*KEY*
*KEY*
Mr. Dolgos
Regents Chemistry
PRACTICE PACKET
Unit 9: Acids, Bases & Salts
HC2H3O2(aq)
+
H2O(l)
↔
1
C2H3O2-(aq)
+
H3O+(aq)
Acid/Base/Salt Characteristics:
On the line on the left, write A if the statement is a property of an acidic
solution. Write B if it is a property of a basic solution. Write X if it is a
property of both acidic and basic solutions.
BASE
1) Often feels smooth and slippery
ACID
2) Has a sour taste
ACID/BASE 3) Stings in open wounds
ACID
4) Typically reacts vigorously with metals
BASE
5) Has a bitter taste
ACID
6) Turns litmus paper from blue to red
ACID/BASE 7) Is an electrolyte
ACID/BASE 8) Often looks like pure water
11.
BASE
9) Turns litmus paper from red to blue
BASE
10) Typically does not react with metals
Compare acids and bases in terms of H+ and OH- ion concentrations.
Acids have an excess of H+ in solution (more H+ than OH- ions in
solution), bases have an excess of OH- ions in solution (more OH- than
H+ ions in solution)
12.
Explain what it means to be an electrolyte and why acids, bases and
salts are electrolytes.
Electrolytes are substances that conduct electricity when dissolved in
water. Acids, bases, and salts have mobile ions (or mobile charges) when
dissolved in water which allows them to conduct electricity.
2
3
4
5
6
Multiple Choice Questions:
1) Basic solutions are those that contain an excess of
a) H2 molecules
b) H2O molecules
c) H+ ions
d) OH- ions
2) Acidic solutions are those that contain an excess of
a) H2 molecules
b) H2O molecules
c) H+ ions
d) OH- ions
3) A student accidentally spills an unknown chemical on her hand. She quickly washes it
off, and notices that her skin feels slippery. She has an electrical conductivity tester
at her lab station and tests the conductivity of the solution. It is a good conductor of
electricity. The then places a strip of litmus paper in a sample of the liquid and it
turns blue. She can conclude that the liquid is a
a) strong base
b) weak base
c) strong acid
d) weak acid
4) As 1 gram of sodium hydroxide dissolves in 100 grams of water, the conductivity of
the water will
a) remain the same
b) decrease
c) increase
Recognizing/Naming Acids, Bases, & Salts:
Question: What is the general formula for each of the following?
ACID 
HA or HX
BASE 
XOH
Question: What combinations of elements or ions qualify as a salt?
SALT 
Substance
1. NaOH
metal & nonmetal
metal & polyatomic ion
polyatomic ion & nonmetal
2 polyatomic ions
Acid, Base, or Salt?
BASE
Name
Sodium hydroxide
2. NH3
BASE
Ammonia
3. HCl
ACID
Hydrochloric acid (hydrogen chloride)
4. NaCl
SALT
Sodium chloride
7
5. HF
ACID
Hydrofluoric acid (hydrogen fluoride)
6. K2SO4
SALT
Potassium sulfate
7. AlPO4
SALT
Aluminum phosphate
8. Fe(OH)3
BASE
Iron (III) hydroxide
9. H2SO4
ACID
Sulfuric acid (dihydrogen sulfate)
10. H2CO3
ACID
Carbonic acid (dihydrogen carbonate)
11. LiC2H3O2
SALT
Lithium acetate
12. H3PO4
ACID
Phosphoric acid (trihydrogen phosphate)
13. Ca(NO3)2
SALT
Calcium nitrate
14. KOH
BASE
Potassium hydroxide
15. MgCO3
SALT
Magnesium carbonate
16. NH4Br
SALT/ACID
Ammonium bromide
17. HNO3
ACID
Nitric acid (hydrogen nitrate)
18. Ca(OH)2
BASE
Calcium hydroxide
19. MgCO3
SALT
Magnesium carbonate
20. NaNO3
SALT
Sodium nitrate
21. HCl
ACID
Hydrochloric acid (hydrogen chloride)
22. KCl
SALT
Potassium chloride
23. Ba(OH)2
BASE
Barium hydroxide
24. KOH
BASE
Potassium hydroxide
8
25. H2S
ACID
26. Al(NO2)3
SALT
Hydrosulfuric acid (hydrogen sulfide,
dihydrogen monosulfide)
Aluminum nitrite
27. CaCl2
SALT
Calcium chloride
28. Na2SO4
SALT
Sodium sulfate
29. Mg(OH)2
BASE
Magnesium hydroxide
30. NH4OH
BASE
Ammonium hydroxide
SALT/ACID
Ammonium chloride
32. HBr
ACID
Hydrobromic acid (hydrogen bromide)
33. FeBr3
SALT
Iron (III) bromide
34. HC2H3O2
ACID
Acetic acid (hydrogen acetate)
35. CuCl2
SALT
Copper (II) chloride
36. HNO2
ACID
Nitrous acid (hydrogen nitrite)
37. HClO
ACID
Hypochlorous acid (hydrogen hypochlorite)
38. HClO2
ACID
Chlorous acid (hydrogen chlorite)
39. HClO3
ACID
Chloric acid (hydrogen chlorate)
40. HClO4
ACID
Perchloric acid (hydrogen perchlorate)
41. H2SO3
ACID
Sulfurous acid (dihydrogen sulfite)
42. Al(OH)3
BASE
Aluminum hydroxide
43. LiOH
BASE
Lithium hydroxide
44. HI
ACID
Hydroiodic acid (hydrogen iodide)
31. NH4Cl
9
45. H2Se
ACID
Hydroselenic acid (dihydrogen selenide)
46. H2CrO4
ACID
Chromic acid
47. AgOH
BASE
Silver hydroxide
48. Fe(OH)2
BASE
Iron (II) hydroxide
Bronsted-Lowry Problems:
According to the Bronsted-Lowry theory, an acid is a proton (H+) donor and a base is a proton
(H+) acceptor.
Example:
HCl
+
OH-
Cl-

+
H2O
In the following equations, draw brackets between conjugate acid-base pairs and label each
species as a Bronsted-Lowry acid or base, and answer the question.
1) According to the Bronsted-Lowry theory, what does H3O+ act as in the following
reaction?
ACID
CH3COO- + H3O+  CH3COOH + H2O
2) According to the Bronsted-Lowry theory, what does H2O act as in the following
reaction?
BASE
HCl + H2O  H3O+ + Cl-
3) According to the Bronsted-Lowry theory, what does NH3 act as in the following
reaction?
ACID
NH2-
+
H2O

NH3
+
OH-
4) According to the Bronsted-Lowry theory, what does H3O+ act as in the following
reaction?
ACID
H3O+ + OH-  H2O + H2O
10
5) According to the Bronsted-Lowry theory, what does CN- act as in the following
reaction?
BASE
CN- + H2O  HCN + OH6) According to the Bronsted-Lowry theory, what does CH3COOH act as in the following
reaction?
BASE
HClO4 + CH3COOH
 ClO4- + CH3COOH2+
7) According to the Bronsted-Lowry theory, what does HCN act as in the following
reaction?
ACID
HCN + H2O  H3O+ + CN-
8) According to the Bronsted-Lowry theory, what does NH4+ act as in the following
reaction?
ACID
NH4+ + HSO4-  NH3 + H2SO4
9) According to the Bronsted-Lowry theory, what does Al(H2O)5(OH)+2 act as in the
following reaction?
BASE
HCl + Al(H2O)5(OH)+2  Cl- + Al(H2O)6+3
Challenge Problems:
A
10) HCl
CB
+
NaOH
NaCl

+
H2O
B
11) KOH
A
HNO3
+
B
12) H2CO3
A
CA

B
+
2H2O
CB
KNO3
+
CA

H3O+ +
H2O
CA
CO2
CB
11
A
CB
13) HCl
+
NH3
NH4+

B
A
14) H2O
+
+
Cl-
CA
NH3
CB
NH4+

B
+
OH-
CA
A
CB
15) H2O
+
H2O
H3O+

B
A
16) NH3
+
OH-
CA
NH3
CB
NH4+

B
+
NH2-
CA
A
CB
17) H2SO4
+
Ca(OH)2
CaSO4

+
2H2O
B
CA
A
CB
18) O3ClOH
+
H2O
H3O+

B
+
HI
O3ClO-
CA
A
19) H2O
+
CB
H3O+

B
+
I-
CA
A
CB
20) CH3COOH
+
H2O

CH3COO -
+
B
CA
A
21)
CB
NH4+
+
OH
-
NH3

+
H2O
B
CA
A
22) H2SO4
CB
+

B
A
23) HSO4-
OH-
+
H2O
B
H3O+
HSO4-
+
CA
CB

SO4-2
H2O
+
H3O+
CA
12
13
14
15
16
17
More Bronsted-Lowry Acids and Bases:
Directions: For questions 1-4 please circle the correct answer.
1. What are the two acids in the following reaction?
A
H2O
+
HI
H3O+
↔
B
CA
a. H2O and HI
c. H2O and I-
CB
I-
+
b. HI and Id. HI and H3O+
2. What are the two acids in the following reaction?
A
CB
CH3COOH
+
H2O
↔
CH3COO-
B
H3O+
+
CA
a. CH3COOH and H3O+
c. CH3COO- and H2O
b. CH3COOH and CH3COOd. CH3COO- and H3O+
3. What are the bases in the following reaction?
A
CB
H3PO4
+
H2O
↔
H2PO4-
+
B
CA
b. H2O and H2PO4d. H2PO4- and H3O+
a. H3PO4 and H2O
c. H3PO4 and H2PO4-
4. What are the bases in the following reaction?
A
H2O
+
H2SO4
H3O+
H3O+
↔
B
+
CA
a. H2O and H2SO4
c. H2O and H3O+
CB
HSO4-
b. H2O and HSO4d. H3O+ and HSO4-
Directions: For questions 5-13 please circle the acids and underline the bases in
the following reactions.
5. CH3COO-
+
6. H3O+
OH-
↔
H2O
↔
7. HCl
+
+
H3O+
↔
H2O
H3O+
CH3COOH
+
H2O
+
Cl-
18
+
H2O
8. NH2-
+
H2O
9. NH4+ +
10. HCN
HSO4+
+
12. SO42-
+
13. CN-
+
CH3COOH
H2O
HNO3
↔
+
H3O+
↔
H2SO4
+
CN-
ClO4-
↔
HSO4- +
↔
HCN
OH-
+
NH3
↔
H2O
11. HClO4
NH3
↔
+
+
CH3COOH2+
NO3-
OH-
14. What is an amphoteric substance?
A substance that can act as either a base or an acid.
19
_
The Power of pH:
For each question, the two pH values are being compared. How many times
more acidic or basic does the pH of the solution become?
1) pH 5  pH 3 102 or 100 x more acidic
2) pH 8  pH 4 104 or 10,000 x more acidic
3) pH 10  pH 7 103 or 1,000 x more acidic
4) pH 14  pH 7 107 or 10,000,000 x more acidic
5) pH 4  pH 3 101 or 10 x more acidic
6) pH 7  pH 3 104 or 10,000 x more acidic
7) pH 5  pH 1 104 or 10,000 x more acidic
8) pH 9  pH 3 106 or 1,000,000 x more acidic
9) pH 8  pH 6 102 or 100 x more acidic
10) pH 3  pH 6 103 or 1,000 x more basic
11) pH 1  pH 3 102 or 100 x more basic
12) pH 2  pH 7 105 or 100,000 x more basic
Circle the answer the best completes the following sentences:
13) The pH scale was developed to express ([H+]/[OH-]) as a number between 0
and 14.
14) A pH of 1 is a (strong/weak) (acid/base).
15) A pH of 8 is a (strong/weak) (acid/base).
16) In an acid, the [H+] </> [OH-].
17) In a base, the [H+] </> [OH-].
18) A decrease from 5 to 4 on the pH scale represents a tenfold
(increase/decrease) in the concentration of ([H+] / [OH-]).
19) Strong acids and bases will dissociate (completely/slightly).
20
21
22
23
The pH Scale:
A liquid may be an acid, base, or neutral. The degree of acidity or basicity
can be measured by using the pH scale. The initials pH stand for the “power
of Hydrogen” or for “Potential of Hydrogen.” The scale is divided into three
areas: Acid (readings below 7), neutral (reading of 7), and basic (readings
above 7). The strength of an acid or base depends on its ability to
dissociate to form ions. When an acid or base completely ionizes or breaks
down then we have a strong acid or base. For example, when 100 molecules
of HCl dissolve in water, all 100 molecules dissociate to form H+ ions and Clions:
HCl +
H20
↔
H+ (aq)
+
Cl- (aq)
A weak acid or base however only ionize or break down slightly. The fact
that HCl dissociates so easily makes it a strong acid, and a good electrolyte.
A weak acid on the other hand may only dissociate to form 1 H+ ion out of
100.
Each pH unit represents a tenfold difference of the H+ and OHconcentration. It is this mathematical feature that makes the pH scale so
compact. For example a solution of pH 2 is not twice as acidic as a solution of
pH 4, but a hundred times more acidic. The pH of 5 is ten times more acidic
than a pH of 6. So when the pH of a solution changes slightly, it actually
changes the concentrations of H+ and OH- substantially.
Measuring pH:
To measure the pH of a solution we use pH indicators. A pH indicator is a
paper strip or liquid solution that contains special chemicals or dyes that will
change colors at different pH’s. An indicator is actually something called a
Bronsted-Lowry conjugate acid-base pair in which the acid is a different
color then the base. Common pH indicators can be found in Table M of your
reference table.
Let’s take a look at table M. You will notice that it lists common acid-base
indicators. For each indicator the name, an approximate pH range for color
change and the color change is noted. Looking at bromthymol blue you will
see that the color will change from yellow to blue at 6.0-7.6. Therefore,
acids will maintain a yellow color, while bases will be blue. The diagram on
the following page indicates the color change you will observe when using
bromthymol blue at various pH’s.
24
0
6.0 7.6
14
Approximate pH range for color change: 6.0-7.6
Color of acid form: yellow
Color of base form: blue
1. Given the pH scale below shade acids red, bases blue, and any neutral
values green.
1
2
3
4
5
6
7
8
9
10
11
12
13
14
2. Will an acidic solution have more [H+] or [OH-] in solution?
More [H+]
3. Will a basic solution have more [H+] or [OH-] in solution?
More [OH-]
4. Will a neutral solution have more [H+] or [OH-] in solution?
[H+] = [OH-]
5. A pH change from 5 to 6 will result in a change in [H+] by how much?
101 or 10 x less [H+]
6. A pH change from 9 to 7 will result in a change in [H+] by how much?
102 or 100 x more [H+]
7. What is a pH indicator?
A substance that permanently changes color within a given pH range
25
pH & Indicators:
Given the pH of the following common substances determine what color the indicator will
turn when placed in each substance.
Substance
pH
Stomach
Acid
Cola Drink
2
Blood
3
Methyl Bromthymol Phenolphthalein Litmus Bromcresol
Orange
Blue
green
Red
Yellow
Colorless
Red
Yellow
Thymol
blue
Yellow
Red
Yellow
Colorless
Red
Yellow
Yellow
7.5
Yellow
Green
Colorless
Purple
Blue
Yellow
Pure
Water
Oven
Cleaner
Tomatoes
7.0
Yellow
Green
Colorless
Purple
Blue
Yellow
14
Yellow
Blue
Pink
Blue
Blue
Blue
4
Orange
Yellow
Colorless
Red
Green
Yellow
Milk
6.5
Yellow
Green
Colorless
Purple
Blue
Yellow
Detergent 10
Yellow
Blue
Pink
Blue
Blue
Blue
Coffee
5
Yellow
Yellow
Colorless
Purple
Green
Yellow
Household 11
Cleaners
Yellow
Blue
Pink
Blue
Blue
Blue
For the following choose an appropriate indicator to note a transformation.
20)
endpoint pH = 9 thymol blue, phth, *litmus
21)
endpoint pH = 5 bromcresol green, *litmus, *methyl orange
22)
endpoint pH = 3 methyl orange, bromcresol green
26
pH:
pH is a scale that measures the hydronium ion (H+) concentration of a solution. A pH of less
than 7 indicates an acidic solution. A solution with a pH of 7 is neutral. A solution with a pH
of 7 to 14 is basic and contains a higher concentration of hydroxide ions than hydronium ions.
Indicators are substances that change color in the presence of certain ions. Phenolphthalein
is colorless in an acid and a neutral solution, but pink in a base. Litmus is red in an acid and
blue in a base. This is outlined on Table M of the Reference Tables.
Solution
PH range Methyl Thymol
Orange Blue
Litmus
Vinegar
1.3
Red
Yellow
Red
BromCresol
Green
Yellow
Soap
8.4
Yellow
Green
Blue
Blue
Cola
3.2
Orange Yellow
Red
Yellow
Light
Pink
Colorless
Ammonia
12
Yellow
Blue
Blue
Blue
Pink
Blue
Base
Rain
6.4
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
Milk of
Magnesia
8.1
Yellow
Green
Purple
Blue
Colorless
Blue
Base
Milk
6.6
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
Saliva
6.5
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
Coffee
5.2
Yellow
Yellow
Red
Green
Colorless
Yellow
Acid
Gastric juices
1.5
Red
Yellow
Red
Yellow
Colorless
Yellow
Acid
Human blood
7.4
Yellow
Yellow
Purple
Blue
Colorless
Green
Base
OJ
2.1
Red
Yellow
Red
Yellow
Colorless
Yellow
Acid
Kool-Aid
6.4
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
Drain cleaner
1.8
Red
Yellow
Red
Yellow
Colorless
Yellow
Acid
Bleach
6.2
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
Shampoo
6.3
Yellow
Yellow
Purple
Blue
Colorless
Green
Acid
27
PhenolPhthalein
Colorless
Bromthymol
blue
Yellow
Acid or
Base?
Blue
Base
Yellow
Acid
Acid
Neutralization Reactions:
Remember that:
Acid + Base  Salt + Water
Using the above general reaction, complete the following reactions with correct
formulas. Then balance the entire double replacement reaction. Also name the
salt that is produced in the space provided below the product side of the reaction.
1)
____ HNO3(aq) + ____ KOH(aq)
 ____ HOH
+
____ KNO3
2)
__2_ HCl(aq) + ____ Ca(OH)2(aq)  ____ HOH
+
____ CaCl2
3)
____ H2SO4(aq) +
__2_ NaOH(aq)
4)
____ H3PO4(aq) +
__3_ NaOH(aq)  __3_ HOH
5)
____ NH4OH(aq) +
6)
____ HClO(aq)
7)
____ Mg(OH)2 +
8)
__3_ HNO3
+
____ Al(OH)3  __3_ HOH
9)
____ H3PO4
+
__3_ LiOH  __3_ HOH
+
10) ____ H2SO4
+
11) ____ NH4OH
+
 __2_ HOH
____ HI(aq)  ____ HOH
+
+
+
____ NaClO
__2_ CH3COOH  __2_ HOH +
+
____ Mg(OH)2  __2_ HOH
____ HCl  ____ HOH
28
+
____ Na3PO4
____ NH4I
____ NaOH(aq)  ____ HOH +
+
____ Na2SO4
____ Mg(CH3COO)2
____ Al(NO3)3
____ Li3PO4
+
____ MgSO4
____ NH4Cl
Writing Balanced Reactions:
Directions: In the following reactions an acid is reacting with a base in neutralization
reactions. Write out the reaction and balance the equation.
1. Hydrochloric acid reacts with potassium
hydroxide
2. A sample of hydrochloric acid neutralizes
calcium hydroxide
HCl + KOH → H2O + KCl
3. Ammonia reacts with perchloric acid
NH3+ HClO4 → NH4+ + ClO4-
5. Hydrobromic acid neutralizes a sample of
sodium hydroxide
2HCl + Ca(OH)2 → 2H2O + CaCl2
4. Aluminum hydroxide is mixed with
sulfuric acid
Al(OH)3 + 3H2SO4 → 6H2O + Al2(SO4)3
6. A solution of HCl reacts with a solution
of Ba(OH)2
HBr + NaOH → H2O + NaBr
7. KCN neutralizes HClO
2HCl + Ba(OH)2 → 2H2O + BaCl2
8. HBr neutralizes calcium hydroxide
KCN + HClO → HCN + KClO
2HBr + Ca(OH)2 → 2H2O + CaBr2
9. HCN reacts with NaOH
HCN + NaOH → H2O + NaCN
CHALLENGE:
A volume of 10 mL of 0.75 M sodium hydroxide neutralizes a 30 mL sample of
hypochlorous acid. Write a balanced equation for the reaction and calculate the
concentration of the acid.
29
ACID-BASE TITRATIONS:
To determine the concentration of an acid (or base), we can react it with a base (or acid)
of known concentration until it is completely neutralized. This point of exact
neutralization, know as the endpoint or equivalence point, is noted by the change in color
of the indicator.
We use the following Titration formula from our Table T (Reference Tables):
MAVA = MBVB
Solve the following problems. SHOW ALL WORK!
1. A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 M NaOH.
What is the molarity of the HCl?
1.2 M HCl
2. A 10.0 mL sample of H2SO4 was exactly neutralized by 13.5 mL of 1.0 M KOH. What is
the molarity of the H2SO4?
0.675 M H2SO4
3. How much 1.5 M NaOH is necessary to exactly neutralize 20.0 mL of 2.5 M H3PO4?
.100 L or 100. mL NaOH
4. How much of 0.5 M HNO3 is necessary to titrate 25.0 mL of 0.05 M Ca(OH)2 solution
to the endpoint?
5.00 x 10-3 L or 5.00 mL of HNO3
5. What is the molarity of a NaOH solution if 15.0 mL is exactly neutralized by 7.5 mL of
a 0.02 M HC2H3O2 solution?
.01 M NaOH
30
Titration Practice:
A titration was set up and used to determine the unknown molar concentration
of a solution of NaOH. A 1.2 M HCl solution was used as the titration standard.
The following data were collected.
Trial 1
Volume of
1.2 M HCl
Initial Reading
of NaOH
Final Reading of
NaOH
Volume of
NaOH used
(mL)
Molarity of
NaOH (M)
Trial 2
Trial 3
Trial 4
10.0 mL
10.0 mL
10.0 mL
10.0 mL
0.0 mL
12.2 mL
23.2 mL
35.2 mL
12.2 mL
23.2 mL
35.2 mL
47.7 mL
12.2 mL
11.0 mL
12.0 mL
12.5 mL
.984 M
1.09 M
1.00 M
.960 M
1) Calculate the volume of NaOH used to neutralize the acid for each trial. Record in
data table above. Show one sample calculation below.
2) Using the MAVA = MBVB formula calculate the molarity of the base for each trial.
Record in data table above. Show one sample calculation below.
3) Calculate the average molarity of the NaOH using your results from question 2.
Your answer must include the correct number of significant figures and the
correct units.
1.01 M NaOH
31
4) According to Reference Table M, what indicator would be most appropriate in
determining the end point of this titration? Explain the reasoning behind your
choice.
Bromothymol Blue – end point has pH of 7.0, which falls in the range for
b.blue (6.0-7.6)
5) Explain why it is better to use the average data from multiple trials rather than
the data from a single trial to calculate the results of the titration.
Any “bad data” will have less impact on the overall precision with a
greater # of trials; greater # of trials helps to identify and overcome
aberrations or experimental error.
6) If 3.00 liters of 2M HCl neutralizes 1.00 liter of NaOH, what is the molarity of
the NaOH? 6 mol/L
7) If 40mL of 2.50M HCl neutralizes 500mL of KOH, what is the molarity of the
KOH? 0.2 mol/L
8) If 2.00 liters of 4.00M KOH neutralizes a HNO3 solution whose concentration is
8.00M, how many liters of HNO3 were neutralized? 1.00 L
9) How many mL of 1.00M HCl are needed to neutralize 400mL of 0.200M NaOH?
80 mL
32
10) How many milliliters of 4.00 M NaOH are required to exactly neutralize 50.0
milliliters of a 2.00 M solution of HNO3? 25 mL
11) ** If 21.0mL of 0.100M H2SO4 neutralizes 42.0mL of NaOH, what is the molarity of
the NaOH? 0.10 mol/L
12) ** How many mL of 0.500M HNO3 are needed to neutralize 250mL of 2.50M
Ca(OH)2? 2,500 mL
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Titration Calculation Chart:
MA
VA
MB
VB
1
1.00M
25mL
4.00M
6.25 mL
2
2.00M
25mL
1 M
50mL
3
3.00M
50mL
1.5 M
100mL
4
6 M
1L
3.00M
2L
5
1.50M
1,000 mL
3.00M
500mL
6
6.00M
25 mL
2.00M
75mL
7
3 M
200mL
4.00M
150mL
8
5.00M
100mL
2.50M
200 mL
9
3.5M
400 mL
7.00M
200mL
10
2.50M
250mL
5.00M
125 mL
*Assume all acids and bases are MONOPROTIC
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More Titration Calculations:
1) How many milliliters of 0.2M KOH are
needed to neutralize 20mL of 0.1M
HCl?
VB = 10 mL
6) What is the molarity of a 250mL HCl
solution that contains 0.25 moles of HCl?
MB = 1.0 mol/L
2) How many moles of HCl are in 20mL of a
0.1M solution? 2 x 10-3 moles
7) Equal volumes of 0.5M HCl and 0.5M NaOH
are mixed. The total volume of the mixture
is 2L. What is the pH of the solution?
pH = 7
3) If 6mL of 1M HCl is exactly neutralized
by 3mL of KOH, what is the molarity of
the KOH? MB = 2 mol/L
8) How many moles of HCl can be neutralized
by 0.1 liters of a 0.5M NaOH?
5 x 10-2 moles
4) A 30 mL sample of HCl is completely
neutralized by 10mL of a 1.5M NaOH
solution. What is the molarity of the
HCl solution? MA = 0.5 mol/L
9) How many milliliters of 5M NaOH are
needed to neutralize 40mL of 2M H2SO4?
VB = 32 mL
5) What is the total number of moles of
hydrogen ion that will be neutralized by
2.0 moles of hydroxide ion?
10) How many liters of 0.2M HCl are needed to
neutralize 20 liters of 0.1M Ca(OH)2?
VA = 20 L
2.0 moles
35
Neutralization Reactions & Titrations:
1) When 34.2 mL of a 1.02 M sodium hydroxide solution is added from a
burette to 25.00 mL of a phosphoric acid solution that contains
phenolphthalein, the solution changes from colorless to red.
A.)
Write the balanced equation for the titration reaction.
3NaOH + H3PO4 → 3H2O + Na3PO4
B.)
Calculate the molarity of the phosphoric acid.
.465 mol/L
2) 34.57 mL of an acetic acid solution are needed to neutralize 25.19 mL of
0.1025 M sodium hydroxide.
A.)
Write the balanced equation for the titration reaction.
HC2H3O2 + NaOH → H2O + Na C2H3O2
B.)
Calculate the molarity of the acetic acid solution.
.07469 mol/L
3) 0.300M nitric acid is titrated with 24 mL of 0.250M potassium hydroxide.
A.)
Write the balanced equation for the titration reaction.
HNO3 + KOH → H2O + KNO3
B.)
Calculate the volume of the nitric acid.
36
20. mL or .020 L
4) 0.250M sodium hydroxide is used to neutralize 116 mL of 0.0625M
sulfuric acid.
A.)
Write the balanced equation for the titration reaction.
2NaOH + H2SO4 → 2H2O + Na2SO4
B.)
Calculate the volume of the sodium hydroxide.
37
58 mL or .O58 L
Show all work for the following word problems:
1) How many milliliters of 2.5 M HCl are required to exactly neutralize 1.5 L
of 5.0 M NaOH? Use Table T.
3.0 x 103 mL
2) A 2.0-mL sample of NaOH solution is exactly neutralized by 4.0 mL of 3.0
M HCl solution. What is the concentration of the NaOH solution?
6.0 M NaOH
3) A 30. mL volume of HCl is titrated with 23 mL of 0.20 M NaOH. What is
the molarity of HCl in this solution?
0.15 M HCl
4) A 26 mL volume of NH3 is titrated with 23 mL of 0.20 M HCl. What is
the molarity of NH3 in this solution?
0.18 M NH3
5) A 40. mL volume of H2SO4 is titrated with 38 mL of 0.24 M NaOH. What is the
molarity of H2SO4 in this solution? (Be careful with this one!)
0.11 M H2SO4 (diprotic acid)
38
Reactions with Acids and Bases:
1) Using Table J in your Reference Tables, list two metals that will react with H2 (or an
acid) Any metals above H2 on the table
2) Using Table J in your Reference Tables, list two metals that will NOT react with H2
(or an acid) Any metals below H2 on the table
3) What type of reaction (of the four we have learned) is involved when an acid reacts
with a metal? Single replacement
4) Write the general formula (using ABC etc.) for this type of reaction
X + HA → H2 + XA
5) Predict the products of the following reaction:
Mg + 2HNO3 
H2(g) + Mg(NO3)2
5) Will copper react with an acid? NO Explain your answer in terms of activity
Copper is less active than H2; copper doesn’t give up its e- as easily as H2
6) Predict the products of the following neutralization reaction:
RbOH + HBr  RbBr + H2O
7) Set up a reaction below that would occur between HNO3 and LiOH. Predict the
products using your general reaction for neutralization reactions.
HNO3 + LiOH → H2O + LiNO3
8) Predict the products of the following reaction. Remember to create your formulas
using the criss cross rule! BALANCE the reaction also.
H2SO4
+
Ca(OH)2

2H2O + CaSO4
Name salt that was produced Calcium Sulfate
9) According to your reference tables, which metal would react spontaneously with
hydrochloric acid?
a. Gold
b. Silver
c. Copper
39
d. Zinc
WORKSHEET ON THE REACTIVITY SERIES
1) Use table J and your knowledge of chemistry to answer the following questions in
complete sentences.
a) Why does gold occur native (uncombined) whereas zinc does not?
Gold is a much less active metal than zinc.
b) Why was silver used to make coins in the past?
Silver is a rare metal (very valuable) and an unreactive metal (very safe).
c) Why is copper used to make electrical cables and wires?
Copper is an excellent electrical conductor.
d) Why do we know so little about the lifestyles of the people of the Iron Age?
Iron is a fairly active/reactive metal and corrodes/rusts easily.
2) Rank the following metals in order of reactivity (most reactive = 1, least reactive = 4)
3 zinc 1 sodium 2 magnesium 4 copper
a) Which metals will react when added to dilute hydrochloric acid? Describe the
reaction.
Sodium, magnesium, and zinc will react with HCl by forcing their electrons onto
hydrogen and forming H2 gas.
b) Which of the four metals would be suitable for making saucepans? Explain why the
others are not.
Copper because it is not an active metal. The other metals would react with
water or anything acidic in the food being cooked.
c) Which of the four metals forms a protective coating when it oxidizes?
Zinc
3) Describe what you would see if you dropped a piece of magnesium ribbon into some
copper sulphate solution in a test tube. Write a word equation for the reaction.
You would see fizzing and bubbling, the color would fade from (blue to clear), and
solid copper would precipitate out of solution while the magnesium ribbon dissolved.
Solid magnesium metal loses electrons to copper ions.
40
4) Complete the following word equations.
a) zinc + lead nitrate solution → lead + zinc nitrate solution
b) iron + zinc sulphate solution → no rxn
c) lead + copper nitrate solution → copper + lead nitrate solution
d) magnesium + zinc chloride solution → zinc + magnesium chloride solution
e) copper + sodium chloride solution → no rxn
f) zinc + iron sulphate solution → iron + zinc sulphate solution
g) gold + silver nitrate solution → no rxn
h) magnesium + calcium nitrate solution → no rxn
5) Three metals X, Y and Z have the following reactions:Y will displace X from a solution of its salt.
Z will displace both X and Y from solutions of their salts.
Place the three metals in order of reactivity, starting with the least reactive.
X, Y, Z
6) Here is a list of metals in order of decreasing reactivity. Q and R are mystery metals.
K > Q > Ca > Mg > Al > Zn > R > Fe > Cu
a) Will Q react with cold water?
Yes
b) Will R react with cold water?
No
c) Will R react with dilute hydrochloric acid?
Yes
d) Will R displace copper from copper sulphate solution?
Yes
e) Write word equations for any reactions in parts a) to d)
a) Q + water → QOH(aq) + H2(g)
or
Q + water → Q(OH)2(aq) + H2(g)
c) R + HCl → RCl(aq) + H2(g)
d) R + CuSO4(aq) → Cu(s) + R2SO4
or
41
R + CuSO4(aq) → Cu(s) + RSO4
a) Yes: iron + copper (II) sulphate solution → copper + iron (II) sulphate solution
or
iron + copper (II) sulphate solution → copper + iron (III) sulphate solution
b) No rxn
c) Yes: copper + silver nitrate solution → silver + copper nitrate solution
d) Yes: zinc + lead nitrate solution → lead + zinc nitrate solution
42
a) Yes: iron + copper (II) oxide → copper + iron (II) oxide
or
iron + copper (II) oxide → copper + iron (III) oxide
b) Yes: aluminum + iron oxide → iron + aluminum oxide
c) No rxn
d) Yes: magnesium + zinc oxide → zinc + magnesium oxide
43