Download Unit 10 PRACTICE Test with Answers

Name …………………………………………………….
Period …….
1. Which substance is an Arrhenius base?
(1) CH3OH
(2) CH3Cl
(3) LiOH
(4) LiCl
Acids, Bases, & Salts PRACTICE Test
8. Which pH change represents a hundredfold
increase in the concentration of H3O+?
(1) pH 5 to pH 7
(2) pH 3 to pH 1
(3) pH 13 to pH 14
(4) pH 4 to pH 3
2. One acid-base theory states that an acid is
(1) an electron donor
(2) an H+ donor
(3)
(4)
a neutron donor
an OH– donor
3. The compound HNO3 can be described as an
(1)
(2)
(3)
(4)
Arrhenius acid and an electrolyte
Arrhenius acid and a nonelectrolyte
Arrhenius base and an electrolyte
Arrhenius base and a nonelectrolyte
4. What is the color of the indicator methyl orange in a
solution that has a pH of 2?
(1) blue
(2) orange
(3) yellow
(4) red
5. In which solution will bromthymol blue indicator
appear blue?
(1) 0.1 M CH3COOH (3) 0.1 M KOH
(2) 0.1 M HCl
(4) 0.1 M H2SO4
6. A hydrogen ion, H+, in an aqueous solution may
also be written as
(3) H3O+
(4) OH–
(1) H2O
(2) H2O2
9. Which compound releases hydroxide ions in an
aqueous solution?
(1) CH3COOH
(2) CH3OH
(3) HCl
(4) KOH
10. What are the products of a reaction between
KOH (aq) and HCl (aq)?
(1) H2 and KClO
(2) H2O and KCl
(3) KH and HClO
(4) KOH and HCl
11. The pH of a solution changes from 4 to 3 when
the hydrogen ion concentration in the solution is
(1)
(2)
(3)
(4)
decreased by a factor of 100
increased by a factor of 100
decreased by a factor of 10
increased by a factor of 10
12. In which laboratory process could a student use
0.10 M NaOH (aq) to determine the concentration
of an aqueous solution of HBr?
(1) chromatography
(2) pH testing
(3) filtration
(4) titration
13. Which statement correctly describes a solution
with a pH of 9?
7. Given the reaction:
NH3 +
HCl
→ NH4
+
+ Cl
–
In this reaction, ammonia molecules (NH3) act
as a base because they
(1)
(2)
(3)
(4)
accept hydrogen ions (H+)
accept hydroxide ion (OH–)
donate hydrogen ions (H+)
donate hydroxide ions (OH–)
(1) It has a higher concentration of H3O+ than
OH– and causes litmus to turn blue.
(2) It has a higher concentration of OH– than
H3O+ and causes litmus to turn blue.
(3) It has a higher concentration of H3O+ than
OH– and causes methyl orange to turn red.
(4) It has a higher concentration of OH– than
H3O+ and causes methyl orange to turn red.
14. Identify two indicators from Reference Table M that are yellow in solutions with a pH of 5.5.
any two of the following:
methyl orange, bromthymol blue, thymol blue
15. Complete the equation representing a neutralization reaction by writing the formulas of the products.
Balance the equation to show conservation of mass.
___ Al(OH)3 + _3_ HNO3 →
_3_ H2O + ___ Al(NO3)3
16. A student was studying the pH differences in samples from two Adirondack streams. The student measured a pH of
4.5 in stream A and a pH of 3.9 in stream B.
(a) Compare the hydronium ion concentration in stream A to the hydronium ion concentration in stream B.
The hydronium ion concentration is less in stream A than in stream B.
(b) Identify one compound that could be used to neutralize the sample from stream A. a base, NaOH, KOH, etc.
(c) Identify an indicator the student can use to differentiate between the samples from stream A and stream B.
Methyl orange
17. Samples of acid rain are brought to a laboratory for analysis. Several titrations are performed and it is determined that
a 20.0-milliliter sample of acid rain is neutralized with 6.50 milliliters of 0.010 M NaOH. What is the molarity of the
H+ ions in the acid rain? Your response must include both a correct numerical setup and the final answer.
MAVA = MBVB …………..MA(20.0) = (0.010)(6.50) ………………MA = 0.00325 M
18. A truck carrying concentrated nitric acid overturns and spills its contents. The acid drains into a nearby pond. The
pH of the pond water was 8.0 before the spill. After the spill, the pond water is 1,000 times more acidic.
(a) What is the chemical formula for nitric acid? __________HNO3 (on Table K!)
(b) What is the new pH of the pond water after the spill? _______ (1000 = 103; the pH decreases by 3)
Ans: pH = 5.0
19. Indigestion may be caused by excess stomach acid (HCl). Some products used to treat indigestion contain Mg(OH)2.
The Mg(OH)2 neutralizes some of the stomach acid. The amount of acid that can be neutralized by three different
brands of antacids is shown in the data table below.
(a) What is the chemical name for the base Mg(OH)2?
magnesium hydroxide
(b) If a sample of antacid X has a molarity of 0.50 M, what
is the volume required to neutralize 10. mL of 1.0 M
HCl? Your response must include both a correct
numerical setup and the final answer.
MAVA = MBVB …………..(1.0)(10.) = (0.50)VB ……………… VB = 20. mL
20. Many ancient cultural statues and buildings were made out of marble. Marble is a type of rock which contains the
metal calcium in it. Explain, using Table J, why marble statues are damaged by acid rain.
Ca metal reacts with acids to form hydrogen gas and a salt