Sections 16.3 – 16.6 Acid-Base Equilibria
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Transcript of Sections 16.3 – 16.6 Acid-Base Equilibria
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Sections 16.3 – 16.6Acid-Base Equilibria
Bill ViningSUNY Oneonta
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Acid-Base Equilibria
In these sections…
a.Relative acid-base strengthb.Determining Ka and Kb experimentallyc.Estimating pH of solutionsd.Acid-Base Properties of Saltse.Molecular control of acid-base strength
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Acid-Base EquilibriaBronsted 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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Strong vs. Weak Acids
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Weak Acid-Base Strength Varies Greatly Depending on the Equilibrium Constant
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Trends in relative acid/base strength for conjugate pairs.
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Relationship Between Ka and Kb for an Acid-Base Conjugate Pair
Ka x Kb = 1.0 x 10-14
Ammonia is a base with Kb = 1.8 x 10-5. What is the conjugate acid, and what is its Ka value?
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Determining the Ka Value Experimentally
Measure pH for a solution of known concentration.pH [H3O+] x in an ICE table all [ ]’s Ka
What is the value of Ka for an acid, HA, for which a 0.240 M solution has a pH of 3.28?
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Determining Kb:
A 0.300 M solution of a weak base has a pH of 9.20. What is Kb?
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Estimating the pH when [HA] and Ka are known
Set up ICE Table x = [H3O+] pH
What is the pH of a 0.150 M solution of HF?
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Estimate when [HA]o > 100 x Ka
What is the pH of a 0.150 M solution of HCN?
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Estimating pH of weak base solutions
What is the pH of a 0.150 M solution of NH3?
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