1). In considering the autoionization of water:

H20⇌H+ +OH-­‐‑

Why can we essentially ignore the concentration of water as a reactant in

formulating the equilibrium expression for Kw

2). How does an acid (HA) increase [H+] in aqueous solutions? What is the difference between a strong acid and a weak acid in H20? Use diagrams to illustrate your discussion.

3). How can water act as an acid or as a base? Use diagrams to illustrate your discussion.

4). Why do pH and pOH of aqueous solutions sum to 14.00 (at 25°C)? 5). Is it possible for a solution to have a pH less than 0? Explain

6). What is the difference between a Lewis base and Bronsted-­‐‑Lowry base? How important is this distinction for aqueous solutions?

7). The neutral pH of H2O at 50°C is 6.63. Is the autoionization of water exothermic, endothermic or neither? Explain.