Sections 16.3 – 16.6 Acid-Base Equilibria Bill Vining SUNY Oneonta.

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Presentation transcript:

Sections 16.3 – 16.6 Acid-Base Equilibria Bill Vining SUNY Oneonta

Acid-Base Equilibria In these sections… a.Relative acid-base strength b.Determining Ka and Kb experimentally c.Estimating pH of solutions d.Acid-Base Properties of Salts e.Molecular control of acid-base strength

Acid-Base Equilibria Bronsted Acid: H + (proton) donor Bronsted Base: H + acceptor Acid-Base reactions: H + transfer reaction Conjugate Acid-Base Pairs: acid conjugate base HFF - NH 4 + NH 3

Strong vs. Weak Acids

Weak Acid-Base Strength Varies Greatly Depending on the Equilibrium Constant

Trends in relative acid/base strength for conjugate pairs.

Relationship Between K a and K b for an Acid-Base Conjugate Pair K a x K b = 1.0 x Ammonia is a base with K b = 1.8 x What is the conjugate acid, and what is its K a value?

Determining the K a Value Experimentally Measure pH for a solution of known concentration. pH  [H 3 O + ]  x in an ICE table  all [ ]’s  K a What is the value of K a for an acid, HA, for which a M solution has a pH of 3.28?

Determining K b : A M solution of a weak base has a pH of What is K b ?

Estimating the pH when [HA] and K a are known Set up ICE Table  x = [H 3 O + ]  pH What is the pH of a M solution of HF?

Estimate when [HA] o > 100 x K a What is the pH of a M solution of HCN?

Estimating pH of weak base solutions What is the pH of a M solution of NH 3 ?