1. Acid-Base Equilibria pH 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

3. pH/pOH Calculations [H 3 O + ][OH - ] = 1.0 x 10 -14 pH = -log[H 3 O + ] pOH = -log[OH - ] [H 3 O + ] = 10 -pH [OH - ] = 10 -pH pH + pOH = 14.00 What is the pH of a solution with [H 3 O + ] = 4.6 x 10 -5 What is the pOH of a solution with [OH - ] = 3.3 x 10 -4 What is the pOH of a solution with [H 3 O + ] = 2.4 x 10 -3 What is [H 3 O + ] when pH = 4.2

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

6. Acid-Base Strength: Depends on Equilibrium Constant

8. Determining the K a Value What is the value of K a for an acid for which a 0.240 M solution has a pH of 3.28?

9. Determining K b : A 0.300 M solution of a weak acid has a pH of 9.20. What is K b ?

10. What is the pH of a 0.150 M solution of HCl?

11. What is the pH of a 0.150 M solution of HF

12. What is the pH of a 0.150 M solution of HCN?

13. What is the pH of a 0.150 M solution of Ca(OH) 2 ?

14. What is the pH of a 0.150 M solution of NH 3 ?

15. Polyprotic Acids H 2 CO 3 HCO 3 - CO 3 2- H 3 PO 4 H 2 PO 4 - HPO 4 2- PO 4 3-