Acids and Bases
1. The properties of acids include _____________.
a. reacting with metals to produce oxygen
b. giving foods a sour taste
c. forming solutions that conduct electricity
d. acting as an electrolyte
2. Is the following sentence true of false? Acids react with compounds
containing hydroxide ions to form water and a salt.
3. Bases are compounds that react with acids to form salt and a(n) _water_.
4. The properties of bases include ________. (circle all that apply)
a. Tasting bitter
b. Feeling slippery
c. Changing the color of an indicator
d. Always acting as a strong electrolyte
5. What is an acid? Proton donor, electron pair acceptor, compound that forms
hydrogen ions in aqueous solution
6. When the name of an anion in an acid ends in –ide, the acid name begins
with the prefix _hydro_ and ends with the suffix __ic___.
7. When there are more than two elements in the acid, the name of the acid
begins with the prefix _of the polyatomic ion_; and when the suffix on the
polyatomic ion is –ite, the suffix of the acid is __ous_ and when suffix on the
polyatomic ion is –ate, the suffix on the acid is _ic__.
8. Write the formula for and name the acid formed between hydrogen and the
following ions:
a. F-
HF hydrofluoric acid
b. ClO-1 HClO hypochloric acid
c. Br- HBr hydrobromic acid
d. PO3-3 H3PO3 phosphorous acid
e. S-2 H2S hydrosulfuric acid
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Acids and Bases
9. Acids are compounds that dissolve in water to form _hydrogen_ ions.
10. Bases are compounds that dissolve n water to form hydroxide ions.
11. What do we call a water molecule that gains a hydrogen ion? Hydronoum ion
12. A hydrogen ion is simply which subatomic particle? proton
13. The reaction in which two water molecules react to form ions is known as the
self-ionization of water.
14. True or false: Any aqueous solution in which the [H+] and [OH-] are equal is
described as a neutral solution.
15. Explain the following definitions of acids and bases:
a. Arrhenius definition acid – substance that releases hydrogen ions in
aqueous solution; base substance that releases hydroxide ions in
solution
b. Bronsted-Lowery definition acid – hydrogen ion (proton) donor;
base – hydrogen ion (proton) acceptor
c. Lewis definition base – electron pair donor; acid – electron pair
acceptor
16. Which definition of acids and bases is solvent dependent? Which solvent is
specified? Arrhenius; water
17. Write the equation for the production of the hydronium ion.
HOH + HOH   H3O+ + OH-
18. What term describes an acid, base of salt which, when dissolved in water
conducts and electrical current? Electrolyte
19. The conjugate base of an acid is the particle that remains after a proton
has been released by the acid.
20. The conjugate acidof a base is the particle that forms when the base
accepts a proton.
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Acids and Bases
21. What is the relationship between an acid and its conjugate base? Acid
loses a proton to form conjugate base, conjugate base could add a proton
to reform acid between a base and its conjugate acid? Base adds a proton
to form conjugate acid, conjugate acid could lose a proton to reform base
22. What is the term for a substance that can act as either an acid or a
base? amphoteric
23. What substance is the most common example of the above?
water
24. Identify the acid, base, conjugate acid and conjugate base in each of the
following:
a. H2SO3 + OH-   HSO3- + H2 O
A
B
CB
CA
b. HSO3 + OH   S03 + H2O
A
B
CB
CA
c. HCHO2 + H2O   CHO2 + H3O+
A
B
CB
CA
+
d. C5 H5 N + H2O   C5 H5 NH + OHB
A
CA
CB
25. Write the conjugate acid/base of the following:
a. NH4+ NH3
b. ClO- HClO
c. OH- H2O
d. HCl Cle. H30+
H2O
f. H2O H30+ or OHH2SO4 SO4-2
26. Write both the conjugate acid and the conjugate base of HSO4-
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Acids and Bases
Match the following terms with the correct description.
_D__
27. a base that dissociates completely in
solution
__E_
28. an oxide that produces an acid when
dissolved in water
_C__
_F__
__A__
__B_
29. an acid that ionizes completely in
solution
30. an oxide that produces a base when
dissolved in water
31. an acid that dissociates slightly when
in solution
32. a base that only partially dissociates in
solution
A. weak acid
B. weak base
C. strong acid
D. strong base
E. acidic anhydride
F. basic anhydride
33. Classify each of the following as a strong acid, strong base, weak acid or weak
base:
a. NaOH SB
b. HCl SA
c. NH4+ WA
d. NH3 WB
e. Cl- WB
f. HI SA
g. H2SO4 SA
h. H2CO3 WA
i. HNO3 SA
34. Give two properties of an acid and a base that would enable you identify them in
the lab Acid – pH <7, electrolyte; base – pH >7, slippery
35. What is a salt? How is it formed? Give 3 examples. Ionic compound that is not an
acid or a base, forme from the reaction between an acid and a base, or between an
anhydride with and acid or base
36. What is a neutralization reaction? What compound is always a product?
reaction between and acid and a base, that forms water and a salt
37. Complete the following neutralization reactions – if the acid is polyprotic, write
the reaction in mutilple steps:
a. KOH + HCl KCl + H2O
b. Ca(OH)2 + HNO3  Ca(NO3)2 + H2O
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Acids and Bases
c. H2SO4 + Mg(OH)2 HSO4- + H2O + Mg2+  2 H2O + MgSO4
d. NaOH + H2CO3  HCO3- + H2O + Na+  2 H2O + NaOH
e. HC2H3O2 + KOH KC2H3O2 + H2O
38. Are all salt solutions neutral?
no
39. What is hydrolysis?
addition of water
40. In the reactions in question 38, are the salt solutions formed acidic, basic or
neutral? A neutral, B neutral, C neutral, D basic, E basic
41. Identify each of the following salts as acidic, basic or neutral in solution?
a. K2CO3 basic
b. NH4NO3 acidic
c. AlCl3 neutral
d. KNO3 neutral
e. PbSO4 neutral
42. What is the molarity of a solution containing 10.0g of NaOH in 200.0 ml of
solution?
1.25M
43. How many grams of NaOH must be dissolved in 300.0 ml of solution to make a
1.3M solution?
15.6 g
44. If 26.4 cm3 of LiOH solution are required to neutralize 21.7 ml of 0.500M HBr,
what is the concentration of the basic solution?
(1)(21.7ml)(0.500M) = (M)(26.4ml)(1)
.41M
45. If 23.4 cm3 of 0.55M NaOH is used to titrate 50.0cm3 of the HCl to the endpoint,
what is the concentration of the HCl solution?
(1)(M)(50.0 ml) = (0,55M)(23.4 ml)(1)
.26M
46. If 75.0 cm3 of 0.823M HClO4 required 95.5 cm3 of Ba(OH)2 for complete
neutralization, what is the concentration of the Ba(OH)2 solution?
(1)(0.823M)(75.0ml) = (M)(95.5ml)(2)
.32M
47. If 40.0 cm3 of 0.106M sulfuric acid neutralized 50.0 cm3 of potassium hydroxide
solution, find the concentration of the base?
.169M
48. How many ml of 0.18M Al(OH)3 are needed to neutralize 25.0 ml of 0.25M
HNO3?
11.6ml
49. How many ml of 0.25M liOH are needed to neutralize 25.0ml of 0.10M H2SO4?
20 ml
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Acids and Bases
50. Write the formulas for the anhydrides of the following:
a. H2CO3 CO2
b. H2SO4 SO3
c. H2SO3 SO2
d. NaOH Na2O
e. Ca(OH)2 CaO
f. HNO3 N2O5
51. True or False: Most pH values are whole numbers.
52. If the [H+] is written in scientific notation, but the coefficient is not 1, what
mathematical factor do you need to determine the pH?
-log
53. True or False: You can calculate the hydrogen ion concentration of a solution if
you know the pH.
54. What is an indicator?
solution that changes color at a particular pH
55. When do you use indicators and when do you use a pH meter to measure pH?
indicator qualitative, pH meter quantitative
56. How is an indicator a valuable tool in determining pH?
determines if a solution is acid or base
57. why do you need many different indicators to span the entire pH spectrum?
to identify multiple pH changes
58. What is a buffer and how does it work?
solution containing a salt and an acid or base that stabilizes the pH of the solution
59. Define pH and pOH
pH – percent hydrogen; pOH – percent hydroxide
60. Find the pH of solutions with the following hydrogen ion concentration:
a. 1.00 x 10-3M 3
b. 1.00 x 10-6 M 6
c. 6.49 x 10-10M 9.19
d. 7.01 x 10-6M 5.15
e. 9.47 x 10-8M 7.02
f. 6.89 x 10-14M 13.16
61. Find the hydrogen ion concentration of the following solutions:
a. pH = 3.00 1 x 10-3
b. pH = 10.00 1 x 10-10
c. pH = 6.607 2,47 x 10-7
d. pH = 2.253 5,58 x 10-3
e. pH = 6.149 7.10 x 10-7
f. pH = 7.662 2.18 x 10-8
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Acids and Bases
62. Find the pH of the following solutions:
a. pOH = 2.00 12
b. pOH = 7.00 7
c. pOH = 1.23 12.77
d. pOH = 1.263 12.737
e. pOH = 4.976 9.024
f. pOH = 9.714 4.286
g. pOH = 3.004 10.996
63. Differentiate between a strong acid and a weak acid.
strong acid dissociates to a great degree, weak acid to a lesser degree
64. Distinguish between strong and concentrated acids.
strong base dissociates to a great degree, weak base to a lesser
degree
65. Given the solutions below:
a.
b.
c.
d.
e.
Solution
pH
A
2
B
10
C
5
D
1
E
13
Which are acid solutions A,C,D
Name the strongest acid and the strongest base Acid – D; Base
-E
Which has the highest [H3O+]? D
Which has the highest [OH-]? E
Calculate the [OH-] and the [H3O+] for each solution
A [H] = 1 x 10-2; [OH} = 1 x 10-12
C [H] = 1 x 10-5; [OH] = 1 x 10-9
66. What is Ka, Kb. and Kw?
a. Write the Ka expressions for HC2H3O2 and H2SO4
b. Write the Kb expressions for an NH3 solution in water.
c. Write the Kw expression.
67.
In a water solution where 2H2O ↔ OH- + H3O+
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68.
69.
70.
a. What happens to the equilibrium if additional OH- is added to
the solution?
b. What happens to the concentration of H3O+ when additional
OH- is added?
c. What happens to the pH when additional OH- is added?
d. [OH-][H3O+] = ______________
Given the equilibrium HC2H3O2 ↔ H+ + C2H3O2-, if Na C2H3O2 is added
to the solution
a. Which direction will the equilibrium shift? left
b. What happens to the concentration of [H+]? decrease
c. What happens to the pH? increase
d. Since this solution contains a weak acid and a salt, it is an
example of a __buffer_. What is the benefit of this type of
solution?
e. How could a solution of NH3 be buffered?
ammonium salt
Using the ionization reaction above for acetic acid,
a. Write the Ka expression
Ka = [H][C2H3O2]
[HC2H3O2]
b. Calculate the [H+] for a 0.1M solution of HC2H3O2 if Kb = 1.8 x
10-5
1.8 x 10-5 = [X][X]
[0.1M]
-4
4.24 x 10
The Ka for HNO2 is 4.6 x 10-4. Find the [H+] in a 0.01M solution.
71.
In a 0.3M solution of H2CO3, the concentration of the HCO3- is 3.6 x
10-4M. What is the percent ionization of the H2CO3 molecule?
72.
The Ka for HF is 3.53 x 10-4. Find the % ionization in a 0.50M solution.
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