Name _____________________________________________ Date _________________ Period ____
Homework and Test Grade Recovery
Chapter 4: Aqueous Reactions and Solution Stoichiometry
Exercises: Sections 4.3: Acid-Base Reactions
1. Define the following terms:
(a) acid.
(b) proton donor
(c) monoprotic acid
(d) diprotic acid
(e) triprotic acid
2. Sulfuric acid is a diprotic acid that ionizes in two steps in aqueous solution. The first deprotonation is
complete but second deprotonation is not. Write a balanced chemical equation for each step.
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3. Acetic acid has 4 hydrogen, but only one is capable of being ionized in water. Explain.
4. The structural formula for citric acid, a main component of citrus fruit, is shown below:
How any H+(aq) can be generated by each citric acid molecule when citric acid is dissolved in water?
Explain.
5.
(a) What are the names and chemical formulas of the 7 strong acids?
(b) Why are these 7 acids called strong acids?
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6. Define a base.
7.
(a) Explain how ionic hydroxides act as bases when they dissolve in water.
(b) Write a balanced chemical equation to show how barium hydroxide acts as a base in aqueous
solution.
8.
(a) Explain how some substances can cause an increase in OH− ions by accepting H+ ions.
(b) Write a balanced chemical equation to show how ammonia acts as a proton acceptor and causes an
increases in OH− ions. (NOTE: ammonia is a WEAK base!)
9.
(a) What are the chemical formulas of the 8 strong hydroxide bases?
(b) Why are these 8 bases called strong bases?
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10.
(a) Which ionic compounds are strong electrolytes?
____________________________________
(b) Which molecular compounds are strong electrolytes?
____________________________________
(c) Which ionic compounds are weak electrolytes?
____________________________________
(d) Which molecular compounds are weak electrolytes?
____________________________________
(e) which ionic compounds are nonelectrolytes?
____________________________________
(f) Which molecular compounds are nonelectrolytes?
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11. Consider equal volumes of the following solutions, each containing the specified amount of dissolved
substance. Which of the following solutions is the most basic? Explain.
a) 0.1 moles NH3
b) 0.1 moles KOH
c) 0.1 moles Ca(OH)2
12. Explain the following observations:
a) HF is called a weak acid, and yet it is very reactive.
b) although sulfuric acid is a strong electrolyte, an aqueous solution of sulfuric acid contains more
hydrogen sulfate ions than sulfate ions.
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13. Classify each of the following as a strong or weak acid or base:
a) H2CO3
_______________
c) HBr
b) Ca(OH)2 _______________
_______________
d) HC7H5O2 _______________
14. Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the
substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of
molecules and ions.
Substance
Acid(A),
Base (B),
Salt (S),
or
None of these (N)
Existence in Aqueous Solution
(Please mark with a √ those that apply)
Moleular
form
Ions
Mixture
a) HF
b) Acetonitrile, CH3CN
c) NaClO4
d) Ba(OH)2
15. What is the relationship between the solubility rules in Table 4.1 and the list of strong bases in table 4.2?
Another way of asking this question might be " Why is Cd(OH)2 not listed as a strong base in Table 4.2?"
16. Classify each of the following aqueous solutions as a nonelectrolyte (NE), weak electrolyte (WE), or strong
electrolyte (SE).
(a) HBrO
__________
(c) KOH
__________
(e) C12H22O11 __________
(b) HNO3
__________
(d) CoSO4
__________
(f) O2
__________
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17. Define the following terms:
(a) neutralization reaction.
(b) salt
18. What are the products of a neutralization reaction between an acid and a metal hydroxide?
19. Write the balanced 1) molecular, 2) complete ionic, and 3) net ionic equations for each of the following
neutralization reactions. In each case identify the name of the salt which is formed. Don't forget phases of
matter!
a) Aqueous acetic acid is neutralized by aqueous potassium hydroxide. (REMEMBER - acetic acid is a
weak acid!)
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19. Continued:
b) Solid calcium hydroxide reacts with nitric acid. (REMEMBER - nitric acid is a strong acid!)
c) Fe(OH)3(s) and HClO4(aq) react. (REMEMBER - perchloric acid is a strong acid!)
20. Why is carbonic acid considered and unstable acid? Write a balanced chemical equation to help illustrate
your answer.
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21. Consider your answer to Question 20 as you write the molecular, complete and net ionic equations for the
following reaction.
Solid CaCO3 reacts with an aqueous solution of nitric acid to form a salt, water, and a gas
22. Write the molecular and complete and net ionic equations for the following reaction.
Solid iron (II) sulfide reacts with an aqueous solution of hydrobromic acid to form a salt and
the gas hydrogen sulfide
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23. As solid K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions.
a) Write the molecular and complete and net ionic equations for this reaction.
b) Based on the definitions of acid and base, what ion is the base in this reaction? _________________
c) What is the acid? _________________________________
d) What is the spectator ion in this reaction? ____________
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