Acids

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Acids Bases
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Text book

• Section 8.2A
• Sections 16.1 16.2

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Self-ionization of water(Autoionization)
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TruthH2O H2O ? H3O OH-Convenient LieH2O
? H OH-
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H3O hydronium ionH hydrogen ionOH-
hydroxide ion
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ACID BASE
Taste
Slippery?
Litmus
Phenol-phthalein
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ACID BASE
Taste Sour Bitter
Slippery?
Litmus
Phenol-phthalein
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ACID BASE
Taste Sour Bitter
Slippery? No Yes
Litmus
Phenol-phthalein
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ACID BASE
Taste Sour Bitter
Slippery? No Yes
Litmus Red Blue
Phenol-phthalein
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ACID BASE
Taste Sour Bitter
Slippery? No Yes
Litmus Red Blue
Phenol-phthalein Colorless Red
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P H E N O L P H T H A L E I N
?acid
?base
Page 583
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Acids react with active metals to produce
hydrogen gas. (Page 264)M HA ? MA
H2Example Zn 2 HCl ? ZnCl2 H2(A single
replacement reaction)
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Salt cation plus the anion of an acid
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Acids react with active metals to produce
hydrogen gas.M HA ? MA H2Example Zn 2
HCl ? ZnCl2 H2Ionic Zn 2H ? Zn2 H2
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Acids react with carbonates and hydrogen
carbonates to produce carbon dioxide and water.
(Page 264)
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HA MCO3 ? MA CO2
H2OExample2 HCl CaCO3 ? CaCl2
CO2 H2O
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Whats really happening? 2 HCl CaCO3 ?
CaCl2 H2CO3A double replacement
reaction.
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BUT H2CO3 isnt stable at room temperature and
pressure. It spontaneously decomposesH2CO3 ??
H2O CO2
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So 2 HCl CaCO3 ? CaCl2 CO2 H20
Ionic 2 H CaCO3 ? Ca2
CO2 H20
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HA MHCO3 ? MA CO2 H2O EX
HC2H3O2 NaHCO3? NaC2H3O2 CO2 H2O
Ionic HC2H3O2 HCO3- ? C2H3O2-
CO2 H2O
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Homework

• Predict the products and write complete balanced
  reactions.
• Mg(s) HBr(aq) ?
• Al(s) HNO3(aq) ?
• H2SO4(aq) K2CO3(aq) ?
• MgCO3(s) HClO4(aq) ?

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ACID BASE
Arrhenius Make H ion in water Make OH- ion in water
H3O to OH-
Bronsted
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ACID BASE
Arrhenius Make H Ion in water Make OH- Ion in water
H3O to OH- H3O gt OH- H3O lt OH-
Bronsted
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ACID BASE
Arrhenius Make H Ion in water Make OH- Ion in water
H3O to OH- H3O gt OH- H3O lt OH-
Bronsted proton (H) donor proton(H) acceptor
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Definitions

• monoprotic can donate one proton (HA, EX HCl)
• diprotic can donate two protons (H2A, EX
  H2SO4)
• triprotic can donate three protons (H3A, EX
  H3PO4)
• polyprotic diprotic and triprotic

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Electrolyte formation AcidsTruthHA H2O ?
H3O A-Convenient LieHA ? H A-Ionization
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Electrolyte formation AcidsSee page
563TruthHCl H2O ? H3O Cl-Convenient
LieHCl ? H Cl-Ionization
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Acid Strength

• Strong acids ionize completely.
• Weak acids do not ionize completely.
• See solubility rules for list of strong acids.
• Figure 16.1 on page 567

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Electrolyte formation BaseCation(OH) ? Cation
OH-Ex Ca(OH)2 ? Ca2 2 OH-
(dissociation)
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Electrolyte formation BaseCation(OH) ? Cation
OH-Ex Ca(OH)2 ? Ca2 2 OH-
(dissociation) B H2O ? BH OH-(B base,
BH protonated base)Ex NH3 H2O ? NH4
OH-(ionization)
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Base Strength

• Strong bases are hydroxide compounds that
  dissociate completely.
• See solubility rules for a list of strong bases.
• Weak bases are other hydroxide compounds (they
  dont dissolve significantly into cations and
  hydroxide) AND all molecular bases (EX NH3)

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Concentration -v- Strength

• These two concepts have nothing to do with each
  other.
• An acid/base can be dilute and strong (Ex 0.01M
  HCl)
• An acid/base can be concentrated and weak (Ex
  8M H2SO3)

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Homework

• Page 273, 20 (Truth and
  convenient lie)
• Page 273, 21

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Arrhenius neutralization acid base ? water
saltHBr NaOH ?H2O NaBrIonic H OH- ?
H2O
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Homework

• Page 273, 22 23

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BronstedNeutralizationacid base ? protonated
base anionHA B ? BH A-
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BronstedNeutralizationHA B ? BH A-HCl
NH3 ? NH4 Cl- Ionic H NH3 ? NH4
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Bronsted conjugates(Page 563)

• Acid HA
• ? Conjugate base A-
• Base B
• ? Conjugate acid HB

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SoAn acid loses proton to become a conjugate
base (ready to accept a proton)
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And..A base gains a proton to become a
conjugate acid (ready to loose a proton)
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Acid-base reaction

• One substance donates a proton
• One substance accepts a proton

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Page 564

• Example 16.1 16.2
• Practice 16.2
• Homework Page 572, Section Review 1-5

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Relative strength

• See page 567.
• Strong acid ? weak conjugate base
• Weak acid ? strong conjugate base
• Strong base ? weak conjugate acid
• Weak base ? strong conjugate acid

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Homework

• Page 589, 13-16

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Water can accept or donate a proton(Recall
autoionization.)

• amphoteric

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ExamplesHCl H2O ? H3O Cl-NH3 H2O?NH4
OH-
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HCl H2O ? H3O Cl-acid base ca
cbNH3 H2O?NH4 OH-base acid ca
cb
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Lewis definition

• Acid electron pair acceptor
• Base electron pair donor

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coordinate bonding

• One atom donates both of the electrons in the
  covalent bond
• A coordination complex is formed.

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coordinate bonding ? coordination complex
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