CaSO4 given at a certain temperature the solubility is 7.965 x 10-2 g/L?
A.
B.
C.
D.
E.
3.42 x 10-7
5.37 x 10-8
6.46 x 10-7
6.46
None of the above
18. Find the solubility for CaF2 given:
 Ksp = 4.0 x 10-12
 In solution of 3.5 x 10-2 M of NaF
A.
B.
C.
D.
E.
3.3 x 10-8
1.9 x 10-9
3.6 x 10-7
5.5 x 10-9
None of the above (3.3 x 10-9)
19. pH has no effect on solubility for which one?
A.
B.
C.
D.
CuF
SrCO3
AgNO3
All are affected by pH
20. Find the solubility for silver chloride given:
 AgCl Ksp = 1.6 x 10-10
 In solution of 1 x 10-2 M FeCl3
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