CP Chemistry
Mrs. Klingaman
Chapters 14 & 15:
Acids and Bases
Name: ___________________________________
Mods: __________________
Conjugate Acid-Base Pairs
1.
Bronsted-Lowry Acid:
2.
Bronsted-Lowry Base:
3.
Conjugate Acid-Base Pair:
A. Label the acid (A), base (B), conjugate acid (CA) and conjugate base (CB) in each of the
following reactions:
1. H2SO4 (aq) + NH3 (aq)  HSO4- (aq) + NH4+ (aq)
2. HC2H3O2 (aq)+ H2O (l) H3O+ (aq) + C2H3O2- (aq)
3. HCO3- (aq) + HCl (aq)  Cl- (aq) + H2CO3 (aq)
B. Give the conjugate base for each of the following Bronsted-Lowry acids:
1. HI
___________________
3. H2CO3
__________________
2. NH4+
___________________
4. HNO3
__________________
C. Give the conjugate acid for each of the following Bronsted-Lowry bases:
1. CN-
___________________
2. CO32- ___________________
3. NO2-
__________________
4. HPO42-
__________________
Naming Acids Notes
Acids are compounds that can donate the hydrogen ion, H+. When the formula for an acid is written
the symbol for hydrogen generally appears at the beginning of the formula. For example, the formula for
hydrochloric acid is written as HCl and the formula for phosphoric acid is H3PO4. Notice that both formulas
begin with hydrogen (H). In both cases the caid is made up of one or more hydrogen ions and a negative
ion, known as the anion.
The name for an acid is based on the name of the anion.If the anion ends with the letters –ide, the
acid is named one way while acids containing anions that end with –ate use a different rule. Remember
that monatomic anions (such as Br - and S2-) typically end with –ide. The rules for naming acids are
summarized below.
Rules for Naming Acids:
Anion called: ___________-ide
Anion called ___________-ite
Anion called ___________-ate
Example:
sulfide, S2-
Example:
chlorite, ClO2-
Example:
chlorate, ClO3-
Acid called:
Acid called:
Acid called:
Hydro___________-ic acid
___________-ous acid
___________-ic acid
Example:
hydrosulfuric acid, H2S
Example:
chlorous acid, HClO2
Example:
chloric acid, HClO3
ite  ous
ate  ic
Examples:
#1) Write the chemical formula for sulfurous acid
 This acid contains the hydrogen ion and the sulfite anion
(this is known due to the acid name ending in –ous)
#2) Name the following acid: H2CO3

This acid contains the hydrogen ion and the carbonate anion
(to determine this, remove all the hydrogen ions to see what anion is left over as the root of
the acid)
Acid Names & Formulas Practice WS
Directions: Fill in the following table with the missing information:
Formula
Cation
Formula for Anion
Name of Anion
1
HCl
H+
Cl-
chloride
2
HNO3
H+
3
nitrate
H+
FSO42-
4
H2SO4
H+
5
H2SO3
H+
hydrofluoric acid
sulfite
6
H+
7
H+
phosphate
H+
oxalate
8
H2C2O4
Name of Acid
ClO3-
chloric acid
9
H+
hydrocyanic acid
10
H+
acetic acid
11
H+
12
H+
13
HClO
I-
sulfide
H+
14
H+
15
H+
AsO43-
arsenate
nitrous acid
Acid and Base Notes Page
pH – a measure of the hydrogen ion concentration [H+] used to express the
acidity or basicity of a compound
pH
[H+]
pOH
[OH-]
Example
0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
1.0 x 10-0
1.0 x 10-1
1.0 x 10-2
1.0 x 10-3
1.0 x 10-4
1.0 x 10-5
1.0 x 10-6
1.0 x 10-7
1.0 x 10-8
1.0 x 10-9
1.0 x 10-10
1.0 x 10-11
1.0 x 10-12
1.0 x 10-13
1.0 x 10-14
14
13
12
11
10
9
8
7
6
5
4
3
2
1
0
1.0 x 10-14
1.0 x 10-13
1.0 x 10-12
1.0 x 10-11
1.0 x 10-10
1.0 x 10-9
1.0 x 10-8
1.0 x 10-7
1.0 x 10-6
1.0 x 10-5
1.0 x 10-4
1.0 x 10-3
1.0 x 10-2
1.0 x 10-1
1.0 x 10-0
Gastric Juice
Lemon Juice
Vinegar
Tomatoes
Black Coffee
Saliva
Distilled Water
Baking Soda
Borax
Milk of Magnesia
Lime Water
Ammonia
Bleach
pH < 7: ________________
Important Equations:
pH = 7: _______________
pH = - log [H+]
pH + pOH = 14
pH > 7: _________________
pOH = - log [OH-]
Day 1 Examples:
a) Find the pH of a solution with [H+] = 1 x 10-5 M. Is this solution acidic, basic or neutral?
b) Find the pOH of a solution with a pH of 10.5. Is this solution acidic, basic or neutral?
c) Find the pH of a solution with [OH-] = 1 x 10-3 M. Is this solution acidic, basic or neutral?
Day 2 Examples:
a) Find the pH of a solution with [H+] = 6.0 x 10-4 M. Is this solution acidic, basic or neutral?
b) Find the pH of a solution with [OH-] = 6.2 x 10-6 M. Is this solution acid, basic or neutral?
c) Find the pH of 75 mL of a solution containing 0.006 grams of hydrochloric acid.
Day 1 Homework: pH, pOH, [H+] and [OH-] Calculations
1. Find the pH of a solution with [H+] = 1.0 x 10-7 M. Is this solution acidic, basic or neutral?
2. Find the pH of a solution with [H+] = 1.0 x 10-3 M. Is this solution acidic, basic or neutral?
3. Find the pOH of a solution with [OH-] = 1.0 x 10-11.5 M. Is this solution acidic, basic or neutral?
4. Find the pH of a solution with [OH-] = 1.0 x 10-4 M. Is this solution acidic, basic or neutral?
5. Find the [H+] of a solution with pH = 12.
6. Find the [OH-] of a solution with pH = 8.
7. Complete the following chart:
[H+]
1.
pH
1 x 10-5 M
2.
1 x 10-4 M
1 x 10-2 M
11
6.
12
7.
1 x 10-5 M
1 x 10-11 M
9.
10.
13
6
Acidic, Basic or
Neutral?
Acidic
7
5.
8.
pOH
1 x 10-9 M
3.
4.
[OH-]
Day 2 Homework: pH, pOH, [H+] and [OH-] Calculations
Directions: Find the pH of the following acidic solutions.
1. A 0.001 M solution of HCl (Name: ____________________________________).
2. A 0.09 M solution of hydrobromic acid (Formula: _______________).
3. A 1.34 x 10-4 M solution of HNO3 (Name: ___________________________________).
4. A 2.234 x 10-6 M solution of chloric acid (Formula: _______________).
5. A 7.98 x 10-2 M solution of HI (Name: ______________________________________).
6. 12 L of a solution containing 1 mole of chloric acid.
7. 735 L of a solution containing 0.34 moles of nitric acid.
8. 1098 L of a solution containing 8.543 moles of hydroiodic acid.
9. 660 L of a solution containing 0.0074 moles of hydrobromic acid.
10. 120 mL of a solution containing 0.005 grams of hydrochloric acid.
Neutralization and Titration
1. Give the word equation for the neutralization reaction of an acid and a base.
2. Complete these neutralization reactions:
a) HCl (aq) + LiOH (aq) 
b) HC2H3O2 (aq) + NaOH (aq) 
3. A ____________________ is a laboratory method used to determine the concentration of an
acid or a ______________ in solution by performing a ______________________ reaction
with a standard solution.
4. At the ________ _____________ of the titration, the indicator changes color; this indicates
neutralization. Once neutralized, moles of ____________ and moles of _____________ are
equal.
5. Give the formula for finding the molarity of either an acid or a base in a neutralization reaction.
6. In a titration of HCl with NaOH, 95.0 mL of the base was required to neutralize 20.0 mL of
5.0 M HCl. What is the molarity of the base? Be sure to write the neutralization reaction.
7. In a titration of HBr with LiOH, 60.0 mL of 0.020 M LiOH was needed to neutralize 15.0 mL of
HBr. What is the molarity of the acid? Be sure to write the neutralization reaction.
8. If 10.0 mL of 0.300 M KOH are required to neutralize 30.0 mL of gastric juice (HCl), what is the
molarity of the gastric juice? Be sure to write the neutralization reaction.
Homework: More Neutralization and Titration Practice Problems
Directions: Find the requested quantities in the following problems.
1. If it takes 54 mL of 0.1 M LiOH to neutralize 125 mL of HCl solution, what is the concentration
of the HCl? Be sure to write the neutralization reaction.
2. If it takes 25 mL of 0.05 M HBr to neutralize 345 mL of NaOH solution, what is the
concentration of the NaOH solution? Be sure to write the neutralization reaction.
3. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 125 mL of HNO3 solution, what
is the concentration of the HNO3 solution? Be sure to write the neutralization reaction.
4. If it takes 19.1 mL of 0.118 M HI to neutralize 25.0 mL of LiOH solution, what is the
concentration of the LiOH solution? Be sure to write the neutralization reaction.
5. Can I titrate a solution of known concentration with another solution of unknown concentration
and still get a meaningful answer? Explain.
Chapter 14 & 15 Test Review: Acids and Bases
Part I: Circle the correct choice.
1) Feel slippery.
Acids
Bases
Both
2) Conduct electricity.
Acids
Bases
Both
3) Feel like water.
Acids
Bases
Both
4) React with metals.
Acids
Bases
Both
5) Taste sour.
Acids
Bases
Both
6) Taste bitter.
Acids
Bases
Both
7) Turn litmus paper blue.
Acids
Bases
Both
+
8) Donate a hydrogen (H ) ion.
Acids
Bases
Both
9) Turn litmus paper red.
Acids
Bases
Both
10) Accept a hydrogen (H+) ion.
Acids
Bases
Both
Part II: Name the following acids.
a) H2SO4 ___________________________ b) HCl ________________________________
c) HNO2 ____________________________ d) H3PO4 ______________________________
Part III: Give the conjugate base for each of the following Bronsted-Lowry acids:
a) HBr _____________
b) H3O+ ______________
c) HSO4- _____________
Give the conjugate acid for each of the following Bronsted-Lowry bases:
a) C2H3O2- _________________
b) NH3 ________________
c) CrO42- _______________
Part III: Complete the following table.
[H+]
1 x 10-2 M
pH
[OH-]
pOH
Acid or Base
8
1 x 10-11 M
10
Neutral
5
1 x 10-1 M
6
1 x 10-10 M
Part IV: Perform the following calculations.
11) Calculate the pH of a solution with [H+] = 1.0 x 10-7 M. Is the solution acidic, basic or neutral?
12) Calculate the pH of a solution with [OH-] = 1.0 x 10-3 M. Is the solution acidic, basic or neutral?
13) Calculate the pOH of a 1.0 x 10-10.5 M solution of sodium hydroxide (NaOH).
14) Calculate the pH of a 1.0 x 10-2 M solution of hydrochloric acid (HCl).
15) Calculate the pH of a solution with [H+] = 4.3 x 10-3 M. Is this solution acidic, basic or neutral?
16) Calculate the pOH of a solution with [H+] = 5.2 x 10-13 M.
17) Calculate the pH of 845 mL of a solution containing 0.46 moles of nitric acid (HNO3).
18) Calculate the pOH of 0.14 L of a solution containing 0.007 grams of hydrobromic acid (HBr).
19) If it takes 50 mL of 0.2 M NaOH to neutralize 120 mL of an HCl solution, what is the
concentration of HCl? Be sure to write the neutralization reaction.
20) If it takes 25 mL of 0.06 M HBr to neutralize 400 mL of an KOH solution, what is the
concentration of the KOH solution? Be sure to write the neutralization reaction.