Transcript Document 7707549

Chapter 15: Aqueous Equilibria: Acids and Bases
1. acid/base
characteristics
reactions (Arrhenius, Bronsted-Lowry, gas formation)
hydronium ion
polyprotic, amphiprotic acids
conjugate pairs
strong vs. weak acids/bases
2. water autoionization, KW, pH and pOH
3. measuring pH
4. pH of solutions of strong acids/bases (calculations)
5. weak acids
equilibria & Ka; calculations (pH from Ka and Ka from
pH); %ionization; polyprotic acids
6. weak bases
calculations
relationship to Ka
7. salts
reactions
calculations
Chapter 15 Notes
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Chapter 15: Aqueous Equilibria: Acids and Bases
8. factors affecting acid/base strength
9. Lewis acids/bases
1. acids & bases:
characteristics
Acids
Bases
taste sour
taste bitter
corrosive to metal
feel slippery
aqueous acids conduct
(electrolytes)
acids turn litmus red
aqueous bases conduct
(electrolytes)
bases turn litmus blue
acids: rainwater, coffee, fruit, carbonated water, vinegar,
stomach
neutral: blood, tears, saliva, milk
bases: ammonia, lime water, borax, baking soda, lye, soap
Chapter 15 Notes
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1. acids & bases:
reactions
1. Arrhenius acid/base reaction:
acid donates H1+ and base donates OH1general reaction: acid+basesalt+water
examples:
HCl(aq)+NaOH(aq)  NaCl(aq)+H2O(l)
HNO3(aq)+KOH(aq) 
net ionic equation:
what about NH3? and Na2CO3? both are bases - how to
understand?
2. Bronsted-Lowry reaction: more general
acid supplies H1+ and base grabs H1+
acid must have H1+ to donate and base must have lone pair
of e1Chapter 15 Notes
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1. acids & bases:
reactions
2. Bronsted-Lowry reaction: more general
acid supplies H1+ and base grabs H1+
acid must have H1+ to donate and base must have lone pair
of e1examples: (identify the acid and base in each)
CO32-(aq)+HCl(aq)HCO31-(aq)+Cl1-(aq)
HSO31-(aq)+H2O(l) 
HBr(aq)+NH3(aq) 
HNO3(aq)+CH3NH2(aq) 
Chapter 15 Notes
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1. acids & bases:
reactions
•HCN & H2S: solubility in water low; gaseous HCN & H2S
bubble out of sol’n at high concentrations
•H2CO3 and H2SO3: decompose at high concentrations
example:
HCl(aq)+HS1-(aq)H2S(g)+Cl1HBr(aq)+CN1-(aq) 
HCO31-(aq)+HNO3(aq) H2CO3(aq)+NO31-(aq)
H2O(l)+CO2(g)
hydronium ion: H3O1+; hydrated H1+ [H(H2O)n1+, where n=1,2,3...]
polyprotic: can donate >1 H1+; H2SO4, H2CO3, H3PO4, H2S
amphiprotic: can donate and accept H1+: H2O, HCO31-, HS1-, H2PO4-,
HPO42-,
Chapter 15 Notes
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1. acids & bases:
conjugate pairs: acid/base pairs that differ by transfer of H1+
examples- acid/base: H2O/OH1-; HC2H3O2/C2H3O21-; HCl/Cl1-;
name the conjugate acid of: H2O
NO31Br1-
HS1CH3NH2
name the conjugate base of: H3O1+
H3PO4
CO32strong vs. weak
strong: strong electrolyte, dissociates 100% in water
in water, exists as:
weak: weak electrolyte, dissociates <10% in water
in water, exists as:
driving force in acid/base reactions:
1. from strong to weak
2. strong acids, bases are dissociated, weak acids, bases
are molecular
Chapter 15 Notes
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Chapter 15 Notes
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1. acids & bases:
strong vs. weak
example:
predict the products, then predict whether the reaction goes left,
right, or “can’t tell”
HCl(aq)+NO2-1
Br1-(aq)+NH41+(a q) 
HC2H3O2(aq)+HS1-(aq) 
NO31-(aq)+CH3NH31+(aq) 
Chapter 15 Notes
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