Name: 
 

Chemistry 12 - Chapter 8 Quiz



True/False
Indicate whether the sentence or statement is true or false.
 

1. 

The stronger a Brønsted–Lowry acid is, the stronger is its conjugate base.
 

2. 

Group 1 metal ions produce basic aqueous solutions.
 

3. 

Cations that are conjugate acids of weak bases lower the pH of an aqueous solution.
 

4. 

In the titration of a weak acid with a strong base, the pH at the equivalence point is greater than 7.
 

5. 

Given that the bicarbonate ion, HCO3-(aq), is amphoteric with Ka  = 5.6 c12-ch8_files/i0060000.jpg 10-11 and Kb  =
2.4 c12-ch8_files/i0060001.jpg  10-8 , a solution of sodium bicarbonate is neutral.
 

6. 

Given that Kw  = 3.0 c12-ch8_files/i0070000.jpg  10-14 at 40°C, the pH of pure water is 7.00 at this temperature.
 

7. 

A buffer may be composed of an acid and the salt of its conjugate base in unequal concentrations.
 

8. 

Most dyes that act as acid–base indicators are strong bases.
 

9. 

An acid–base indicator should be selected for a particular titration if its pKIn equals the pH at the equivalence point of the titration.
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

10. 

A Brønsted–Lowry base is defined as
a.
a proton donor.
b.
a proton acceptor.
c.
a hydroxide donor.
d.
a hydroxide acceptor.
e.
an electron pair acceptor.
 

11. 

The pH of a 1.25 ´ 10-3 mol/L NaOH(aq) solution is
a.
7.00.
b.
11.10.
c.
12.00.
d.
3.90.
e.
4.90.
 

12. 

Arsenic acid, H3AsO4(aq), reacts with water as follows:
H3AsO4(aq)  + H2O(l)  c12-ch8_files/i0140000.jpg  H2AsO4-(aq)  + H3O+(aq)
      The conjugate base of H3AsO4(aq) in this reaction is:
a.
H3AsO4(aq)
b.
H2O(l)
c.
H3O+(aq)
d.
OH-(aq)
e.
H2AsO4-(aq)
 

13. 

What is the value of Ka for the reaction
NH4+(aq)  + H2O(l) c12-ch8_files/i0150000.jpg  NH3(aq)  + H3O+(aq)
            at SATP, given that Kb for ammonia is 1.74 c12-ch8_files/i0150001.jpg 10-5 at SATP?
a.
5.75  c12-ch8_files/i0150002.jpg 10-10
b.
5.75  c12-ch8_files/i0150003.jpg 104
c.
1.74  c12-ch8_files/i0150004.jpg 10-5
d.
2.98  c12-ch8_files/i0150005.jpg 10-2
e.
112
 

14. 

Which of the following 0.1 mol/L aqueous solutions would be basic?
a.
NH4(ClO4)(aq)
b.
NaCN(aq)
c.
Ca(NO3)2(aq)
d.
H2C2O4(aq)
e.
NaCl(aq)
 

15. 

The pH of a 0.10 mol/L aqueous solution of Fe(NO3)3 is not 7.00. The equation that best accounts for this observation is:
a.
Fe3+(aq) + 3H2O(l) c12-ch8_files/i0170000.jpg  Fe(OH)3(aq) + 3 H+(aq)
b.
NO3-(aq) + H2O(l)  c12-ch8_files/i0170001.jpg  HNO3(aq) + OH-(aq)
c.
Fe(H2O)63+(aq) + H2O(l)  c12-ch8_files/i0170002.jpg
                            Fe(H2O)5(OH)2+(aq)  + H3O+(aq)
d.
Fe(H2O)63+(aq) + H2O(l)  c12-ch8_files/i0170003.jpg 
                         Fe(OH2)5(H3O)4+(aq)  + OH-(aq)
e.
HNO3(aq) + H2O(l)  c12-ch8_files/i0170004.jpg H3O+(aq)  + NO3-(aq)
 

16. 

The percentage ionization in a 0.05 mol/L NH3(aq) solution whose pH  is 11.00 is
a.
11%.
b.
0.02%.
c.
3%.
d.
5%.
e.
2%.
 

17. 

In a titration, 50.0 mL of an acetic acid solution required 20.0 mL of a standard solution of
0.200 mol/L NaOH(aq). The concentration of the acetic acid solution is
a.
0.08 mol/L.
b.
0.50 mol/L.
c.
0.05 mol/L.
d.
1.0 mol/L.
e.
0.30 mol/L.
 

18. 

Which of the following titrations might begin at
pH = 11 and end with pH = 1?
a.
strong acid with strong base
b.
weak base with strong acid
c.
weak acid with strong base
d.
weak acid with weak base
e.
none of the above
 

19. 

Which of the following titrations has pH = 7 at the equivalence point?
a.
hydrochloric acid and sodium hydroxide
b.
hydrochloric acid and ammonia
c.
nitric acid and ammonia
d.
acetic acid and sodium hydroxide
e.
acetic acid and ammonia
 



 
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