Unit : Chp. 14.1, 14.5-14.8– Acids and Bases
14.1 Arrhenius Acids/ Bases
 Acid/ Base Properties &
Nomenclature
 Dissociation Equations
14.5-6 pH Scale
 KW
 pH and pOH calculations
14.7-8 Acid/Base Reactions &
Titrations
 Neutralization Reactions
 Acid/Base Titrations
I Can Statements:
(14.1) Arrhenius Acids/Bases
1. Explain what it means for a chemical to dissociates (ionize) in aqueous solution
2. Identify solutes as strong electrolytes, weak electrolytes, and nonelectrolytes based on their degree
of dissociation in aqueous solution.
3. List which types of substances are strong electrolytes, weak electrolytes, and nonelectrolytes
4. Identify which substances are strong electrolytes, weak electrolytes, and nonelectrolytes when given a list
5. Explain using diagrams what occurs when strong and weak electrolytes are in solution
6. Name and identify the symbols for the hydronium ion, H+/ H3O+ and the hydroxide ion , OH ─
7. Identify acids as substances that increase the hydronium ion concentration [H+ / H3O+] of an aqueous
solution
8. Identify bases as substances that increase the hydroxide ion concentration [OH─] of an aqueous solution
9. List the 7 strong acids /bases and explain what distinguishes strong from a weak acids or bases
10. Identify the ammonia molecule as a base and explain how it acts as such
11. Identify the ammonium polyatomic ion as an acid and explain how it acts as such
11. Interpret and write dissociation equations for strong and weak acids and bases
12. Use nomenclature rules to name or write the chemical formulas for binary and oxy-acids, including “ic”
and “ous” suffixes and “per” and “hypo” prefixes
13. Use nomenclature rules to name or write chemical formulas for hydroxide bases
(14.5, 14.6) K W and pH/ pOH
1.
2.
3.
4.
5.
6.
7.
8.
9.
Write a chemical equation to illustrate the dissociation of pure water
State the value of the [H+] and [OH-] of pure water
Explain that the ion product constant of water, KW = the product of [H+] and [OH-]
State the value of KW for pure water at 25oC
Use KW to calculate the [H+] and [OH-] of any solution
Explain how the numbers on a pH scale are related to [H+] and [OH-]
Compare the strength of an acid/ base based on their pH / pOH
Convert [H+] and [OH-] to pH or pOH and vice-versa
Calculate pH or pOH of a solution when given [H+] or [OH-] values
(14.7, 14.8) Acid-Base Reactions and Titrations
1.
2.
3.
3.
4.
5.
7.
8.
Define what makes a compound a salt and identify salts in chemical equations
List the fundamental reactants and products in any neutralization reaction
Predict the products and write chemical equations for the neutralization reactions of acids with bases
Explain how titrant can be used in a titration to determine the unknown concentration of an acid or base
Explain how the indicator phenolphthalein is used to determine the endpoint in a chemical titration
Calculate the volume of titrant needed to neutralize an acid or base of known molarity
Determine the end point when using a buret and Erlenmeyer flask for an acid/base titration
Use data gathered in a titration to calculate the molarity of an unknown acid or base
1
Vocabulary 14.1, 14.5-14.8
Kw (Ion product
constant)
Acid
Base
Binary acids
Buret
Dissociate(dissociation)
Electrolyte
Endpoint
Erlenmeyer Flask
Hydronium ion[H3O+] / [H+]
Hydroxide ion [OH-]
Indicator
Ionize
Neutralization Reaction
Nonelectrolyte
Oxy-acids
pH / pOH
Phenolphthalein
Salt
Titrant
Titration
Achievement Scale 14.1, 14.5-14.8
Goal
C Level
B Level
A Level
14.1
Arrhenius
Acids/
Bases
 Explain what it means for a chemical to dissociates
(ionize) in aqueous solution
 Identify solutes as strong electrolytes, weak electrolytes,
and nonelectrolytes based on their degree of dissociation in
aqueous solution.
 List which types of substances are strong electrolytes,
weak electrolytes, and nonelectrolytes
 Name and identify the symbols for the hydronium ion, H +/
H3O+ and the hydroxide ion , OH ─
 Identify acids as substances that increase the hydronium
ion concentration [H+ / H3O+] of an aqueous solution
 Identify bases as substances that increase the hydroxide
ion concentration [OH─] of an aqueous solution
 List the 7 strong acids /bases and explain what
distinguishes strong from a weak acids or bases
 Identify the ammonia molecule as a base
 Identify the ammonium polyatomic ion as an acid
 Interpret dissociation equations for strong and weak acids
and bases
 Use nomenclature rules to name or write the chemical
formulas for binary acids
 Use nomenclature rules to name or write chemical
formulas for hydroxide bases
 Write a chemical equation to illustrate the dissociation of
pure water
 State the value of the [H+] and [OH-] of pure water
 Explain that the ion product constant of water, KW = the
product of [H+] and [OH-]
 State the value of KW for pure water at 25oC
 Explain how the numbers on a pH scale are related to [H+]
and [OH-]
 Compare the strength of an acid/ base based on their pH /
pOH
 Convert [H+] and [OH-] to pH or pOH and vice-versa
 Define what makes a compound a salt
 List the fundamental reactants and products in any
neutralization reaction
 Explain how titrant can be used in a titration to determine
the unknown concentration of an acid or base
 Explain how the indicator phenolphthalein is used to
determine the endpoint in a chemical titration
 Determine the end point when using a buret and
Erlenmeyer flask for an acid/base titration
 Identify which
substances are
strong electrolytes,
weak electrolytes,
and nonelectrolytes
when given a list
 Use nomenclature
rules to name or
write the chemical
formulas oxy-acids
 Explain using diagrams
what occurs when strong
and weak electrolytes are
in solution
 Write dissociation
equations for strong and
weak acids and bases
 Explain how the ammonia
molecule acts as a base
 Explain how the
ammonium polyatomic ion
acts as an acid
 Use nomenclature rules to
name or write the chemical
formulas for binary and
oxy-acids, including “ic”
and “ous” suffixes and
“per” and “hypo” prefixes
 Use KW to calculate
the [H+] and [OH-]
of any solution
 Calculate pH or pOH of a
solution when given [H+] or
[OH-] values
 Identify salts in
chemical equations
 Predict the products
for the
neutralization
reactions of acids
with bases
 Write chemical equations for
the neutralization reactions of
acids with bases
 Calculate the volume of
titrant needed to neutralize
an acid or base of known
molarity
 Use data gathered in a
titration to calculate molarity
of an unknown acid or base
14.5, 14.6
KW
and
pH/ pOH
14.7, 14.8
Acid-Base
Reactions
and
Titrations
2
Sample Questions 14.1, 14.5-14.8
C Level:
1. Identify each of the following as a strong electrolyte, weak electrolyte, or nonelectrolyte. Explain each
choice.
(a) CuCO3(s)
Cu2+(aq) + CO22−(aq)
(b) C6H12O6(s) → C6H12O6(aq)
(c) KNO3(s) → K+(aq) + NO3−(aq)
(a) = a weak electrolyte, the two-way arrow indicates that it is only weakly ionized
(b) = a nonelectrolyte, the product is dissolved (aq), but not ionized
(c) = a strong electrolyte, the one-way arrow indicates that it is 100% ionized
2. List the chemical formula for hydrochloric acid HCl
hydrosulfuric acid
3. Name the following acids: H2S
4. What is the difference between a base and an acid in aqueous solution?
base= increases the [OH-]
acid = increases the [H+]
5. Which of the following equations represents a strong base? Explain.
(i) Cu(OH)2
Cu2+ + 2 OH-
(ii) Ba(OH)2
→
Ba2+ + 2 OH-
(ii) represents the stronger base; we know this b/c the one-way arrow indicates that this
base dissociates 100% in aqueous solution
6.
List the chemical formula and name of the 7 strong acids:
HCl,
hydrochloric
HBr,
hydrobromic
HI,
hydroioidic
H2SO4,
sulfuric
HClO3,
chloric
HClO4
perchloric
HNO3,
nitric
7. Identify each of the following as an acid or a base in aqueous solution:
(a) NH4+(aq)
Base
(b) NH3(aq)
Acid
8. If [OH-] > 1.0 x 10-7 M the solution is Basic
9. Write the dissociation equation for pure water.
H2O(l)
H+(aq) + OH−(aq)
3
10.
11.
12.
(a) What is the formula for the ion product constant of water, KW?
KW = [H+] [OH-]
(b) What is the value of KW?
1.0 x 10−14
(a) what is the [H+] of a solution with a pH of 6.20?
10−6.20 = [H+] = 6.310 x 10-7 M
(b) Is this solution acidic or basic?
Acidic
(a) The pH scale is a logarithmic scale. Explain what this means.
the concentration of [H+] increases by 10 between each number on the scale....
so .... a pH of 6 has
10 times more [H+] than a pH of 7
a pH of has 10 × 10
or 100 times more [H+] than a pH of 7
a pH of has 10 × 10 × 10 or 1000 times more [H+] than a pH of 7
etc.
(b) How does the pH scale correspond to the [H+] of an aqueous solution? Use an example to help
explain your answer.
each number on the scale represents an exponent, called a logarithm, to which
the base 10 must be raised to equal the [H+] ......however, since neutral water
has an [H+] of 1.0 x 10−7 M (a number less than 10), the base must be raised to
the negative value of pH
example: if pH = 9.00....then.....10−9.00 = 1.0 x 10−9 M = [H+]
13. What are the products of a neutralization reaction between an acid and a base? salt and water
14.
(a) What is a salt?
an ionic compound that does not have H+ as the cation or OH− as the anion
(b) write the chemical formula of two salts NH4Cl and Zn(NO3)2
15.
(a) For what is a titration used?
a laboratory procedure used to determine the molarity of a solution of
unknown concentration .. a solution of unknown molarity is titrated with a
solution of known molarity
(b) What is a titrant
in a titration, the titrant is the solution in the buret - regardless of whether or
not it's concentration is known
16. What color is the indicator phenolphthalein in an acidic solution? colorless in a basic solution? pink
4
B Level:
17. Use a solubility chart and your knowledge of ionic and molecular compounds to predict whether each of
the following are strong, weak, or non-electrolytes in aqueous solution. Explain your choice in each case.
(a) CO2(g)
nonelectrolyte, molecular compound
(b) PbCl2(s)
weak electrolyte, insoluble in water
(c) NH4NO3
strong electrolyte, ionic compound which is 100% soluble
18. List the chemical formula for chloric acid
HClO3
19. Name the following acids: H2SO4
sulfuric acid
20.
Calculate the [H+] of coffee if it has an [OH-] of 1.0 x 10-9
KW = [H+] [OH-] → [H+] =
𝑲𝑾
[ 𝑶𝑯− ]
→ [H+] =
𝟏.𝟎 𝒙 𝟏𝟎−𝟏𝟒
𝟏.𝟎 𝒙 𝟏𝟎−𝟗 𝑴
→
1.0 x 10-5 = [H+]
21. Predict the products of the following neutralization reaction.
HCl(aq) + NaOH(s) →
NaCl(aq) + H2O(l)
22. Identify the salt in the equation for #12. NaCl
A Level:
23. Draw an illustration of three different solutions. (1) containing a strong electrolyte, (2) containing a weak
electrolyte, and (3) containing a nonelectrolyte.
strong
electrolyte
weak
electrolyte
nonelectrolyte
100%
ionized
weakly
ionized
nonionized
5
24. List the chemical formula for perchloric
HClO4
25. Name the following acids: H2SO3
sulfurous acid
26. Write the dissociation equation for each of the following:
(a)
nitric acid:
NaNO3(aq) → Na+(aq) + NO3−(aq)
(b)
HNO2(aq):
NaNO2(aq)
(c)
Ca(OH)2(s)
Ca(OH)2(s) → Ca2+(aq) + 2 OH−(aq)
Na+(aq) + NO3−(aq)
27. Use a chemical equation to illustrate each of the following:
NH4+ (aq)
(b) NH4+(aq) acting as a base
28.
NH4+(aq) + OH−(aq)
NH3(aq) + H2O
(a) NH3(aq) acting as a base
NH3(aq) + H+(aq)
Calculate the pH of a solution that has an [OH−] of 1.0 x 10-9 M
step 1: calculate the [H+] concentration
KW = [H+] [OH-] → [H+] =
𝑲𝑾
[ 𝑶𝑯− ]
→ [H+] =
step 2: use [H+] to determine pH
pH = −log [H+] → −log (1.0 x 10-5 M) →
𝟏.𝟎 𝒙 𝟏𝟎−𝟏𝟒
𝟏.𝟎 𝒙 𝟏𝟎−𝟗 𝑴
→
1.0 x 10-5 M = [H+]
pH = 5
29. Calculate the molarity of a 25.0 mL of an HCl solution which has been titrated with 32.6 mL of a 0.185 M
NaOH solution.
(i) Write a balanced chemical equation to determine the stoichiometry between acid and base
NaOH + HCl → H2O + NaCl
the stoichiometry is 1:1
it takes 1 mole of NaOH to neturalize 1 mole of HCl
(ii) determine the moles of titrant used
𝟎.𝟏𝟖𝟓 𝒎𝒐𝒍 𝑵𝒂𝑶𝑯
𝑳
(0.0326 L ) = 0.00603 moles of NaOH used
= 0.00603 moles of HCl neutralized
(ii) calculate the molarity of the unknown
𝟎.𝟎𝟎𝟔𝟎𝟑 𝒎𝒐𝒍𝒆𝒔 𝑯𝑪𝒍
𝟎.𝟎𝟐𝟓𝟎 𝑳
= 0.241 M HCl
6