Name _______________________________________________________
Date _______________________
Acids, Bases, and Salts Review Packet
1. Which species can conduct an electric current?
(1) NaOH (s)
(2) CH3OH (aq)
(3) H2O (s)
(4) HCl (aq)
2. An aqueous solution of an ionic compound turns red litmus blue, conducts electricity, and
reacts with an acid to form a salt and water. This compound could be
(1) HCl
(2) NaI
(3) KNO3
(4) LiOH
3. According to Table J, which metal will react with 0.1 M HCl?
(1) Au (s)
(2) Ag (s)
(3) Hg ()
(4) Mg (s)
4. Which 0.1 M solution turns phenolphthalein pink and red litmus blue?
(1) HCl (aq)
(2) CO2 (aq)
(3) NaOH (aq)
(4) CH3OH (aq)
5. Which compound reacts with an acid to form a salt and water?
(1) CH3Cl
(2) CH3COOH
(3) KCl
6. Which substance can be classified as an Arrhenius acid?
(1) HCl
(2) NaCl
(3) LiOH
(4) KOH
(4) KOH
7. In an aqueous solution, which substance yields hydrogen ions as the only positive ions?
(1) C2H5OH
(2) CH3COOH
(3) KH
(4) KOH
8. Which substance, when dissolved in water, is an acid according to the alternative theory?
(1) CH3OH
(2) NaOH
(3) C2H5COOH
(4) CH3COO9. In the reaction:
NH3 (g) + H2O ()  NH4+ (aq) + OH- (aq)
According to the alternate theory, the NH3 (g) acts as
(1) an acid only (2) a base only (3) both acid and base
(4) neither acid nor base
10. Which reaction best illustrates amphoterism?
(1) H2O + HCl  H3O+ + Cl(2) NH3 + H2O  NH4+ + OH(3) H2O + H2SO4  H3O+ + HSO4(4) H2O + H2O  H3O+ + OH11. Given the equation:
H+ + OH-  H2O
Which type of reaction does this equation represent?
(1) esterification
(2) decomposition
(3) hydrolysis
(4) neutralization
12. How many milliliters of 0.20 M HCl are needed to exactly neutralize 40 mL of 0.4 M KOH?
(1) 2 mL
(2) 40 mL
(3) 80 mL
(4) 160 mL
13. How many milliliters of 4 M HCl are needed to exactly neutralize 20 mL of 2 M Ca(OH)2?
(1) 2 mL
(2) 4 mL
(3) 10 mL
(4) 20 mL
14. A 3 mL sample of HNO3 solution is exactly neutralized by 6 mL of 0.5 M KOH. What is the
molarity of HNO3?
(1) 1.0 M
(2) 0.5 M
(3) 3 M
(4) 1.5 M
15. Which type of reaction occurs when 50 mL quantities of Ba(OH)2 (aq) and H2SO4 (aq) are
combined?
(1) hydrolysis
(2) ionization
(3) hydrogenation
(4) neutralization
16. What are the relative ion concentrations in an acid solution?
(1) more H+ ions than OH- ions
(2) fewer H+ ions than OH- ions
(3) equal number of both ions
(4) H+ ions but no OH- ions
17. What is the pH of a solution with a hydronium ion concentration of 0.01 mole per liter?
(1) 1
(2) 2
(3) 10
(4) 14
18. Which pH value indicates the most basic solution?
(1) 7
(2) 8
(3) 3
(4) 11
19. An aqueous solution with a pH of 4 would have a hydroxide ion concentration of
(1) 1 x 10-4 M
(2) 1 x 10-7 M
(3) 1 x 10-10 M
(4) 1 x 10-14 M
20. An aqueous solution with a pH of 2 would have a hydrogen ion concentration of
(1) .001 M
(2) .01 M
(3) .1 M
(4) 1 M
Part 2 Questions
1. Name the following:
a) HBr
b) HNO3
c) HNO2
d) CH3COOH
e) Mg(OH)2
2. Write the formula for the following:
a) Hydrofluoric Acid b) Sulfuric Acid c) Carbonic Acid d) Chlorous Acid
e) Calcium Hydroxide
3. What is an electrolyte? Which groups of substances are considered electrolytes?
Nonelectrolytes?
4. What is an Arrhenius acid? An Arrhenius base? How can you tell if they are strong or weak?
5. What is the Alternative Theory?
6. List the properties of acids and bases.
7. Complete the following:
Zn (s) + HCl (aq) 
Mg (s) +
NaOH (aq) 
H2SO4 (aq) + Ca(OH)2 (aq) 
8. What is the pH and the relationship between [H+] and [OH-] in acidic, basic, and neutral
solutions?
9. a) If a lake at pH 6 experiences a 1,000-fold increase in H+ ions, what is the new pH?
b) If a lake at pH 5 experiences a 10-fold decrease in OH- ions, what is the new pH?
10. A solution was yellow in bromthymol blue and blue in bromcresol green. What is the pH
range of this solution?
Answer Key
1.
2.
3.
4.
5.
4
4
4
3
4
6. 1
7. 2
8. 3
9. 2
10. 4
11.
12.
13.
14.
15.
4
3
4
1
4
16.
17.
18.
19.
20.
1
2
4
3
2
Part 2
1. a) hydrobromic acid b) nitric acid c) nitrous acid d) acetic acid e) magnesium hydroxide
2. a) HF b) H2SO4 c) H2CO3 or CO2 (aq) d) HClO2 e) Ca(OH)2
3. An electrolyte is a substance that produces ions and can conduct electricity in solution.
Electrolytes include acids, bases, and salts. Nonelectrolytes include sugars and alcohols.
4. An Arrhenius acid produces H+ (hydrogen) (H3O+ (hydronium)) ions in solution. An
Arrhenius base produces OH- (hydroxide) ions in solution. Strength of acids and bases
depend on how much the substance breaks up (ionizes) and its molarity.
5. According to the Alternative Theory, an acid is a proton (H+) donor and a base is a proton
(H+) acceptor (BAAD). This theory explains why ammonia, NH 3, is a base.
6. Acids – taste sour, electrolytes, react with bases to form water and salt in a neutralization
reaction, react with active metals (higher than H2 on Table J) to form hydrogen gas and salt,
turn indicators colors (red in litmus, clear in phenolphthalein).
Bases – taste bitter, feel slippery/soapy, electrolytes, react with acids to form water and salt
in a neutralization reaction, do not react with metals, turn indicators colors (blue in litmus,
pink in phenolphthalein).
7. Zn (s) + 2 HCl (aq)  H2 (g) + ZnCl2 (aq)
Mg (s) + NaOH (aq)  no reaction
H2SO4 (aq) + Ca(OH)2 (aq)  2 H2O () + CaSO4 (s)
8. Acidic – pH below 7, [H+] > [OH-]
Basic – pH above 7, [H+] < [OH-]
Neutral – pH = 7, [H+] = [OH-]
9. a) pH = 3
10. 5.4 – 6.0
b) pH = 4