Which of the following statements is not true concerning the following aqueous equilibrium?

1.
(Points: 1)     Which of the following statements is not true concerning the following aqueous equilibrium?
H+(aq) + NO3-(aq) <=> HNO3 (aq)


 a. The equilibrium lies to the left.
 b. The equilibrium lies to the right.
 c. The concentration of protons equals the concentration of aqueous HNO3.
 d. The concentration of protons equals the concentration of nitrate.
 e. Both B and C.
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2.
(Points: 1)     Match each acid or base to the appropriate description:
Column preview
H2SO4   Lewis acid
   
H2SO3   Weak Bronsted acid
   
BCl3   Weak Bronsted base
   
OH-   Strong Bronsted acid
   
NH3   Strong Bronsted base
   

Matching pairs
H2SO4   

H2SO3   

BCl3   

OH-   

NH3   

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3.
(Points: 1)     What is the degree of ionization for 0.504 M aqueous benzoic acid?

 a. 0.8%
 b. 1.1%
 c. 1.6%
 d. 98.9%
 e. 99.2%
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4.
(Points: 1)     Which of the following acids produces the weakest conjugate base (smallest Kb)?

 a. HNO2
 b. HNO3
 c. NH4+
 d. H2O
 e. CH3CO2H
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5.
(Points: 1)     Match the following bases with the corresponding conjugate acid:

Column preview
1. (CH3)2NH   a. (CH3)2NH2+
   
2. (CH3)2N-   b. HO-
   
3. HO-   c. H3O+
   
4. H2O   d. (CH3)2NH
   
5. O2-   e. H2O
   

Matching pairs
1   

2   

3   

4   

5   

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6.
(Points: 1)     Rank the following acids based on increasing Ka:
Matching pairs
HBrO2   

HBrO3   

HBrO4   

HClO4   

HBrO   

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7.
(Points: 1)     Which of the following statements is not true for a neutral aqueous solution?

 a. [H+] = [OH-]
 b. [OH-] = 10-14
 c. pH = pOH
 d. [H+] [OH-] = 10-14
 e. Both B and C.
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8.
(Points: 1)     What is the pH of 3.5 x 10-3 M HClO4?

 a. 3.5 x 10-3
 b. 2.5
 c. 3.0
 d. 3.5
 e. 10.5
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9.
(Points: 1)     What is the pH of 1.20 M HClO2?

 a. -0.08
 b. 0.08
 c. 0.66
 d. 0.96
 e. 1.96
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10.
(Points: 1)     What is the pH of 0.220 M sodium acetate?

 a. 13.34
 b. 9.05
 c. 4.95
 d. 4.65
 e. 0.66
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11.
(Points: 1)     What is the pH of an aqueous solution prepared with 150 mL of 0.150 M ammonia and 15.0 mL of 1.20 M HCl?

 a. 9.85
 b. 9.35
 c. 9.25
 d. 9.15
 e. 8.65
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12.
(Points: 1)     What is the solubility of lead (II) bromide in pure water?

 a. 1.9 x 10-2 M
 b. 1.5 x 10-2 M
 c. 1.2 x 10-2 M
 d. 2.6 x 10-3 M
 e. 6.6 x 10-6 M
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13.
(Points: 1)     What is the solubility of lead (II) bromide in 1.2 M potassium bromide (KBr)?

 a. 4.6 x 10-6 M
 b. 5.5 x 10-6 M
 c. 2.6 x 10-3 M
 d. 1.2 x 10-2 M
 e. 1.9 x 10-2 M
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14.
(Points: 1)     What is the change in oxidation number for chromium in the following aqueous reaction?
2 H+ + Cr2O72- + 3 Mn2+ -> 2 Cr3+ + 3 MnO2 (s) + H2O


 a. +12 to +6
 b. -2 to +3
 c. -2 to +6
 d. +6 to +3
 e. +6 to 0
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15.
(Points: 1)     Which of the following statements is not true for an electrolytic cell?

 a. Electrons will spontaneously flow between the anode and cathode.
 b. Electrons will not spontaneously flow between the anode and cathode.
 c. Energy must be applied to cause electrons to flow between the anode and cathode.
 d. An oxidation half-reaction occurs at the anode.
 e. Electrons flow into the the cathode.
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16.
(Points: 1)     Which of the following elements does not appear in the table of standard reduction potentials in Appendix 6 of the textbook?

 a. Gold
 b. Iodine
 c. Manganese
 d. Platinum
 e. Sodium
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17.
(Points: 1)     What is the value of standard cell potential (Eocell) for the following reaction?
Ag+(aq) + Cr2+(aq) -> Ag(s) + Cr3+(aq)


 a. -1.21 V
 b. -0.39 V
 c. 0.41 V
 d. 0.80 V
 e. 1.21 V
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18.
(Points: 1)     What is the value of standard cell potential (Eocell) for the following reaction?
Sn4+(aq) + Cu(s) -> Sn2+(aq) + Cu2+(aq)


 a. -0.49 V
 b. -0.19
 c. 0.15
 d. 0.19 V
 e. 0.49 V
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19.
(Points: 1)     How many electrons are transferred (n) in the following redox reaction?
3 Fe3+(aq) +MnO2 (s) + 4 OH-(aq) -> 3 Fe2+(aq) + MnO4- (aq) + 2 H2O(s)


 a. 1
 b. 2
 c. 3
 d. 4
 e. 5
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20.
(Points: 1)     What is the value of standard cell potential (Eo) for the following reaction?
3 Fe3+(aq) +MnO2 (s) + 4 OH-(aq) -> 3 Fe2+(aq) + MnO4- (s) + 2 H2O


 a. -1.36 V
 b. -0.18 V
 c. 0.18 V
 d. 1.36 V
 e. 1.72 V
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21.
(Points: 1)     What is the value of standard change in Gibb's free energy (deltaGo) of the following reaction?
3 Fe3+(aq) +MnO2 (s) + 4 OH-(aq) -> 3 Fe2+(aq) + MnO4- (s) + 2 H2O


 a. 390 kJ/mole
 b. 52 kJ/mole
 c. -52 kJ/mole
 d. -390 kJ/mole
 e. -500 kJ/mole
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22.
(Points: 1)     What half reaction occurs at the cathode in the following electrochemical cell if all the aqueous ions are at 1 M?
Pt(s) | Cu+(aq) , Cu2+(aq) || Fe2+ (aq) , Fe3+(aq) | Pt(s)


 a. Pt+ + e- -> Pt
 b. Fe+3 + e- -> Fe+2
 c. Fe+2 -> Fe+2 + e-
 d. Cu+2 + e- -> Cu+
 e. Cu+ -> Cu2+ + e-
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23.
(Points: 1)     What is the predicted value of cell potential (Eo) for the following electrochemical cell at 298 K?
Pt(s) | Ag(s) | Ag+(0.225 M) || Hg2+(0.105 M) | Hg(l) | Pt(s)


 a. 0.03 V
 b. 0.04 V
 c. 0.05 V
 d. 0.06 V
 e. 0.07 V
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24.
(Points: 1)     What is the concentration of Cu+(aq) in the following electrochemical cell if Ecell = 0.501 V?
Cd(s) | Cd2+(0.120 M) || Cu+(aq), Cu2+(0.021 M) | Pt(s)


 a. 3.57 M
 b. 1.93 M
 c. 0.52 M
 d. 0.18 M
 e. 0.03 M