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Review Topic 12: Acids and Bases and Concentrations
Name: Score: 25 / 25 points (100%)
Review Topic 12: Acids and Bases and Concentrations
Multiple Choice
Identify the choice that best completes the statement or answers the question.
C 1. a.
b.
C 2. c.
d.
ANSWER: C
Acids turn the litmus paper red, so the choice that is an acid is HCl.
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a. 0.186 M
b. 0.465 M
c. 0.930 M
d. 1.860 M
ANSWER: C
Molarity = mol/L = 0.465/0.500 = 0.93
27.2 g x B 3. = 0.465 mol
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Review Topic 12: Acids and Bases and Concentrations
a. an acid
b. a base
c. an indicator
d. a colloid
ANSWER: B
Bases neutralize acids
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B 4. How many grams of sodium chloride
are required to prepare 500.0 mL of a
0.100 M solution?
a. 1.46 g
b. 2.93 g
c. 29.3 g
d. 58.5 g
ANSWER: B
0.100 = x/0.500
x = 0.05 mol x = 2.925
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C 5. What is represented by the pH of a solution?
a. Partial pressure of hydrogen ions in the solution
b. Electronegativity of dissociated hydrogen ions in the solution
c. Concentration of hydrogen ions in the solution
d. Temperature of hydrogen ions in the solution
D 6. ANSWER: C
pH stands for the power of hydrogen, which means pH deals with the
concentration of hydronium (hydrogen ions)
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Review Topic 12: Acids and Bases and Concentrations
Which is the best indicator for giving a color change at the equivalence point?
a. Bromocresol green
c. Neutral red
b. Indigo carmine
d. Phenolphthalein
ANSWER: D
The only indicator that the equivalence point of 8.5 falls within is
phenolphthalein.
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A 7. Which pair of solutions would be acidic if mixed in equal quantities?
a. A and B
c. B and D
b. B and C
d. C and D
ANSWER: A
Average the two solutions are:
a ­ 4 ­ acidic
b ­ 7.5 ­ basic
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D 8. Review Topic 12: Acids and Bases and Concentrations
c ­ 9 ­ basic
d ­ 10.5 ­ basic
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Methyl mercury, found in some stream sediments, is highly toxic to animal life. Using
the graphed results of the study shown, the best analysis of the data reveals that the
methyl mercury concentration in the stream sediment is —
a. steadily increasing, accelerating in the fall of each year
b. increasing overall but reaches a minimum in the winter
c. constantly declining throughout each month of the year
d. decreasing but reaches a maximum at the end of summer
B 9. ANSWER: D
The levels overall are going down but they increase during the summer
months.
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Which is the base in the reaction?
a. H2O
b. KOH
c. K+
d. H2SO4
ANSWER: B
The base is KOH, because bases tend to give off OH­
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A 10. What does pH measure?
a. Hydrogen ion concentration
c. Acid density
b. Hydroxide ion concentration
d. Base density
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Review Topic 12: Acids and Bases and Concentrations
ANSWER: A
pH stands for the power of hydrogen, which means pH deals with the
concentration of hydronium (hydrogen ions)
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C 11. A 0.67 L solution of ammonium sulfate, (NH4)2SO4, contains 0.81 mole of the solute. What is the approximate molarity of the solution?
a. 0.54 M
c. 1.2 M
b. 0.83 M
d. 1.5 M
ANSWER: C
Molarity = mol/L = 0.81/0.67 = 1.21 M
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A 12. The pH of a 0.1 molar aqueous solution of HCl would equal —
a. 1
c. 11
b. ­1
d. 13
ANSWER: A
­log(0.1) = 1
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B 13. What is the final concentration if 50.0 mL of a 2.00 M solution are diluted to 500.0
mL?
a. 0.100 M
c. 0.400 M
b. 0.200 M
d. 1.00 M
ANSWER: B
Dilution Problem ­ M1V1 = M2V2 so (50)(2) = (500)x
x = 0.200 M
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D 14. A solution contains 225 g of glucose, C6H12O6, dissolved in enough water to make 0.825
L of solution. What is the molarity of the solution?
a. 0.66 M
c. 1.03 M
b. 0.97 M
d. 1.52 M
ANSWER: D
molarity = mol/L
= 1.25 mol/0.825L = 1.5151M
moles = 225/180 = 1.25 mol
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A 15. How many milliliters of 2.00 M H2SO4 are needed to provide 0.250 mole of H2SO4?
a. 125 mL
c. 8.00 x 103 mL
b. 1.25 x 101 mL
d. 8.00 mL
ANSWER: A
M=mol/L
2 = 0.250mol/L
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Review Topic 12: Acids and Bases and Concentrations
L=0.250/2=0.125 Lx
=125 mL
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C 16. The formula H2SO4 is representative of which of the following?
a. A catalyst
c. An acid
b. A base
d. An organic compound
ANSWER: C
Starts with H
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B 17. The hydrogen ion concentration is 1x10­7. What is the pH of this solution?
a. 1
c. 10
b. 7
d. 14
B 18. ANSWER: B
­log(1x10­7) = 7
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Four aqueous solutions and their concentrations are shown in the above illustration. Which of the
solutions is most likely to be the strongest conductor of electricity?
a. I
b. II
c. III
d. IV
ANSWER: B
C6H12O6 ­ all nonmetals = covalent bonds = nonelectrolyte, so III and IV are
out
NaCl ­ ionic­ electrolyte and there is more in II than I. More you have, the
greater the conductivity.
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C 19. Which is the best estimate of the pH of a solution that has a hydroxide ion concentration of
1.25 x 10­5 M?
a. ­4.903
c. 9.097
b. 4.903
d. ­9.097
ANSWER: C
First remember that hydroxide is [OH­], so first we need to find pOH first by
doing ­log (1.25 x 10­5 M) = 4.903 then taking 14 ­ that answer = 14­4.903 =
9.097
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Review Topic 12: Acids and Bases and Concentrations
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C 20. What is the molarity of a solution with 0.2 moles of potassium permanganate (KMnO4)
dissolved in enough water to make a 500.0 mL solution?
a. 0.0004 M
c. 0.4 M
b. 0.1 M
d. 100 M
ANSWER: C
molarity is mol/L. M=0.2mol/0.500L=0.4M
(500mL ­­> L; you have to divide by 1000)
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B 21. Which of the four substances on this pH scale is slightly basic?
a. Calcium hydroxide
b. Human blood
c. Whole milk
d. Lemon juice
ANSWER: B
A pH of 7 is neutral
less than 7 is an acid
greater than 7 is a base
We want the option that is slightly greater than 7
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Review Topic 12: Acids and Bases and Concentrations
B 22. A common product of acid­base neutralization reactions is ­
a. hydrogen
c. carbon dioxide
b. water
d. oxygen
D 23. ANSWER: B
During a neutralization reaction, an acid (tends to start with H) and a base
(tends to end with OH) react to form water (results from the H and OH coming
together) and a salt.
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Solution
NaHCO3
HClO
NaNO3
CH3NH2
Data Table
Brightness of Light
Bulb
Bright
Dim
Bright
Dim
pH
8.4
3.7
7.0
8.0
Based on the information provided, which solution is a base and a weak electrolyte?
a. NaHCO3
c. NaNO3
b. HClO
d. CH3NH2
ANSWER: D
A weak electrolyte would make the light bulb glow dimly (strong electrolytes
would make it bright). A base has a pH greater than 7. So we need to look for
something that is dim and a pH>7.
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Numeric Response
24. Directions: Type your answer in this box. Use significant figures in your answer.
Calculate the molar mass of a solute in a 1.30 L solution with a molarity of 0.50 M
containing 10.5 g of solute.
RESPONSE: 16
ANSWER: 16
This problem the unit gives you the clue that you need to solve the problem. Molar Mass is grams/moles. They gave you the grams, we just need moles.
Molarity is mol/L, so
0.50 = x/1.30
x = 0.5*1.3
x=0.65
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Review Topic 12: Acids and Bases and Concentrations
The final answer will be 10.5/0.65 = 16.15
Directions are very important on this new SOL so we have to do significant
figures. Since 0.50 has two, our answer must have two.
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POINTS: Directions: Type your answer in the box.
25. Calculate the number of moles of Li3PO4 in 2.2 L of a 0.60 M Li3PO4 solution.
RESPONSE: 1.32
ANSWER: 1.32
Acceptable answers are: 1, 1., 1.3, 1.32, 1.33, 1.4, 2, or 2.
M=mol/L
0.60 = x/2.2
POINTS: x= 1.32
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