Download - Sections 16.1-2 Acids and Bases and pH
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Sections 16.1-2Acids and Bases and pH
Bill ViningSUNY Oneonta
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Equilibrium systems
Acid base
Precipitation
Complexation
Simultaneous Equilibria
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Acid-Base EquilibriapH and pOH• Relationship of Conjugate Pair acid-base strength.• When acids or bases control pH:
determine K predict pH
• When pH controls acid/base state: predict acid/base state use acid/base state to determine pH
• Buffer action• pH titration curves
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Bronsted Acids and BasesBronsted Acid: H+ (proton) donorBronsted Base: H+ acceptor
Acid-Base reactions: H+ transfer reaction
Conjugate Acid-Base Pairs: acid conjugate base HF F-
NH4+ NH3
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What is the conjugate base of HNO2?
1. H2NO2+
2. HNO3
3. NO2-
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What is the conjugate acid of HPO42-?
1. H2PO4-
2. H3PO4
3. PO43-
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What is the conjugate base of HPO42-?
1. H2PO4-
2. H3PO4
3. PO43-
What is the conjugate acid of HPO42-?
1. H2PO4-
2. H3PO4
3. PO43-
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+ -2 3
-14 + -a 3
2 H O H O + OH
K = 1.0 10 = [H O ][OH ]
pH/pOH Relationships and Calculations
[H3O+][OH-] = 1.0 x 10-14
pH = -log[H3O+] pOH = -log[OH-]
[H3O+] = 10-pH [OH-] = 10-pH
pH + pOH = 14.00
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+ -2 3
-14 + -a 3
2 H O H O + OH
K = 1.0 10 = [H O ][OH ]
Neutral, Acidic and Basic Solutions
Neutral Acidic Basic
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What is [H3O+] when [OH-] = 5.4 x 10-3 M?
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What is the pH of a solution with [H3O+] = 4.6 x 10-5 M?
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What is [H3O+] in a solutionwith pH = 8.24?
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What is the pOH of a solution with [OH-] = 3.3 x 10-4 M?
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What is the pH of a solution with [OH-] = 2.4 x 10-3 M?
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Strong acids and basesFor strong acid solutions, [H3O+] = [acid] (except for H2SO4)
For strong bases LiOH, NaOH, KOH, RbOH, [OH-] = [base]
For strong bases Ca(OH)2, Ba(OH)2, etc., [OH-] = 2 x [base]
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What is the pH of a 0.150 M solution of HCl?
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What is the pH of a 0.150 M solution of Ca(OH)2?