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Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Objectives
• List five general properties of aqueous acids and
bases.
• Name common binary acids and oxyacids, given
their chemical formulas.
• List five acids commonly used in industry and the
laboratory, and give two properties of each.
• Define acid and base according to Arrhenius’s theory
of ionization.
• Explain the differences between strong and weak
acids and bases.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acids
1. Aqueous solutions of acids have a sour taste.
2. Acids change the color of acid-base indicators.
3. Some acids react with active metals and release
hydrogen gas, H2.
Ba(s) + H2SO4(aq) BaSO4(s) + H2(g)
Chapter 14
Section 1 Properties of Acids and
Bases
4. Acids react with bases to produce salts and water.
5. Acids conduct electric current.
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acids, continued
Acid Nomenclature
• A binary acid is an acid that contains only two
different elements: hydrogen and one of the more
electronegative elements.
• HF, HCl, HBr, and HI
• Binary Acid Nomenclature
1. The name of a binary acid begins with the prefix
hydro-.
2. The root of the name of the second element
follows this prefix.
3. The name then ends with the suffix -ic.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acids, continued
Acid Nomenclature, continued
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acids, continued
Acid Nomenclature, continued
• An oxyacid is an acid that is a compound of
hydrogen, oxygen, and a third element, usually a
nonmetal.
• HNO3, H2SO4
• The names of oxyacids follow a pattern.
• The names of their anions are based on the names of
the acids.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acids, continued
Acid Nomenclature, continued
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Some Common Industrial Acids
• Sulfuric Acid
• Sulfuric acid is the most commonly produced industrial
chemical in the world.
• Nitric Acid
• Phosphoric Acid
• Hydrochloric Acid
• Concentrated solutions of hydrochloric acid are commonly
referred to as muriatic acid.
• Acetic Acid
• Pure acetic acid is a clear, colorless, and pungent-smelling
liquid known as glacial acetic acid.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Monoprotic and Polyprotic Acids
• A monoprotic acid is an acid that can donate only
one proton (hydrogen ion) per molecule.
• HClO4, HCl, HNO3
• only one ionization step
HCl(g) + H2
O(l) → H3
O+
(aq) + ClĞ
(aq)
Chapter 14 Section 2 Acid-Base Theories
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Monoprotic and Diprotic Acids
Chapter 14 Section 2 Acid-Base Theories
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Monoprotic and Polyprotic Acids, continued
• A polyprotic acid is an acid that can donate more
than one proton per molecule.
• H2SO4, H3PO4
• Multiple ionization stepsH2
SO4
(l) + H2
O(l) → H3
O+
(aq) + HSO4
Ğ
(aq)
HSO4
Ğ
(aq) + H2
O(l)  →←  H3
O+
(aq) + SO4
2Ğ
(l)
HSO4
Ğ
and SO4
2Ğ
Chapter 14 Section 2 Acid-Base Theories
(1)
(2)
• Sulfuric acid solutions contain H3O+
,
ions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Monoprotic and Polyprotic Acids, continued
• A diprotic acid is the type of polyprotic acid that can
donate two protons per molecule
• H2SO4
• A triprotic acid is the type of polyprotic acid that can
donate three protons per molecule.
• H3PO4
Chapter 14 Section 2 Acid-Base Theories
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Bases
1. Aqueous solutions of bases taste bitter.
2. Bases change the color of acid-base indicators.
3. Dilute aqueous solutions of bases feel slippery.
4. Bases react with acids to produce salts and water.
5. Bases conduct electric current.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases
• An Arrhenius acid is a chemical compound that
increases the concentration of hydrogen ions, H+
, in
aqueous solution.
• An Arrhenius base is a substance that increases the
concentration of hydroxide ions, OH−
, in aqueous
solution.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases, continued
Aqueous Solutions of Acids
• Arrhenius acids are molecular compounds with
ionizable hydrogen atoms.
• Their water solutions are known as aqueous acids.
• All aqueous acids are electrolytes.
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases, continued
Aqueous Solutions of Acids, continued
• Common Aqueous Acids
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases, continued
Strength of Acids
• A strong acid is one that ionizes completely in
aqueous solution.
• a strong acid is a strong electrolyte
• HClO4, HCl, HNO3
• A weak acid releases few hydrogen ions in aqueous
solution.
• hydronium ions, anions, and dissolved acid
molecules in aqueous solution
• HCN
• Organic acids (—COOH), such as acetic acid
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases, continued
Aqueous Solutions of Bases
• Most bases are ionic compounds containing metal
cations and the hydroxide anion, OH−
.
• dissociate in water
+ −
→s aq + aq2H O
NaOH( ) Na ( ) OH ( )
+ −→¬ aq + l aq + aq3 2 4NH ( ) H O( ) NH ( ) OH ( )
Chapter 14
Section 1 Properties of Acids and
Bases
• Ammonia, NH3, is molecular
• Ammonia produces hydroxide ions when it reacts
with water molecules.
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Arrhenius Acids and Bases, continued
Strength of Bases
• The strength of a base depends on the extent to
which the base dissociates.
• Strong bases are strong electrolytes
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Neutralization Reactions
Strong Acid-Strong Base Neutralization
• In aqueous solutions, neutralization is the reaction
of hydronium ions and hydroxide ions to form water
molecules.
• A salt is an ionic compound composed of a cation
from a base and an anion from an acid.
HCl(aq) + NaOH(aq) → NaCl(aq) + H2
O(l)
Chapter 14 Section 3 Acid-Base Reactions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Objectives
• Define and recognize Brønsted-Lowry acids and
bases.
• Define a Lewis acid and a Lewis base.
• Name compounds that are acids under the Lewis
definition but are not acids under the Brønsted-Lowry
definition.
Chapter 14 Section 2 Acid-Base Theories
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Brønsted-Lowry Acids and Bases
• A Brønsted-Lowry acid is a molecule or ion that is a
proton donor.
• Hydrogen chloride acts as a Brønsted-Lowry acid
when it reacts with ammonia.
+ −
+ → +3 4HCl NH NH Cl
+ −→¬ l + aq aq + aq2 3 4H O( ) NH ( ) NH ( ) OH ( )
Chapter 14 Section 2 Acid-Base Theories
• Water can act as a Brønsted-Lowry acid.
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Brønsted-Lowry Acids and Bases, continued
• A Brønsted-Lowry base is a molecule or ion that is
a proton acceptor.
• Ammonia accepts a proton from the hydrochloric
acid. It acts as a Brønsted-Lowry base.
+ −
+ → +3 4HCl NH NH Cl
Chapter 14 Section 2 Acid-Base Theories
• The OH−
ion produced in solution by Arrhenius
hydroxide bases (NaOH) is the Brønsted-Lowry
base.
• The OH−
ion can accept a proton.
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Brønsted-Lowry Acids and Bases, continued
• In a Brønsted-Lowry acid-base reaction, protons
are transferred from one reactant (the acid) to
another (the base).
+ −
+ → +3 4HCl NH NH Cl
Chapter 14 Section 2 Acid-Base Theories
acid base
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Lewis Acids and Bases
• A Lewis acid is an atom, ion, or molecule that
accepts an electron pair to form a covalent bond.
• The Lewis definition is the broadest of the three
acid definitions.
• A bare proton (hydrogen ion) is a Lewis acid
Chapter 14 Section 2 Acid-Base Theories
H+
(aq) + :NH3(aq)  [H – NH3]+
(aq) or [NH4]+
(aq)
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Lewis Acids and Bases, continued
• The formula for a Lewis acid need not include
hydrogen.
• The silver ion can be a Lewis acid
BF3
(aq) + FĞ
(aq) → BF4
Ğ
(aq)
Chapter 14 Section 2 Acid-Base Theories
• Any compound in which the central atom has three
valence electrons and forms three covalent bonds
can react as a Lewis acid.
Ag+
(aq) + 2 :NH3(aq)  [H3N – Ag – NH3]+(aq) or [Ag(NH3)2]+
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Lewis Acids and Bases, continued
Acid Base Definitions
Chapter 14 Section 2 Acid-Base Theories
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Objectives
• Describe a conjugate acid, a conjugate base, and an
amphoteric compound.
• Define acid rain, give examples of compounds that
can cause acid rain, and describe effects of acid rain.
Chapter 14 Section 3 Acid-Base Reactions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Conjugate Acids and Bases
• The species that remains after a Brønsted-Lowry
acid has given up a proton is the conjugate base of
that acid.
− +→¬ aq + l aq + aq2 3HF( ) H O( ) F ( ) H O ( )
Chapter 14 Section 3 Acid-Base Reactions
acid conjugate
base
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Conjugate Acids and Bases, continued
• Brønsted-Lowry acid-base reactions involve two
acid-base pairs, known a conjugate acid-base pairs.
Chapter 14 Section 3 Acid-Base Reactions
acid1 base2 base1 acid2
− +→¬ aq + l aq + aq2 3HF( ) H O( ) F ( ) H O ( )
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Neutralization Reactions
Chapter 14 Section 3 Acid-Base Reactions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Conjugate Acids and Bases, continued
Strength of Conjugate Acids and Bases
• The stronger an acid is, the weaker its conjugate
base
• The stronger a base is, the weaker its conjugate acid
+ −
→g + l aq + aq2 3HCl( ) H O( ) H O ( ) Cl ( )
Chapter 14 Section 3 Acid-Base Reactions
strong acid base acid weak base
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Conjugate Acids and Bases, continued
Strength of Conjugate Acids and Bases, continued
• Proton transfer reactions favor the production of the
weaker acid and the weaker base.
+ −
→aq + l aq + aq4 2 3 4HClO ( ) H O( ) H O ( ) ClO ( )
+ −
¬aq + l aq + aq3 2 3 3CH COOH( ) H O( ) H O ( ) CH COO ( )
Chapter 14 Section 3 Acid-Base Reactions
stronger acid stronger base weaker acid weaker base
• The reaction to the right is more favorable
weaker acid weaker base stronger acid stronger base
• The reaction to the left is more favorable
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Relative Strengths of Acids and Bases
Chapter 14 Section 3 Acid-Base Reactions
Relative Strengths of Acids and Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Amphoteric Compounds
• Any species that can react as either an acid or a
base is described as amphoteric.
• example: water
• water can act as a base
+ −
→aq + l aq + aq2 4 2 3 4H SO ( ) H O( ) H O ( ) HSO ( )
+ −→ +¬ g + l aq aq3 2 4NH ( ) H O( ) NH ( ) OH ( )
Chapter 14 Section 3 Acid-Base Reactions
acid1 base2 acid2 base1
• water can act as an acid
base1 acid2 acid1 base2
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Amphoteric Compounds, continued
–OH in a Molecule
• The covalently bonded -OH group in an acid is
referred to as a hydroxyl group.
• Molecular compounds containing —OH groups can
be acidic or amphoteric.
• The behavior of a compound is affected by the
number of oxygen atoms bonded to the atom
connected to the —OH group.
Chapter 14 Section 3 Acid-Base Reactions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Oxyacids of Chlorine
Chapter 14 Section 3 Acid-Base Reactions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Relationship of [H3O+
] to [OH–
]
Chapter 14
Section 1 Properties of Acids and
Bases
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Acid Rain
• NO, NO2, CO2, SO2, and SO3 gases from industrial
processes can dissolve in atmospheric water to
produce acidic solutions.
SO3
(g) + H2
O(l) → H2
SO4
(aq)
Chapter 14 Section 3 Acid-Base Reactions
• example:
• Very acidic rain is known as acid rain.
• Acid rain can erode statues and affect ecosystems.
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ResourcesChapter menu
Visual Concepts
Acid Precipitation
Chapter 14

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Ch 14 notes for upload

  • 1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives • List five general properties of aqueous acids and bases. • Name common binary acids and oxyacids, given their chemical formulas. • List five acids commonly used in industry and the laboratory, and give two properties of each. • Define acid and base according to Arrhenius’s theory of ionization. • Explain the differences between strong and weak acids and bases. Chapter 14 Section 1 Properties of Acids and Bases
  • 2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acids 1. Aqueous solutions of acids have a sour taste. 2. Acids change the color of acid-base indicators. 3. Some acids react with active metals and release hydrogen gas, H2. Ba(s) + H2SO4(aq) BaSO4(s) + H2(g) Chapter 14 Section 1 Properties of Acids and Bases 4. Acids react with bases to produce salts and water. 5. Acids conduct electric current.
  • 3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acids, continued Acid Nomenclature • A binary acid is an acid that contains only two different elements: hydrogen and one of the more electronegative elements. • HF, HCl, HBr, and HI • Binary Acid Nomenclature 1. The name of a binary acid begins with the prefix hydro-. 2. The root of the name of the second element follows this prefix. 3. The name then ends with the suffix -ic. Chapter 14 Section 1 Properties of Acids and Bases
  • 4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acids, continued Acid Nomenclature, continued Chapter 14 Section 1 Properties of Acids and Bases
  • 5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acids, continued Acid Nomenclature, continued • An oxyacid is an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal. • HNO3, H2SO4 • The names of oxyacids follow a pattern. • The names of their anions are based on the names of the acids. Chapter 14 Section 1 Properties of Acids and Bases
  • 6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acids, continued Acid Nomenclature, continued Chapter 14 Section 1 Properties of Acids and Bases
  • 7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Some Common Industrial Acids • Sulfuric Acid • Sulfuric acid is the most commonly produced industrial chemical in the world. • Nitric Acid • Phosphoric Acid • Hydrochloric Acid • Concentrated solutions of hydrochloric acid are commonly referred to as muriatic acid. • Acetic Acid • Pure acetic acid is a clear, colorless, and pungent-smelling liquid known as glacial acetic acid. Chapter 14 Section 1 Properties of Acids and Bases
  • 8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Monoprotic and Polyprotic Acids • A monoprotic acid is an acid that can donate only one proton (hydrogen ion) per molecule. • HClO4, HCl, HNO3 • only one ionization step HCl(g) + H2 O(l) → H3 O+ (aq) + ClĞ (aq) Chapter 14 Section 2 Acid-Base Theories
  • 9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Monoprotic and Diprotic Acids Chapter 14 Section 2 Acid-Base Theories
  • 10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Monoprotic and Polyprotic Acids, continued • A polyprotic acid is an acid that can donate more than one proton per molecule. • H2SO4, H3PO4 • Multiple ionization stepsH2 SO4 (l) + H2 O(l) → H3 O+ (aq) + HSO4 Ğ (aq) HSO4 Ğ (aq) + H2 O(l)  →←  H3 O+ (aq) + SO4 2Ğ (l) HSO4 Ğ and SO4 2Ğ Chapter 14 Section 2 Acid-Base Theories (1) (2) • Sulfuric acid solutions contain H3O+ , ions
  • 11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Monoprotic and Polyprotic Acids, continued • A diprotic acid is the type of polyprotic acid that can donate two protons per molecule • H2SO4 • A triprotic acid is the type of polyprotic acid that can donate three protons per molecule. • H3PO4 Chapter 14 Section 2 Acid-Base Theories
  • 12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Bases 1. Aqueous solutions of bases taste bitter. 2. Bases change the color of acid-base indicators. 3. Dilute aqueous solutions of bases feel slippery. 4. Bases react with acids to produce salts and water. 5. Bases conduct electric current. Chapter 14 Section 1 Properties of Acids and Bases
  • 13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases • An Arrhenius acid is a chemical compound that increases the concentration of hydrogen ions, H+ , in aqueous solution. • An Arrhenius base is a substance that increases the concentration of hydroxide ions, OH− , in aqueous solution. Chapter 14 Section 1 Properties of Acids and Bases
  • 14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases, continued Aqueous Solutions of Acids • Arrhenius acids are molecular compounds with ionizable hydrogen atoms. • Their water solutions are known as aqueous acids. • All aqueous acids are electrolytes. Chapter 14 Section 1 Properties of Acids and Bases
  • 15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases, continued Aqueous Solutions of Acids, continued • Common Aqueous Acids Chapter 14 Section 1 Properties of Acids and Bases
  • 16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases, continued Strength of Acids • A strong acid is one that ionizes completely in aqueous solution. • a strong acid is a strong electrolyte • HClO4, HCl, HNO3 • A weak acid releases few hydrogen ions in aqueous solution. • hydronium ions, anions, and dissolved acid molecules in aqueous solution • HCN • Organic acids (—COOH), such as acetic acid Chapter 14 Section 1 Properties of Acids and Bases
  • 17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases, continued Aqueous Solutions of Bases • Most bases are ionic compounds containing metal cations and the hydroxide anion, OH− . • dissociate in water + − →s aq + aq2H O NaOH( ) Na ( ) OH ( ) + −→¬ aq + l aq + aq3 2 4NH ( ) H O( ) NH ( ) OH ( ) Chapter 14 Section 1 Properties of Acids and Bases • Ammonia, NH3, is molecular • Ammonia produces hydroxide ions when it reacts with water molecules.
  • 18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Arrhenius Acids and Bases, continued Strength of Bases • The strength of a base depends on the extent to which the base dissociates. • Strong bases are strong electrolytes Chapter 14 Section 1 Properties of Acids and Bases
  • 19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Neutralization Reactions Strong Acid-Strong Base Neutralization • In aqueous solutions, neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules. • A salt is an ionic compound composed of a cation from a base and an anion from an acid. HCl(aq) + NaOH(aq) → NaCl(aq) + H2 O(l) Chapter 14 Section 3 Acid-Base Reactions
  • 20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives • Define and recognize Brønsted-Lowry acids and bases. • Define a Lewis acid and a Lewis base. • Name compounds that are acids under the Lewis definition but are not acids under the Brønsted-Lowry definition. Chapter 14 Section 2 Acid-Base Theories
  • 21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Brønsted-Lowry Acids and Bases • A Brønsted-Lowry acid is a molecule or ion that is a proton donor. • Hydrogen chloride acts as a Brønsted-Lowry acid when it reacts with ammonia. + − + → +3 4HCl NH NH Cl + −→¬ l + aq aq + aq2 3 4H O( ) NH ( ) NH ( ) OH ( ) Chapter 14 Section 2 Acid-Base Theories • Water can act as a Brønsted-Lowry acid.
  • 22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Brønsted-Lowry Acids and Bases, continued • A Brønsted-Lowry base is a molecule or ion that is a proton acceptor. • Ammonia accepts a proton from the hydrochloric acid. It acts as a Brønsted-Lowry base. + − + → +3 4HCl NH NH Cl Chapter 14 Section 2 Acid-Base Theories • The OH− ion produced in solution by Arrhenius hydroxide bases (NaOH) is the Brønsted-Lowry base. • The OH− ion can accept a proton.
  • 23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Brønsted-Lowry Acids and Bases, continued • In a Brønsted-Lowry acid-base reaction, protons are transferred from one reactant (the acid) to another (the base). + − + → +3 4HCl NH NH Cl Chapter 14 Section 2 Acid-Base Theories acid base
  • 24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Lewis Acids and Bases • A Lewis acid is an atom, ion, or molecule that accepts an electron pair to form a covalent bond. • The Lewis definition is the broadest of the three acid definitions. • A bare proton (hydrogen ion) is a Lewis acid Chapter 14 Section 2 Acid-Base Theories H+ (aq) + :NH3(aq)  [H – NH3]+ (aq) or [NH4]+ (aq)
  • 25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Lewis Acids and Bases, continued • The formula for a Lewis acid need not include hydrogen. • The silver ion can be a Lewis acid BF3 (aq) + FĞ (aq) → BF4 Ğ (aq) Chapter 14 Section 2 Acid-Base Theories • Any compound in which the central atom has three valence electrons and forms three covalent bonds can react as a Lewis acid. Ag+ (aq) + 2 :NH3(aq)  [H3N – Ag – NH3]+(aq) or [Ag(NH3)2]+
  • 26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Lewis Acids and Bases, continued Acid Base Definitions Chapter 14 Section 2 Acid-Base Theories
  • 27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives • Describe a conjugate acid, a conjugate base, and an amphoteric compound. • Define acid rain, give examples of compounds that can cause acid rain, and describe effects of acid rain. Chapter 14 Section 3 Acid-Base Reactions
  • 28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Conjugate Acids and Bases • The species that remains after a Brønsted-Lowry acid has given up a proton is the conjugate base of that acid. − +→¬ aq + l aq + aq2 3HF( ) H O( ) F ( ) H O ( ) Chapter 14 Section 3 Acid-Base Reactions acid conjugate base
  • 29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Conjugate Acids and Bases, continued • Brønsted-Lowry acid-base reactions involve two acid-base pairs, known a conjugate acid-base pairs. Chapter 14 Section 3 Acid-Base Reactions acid1 base2 base1 acid2 − +→¬ aq + l aq + aq2 3HF( ) H O( ) F ( ) H O ( )
  • 30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Neutralization Reactions Chapter 14 Section 3 Acid-Base Reactions
  • 31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases • The stronger an acid is, the weaker its conjugate base • The stronger a base is, the weaker its conjugate acid + − →g + l aq + aq2 3HCl( ) H O( ) H O ( ) Cl ( ) Chapter 14 Section 3 Acid-Base Reactions strong acid base acid weak base
  • 32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases, continued • Proton transfer reactions favor the production of the weaker acid and the weaker base. + − →aq + l aq + aq4 2 3 4HClO ( ) H O( ) H O ( ) ClO ( ) + − ¬aq + l aq + aq3 2 3 3CH COOH( ) H O( ) H O ( ) CH COO ( ) Chapter 14 Section 3 Acid-Base Reactions stronger acid stronger base weaker acid weaker base • The reaction to the right is more favorable weaker acid weaker base stronger acid stronger base • The reaction to the left is more favorable
  • 33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Relative Strengths of Acids and Bases Chapter 14 Section 3 Acid-Base Reactions Relative Strengths of Acids and Bases
  • 34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Amphoteric Compounds • Any species that can react as either an acid or a base is described as amphoteric. • example: water • water can act as a base + − →aq + l aq + aq2 4 2 3 4H SO ( ) H O( ) H O ( ) HSO ( ) + −→ +¬ g + l aq aq3 2 4NH ( ) H O( ) NH ( ) OH ( ) Chapter 14 Section 3 Acid-Base Reactions acid1 base2 acid2 base1 • water can act as an acid base1 acid2 acid1 base2
  • 35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Amphoteric Compounds, continued –OH in a Molecule • The covalently bonded -OH group in an acid is referred to as a hydroxyl group. • Molecular compounds containing —OH groups can be acidic or amphoteric. • The behavior of a compound is affected by the number of oxygen atoms bonded to the atom connected to the —OH group. Chapter 14 Section 3 Acid-Base Reactions
  • 36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Oxyacids of Chlorine Chapter 14 Section 3 Acid-Base Reactions
  • 37. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Relationship of [H3O+ ] to [OH– ] Chapter 14 Section 1 Properties of Acids and Bases
  • 38. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Acid Rain • NO, NO2, CO2, SO2, and SO3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions. SO3 (g) + H2 O(l) → H2 SO4 (aq) Chapter 14 Section 3 Acid-Base Reactions • example: • Very acidic rain is known as acid rain. • Acid rain can erode statues and affect ecosystems.
  • 39. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Acid Precipitation Chapter 14