Accelerated chemistry with Ms. Lara
Final revision
Revision I
1. What is the difference between the end point and the equivalence point? [2]
2. A titration is done between a strong acid and a weak base. Will the pH at the equivalence
point be less than 7, exactly 7, or greater than 7? Why? [2]
Q2. Complete the table. [7]
Acid
Base
1
HNO2
H2O
2
H2O
F-
Conjugate Acid Conjugate Base
HNO2 + H2O → NO2– + H3O+
HF
OHNH3 + HCN → NH4+ + CN–
3
4
5
H2O
HSO4-
ClO3-
PO4-3
S2– + H2O → OH– + HS–
6
7
Equation
HCO2H
OH-
Multiple choice :
1. Acids taste: [1]
a. Sweet
b. Sour
c. Bitter
d. Salt
2. Acids make litmus paper turn [1]
a. Red
b. Yellow
c. Blue
d. Blac
Accelerated chemistry with Ms. Lara
Final revision
3. Bases feel
a. Rough
b. Moist
4. Bases react with
a. Acids to produce salts &
water
b. Salts to produce acids &
water
c. Slippery
d. Dry
c. Water to produce acids &
salts
d. Neither acids, salts, nor water
5. Which is the product of the chemical reaction between potassium hydroxide and
hydrobromic acid? [1]
a. Acidic
c. Neutral
b. Basic
d. I dunno Mr. Saad
6. What is the pH when the hydrogen ion concentration is 1x10-3 M
a. 2
c. 3
b. 2.7
d. 3.3
7. A solution with a pH of 5.0 ____
a. is basic
b. has a hydrogen-ion concentration of 5.0M
c. is neutral
d. has a hydroxide-ion concentration 1x10-9M
Problems 8-11 relate to the following table.
Some thoughts:
Acids and bases could be strong or weak, a laboratory technique that could be used to
differentiate between a strong acid and a weak acid is by electrical conductivity.
Remember strong acids ionize completely while weak ionize partially.
Solution
Electrical Conductivity
Original Color of
Color of Litmus Paper After
No.
of solution
Litmus Paper
Dipping in Solution
1
Very High
Red
Blue
2
Low
Blue
Red
3
Moderate
Red
Red
4
Very High
Blue
Red
8. The table shows data from an investigation designed to find a liquid solution that is both
an acid and a strong electrolyte. Based on the data, a solution that is both an acid and a
strong electrolyte is a. Solution 1
c. Solution 3
b. Solution 2
d. Solution 4
Accelerated chemistry with Ms. Lara
Final revision
9. Which of the following solutions is the weakest acid [1]
a. Solution 1
c. Solution 3
b. Solution 2
d. Solution 4
10. Which of the following solutions is the strongest base [1]
a. Solution 1
c. Solution 3
b. Solution 2
d. Solution 4
11. Which of the following solution pairs make the best electric conductors [1]
a. Solutions 1 & 2
c. Solutions 3 & 4
b. Solutions 2 & 3
d. Solutions 4 & 1
12. Which statement about Arrhenius acids is FALSE [1]
a. Their water solutions are called aqueous acids
b. They are molecular compounds with ionizable hydrogen atoms.
c. Their pure aqueous solutions are electrolytes.
d. They increase the concentration of hydroxide ions in aqueous solution.
13. Strong bases are [1]
a. Strong electrolytes
b. Weak electrolytes
c. Nonelectrolytes
d. Also strong acids
14. Whose definition of acids & bases emphasizes the role of protons? [1]
a. Bronsted-Lowry
c. Arrhenius
b. Lewis
d. Faraday
15. What is the pH of a 1x10-4 M HCl solution? [1]
a. 4
b. 6
c. 8
d. 10
16. What is the pH of a 1x10-5 M KOH solution? [1]
a. 3
b. 5
c. 9
d. 11
17. Two clear solutions are place in separate beakers. The first solution has a pH of 4, and the
pH of the second solution is unknown. If the two solutions are mixed and the resulting
pH is 5, the second solution must have [1]
a. Fewer suspended solids
b. A lower temperature
c. More dissolved salt NaCl particles
d. A higher concentration of OH- ions
18. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL
of 0.400 M NaOH? [1]
a. 0.200 M
c. 0.320 M
b. 0.280 M
d. 0.500 M
Accelerated chemistry with Ms. Lara
Final revision
19. Which of the following is a weak acid [1]
a. HNO3
b. HI
c. HBr
d. H
Q4. Lab based Questions
1. Design an experiment Describe how you would set-up and perform a titration in which
you use 0.250M HNO3 to determine the molarity of a cesium hydroxide (CsOH) solution.
Include the formula and net ionic equations. [4]
2. After you carry out your experiment, it takes 25.0 mL of HNO3 to neutralize a 40.0 mL
sample of CsOH. Calculate the concentration of the cesium hydroxide sample. [4]
Accelerated chemistry with Ms. Lara
Final revision
Revision II
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
1. What is the concentration of H3O+ ions in pure water?
a. 10–7 M
c. 55.4 M
b. 0.7 M
d. 107 M
____
2. What is the pH of a 10–5 M KOH solution?
a. 3
c. 9
b. 5
d. 11
____
3. How would you classify CH3COOH in the equation below?
a. a weak acid
b. a strong acid
c. a weak base
d. a strong base
____
4. The pH range over which an indicator changes color is its
a. equivalence point.
c. transition interval.
b. end point.
d. pH interval.
____
5. An acid-base titration involves a
a. composition reaction.
b. neutralization reaction.
c. single-displacement reaction.
d. decomposition reaction.
____
6. Which quantity is directly measured in a titration?
a. mass
c. volume
b. concentration
d. Density
____
7. During an acid-base titration, a very rapid change in pH
a. occurs when the first addition of the known solution is made.
b. occurs when the amounts of H3O+ ions and OH– ions are nearly equivalent.
c. occurs at several points during the titration.
d. does not occur during titration.
Accelerated chemistry with Ms. Lara
Final revision
____
8. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of
0.400 M NaOH?
a. 0.200 M
c. 0.320 M
b. 0.280 M
d. 0.500 M
____
9. What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247
M H2SO4?
a. 0.0101 M
c. 0.0402 M
b. 0.0201 M
d. 0.0805 M
____ 10. The Haber process for producing ammonia commercially is represented by the equation N2(g) +
3H2(g) 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many
moles of nitrogen gas are required?
a. 1.0 mol
c. 3.0 mol
b. 2.0 mol
d. 6.0 mol
____ 11. In the equation 2KClO3 2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol
of KClO3 decompose completely?
a. 1.0 mol
c. 3.0 mol
b. 2.5 mol
d. 4.5 mol
Accelerated chemistry with Ms. Lara
Final revision
Use the table below to answer the following questions.
Element
Bromine
Calcium
Carbon
Chlorine
Cobalt
Copper
Fluorine
Hydrogen
Iodine
Iron
Lead
Magnesium
Mercury
Nitrogen
Oxygen
Potassium
Sodium
Sulfur
Symbol
Br
Ca
C
Cl
Co
Cu
F
H
I
Fe
Pb
Mg
Hg
N
O
K
Na
S
Atomic Mass
79.90
40.08
12.01
35.45
58.93
63.55
19.00
1.01
126.90
55.85
207.2
24.30
200.59
14.01
15.00
39.10
22.99
32.01
____ 12. For the reaction represented by the equation 2H2 + O2
produced from 6.00 mol of hydrogen?
a. 2.00 g
c. 54.0 g
b. 6.00 g
d. 108 g
2H2O, how many grams of water are
____ 13. For the reaction represented by the equation Pb(NO3)2 + 2KI PbI2 + 2KNO3, how many moles
of lead(II) iodide are produced from 300. g of potassium iodide and an excess of Pb(NO3)2?
a. 0.904 mol
c. 3.61 mol
b. 1.81 mol
d. 11.0 mol
____ 14. For the reaction represented by the equation 2Na + 2H2O 2NaOH + H2, how many grams of
hydrogen are produced if 120. g of sodium and 80. g of water are available?
a. 4.5 g
c. 80. g
b. 45 g
d. 200 g
____ 15. For the reaction represented by the equation SO3 + H2O H2SO4, calculate the percentage yield
if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid.
a. 82.7%
c. 91.2%
b. 88.3%
d. 93.9%
Accelerated chemistry with Ms. Lara
Final revision
____ 16. For the reaction represented by the equation CH4 + 2O2 2H2O + CO2, calculate the percentage
yield of carbon dioxide if 1000. g of methane react with excess oxygen to produce 2300. g of
carbon dioxide.
a. 83.88%
c. 92.76%
b. 89.14%
d. 96.78%
Short Answer
17. How can the equivalence point in a titration be detected by using a pH meter?
Use the graph below to answer the following questions.
18. What is the approximate volume of the titration standard added to reach the equivalence point,
and what is the pH of the solution at this point?
19. Is the unknown solution an acid or a base, and what is its relative strength (weak or strong)? Is
the titration standard an acid or base, and what is its relative strength?
Accelerated chemistry with Ms. Lara
Revision II answers
MULTIPLE CHOICE
1. ANS: A
2. ANS: C
Solution:
3. ANS: A
4. ANS: C
5. ANS: B
6. ANS: C
7. ANS: B
8. ANS: C
Solution:
9. ANS: C
Solution:
10. ANS: C
11. ANS: D
12. ANS: D
Final revision
Accelerated chemistry with Ms. Lara
Final revision
Solution:
13. ANS: A
Solution:
14. ANS: A
Solution:
Since Na would produce the most H2, H2O is the limiting reactant, thus 4.5 g H2 is produced.
15. ANS: D
Solution:
16. ANS: A
Solution:
Accelerated chemistry with Ms. Lara
Final revision
SHORT ANSWER
17. ANS:
The equivalence point is detected by noting a shape change in the titration graph.
18. ANS:
Approximately 23 mL of titration standard is added to reach the equivalence point.
The pH is about 5.0 at this point.
19. ANS:
The graph is an example of a weak base titrated with a strong acid.
Revision III
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
1. If colliding molecules have an orientation that favors reaction, they have
a. the correct angles and distances between atoms.
b. sufficient energy for each molecule.
c. speeds that are neither too fast nor too slow.
d. entropy values in the proper range.
____
2. Raising the temperature of gas particles
a. increases both collision energy and favorability of orientation.
b. increases neither collision energy nor favorability of orientation.
c. increases collision energy but does not increase favorability of orientation.
d. increases favorability of orientation but does not increase collision energy.
____
3. If a collision between molecules is very gentle, the molecules are
a. more likely to be favorably oriented. c. more likely to react.
b. less likely to be favorably oriented.
d. more likely to rebound without
reacting.
____
4. The minimum energy required for an effective collision is called
a. energy of enthalpy.
c. free energy.
b. activation energy.
d. kinetic energy.
Accelerated chemistry with Ms. Lara
Final revision
____
5. Activation energy is
a. the energy required to form the activated complex.
b. the net energy required to turn reactants into products.
c. the enthalpy of reaction.
d. free energy.
____
6. The decrease in reactant concentration per unit time in a reaction is a measure of the
a. reaction rate.
c. overall reaction.
b. heterogeneous reaction.
d. reaction mechanism.
____
7. Which of the following burns most slowly?
a. a large lump of coal
c. powdered coal
b. small pieces of coal
d. All of these burn at the same rate.
____
8. If the surface area of reactants is larger,
a. the reaction rate is generally higher.
b. the reaction rate is generally lower.
____
c. the reaction rate is not affected.
d. the rate-determining step is eliminated.
9. Catalysts generally affect chemical reactions by
a. increasing the temperature of the system.
b. increasing the surface area of the reactants.
c. providing an alternate pathway with a lower activation energy.
d. providing an alternate pathway with a higher activation energy.
Accelerated chemistry with Ms. Lara
Revision III answers
MULTIPLE CHOICE
1. ANS: A
2. ANS: C
3. ANS: D
4. ANS: B
5. ANS: A
6. ANS: A
7. ANS: A
8. ANS: A
9. ANS: C
Final revision