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CHAPTER 8: ACID – BASE EQUILIBRIUM 4 U CHEMISTRY
P 526 – SEE KEY IDEAS
- examples f acids and bases.
8.1: The Nature of Acid – Base Equilibria:
- Arrhenius acids – H ions in water, bases – hydroxide ions in water
- acids – sour, turn blue litmus to red (pink), conduct electricity
- bases – bitter, soapy taste, slippery, conduct electricity, turn red litmus to blue
Bronsted – Lowry Theory:
- acids – donate proton, bases accept proton
- ex: HCl donates proton to water ( not reversible )
- ex: water donates proton to ammonia – reversible
- Amphoteric substances: ____________________________________________________________
- Advantage of B-L definition:
- 1. reactions can be identified as acid-base neutralization reactions without water
- 2. salts that form acidic or basic solutions when dissolved can be explained
Reversible Acid – Base Reactions
- many B-L acid-base reactions are reversible
- Conjugate acid – base pair – differ only by one H
- ex: H2O and H3O +
A Competition for Protons
- stronger c-acid succeeds in donating the most protons, has a weaker c-base
- stronger c-base succeeds in accepting the most protons, has a weaker c-acid
- the strong acid and strong base are always on the same side of the reaction arrow
- 99 % ionized = strong acid, ex: HCl
SUMMARY p 531 p 532 practice # 1, 2, 3.
The Autoionization of Water
- 2 molecules may collide and one molecule accepts a proton from the other – see p 532
- equilibrium of the reversible reaction – can write the constant
- Kw = [H +] [OH –1 ] = (1.0 x 10 –7 )2 = 1.0 x 10 –14
- Kw changes at different temp ( remember concept from ch 7 )
- so pH of pure water changes with diff temp
- but pure water always neutral since # protons = # hydroxide ions
Strong Acids
- ionize more than 99 % in water ex: HCl
- monoprotic acids – have only one ionizable H ex: HNO3 p 537 practice # 4, 5, 6.
Strong Bases:
- ionic substances, dissociate 100 % in water,
P 526 – SEE KEY IDEAS
- examples f acids and bases.
8.1: The Nature of Acid – Base Equilibria:
- Arrhenius acids – H ions in water, bases – hydroxide ions in water
- acids – sour, turn blue litmus to red (pink), conduct electricity
- bases – bitter, soapy taste, slippery, conduct electricity, turn red litmus to blue
Bronsted – Lowry Theory:
- acids – donate proton, bases accept proton
- ex: HCl donates proton to water ( not reversible )
- ex: water donates proton to ammonia – reversible
- Amphoteric substances: ____________________________________________________________
- Advantage of B-L definition:
- 1. reactions can be identified as acid-base neutralization reactions without water
- 2. salts that form acidic or basic solutions when dissolved can be explained
Reversible Acid – Base Reactions
- many B-L acid-base reactions are reversible
- Conjugate acid – base pair – differ only by one H
- ex: H2O and H3O +
A Competition for Protons
- stronger c-acid succeeds in donating the most protons, has a weaker c-base
- stronger c-base succeeds in accepting the most protons, has a weaker c-acid
- the strong acid and strong base are always on the same side of the reaction arrow
- 99 % ionized = strong acid, ex: HCl
SUMMARY p 531 p 532 practice # 1, 2, 3.
The Autoionization of Water
- 2 molecules may collide and one molecule accepts a proton from the other – see p 532
- equilibrium of the reversible reaction – can write the constant
- Kw = [H +] [OH –1 ] = (1.0 x 10 –7 )2 = 1.0 x 10 –14
- Kw changes at different temp ( remember concept from ch 7 )
- so pH of pure water changes with diff temp
- but pure water always neutral since # protons = # hydroxide ions
Strong Acids
- ionize more than 99 % in water ex: HCl
- monoprotic acids – have only one ionizable H ex: HNO3 p 537 practice # 4, 5, 6.
Strong Bases:
- ionic substances, dissociate 100 % in water,