acids & bases
DESCRIPTION
Acids & Bases. Text book. Section 8.2A Sections 16.1 & 16.2. Self-ionization of water (Autoionization). Truth H 2 O + H 2 O H 3 O + + OH - Convenient Lie H 2 O H + + OH -. H 3 O + = hydronium ion H + = hydrogen ion OH - = hydroxide ion. P H E N O L P H T H A L E I N. - PowerPoint PPT PresentationTRANSCRIPT
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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 ion
H+ = hydrogen ion
OH- = 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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acid
base
PHENOLPHTHALEIN
Page 583
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Acids react with active metals to produce hydrogen gas.
(Page 264)
M + HA MA + H2
Example: 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 + H2
Example: Zn + 2 HCl ZnCl2 + H2
Ionic: 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 + H2O
Example:2 HCl + CaCO3 CaCl2 + CO2 + H2O
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What’s really happening?
2 HCl + CaCO3 CaCl2 + H2CO3
A double replacement reaction.
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BUT H2CO3 isn’t stable at room temperature and pressure. It spontaneously decomposes:
H2CO3 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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HomeworkPredict the products and write complete
balanced reactions.1) Mg(s) + HBr(aq) → 2) Al(s) + HNO3(aq) →3) H2SO4(aq) + K2CO3(aq) →4) MgCO3(s) + HClO4(aq) →
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ACID BASE
ArrheniusMake H+
ion in water
Make OH-
ion in water
[H3O+] to [OH-]
Bronsted
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ACID BASE
ArrheniusMake H+
Ion in water
Make OH-
Ion in water
[H3O+] to [OH-]
[H3O+] > [OH-] [H3O+] < [OH-]
Bronsted
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ACID BASE
ArrheniusMake H+
Ion in water
Make OH-
Ion in water
[H3O+] to [OH-]
[H3O+] > [OH-] [H3O+] < [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: AcidsTruth
HA + H2O H3O+ + A-
Convenient LieHA H+ + A-
Ionization
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Electrolyte formation: AcidsSee page 563
TruthHCl + 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 don’t 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 + salt
HBr + NaOH H2O + NaBr
Ionic: H+ + OH- H2O
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Homework• Page 273, #22 & 23
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BronstedNeutralizationacid + base protonated base + anion
HA + 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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So……An 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 lose 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 or amphiprotic
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Examples:
HCl + H2O H3O+ + Cl-
NH3 + H2ONH4+ + OH-
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HCl + H2O H3O+ + Cl-
acid base ca cb
NH3 + H2ONH4+ + 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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