Chemistry: Molecular Nature of Matter and Change, 6th Edition (Silberberg)

Chapter 19: Ionic Equilibria in Aqueous Systems

Self-Assessment Quiz 1

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1
If an acid HA has Ka = 10-5, what is the pH of a mixture of 0.1 mole of the acid and 0.1 mole of its conjugate base in 1.0 liter of water?
A)5
B)9
C)3
D)4
E)6
2
A solution contains equimolar amounts of NaH2PO4 and Na2HPO4. What is its pH? (for H3PO4, the Ka values are, respectively, 7.5 x 10-3; 6.2 x 10-8; 4.8 x 10-13)
A)3
B)5
C)7
D)9
E)13
3
What is the optimum pH of a sodium formate/formic acid buffer? (Ka = 1.7 x 10-4)
A)7.0
B)6.2
C)3.8
D)3.0
E)1.7
4
A buffer is prepared by mixing 100 mL of 0.500 M HCl and 200 mL of 0.500 M sodium acetate. The Ka for acetic acid is 1.8 x 10-5. Calculate the pH of the buffer.
A)4.44
B)4.74
C)5.05
D)5.45
E)6.13
5
A sample of vinegar (dilute acetic acid) weighing 5.056 g is titrated with 30.25 mL of 0.1022 M NaOH. What is the weight percent of acetic acid (CH3COOH) in the sample?
A)3.025%
B)3.669%
C)3.710%
D)4.221%
E)4.302%
6
An acid with a Ka of 1 x 10-8 is titrated with NaOH, both solutions being 0.020 M. What should the Ka of the indicator be, in order to obtain the best end point?
A)10-4
B)10-6
C)10-7
D)10-8
E)10-10
7
Consider the titration of 0.1000 M HBr with 0.1000 M KOH. Calculate the pH after 55.00 mL of the base has been added to 50.00 mL of the HBr solution.
A)6.62
B)7.35
C)8.90
D)11.68
E)12.50
8
Consider the titration of 0.1000 M NH3 (Kb = 1.76 x 10-5) with 0.1000 M HNO3. The pH at the equivalence point is
A)between 2.0 and 4.0
B)between 4.5 and 6.5
C)approximately 7.0
D)between 7.5 and 9.5
E)between 11.0 and 13.0
9
Which one of the following gases is not involved in producing acidic precipitation?
A)SO2
B)SO3
C)NO
D)N2O
E)NO2
10
What is the solubility product constant expression (Ksp) for PbCl2?
A)[Pb2+](2)[Cl-]
B)[Pb2+] [Cl-]/2
C)[Pb2+][Cl-]2/[PbCl2]
D)[Pb2+] [Cl-]/[PbCl2]
E)[Pb2+][Cl-]2
11
The molar solubility of PbCl2 is 3.9 x 10-2 mol/L. What is the Ksp of PbCl2?
A)5.9 x 10-5
B)4.1 x 10-5
C)1.5 x 10-3
D)2.4 x 10-4
E)3.9 x 10-2
12
Calculate the pH of a saturated solution of Mg(OH)2 (Ksp for Mg(OH)2 = 1.2 x 10-11)
A)3.5
B)10.2
C)10.5
D)11.0
E)11.3
13
Calculate the concentration of calcium ions in a saturated calcium phosphate solution.
(Ksp for Ca3(PO4)2 = 1.3 X 10-26)
A)1.2 x 10-5 mol/L
B)2.0 x 10-5 mol/L
C)6.6 x 10-6 mol/L
D)7.8 x 10-6 mol/L
E)8.3 x 10-6 mol/L
14
Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution.
(Ksp for Ag2CO3 = 8.1 x 10-12)
A)8.1 x 10-12 M
B)2.8 x 10-6 M
C)1.4 x 10-6 M
D)1.4 x 10-8 M
E)2.0 x 10-4 M
15
Calculate the concentration of uncomplexed silver ions in a solution that contains 0.10 M Ag(NH3)2+ and 1.0 M NH3. (Kf for Ag(NH3)2+ = 1.5 x 107)
A)6.7 x 10-8 M
B)6.7 x 10-9 M
C)1.5 x 10-7 M
D)0.15 M
E)8.2 x 10-5 M
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