Chem II Block: 11.3.14
Objectives:
• Redox Reaction Exam with stoichiometry
• Introduction to Acid/Base Reactions
Chem II Block: 11.5.14
Objectives:
• Redox Reaction Exam with stoichiometry
• Introduction to Acid/Base Reactions
Acid/Base Reactions-Due Wed.
1. Distinguish between acidic and basic properties;
give applications of both (Venn diagram).
2. a. Identify and distinguish between the three
types of acid/base definitions.
b. Which definition above best explains how you
classify acids and bases? Explain your answer.
c. Which definition above do you think classifies
acids and bases the best? Explain your answer.
Acid/Base Reactions-Due Wed.
1. Distinguish between acidic and basic properties;
give applications of both (Venn diagram).
2. a. Identify and distinguish between the three
types of acid/base definitions.
b. Which definition above best explains how you
classify acids and bases? Explain your answer.
c. Which definition above do you think classifies
acids and bases the best? Explain your answer.
Acidic vs. Basic Properties
Acidic/Basic Definitions
Acidic/Basic Definitions
Arrhenius
Bronstead-Lowry
Lewis
Acidic and Basic
Definitions
Example
Chem II Block: 11.6.14
Objectives:
• I can identify acids and bases in a reaction based
on the acid/base definitions.
• I can distinguish between strong and weak
acids/bases.
• I can establish the net ionic equations of
neutralization reactions.
• I can identify the conjugate acid and conjugate
base in an acid/base reaction.
• I can apply stoichiometry with neutralization
reactions.
Strong or Weak Acids/Bases
• Explain which reaction below consists of a
strong acid and which consists of a weak acid.
a. HBr + H2O -----> H3O+ + HSb. H2S + H2O -----> H3O+ HS-
Acidic/Basic Definitions
Acidic/Basic Definitions
Arrhenius
Bronstead-Lowry
Lewis
Acidic and Basic
Definitions
Example
Acidic/Basic Definitions
1. Determine which type of base is represented in each
reaction below (arrhenius base, Bronstead-Lowry
base, and Lewis base).
a. NaOH (s) ---------> Na+ (aq) + OH- (aq)
b. HF (aq) + H2O (l) -----> F- (aq) + H3O+ (aq)
c. H+(aq) + NH3 (aq) ------> NH4+ (aq)
2. Identify which reactant below is the acid and the
base. Which definition best explains your
classification?
H2CO3 + H2O ------> HCO3- + H3O+
Neutralization Reactions
Objectives:
• Establish Net Ionic Equations
• Apply Stoichiometry
• Assigned textbook problems
Chem II Block: 11.7.14
Due: Textbook Problems
Objectives:
• I can identify acids and bases in a reaction based
on the acid/base definitions.
• I can distinguish between strong and weak
acids/bases.
• I can establish the net ionic equations of
neutralization reactions.
• I can identify the conjugate acid and conjugate
base in an acid/base reaction.
• I can apply stoichiometry with neutralization
reactions.
Text Practice Problems
Stoichiometry Map
Mole Conversion Map
http://mysite.cherokee.k12.ga.us
Chem II Block: 11.10.14
Due:
Textbook Problems
Objectives:
• I can identify acids and bases in a reaction based on the
acid/base definitions.
• I can distinguish between strong and weak acids/bases.
• I can establish the net ionic equations of neutralization
reactions.
• I can apply stoichiometry with neutralization reactions.
• I can identify the conjugate acid and conjugate base in
acid/base reactions.
• I can calculate the molar concentration of H+ and OH- in
aqueous solutions.
• I can understand and calculate the pH and pOH values of
aqueous solutions.
Homework Qts.
Acid/Base Review: Bell Ringer
1. Identify the acid and base for each reaction
below. Determine which definition best classifies
each reactant as an acid/base.
a. H2(SO4)(aq) + H2O (l) ----> H3O+ (aq) + HSO4- (aq)
b. BF3 (aq) + F-(aq) -----> BF4- (aq)
c. HNO3 (aq) + Al(OH)3(aq) -----> H2O (l) + Al(NO3)3 (aq)
2. Establish the net ionization reaction for 1c.
Conjugate Acids and Bases
• What are conjugate acids and bases?
• Which acid/base definition best describes
acid/base conjugates?
Conjugate Acids/Bases
• HF + H2O
F-
• Strength of CA and CB:
+
H3O+
Chem II Block: 11.11.14
Due:
Textbook Problems due-place in tray.
Objectives:
• SRI Testing: password: LLeeper
• I can identify the conjugate acid and conjugate
base in acid/base reactions.
• I can calculate the molar concentration of H+ and
OH- in aqueous solutions.
• I can understand and calculate the pH and pOH
values of aqueous solutions.
Strong Acids and Bases
Strong Acids
Strong Bases
HCl
LiOH
HBr
NaOH
HI
KOH
HClO4
RbOH
HClO3
CsOH
HNO3
Ca(OH)2
H2SO4
Sr(OH)2
Ba(OH)2
Can the periodic table be helpful in identifying strong acids and bases?
Conjugate Acids and Bases
• Complete qts. 23 from textbook:
Also, identify if the CA and CB are considered
weak or strong.
Chem II Block: 11.12.14
Due: *those absent yesterday*:
Textbook Problems due-place in tray.
Objectives:
• I can identify the conjugate acid and conjugate
base in acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions.
• I can associate pH values with molar
concentration of H3O+ions; pOH values with molar
concentrations of OH-ions.
Strong Acids and Bases
Strong Acids
Strong Bases
HCl
LiOH
HBr
NaOH
HI
KOH
HClO4
RbOH
HClO3
CsOH
HNO3
Ca(OH)2
H2SO4
Sr(OH)2
Ba(OH)2
Identify ways in which the periodic table can help you remember strong acids and bases.
Acid/Base and Conjugate Pairs Review
• HC2H3O2 + H2O
H3O+ + C2H3O2-
a. Identify the acid and base and their
conjugate pairs.
b. Determine whether or not the acid and base
or their conjugate pair is stronger.
c. Knowing which substances are stronger,
predict which direction is favored in the
reaction.
Acid/Base and Conjugate Pairs Review
• HC2H3O2 + H2O
H3O+ + C2H3O2-
a. Identify the acid and base and their
conjugate pairs.
b. Determine whether or not the acid and base
or their conjugate pair is stronger.
c. Knowing which substances are stronger,
predict which direction is favored in the
reaction.
Acid/Base and Conjugate Pairs Review
• HC2H3O2 + H2O ------> H3O+ + C2H3O2a. Identify the acid and base and their
conjugate pairs.
b. Determine whether or not the acid and base
or their conjugate pair is stronger.
c. Knowing which substances are stronger,
predict which direction is favored in the
reaction.
Strong Acids and Bases
Strong Acids
Strong Bases
HCl
LiOH
HBr
NaOH
HI
KOH
HClO4
RbOH
HClO3
CsOH
HNO3
Ca(OH)2
H2SO4
Sr(OH)2
Ba(OH)2
Identify ways in which the periodic table can help you remember strong acids and bases.
Strengths of Acids and Bases
Water: Self-Ionization
H2O + H2O
H3O+ + OH-
@25oC
• What did we learn yesterday that scientist
gained from studying the self-ionization of
water or what can you conclude from the
reaction above?
Water: Self-Ionization
• H2O + H2O
H3O+ + OH-
• This is a reversible reaction.
• Water is considered a weak electrolyte.
• Draw the reversible arrows, indicating which
direction is more favorable.
Kw: Water Ionization Constant
• Always constant in water and dilute aqueous
solutions.
• Temperature dependent, direct relationship.
• The product of [H3O+] and [OH-].
Kw= [H3O+] [OH-] =
Chem II Block: 11.13.14
Due: *those absent yesterday*:
Textbook problems (14, 16, 26, 32, 33)
Infinite Campus:
• Hydrogen Peroxide Lab (15pts.)
• Acid/Base Textbook Problems (10pts.)
Objectives:
• I can identify the conjugate acid and conjugate base
in acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions.
• I can associate pH values with molar concentration of
H3O+ions; pOH values with molar concentrations of
OH-ions.
Kw: Water Ionization Constant
Calculating [H3O+] and [OH-] Concentrations
A 1.0 x10-4 M solution of HNO3 has been
prepared for a laboratory experiment.
a. Calculate the [H3O+] of this solution.
b. Calculate the [OH-] of this solution.
Chem II Block: 11.14.14
Due: *those absent yesterday*:
Textbook problems (14, 16, 26, 32, 33)
Objectives:
• I can identify the conjugate acid and conjugate
base in acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions in solutions
containing strong acids and bases.
• I can associate pH values with molar
concentration of H3O+ions; pOH values with molar
concentrations of OH-ions.
pH Scale vs. [H3O+] concentration
Explain the relationship between the [H3O+] concentration and pH scale at neutral,
acidic, and basic conditions.
pH value vs. [H3O+] concentration
a. What is the pH of a 2.6x10-3 M H2SO4 solution?
b. What is the pH of a 4.2x10-3 Na(OH) solution?
Aqueous Solutions
Aqueous Solutions: Calculations
0.03M HBr solution at 25oC.
a. Establish the ionization equation and identify the
acid, base, and conjugate pairs.
b. Which direction is favored in the ionization equation?
c. Calculate the [H3O+] and the [OH-] in this solution.
d. What is the pH of this solution?
e. What is the pOH of this solution?
f. Using evidence above, prove why this is an acidic
solution.
Aqueous Solutions: Calculations
2.4x10-3 M HNO3 solution at 25oC.
a. Establish the ionization equation and identify the
acid, base, and conjugate pairs.
b. Which direction is favored in the ionization equation?
c. Calculate the [H3O+] and the [OH-] in this solution.
d. What is the pH of this solution?
e. What is the pOH of this solution?
f. Using evidence above, prove why this is an acidic
solution.
Aqueous Solutions: Calculations
5.4x10-3 M HClO4 solution at 25oC.
a. Establish the ionization equation and identify the
acid, base, and conjugate pairs.
b. Which direction is favored in the ionization equation?
c. Calculate the [H3O+] and the [OH-] in this solution.
d. What is the pH of this solution?
e. What is the pOH of this solution?
f. Using evidence above, prove why this is an acidic
solution.
Aqueous Solutions: Calculations
7.3x10-2 M HNO3 solution at 25oC.
a. Establish the ionization equation and identify the
acid, base, and conjugate pairs.
b. Which direction is favored in the ionization equation?
c. Calculate the [H3O+] and the [OH-] in this solution.
d. What is the pH of this solution?
e. What is the pOH of this solution?
f. Using evidence above, prove why this is an acidic
solution.
Aqueous Solutions: Calculations
2.5x10-4 HCl solution at 25oC.
a. Establish the ionization equation and identify the
acid, base, and conjugate pairs.
b. Which direction is favored in the ionization equation?
c. Calculate the [H3O+] and the [OH-] in this solution.
d. What is the pH of this solution?
e. What is the pOH of this solution?
f. Using evidence above, prove why this is an acidic
solution.
Chem II Block: 11.17.14
Objectives:
• I can identify the conjugate acid and conjugate
base in acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions in solutions
containing strong acids and bases.
• I can associate pH values with molar
concentration of H3O+ions; pOH values with molar
concentrations of OH-ions.
• I can use acid-base reactions to calculate
concentration of unknown solutions.
Chem II Block: 11.18.14
Objectives:
• I can identify the conjugate acid and conjugate
base in acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions in solutions
containing strong acids and bases.
• I can associate pH values with molar
concentration of H3O+ions; pOH values with molar
concentrations of OH-ions.
• I can use acid-base reactions to calculate
concentration of unknown solutions.
Brain Teaser: pH Values
• 0.1 M HCl
• 0.1 M H2SO4
• 0.1 M HF
Weak Acids and Bases
• What are weak acids and bases?
Weak Acids and Bases
• How can we calculate the [H3O+] and [OH-]
concentration in solutions containing weak acids
and bases?
Weak Acids and Bases
• How can we calculate the [H3O+] and [OH-]
concentration in solutions containing weak acids
and bases?
http://www.sensorland.com/HowPage037.html
pH Calculations
• Complete practice problems: 1-4 on pg. 490.
Acid-Base Indicators
http://acid-base-titration.blogspot.com/
Chem II Block: 11.19.14
Infinite Campus:
• Acid/Base pH and pOH practice problem (10pts.)
• Acid/Base Quiz (22pts.)
Objectives:
• I can identify the conjugate acid and conjugate base in
acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions in solutions containing
strong acids and bases.
• I can associate pH values with molar concentration of
H3O+ions; pOH values with molar concentrations of OH-ions.
• I can use acid-base reactions to calculate concentration of
unknown solutions.
Acid/Base Quiz
Titrations and Molarity
Equivalence Point:
End Point:
Chem II Block: 11.20.14
Objectives:
• I can identify the conjugate acid and conjugate base in
acid/base reactions.
• I can use the Kw constant to calculate the molar
concentrations of H3O+ and OH- ions in solutions
containing strong acids and bases.
• I can associate pH values with molar concentration of
H3O+ions; pOH values with molar concentrations of OHions.
• I can use acid-base reactions to calculate concentration of
unknown solutions.
• Homework: Test tomorrow over Acid/Base Reactions
Titrations and Molarity
MA x VA = MB x VB
+
moles A = moles B, *if 1:1 ratio of H to OH
http://chemwiki.ucdavis.edu
-
Titrations and Molarity: Bell Ringer
1. The molarity of a NaOH solution can be determined by
titrating a known volume of the solution with a HCl solution of
known concentration. If 19.1 mL of 0.118M HCl is required to
neutralize 25.00 mL of a NaOH solution, what is the molarity of
the NaOH?
2. If 8.6 mL of 0.0994 M HNO3 is required to neutralize 25.00 mL
of a Sr(OH)2 solution, what is the molarity of the Sr(OH)2?
Titrations and Molarity: Bell Ringer
1. The molarity of a NaOH solution can be determined by
titrating a known volume of the solution with a HCl solution of
known concentration. If 19.1 mL of 0.118M HCl is required to
neutralize 25.00 mL of a NaOH solution, what is the molarity of
the NaOH?
2. If 8.6 mL of 0.0994 M HNO3 is required to neutralize 25.00 mL
of a Sr(OH)2 solution, what is the molarity of the Sr(OH)2?
Acid/Base Review: Gallery Walk
• Record answers on separate sheet of paperpick-up tomorrow for credit.
• Acid/Base Test: tomorrow, Friday 11.21
Aqueous Solutions Calculations
1. The pH of a solution is determined to be 5.0.
a. What is the hydronium ion concentration of
this solution?
b. What is the hydroxide ion concentration of
this solution?
c. What is the pOH value of this solution?
Aqueous Solutions Calculations
1. The pH of an aqueous solution is measured
to be 1.50.
a. Calculate the hydronium ion concentration in
solution.
b. Calculate the hydroxide ion concentration in
solution.
c. What is the pOH value of this solution?