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Drop the Base
Anger is an acid that can do more harm to the vessel in which it is stored than to anything on which it is
poured.- Mark Twain
What we already know…
Acids are solutions with hydronium ions in solution.
Bases are solutions with hydroxide ions in solution.
Acids and Bases can be classified as Strong if they ionize completely
Acids and Bases can be classified as Weak if they do NOT ionize completely
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What’s an Acid?Arrhenius – a substance that increase the number of [H+] ions when mixed with water
Brǿwnsted-Lowry – substances that donate protons (H+)
Lewis – a substance that can accept electrons
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Common Acids
Acetic AcidCarbonic AcidCitric AcidHydrochloric AcidPhosphoric AcidSulfuric Acid
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What’s a Base?
Arrhenius Base – a substance that increase the number of [OH] ions when mixed with water
Brǿwnsted-Lowry Base – substances that accepts protons
Lewis Base – a substance that can donates electrons
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Common Bases
AcetoneAmmoniaCalcium hydroxideLithium hydroxidePyridineSodium hydroxide
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All thumbs are fingers but not all fingers are thumbs…
All Arrhenius acids are Brǿwnsted-Lowry acids, and all BL acids are Lewis acids
Not all Lewis acids are Brǿwnsted-Lowry or Arrhenius acids
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Example
Draw a mechanism showing how HCl acid meets the definition for each type of acid.
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Strong Acids & Strong Bases (MEMORIZE!)Strong Acids and Bases completely disassociate in water (Arrhenius).
Name Chemical Formula
Hydroiodic acid
HI
Hydrobromic acid
HBr
Perchloric acid HClO4
Hydrochloric acid
HCl
Sulfuric acid H2SO4
Nitric acid HNO3
Name Chemical Formula
Sodium hydroxide NaOH
Potassium hydroxide KOH
lithium hydroxide LiOH
Rubidium hydroxide RbOH
Cessium hydroxide CsOH
Calcium hydroxide Ca(OH)2
barium hydroxide Ba(OH)2
strontium hydroxide Sr(OH)2
Naming Acids
Similar to polyatomic ions but one BIG change
Anions Name Change -ate -ic-ous -ite-ide hyrdo-____-ic
Naming Bases
Bases follow the same rules as polyatomic ions.
Name the cation followed by the anion (hydroxide)
If the cation is a transition metal indicate the oxidation number
Conjugate Acids and Bases
What about water?
Measuring Acid Strength
pH = -log [H+]
Name Variable Definition Units Measured by
Acid Strength
pH Logarithmic measurement of the ability of a substance to form hydronium ions in solution
NONE pH probe, litmus paper
Hydrogen Ion
Concentration
[H+] The concentration of hydronium ions present in solution
M Calculated or Counted (not
feasible)
Measuring Base Strength
pOH = -log [OH-]
Name Variable Definition Units Measured by
Base Strength
pOH Logarithmic measurement of the ability of a substance to form hydroxide ions in solution
NONE pH probe, litmus paper
Hydroxide Concentrati
on
[OH-] The concentration of hydroxide ions present in solution
M Calculated or Counted (not
feasible)
pH Scale
Measuring Acid Strength
pH probes
Litmus Paper
Water Disassociation
Water will disassociate by itself in a very small amount
H2O [H+][OH-]
Kw = [H+][OH-] = 1.0 X 10-14
[H2O]
Relating pH to pOH
pH + pOH = 14
Name Variable Definition Units Measured by
Base Strength
pOH Logarithmic measurement of the ability of a substance to form hydroxide ions in solution
NONE pH probe, litmus paper
Acid Strength
pH Logarithmic measurement of the ability of a substance to form hydronium ions in solution
NONE pH probe, litmus paper
Example B-1
H2SO4 is a strong acid. What is the name, pH and pOH of a solution of a 15.8 M solution?
Example B-2
Write an equation for the ionization of water. What is the pH and pOH of water?
Example B-3
A has a pH of 3.6. How many hydronium ions are present in a 25 mL sample of solution?
Example B-4
What is the pH of a solution containing 1.4 X 10-
10 M [H+]? Classify the substance as an acid, neutral or base.
Acid Disassociation
Acids and Bases disassociate very similar to ions
HA [H+][A-]
We can write a disassociation expression as:
Strong Acids
Strong Acids disassociate COMPLETELY (or close to it)
The expression is meaningless/infinity
And this simplifies to
Initial Concentration of S.A. = Final Concentration of [H+]
Weak Acids
Weak Acids partially disassociate
The expression is crucial to determining [H+] Concentration
Initial Concentration of S.A. = Final Concentration of [H+]
Example D-1
The acid disassociation constant for acetic acid is 1.58 X 10-5. What is the pH of a solution of 0.15 M acetic acid? How does this compare to the pH of 0.15 M hydrochloric acid?
Base Disassociation
Bases disassociate very similar to ions
BOH [B+][OH-]
We can write a disassociation expression as:
Strong Bases
Strong bases disassociate COMPLETELY (or close to it)
The expression is meaningless/infinity
And this simplifies to
Initial Concentration of S.B. = Final Concentration of [OH-]
Weak Bases
Weak Bases partially disassociate
The expression is crucial to determining [OH-] Concentration
Initial Concentration of S.B. = Final Concentration of [OH-]
Example E-1
The disassociation constant for pyridine is 1.8 X 10-9. What is the pH of a solution of 0.15 M pyridine?
Percent Ionization
Percent Ionization = Concentration Ionized X 100 Original Concentration
Example D-1
Calculate the percent ionization for a solution of 0.01 M benzoic acid where Ka = 6.31 X 10-5.